INORGANIC: CHEMISTRYALTHOUGH no work of outstanding importance has appeared, thereis a, distinct improvement in the papers on Inorga,nic Chemistrywhich have been published during the past year, both as regardsthe quality of the work and the conciseness of its presentation.A tendency is apparent in some quarters towards duplication oreven triplication of publication-in journals of different types.This has several undesirable consequences: it swells the bulk ofjournal literature unnecessarily, and it results either in several ab-stracts of what is really the same work or in an abstract of the firstpaper only, which is itself usually more or less in the nature of anabstract.Atomic Weights and Separation of Isotopes.It begins to look as though hydrogen may be the only simpleelement.Carbon,l nitrogen,2 and oxygen3 all appear to be com-plex, containing very small proportions of the isotopes C13, N15, and017 and 0l8. The oxygen isotopes are only present to the extentof about 1 in lo4 and 1 in 1250 respectively, which is too small tointroduce appreciable error when oxygen is taken as the basis of theatomic-weight ~ystern.~ The divergence of the atomic weight ofoxygen from 16 is about 1-25 parts in ten th~usand.~K. P. Jakovlev 6 has reviewed the methods which have been usedfor the separation of isotopes and has himself designed an apparatusby which it is possible, by using a bundle of positive rays, to separatesmall quantities of isotopes in a pure condition.Potassium.-According to H. H. LowryY7 the atomic weight ofpotassium from plant ash is normal, and this lends no support toa remarkable result recorded by F.H. Loring and J. G. F. Druce.8Nitrogen ; Phosphorus.-The method of limiting densities applied1 A. S. King and R. T. Birge, Astrophys. J . , 1930, 72, 19; A., 1931, 15.2 $3. M. Naud6, Physical Rev., 1930, (ii), 36, 333; &4., 1232; G. Herzberg,R. Mecke and K. Wurm, 2. Physilc, 1930,61, 37; a., 615; E. Ruchardt,2. physikal. Chem., 1930, [ B ] , 9, 43; A., 1084.Naturwiss., 1930,18, 534; A., 975.4 E. Moles, Anal. Fis. Quim., 1930, 28, 127; A., 515.F. W. Aston, Nature, 1930, 126, 953.ti 2. Physik, 1930, 64, 378; A . , 1337.J . Arner. Chem. SOC., 1930, 52, 4322.8 Chem. News, 1930,140, 34INORGANIC! CHEMISTRY. 53to ammonia9 and to phosphine1O has given values of 14.009 and30.977 for the atomic weights of nitrogen and phosphorus respectively.Arsenic.-Analysis of arsenic trichloride gave the value 74.936 rt0.001 for the atomic weight of arsenic.llVanadium.-The atomic weight of vanadium was found to be50.947 from a determination of the ratio VOC1, : 3Ag.12I'antcaZum.-K.R. Krishnaswami,13 from a careful determinationof the ratios TaBr, : 5Ag : 5AgBr and TaCl, : 5Ag : 5AgC1, findsthe atomic weight of this element to be 181.36.Sulphur.-By synthesising silver sulphide from its elements,0. Honigschmid14 finds the atomic weight of sulphur to be32.0685 & 0-0006.Molybdenum-The mass spectrum of the carbonyl shows thatmolybdenum has 7 isotopes. From the mass numbers, the approxi-mate abundances, and the packing fractions, the value 95-97 &- 0.05is calculated for the atomic weight of m01ybdenurn.l~Chlorine.-According to A.F. Scott and C. R. Johnson,lG adirect determination of the solubility of silver chloride in 0-1M-nitric acid a t 0.5" shows that the value accepted by Honigschmidand Chanl' is too low, so that their determination of the atomicweight of chlorine is about 0.001 unit too high.Rhenium.-The atomic weight of rhenium (188.7) appears for thefirst time in the Report of the German Commission on atomicweights.ls Methods available for determining this value havebeen critically examined by 0. Honigschmid and R. Sachtleben,lgwho obtain the value 186.31 0.02 from the ratio AgReO, : AgBr.Intensive Drying.A paper of considerable importance in connexion with the problemof intensive drying has appeared,20 in which it is shown that waterhas an abnormally high activity when present in traces in suchliquids as benzene, in which its solubility is very low.DecreaseE. Moles and T. Batuecas, Anal. pis. Quirn., 1930, 28, 871 ; A., 1357.lo M. Ritchie, Proc. Roy. SOC., 1930, [ A ] , 128, 551 ; A., 1104.l1 J. H. Ki.epelka, J . Czech. Chem. Comm., 1930,2,256; A., 976.l2 A. F. Scott and C. R. Johnson, J . Amer. C?bem. SOC., 1930,52, 2638; A.,l3 J., 1930,1277; A., 975.l4 2. Elektrochem., 1930, 36, 689; A., 1337.l6 F. W. Aston, Nature, 1930,126, 348 ; A., 1338.lo J . Amer. Chem. Xoc., 1930, 52, 3586; A., 1337.l7 2. anorg. Chem., 1927, 163, 315; A., 1927, 806.*1084.M. Bodenstein, A. Hahn, 0. Honigschmid, and R. J. Meyer, Ber., 1930,63, [B], 1; A., 269.l9 2. anorg. Chem., 1930, 191, 309; A., 1338.2o (Miss) E. J. Greer, J . Amer. Chem. SOC., 1930,52, 4191 ; A., 1931, 3454 BASSETT :in the vapour pressure of such liquids by intensive drying can beexplained by the removal of the abnormally high partial pressure ofthe water, and there is no need to assume any catalytic effect of thelatter on an inner equilibrium.Superconductors.Niobium 21 and ruthenium 22 have been shown to become snper-conducting between 8-74" and 8.18" Abs. jand at 2-04" Abs.,respectively. Titanium has almost become a superconductor at1.16" Abs., and it is considered that many if not all metals arelikely to show superconductivity if the temperature is low enough.23The conductivities of many metals and alloys have been examineddown to temperatures as low as 1-43' Abs., and several supercon-ducting alloys were foundY24 of which Rose's alloy showed aresistance-temperature hysteresis.25 Titanium nitride (1.2" Abs.), vanadiumnitride (1.2"), and the carbides of molybdenum (7"), niobium (lo"),and tantalum (9") become superconducting at the temperaturesshown.26 Niobium carbide shows this phenomenon at a highertemperature than is known for any other substance.X-Ray8 and Chemical Problems.It is more and more becoming standard practice to supplementmetallographical and other investigations of a chemical natureby an X-ray examination of the substances which are being studied.Zirconium dioxide 27 has been shown in this way to occur in threedifferent varieties. According to W.Morris-Jones andE. G. Bowen,2* the compound SnSb, which forms good cubiccrystals, has a sodium chloride lattice, and so is ionic in structureand probably contains tervalent tin.Co-ordination.Equations have been developed by F. J. Garrick 29 which enablehim to calculate the maximum co-ordination numbers of uni- and21 W. Meissner and H . Franz, 2. Physik, 1930,63, 668; A., 1102.22 J. C. McLennan, Nature, 1930, 125, 168; A., 281; J. C. McLennan,J. F. Allen, and J. 0. Wilhelm, Trans. Roy. SOC. Canadu, 1929, (iii), 23, 111,383 ; A., 632.23 W. Meissner, 2. Physik, 19$0,60, 181; A , , 631.24 J. C. McLennan, L.E. Howlett, and J. 0. Wilhelm, Trans. Roy. SOC.Cuncbda, 1929, (iii), 23,111, 287; A , , 631 ; W. J. de Haas, E. van Aubel, andJ. Voogd, Proc. K. Akad. Wetensch. Amsterdam, 1930, 33, 268; A., 676.25 J. C. McLennan, Nature, 1930,125, 447; B., 610.26 W. Meissner and H. Franz, Ncrturwis~., 1930, 18, 418; A., 846; 2.27 W. M. Cohn and S. Tolksdorf, 2. physikal. Ghem., 1930, [ B ] , 8, 331 ; A .,t 8 Nature, 1930,126, 846; A., 1931, 33.29 PhiE. Mag., 1930, [vii], 9, 131; 10, 76, 77; A . , 276, 1096.Phyeik, 1930, 65, 30; A., 1507.1099INORGANIC CHEMISTRY. 55bi-valent kations. The assumption is made that the most stablecomplexes are those in which the electrostatic energy is a maximumand the values so calculated are on the whole in good agreementwith Sidgwick's rule.Corrosion and Passivity of Metals.Much work on the anodic passification of metals has been publishedduring the past year.30 The transparent film responsible for thepassivity of iron made anodic in dilute sulphuric acid has beenisoIated.31 Potential-time curves have been constructed for anumber of iron alloys, as well as for iron and aluminium, in order tostudy the effect of various treatments of thg metal on its passivity?2The capacity for different anions to penetrate the protective filmhas been examinedF3 whilst the influence of acids in passivity andcorrosion and the reproducibility of results in corrosion work havebeen c0nsidered.~4 The theoretical aspect of corrosion has also beendealt with by F.Todt.35 A new explanation of the passivity ofiron based on its behaviour as a higher oxide electrode has beenput f o r ~ a r d .3 ~ ~Group 0.The m. p.'s of krypton and xenon are -157.0" 0.5" and - 112-0"&04" respectively. Solid krypton appears to have a transitionpoint at about -185".36 The m. p.'s of hydrogen, neon, andnitrogen have been determined for pressures up to 5000 kg. persq. cm., and those of argon up to 3400 kg. per sq. Thesolubilities of helium, neon, and argon for the range 15-37" havebeen determined in water and several organic solvents.38Group 1.The inner equilibrium of the a- and the p-form of hydrogen hasbeen considered by A. S m i t ~ . ~ ~ The conversion of active hydrogen30 W. J. Miiller, L. Holleck, I(. Konopicky, and W. Machu, Monats?