ISORGANIC CHEMISTRY. 101 I n o r g a n i c C h e m i s t P y. Preparation of Chemically Pure Hydrogen Peroxide. By MANN (Chem. Zeit., 12, 857).-Hiydrogen peroxide of commerce con- tains many impurities ; it is niixed with a 4 per cent. of phosphoric acid and then, while stirring vigorously, barium hydroxide is added until the solution is exactly neutral to litnius. The clear solution is poured into a cold saturated aolution of barium hydroxide, and the precipitate of barium peroxide is well washed and may be kept for the preparation of pure hydrogen peroxide. For this purpose, i t i8 made into a thin magma and carefully decomposed by dropping steadily into dilute sulphuric acid containing 18 per cent. of con- centrated acid; any excess of sulphuric acid being removed by hydroxide, and vice verSd.Excess of barium peroxide must be avoided as it decomposes hjdrogen peroxide. D. A. L.2 02 ABSTRACTS OF CHEMICAL PAPERS. t. 1 P. Compounds Of Chlorine with Iodine. By w. STosTENBEKER ( R e c . Trav. Chinz., 7, 152-205).-The only compounds of iodine with chlorine which are capable of existing in the solid state are IC1 and ICI,. Two modifications of the first exist which the author terms a and /3. IC1 is best, prepared by passing dry chlorine over iodine and then distilling the product with a few grams of iodine. If the distillate is allowed to solidify at -25", the a-modification is obtained in long, dark-red needlcs, melting a t 27.2". If the crystal- lisation take place between +5" and -lo", modification p is usually, but not invariably, obtained.When slowly formed, it crystullises in dark-red plates meltirig a t 13.9'. It is unstable and readily converted into the a-modification, into which it is gradually changed. The most favourable temperatures for its existence are between 0" and -10". If cooled below -12" it changes into the a-modifica- tion. The trichloride ICl, is prepared by treating iodine, or the liquid IC1 with excess of chlorine. It sublimes very readily and settles on the sides of the apparatus in slender, yellow needles. It melts a t the ordinary pressure a t temperatures varying between 20" and GO", but under a pressure of 16 atmos. melts regularly at 101". After fusion, it solidifies in brownish-red crystals. The author further shows tbat every mixture of the two elements, chlorine and iodine, is possible in the liquid state above a certain temperature which depends on the proportion of the two elements.Below that temperature, one of the substances Iz, ICla, IClP, ICI,, or c1, will separate in the solid state. I€ on a diagram representing pressures and temperatures the two points be taken at which chlorine and iodine melt, corresponding wlth the temperatures - 102" and 114.3', then between these points will lie the curve which is the locus of the points a t which the various mixtures of chlorine and iodine exist in the liquid state. These t w o end points are triple points for the pure elements, and on the intermediate curve will be found three quadruple points, each corresponding to equilibrium between four phases (comp. Roozeboom, Abstr., 1888, 1151).Phases present. Complete solidification will only occw a t the three distinct tern- peratures of the quadruple points, when separation of a mixture of the solids I, + IC1, IC1 + Ic13 or ICI, + C1, will take place. A study of the compounds of iodine and chlorine in the gaseous state shows that molecules IC1 exist i n that condition, and only suiTey slight dissociation even a t 80°, whereas ICl3 cannot exist as gas, the molecules undergoing complete dissociation. H. C.INORGANIC CHEMISTRY. 103 Theory of the Lead Chamber Process. By F. RASCHIG (Anualen, 248, 123-140), and by G. LUNGE ( B e y , , 21, 3223-3240). -Controversial papers. Compounds of Ammonia with Selenious Anhydride. By C. A. CAMERON and J. MACALLAN (Proc. Boy. Soc., 44, 112-115).-Dry ammonia passed into an alcoholic solution of selenious anhydride forrris amrnoiLiurn seEenosamate, NH4*Se0,*NH2, which crys tallises in hexa- gonal prisms and pyramids. It loses ammonia very easily even on exposure to air or treatment with solvents and on heating.It is only partially converted into ammonium selenate by the action of water even after continued boiling. Potassium hydroxide a t once liberates ammonia. Sulphuric acid reacts violently with it, and chlorine oxidises it to ammonium selenate. Sulphurous anhydride and stannous chloride reduce it with separation of selenium. The acid salt formed from the above by loss of ammonia has the composi- tion (NH4)H(SeO2-NH2),, and is a deliquescent salt soluble in alcohol. It behaves like the normal salt, but is much more stable. When strongly heated, it is decomposed iiito ammonium selenite, ammonia, water, nitrogen and fused selenium.These compounds of selenious anhydride are more akin to the compounds of sulphuric anhydride with ammonia than to those of sulphurous anhydride. By V. WEDENSKY ( J . BUSS. Chem. Xoc., 1888, 20, 29--32).-When phosphorous acid is dis- solved in acetic anhydride, a colourless crystalline substance separates after a time. This is washed with ether and analysed ; the results agree with the formula of a monacetyl-derivative of phosphorous acid, (C,H,O) H2POs. When acetic anhydride acts on phosphorus trichloride, an analogous compound is obtained ; this, however, seems to be a mixture, and cannot be obtained free from chlorine.A H. K. 1’. Constitution of Phosphorous Acid. phosphorous triacetyl-derivative could not be obtained. B. l3. Compounds of Arsenious Acid with Sodium Iodide and Bromide. By F. R~~DORFF (Ber., 21, 30.51--305.3).