,a ,,system ,,of ,,instruction ,,in ,,the ,,practical ,,use ,,of ,,the ,,blowpipe4 ,,being ,a ,,graduated ,,course ,,of ,,analysis ,,for ,,the ,,use ,,of ,,students ,,and ,,all ,,those ,,engaged ,,in ,,the ,,examination ,,of ,,metallic ,,combinations4 ,,new ,,york3 ,h4 ,,bailli,,re1 #bij ,,broadway1 ,,and #bai ,,regent ,,street1 ,,london4 ,,paris3 ,j4,b4 ,,bailli,,re ,,et ,,fils1 ,,rue ,,hautefeuille4 ,,madrid3 ,c4 ,,bailly-,,bailli,,re1 ,,calle ,,del ,,principe4 #aheh4 99 99 99 99 99 ,,entered according to ,act of ,congress1 in the year #aheh1 by ,c4,e4 ,,bailli,,re1 ,in the ,clerk's ,office of the ,district ,court of the ,united ,states1 for the ,southern ,district of ,new ,york4 ,w4,h4 ,,tinson1 ,printer and ,stereotyper1 #dc ,centre ,street4 99 99 99 99 99 ,,table ,,of ,,contents4 ,,part ,i4 ,preface1 #g ,the ,use of the ,blowpipe1 #i ,utensils--,the ,blowpipe1 #ab ,the ,oil ,lamp1 #bb ,the ,spirit ,lamp1 #bc ,charcoal ,support1 #bd ,platinum ,supports1 #bf ,iron ,spoons1 #bh ,glass ,tubes1 #bh ,other ,apparatus necessary1 #ca ,,the ,,reagents1 #cd ,reagents of ,general ,use1 #cd ,carbonate of ,soda1 #cd ,hydrate of ,baryta1 #ce ,bi-sulphate of ,potassa1 #ce ,oxalate of ,potassa1 #cf ,cyanide of ,potassium1 #cf ,nitrate of ,potassa1 #cg ,borax1 #ch ,microcosmic ,salt1 #ci ,nitrate of ,cobalt1 #dj ,tin1 #da ,silica1 #db ,test ,papers1 #db ,,especial ,,reagents1 #dc ,boracic ,acid1 #dc ,fluorspar1 #dc ,oxalate of ,nickel1 #dc ,oxide of ,copper1 #dc ,antimoniate of ,potassa1 #dd ,silver ,foil1 #dd ,nitroprusside of ,sodium1 #dd ,,part ,,ii4 ,initiatory ,analysis1 #dg ,examination with the ,glass ,bulb1 #dg in the ,open ,tube1 #eb upon ,charcoal1 #ee in the ,platinum ,forceps1 #fa in the ,borax ,bead1 #fi in ,microcosmic ,salt1 #gb ,table ,i4--,colors of ,beads of ,borax and ,microcosmic ,salt1 #ge ,table ,,ii4--,behavior of ,metallic ,oxydes with ,borax and ,microcosmic ,salt1 #he ,examinations with ,carbonate of ,soda1 #ajc ,,part ,,iii4 ,special ,reactions1 #aji ,a4--,,metallic ,,oxides3 ,first ,group4--,the ,alkalies3 ,potassa1 ,soda1 ,ammonia1 and ,lithia1 #aaj ,second ,group4--,the ,alkaline ,earths3 ,baryta1 ,strontia1 ,lime1 and ,magnesia1 #aae ,third ,group4--,the ,earths3 ,alumina1 ,glucina1 ,yttria1 ,thorina1 and ,zirconia1 #aba ,fourth ,group4--,cerium1 ,lanthanium1 ,didymium1 ,columbium1 ,niobium1 ,pelopium1 ,titanium1 ,uranium1 ,vanadium1 ,chromium1 ,manganese1 #abd ,fifth ,group4--,iron1 ,cobalt1 ,nickel1 #ace ,sixth ,group4--,zinc1 ,cadmium1 ,antimony1 ,tellurium1 #adj ,seventh ,group4--,lead1 ,bismuth1 ,tin1 #adi ,eighth ,group4--,mercury1 ,arsenic1 #aeg ,ninth ,group4--,copper1 ,silver1 ,gold1 #afa ,tenth ,group4--,molybdenum1 ,osmium1 #afe ,eleventh ,group4--,platinum1 ,palladium1 ,iridium1 ,rhodium1 ,ruthenium1 #afg ,non-,metallic ,substances1 #afh ,tabular ,statement of the ,reactions of ,minerals before the ,blowpipe1 #agh ,carbon and ,organic ,minerals1 #aha ,potassa1 #ahd ,soda1 #ahf ,baryta and ,strontia1 #aij ,lime1 #aib ,magnesia1 #aif ,alumina1 #bjj ,silicates1 #bjd ,uranium1 #bab ,iron1 #bad ,manganese1 #bbb ,nickel and ,cobalt1 #bbf ,zinc1 #bcb ,bismuth1 #bcd ,lead1 #bch ,copper1 #bdh ,antimony1 #bef ,arsenic1 #bfj ,mercury1 #bfb ,silver1 #bfd 99 99 99 99 99 ,,preface4 ,it is believed the arrangement of the present work is superior to that of many of its predecessors1 as a vehicle for the facilitation of the student's progress4 ,while it does not pretend to any other rank than as an introduction to the larger works1 it is hoped that the arrangement of its matter is such that the beginner may more readily comprehend the entire subject of ,blowpipe ,analysis than if he were to begin his studies by the perusal of the more copious works of ,berzelius and ,plattner4 ,when the student shall have gone through these pages1 and repeated the various reactions described1 then he will be fully prepared to enter upon the study of the larger works4 ,to progress through them will then be but a comparatively easy task4 ,the arrangement of this little work has been such as the author and his friends have considered the best that could be devised for the purpose of facilitating the progress of the student4 ,whether we have succeeded is left for the public to decide4 ,the author is indebted to several of his friends for valuable contributions and suggestions4 ,s4 ,,cincinnati1 ,june1 #aheg4 99 99 99 99 99 ,,the ,,blowpipe4 99 99 99 99 99 ,part ,first4 ,,the ,,use ,,of ,,the ,,blowpipe4 ,perhaps during the last fifty years1 no department of chemistry has been so enriched as that relating to analysis by means of the ,blowpipe4 ,through the unwearied exertions of men of science1 the use of this instrument has arrived to such a degree of perfection1 that we have a right to term its use1 ,analysis in the dry way1 in contradistinction to analysis in the wet way4 ,the manipulations are so simple and expeditious1 and the results so clear and characteristic1 that the ,blowpipe analysis not only verifies and completes the results of analysis in the wet way1 but it gives in many cases direct evidences of the presence or absence of many substances1 which would not be otherwise detected1 but through a troublesome and tedious process1 involving both prolixity and time2 for instance1 the detection of manganese in minerals4 ,many substances have to go through ,blowpipe manipulations before they can be submitted to an analysis in the wet way4 ,the apparatus and reagents employed are compendious and small in number1 so that they can be carried easily while on scientific excursions1 a considerable advantage for mineralogists and metallurgists4 ,the principal operations with the ,blowpipe may be explained briefly as follows3 7a47 ,by ,ignition is meant the exposure of a substance to such a degree of heat1 that it glows or emits light1 or becomes red-hot4 ,its greatest value is in the separation of a volatile substance from one less volatile1 or one which is entirely fixed at the temperature of the flame4 ,in this case we only take cognizance of the latter or fixed substance1 although in many instances we make use of ignition for the purpose of changing the conditions of a substance1 for example1 the sesquioxide of chromium 7,cr#b,o#c7 in its insoluble modification2 and as a preliminary examination for the purpose of ascertaining whether the subject of inquiry be a combination of an organic or inorganic nature4 ,the apparatus used for this purpose are crucibles of platinum or silver1 platinum foil1 a platinum spoon1 platinum wire or tongs1 charcoal1 glass tubes1 and iron spoons4 7b47 ,sublimation is that process by which we convert a solid substance into vapor by means of a strong heat4 ,these vapors are condensed by refrigeration into the solid form4 ,it may be termed a distillation of a solid substance4 ,sublimation is of great consequence in the detection of many substances2 for instance1 arsenic1 antimony1 mercury1 etc4 ,the apparatus used for the purposes of sublimation consist of glass tubes closed at one end4 7c47 ,fusion4--,many substances when exposed to a certain degree of heat lose their solid form1 and are converted into a liquid4 ,those substances which do not become converted into the liquid state by heat1 are said to be infusible4 ,it is a convenient classification to arrange substances into those which are fusible with difficulty1 and those which are easily fusible4 ,very often we resort to fusion for the purpose of decomposing a substance1 or to cause it to enter into other combinations1 by which means it is the more readily detected4 ,if insoluble substances are fused with others more fusible 7reagents7 for the purpose of causing a combination which is soluble in water and acids1 the operation is termed unclosing4 ,these substances are particularly the silicates and the sulphates of the alkaline earths4 ,the usual reagents resorted to for this purpose are carbonate of soda 7,na,o1 ,,co#b71 carbonate of potash 7,,ko1 ,,co#b71 or still better1 a mixture of the two in equal parts4 ,in some cases we use the hydrate of barytes 7,ba,o1 ,,ho7 and the bisulphate of potash 7,,ko1 #b,,so#c74 ,the platinum spoon is generally used for this manipulation4 ,substances are exposed to fusion for the purpose of getting a new combination which has such distinctive characteristics that we can class it under a certain group2 or for the purpose of ascertaining at once what the substance may be4 ,the reagents used for this purpose are borax 7,na,o1 #b;,br,o#c7 and the microcosmic salt 7,na,o1 ,,nh#d,o1 ,,po#e1 ,,ho74 ,charcoal and the platinum wire are used as supports for this kind of operation4 7d47 ,oxidation4--,the chemical combination of any substance with oxygen is termed oxidation1 and the products are termed oxides4 ,as these oxides have qualities differing from those which are non-oxidized1 it therefore frequently becomes necessary to convert substances into oxides2 or1 if they are such1 of a lower degree1 to convert them into a higher degree of oxidation4 ,these different states of oxidation frequently present characteristic marks of identity sufficient to enable us to draw conclusions in relation to the substance under examination4 ,for instance1 the oxidation of manganese1 of arsenic1 etc4 ,the conditions necessary for oxidation1 are high temperature and the free admission of air to the substance4 ,if the oxidation is effected through the addition of a substance containing oxygen 7for instance1 the nitrate or chlorate of potash7 and the heating is accompanied by a lively deflagration and crackling noise1 it is termed detonation4 ,by this process we frequently effect the oxidation of a substance1 and thus we prove the presence or the absence of a certain class of substances4 ,for instance1 if we detonate 7as it is termed by the ,german chemists7 the sulphide of antimony1 or the sulphide of arsenic with nitrate of potash1 we get the nitrate of antimony1 or the nitrate of arsenic4 ,the salts of nitric or chloric acid are determined by fusing them with the cyanide of potassium1 because the salts of these acids detonate4 7e47 ,reduction4--,if we deprive an oxidized substance of its oxygen1 we term the process reduction4 ,this is effected by fusing the substance under examination with another which possesses a greater affinity for oxygen4 ,the agents used for reduction are hydrogen1 charcoal1 soda1 cyanide of potassium1 etc4 ,substances generally1 when in the unoxidized state1 have such characteristic qualities1 that they cannot very readily be mistaken for others4 ,for this reason1 reduction is a very excellent expedient for the purpose of discerning and classifying many substances4 ,b4 ,,utensils4 ,we shall give here a brief description of the most necessary apparatus used for analysis in the dry way1 and of their use4 ,the ,blowpipe is a small instrument1 made generally out of brass1 silver1 or ,german silver1 and was principally used in earlier times for the purpose of soldering small pieces of metals together4 ,it is generally made in the form of a tube1 bent at a right angle1 but without a sharp corner4 ,the largest one is about seven inches long1 and the smallest about two inches4 ,the latter one terminates with a small point1 with a small orifice4 ,the first use of the blowpipe that we have recorded is that of a ,swedish mining officer1 who used it in the year #agch for chemical purposes1 but we have the most meagre accounts of his operations4 ,in #ageh another ,swedish mining officer1 by the name of ,cronstedt1 published his ,use of the ,blowpipe in ,chemistry and ,mineralogy1 translated into ,english1 in #aggj1 by ,van ,engestroem4 ,bergman extended its use1 and after him ,ghan and the venerable ,berzelius 7#ahba74 ,the blowpipe most generally used in chemical examinations is composed of the following parts3 7,fig4 #a47 ,a is a little reservoir made air-tight by grinding the part ,b into it4 ,this reservoir serves the purpose of retaining the moisture with which the air from the mouth is charged4 ,a small conical tube is fitted to this reservoir4 ,this tube terminates in a fine orifice4 ,as this small point is liable to get clogged up with soot1 etc41 it is better that it should be made of platinum1 so that it may be ignited4 ,two of these platinum tubes should be supplied1 differing in the size of the orifice1 by which a stronger or lighter current of flame may be projected from it4 ,metals1 such as brass or ,german silver1 are very liable to become dirty through oxidation1 and when placed between the lips are liable to impart a disagreeable taste4 ,to avoid this1 the top of the tube must be supplied with a mouthpiece of ivory or horn ,c4 ,the blowpipe here represented is the one used by ,ghan1 and approved by ,berzelius4 ,the trumpet mouthpiece was adopted by ,plattner2 it is pressed upon the lips while blowing1 which is less tiresome than holding the mouthpiece between the lips1 although many prefer the latter mode4 ,illustration3 ,fig4 #a ,dr4 ,black's blowpipe is as good an instrument and cheaper4 ,it consists of two tubes1 soldered at a right angle2 the larger one1 into which the air is blown1 is of sufficient capacity to serve as a reservoir4 ,a chemist can1 with a blowpipe and a piece of charcoal1 determine many substances without any reagents1 thus enabling him1 even when travelling1 to make useful investigations with means which are always at his disposal4 ,there are pocket blowpipes as portable as a pencil case1 such as ,wollaston's and ,mitscherlich's2 these are objectionable for continued use as their construction requires the use of a metallic mouthpiece4 ,mr4 ,casamajor1 of ,new ,york1 has made one lately which has an ivory mouthpiece1 and which1 when in use1 is like ,dr4 ,black's4 ,illustration3 ,fig4 #b ,the length of the blowpipe is generally seven or eight inches1 but this depends very much upon the visual angle of the operators4 ,a short-sighted person1 of course1 would require an instrument of less length than would suit a far-sighted person4 ,the purpose required of the blowpipe is to introduce a fine current of air into the flame of a candle or lamp1 by which a higher degree of heat is induced1 and consequently combustion is more rapidly accomplished4 ,by inspecting the flame of a candle burning under usual circumstances1 we perceive at the bottom of the flame a portion which is of a light blue color 7a b71 ,fig4 #b1 which gradually diminishes in size as it recedes from the wick1 and disappears when it reaches the perpendicular side of the flame4 ,in the midst of the flame there is a dark nucleus with a conical form 7c74 ,this is enveloped by the illuminating portion of the flame 7d74 ,at the exterior edge of the part d we perceive a thin1 scarcely visible veil1 a1 e1 e1 which is broader near the apex of the flame4 ,the action of the burning candle may be thus explained4 ,the radiant heat from the flame melts the tallow or wax1 which then passes up into the texture of the wick by capillary attraction until it reaches the glowing wick1 where the heat decomposes the combustible matter into carbonated hydrogen 7,c#d;,h#d71 and into carbonic oxide 7,,co74 ,while these gases are rising in hot condition1 the air comes in contact with them and effects their combustion4 ,the dark portion1 c1 of the flame is where the carbon and gases have not a sufficiency of air for their thorough combustion2 but gradually they become mixed with air1 although not then sufficient for complete combustion4 ,the hydrogen is first oxidized or burnt1 and then the carbon is attacked by the air1 although particles of carbon are separated1 and it is these1 in a state of intense ignition1 which produce the illumination4 ,by bringing any oxidizable substance into this portion of the flame1 it oxidizes very quickly in consequence of the high temperature and the free access of air4 ,for that reason this part of the flame is termed the oxidizing flame1 while the illuminating portion1 by its tendency to abstract oxygen for the purpose of complete combustion1 easily reduces oxidated substances brought into it1 and it is1 therefore1 called the flame of reduction4 ,in the oxidizing flame1 on the contrary1 all the carbon which exists in the interior of the flame is oxidized into carbonic acid 7,,co#b7 and carbonic oxide 7,,co71 while the blue color of the cone of the flame is caused by the complete combustion of the carbonic oxide4 ,these two portions of the flame--the oxidizing and the reducing--are the principal agents of blowpipe analysis4 ,if we introduce a fine current of air into a flame1 we notice the following3 ,the air strikes first the dark nucleus1 and forcing the gases beyond it1 mixes with them1 by which oxygen is mingled freely with them4 ,this effects the complete combustion of the gases at a certain distance from the point of the blowpipe4 ,at this place the flame has the highest temperature1 forming there the point of a blue cone4 ,the illuminated or reducing portion of the flame is enveloped outside and inside by a very hot flame1 whereby its own temperature is so much increased that in this reduction-flame many substances will undergo fusion which would prove perfectly refractory in a common flame4 ,the exterior scarcely visible part loses its form1 is diminished1 and pressed more to a point1 by which its heating power is greatly increased4 ,the ,blast of ,air4--,by using the blowpipe for chemical purposes1 the effect intended to be produced is an uninterrupted steady stream of air for many minutes together1 if necessary1 without an instant's cessation4 ,therefore1 the blowing can only be effected with the muscles of the cheeks1 and not by the exertion of the lungs4 ,it is only by this means that a steady constant stream of air can be kept up1 while the lungs will not be injured by the deprival of air4 ,the details of the proper manner of using the blowpipe are really more difficult to describe than to acquire by practice2 therefore the pupil is requested to apply himself at once to its practice1 by which he will soon learn to produce a steady current of air1 and to distinguish the different flames from each other4 ,we would simply say that the tongue must be applied to the roof of the mouth1 so as to interrupt the communication between the passage of the nostrils and the mouth4 ,the operator now fills his mouth with air1 which is to be passed through the pipe by compressing the muscles of the cheeks1 while he breathes through the nostrils1 and uses the palate as a valve4 ,when the mouth becomes nearly empty1 it is replenished by the lungs in an instant1 while the tongue is momentarily withdrawn from the roof of the mouth4 ,the stream of air can be continued for a long time1 without the least fatigue or injury to the lungs4 ,the easiest way for the student to accustom himself to the use of the blowpipe1 is first to learn to fill the mouth with air1 and while the lips are kept firmly closed to breathe freely through the nostrils4 ,having effected this much1 he may introduce the mouthpiece of the blowpipe between his lips4 ,by inflating the cheeks1 and breathing through the nostrils1 he will soon learn to use the instrument without the least fatigue4 ,the air is forced through the tube against the flame by the action of the muscles of the cheeks1 while he continues to breathe without interruption through the nostrils4 ,having become acquainted with this process1 it only requires some practice to produce a steady jet of flame4 ,a defect in the nature of the combustible used1 as bad oil1 such as fish oil1 or oil thickened by long standing or by dirt1 dirty cotton wick1 or an untrimmed one1 or a dirty wickholder1 or a want of steadiness of the hand that holds the blowpipe1 will prevent a steady jet of flame4 ,but frequently the fault lies in the orifice of the jet1 or too small a hole1 or its partial stoppage by dirt1 which will prevent a steady jet of air1 and lead to difficulty4 ,with a good blowpipe the air projects the entire flame1 forming a horizontal1 blue cone of flame1 which converges to a point at about an inch from the wick1 with a larger1 longer1 and more luminous flame enveloping it1 and terminating to a point beyond that of the blue flame4 ,to produce an efficient flame of oxidation1 put the point of the blowpipe into the flame about one third the diameter of the wick1 and about one twelfth of an inch above it4 ,this1 however1 depends upon the size of the flame used4 ,blow strong enough to keep the flame straight and horizontal1 using the largest orifice for the purpose4 ,upon examining the flame thus produced1 we will observe a long1 blue flame1 a b1 ,fig4 #c1 which letters correspond with the same letters in ,fig4 #b4 ,but this flame has changed its form1 and contains all the combustible gases4 ,it forms now a thin1 blue cone1 which converges to a point about an inch from the wick4 ,this point of the flame possesses the highest intensity of temperature1 for there the combustion of the gases is the most complete4 ,in the original flame1 the hottest part forms the external envelope1 but here it is compressed more into a point1 forming the cone of the blue flame1 and likewise an envelope of flame surrounding the blue one1 extending beyond it from a to c1 and presenting a light bluish or brownish color4 ,the external flame has the highest temperature at d1 but this decreases from d to c4 ,illustration3 ,fig4 #c ,if there is a very high temperature1 the oxidation is not effected so readily in many cases1 unless the substance is removed a little from the flame2 but if the heat be not too high1 it is readily oxidized in the flame1 or near its cone4 ,if the current of air is blown too freely or violently into the flame1 more air is forced there than is sufficient to consume the gases4 ,this superfluous air only acts detrimentally1 by cooling the flame4 ,in general the operation proceeds best when the substance is kept at a dull red heat4 ,the blue cone must be kept free from straggling rays of the yellow or reduction flame4 ,if the analysis be effected on charcoal1 the blast should not be too strong1 as a part of the coal would be converted into carbonic oxide1 which would act antagonistically to the oxidation4 ,the oxidation flame requires a steady current of air1 for the purpose of keeping the blue cone constantly of the same length4 ,for the purpose of acquiring practice1 the following may be done3 ,melt a little molybdenic acid with some borax1 upon a platinum wire1 about the sixteenth of an inch from the point of the blue cone4 ,in the pure oxidation flame1 a clear yellowish glass is formed2 but as soon as the reduction flame reaches it1 or the point of the blue cone touches it1 the color of the bead changes to a brown1 which1 finally1 after a little longer blowing1 becomes quite dark1 and loses its transparency4 ,the cause of this is1 that the molybdenic acid is very easily reduced to a lower degree of oxidation1 or to the oxide of molybdenum4 ,the flame of oxidation will again convert this oxide into the acid1 and this conversion is a good test of the progress of the student in the use of the blowpipe4 ,in cases where we have to separate a more oxidizable substance from a less one1 we use with success the blue cone1 particularly if we wish to determine whether a substance has the quality1 when submitted to heat in the blue cone1 of coloring the external flame4 ,a good reduction flame can be obtained by the use of a small orifice at the point of the blowpipe4 ,in order to produce such a flame1 hold the point of the blowpipe higher above the wick1 while the nozzle must not enter the flame so far as in the production of the oxidation flame4 ,the point of the blowpipe should only touch the flame1 while the current of air blown into it must be stronger than into the oxidation flame4 ,if we project a stream1 in the manner mentioned1 into the flame1 from the smaller side of the wick to the middle1 we shall perceive the flame changed to a long1 narrow1 luminous cone1 a b1 ,fig4 #d1 the end a of which is enveloped by the same dimly visible blueish colored portion of the flame a1 c1 which we perceive in the original flame1 with its point at c4 ,the portion close above the wick1 presenting the dull appearance1 is occasioned by the rising gases which have not supplied to them enough oxygen to consume them entirely4 ,the hydrogen is consumed1 while the carbon is separated in a state of bright ignition1 and forms the internal flame4 ,illustration3 ,fig4 #d ,directly above the wick1 the combustion of the gases is least complete1 and forms there likewise1 as is the case in the free flame1 a dark blue nucleus d4 ,if the oxide of a metal is brought into the luminous portion of the flame produced as above1 so that the flame envelopes the substance perfectly1 the access of air is prevented4 ,the partially consumed gases have now a strong affinity for oxygen1 under the influence of the intense heat of that part of the flame4 ,the substance is thus deprived of a part1 or the whole1 of its oxygen1 and becomes reduced according to the strength of the affinity which the substance itself has for oxygen4 ,if the reduction of a substance is undertaken on platinum1 by fusion with a flux1 and if the oxide is difficult to reduce1 the reduction will be completely effected only in the luminous part of the flame4 ,but if a substance be reduced on charcoal1 the reduction will take place in the blue part of the flame1 as long as the access of air is cut off2 but it is the luminous part of the flame which really possesses the greatest reducing power4 ,the following should be observed in order to procure a good reduction flame3 ,the wick should not be too long1 that it may make a smoke1 nor too short1 otherwise the flame will be too small to produce a heat strong enough for reduction4 ,the wick must be free from all loose threads1 and from charcoal4 ,the blast should be continued for a considerable time without intermission1 otherwise reduction cannot be effected4 ,for the purpose of acquiring practice1 the student may fuse the oxide of manganese with borax1 upon a platinum wire1 in the oxidation flame1 when a violet-red glass will be obtained2 or if too much of the oxide be used1 a glass of a dark color and opaque will be obtained4 ,by submitting this glass to the reduction flame1 it will become colorless in correspondence to the perfection with which the flame is produced4 ,or a piece of tin may be fused upon charcoal1 and kept in that state for a considerable time1 while it presents the appearance of a bright metal on the surface4 ,this will require dexterity in the operator2 for1 if the oxidation flame should chance to touch the bright metal only for a moment1 it is coated with an infusible oxide4 ,,combustion4--,any flame of sufficient size can be used for blowpipe operations4 ,it may be either the flame of a candle of tallow or wax1 or the flame of a lamp4 ,the flame of a wax candle1 or of an oil lamp is most generally used4 ,sometimes a lamp is used filled with a solution of spirits of turpentine in strong alcohol4 ,if a candle is used1 it is well to cut the wick off short1 and to bend the wick a little toward the substance experimented upon4 ,but candles are not the best for blowpipe operations1 as the radiant heat1 reflecting from the substance upon the wax or tallow1 will cause it to melt and run down the side of the candle2 while again1 candles do not give heat enough4 ,the lamp is much the most desirable4 ,the subjoined figure1 from ,berzelius1 is perhaps the best form of lamp4 ,it is made of japanned tin-plate1 about four inches in length1 and has the form and arrangement represented in ,fig4 #e4 ,k is the lamp1 fastened on the stand1 ,s1 by a screw1 ,c1 and is movable upwards or downwards1 as represented in the figure4 ,the posterior end of the lamp may be about one inch square1 and at its anterior end1 ,e1 about three-quarters of an inch square4 ,the under side of this box may be round1 as seen in the figure4 ,the oil is poured into the orifice1 ,a1 which has a cap screwed over it4 ,c' is a wickholder for a flat lamp-wick4 a is a socket containing the wick1 which1 when not in use1 is secured from dirt by the cap4 ,the figures ,b and a' give the forms of the cap and socket4 ,the best combustible for this lamp is the refined rape-seed oil1 or pure sweet oil4 ,when this lamp is in use1 there must be no loose threads1 or no charcoal on the wick1 or these will produce a smoky flame4 ,the wick1 likewise1 should not be pulled up too high1 as the same smoky flame would be produced4 ,illustration3 ,fig4 #e ,,the ,,spirit-,,lamp4--,this is a short1 strong glass lamp1 with a cap1 ,b1 ,fig4 #f1 fitted to it by grinding1 to prevent the evaporation of the alcohol4 ,the neck a contains a tube ,c1 made of silver1 or of tin plate1 and which contains the wick4 ,brass would not answer so well for this tube1 as the spirits would oxidize it1 and thus impart color to the flame4 ,the wickholder must cover the edge of the neck1 but not fit tight within the tube1 otherwise1 by its expansion1 it will break the glass4 ,it is not necessary that alcohol1 very highly rectified1 should be burnt in this lamp1 although if too much diluted with water1 enough heat will not be given out4 ,alcohol of specific gravity #j4hd to #j4hf is the best4 ,illustration3 ,fig4 #f ,this lamp is generally resorted to by blowpipe analysts1 for the purpose of experiments in glass apparatus1 as the oily combustibles will coat the glass with soot4 ,some substances1 when exposed to the dark part of the flame1 become reduced and1 in statu nascendi1 evaporated2 but by passing through the external part of the flame1 they become oxidized again1 and impart a color to the flame4 ,the spirit flame is the most efficient one for the examination of substances the nature of which we wish to ascertain through color imparted to the flame1 as that of the spirit-lamp being colorless1 is1 consequently1 most easily and thoroughly recognized by the slightest tinge imparted to it4 ,it is necessary that in operating with such minute quantities of substances as are used in blowpipe analysis1 that they should have some appropriate support4 ,in order that no false results may ensue1 it is necessary that the supports should be of such a nature that they will not form a chemical combination with the substance while it is exposed to fusion or ignition4 ,appropriate supports for the different blowpipe experiments are charcoal1 platinum instruments1 and glass tubes4 7a47 ,charcoal4--,the value of charcoal as a support may be stated as follows3 #a4 ,the charcoal is infusible1 and being a poor conductor of heat1 a substance can be exposed to a higher degree of heat upon it than upon any other substance4 #b4 ,it is very porous1 and therefore allows easily fusible substances 7such as alkalies and fluxes7 to pass into it1 while other substances less fusible1 such as metals1 to remain unabsorbed4 #c4 ,it has likewise a great reducing power4 ,the best kind of charcoal is that of pinewood1 linden1 willow1 or alderwood1 or any other soft wood4 ,coal from the firwood sparkles too freely1 while that of the hard woods contains too much iron in its ashes4 ,smooth pieces1 free from bark and knots1 should be selected4 ,it should be thoroughly burnt1 and the annual rings or growths should be as close together as possible4 ,if the charcoal is in masses1 it should be sawed into pieces about six inches in length by about two inches broad1 but so that the year-growths run perpendicular to the broadest side1 as the other sides1 by their unequal structure1 burn unevenly4 ,that the substance under examination may not be carried off by the blast1 small conical concavities should be cut in the broad side of the charcoal1 between the year-growths1 with a conical tube of tin plate about two or three inches long1 and one quarter of an inch at one end1 and half an inch at the other4 ,these edges are made sharp with a file4 ,the widest end of this charcoal borer is used for the purpose of making cavities for cupellation4 ,in places where the proper kind of charcoal is difficult to procure1 it is economical to cut common charcoal into pieces about an inch broad1 and the third of an inch thick4 ,in each of these little pieces small cavities should be cut with the small end of the borer4 ,when these pieces of charcoal are required for use1 they must be fastened to a narrow slip of tin plate1 one end of which is bent into the form of a hook1 under which the plate of charcoal is pushed4 ,in general1 we use the charcoal support where we wish to reduce metallic oxides1 to prevent oxidation1 or to test the fusibility of a substance4 ,there is another point to which we would direct the student4 ,those metals which are volatile in the reduction flame1 appear as oxides in the oxidation flame4 ,these oxides make sublimates upon the charcoal close in the vicinity of the substance1 or where it rested1 and by their peculiar color indicate pretty correctly the species of minerals experimented upon4 7b47 ,platinum ,supports4--,the metal platinum is infusible in the blowpipe flame1 and is such a poor conductor of heat that a strip of it may be held close to that portion of it which is red hot without the least inconvenience to the fingers4 ,it is necessary that the student should be cognizant of those substances which would not be appropriate to experiment upon if placed on platinum4 ,metals should not be treated upon platinum apparatus1 nor should the easily reducible oxides1 sulphides1 nor chlorides1 as these substances will combine with the platinum1 and thus render it unfit for further use in analysis4 7c47 ,platinum ,wire4--,as the color of the flame cannot be well discerned when the substance is supported upon charcoal1 in consequence of the latter furnishing false colors1 by its own reflection1 to the substances under examination1 we use platinum wire for that purpose1 when we wish to examine those substances which give indications by the peculiar color which they impart to fluxes4 ,the wire should be about as thick as ,no4 #af or #ah wire1 or about #j4d millimetre1 and cut into pieces about from two and a half to three inches in length4 ,the end of each piece is crooked4 ,in order that these pieces should remain clear of dirt1 and ready for use1 they should be kept in a glass of water4 ,to use them1 we dip the wetted hooked end into the powdered flux 7borax or microcosmic salt7 some of which will adhere1 when we fuse it in the flame of the blowpipe to a bead4 ,this bead hanging in the hook1 must be clear and colorless4 ,should there not adhere a sufficient quantity of the flux in the first trial to form a bead sufficiently large1 the hook must be dipped a second time in the flux and again submitted to the blowpipe flame4 ,to fix the substance to be examined to the bead1 it is necessary1 while the latter is hot1 to dip it in the powdered substance4 ,if the hook is cold1 we moisten the powder a little1 and then dip the hook into it1 and then expose it to the oxidation flame1 by keeping it exposed to a regular blast until the substance and the flux are fused together1 and no further alteration is produced by the flame4 ,the platinum wire can be used except where reduction to the metallic state is required4 ,every reduction and oxidation experiment1 if the results are to be known by the color of the fluxes1 should be effected upon platinum wire4 ,at the termination of the experiment or investigation1 if it be one1 to1 clean the wire1 place it in water1 which will dissolve the bead4 7d47 ,platinum ,foil4--,for the heating or fusing of a substance1 whereby its reduction would be avoided1 we use platinum foil as a support4 ,this foil should be of the thickness of good writing paper1 and from two and a half to three inches long1 by about half an inch broad1 and as even and smooth as possible4 ,if it should become injured by long use1 cut the injured end off1 and if it should prove too short to be held with the fingers1 a pair of forceps may be used to grasp it1 or it may be placed on a piece of charcoal4 7e47 ,platinum ,spoon4--,when we require to fuse substances with the acid sulphate of potash1 or to oxidize them by detonation with nitrate of potash1 whereby we wish to preserve the oxide produced1 we generally use a little spoon of platinum1 about from nine to fifteen millimetres#a in diameter1 and shaped as represented in ,fig4 #g4 ,the handle of this spoon is likewise of platinum1 and should fit into a piece of cork1 or be held with the forceps4 #a ,the ,french millimetre is about the twenty-fifth part of an ,english inch4 ,illustration3 ,fig4 #g4 7f47 ,platinum ,forceps or ,tongs4--,we frequently are necessitated to examine small splinters of metals or minerals directly in the blowpipe flame4 ,these pieces of metallic substances are held with the forceps or tongs represented as in ,fig4 #h1 where ac is formed of steel1 and aa are platinum bars inserted between the steel plates4 ,at bb are knobs which by pressure so separate the platinum bars aa1 that any small substance can be inserted between them4 ,illustration3 ,fig4 #h4 7g47 ,iron ,spoons4--,for a preliminary examination iron spoons are desirable4 ,they may be made of sheet iron1 about one-third of an inch in diameter1 and are very useful in many examinations where the use of platinum would not be desirable4 7h47 ,glass ,tubes4--,for the separation and recognition of volatile substances before the blowpipe flame1 we use glass tubes4 ,these should be about one-eighth of an inch in diameter1 and cut into pieces about five or six inches in length4 ,these tubes should have both ends open4 ,tubes are of great value in the examination of volatile substances which require oxidizing or roasting1 and heating with free access of air4 ,also to ascertain whether a substance under examination will sublimate volatile matter of a certain appearance4 ,such substances are selenium1 sulphur1 arsenic1 antimony1 and tellurium4 ,these substances condense on a cool part of the tube1 and they present characteristic appearances1 or they may be recognized by their peculiar smell4 ,these tubes must be made of the best kind of glass1 white and difficult of fusion1 and entirely free from lead4 ,the substance to be examined must be put in the tube near one end1 and exposed to the flame of the blowpipe4 ,the end containing the substance must be held lower than the other end1 and must be moved a little over the spirit-lamp before a draught of air is produced through the tube4 ,it is a good plan to have a number of these tubes on hand4 ,after having used a tube we cut off that end of it which contained the substance1 with a file1 and clean it from the sublimate1 either by heating it over the spirit-lamp1 or with a piece of paper wound around a wire4 ,it sometimes happens that the substance falls out of the tube before it becomes sufficiently melted to adhere to the glass4 ,to obviate this1 we bend the tube not far from the end1 at an obtuse angle1 and place the substance in the angle1 whereby the tube may be lowered as much as necessary4 ,fig4 #i will give the student a comprehension of the processes described1 and of the manner of bending the tubes4 ,illustration3 ,fig4 #i4 7i47 ,glass ,tubes closed at one ,end4--,if we wish to expose volatile substances to heat1 with the exclusion of air as much as possible1 or to ascertain the contents of water1 or other volatile fluids1 or for the purpose of heating substances which will decrepitate1 we use glass tubes closed at one end4 ,these tubes must be about one-eighth of an inch wide1 and from two to three inches in length4 ,they should be made of white glass1 difficult of fusion1 and free from lead4 ,they should be closed at one end1 as figured in the margin1 ,fig4 #aj4 ,illustration3 ,fig4 #aj4 ,when a substance is to be examined for the purpose of ascertaining whether it contains combustible matter1 as sulphur or arsenic1 and where we wish to avoid oxidation1 we use these tubes without extending the closed end1 in order that there may be as little air admitted as possible1 as is represented in tube ,b4 ,but when a substance to be examined is to be tested for water1 or other incombustible volatile matters1 we employ tubes with little bulbs blown at one end1 such as represented at tube ,a4 ,here there is room for a circulation of air at the bottom of the tube1 by which the volatile matter rises more easily4 ,in some cases1 it is necessary to draw the closed end out to a fine point1 as in the tubes ,c and ,d4 ,either one or the other of these tubes is employed1 depending upon the nature of the substance used4 ,the sublimates condense at the upper part of the tube a1 and can be there examined and recognized4 ,these tubes1 before being used1 must be thoroughly dried and cleaned4 ,in experimenting with them1 they should not be exposed at once to the hottest part of the flame1 but should be submitted to the heat gradually4 ,if the substance is of such a nature that it will sublime at a low heat1 the tube should be held more horizontal1 while a higher heat is attained by bringing the tube to a more vertical position4 ,,various ,,apparatus ,,necessary4 ,edulcorator or ,washing ,bottle4--,take a glass bottle of the capacity of about twelve ounces1 and close the mouth of it very tight with a cork1 through which a short glass tube is fitted airtight4 ,the external end of this tube is drawn out to a point1 with a very fine orifice4 ,the bottle should be filled about half full of water4 ,by blowing air into the bottle through the tube1 and then turning it downwards1 the compressed air will expel a fine stream of water through the fine orifice with considerable force4 ,we use this washing bottle1 ,fig4 #aa1 for the purpose of rinsing the small particles of coal from the reduced metals4 ,illustration3 ,fig4 #aa4 ,agate ,mortar and ,pestle4--,this mortar is used for the purpose of pulverizing hard substances1 and for mixing fluxes4 ,as this mortar will not yield to abrasion1 there is no danger of any foreign matter becoming mixed with the substance pulverized in it4 ,it should be cleaned after use with pumice stone4 ,steel mortars are very useful for the pulverization of hard bodies2 but for all those substances which require great care in their analysis1 and which can be obtained in very minute quantity1 the agate mortar alone should be used4 ,a hammer made of steel is necessary4 ,this should have the edge square4 ,a small anvil1 polished on the surface1 is also required4 ,it is frequently used to test the malleability of metals4 ,a knife1 for the purpose of ascertaining the hardness of minerals4 ,the student should also be provided with several three-edged files1 and likewise with some flat ones4 ,a microscope1 an instrument with two lenses1 or with such a combination of lenses1 that they may be used double or single1 is frequently necessary for the examination of blowpipe experiments1 or the reaction of the fluxes4 ,common lenses1 howsoever cheap they may be1 are certainly not recommended4 ,a microscope with achromatic lenses can now be purchased so cheap that there is no longer any necessity of procuring one with the common lens4 ,besides1 there is no reliability whatever to be placed in the revelations of the common lens2 while on the contrary1 the deceptive appearances which minute objects assume beneath such lenses are more injurious than otherwise4 ,a small cheap set of magnifying glasses are all that is required for the purpose of blowpipe analysis1 ,fig4 #ab4 ,illustration3 ,fig4 #ab4 ,a small magnet should be kept on hand1 for the purpose of testing reduced metals4 ,nippers1 for the purpose of breaking off pieces of minerals for analysis1 without injuring the entire piece1 are indispensable1 ,fig #ac4 ,illustration3 ,fig4 #ac4 ,a pair of scissors is required to trim the wick of the and for the trimming of the edge of platinum foil4 ,a small spatula should be kept for the purpose of mixing substances with fluxes4 ,,the ,,reagents4 ,those substances which possess the property of acting upon other substances1 in such a characteristic manner that they can be recognized1 either by their color1 or by their effervescence1 or by the peculiar precipitation produced1 are termed reagents4 ,the phenomena thus produced is termed reaction4 ,we use those reagents1 or tests1 for the purpose of ascertaining the presence or the absence of certain substances1 through the peculiar phenomena produced when brought in contact with them4 ,the number of reagents employed in blowpipe analysis is not great1 and therefore we shall here give a brief description of their preparation and use4 ,it is indispensably necessary that they should be chemically pure1 as every admixture of a foreign substance would only produce a false result4 ,some of them have a strong affinity for water1 or are deliquescent1 and consequently absorb it greedily from the air4 ,these must be kept in glass bottles1 with glass stoppers1 fitted air-tight by grinding4 ,a4 ,,reagents ,,of ,,general ,,use4 #a4 ,carbonate of ,soda4--7,na,o1 ,,co#b7 ,wash the bicarbonate of soda 7,na,o1 #b;,,co#b7 upon a filter1 with cold water1 until the filtrate ceases to give1 after neutralization with diluted nitric acid 7,,no#e71 a precipitate with nitrate of baryta1 7,ba,o1 ,,no#e71 or nitrate of silver1 7,ag,o1 ,,no#e74 ,that left upon the filter we make red hot in a platinum1 silver1 or porcelain dish4 ,one atom of carbonic acid is expelled1 and the residue is carbonate of soda4 ,a solution of soda must not be changed by the addition of sulphide of ammonium4 ,and when neutralized with hydrochloric acid1 and evaporated to dryness1 and again dissolved in water1 there must be no residue left4 ,carbonate of soda is an excellent agent in reduction1 in consequence of its easy fusibility1 whereby it causes the close contact of the oxides with the charcoal support1 so that the blowpipe flame can reach every part of the substance under examination4 ,for the decomposition and determination of insoluble substances1 particularly the silicates1 carbonate of soda is indispensable4 ,but for the latter purpose1 we use with advantage a mixture of ten parts of soda and thirteen parts of dry carbonate of potash1 which mixture fuses more easily than the carbonate of soda alone4 #b4 ,hydrate of ,baryta 7,ba,o1 ,,ho74--,this salt is used sometimes for the detection of alkalies in silicates4 ,mix one part of the substance with about four parts of the hydrate of baryta1 and expose it to the blowpipe flame4 ,the hydrate of baryta combines with the silicic acid1 and forms the super-basic silicate of baryta1 while the oxides become free4 ,the fused mass must be dissolved in hydrochloric acid1 which converts the oxides into chlorides4 ,evaporate to dryness1 and dissolve the residue in water4 ,the silicic acid remains insoluble4 ,the hydrate of baryta is prepared by mixing six parts of finely powdered heavy-spar 7,ba,o1 ,,so#c7 with one part of charcoal and one and a half parts of wheat flour1 and exposing this mixture in a ,hessian crucible with a cover to a strong and continuous red heat4 ,the cooled chocolate-brown mass must be boiled with twenty parts of water1 and1 while boiling1 there must be added the oxide of copper in sufficient quantity1 or until the liquid will not impart a black color to a solution of acetate of lead 7,pb,o1 ,a74 ,the liquid must be filtered while hot1 and as it cools the hydrate of baryta appears in crystals4 ,these crystals must be washed with a little cold water1 and then heated at a low temperature in a porcelain dish until the crystal water is expelled4 ,the hydrate of baryta melts by a low red heat without losing its water of hydration4 #c4 ,bisulphate of ,potassa 7,,ko1 #b,,so#c74--;,at a red heat the half of the sulphuric acid of this salt becomes free1 and thus separates and expels volatile substances1 by which we can recognize lithium1 boracic acid1 nitric acid1 fluoric acid1 bromine1 iodine1 chlorine2 or it decomposes and reveals some other compounds1 as1 for instance1 the salts of the titanic1 tantalic and tungstic acids4 ,the bisulphate of potash is also used for the purpose of converting a substance into sulphate1 or to free it at once from certain constituents4 ,these sulphates are dissolved in water1 by which we are enabled to effect the separation of its various constituents4 ,,preparation4--,two parts of coarsely powdered sulphate of potash are placed in a porcelain crucible1 and one part of pure sulphuric acid is poured over it4 ,expose this to heat over the spirit-lamp1 until the whole becomes a clear liquid4 ,the cooled mass must be of a pure white color1 and may be got out of the crucible by inverting it4 ,it must be kept in a fine powder4 #d4 ,oxalate of ,potassa 7,,ko1 ,o74--,dissolve bioxalate of potash in water1 and neutralize with carbonate of potash4 ,evaporate the solution at a low heat to dryness1 stirring constantly towards the close of the operation4 ,the dry residue is to be kept in the form of a powder4 ,the oxalate of potash1 at a low red heat1 eliminates a considerable quantity of carbonic oxide1 which1 having a strong affinity for oxygen1 with which it forms carbonic acid1 it is therefore a powerful agent of reduction4 ,it is in many cases preferable to carbonate of soda4 #e4 ,cyanide of ,potassium 7,cy1 ,k74--,in the dry method of analysis1 this salt is one of the most efficient agents for the reduction of metallic oxides4 ,it separates not only the metals from their oxygen compounds1 but likewise from their sulphur compounds1 while it is converted through the action of the oxygen