~, 1929,52, 409, 426, 442, 463, 474; A., 298.31 U.R. Evans, Nature, 1930,126,130; A., 1126.32 L. C. Bannister and U. R. Evans, J., 1930,1361 ; A., 999.33 S . C. Britton and U. R. Evans, ibid., p. 1773; A., 1268.a4 U. R. Evans, ibid., p. 478; B., 462; Amer. Electrochem. SOC., May,36 2. physikal. Chem., 1930, 148, 434; A., 1126.36a J. F. Chittum, J. Physical Chem., 1930,34,2267; A., 1627.36 K. Peters and K. Weil, 2. physikal. Chem., 1930, 148, 27; A., 986;F. J. Allen and R. B. Moore, J. Arner. Chem. SOC., 1930, 52, 4173; A., 1608.37 F. Simon, M. Ruhemann, and W. A. M. Edwards, 2. physikal. Chem.,1930, [ B ] , 8, 331; 7, 80; A., 403,633.38 A. Lannung, J. Amer. Chem. SOC., 1930,52, 68; A., 406.8e Proc. K . Akad. Wetensch. Amsterdam, 1929, 32, 1118; A ., 293; Physikal.1930, Advance Copy; B., 463.Z . , 1930,31,172,178; A,, 39356 BASSETT :into molecular hydrogen is greatly delayed if the walls of thedischarge tube are washed with phosphoric acid. Metallic leadyields it volatile hydride by the action of active hydrogen.*O Ipatievhas continued his investigations of the displacement of metals fromsolutions by hydrogen under high pressure, by investigating thecase of arsenic.41 The behaviour of aqueous solutions of a numberof nitrates towards hydrogen under pressure has also beenas well as the displacement of lead from its organo-metallic COM-pounds .BSmall quantities of any of the alkali metals can be obtained byheating such salts as the chromate or dichromate with excess ofzirconium in a vacuum:44The vapour density of sodium shows that some Na, molecules arepresent.45 Metallic sodium and silver iodide or chloride in liquidammonia solution react sharply in accordance with the equationNa + AgX = NaX + Ag.46 Pure sodium hydride has beenprepared 47 as fine white needles by the interaction of hydrogen andsodium vapour a t 400-450".Its heat of formation has beendetermined.The melting-point curve of NaC1,2H2Q has been followed up topressures of 12,000 bars (c. g. s. atmospheres). It passes through amaximum at 25.8" and 9500 bars. The melting point is + 0.1" at1 bar pressure.48Anhydrous sodium sulphate appears to exist in five differentand the existence of three forms of potassium nitrate hasbeen e~tablished.~OThe reaction between sodium hydroxide and metallic oxidesxRQ, + 2NaOH --+ Na,R,O(,,+ + H,O has been followed bydetermining the water formed and also, by means of suitable40 H.von Wartenberg, G . Schultze, and E. Muller, 2. physikal. Clhem., 1930,[B], 6, 261 ; A., 302.41 V. Ipatiev, G. Razubaiev, and V. Malinovski, Ber., 1930, 63, [ B ] , 166,2812; A., 1930, 306; 1931, 52.42 V. Ipatiev and B. Muromtzev, ibid., p. 160; A., 306.43 V. N. Ipatiev, G. A. Razubaiev, and I . I?. Bogdanov, J. Buss. Phys.44 J. H. de Boer, J. Broos, and H. Emmens, 2. anorg. Chem., 1930, 191,46 W. H. Rodebush and E. G. Walters, J. Amer. Ckem. SOC., 1930,52,2654;40 W. M. Burgess and E. H. Smoker, ibid., p. 3573; A., 1386.47 H. Hagen and A. Sieverts, 2. anorg.Chem., 1930,185, 239; A , , 307.4 8 L. H. Adams and R. E. Gibson, J. Amer. Chem. SOC., 1930,52,4252 ; A .49 F. C. Kracek and R. E. Gibson, J. Physical Chem., 1930, 34, 188; A . ,li0 F. C. Kracek, ibid., p. 225; A . , 402.Chem. SOC., 1929,61, 1791; A., 428; Ber., 1930,63, [ B ] , 335; A., 463.113; A . , 1136.R . , 1104.1931, 40.281; F. C. Kracek and C. J. Ksanda, ibid., p. 1741; A., 1099INORGANIC CHEMISTRY. 57dissolution, the quantity of metallic oxide which has entered into thechange. By using excess of alkali hydroxide and of metallic oxidein different experiments, the compounds richest and poorest inalkali can be established with a large measure of certainty. Anumber of compounds derived from the oxides of Si, Ti, Zr, Ce, Al, Fe,and Cr have been characterised in this way.51A careful revision of most of the older work on the polysulphidesof sodium has been carried out by T.G . Pearson and P. L. Robinson.52The mono-, di-, tri-, tetra-, and penta-sulphides all exist both in theanhydrous condition and hydrated.The compounds K2PbCu(N02) 6, K,PbNi(NO,) 6, and K2PbCo(N02) 6are obtained by precipitation with potassium nitrite of mixed solu-tions of lead and copper (or nickel) acetates or of lead and cobaltnitrate.% X-Ray examination shows that they aU have a cubiclattice very similar to that of K,CO(N~,)~,~H,O, from which it isconcluded that the 3 molecules of water in the latter compoundare zeolitic in character and entangled in the crystal lattice. It isconsidered that the above lead compounds contain ions of the type[M(N02)6]””, where M is Cu, Co, or Ni.Several complex saltsderived from potassium manganese (cobalt or zinc) double oxalatesby replacement of C20, groups by (NO,),, (CNS),, or S203 have beendescribed. 54From an examination of the system iodine-potassium iodide,it is concluded that neither the tri-iodide nor any other polyiodideof potassium can exist as stable solid above 25”.s5 In the case ofcesium, the tetraiodide and the tri-iodide can separate either frommelts or from aqueous solutions, but the pentaiodide does notexist .56German carnallite contains, on the average, 0.02% of rubidiumchloride and 0~0002~0 of cesium chloride, and full details havebeen published 57 of a comparatively rapid and simple method bywhich practically the whole of this can be recovered in a high state ofpurity.The whole of the rubidium and cesium with some potassiumis precipitated as silicomolybdate from an acid solution of the once5 1 J. D’Ans and J. Loffler, Ber., 1930, 03, [B], 1446; A., 1005.G2 J . , 1930, 1473; A., 1136.53 A. Ferrari and C. Colla, Atli R. Accad. Lincei, 1930, [vi], 11, 755; A.,54 R. Scholder and C. F. Linstrom, Ber., 1930,83, [B], 2828 ; A., 1931, 66.b 5 T. R. Briggsand W. F. Geigle, J. Physical Chem., 1930,34,2250; A., 1521.56 T. R. Briggs, J. A. Greenwald, and J. N. Leonard, ibid., p. 1951; A.,1374; T. R. Briggs, ibid., p. 2260; A., 1522.G7 G. Jander and H. Faber, 2. anorg. Chem., 1929,179,321 ; B., 1929,641 ;G. Jander and F.Busch, ibid., 1030,187, 165; 104, 38; A., 1930, 435; 1931,49.138858 BASSETT :recrystallised carnallite. The molybdenum is removed by volatilisa-tion as oxychloride in a current of hydrogen chloride. If in thefirst instance only enough silicomolybdic acid is added to precipitate10% of the total rubidium and caesium, the precipitate contains allthe caesium and practically no potassium; the remaining rubidiumis thrown down by a second addition of silicomolybdic acid. Bycarrying out the silicomolybdate precipitation thus in two stages,the separation of pure caesium and rubidium preparations is greatlyfacilitated.The pentaborates of potassium, rubidium, and casium,5B203 ,l&0,8H,O, form isomorphous (orthorhombic) crystals. 58With the exception of the lithium compound, nitrides of the alkalimetals are difficult to prepare, and in no case had it been demon-strated that they are of the type M,N.Under the influence of theglow discharge, the alkali metals and their amalgams take upnitrogen. When this occurs at room temperature the compoundformed is practically entirely a ~ i d e , ~ ~ but at higher temperaturesand with excess of alkali metal, nitride formation is favoured.60 Asmall amount of nitride is formed during the thermal decompositionof alkali azides, and it has now been shown that rubidium and caesiumnitrides formed in this way have the formule Rb,N and CS,N.~~H. J. S. King has prepared a large number of ammines of cupricsalts of monobasic acids, including some of cupric iodide.61a Theammines and ammine hydrates of cupric selenate 62 and selenite 63have been prepared and examined, and a large number of alkalicupric carbonates are stated to exist.64Some interesting studies of the dehydration of single crystals ofcopper sulphate pentahydrate have been made by W.E. Garner andM. G. Tanner.65The solubilities of silver chloride, bromide, and iodide in methyland ethyl alcohols have been determined by an electrochemicalmethod,66 and it is suggested that the solubility of silver iodide inacetone solutions of sodium iodide is due to the formation of ananion [I(IAg),]'. Several sodium argentothiosulphates and theacid H(AgS,O,),H,O have been prepared.67s8 A. P. Rollet and L. And&, Compt. rend., 1930,191, 567; A., 1386.59 W.Moldenhauer and H. Mottig, Ber., 1929,62, [ B ] , 1954; A . , 1029, 1247.oo H. Wattenberg, ibid., 1930,63, [B], 1667; A., 1137.61 K. Clusius, 2. anorg. Chem., 1930, 194, 47; A., 1931, 50.61@ J., 1930, 2307; A., 1536.62 L. C. Hurd and V. Lenher, J . Amer. Chem. SOC., 1930,52,3857 ; A., 1536.63 L. C. Hurd, G. I. Kemmerer, and V. W. Meloche, ibid., p. 3881 ; A., 1536.64 A. Cocosinschi, Bull. A c d . Sci. Roumaine, 1929,12,19; A., 307.135 J., 1930, 47; A., 428.6 6 F. K. V. Koch,ibid., pp. 1561,2386; A., 1107, 1511.6'1 H. Bahea,&bicE., 1929,2763; A., 176INORGANIC CHEMISTRY. 59Cryoscopic measurements of the molecular weight of gold dis-solved in various metals show that it is unimolecular between400" and 1550".68A number of triple bromides of rubidium, tervalent gold, andcopper, cadmium, mercury, thallium, bismuth, or antimony havebeen prepared and their properties described .69Aurous chloride carbonyl is formed quantitatively from aurouschloride and carbon monoxide in benzene a t 15" or from auricchloride in tetrachloroethylene at 130-140".It has M , 223 (calc.,260) in freezing benzene, and dissociates in a vacuum or in hotsolvents to give pure aurous chloride. It reacts with nitrogenousbases, the carbonyl group being displaced by 1 mol. of ba~e.