-The compound NaEh,2As2O, is obtained when arsenious acid (20 grams) and sodium bromide (120 grams) are dissolved in boiling water (350 c.c.), and the filtered solution allowed to cool slowly (compare Abstr., 1887, 107). It crjstallises in hexagonal plates and is decomposed when warmed with water. The compound NaI, 2As203, prepai-ed by dissolving arsenious acid (22 grams) and sodium iodide (60 grams) in hot water (500 c.c.), cry stallises in hexagonal plates and is decomposed by hot water. Preparation of Boron and Silicon by Electrolysis. By W. HANPE (Chem.Zeit., 12, 841).-When fused borax is submitted to electrolysis in a gas-carbon crucible with a platinum positive and a gas-carbon negative electrode, oxygen is evolved from the platinum, whilst in the first instance sodium separates a t the negative electrode, but this by a secondary reaction liberates boron. The negative electrode is from time to time withdrawn from the crucible, and P. S. K.104 ABSTRACTS OF CHEJTICXL PAPERS. when cool, the slag carrying the boron i q carefully knocked off. Th;s is treated with hydrochloric acid and water, leaving pure amorphous boron mixed with a small quantity OF carbon and some isolated microscopic crystals of, a t present, anknown composition. Fused boric anhydride does not conduct. But amorphous silicon may be prepared in a similar manner from fused sodium silicate.Beryllium Silicates. By P. HAumFEuTLLF: and A. PERREY (Compt. rend., 107, 786-789) .-If the constituents of an aluminium or beryllium leucite are fused a t 600-800" with excess of potassium vanadate, mineralisation takes place rapidly, b u t the cornposition of the product varies as the vanadate gives up more or less of its alkali, and it is rarely homogeneous. The product is washed with water and very dilute potash, and tJhe crystalline constituents are separated by solutions of cadmium tungstoborate of varying specific gravity. I n the alum- inium compounds, the potassium and aluminium are always present in the proportion A1,03 : &O, whilst in the beryllium com- pounds the ratio of beryllia to potash varies from 1.25 to 0.5.The silicate containing Be,03,2K20 is obtained with r), mixture which always contains an excess of alkali, whilst the silicate containing Be,03,K20 is obtained with a neutral mixtme. In the aiuminium compounds, the ratio of silica to potash varies from 4 ko 5, whilst in the beryllium compounds the same ratio varies from 4.5 to 5.0, In the latter case, the product is always heterogeneous, and probably results from the simultaneous crgstallisation of silicates containing 4sio2 and 5Si02. The silicate 4SiO2,Re,O3,KZO is obtained in icosi- tetrahedrons by rapidly heating its constituents to st high temperature and cooling very gradually. Products were also obtained containing both alumina and beryllia. They are all fusible, and are homogeneous with respect to sp.gr. The following ratios were observed :-K,O : SiO, : : 1 : 4.5-4.8 ; K,O : R,O, : : 1 : 0*75-1*0 ; Be,O, : A120, : : 1 : 0.5-1.75. Silicates containing beryllia and ferric oxide are yellowiRh, crystallise in the same form, and are bomogeneoiis with respect to specific gravity. The following ratios were observed :-KzO : SiO, : : 1 : 4.59-5.0; K,O : R20, : : 1 : 0.6-1-3 ; Be203 : 'Fez03 : : 1 : 0.3-1.3. Alumina and silica in the proportion of 1 mol. of A1203 to 6 mols. of Si03, heated with potassium vanadate, yield orthoclase in macled, prismatic crystals ; but with beryllia in place of alumina, the crystals are always icositetrahedrons. With a mixture of alumina and I,eryllia, however, non-macled, prismatic, crystals, of the composition GSi02,Rz03,K20 are obtained, and are homogeneous with respect to bpecific gravity.The ratio SiO, : K,O remains constant, whilst the iatio A1203 : BezO, varies. The silicates obtained w i t h beryllium may be regarded as mixtures of the following compounds :- D A. L. All the products crystallise i n icositetrahedrons, a2. 8Si02,Be203,2K20 4Si02,Rez03, K 2 0 5Si02,Be203,K,0. 10 S i O,, Be203, 2K20, The fact that the beryllia can be replaced by alumina and ferricIN0 RGANIC CHEMl ST RY. 105 oxide in these compounds, and can replace alumina in orthoclase, combined with the well-known relations of beryllium to magnesium, would seem to indicate that beryllia has sometimes the functions of a monoxide and sometimes those of a sesquioxide. Occlusion of Gas by Electrolytic Copper.By A. SORET (Qompt. r e d . , 107, 733-734) .