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Proceedings of the Chemical Society, Vol. 13, No. 183 |
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Proceedings of the Chemical Society, London,
Volume 13,
Issue 183,
1897,
Page 165-216
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摘要:
PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE SECRETARIES. ~ ~~ No. 183. Session 1896-7. The following are the abstracts of papers received- during the vacation, and published in the Transactions :-96. (( The ethers of camphoroxime." By M. 0. Forster, Ph.D. The methyl ether of camphoroxime boils at 181.5-182-5" under a pressure of 357 mu. ; it has the sp. gr. = 0,9631, and the specific rotatory power [a],,= -13.05' at 20". It does not reduce an am- moniacal solution of silver nitrate, and dissolves in mineral acids without undergoing change. The nitrate crystallises from benzene in needles melting at 81-82', and has [a]D = -16.9" in benzene ;the h9dyiodide is amorphous, and melts at 157"with vigorous effervescence. The ethyl ether (Nageli) boils at 185' under a pressure of 336 mm., and has the sp.gr. = 0.9470 ; the specific rotatory power [a]D = -1goOo at 23.5'. The 6enzgZ ethey is a colourless oil, which on distillation is in part resolved into benzaldehy de and camphorimine, as represented by the equation C,oH,6:NO*CH,-C6H,=C,,H,,:NH +C,H,* CHO ; it has [a], = -16.4' in alcohol, and forms an amorphous hyclriodide which melts at 91'. Concent-rated sulphuric acid resolves the ether into camphoroxime and the resinous hydrocarbon, C14H12,obtained on dissolving benzylic alcohol in concentrated sulphuric acid. Alcoholic hydrochloric acid eliminates a-benzylhydroxylamine from the ether ; the platinochloride of this base forms golden-yellow scales, and does not melt below 250'. The acetyl derivative of camphoroxime is a colourless liquid, and is completely converted into acetic acid and campholenonitrile on distilla-tion; it has the specific rotatory power [a]== -45.8"in alcohol, and on treatment with cold phenylhydrazine yields symmetrical acetyl- phenylhydrazine and camphoroxime. 166 The benxoyl derivative crystallises from acetone in magnificent six-sided prisms, and melts at 88--90°; it has [a],,= -40.7' in alcohol, and yields benzanilicle when heated with aniline.Cold phenylhydrazine gives rise to benzoylphenylhydrazine and cam-phoroxime. Carnphoroxinae hydrobronzide melts and evolves hydrogen bromide at 174"; it has = -35.8" in alcohol, and is converted by glacial acetic acid in to campholenonitrile and hydrogen bromide.Cawiphoroxirne platinochloride crystallises in transparent prisms which become opaque in the desiccator, and melts at 156.5" with vigorous eflervescence ;cold water regenerates the oxime. Inactive camphoroxirne melts like the active modification at 118' ; it crystallises from petro- leum in diamond-shaped plates, and is racemic according to the classification recently suggested by Kipping and Pope (this vol., 135). 97. "The action of nitrogen trioxide and tetroxide on alcohols. Part I." By Julius Berend Cohen, Ph,D., and Harry Thornton Calvert, B.Sc. The authors have found that when nitrogen trioxide or tetroxide dissolved in chloroform is allowed to act upon benzyl alcohol, that water is in both cases eliminated, and compounds of the formula C,H,CHN,O, and C,H,CHN,O, are probably formed, which rapidly decompose on standing into benzaldehyde, with the separation in the first case of nitric oxide, and in the second of nitrogen trioxide, according to the following equations, (1) c,H,CHN,O, =C,H,COH + 2N0, (2) C,H,CHN,O, =C,ET,COH +N2OT The latter substance, which may be termed benzylidene nitrosate, is decomposed by water into a.compound of the formula C7H7N0,, which is probably identical with a substance obtained by Lippmann and Hawliczek (Bey., 1876, Q, 1463) by the action cf nitric acid upon benzaldehyde.By the action of reducing agents it is converted into benzyl alcohol, benzylamine and ammonia. 98. ''The action of nitrogen tetroxide on ortho- and para-nitrobenzyl- alcohol." By Julius B.Cohen, Ph.D., and William H. Harrison, B,Sc. The authors have discovered a simple method for preparing the aldehydes corresponding to ortho- and para-nitrobenzylalcohol. The reaction consists in treating the alcohol with a small quantity of nitrogen tetroxide in presence of air. A nearly theoretical yield of these aldehydes, hitherto very difficult to prepare, has been e$ected by this method, 167 99. “The action of aromatic amines upon diacetyltartaric an-hydride.” By Julius Berend Cohen, Ph.D., and William Hudson Harrison, B,Sc. In attempting to prepare the isomeric toluido-acetyl tartaric acids, by acting upon diacetyltartaric anhydride with the isomeric toluidines, with a view to comparing their optical characters, the authors were unsuccessful; but obtained, on the other hand, by this reaction with different aromatic amines, a series of golden-yellow crystalline com- pounds.The formula of the aniline compound is probably Cl6HI2N2o3, that of the paratoluidine compound ClSH16N203,and of the a-naphthyl- amine compound C27H16N203.The constitution of these compounds has not yet been ascertained. The reaction in all cases is very complex, and the yield of the yellow substances very small. 