into carbonate of potash1 or1 in the latter case1 combines with the sulphur and forms the sulphureted cyanide of potassium4 ,this separation is facilitated by its easy fusibility4 ,but in many cases it melts too freely1 and therefore it is better to mix it1 for blowpipe analysis1 with an equal quantity of soda4 ,this mixture has great powers of reduction1 and it is easily absorbed by the charcoal1 while the globules of reduced metal are visible in the greatest purity4 ,,preparation4--,deprive the ferrocyanide of potassium 7#b,k,cy ,fe,cy7 of its water by heating it over the spirit-lamp in a porcelain dish4 ,mix eight parts of this anhydrous salt with three parts of dry carbonate of potash1 and fuse the mixture by a low red heat in a ,hessian1 or still better1 in an iron crucible with a cover1 until the mass flows quiet and clear1 and a sample taken up with an iron spatula appears perfectly white4 ,pour the clear mass out into a china or porcelain dish or an iron plate1 but with caution that the fine iron particles which have settled to the bottom1 do not mix with it4 ,the white fused mass must be powdered1 and kept from the air4 ,the cyanide of potassium thus prepared1 contains some of the cyanate of potassa1 but the admixture does not deteriorate it for blowpipe use4 ,it must be perfectly white1 free from iron1 charcoal1 and sulphide of potassium4 ,the solution of it in water must give a white precipitate with a solution of lead1 and when neutralized with hydrochloric acid1 and evaporated to dryness1 it must not give an insoluble residue by dissolving it again in water4 #f4 ,nitrate of ,potassa1 ,saltpetre 7,,ko1 ,,no#e74--,saturate boiling water with commercial saltpetre1 filter while hot in a beaker glass1 which is to be placed in cold water1 and stir while the solution is cooling4 ,the greater part of the saltpetre will crystallize in very fine crystals4 ,place these crystals upon a filter1 and wash them with a little cold water1 until a solution of nitrate of silver ceases to exhibit any reaction upon the filtrate4 ,these crystals must be dried and powdered4 ,saltpetre1 when heated with substances easy of oxidation1 yields its oxygen quite readily1 and is1 therefore1 a powerful means of oxidation4 ,in blowpipe analysis1 we use it particularly to convert sulphides 7as those of arsenic1 antimony1 c47 into oxides and acids4 ,we furthermore use saltpetre for the purpose of producing a complete oxidation of small quantities of metallic oxides1 which oxidize with difficulty in the oxidation flame1 so that the color of the bead1 in its highest state of oxidation1 shall be visible1 as for instance1 manganese dissolved in the microcosmic salt4 #g4 ,biborate of soda1 borax--7,na,o #b;,,bo#c74--;,commercial borax is seldom pure enough for a reagent4 ,a solution of borax must not give a precipitate with carbonate of potassa2 or1 after the addition of dilute nitric acid1 it must remain clear upon the addition of nitrate of silver1 or nitrate of baryta4 ,or a small piece of the dry salt1 fused upon a platinum wire1 must give a clear and uncolored glass1 as well in the oxidation flame as in the reduction flame4 ,if these tests indicate a foreign admixture1 the borax must be purified by re-crystallization4 ,these crystals are washed upon a filter1 dried1 and heated1 to expel the crystal water1 or until the mass ceases to swell up1 and it is reduced to powder4 ,boracic acid is incombustible1 and has a strong affinity for oxides when fused with them2 therefore1 it not only directly combines with oxides1 but it expels1 by fusion1 all other volatile acids from their salts4 ,furthermore1 boracic acid promotes the oxidation of metals and sulphur1 and induces haloid compounds1 in the oxidation flame1 to combine with the rising oxides4 ,borates thus made1 melt generally by themselves2 but admixed with borate of soda1 they fuse much more readily1 give a clear bead4 ,borax acts either as a flux1 or through the formation of double salts4 ,in borax1 we have the action of free boracic acid1 as well as borate of soda1 and for that reason it is an excellent reagent for blowpipe analysis4 ,all experiments in which borax is employed should be effected upon platinum wire4 ,the hook of the wire should be heated red hot1 and then dipped into the powdered borax4 ,this should be exposed to the oxidation flame1 when it will be fused to a bead1 which adheres to the hook4 ,this should be then dipped into the powdered substance1 which will adhere to it if it is hot2 but if the bead is cool1 it must be previously moistened4 ,expose this bead to the oxidation flame until it ceases to change1 then allow it to cool1 when it should be exposed to the reduction flame4 ,look for the following in the oxidation flame3 7#a47 ,whether the heated substance is fused to a clear bead or not1 and whether the bead remains transparent after cooling4 ,the beads of some substances1 for instance those of the alkaline earths1 are clear while hot2 but upon cooling1 are milk-white and enamelled4 ,some substances give a clear bead when heated and when cold1 but appear enamelled when heated intermittingly or with a flame which changes often from oxidation to reduction1 or with an unsteady flame produced by too strong a blast4 ,the reason is an incomplete fusion1 while from the basic borate compound a part of the base is separated4 ,as the boracic acid is capable of dissolving more in the heat1 a bead will be clear while hot1 enamelled when cold1 as a part in the latter instance will become separated4 7#b47 ,whether the substance dissolves easily or not1 and whether it intumesces from arising gases4 7#c47 ,whether the bead1 when exposed to the oxidation flame1 exhibits any color1 and whether the color remains after the bead shall have cooled1 or whether the color fades4 7#d47 ,whether the bead exhibits any other reaction in the reduction flame4 ,the bead should not be overcharged with the substance under examination1 or it will become colored so deeply as not to present any transparency1 or the color light enough to discern its hue4 #h4 ,microcosmic ,salt--,phosphate of ,soda and ,ammonia--7,na,o1 ,,nh#d,o ,,po#e74--;,dissolve six parts of phosphate of soda 7#b,na,o1 ,,ho1 ,,po#e71 and one part of pure chloride of ,ammonium 7,,nh#d;,cl471 in two parts of boiling water1 and allow it to cool4 ,the greatest part of the formed double salt crystallizes1 while the mother-liquid contains chloride of sodium1 and some of the double salt4 ,the crystals must be dissolved in as little boiling water as possible1 and re-crystallized4 ,these crystals must be dried and powdered4 ,when this double salt is heated1 the water and the ammonia escape1 while the incombustible residue has a composition similar to borax1 viz41 a free acid and an easily fusible salt4 ,the effect of it is1 therefore1 similar to the borax4 ,the free phosphoric acid expels1 likewise1 most other acids from their combinations1 and combines with metallic oxides4 ,for supports1 the platinum wire may be used1 but the hook must be smaller than when borax is used1 or the bead will not adhere4 ,as for all the other experiments with this salt1 the microscosmic salt is used the same as borax4 #i4 ,nitrate of ,cobalt4--7,co,o1 ,,no#e74--,this salt can be prepared by dissolving pure oxide of cobalt in diluted nitric acid1 and evaporating to dryness with a low heat4 ,the dry residue should be dissolved in ten parts of water1 and filtered4 ,the filtrate is now ready for use1 and should be kept in a bottle with a glass stopper4 ,if the pure oxide of cobalt cannot be procured1 then it may be prepared by mixing two parts of finely powdered glance of cobalt with four parts of saltpetre1 and one part of dry carbonate of potassa with one part of water free from carbonate of soda4 ,this mixture should be added in successive portions into a red-hot ,hessian crucible1 and the heat continued until the mass is fused1 or at least greatly diminished in volume4 ,the cooled mass must be triturated with hot water1 and then heated with hydrochloric acid until it is dissolved and forms a dark green solution1 which generally presents a gelatinous appearance1 occasioned by separated silica4 ,the solution is to be evaporated to dryness1 the dry residue moistened with hydrochloric acid1 boiled with water1 filtered and neutralized while hot with carbonate of ammonia1 until it ceases to give an acid reaction with test-paper4 ,this must now be filtered again1 and carbonate of potassa added to the filtrate as long as a precipitate is produced4 ,this precipitate is brought upon a filter and washed thoroughly1 and then dissolved in diluted nitric acid4 ,this is evaporated to dryness1 and one part of it is dissolved in ten parts of water for use4 ,the oxide of cobalt combines1 with strong heat in the oxidation flame1 with various earths and infusible metallic oxides1 and thus produces peculiarly colored compounds1 and is therefore used for their detection2 7alumina1 magnesia1 oxide of zinc1 oxide of tin1 etc47 ,some of the powdered substance is heated upon charcoal in the flame of oxidation1 and moistened with a drop of the solution of the nitrate of cobalt1 when the oxidation flame is thrown upon it4 ,alumina gives a pure blue color1 the oxide of zinc a bright green1 magnesia a light red1 and the oxide of tin a bluish-green color2 but the latter is only distinctly visible after cooling4 ,the dropping bottle1 is the most useful apparatus for the purpose of getting small quantities of fluid4 ,it is composed of a glass tube1 drawn out to a point1 with a small orifice4 ,this tube passes through the cork of the bottle4 ,by pressing in the cork into the neck of the bottle1 the air within will be compressed1 and the liquid will rise in the tube4 ,if now we draw the cork out1 with the tube filled with the fluid1 and pressing the finger upon the upper orifice1 the fluid can be forced out in the smallest quantity1 even to a fraction of a drop4 #aj4 ,tin4--,this metal is used in the form of foil1 cut into strips about half an inch wide4 ,tin is very susceptible of oxidation1 and therefore deprives oxidized substances of their oxygen very quickly1 when heated in contact with them4 ,it is employed in blowpipe analysis1 for the purpose of producing in glass beads a lower degree of oxidation1 particularly if the substance under examination contains only a small portion of such oxide4 ,these oxides give a characteristic color to the bead1 and thus are detected4 ,the bead is heated upon charcoal in the reduction flame1 with a small portion of the tin1 whereby some of the tin is melted and mixes with the bead4 ,the bead should be reduced quickly in the reduction flame1 for by continuing the blast too great a while1 the oxide of tin separates the other oxides in the reduced or metallic state1 while we only require that they shall only be converted into a sub-oxide1 in order that its peculiar color may be recognized in the bead4 ,the addition of too much tin causes the bead to present an unclean appearance1 and prevents the required reaction4 #aa4 ,silica 7,si,o#c74--,this acid does not even expel carbonic acid in the wet way1 but in a glowing heat it expels the strongest volatile acids4 ,in blowpipe analysis1 we use it fused with carbonate of soda to a bead1 as a test for sulphuric acid1 and in some cases for phosphoric acid4 ,also with carbonate of soda and borax1 for the purpose of separating tin from copper4 ,finely powdered quartz will answer these purposes4 ,if it cannot be procured1 take well washed white sand and mix it with two parts of carbonate of soda and two parts of carbonate of potassa4 ,melt the materials together1 pound up the cooled mass1 dissolve in hot water1 filter1 add to the filtrate hydrochloric acid1 and evaporate to dryness4 ,moisten the dry residue with hydrochloric acid1 and boil in water4 ,the silica remains insoluble4 ,it should be washed well1 dried1 and heated1 and then reduced to powder4 #ab4 ,,test-,,papers4--7a47 ,blue1 ,litmus ,paper4--,dissolve one part of litmus in six or eight parts of water1 and filter4 ,divide the filtrate into two parts4 ,in one of the parts neutralize the free alkali by stirring it with a glass rod dipped in diluted sulphuric acid1 until the fluid appears slightly red4 ,then mix the two parts together1 and draw slips of unsized paper1 free from alkali1 such as fine filtering paper4 ,hang these strips on a line to dry1 in the shade and free from floating dust4 ,if the litmus solution is too light1 it will not give sufficient characteristic indications1 and if too dark it is not sensitive enough4 ,the blue color of the paper should be changed to red1 when brought in contact with a solution containing the minutest trace of free acid2 but it should be recollected that the neutral salts of the heavy metals produce the same change4 7b47 ,red ,litmus ,paper4--,the preparation of the red litmus paper is similar to the above1 the acid being added until a red color is obtained4 ,reddened litmus paper is a very sensitive reagent for free alkalies1 the carbonates of the alkalies1 alkaline earths1 sulphides of the alkalies and of the alkaline earths1 and alkaline salts with weak acids1 such as boracic acid4 ,these substances restore the original blue color of the litmus4 7c47 ,logwood ,paper4--,take bruised logwood1 boil it in water1 filter1 and proceed as above4 ,logwood paper is a very delicate test for free alkalies1 which impart a violet tint to it4 ,it is sometimes used to detect hydrofluoric acid1 which changes its color to yellow4 ,all the test-papers are to be cut into narrow strips1 and preserved in closely stopped vials4 ,the especial employment of the test-papers we shall allude to in another place4 ,b4 ,,especial ,,reagents4 #ac4 ,fused ,boracic ,acid 7,,bo#c74--,the commercial article is sufficiently pure for blowpipe analysis4 ,it is employed in some cases to detect phosphoric acid1 and also minute traces of copper in lead compounds4 #ad4 ,fluorspar 7,ca,fl#b74--,this substance should be pounded fine and strongly heated4 ,fluorspar is often mixed with boracic acid1 which renders it unfit for analytical purposes4 ,such an admixture can be detected if it be mixed with bisulphate of potassa1 and exposed upon platinum wire to the interior or blue flame4 ,it is soon fused1 the boracic acid is reduced and evaporated1 and by passing through the external flame it is reoxidized1 and colors the flame green4 ,we use fluorspar mixed with bisulphate of potassa as a test for lithia and boracic acid in complicated compounds4 #ae4 ,oxalate of ,nickel 7,ni,o1 ,o74--,it is prepared by dissolving the pure oxide of nickel in diluted hydrochloric acid4 ,evaporate to dryness1 dissolve in water1 and precipitate with oxalate of ammonia4 ,the precipitate must be washed with caution upon a filter1 and then dried4 ,it is employed in blowpipe analysis to detect salts of potassa in the presence of sodium and lithium4 #af4 ,oxide of ,copper 7,cu,o74--,pure metallic copper is dissolved in nitric acid4 ,the solution is evaporated in a porcelain dish to dryness1 and gradually heated over a spirit-lamp1 until the blue color of the salt has disappeared and the mass presents a uniform black color4 ,the oxide of copper so prepared must be powdered1 and preserved in a vial4 ,it serves to detect1 in complicated compounds1 minute traces of chlorine4 #ag4 ,antimoniate of ,potassa 7,,ko1 ,sb,o#f74--,mix four parts of the bruised metal of antimony1 with nine parts of saltpetre4 ,throw this mixture1 in small portions1 into a red-hot ,hessian crucible1 and keep it at a glowing heat for awhile after all the mixture is added4 ,boil the cooled mass with water1 and dry the residue4 ,take two parts of this1 and mix it with one part of dry carbonate of potassa1 and expose this to a red heat for about half an hour4 ,then wash the mass in cold water1 and boil the residue in water2 filter1 evaporate the filtrate to dryness1 and then1 with a strong heat1 render it free of water4 ,powder it while it is warm1 and preserve it in closed vials4 ,it is used for the detection of small quantities of charcoal in compound substances1 as it shares its oxygen with the carbonaceous matter1 the antimony becomes separated1 and carbonate of potassa is produced1 which restores red litmus paper to blue1 and effervesces with acids4 #ah4 ,silver ,foil4--,a small piece of silver foil is used for the purpose of detecting sulphur and the sulphides of the metals1 which impart a dark stain to it4 ,if no silver foil is at hand1 strips of filtering paper1 impregnated with acetate of lead1 will answer in many cases4 #ai4 ,nitroprusside of ,sodium 7,fe#b;,cy#e1 ,,no#e1 #b,na74--,this is a very delicate test for sulphur1 and was discovered by ,dr4 ,playfair4 ,this test has lately been examined with considerable ability by ,prof4 ,j4,w4 ,bailey1 of ,west ,point4 ,if any sulphate or sulphide is heated by the blowpipe upon charcoal with the carbonate of soda1 and the fused mass is placed on a watch-glass1 with a little water1 and a small piece of the nitroprusside of sodium is added1 there will be produced a splendid purple color4 ,this color1 or reaction1 will be produced from any substance containing sulphur1 such as the parings of the nails1 hair1 albumen1 etc4 ,in regard to these latter substances1 the carbonate of soda should be mixed with a little starch1 which will prevent the loss of any of the sulphur by oxidation4 ,coil a piece of hair around a platinum wire1 moisten it1 and dip it into a mixture of carbonate of soda1 to which a little starch has been added1 and then heat it with the blowpipe1 when the fused mass will give with the nitroprusside of sodium the characteristic purple reaction1 indicative of the presence of sulphur4 ,with the proper delicacy of manipulation1 a piece of hair1 half an inch in length1 will give distinct indications of sulphur4 ,preparation4--,the nitroprussides of sodium and potassium 7for either salt will give the above reactions71 are prepared as follows3 ,one atom 7#dbb grains7 of pulverized ferrocyanide of potassium is mixed with five atoms of commercial nitric acid1 diluted with an equal quantity of water4 ,one-fifth of this quantity 7one atom7 of the acid is sufficient to transfer the ferrocyanide into nitroprusside2 but the use of a larger quantity is found to give the best results4 ,the acid is poured all at once upon the ferrocyanide1 the cold produced by the mixing being sufficient to moderate the action4 ,the mixture first assumes a milky appearance1 but after a little while1 the salt dissolves1 forming a coffee-colored solution1 and gases are disengaged in abundance4 ,when the salt is completely dissolved1 the solution is found to contain ferrocyanide 7red prussiate7 of potassium1 mixed with nitroprusside and nitrate of the same base4 ,it is then immediately decanted into a large flask1 and heated over the water-bath4 ,it continues to evolve gas1 and after awhile1 no longer yields a dark blue precipitate with ferrous salts1 but a dark green or slate-colored precipitate4 ,it is then removed from the fire1 and left to crystallize1 whereupon it yields a large quantity of crystals of nitre1 and more or less oxamide4 ,the strongly-colored mother liquid is then neutralized with carbonate of potash or soda1 according to the salt to be prepared1 and the solution is boiled1 whereupon it generally deposits a green or brown precipitate1 which must be separated by filtration4 ,the liquid then contains nothing but nitroprusside and nitrate of potash or soda4 ,the nitrates being the least soluble1 are first crystallized1 and the remaining liquid1 on farther evaporation1 yields crystals of the nitroprusside4 ,the sodium salt crystallizes most easily4--7,,playfair47 ,as some substances1 particularly in complicated compounds1 are not detected with sufficient nicety in the dry way of analysis1 it will often be necessary to resort to the wet way4 ,it is therefore necessary to have prepared the reagents required for such testing1 as every person1 before he can become an expert blowpipe analyst1 must be acquainted with the characteristic tests as applied in the wet way4 99 99 99 99 99 ,part ,,ii4 ,,initiatory ,,analysis4 ,qualitative analysis refers to those examinations which relate simply to the presence or the absence of certain substances1 irrespective of their quantities4 ,but before we take cognizance of special examinations1 it would facilitate the progress of the student to pass through a course of ,initiatory ,exercises4 ,these at once lead into the special analysis of all those substances susceptible of examination by the blowpipe4 ,the ,initiatory ,analysis is best studied by adopting the following arrangement3 #a4 ,,examinations ,,with ,,the ,,glass ,,bulb4 ,the glass of which the bulb is made should be entirely free from lead1 otherwise fictitious results will ensue4 ,if the bulb be of flint glass1 then by heating it1 there is a slightly iridescent film caused upon the surface of the glass1 which may easily be mistaken for arsenic4 ,besides1 this kind of glass is easily fusible in the oxidating flame of the blowpipe1 while1 in the reducing flame1 its ready decomposition would preclude its use entirely4 ,the tube should be composed of the potash or hard ,bohemian glass1 should be perfectly white1 and very thin1 or the heat will crack it4 ,the tube should be perfectly clean1 which can be easily attained by wrapping a clean cotton rag around a small stick1 and inserting it in the tube4 ,before using the tube1 see also that it is perfectly dry4 ,the quantity of the substance put into the tube for examination should be small4 ,from one to three grains is quite sufficient1 as a general rule1 but circumstances vary the quantity4 ,the sides of the tube should not catch any of the substance as it is being placed at the bottom of the tube1 or into the bulb4 ,if any of the powder1 however1 should adhere1 it should be pushed down with a roll of clean paper1 or the clean cotton rag referred to above4 ,in submitting the tube to the flame1 it should be heated at first very gently1 the heat being increased until the glass begins to soften1 when the observations of what is ensuing within it may be made4 ,if the substance be of an organic nature1 a peculiar empyreumatic odor will be given off4 ,if the substance chars1 then it may be inferred that it is of an organic nature4 ,the matters which are given off and cause the empyreumatic odor1 are a peculiar oil1 ammonia1 carbonic acid1 acetic acid1 water1 cyanogen1 and frequently other compounds4 ,if a piece of paper is heated in the bulb1 a dark colored oil condenses upon the sides of the tube1 which has a strong empyreumatic odor4 ,a piece of litmus paper indicates that this oil is acid1 as it is quickly changed to red by contact with it4 ,a black residue is now left in the tube1 and upon examination we will find that it is charcoal4 ,if1 instead of the paper1 a piece of animal substance is placed in the bulb1 the reddened litmus paper will be converted into its original blue color1 while charcoal will be left at the bottom of the tube4 ,a changing of the substance1 however1 to a dark color1 should not be accepted as an invariable indication of charcoal1 as some inorganic bodies thus change color1 but the dark substance will not be likely to be mistaken for charcoal4 ,by igniting the suspected substance with nitrate of potassa1 it can quickly be ascertained whether it is organic or not1 for if the latter1 the vivid deflagration will indicate it4 ,if the substance contains water1 it will condense upon the cold portion of the tube1 and may be there examined as to whether it is acid or alkaline4 ,if the former1 the matter under examination is1 perhaps1 vegetable2 if the latter1 it is of an animal nature4 ,the water may be that fluid absorbed1 or it may form a portion of its constitution1 ,if the substance contain sulphur1 the sublimate upon the cold part of the tube may be recognized by its characteristic appearance1 especially if the substance should be a sulphide of tin1 copper1 antimony1 or iron4 ,the hyposulphites1 and several other sulphides1 also give off sulphur when heated4 ,the volatile metals1 mercury and arsenic1 will1 however1 sublime without undergoing decomposition4 ,as the sulphide of arsenic may be mistaken1 from its color and appearance1 for sulphur1 it must be examined especially for the purpose of determining that point4 ,selenium will likewise sublime by heat as does sulphur4 ,this is the case if selenides are present4 ,selenium gives off the smell of decayed horse-radish4 ,when the persalts are heated they are reduced to protosalts1 with the elimination of a part of their acid4 ,this will be indicated by the blue litmus paper4 ,if some of the neutral salts containing a volatile acid be present1 they will become decomposed4 ,for instance1 the red nitrous acid water of the nitrates will indicate the decomposition of the salt1 especially if it be the nitrate of a metallic oxide4 ,if there is an odor of sulphur1 then it is quite probable1 if no free sulphur be present1 that a hyposulphite is decomposed4 ,if an oxalate be present1 it is decomposed with the evolution of carbonic oxide1 which may be inflamed at the mouth of the tube2 but there are oxalates that give off carbonic acid gas1 which1 of course1 will not burn4 ,a cyanide will become decomposed and eliminate nitrogen gas1 while the residue is charred4 ,some cyanides are1 however1 not thus decomposed1 as the dry cyanides of the earths and alkalies4 ,there are several oxides of metals which will sublime1 and may be thus examined in the tube4 ,arsenious acid sublimes with great ease in minute octohedral crystals4 ,the oxides of tellurium and antimony will sublime1 the latter in minute glittering needles4 ,there are several metals which will sublime1 and may be examined in the cold portion of the tube4 ,mercury condenses upon the tube in minute globules4 ,these often do not present the metallic appearance until they are disturbed with a glass rod1 when they attract each other1 and adhere as small globules4 ,place in the tube about a grain of red precipitate of the drug stores and apply heat1 when the oxide will become decomposed1 its oxygen will escape while the vaporized mercury will condense upon the cold portion of the tube1 and may there be examined with a magnifying glass4 ,arsenic1 when vaporized1 may be known by its peculiar alliaceous odor4 ,arsenic is vaporized from its metallic state1 and likewise from its alloys4 ,several compounds which contain arsenic will also sublime1 such as the arsenical cobalt4 ,place in the bulb a small piece of arsenical cobalt or fly-stone1 and apply heat4 ,the sulphide of arsenic will first rise1 but soon the arsenic will adhere to the sides of the tube4 ,the metals tellurium and cadmium are susceptible of solution1 but the heat required is a high one4 ,this is best done upon charcoal4 ,the perchloride of mercury sublimes undecomposed in the bulb1 previously undergoing fusion4 ,the protochloride of mercury likewise sublimes1 but it does not undergo fusion first1 as is the case with the corrosive sublimate4 ,the ammoniacal salts all are susceptible of sublimation1 which they do without leaving a residue4 ,there are1 however1 several which contain fixed acids1 which latter are left in the bulb4 ,this is particularly the case with the phosphates and borates4 ,a piece of red litmus paper will readily detect the escaping ammonia1 while its odor will indicate its presence with great certainty4 ,the halogen compounds of mercury1 we should have mentioned1 also sublime1 the red iodide giving a yellow sublimate4 ,the bulb is also a convenient little instrument for the purpose of heating those substances which phosphoresce1 and likewise those salts that decrepitate4 ,should the above reactions not be readily discerned1 it should not be considered as an indication that the substances are not present1 for they are frequently expelled in such combinations that the above reactions will not take place4 ,this is often the case with sulphur1 selenium1 arsenic1 and tellurium4 ,it frequently happens1 likewise1 that these substances are in such combinations that heat alone will not sublime them2 or else two or more of them may arise together1 and thus complicate the sublimate1 so that the eye cannot readily detect either substance4 ,sometimes sulphur and arsenic will coat the tube with a metal-like appearance1 which is deceptive4 ,this coating presents a metallic lustre at its lower portion1 but changing1 as it progresses upward1 to a dark brown1 light brown1 orange or yellow2 this sublimate being due to combinations of arsenic and sulphur1 which compounds are volatilized at a lower temperature than metallic arsenic4 ,if certain reagents are mixed with many substances1 changes are effected which would not ensue with heat alone4 ,formiate of soda possesses the property of readily reducing metallic oxides4 ,when this salt is heated1 it gives off a quantity of carbonic oxide gas4 ,this gas1 when in the presence of a metallic oxide1 easily reduces the metal1 by withdrawing its oxygen from it1 and being changed into carbonic oxide4 ,if a little fly-stone is mixed with some formiate of soda1 and heated in the bulb1 the arsenic is reduced1 volatilized1 and condenses in the cool portion of the tube4 ,by this method1 the smallest portion of a grain of the arsenical compound may be thus examined with the greatest readiness4 ,if the residue is now washed1 by which the soda is got rid of1 the metallic arsenic may be obtained in small spangles4 ,if the compound examined be the sulphide of antimony1 the one-thousandth part can be readily detected1 and hence this method is admirably adapted to the examination of medicinal antimonial compounds4 ,the arsenites of silver and copper are reduced by the formiate of soda to their metals1 mixed with metallic arsenic4 ,the mercurial salts are all reduced with the metal plainly visible as a bright silvery ring on the cool portion of the tube4 ,the chloride and nitrate of silver are completely reduced1 and may be obtained after working out the soda1 as bright metallic spangles4 ,the salts of antimony and zinc are thus reduced2 also the sulphate of cadmium4 ,the sublimate of the latter1 although in appearance not unlike that of arsenic1 can easily be distinguished by its brighter color4 ,it is1 in fact1 the rich yellow of this sublimate which has led artists to adopt it as one of their most valued pigments4 #b4 ,,examinations ,,in ,,the ,,open ,,tube4 ,the substance to be operated upon should be placed in the tube1 about half an inch from the end1 and the flame applied at first very cautiously1 increasing gradually to the required temperature4 ,the tube1 in all these roasting operations1 as they are termed1 should be held in an inclined position4 ,the nearer perpendicular the tube is held1 the stronger is the draught of air that passes through it4 ,if but little heat is required in the open tube operation1 the spirit-lamp is the best method of applying the heat4 ,but if a greater temperature is required1 then recourse must be had to the blowpipe4 ,upon the angle of inclination of the tube depends the amount of air that passes through it1 and therefore1 the rapidity of the draught may be easily regulated at the will of the operator4 ,the inclination of the tube may1 as a general rule1 be about the angle represented in ,fig4 #ad4 ,illustration ,fig4 #ad4 ,the length of the tube must be about six inches1 so that the portion upon which the substance rested in a previous examination may be cut off4 ,the portion of the tube left will answer for several similar operations4 ,when the substance is under examination1 we should devote our attention to the nature of the sublimates1 and to that of the odors of the gases4 ,if sulphur be in the substance experimented upon1 the characteristic odor of sulphurous acid gas will readily indicate the sulphur4 ,if metallic sulphides1 for instance1 are experimented upon1 the sulphurous acid gas eliminated will readily reveal their presence4 ,as it is a property of this gas to bleach1 a piece of ,brazil-wood test paper should be held in the mouth of the tube1 when its loss of color will indicate the presence of the sulphurous acid4 ,it often happens1 too1 that a slight deposition of sulphur will be observed upon the cool portion of the tube4 ,this is particularly the case with those sulphides1 which yield sublimates of sulphur when heated in the bulb4 ,selenium undergoes but slight oxidation1 but it becomes readily volatilized1 and may be observed on the cool portion of the tube4 ,at the same time the nose1 if applied close to the end of the tube1 will detect the characteristic odor of rotten horse-radish4 ,arsenic also gives its peculiar alliaceous odor1 which is so characteristic that it can be easily detected4 ,a few of the arsenides produce this odor4 ,the sublimates should be carefully observed1 as they indicate often with great certainty the presence of certain substances2 for instance1 that of arsenic4 ,the sublimate1 in this case1 presents itself as the arsenious acid1 or the metallic arsenic itself4 ,if it be the former1 it may be discerned by aid of the magnifying glass as beautiful glittering octohedral crystals4 ,if the latter1 the metallic lustre will reveal it4 ,but it will be observed that while some of the arsenides are sublimed at a comparatively low temperature1 others require a very high one4 ,antimony gives a white sublimate when its salts are roasted1 as the sulphide1 or the antimonides themselves1 or the oxide of this metal4 ,this white sublimate is not antimonious acid1 but there is mixed with it the oxide of antimony with which the acid is sublimed4 ,as is the case with arsenious acid1 the antimonious acid may1 by dexterous heating1 be driven from one portion of the tube to another4 ,tellurium1 or its acid and oxide1 may be got as a sublimate in the tube4 ,the tellurious acid1 unlike the arsenious and antimonious acids1 cannot be driven from one portion of the tube to another1 but1 on the contrary1 it fuses into small clear globules1 visible to the naked eye sometimes1 but quite so with the aid of the magnifying glass4 ,lead1 or its chloride1 sublimes like tellurium1 and1 like that substance1 fuses into globules or drops4 ,bismuth1 or its sulphide1 sublimes into an orange or brownish globules1 when it is melted1 as directed above1 for tellurium4 ,the color of the bismuth and lead oxides are somewhat similar1 although that of the latter is paler4 ,if any mineral containing fluorine1 is fused1 first with the microcosmic salt bead1 then put into the tube1 and the flame of the blowpipe be directed into the tube upon the bead1 hydrofluoric acid is disengaged and attacks the inside of the tube4 ,the fluoride of calcium1 or fluorspar1 may be used for this experiment4 ,during the roasting1 a brisk current of air should be allowed to pass through the tube1 whereby unoxidized matter may be prevented from volatilization1 and the clogging up of the substance under examination be prevented4 #c4 ,,examinations ,,upon ,,charcoal4 ,in making examinations upon charcoal1 it is quite necessary that the student should make himself familiar with the different and characteristic appearances of the deposits upon the charcoal4 ,in this case ,i have found the advice given by ,dr4 ,sherer to be the best2 that is1 to begin with the examination of the pure materials first1 until the eye becomes familiarized with the appearances of their incrustations upon charcoal4 ,the greater part of the metals fuse when submitted to the heat of the blowpipe1 and if exposed to the outer flame1 they oxidize4 ,these metals1 termed the noble metals1 do not oxidize1 but they fuse4 ,the metals platinum1 iridium1 rhodium1 osmium and palladium do not fuse4 ,the metal osmium1 if exposed to the flame of oxidation1 fuses and is finally dissipated as osmic acid4 ,in the latter flame1 the salts of the noble metals are reduced to the metallic state1 and the charcoal is covered with the bright metal4 ,we shall give a brief description of the appearance of the principal elementary bodies upon being fused with charcoal4 ,this plan is that deemed the most conducive to the progress of the student1 by ,berzelius1 ,plattner1 and ,sherer4 ,experience has taught us that this method is the most efficient that could have been devised as an initiatory exercise for the student1 ere he commences a more concise and methodical method of analysis4 ,in these reactions upon charcoal1 we shall follow nearly the language of ,plattner and ,sherer4 ,,selenium is not difficult of fusion1 and gives off brown fumes in either the oxidation or reduction flame4 ,the deposit upon the charcoal is of a steel-grey color1 with a slightly metallic lustre4 ,the deposit however that fuses outside of this steel-grey one is of a dull violet color1 shading off to a light brown4 ,under the flame of oxidation this deposit is easily driven from one portion of the charcoal to another1 while the application of the reducing flame volatilizes it with the evolution of a beautiful blue light4 ,the characteristic odor of decayed horse-radish distinguishes the volatilization of this metal4 ,,tellurium4--,this metal fuses with the greatest readiness1 and is reduced to vapor under both flames with fumes1 and coats the charcoal with a deposit of tellurous acid4 ,this deposit is white near the centre1 and is of a dark yellow near the edges4 ,it may be driven from place to place by the flame of oxidation1 while that of reduction volatilizes it with a green flame4 ,if there be a mixture of selenium present1 then the color of the flame is bluish-green4 ,,arsenic4--,this metal is volatilized without fusing1 and covers the charcoal both in the oxidizing and reducing flames with a deposit of arsenious acid4 ,this coating is white in the centre1 and grey towards the edges1 and is found some distance from the assay4 ,by the most gentle application of the flame1 it is immediately volatilized1 and if touched for a moment with the reducing flame1 it disappears1 tinging the flame pale blue4 ,during volatilization a strong garlic odor is distinctly perceptible1 very characteristic of arsenic1 and by which its presence in any compound may be immediately recognized4 ,,antimony4--,this metal fuses readily1 and coats the charcoal under both flames with antimonious acid4 ,this incrustation is of a white color where thick1 but of a bluish tint where it is thin1 and is found nearer to the assay than that of arsenic4 ,when greatly heated by the flame of oxidation1 it is driven from place to place without coloring the flame1 but when volatilized by the flame of reduction1 it tinges the flame blue4 ,as antimonious acid is not so volatile as arsenious acid1 they may thus be easily distinguished from one another4 ,when metallic antimony is fused upon charcoal1 and the metallic bead raised to a red heat1 if the blast be suspended1 the fluid bead remains for some time at this temperature1 giving off opaque white fumes1 which are at first deposited on the surrounding charcoal1 and then upon the bead itself1 covering it with white1 pearly crystals4 ,the phenomenon is dependent upon the fact1 that the heated button of antimony1 in absorbing oxygen from the air1 developes sufficient heat to maintain the metal in a fluid state1 until it becomes entirely covered with crystals of antimonious acid so formed4 ,,bismuth4--,this metal fuses with ease1 and under both flames covers the charcoal with a coating of oxide1 which1 while hot1 is of an orange-yellow color1 and after cooling1 of a lemon-yellow color1 passing1 at the edges1 into a bluish white4 ,this white coating consists of the carbonate of bismuth4 ,the sublimate from bismuth is formed at a less distance from the assay than is the case with antimony4 ,it may be driven from place to place by the application of either flame2 but in so doing1 the oxide is first reduced by the heated charcoal1 and the metallic bismuth so formed is volatilized and reoxidized4 ,the flame is uncolored4 ,,lead4--,this metal readily fuses under either flame1 and incrusts the charcoal with oxide at about the same distance from the assay as is the case with bismuth4 ,the oxide is1 while hot1 of a dark lemon-yellow color1 but upon cooling1 becomes of a sulphur yellow4 ,the carbonate which is formed upon the charcoal1 beyond the oxide1 is of a bluish-white color4 ,if the yellow incrustation of the oxide be heated with the flame of oxidation1 it disappears1 undergoing changes similar to those of bismuth above mentioned4 ,under the flame of reduction1 it1 however1 disappears1 tinging the flame blue4 ,,cadmium4--,this metal fuses with ease1 and1 in the flame of oxidation1 takes fire1 and burns with a deep yellow color1 giving off brown fumes1 which coat the charcoal1 to within a small distance of the assay1 with oxide of cadmium4 ,this coating exhibits its characteristic reddish-brown color most clearly when cold4 ,where the coating is very thin1 it passes to an orange color4 ,as oxide of cadmium is easily reduced1 and the metal very volatile1 the coating of oxide may be driven from place to place by the application of either flame1 to neither of which does it impart any color4 ,around the deposit of oxide1 the charcoal has occasionally a variegated tarnish4 ,,zinc4--,this metal fuses with ease1 and takes fire in the flame of oxidation1 burning with a brilliant greenish-white light1 and forming thick white fumes of oxide of zinc1 which coat the charcoal round the assay4 ,this coating is yellow while hot1 but when perfectly cooled1 becomes white4 ,if heated with the flame of oxidation1 it shines brilliantly1 but is not volatilized1 since the heated charcoal is1 under these circumstances1 insufficient to effect its reduction4 ,even under the reducing flame1 it disappears very slowly4 ,,tin4--,this metal fuses readily1 and1 in the flame of oxidation1 becomes covered with oxide1 which1 by a strong blast1 may be easily blown off4 ,in the reducing flame1 the fused metal assumes a white surface1 and the charcoal becomes covered with oxide4 ,this oxide is of a pale yellow color while hot1 and is quite brilliant when the flame of oxidation is directed upon it4 ,after cooling1 it becomes white4 ,it is found immediately around the assay1 and cannot be volatilized by the application of either flame4 ,,molybdenum4--,this metal1 in powder1 is infusible before the blowpipe4 ,if heated in the outer flame1 it becomes gradually oxidized1 and incrusts the charcoal1 at a small distance from the assay1 with molybdic acid1 which1 near the assay1 forms transparent crystalline scales1 and is elsewhere deposited as a fine powder4 ,the incrustation1 while hot1 is of a yellow color1 but becomes white after cooling4 ,it may be volatilized by heating with either flame1 and leaves the surface of the charcoal1 when perfectly cooled1 of a dark-red copper color1 with a metallic lustre1 due to the oxide of molybdenum1 which has been formed by the reducing action of the charcoal upon the molybdic acid4 ,in the reducing flame1 metallic molybdenum remains unchanged4 ,,silver4--,this metal1 when fused alone1 and kept in this state for some time1 under a strong oxidizing flame1 covers the charcoal with a thin film of dark reddish-brown oxide4 ,if the silver be alloyed with lead1 a yellow incrustation of the oxide of that metal is first formed1 and afterwards1 as the silver becomes more pure1 a dark red deposit is formed on the charcoal beyond4 ,if the silver contains a small quantity of antimony1 a white incrustation of antimonious acid is formed1 which becomes red on the surface if the blast be continued4 ,and if lead and antimony are both present in the silver1 after the greater part of these metals have been volatilized1 a beautiful crimson incrustation is produced upon the charcoal4 ,this result is sometimes obtained in fusing rich silver ores on charcoal4 ,,sulphides1 ,,chlorides1 ,,iodides1 ,,and ,,bromides4 ,in blowpipe experiments1 it rarely occurs that we have to deal with pure metals1 which1 if not absolutely non-volatile1 are recognized by the incrustation they form upon charcoal4 ,some compound substances1 when heated upon charcoal1 form white incrustations1 resembling that formed by antimony1 and which1 when heated1 may1 in like manner1 be driven from place to place4 ,among these are certain sulphides1 as sulphide of potassium1 and sulphide of sodium1 which are formed by the action of the reducing flame upon the sulphates of potassa and soda1 and are1 when volatilized1 reconverted into those sulphates1 and as such deposited on the charcoal4 ,no incrustation is1 however1 formed1 until the whole of the alkaline sulphate has been absorbed into the charcoal1 and has parted with its oxygen4 ,as sulphide of potassium is more volatile than sulphide of sodium1 an incrustation is formed from the former sooner than from the latter of these salts1 and is considerably thicker in the former case4 ,if the potash incrustation be touched with the reducing flame1 it disappears with a violet-colored flame2 and if a soda incrustation be treated in like manner1 an orange-yellow flame is produced4 ,sulphide of lithium1 formed by heating the sulphate in the reducing flame1 is volatilized in similar manner by a strong blast1 although less readily than the sulphide of sodium4 ,it affords a greyish white film1 which disappears with a crimson flame when submitted to the reducing flame4 ,besides the above1 the sulphides of bismuth and lead give1 when heated in either flame1 two different incrustations1 of which the more volatile is of a white color1 and consists in the one case of sulphate of lead1 and in the other of sulphate of bismuth4 ,if either of these be heated under the reducing flame1 it disappears in the former case with a bluish flame1 in the latter unaccompanied by any visible flame4 ,the incrustation formed nearest to the assay consists of the oxide of lead or bismuth1 and is easily recognized by its color when hot and after cooling4 ,there are many other metallic sulphides1 which1 when heated by the blowpipe flame1 cover the charcoal with a white incrustation1 as sulphide of antimony1 sulphide of zinc1 and sulphide of tin4 ,in all these cases1 however1 the incrustation consists of the metallic oxide alone1 and either volatilizes or remains unchanged1 when submitted to the oxidizing flame4 ,of the metallic chlorides there are many which1 when heated on charcoal with the blowpipe flame1 are volatilized and redeposited as a white incrustation4 ,among these are the chlorides of potassium1 sodium1 and lithium1 which volatilize and cover the charcoal immediately around the assay with a thin white film1 after they have been fused and absorbed into the charcoal1 chloride of potassium forms the thickest deposit1 and chloride of lithium the thinnest1 the latter being moreover of a greyish-white color4 ,the chlorides of ammonium1 mercury1 and antimony volatilize without fusing4 ,the chlorides of zinc1 cadmium1 lead1 bismuth1 and tin first fuse and then cover the charcoal with two different incrustations1 one of which is a white volatile chloride1 and the other a less volatile oxide of the metal4 ,some of the incrustations formed by metallic chlorides disappear with a colored flame when heated with the reducing flame2 thus chloride of potassium affords a violet flame1 chloride of sodium an orange one1 chloride of lithium a crimson flame1 and chloride of lead a blue one4 ,the other metals mentioned above volatilize without coloring the flame4 ,the chloride of copper fuses and colors the flame of a beautiful blue4 ,moreover1 if a continuous blast be directed upon the salt1 a part of it is driven off in the form of white fumes which smell strongly of chlorine1 and the charcoal is covered with incrustations of three different colors4 ,that which is formed nearest to the assay is of a dark grey color1 the next1 a dark yellow passing into brown1 and the most distant of a bluish white color4 ,if this incrustation be heated under the reducing flame1 it disappears with a blue flame4 ,metallic iodides and bromides behave upon charcoal in a similar manner to the chlorides4 ,those principally deserving of mention are the bromides and iodides of potassium and sodium4 ,these fuse upon charcoal1 are absorbed into its pores1 and volatilize in the form of white fumes1 which are deposited upon the charcoal at some distance from the assay4 ,when the saline films so formed are submitted to the reducing flame1 they disappear1 coloring the flame in the same manner as the corresponding chlorides4 #d4 ,,examinations ,,in ,,the ,,platinum ,,forceps4 ,before the student attempts to make an examination in the platinum forceps or tongs1 he should first ascertain whether or not it will act upon the platinum4 ,if the substance to be examined shall act chemically upon the platinum1 then it should be examined on the charcoal1 and the color of the flame ascertained as rigidly as possible4 ,the following list of substances produce the color attached to them4 ,a4 ,,violet4 ,potash1 and all its compounds1 with the exception of the phosphate and the borate1 tinge the color of the flame violet4 ,b4 ,,blue4 ,chloride of copper1 ,intense blue4 ,lead1 ,pale clear blue4 ,bromide of copper1 ,bluish green4 ,antimony1 ,bluish green4 ,selenium1 ,blue4 ,arsenic1 ,english green4 ,c4 ,,green4 ,ammonia1 ,dark green4 ,boracic acid1 ,dark green4 ,copper1 ,dark green4 ,tellurium1 ,dark green4 ,zinc1 ,light green4 ,baryta ,apple green4 ,phosphoric acid1 ,pale