-With dilute copper solutions, unless the current is very weak, the precipitated metal is spongy, the nature of the deposit depending not only on the strength of the solution and the intensity of the current, but also on the proportion of free acid present. Lenz obtained 4.4 vols. of hydrogen from 1 vol. of deposited copper. The author finds that eleclroljtic copper always contains hydrogen, which, however, is simply occluded. There is a connection between the volume of gas occluded and the temperature and acidity of the soliltion. These conditions also affect the malleability of the metallic deposit. The occluded hydrogen sometimes contains small quantities of carbonic anhydride and traces of carbonic oxide. Mechanical Properties of Metals in Relation to the Periodic Law.By W. C. KOBERTS-AUSTEN (Proc. Roy. Xoc., 43, 425-428). -Very pure gold was alloyed with 0.2 per cent. of various metals, and the tensile strength determined. The tenacity was found to be affected by the elements in the order of their atomic volumes, those elements which have a higher atomic volume than gold diminishing its tenacity very considerably, whilst silver, which has nearly the same atomic volume as gold, hardly affects either its tenacity or extensibility. Hence it appears that Carnelley’s law-that ‘‘ the properties of compounds of the elements are a periodic function of their atomic weights,” may also be applied to alloys. Tenacity was chosen for examination, since those metals which are most tenacious liave the highest melting points, and the melting point, according to Pictet, is intimately connected with the lengths of the molecular oscillations.H. I(. T. Dissolution of Iron in Aqueous Soda. By G. ZIRNIT~ (Chem. Zeit., 12, 355).-When a strong current of air is blown into a hot, concentrated solution of soda containing about 34 per cent. of hydr- oxide, standing in an iron vessel, or to which finely divided hydrated ferric oxide has been added, perceptible quantities of iron are dis- solved without colouring the liquid. The solution remains clear and colourless for several days at tlhe ordinary temperature, but ultimately becomes turbid, yellow, and finally red, owing to the separation of the hydrated ferric oxide ; this colour, howerer, disappears again on heating.When the colourless solution is diluted, the ferric oxide is precipitated in about half an hour, but is redissolved by concentrating the diluted solution. Hydrogen sulphide a t first produces a deep, cherry-red coloration in the colourless liquid, and on continuing the action a greenish-black precipitate is formed, leaving a clear solution free from iron, but slightly yellow from sodium sulphide. It is suggested that the iron exists in solution as sodium perferrate, NaFe04. D. A. L. VOL. LVI. i C. B. B. C. H. B.106 ABSTRACTS OF CHEMICAL PAPERS. Ammonium Fluoroxymolybdates. By F. MAURO (Chsnz. CPntr., 1888, 1056-1057, from Hem. R. Acad. dei Lincei [4], 4, 481-488). - Triummonium Jluoroxyrnoly bd Ute, Mooz F2,3NH4F, prepared by evaporating a solution of ammonium molybdate in excess of am- monium fluoride solution acidified with hydrogen fluoride, is obtained in clear and colourless rhombic prisms.The faces (loo), (OlO), (120), and (011)-were observed, and the angles (100) : (110) = 28" 36', (011) : (011) = 82" 29', and (011) : (110) = 71" 36'. Axial ratio, a : b : c = 0.5452 : 1 : 0.8767. It is soluble in water, pro- ducing an acid solution. On heating, white fumes are evolved and anhydrous molybdic acid remains. It contains no water of crystal- lisat ion. Fluorurnmonium-moly bdic anhydride, Moo3, ZNH4F, prepared by adding ammonia to the solution of the last-named salt, and is thus obtained as a white, microscopic, crystalline precipitate. Larger crystals may be obtained by dissolving the compound in a hot solu- tion of ammonium fluoride and ammonia, and allowing to evaporate spontaneously by exposure to the air o r over sulphuric acid, when the salt crystallises out-at first as prisms, but later in octahedrons.If the precipitated salt is simply dissolved in ammonia and then allowed to evaporate, monoclinic crystals of hydrated ammonium mol ybdate separate first, then, later, the prisms and octahedrons of the new salt. The crystals appear usually in the form of twins, grown together in such a manner as to give the crystal the appearance of it hexagonal prism. They are shining, transparent, light-yellow, and belong to the rhombic system; u : h : c = 0.57464 : 1 : 0.67705. The faces (OlO), (Ool), (110), and (011) were ob,served. Twinning plane (110). The angles measured were: (110) : (110) = 59" 46'; (010) : (110) = 60" 7' ; (010) : (011) = 55" 54'; and (110) : (011) = 7 3 O 47". This salt is decomposed by water.It is anhydrous, and is decomposed on heating above looo, molybdic acid remaining. Normal ammonium Jluoroxy moly bda.te? Mo02F2,2NH4F, is prepared from the last-named salt by spontaneous evaporation of the aqueous solution, rendered acid with hydrogen fluoride. It consists of brightly shining, transparent, colourless plates or prisms belonging to the rhombic system; a : b : c = 0.8413 : 1 : 1.0164. The faces (OlO), (OOl), ( O l l ) , (eel), and (221) were observed. The angles measured were: (001) : (201) = 67" 31'; (001) : (011) = 45" 28'; (001) : (221) = 72" 26'; (291) : (011) = 74" 27' ; (011) : (221) = 49" 31' ; and (201) : (221) = 37" 52'.This salt is sparingly soluble in water, and is decomposed by heating above 100"; ammonium fluoride and hydrogen fluoride are evolved, leaving molybdic acid. Octahedric ammonium Jluoroxymolybdate, MoO~F~,~NH~F, (NH~)~MoO~, a double salt of ammonium flnoroxymolybdate with ammonium molyb- date, is prepared by allowing a solution of triammonium fluoroxy- molybdate i n ammonia to evaporate spontaneously in the air or over sulphuric acid. It forms small, colourless, transparent, lustrous octa- hedrons, which gradually disintegrate when exposed to the air. It is isomvrphous with the corresponding double salt of tungsten. It isINORQANIC CHENISTRY. 