~OGroup I I .A question, which has nowadays lost the interest it once had,has been revived by P. Pfeiffer, T. Fleitmann, and R. Hansen 71 ina discussion as to whether beryllium and magnesium are betterclassed with zinc and cadmium or with calcium, strontium, andbarium.The question is considered with reference to the degreeof hydration and ammoniation of the salts of various aromaticsulphonic acids, and it is concluded that beryllium and magnesiumare better classed with zinc and cadmium. A number of such salts ofnickel, copper, zinc, and cadmium were also made. The berylliump-toluenesulphonate and p-naphthalenesulphonate have six mole-cules of water of crystallisation, although the a-naphthalenesul-phonate only has four and the ammines never have more than 4mols. of ammonia. The first two salts are considered to be the firstcertain cases of salts containing 6-co-ordinated beryllium. It isplain that alternative explanations are possible, however.Pure beryllium can be deposited electrolytically from solutions ofits anhydrous salts in liquid ammonia.72The molecular weight of magnesium dissolved in other metalscorresponds to a monatomic molecule above 700".73 Anhydrousmagnesium perchlorate 74 and barium oxide 75 have been recom-68 E. S . Burkser, S. G. Rublov, and A. M. Scharnovsky, 2. anorg. Chem.,7 O M. S. Kharasch and H. S. Isbell, J . Amer. Chem. SOC., 1930, 52, 2919;71 J . p r . Chem., 1930, 128, 47; A., 1536; P. Pfeifk, T. Fleitmann, andH. S. Booth and G. G. Torrey, J . Amer. Chem. Soc., 1930, 52, 2581; A.,A. Jouniaux, Bull. SOC. chim., 1930, [iv], 47, 682; A., 1243.1029,185, 144; A., 176.A., 1277.T. Inoue, 2. anorg. Chem., 1930,192,346; A., 1390.1004.78 A. Jouniaux, Bull.SOC. china., 1930, [iv], 47, 686; A., 1243.74 S. Lenher and G. B. Taylor, I d . Eng. Chem. (Anal.), 1930,2,58; A., 568.7 5 H. 8. Booth and L. H. McIntyre, ibid., p. 12 ; A., 66860 BASSETT :mended as drying agents, It is concluded from spectroscopicobservations that in a magnesium arc burning in wafer vapour thereis not merely displacement of hydrogen by the magnesium, but alsoa second reaction resulting in the simultaneous formation of mag-nesium oxide and hydride.76 In continuation of his studies of oxidehydrates, Huttig has published papers dealing with the oxides ofberyllium, 77 magnesium,78 calcium,7g strontiurn,sO and cadmium.81A number of points connected with the technique of such investiga-tions, such as the measurement of water-vapour pressure of hydrox-ide gels, have been discussed.82 It has been shown that when due at-tention is paid to the preparation of pure products, the hydratedperoxides of calcium, strontium, and barium all correspond to the for-mula M0,,8H,0.83 Several papers have been published on magnesiumcarbonate^,^^ and it is said that a very unstable monohydrate ofcalcium carbonate exists besides the much more stable hexah~drate.~SThe calcium aluminates have been investigated by several workers.86The action of nitrogen peroxide on calcium carbonate, lime, andcalcium phosphate has been investigated, and that of sulphurdioxide on calcium carbonate and phosphate.The use of calciumcarbonate in the recovery of nitrous gases is suggested.*' Thesolubilities of several radium salts have been determined.88The supposed allotropic changes undergone by zinc and bismuthare really due to impurities, but thallium and cobalt undergoreversible changes respectively at 225.2" and at 444" and 1128°.897 6 G.Piccardi, CTazzetta, 1930, 60, 337; A., 1006.7 7 G. F. Hiittig and K. Toischer, 2. anorg. Chem., 1930, 190, 364; A . , 996.7 8 G. F. Huttig and W. Frankenstein, ibid., 185, 413; A . , 293.7 9 G. F. Hiittig, A. Arbes, Z. Herrmann, and C. Slonim, ibid., 191, 161 ; A.,1372.G. F. Huttig and A. Arbes, ibid., 192, 226; A., 1373.81 G. F. Huttig end R. Mytyzek, ibid., 190,353 ; A., 996.G. F. Huttig and K. Toischer, KoEEoidchem. Beih., 1930,31, 347; A . , 1373.83 C . Nogareda, Anal. Fig. Quim., 1930,28,461; A ., 1006.84 H. Menzel, A. Bruckner, and H. Schulz, 2. Elektrochern., 1930, 36, 188;A . , 718; H. Menzel and A. Bruckner, ibid., p. 63 ; A . , 436; G. F. Hiittig andW. Frankenstein, 8. anorg. Chem., 1930,185, 413; A . , 293.8 5 F. Krauss and W. Schriever, 2. anorg Chem., 1930, 188, 259; A . ,718.86 S. Nagai and R. Naito, J. SOC. Chem. Ind. Japan, 1930,33, 17 ; A., 436 ;T. Thorvaldson and N. S. Grace, Canad. J . Ree., 1929, 1, 36; A., 436;G. Assarson, 2. anorg. Chem., 1930, 191, 333; A., 1262; A. Travers andJ. Sehnoutka, Ann. Chim., 1930, [XI, 13,265; A., 872.87 E. Briner, J. P. Lugrin, and R. Monnier, Helv. China. Acta, 1930, 13, 64,76, 80 ; A., 436.8 8 0. Erbacher, Ber., 1930,63, [B], 141 ; A., 406.8 9 A. Schulze, 2. Metallk., 1930, 22, 194, 308; B., 1073; 2.tech. Physik,1930,11, 16; A., 1355INORGANIC CHEMISTRY. 61Zinc hydroxide exists in five different crystalline formsg0 and anumber of well-defined basic salts are formed by prolonged actionof the hydroxide or oxide on solutions of zinc salts.g' The complexnature of the curious fractional hydrates of zinc chloride is indicatedby the solid solutions containing cobalt chloride which they form?2The degree of association of cadmium iodide and of mercuric chlorideand bromide in acetone solution has been determined, as also thesolubilities, which are lower than those reported by previousworkers .93The solubilities of cadmium in its molten halides, of mercury inmercuric iodide, and of zinc and magnesium in their respectivechlorides have been determined.The solution of cadmium in moltencadmium chloride is due to formation of a subchloride which is onlystable whilst the mixture is liquid.94The conditions under which tetramminomercuric salts can beformed have been discussed, and a number of these salts, as well assome diammino-salts, have been prepared.95 The action of am-monia on the compounds HgC4,2NH3 and HgBr2,2NH3 has beenstudied, and the compounds Hg2NBr and Hg$C1,H20 prepared.96Unlike most bi- and ter-valent metals, mercury and bismuth do notform inner complex phenoxides with 8-hydroxyquinoline ; variouscompounds are formed, however, and a number have been prepared,such as those formulated as [HgC4(CgH,0N)]C1 andBiC13( CgH,ON,HC1),,EtOH .97Group I I I .F.Faltis 98 has put forward views with regard to the structure ofthe boron hydrides involving cyclic structures for the higher members.E. Wiberg 99 considers that boron is quinquevalent towards hydrogenand ip so in B,H,, the two boron atoms being doubly bound.Aluminium and cerium borides on treatment with acids give smallyields of the same boron hydrides as are furnished by magnesiumb0ride.l Beryllium boride has the advantage over magnesiumW. Feitknecht, Helv. Chim. A&, 1930,13,314; A., 700.O L Idem, ibid., p. 22; A., 436.92 H. Bassett and H. H. Croucher, J., 1930, 784; A,, 1251.Q8 C. Zapata y Zapata, Anal. Pis. Quim., 1930,28, 603; A., 1362.94 G. von Hevesy and E. Lowenstein, 2. anorg. Chem., 1930,187, 266; A.,95 E.Weitz, K. Blasberg, and E. Wernicke, ibid., 188,344; A., 719.s6 M. Franqois, Compt. rend., 1930, 190, 125, 744, 1607; Bull. Soc. chim.,97 L. Dede and W. Hessler, 2. anovg. Chem., 1930,188, 325; A , , 719.98 Ibid., 187, 369; A., 624.99 Ibid., p. 362 ; A., 624.437.1930, [iv], 47, 166,569, 826; A., 307,667,1006, 1138, 1262.B. D. Steele and J. E. Mills, J . , 1930, 74; A . , 43782 BASSETT :boride for the preparation of boron hydrides because it furnishesa gas free from silanes which are troublesome to remove.2 B4H1,has now been prepared in quantity, and its reactions with hydrogenchloride, sodium amalgam, and ammonia studied in detail.3Phenylborine, BH2Ph, and boronbenzene, BPh : BPh, aredescribed by E. Pace.4 The distillation of boric acid in steamhas been studied by G.Banchi and M. Giann~tti.~ Structuresfor the various boric acids and borates have been put forwardwhich fall into line with those now customary for poly- and hetero-poly-acids, with a central boron atom to which boric acid residuesare co-ordinated.6 They seem preferable to the long-chain formuhproposed by E. Wiberg.' By electrolysis of fused borates and borate-fluoride mixtures, amorphous boron has been obtained as well asborides of many metals of Groups 111, IV, V, VI, and VII.8Fluoroborates other than those corresponding with the formulaMBF, are said to exist.gThe changes undergone by hydrated alumina during dehydrationand heating have been followed by X-ray examination.10A number of spinels, M11M211104 (MI1 = Cu,Mg,Zn,Mn ;MI11 = Al,Fe,Cr), have been prepared by precipitation of themixed oxides or evaporation of mixed nitrates and calcination atabout 800" in each case.ll Anhydrous aluminium alums of thegeneral formula MAl( SO,), are precipitated by addition of hotconcentrated sulphuric acid to the hot concentrated mixed sulphatesolutions.l2Gallium tribromide, tri-iodide,13 and trisulphidel* have beenA. Stock, E. Wiberg, and H. Martini, 2. anorg. Chem., 1930, 188, 32;Idem, Ber., 1930, [B], 63, 2927; A., 1931, 50.A., 720.4 Atti R. A d . Lincei, 1929, [vi], 10, 193; A., 354.6 Ann. Chim. Appl., 1930,20,271,286,296; A., 1361.F. L. Hahn, 2. anorg. Chem., 1930,193, 316; A., 1502.Ibid., 191, 43; A., 1096.8 L. Andrieux, Ann. Chim., 1929, [XI, 12, 423; A., 305.9 A.Travers and L. Malaprade, Bull. SOC. chim., 1930, [iv], 47, 788; A . ,1261.10 W. Biltz, A. Lemke, and K. Meisel, 2. unorg. Chem., 1930,186, 373; A.,399; N. Parravano and E. Onorato, Atti R. Accad. Lincei, 1929, [vi], 10,475; A., 437; G. F. Huttig and 0. Kostelita, 2. unorg. Chem., 1930, 187, 1 ;A., 543.11 L. Passerini, Gaxzetta, 1930, 60, 389; A., 1007.12 N. Schischkin, 2. anorg. Chem., 1930,189, 289; A., 720.13 W. C. Johnson and J. B. Parsons, J . Physical Chem., 1930,34,1210 ; A .,874.14 A. Brukl and G. Ortner, Natumoies., 1930, 18, 393; A., 720; Monatah.,1930, 56, 368; A,, 1537; W. C. Johnson and B. Warren, NUtUWi88., 1930, 18,666; A., 1138INORGANIC CHEMISTRY. 