green4 ,molybdic acid1 ,apple green4 ,telluric acid1 ,light green4 ,d4 ,,yellow4 ,soda1 ,intense yellow4 ,water1 ,feeble yellow4 ,e4 ,,red4 ,strontia1 ,intense crimson4 ,lithia1 ,purplish red4 ,potash1 ,violet red4 ,lime1 ,purplish red4 ,the student may often be deceived in regard to the colors3 for instance1 if a small splinter of almost any mineral be held at the point of the flame of oxidation1 it will impart a very slight yellow to the flame4 ,this is caused1 doubtless1 by the water contained in the mineral4 ,if the piece of platinum wire is used1 and it should be wet with the saliva1 as is frequently done by the student1 then the small quantity of soda existing in that fluid will color the flame of a light yellow hue4 ,a4 ,,the ,,violet ,,color4 ,the salts of potash1 with the exception of the borate and the phosphate1 color the flame of a rich violet hue4 ,this color is best discovered in the outer flame of the blowpipe1 as is the case with all the other colors4 ,the flame should be a small one1 with a lamp having a small wick1 while the orifice of the blowpipe must be quite small4 ,these experiments should likewise be made in a dark room1 so that the colors may be discerned with the greatest ease4 ,in investigating with potash for the discernment of color1 it should be borne in mind that the least quantity of soda will entirely destroy the violet color of the potash1 by the substitution of its own strong yellow color4 ,if there be not more than the two hundredth part of soda1 the violet reaction of the potash will be destroyed4 ,this is likewise the case with the presence of lithia1 for its peculiar red color will destroy the violet of the potash4 ,therefore in making investigations with the silicates which contain potash1 the violet color of the latter can only be discerned when they are free from soda and lithia4 ,b4 ,,the ,,blue ,,color4 7a47 ,the ,chloride of ,copper4--,any of the chlorides produce a blue color in the blowpipe flame1 or any salt which contains chlorine will show the blue tint1 as the color in this case is referable to the chlorine itself4 ,there are1 however1 some chlorides which1 in consequence of the peculiar reactions of their bases1 will not produce the blue color1 although in these cases the blue of the chlorine will be very likely to blend itself with the color produced by the base4 ,the chloride of copper communicates an intense blue to the flame1 when fused on the platinum wire4 ,if the heat be continued until the chlorine is driven off1 then the greenish hue of the oxide of copper will be discerned4 7b47 ,lead4--,metallic lead communicates to the flame a pale blue color4 ,the oxide reacts in the same manner4 ,the lead-salts1 whose acids do not interfere with the color1 impart also a fine blue to the flame1 either in the platina forceps1 or the crooked wire4 7c47 ,bromide of ,copper4--,this salt colors the flame of a bluish-green color1 but when the bromine is driven off1 then we have the green of the oxide of copper4 7d47 ,antimony4--,this metal imparts a blue color to the blowpipe flame1 but if the metal is in too small a quantity1 then the color is a brilliant white4 ,if antimony is fused on charcoal1 the fused metal gives a blue color4 ,the white sublimate which surrounds the fused metal1 being subjected to the flame of oxidation1 disappears from the charcoal with a bluish-green color4 7e47 ,selenium4--,if fused in the flame of oxidation1 it imparts to the flame a deep blue color4 ,the incrustation upon charcoal gives to the flame the same rich color4 7f47 ,arsenic4--,the arseniates and metallic arsenic itself impart to the blowpipe flame a fine blue color1 provided that there is no other body present which may have a tendency to color the flame with its characteristic hue4 ,the sublimate of arsenious acid which surrounds the assay1 will give the same blue flame1 when dissipated by the oxidation flame4 ,the platinum forceps will answer for the exhibition of the color of arsenic1 even though the salts be arseniates1 whose bases possess the property of imparting their peculiar color to the flame1 such as the arseniate of lime4 ,c4 ,,the ,,green ,,color4 7a47 ,ammonia4--,the salts of ammonia1 when heated before the blowpipe1 and just upon the point of disappearing1 impart to the flame a feeble though dark green color4 ,this color1 however1 can only be discerned in a dark room4 7b47 ,boracic ,acid4--,if any one of the borates is mixed with two parts of a flux composed of one part of pulverized fluorspar1 and four and a half parts of bisulphate of potash1 and after being melted1 is put upon the coil of a platinum wire1 and held at the point of the blue flame1 soon after fusion takes place a dark green color is discerned1 but it is not of long duration4 ,the above process is that recommended by ,dr4 ,turner4 ,the green color of the borates may be readily seen by dipping them1 previously moistened with sulphuric acid1 into the upper part of the blue flame1 when the color can be readily discerned4 ,if soda be present1 then the rich green of the boracic acid is marred by the yellow of the soda4 ,borax1 or the biborate of soda 7,na,o1 #b;,,bo#c7 may be used for this latter reaction1 but if it be moistened with sulphuric acid1 the green of the boracic acid can then be seen4 ,if the borates1 or minerals which contain boracic acid1 are fused on charcoal with carbonate of potash1 then moistened with sulphuric acid and alcohol1 then the bright green of the boracic acid is produced1 even if the mineral contains but a minute portion of the boracic acid4 7c47 ,copper4 ,nearly all the ores of copper and its salts1 give a bright green color to the blowpipe flame4 ,metallic copper likewise colors the flame green1 being first oxidized4 ,if iodine1 chlorine1 and bromine are present1 the flame is considerably modified1 but the former at least intensifies the color4 ,many ores containing copper also color the flame green1 but the internal portion is of a bright blue color if the compound contains lead1 the latter color being due to the lead4 ,the native sulphide and carbonate of copper should be moistened with sulphuric acid1 while the former should be previously roasted4 ,if hydrochloric acid is used for moistening the salts1 then the rich green given by that moistened with the sulphuric acid is changed to a blue1 being thus modified by the chlorine of the acid4 ,silicates containing copper1 if heated in the flame in the platinum forceps1 impart a rich green color to the outer flame4 ,in fact1 if any substance containing copper be submitted to the blowpipe flame1 it will tinge it green1 provided there be no other substance present to impart its own color to the flame1 and thus modify or mar that of the copper4 7d47 ,tellurium4--,if the flame of reduction is directed upon the oxide of tellurium placed upon charcoal1 a green color is imparted to it4 ,if the telluric acid be placed upon platinum wire in the reduction flame1 the oxidation flame is colored green4 ,or if the sublimate be dissipated by the flame of oxidation1 it gives a green color4 ,if selenium be present1 the green color is changed to a blue4 7e47 ,zinc4--,the oxide of zinc1 when strongly heated1 gives a blue flame4 ,this is especially the case in the reducing flame4 ,the flame is a small one1 however1 and not very characteristic1 as with certain preparations of zinc the blue color is changed to a bright white4 ,the soluble salts of zinc give no blue color4 7f47 ,baryta4--,the soluble salts of baryta1 moistened1 and then submitted to the reduction flame1 produce a green color4 ,the salt should be moistened1 when the color will be strongly marked in the outer flame4 ,the insoluble salts do not produce so vivid a color as the soluble salts1 and they are brighter when they have previously been moistened4 ,the carbonate does not give a strong color1 but the acetate does1 so long as it is not allowed to turn to a carbonate4 ,the chloride1 when fused on the platinum wire1 in the point of the reduction flame1 imparts a fine green color to the oxidation flame4 ,this tint changes finally to a faint dirty green color4 ,the sulphate of baryta colors the flame green when heated at the point of the reduction flame4 ,but neither the sulphate1 carbonate1 nor1 in fact1 any other salt of baryta1 gives such a fine green color as the chloride4 ,the presence of lime does interfere with the reaction of baryta1 but still does not destroy its color4 7g47 ,phosphoric ,acid4--,the phosphates give a green color to the oxidation flame1 especially when they are moistened with sulphuric acid4 ,this is best shown with the platinum forceps4 ,the green of phosphoric1 or the phosphates1 is much less intense than that of the borates or boracic acid1 but yet the reaction is a certain one1 and is susceptible of considerable delicacy1 either with the forceps1 or still better upon platinum wire4 ,sulphuric acid is a great aid to the development of the color1 especially if other salts be present which would be liable to hide the color of the phosphoric acid4 ,in this reaction with phosphates1 the water should be expelled from them previous to melting them with sulphuric acid4 ,they should likewise be pulverized4 ,should soda be present it will only exhibit its peculiar color after the phosphoric acid shall have been expelled2 therefore1 the green color of the phosphoric acid should be looked for immediately upon submitting the phosphate to heat4 7h47 ,molybdic ,acid4--,if this acid or the oxide of molybdenum be exposed upon a platinum wire to the point of the reduction flame1 a bright green color is communicated to the flame of oxidation4 ,take a small piece of the native sulphide of molybdenum1 and expose it in the platinum tongs to the flame referred to above1 when the green color characteristic of this metal will be exhibited4 7i47 ,telluric ,acid4--,if the flame of reduction is directed upon a small piece of the oxide of tellurium placed upon charcoal1 a bright green color is produced4 ,or if telluric acid be submitted to the reduction flame upon the loop of a platinum wire1 it communicates to the outer flame the bright green of tellurium4 ,if the sublimate found upon the charcoal in the first experiment be submitted to the blowpipe flame1 the green color of tellurium is produced while the sublimate is volatilized4 ,if selenium be present the green color is changed to a deep blue one4 ,d4 ,,yellow4 ,the salts of soda all give a bright yellow color when heated in the platinum loop in the reduction flame4 ,this color is very persistent1 and will destroy the color of almost any other substance4 ,every mineral of which soda is a constituent1 give this bright orange-yellow reaction4 ,even the silicate of soda itself imparts to the flame of oxidation the characteristic yellow of soda4 ,e4 ,,red4 7a47 ,strontia4--,moisten a small piece of the chloride of strontium1 put it in the platinum forceps and submit it to the flame of reduction1 when the outer flame will become colored of an intense red4 ,if the salt of strontia should be a soluble one1 the reaction is of a deeper color than if an insoluble salt is used1 while the color is of a deeper crimson if the salt is moistened4 ,if the salt be a soluble one1 it should be moistened and dipped into the flame1 while if it be an insoluble salt1 it should be kept dry and exposed beyond the point of the flame4 ,the carbonate of strontia should be moistened with hydrochloric acid instead of water1 by which its color similates that of the chloride of strontium when moistened with water4 ,in consequence of the decided red color which strontia communicates to flame1 it is used by pyrotechnists for the purpose of making their crimson fire4 7b47 ,lithia4--,the color of the flame of lithia is slightly inclined to purple4 ,the chloride1 when placed in the platinum loop1 gives to the outer flame a bright red color1 sometimes with a slight tinge of purple4 ,potash does not prevent this reaction1 although it may modify it to violet2 but the decided color of soda changes the red of lithia to an orange color4 ,if much soda be present1 the color of the lithia is lost entirely4 ,the color of the chloride of lithium may be distinctly produced before the point of the blue flame1 and its durability may be the means of determining it from that of lithium1 as the latter1 under the same conditions1 is quite evanescent4 ,the minerals which contain lithia1 frequently contain soda1 and thus the latter destroys the color of the former4 7c47 ,potash4--,the salts of potash1 if the acid does not interfere1 give a purplish-red color before the blowpipe2 but as the color is more discernibly a purple1 we have classed it under that color4 7d47 ,lime4--,the color of the flame of lime does not greatly differ from that of strontia1 with the exception that it is not so decided4 ,arragonite and calcareous spar1 moistened with hydrochloric acid1 and tried as directed for strontia1 produce a red light1 not unlike that of strontia4 ,the chloride of calcium gives a red tinge1 but not nearly so decided as the chloride of strontium4 ,the carbonate of lime will produce a yellowish flame for a while1 until the carbonic acid is driven off1 when the red color of the lime may be discerned4 ,if the borate or phosphate of lime be used1 the green color of the acids predominates over the red of the lime4 ,baryta also destroys the red color of the lime1 by mixing its green color with it4 ,there is but one silicate of lime which colors the flame red1 it is the variety termed tabular spar4 #e4 ,,examinations ,,in ,,the ,,borax ,,bead4 ,in order to examine a substance in borax1 the loop of the platinum wire should1 after being thoroughly cleaned1 and heated to redness1 be quickly dipped into the powdered borax1 and then quickly transferred to the flame of oxidation1 and there fused4 ,if the bead is not large enough to fill the loop of the wire1 it must be subjected again to the same process4 ,by examining the bead1 both when hot and cold1 by holding it up against the light1 it can be soon ascertained whether it is free from dirt by the transparency1 or the want of it1 of the bead4 ,in order to make the examination of a substance1 the bead should be melted and pressed against it1 when enough will adhere to answer the purpose4 ,this powder should then be fused in the oxidation flame until it mixes with1 and is thoroughly dissolved by the borax bead4 ,the principal objects to be determined now are3 the color of the borax bead1 both when heated and when cooled2 also the rapidity with which the substance dissolves in the bead1 and if any gas is eliminated4 ,if the color of the bead is the object desired1 the quantity of the substance employed must be very small1 else the bead will be so deeply colored1 as in some cases to appear almost opaque1 as1 for instance1 in that of cobalt4 ,should this be the case1 then1 while the bead is still red hot1 it should be pressed flat with the forceps2 or it may1 while soft1 be pulled out to a thin thread1 whereby the color can be distinctly discovered4 ,some bodies1 when heated in the borax bead1 present a clear bead both while hot and cold2 but if the bead be heated with the intermittent flame1 or in the flame of reduction1 it becomes opalescent1 opaque or milk-white4 ,the alkaline earths are instances of this kind of reaction1 also glucina oxide of cerium1 tantalic and titanic acids1 yttria and zirconia4 ,but if a small portion of silica should be present1 then the bead becomes clear4 ,this is likewise the case with some silicates1 provided there be not too large a quantity present1 that is3 over the quantity necessary to saturate the borax1 for1 in that case1 the bead will be opaque when cool4 ,if the bead be heated on charcoal1 a small tube or cavity must be scooped out of the charcoal1 the bead placed in it1 and the flame of reduction played upon it4 ,when the bead is perfectly fused1 it is taken up between the platinum forceps and pressed flat1 so that the color may be the more readily discerned4 ,this quick cooling also prevents the protoxides1 if there be any present1 from passing into a higher degree of oxidation4 ,the bead should first be submitted to the oxidation flame1 and any reaction carefully observed4 ,then the bead should be submitted to the flame of reduction4 ,it must be observed that the platinum forceps should not be used when there is danger of a metallic oxide being reduced1 as in this case the metal would alloy with the platinum and spoil the forceps4 ,in this case charcoal should be used for the support4 ,if1 however1 there be oxides present which are not reduced by the borax1 then the platinum loop may be used4 ,tin is frequently used for the purpose of enabling the bead to acquire a color for an oxide in the reducing flame1 by its affinity for oxygen4 ,the oxide1 thus being reduced to a lower degree of oxidation1 imparts its peculiar tinge to the bead as it cools4 ,the arsenides and sulphides1 before being examined1 should be roasted1 and then heated with the borax bead4 ,the arsenic of the former1 it should be observed1 will act on the glass tube in which the sublimation is proceeding1 if the glass should contain lead4 ,it should be recollected that earths1 metallic oxides1 and metallic acids are soluble in borax1 except those of the easily reducible metals1 such as platinum or gold1 or of mercury1 which too readily vaporize4 ,also the metallic sulphides1 after the sulphur has been driven off4 ,also the salts of metals1 after their acids are driven off by heat4 ,also the nitrates and carbonates1 after their acids are driven off during the fusion4 ,also the salts of the halogens1 such as the chlorides1 iodides1 bromides1 etc41 of the metals4 ,also the silicates1 but with great tardiness4 ,also the phosphates and borates that fuse in the bead without suffering decomposition4 ,the metallic sulphides are insoluble in borax1 and many of the metals in the pure state4 ,there are many substances which give clear beads with borax both while hot and cold1 but which1 upon being heated with the intermittent oxidation flame1 become enamelled and opaque4 ,the intermittent flame may be readily attained1 not by varying the force of the air from the mouth1 but by raising and depressing the bead before the point of the steady oxidating flame4 ,the addition of a little nitrate of potash will often greatly facilitate the production of a color1 as it oxidizes the metal4 ,the hot bead should be pressed upon a small crystal of the nitrate1 when the bead swells1 intumesces1 and the color is manifested in the surface of the bead1 #f4 ,,examinations ,,in ,,microcosmic ,,salt4 ,microcosmic salt is a better flux for many metallic oxides than borax1 as the colors are exhibited in it with more strength and character4 ,microcosmic salt is the phosphate of soda and ammonia4 ,when it is ignited it passes into the biphosphate of soda1 the ammonia being driven off4 ,this biphosphate of soda possesses an excess of phosphoric acid1 and thus has the property of dissolving a great number of substances1 in fact almost any one1 with the exception of silica4 ,if the substances treated with this salt consist of sulphides or arsenides1 the bead must be heated on charcoal4 ,but if the substance experimented upon consists of earthly ingredients or metallic oxides1 the platinum wire is the best4 ,if the latter is used a few additional turns should be given to the wire in consequence of the greater fluidity of the bead over that of borax4 ,the microcosmic salt bead possesses the advantage over that of borax1 that the colors of many substances are better discerned in it1 and that it separates the acids1 the more volatile ones being dissipated1 while the fixed ones combine with a portion of the base equally with the phosphoric acid1 or else do not combine at all1 but float about in the bead1 as is the case particularly with silicic acid4 ,many of the silicates give with borax a clear bead1 while they form with microcosmic salt an opalescent one4 ,it frequently happens1 that if a metallic oxide will not give its peculiar color in one of the flames1 that it will in the other1 as the difference in degree with which the metal is oxidized often determines the color4 ,if the bead is heated in the reducing flame1 it is well that it should be cooled rapidly to prevent a reoxidation4 ,reduction is much facilitated by the employment of metallic tin1 whereby the protoxide or the reduced metal may be obtained in a comparatively brief time4 ,the following tables1 taken from ,plattner and ,sherer1 will present the reactions of the metallic oxides1 and some of the metallic acids1 in such a clear light1 that the student cannot very easily be led astray1 if he gives the least attention to them4 ,it frequently happens that a tabular statement of reactions will impress facts upon the memory when long detailed descriptions will fail to do so4 ,it is for this purpose that we subjoin the following excellent tables4 99 99 99 99 99 ,,table ,i4 ,a4 ,,borax4 #a4 ,oxydizing flame4 #b4 ,reducing ,b4 ,,microcosmic ,,salt4 #a4 ,oxydizing flame4 #b4 ,reducing ,a4 ,,borax #a4 ,oxydizing flame ---------------------------------------- ---------------------------------- ,color of ,bead4 ---------------------------------------- --------------------------------- ,substances which produce this color ---------------------------------------- ------------------------------ in the hot bead4 in the cold bead4 ---------------------------------------- -------------------------------- ,colorless ---------------------------------------- --------------------------------- ,silica ,silica ,alumina ,alumina ,oxide of ,tin ,oxide of ,tin ,telluric ,acid ,telluric ,acid ,baryta ,baryta ,strontia ,strontia ,lime ,lime ,magnesia ,magnesia ,glucina ,in all ,glucina ,yttria proportions4 ,yttria ,zirconia ,zirconia ,thoria ,thoria ,with ,oxide of ,lanthanum ,oxide of ,lanthanum intermittent ,silver flame ,tantalic ,acid ,tantalic ,acid opaque ,niobic ,niobic white4 ,pelopic _/ ,pelopic ,titanic _/ ,titanic ,tungstic ,in small ,tungstic ,molybdic quantity ,molybdic ,oxide of ,zinc only4 ,oxide of ,zinc _/ ,cadmium ,cadmium_/ ,lead ,in large ,lead ,bismuth _/ quantity ,bismuth ,antimony _/ yellow4 ,antimony ---------------------------------------- ------------------------------- ,yellow1 orange-red and reddish-brown4 ---------------------------------------- ------------------------------- ,titanic ,acid1 yellow ,tungstic ,acid1 yellow ,molybdic ,acid1 dark yellowwhen in ,oxide of ,zinc1 pale-yellowlarge ,oxide of ,cadmium1 quantity4 pale-yellow ,otherwise ,oxide of ,lead1 yellow colorless4 ,oxide of ,bismuth1 orange _/ ,oxide of ,antimony1 yellow_/ ,oxide of ,cerium1 red ,oxide of ,cerium with interm4 ,oxide of ,iron1 dark red flame opaque white4 ,oxide of ,uranium1 red ,oxide of ,iron1 yellow ,oxide of ,silver ,oxide of ,uranium with interm4 flame opaque yellow4 ,oxide of ,silver in large proportion1 with interm4 flame yellow4 ,vanadic ,acid1 yellow ,vanadic ,acid1 yellow4 ,oxide of ,chromium1 dark-red ,oxide of ,nickel1 reddish-brown4 ,oxide of ,manganese1 red to violet4 ---------------------------------------- -------------------------------- ,violet or ,amethyst4 ---------------------------------------- -------------------------------- ,oxide of ,nickel ,manganese ,oxide of ,didymium4 ,didymium ---------------------------------------- -------------------------------- ,blue4 ---------------------------------------- -------------------------------- ,oxide of ,cobalt ,oxide of ,cobalt4 ,copper1 blue to greenish-blue4 ---------------------------------------- -------------------------------- ,green4 ---------------------------------------- -------------------------------- ,oxide of ,copper ,oxide of ,chromium1 with yellowish tinge4 ---------------------------------------- -------------------------------- ,a4 ,,borax #b4 ,reducing flame ---------------------------------------- -------------------------------- ,color of ,bead4 ---------------------------------------- --------------------------------- ,substances which produce this color ---------------------------------------- ------------------------------ in the hot bead4 in the cold bead4 ---------------------------------------- -------------------------------- ,colorless ---------------------------------------- -------------------------------- ,silica ,silica ,alumina ,alumina ,oxide of ,tin ,oxide of ,tin ,baryta ,baryta ,strontia ,strontia ,lime ,lime ,magnesia ,magnesia ,with ,glucina ,glucina intermittent ,yttria ,yttria flame ,zirconia ,zirconia opaque-white4 ,thoria ,thoria only when saturated ,oxide of ,lanthanum ,oxide of ,lanthanum ,cerium ,cerium _/ ,tantalic ,acid ,tantalic ,acid _/ ,oxide of ,didymium ,oxide of ,didymium ,manganese ,manganese ,niobic ,acid ,in small ,niobic ,acid ,in small ,pelopic proportions4 ,pelopic proportions4 _/ _/ ,oxide of ,silver ,oxide of ,silver ,after ,zinc ,after long ,zinc long ,cadmium continued ,cadmium continued ,lead blowing4 ,lead blowing4 ,bismuth ,otherwise ,bismuth ,otherwise ,antimony grey4 ,antimony grey4 ,nickel _/ ,nickel _/ ,telluric ,acid _/ ,telluric ,acid _/ ---------------------------------------- -------------------------------- ,yellow to brown4 ---------------------------------------- -------------------------------- ,titanic ,acid ,titanic ,acid4 ,tungstic ,tungstic ,molybdic ,molybdic ,vanadic ---------------------------------------- -------------------------------- ,blue4 ---------------------------------------- -------------------------------- ,oxide of ,cobalt4 ,oxide of ,cobalt4 ,titanic ,acid with intermittent flame opaque-blue4 ---------------------------------------- -------------------------------- ,green4 ---------------------------------------- -------------------------------- ,oxide of ,iron ,oxide of ,iron1 bottle-green4 ,uranium ,oxide of ,uranium1 bottle- ,chromium green4 ,oxide of ,chromium1 emerald- green4 ,vanadic ,acid1 emerald-green4 ---------------------------------------- -------------------------------- ,opaque-grey4 7,the opacity generally becomes distinct during cooling47 ---------------------------------------- -------------------------------- ,oxide of ,silver ,oxide of ,silver4 ,zinc ,after ,zinc ,after ,cadmium short ,cadmium short ,lead blowing4 ,lead blowing4 ,bismuth ,otherwise ,bismuth ,otherwise ,antimony colorless4 ,antimony colorless4 ,nickel _/ ,nickel _/ ,telluric ,acid _/ ,telluric ,acid _/ ,niobic ,acid ,after long ,niobic ,acid ,after long ,pelopic continued blowing ,pelopic continued and in blowing and considerable in considerable _/ proportion4 _/ proportion4 ---------------------------------------- -------------------------------- ,opaque red and reddish-brown4 ---------------------------------------- -------------------------------- ,oxide of ,copper ,oxide of ,copper4 ---------------------------------------- -------------------------------- ,b4 ,,microcosmic ,,salt4 #a4 ,oxydizing flame4 ---------------------------------------- -------------------------------- ,color of ,bead4 ---------------------------------------- --------------------------------- ,substances which produce this color ---------------------------------------- ------------------------------ in the hot bead4 in the cold bead4 ---------------------------------------- -------------------------------- ,colorless ---------------------------------------- -------------------------------- ,silica 7only ,silica slightly soluble7 ,alumina ,alumina ,oxide of ,tin ,oxide of ,tin ,telluric ,acid ,telluric ,acid ,baryta ,baryta ,strontia ,strontia ,with ,lime ,in all ,lime intermittent ,magnesia proportions4 ,magnesia flame ,glucina ,glucina opaque ,yttria ,yttria white4 ,zirconia ,zirconia ,thoria ,thoria _/ ,oxide of ,lanthanum ,oxide of ,lanthanum_/ ,cerium ,niobic ,acid _/ ,niobic ,acid ,pelopic _/ ,pelopic ,tantalic ,tantalic ,titanic ,titanic ,tungstic ,tungstic ,oxide of ,zinc ,in small ,oxide of ,zinc ,cadmium quantity only4 ,cadmium ,lead ,in large ,lead ,bismuth quantity ,bismuth ,antimony _/ yellow4 ,antimony _/ ---------------------------------------- -------------------------------- ,yellow1 orange1 red and brown4 ---------------------------------------- -------------------------------- ,tantalic ,acid ,titanic ,tungstic ,oxide of ,zinc ,in large ,cadmium quantity4 ,lead ,bismuth ,antimony _/ ,silver ,oxide of ,silver4 ,cerium ,iron ,oxide of ,iron4 ,nickel ,nickel4 ,uranium ,uranium1 yellowish-green4 ,vanadic ,acid ,vanadic ,acid4 ,oxide of ,chromium ---------------------------------------- -------------------------------- ,violet or ,amethyst4 ---------------------------------------- -------------------------------- ,oxide of ,manganese ,oxide of ,manganese4 ,didymium ,didymium4 ---------------------------------------- -------------------------------- ,blue4 ---------------------------------------- -------------------------------- ,oxide of ,cobalt ,oxide of ,cobalt ,oxide of ,copper1 to greenish-blue4 ---------------------------------------- -------------------------------- ,green4 ---------------------------------------- -------------------------------- ,molybdic ,acid1 yellowish-green ,molybdic ,acid1 yellowish-green4 ,oxide of ,copper ,oxide of ,uranium1 yellowish-green4 ,oxide of ,chromium1 emerald-green4 ---------------------------------------- -------------------------------- ,b4 ,,microcosmic ,,salt4 #b4 ,reducing flame4 ---------------------------------------- -------------------------------- ,color of ,bead4 ---------------------------------------- --------------------------------- ,substances which produce this color ---------------------------------------- ------------------------------- in the hot bead4 in the cold bead4 ---------------------------------------- -------------------------------- ,colorless ---------------------------------------- -------------------------------- ,silica 7only slightly soluble7 ,silica 7only slightly soluble74 ,alumina ,alumina4 ,oxide of ,tin ,oxide of ,tin4 ,baryta ,baryta ,strontia ,strontia ,lime ,lime ,magnesia ,magnesia ,with an ,glucina ,glucina intermittent ,yttria ,yttria flame ,zirconia ,zirconia opaque- ,thoria ,thoria only when white4 saturated _/ ,oxide of ,lanthanum ,oxide of ,lanthanum_/ ,cerium ,cerium4 ,didymium ,didymium4 ,manganese ,manganese4 ,tantalic ,acid ,tantalic ,acid4 ,oxide of ,silver ,oxide of ,silver ,zinc ,zinc ,after ,cadmium ,after long ,cadmium long ,lead continued ,lead continued ,bismuth blowing4 ,bismuth blowing4 ,antimony ,otherwise grey4 ,antimony ,otherwise ,nickel _/ ,nickel _/ grey4 ,telluric ,acid _/ ,telluric ,acid _/ ---------------------------------------- -------------------------------- ,yellow1 red1 and brown4 ---------------------------------------- -------------------------------- ,oxide of ,iron1 red ,oxide of ,iron4 ,titanic ,acid1 yellow ,pelopic ,acid1 brown ,pelopic ,acid4 ,ferruginous ,titanic ,acid1 blood red ,ferruginous ,titanic ,acid4 ,niobic ,niobic ,pelopic ,pelopic ,tungstic ,tungstic ,vanadic ,acid1 brownish ,oxide of ,chromium1 reddish ---------------------------------------- -------------------------------- ,violet or ,amethyst4 ---------------------------------------- -------------------------------- ,niobic ,acid in large proportion ,niobic ,acid in large proportion4 ,titanic ,acid4 ---------------------------------------- -------------------------------- ,blue4 ---------------------------------------- -------------------------------- ,oxide of ,cobalt ,oxide of ,cobalt4 ,tungstic ,acid ,tungstic ,acid4 ,niobic ,acid in very large proportion4 ,niobic ,acid in very large proportion4 ---------------------------------------- -------------------------------- ,green4 ---------------------------------------- -------------------------------- ,oxide of ,uranium ,oxide of ,uranium4 ,molybdic ,acid ,molybdic ,acid4 ,vanadic ,oxide of ,chromium4 ---------------------------------------- -------------------------------- ,opaque-grey4 7,the opacity generally becomes distinct during cooling47 ---------------------------------------- -------------------------------- ,oxide of ,silver ,oxide of ,silver4 ,zinc ,zinc4 ,cadmium ,cadmium4 ,lead ,lead4 ,bismuth ,bismuth4 ,antimony ,antimony4 ,nickel ,nickel4 ,telluric ,acid ,telluric ,acid4 ---------------------------------------- -------------------------------- ,opaque-red and reddish brown4 ---------------------------------------- -------------------------------- ,oxide of ,copper ,oxide of ,copper4 ---------------------------------------- -------------------------------- 99 99 99 99 99 ,,table ,,ii4 ,metallic ,oxides #a4 ,oxide of ,cerium1 ,c#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves into a red or dark yellow glass 7similar to that produced by iron74 ,during cooling1 the color diminishes in the intensity and becomes finally yellow4 ,if much oxide be dissolved1 an opaque bead may be obtained with an intermittent flame1 and a still larger quantity renders it opaque spontaneously4 in the reducing flame4 ,the color of the bead becomes paler1 so that a bead1 which is yellow in the oxidizing flame1 is rendered colorless4 ,with a large quantity of oxide the bead becomes white and crystalline on cooling4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 ,during the process of cooling the color entirely disappears4 in the reducing flame4 ,both1 when hot and cold1 the bead is colorless1 by which character oxide of cerium may be distinguished from oxide of iron4 ,the glass remains clear even when containing a large quantity of the oxide4 99 99 99 99 99 #b4 ,oxide of ,lanthanum1 ,la,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves into a colorless glass1 which1 when sufficient oxide is present1 may be rendered opaque with an intermittent flame1 and becomes so spontaneously on cooling1 when a still larger amount is dissolved4 in the reducing flame4 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 in the reducing flame4 ,no reaction4 99 99 99 99 99 #c4 ,oxide of ,didymium1 ,,do4 ,behavior with ,borax on ,platinum wire in the oxidizing flame3 ,dissolves to a clear dark amethystine glass4 in the reducing flame4 ,no reaction4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 in the reducing flame4 ,no reaction4 99 99 99 99 99 #d4 ,oxide of ,manganese1 ,mn#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,affords an intense amethyst color1 which on cooling becomes violet4 ,a large quantity of the oxide produces an apparently black bead1 which however1 if pressed flat1 is seen to be transparent4 in the reducing flame4 ,the colored bead becomes colorless4 ,with a large amount of the oxide1 this reaction is best obtained upon charcoal1 and is facilitated by the addition of tin foil4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,with a considerable quantity of oxide an amethyst color is obtained1 but never so dark as in borax4 ,with but little oxide a colorless bead is obtained1 in which1 however1 the amethyst-color may be brought out by adding a little nitre4 ,while the bead is kept fused1 it froths and gives off bubbles of gas4 in the reducing flame4 ,the colored bead immediately loses its color1 either on platinum wire or on charcoal4 ,after the reduction the fluid bead remains still4 99 99 99 99 99 #e4 ,oxide of ,iron1 ,fe#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,with a small proportion of oxide1 the glass is of a yellow color1 while warm1 and colorless when cold2 with a larger proportion1 red1 while warm1 and yellow1 when cold2 and with a still larger amount1 dark-red1 while warm1 and dark-yellow1 when cold4 in the reducing flame4 ,treated alone on platinum wire1 the glass becomes of a bottle-green color 7,f#c,o#d71 and if touched with tin1 it becomes of a pale sea-green4 ,on charcoal with tin1 it assumes at first a bottle-green color1 which by continued blowing changes to a sea-green 7,fe,o74 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,with a certain amount of oxide1 the glass is of a yellowish-red color1 which on cooling changes to yellow1 then green1 and finally becomes colorless4 ,with a large addition of oxide1 the color is1 when warm1 dark red1 and passes1 while cooling1 into brownish-red1 dark green1 and finally brownish-red4 ,during the cooling process1 the colors change more rapidly than with borax4 in the reducing flame4 ,with a small proportion of oxide there is no reaction4 ,with a larger amount the bead is red1 while warm1 and becomes on cooling successively yellow1 green1 and russet4 ,with the addition of tin the glass becomes1 during cooling1 first green and then colorless4 99 99 99 99 99 #f4 ,oxide of ,cobalt1 ,co,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame3 ,colors the glass of an intense smalt blue both whilst hot and when cold4 ,when much oxide is present1 the color is so deep as to appear black4 in the reducing flame3 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax1 but less intensively colored4 ,during cooling the color becomes somewhat paler4 in the reducing flame4 ,as in the oxidizing flames4 99 99 99 99 99 #g4 ,oxide of ,nickel1 ,ni,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,colors intensely4 ,a small amount of oxide affords a glass which1 while warm1 is violet1 and becomes of a pale reddish-brown on cooling4 ,a larger addition produces a dark violet color in the warm and reddish-brown in the cold bead4 in the reducing flame4 ,the oxide is reduced and the metallic particles give the bead a turbid grey appearance4 ,if the blast be continued the metallic particles fall together without fusing1 and the glass becomes colorless4 ,this reaction is readily obtained with tin upon charcoal1 and the reduced nickel fuses to a bead with the tin4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves into a reddish glass which becomes yellow on cooling4 ,with a large addition of the oxide1 the glass is brownish while hot1 and orange when cold4 in the reducing flame4 ,on platinum wire the nickeliferous bead undergoes no change4 ,treated with tin upon charcoal1 it becomes at first opaque and grey1 and after long continued blowing the reduced nickel forms a bead1 and the glass remains colorless4 99 99 99 99 99 #h4 ,oxide of ,zinc1 ,zn,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves easily into a clear colorless glass1 which1 when much oxide is present1 may be rendered opaque and flocculent by an intermittent flame1 and becomes so spontaneously with a still larger addition4 ,when a considerable quantity is dissolved1 a glass is obtained which is pale yellow1 while hot1 and colorless when cold4 in the reducing flame4 ,on platinum wire the saturated glass becomes at first opaque and grey1 but by a sustained blast is again rendered clear4 ,on charcoal the oxide is gradually reduced2 the metal is volatilized and in crusts the charcoal with oxide4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 in the reducing flame4 ,as with borax4 99 99 99 99 99 #i4 ,oxide of ,cadmium1 ,cd,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,when in very large proportion1 dissolves to a clear yellow glass1 which becomes nearly colorless on cooling4 ,when the oxide is present in any considerable quantity1 the glass can be rendered opaque with an intermittent flame1 and1 with a larger addition1 it becomes so spontaneously on cooling4 in the reducing flame4 ,upon charcoal ebullition takes place and the oxide is reduced4 ,the metallic cadmium is volatilized and incrusts the charcoal with its characteristic deep yellow oxide4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,when in very large proportion dissolves to a clear glass1 having a yellow tinge1 while hot1 which disappears on cooling1 and when perfectly saturated1 becomes milk-white4 in the reducing flame4 ,on charcoal the oxide is slowly and imperfectly reduced4 ,the reduced metal forms the characteristic incrustation on the charcoal1 but the is thin and does not exhibit its color clearly until quite cold4 ,the addition of tin hastens the reaction4 99 99 99 99 99 #aj4 ,oxide of ,lead1 ,pb,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear yellow glass1 which loses its color upon cooling1 and when containing much oxide can be rendered dull under an intermittent flame4 ,with a still larger addition of oxide it becomes opaline yellow on cooling4 in the reducing flame4 ,the plumbiferous glass spreads out on charcoal1 becomes turbid1 bubbles up1 until the whole of the oxide is reduced1 when it again becomes clear4 ,it is1 however1 difficult to bring the lead together into a bead4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax1 but a larger addition of oxide1 required to produce a yellow color in the warm bead4 in the reducing flame4 ,on charcoal the plumbiferous glass becomes grey and dull4 ,with an over dose of oxide a part is volatilized and forms an incrustation on the charcoal beyond the bead4 ,the addition of tin does not render the glass opaque1 but somewhat more dull and grey than in its absence4 99 99 99 99 99 #aa4 ,oxide of ,tin1 ,sn,o#b4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,in small quantity dissolves slowly into a clear colorless glass1 which1 when cold1 remains clear1 and cannot be rendered opaque with an intermittent flame4 ,if a saturated bead1 which has been allowed to cool1 be reheated to incipient redness1 it loses its rounded form and exhibits imperfect crystallization4 in the reducing flame4 ,a glass containing but little oxide undergoes no change4 ,if much of the latter be present1 a part may be reduced upon charcoal4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,in small quantity dissolves very slowly to a colorless glass1 which remains clear on cooling4 in the reducing flame4 ,the glass undergoes no change1 either on charcoal or platinum wire4 99 99 99 99 99 #ab4 ,oxide of ,bismuth1 ,bi,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear glass which with a small amount of the oxide is yellow1 while warm1 and becomes colorless on cooling4 ,with a larger addition1 the glass is1 in the hot state1 of a deep orange color1 which changes to yellow and finally becomes opaline in process of cooling4 in the reducing flame4 ,a glass becomes at first grey and turbid1 then begins to effervesce1 which action continues during the reduction of the oxide1 and it finally becomes perfectly clear4 ,if tin be added1 the glass becomes at first grey from the reduced bismuth1 but1 when the metal is collected into a bead1 the glass is again clear and colorless4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves in small quantity to a clear colorless glass4 ,a larger addition affords a glass which1 while warm1 is yellow1 and becomes colorless on cooling4 ,when in sufficient proportion the glass may be rendered opaque under an intermittent flame1 and a still larger addition of oxide renders the bead spontaneously opaque on cooling4 in the reducing flame4 ,on charcoal1 and especially with the addition of tin1 the glass remains colorless and clear1 while warm1 but becomes on cooling of a dark grey color and opaque4 99 99 99 99 99 #ac4 ,oxide of ,uranium1 ,u#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,behaves similarly to oxide of iron1 with the exception that the color of the former is somewhat paler4 ,when sufficiently saturated1 the glass may be rendered of an opaque yellow by an intermittent flame4 in the reducing flame4 ,affords the same color as the oxide of iron4 ,the green glass obtained in this flame1 if sufficiently saturated1 can be rendered black by an intermittent flame1 but it has under these circumstances no enameline appearance4 ,on charcoal1 with the addition of tin1 the glass takes a dark green color4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves to a clear yellow glass1 which assumes a yellowish-green color on cooling4 in the reducing flame4 ,the glass assumes a beautiful green color1 which becomes more brilliant as the bead cools4 ,the addition of tin upon charcoal produces no further change4 99 99 99 99 99 #ad4 ,oxide of ,copper1 ,cu,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,produces an intense coloration4 ,if in small quantity1 the glass is green1 while warm1 and becomes blue on cooling4 ,if in large proportion1 the green color is so intense as to appear black4 ,when cool1 this becomes paler1 and changes to a greenish blue4 in the reducing flame4 ,if not too saturated1 the cupriferous glass soon becomes nearly colorless1 but immediately on solidifying assumes a red color and becomes opaque4 ,by long continued blowing on charcoal1 the copper in the bead is reduced and separates out as a small metallic bead1 leaving the glass colorless4 ,with the addition of tin1 the glass becomes of an opaque dull-red on cooling4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,with an equal proportion of oxide1 this salt is not so strongly colored as borax4 ,a small amount imparts a green color in the warm and a blue in the cold4 ,with a very large addition of oxide1 the glass is opaque in the hot state1 and after cooling of a greenish-blue4 in the reducing flame4 ,a tolerably saturated glass assumes a dark green color under a good flame1 and on cooling becomes of an opaque brick-red1 the moment it solidifies4 ,a glass containing but a small proportion of the oxide becomes equally red and opaque on cooling1 if treated with tin upon charcoal4 99 99 99 99 99 #ae4 ,oxide of ,mercury1 ,hg,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,no reaction4 in the reducing flame4 ,no reaction4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,no reaction4 in the reducing flame4 ,no reaction4 99 99 99 99 99 #af4 ,oxide of ,silver1 ,ag,o4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,the oxide is partly dissolved and partly reduced4 ,in small quantity1 it colors the glass yellow while warm1 the color disappearing on cooling4 ,in larger quantity1 the glass is yellow while warm1 but during cooling becomes paler to a certain point1 and then again deeper4 ,if reheated slightly1 the glass becomes opalescent4 in the reducing flame4 ,on charcoal the argentiferous glass becomes at first grey from the reduced metal1 but afterwards1 when the silver is collected into a bead1 it becomes clear and colorless4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,both the oxide and the metal afford a yellowish glass1 which1 when containing much oxide becomes opaline1 exhibiting a yellow color by daylight and a red one by artificial light4 in the reducing flame4 ,as in borax4 99 99 99 99 99 #ag4 ,oxide of ,platinum1 ,pt,o#b4 #ah4 ,oxide of ,palladium1 ,pd,o#b4 #ai4 ,oxide of ,rhodium1 ,r#b,o#c4 #bj4 ,oxide of ,iridium1 ,ir#b,o#c4 #ba4 ,oxide of ,ruthenium1 ,ru#b,o#i4 #bb4 ,oxide of ,osmium ,os,o#b4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,are reduced without being dissolved4 ,the reduced metal1 being infusible1 cannot however be collected into a bead4 in the reducing flame4 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as in borax4 in the reducing flame4 ,as in borax4 99 99 99 99 99 #bc4 ,oxide of ,gold1 ,au#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,is reduced without being dissolved and can be collected into a bead on charcoal4 in the reducing flame4 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as in borax4 in the reducing flame4 ,as in borax4 99 99 99 99 99 #bd4 ,titanic ,acid1 ,ti,o#b ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear glass which1 when but little acid is present1 is colorless1 but when in larger proportion1 yellow1 and1 on cooling1 colorless4 ,when sufficiently saturated1 it may be rendered opaque with an intermittent flame1 and with a still larger addition of the acid becomes so spontaneously on cooling4 in the reducing flame4 ,in small proportion1 it renders the glass yellow in larger quantity dark-yellow or brown4 ,a saturated bead assumes a blue enamel-like appearance under an intermittent flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear glass1 which1 when sufficiently saturated1 is yellow white hot1 and becomes colorless on cooling4 in the reducing flame4 ,the glass obtained in the oxidizing glame becomes yellow in the hot state1 but on cooling assumes a beautiful violet color4 ,if too saturated1 this color is so deep as to appear opaque1 but is not enameline4 ,if the titanic acid contains iron1 the glass becomes on cooling of a brownish-yellow or red color4 ,the addition of tin neutralizes the iron1 and the glass then becomes violet4 99 99 99 99 99 #be4 ,tantalic ,acid1 ,ta,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear colorless glass1 which1 when sufficiently saturated1 may be rendered opaque with an intermittent flame1 and with a larger addition of the acid becomes spontaneously enameline on cooling4 in the reducing flame4 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear glass1 which1 when it contains a large proportion of the acid1 is yellow while warm1 but becomes colorless on cooling4 in the reducing flame4 ,the glass obtained in the oxidizing flame undergoes no change1 nor does it1 according to ,h4 ,rose1 alter by the addition of sulphate of iron4 99 99 99 99 99 #bf4 ,niobic ,acid1 ,ni#b,o#c ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,behaves in a similar manner to tantalic acid1 but the glass requires a very large dose of the acid to render it opaque under an intermittent flame4 ,with an increased amount of the acid1 the glass is clear and yellow1 while warm1 but becomes on cooling turbid1 and when quite cold is white4 in the reducing flame4 ,the glass obtained in the oxidizing flame and which has become opalescent on