1 0 I soluble in water, and does not again crystallise out of the solution. It suffers decomposition, like the other salts, when heated above 100".Ammonium dimolybdate, 2Mo03,(NH&0 + H,O, prepared by dis- solving flnorammonium-molybdic anhydride in ammonia andC allowing ths solution to remain. It forms transparent, colourless, lwstwus, monoclinic crystals-usualiy pyramidal ; a : b : c = 0.99628 : 1 : 0'94497 ; /3 = 'IS0 47' 41". TJe faces observed were: (loo), (OlO), (Oll), (lOi), ( l l l ) , and (111) ; the ;t_ngles : (001) : (100) = 72" 48' ; (001) : (iOl) = 52'44' ; (100) : (101) = 5P" 28'. By heating above 100" this compound behaves exactly like the other members of the series, and leaves a residue of molybdic acid. By L. VIGRON (Compt. r m d . , 107, 734-'737).-When sheet zinc is immersed in a solution of a kin salt which contains no free acid, and the precipitated tin is washed with water and dried in coil- tact with air, the product is iafusible and burns like tinder wlieii heated in presence o€ air.If heated to redness in a porcelain tube in a current of carbonic anhydride for two hours, it separates into small globules of fused tin and a grey powder. These are separated by levigrttion, and atfter the powder has been dried, it burns readily when heated in the air. The infusible tin occurs in slender, denriritica forms of sp. gr. 6.910 to 7.198 at -15", and contains 96 to 97.3 p ~ r cent. of tin. I t dissolves readily in hydrochloric acid with evolutioir of hydrogen. The alteration in the properties of the tin does not, tako place during precipitation, but when the tin is dried in contact wlttl air it is partially converted into stannous oxide, the alteration taking place the more readily the less the proportion of free acid in the liquid from which the tin is precipitated.If much free acid is present, the tin does not oxidise when dried. The proportion of stannous oxide in the oxidised tin varies from 22.5 to 33.4 per cent., and when combustion takes place shannic oxide is formed. J. W. L. Tin. C. €I. B. Fluorine-derivatives of Vanadium and its Analogues. fiY E. PETERSEN (Ber., 21, 3257--3259).-The following compounds were prepared by treating the oxides dissolved in hydrofluoric wid, wibh a solution of the various fluorides. ( I . ) Compounds derived fyont the 8esgwioxide.-(1) V,F,, + 6Hz0, large, readily soluble, dark green rhombohedra; (2) V2Ffi,4KF + 2H20, bright green, sparingly soluble, crystalline powder ; (3) \T,F6,6AmF, small, grass-green, regular octahedra; (4) CrZF6,6AmF( Wagner, Abstr., 1886, 676), rather darker green octahedra ; (5) Ti,F',,GAmF (Picciiii, Comnpt. rend., 97), small, red-violet octahedra ; (6) A1,Ffi,6AmF, spay- ingly soluble, dazzling white, crystalline powder ; (7) V2F6,4AmF + 2Hz0, emerald-green, rather large crystals, like octahedra, but politr- king ; (8) V2F6,2AmF' + 4H20, darker green, laniellar aggregates ; (9) V2F6,5NaF + HJ), bright green, sparingly soluble.crystalline powder ; (10) VzF6,2CoF~ + 14H20, small, dark green, monoclinic prisms ; (11) CrzFfi,2CoPz + 1PH20, pure dark green, monochic prisms ; (la) V2J?6,2XiF2 + 14H20, grass-green, monoclinic prisms ; i 2LO8 ABSTRACTS OF CHEUICXL PAPERS.(13) Cr2F,,2NiF’, + 14H20. emerald-green, monoclinic prisms. last four compounds are isomorphous. (11.) Compounds corresponding with Vanadium Dioxide.- (14) VOF2,3AmF, small, blue, almost regular octahedra, but polar- ising; (15) VOF2,2AmF + H20 (Baker, Trans., 2878, 392), larger, dark blue prisms ; (16) 4VOF2,7AmP + FiH,O, still darker blue, lamellar aggregates ; (17) 4VF4,2AmF + zH,O, small, blue-green prisms, stable only in solutions, strongly acidified with hvdrogen fluoride; (18) 3VOF2,7KF ; ( 1 9 ) VOF,,SKF ; (20) 3VOF2,8NaF + 2H20. These three form bright blue, sparingly soluble, crystalline powders. (111.) Compourds derived from the Pentoaide.--(21) VOF,,ZKF, colourless, crystalline powder ; (22) 2VOF3,3KF,HF, white, lustrous prisms ; ( 2 3 ) VP5,VOB’,,4KF, colourless aggregates of very slender needles ; ( 2 4 ) VOZF,2KF, golden-yellow, lustrous, hexagonal prisms, (25) 2\T02F,3KF, bright yellow prisms ; (26) 5VOF3,9AmF,3HF, colourless, dull lustrous prisms ; (27) V02F,3AmF, larger, straw- coloured, probably rhombic crvstals ; (28) 4V02F,7AmF,HP, white, lustrous aggregates ; (29) 2Nb205,3KF + 5H20, lust’rous white, sparingly soluble, crystalline powder ; (30) Nb205,KF + 3H20, colourless prisms. The compounds 14, 19, and 27 seem to be identical with those prepared by Piccini and Giorgis (Atti d.R. Acc. d e i Lincei, 1888, 590, and GIaz., 18, 186). The thermochemical relation of hydrogen fluoride to the sesqui- oxides of iron, chromium, and vanadium was determined. The following numbers were obtained for the heat of neutralisation in dilute aqueous solutions:-(Fe,0,H6,6HF + Aq) = 47500 cal., (Cr2o6€T6,6AF + Aq) = 50330 cal., (VZ(J6H,,6HF + Aq) = 52240 cal.The N. H. M. Decomposition of Antimony Sulphide by Boiling Water. By W. ELBERS (Chelrz. Zeit., 12, 355-356).