63prepared directly from the elements. By reduction of Ga,S, withhydrogen Gas is obtained, and on being heated in a high vacuum,this breaks up into Ga,S and Ga,S,.Thallic oxide does not appear to form any definite hydrate.15A number of alkali ceric oxalates have been described.16Europium may be separated from samarium and gadolinium asEuSO,, which is insoluble in dilute acid, by electrolytic reductionin presence of su1phate.l' Ytterbium can be similarly separated,practically quantitatively, in one operation as YbSO,,xH,O of 98%purity, from the pink yttria-group oxides containing yttrium anderbium with small amounts of thulium and ytterbium.The Yb"ion is green.l*Samarium di-iodide is best prepared by thermal dissociation ofthe tri-iodide in a high vacuum. On strong heating in a vacuum,SmC1, undergoes the type of decomposition characteristic of lower-valency compounds to give metal and SmCl,.l9The sulphides of a large number of rare-earth metals have beenprepared by heating the chloride or sulphate in a current of hydrogensulphide. They fall into two groups with different crystal lattices anddifferent colours.20 Praseodymium forms two different doublesulphates with ammonium sulphate.21 The solubilities of severalrare-earth salts have been determined.22Group I V .Measurements of parachors and dipole moments have furnished.important evidence for the structure of the compounds of bivalentcarbon, which are shown to be best formulated thus : Carbonmonoxide, CEO ; the isocyanides, R-N"C.23Purified wood charcoal reacts spontaneously with fluorine a tthe ordinary temperature, a variety of carbon fluorides beingl6 G.F. Huttig and R. Mytyzek, 2. anorg. Chem., 1930,192, 187; A., 1373.1% J. 8ttkba-Bohrn and A. Pisafilsek, J . Czech. Chem. Comm., 1930,2, 244;1' L. F. Yntema, J . Amer. Chem. SOC., 1930, S2,2782; A., 1134.1* R. W. Ball and L. F. Yntema, ibid., p. 4264; A., 1931, 51.l@ G. Jantsch, Nuturwiss., 1930,18,166 ; A,, 437 ; G. Jantsch and N. Skalla,2. anorg. Chenz., 1930, 193, 391 ; ri., 1931, 51.20 W. Klemm, K. Meisel, and H. U. von Vogel, 2. anorg. Chem., 1930,190,123 ; A., 874.z1 F. Zambonini and S. Restaino, Atti R. Accad. Gncei, 1930, [vi], 11, 774;A., 1387.82 K. S. Jackson and G. Rieniicker, J., 1930, 1687; A., 1107; J. A. N.Friend, ibicE., pp. 1633, 1903; A., 1107, 1246.23 D.L. Hammick, R. C. A. New, N. V. Sidgwick, and L. E. Sutton, ibid., p.1876; A,, 1239; H. Lindemann and L. Wiegrebe, Ber., 1930, 63, [B], 1660;A., 1171.A., 100704 BASSETT :formed. The chemical and physical properties of the tetrafluoridehave been examined.24The reaction COX + 2NH3 = CO(NH,), + H2S affords a moresuitable method for the manufacture of carbamide than the olderprocess using ammonia and carbon dioxide.25Carbonyl chloride is produced when carbon monoxide is passedover the heated chlorides of ruthenium, platinum, and gold, but notof rhodium, palladium, or osmium.26The hydrolysis of the cyanides of sulphur, selenium, tellurium,and phosphorus has been their molecular volumesmeasured,28 and the mobility of the OCN, SCN, SeCN, N(CN),,C(CN),, and N3 ions determined.29Vapour-pressure curves are taken to indicate the existence of fivedefinite silica hydrates.30 Very slow potentiometric titration of silicatesolutions has been tried as a means of studying the silicic acids,but without very definite results.31The attack of silica by hydrofluoric acid is not primarily dependentupon the concentration of the latter but upon that of the HF,' ion,and is directly proportional to it when the total ionic concentrationis high.31~Anhydrous titanium di- and tri-bromides have been prepared forthe first the latter by reduction of the tetrabromide at a redheat with hydrogen.On being heated at 400" in an atmosphere ofhydrogen, the tribromide breaks up in accordance with the equation2TiBr3 -+ TiBr, + TiBr,; the dibromide itself undergoes thereaction STiRr, --+ Ti + TiBr,, but only slowly a t 650".Boththe lower bromides react with hydrogen bromide to form thetetrabromide, and the reaction is rapid above 350". Titaniummetal reacts with hydrogen bromide above 300", and the lower thetemperature the more di- and tri-bromide are formed, which is similarto what was found for the reaction of hydrogen bromide with silicon.3324 0. Ruff and R. Keim, 2. anorg. Chem., 1930,192,249; A., 1387 ; P. Lebeauand A. Damiens, Compt. rend., 1930, 191, 939; A., 1931, 52.25 A. Klemenc, 2. anorg. Chem., 1930,191,246; A., 1387.26 W. Manchot and G. Lehmann, Ber., 1930,63, [B], 1221 ; A., 875.27 L. Birckenbach, K.Huttner, W. Stein, and I?. Ensslin, 2. anorg. Chem.,1930,190,l; A., 876.K. Huttner and S. Knappe, ibid., p. 27; A., 876.2s L. Birckenbach and K. Huttner, ibid., p. 38 ; A., 876.P. A. Thiessenand O.Koerner, 2.anorg. Chem., 1930,189,168,174 ; A., 720.31 W. D. Treadwell and W. Wieland, Helv. Chim. Actu, 1930, 13, 842; A . ,31a W. G. Palmer, J., 1930, 1666; A., 1133.32 R. C. Young and W. C. Schumb, J. Amer. Chem. SOC., 1930,52,4233; A , ,33 Idem, {bid., p. 1464; A., 720.1637.1931, 51INORGANIC CHEMISTRY. 65The existence of various zirconates has been demonstrated bymeans of fusion diagrams.34Pure zirconium and hafnium metals have been prepared bythermal decomposition of the iodides.35 The melting point anddensity of metallic hafnium are about 2500" Abs.and 13.31respectively .The precautions necessary to ensure the absence of impuritieswhen preparing pure hafnium salts have been described.36 Thesolubilities of the oxyfluorides and oxybromides of zirconium andhafnium in hydrofluoric and hydrobromic acid solutions have beendetermined.37The lowest hydrate of thorium nitrate is Th(N03)4,2H,0 butthoryl nitrate, ThO(NO,),,&H,O, can be obtained by desiccationof thorium nitrate in a current of air, carrying nitric acid vapour,above l l O O . 3 8Germanium monohydride, a dark brown powder, is formed by theaction of cold water on sodium germa~Gde.~~ Amorphous andcrystalline germanium monoxide and monosulphide have beendescribedtO as also several sulpho- and per-germanatestl andseveral phenyl germanium compounds.42 Germanium imide,germanam (Geg3H), and germanium nitride are formed whenammonia acts upon germanium tetrachloride.& R.Schwarz andH. Giese show that germanium tetrachloride forms no compoundwith hydrogen chloride corresponding to H,GeF,. In this respectgermanium is like silicon and unlike tin. They have also prepared12-molybdogermanic acid, H,[Ge(Mo,O,),], and the correspondingtungsten compound and their guanidinium salts.44 Several saltsof the 12-tungstogermanic acid have been described.44"84 H. von Wartenberg and H. Werth, 2. anorg. Chem., 1930, 190, 178 ; A.,85 J. H. de Boer and J. D. Fast, 2. anorg. Chem., 1930,187, 177, 193; A.,36 J. H. de Boer and J. Broos, ibid., p. 190; A., 438.37 G. von Hevesy and 0.H. Wagner, ibid., 191, 194; A., 1362.38 E. Chauvenet and Mme. Souteyrand-Franck, Bull. SOC. chim., 1930, [iv],39 L. M. Dennis and N. A. Skow, J . Amer. Chem. SOC., 1930, 52, 2369; A.,40 L. M. Dennis and R. E. Hdse, ibid., p. 3653; A., 1388; W. Pugh, J.,41 R. Schwarz and H. Giese, Ber., 1930,63, [BJ, 778 ; A., 720.42 C. A. Kraus and C. B. Wooster, J . Amer. Chem. Soc., 1930, 52, 372; A.,48 R. Schwarz and P. W. Schenk, Ber., 1930,63, [B], 296; A., 437.44 Ibid., p. 2428 ; A., 1637.44a A. Brukl, Monatsh., 1930,56, 179; A., 1638.847.437.47,1128; A., 1638.1007.1930,2369; A., 1637.364; C. A. Kraus and C. L. Brown, ibid., p. 4031; A., 1602.REP.-VOL. XXVII. 66 BASSETT :It is doubtful whether octammines of tin have been prepared.45Products supposed to be such were found to correspond to theformula [Sn,xNH3,yH,0]14, where x + y was approximately equalto 8.Lead perchlorate and its mono- and tri-hydrates have beenmade.The anhydrous salt is extremely soluble in water and isalso soluble in organic solvents.45a Crystalline and hydratedlead dioxides have been prepared, and the dehydration curves of thelatter examined.46 A dihydrate of lead oxalate is precipitated at0" and it is shown that lead oxalate (and manganous oxalate) areprobably complex.47Group V.Attempts to separate nitrogen into para- and ortho-forms similarto those of hydrogen have not been successfu1,48 although Smitsconsiders that he has evidence which indicates the complexity ofnitr~gen.~gFurther work has been published on the constituents of activenitrogen 5O and on the decay of its aftergl~w.~l The amount ofactive nitrogen present can be determined by shaking the gas withmercury at room temperature and estimating the ammonia formedby treatment of the product with 2.5% sodium hydroxide.Themost suitable phosphor for use with active nitrogen is boron nitrideactivated with carb0n.5~Some hydrazine is formed when a mixture of ammonia and nitrogenis passed over nickel gauze a t 340-355' or during the catalyticoxidation of ammonia by fine copper gauze at 340400' at lowpressures, the ammonia being in excess. It can also be obtainedby burning oxygen in ammonia.53 Reduction of nitric oxide byplatinised platinum in dilute hydrochloric acid produces smallamounts of hydroxylamine and ammonia.54 Nitrosyl perchlorate46 A. J. Cooper and W. Wardlaw, J., 1930, 1141 ; A., 874.OSa H. H. Willard and J. L. Kassner, J . Amer. Chem. Soc., 1930, 52, 2391 ;4 6 A. Simon, Z . anorg. Chem., 1930,185, 280, 300 ; A., 289, 308.4 7 R. Scholder and C . F. Linstrom, Ber., 1930,63, [B], 2831 ; A., 1931, 66.48 E. Justi, Naturwiss., 1930, 18, 227, 393; A . , 524, 721 ; P. Harteck andH. W. Schmidt, ibid., p. 282 ; A., 557.49 A. Smits and J. de Gruyter, Proc. K . Akad. Wetensch. Amsterdam, 1930,33, 86; Physikal. Z . , 1930, 31, 435; A . , 659; A. Smits, H. Gerding, and (Miss)W. Hertogh, Proc. K . Akad. Wetensch. Amsterdam, 1930,33,626 ; Physikal. z.,1930, 31, 768; A., 1096.Z. Bay and W. Steiner, Z .physikal. Chem., 1930, [B], 9, 93; A., 1087.A., 1007.s1 E. J. B. Willey, J . , 1930, 336, 1146; A., 624, 838.s2 E. Tiede and H. Chomse, Ber., 1930,63, [B], 1839; A., 1139.63 K. A. Hofmann and J. Korpiun, Ber., 1929,62, [B], 3000; A., 171.54 A. J. Butterworth and J. R. Partington, Tram. Farachy SOC., 1930, 26,144; A . 