cooling1 is rendered clear in the reducing flame4 ,with a larger addition of the acid1 it becomes dull1 and of a bluish-grey color on cooling1 and a still larger amount of renders it opaque and bluish grey4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves in large quantities to a clear colorless glass4 in the reducing flame4 ,if the acid be not present in too large a proportion1 the glass remains unchanged4 ,an additional amount of the acid renders it violet1 and a still larger quantity affords a beautiful pure blue color1 similar to that produced by tungstic acid4 ,if to such a bead some sulphate of iron be added1 the glass becomes blood-red4 ,the addition of peroxide of iron renders the glass deep yellow while warm1 the color becomes paler on cooling4 99 99 99 99 99 #bg4 ,pelopic ,acid1 ,pp#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,behaves similarly to the preceding4 in the reducing flame4 ,a bead containing sufficient of the acid to render it spontaneously opaque on cooling1 has a greyish color4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves even in large quantity to a colorless glass4 in the reducing flame4 ,with sufficient dose of the acid1 the bead becomes brown with a violet tinge4 ,this reaction is readily obtained upon charcoal4 ,sulphate of iron renders the bead blood-red4 99 99 99 99 99 #bh4 ,oxide of ,antimony1 ,sb,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,even when in large proportion1 dissolves to a clear glass1 which is yellow when warm1 but almost entirely loses its color on cooling4 ,on charcoal1 the antimonious acid may be almost expelled1 so that tin produces no further change4 in the reducing flame4 ,a bead1 that has only been treated for a short time in the oxidizing flame1 when submitted to the reducing flame becomes grey and turbid from the reduced antimony4 ,this soon volatizes and the glass again becomes clear4 ,the addition of tin renders the glass ash-grey or black1 according to the amount of oxide it contains4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves with ebullition to a glass of a pale yellow color while warm4 in the reducing flame4 ,on charcoal1 the saturated glass becomes at first dull1 but as soon as the reduced antimony is volatilized1 it again becomes clear4 ,with tin1 the glass is at first rendered grey by the reduced antimony1 but by continued blowing is restored to clearness4 ,even when the glass contains but little oxide1 tin produces this reaction4 99 99 99 99 99 #bi4 ,tungstic ,acid1 ,,wo#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily to a clear colorless glass4 ,in large proportion it renders the borax yellow1 while warm1 and with a still greater addition the bead may be made opaque with an intermittent flame4 ,if more be then added1 this reaction takes place spontaneously4 in the reducing flame4 ,when the oxide is present in small quantity1 the glass undergoes no change4 ,with a larger proportion1 the glass is deep yellow while warm1 and yellowish-brown when cold4 ,this reaction takes place upon charcoal1 with a small quantity of the acid4 ,tin produces a dark coloration1 when the acid is not present in too great a quantity4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves to a clear glass1 which1 when saturated1 is yellow in the hot state4 in the reducing flame4 ,the glass is of a pure blue4 ,if the tungstic acid contain iron1 the glass becomes blood-red on cooling1 similar to titanic acid4 ,in this case1 tin restores the blue color1 or1 if iron be in considerable quantity1 renders it green4 99 99 99 99 99 #cj4 ,molydbic ,acid1 ,,mo#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves readily and in large quantity4 ,when but little is dissolved1 the glass is yellow while hot and colorless when cold4 ,when in larger quantity yellow while warm and opaline when cold1 and a further addition of acid renders it yellow when warm1 the color1 on cooling1 changing first to a pale enamel blue1 and then to an enamel white4 in the reducing flame4 ,the glass1 which has been treated in the oxidizing flame1 becomes1 when the acid is not present in too large a quantity1 brown1 and when in large quantity1 perfectly opaque4 ,in a strong flame1 oxide of molybdenum is formed which is visible in the yellow glass in the form of black flakes4 ,if the glass appear opaque1 it should be flattened with the forceps4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves to a clear glass1 which1 when sufficient acid is present1 is of a yellowish-green color when warm1 and becomes nearly colorless on cooling4 ,on charcoal1 the glass becomes dark1 and when cool has a beautiful green color4 in the reducing flame4 ,the glass becomes of a bottle-green color1 which on cooling1 changes to a brilliant green1 similar to that produced by oxide of chromium4 ,the reaction on charcoal is precisely similar4 ,tin renders the color somewhat darker4 99 99 99 99 99 #ca4 ,vanadic ,acid1 ,va,o#h4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves to a clear glass1 which is colorless when only a small quantity of acid is present1 and yellow when containing a larger proportion4 in the reducing flame4 ,the yellow color of the glass changes to a brown when warm and a chrome-green on cooling4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 in the reducing flame4 ,as with borax4 99 99 99 99 99 #cb4 ,oxide of ,chromium1 ,cr#b,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,affords an intense color1 but dissolves slowly4 ,a small proportion colors the glass yellow when warm1 and yellowish green when cold2 a larger addition produces a dark red color when warm1 which1 on cooling1 becomes yellow and finally a brilliant green with a tinge of yellow4 in the reducing flame4 ,a small quantity of the oxide renders the glass beautifully green both when warm and when cold4 ,a larger addition changes it to a darker emerald green4 ,tin produces no change in the color4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,dissolves to a clear glass which has a pink tinge while warm1 but on cooling becomes dusky green1 and finally brilliantly green4 in the reducing flame4 ,as in the oxidizing flame1 except that the colors are somewhat darker4 ,tin produces no further change4 99 99 99 99 99 #cc4 ,arsenious ,acid1 ,as,o#c4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,no reaction4 in the reducing flame4 ,no reaction4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,no reaction4 in the reducing flame4 ,no reaction4 99 99 99 99 99 #cd4 ,tellurous ,acid1 ,te,o#b4 ,behavior with ,borax on ,platinum wire in the oxidizing flame4 ,dissolves to a clear colorless glass which1 when treated on charcoal1 becomes grey and dull from particles of reduced tellurium4 in the reducing flame4 ,as in the oxidizing flame4 ,behavior with ,mic4 ,salt on ,platinum wire in the oxidizing flame4 ,as with borax4 in the reducing flame4 ,as with borax4 99 99 99 99 99 #g4 ,,examinations ,,with ,,carbonate ,,of ,,soda4 ,the carbonate of soda is pulverized and then kneaded to a paste with water2 the substance to be examined1 in fine powder1 is also mixed with it4 ,a small portion of this paste is placed on the charcoal1 and gradually heated until the moisture is expelled1 when the heat is brought to the fusion of the bead1 or as high as it can be raised4 ,several phenomena will take place1 which must be closely observed4 ,notice whether the substance fuses with the bead1 and if so1 whether there is intumescence or not4 ,or1 whether the substance undergoes reduction2 or1 whether neither of these reactions takes place1 and1 on the contrary1 the soda sinks into the charcoal1 leaving the substance intact upon its surface4 ,if intumescence takes place1 the presence of either tartaric acid1 molybdic acid1 silicic1 or tungstic acid1 is indicated4 ,the silicic acid will fuse into a bead1 which becomes clear when it is cold4 ,titanic acid will fuse into the bead1 but may be easily distinguished from the silicic acid by the bead remaining opaque when cold4 ,strontia and baryta will flow into the charcoal1 but lime will not4 ,the molybdic and tungstic acids combine with the soda1 forming the respective salts4 ,these salts are absorbed by the charcoal4 ,if too great a quantity of soda is used1 the bead will be quite likely to become opaque upon cooling1 while1 if too small a quantity of soda is used1 a portion of the substance will remain undissolved4 ,these can be equally avoided by either the addition of soda1 or the substance experimented upon1 as may be required4 ,as silica and titanic acid are the only two substances that produce a clear bead1 the student1 if he gets a clear bead1 may almost conclude that he is experimenting with silica1 titanic acid being a rare substance4 ,when soda is heated with silica1 a slight effervescence will be the first phenomenon noticed4 ,this is the escape of the carbonic acid of the carbonate of soda1 while the silicic acid takes its place1 forming a glass with the soda4 ,as titanic acid will not act in the same manner as silica1 it can be easily distinguished by its bead not being perfectly pellucid4 ,if the bead with which silica is fused should be tinted of a hyacinth or yellow color1 this may be attributed to the presence of a small quantity of sulphur or a sulphate1 and this sometimes happens from the fact of the flux containing sulphate of soda4 ,the following metals1 when exposed with carbonate of soda to the reducing flame1 are wholly or partially reduced1 viz4 the oxides of all the noble metals1 the oxides and acids of tungsten1 molybdenum1 arsenic1 antimony1 mercury1 copper1 tellurium1 zinc1 lead1 bismuth1 tin1 cadmium1 iron1 nickel1 and cobalt4 ,mercury and arsenic1 as soon as they are reduced1 are dissipated1 while tellurium1 bismuth1 lead1 antimony1 cadmium1 and zinc1 are only partially volatilized1 and1 therefore1 form sublimates on the charcoal4 ,those metals which are difficult of reduction should be fused with oxalate of potassa1 instead of the carbonate of soda4 ,the carbonic oxide formed from the combustion of the acid of this salt is very efficient in the reduction of these metals4 ,carbonate of soda is very efficient for the detection of minute quantities of manganese4 ,the mixture of the carbonate of soda with a small addition of nitrate of potassa1 and the mineral containing manganese1 must be fused on platinum foil4 ,the fused mass1 when cooled1 presents a fine blue color4 99 99 99 99 99 #a4 ,the following minerals1 according to ,griffin1 produce beads with soda1 but do not fuse when heated alone3 quartz1 agalmatolyte1 dioptase1 hisingerite1 sideroschilosite1 leucite1 rutile1 pyrophyllite1 wolckonskoite4 #b4 ,the following minerals produce only slags with soda3 allophane1 cymophane1 polymignite1 schynite1 oerstedtite1 titaniferous iron1 tantalite1 oxides of iron1 yttro-tantalite1 oxides of manganese1 peroxide of tin 7is reduced71 hydrate of alumina1 hydrate of magnesia1 spinel1 gahnite1 worthite1 carbonate of zinc1 pechuran1 zircon1 thorite1 andalusite1 staurolite1 gehlenite1 chlorite spar1 chrome ochre1 uwarowite1 chromate of iron1 carbonates of the earths1 carbonates of the metallic oxides1 basic phosphate of yttria1 do4 of alumina1 do4 of lime1 persulphate of iron1 sulphate of alumina1 aluminite1 alumstone1 fluoride of cerium1 yttrocerite1 topaz1 corundum1 pleonaste1 chondrodite4 #c4 ,the following minerals produce beads with a small quantity of soda1 but produce slags if too much soda is added3 phenakite1 pierosmine1 olivine1 cerite1 cyanite1 talc1 gadolinite1 lithium-tourmaline4 99 99 99 99 99 #a4 ,the following minerals1 when fused alone1 produce beads4 ,of these minerals the following produce beads with soda3 the zeolites1 spodumene1 soda-spodumene1 labrador1 scapolite1 sodalite 7,greenland71 elolite1 mica from primitive lime-stone1 black talc1 acmite1 krokidolite1 lievrite1 cronstedtite1 garnet1 cerine1 helvine1 gadolinite1 boracic acid1 hydroboracite1 tincal1 boracite1 datholite1 botryolite1 axinite1 lapis lazuli1 eudialyte1 pyrosmalite1 cryolite4 #b4 ,the following minerals produce beads with a small quantity of soda1 but if too much is added they produce slags3 okenite1 pectolite1 red silicate of manganese1 black hydro-silicate of manganese1 idocrase1 manganesian garnets1 orthite1 pyrorthite1 sordawalite1 sodalite1 fluorspar4 #c4 ,the following minerals produce a slag with soda3 brevicite1 amphodelite1 chlorite1 fahlunite1 pyrope1 soap-stone 7,cornish7 red dichroite1 pyrargillite1 black potash tourmaline1 wolfram1 pharmacolite1 scorodite1 arseniate of iron1 tetraphyline1 hetepozite1 uranite1 phosphate of iron1 do4 of strontia1 do4 of magnesia1 polyhalite1 hauyne4 #d4 ,the following metals are reduced by soda3 tungstate of lead1 molybdate of lead1 vanadate of lead1 chromate of lead1 vauquelinite1 cobalt bloom1 nickel ochre1 phosphate of copper1 sulphate of lead1 chloride of lead1 and chloride of silver4 99 99 99 99 99 ,the following minerals fuse on the edges alone1 when heated in the blowpipe flame3 #a4 ,the following produce beads with soda3 steatite1 meerschaum1 felspar1 albite1 petalite1 nepheline1 anorthite1 emerald1 euclase1 turquois1 sodalite 7,vesuvius74 #b4 ,the following minerals produce beads with a small quantity of soda1 but with the addition of more produce slags3 tabular spar1 diallage1 hypersthene1 epidote1 zoisite4 #c4 ,the following minerals produce slags only with soda3 stilpnosiderite1 plombgomme1 serpentine1 silicate of manganese 7from ,piedmont71 mica from granite1 pimelite1 pinite1 blue dichroite1 sphenc1 karpholite1 pyrochlore1 tungstate of lime1 green soda tourmaline1 lazulite1 heavy spar1 gypsum4 99 99 99 99 99 ,the reactions of substances1 when fused with soda in the flame of oxidation may be of use to the student4 ,a few of them are therefore given4 ,silica gives a clear glass4 ,the oxide of tellurium and telluric acid gives a clear bead when it is hot1 but white after it is cooled4 ,titanic acid gives a yellow bead when hot4 ,the oxide of chromium gives also a clear yellow glass when hot1 but is opaque when cold4 ,molybdic acid gives a clear bead when hot1 but is turbid and white after cooling4 ,the oxides and acids of antimony give a clear and colorless bead while hot1 and white after cooling4 ,vanadic acid is absorbed by the charcoal1 although it is not reduced4 ,tungstic acid gives a dark yellow clear bead while hot1 but is opaque and yellow when cold4 ,the oxides of manganese give to the soda bead a fine characteristic green color4 ,this is the case with a very small quantity4 ,this reaction is best exhibited on platinum foil4 ,oxide of cobalt gives to the bead while hot a red color1 which1 upon being cooled1 becomes grey4 ,the oxide of copper gives a clear green bead while hot4 ,the oxide of lead gives a clear colorless bead while hot1 which becomes1 upon cooling1 of a dirty yellow color and opaque4 99 99 99 99 99 ,the following metals1 when they are fused with soda on charcoal1 in the flame of reduction1 produce volatile oxides1 and leave an incrustation around the assay1 viz4 bismuth1 zinc1 lead1 cadmium1 antimony1 selenium1 tellurium1 and arsenic4 ,bismuth1 under the reduction flame1 yields small particles of metal1 which are brittle and easily crushed4 ,the incrustation is of a flesh color1 or orange1 when hot1 but gets lighter as it cools4 ,the sublimate may be driven about the charcoal from place to place1 by either flame1 but is finally dissipated4 ,while antimony and tellurium1 in the act of dissipation1 give color to the flame1 bismuth does not1 and may thus be distinguished from them4 ,zinc deposits an incrustation about the assay1 which is yellow while hot1 but fades to white when cold4 ,the reduction flame dissipates this deposit1 but not that of oxidation4 ,all the zinc minerals deposit the oxide incrustation about the assay1 which1 when moistened with a solution of cobalt and heated1 changes to green4 ,lead is very easily reduced1 in small particles1 and may be easily distinguished by its flattening under the hammer1 unlike bismuth4 ,it leaves an incrustation around the assay resembling that of bismuth1 in the color of it1 and in the peculiar manner in which it lies around the assay4 ,cadmium deposits a dull reddish incrustation around the assay4 ,either of the flames dissipate the sublimate with the greatest readiness4 ,antimony reduces with readiness4 ,at the same time it yields considerable vapor1 and deposits an incrustation around the assay4 ,this deposit can be driven about on the charcoal by either of the flames4 ,the flame of reduction1 however1 produces the light blue color of the antimony4 ,selenium is deposited on the charcoal as a grey metallic-looking sublimate1 but sometimes appearing purple or blue4 ,if the reduction flame is directed on this deposit1 it is dissipated with a blue light4 ,tellurium is deposited on the charcoal as a white sublimate1 sometimes changing at the margin to an orange or red color4 ,the oxidation flame drives the deposit over the charcoal1 while the reduction-flame dissipates it with a greenish color4 ,arsenic is vaporized rapidly1 while there is deposited around the assay a white incrustation of arsenious acid4 ,this deposit will extend to some distance from the assay1 and is readily volatilized1 the reducing flame producing the characteristic alliaceous color4 99 99 99 99 99 ,the following metals1 or their compounds1 are reduced when fused with soda on charcoal1 in the flame of reduction4 ,they are reduced to metallic particles1 but give no incrustation1 viz4 nickel1 cobalt1 iron1 tin1 copper1 gold1 silver1 platinum1 tungsten1 and molybdenum4 ,the particles of iron1 nickel1 and cobalt1 it should be borne in mind1 are attracted by the magnet4 ,the following substances are neither fused nor reduced in soda1 viz4 alumina1 magnesia1 lime1 baryta1 strontia1 the oxide of uranium1 the oxides of cerium1 zirconia1 tantalic acid1 thorina1 glucina1 and yttria4 ,neither are the alkalies1 as they sink into the charcoal4 ,the carbonates of the earths1 strontia1 and baryta fuse4 99 99 99 99 99 ,part ,,iii ,,special ,,reactions2 ,,or1 ,,the ,,behavior ,,of ,,substances ,,before ,,the ,,blowpipe4 ,analytical chemistry may be termed the art of converting the unknown constituents of substances1 by means of certain operations1 into new combinations which we recognize through the physical and chemical properties which they manifest4 ,it is1 therefore1 indispensably necessary1 not only to be cognizant of the peculiar conditions by which these operations can be effected1 but it is absolutely necessary to be acquainted with the forms and combinations of the resulting product1 and with every modification which may be produced by altering the conditions of the analysis4 ,we shall first give the behavior of simple substances before the blowpipe2 and the student should study this part thoroughly1 by repeating each reaction1 so that he can acquire a knowledge of the color1 form1 and physical properties in general1 of the resulting combination4 ,there is nothing1 perhaps1 which will contribute more readily to the progress of the pupil1 than thorough practice with the reactions recommended in this part of the work1 for when once the student shall have acquired a practical eye in the discernment of the peculiar appearances of substances after they have undergone the decompositions produced by the strong heat of the blowpipe flame1 together with the reactions incident to these changes1 then he will have greatly progressed in his study1 and the rest will be comparatively simple4 ,a4 ,,metallic ,,oxides4 ,,group ,,first4--,,the ,,alkalies3 ,,potassa1 ,,soda1 ,,ammonia1 ,,and ,,lithia4 ,the alkalies1 in their pure1 or carbonated state1 render reddened litmus paper blue4 ,this is likewise the case with the sulphides of the alkalies4 ,the neutral salts of the alkalies1 formed with the strong acids1 do not change litmus paper1 but the salts formed with the weak acids1 render the red litmus paper blue2 for instance1 the alkaline salts with boracic acid4 ,fused with borax1 soda1 or microcosmic salt1 they give a clear bead4 ,the alkalies and their salts melt at a low red heat4 ,the alkalies cannot be reduced to the metallic state before the blowpipe4 ,they are not volatile when red hot1 except the alkali ammonia1 but they are volatile at a white heat4 7a47 ,potassa47,,ko74--,it is not found free1 but in combination with inorganic and organic acids1 as well in the animal as in the vegetable organism1 as in the mineral kingdom4 ,in the pure1 or anhydrous state1 or as the carbonate1 potassa absorbs moisture1 and becomes fluid1 or is deliquescent1 as it is termed4 ,by exposing potassa1 or its easily fusible salts 7except the phosphate or borate71 upon platinum wire1 to the point of the blue flame1 there is communicated to the external flame a violet color1 in consequence of a reduction and reoxidation4 ,this color1 though characteristic of all the potassa compounds1 is scarcely visible with the phosphate or borate salts of that alkali4 ,the admixture of a very little soda 7#a_/cjjth7 destroys the color imparted by the potassa1 while the flame assumes a yellow color1 characteristic of the soda4 ,the presence of lithia changes the violet color of the potash into red4 ,the silicates of potassa must exist in pretty large proportion before they can be detected by the violet color of the flame1 and those minerals must melt easily at the edges4 ,the presence of a little soda in these instances conceals the reaction in the potassa entirely4 ,if alcohol is poured over potassa compounds which are powdered1 and then set on fire1 the external flame appears violet-colored1 particularly when stirred with a glass rod1 and when the alcohol is really consumed4 ,the presence of soda in lithia will1 in this case likewise1 hide by their own characteristic color1 that of the potassa4 ,the salts of potassa are absorbed when fused upon charcoal4 ,the sulphur1 bromine1 chlorine1 and iodine compounds of potassa give a white1 but easily volatile sublimate upon the charcoal1 around the place where the fused substance reposed4 ,this white sublimate manifests itself only when the substance is melted and absorbed within the charcoal1 and ceases to be visible as soon as it is submitted to the reducing flame1 while the external flame is colored violet2 sulphate of potassa1 for instance1 is reduced by the glowing charcoal into the sulphide4 ,this latter is somewhat volatile1 but by passing through the oxidation flame1 it is again oxidized into the sulphate4 ,this1 being less volatile1 sublimes upon the charcoal1 but by exposing it again to the flame of reduction1 it is reduced and carried off to be again oxidized by its passage through the oxidation flame4 ,potassa and its compounds give1 with soda1 borax or microcosmic salt1 as well when hot as cold1 colorless beads1 unless the acid associated with the alkali should itself produce a color4 ,when borax is fused with some pure boracic acid1 and sufficient of the oxide of nickel is added1 so that the beads appear of a brown color after being cooled1 and then the bead thus produced fused with the substance suspected to contain potassa1 in the oxidation flame1 the brown color is changed to blue4 ,the presence of the other alkalies does not prevent this reaction4 ,as it is not possible to detect potassa compounds with unerring certainty by the blowpipe flame1 the the wet method should be resorted to for the purpose of confirming it4 ,the silicates of potassa must be prepared as follows1 for analytical purposes by the wet way4 ,mix one part of the finely powdered substance with two parts of soda 7free from potassa71 and one part of borax4 ,fuse the mixture upon charcoal in the oxidation flame to a clear1 transparent bead4 ,this is to be exposed again with the pincers to the oxidation flame1 to burn off the adhering coal particles4 ,then pulverize and dissolve in hydrochloric acid to separate the silica2 evaporate to dryness1 dissolve the residue in water1 with the admixture of a little alcohol1 and test the filtrate with chloride of platinum for potassa4 7b47 ,soda 7,na,o74--,this is one of the most abundant substances1 although seldom found free1 but combined with chlorine or some other less abundant compound4 ,soda1 its hydrate and salts manifest in general the same properties as their respective potash compounds2 but the salts of soda mostly contain crystal water1 which leaves the salts if they are exposed to the air1 and the salts effervesce4 ,by exposing soda or its compounds upon a platinum wire to the blue flame1 a reddish-yellow color is communicated to the external flame1 which appears as a long brilliant stream and considerably increased in volume4 ,the presence of potash does not prevent this reaction of soda4 ,if there is too large a quantity of potash1 the flame near to the substance is violet-colored1 but the edge of the flame exhibits the characteristic tint of the soda4 ,the presence of lithia changes the yellow color to a shade of red4 ,when alcohol is poured over powdered soda compounds and lighted1 the flame exhibits a reddish-yellow color1 particularly if the alcohol is stirred up with a glass rod1 or if the alcohol is nearly consumed4 ,fused upon charcoal1 soda compounds are absorbed by the coal4 ,the sulphide1 chloride1 iodide1 and bromide of soda yield a white sublimate around the spot where the substance is laid1 but this sublimate is not so copious as that of the potash compounds1 and disappears when touched with the reduction flame1 communicating a yellow color to the external flame4 ,the presence of soda in compounds must likewise be confined by reactions in the wet way4 7c47 ,ammonia 7,,nh#d,o74--,in the fused state1 and at the usual temperature1 ammonia is a pungent gas1 and exerts a reaction upon litmus paper similar to potash and soda4 ,ammonium is considered by chemists as a metal1 from the nature of its behavior with other substances4 ,it has not been isolated1 but its existence is now generally conceded by all chemists4 ,the ammonia salts are volatile1 and many of them sublimate without being decomposed4 ,the salts of ammonia1 on being heated in the point of the blue flame1 produce a feeble green color in the external flame1 just previous to their being converted into vapor4 ,but this color is scarcely visible1 and presents nothing characteristic4 ,when the ammonia salts are mixed with the carbonate of soda1 and heated in a glass tube closed at one end1 carbonate of ammonia is sublimed1 which can be readily recognized by its penetrating smell of spirits of hartshorn4 ,this sublimate will render blue a slip of red litmus paper4 ,this can be easily done by moistening the litmus paper1 and then inserting the end of it in the tube4 ,by holding a glass rod1 moistened with dilute hydrochloric acid1 over the mouth of the tube1 a white vapor is instantly rendered visible 7sal ammoniac74 7d47 ,lithia 7,li,o74--,in the pure state1 lithia is white and crystalline1 not easily soluble in water1 and does not absorb moisture4 ,it changes red litmus to blue1 and at a low red heat it melts4 ,lithia or its salts1 exposed to the point of the blue flame1 communicates a red color to the external or oxidation flame1 in consequence of a reduction1 sublimation1 and re-oxidation of the lithia4 ,an admixture of potash communicates to this flame a reddish-violet color1 and the presence of soda that of a yellowish-red or orange4 ,if the soda1 however1 is in too great proportion1 then its intense yellow hides the red of the lithia4 ,in the latter case the substance under test must be only imperfectly fused in the oxidation flame1 and then dipped in wax or tallow4 ,by exposing it now to the reduction flame1 the red color imparted to the external flame by the lithia becomes visible1 even if a considerable quantity of soda be present4 ,a particular phenomenon appears with the phosphate of lithia1 viz41 the phosphoric acid itself possesses the property of communicating to the flame a bluish-green color4 ,by its combination with lithia it still exhibits its characteristic color1 while the latter presents likewise its peculiar tint4 ,then we perceive a green flame in the centre of the flame1 while the red color of lithia surrounds it4 ,the silicates1 which contain only a little lithia1 produce only a slight hue in the flame1 and often none at all4 ,we have to mix one part of the silicate with two parts of a mixture composed of one part of fluorspar and one and a half parts of bisulphate of potassa4 ,moisten the mass with water so that the mass will adhere1 and then melt it upon a platinum wire in the reduction flame1 when that of oxidation will present the red color of lithia4 ,the ,borates of lithia produce at first a green color1 but it soon yields to the red of lithia4 ,when alcohol is poured over lithia or its compounds1 and inflamed1 it burns with a deep red color1 particularly if the fluid is stirred up with a glass rod1 or when the alcohol is nearly consumed4 ,this color presents the same modifications as the corresponding ones communicated to the blowpipe as mentioned above4 ,the salts of lithia are absorbed by charcoal when fused upon it4 ,the sulphide1 bromide1 iodide1 and chloride of lithia produce upon the charcoal a greyish-white sublimate1 although not so copiously as the corresponding compounds of potash and soda4 ,this sublimate disappears when touched by the reduction flame1 while the oxidation flame gives the characteristic color of lithia4 ,,second ,,group4--,,the ,,alkaline ,,earths1 ,,baryta1 ,,strontia1 ,,lime1 ,,and ,,magnesia4 ,in the pure state1 the alkaline earths are caustic1 cause red litmus paper to become blue1 and are more or less soluble in water4 ,their sulphides are also soluble4 ,the carbonates and phosphates of the alkaline earths are insoluble in water4 ,by igniting the carbonates1 their carbonic acid is expelled1 and the alkaline earths are left in the caustic state4 ,the alkaline earths are not volatile1 and their organic salts are converted1 by ignition1 into carbonates4 7a47 ,baryta4 7,ba,o74--,this alkaline earth does not occur free in nature1 but combined with acids1 particularly with carbonic and sulphuric acids4 ,in the pure state1 baryta is of a greyish-white color1 presents an earthy appearance1 and is easily powdered4 ,when sparingly moistened with water1 it slakes1 becomes heated1 and forms a dry1 white powder4 ,with still more water it forms a crystalline mass1 the hydrate of baryta1 which is completely soluble in hot water4 ,pure baryta is infusible2 the hydrate fuses at a red heat1 without the loss of its hydratic water2 if caustic baryta is exposed for too great a length of time to the flame1 it absorbs water1 originated by the combustion1 and becomes a hydrate1 when it will melt4 ,salts of baryta1 formed with most acids1 are insoluble in water2 for instance1 the salts with sulphuric1 carbonic1 arsenic1 phosphoric1 and boracic acids4 ,the salts of baryta1 soluble in water1 are decomposed by ignition1 except the chloride4 ,carbonate of baryta loses its carbonic acid at a red heat1 becomes caustic1 and colors red litmus paper blue4 ,by exposing baryta or its compounds upon a platinum wire1 or a splinter of the substance held with the platinum tongs1 to the point of the blue flame1 a pale apple-green color is communicated to the external flame4 ,this color appears at first very pale1 but soon becomes more intense4 ,this color is most visible if the substance is operated with in small quantities4 ,the chloride of barium produces the deepest color4 ,this color is less intense if the carbonate or sulphate is used4 ,the presence of strontia1 lime1 or magnesia1 does not suppress the reaction of the baryta1 unless they greatly predominate4 ,when alcohol is poured over baryta or its salts1 and inflamed1 a feeble green color is communicated to the flame1 but this color should not be considered a characteristic of the salt4 ,baryta and its compounds give1 when fused with carbonate of soda upon platinum foil1 a clear bead4 ,fused with soda upon charcoal1 it is absorbed4 ,the sulphate fuses at first to a clear bead1 which soon spreads1 and is absorbed and converted while boiling into a hepatic mass4 ,if this mass is taken out1 placed upon a piece of polished silver and moistened with a little water1 a black spot of sulphide of silver is left after washing off the mass with water4 ,borax dissolves baryta and its compounds with a hissing noise1 as well in the flame of oxidation as in that of reduction4 ,there is formed a clear bead which1 with a certain degree of saturation1 is clear when cold1 but appears milk-white when overcharged1 and of an opal1 enamel appearance1 when heated intermittingly1 or with a vacillating flame1 that changes frequently from the oxidating to the reducing flame4 ,baryta and its compounds produce the same reactions with microcosmic salt4 ,baryta and its compounds fuse when exposed to ignition in the oxidizing flame4 ,moistened with the solution of nitrate of cobalt1 and heated in the oxidation flame1 it presents a bead1 colored from brick-red to brown1 according to the quantity used4 ,this color disappears when cold1 and the bead falls to a pale grey powder after being exposed awhile to the air4 ,when heated again1 the color does not appear until fusion is effected4 ,if carbonate of soda is fused upon platinum wire with so much of the sesquioxide of manganese that a green bead is produced1 this bead1 when fused with a sufficient quantity of baryta1 or its compounds1 after cooling1 will appear of a bluish-green1 or light blue color4 7b47 ,strontia 7,sr,o74--,strontia and its compounds are analogous to the respective ones of baryta4 ,the hydrate of strontia has the same properties as the hydrate of baryta1 except that it is less soluble in water4 ,the carbonate of strontia fuses a little at a red heat1 swells1 and bubbles up like cauliflower4 ,this produces1 in the blowpipe flame1 an intense and splendid light1 and now produces an alkaline reaction upon red litmus paper4 ,the sulphate of strontia melts in the oxidation flame upon platinum foil1 or upon charcoal1 to a milk-white globule4 ,this fuses upon charcoal1 spreads and is reduced to the sulphide1 which is absorbed by the charcoal4 ,it now produces the same reactions upon polished silver as the sulphate of baryta under the same conditions4 ,by exposing strontia and its compounds upon platinum wire1 or as a splinter with the platinum tongs1 to the point of the blue flame1 the external flame appears of an intense crimson color4 ,the deepest red color is produced by the chloride of strontium1 particularly at the first moment of applying the heat4 ,after the salt is fused1 the red color ceases to be visible in the flame1 by which it is distinguished from the chloride of lithium4 ,the carbonate of strontia swells up and produces a splendid white light1 while the external flame is colored of a fine purple-red4 ,the color produced by the sulphate of strontia is less intense4 ,the presence of baryta destroys the reaction of the strontia1 the flame presenting the light green color of the baryta4 ,if alcohol is poured over powdered strontia and inflamed1 the flame appears purple or deep crimson1 particularly if the fluid is stirred with a glass rod1 and when the alcohol is nearly consumed4 ,the insoluble salts of strontia do not produce a very intense color4 ,baryta does not prevent the reaction of the soluble salts of strontia1 unless it exists greatly in excess4 ,in the presence of baryta1 strontia can be detected by the following process3 mix some of the substance under examination with some pure graphite and water1 by grinding in an agate mortar4 ,place the mixture upon charcoal1 and expose it for a while to the reduction flame4 ,the substance becomes reduced to sulphide of barium and sulphide of strontium1 when it should be dissolved in hydrochloric acid4 ,the solution should be evaporated to dryness1 redissolved in a little water1 and enough alcohol added that a spirit of #hj per cent4 is produced4 ,inflame the spirit1 and if strontia is present1 the flame is tinged of a red color4 ,this color can be discerned more distinctly by moistening some cotton with this spirit and inflaming it4 ,if strontia or its compounds are fused with a green bead of carbonate of soda and sesquioxide of manganese1 as described under the head of baryta1 a bead of a brown1 brownish-green1 or dark grey color is produced4 ,carbonate of soda does not dissolve pure strontia4 ,the carbonate and sulphate of strontia melt with soda upon platinum foil to a bead1 which is milk-white when cold1 but fused upon charcoal they are absorbed4 ,strontia or its compounds produce with borax1 or microcosmic salt1 the same reactions as baryta4 ,when they are moistened with nitrate of cobalt1 and ignited in the oxidizing flame1 a black1 or grey infusible mass is produced4 7c47 ,lime1 ,oxide of ,calcium 7,ca,o74--,lime does not occur free in nature1 but in combination with acids1 chiefly the carbonic and sulphuric4 ,the phosphate occurs principally in bones4 ,the hydrate and the salts of lime are in their properties similar to those of the two preceding alkaline earths4 ,in the pure state1 the oxide of calcium is white2 it slakes1 produces a high temperature1 and falls into a white powder when sprinkled with a little water4 ,it is now a hydrate1 and has greatly increased in volume4 ,the hydrate of lime is far less soluble in water than either those of baryta or strontia1 and is less soluble in hot water than in cold4 ,lime1 its hydrate and sulphide of calcium1 have a strong alkaline reaction upon red litmus paper4 ,lime and its hydrate are infusible1 but produce at a strong red heat a very intense and splendid white light1 while the hydrate loses its water4 ,the carbonate of lime is also infusible1 but at a red heat the carbonic acid is expelled1 and the residue becomes caustic1 appears whiter1 and produces an intenser light4 ,the sulphate of lime melts with difficulty1 and presents the appearance of an enamelled mass when cold4 ,by heating it upon charcoal it fuses in the reducing flame1 and is reduced to a sulphide4 ,this has a strong hepatic odor1 and exerts an alkaline reaction upon red litmus paper4 ,by exposing lime1 or its compounds1 upon platinum wire--or as a small splinter of the mineral in the platinum tongs--to the point of the blue flame1 a purple color1 similar to that of lithia and strontia1 is communicated to the external flame1 but this color is not so intense as that produced by strontia1 and appears mixed with a slight tinge of yellow4 ,this color is most intense with the chloride of calcium1 while the carbonate of lime produces at first a yellowish color1 which becomes red1 after the expulsion of the carbonic acid4 ,sulphate of lime produces the same color1 but not so intense4 ,among the silicates of lime only the tablespar 7#c;,ca,o1 #b,si,o#c7 produces a red color4 ,fluorspar 7,ca,fl7 produces a red as intense as pure lime1 and fuses into a bead4 ,phosphate and borate of lime produce a green flame which is only characteristic of their acids4 ,the presence of baryta communicates a green color to the flame4 ,the presence of soda produces only a yellow color in the external flame4 ,if alcohol is poured over lime or its compounds and inflamed1 a red color is communicated to the flame4 ,the presence of baryta or soda prevents this reaction4 ,lime and its compounds do not dissolve much by fusion with carbonate of soda4 ,if this fusion is effected on charcoal1 the carbonate of soda is absorbed and the lime remains as a half-globular infusible mass on the charcoal4 ,this is what distinguishes lime from baryta and strontia1 and is a good method of separating the former from the latter4 ,lime and its compounds fuse with borax in the oxidizing and reducing flames to a clear bead1 which remains clear when cold1 but when overcharged with an excess or heated intermittingly1 the bead appears1 when cold1 crystalline and uneven1 and is not so milk-white as the bead of baryta or strontia1 produced under the same circumstances4 ,the carbonate of lime is dissolved with a peculiar hissing noise4 ,microcosmic salt dissolves a large quantity of lime into a clear bead1 which is milky when cold4 ,when the bead has been overcharged with lime1 by a less excess1 or by an intermittent flame1 we will perceive in the bead1 when cold1 fine crystals in the form of needles4 ,lime and its compounds form by ignition with nitrate of cobalt1 a black or greyish-black infusible mass4 7d47 ,magnesia 7,mg,o74--,magnesia occurs in nature in several minerals4 ,it exists in considerable quantity combined with carbonic1 sulphuric1 phosphoric1 and silicic acids1 etc4 ,magnesia and its hydrate are white and very voluminous1 scarcely soluble in hot or cold water1 and restores moistened red litmus paper to its original blue color4 ,magnesia and its hydrate are infusible1 the latter losing its water by ignition4 ,the carbonate of magnesia is infusible1 loses its carbonic acid at a red heat1 and shrinks a little4 ,it now exerts upon red litmus paper an alkaline reaction4 ,the sulphate of magnesia1 at a red heat1 loses its water and sulphuric acid1 is entirely infusible1 and gives now an alkaline reaction4 ,the artificial ,astrachanit 7,na,o1 ,,so#c ,mg,o1 ,,so#c #d;,,ho7 fuses easily4 ,when fused on charcoal1 the greater part of the sulphate of soda is absorbed1 and there remains an infusible mass4 ,magnesia and its compounds do not produce any color in the external flame1 when heated in the point of the blue flame4 ,the most of the magnesia minerals yield some water when heated in a glass tube closed at one end4 ,magnesia1 in the pure state1 or as the hydrate1 does not fuse with soda4 ,some of its compounds are infusible likewise with soda1 and swell up slightly1 while others of them melt with soda to a slightly opaque mass4 ,some few 7such as the borate of magnesia7 give a clear bead with soda1 though it becomes slightly turbid by cooling when saturated with magnesia1 and crystallizes in large facets4 ,magnesia and its compounds give beads with borax and microcosmic salt similar to those of lime4 ,by igniting magnesia or its compounds very strongly in the oxidizing flame1 moistening with nitrate of cobalt1 and re-igniting in the oxidation flame1 they present1 after a continued blowing1 a pale flesh-color1 which is more visible when cold4 ,it is indispensable that the magnesia compounds should be completely white and free of colored substances1 or the color referred to cannot be discerned4 ,in general the reactions of magnesia before the blowpipe are not sufficient1 and it will be necessary to confirm its presence or absence by aid of reagents applied in the wet way4 ,,third ,,group4--,,the ,,earths1 ,,alumina1 ,,glucina1 ,,yttria1 ,,thorina1 ,,and ,,zirconia4 ,the substances of this group are distinguished from the preceding by their insolubility in water1 in their pure or hydrated state--that they have no alkaline reaction upon litmus paper1 nor form salts with carbonic acid4 ,the earths are not volatile1 and1 in the pure state1 are infusible4 ,they cannot be reduced to the metallic state before the blowpipe4 ,the organic salts are destroyed by ignition1 while the earths are left in the pure state1 mixed with charcoal1 from the organic acids4 ,the most of their neutral salts are insoluble in water2 the soluble neutral salts change blue litmus paper to red1 and lose their acids when ignited4 7a47 ,alumina 7,al#b,o#c74--,this earth is one of our most common minerals4 ,it occurs free in nature in many minerals1 as sapphire1 etc42 or in combination with sulphuric acid1 phosphoric acid1 and fluorine1 and chiefly silicates4 ,pure alumina is a white crystalline powder1 or yellowish-white1 and amorphous when produced by drying the hydrate1 separated chemically from its salts4 ,alumina is quite unalterable in the fire2 the hydrate1 however1 losing its water at a low red heat4 ,the neutral salts of alumina1 with most acids1 are insoluble in water4 ,those soluble in it have an acid reaction upon litmus paper1 changing the blue into red4 ,the sulphates of alumina eliminate water when heated in a glass tube closed at one end4 ,by ignition1 sulphurous acid 7,,so#b7 is given off1 which can be recognized by its smell1 and by its acid reaction upon blue litmus paper1 when a small strip of it moistened is brought within the orifice of the tube2 an infusible residue is left in the tube4 ,the greater part of the alumina compounds give off water with heat2 the most of them are also infusible1 except a few phosphates and silicates4 ,pure alumina does not fuse with carbonate of soda4 ,the sulphates1 when exposed upon charcoal with soda to the reducing flame1 leave a hepatic residue4 ,the phosphates melt with a little soda1 with a hissing noise1 to a semi-transparent mass1 but they are infusible with the addition of soda1 and give only a tough mass4 ,this is the case1 likewise1 with the silicates of alumina4 ,fluoride of aluminium melts with carbonate of soda to a clear bead1 spreads by cooling1 and appears then milk-white4 ,borax dissolves the alumina compounds slowly in the oxidizing and reducing flames to a clear bead1 which is also clear when cold1 or heated intermittingly with a vacillating flame4 ,the bead is turbid1 as well in the heat as the cold1 when an excess of alumina is present4 ,when the alumina compound is added to excess in the powdered form1 the bead appears crystalline upon cooling1 and melts again with great difficulty4 ,alumina and its compounds are slowly dissolved in the microcosmic salt to a bead1 clear in both flames1 and when hot or cold4 ,when alumina is added to excess1 the undissolved portion appears semi-transparent4 ,alumina melts with bisulphate of potash into a mass soluble in water4 ,when the powdered alumina compounds are strongly ignited in the oxidizing flame1 then moistened with nitrate of cobalt1 and re-ignited in the oxidizing flame1 an infusible mass is left1 which appears1 when cooled1 of an intense blue color4 ,the presence of colored metallic oxides1 in considerable quantity1 will alter or suppress this reaction4 ,the silicates of the alkalies produce1 in a very strong heat1 or continued heat1 with nitrate of cobalt1 a pale blue color4 ,the blue color produced by alumina is only distinctly visible by daylight2 by candle-light it appears of a dirty violet color4 7b47 ,glucina4 7,g#b,o#c74--;,glucina only occurs in a few rare minerals1 in combination with silica and alumina4 ,it is white and insoluble in the pure state1 and its properties generally are similar to those of alumina4 ,the most of its compounds are infusible1 and yield water by distillation4 ,carbonate of soda does not dissolve glucina by ignition4 ,silicate of glucina melts with carbonate of soda to a colorless globule4 ,borax and microcosmic salt dissolve glucina and its compounds to a colorless bead which1 when overcharged with glucina1 or heated with the intermittent flame appears1 after cooling1 turbid or milk-white4 ,glucina yields1 by ignition with nitrate of cobalt1 a black1 or dark grey infusible mass4 7c47 ,yttria 7,,yo7 occurs only in a few rare minerals1 and usually in company with terbium and erbium4 ,its reactions before the blowpipe are similar to the preceding1 but for its detection in compounds it will be necessary to resort to analysis in the wet way4 7d47 ,zirconia 7,zr#b,o#c74--,this substance resembles alumina in appearance1 though it occurs only in a few rare minerals4 ,it is in the pure state infusible1 and at a red heat produces such a splendid and vivid white light that the eyes can scarcely endure it4 ,its other reactions before the blowpipe are analogous to glucina4 ,microcosmic salt does not dissolve so much zirconia as glucina1 and is more prone to give a turbid bead4 ,zirconia yields with nitrate of cobalt1 when ignited1 an infusible black mass4 ,to recognize zirconia in compounds we must resort to fluid analysis4 7e47 ,thorina 7,th,o74--,this is the rarest among the rare minerals4 ,in the pure state it is white and infusible1 and will not melt with the carbonate of soda4 ,borax dissolves thorina slowly to a colorless1 transparent bead1 which will remain so when heated with the intermittent flame4 ,if overcharged with the thorina1 the bead presents1 on cooling1 a milky hue4 ,microcosmic salt dissolves the thorina very tardily4 ,by ignition with nitrate of cobalt1 thorina is converted into an infusible black mass1 ,,class ,,ii4 ,,fourth ,,group4 ,,cerium1 ,,lanthanium1 ,,didymium1 ,,columbium1 ,,niobium1 ,,pelopium1 ,,titanium1 ,,uranium1 ,,vanadium1 ,,chromium1 ,,manganese4 ,the substances of this group cannot be reduced to the metallic state1 neither by heating them per se1 nor by fusing them with reagents4 ,they give by fusion with borax or microcosmic salt1 colored beads1 while the preceding groups give colorless beads4 7a47 ,cerium 7,ce74--,this metal occurs in the oxidated state in a few rare minerals1 and is associated with lanthanium and didymium1 combined with fluorine1 phosphoric acid1 carbonic acid1 silica1 etc4 ,when reduced artificially1 it forms a grey metallic powder4 7a47 ,protoxide of ,cerium 7,ce,o74--,it exists in the pure state as the hydrate1 and is of a white color4 ,it soon oxidizes and becomes yellow1 when placed in contact with the air4 ,when heated in the oxidation flame1 it is converted into the sesquioxide1 and then is changed into light brick-red color4 ,in the oxidation flame it is dissolved by borax into a clear bead1 which appears of an orange