- When antimonious sulphide is boiled with water, it is decomposed with the evolution of hydrogen sulphide and the formation of antimonious anhydride. I n this way 0.05 gram of the sulphide was completely converted into the anhydride in 14 hours; the liquid then had a slightly alitaline reaction. D. A. L.ISORGANIC CHEMISTRY. 101I n o r g a n i c C h e m i s t P y.Preparation of Chemically Pure Hydrogen Peroxide. ByMANN (Chem. Zeit., 12, 857).-Hiydrogen peroxide of commerce con-tains many impurities ; it is niixed with a 4 per cent.of phosphoricacid and then, while stirring vigorously, barium hydroxide is addeduntil the solution is exactly neutral to litnius. The clear solution ispoured into a cold saturated aolution of barium hydroxide, and theprecipitate of barium peroxide is well washed and may be kept forthe preparation of pure hydrogen peroxide. For this purpose, i t i8made into a thin magma and carefully decomposed by droppingsteadily into dilute sulphuric acid containing 18 per cent. of con-centrated acid; any excess of sulphuric acid being removed byhydroxide, and vice verSd. Excess of barium peroxide must beavoided as it decomposes hjdrogen peroxide. D. A. L2 02 ABSTRACTS OF CHEMICAL PAPERS.t.1 P.Compounds Of Chlorine with Iodine. By w. STosTENBEKER( R e c . Trav. Chinz., 7, 152-205).-The only compounds of iodinewith chlorine which are capable of existing in the solid state areIC1 and ICI,. Two modifications of the first exist which the authorterms a and /3. IC1 is best, prepared by passing dry chlorine overiodine and then distilling the product with a few grams of iodine.If the distillate is allowed to solidify at -25", the a-modification isobtained in long, dark-red needlcs, melting a t 27.2". If the crystal-lisation take place between +5" and -lo", modification p is usually,but not invariably, obtained. When slowly formed, it crystullisesin dark-red plates meltirig a t 13.9'. It is unstable and readilyconverted into the a-modification, into which it is gradually changed.The most favourable temperatures for its existence are between0" and -10".If cooled below -12" it changes into the a-modifica-tion.The trichloride ICl, is prepared by treating iodine, or the liquidIC1 with excess of chlorine. It sublimes very readily and settles onthe sides of the apparatus in slender, yellow needles. It melts a t theordinary pressure a t temperatures varying between 20" and GO", butunder a pressure of 16 atmos. melts regularly at 101". After fusion, itsolidifies in brownish-red crystals.The author further shows tbat every mixture of the two elements,chlorine and iodine, is possible in the liquid state above a certaintemperature which depends on the proportion of the two elements.Below that temperature, one of the substances Iz, ICla, IClP, ICI,, or c1, will separate in the solid state.I€ on a diagram representingpressures and temperatures the two points be taken at which chlorineand iodine melt, corresponding wlth the temperatures - 102" and114.3', then between these points will lie the curve which is thelocus of the points a t which the various mixtures of chlorine andiodine exist in the liquid state. These t w o end points are triplepoints for the pure elements, and on the intermediate curve will befound three quadruple points, each corresponding to equilibriumbetween four phases (comp. Roozeboom, Abstr., 1888, 1151).Phases present.Complete solidification will only occw a t the three distinct tern-peratures of the quadruple points, when separation of a mixture ofthe solids I, + IC1, IC1 + Ic13 or ICI, + C1, will take place.A study of the compounds of iodine and chlorine in the gaseousstate shows that molecules IC1 exist i n that condition, and only suiTeyslight dissociation even a t 80°, whereas ICl3 cannot exist as gas, themolecules undergoing complete dissociation.H. CINORGANIC CHEMISTRY. 103Theory of the Lead Chamber Process. By F. RASCHIG(Anualen, 248, 123-140), and by G. LUNGE ( B e y , , 21, 3223-3240).-Controversial papers.Compounds of Ammonia with Selenious Anhydride. By C. A.CAMERON and J. MACALLAN (Proc. Boy. Soc., 44, 112-115).-Dryammonia passed into an alcoholic solution of selenious anhydride forrrisamrnoiLiurn seEenosamate, NH4*Se0,*NH2, which crys tallises in hexa-gonal prisms and pyramids.It loses ammonia very easily even onexposure to air or treatment with solvents and on heating. It isonly partially converted into ammonium selenate by the action ofwater even after continued boiling. Potassium hydroxide a t onceliberates ammonia. Sulphuric acid reacts violently with it, andchlorine oxidises it to ammonium selenate. Sulphurous anhydrideand stannous chloride reduce it with separation of selenium. Theacid salt formed from the above by loss of ammonia has the composi-tion (NH4)H(SeO2-NH2),, and is a deliquescent salt soluble in alcohol.It behaves like the normal salt, but is much more stable. Whenstrongly heated, it is decomposed iiito ammonium selenite, ammonia,water, nitrogen and fused selenium.These compounds of seleniousanhydride are more akin to the compounds of sulphuric anhydridewith ammonia than to those of sulphurous anhydride.By V. WEDENSKY ( J . BUSS.Chem. Xoc., 1888, 20, 29--32).