429INORGANIC CHEMISTRY. 67and nitrosylsulphuric acid are considered to be salts,s5 [NO]’[ClO,]’and [NO]’[HO*SO,]’. The additive compounds of phosphine and thetetrahalides of the elements of Group IV have been examined.56An investigation of the oxidation of phosphorus by oxygen andby air, both alone and in presence of moisture and of substancesinhibiting phosphorescence, has led to the conclusion that theoxidation has its seat in the gas phase and is autocatalysed byatomic oxygen.57The vapour pressures of phosphoric oxide under various conditionsof heating have been determined, and the results interpreted interms of the author’s theory of allotropy.58 Diammoniumamidopyrophosphate is formed by the action of gaseous ammoniaon phosphoric oxide.59The small amount of hexafluorophosphoric acid produced by theaction of phosphoric oxide on aqueous hydrofluoric acid can beisolated as the nitron salt.A large number of salts of the acid havebeen prepared and described. The nitron salts of hexafluoroar-senate and hexafluoroantimonate have been prepared by evaporationof potassium dihydrogen arsenate or potassium pyroantimonatewith hydrofluoric acid, followed by addition of ammonium andnitron acetates.60The variations in the colour of arsenious sulphide are purelyphysical in nature.61 L.W. McCay and W. Foster e2 showed thata very rapid current of hydrogen sulphide precipitates arsenicpentasulphide from solutions of arsenic acid after primary formationof monothioarsenic acid. This has been confirmed.63 Pyroarsenicacid itself and a number of pyroarsenates have been prepared.64Some further work on explosive antimony has been published,656 5 A. Hantzsch and K. Berger, 2. anorg. Chem., 1930, 190, 321 ; A., 1007.6 6 R. Holtje, ibid., p. 241 ; A., 876.67 J. Tausz and H. Gorlacher, ibid., p. 95; A., 876.58 A. Smits and H. W. Deinum, Proc. K . Akad. Wetensch. Amsterdam, 1930,69 A. Sanfourche, A. Hernette, and M.Fau, Bull. SOC. chim., 1930, [iv],6o W. Lange and E. Muller, Ber., 1930, 63, [ B ] , 1058; A., 877.61 H. B. Weiser, J . Physieal Chem., 1930, 34, 1021 ; A , , 721.33, 514, 619; 2. physikal. Chem., 1930,149, 337; A., 1096, 1372, 1251.47,273 ; A., 557.L. W. McCay, Amer. Chem. J . , 1888,10, 459; 2. anal. Chem., 1888, 27,632; A., 1889, ii, 15; L. W. McCay and W. Foster, Ber., 1904, 37, 573; A.,1904, ii, 253; W. Foster, J . Amer. Chem. SOC., 1916, 38, 62; A., 1916, ii,246.63 F. Foerster, G. Pressprich, and W. Reuss, 2. anorg. Chem., 1930, 188,90; A., 721.64 A. Rosenheim and H. Antelmann, ibid., 187,385 ; A., 558 ; A. Rosenheim,ibid., 193, 73; A., 1388.66 E. Cohen and C. C. Coffin, 2. physikd. Chem., 1930,149,417; A., 1268;H. von Steinwehr and A.Schulze, 2. Phyeilc, 1930,63,816 ; A., 126868 BASSETT :and a number of very complex chloroantimonates 66 and bromo-antimonites 67 are said to be formed by methods given.The preparation and analysis of K,V(CN), has been described.68Vapour-pressure measurements have been carried out with theprecipitated vanadic, niobic, and tantalic acids, but only with thefirst was there any indication of the existence of definite hydrates.69The isotherms and isobars of the system niobium-hydrogen aresimilar in form to those for vanadium and tantalum h y d r i d e ~ . ~ ~Borides of niobium and tantalum have been prepared,71 and thereaction of tantalum pentoxide with hydrogen chloride has beeninvestigated. 72It has been pointed out that element 91 (protoactinium) ischemically more like zirconium and thorium than like tantalum,and the carrier of this element in the residues from radium refiningis zirconium phosphate and not tantalum pentoxide.A dueappreciation of these facts facilitates the extraction of protoactinium,which occurs to the extent of about 0.6 mg. per g. of radium inuranium ores. Protoactinium (= ekatantalum) pentoxide is aheavy white powder, not acidic but definitely, though feebly, basic,soluble in fused sodium hydrogen sulphate, but not in fused sodiumcarbonate. 73croup V I .The mean normal boiling point of oxygen is - 182.97" & O-O10°.74The colour produced by the action of ozone on ammonia dependson the amount of water present and upon the temperat~re.~~Ozone decomposes sodium p e r b ~ r a t e .~ ~ A still for producingconductivity water has been described which is claimed to be cheap,strong, compact, durable, and easy to erect and to ~ o r k . ~ 7Experiments have been described which suggest that S, is a gel.In agreement with this, it is found that the Tyndall effect is to be66 L. I. Sauciuc, Bul. SOC. Chim. Romdnia, 1930,12, 36; A., 1388.6 8 A. Yakimach, Compt. rend., 1930,191, 789; A., 1031, 52.6Q G. F. Huttig and A. Konig, 2. anorg. Chem., 1930, 193, 81, 93, 100; A.,70 H. Hagen and A. Sieverts, ibid., 185, 225; A., 308.71 L. Andrieux, Compt. rend., 1929, 189, 1279; A., 178.72 V. Spitzin and L. Kaschtanov, J. Ruse. Phye. Chem. Soc., 1930,62, 295 ;73 A. von Grosse, 2. anorg. Chem., 1930, 186, 38; A,, 516; J .Amer.7* W. H. Keesom, (Miss) a. van der Horst, and (Miss) A. F. J. Jansen,75 W. Manchot, Ber., 1930, 63, (B], 1226; A., 877.78 F. Fichter and A. Goldach, Hdv. Chim. Actcc, 1930,13, 1200. '' J. M. Stuart and F. Wormwell, J., 1930, 86; A., 434.A. C. Vournazos, 2. anorg. Chem., 1030, 192, 369; A., 1388.1538.A,, 877.Chem. SOC., 1930, 52, 1742; A,, 883.Proc. K . Akad. Wetensch. Amsterdam, 1929, 32, 1167; A., 403INORGANIC CHEMISTRY. 69observed in pure molten sulphur.78 The cryoscopic behaviour ofa number of substances in molten sulphur has been inve~tigahd.'~Very pure sulphur hexafluoride has been prepared, and its vapourpressure measured between -72" and - 45". The b. p. (760 mm.) is- 63.8", and them. p. - 5043" & 0.2".80The best conditions for the preparation of pure hydrogen disul-phide have been described, and many of the physical constants ofthe compound determined;sl its parachor (130.0) shows that themolecule contains no double or co-ordinated valency linkage.Thef. p. curve of the system sulphur-hydrogen disulphide has no breakcorresponding with hydrogen trisulphide, so the latter compoundappears not to be a molecular compound of sulphur and hydrogendisulphide.The structure M,[SO,-SO] is proposed for the hyposulphites andis considered to agree with various decompositions and reactionswhich they undergo.82 The reactions between thiosulphate andsulphurous acid have been studied in detail, and upon them havebeen based good methods for preparing not only solid potassiumtrithionate but also solid sodium or ammonium tetrathi~nate.~~The PO,F ion of the fluorophosphates can replace the SO4 ionisomorphously and a number of fluorophosphates belonging to theferrous ammonium sulphate group and to the alums have beenprepared, as well as simple fluorophosphates.84Solid hexabromoselenous acid slowly loses bromine with formationof selenium monobromide.It will then give colloidal selenium ontreatment with water, but the pum acid dissolves in water withoutany such separation of selenium.85 The preparation of pure seleniumand tellurium tetrachlorides has been described, and many of theirphysical constants have been measured.86 The parachors of anumber of tellurium compounds now determined give a mean con-stant for tellurium of 79.4, which lies satisfactorily between theconstants for iodine and antimony.87The m.p. of tellurium purified by fractional distillation is 452.0"78 D. L. Hammick and M. Zvegintzov, J . , 1930,273 ; A., 419.79 C. R. Platzmann, Bull. Chem. SOC. Japan, 1929,4, 235; 1930,5, 79; A.,80 W. C. Schumb and E. L. Gamble, J . Amer. Chem. SOC., 1930, 52, 4302;81 K. H. Butler and 0. Maass, ibid., p. 2184; A., 1008.82 0. von Deines and G. Elstner, 2. anorg. Chem., 1930,191, 340; A., 1262.83 A. Kurtenacker and J. A. Ivanov, ibid., 185, 337; A., 302; A. Kurten-acker and K. Matejka, ibid., 193, 367; A., 1931, 52.s4 P. C. Rhy, Nature, 1930,126, 310; A., 1351.8 5 J. Meyer and V. Wurm, 2. anorg. Chem., 1930,190,90 ; A., 877.86 J.H. Simons, J . Amer. Che?n. Soo., 1930,52,3483,3488; A , , 1366.8' F. H. Burstall and S. Sugden, J., 1930, 229; A., 899.143, 568.A., 1931, 5270 BASSETT :(vac.) and is lowered in hydrogen and carbon dioxide by 0.15" and0.2 O respectively . *A method for preparing telluric acid directly from finely powderedtellurium by oxidation with chloric acid has been described.89Several mixed crystals of hexacarbamidochromic salts have beenprepared, such as those of permanganate and perchlorate, per-manganate and fluorob~rate,~~ and numerous complex chromiccompounds have been de~cribed,~~ of which a number of chromi-cyanides raise some interesting questions concerning the stabilityof polynuclear complexes which are important in connexion withother complex cyanides. A new type of red perchromate has beenprepared as the calcium salt Ca3Cr2012,12H20 by adding 30%hydrogen peroxide to a saturated calcium chromate solution atHydrazine in strongly acid boiling solution reduces sexavalentto quinquevalent molybdenum.In feebly acid solutions, complexescontaining both quinque- and sexa-valent molybdenum are pro-d ~ c e d . ~ , By the interaction of molybdenum pentachloride andvarious organic solvents, a number of substances have been obtainedwhich are formulated as derivatives of molybdenyl chloride, MoOCl,,and of molybdenum tetra~hloride.