or red while hot1 but becomes yellow upon cooling4 ,when highly saturated with the metal1 or when heated with a fluctuating flame1 the bead appears enamelled as when cold4 ,in the reduction flame it is dissolved by borax to a clear yellow bead1 which is colorless when cold4 ,if too much of the metal exists in the bead1 it then appears enamelled when cooled4 ,microcosmic salt dissolves it1 in the oxidation flame1 to a clear bead1 which is colored dark yellow or orange1 but loses its color when cold4 ,in the reduction flame the bead is colorless when either hot or cold4 ,even if highly saturated with the metal1 the bead remains colorless when cold4 ,by fusing it with carbonate of soda upon charcoal in the reduction flame1 the soda is absorbed by the charcoal1 while the protoxide of the metal remains as a light grey powder4 7,b47 ,sesquioxide of ,cerium 7,ce#b,o#c74--,this oxide1 in the pure state1 is a red powder4 ,when heated with hydrochloric acid1 it produces chlorine gas1 and is dissolved to a salt of the protoxide4 ,it is not affected by either the flame of oxidation or of reduction2 when fused with borax or microcosmic salt1 it acts like the protoxide4 ,it does not fuse with soda upon charcoal4 ,in the reduction flame it is reduced to the protoxide1 which remains of a light grey color1 while the soda is absorbed by the charcoal4 7b47 ,lanthanium 7,la47--,this metal is invariably associated with cerium4 ,it presents1 in its metallic state1 a dark grey powder1 which by compression acquires the metallic lustre4 ,the oxide of lanthanium 7,la,o7 is white1 and its salts are colorless4 ,heated upon charcoal1 it does not change either in the oxidation flame or that of reduction4 ,with borax1 in the flame of oxidation or reduction1 it gives a clear colorless bead4 ,this bead1 if saturated1 and when hot1 presents a yellow appearance1 but is clouded or enamelled when cold4 ,with microcosmic salt the same appearance is indicated4 ,it does not fuse with carbonate of soda1 but the soda is absorbed by the charcoal1 while the oxide remains of a grey color4 7c47 ,didymium 7,d74--,this metal occurs only in combination with the preceding ones1 and it is therefore1 like them1 a rare one4 ,oxide of ,didymium 7,,do74--,this oxide is of a brown color1 while its salts present a reddish-violet or amethyst color4 ,the oxide is infusible in the oxidation flame1 and in that of reduction it loses its brown color and changes to grey4 ,with borax in the oxidation flame1 it fuses to a clear dark red or violet bead1 which retains its clearness when highly saturated with the oxide1 or if heated with a fluctuating flame4 ,the reactions with microcosmic salt are the same as with borax4 ,it does not melt with carbonate of soda upon charcoal1 but the oxide remains with a grey color1 while the soda is absorbed by the charcoal4 7d47 ,columbium1 7,tantalum--,ta74--,this rare metal occurs quite sparingly in the minerals tantalite1 yttrotantalite1 etc41 as columbic acid4 ,in the metallic state1 it presents the appearance of a black powder1 which1 when compressed1 exhibits the metallic lustre4 ,when heated in the air it is oxidized into columbic acid1 and is only soluble in hydrofluoric acid1 yielding hydrogen4 ,it is oxidized by fusion with carbonate of soda or potash4 ,columbic ,acid 7,ta#b,o#c7 is a white powder1 and is infusible4 ,when heated in the flame of oxidation or reduction1 it appears of a light yellow while hot1 but becomes colorless when cold4 ,with borax1 in the flames of oxidation and reduction1 it fuses to a clear bead1 which appears by a certain degree of saturation1 of a yellow color so long as it continues hot1 but becomes colorless when cold4 ,if overcharged1 or heated with an intermittent flame1 it presents an enamel white when cool4 ,it melts with microcosmic salt quite readily in both of the flames1 to a clear bead1 which appears1 if a considerable quantity of columbic acid be present1 of a yellow color while hot1 but colorless when cold1 and does not become clouded if the intermittent flame be applied to it4 ,with carbonate of soda it fuses with effervescence to a bead which spreads over the charcoal4 ,melted with more soda1 it becomes absorbed by the charcoal4 ,it yields1 moistened with a solution of nitrate of cobalt1 and exposed to the oxidation flame after continued blowing1 an infusible mass1 presenting while hot a light grey color1 but after being cooled that of a light red1 similar to the color presented by magnesia under the same circumstances4 ,but if there be some alkali mixed with it1 a fusion at the edges will be manifest1 and it will yield by cooling a bluish-black mass4 7e47 ,niobium 7,ni74--,this metal occurs as niobic acid in columbite 7tantalite74 ,niobic acid is in its properties similar to columbic acid4 ,it is white and infusible4 ,by heating it either in the flames of reduction or oxidation1 it presents as long as it continues hot1 a greenish-yellow color1 but becomes white when cool4 ,borax dissolves it in the oxidation flame quite readily to a clear bead1 which1 with a considerable quantity of niobic acid1 is yellow when hot1 but transparent and colorless when cold4 ,a saturated bead is clear when either hot or cold1 but becomes opaque when heated intermittingly4 ,in the flame of reduction1 borax is capable of dissolving more of the niobic acid1 so that a bead overcharged and opaque in the oxidation flame appears quite clear when heated in the flame of reduction4 ,a bead overcharged in the flame of reduction1 appears by cooling dim and bluish-grey4 ,microcosmic salt dissolves in the flame of oxidation a great quantity of it to a clear bead1 which is yellow while hot1 but colorless when cold4 ,in the flame of reduction1 and in presence of a considerable quantity of niobic acid1 the bead appears while hot of a light dirty blue color1 and when cold1 of a violet hue2 but by the addition of more niobic acid1 the bead1 when hot1 is of a dirty dark blue color1 and when cold1 of a transparent blue4 ,in the presence of the oxides of iron1 the bead is1 while hot1 of a brownish-red color1 but changing when cool to a dark yellow4 ,this acid fuses with an equal quantity of carbonate of soda upon charcoal1 to a bead which spreads very quickly1 and is then infusible4 ,when fused with still more soda1 it is absorbed4 ,when moistened with nitrate of cobalt1 and heated in the flame of oxidation1 it yields an infusible mass which appears grey when hot1 and dirty green when cold2 but if the heat has been too strong1 it is fused a little at the edges1 which present a dark bluish-grey color4 ,pelopium 7,pe74--,this metal occurs as an acid in the mineral columbite 7tantalite71 and is very similar to the two preceding metals4 7f47 ,pelopic ,acid 7,pe,o#c74--,this acid is white1 and appears yellow when heated1 but resumes its white color when cold4 ,borax dissolves it in the oxidation flame to a clear colorless bead1 which appears1 when overcharged and heated intermittingly1 enamel-white when cold4 ,this is likewise the case in the flame of reduction1 but when overcharged the color is light grey1 when the bead is cooled4 ,microcosmic salt dissolves it in the flame of oxidation1 to a clear yellow bead1 which loses its color when cold4 ,in the reduction flame1 when the bead is highly saturated1 a violet-brown color is produced4 ,in presence of the oxides of iron1 the reactions are like those of niobic acid4 ,with carbonate of soda1 the reactions are similar to those of niobic acid4 ,by heating with nitrate of cobalt1 it yields a light grey infusible mass4 7g47 ,titanium 7,ti74--,this metal occurs occasionally in the slags of iron works1 in the metallic state1 as small cubical crystals of a red color4 ,it is a very hard metal1 and very infusible4 ,titanic acid occurs in nature crystallized in anatase1 arkansite1 brookite1 and rutile4 ,titanium is harder than agate1 entirely infusible1 and loses only a little of its lustre1 which can be regained by fusion with borax4 ,it does not melt with carbonate of soda1 borax1 or microcosmic salt1 and is insoluble in every acid except the hydrofluoric4 ,by ignition with saltpetre it is converted into titanic acid1 which combines with the potassium1 forming the titanate of potassium4 ,titanic ,acid 7,ti,o#b7 is white1 insoluble1 and1 when heated1 it appears yellow while hot1 but resumes upon cooling its white color4 ,borax dissolves it in the oxidation flame to a clear yellow bead1 which when cool is colorless4 ,when overcharged1 or heated with the intermitting flame1 it is enamel-white after being cooled4 ,in the reduction flame1 the bead appears yellow1 if the acid exists in small quantity1 but if more be added1 then it is of an orange1 or dark yellow1 or even brown4 ,the saturated bead1 when heated intermittingly1 appears when cold of an enamelled blue4 ,by addition of the acid1 and by heating the bead on charcoal in the reduction flame1 it becomes dark yellow while hot1 but dark blue1 or black and opaque when cold4 ,this bead appears1 when heated intermittingly1 of a light blue1 and when cold1 enamelled4 ,microcosmic salt fuses with it in the oxidation flame to a clear colorless bead1 which appears yellow only in the presence of a quantity of titanic acid1 though by cooling it loses its color4 ,in the reduction flame this bead exhibits a yellow color when hot1 but is red while cooling1 and when cold of a beautiful bluish-violet4 ,if the bead is overcharged1 the color becomes so dark that the bead appears opaque1 though not presenting an enamel appearance4 ,by heating the bead again in the oxidation flame the color disappears4 ,the addition of some tin promotes the reduction4 ,if the titanic acid contains oxide of iron1 or if some is added1 the bead appears1 when cold1 brownish-yellow1 or brownish-red4 ,by fusion with carbonate of soda1 titanic acid is dissolved with effervescence to a clear dark yellow bead1 which crystallizes by cooling1 whereby so much heat is eliminated1 that the bead1 at the instant of its crystallization1 glows with great brightness4 ,a reduction to a metal cannot1 however1 be effected4 ,by ignition with a solution of nitrate of cobalt in the oxidation flame1 it yields an infusible yellowish-green mass4 7h47 ,uranium 7,u74--,this rare metal occurs in the form of protoxide along with other oxides1 in the mineral pitch-blende2 as peroxide in uranite and uran-mica1 associated with phosphoric acid and lime4 ,in the metallic state it presents the appearance of a dark grey mass1 which is infusible1 and remains unchanged when under water1 or when exposed to dry air1 but1 when heated in the oxidation flame1 it becomes oxidized1 with lively sparkling1 to a dark green mass1 composed of the protoxide and peroxide4 ,the protoxide of uranium 7,,uo7 is black1 uncrystalline1 or forms a brown powder4 ,when exposed to heat it is converted partially into peroxide1 when it has a dark green color4 ,the peroxide of uranium 7,u#b,o#c7 is of an orange color1 while its hydrate is of a fine yellow color1 and in the form of a powder4 ,the salts are yellow4 ,by heating it in the oxidation flame1 it acquires a dark green color1 and is partly reduced to protoxide4 ,in the reduction flame it presents a black appearance1 and is there completely reduced to protoxide4 ,borax dissolves it in the oxidation flame to a clear dark yellow bead1 which is colorless when cold1 if the metal is not present in great quantity4 ,if more of the metal1 or peroxide1 be added1 the bead changes to orange when hot1 and light yellow when cold4 ,when heated with the intermittent flame1 it requires a large quantity of the peroxide to produce an enamel appearance in the cooled bead4 ,in the flame of reduction the bead becomes of a dirty green color1 being partly reduced to protoxide1 and appears1 with a certain degree of saturation1 black1 when heated intermittingly1 but never enamelled4 ,the bead appears on charcoal1 and with the addition of tin1 of a dark green color4 ,it fuses with microcosmic salt in the oxidation flame to a clear yellow bead1 which is greenish-yellow when cold4 ,in the reduction flame it produces a beautiful green bead1 which increases when cold4 ,when fused upon charcoal with the addition of tin1 its color is darker4 ,carbonate of soda does not dissolve it1 although with a very small portion of soda it gives indications of fusion1 but with still more of the soda it forms a yellow1 or light-brown mass1 which is absorbed by the charcoal1 but it is not reduced to the metallic state4 7i47 ,vanadium 7,v74--,this very rare mineral is found in small quantity in iron-ores1 in ,sweden1 and as vanadic acid in a few rare minerals4 ,the metal presents the appearance of an iron-grey powder1 and sometimes that of a silver-white mass4 ,it is not oxidized either by air or water1 and is infusible4 ,vanadic ,acid 7,,vo#c7 fuses upon platinum foil to a deep orange liquid1 which becomes crystalline after cooling4 ,when fused upon charcoal1 one part of it is absorbed1 while the rest remains upon the charcoal and is reduced to protoxide similar in appearance to graphite4 ,a small portion of it fuses with borax in the oxidation flame to a clear colorless bead1 which appears1 with the addition of more vanadic acid1 of a yellow color1 but changes to green when cold4 ,in the reduction flame the bead is brown while hot1 but changes1 upon cooling1 to a beautiful sapphire-green4 ,at the moment of crystallization1 and at a degree of heat by which at daylight no glowing of the heated mass is visible it begins to glow again4 ,the glow spreads from the periphery to the centre of the mass1 and is caused by the heat liberated by the sudden crystallization of the mass4 ,it now exhibits an orange color1 and is composed of needle crystals in a compact mass4 ,microcosmic salt and vanadic acid fuse in the oxidation flame to a dark yellow bead which1 upon cooling1 loses much of its color4 ,in the reduction flame the bead is brown while hot1 but1 upon cooling1 acquires a beautiful green color4 ,vanadic acid fuses with carbonate of soda upon charcoal1 and is absorbed4 7k47 ,chromium 7,cr7 occurs in the metallic state only in a very small quantity in meteoric iron1 but is frequently found in union with oxygen1 as oxide in chrome iron ore1 and as chromic acid in some lead ores4 ,in the metallic state it is of a light grey color1 with but little metallic lustre1 very hard1 and not very fusible4 ,acids do not act upon it1 except the hydrofluoric2 fused with nitre1 it forms chromate of potassa4 ,it is unaltered in the blowpipe flame4 ,sesquioxide of ,chromium 7,cr#b,o#c74--,this oxide forms black crystals of great hardness1 and is sometimes seen as a green powder4 ,its hydrate 7,cr#b,o#c #f;,,ho7 is of a bluish-grey color4 ,it forms with acids two classes of isomeric salts1 some of which are of a green color1 and the others violet-red or amethyst4 ,the neutral and soluble salts have an acid reaction upon blue litmus paper1 and are decomposed by ignition4 ,sesquioxide of chromium in the oxidation and reduction flames is unchangable4 ,when exposed to heat1 the hydrate loses its water1 and gives a peculiarly beautiful flame4 ,in the oxidation flame borax dissolves the sesquioxide of chromium slowly to a yellow bead 7chromic acid7 which is yellowish green when cold4 ,upon the addition of more of the oxide1 the bead is dark red while hot1 but changes to green as it becomes cold4 ,in the reduction flame the bead is of a beautiful green color1 both while hot and when cold4 ,it is here distinguished from vanadic acid1 which gives a brownish or yellow bead while hot4 ,with microcosmic salt it fuses in the oxidation flame to a clear yellow bead1 which appears1 as it cools1 of a dirty-green1 color1 but upon being cool is of a fine green color4 ,if there be a superabundance of the oxide1 so that the microcosmic salt cannot dissolve it1 the bead swells up1 and is converted into a foamy mass1 in consequence of the development of gases4 ,in the reduction flame it fuses to a fine green bead4 ,the addition of a little tin renders the green still deeper4 ,sesquioxide of chromium fuses with carbonate of soda upon platinum foil to a brown or yellow bead1 which1 upon cooling1 appears of a lighter color and transparent 7chromate of sodium74 ,when fused with soda upon charcoal1 the soda is absorbed1 and the green oxide is left upon it1 but is never reduced to the metallic state4 ,chromic ,acid 7,cr,o#c7 crystallizes in the form of deep ruby red needles4 ,it is decomposed into sesquioxide and oxygen when heated4 ,this decomposition is attended with a very lively emission of light1 but this is not the case if the chromic acid has been attained by the coperation of an aqueous solution1 unless the reduction is effected in the vapor of ammonia4 ,before the blowpipe chromic acid produces the same reactions as the sesquioxide4 7l47 ,manganese 7,mn74--,this metal occurs in considerable abundance1 principally as oxides1 less frequently as salts1 and sometimes in combination with sulphur and arsenic4 ,it is found in plants1 and passes with them into the animal body4 ,in the metallic state1 it is found frequently in cast iron and steel4 ,it is a hard1 brittle metal1 fusible with difficulty1 and of a light grey color4 ,it tarnishes upon exposure to the air and under water1 and falls into a powder4 ,protoxide of ,manganese exists as a green powder2 as hydrate separated by caustic alkalies1 it is white1 but oxidizes very speedily upon exposure to the air4 ,the protoxide is the base of the salts of manganese4 ,these salts1 which are soluble in water1 are decomposed when heated in the presence of the air--except the sulphate 7,mn,o1 ,,so#c71 but if the latter is exposed to ignition for awhile1 it then ceases to be soluble in water1 or at least only sparingly so4 ,sesquioxide of ,manganese 7,mn#b,o#c7 ,occurs very sparingly in nature as small black crystals 7,braunite7 which give1 when ground1 a brown powder4 ,when prepared by chemical process1 it is in the form of a black powder4 ,the hydrate occurs sometimes in nature as black crystals 7manganite74 ,by digestion with acids1 it is dissolved into salts of the protoxide4 ,with hydrochloric acid1 it yields chlorine4 ,the prot-sesquioxide of manganese 7,mn,o ,mn#b,o#c7 occurs sometimes in black crystals 7hausmannite74 ,prepared artificially1 it is in the form of a brown powder4 ,peroxide of ,manganese 7,mn,o#b7 occurs in considerable abundance as a soft black amorphous mass1 or crystallized as pyrolusite1 also reniform and fibrous4 ,it is deprived of a part of its oxygen when exposed to ignition4 ,it eliminates a considerable quantity of chlorine from hydrochloric acid1 and is thereby converted into chloride of manganese 7,cl,mn74 ,most of the manganese compounds which occur in nature yield water when heated in a glass tube closed at one end4 ,the sesquioxide and peroxide give out oxygen when strongly heated1 which can be readily detected by the increased glow which it causes1 if a piece of lighted wood or paper is brought to the mouth of the tube4 ,the residue left in the tube is a brown mass 7,mn,o ,mn#b,o#c74 ,when exposed to ignition with free access of air1 all manganese oxides are converted into 7,mn,o ,mn#b,o#c71 but without fusion4 ,such1 at least1 is the statement of some of the ,german chemists1 although it will admit perhaps of further investigation4 ,manganese oxides fuse with borax in the oxidation flame to a clear and intensely colored bead1 of a violet hue while hot1 but changing to red as it cools4 ,if a considerable quantity of the oxide is added1 the bead acquires a color so dark as to become opaque4 ,if such be the case1 we have to press it flat1 by which its proper color will become manifest4 ,in the reduction flame the bead is colorless4 ,a very dark colored bead must be fused upon charcoal with the addition of some tin4 ,the bead must be cooled very suddenly1 for if it cools too slowly1 it then has time to oxidize again4 ,this may be effected by pushing it off the platinum wire1 or the charcoal1 and pressing it flat with the forceps4 ,the oxides of manganese fuse with microcosmic salt in the oxidation flame1 to a clear brownish-violet bead1 which appears reddish-violet while cooling4 ,this bead does not become opaque when overcharged with manganese4 ,as long as it is kept in fusion a continued boiling or effervescence takes place1 produced by the expulsion of oxygen1 in consequence of the fact that the microcosmic salt cannot dissolve much sesquioxide1 while the rest is reduced to protoxide1 is re-oxidated1 and instantly again reduced4 ,if the manganese is present in such a minute quantity as not to perceptibly tinge the bead1 the color may be made to appear by the contact of a crystal of nitre while hot4 ,the bead foams up upon the addition of the nitre1 and the foam appears1 after cooling1 of a rose-red or violet color4 ,in the reduction flame the bead sometimes becomes colorless4 ,the oxides of manganese fuse with carbonate of soda upon platinum foil or wire1 to a clear green bead1 which appears bluish-green and partially opaque when cold 7manganate of soda ,na,o ,mn,o#c74 ,a very minute trace of manganese will produce this green color4 ,the oxides of manganese cannot be reduced upon charcoal with carbonate of soda before the blowpipe4 ,the soda is absorbed1 and 7,mn,o ,mn#b,o#c7 is left4 ,,group ,,fifth4--,,iron1 ,,cobalt1 ,,nickel4 ,the oxides of this group are reduced to the metallic state when fused with carbonate of soda upon charcoal in the reduction flame4 ,metals when thus reduced form powders1 are not fusible or volatile in the blowpipe flame1 but they are attracted by the magnet4 ,furthermore1 these oxides are not dissolved by carbonate of soda in the oxidation flame1 but they produce colored beads with borax and microcosmic salt4 7a47 ,iron4--,it occurs in great abundance in nature4 ,it is found in several places in ,america in the metallic state1 and it likewise occurs in the same state in meteors4 ,it occurs chiefly as the oxide 7red hematite1 brown hematite1 magnetic oxide1 etc471 and frequently in combination with sulphur4 ,iron also forms a constituent of the blood4 ,metallic iron is of a grey color1 and presents the metallic lustre vividly when polished4 ,it is very ductile1 malleable1 and tenacious4 ,it is very hard at common temperatures1 but soft and yielding at a red heat4 ,in dry and cold air1 iron does not oxidize1 but when the air is dry and moist1 it oxidizes rapidly4 ,this likewise takes place with great rapidity when the metal is heated to redness4 ,when submitted to a white heat iron burns with brilliant scintillations4 ,protoxide of ,iron 7,fe,o74--,this oxide does not occur pure in nature1 but in union with the peroxide of iron and other substances4 ,it presents the form of a black powder1 and has some metallic lustre1 is brittle1 and fuses at a high temperature to a vitreous looking mass4 ,it is attracted by the magnet1 and of course is susceptible of becoming magnetic itself4 ,it forms with water a hydrate1 but this passes so rapidly into a state of higher oxidation1 that it is difficult to keep it in the pure state4 ,magnetic ,oxide of ,iron 7,fe,o ,fe#b,o#c74--,this peculiar oxide is of a dark color1 and is magnetic1 so that tacks or small nails adhere to it when brought in contact with it4 ,it is the variety of the oxide termed loadstone4 ,it is found frequently crystallized in octahedrons in ,scandinavia and other places4 ,magnetic oxide of iron is produced when red-hot iron is hammered4 ,sesquioxide of ,iron 7,fe#b,o#c74--,this oxide is found native in great abundance as red hematite and specular iron1 crystallized in the rhombic form4 ,in the crystalline state it is of a blackish-grey color1 and possessed of the metallic lustre4 ,when powdered1 it forms a brownish-red mass4 ,when artificially prepared1 it presents the appearance of a blood-red powder4 ,it is not magnetic1 and has less affinity for acids than the protoxide4 ,its hydrate is found native as brown hematite4 ,by exposing the peroxide of iron to the oxidation flame1 it is not acted upon1 but in the reduction flame it becomes reduced to the magnetic oxide4 ,the oxides of iron are dissolved by borax in the oxidation flame to a clear dark-yellow or dark-red bead1 which appears lighter while cooling1 and yellowish when cold4 ,in the presence of a very small quantity of iron1 the bead appears colorless when cold4 ,if the iron is increased1 the bead is opaque while cooling1 and of a dirty dark-yellow color when cold4 ,in the reduction flame1 and fused upon platinum wire1 the bead appears dark green 7,fe,o ,fe#b,o#c74 ,by the addition of some tin1 and fused upon charcoal1 the bead appears bluish-green1 or not unlike that of sulphate of iron4 ,microcosmic salt dissolves the oxides of iron in the oxidation flame to a clear bead1 which1 by the addition of a considerable quantity of iron1 becomes of an orange color while hot1 but gets lighter while cooling1 presenting finally a greenish hue1 and gradually becoming lighter1 till1 when cold1 it is colorless4 ,if the iron is increased1 the hot bead presents a dark red color1 but while cooling a brownish-red1 which changes to a dirty-green1 and1 when cold1 to a brownish-red color4 ,the decrease of the color during the transition from the hot to the cold state is still greater in the bead formed by the microcosmic salt4 ,in the reduction flame no change is visible if the quantity of iron be small4 ,by the addition of more iron1 the hot bead appears red1 and while cooling1 changes to yellow1 then green1 and1 when cold1 is of a dull red4 ,by fusing the bead on charcoal with a small addition of tin1 it exhibits1 while cooling1 a bluish-green color1 but1 when cold1 is colorless4 ,the oxides of iron are not dissolved in the oxidation flame by fusion with carbonate of soda4 ,by ignition with soda upon charcoal in the reduction flame1 they are absorbed and reduced to the metallic state4 ,cut out this portion of the charcoal2 grind it with the addition of some water in an agate mortar1 for the purpose of washing off the carbon particles1 when the iron will remain as a grey magnetic powder4 7b47 ,cobalt 7,co7 occurs in combination with arsenic and sulphur1 and associated with nickel and iron4 ,it is found occasionally in combination with selenium1 and there are a traces of it in meteoric iron4 ,in the metallic state it is of a light1 reddish-grey color1 rather brittle1 and only fusible at a strong white heat2 at common temperatures it is unalterable by air or water4 ,at a red heat1 it oxidizes slowly and decomposes water2 at a white heat it burns with a red flame4 ,cobalt is soluble in dilute sulphuric or hydrochloric acid by the aid of heat1 whereby hydrogen is eliminated4 ,these solutions have a fine red color4 ,protoxide of ,cobalt 7,co,o74--,it is an olive-green powder1 but1 by exposure to the air1 it becomes gradually brown4 ,its hydrate is a rich red powder4 ,the solution of its salts is red1 but the aqueous solution is often blue4 ,when heated in the oxidation flame1 the protoxide is converted into the black proto-sesquioxide 7,co,o ,co#b,o#c74 ,in the reduction flame it shrinks and is reduced without fusion to the metallic state4 ,it is now attracted by the magnet and acquires lustre by compression4 ,borax dissolves it in the oxidation flame1 and produces a clear1 intensely colored blue bead1 which remains transparent and of the same beautiful blue when cold4 ,this blue is likewise manifest even if the bead be heated intermittingly4 ,if the cobalt exists in considerable quantity1 the color of the bead is so intense as to appear almost black4 ,this reaction of cobalt is so characteristic and sensitive that it can detect a minute trace4 ,with microcosmic salt the same reaction is exhibited1 but not so sensitive1 nor is the bead so intensely colored when cold as that with borax4 ,by fusion with carbonate of soda upon a platinum wire1 with a very small portion of cobalt1 a bright red colored mass is produced which appears grey1 or slightly green when cold4 ,by fusion upon platinum foil the fused portion floats down from the sides1 and the foil is coated around the undissolved part1 with a thin1 dark-red sublimate4 ,when fused upon charcoal1 and in the reduction flame1 it is reduced with soda to a grey powder1 which is attracted by the magnet1 and exhibits the metallic lustre by compression4 ,sesquioxide of ,cobalt 7,co#b,o#c74--;,it is a dark brown powder4 ,its hydrate 7#b;,,ho ,co#b,o#c7 is a brown powder4 ,it is soluble only in acetic acid as the acetate of the sesquioxide4 ,all other acids dissolve its salts to protoxide1 the hydrochloric acid producing chloric gas4 ,by ignition in the oxidation flame1 it is converted into the proto-sesquioxide 7,co,o ,co#b,o#c7 and produces with reagents before the blowpipe the same reactions as the protoxide4 7c47 ,nickel 7,ni74--,this metal occurs invariably associated with cobalt1 and in analogous combinations1 chiefly as the arsenical nickel4 ,in the metallic state it is greyish1 silver-white1 has a high lustre1 is hard1 and malleable both cold and hot4 ,at common temperatures1 it is unalterable either in dry or moist air4 ,when ignited1 it tarnishes4 ,it is easily dissolved by nitric acid1 but very slowly by dilute sulphuric or hydrochloric acid1 producing hydrogen4 ,protoxide of ,nickel 7,ni,o74--,it is in the form of small greyish-black octahedrons1 or a dark1 greenish-grey powder4 ,its hydrate is a green powder4 ,both are unalterable in the air1 and are soluble in nitric1 sulphuric1 and hydrochloric acids1 to a green liquid4 ,the protoxide is the base of the salts of nickel1 which in the anhydrous state are yellow1 and when hydrated are green4 ,the soluble neutral salts change blue litmus paper to red4 ,by ignition in the oxidation flame1 protoxide of nickel is unaltered4 ,in the reduction flame and upon charcoal1 it becomes reduced1 and forms a grey adherent powder1 which is infusible1 and presents the metallic lustre by compression1 and is magnetic4 ,borax dissolves it in the oxidation flame very readily to a clear bead1 of a reddish-violet or dark yellow color1 but yellow or light red when cold4 ,if there is but a small quantity of the oxide present1 it is colorless4 ,if more of the oxide be present1 the bead is opaque and dark brown1 and appears1 while cooling1 transparent and dark red4 ,by the addition of a salt of potassa 7the nitrate or carbonate7 a blue or a dark purple colored bead is produced4 ,the borax bead1 in the reduction flame1 is grey1 turbid1 or completely opaque from the reduced metallic particles4 ,after a continued blast1 the bead becomes colorless1 although the particles are not fused4 ,if the nickel contains cobalt1 it will now be visible with its peculiar blue color4 ,upon charcoal1 and by the addition of some tin1 the reduction of the oxide of nickel is easily effected1 while the reduced nickel fuses with the tin4 ,the oxide of nickel is dissolved by microcosmic salt in the oxidation flame to a clear bead1 which appears reddish while hot1 but yellow and sometimes colorless when cooling4 ,if a considerable quantity of nickel be present the heated bead is of a brown color1 but orange when cooled4 ,in the reduction flame1 and upon platinum wire1 the color of the bead is orange when cold2 but upon charcoal1 and with the addition of a little tin1 the bead appears grey and opaque4 ,after being submitted to the blowpipe flame all the nickel is reduced1 and the bead becomes colorless4 ,carbonate of soda does not affect it in the oxidation flame1 but in the reduction flame and upon charcoal1 it is absorbed and reduced1 and remains1 after washing off the carbon1 as a white metallic powder1 which is infusible1 and has a greater attraction for the magnet than iron4 ,sesquioxide of ,nickel 7,ni#b,o#c74--;,it is in the form of a black powder1 and does not combine with other substances1 unless it is reduced to the protoxide4 ,it exhibits before the blowpipe the same behavior as the protoxide4 ,,group ,,sixth4--,,zinc1 ,,cadmium1 ,,antimony1 ,,tellurium4 ,the substances of this group can be reduced upon charcoal by fusion with carbonate of soda1 but the reduced metals are volatilized1 and cover the charcoal with sublimates4 7a47 ,zinc 7,zn74--,this metal is found in considerable abundance1 but never occurs in the pure metallic state1 but in combination with other substances1 chiefly as sulphide in zinc blende1 as carbonate in calamine1 and as the silicate in the kieselzinc ore2 also1 with sulphuric acid1 the vitriol of zinc4 ,zinc is of a bluish-white color and metallic lustre1 is crystalline and brittle when heated #djj;,f41 but malleable and ductile between #bjj and #cjj4 ,it will not oxidize in dry air1 but tarnishes if exposed to air containing moisture1 first becomes grey1 and then passes into the white carbonate4 ,it decomposes in water at a glowing heat4 ,it is dissolved by diluted acids1 while hydrogen is eliminated4 ,it melts at about #gge1 and distills when exposed to a white heat in a close vessel4 ,when heated over #ajjj in the open air1 it takes fire1 and burns with a bluish-white light1 and with a thick white smoke of oxide of zinc4 ,oxide of ,zinc 7,zn,o74--,in the pure state1 oxide of zinc is a white powder1 infusible1 and not volatile4 ,it is readily soluble in acids after being heated strongly4 ,its soluble neutral salts1 when dissolved in water1 change blue litmus paper to red4 ,its salts1 with organic acids1 are decomposed by ignition1 and the carbonate of zinc remains4 ,the oxide of zinc turns yellow by being ignited in the oxidation flame1 but it is only visible by daylight2 this color changes to white when cold4 ,it does not melt1 but produces a strong light1 and it is not volatile4 ,it disappears gradually in the flame of reduction1 while a white smoke sublimates upon the charcoal4 ,this sublimate is yellow while hot1 but changes to white when cold4 ,the cause of this is1 that the oxide is reduced1 is volatilized1 and re-oxidized1 by going through the external flame in the form of a metallic vapor4 ,borax dissolves oxide of zinc in the flame of oxidation easily to a clear bead1 which is yellow while hot1 and colorless when cold4 ,the bead becomes1 by the addition of more oxide1 enamelled1 while cooling4 ,if the bead is heated with the intermittent flame1 it is milk-white when cold4 ,when heated in the flame of reduction upon platinum wire1 the bead at first appears opaque1 and of a greyish color1 but becomes clear again after a continued blast4 ,when heated upon charcoal in the reduction flame1 it is reduced to a metal2 but1 at the same moment1 is volatilized1 and sublimes as oxide of zinc upon the charcoal1 about one line's distance from the assay4 ,this is likewise the case with the microcosmic salt1 except that it is more easily volatilized in the reduction flame4 ,carbonate of soda does not dissolve the oxide of zinc in the flame of oxidation4 ,in the reduction flame and upon charcoal1 the oxide of zinc is reduced to the metallic state1 and is volatilized with a white vapor of the zinc oxide1 which sublimes on the charcoal and exhibits a yellow color while hot1 and which changes to white when cold4 ,by a strong heat the reduced zinc burns with a white flame4 ,moistened with a solution of cobalt oxide1 and heated strongly in the flame of oxidation1 zinc oxide becomes of a yellowish-green color while hot1 and changes to a beautiful green color when cold4 7b47 ,cadmium 7,cd74--,this is one of the rare metals4 ,it occurs in combination with sulphur in greenockite1 and in some ores of zinc4 ,it was detected first in the year #ahah1 and presents itself as a tin-white metal of great lustre1 and susceptible of a fine polish4 ,it has a fibrous structure1 crystallizes easily in regular octahedrons1 presenting often the peculiar arborescent appearance of the fern4 ,it is soft1 but harder and more tenacious than tin2 it can be bent1 filed1 and easily cut3 it imparts to paper a color like that of lead4 ,it is very malleable and ductile1 and can be hammered into thin leaves4 ,it is easily fused1 and melts before it glows 7#dej74 ,at a temperature not much over the boiling point of mercury1 it begins to boil1 and distills1 the vapor of the metal possessing no peculiar odor4 ,it is unalterable in the air for a long time1 but at length it tarnishes and presents a greyish-white1 half metallic color4 ,this metal easily takes fire when heated in the air1 and burns with a brownish-yellow vapor1 while it deposits a yellow sublimate upon surrounding bodies4 ,it is easily soluble in acids with the escape of hydrogen1 the solutions being colorless4 ,its salts1 soluble in water1 are decomposed by ignition in free air4 ,its soluble neutral salts change blue litmus paper to red4 ,the salts1 insoluble in water1 are readily dissolved in acids4 ,oxide of ,cadmium 7,cd,o74--,this oxide is of a dark orange color4 ,it does not melt1 and is not volatile1 not even at a very high temperature4 ,its hydrate is white1 loses in the heat its hydratic water1 and absorbs carbonic acid from the air when it is kept in open vessels4 ,cadmium oxide is unaltered when exposed upon platinum wire in the flame of oxidation4 ,when heated upon charcoal in the flame of reduction it disappears in a very short time1 while the charcoal is coated with a dark orange or yellow powder1 the color of which is more visible after it is cooled4 ,the portions of this sublimate furthest from the assay present a visible iridescent appearance4 ,this reaction of cadmium is so characteristic and sensitive that minerals 7for instance1 calamine1 carbonate of zinc7 which contains from one to five per cent4 of carbonate of cadmium1 will give a dark yellowish ring of cadmium oxide1 a little distance from the assay1 after being exposed for a few moments to the flame of reduction4 ,this sublimate is more visible when cold1 and is produced some time previous to the reduction of the zinc oxide4 ,if a vapor of the latter should appear1 it indicates that it has been exposed too great a length of time to the flame4 ,borax dissolves a considerable quantity of cadmium oxide upon a platinum wire to a clear yellow bead1 which1 when cold1 is almost colorless4 ,if the bead is nearly saturated with the cadmium oxide1 it appears milk-white when intermittingly heated4 ,if the bead is completely saturated1 it retains its opalescent appearance4 ,upon charcoal1 and in the flame of reduction1 the bead intumesces1 the cadmium oxide becomes reduced to metal2 this becomes volatilized and re-oxidized1 and sublimes upon the charcoal as the yellow cadmium oxide4 ,in the oxidation flame1 microcosmic salt dissolves a large quantity of it to a clear bead1 which1 when highly saturated and while hot1 is yellowish colored1 but colorless when cold4 ,by complete saturation1 the bead is enamel-white when cold4 ,upon charcoal1 in the flame of reduction1 the bead is slowly and only partially reduced1 a scanty sublimate being produced on the charcoal4 ,the addition of tin promotes the reduction4 ,carbonate of soda does not dissolve cadmium oxide in the oxidation flame4 ,in the reduction flame1 upon charcoal1 it is reduced to metal1 and is volatilized to a red-brown or dark1 red sublimate of cadmium oxide upon the charcoal1 at a little distance from the assay the charcoal presenting the characteristic iridescent appearance4 ,this reaction is still more sensitive if the cadmium oxide is heated per se in the reduction flame4 ,antimony 7,sb74--,this metal is found in almost every country4 ,it principally occurs as the tersulphide 7,sb,s#c71 either pure or combined with other sulphides1 particularly with basic sulphides4 ,sometimes it occurs as the pure metal1 and rarer in a state of oxidation as an antimonious acid and as the oxysulphide4 ,in the pure state1 antimony has a silver-white color1 with much lustre1 and presents a crystalline structure4 ,the commercial and impure metal is of a tin-white color1 and may frequently be split in parallel strata4 ,it is brittle and easily pulverized4 ,it melts at a low red heat 7#haj71 is volatilized at a white heat1 and can be distilled4 ,at common temperatures it is not affected by the air4 ,at a glowing heat it takes fire1 and burns with a white flame1 and with white fumes1 forming volatile antimonious acid4 ,common acids oxidize antimony1 but dissolve it slightly4 ,it is soluble in aqua regia 7nitro-hydrochloric acid74 ,sesquioxide of ,antimony 7,sb#b,o#c74--;,in the pure state this oxide is a white powder1 is fusible at a dull red heat to a yellow liquid1 which1 after cooling1 is greyish-white and crystalline4 ,if it is heated excluded from the air1 it can be volatilized completely2 it sublimes in bright crystals having the form of needles4 ,it occurs sometimes in nature as white and very bright crystals4 ,it takes fire when heated in the open air1 and burns with a white vapor to antimonious acid4 ,it fuses with the ter-sulphide of antimony to a red bead4 ,it is distinguished from the other oxides of antimony by the readiness with which it is reduced to the metallic state upon charcoal1 and by its easy fusibility and volatility4 ,the sesquioxide is the base of some salts--for instance1 the tartar emetic4 ,it is not soluble in nitric acid1 but is soluble in hydrochloric acid4 ,this solution becomes milky by the addition of water4 ,a part of the salts of the sesquioxide of antimony are decomposed by ignition4 ,the haloid salts are easily volatilized1 without decomposition4 ,its soluble neutral salts change blue litmus paper to red1 and are converted1 by admixture of water1 into insoluble basic and soluble acid salts4 ,antimonious acid 7antimoniate of sesquioxide of antimony1 ,sb#b,o#c ,sb#b,o#e7 is of a white color1 but1 when heated1 of a light yellow color1 but changes to white again when cold4 ,it is infusible and unaltered by heat4 ,it forms a white hydrate1 and both are insoluble in water and nitric acid4 ,it is partly soluble in hydrochloric acid1 with the application of heat4 ,the addition of water causes a precipitate in this solution4 ,antimonic ,acid 7,sb#b,o#e74--;,in the pure state this acid is a light yellow-colored powder4 ,its hydrate is white1 and is insoluble in water and nitric acid4 ,it is sparingly soluble in hot concentrated hydrochloric acid4 ,it forms salts with every base1 some of which are insoluble1 and others sparingly so4 ,notwithstanding that antimonic acid is insoluble in water1 it expels the carbonic acid from the solutions of the carbonates of the alkalies4 ,antimonic acid and its hydrate changes moistened blue litmus paper to red4 ,behavior of ,antimony and its ,oxides before the ,blowpipe4 ,metallic ,antimony fuses easily upon charcoal4 ,when heated to glowing1 and then removed from the flame1 it continues to glow for awhile1 and produces a thick white smoke4 ,the vapor crystallizes gradually1 and coats the assay with small crystals which iridesce like mother of pearl 7sesquioxide of antimony74 ,it is not volatile at the temperature of melted glass4 ,ignited in an open glass tube1 it burns slowly with a white vapor1 which condenses upon the cool part of the tube1 and exhibits some indications of crystallization4 ,this vapor consists of the sesquioxide1 and can be driven by heat from one place to another1 without leaving a residue4 ,if the metallic antimony contains sulphide of antimony1 there is a corresponding portion of antimonious acid produced1 which remains as a white sublimate after the sesquioxide is removed4 ,sesquioxide of antimony melts easily1 and sublimes as a white vapor4 ,it may be prepared by precipitating and drying4 ,when heated1 it takes fire previous to melting1 glows like tinder1 and is converted into antimonious acid1 which is now infusible4 ,when heated upon charcoal in the flame of reduction1 it is reduced to the metallic state1 and partly volatilized4 ,a white vapor sublimates upon the charcoal1 while the external flame exhibits a greenish-blue color4 ,antimonious acid is infusible1 produces a strong light1 and is diminished in volume when heated in the external flame1 during which time a dense white vapor sublimes upon the charcoal4 ,it is not1 however1 in this manner reduced to the metallic state like the sesquioxide4 ,antimonic acid1 when first heated1 becomes white1 and is converted into antimonious acid4 ,hydrated antimonic acid1 which is originally white1 appears at first yellow while giving off water1 and then becomes white again1 while oxygen is expelled1 and it is converted into antimonious acid4 ,the oxides of antimony produce1 with blowpipe reagents1 the following reactions3 borax dissolves oxides of antimony in the oxidation flame in considerable quantity to a clear bead1 which is yellow while hot1 but colorless when cold4 ,if the bead is saturated1 a part of the oxide is volatilized as a white vapor4 ,upon charcoal1 in the oxidation flame1 it is completely volatilized1 and the charcoal is covered with a white sublimate4 ,heated upon charcoal in the reducing flame1 the bead is of a greyish color1 and partially1 if not wholly opaque1 from the presence of reduced metallic particles4 ,a continued heat will volatilize them1 and the bead becomes clear4 ,the addition of tin promotes the reduction4 ,microcosmic salt dissolves the compounds of antimony in the flame of oxidation with intumescence1 to a clear light-yellow colored bead1 which when cold is colorless4 ,heated upon charcoal in the reduction flame1 the bead is first turbid1 but soon becomes transparent4 ,the addition of tin renders the bead greyish while cooling1 but a continued blast renders it transparent4 ,soda dissolves the compounds of antimony upon platinum wire in the oxidation flame1 to a clear colorless bead1 which is white when cold4 ,upon charcoal1 both in the oxidation and reduction flames1 the antimony compounds are readily reduced to the metal1 which is immediately volatilized1 and produces a white incrustation of oxide of antimony upon the charcoal4 ,if the antimony compounds are heated upon charcoal in the flame of reduction1 with a mixture of carbonate of soda and cyanide of potassium 7,k,cy71 there are produced small globules of metallic antimony4 ,at the same time1 a part of the reduced metal is volatilized 7this continues after the assay is removed from the flame7 and re-oxidized4 ,a white incrustation appears upon the charcoal1 and the metallic globules are covered with small white crystals4 ,if this white sublimate upon the charcoal is moistened with a solution of cobalt-oxide1 and exposed to the reduction flame1 a part of it is volatilized1 while the other part passes into higher oxidation1 and remains1 after cooling1 of a dirty dark-green color4 7d47 ,tellurium 7,te74--,this is one of the rare metals4 ,it occurs very seldom in the metallic state1 but often with bismuth1 lead1 silver1 and gold4 ,tellurium1 in the pure state1 is silver-white1 very bright1 of a foliated or lamellar structure1 brittle1 and easily triturated4 ,it is inclined to crystallize4 ,it is soluble in concentrated sulphuric acid without oxidation4 ,the solution is of a fine purple color1 and gives a precipitate with the addition of water4 ,tellurium in the ,metallic form4--,by the aid of heat it is oxidized in sulphuric acid1 a portion of the oxygen of the acid oxidizing the metal1 while sulphurous acid gas escapes4 ,this solution is colorless1 and is tellurous acid1 dissolved in sulphuric acid4 ,it melts at a low red heat1 and volatilizes at a higher temperature4 ,if tellurium is heated with free access of air1 it takes fire1 and burns with a blue color1 the flame being greenish at the edges1 while a thick white vapor escapes1 which has a feeble acidulous odor4 ,tellurous ,acid 7,te,o#b7 is of a fine1 granulous1 crystalline or white earthy mass1 which is partly soluble in water4 ,the solution has a strong metallic taste1 and an acid reaction upon litmus paper4 ,heated in a tube closed at one end until it begins to glow1 it fuses to a yellow liquid which is colorless1 crystalline1 and opaque when cold4 ,beads of it remain usually transparent like glass4 ,heated upon platinum wire in the flame of oxidation1 it melts1 and is volatilized as a white vapor4 ,when heated upon charcoal in the oxidation flame1 it melts1 and is reduced to the metallic state1 but volatilizes and a sublimate of white tellurous acid is formed upon the charcoal4 ,the edge of this deposit is usually red or dark-yellow4 ,heated upon charcoal in the flame of reduction1 it is rapidly reduced1 the external flame exhibiting a bluish-green color4 ,borax dissolves it in the oxidation flame upon platinum wire to a clear colorless bead which turns grey when heated upon charcoal1 through the presence of reduced metallic particles4 ,upon charcoal1 in the reduction flame1 the bead is grey1 caused by the reduced metal4 ,after a continued blast1 tellurium is completely volatilized1 and the bead appears clear again1 while a white sublimate is deposited upon the charcoal4 ,with microcosmic salt1 the same reactions are produced4 ,with carbonate of soda1 tellurous acid fuses upon platinum wire to a clear colorless bead1 which is white when cold4 ,upon charcoal it is reduced1 and forms tellur-sodium1 which is absorbed by the charcoal1 and metallic tellurium1 which is volatilized1 and deposits upon the charcoal a white incrustation 7tellurous acid74 ,if tellurous acid1 finely powdered charcoal1 and carbonate of soda are mixed together1 and the mixture be well ignited in a closed tube1 until fusion is effected1 and a few drops of boiled water are brought into the tube1 they are colored