-When phosphorous acid is dis-solved in acetic anhydride, a colourless crystalline substance separatesafter a time. This is washed with ether and analysed ; the resultsagree with the formula of a monacetyl-derivative of phosphorousacid, (C,H,O) H2POs. When acetic anhydride acts on phosphorustrichloride, an analogous compound is obtained ; this, however, seemsto be a mixture, and cannot be obtained free from chlorine. AH. K. 1’.Constitution of Phosphorous Acid.phosphorous triacetyl-derivative could not be obtained.B.l3.Compounds of Arsenious Acid with Sodium Iodide andBromide. By F. R~~DORFF (Ber., 21, 30.51--305.3).-The compoundNaEh,2As2O, is obtained when arsenious acid (20 grams) andsodium bromide (120 grams) are dissolved in boiling water (350 c.c.),and the filtered solution allowed to cool slowly (compare Abstr.,1887, 107). It crjstallises in hexagonal plates and is decomposedwhen warmed with water.The compound NaI, 2As203, prepai-ed by dissolving arseniousacid (22 grams) and sodium iodide (60 grams) in hot water (500 c.c.),cry stallises in hexagonal plates and is decomposed by hot water.Preparation of Boron and Silicon by Electrolysis. By W.HANPE (Chem. Zeit., 12, 841).-When fused borax is submitted toelectrolysis in a gas-carbon crucible with a platinum positive and agas-carbon negative electrode, oxygen is evolved from the platinum,whilst in the first instance sodium separates a t the negative electrode,but this by a secondary reaction liberates boron. The negativeelectrode is from time to time withdrawn from the crucible, andP.S. K104 ABSTRACTS OF CHEJTICXL PAPERS.when cool, the slag carrying the boron i q carefully knocked off. Th;sis treated with hydrochloric acid and water, leaving pure amorphousboron mixed with a small quantity OF carbon and some isolatedmicroscopic crystals of, a t present, anknown composition. Fusedboric anhydride does not conduct. But amorphous silicon may beprepared in a similar manner from fused sodium silicate.Beryllium Silicates.By P. HAumFEuTLLF: and A. PERREY(Compt. rend., 107, 786-789) .-If the constituents of an aluminiumor beryllium leucite are fused a t 600-800" with excess of potassiumvanadate, mineralisation takes place rapidly, b u t the cornposition ofthe product varies as the vanadate gives up more or less of its alkali,and it is rarely homogeneous. The product is washed with waterand very dilute potash, and tJhe crystalline constituents are separatedby solutions of cadmium tungstoborate of varying specific gravity.I n the alum-inium compounds, the potassium and aluminium are alwayspresent in the proportion A1,03 : &O, whilst in the beryllium com-pounds the ratio of beryllia to potash varies from 1.25 to 0.5. Thesilicate containing Be,03,2K20 is obtained with r), mixture whichalways contains an excess of alkali, whilst the silicate containingBe,03,K20 is obtained with a neutral mixtme.In the aiuminiumcompounds, the ratio of silica to potash varies from 4 ko 5, whilst inthe beryllium compounds the same ratio varies from 4.5 to 5.0, Inthe latter case, the product is always heterogeneous, and probablyresults from the simultaneous crgstallisation of silicates containing4sio2 and 5Si02. The silicate 4SiO2,Re,O3,KZO is obtained in icosi-tetrahedrons by rapidly heating its constituents to st high temperatureand cooling very gradually.Products were also obtained containing both alumina and beryllia.They are all fusible, and are homogeneous with respect to sp. gr.The following ratios were observed :-K,O : SiO, : : 1 : 4.5-4.8 ;K,O : R,O, : : 1 : 0*75-1*0 ; Be,O, : A120, : : 1 : 0.5-1.75. Silicatescontaining beryllia and ferric oxide are yellowiRh, crystallise in thesame form, and are bomogeneoiis with respect to specific gravity.The following ratios were observed :-KzO : SiO, : : 1 : 4.59-5.0;K,O : R20, : : 1 : 0.6-1-3 ; Be203 : 'Fez03 : : 1 : 0.3-1.3.Alumina and silica in the proportion of 1 mol.of A1203 to 6 mols. ofSi03, heated with potassium vanadate, yield orthoclase in macled,prismatic crystals ; but with beryllia in place of alumina, the crystalsare always icositetrahedrons. With a mixture of alumina andI,eryllia, however, non-macled, prismatic, crystals, of the compositionGSi02,Rz03,K20 are obtained, and are homogeneous with respect tobpecific gravity.The ratio SiO, : K,O remains constant, whilst theiatio A1203 : BezO, varies.The silicates obtained w i t h beryllium may be regarded as mixturesof the following compounds :-D A. L.All the products crystallise i n icositetrahedrons, a2.8Si02,Be203,2K204Si02,Rez03, K 2 0 5Si02,Be203,K,0.10 S i O,, Be203, 2K20,The fact that the beryllia can be replaced by alumina and ferriIN0 RGANIC CHEMl ST RY. 105oxide in these compounds, and can replace alumina in orthoclase,combined with the well-known relations of beryllium to magnesium,would seem to indicate that beryllia has sometimes the functions of amonoxide and sometimes those of a sesquioxide.Occlusion of Gas by Electrolytic Copper. By A. SORET(Qompt.r e d . , 107, 733-734) .-With dilute copper solutions,unless the current is very weak, the precipitated metal is spongy,the nature of the deposit depending not only on the strength of thesolution and the intensity of the current, but also on the proportionof free acid present. Lenz obtained 4.4 vols. of hydrogen from 1 vol.of deposited copper.The author finds that eleclroljtic copper always contains hydrogen,which, however, is simply occluded. There is a connection betweenthe volume of gas occluded and the temperature and acidity of thesoliltion. These conditions also affect the malleability of the metallicdeposit. The occluded hydrogen sometimes contains small quantitiesof carbonic anhydride and traces of carbonic oxide.Mechanical Properties of Metals in Relation to the PeriodicLaw. By W.C. KOBERTS-AUSTEN (Proc. Roy. Xoc., 43, 425-428).