~~ Molybdenum-blue has a vari-able chemical composition. It is soluble in many organic solventsand, although it is a colloid, it is immediately extracted from itsaqueous solutions when they are shaken with certain organicMolybdic, tungstic (and vanadic) acids have beenstudied by the methods of potentiometric and conductometrictitration but, on the whole, the results are disappointing and notalways easy to interpret.95 X-Ray methods also have been appliedto the tungstic A large number of paratungstates and- 5O.92** A.Simek and B. Stehlik, J . Czech. Chem. Comm., 1930, 2, 304; A.,8 9 J. Meyer and W. Franke, 2. anorg. Chem., 1930,193, 191 ; A., 1389.90 E. Wilke-Dorfurt and R. Pfau, 2. Elektrochem., 1930, 36, 118; A., 722.9 1 R. Weinland and J. Lindner, 2. anorg. Chem., 1930,190, 285; A., 878;H. I. Schlesinger and (Miss) R. K. Worner, J . Amer. Chem. SOC., 1928,51, 3520; A., 178; H.I. Schlesinger and D. N. Rickles, ibid., p. 3523; A.,178; H. Reihlen and F. Kraut, Annalen, 1930, 478, 219; A., 686.92 J. A. Raynolds and J. H. Reedy, J . Amer. Chem. SOC., 1930,52,1861; A.,873.93 W. F. Jakbb and W. Kozlowski, Rocz. Chem., 1929,9, 667; A., 308.g4 W. Wardlaw and H. W. Webb, J . , 1930,2100; A., 1389.93a J. Duclaux and R. Titeica, Rev. gdn. Colloid., 1929,7, 289; A., 289.9 5 H. T. S . Brittonand W. L. German, J . , 1930, 1249, 2164; A., 860, 1371 ;H. T. S. Britton and R. A. Robinson, ibid., pp. 1261, 2328; A., 860, 1522;0. Jander and W. Heukeshoven, 2. anorg. Chem., 1930,187, 60; A., 438.986.e5a A. M. Morley, J., 1930, 1987; A., 1262INORGANIC CHEMISTRY. 71heteropolytungstates have been de~cribed.~~ With organic basesuranyl fluoride forms double salts of three different types, viz.,M(UO,)F,pH,O, M(UO,),F,,nH,O, and M(U0,),F7,nH,0.97Group VII.The b.p. of fluorine has been found to be 84.93' Abs., and itscritical temperature and pressure are about 144" Abs. and 55 atmos.Its vapour pressure has been measured over the range 72-86"A ~ S . ~ ~The solid compounds formed by the union of hydrogen fluoridewith perchloric acid and with boron fluoride are regarded asacidium salts by A. Hantzsch 99 and formulated as [FH,]'ClO,' and[FH,]'BF,', and several reactions of hydrogen fluoride and hydrogenchloride are interpreted in terms of the above [FH,]' ion and thecorresponding [ClH,]* ion. It has been shown that KF,3HF is adefinite compound, and a convenient apparatus for preparingfluorine by the electrolysis of this compound in the fluid conditiona t 100" has been described, with full details of procedure.1 Agood deal of work has been done on oxygen difluoride, the existenceof which is now well established.It is a colourless gas condensingto a yellow liquid, b. p. - 146.5', m. p. - 223-8', heat of formation- 4-6 & 2 kg.-cals.2 The m. p. of nitrogen trifluoride was deter-mined at the same time and found to be somewhat above - 216.6O.3According to H. von Wartenberg and G. Klinkott the heat of forma-tion of oxygen difluoride is - 11 kg.-cals.; these authors haveexamined the chemical reactions of the gas in some detail. Withpotassium iodide solution the reaction F20 + 4HI = 41 +2HF + H,O occurs, and this was made the basis of its estimation.Hydrobromic acid acts similarly, and so does hydrochloric acid, butvery slowly.With alkali the much slower reaction F,O + 2NaOH=2NaF + H,O + 0, occurs-no fluoroxy-acids being formed. Benzeneabsorbs the gas quantitatively, quinol and benzoquinonebeing formed. Reducing agents such as sodium thiosulphate,stannous chloride, ferrous sulphate, and arsenious oxide absorboxygen as well as the difluoride from mixtures containing both, butonly slowly. The oxygen difluoride is always prepared by P.A. Rosenheim, A. Wolff, J. E. Koch, and M. Siao, 2. anorg. Chem., 1930,193,47,64 ; A., 1389.9 7 F. Olsson, ibid., 187, 112; rl., 439.98 G. H. Cady and J. H. Hildebrand, J . Amer. Chem. Soc., 1930, 52, 3839 ;95 Ber., 1930, 63, [B], 1789; A , , 1140.A., 1508.1 2.anorg. Chem., 1930,193,409; A., 1931, 42.2 0. Ruff and W. Menzel, ibid., 190, 257 ; A., 877.3 0. Ruff and K. Clusius, ;bid., p. 267; A., 98672 BASSETT :Lebeau and A. Damiens's* method of passing fluorine in a finestream through weak sodium hydroxide solution. The oxidisingaction of fluorine on potassium hydrogen sulphate solution, on silver,stannous, ferrous, and cobaltous salts, and on titanic, vanadic, andmolybdic acids has been studied by F. Fichter and A. G~ldach.~By distribution experiments between nitrobenzene and waterand between benzene and water, it is shown that in both non-aqueoussolvents the concentration of hydrogen chloride is proportional toits partial pressure, indicating absence of ionisation.Since thedielectric constants of nitrobenzene and benzene are 34 and 2.2respectively, the ionisation of hydrochloric acid cannot be deter-mined by the dielectric constant of the solvent. The vapour-pressure data for aqueous hydrochloric acid solutions indicate thatonly hydrated molecules of the hydrogen chloride are ionised, andthat they exert a negligible partial pressure. It is the basiccharacter of the water, not its high dielectric constant, whichdetermines its capacity to cause ionisation.s The reactivities ofvarious oxides at different temperatures towards hydrogen chlorideand towards chlorine have been investigated.' The parachor ofchlorine dioxide has been determined, and several possible structuresof the molecule are considered.*A new chlorine fluoride, CIF,, has been prepared9 by heatingeither chlorine or its monofluoride with excess of fluorine.It is acolourless gas forming a pale green liquid, b. p. ll', and a whitesolid, m. p. - 83". It is chemically extremely active. A newfluoride of iodine, IF,, has also been obtained by heating a mixtureof iodine pentachloride and fluorine at 270-400'. It also is veryreactive chemically, and is colourless.1°The existence of bromine chloride has been confirmed by thenature of the products formed when mixtures of chlorine andbromine react with aliphatic diazo-compounds.ll According toH. Lux,la it is an ochre-yellow solid, m. p. - 54', which rapidlydecomposes in the vapour phase.According to 3'. A. Philbrick,13 the behaviour of iodine mono-4 Compt.rend., 1927, 185, 652; 1929, 188, 1263; A., 1927, 1044; 1929,Helv. Chim. Acta, 1930,13, 99, 378, 713, 1200; A,, 435, 722, 1140, 1537.13 W. F. K. Wynne-Jones, J . , 1930, 1064; A., 859.7 R. Wasmuht, 2. angew. Chem., 1930, 43, 98, 125; A., 439; V. Spitzin,779 ; Ann. Reports, 1929, 26, 63.2. anorg. Chem., 1930,189, 337 ; A., 874.G. H. Cheesman, J., 1930, 35 ; A., 278.a 0. Ruff and H. Krug, 2. unorg. Chem., 1930,190,270; A., 878.lo Idem, ibid., 193, 176 ; A , , 1390.T. W. J. Taylor and L. A. Forscey, J . , 1930, 2272; A,, 1565.l2 Ber., 1930, 63, [B], 1156; A., 878.l3 J., 1930, 2254; A., 1520INORGANIC CHEMISTRY. 73chloride in hydrochloric acid solution indicates that it is ionised toI' and Cl'.Small amounts of a volatile oxide of bromine, probably Br,O, areformed by the action of bromine on specially prepared, and veryreactive, mercuric oxide between 50" and 100°.14Potassium iodide can be partly converted into iodate by heatingin oxygen under pressure, and if the iodide is mixed with potassiumhydroxide the oxidation takes place still more readily, some periodatealso being formed.16The change of pink manganese sulphide into the orange and thegreen form occurs much more slowly if ammonium sulphide is usedfor precipitation instead of ammonium hydrogen sulphide and theaddition of ammonia before that of its sulphide hinders the changevery greatly.The green form is crystalline, but the other two areamorphous. 16Two series of complex manganifluorides have been obtained, vix.,MMnF,,nH,O and M.JHnF6, where M is an organic base.Theformer represents a new type, whilst the latter corresponds to thealkali manganif€uorides.l7Manganese dioxide may be prepared from any lower oxide bydirect oxidation with oxygen; by using sodium hydroxide ascatalyst at 400-500", a product containing 5 6 9 5 % MnO, may beobtained.18 K,Mn(CN), may be prepared by the addition of asaturated solution of potassium permanganate to an 80% solutionof potassium cyanide until red acicular crystals are produced.l9Some new perchlorates and permanganates have been described,as well as a number of fluorosulphonates which are isomorphouswith them.20One hears no more of masurium nowadays, but rhenium isthoroughly well established among the elements.Very purepotassium per-rhenate can, in fact, now be obtained commerciallyfrom the " Vereinigten Fabriken zu Leopoldshall." Its technicalpreparation has been described by W. Peit.21The formation of per-rhenate occurs so extremely easily that thel4 E. Zintl and G. Rieniicker, Ber., 1930,83, [B], 1098; A., 878.15 F. A. Henglein and L. Teichmann, 2. anorg. Chem., 1930,188, 138 ; A.,lo G. Landesen and M. Reistal, ibid., 193, 277 ; A., 1639.l7 F. Olsson, ibid., 187,313; A., 688.722.Y . Kato and T . Matsuhashi, J . 