purple1 indicating the presence of tellur-sodium4 ,telluric ,acid 7,te,o#c7 forms six-sided prismatic crystals4 ,it has not an acid1 but rather a metallic taste4 ,it changes blue litmus paper to red2 is slowly soluble in water1 and rather sparingly4 ,exposed to a high temperature1 but not until glowing1 the crystalline acid loses its water1 and acquires an orange color1 but still it preserves its crystalline form1 although no longer soluble in water1 and is in fact so much changed in its properties as to present the instance of an isomeric modification4 ,if telluric acid is heated gently in a closed tube1 it loses water and turns yellow4 ,heated still more strongly1 it becomes milk-white1 oxygen is expelled1 and it is converted into tellurous acid4 ,the presence of oxygen can be recognized by the more lively combustion which an ignited splinter of wood undergoes when held in it4 ,telluric acid produces the same reactions with the blowpipe reagents as tellurous acid4 ,,seventh ,,group4--,,lead1 ,,bismuth1 ,,tin4 ,the oxides of these metals are also reduced to the metallic state by fusion with soda upon charcoal in the flame of reduction1 but they are volatilized only after a continued blast1 and a sublimate is thrown upon the charcoal4 7a47 ,lead 7,pb74--,this metal occurs in considerable quantity in nature1 chiefly as galena or lead-glance 7sulphide of lead74 ,likewise1 but more rarely1 as a carbonate2 also as a sulphate1 and sometimes combined with other acids and metals4 ,in the metallic state1 lead is of a bluish-grey color1 high lustre1 and sp4 gr4 #aa4d4 ,it is soft1 and communicates a stain to paper4 ,it is malleable1 ductile1 but has very little tenacity4 ,it melts at about #fab4 ,exposed to the air it soon tarnishes1 being covered with a grey matter1 which some regard as a suboxide 7,pb#b,o71 and others as simply a mixture of lead and protoxide4 ,at a glowing heat it is oxidized to a protoxide1 and at a white heat it is volatilized4 ,it is insoluble in most acids4 ,it is1 however1 soluble in nitric acid1 but without decomposing water4 7,l47 ,protoxide of ,lead 7,pb,o74--,it is an orange-colored powder1 which melts at a glowing temperature1 and forms a lamellar mass after cooling4 ,protoxide of lead absorbs oxygen from the atmosphere while melting1 which is given off again by cooling4 ,being exposed for a longer while to the air1 it absorbs carbonic acid and water1 and becomes white on the surface4 ,it is soluble in nitric acid and caustic alkalies4 ,it forms with most acids insoluble salts4 ,it is slightly soluble in pure water1 but not in water which contains alkaline salts4 ,this hydrate is white4 7beta47 ,red ,oxide of ,lead 7,pb,o#b1 ,pb,o74--,it forms a puce-colored powder4 ,it is insoluble in caustic alkalies4 ,hydrochloric acid dissolves it and forms a yellow liquid1 which is soon decomposed into chloride of lead and chlorine4 ,it is reduced by ignition to the protoxide4 7gamma47 ,peroxide of ,lead 7,pb,o#b74--;,it is a dark-brown powder4 ,it yields with hydrochloric acid the chloride of lead and chlorine gas4 ,when heated it liberates oxygen1 and is reduced to the protoxide4 ,lead combinations give the following reactions before the blowpipe3 ,metallic lead tarnishes when heated in the oxidation flame1 and is instantly covered with a grey matter1 consisting of the protoxide and the metal4 ,it fuses quickly1 and is then covered with a yellowish-brown protoxide until all the lead is converted into the protoxide1 which melts to a yellow liquid4 ,in the reduction flame and upon charcoal1 it is volatilized1 while the charcoal becomes covered with a yellow sublimate of oxide4 ,a little distance from the assay1 this sublimate appears white 7carbonate of lead74 ,protoxide of lead melts in the flame of oxidation to a beautiful dark yellow bead4 ,in the flame of reduction1 and upon charcoal1 it is reduced with intumescence to metallic lead1 which is volatilized by a continued blast1 and sublimates on charcoal1 as mentioned above4 ,red oxide of lead turns black when heated in the glass tube closed at one end1 and liberates oxygen1 which is easily detected by the introduction of an ignited splinter1 when a more lively combustion of the wood proves the presence of uncombined oxygen4 ,the red oxide in this case is reduced to the protoxide4 ,heated upon platinum foil1 it first turns black1 is reduced to the protoxide1 and melts into a dark yellow liquid4 ,in the reduction flame1 upon charcoal1 it is reduced to the metal with intumescence4 ,after a continued blast1 a yellow sublimate of protoxide is produced upon the charcoal1 and at a little distance off1 around this sublimate1 a white one of carbonate of lead is produced4 ,this sublimate disappears when touched by the flame of reduction1 while it communicates an azure blue-tinge to the external flame4 ,this is likewise the case with the peroxide of lead4 ,the different oxides of lead produce with the blowpipe reagents the same reactions4 ,borax dissolves lead compounds with the greatest readiness upon platinum wire in the oxidation flame to a transparent bead1 which is yellow when hot1 but colorless after being cooled4 ,with the addition of more of the lead oxide1 it becomes opalescent4 ,when heated by the intermittent flame1 and with still more of the oxide1 it acquires a yellow enamel after cooling4 ,heated upon charcoal1 in the flame of reduction1 the bead spreads and becomes opaque4 ,after a continued blast1 all the oxide is reduced with effervescence to metallic lead1 which melts and runs towards the edges of the bead1 while the bead again becomes transparent4 ,microcosmic ,salt dissolves oxides of lead upon platinum wire in the flame of oxidation easily to a clear1 colorless bead1 which appears1 when highly saturated1 yellow while hot4 ,a saturated bead becomes enamel-like after cooling4 ,the bead appears in the flame of reduction1 and upon charcoal1 of a greyish color and dull4 ,by the addition of more oxide1 a yellow sublimate of protoxide is produced upon the charcoal4 ,by the addition of tin1 the bead appears of a darker grey1 but it is never quite opaque4 ,carbonate of ,soda dissolves oxide of lead in the flame of oxidation upon platinum wire quite readily to a transparent bead1 which becomes yellow when cooling1 and is opaque4 ,upon charcoal in the flame of reduction1 it is rapidly reduced to metallic lead1 which yields1 after a continued blast1 a yellow sublimate of oxide upon the charcoal4 7b47 ,bismuth 7,bi74--,this metal occurs mostly in the metallic state1 and less frequently as the sulphide4 ,in the pure metallic state1 it is of a reddish-white color and great lustre4 ,it crystallizes in cubes4 ,it is brittle1 and may be readily pulverized4 ,it melts at #dgf1 and is volatilized at a white heat4 ,it is soluble in nitric acid1 and forms the nitrate of bismuth4 7alpha47 ,oxide of ,bismuth 7,bi#b,o#c74--,this oxide is a light yellow powder1 fusible at a red heat1 insoluble in caustic potash and ammonia4 ,it is the base of the salts of bismuth4 ,its hydrate is white1 and easily soluble in acids4 ,the addition of water causes these solutions to become milky1 because they are decomposed into a soluble acidulous and an insoluble basic salt of bismuth4 7beta47 ,peroxide of ,bismuth 7,bi,o#b7 is a dark-colored powder1 completely soluble in boiling nitric acid1 and yielding oxygen2 produces1 with hydrochloric acid1 chlorine gas4 ,it can be heated up to the temperature of #fbj without being decomposed2 but1 exposed to a temperature of #fcj it yields oxygen4 ,mixed with combustible substances1 it glows with brightness4 7gamma47 ,bismuthic ,acid 7,bi#b,o#e7 is a brown powder similar to the peroxide1 but is converted by boiling nitric acid into a green1 scarcely soluble substance 7,bi#b,o#c1 ,bi#b,o#e74 ,its hydrate is of a red color4 ,,blowpipe ,,reactions4--,metallic bismuth is converted1 when exposed upon platinum wire to the flame of oxidation1 into a dark brown oxide1 which turns light yellow while cooling4 ,it is slowly volatilized when heated1 and a yellow sublimate of oxide is produced upon the charcoal4 ,oxide of bismuth melts upon platinum foil in the flame of oxidation very easily into a dark-brown liquid1 which changes to a light yellow while cooling4 ,by too strong a heat1 it is reduced and penetrates the platinum foil4 ,upon charcoal1 in the flame of oxidation and of reduction1 it is reduced to metallic bismuth1 which melts into one or more globules4 ,by a continued blast they are slowly volatilized1 and produce a yellow sublimate of oxide upon the charcoal1 beyond which a white sublimate of carbonate of bismuth is visible4 ,these sublimates disappear in the flame of reduction1 but without communicating any color to it4 ,borax dissolves oxide of bismuth upon platinum wire1 in the flame of oxidation1 easily to a clear yellow bead1 which appears colorless after cooling4 ,by the addition of more oxide1 the hot bead becomes orange4 ,it turns more yellow while cooling1 and when cool is opalescent4 ,upon charcoal in the flame of reduction1 the bead becomes turbid and greyish colored4 ,the oxide is reduced with intumescence to the metallic state1 and the bead becomes clear again4 ,the addition of tin promotes the reduction4 ,microcosmic ,salt dissolves oxide of bismuth upon platinum wire1 in the flame of oxidation1 to a yellow bead1 which becomes colorless after cooling4 ,by the addition of more oxide1 the bead is yellowish-brown while hot1 and colorless after cooling1 but not quite transparent4 ,this bead becomes enamelled when heated by the intermittent flame2 also1 by the addition of still more of the oxide1 after it is cooled4 ,upon charcoal1 in the flame of reduction1 and particularly with the addition of tin1 the bead is colorless and transparent while hot1 but while cooling becomes of a dark-gray color and opaque4 ,oxide of bismuth is reduced1 by fusion with carbonate of soda1 as well in the oxidating as in the reducing flame1 instantly to metallic bismuth4 ,as the above mentioned higher oxides of bismuth are converted by ignition into oxide of the metal and free oxygen1 they have the same behavior before the blowpipe4 ,as bismuth occurs mostly in the metallic form1 it is necessary to know how to distinguish it from metals similar to it4 ,its brittleness distinguishes it from lead1 zinc and tin1 as they are readily flattened by a stroke of the hammer1 while bismuth is broken to pieces4 ,bismuth1 in this latter respect1 might perhaps be mistaken for antimony or tellurium2 but1 by the following examination1 it is easy to separate bismuth from antimony or tellurium4 #a4 ,neither bismuth nor antimony sublimates when heated in a glass tube closed at one end4 ,at a temperature which is about to fuse the glass1 tellurium yields a small quantity of a white vapor 7some tellurium is oxidized to tellurous acid by the oxygen of the air in the tube74 ,after that1 a grey metallic sublimate settles on the sides of the tube4 #b4 ,heated in an open tube1 antimony yields a white vapor1 which coats the inside of the glass tube1 and can be driven by heat from one part of the tube to another without leaving a residue4 ,the metallic globule is covered with a considerable quantity of fused oxide4 ,tellurium produces1 under the same circumstances1 an intense vapor1 and deposits on the glass a white powder1 which melts by heat into globules that run over the glass4 ,the metallic globules are covered by fused1 transparent1 and nearly colorless oxide1 which becomes white while cooling4 ,by a high temperature1 and with little access of air1 metallic tellurium sublimes with the deposition of a grey powder4 ,bismuth produces1 under similar treatment1 scarcely any vapor1 unless it is combined with sulphur4 ,the metal is enveloped by fused oxide of a dark yellow color1 which appears light yellow after being cooled4 ,it acts upon the glass1 and dissolves it4 #c4 ,upon charcoal1 exposed to the blowpipe flame1 the three metals are volatilized1 and yield a sublimate upon the charcoal4 ,that of antimony is white1 while those of bismuth and tellurium are dark yellow4 ,by exposing them to the flame of reduction1 the sublimate of tellurium disappears and communicates an intense green color to the flame4 ,the antimony incrustation gives a feeble greenish-blue color1 while the sublimate of bismuth gives no perceptible color in the light4 ,it is1 however1 worthy of notice that if the operation takes place in the dark1 a very pale blue flame will be seen with the bismuth4 7c47 ,tin 7,sn74--,this metal does not occur in nature in the metallic state1 very seldom in the sulphide1 but chiefly in the oxide 7tinstone74 ,in the metallic state it is silver-white1 possesses a very high lustre1 is soft 7but harder than lead71 ductile1 but has not much tenacity1 and it is very malleable4 ,the metal when it is cast gives a peculiar creaking noise when twisted or bent1 which proceeds from the crystalline structure of the metal4 ,this crystallization is quite clearly manifested by attacking the surface of the metal1 or that of tin plate1 with acids4 ,tin is very slightly tarnished by exposure to the air4 ,it fuses at #ddb1 and becomes grey1 being a mixture of the oxide and the metal4 ,at a high temperature even1 tin is but little subject to pass off as vapor4 ,it is soluble in aqua regia1 and with the liberation of hydrogen1 in hot sulphuric and hydrochloric acids1 and in cold dilute nitric acid1 without decomposing water1 or the production of a gas1 while nitrate of tin and nitrate of ammonia are formed4 ,concentrated nitric acid converts tin into insoluble tin acids4 7alpha47 ,protoxide of ,tin 7,sn,o7 is a dark-grey powder4 ,its hydrate is white1 and is soluble in caustic alkalies4 ,when this solution is heated1 anhydrous crystalline black protoxide is separated4 ,the soluble neutral salts of tin-protoxide are decomposed by the addition of water1 and converted into acid soluble1 and basic insoluble salts4 ,when protoxide of tin is ignited with free access of air1 it takes fire and is converted with considerable intensity into the acids1 producing white vapors4 ,this is likewise the case if it is touched by a spark of fire from steel4 ,the hydrate of the protoxide of tin can be ignited by the flame of a candle1 and glows like tinder4 7beta47 ,sesquioxide of ,tin 7,sn#b,o#c7 is a greyish-brown powder4 ,its hydrate is white1 with a yellow tinge4 ,it is soluble in aqua ammonia and in hydrochloric acid2 this solution forms with solution of gold the purple of ,cassius4 7gamma47 ,stannic ,acid 7peroxide1 ,sn,o#b74--,this acid occurs in nature crystallized in quadro-octahedrons1 of a brown or an intense black color1 and of great hardness 7tinstone74 ,artificially prepared1 it is a white or yellowish-white powder4 ,it exists in two distinct or isomeric modifications1 one of which is insoluble in acids 7natural tin-acid7 while the other 7tin-acid prepared in the wet way7 is soluble in acids4 ,by ignition the soluble acid is converted into the insoluble4 ,both modifications form hydrates4 ,reactions before the ,blowpipe4--,metallic tin melts easily4 ,it is covered in the flame of oxidation into a yellowish-white oxide1 which is carried off sometimes by the stream of air which propels the flame4 ,in the reduction flame1 and upon charcoal1 melting tin retains its metallic lustre1 while a thin sublimate is produced upon the charcoal4 ,this sublimate is light-yellow while hot1 and gives a strong light in the flame of oxidation1 and turns white while cooling4 ,this sublimate is found near to the metal1 and cannot be volatilized in the oxidation flame4 ,in the flame of reduction it is reduced to metallic tin4 ,sometimes this incrustation is so imperceptible that it can scarcely be distinguished from the ashes of the charcoal4 ,if such be the case1 moisten it with a solution of cobalt1 and expose it to the flame of oxidation1 when the sublimate will exhibit1 after cooling1 a bluish-green color4 ,protoxide of tin takes fire in the flame of oxidation1 and burns with flame and some white vapor into tin acid1 or stannic acid4 ,in a strong and continued reduction flame1 it may be reduced to metal1 when the same sublimate above mentioned is visible4 ,the sesquioxide of tin behaves as the above4 ,stannic acid1 heated in the flame of oxidation1 does not melt and is not volatilized1 but produces a strong light1 and appears yellowish while hot1 but changing as it cools to a dirty-yellow white color4 ,in a strong and continued flame of reduction1 it may be reduced likewise to the metallic state1 with the production of the same sublimate as the above4 ,borax dissolves tin compounds in the flame of oxidation1 and upon platinum wire1 very tardily1 and in small quantity1 to a transparent colorless bead1 which remains clear after cooling1 and also when heated intermittingly4 ,but if a saturated bead1 after being completely cool1 is exposed again to the flame of oxidation1 at a low red heat1 the bead while cooling is opaque1 loses its globular form1 and exhibits an indistinct crystallization4 ,this is the case too in the flame of reduction1 but if the bead is highly saturated1 a part of the oxide is reduced4 ,microcosmic ,salt dissolves the oxides in the flame of reduction very tardily in a small quantity to a transparent colorless bead1 which remains clear while cooling4 ,if to this bead sesquioxide of iron is added in proper proportion1 the sesquioxide loses its property of coloring the bead1 but of course an excess of the iron salt will communicate to the bead its own characteristic color4 ,in the flame of reduction no further alteration is visible4 ,tin-oxides combine with carbonate of soda1 in the flame of oxidation upon platinum wire1 with intumescence to a bulky and confused mass1 which is insoluble in more soda4 ,upon charcoal1 in the reduction flame1 it is easily reduced to a metallic globule4 ,certain compounds of tin-oxides1 particularly if they contain tantalum1 are by fusion with carbonate of soda reduced with difficulty2 but by the addition of some borax1 the reduction to the metallic state is easily effected4 ,tin-oxides exposed to the oxidation flame1 then moistened with a solution of cobalt1 and exposed again to the flame of oxidation1 will exhibit1 after having completely cooled1 a bluish-green color4 ,,eighth ,,group4--,,mercury1 ,,arsenic4 ,these two metals are volatilized at a temperature lower than that of a red heat1 and produce1 therefore1 no reactions with borax and microcosmic salt4 ,their oxides are easily reduced to the metallic state4 7a47 ,mercury 7,hg74--,this metal occurs in nature chiefly combined with sulphur as a bisulphide4 ,it occurs still more rarely in the metallic form1 or combined with silver1 selenium1 or chlorine4 ,mercury1 in the metallic state1 has a strong lustre1 and is liquid at ordinary temperatures1 whereby it is distinguished from any other metal4 ,it freezes at #dj and boils at #fbj1 but it evaporates at common temperatures4 ,pure mercury is unalterable4 ,upon being exposed to the air1 it tarnishes only by admixture with other metals1 turns grey on the surface1 and loses its lustre4 ,it is soluble in cold nitric acid and in concentrated hot sulphuric acid1 but not in hydrochloric acid4 7chi47 ,protoxide of ,mercury 7,hg#b,o74--,it is a black powder1 which is decomposed by ignition into metallic mercury and oxygen4 ,by digestion with certain acids1 and particularly with caustic alkalies1 it is converted into metallic mercury and peroxide4 ,some neutral salts of the protoxide are only partly soluble in water1 as they are converted into basic insoluble and acid soluble salts4 ,protoxide of mercury is completely insoluble in hydrochloric acid4 ,its neutral salts change blue litmus paper to red4 7beta47 ,peroxide of ,mercury 7,hg,o74--,this oxide exists in two allotropic modifications4 ,one is of a brick-red color1 and the other is orange4 ,being exposed to heat1 they turn black1 but regain their respective colors upon cooling4 ,they are decomposed at a high temperature into metallic mercury and oxygen4 ,they yield with acids their own peculiar salts4 ,mercury1 in the metallic form1 can never be mistaken for any other metal in consequence of its fluid condition at ordinary temperatures4 ,exposed to the blowpipe flame1 it is instantly volatilized4 ,this is also the case with it when combined with other metals4 ,the oxides of mercury are1 in the oxidation and reduction flames1 instantly reduced and volatilized4 ,they do not produce any alteration with fluxes1 as they are volatilized before the bead melts4 ,heated with carbonate of soda in a glass tube closed at one end1 they are reduced to metallic mercury1 which is volatilized1 and condenses upon a cool portion of the tube as a grey powder4 ,by cautious knocking against the tube1 or by rubbing with a glass rod1 this sublimate can be brought together into one globule of metallic mercury4 ,compounds of mercury can be most completely reduced by a mixture of neutral oxalate of potassa and cyanide of potassium4 ,if the substance under examination contains such a small quantity of mercury that it cannot be distinguished by volatilization1 a strip of gold leaf may be attached to an iron wire1 and introduced during the experiment in the glass tube4 ,the smallest trace of mercury will whiten the gold leaf in spots4 7b47 ,arsenic 7,as74--,this metal occurs in considerable quantity in nature1 chiefly combined with sulphur or metals4 ,arsenic1 in the metallic state1 is of a whitish-grey color1 high lustre1 and is crystalline1 of a foliated structure1 and is so brittle that it can be pulverized4 ,it does not melt1 but is volatilized at #cef4 ,its vapor has a strong alliaceous odor4 ,arsenic sublimes in irregular crystals4 ,by exposure to the air it soon tarnishes1 and is coated black4 ,being mixed with nitrate of potassa and inflamed1 it detonates with vehemence4 ,mixed with carbonate of potassa1 it is inflamed by a stroke of the hammer1 and detonates violently4 ,heated in oxygen gas1 it is inflamed1 and burns with a pale blue flame to arsenious acid4 7beta47 ,arsenious ,acid 7,as,o#c74--,this acid crystallizes in octahedrons1 or1 when fused1 forms a colorless glass1 which finally becomes opaque and enamel-like1 or forms a white powder4 ,it sublimes without change or decomposition4 ,when heated for a longer while below the temperature of sublimation1 it melts into a transparent1 colorless1 tough glass4 ,the opaque acid is sparingly soluble in cold water1 and still more soluble in hot water4 ,it is converted1 by continued boiling1 into the transparent acid1 which is much more soluble in water4 ,arsenious acid is easily dissolved by caustic potassa4 ,it is also soluble in hydrochloric acid4 ,this acid occurs associated with antimonious acid1 protoxide of tin1 protoxide of lead1 and oxide of copper4 ,it occurs likewise in very small quantity in ferruginous mineral springs4 7gamma47,arsenic ,acid 7,as,o#e7 is a white mass1 which readily absorbs moisture and dissolves4 ,it will not volatilize at a low red heat1 nor will it decompose4 ,exposed to a strong heat1 it is decomposed1 yielding oxygen1 and passing into arsenious acid4 ,reactions before the ,blowpipe4 ,metallic arsenic1 heated in a glass tube closed at one end1 yields a black sublimate of a metallic lustre1 and at the same time gives out the characteristic alliaceous odor4 ,this is the case too with alloys of arsenic1 if there is a maximum quantity of arsenic present4 ,when heated in a glass tube open at both ends1 metallic arsenic is oxidized to arsenious acid1 which appears as a white crystalline sublimate on the sides of the glass tube4 ,this deposit will occur at some distance from the assay1 in consequence of the great volatility of the arsenic4 ,the sublimate can be driven from one place upon the tube to another1 by a very low heat4 ,alloys of arsenic are converted into basic arseniates of metal oxides1 while surplus arsenic is converted into arsenious acid1 which sublimes on the tube4 ,if too much arsenic is used for this experiment1 a dark-brown incrustation will sublime upon the sides of the tube which will give an alliaceous smell4 ,if this sublimate should be deposited near the assay1 then it resembles the white sublimate of arsenious acid4 ,heated upon charcoal1 metallic arsenic is volatilized before it melts1 and incrusts the charcoal in the flame of oxidation as a white deposit of arsenious acid4 ,this sublimate appears sometimes of a greyish color1 and takes place at some distance from the assay4 ,when heated slightly with the blowpipe flame1 this sublimate is instantly driven away1 and being heated rapidly in the reduction flame1 it disappears with a light blue tinge1 while the usual alliaceous or garlic smell may be discerned4 ,arsenious acid sublimes in both glass tubes very readily1 as a white crystalline sublimate4 ,these crystals appear to be regular octahedrons when observed under the microscope4 ,upon charcoal it instantly volatilizes1 and when heated1 the characteristic garlic smell may be observed4 ,arsenic acid yields1 heated strongly in a glass tube closed at one end1 oxygen and arsenious acid1 the latter of which sublimes in the cool portions of the tube4 ,compounds of arsenic produce1 in consequence of their volatility1 no reactions with fluxes4 ,being heated upon charcoal with carbonate of soda1 they are reduced to metallic arsenic which may be detected by the alliaceous odor peculiar to all the arsenic compounds when volatilized4 ,,ninth ,,group4--,,copper1 ,,silver1 ,,gold4 ,these metals are not volatile1 neither are their oxides4 ,they are reduced to the metallic state1 by fusion with carbonate of soda1 when they melt to a metallic grain4 ,the oxides of silver and gold are reduced per se to the metallic state by ignition4 ,in the reduction of the oxides of this group1 no sublimate is visible upon the charcoal4 7a47 ,copper 7,cu74--,this metal occurs in the metallic state1 also as the protoxide1 and as oxides combined with acids in different salts 7carbonate of copper as malachite1 etc47 ,the sulphide of copper is the principal ore of copper occurring in nature4 ,in the metallic state1 copper is of a red color1 has great lustre and tenacity1 is ductile and malleable1 and crystallizes in octahedrons and cubes4 ,it melts at a bright red heat1 is more difficult than silver to fuse1 but fuses more readily than gold4 ,it absorbs oxygen while melting4 ,there arises from its surface a fine dust of metallic globules1 which are covered with the protoxide4 ,the surface of the metal is likewise covered with the protoxide4 ,copper exposed to moist air tarnishes1 and is converted into hydratic carbonate of copper4 ,when ignited in the open air1 it is soon covered with the brownish-red protoxide4 7chi47 ,protoxide of ,copper 7,cu#b,o74--,this oxide occurs in nature1 crystallized in octahedrons of a ruby-red color1 of a lamellar structure1 and transparent4 ,artificially prepared1 it forms a powder of the same color4 ,it is decomposed by dilute acids into salts of peroxide and metal4 ,it is converted by ignition1 with free access of air1 into peroxide4 7beta47 ,oxide of ,copper 7,cu,o74--,this oxide is a dark-brown or black powder4 ,it is dissolved by acids1 with a blue or green-colored solution4 ,it is soluble in aqua ammonia1 and the solution is of a dark blue color4 ,reactions before the ,blowpipe4--,oxide of copper exposed upon platinum wire to the inmost flame 7the blue flame71 communicates to the external flame a green color4 ,heated upon charcoal in the oxidation flame1 it melts to a black ball1 soon spreads over the charcoal1 and is partially reduced4 ,exposed to the reduction flame1 at a temperature which will not melt copper1 it is reduced with a bright metallic lustre1 but as soon as the blast ceases1 the surface of the metal becomes oxidized1 and appears dark brown or black4 ,if the temperature is continued still higher1 it melts to a metallic grain4 ,borax dissolves the oxide of copper in the flame of oxidation to a clear green-colored bead1 even if the quantity of oxide be quite small1 but by cooling1 the bead becomes blue4 ,in the flame of reduction upon platinum wire1 the bead soon becomes colorless1 but while cooling presents a red color 7protoxide of copper74 ,this bead is opaque1 but1 if too much of the oxide is added1 a part of it is reduced to metal1 which is visible by breaking the metallic grain4 ,upon charcoal1 the oxide is reduced to the metal1 and the bead appears colorless after cooling4 ,with the addition of some tin1 the bead becomes brownish-red and opaque after cooling4 ,microcosmic ,salt dissolves oxide of copper in the flame of oxidation to a green bead1 not so intensely colored as the borax bead4 ,in the reduction flame the bead1 if pretty well saturated1 becomes dark-green while hot1 and brownish-red when cool1 opaque and enamel-like4 ,if the oxide is so little that no reaction is visible1 by the addition of some tin1 the bead appears colorless while hot1 and dark brownish-red and opaque when cold4 ,carbonate of ,soda dissolves oxide of copper in the oxidation flame upon platinum wire1 to a clear1 green bead1 which loses its color when cooling1 and becomes opaque4 ,upon charcoal1 it is reduced to the metal1 the soda is absorbed by the charcoal1 and the metallic particles melt with sufficient heat to a grain4 7b47 ,silver 7,ag74--,this metal occurs in nature in the metallic state1 and in combination with other metals1 particularly with lead4 ,it also occurs as the sulphide in several mines4 ,it crystallizes in cubes and octahedrons2 is of a pure white color1 great lustre1 is very malleable and ductile1 and is softer than copper1 but harder than gold4 ,it is not oxidizable1 neither at common temperatures nor at those which are considerably higher4 ,it is soluble in dilute nitric acid1 and in boiling concentrated sulphuric acid4 7chi47 ,protoxide of ,silver 7,ag#b,o74--,it is a black powder4 ,it is converted by acids and ammonia into oxide and metal4 7beta47 ,oxide of ,silver 7,ag,o74--,it is a greyish-brown or black powder1 and is the base of the silver salts4 ,with aqua ammonia1 it is converted into the black1 fulminating silver4 7gamma47 ,superoxide or ,binoxide of ,silver 7,ag,o#b74--,this oxide occurs in black needles or octahedral crystals of great metallic lustre4 ,it is dissolved by the oxygen acids with the disengagement of oxygen gas4 ,behavior before the ,blowpipe4--,when exposed to the flames of oxidation and reduction1 the oxides of silver are instantly reduced to the metallic state4 ,borax dissolves silver-oxides upon platinum wire in the oxidation flame but partially1 while the other portion is reduced1 the bead appearing opalescent after cooling1 in correspondence to the degree of saturation4 ,the bead becomes grey in the flame of reduction1 the reduced silver melting to a grain1 and the bead is rendered clear and colorless again4 ,microcosmic ,salt dissolves oxides of silver in the flame of oxidation upon platinum wire to a transparent yellowish bead1 which presents1 when much of the oxide is present1 an opalescent appearance4 ,in the flame of reduction1 the reaction is analogous to that of borax4 ,by fusion with carbonate of soda in the oxidation and reduction flames1 the silver oxides are instantly reduced to metallic silver1 which fuses into one or more grains4 7c47 ,gold 7,au74--,this metal occurs mostly in the metallic state1 but frequently mixed with ores1 and with other metals4 ,gold crystallizes in cubes and octahedrons1 is of a beautiful yellow color1 great lustre1 and is the most malleable and ductile of all the metals4 ,it melts at a higher temperature than copper1 gives a green colored light when fused1 and contracts greatly when cooling4 ,it does not oxidize at ordinary temperatures1 nor when heated much above them4 ,it is soluble in nitro-hydrochloric acid 7aqua regia74 7chi47 ,protoxide of ,gold 7,au#b,o74--,this oxide is a dark violet colored powder which is converted by a temperature of #edj into metallic gold and oxygen4 ,it is only soluble in aqua regia4 ,treated with hydrochloric acid1 it yields the chloride of gold and the metal4 ,with aqua ammonia1 it yields the fulminating gold1 which is a blue mass and very explosive4 7chi47 ,peroxide of ,gold 7,au#b,o#c74--,this oxide is an olive-green or dark brown powder1 containing variable quantities of water4 ,decomposed at #ecj1 it yields metallic gold and oxygen4 ,reactions before the ,blowpipe4--,oxides of gold are reduced1 in both the oxidation and reduction flames1 to the metal1 which fuses to grains4 ,borax does not dissolve it1 but it is reduced to the metallic state in this flux in either flame4 ,the reduced metal fuses upon charcoal to a grain4 ,microcosmic ,salt presents the same reactions as borax4 ,when fused with soda1 upon charcoal1 the soda is absorbed1 and the gold remains as a metallic grain4 ,,tenth ,,group4--,,molybdenum1 ,,osmium4 ,these metals are not volatile1 and are infusible before the blowpipe2 but some of their oxides are volatile1 and can be reduced to an infusible metallic powder4 7a47 ,molybdenum 7,mo7 occurs in the metallic state2 also combined with sulphur1 or as molybdic acid combined with lead4 ,it is a white1 brittle metal1 and is unaltered by exposure to the air4 ,when heated until it begins to glow1 it is converted into a brown oxide4 ,heated at a continued dull red heat1 it turns blue4 ,at a higher temperature1 it is oxidized to molybdic acid1 when it glimmers and smokes1 and is converted into crystallized molybdic acid upon the surface4 7chi47 ,protoxide of ,molybdenum 7,mo,o74--,this oxide is a black powder4 7chi47 ,deutoxide of ,molybdenum 7,mo,o#b74--,this oxide is a dark copper-colored crystalline powder4 ,reactions before the ,blowpipe4--,metallic molybdenum1 its protoxide and binoxide1 are converted in the oxidation flame into molybdic acid4 ,this acid fuses in the flame of oxidation to a brown liquid1 which spreads1 volatilizes1 and sublimes upon the charcoal as a yellow powder1 which appears crystalline in the vicinity of the assay4 ,this sublimate becomes white after cooling4 ,beyond this sublimate there is visible a thin and not volatile ore of binoxide1 after cooling2 this is of a dark copper-red color1 and presenting a metallic lustre4 ,heated in a glass tube1 closed at one end1 it melts to a brown mass1 vaporizes and sublimates to a white powder upon a cool portion of the tube4 ,immediately above the assay1 yellow crystals are visible2 these crystals are colorless after cooling1 and the fused mass becomes light yellow-colored and crystalline4 ,upon platinum foil1 in the flame of oxidation1 it melts and vaporizes1 and becomes light yellow and crystalline after cooling4 ,in the reduction flame it becomes blue1 and brown-colored if the heat is increased4 ,upon charcoal1 in the reduction flame1 it is absorbed by the charcoal2 and1 with an increase of the temperature1 it is reduced to the metal1 which remains as a grey powder after washing off the particles of charcoal4 ,borax dissolves it1 in the oxidation flame1 upon platinum wire easily1 and in great quantity1 to a clear yellow1 which becomes colorless while cooling4 ,by the addition of more of the molybdenic acid the bead is dark yellow1 or red while hot1 and opalescent when cold4 ,in the reduction flame1 the color of the bead is changed to brown and transparent4 ,by the addition of more of the acid1 it becomes opaque4 ,microcosmic ,salt dissolves it in the oxidation flame1 upon platinum wire1 to a clear1 yellowish-green bead1 which becomes colorless after cooling4 ,in the reduction flame the bead is very dark and opaque1 but becomes of a bright green after cooling4 ,this is the case likewise upon charcoal4 ,carbonate of ,soda dissolves it upon platinum wire in the oxidation flame with intumescence1 to a clear bead1 which appears milk-white after cooling4 ,upon charcoal the soda and the molybdic acid are absorbed1 the latter is reduced to the metallic state1 the metal remaining as a grey powder after washing off the particles of charcoal4 ,when molybdic acid1 or any other oxide of this metal1 is exposed upon platinum wire1 or with platinum tongs1 to the point of the blue flame1 a yellowish-green color is communicated to the external flame4 ,if also any of the compounds of molybdenum are mixed in the form of a powder with concentrated sulphuric acid and alcohol1 and the latter inflamed1 the flame of the alcohol appears colored green4 7c47 ,osmium 7,os74--,this metal occurs associated with platinum4 ,it is of a bluish-grey color1 and is very brittle4 ,ignited in the open air1 it is oxidized to volatile osmic acid1 which is possessed of a pungent smell1 and affects the eyes4 ,it communicates a bright white color to the flame of alcohol4 ,osmium oxide 7,os,o#b7 is converted in the oxidation flame to osmic acid1 which is volatilized with a peculiar smell1 leaving a sublimate4 ,in the reduction flame it is reduced to a dark-brown infusible metallic powder4 ,it produces no reactions with fluxes4 ,carbonate of soda reduces it upon charcoal to an infusible metallic powder1 which appears1 after washing off the particles of charcoal1 of a dark-brown color4 ,,eleventh ,,group4--,,platinum1 ,,palladium1 ,,iridium1 ,,rhodium1 ,,ruthenium4 ,these metals are infusible before the blowpipe4 ,they are not volatile1 nor are they oxidizable4 ,their oxides are1 in both flames1 reduced to a metallic and infusible powder4 ,they give no reactions with fluxes1 but are separated in the metallic form4 ,these metals are generally found associated together in the native platinum1 also with traces of copper1 lead1 and iron4 ,the metal palladium is found native1 associated with iridium and platinum4 ,this metal generally occurs in greatest quantity in ,brazil4 ,the metal rhodium is found along with platinum1 but in very small quantities4 ,iridium occurs in nature associated with osmium1 gold1 and platinum1 in the mines of ,russia4 ,its great hardness has rendered it desirable for the points of gold pens4 ,in ,south ,america this metal is found native1 associated with platinum and osmium4 ,the latter metal1 associated with platinum and iridium1 has been found in ,south ,america4 ,as these metals will not oxidize or dissolve1 they cannot be separated from each other by the blowpipe with the reagents peculiar to that species of analysis4 ,it is true that colors may be discerned in the beads1 but these tints proceed from the presence of small traces of copper1 iron1 etc4 ,the ore of osmium and iridium can be decomposed1 and the former recognized by its fetid odor4 ,this metal1 strongly ignited in a glass tube with nitrate of potash1 is converted to the oxide of osmium1 which gives an odor not unlike the chloride of sulphur4 ,as the metals of this group are very rare ones1 especially the last four ones1 we shall not devote an especial division to each of them4 ,for a more detailed statement of their reactions1 the student is referred to the large works upon blowpipe analysis4 ,,class ,,iii4 ,,non-,,metallic ,,substances4 #a4 ,water--#b4 ,nitric ,acid--#c4 ,carbon--#d4 ,phosphorus --#e4 ,sulphur--#f4 ,boron--#g4 ,silicon--#h4 ,chlorine --#i4 ,bromine--#aj4 ,iodine--#aa4 ,fluorine--#ab4 ,cyanogen --#ac4 ,selenium4 7#a47 ,water 7,,ho74--,pure distilled water is composed of one volume of oxygen1 and two volumes of hydrogen gases2 or1 by weight1 of one part of hydrogen to eight parts of oxygen gases4 ,water is never found pure in nature1 but possessing great solvent properties1 it always is found with variable proportions of those substances it is most liable to meet with1 dissolved in it4 ,thus it derives various designations depending upon the nature of the substance it may hold in solution1 as lime-water1 etc4 ,in taking cognizance of water in relation to blowpipe analysis1 we regard it only as existing in minerals4 ,the examination for water is generally performed thus3 the substance may be placed in a dry tube1 and then submitted to heat over a spirit-lamp4 ,if the water exists in the mineral mechanically it will soon be driven off1 but if it exists chemically combined1 the heat will fail to drive it off1 or if it does1 it will only partially effect it4 ,the water will condense upon the cool portions of the tube1 where it can be readily discerned4 ,if the water exists chemically combined1 a much stronger heat must be applied in order to separate it4 ,many substances may be perhaps mistaken for water by the beginner1 such as the volatile acids1 etc4 7#b47 ,nitric ,acid 7,,no#e74--,nitric acid occurs in nature in potash and soda saltpetre4 ,these salts are generally impure1 containing lime1 as the sulphate1 carbonate and nitrate1 and also iron in small quantity4 ,the soda saltpetre generally contains a quantity of the chloride of sodium4 ,the salts containing nitric acid deflagrate when heated on charcoal4 ,substances containing nitric acid may be heated in a glass tube closed at one end1 by which the characteristic red fumes of nitrous acid are eliminated4 ,if the acid be in too minute a quantity to be thus distinguished1 a portion of the substance may be intimately mixed with some bisulphate of potash1 and treated as above4 ,the sulphuric acid of the bisulphate combines with the base1 and liberates the nitric acid1 while the tube contains the nitrous acid gas4 ,the nitrate of potassa1 when heated in a glass tube1 fuses to a clear glass1 but gives off no water4 ,when fused on platinum wire1 it communicates to the external flame the characteristic violet color4 ,when fused and ignited on charcoal1 its surface becomes frothy1 indicating the nitric acid4 7#c47 ,carbon 7,c74--,carbon is found in nature in the pure crystallized state as the diamond4 ,it occurs likewise in several allotropic states as graphite1 plumbago1 charcoal1 anthracite1 etc4 ,it exists in large quantities combined with oxygen as carbonic acid4 ,the diamond1 although combustible1 requires too high a heat for its combustion to enable us to burn it with the blowpipe4 ,when excluded from the air1 it may be heated to whiteness without undergoing fusion1 but with the free access of air it burns at a temperature of #gjc ,c1 and is converted into carbonic acid4 ,if mixed with nitre1 the potassa retains the carbonic acid1 and the carbon may be thus easily estimated4 ,if a mineral containing carbonic acid is heated1 the gas escapes with effervescence1 or a strong mineral acid as the hydrochloric will expel the acid with the characteristic effervescence4 7#d47 ,phosphorus1 ,phosphoric ,acid 7,,po#f74--,this acid occurs in a variety of minerals1 associated with yttria1 copper1 uranium1 iron1 lead1 manganese1 etc4 ,phosphoric acid may be detected in minerals by pursuing the following process3 dip a small piece of the mineral in sulphuric acid1 and place it in the platinum tongs3 this is heated at the point of the blue flame1 when the outer flame will become colored of a greenish-blue hue4 ,this color will not be mistaken for those of boracic acid1 copper1 or baryta4 ,some of the phosphoric minerals1 when heated in the inner flame1 will color the outer flame green4 ,if alumina be present with the phosphoric acid1 the following wet method should be adopted for the detection of the latter3 the substance should be powdered in the agate mortar with a mixture of six parts of soda1 and one and a half parts of silica4 ,the entire mass should now be placed on charcoal1 and melted in the flame of oxidation4 ,the residue should be treated with boiling water1 which dissolves the phosphate and the excess of carbonate of soda1 while the silicate of alumina1 with some of the soda1 is left4 ,the clear liquor is now treated with acetic acid1 and heated over the spirit-lamp1 and a small portion of crystallized nitrate of silver added2 a lemon-yellow precipitate of phosphate of silver is quickly developed4 ,previous to the addition of the nitrate1 the liquor should be well heated2 otherwise1 a white precipitate of dipyrophosphate of silver will be produced4 ,if the examination be of any of the metallic phosphides1 the substances should be powdered in the agate mortar1 and fused with nitrate of potassa on the platinum wire2 the fused mass should be treated with soda in the same manner as any substance containing phosphoric acid4 ,the metal and the phosphorus are oxidized1 while the phosphate of potassa is fused1 and the metallic oxide separates4 7#e47 ,sulphur 7,s74--,sulphur is found native in crystals ,it is frequently found associated with lime1 iron1 silica1 carbon1 etc41 and combined extensively with metals4 ,the principal acid of sulphur 7the sulphuric1 ,,so#c7 occurs combined with the earths1 the alkalies1 and the metallic oxides4 ,native sulphur is recognized1 when heated upon charcoal1 by its odor 7sulphurous acid7 and the blue color of its flame4 ,the compounds of sulphur may be detected by several methods4 ,if the substance is heated in a glass tube1 closed at one end1 the yellow sublimate of sulphur will subside upon the cool portions of the tube2 if the substance should also contain arsenic1 the sublimate will present itself as a light brown incrustation1 consisting of the sulphide of arsenic4 ,if the assay is heated in the open glass tube1 sulphurous acid will thus be generated2 but1 if the gas is too little to be detected by the smell1 a strip of moistened litmus paper will indicate the presence of the acid4 ,the assay will give off sulphurous fumes if heated in the flame of oxidation4 ,if the powdered substance is fused with two parts of soda1 and one part of borax1 upon charcoal1 the sulphide of sodium is formed4 ,this salt1 if moistened and applied to a polished silver surface1 will blacken it4 ,the borax serves no other purpose than to prevent the absorption of the formed sulphide of sodium by the charcoal4 ,as selenium will blacken silver in the manner above indicated1 the presence of this substance should be first ascertained1 by heating the assay2 when1 if it be present1 the characteristic horse-radish odor will reveal the fact4 ,sulphuric acid may be detected by fusing the substance with two parts of soda1 and one part of borax1 on charcoal1 in the flame of reduction2 the mass must now be wetted with water1 and placed in contact with a surface of bright silver2 when1 if sulphuric acid be present1 the silver will become blackened4 ,or the substance may be fused with silicate of soda in the flame of reduction4 ,in this case1 the soda combines with a portion of the sulphuric acid1 which is then reduced to the sulphide1 while the bead becomes of an orange or red color1 depending upon the amount of the sulphuric acid present4 ,if the assay should1 however1 be colored1 then the previous treatment should be resorted to4 7#f47 ,boron1 ,boracic ,acid 7,,bo#c74--,this acid occurs in nature in several minerals combined with various bases1 such as magnesia1 lime1 soda1 alumina1 etc4 ,combined with water1 this acid exists in nature as the native boracic acid2 this acid gives with test paper prepared from ,brazil wood1 when moistened with water1 a characteristic reaction1 for the paper becomes completely bleached4 ,an alcohol solution turns curcuma test paper brown4 ,heated on charcoal1 it fuses to a clear bead2 but1 if the sulphate of lime be present1 the bead becomes opaque upon cooling4 ,the following reaction is a certain one3 the substance is pulverized and mixed with a flux of four and a half parts of bisulphate of potassa1 and one part of pulverized fluoride of calcium4 ,the whole is made into a paste with water1 and the assay is placed on the platinum wire1 and submitted to the point of the blue flame4 ,while the assay is melting1 fluoboric gas is disengaged1 which tinges the outer flame green4 ,if but a small portion of boracic acid is present1 the color will be quite evanescent4 7#g47 ,silica1 ,silicic ,acid 7,si,o#c74--,this acid exists in the greatest plenty1 forming no inconsiderable portion of the solid part of this earth4 ,it exists nearly pure in crystallized quartz1 chalcedony1 cornelian1 flint1 etc41 the coloring ingredients of these minerals being generally iron or manganese4 ,with microcosmic salt1 silica forms a bead in the flame of oxidation which1 while hot1 is clear1 while the separated silica floats in it4 ,a platinum wire is generally used for the purpose1 the end of it being first dipped in the salt which is fused into a bead1 after which the silica must be added1 and then the bead submitted to the flame of oxidation4 ,the silicates dissolve in soda but partially1 and then with effervescence4 ,if the oxygen of the acid be twice that of the base1 a clear bead will be obtained that will retain its transparency when cold4 ,if the soda be added in small quantity1 the bead will then be opaque4 ,in the first instance1 a part of the base which separates is re-dissolved1 and1 therefore1 the transparency of the glass2 but1 if too large a quantity of the soda is added1 the separation of the base is sufficient to render the assay infusible4 7#h47 ,chlorine 7,cl74--,chlorine exists in nature always in combination1 as the chlorides of sodium1 potassium1 calcium1 ammonium1 magnesia1 silver1 mercury1 lead1 copper1 etc4 ,the chlorine existing in metallic chlorides may be detected as follows3 the wet way may be accomplished in the following manner4 ,if the substance is insoluble1 it must be melted with soda to render it soluble2 if it be already soluble it must be dissolved in pure water1 and nitrate of silver added1 when the one ten-thousandth part of chlorine will manifest its presence by imparting a milky hue to