-Very pure gold was alloyed with 0.2 per cent. of various metals,and the tensile strength determined. The tenacity was found to beaffected by the elements in the order of their atomic volumes, thoseelements which have a higher atomic volume than gold diminishingits tenacity very considerably, whilst silver, which has nearly thesame atomic volume as gold, hardly affects either its tenacity orextensibility. Hence it appears that Carnelley’s law-that ‘‘ theproperties of compounds of the elements are a periodic function oftheir atomic weights,” may also be applied to alloys. Tenacity waschosen for examination, since those metals which are most tenaciousliave the highest melting points, and the melting point, according toPictet, is intimately connected with the lengths of the molecularoscillations.H. I(. T.Dissolution of Iron in Aqueous Soda. By G. ZIRNIT~ (Chem.Zeit., 12, 355).-When a strong current of air is blown into a hot,concentrated solution of soda containing about 34 per cent. of hydr-oxide, standing in an iron vessel, or to which finely divided hydratedferric oxide has been added, perceptible quantities of iron are dis-solved without colouring the liquid. The solution remains clear andcolourless for several days at tlhe ordinary temperature, but ultimatelybecomes turbid, yellow, and finally red, owing to the separation of thehydrated ferric oxide ; this colour, howerer, disappears again onheating.When the colourless solution is diluted, the ferric oxide isprecipitated in about half an hour, but is redissolved by concentratingthe diluted solution. Hydrogen sulphide a t first produces a deep,cherry-red coloration in the colourless liquid, and on continuing theaction a greenish-black precipitate is formed, leaving a clear solutionfree from iron, but slightly yellow from sodium sulphide. It issuggested that the iron exists in solution as sodium perferrate,NaFe04. D. A. L.VOL. LVI. iC. B. B.C. H. B106 ABSTRACTS OF CHEMICAL PAPERS.Ammonium Fluoroxymolybdates. By F. MAURO (Chsnz. CPntr.,1888, 1056-1057, from Hem. R. Acad. dei Lincei [4], 4, 481-488).- Triummonium Jluoroxyrnoly bd Ute, Mooz F2,3NH4F, prepared byevaporating a solution of ammonium molybdate in excess of am-monium fluoride solution acidified with hydrogen fluoride, is obtainedin clear and colourless rhombic prisms.The faces (loo), (OlO),(120), and (011)-were observed, and the angles (100) : (110) =28" 36', (011) : (011) = 82" 29', and (011) : (110) = 71" 36'. Axialratio, a : b : c = 0.5452 : 1 : 0.8767. It is soluble in water, pro-ducing an acid solution. On heating, white fumes are evolved andanhydrous molybdic acid remains. It contains no water of crystal-lisat ion.Fluorurnmonium-moly bdic anhydride, Moo3, ZNH4F, prepared byadding ammonia to the solution of the last-named salt, and is thusobtained as a white, microscopic, crystalline precipitate. Largercrystals may be obtained by dissolving the compound in a hot solu-tion of ammonium fluoride and ammonia, and allowing to evaporatespontaneously by exposure to the air o r over sulphuric acid, when thesalt crystallises out-at first as prisms, but later in octahedrons.Ifthe precipitated salt is simply dissolved in ammonia and then allowedto evaporate, monoclinic crystals of hydrated ammonium mol ybdateseparate first, then, later, the prisms and octahedrons of the new salt.The crystals appear usually in the form of twins, grown together insuch a manner as to give the crystal the appearance of it hexagonalprism. They are shining, transparent, light-yellow, and belong tothe rhombic system; u : h : c = 0.57464 : 1 : 0.67705. The faces(OlO), (Ool), (110), and (011) were ob,served.Twinning plane (110).The angles measured were: (110) : (110) = 59" 46'; (010) : (110) =60" 7' ; (010) : (011) = 55" 54'; and (110) : (011) = 7 3 O 47". Thissalt is decomposed by water. It is anhydrous, and is decomposed onheating above looo, molybdic acid remaining.Normal ammonium Jluoroxy moly bda.te? Mo02F2,2NH4F, is preparedfrom the last-named salt by spontaneous evaporation of the aqueoussolution, rendered acid with hydrogen fluoride. It consists of brightlyshining, transparent, colourless plates or prisms belonging to therhombic system; a : b : c = 0.8413 : 1 : 1.0164. The faces (OlO), (OOl),( O l l ) , (eel), and (221) were observed. The angles measured were:(001) : (201) = 67" 31'; (001) : (011) = 45" 28'; (001) : (221) =72" 26'; (291) : (011) = 74" 27' ; (011) : (221) = 49" 31' ; and(201) : (221) = 37" 52'.This salt is sparingly soluble in water, andis decomposed by heating above 100"; ammonium fluoride andhydrogen fluoride are evolved, leaving molybdic acid.Octahedric ammonium Jluoroxymolybdate,MoO~F~,~NH~F, (NH~)~MoO~,a double salt of ammonium flnoroxymolybdate with ammonium molyb-date, is prepared by allowing a solution of triammonium fluoroxy-molybdate i n ammonia to evaporate spontaneously in the air or oversulphuric acid. It forms small, colourless, transparent, lustrous octa-hedrons, which gradually disintegrate when exposed to the air. It isisomvrphous with the corresponding double salt of tungsten. It iINORQANIC CHENISTRY. 