8oc. Chem. Ind. Japan, 1929,32, 313 B,316 B ; A., 1930, 308.19 A. Yakimach, Compt. rend., 1930, 190, 681; A., 658.20 E. Wilke-Dorfurt, G. Balz, and A. Weinhardt, 2. anorg. Chem., 1930,21 2.angew. Chem., 1930,43,469; B., 822.185,417 ; A., 308.c 74 BASSETT :preparation of compounds of the lower oxidation stages is verydifficult. It has been shown that zinc and hydrochloric acidreduce per-rhenate through the various intermediate stages to metal,with the possibility of halting a t these stages. Sodium amalgamand hydrazine both reduce i t to metal, but in each case someadmixture of lower oxides is present.22 The electrical conductivityof potassium per-rhenate for concentrations between 0.04 and 0.0005g.-mol. per litre has been determined a t 18", 25", 30", and 40".23From weakly acid solutions soluble per-rhenates can be precipitatedand estimated quantitatively by means of " nitron." 24Group V I I I .The conditions under which iron reacts with carbon monoxide toform oxide, carbide, or graphite have been examined,25 as havethose necessary for the oxidation of ferrous hydroxide to ferrousferrite rather than to ferric hydroxide.26 Different forms of ferrichydroxide, y- and tc-, result according as ferrous ferrite is or is not anintermediate stage.27 The results of recent work leave it doubtfulwhat hydrates of ferric oxide actually exist.28 The action of iron a thigh temperatures on hydrogen sulphide, hydrogen selenide, andcarbon disulphide has been examined,29 and a full investigation hasbeen made of the reaction FeS, zz FeS + S.30 It has beenshown that carbonyl groups in iron pentacarbonyl can be replacedby various amines, and a number of the compounds so obtained aredescribed.31 Several compounds of metal carbonyls with ironhalides have been prepared, and the space occupied by carbonmonoxide in various complex metal compounds has beenestimated.32 Iron tetracarbonyl, prepared by the action of alkalialkoxide on iron pentacarbonyl, has been shown to be [Fe(CO),],.Details of many of its reactions and derivatives are given.33zp F.Krauss and H. Steinfeld, 2. anorg. Chem., 1930,193, 385; A., 1931,63.23 N. A. Puschin and P. S. Tutundiib, ibid., p. 420; A., 1931, 43.24 W. Geilmann and A. Voigt, ibid., p. 311 ; A., 1547.2 5 V. Hofmann and E. Groll, ibid., 191, 414; A., 1263.z 6 C. Sandonnini, Gazzetta, 1930, 60, 321 ; A . , 878.2 7 G. Schikorr, 2. anorg. Chem., 1930, 191, 322; A., 1263.z * P.A. Thiessen and R. Koppen, 2. anorg. Chem., 1930,189, 113; A., 559;V. Rodt, Rec. trav. chim., 1930,49,441; A., 723 ; G. F. Huttig and A. Ziirner,2. EZektroch>em., 1930, 36, 259 ; A . , 723.*' J. B. Peel, P. L. Robinson, and C. L. Mavin, Proc. Univ. Durham Phil.Soc., 1929, 8, 153 ; A., 179.30 F. de Rudder, BUZZ. Xoc. chim., 1930, [iv], 47, 1225.31 W. Hieber, Naturwiss., 1930,18, 33 ; A., 309 ; W. Hieber, F. Sonnenkalb,32 W. Hieber, K. Ries, and G. Bader, 2. anorg. Chem., 1930,190, 193, 215;33 W. Hieber and E. Becker, Ber., 1930,63, [B], 1405; A., 1008.and E. Becker, Ber., 1930,63, [ B ] , 973 ; A., 723.A . , 875INORGANIC CHEMISTRY. 75It is said that the compound supposed by W. Manchot andto be Fe(N0),2MeOH is, in reality, a derivative of bivalent H.GallCH 0 .,,,NO .,... OH iron, with the structure c~~o>Fe~.~~No~,,.Fe<OCH3. By theaction of nitric oxide on nickel carbonyl, a somewhat similar com-pound, Ni(NO)(OCH,)OH + CH30H, was obtained.35R. Brunner has described the preparation of several compoundsfrom sodium nitroprusside,36 and numerous compounds of hem-methylenetetramine with ferro- and ferri-cyanides have beenobtained .37A phase-rule study of the cobalt chloride colour change has beenmade, and the red salt [Co(H,O),]HgCl, and the blue salt[Mg((H20)2},]CoCl, were isolated as well as several series of redsolid solutions containing zinc chloride. Neither the simple dehydra-tion theory nor the " variable co-ordination " theory of the colourchanges is supported by the data.It is considered to be largelyaccidental that red cobalt chloride solutions contain red kations andblue solutions blue anions. In a more general way, the colour of cobalt -ous compounds is determined by the character of the electronicshift which is possible in the cobalt atom of the compound inquestion.38 The electro-deposition of cobalt from red and fromblue solutions has been examined, and found to be reversible onlyfrom the latter.39The dehydration curves of hydrated cobaltous oxide prepared indifferent ways have been determined, as well as the catalyticactivity of the metal reduced from various types of oxide.*O Themolybdates of various cobaltic ammines have been prepared.4lVapour pressures of nickel carbonyl have been measured over thetemperature range -35" to 40°.42 Nickel thiosulphate forms ahexammine, a tetrammine, and a diammine, but not the pentamminedescribed by Ephraim.& The dehydration curves and X-raydiagrams of hydrated nickelous and nickelic oxides have beenexamined.44 The latter forms a monohydrate which breaks upirreversibly thus, 2(Ni,03,H20) -+ 4Ni0 + 2H20 + 0,.Accord-34 Ann. Reports, 1929, 26, 66.36 H. Reihlen, A. Gruhl, G. von Hessling, and 0. Pfrengle, Annnlen, 1930,36 2. anorg. Chem., 1930,190,384; A., 1009.37 G. A. Barbieri, Gazzetta, 1930, 60, 229 ; A., 752.38 H. Bassett and H. H. Croucher, J., 1930, 1784 ; A., 1251.39 R. Brdizka, J . Czech. Chem. Comm., 1930,2,489; A . , 1254.40 G. F. Huttig and R. Kassler, 2. anorg. Chem., 1930,187, 16,24; A., 543.41 P.R. RBy and S. N. Maulik, J . Indian Chem. SOC., 1930,7,607 ; A., 1390.42 J. S. Anderson, J., 1930, 1653: A., 1104.43 L. le Boucher, Anal. Pk. Quim., 1930,28,895; A., 1391. '* G. F. Huttig and A. Peter, 2. artorg. Chem., 1930,180, 183, 190; A., 700.482,161 ; A., 153976 BASSETT :ing to D. K. Goralevitsch,46 colourless alkaline-earth salts ofnickelic acid, H2Ni04, can be obtained by fusion of nickel oxide withpotassium nitrate or chlorate and potassium hydroxide, followedby extraction with water and addition of the appropriate reagentto the green solution. BaNiO,, NO4, and Ni,O, are also said to havebeen 0btained.4~"as well as somealkali-metal bromides of rhodium 47 and some rhodium pyridinebromides.48 The ruthenium analogue of potassium nitroprusside,K2[ Ru( CN) ,NO J,2H20 (also anhydrous), has been prepared byW.Manchot and J. Diising;48a and by the action of carbon monox-ide on ruthenium tribromide the compound RuBr( CO) containingunivalent ruthenium has been obtained.49The remarkable case of lithium platinocyanide, the trihydrate ofwhich was supposed to become unstable with reference to thedihydrate at lower temperaturesY50 has been shown to have anentirely different e~planation.~lBy the action of sodium amalgam on solutions of potassium (orbarium) platinocyanide or potassium palladocyanide, colourless,strongly reducing solutions are obtained which contain univalentplatinum or palladium. 62The thermal decomposition of platinous and platinic sulphideshas been studied, but no indication of any other sulphide was ob-tained.63 Platinum diarsenide identical with the mineral sperrylitehas been prepared.64The brownish-yellow double salt PtC12,2NH,,4(PtC~,4NH,)can form solid solutions in PtC12,4NH,,nH20, and this is the cause ofthe yellowish-brown colour which the latter compound has whenprepared by the action of ammonia on K2PtC1,.65Numerous nitro-ammines of platinum have been described .5645 J .Russ. Phys. Chem. SOC., 1930, 62, 897; A . , 1141.46a Idem, ibid., p. 1166; A., 1540.46 A. W. Mond, J . , 1930,1247; A., 891.4 7 P. Poulenc, Compt. rend., 1930, 190, 639; A . , 559.4 8 Idem, ibid., 191, 64; A., 1391. 48a Ber., 1930, 63, [ B ] , 1226.4@ W. Manchot and E. Enk, ibid., p.1635; A . , 1141.61 H. Terrey, ibid., 1930, [ A ] , 128,359; A., 1141.6a W. Manchot and G. Lehmann, Ber., 1930, 63, [ B ] , 2776; A., 1931, 53;53 W. Biltz and R. Juza, 2. anorg. Chem., 1930,190,161 ; A., 861.64 L. Wohler, ibid., 186, 324; A., 440.6 5 N. S. Kurnakov and I. A. Andrhvski, 2. anorg. Chem., 1930,189, 137;A., 560; Ann. Inst. Platine, 1929, 7, 161; A., 1930, 180.66 I. I. Tschernaiev, ibid., 1929, 7, 52; A., 179; I. I. Tschernaiev andA. N. Fedorova, ibid., p. 73 ; A., 180; I. I. Tschernaiev and F. M. Klatschkin,ibid., p. 84; A., 180.The acetates of ruthenium have beenJ. E. Reynolds, PTOC. Roy. SOC., 1909, [ A ] , 82, 380; A., 1909, i, 659.W. Manchot and H. Schmid, ibid., p. 2782; A., 1931, 53INORGANIC CHEMISTRY. 77A large number of platinum tetrammine salts have been preparedand examined, and from the character of their electrical conductivityand absorption spectra it is concluded that they possess six co-ordinatively bound groups, and not four as hitherto assumed.57They should be formulated as [Pt(NH,),X,], although in solventssuch as water, alcohol, or acetone they are readily converted intostable salts of the type [Pt(NH3)4(solvent)2] X,.The ammine amides of 4-valent platinum, such as[Pt(NH,),* (NH,)*CllC~,,have been investigated with respect to their behaviour towardsacids and bases.58 Of the ammonia compounds examined, the3-amido-diammine was the most basic.The behaviour of allthe compounds is adequately represented by the equation[R - Pt . . . NH3In+l +- [R - Pt - NH,]"+ H .Someinteresting stereochemical questions are raised in two papers onplatinum compounds by F. G. Angell, H. D. K. Drew, andW. ward la^,^^ and by F. G. Mann 6o respectively. These are dealtwith in another section of the present volume (pp. 164, 166).Systems and Equilibria.Platinum-iron ;61 platiniim-iridium ;62 rhodium-bismuth ;63palladium-antimony gold-antimony ; 65 iron-beryllium andiron-boron ;ss iron-manganese ;67 nickel-copper ;68 silver-copper ;69cuprous iodide-silver iodide ; 70 potassium selenate-water ; 7 1 copper-oxygen ; 72 titanium-hydrogen ;73 nitrogen pentoxide-nitric acid ;74zirconium dioxide-beryllium oxide ; 75 tellurium dioxidehydrogen676869606 1626364656%67A. Hantzsch and F.Rosenblatt, 2. anorg. Chem., 1930,187,241 ; A., 440.A. A. Griinberg and G. P. Faormann, ibid., 193, 193; A., 1540.J., 1930, 349 ; A., 559.Ibid., p. 1746; A., 1404.V. A. Nemilov, Ann. Inst. PZatine, 1929,7, 1 ; A., 147.Idem, ibid., p. 14; A., 148.E. J. Rode, ibid., p. 21; A., 148.A. T. Grigoriev, ibid., p. 32; A., 148.Idem, ibid., p. 45; A., 148.F. Wever, 2. tech. Physik, 1929, 10, 137; A., 148.W. Schmidt, Arch. Eikenhiittenw., 1929-1930, 3, 293 ; Stahl iind Eisen,1929, 49, 1696; A., 148.1929, 32, 912, 921; A., 148.68 A. Krupkowski and W. J. de Haas, PTOC. K. Akad. Wetensch. Amsterdam,139 0. Weinbaum, 2. Metallb., 1929,21,397; A., 149.?