the fluid4 ,by the blowpipe1 chlorine may be detected in the following manner3 ,oxide of copper is dissolved in microcosmic salt on the platinum wire in the flame of oxidation1 and a clear bead is obtained4 ,the substance containing the chlorine is now added1 and heat is applied4 ,the assay will soon be enveloped by a blue or purplish flame4 ,as none of the acids that occur in the mineral kingdom give this reaction1 chlorine cannot be confounded with them1 for those which impart a color to the flame1 when mixed with a copper salt1 will not do so when tested in the microcosmic salt bead as above indicated4 ,if the assay is soluble in water1 the following method may be followed3 a small quantity of sulphate of copper or iron is dissolved2 a few drops of the solution is placed upon a bright surface of silver1 and the metallic chloride added2 when1 if chlorine is present1 the silver is blackened4 ,if the chloride is insoluble in water1 it must be rendered soluble by fusion upon a platinum wire with soda1 and then treated as above4#b #b ,plattner4 7#i47 ,bromine 7,br74--,the bromide of magnesium and sodium exists in many salt springs1 and it is from these that the bromine of commerce is obtained4 ,the metallic bromides give the same reactions on silver with the microcosmic bead and copper salt as the metallic chlorides4 ,the purplish color which1 however1 characterizes the chlorides1 is more inclined to greenish with the bromides4 ,if the substance be placed in a flask or glass tube1 and fused with bisulphate of potassa1 over the spirit-lamp1 sulphurous gas and bromine will be eliminated4 ,bromine will be readily detected by its yellow color and its smell4 ,bromine may be readily detected by passing a current of chlorine through the fluid1 after which ether is added and the whole is agitated4 ,the ether rises to the top1 carrying with it the bromine in solution2 after being withdrawn1 this ether is mixed with potassa1 by which the bromide and bromate of potassa are formed4 ,the solution is evaporated to dryness1 the residue is fused in a platinum vessel1 the bromate is decomposed1 while the bromide remains2 this must be distilled with sulphuric acid and the binoxide of manganese4 ,a red or brown vapor will then appear1 indicating the presence of bromine2 this vapor will color starch paste--which may be put in the receiver on purpose--of a deep orange color4 ,if1 to a solution containing a bromide1 concentrated sulphuric or nitric acid be added1 the bromine is liberated and colors the solution yellow or red4 ,the hypochlorites act in the same manner4 ,the bromine salts are coming into use extensively in photography1 in consequence of their greater sensitiveness to the action of light than the chlorides alone4 7#aj47 ,iodine 7,i74--,this element occurs in salt-springs1 generally combined with sodium2 it also exists in rock-salt2 it has likewise been found in sea-water1 also in a mineral from ,mexico1 in combination with silver1 and in one from ,silesia1 in combination with zinc4 ,as sea-water contains iodine1 we would consequently expect to find it existing in the sea-weeds1 and it is generally from the ashes of these that it is obtained in commerce4 ,when the metallic iodides are fused with the microcosmic salt and copper1 as previously indicated1 they impart a green color to the flame4 ,this color cannot be mistaken for the color imparted to the flame by copper alone4 ,when the metallic iodides are fused in a glass tube1 closed at one end1 with the bisulphate of potassa1 the vapor of iodine is liberated1 and may be recognized by its characteristic color4 ,those mineral waters containing iodine can be treated the same as for bromine1 as previously indicated1 while the violet-colored vapor of the iodine can be easily discerned4 ,the nitrate of silver is the best test for iodine1 the yellow color of the iodide of silver being not easily mistaken1 while its almost insolubility in ammonia will confirm its identity4 ,the chloride of silver1 on the contrary1 dissolves in ammonia with the greatest facility4 ,the reactions of iodine are similar to those of bromine with concentrated sulphuric acid and binoxide of manganese1 and with nitric acid3 ,the iodine is released and1 if the quantity be not too great1 colors the liquid brown4 ,if there be a considerable quantity of iodine present1 it is precipitated as a dark colored powder4 ,either of these1 when heated1 gives out the violet-color of the iodine4 ,with starch paste free iodine combines1 producing a deep blue compound4 ,if1 however1 the iodine be in very minute quantity1 the color1 instead of being blue1 will be light violet or rose color4 ,if to a solution of the sulphate of copper1 to which a small portion of sulphurous acid has been added1 a liquid containing iodine and bromine is poured in1 a dirty1 white precipitate of the subiodide of copper is produced1 and the bromine remains in the solution4 ,the latter may then be tested for the bromine by strong sulphuric acid4 7#aa47 ,fluorine 7,fl74--,this element exists combined with sodium1 calcium1 lithium1 aluminium1 magnesium1 yttrium1 and cerium4 ,fluorine also exists in the enamel of the teeth1 and in the bones of some animals4 ,this element has a strong affinity for hydrogen1 and1 therefore1 we find it frequently in the form of hydrofluoric acid4 ,brazil-wood paper is the most delicate test for hydrofluoric acid1 which it tinges of a light yellow color4 ,phosphoric acid likewise colors ,brazil paper yellow1 but as this acid is not volatile at a heat sufficient to examine hydrofluoric acid1 there can be no mistake4 ,if the substance is supposed to contain this acid1 it should be placed on a slip of glass1 and moistened with hydrochloric acid1 when the test paper may be applied1 and the characteristic yellow color will indicate the presence of the fluorine4 ,as hydrofluoric acid acts upon glass1 this property may be used for its detection4 ,the substance may be put into a glass tube1 and sulphuric acid poured upon it in sufficient quantity to moisten it2 a slight heat applied to the tube will develop the acid1 which will act upon the glass of the tube4 ,if the acid is retained in the mineral by a feeble affinity1 and water be present1 a piece of it may be put in the tube and heated1 when the acid gas will be eliminated4 ,the test paper will indicate its presence1 even before it has time to act upon the glass4 ,if the temperature be too high1 fluosilicic acid is generated1 and will form a silicious incrustation upon the cool portion of the tube4 ,if the fluorine is too minute to produce either of the above reactions1 then the following process1 recommended by ,plattner1 should be followed3 the assay should be mixed with metaphosphate of soda1 formed by heating the microcosmic salt to dull redness4 ,the mass must then be placed in an open glass tube1 in such a position that there will be an access of hot air from the flame4 ,thus aqueous hydrofluoric acid is formed1 which can be recognized by its smell being more suffocating than chlorine1 and also by the etching produced by the condensation of vapor in the tube4 ,moist ,brazil paper1 applied to the extremity of the tube1 will be instantly colored yellow4 ,merlet's method for the detection of this acid is the following3#c ,pulverize the substance for examination1 then triturate it to an impalpable powder1 and mix it with an equal part of bisulphate of potassa4 ,heat the mass gradually in a moderately wide test-tube4 ,the judicious application of heat must be strictly observed1 for if the operator first heats the part of the tube where the assay rests1 the whole may be lost on account of the glass being shattered4 ,the spirit-flame must be first applied to the fore part of the tube1 and then made to recede slowly until it fuses the assay4 ,after the mixture has been for some time kept in a molten state1 the lamp must be withdrawn1 and the part containing the assay severed with a file4 ,the fore part of the tube must then be well washed1 and afterwards dried with bibulous paper4 ,should the fluorine contained in the substance be appreciable1 the glass tube1 when held up to the light1 will be found to have lost its transparency1 and to be very rough to the touch4 #c ,quoted by ,plattner4 ,great care should be observed not to allow this very corrosive acid to come into contact with the skin1 as an ulcer will be the consequence that will be extremely difficult to heal4 ,when hydrofluoric acid comes in contact with any silicious substance1 hydrofluosilicic acid gas is always formed4 7#ab47 ,selenium 7,se74--,this element occurs in combination with lead as the selenide1 and with copper as the selenide of copper4 ,it exists also combined with cobalt and lead1 as the selenide of these metals2 also as the selenide of lead and mercury4 ,the smallest trace of selenium may be detected by igniting a small piece of charcoal in the flame of oxidation1 when the peculiar and unmistakable odor of decayed horse-radish will indicate the presence of that element4 ,an orange vapor is eliminated if the selenium be present in any quantity1 while there is an incrustation around the assay of a grey color1 with a metallic lustre4 ,this incrustation frequently presents a reddish-violet color at its exterior edges1 often running into a deep blue4 ,if a substance containing selenium be placed in a glass tube1 closed at one end1 and submitted to heat1 the selenium is sublimed1 with an orange-colored vapor1 and with the characteristic odor of that substance4 ,upon the cool portions of the tube a steel-grey sublimate is deposited1 and1 beyond that1 can be discerned small crystals of selenic acid4 ,if the mineral be the seleniferous lead glance1 sulphurous acid gas will be given off1 and may be detected by the smell1 or by a strip of moistened litmus paper4 ,if arsenic is present1 heating upon charcoal will quickly lead to the determination of the one from the other4 99 99 99 99 99 ,,tabular ,,statement ,,of ,,the ,,reactions ,,of ,,minerals ,,before ,,the ,,blowpipe4 ,in ,,part ,,third of this work1 commencing at page #aji1 the student will find a sufficiently explicit description of the blowpipe reactions of those principal substances that would be likely to come beneath his attention4 ,the following tabular statement of those reactions--which we take from ,scheerer and ,blanford's excellent little work upon the blowpipe--will be of great benefit1 as a vehicle for consultation1 when the want of time--or during the hurry of an examination--precludes the attentive perusal of the more lengthy descriptions in the text4 ,in the examination of minerals1 before the student avails himself of the aid of the blowpipe1 he should not neglect to examine the specimen rigidly in relation to its physical characters1 such as its hardness1 lustre1 color1 and peculiar crystallization4 ,it is where the difference of two minerals cannot be distinguished by their physical appearance1 that the aid of the blowpipe comes in most significantly as an auxiliary4 ,for instance1 the two minerals molybdenite and graphite resemble each other very closely1 when examined in regard to their physical appearance1 but the blowpipe will quickly discriminate them1 for if a small piece of the former mineral be placed in the flame of oxidation1 a bright green color will be communicated to the flame beyond it1 while in the latter there will be no color4 ,thus1 in a very short time1 these two minerals can be distinguished from each other by aid of the blowpipe1 while no amount of physical examination could determine that point4 ,the blowpipe is equally an indispensable instrument in the determination of certain minerals which may exist in others as essential or non-essential constituents of them4 ,for instance1 should a minute quantity of manganese be present in a mineral1 it must be fused with twice its bulk of a mixture of two parts of carbonate of soda1 and one part of the nitrate of potassa1 in the flame of oxidation upon platinum foil4 ,the manganate of soda thus formed will color the fused mass of a bluish-green tint4 ,or a slight quantity of arsenic may be discerned by the following process recommended by ,plattner3#d one grain of the finely pulverized metal is mixed with six grains of citrate of potassa1 and slowly heated on the platinum spoon4 ,by this means the metals are oxidized1 while the arseniate of potassa is obtained4 ,then boil the fused mass in a small quantity of water in a porcelain vessel till all tho arseniate is dissolved4 ,the metallic oxides are allowed to subside1 and the above solution decanted off into another porcelain vessel4 ,a few drops of sulphuric acid are added1 and the solution boiled to expel the nitric acid1 after which it is evaporated to dryness4 ,in this operation1 the sulphuric acid should be added only in sufficient quantity to drive off the nitric acid1 or1 at the utmost1 to form a bisulphate with the excess of potassa4 ,when dry1 the salt thus obtained is pulverized in an agate mortar1 and mixed with about three times its volume of oxalate of potassa1 and a little charcoal powder4 ,the mixture is introduced into a glass bulb having a narrow neck1 and gently warmed over a spirit-lamp in order to drive off the moisture1 which must be absorbed by a piece of blotting-paper in the neck of the bulb4 ,after a short time1 the temperature is increased to a low red heat1 at which the arsenious acid is reduced and the metallic arsenic sublimed1 and which re-condenses in the neck of the bulb4 ,if there the arsenic be so small in quantity as to exhibit no metallic lustre1 the neck of the bulb may be cut off with a file immediately above the sublimate1 and the latter exposed to the flame of the blowpipe1 when the arsenic is volatilized1 and may be recognized by its garlic odor4 #d ,quoted by ,scheerer4 ,if the presence of cadmium is suspected in zinc-blende1 it may be detected by fusing a small piece of the blende upon charcoal in carbonate of soda4 ,the peculiar bright yellow sublimate of the oxide of cadmium1 if it be present1 will not fail to indicate it4 ,this incrustation can be easily distinguished from that of zinc4 ,thus1 with the three illustrations we have given1 the student will readily comprehend the great utility of the blowpipe in the examination of minerals4 ,although the following tables were not arranged especially for the last part of this work1 still this arrangement is so good that by their consultation the student will readily comprehend at a glance what requires some detail to explain1 and we feel no hesitation in saying that1 although they are not very copious1 they will not fail to impart a vast amount of information1 if consulted with any degree of carefulness4 ,the minerals given are such as are best known to ,english and ,american mineralogists under the names specified4 ,for more detailed reactions than could be crowded into a table1 the student will have to consult the particular substance as treated in ,part ,third4 ,if this part is perused carefully previous to consulting the tables1 these will be found eminently serviceable as a refresher of the memory1 and may thus save much time and trouble4 ,and1 finally1 we would certainly recommend the student1 after he shall have gone through our little volume 7if he is ambitious of making himself a thorough blowpipe analyst71 to then take up the larger works of ,berzelius and ,plattner1 for our treatise pretends to nothing more than a humble introduction to these more copious and scientific works4 99 99 99 99 99 ,mineral4 ,diamond ,formula4 ,c ,behavior in glass-bulb4 -- on platinum foil4 ,in fine powder is slowly consumed without residue in a strong oxidizing ,flame4 99 99 99 99 99 ,mineral4 ,graphite ,formula4 ,c with some iron silica1 etc4 ,behavior in glass-bulb4 ,generally gives off water4 on platinum foil4 ,is slowly consumed leaving more or less ash1 principally ,fe#b,o#c4 99 99 99 99 99 ,mineral4 ,anthracite ,formula4 ,c x4,h ,behavior in glass-bulb4 ,evolves water4 on platinum foil4 ,is slowly consumed with the exception of a small quantity of ash4 99 99 99 99 99 ,mineral4 ,wallsend-coal ,formula4 ,c1 ,h1 ,o1 ,s and ash4 ,behavior in glass-bulb4 ,intumesces and gives off water and tarry matters which partly condense in bulb1 and leave a porous coke4 on platinum foil4 ,takes fire under blowpipe flame1 and burns with a smoky flame1 depositing much soot and leaving a porous cinder which burns slowly and leaves a small ash4 99 99 99 99 99 ,mineral4 ,cannel-coal ,formula4 ,c1 ,h1 ,n1 ,o1 ,s and ash4 ,behavior in glass-bulb4 ,as the preceding but gives off more tar4 on platinum foil4 ,similar to the preceding4 ,if held to the lamp-flame1 takes fire and burns for some seconds4 99 99 99 99 99 ,mineral4 ,brown-coal ,formula4 ,c1 ,h1 ,n1 ,o1 ,s1 and ash4 ,behavior in glass-bulb4 ,gives off much water and tar1 and leaves a porous cinder retaining the form of the original fragment4 on platinum foil4 ,burns slowly and without flame1 leaving some ash4 99 99 99 99 99 ,mineral4 ,asphaltum ,formula4 ,c ,h ,o4 ,behavior in glass-bulb4 ,fuses with ease affording an empyreumatic oil having an alkaline reaction1 and combustible gasses1 and leaves a carbonaceous residue1 which is entirely consumed under the blowpipe flame1 except a little ash4 on platinum foil4 ,takes fire and burns with a bright flame and a thick smoke4 99 99 99 99 99 ,mineral4 ,elaterite ,formula4 ,c ,h4 ,behavior in glass-bulb4 ,fuses and gives off water having an acid reaction1 naphtha and a tarry fluid1 which chiefly condense in the neck of the bulb1 and leave a light1 pulverulent carbonaceous residue4 on platinum foil4 ,fuses1 takes fire1 and burns with a smoky flame1 leaving a carbonaceous residue1 which under the blowpipe flame1 is quickly consumed1 with the exception of the ashes4 99 99 99 99 99 ,mineral4 ,hachettine ,formula4 ,c ,h4 ,behavior in glass-bulb4 ,fuses to a clear colorless liquid1 which solidifies on cooling and has a tallow-like smell4 on platinum foil4 ,fuses1 takes fire1 and burns with a bright flame until entirely consumed4 99 99 99 99 99 ,mineral4 ,ozokerite ,formula4 ,c ,h4 ,behavior in glass-bulb4 ,fuses readily to a clear brown oily fluid1 which solidifies on cooling4 on platinum foil4 ,as the preceding4 99 99 99 99 99 ,mineral4 ,amber ,formula4 ,c ,h ,o4 ,behavior in glass-bulb4 ,fuses with difficulty1 and affords water1 an empyreumatic oil1 and succinic acid which condense in the neck of the bulb leaving a shining black residue4 on platinum foil4 ,takes fire and burns with a yellow flame and a peculiar aromatic odor4 99 99 99 99 99 ,mineral4 ,mellite ,formula4 444,al,m#c #ae4;,h ,behavior in glass-bulb4 ,gives off water4 ,if heated to redness1 is carbonized1 and gives a slight empyreumatic odor4 on platinum foil4 ,on charcoal burns to a white ash1 which moistened with nitrate of cobalt and heated shows the alumina reaction4 99 99 99 99 99 ,,potash4 99 99 99 99 99 ,mineral4 ,nitre ,formula4 4,k44444,n ,behavior 7#a7 in glass-bulb4 ,fuses readily to a clear liquid and with a strong heat boils with the evolution of oxygen4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,deflagrates leaving a saline mass1 which is absorbed into charcoal and gives a sulphur reaction on silver4 7#d7 in forceps4 ,on platinum wire fuses and colors the flame violet more or less modified by lime and soda4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,with bisulphate of potassa in the glass-bulb evolves nitrous fumes4 99 99 99 99 99 ,mineral4 ,polyhalite ,formula4 4,k444,s4,mg444,s#b4;,ca444,s#b4;,h ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a reddish bead1 which in the reducing flame solidifies and shrinks to a hollow crust4 7#d7 in forceps4 ,on platinum wire fuses and colors the flame yellow from a small quantity of soda4 7#e7 in borax4 ,dissolves with ebullition to a clear glass1 which is slightly colored by iron1 and when saturated become opaque on cooling4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses4 ,the alkalies are absorbed by the charcoal leaving the lime and magnesia infusible on the surface4 7#h7 ,special reactions4 ,the alkaline mass when laid on silver gives a sulphur reaction4 99 99 99 99 99 ,,soda4 99 99 99 99 99 ,mineral4 ,rock-salt ,formula4 ,na,cl4 ,behavior 7#a7 in glass-bulb4 ,fuses to a clear liquid 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 is absorbed by the charcoal and partially volatilized incrusting the charcoal around4 7#d7 in forceps4 ,fuses with great ease and colors the flame yellow4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,gives the chlorine reactions4 99 99 99 99 99 ,mineral4 ,natron ,formula4 4,na44,c #aj4;,h ,behavior 7#a7 in glass-bulb4 ,fuses1 with the evolution of water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 and is absorbed into the pores of the charcoal4 7#d7 in forceps4 ,fuses and behaves as the preceding4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,dissolves in acid with violent effervescence4 99 99 99 99 99 ,mineral4 ,soda-nitre ,formula4 4,na44444,n4 ,behavior 7#a7 in glass-bulb4 ,fuses and if strongly heated evolves nitrous fumes4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,deflagrates and is absorbed into the charcoal4 7#d7 in forceps4 ,deflagrates on platinum wire1 coloring the flame yellow4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,in a glass-bulb with bisulphate of potassa1 gives the ,,no#e-reaction4 99 99 99 99 99 ,mineral4 ,glauber-salt ,formula4 4,na444,s #aj4;,h4 ,behavior 7#a7 in glass-bulb4 ,fuses and gives off water having a neutral reaction4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 and is absorbed by the charcoal4 ,the saturated charcoal laid upon silver gives the sulphur reaction 7#d7 in forceps4 ,fuses and colors the flame yellow4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,gives the ,,so#c-reaction4 99 99 99 99 99 ,mineral4 ,glauberite ,formula4 4,na444,s 4,ca444,s4 ,behavior 7#a7 in glass-bulb4 ,decrepitates with the evolution of more or less water1 and when strongly heated fuses to a clear liquid4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a clear bead1 then spreads out2 the soda is absorbed and the lime left on the surface4 ,laid on silver1 the fused mass gives a sulphur reaction4 7#d7 in forceps4 ,fuses easily to a clear glass1 coloring the flame yellow4 7#e7 in borax4 ,fuses easily and gives the lime reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone in charcoal4 7#h7 ,special reactions4 ,as in preceding4 99 99 99 99 99 ,mineral4 ,borax ,formula4 4,na444,b#baj4;,h4 ,behavior 7#a7 in glass-bulb4 ,intumesces with the evolution of water1 and under a strong heat fuses4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,intumesces and fuses to a clear bead more or less colored by impurities4 7#d7 in forceps4 ,as on charcoal4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,fuses to a clear bead1 which becomes crystalline on cooling4 7#h7 ,special reactions4 ,gives the boracic-acid-reaction4 99 99 99 99 99 ,mineral4 ,cryolite ,formula4 #c,na,fl,al#b;,fl#c4 ,behavior 7#a7 in glass-bulb4 ,decrepitates slightly and gives a trace of water4 7#b7 in open tube4 ,if heated so that the flame be allowed to play up the tube upon the mineral1 flourine is evolved1 which corrodes the interior of the tube4 7#c7 on charcoal4 ,fuses to a limpid bead1 which on cooling becomes a white enamel4 ,if heated for some time1 it bubbles1 gives off fluorine and becomes infusible4 7#d7 in forceps4 ,fuses1 coloring the flame yellow4 7#e7 in borax4 ,dissolves to a clear bead1 which is rendered opaque by a large addition4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a clear bead1 then spreads out on the charcoal1 the soda is absorbed1 and an infusible mass of alumina remains4 7#h7 ,special reactions4 ,if the alumina residue obtained be moistened with cobalt solution and heated strongly1 it assumes a beautiful blue color4 99 99 99 99 99 ,,baryta ,,and ,,strontia4 99 99 99 99 99 ,mineral4 ,heavy-spar ,formula4 4,ba444,s4 ,behavior 7#a7 in glass-bulb4 ,sometimes decrepitates and gives off more or less water 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses in the reducing flame4 7#d7 in forceps4 ,fuses with difficulty on edges4 ,colors the outer flame green4 ,in reducing flame forms ,ba,s1 which fuses readily4 7#e7 in borax4 ,gives the baryta-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a clear bead2 then spreads out and is absorbed into the charcoal4 ,the fused mass laid on silver gives the ,s-reaction4 7#h7 ,special reactions4 ,if fused with potassa on platinum1 gives the ,,so#c-reaction4 99 99 99 99 99 ,mineral4 ,celestine ,formula4 4,sr444,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a milk-white bead4 7#d7 in forceps4 ,colors the flame crimson4 7#e7 in borax4 ,gives the strontia-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,similar to the preceding4 7#h7 ,special reactions4 ,similar to the preceding4 99 99 99 99 99 ,mineral4 ,witherite ,formula4 4,ba44,c4 ,behavior 7#a7 in glass-bulb4 ,decrepitates more or less and evolves ,water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 effervesces1 and is partially absorbed by the charcoal4 7#d7 in forceps4 ,colors the outer flame intensely green4 7#e7 in borax4 ,dissolves with effervescence and gives the baryta-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a clear bead2 then spreads out and passes into the charcoal4 7#h7 ,special reactions4 ,in dilute ,h,cl dissolves with much effervescence4 99 99 99 99 99 ,mineral4 ,strontianite ,formula4 4,sr44,c4 ,behavior 7#a7 in glass-bulb4 ,becomes opaque4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,as in the forceps4 7#d7 in forceps4 ,exfoliates and becomes arborescent4 ,the filaments glow brilliantly and fuse on the point4 ,colors the flame brilliantly crimson4 7#e7 in borax4 ,resembles the preceding4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,as the preceding4 99 99 99 99 99 ,mineral4 ,barytocalcite4 ,formula4 4,ba44,c 4,ca44,c4 ,behavior 7#a7 in glass-bulb4 ,as in the preceding4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in powder frits together1 but does not fuse4 7#d7 in forceps4 ,colors the flame green in the centre and red towards the point4 7#e7 in borax4 ,dissolves with effervescence4 ,in large quantities gives a semi-crystalline bead4 7#f7 in mic4 salt4 ,as in borax1 but the saturated bead is milk-white4 7#g7 with carb4 soda4 ,fuses1 and is partially absorbed leaving the lime on the surface4 7#h7 ,special reactions4 ,as witherite4 99 99 99 99 99 ,,lime4 99 99 99 99 99 ,mineral4 ,gypsum ,formula4 4,ca444,s #b4;,h4 ,behavior 7#a7 in glass-bulb4 ,turns white1 giving off water and being converted into plaster of ,paris4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in the reducing flame forms ,ca,s1 which has an alkaline reaction on test paper1 and gives a sulphur-reaction when laid on silver and moistened4 7#d7 in forceps4 ,fuses with difficulty to a bead1 coloring the flame red4 7#e7 in borax4 ,dissolves to a clear bead1 which gives the lime- reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,behaves as lime4 ,the alkaline mass laid on silver and moistened gives the sulphur-reaction4 7#h7 ,special reactions4 ,gives the sulphuric-acid reaction4 99 99 99 99 99 ,mineral4 ,apatite ,cl ,formula4 4,ca -- #c4;,ca#c44444,p ,fl ,behavior 7#a7 in glass-bulb4 ,occasionally decrepitates and gives off some water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,,iv4 ,previously dipped in ,,so#c colors the flame green1 afterwards red4 7#e7 in borax4 ,dissolves easily and when in some quantity gives an opaline bead4 7#f7 in mic4 salt4 ,gives the lime-reaction4 7#g7 with carb4 soda4 ,is infusible4 ,the alkali is absorbed1 leaving the lime on the on the surface of the charcoal4 7#h7 ,special reactions4 ,with microcosmic salt and oxide of copper1 gives the chlorine-reaction4 ,with microcosmic salt in the open tube evolves fluorine4 99 99 99 99 99 ,mineral4 ,pharmacolite ,formula4 4,ca#b44444;,as #f4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water1 and emits an arsenical odor4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to an opaque bead and emits a strong smell of arsenic4 7#d7 in forceps4 ,fuses to a translucent violet colored bead1 the color being due to cobalt4 ,colors the flame blue at first1 then faintly red4 7#e7 in borax4 ,dissolves readily to a bead strongly colored by cobalt1 which obscures the lime-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses1 and emits ,as4 ,the alkali is then absorbed by the charcoal1 as in the preceding4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,calespar ,formula4 4,ca44,c4 ,behavior 7#a7 in glass-bulb4 ,turns white and sometimes decrepitates4 ,strongly heated loses ,,co#b and becomes caustic4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,turns white1 or brown if containing much iron or manganese and glows brilliantly4 7#d7 in forceps4 ,glows brilliantly1 coloring the flame red4 ,becomes caustic and shows a strong alkaline reaction4 7#e7 in borax4 ,dissolves with evolution of ,,co#b and when pure gives the lime-reaction4 ,the bead is generally more or less colored by iron and manganese4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses1 and behaves as other lime-salts4 7#h7 ,special reactions4 ,dissolves with effervescence in cold ,h,cl4 99 99 99 99 99 ,mineral4 ,fluorspar ,formula4 ,ca,fl ,behavior 7#a7 in glass-bulb4 ,phosphoresces with various colors1 when heated in the dark4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses easily to a clear bead1 which becomes opaque on cooling1 then loses fluorine1 glows brilliantly and becomes infusible4 7#d7 in forceps4 ,as on charcoal4 ,colors the flame red4 7#e7 in borax4 ,gives the lime-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a clear bead1 opaque on cooling4 ,with an addition of the alkali behaves as lime4 7#h7 ,special reactions4 ,with microcosmic salt in open tube gives the fluorine-reaction4 99 99 99 99 99 ,,magnesia4 99 99 99 99 99 ,mineral4 ,brucite ,formula4 4,mg4,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 7#e7 in borax4 ,behaves as magnesia4 ,sometimes gives a faint iron-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,behaves as magnesia4 7#h7 ,special reactions4 ,with nitrate of cobalt1 gives the magnesia reaction 99 99 99 99 99 ,mineral4 ,epsomite ,formula4 4,mg444,s #g4;,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water having an acid reaction on test paper4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,gives of ,,ho and ,,so#c1 shines brilliantly1 and becomes alkaline and caustic4 7#d7 in forceps4 ,v4 ,as on charcoal4 7#e7 in borax4 ,behaves as magnesia4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,the alkali is absorbed leaving the magnesia on surface of the charcoal4 ,gives the sulphur-reaction on silver4 7#h7 ,special reactions4 ,the magnesian residue obtained on treating with carbonate of soda 7#g71 assumes a flesh-tint1 when treated with cobalt4 99 99 99 99 99 ,mineral4 ,boracite ,formula4 4,mg444,b#b #b4,mg444,b4 ,behavior 7#a7 in glass-bulb4 ,occasionally gives off a trace of water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses with intumescence to a white crystalline bead4 7#d7 in forceps4 ,i4 ,as on charcoal4 ,colors the flame green4 7#e7 in borax4 ,fuses easily to a clear bead1 which is crystalline1 when containing much of the mineral1 and is usually slightly tinted by iron4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,with a small quantity of alkali fuses to a clear bead on cooling4 ,with a larger quantity gives a clear1 uncrystallizable bead4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,magnesite ,formula4 4,mg44,c4 ,behavior 7#a7 in glass-bulb4 ,sometimes gives off a small quantity of water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,is infusible4 ,with cobalt-solution1 assumes a dusky flesh tint4 7#d7 in forceps4 -- 7#e7 in borax4 ,behaves as magnesia4 ,sometimes a slight iron-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a bead1 the soda is then absorbed1 leaving an infusable mass of magnesia4 7#h7 ,special reactions4 ,the magnesian residue obtained by fusing with carbonate of soda gives the magnesian-reaction with nitrate of cobalt4 ,dissolves with effervescence in warm ,h,cl4 99 99 99 99 99 ,mineral4 ,mesitine spar ,formula4 74,mg4,fe4,mn744,c4 ,behavior 7#a7 in glass-bulb4 ,as magnesite4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,is infusible4 ,assumes a deep brown color4 7#d7 in forceps4 ,v4 7#e7 in borax4 ,gives the iron and manganese-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as magnesite1 but the residual mass has a dark color from iron and manganese4 7#h7 ,special reactions4 ,dissolves with effervescense in warm ,h,cl4 ,with carbonate of soda and nitre gives a manganese-reaction4 99 99 99 99 99 ,,alumina4 99 99 99 99 99 ,mineral4 ,sapphire ,corundum ,emery ,formula4 444,al4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 7#e7 in borax4 ,in fine powder dissolves slowly to a colorless glass4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,in fine powder moistened with cobalt-solution and heated yields a blue color4 99 99 99 99 99 ,mineral4 ,websterite ,formula4 444,al444,s #i4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water1 and1 when heated to incipient redness1 sulphurous acid4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,gives off water and ,,so#c1 leaving an infusible mass4 7#d7 in forceps4 ,v4 7#e7 in borax4 ,behaves as alumina4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,yields an infusible mass1 which laid on silver and moistened1 produces a black stain4 7#h7 ,special reactions4 ,fused with potassa in platinum has no action on silver4 ,cobalt-solution produces the alumina reaction4 99 99 99 99 99 ,mineral4 ,native ,alum ,formula4 4,r444,s 444,al444,s#c #bd4;,h4 ,behavior 7#a7 in glass-bulb4 ,intumesces greatly and gives off much water4 ,strongly heated1 evolves ,,so#c1 which reddens litmus4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,intumesces and become infusible4 7#d7 in forceps4 ,v4 ,colors the flame violet if a potassa alum--yellow if soda--be present4 7#e7 in borax4 ,dissolves and gives the iron and manganese reaction1 if these oxides be present4 ,otherwise the bead is colorless4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,the alkali is absorbed into the charcoal1 leaving an infusable mass which gives the sulfur reaction on silver4 7#h7 ,special reactions4 ,if not containing too much iron or manganese gives an alumina reaction with nitrate of of cobalt4 ,in other respects as the preceding4 99 99 99 99 99 ,mineral4 ,turquoise ,formula4 444,al#b44444,p #e4;,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water1 occasionally decrepitates and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,turns brown1 but remains infusible4 7#d7 in forceps4 ,v4 ,as on charcoal4 ,colors the outer flame green4 7#e7 in borax4 ,in the oxidizing flame1 gives a green bead1 due to copper and iron4 ,in reducing flame1 opaque red4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,intumesces1 then fuses to a semi-clear glass colored by iron4 ,with more alkali yields an infusible mass4 7#h7 ,special reactions4 ,gives the phosphoric-acid reaction4 99 99 99 99 99 ,mineral4 ,wavellite ,formula4 ,al,f#c #c7444;,al#d44444,p#c #ah4;,h47 ,behavior 7#a7 in glass-bulb4 ,evolves water and some fluorine1 which attacks the glass4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,exfoliates and turns white4 7#d7 in forceps4 ,v4 ,as on charcoal4 ,colors the outer flame green1 especially if moistened with ,,so#c4 7#e7 in borax4 ,as alumina4 ,generally gives also a slight iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms an infusible white mass4 7#h7 ,special reactions4 ,with cobalt-solution on charcoal gives the alumina reaction4 99 99 99 99 99 ,mineral4 ,spinel ,formula4 4,r444,al4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 7#e7 in borax4 ,gives a slight iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses partially and forms a porous mass4 7#h7 ,special reactions4 ,with nitrate of cobalt gives the alumina reaction4 ,with nitre and carbonate of soda a slight manganese reaction4 99 99 99 99 99 ,,silicates4 ,the presence of silica in a mineral can easily be ascertained by treating a small fragment in a bead of microcosmic salt4 ,the bases will dissolve out with more or less difficulty in the salt1 and the silica being insoluble will remain suspended in the bead1 retaining the original form of the fragment4 ,in borax1 the silicates of lime and magnesia generally dissolve with considerable ease1 but those of alumina slowly and with difficulty4 ,the silicates of lime are moreover frequently characterized by intumescence or ebullition1 when heated in the forceps in the blowpipe flame4 ,the minerals presenting this character are marked in the table4 ,as the most convenient mode of classifying the silicates for blowpipe examination1 the following arrangement will be adopted3 ,,table ,i4--,,anhydrous ,,silicates4 ,,table ,,ii4--,,hydrous ,,silicates4 ,,fusibility4 ,i4 ,readily fusible to a bead4 ,,ii4 ,with difficulty fusible to a bead4 ,,iii4 ,readily fusible on the edges4 ,,iv4 ,with difficulty fusible on the edges4 ,v4 ,infusible4 a4 ,afford a fluid bead with carbonate of soda4 b4 ,afford a fluid bead with but little of that salt1 but with a larger quantity a slaggy mass4 c4 ,afford a slaggy mass only4 ,this classification of minerals1 according to their fusibility and their behavior with carbonate of soda1 was originally proposed by ,berzelius1 and a table of the principal oxidized minerals arranged according to these characters is given in his handbook of the blowpipe1 and thence adopted1 with some alterations by ,plattner1 in the very excellent and detailed work already many times cited4 ,in the following general table ,i41 the more important silicates only are included1 and in table ,,ii4 are enumerated in alphabetical order those which afford characteristic reactions4 ,,table ,i4 ,anhydrous ,silicates4 ,fus4 alone and with ,na,c4 ,mineral4 ,formula4 ,i4 a4 ,axinite 74,ca4,mg7#c7444;,b444,si7#c 7444,al444,fe444,mn7#b7444,si444,b7 ,int4 ,elaolite 74,k4,na7#c444,si #c444;,al444,si ,int4 ,garnet 4,r#c444,si 4,r444,si ,oligoclase 4,na444,si 444,al444,si#b ,scapolite 74,ca4,na7#c444,si#b #b444;,al444,si ,int4 ,spodumene 74,li4,na7#c444,si#b #d444;,al444,si#b;,int4 b4 ,asbestos ,as ,hornblende to ,,ii4 ,augite 74,ca4,mg4,fe4,mn7#c444,si#b ,int4 some var4 ,epidote 74,ca,fe7#c444,si ,int4 to ,,iii4 #b7444;,al444,fe444,mn7444,si ,hornblende 74,ca4,mg4,fe7#d 7444,si444,al7#c ,int4 some var4 ,sodalite 4,na#c444,si #c444;,al444,si ,na,cl ,int4 to ,,iii4 ,vesuvian #c74;,ca4,mg7#c444,si #b7444;,al444,fe7444,si ,int4 c4 ,biaxial ,mica 4,k444,si #d7444;,al444,fe7444,si to ,,iii4 ,hauyne 74,k4,na7#c444,si #c444;,al444,si 4,na444,si ,tourmaline 74,r444,r444,b7#d444,si#c ,int4 to ,v4 ,,ii4 a4 ,labradorite 74,ca4,na4,k7444,si 7444,al444,fe7444,si ,lepidolite 7,k,na,l7,f 7444,al444,fe7444,si#b8 ,ryacolite 4,k444,si 444,al444,si#b ,albite 4,na444,si 444,al444,si#c b4 ,augite 4,r#c444,si#b some var4 ,actinolite 74,ca4,mg4,fe7#d444,si#c ,int4 ,diopside 74,ca4,mg7#c444,si#b ,humboltilite #b74;,ca4,mg4,na4,k7444,si 7444,al444,fe7444,si ,sahlite ,as ,augite ,tremolite 74,ca4,mg7#d444,si#c c4 ,pyrope 74,ca4,mg4,fe7#c444,si ,al444,si m444,cr8 ,,iii4 a4 ,anorthite 74,ca4,mg4,na4,k7#c444,si #c7444;,al444,fe7444,si ,nepheline 74,na4,k4,ca7#b444,si #b444;,al444,si ,obsidian 444,si1444,al1444,fe14,fe14,ca4,na4,k ,int4 ,orthoclase 74,k4,na7444,si 444,al444,si#c ,petalite 74,li4,na7#c444,si#d #d444;,al444,si#d ,pumice 444,si1444,al14,ca14,k14,na14,h ,int4 b4 ,gadolinite 74,y4,ce4,la4,fe4,ca7#c444,si to ,v4 ,nephrite 74,ca4,mg4,fe7#d444,si#c8 ,int4 ,wollastonite 4,ca#c444,si#b c4 ,iolite 74,mg4,fe7#c444,si#b #c444;,al444,si ,,iv4 a4 ,beryl 444,be444,si#b 444,al444,si#b b4 ,diallage 74,ca4,mg4,fe7#c7444,si444,al7#b ,hypersthene 74,mg4,fe7#c444,si#b c4 ,fuchsite 74,k#e444,si7#b #i7444;,al444,cr7#f444,si#f ,v4 a4 ,leucite 4,k#c444,si#b 444,al444,si#b b4 ,chondrodite 74,mg14,mg,f7#d7444,si,si,f#c7 ,olivine 74,mg4,fe4,ca7#b444,si c4 ,andalusite 7444,al,fe7#c444,si#b ,chrysoberyl 444,be 444,al ,kaynite 444,al#c444,si#b ,pycnite #f444;,al#c444,si#b 7#c444;,al,f#c #b444,si,f#c7 ,topaz #f444;,al#c444,si#b 7#c444;,al,f#c #b444,si,f#c7 ,zircon 444,zr444,si ,staurolite 7444,al,fe7#b444,si ,hydrous ,silicates4 ,fus4 alone and with ,na,c4 ,mineral4 ,formula4 ,i4 a4 ,analcime 4,na#c444,si#b #c444;,al444,si#b #f4;,h ,int4 ,apophyllite 74,k1 ,,kf77444,si1 ,si,f#c7 #f4;,ca444,si #ae4;,h ,int4 ,brewsterite 74,sr4,ba7444,si 444,al444,si#c #e4;,h ,int4 ,chabasite 74,ca14,na14,k7#c444,si #c444;,al444,si#b #ah4;,h ,int4 ,lapis ,lazuli 444,si1444,s1444,al1 ,fe1 4,ca1 4,na1 4,h ,laumonite 4,ca#c444,si#b #c444;,al444,si#b #ab4;,h ,int4 ,mesotype 74,na4,ca7444,si 444,al444,si #c4;,h ,int4 ,natrolite 4,na444,si 444,al444,si #b4;,h ,int4 ,prehnite 4,ca#b444,si 444,al444,si 4,h ,int4 ,scolezite 4,ca444,si 444,al444,si #c4;,h ,int4 ,thomsonite 74,ca4,na7#c444,si #c444;,al444,si #g4;,h ,int4 ,datholite #b4;,ca#c444,si 444,b#c444,si#b #c4;,h ,int4 ,heulandite 4,ca444,si 444,al444,si#c #e4;,h ,int4 ,stilbite 4,ca444,si 444,al444,si#c #f4;,h ,int4 b4 ,okenite 4,ca#c444,si#d #f4;,h ,int4 ,pectolite 74,ca4,na7#d444,si#c 4,h ,int4 c4 ,saponite #b4,mg#c444,si#b 444,al444,si #aj or #f4;,h ,,ii4 a4 ,antrimolite #c74;,ca4,k7444,si #e444;,al444,si #ae4;,h ,harmatome 444,ba444,si 444,al,s#b #e4;,h b4 ,brevicite 4,na444,si 444,al444,si #b4;,h ,orthite 4,r#c444,si 444,r444,si 74,h87 ,int4 ,,iii4 c4 ,pitchstone 444,si1444,al1 ,fe1 4,mg4,na1 4,k4,h ,talc to ,v4 4,mg#f444,si#e #b4;,h ,chlorite #c74,mg,fe7#c444,si 7444,al,fe7#b444,si #i4;,h ,pinite 444,si1444,al14,fe14,k14,mg14,h ,,iv4 a4 ,steatite 4,mg#f444,si#e #d4;,h c4 ,gilbertite 444,si1444,al14,fe14,mg14,h ,int4 ,meerschaum 4,mg444,si 4,h ,serpentine 4,mg#i444,si#d #f4;,h ,v4 a4 ,gismondine 74,ca4,k7#b444,si #b444;,al444,si #i4;,h ,,table ,,ii4 ,analcime ,if transparent becomes white and opaque when heated1 but on incipient fusion resumes its transparency and then fuses to a clear glass4 ,andalusite ,when powdered and treated with cobalt solution on charcoal1 assumes a blue color4 ,apophyllite ,fuses to a frothy white glass4 ,axinite ,imparts a green color to the blowpipe flame1 owing to the presence of boracic acid4 ,this reaction is especially distinct1 if the mineral be previously mixed with fluorspar and bisulphate of potassa4 ,beryl ,sometimes gives a chromium reaction in borax and microcosmic salt4 ,chabasite ,fuses to a white enamel4 ,chondrodite ,evolves fluorine in the glass tube1 both when heated alone and with microcosmic salt4 ,it sometimes also gives off a trace of water4 ,chrysoberyl ,is unattacked by carbonate of soda4 ,with nitrate of cobalt on charcoal the finely powdered mineral assumes a blue color4 ,datholite ,fuses to a clear glass and colors the flame green4 ,diallage ,frequently gives off water in small quantity4 ,fuchsite ,gives the chromium reaction with borax and microcosmic salt4 ,gadolinite ,that from ,hitteroe1 if heated in a partially covered platinum spoon to low redness1 glows suddenly and brilliantly4 ,hauyne ,affords the sulphur reaction both on charcoal and when fused with potassa4 ,it contains both sulphur and sulphuric acid4 ,hypersthene ,as ,diallage4 ,kyanite ,as ,andalusite4 ,lapis ,lazuli ,fuses to a white glass1 and when treated with carbonate of soda on charcoal1 gives the sulphur reaction on silver4 ,laumonite ,when strongly heated1 exfoliates and curls up4 ,lepidolite ,colors the blowpipe flame crimson1 from lithia2 also gives the fluorine reaction with microcosmic salt4 ,leucite ,some varieties1 when treated with cobalt solution1 assume a blue color4 ,meerschaum ,in the glass bulb frequently blackens and evolves an empyreumatic odor due to organic matter4 ,when this is burnt off1 it again becomes white1 and if moistened with nitrate of cobalt solution and heated1 assumes a pink color4 ,okenite ,behaves as ,apophyllite4 ,olivine ,some varieties give off fluorine1 when fused with microcosmic salt4 ,pectolite ,similar to ,apophyllite4 ,petalite ,imparts a slight crimson color to the flame1 like ,lepidolite4 ,prehnite ,as ,chabasite4 ,pycnite ,assumes a blue color1 when treated with nitrate of cobalt4 ,gives the fluorine reaction with microcosmic salt4 ,pyrope ,gives the chromium reaction with borax and microcosmic salt4 ,scolecite ,similar to ,laumonite1 but more marked4 ,scapolite ,occasionally contains a small quantity of lithia1 and colors the flame red when fused with fluorspar and bisulphate of potassa4 ,sodalite ,if mixed with one-fifth its volume of oxide of copper1 moistened to make the mixture cohere1 and a small portion placed upon charcoal and heated with the blue oxidizing flame1 the outer flame will be colored intensely blue from chloride of copper4 ,spodumene ,when not too strongly heated1 colors the blowpipe flame red1 when more strongly1 yellow4 ,stilbite ,as ,chabasite4 ,topaz ,when heated1 remains clear4 ,otherwise as ,pycnite4 ,tourmaline ,gives the boracic acid reaction with flourspar and bisulphate of potassa4 ,wollastonite ,colors the blowpipe flame faintly red from lime4 ,zircon ,the colored varieties become white or colorless and transparent1 when heated4 ,is only slightly attacked by carbonate of soda4 99 99 99 99 99 ,,uranium4 99 99 99 99 99 ,mineral4 ,pitchblende ,formula4 4,u444,u essentially4 ,behavior 7#a7 in glass-bulb4 ,evolves some water and a small quantity of sulphur1 sulphide of arsenic and metallic arsenic4 7#b7 in open tube4 ,evolves ,,so#b and a white sublimate of arsenious acid4 7#c7 on charcoal4 ,gives off arsenical fumes4 7#d7 in forceps4 ,,iii4 ,colors the flame blue beyond the assay1 owing to the presence of ,pb4 ,sometimes also green towards the point1 due to ,cu4 7#e7 in borax4 ,the roasted mineral affords the uranium reaction4 7#f7 in mic4 salt4 ,as borax4 ,also a small residue of silica4 7#g7 with carb4 soda4 ,infusible4 ,affords the characteristic ,pb incrustation1 and sometimes yields minute particles of ,cu4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,uranium ochre ,formula4 444,u4,h#b4 ,behavior 7#a7 in glass-bulb4 ,evolves water and assumes a red color4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,v4 ,in reducing flame assumes a green color4 7#d7 in forceps4 -- 7#e7 in borax4 ,gives the uranium reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,uranite ,formula4 74,ca 444,u#b744444,p #h4;,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water and becomes yellow and opaque4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses with intumescence to a black bead having a semi-crystalline surface4 7#d7 in forceps4 -- 7#e7 in borax4 ,gives the uranium reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms an infusible yellow slag4 7#h7 ,special reactions4 ,gives the ,,po#e reaction4 99 99 99 99 99 ,mineral4 ,chalcolite ,formula4 74,cu444,u#b744444,p #h4;,h4 ,behavior 7#a7 in glass-bulb4 ,as uranite4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,as uranite4 7#d7 in forceps4 ,as uranite4 7#e7 in borax4 ,in the oxidizing flame gives a green bead1 which in the reducing flame becomes of an opaque red1 from ,cu4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,in reducing flame yields a metallic bead of ,cu4 7#h7 ,special reactions4 ,as uranite4 99 99 99 99 99 ,,iron4 99 99 99 99 99 ,mineral4 ,iron pyrites ,formula4 ,fe,s#b4 ,behavior 7#a7 in glass-bulb4 ,gives a considerable yellow sublimate of sulphur1 and sometimes sulphide of arsenic4 ,also ,,hs4 7#b7 in open tube4 ,sulphurous acid and sometimes arsenious acid are evolved4 7#c7 on charcoal4 ,gives off some sulphur1 which burns with a blue flame4 ,residue fuses to a magnetic bead4 7#d7 in forceps4 -- 7#e7 in borax4 ,the roasted mineral gives a strong iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a black mass1 which spreads out on charcoal and gives the sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,magnetic pyrites ,formula4 1,fe#e111;,fe4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,evolves sulphurous acid4 7#c7 on charcoal4 ,fuses to a magnetic bead black on the surface1 and with a yellow shining fracture4 7#d7 in forceps4 -- 7#e7 in borax4 ,as iron pyrites4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as iron pyrites4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,mispickel ,formula4 ,fe,as ,fe,s#b4 ,behavior 7#a7 in glass-bulb4 ,a red sublimate of ,as,s#b is first formed and then a black sublimate of metallic arsenic4 7#b7 in open tube4 ,sulphurous and arsenious acids are evolved1 the latter forming a white sublimate4 7#c7 on charcoal4 ,gives off much arsenic forming a white incrustation and fuses to a magnetic globule4 7#d7 in forceps4 -- 7#e7 in borax4 ,as iron pyrites4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as iron pyrites4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,magnetic iron ore ,formula4 ,fe#c,o#d ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,in the blue flame1 fuses on edges and remains magnetic4 7#e7 in borax4 ,gives the iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,specular iron ,red haematite ,formula4 ,fe#b,o#c ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,in the blue flame is converted into ,fe#b,o#d1 and then behaves as the preceding4 7#e7 in borax4 ,as magnetic iron ore4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,gthite ,formula4 444,fe4,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,as specular iron4 7#e7 in borax4 ,as specular iron4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,franklinite ,formula4 74,fe4,zn4,mn7 7444,fe444,mn74 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,forms a white incrustation on the charcoal1 which moistened with cobalt solution assumes a green color4 7#d7 in forceps4 ,v4 ,in the blue flame fuses on edges and and becomes magnetic4 7#e7 in borax4 ,gives the iron and manganese reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,affords a considerable white incrustation of ,zn,o4 7#h7 ,special reactions4 ,gives a strong manganese reaction with nitre and carbonate of soda4 99 99 99 99 99 ,mineral4 ,ilmenite ,formula4 444,ti and 444,fe4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,in reducing flame fuses on edges and becomes magnetic4 7#e7 in borax4 ,gives the iron reaction4 7#f7 in mic4 salt4 ,in oxidizing flame exhibits the iron reaction4 ,in reducing flame assumes a deep brownish red color4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,chromic iron ,formula4 4,fe444,cr4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,dissolves slowly and gives the chromium reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,on platinum foil with nitre and carbonate of soda affords a yellow mass of chromate of potassa4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,lievrite ,formula4 #c74;,fe4,ca7#c444,si #b444;,fe444,si4 ,behavior 7#a7 in glass-bulb4 ,occasionally gives off some water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a black globule1 which in the reducing flame becomes magnetic4 7#d7 in forceps4 ,i4 ,in reducing flame is magnetic4 7#e7 in borax4 ,gives the iron reaction4 7#f7 in mic4 salt4 ,gives the iron and silica reactions4 7#g7 with carb4 soda4 ,fuses to a black opaque bead4 7#h7 ,special reactions4 ,generally gives the manganese reaction with nitre and carbonate of soda4 99 99 99 99 99 ,mineral4 ,chloropal ,formula4 444,fe444,si#b #c4;,h4 ,behavior 7#a7 in glass-bulb4 ,decrepitates more or less1 gives off much water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,loses color and turns black4 7#e7 in borax4 ,gives the iron reaction4 7#f7 in mic4 salt4 ,gives the iron and silica reaction4 7#g7 with carb4 soda4 ,fuses to a transparent green glass4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,green earth ,formula4 444,si14,fe1444,al14,na14,k14,h1 etc4 ,behavior 7#a7 in glass-bulb4 ,gives off water and becomes darker in color4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,in reducing flame fuses on edges and colors the outer flame yellow 74,na7 or violet 74,k74 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as the preceding4 7#g7 with carb4 soda4 ,forms a slaggy mass4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,siderite ,formula4 4,fe44,c4 ,behavior 7#a7 in glass-bulb4 ,occasionally decrepitates4 ,gives off ,,co#b and turns black and magnetic4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,as in glass bulb4 7#d7 in forceps4 ,behaves similarly to the magnetic oxide4 7#e7 in borax4 ,gives the iron and manganese reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,behaves as an oxide4 ,with nitre and carbonate of soda on platinum generally gives the manganese reaction4 7#h7 ,special reactions4 ,in acid dissolves with effervescense4 99 99 99 99 99 ,mineral4 ,copperas ,formula4 4,fe444,s #g4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water1 and1 when strongly heated1 ,,so#b and ,,so#c1 which reddens litmus paper4 7#b7 in open tube4 ,evolves water and ,,so#b1 which may be recognized by its odor4 7#c7 on charcoal4 ,loses water and ,,so#b1 and is converted into 444,fe4 7#d7 in forceps4 ,gives off ,h and ,,so#b1 and then behaves as the magnetic oxide4 7#e7 in borax4 ,the roasted mineral affords an iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms sulphide of sodium and oxide of iron4 ,the former is absorbed into the charcoal1 and if cut out and laid upon silver and moistened gives the ,s reaction4 7#h7 ,special reactions4 ,if dissolved in water1 and a strip of silver-foil be introduced into the solution1 the metal remains untarnished4 99 99 99 99 99 ,mineral4 ,vivianite ,formula4 4,fe#c44444,p #h4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,froths up and then fuses to a grey metallic bead4 7#d7 in forceps4 ,as on charcoal4 ,singes flame green 744444,p74 7#e7 in borax4 ,gives the iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,in reducing flame becomes magnetic and fuses to a black saggy mass4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,iriphyline ,formula4 74,fe4,mn4,li7#c44444,p4 ,behavior 7#a7 in glass-bulb4 ,gives off water1 having an alkaline reaction1 and assumes a metallic lustre resembling graphite4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses readily to a black magnetic bead with a metallic lustre4 7#d7 in forceps4 ,i4 ,on platinum wire colors the flame crimson 74,li7 and green 744444,p71 towards the point fuses to a black magnetic bead4 7#e7 in borax4 ,gives the iron and manganese reactions4 7#f7 in mic4 salt4 ,gives the iron reaction which overpowers that of the manganese4 7#g7 with carb4 soda4 ,forms an infusible porous mass1 which under the reducing flame becomes magnetic4 7#h7 ,special reactions4 ,gives the manganese reaction with nitre and carbonate of soda on platinum foil4 99 99 99 99 99 ,mineral4 ,scorodite ,formula4 444,fe44444,as #d4;,h4 ,behavior 7#a7 in glass-bulb4 ,evolves water4 7#b7 in open tube4 ,gives off water and ,as,o#c4 7#c7 on charcoal4 ,emits arsenical fume and in the reducing flame fuses to a magnetic mass having a metallic lustre4 7#d7 in forceps4 ,i4 ,as on charcoal4 ,colors the outer flame blue4 7#e7 in borax4 ,the roasted mineral gives an iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 7#h7 ,special reactions4 ,gives the arsenic reactions4 99 99 99 99 99 ,mineral4 ,cube ore ,formula4 4,fe#c44444;,as 444,fe#c44444;,as#b #ah4;,h4 ,behavior 7#a7 in glass-bulb4 ,evolves much water4 7#b7 in open tube4 ,as the preceding4 7#c7 on charcoal4 ,as the preceding4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,as the preceding4 99 99 99 99 99 ,,manganese4 99 99 99 99 99 ,mineral4 ,manganblende ,formula4 ,mn,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,gives off ,,so#b and becomes greyish green on surface4 7#c7 on charcoal4 ,is slowly roasted and converted into oxide4 7#d7 in forceps4 ,v4 7#e7 in borax4 ,the roasted mineral gives a strong manganese reaction4 7#f7 in mic4 salt4 ,in the unroasted state1 dissolves with much ebullition and detonation due to elimination of sulphide of phosphorus4 ,the bead then exhibits the characteristic violet color of manganese4 7#g7 with carb4 soda4 ,forms a slaggy mass1 which laid on silver and moistened1 gives the sulphur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,pyrolusite ,formula4 44,mn4 ,behavior 7#a7 in glass-bulb4 ,frequently gives off a small quantity of water and1 when strongly heated1 oxygen4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 7#e7 in borax4 ,gives the manganese reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms a slaggy mass4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,manganite ,formula4 444,mn4,h4 ,behavior 7#a7 in glass-bulb4 ,gives off much water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,exfoliates slightly4 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,psilomelane ,formula4 74,ba14,ca14,mg14,k7 44,mn 4,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water and1 when strongly heated1 oxygen4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,colors flame faintly green7,ba7 and red towards the point 7,ca74 7#e7 in borax4 ,as pyrolusite4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as pyrolusite4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,wad ,formula4 44,mn14,mn14,h1 also 444,fe1444,al1 4,ba14,cu1444,pb1444,si1 etc4 ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 ,colors flame variously according to its composition4 7#e7 in borax4 ,gives the manganese reaction1 more or less modified by the presence of other oxides4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as pyrolusite4 7#h7 ,special reactions4 ,various according to composition4 ,when strongly heated and then moistened has an alkaline reaction on red litmus paper4 99 99 99 99 99 ,mineral4 ,rhodonite ,formula4 4,mn#c444,si#b4 ,behavior 7#a7 in glass-bulb4 ,gives off more or less water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,under a strong flame fuses to a brown opaque bead4 7#d7 in forceps4 ,,ii4 ,as on charcoal4 7#e7 in borax4 ,in the oxidizing flame gives the manganese reaction4 ,in reducing flame the iron reaction4 7#f7 in mic4 salt4 ,as in borax1 but leaves an insoluble siliceous skeleton4 7#g7 with carb4 soda4 ,with a small quantity of the alkali fuses to a black bead4 ,with a larger quantity forms a slag4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,diallogite ,formula4 4,mn44,c4 ,behavior 7#a7 in glass-bulb4 ,frequently decrepitates and gives off more or less water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,if strongly heated and moistened has an alkaline reaction on litmus paper due to the presence of ,ca4 7#d7 in forceps4 ,v4 ,frequently colors the flame slightly red4 7#e7 in borax4 ,gives the manganese and iron reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms an infusible slag4 7#h7 ,special reactions4 ,in warm acid dissolves with much effervescence4 99 99 99 99 99 ,mineral4 ,triplite ,formula4 744,mn4,fe7#d44444,p4 ,behavior 7#a7 in glass-bulb4 ,generally gives off more or less water4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,i4 ,colors the outer blowpipe flame green 744444,p74 7#e7 in borax4 ,gives the manganese and iron reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms an infusible mass4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,,nickel ,,and ,,cobalt4 99 99 99 99 99 ,mineral4 ,millerite ,formula4 ,ni,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,evolves ,,so#b4 7#c7 on charcoal4 ,fuses with much ebullition to a magnetic bead4 7#d7 in forceps4 -- 7#e7 in borax4 ,the roasted mineral gives a nickel reaction1 slightly modified by small quantities of iron and copper4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses to a slaggy mass1 which on silver gives the sulphur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,coppernickel ,formula4 ,ni#b;,as4 ,behavior 7#a7 in glass-bulb4 ,gives off a little ,as,o#c4 7#b7 in open tube4 ,gives off much ,as,o#c and some ,,so#b and falls to powder4 7#c7 on charcoal4 ,fuses to a magnetic bead1 with the evolution of arsenic1 which colors the flame blue4 7#d7 in forceps4 -- 7#e7 in borax4 ,the arsenical bead obtained by fusing the mineral on charcoal1 if fused upon the same support with borax successively added and removed1 gives firstly an iron reaction1 then cobalt if present1 and lastly nickel4 7#f7 in mic4 salt4 ,if the residual bead which has been treated with borax be further treated with microcosmic salt1 the nickel reaction will be obtained and sometimes a slight copper reaction4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,affords a sublimate of metallic arsenic when treated with cyanide of potassium4 99 99 99 99 99 ,mineral4 ,smaltine ,formula4 ,co,as4 ,behavior 7#a7 in glass-bulb4 ,when strongly heated generally evolves metallic arsenic4 7#b7 in open tube4 ,gives a crystalline sublimate of ,as,o#c4 ,also some ,,so#b4 7#c7 on charcoal4 ,gives off fumes of arsenic1 and fuses to a dark grey magnetic bead1 very brittle1 colors flame blue4 7#d7 in forceps4 -- 7#e7 in borax4 ,as the preceding1 but the cobalt being in large excess requires some time for its perfect oxidation1 before the nickel reaction is exhibited4 7#f7 in mic4 salt4 ,gives the cobalt reaction1 and after the cobalt has been1 removed that of nickel4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,as the preceding4 99 99 99 99 99 ,mineral4 ,glance cobalt ,formula4 ,co,s#b ,co,as4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,as the preceding1 but gives off more ,,so#b4 7#c7 on charcoal4 ,gives off ,s and ,as1 and fuses to a magnetic bead4 ,colors flame blue4 7#d7 in forceps4 -- 7#e7 in borax4 ,gives a cobalt and slight iron reaction when treated as the preceding minerals4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,gives a sulphur reaction of silver4 7#h7 ,special reactions4 ,as the preceding4 99 99 99 99 99 ,mineral4 ,nickel glance ,formula4 ,ni,s#b ,ni,as4 ,behavior 7#a7 in glass-bulb4 ,decrepitates and gives an orange colored sublimate of ,as,s#b4 7#b7 in open tube4 ,as the preceding4 7#c7 on charcoal4 ,as the preceding4 7#d7 in forceps4 -- 7#e7 in borax4 ,as copper nickel4 7#f7 in mic4 salt4 ,gives the nickel reaction occasionally somewhat obscured by cobalt4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,as copper nickel4 99 99 99 99 99 ,mineral4 ,ulmannite ,formula4 ,ni,s#b ,ni7,as,sb7#b4 ,behavior 7#a7 in glass-bulb4 ,gives a slight white sublimate of ,sb,o#c and more or less ,as,s#c4 7#b7 in open tube4 ,gives off thick fumes of ,sb,o#c and ,sb,o#e with ,as,o#c and ,,so#b4 7#c7 on charcoal4 ,as glance cobalt1 but accompanied by dense fumes of ,sb,o#c4 7#d7 in forceps4 -- 7#e7 in borax4 ,as copper nickel4 7#f7 in mic4 salt4 ,as the preceding4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,as copper nickel generally1 but arsenic is not always present4 99 99 99 99 99 ,mineral4 ,cobalt pyrites ,formula4 71,co1,ni1,fe7 7111,co111,ni111,fe74 ,behavior 7#a7 in glass-bulb4 ,when strongly heated gives off sulphur and becomes brown4 7#b7 in open tube4 ,gives off much ,,so#b and a small quantity of ,as,o#c4 7#c7 on charcoal4 ,in the reducing flame small fragments fuse with the evolution of sulphur to a magnetic bead having a bronze colored fracture4 7#d7 in forceps4 -- 7#e7 in borax4 ,in the oxidizing flame on charcoal gives a violet colored glass4 ,in the reducing flame the nickel is reduced and may collected in a gold bead4 ,when the nickel is removed1 the glass exhibits a slight iron reaction while warm4 7#f7 in mic4 salt4 ,as in borax1 but the reduction of the nickel is more difficult than in the latter flux4 7#g7 with carb4 soda4 ,as glance cobalt4 7#h7 ,special reactions4 ,as copper nickel1 but the amount of arsenic is usually very small4 99 99 99 99 99 ,mineral4 ,emerald nickel ,formula4 4,ni#c44;,c #f4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off much water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 -- 7#e7 in borax4 ,dissolves with much effervescence and gives the nickel reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms a slaggy mass4 7#h7 ,special reactions4 ,in warm dilute ,h,cl dissolves with much effervescence4 99 99 99 99 99 ,mineral4 ,cobalt ,bloom ,formula4 4,co#c44444;,as #h4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,evolves arsenical fumes and in the reducing flame fuses to a dark grey bead of arsenide of cobalt4 7#d7 in forceps4 ,in the point of the blue flame fuses and colors the outer flame blue 7,as74 7#e7 in borax4 ,gives the cobalt reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,gives off arsenic with cyanide of potassium in glass tube4 99 99 99 99 99 ,mineral4 ,earthy cobalt ,formula4 4,mn14,co14,cu14,fe14,h1 etc4 ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,emits a slight smell of arsenic1 but does not fuse4 7#d7 in forceps4 ,colors the flame blue4 7#e7 in borax4 ,in oxidizing flame gives the cobalt reaction which obscures those of 4,mn1 4,cu1 etc4 ,in reducing flame occasionally gives the 4,cu reaction4 7#f7 in mic4 salt4 ,as in borax4 ,if a saturated bead be treated on charcoal with tin in the reducing flame for a few seconds1 the 4,cu reaction is sometimes obtained4 7#g7 with carb4 soda4 ,forms an infusible mass4 7#h7 ,special reactions4 ,with carbonate of soda and nitre on platinum foil1 gives a strong manganese reaction4 99 99 99 99 99 ,,zinc4 99 99 99 99 99 ,mineral4 ,zincblende ,formula4 ,zn,s4 ,behavior 7#a7 in glass-bulb4 ,decrepitates strongly4 7#b7 in open tube4 ,evolves ,,so and becomes white or yellow if containing iron4 7#c7 on charcoal4 ,v4 ,in the reducing flame incrusts the charcoal with ,zn,o2 also with ,cd,o1 if that metal be present4 7#d7 in forceps4 -- 7#e7 in borax4 ,the roasted mineral gives a zinc reaction1 and sometimes a slight iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 ,moreover colors the flame blue4 ,the fused alkali gives a ,s reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,red oxide of zinc ,formula4 4,zn4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in the reducing flame forms a thin incrustation of oxide of zinc on the charcoal4 7#d7 in forceps4 ,v4 7#e7 in borax4 ,generally gives a manganese and slight iron reaction in addition to that of zinc4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,on charcoal1 forms a thick incrustation of ,zn,o4 7#h7 ,special reactions4 ,with carbonate of soda and nitre on platinum foil gives manganese reaction4 99 99 99 99 99 ,mineral4 ,electric calamine ,formula4 #b4,zn#c444,si #c4;,h ,behavior 7#a7 in glass-bulb4 ,gives off water and becomes white and opaque4 7#b7 in open tube4 -- 7#c7 on charcoal4 -- 7#d7 in forceps4 ,v4 7#e7 in borax4 ,dissolves to a clear glass1 which cannot be rendered opaque by the intermittent flame4 7#f7 in mic4 salt4 ,dissolves to a clear glass1 which becomes opaque on cooling4 ,silica remains insoluble4 7#g7 with carb4 soda4 ,with carbonate of soda alone is infusible4 ,with #b parts of alkali and #a of borax fuses to a glass and sets free 4,zn1 which incrusts the charcoal4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,calamine ,formula4 4,zn44,c4 ,behavior 7#a7 in glass-bulb4 ,gives off ,,co#b and becomes opaque4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,as the red oxide4 ,sometimes also gives a lead incrustation4 7#d7 in forceps4 ,v4 7#e7 in borax4 ,gives a zinc reaction and frequently an iron and manganese reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,forms a thick incrustation of zinc1 sometimes also of 4,pb and 4,co4 7#h7 ,special reactions4 ,dissolves with much effervescence in cold acid4 99 99 99 99 99 ,,bismuth4 99 99 99 99 99 ,mineral4 ,native bismuth ,formula4 ,bi4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,fuses and is converted into a yellow oxide4 7#c7 on charcoal4 ,fuses to a bead and incrusts the charcoal with oxide4 7#d7 in forceps4 -- 7#e7 in borax4 ,the oxide formed upon charcoal gives the bismuth reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,bismuthine ,formula4 ,bi,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,fuses with ebullition and gives of ,s and ,,so#b4 7#c7 on charcoal4 ,fuses with much spirting and in the reducing flame yields a metallic bead and incrusts the charcoal with oxide4 7#d7 in forceps4 -- 7#e7 in borax4 ,the oxide obtained upon charcoal gives the bismuth reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 ,the fused alkali gives the sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,bismuthblende ,formula4 444,bi#b444,si#c4 ,behavior 7#a7 in glass-bulb4 ,turns yellow and1 when strongly heated1 fuses4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses with ebullition to a brown globule forming an incrustation of 444,bi on the charcoal4 7#d7 in forceps4 ,i4 ,fuses with ease to a yellow bead1 coloring the outer flame bluish green1 especially if moistened with ,h,cl4 ,this color is due to 44444,p4 7#e7 in borax4 ,gives the bismuth and also an iron reaction4 7#f7 in mic4 salt4 ,as in borax1 but leaves a silicious skeleton4 7#g7 with carb4 soda4 ,fuses to a yellow mass4 ,the bismuth is then reduced to the metallic state and partially volatilized1 incrusting the charcoal beyond4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,tetradymite ,formula4 ,bi1 ,te1 ,s4 ,behavior 7#a7 in glass-bulb4 ,occasionally decrepitates and then fuses1 forming a greyish white sublimate immediately above the mineral fragment4 7#b7 in open tube4 ,fuses and gives off white fumes1 part of which pass up the tube and part deposit immediately above the mineral4 ,this latter if heated fuses to clear drops 7,te,o#c74 ,the mineral residue becomes surrounded by fused 444,bi1 characterized by its yellow color4 7#c7 on charcoal4 ,fuses to a metallic bead1 colors the outer flame bluish green 7,te and ,se7 and incrusts the charcoal around with the orange 444,bi1 beyond which is a white incrustation partly consisting of 444,te4 7#d7 in forceps4 -- 7#e7 in borax4 ,the yellow oxide obtained upon charcoal gives the bismuth reaction1 and the white incrustation of bismuth and telluric acid4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,in the reducing flame yields a bead of metallic bismuth1 part of which is part of the tellurium volatilized and incrusts the charcoal around4 7#h7 ,special reactions4 ,the fused alkaline mass gives the sulphur reaction on silver4 ,also gives the tellurium reaction with charcoal and carbonate of soda4 99 99 99 99 99 ,,lead4 99 99 99 99 99 ,mineral4 ,galena ,formula4 ,pb,s4 ,behavior 7#a7 in glass-bulb4 ,generally decrepitates and gives off a small quantity of sulphur4 7#b7 in open tube4 ,gives off ,,so#b1 and when strongly heated1 a white sublimate of 4,pb1 4,s4 7#c7 on charcoal4 ,fuses and is reduced affording a bead of metallic lead1 and forming an incrustation of ,pb,o on the charcoal4 ,colors the outer flame blue4 7#d7 in forceps4 -- 7#e7 in borax4 ,the oxide formed upon charcoal gives the lead reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 ,the fused alkali gives a sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,clausthalite ,formula4 ,pb,se4 ,behavior 7#a7 in glass-bulb4 ,decrepitates slightly4 7#b7 in open tube4 ,forms a sublimate of selenium1 which is grey when thickly deposited1 and red when thin4 7#c7 on charcoal4 ,gives off fumes smelling strongly of selenium and coloring the flame blue4 ,in the reducing flame fuses partially and incrusts the charcoal with ,se and ,pb,o4 ,after some time a black infusible mass alone remains4 7#d7 in forceps4 -- 7#e7 in borax4 ,the infusible residue obtained upon charcoal gives an iron and sometimes copper and cobalt reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,with carbonate of soda1 oxalate of potash yields a metallic bead1 the fused alkali laid upon silver and moistened produces a stain similar to that produced by sulfur4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,jamesonite ,formula4 1,pb#c111,sb#b4 ,behavior 7#a7 in glass-bulb4 ,fuses and gives off some sulphur1 sulphide of antimony and antimony which condense in the neck of the bulb4 7#b7 in open tube4 ,fuses and emits dense white fumes of ,sb,o#c1 which pass off and redden blue litmus paper4 7#c7 on charcoal4 ,fuses with great ease evolving much ,sb,o#c and ,pb,o1 which incrusts the charcoal around the mineral4 ,when the fumes have ceased1 a small bead of metallic lead remains4 7#d7 in forceps4 -- 7#e7 in borax4 ,the yellow incrustation formed upon charcoal gives the reaction of lead1 and the white those of antimony4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 ,the fused alkali gives the sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,minium ,formula4 ,pb#c,o#d4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,is reduced first to litharge 7,pb,o7 and then to metallic lead which forms the usual incrustation4 7#d7 in forceps4 ,colors the outer flame blue4 7#e7 in borax4 ,gives the lead reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,mendipite ,formula4 ,pb,cl #b,pb,o4 ,behavior 7#a7 in glass-bulb4 ,decrepitates slightly and assumes a yellow color4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses readily and is reduced to metallic lead with the evolution of acid fumes4 ,forms a white incrustation of ,pb,cl1 and a yellow one of ,pb,o4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 7#h7 ,special reactions4 ,gives the chlorine reaction with ,cu,o and microcosmic salt4 99 99 99 99 99 ,mineral4 ,cerusite ,formula4 4,pb44,c4 ,behavior 7#a7 in glass-bulb4 ,decrepitates1 gives off ,,co#b1 turns yellow and fuses4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,is reduced to metallic lead1 incrusting the charcoal around with ,pb,o4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,gives the lead reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 7#h7 ,special reactions4 ,in nitric acid dissolves with much effervescence4 99 99 99 99 99 ,mineral4 ,anglesite ,formula4 4,pb444,s4 ,behavior 7#a7 in glass-bulb4 ,decrepitates and gives off a small quantity of water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in the oxidizing flame fuses to a clear bead1 which becomes opaque on cooling4 ,in reducing flame is reduced with much ebullition to a metallic bead and incrusts the charcoal around with ,pb,o4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,gives the lead reaction and occasionally a slight iron and manganese reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,is reduced yielding a metallic lead bead4 ,the fused alkaline mass gives a sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,pyromorphite ,formula4 ,pb,cl #c4,pb#c44444,p4 ,behavior 7#a7 in glass-bulb4 ,decrepitates1 and when strongly heated for some time1 gives a slight white sublimate of ,pb,cl4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in oxidizing flame fuses to a bead having a crystalline surface on cooling1 and forms a thin film of ,pb,cl on the charcoal ,in reducing flame fuses without reduction and on cooling assumes a polyhedral form4 ,incrusts the charcoal slightly with ,pb,o4 7#d7 in forceps4 ,fuses and colors the flame blue4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,is reduced yielding a metallic bead and incrusting the charcoal with ,pb,o4 7#h7 ,special reactions4 ,gives the chlorine reaction with microcosmic salt and ,cu,o4 ,also the phosphoric acid reactions4 99 99 99 99 99 ,mineral4 ,mimetene ,formula4 ,pb,cl #c4,pb#c44444;,as ,behavior 7#a7 in glass-bulb4 ,as the preceding4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 but less easily than the preceding1 gives off ,as,o#c and incrusts the charcoal with ,pb,cl4 ,finally is reduced to a metallic bead and forms an incrustation of ,pb,o4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 ,the oxide formed on charcoal gives the lead reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,gives the chlorine reaction4 99 99 99 99 99 ,mineral4 ,vanadinite ,formula4 ,pb,cl #c4,pb#c444,v8 ,behavior 7#a7 in glass-bulb4 ,as pyromorphite4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,the powdered mineral fuses fuses to a black shining mass1 which in the reducing flame affords a metallic bead4 ,incrusts the charcoal first with a white film of ,pb,cl and afterwards with ,pb,o4 7#d7 in forceps4 ,as pyromorphite4 7#e7 in borax4 ,dissolves readily to a clear glass1 which1 in the oxidizing flame1 is yellow1 while hot1 and colorless when cold4 ,in reducing flame becomes opaque1 and on cooling green4 7#f7 in mic4 salt4 ,in oxidizing flame is yellow while hot1 becoming paler on cooling4 ,in reducing flame brown while warm1 and emerald green when cold4 7#g7 with carb4 soda4 ,on platinum wire fuses to a yellow bead1 which is crystalline on cooling4 ,on charcoal yields a button of metallic lead4 7#h7 ,special reactions4 ,with microcosmic salt and ,cu,o1 gives the chlorine reaction4 ,if fused in a platinum spoon with from #c to #d times its volume of 4,k1444,s#b it forms a fluid yellow mass having an orange color when cold4 99 99 99 99 99 ,mineral4 ,crocoisite ,formula4 4,pb444,cr4 ,behavior 7#a7 in glass-bulb4 ,decrepitates violently and assumes a dark color4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses and detonates yielding ,cr#b,o#c and metallic lead1 and forming an incrustation of ,pb,o on the charcoal4 7#d7 in forceps4 ,as pyromorphite4 7#e7 in borax4 ,dissolves readily and colors the glass yellow while warm1 and green when cold4 7,see ,chromium reaction47 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,on platinum foil gives a dark yellow mass1 which becomes paler on cooling4 ,on charcoal yields a metallic button4 7#h7 ,special reactions4 ,treated as above with 4,k1444,s#b forms a violet colored mass1 which on solidifying becomes reddish and on cooling pale grey4 99 99 99 99 99 ,mineral4 ,molybdate of lead ,formula4 4,pb444,m4 ,behavior 7#a7 in glass-bulb4 ,as the preceding4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses and is partly absorbed into the charcoal leaving a globule of metallic lead1 which is partially oxidized and incrusts the charcoal4 7#d7 in forceps4 ,as pyromorphite4 7#e7 in borax4 ,dissolves readily and gives the molybdena reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,yields metallic lead4 7#h7 ,special reactions4 ,fused as above with 4,k1444,s#b forms a yellow mass1 which becomes white on cooling4 ,if this be dissolved in water and a piece of zinc introduced into the solution1 the latter becomes blue4 99 99 99 99 99 ,mineral4 ,scheeletine ,formula4 4,pb444,w4 ,behavior 7#a7 in glass-bulb4 ,decrepitates more or less4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a bead incrusting the charcoal with ,pb,o4 ,the bead on cooling is crystalline and has a dark metallic surface4 7#d7 in forceps4 ,as pyromorphite4 7#e7 in borax4 ,dissolves to a clear colorless glass1 which in the reducing flame becomes yellow1 and on cooling grey and opaque4 7#f7 in mic4 salt4 ,dissolves to a clear colorless glass1 which in the reducing flame assumes a dusky blue color4 ,after a time becomes opaque4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,with carbonate of soda and nitre gives the manganese reaction4 99 99 99 99 99 ,,copper4 99 99 99 99 99 ,mineral4 ,native ,copper ,formula4 ,cu4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a brilliant metallic bead1 which on cooling becomes covered with a coating of black oxide4 7#d7 in forceps4 ,fuses and colors the outer flame blue4 7#e7 in borax4 ,in the oxidizing flame dissolves and then gives the copper reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,vitreous ,copper ,formula4 ,cu#b,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,evolves ,,so#b and1 when pulverized and gently heated for some time is converted into ,cu,o4 7#c7 on charcoal4 ,fuses to a bead1 which spirts considerably and gives off ,,so#b4 ,when pulverized and gently roasted1 is converted into ,cu,o4 7#d7 in forceps4 -- 7#e7 in borax4 ,the roasted mineral gives the copper reaction1 and sometimes also a slight iron-reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,in the reducing flame is decomposed1 forming ,na,s and metallic copper4 ,if the former be cut out and laid upon silver1 it gives the sulfur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,copper pyrites ,formula4 1,cu111,fe4 ,behavior 7#a7 in glass-bulb4 ,decrepitates1 sometimes gives a sublimate of sulphur and becomes bronze colored on the surface4 7#b7 in open tube4 ,evolves ,,so#b and is finally converted into a dark red mixture of ,fe#b,o#c and ,cu,o4 7#c7 on charcoal4 ,fuses readily with much ebullition and is magnetic on cooling4 7#d7 in forceps4 -- 7#e7 in borax4 ,as the preceding2 but when the copper has been removed by reducing on charcoal1 the bead shows a strong iron color4 7#f7 in mic4 salt4 ,as the preceding1 but the color in the oxidizing flame is green1 owing to the presence of iron4 7#g7 with carb4 soda4 ,yields a bead of metallic copper and some magnetic oxide of iron which remains on the charcoal4 ,the fused gives a sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,fahlerz ,formula4 71,cu1,ag1,fe1,zn7#d 7111,sb111,as74 ,behavior 7#a7 in glass-bulb4 ,sometimes decrepitates1 fuses1 and when very strongly heated1 gives a red sublimate of 111,sb with 444,sb1 also sometimes a black sublimate of 1,hg and occasionally 111,as4 7#b7 in open tube4 ,fuses and gives off thick fumes of ,sb,o#c and ,,so#b1 also generally ,as,o#c1 leaving a black infusible residue4 ,if ,hg be present1 it is sublimed and condenses in the tube in small drops4 7#c7 on charcoal4 ,fuses to a bead1 which fumes strongly and incrusts the charcoal with ,sb,o#c1 and sometimes ,zn,o1 which cannot be volatilized4 ,emits a strong smell of arsenic4 7#d7 in forceps4 -- 7#e7 in borax4 ,the residue obtained on charcoal thoroughly roasted gives a copper reaction1 and when the latter has been removed by reduction upon charcoal1 an iron reaction4 7#f7 in mic4 salt4 ,as in the preceding4 7#g7 with carb4 soda4 ,with this flux and a little borax yields a bead of metallic copper2 on silver1 the alkaline mass gives a sulphur reaction4 7#h7 ,special reactions4 ,if the copper bead obtained by fusing upon carbonate of soda be cupelled with assay lead1 a silver bead will be obtained4 ,or if dissolved in nitric acid and a drop or two of ,h,cl added1 a white precipitate of ,ag,cl will be formed1 which may be collected and reduced with carbonate of soda upon charcoal4 99 99 99 99 99 ,mineral4 ,tennatite ,formula4 71,cu1,fe7#d111;,as4 ,behavior 7#a7 in glass-bulb4 ,decrepitates occasionally and gives a red sublimate of 111,as4 7#b7 in open tube4 ,evolves 44,s and 444,as1 which condense and form a white sublimate4 7#c7 on charcoal4 ,fuses to a magnetic bead giving of arsenical and sulphurous fumes4 7#d7 in forceps4 -- 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as the preceding4 7#g7 with carb4 soda4 ,yields a copper bead and metallic iron in the form of a dark grey powder4 ,the fused alkali gives the sulphur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,bournonite ,formula4 71,pb#b1;,cu7111,sb4 ,behavior 7#a7 in glass-bulb4 ,decrepitates giving off sulfur and1 when strongly heated1 111,sb and 444,sb4 7#b7 in open tube4 ,evolves thick white fumes of 444,sb144444,sb and 4,pb444,sb4 ,also 4,s4 7#c7 on charcoal4 ,fuses readily and incrusts the charcoal with 444,sb and 4,pb leaving a dark colored bead4 7#d7 in forceps4 -- 7#e7 in borax4 ,if the bead obtained on charcoal be fused on that support in the reducing flame with borax1 a slight iron reaction is obtained1 and after a time a copper reaction4 7#f7 in mic4 salt4 ,as with borax4 7#g7 with carb4 soda4 ,yields a bead of metallic copper and lead and incrusts the charcoal with 444,sb and 4,pb4 ,the alkaline mass laid on silver and moistened gives the sulphur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,red oxide of copper ,formula4 ,cu#b,o ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,is converted into the black oxide ,cu,o4 7#c7 on charcoal4 ,in the reducing flame is reduced1 forming a bead of metallic copper4 7#d7 in forceps4 ,fuses and colors the the flame emerald green1 or if previously moistened with ,h,cl1 blue4 7#e7 in borax4 ,gives the copper reaction4 7#f7 in mic4 salt4 ,as with borax4 7#g7 with carb4 soda4 ,is reduced to a bead of metallic copper4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,atacamite ,formula4 ,cu,cl #c4;,cu #f4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off much water1 having an acid reaction1 on test paper1 and forms a light grey sublimate of ,cu,cl4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses1 colors the flame blue1 forms a brown and a pale grey incrustation on the charcoal1 and is reduced to metallic copper1 leaving a small quantity of slag4 7#d7 in forceps4 ,fuses and colors the outer flame intensely blue and green towards the point4 7#e7 in borax4 ,gives the copper reactions4 7#f7 in mic4 salt4 ,as with borax4 7#g7 with carb4 soda4 ,is reduced1 yielding a bead of metallic copper4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,dioptase ,formula4 4,cu#c444,si#b #c4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,in the oxidizing flame becomes black4 ,in the reducing flame red4 7#d7 in forceps4 ,v4 ,colors the outer flame intensely green4 7#e7 in borax4 ,gives the copper reactions4 7#f7 in mic4 salt4 ,as with borax4 ,the silica remains undissolved4 7#g7 with carb4 soda4 ,with a small quantity of carbonate of soda fuses to a bead1 which on cooling is opaque and has a red fracture4 ,with more alkali forms a slag1 containing little beads of reduced copper4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,malachite ,formula4 4,cu#b44;,c 4,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses to a bead with a strong flame is reduced to metallic copper4 7#d7 in forceps4 ,fuses and colors the outer flame brilliantly green4 7#e7 in borax4 ,gives the copper reaction4 7#f7 in mic4 salt4 ,as with borax4 7#g7 with carb4 soda4 ,yields metallic copper4 7#h7 ,special reactions4 ,dissolves in ,h,cl with much effervescence4 99 99 99 99 99 ,mineral4 ,blue vitriol ,formula4 4,cu444,s #e4;,h4 ,behavior 7#a7 in glass-bulb4 ,intumesces1 gives off water and becomes white4 7#b7 in open tube4 ,strongly heated is decomposed1 given off ,,so#b and being converted into ,cu,o4 7#c7 on charcoal4 ,as in the glass-bulb4 ,then fuses1 coloring the outer flame green1 and is reduced to metallic copper and 1,cu4 7#d7 in forceps4 ,fuses and colors the outer flame blue4 7#e7 in borax4 ,the roasted mineral gives copper reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,yields metallic copper4 ,the alkaline mass laid on silver gives ,s reaction4 7#h7 ,special reactions4 ,gives the sulphuric acid reaction4 99 99 99 99 99 ,mineral4 ,libethenite ,formula4 4,cu#d44444,p #b4;,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water and turns black4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,gradually heated1 turns black and fuses to a bead1 having a core of metallic copper4 7#d7 in forceps4 ,fuses but does not color the flame distinctly4 ,on cooling is black and crystalline4 7#e7 in borax4 ,gives the copper reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,with much of the alkali is decomposed1 yielding metallic copper4 ,with small portions successively added first fuses and then intumesces1 fuses with a strong flame1 and is then absorbed into the charcoal1 leaving metallic copper4 7#h7 ,special reactions4 ,gives the phosphoric acid reaction4 99 99 99 99 99 ,mineral4 ,olivenite ,formula4 4,cu#d744444;,as44444,p7 4,h4 ,behavior 7#a7 in glass-bulb4 ,gives off water4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses with detonation and the evolution of arsenical fumes to a brittle regulus1 brown externally and having a white fracture4 7#d7 in forceps4 ,fuses and colors the outer flame green4 ,on cooling has a crystalline surface4 7#e7 in borax4 ,gives the copper reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,is reduced1 yielding metallic copper4 7#h7 ,special reactions4 ,gives the arsenic reactions4 99 99 99 99 99 ,,antimony4 99 99 99 99 99 ,mineral4 ,native antimony ,formula4 ,sb4 ,behavior 7#a7 in glass-bulb4 ,fuses and1 when strongly heated1 volatilizes being redeposited in the tube as a dark grey sublimate4 7#b7 in open tube4 ,fuses and gives off dense white fumes1 which are partly redeposited on the tube4 ,sometimes also gives off arsenical fumes in small quantity4 7#c7 on charcoal4 ,fuses and gives off dense white fumes1 which thickly incrust the charcoal and color the flame blue immediately beyond the assay4 7#d7 in forceps4 -- 7#e7 in borax4 ,the oxide formed upon charcoal gives the antimony reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,the incrustation on the charcoal1 if treated with nitrate of cobalt assumes the characteristic green color4 99 99 99 99 99 ,mineral4 ,grey antimony ,formula4 ,sb,s#c4 ,behavior 7#a7 in glass-bulb4 ,fuses readily and occasionally gives off a small quantity of sulphur4 ,strongly heated forms a brown sublimate of ,sb,s#c and ,sb,o#c4 7#b7 in open tube4 ,fuses and gives off ,,so#b1 which passes off up the tube1 and dense white fumes of ,sb,o#c and ,sb,o#e which are partly deposited in the tube4 7#c7 on charcoal4 ,fuses and is partly absorbed by the charcoal and partly volatilized1 incrusting the charcoal with the characteristic white oxides4 ,colors the flame blue4 7#d7 in forceps4 -- 7#e7 in borax4 ,as the preceding4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,fuses and is reduced1 yielding metallic antimony1 which behaves as the preceding mineral upon charcoal4 ,the alkaline mass gives the sulphur reaction4 7#h7 ,special reactions4 ,as the preceding4 99 99 99 99 99 ,mineral4 ,antimony blende ,formula4 111,sb#b 444,sb4 ,behavior 7#a7 in glass-bulb4 ,fuses easily1 gives off first ,sb,o#c and afterwards an orange colored sublimate4 ,strongly heated1 is decomposed and gives a black sublimate1 which becomes brown on cooling4 7#b7 in open tube4 ,as the preceding4 7#c7 on charcoal4 ,as the preceding4 7#d7 in forceps4 -- 7#e7 in borax4 ,as native antimony4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 ,as native antimony4 99 99 99 99 99 ,mineral4 ,white antimony ,formula4 ,sb,o#c4 ,behavior 7#a7 in glass-bulb4 ,is sublimed and recondensed in the neck of the tube4 7#b7 in open tube4 ,as in the glass-bulb4 7#c7 on charcoal4 ,fuses with the evolution of dense white fumes1 which incrust the surface of the charcoal4 ,in the reducing flame is partly reduced1 yielding metallic antimony4 ,colors flame blue4 7#d7 in forceps4 ,fuses and is volatilized1 coloring the outer flame blue4 7#e7 in borax4 ,gives the antimony reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,in the reducing flame is reduced1 yielding metallic antimony4 7#h7 ,special reactions4 ,as native antimony4 99 99 99 99 99 ,,arsenic4 99 99 99 99 99 ,mineral4 ,native arsenic ,formula4 ,as4 ,behavior 7#a7 in glass-bulb4 ,sublimes without fusion and recondenses as a dark grey metallic sublimate1 sometimes leaving a small residue4 7#b7 in open tube4 ,if gently heated in a good current of air passes off as ,as,o#c1 which is partly condensed as a white sublimate in the upper part of the tube4 7#c7 on charcoal4 ,passes off as ,as,o#c1 which thinly incrusts the charcoal beyond the assay4 7#d7 in forceps4 ,colors the flame blue4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,realgar ,formula4 ,as,s#b4 ,behavior 7#a7 in glass-bulb4 ,fuses1 enters into ebullition and is sublimed as a transparent red sublimate4 7#b7 in open tube4 ,gently heated passes off as ,,so#b and ,as,o#c1 the latter of which is redeposited in the upper part of the tube4 7#c7 on charcoal4 ,fuses and passes off as arsenious and sulphurous acids4 7#d7 in forceps4 ,fuses and colors the flame blue4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,as on charcoal1 except that the ,s combines with the alkali forming ,na,s1 which on silver gives the sulphur reaction4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,orpiment ,formula4 ,as,s#c4 ,behavior 7#a7 in glass-bulb4 ,as the preceding1 except that the sublimate is of a dark yellow color when cold4 7#b7 in open tube4 ,as the preceding4 7#c7 on charcoal4 ,as the preceding4 7#d7 in forceps4 ,as the preceding4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,white arsenic ,formula4 ,as,o#c4 ,behavior 7#a7 in glass-bulb4 ,sublimes without fusion and re-condenses in white crystals4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,sublimes and is partly recondensed on charcoal forming a white incrustation4 7#d7 in forceps4 ,colors the flame blue4 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 ,heated with charcoal in a glass-tube sealed at one end1 is reduced and metallic arsenic sublimes4 99 99 99 99 99 ,,mercury4 99 99 99 99 99 ,mineral4 ,native mercury ,formula4 ,hg4 ,behavior 7#a7 in glass-bulb4 ,volatilizes with little or no residue and recondenses in neck of bulb4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,is volatilized4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,cinnabar ,formula4 ,hg,s4 ,behavior 7#a7 in glass-bulb4 ,volatilizes sometimes leaving a slight earthy residue1 and re-condenses as a black sulphide4 7#b7 in open tube4 ,if gently heated is decomposed into metallic mercury1 which volatilizes and recondenses in the upper part of the tube1 and ,,so#b1 which passes off as is easily recognized by its odor and bleaching properties4 7#c7 on charcoal4 ,is volatilized1 generally leaving a small earthy residue4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,with carbonate of soda and cyanide of potassium is decomposed and metallic mercury volatilized4 7#h7 ,special reactions4 ,when in the preceding experiment the mercury has been entirely dissipated1 the alkaline residue laid on silver gives a sulphur reaction4 99 99 99 99 99 ,mineral4 ,native amalgam ,formula4 ,ag,hg#b4 ,behavior 7#a7 in glass-bulb4 ,as native mercury1 but leaves a residue of pure silver4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,the mercury volatilizes leaving the silver1 which fuses to a bead1 and1 in the oxidizing flame1 incrusts the charcoal with its characteristic oxide4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,,silver4 99 99 99 99 99 ,mineral4 ,native silver ,formula4 ,ag4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses and in a strong oxidizing flame forms an incrustation of dark brown oxide on the charcoal4 ,if any antimony be present1 it affords a crimson incrustation4 7#d7 in forceps4 -- 7#e7 in borax4 ,gives the silver reactions4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 -- 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,antimonial silver ,formula4 ,ag#b,sb4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,gives off dense white fumes1 which are partly deposited in the tube4 7#c7 on charcoal4 ,fuses1 fumes strongly1 forming a white incrustation1 and when the antimony is nearly expelled a crimson one1 a nearly pure silver bead remains4 7#d7 in forceps4 -- 7#e7 in borax4 ,the incrustation formed on charcoal gives an antimony reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,silver glance ,formula4 ,ag,s4 ,behavior 7#a7 in glass-bulb4 -- 7#b7 in open tube4 ,gives off sulphurous acid4 7#c7 on charcoal4 ,gives off ,,so#b and is reduced to metallic silver4 ,if impure1 a small quantity of slag also remains4 7#d7 in forceps4 -- 7#e7 in borax4 ,the residual slag 7if any7 obtained upon charcoal gives an iron reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,as alone on charcoal4 ,the alkaline mass gives a sulphur reaction on polished silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,stephanite ,formula4 1,ag#f111,sb4 ,behavior 7#a7 in glass-bulb4 ,decrepitates1 fuses and gives a slight sublimate of sulphide of antimony4 7#b7 in open tube4 ,fuses and gives off ,,so#b and dense white antimonial fumes4 7#c7 on charcoal4 ,fuses and incrusts the charcoal with antimonious acid1 leaving ,ag with some antimony4 ,if the flame be continued1 a red incrustation is formed and finally a bead of pure silver remains surrounded by a small slag4 7#d7 in forceps4 -- 7#e7 in borax4 ,the residual slag obtained on the charcoal gives an iron and copper reaction4 7#f7 in mic4 salt4 ,as in borax4 7#g7 with carb4 soda4 ,the silver is reduced and the antimony passes off in dense fumes4 ,the fused alkali gives the sulphur reaction on silver4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,pyargyrite ,formula4 1,ag#c111,sb4 ,behavior 7#a7 in glass-bulb4 ,sometimes decrepitates1 fuses readily1 and1 when strongly heated1 gives a red sublimate of ,sb,s#c4 7#b7 in open tube4 ,as in the preceding4 7#c7 on charcoal4 ,fuses with much spirting and covers the charcoal with antimonial fumes4 ,when the residual ,ag,s is heated for some time in the oxidizing flame1 a bead of pure silver is obtained4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,as the preceding4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,proustite ,formula4 1,ag#c111;,as4 ,behavior 7#a7 in glass-bulb4 ,fuses and at a low red heat affords a small sublimate of ,as,s#c4 7#b7 in open tube4 ,gradually heated it gives off ,as,o#c and ,,so#b4 ,sometimes also antimony fumes4 7#c7 on charcoal4 ,as the preceding1 except that a large quantity of ,as,o#c and but little ,sb,o#c are given off4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,as stephanite1 except that much arsenic is given off and but little antimony4 7#h7 ,special reactions4 -- 99 99 99 99 99 ,mineral4 ,horn silver ,formula4 ,ag,cl4 ,behavior 7#a7 in glass-bulb4 ,fuses1 but undergoes no further change4 7#b7 in open tube4 -- 7#c7 on charcoal4 ,fuses readily in the oxidizing flame4 ,in the reducing flame is slowly reduced yielding metallic silver4 7#d7 in forceps4 -- 7#e7 in borax4 -- 7#f7 in mic4 salt4 -- 7#g7 with carb4 soda4 ,is rapidly reduced to metallic silver4 7#h7 ,special reactions4 ,if cut up into small pieces mixed with oxide of copper and then heated before the oxidizing flame upon charcoal1 it colors the flame blue4 ,,the ,,end4 99 99 99 99 99 ,transcriber's ,notes3 ,text italicized in the original book is surrounded by ''4 ,this book had many columnar tables1 often split across pages4 ,these have been transformed in data sheets for readability4 ,the notation is used for superscripted numbers1 indicating the composition of the various chemical compounds4 ,some of the element symbols were differenced by markings that were not defined in the book1 but are supposed to be valence markings4 ,these have been transcribed as follows3 '4' or '1' above element symbol 84,symbol or 81,symbol '-' above element symbol ,symbol '-' through element symbol ,symbol 444 ,so 444,al where the original text had ,al ,m where the original text had ,m 111 111,sb where the original text had ,sb 444 444,fe where the original text had ,fe1 line through the ,fe4