1 0 Isoluble in water, and does not again crystallise out of the solution.Itsuffers decomposition, like the other salts, when heated above 100".Ammonium dimolybdate, 2Mo03,(NH&0 + H,O, prepared by dis-solving flnorammonium-molybdic anhydride in ammonia andC allowingths solution to remain. It forms transparent, colourless, lwstwus,monoclinic crystals-usualiy pyramidal ;a : b : c = 0.99628 : 1 : 0'94497 ; /3 = 'IS0 47' 41".TJe faces observed were: (loo), (OlO), (Oll), (lOi), ( l l l ) , and(111) ; the ;t_ngles : (001) : (100) = 72" 48' ; (001) : (iOl) = 52'44' ;(100) : (101) = 5P" 28'. By heating above 100" this compoundbehaves exactly like the other members of the series, and leaves aresidue of molybdic acid.By L. VIGRON (Compt. r m d . , 107, 734-'737).-When sheetzinc is immersed in a solution of a kin salt which contains no freeacid, and the precipitated tin is washed with water and dried in coil-tact with air, the product is iafusible and burns like tinder wlieiiheated in presence o€ air. If heated to redness in a porcelain tubein a current of carbonic anhydride for two hours, it separates intosmall globules of fused tin and a grey powder. These are separatedby levigrttion, and atfter the powder has been dried, it burns readilywhen heated in the air.The infusible tin occurs in slender, denririticaforms of sp. gr. 6.910 to 7.198 at -15", and contains 96 to 97.3 p ~ rcent. of tin. I t dissolves readily in hydrochloric acid with evolutioirof hydrogen. The alteration in the properties of the tin does not, takoplace during precipitation, but when the tin is dried in contact wlttlair it is partially converted into stannous oxide, the alteration takingplace the more readily the less the proportion of free acid in theliquid from which the tin is precipitated.If much free acid ispresent, the tin does not oxidise when dried. The proportion ofstannous oxide in the oxidised tin varies from 22.5 to 33.4 per cent.,and when combustion takes place shannic oxide is formed.J. W. L.Tin.C. €I. B.Fluorine-derivatives of Vanadium and its Analogues. fiY E. PETERSEN (Ber., 21, 3257--3259).-The following compounds wereprepared by treating the oxides dissolved in hydrofluoric wid, wibh asolution of the various fluorides.( I . ) Compounds derived fyont the 8esgwioxide.-(1) V,F,, + 6Hz0,large, readily soluble, dark green rhombohedra; (2) V2Ffi,4KF + 2H20,bright green, sparingly soluble, crystalline powder ; (3) \T,F6,6AmF,small, grass-green, regular octahedra; (4) CrZF6,6AmF( Wagner, Abstr.,1886, 676), rather darker green octahedra ; (5) Ti,F',,GAmF (Picciiii,Comnpt. rend., 97), small, red-violet octahedra ; (6) A1,Ffi,6AmF, spay-ingly soluble, dazzling white, crystalline powder ; (7) V2F6,4AmF +2Hz0, emerald-green, rather large crystals, like octahedra, but politr-king ; (8) V2F6,2AmF' + 4H20, darker green, laniellar aggregates ;(9) V2F6,5NaF + HJ), bright green, sparingly soluble.crystallinepowder ; (10) VzF6,2CoF~ + 14H20, small, dark green, monoclinicprisms ; (11) CrzFfi,2CoPz + 1PH20, pure dark green, monochicprisms ; (la) V2J?6,2XiF2 + 14H20, grass-green, monoclinic prisms ;i LO8 ABSTRACTS OF CHEUICXL PAPERS.(13) Cr2F,,2NiF’, + 14H20. emerald-green, monoclinic prisms.last four compounds are isomorphous.(11.) Compounds corresponding with Vanadium Dioxide.-(14) VOF2,3AmF, small, blue, almost regular octahedra, but polar-ising; (15) VOF2,2AmF + H20 (Baker, Trans., 2878, 392), larger,dark blue prisms ; (16) 4VOF2,7AmP + FiH,O, still darker blue,lamellar aggregates ; (17) 4VF4,2AmF + zH,O, small, blue-greenprisms, stable only in solutions, strongly acidified with hvdrogenfluoride; (18) 3VOF2,7KF ; ( 1 9 ) VOF,,SKF ; (20) 3VOF2,8NaF +2H20. These three form bright blue, sparingly soluble, crystallinepowders.(111.) Compourds derived from the Pentoaide.--(21) VOF,,ZKF,colourless, crystalline powder ; (22) 2VOF3,3KF,HF, white, lustrousprisms ; ( 2 3 ) VP5,VOB’,,4KF, colourless aggregates of very slenderneedles ; ( 2 4 ) VOZF,2KF, golden-yellow, lustrous, hexagonal prisms,(25) 2\T02F,3KF, bright yellow prisms ; (26) 5VOF3,9AmF,3HF,colourless, dull lustrous prisms ; (27) V02F,3AmF, larger, straw-coloured, probably rhombic crvstals ; (28) 4V02F,7AmF,HP, white,lustrous aggregates ; (29) 2Nb205,3KF + 5H20, lust’rous white,sparingly soluble, crystalline powder ; (30) Nb205,KF + 3H20,colourless prisms. The compounds 14, 19, and 27 seem to beidentical with those prepared by Piccini and Giorgis (Atti d. R. Acc.d e i Lincei, 1888, 590, and GIaz., 18, 186).The thermochemical relation of hydrogen fluoride to the sesqui-oxides of iron, chromium, and vanadium was determined. Thefollowing numbers were obtained for the heat of neutralisationin dilute aqueous solutions:-(Fe,0,H6,6HF + Aq) = 47500 cal.,(Cr2o6€T6,6AF + Aq) = 50330 cal., (VZ(J6H,,6HF + Aq) = 52240 cal.TheN. H. M.Decomposition of Antimony Sulphide by Boiling Water.By W. ELBERS (Chelrz. Zeit., 12, 355-356).- When antimonioussulphide is boiled with water, it is decomposed with the evolution ofhydrogen sulphide and the formation of antimonious anhydride. I nthis way 0.05 gram of the sulphide was completely converted intothe anhydride in 14 hours; the liquid then had a slightly alitalinereaction. D. A. L