* G. Lunde and P. Rosbaud, 2. physikal. Chem., 1929, [B], 6,115; A., 149.7 1 J. A. N. Friend, J., 1929, 2782; A,, 149.73 L.Kirschfeld and A. Sieverts, 2. physikal. Chem., 1929,145,227 ; A., 161.74 E. Berl and H. H. Saenger, Monatsh., 1929,53 and 54,1036; A., 161.76 0. RUB, F. Ebert, and E. Stephan, 2. anwg. Chern., 1929,185, 221; A , ,R. Vogel and W. Pocher, 2. Metallk., 1929,21, 333, 368; A., 161.16278 BASSETT :fluoride-water ;76 nickel-bismuth ;77 lead-germanium ;78 silver-copper-zinc ;79 copper-tin-antimony ;SO potassium chloratesodiumchlorate ;sl calcium chloride-cobalt (or iron, manganese, or cadmium)chloride ;81a metal halides-hydrogen ; metal halides-hydrogenchloride ;82 magnesium sulphate-sodium sulphate-watermagnesium sulphate-sodium nitrate-water ammonium nitrate-potassium sulphate-water ;85 alumina-cryolite-chiolite aceticacid-acetate of potassium (or NH,, Li, Pb, Ba, Ca, Zn);s7 iron-nitrogen nickel-chromium ;8g water-ether-uranyl nitrate orzinc iodide or cadmium iodide silver-aluminium-zinc ;91 sodiumiodate-sodium sulphate-water ;92 sodium chloride-magnesiumsulphate-water ;93 nickel-chromium ;94 ferrous sulphate-water ;95calcium-calcium nitride ; 96 iron-carbon-oxygen ; 97 sodiumhydroxide-sodium nitrate-water ;98 copper sulphate-sulphuricacid-water ;99 zinc oxide-zinc chloride-water ;l potassium sulphate7 6 E.13. R. Prideauxand J. O’N. Millott, J., 1929, 2703; A., 163.7 7 G. Hagg and G. Funke, 2. physikal. Chem., 1930, [B], 6, 272; A., 284.T. R. Briggs and W. S. Benedict, J.*PhysicaZ Chem., 1930, 34, 173; A.,284.79 S. Ueno, Mem. Coll. Sci. Kyoto, 1929, 12, 347; A., 284.So M.Tasaki, ibid., p. 227; A., 285.81 A. P. Vitoria, Anal. Pis. Quim., 1929, 27, 787; A., 293.81a A. Ferrari and A. Inganni, Atti R. Accad. Lincei, 1929, [vi], 10, 253;S 2 K. Jellinek and R. Koop, 2. physikal. Chem., 1929, 145, 305; A . , 294.8 3 W. Schroder, 2. angew. Chem., 1929, 42, 1076; A., 294.84 Idem, 2. anorg. Chem., 1930, 185, 267; A., 294.8 5 E. Janecke, 2. angew. Chem., 1929,42, 1169; A., 294.L. Wasilewski and S. Mantel, Przemysi Chem., 1930,14, 25 ; A., 299.8 7 A. W. Davidson and W. H. McAllister, J . Amer. Chem. SOC., 1930, 52,8 8 S. Epstein, H. C. Cross, E. C. Groesbeck, and I. J. Wymore, U.S. Bur.89 S. Nishigori and M. Hamasumi, Sci. Rep. TGhoku Imp. Univ., 1929, 18,90 (Mlle.) 0. Guempel, Bull. Soc. chim. Belg., 1929, 38, 443; A., 420.91 S.Ueno, Mem. Coll. Sci. Kyoto, 1930, [A], 13, 91 ; A., 536.92 H. W. Footeand J. E. Vance, Amer. J . Sci., 1930, [v], 19, 203; A.,93 V. P. Iljinski and A. F. Sagaidatschni, J . Russ. Phys. Chem. SOC., 1929,g4 Y. Matsunaga, J . Study Met. Japan, 1929,6, 207 ; A., 680.95 F. K. Cameron, J. Physical Chem., 1930, 34, 692; A., 683.B6 A. von Antropoff and E. Falk, 2. anorg. Chem., 1930,187, 406; A., 699.s7 E. Scheil and E. H. Schulz, ibid., 188, 290; A,, 701.98 E. JLinecke, ibid., p. 72; A., 701.09 H. D. Crockford and L. E. Warwick, J. Physical Chem., 1930, 34, 1064;A., 285.507; A., 406.Stand. J . Res., 1929, 3, 1005; A., 419.491 ; A., 419.544.61, 1953; A., 544.A., 701.1 H. C. Holland, J., 1930,643; A., 701INORGATSIC CHEMISTRY.79magnesium sulphate-water ;2 water-alkali sulphate-sulphate ofvitriol type ;3 magnesium sulphate-potassium nitrate-water ;magnesium chloride-sodium nitrate-water ; sodium dichromate-ammonium chloride-water ;6 potassium sulphate (or sulphuric acid)-hexamminocobaltic sulphate-water ;' sodium palmitate-water-sodium chloride ; sodium germanate-sodium silicate and potassiumgermanate-germania ; lead-antimony-magnesium ; 13 potassiumand calcium carbonates and hydroxides-water ;lo iron-manganese ;I1iron-silicon ;I2 iron-nitrogen ;13 sodium sulphate-sodium carbonate-water ;la sodium chloride-magnesium sulphate-water ;15 aluminiumsilicon-copper ;I6 sodium (or potassium) bromide (or iodide)-water ;17phenol-silver nitrate-water ;18 iron-nitrogen ;19 sodium oxide-silica ;20 sodium oxide-boric oxide-water ;21 sodium oxide-silica-zirconium dioxide ;22 calcium chlorate-potassium chloride-water ;23B.A. Starrs and L. Clarke, J. Physical Chem., 1930, 34, 1058; A., 702;A. Benrath and L. Cremers, 2. anorg. Chem., 1930,189, 82; A., 702.A. Benrath, H. Benrath, and H. Wazelle, &id., p. 72; A., 702.A. Sieverts and H. Mdler, ibid., p. 241 ; A., 702.I. Gerasimov, ibid., 187, 321 ; A., 702.P. B. Sarkar and T. P. Barat, J . Indian Chem. SOC., 1930, 7, 119, 199;J. W. McBain, L. H. Lazarus, and A. V. Pitter, 2. physikal. Chem., 1930,B. A. Starrs and H. H. Storch, ibid., p. 2367; A., 1523.A., 702, 1009.147, 87 ; A., 702.8a R. Schwarz and M. Lewinsohn, Ber., 1930,63, [B], 783 ; A., 721.E.Abel, 0. Redlich, and F. Spausta, 2. anorg. Chem., 1930,190, 79; A.,861.lo M. 1. Ussanovitsch and S. A. Borovik, Ukraine Chem. J., 1929, 4, 479;A., 861.l1 A. Osawa, Sci. Rep. TGhoku Imp. Univ., 1930, 19, 247; A., 987; E.ohman, 2. physikaZ. Chem., 1930, [B], 8, 81 ; A., 988.l2 B. Stoughton and E. S. Greiner, Amer. Inst. Met. Eng. Tech. Pub., 1930,No. 309, p. 3 ; A., 988 ; J. L. Haughton and M. L. Backer, J . Iron Steel Inst.,1930,121, 315 ; A., 1931, 32.l3 0. Eisenhut and E. Kaupp, 2. Elektrochem., 1930,36, 392; A., 996.1 4 N. S. Kurnakov and S. Z . Makarov, Ann. Inst. Anal. Phys. Chem., 1930,1 5 N. S. Kurnakov and M. A. Opichtina, ibid., p. 365; A., 997.16 G. G. Urasov, S. A. Pogodin, and G. M. Samorueev, Min. Ssyrje Zwet.1 7 A.F. Scott and E. J. Durham, J . Physical Chem., 1930, 34, 1424; A.,4, 307; A., 997.Met., 1929,4, 160; Chem. Zentr., 1930, i, 1038; A., 1106.1107.C. R. Bailey, J., 1930, 1534; A., 1120.10 E. Lehrer, 2. Elektrochem., 1930,36, 460 ; A., 1121.20 F. C. Kracek, J. Physical Chem., 1930,34, 1683; A., 1121.21 U. Sborgi and L. Amelotti, Gazzetta, 1930, 60, 468; A., 1122.22 J. D'Ans and J. Loffler, 2. anorg. Chem., 1930,191, 1 ; A., 1122.23 Y. Osaka and H. Nishio, Bull. Chem. SOC. Japan, 1930, 5, 181; A.,112280 BASSETT :iron-nickel-sulphur ;24 nickel-chromium ;25 Ca + 2NaC1 Z 2Na + CaCl, ;26 carbamide-ammonium nitrate-sodium nitrate ;27ammonium carbamate-carbamide-water-ammonia ;28 boric oxide-caesium oxide-water ;29 lithium-silver ;30 cadmium-zinc ;31 lead-antimony ;32 lead-tin ;33 manganese oxide-cadmium oxide ;=manganese oxide-magnesium oxide ;35 alumina-chromium sesqui-oxide ;35 alumina-ferric oxide ;35 chromium sesquioxide-ferricoxide ;35 iron-boron ;36 ammonium nitrate-water ;37 carbon dioxide-ammonia-water ;38 alumina-sodium (or potassium) oxid+water ;39cadmium sulphate-potassium (or ammonium) sulphate-water ;40potassium oxide-lime-silica ;41 Fe + NiSiO, rt Ni + PeSiO, ;42silver-strontium and silver-barium water-hydrogen fluoride ;44K2C03 + 2NaHC0, =+ Na,CO, + 2KHC0, ;45 potassium carbonate,bicarbonate, and water ;46 sodium sulphate, fluoride, and chloride andwater ;47 mercuric oxide-sulphur trioxide-water ;48 copper sulphate-24 R. Vogel and W. Tom, Arch. Eisenhuttenw., 1929-30, 3, 769; Staid und25 S. Sekito and Y. Matsunaga, J . Study Met. Japan, 1929,6,229; A., 1245.2 6 E. Rinck, Compt. rend., 1930,191, 404; A., 1252.27 W. J. Howells, J., 1930, 2010; A., 1252.28 H. J. Krase and V. L. Gaddy, J . Amer. Chem. SOC., 1930, 52, 3088; A.,29 A. P. Rollet and L. Andrits, Compt. rend., 1930,191,376; A., 1261.30 S. Pastorello, Bazzetta, 1930, 60, 493 ; A., 1359.31 D. Stockdale, Inst. Metals, Sept. 1930, Advance Copy; A., 1359.32 D. Solomon and W. M. Jones, Phil. Mag., 1930, [vii], 10, 470; A.,33 K. Honda and H. AbB, Sci. Rep. Tdhoku Imp. Univ., 1930,19, 315; A.,34 L. Passerini, Bazzetta, 1930,60, 535; A., 1361.35 Idem, ibid., 644; A., 1361.36 F. Wever and A. Muller, 2. anorg. Chem., 1930,192,317; A., 1372.37 E. Jhnecke and E. Rahlfs, ibid., p. 237; A., 1373.3 8 Idem, 2. Elektrochem., 1930,36, 645; A., 1373.39 R. Fricke and P. Jucaitis, 2. anorg. Chem., 1930,191, 129; A., 1374.40 K. L. Malhotra and H. D. Suri, J. Physical Chem., 1930, 34, 2103; A.,4 1 G. W. Morey, F. C. Kracek, and N. L. Bowen, J . SOC. Glass Tech., 1930,42 H. zur Strassen, 2. anorg. Chem., 1930,191, 209; A., 1375.43 F. Weibke, ibid., 193, 297; A., 1509.44 G. H. Cady and J. H. Hildebrand, J . Amer. Chem. SOC., 1930,52,3843 ; A.,45 A. E. Hill, ibid., p. 3813; A . , 1523.46 Idem, ibid., p. 3817; A., 1523.4 7 H. W. Foote and J. F. Schairer, J . Amer. Chem. SOC., 1930, 52, 4202,48 M. PaiE. Bull. SQC. chim., 1930, 47, 1254; Compt. rend., 1930,190, 1014;Eisen, 1930, 50, 1090; B., 910.1252.1359.1359.1374.14, 149; A., 1374.1521.4210; A., 1931,41.A , . 701INORQANIC OHEMISTRY. 81lithium sulphate-water ;49water (and related systems)Group I.s1sodium chloride-magnesium sulphate-silver iodide-metal chlorides ofH. BASSETT.H. D. Crockford and M. M. Webster, J . Phys~cccl Chem., 1930, 34, 2375;A., 1523.50 N. K. Voskressensks, J . Apppl. Chem. Rueeia, 1930,3,321; A., 1523.61 V. P. Radischtschev, J. Rues. Phys. Chem. SOC., 1930,62,1063 j A., 1623