100. “Studies on citrazinic acid. Part V.” By W. J, Sell, M.A.,and F. W. Dootson, B.A. This investigation was commenced with the view of obtaining some evidence of the positions of the hydroxyl groups in citrazinic acid, by preparing the corresponding dicblorisonicotinic acid, and then replac- ing the chlorine atoms either by cyanogen or methyl, and thus by well-known methods obtaining one of the tricarboxy-acids whose con- stitution has been established.In the preparation of the dichloriso- nicotinic acid by the interaction of phosphorus pentachloride on citrazinic acid, however, such a number of interesting substances were found to be produced that it was determined to publish this part of the work at once, leaving the remainder for a further communica- tion. The following substances-amongst others-have been isolated, and are described in the paper. (1) Chlorhydroxyisonicotinic acid ; (2) dichlorisonicotinic acid ; (3) tetrachlorisonicotinic acid chloride ; (4) apdp’-tetrachlorisonicotinic acid ; (5) tetrachlorpyridine ; (6) pentachlorpyridine ; (7) pentachlor-picoline. 101.“The condensation of choral with resorcinol. 11.” By J. T. Hewitt, M.A., D.Sc.,and Frank (3. Pope. In an earlier paper (Trans., 1896, 69, 1265), the view was expressed that the substanceof the formula Cl4Hl0O5, obtained by the condensa- tion of choral hydrate with resorcinol, was a lactone of 2 :4 :2’ :$-tetra-hydroxydiphenylacetic acid. The authors had overlooked a paper by Michael and Comey (Amer. Chem. Joum., 1883-4, 5,350) in which 168 the formula CsH,03 was attributed to the compound in question. The determination of tho molecular weight by the lowering of freezing point of a phenolic solution gave as result 232; the values required by the formulae C,H,03 and C,,H,,O, being 150 and 258 respectively.The analyses of the acetate and benzoate have further confirmed the authors’ views that the compound possesses three hgdroxyl groups. In addition to this, it has been found that a red salt is precipitated when an excess of sodium ethylate solution is added to an absolute alcoholic solution of the lactone : the salt was found to contain 22.10 per cent. of sodium, whilst the formula, C1,H70,Na3 requires 21.30 per cent. of sodium. The analysis of the salt, obtained by boiling the lactone with water and barium carbonate, led to the formula Ba(C14H1,06)2 ; the soluble zinc salt obtained in a similar way, gave a percentage of zinc which agrees with the formula Zn(C,,H,,O,),.102. ‘‘ On P-oxycellulose.” By Benjamin Samuel Bull, M,A., B.Sc. P-Oxgcellulose has been studied by several workers, and Cross and Bevan have prepared a trinitro-derivative. In this paper a benzoate and nitrate obtained from P-oxycellulose are described. These com- pounds are probably hexa-derivatives of a substance having the empirical formula C,,H,70,,. 103, 6‘ A new synthesis of phloroglucinol.” By David S. Jerdan, B.Sc. When finely divided sodium is dissolved in a benzene solution of ethylic acetone-di-carboxylate and the solution is boiled for some hourp, a gummy deposit is slowly formed. The whole is then shaken with water and the aqueous solution, after separation of the benzene, is acidified with sulphuric acid.The solution becomes milky and a granular precipitate falls after a short time. The new substance may be recrystnllised from glacial acetic acid, and then possesses a composition corresponding with the formula C12H,,07. This compound, when boiled with methylic alcohol containing 3 per cent, of hydrogen chloride, took up a molecule of alcohol, giving a crystalline ester, C1,Hl,Os. The substance C12H1007must therefore be a lactone. Further, on hydrolysis with baryta solution, the lactone gave carbon dioxide, alcohol, malonic acid, and phloroglucinol. The new compound is therefore a phloroglucinol derivative. It is probably formed according to the equation :-2C,,H,,O, + 3Na =C,,H,,07 + 3NaOC,H, + 3H. The immediate product of the reaction must of course be a sodium derivative, the lactone C,,N,& being formed from this on addition of sulphuric acid, 169 104. "Phenanthrone." By Francis R.Japp, F,R.S.,and Alexander Findlay, M.A.,B.Sc. Phenanthrone was regarded by its discoverer, Lachowicz (J.p. C H *?H,Chenz., 1883, [2], 28, 173), as a ketone of the formula l6C,H,* CO Japp and Klingemann (Trans., 1893, 63,770) suggested that it might~~ be a phenol of the formula I 6 4'S" (P-p?benantIbrol).C,H,* C*OH In the hope of deciding between these two formulz, the present authors have prepared various derivatives of phenanthrone. The evidence, however, points in both directions. The compound reacts both in the ketonic and in the phenolic form, although more frequently in the latter.In the great majority of its reactions it is a strict ana- logue of /I-naphthol. In preparing phenanthrone by the method discovered by Japp and Klingemann-reduction of phenanthraquinone with hydriodic acid- the authors find that two other subst,ances are simultaneously formed : /3-phenu.ntIwylc oxide (C,,Hg)20 (m. p. 2 lo'), and tetr~p~~nylenefurfurccn 7GH4*G-f??GH4 (m. p. 306"). The latter was obtained by Japp and CGH,* C* O*C*C,H, Klingemann by the destructive distillution of monacetyl phenan- thraquinol. Phenanthrone and P-phenanthrglic oxide both yield molecular com- pounds with picric acid, C,,H,,O,C,H,(NO,),OH (m. p. 185") and (C,,Hg),0,~C,H,(NO,)~0H (m. p. 148"). Phenanthrone, when in solution, is converted by aerial oxidation into the compound C,sH,sO, (obtained by another process by Japp and Klingemann), which crystallises in dark-red lamin= melting at 156-1557", This compound is broken up by acetic anhydride into phenanthrone, and phenanthraquinone, the former undergoing acetyla- tion.It may be synthesised by the direct union of phenanthrone and phenanfhraquinone. The authors regard it as an aldol condensation compound of these two substances, and ascribe to it the constitution F6H4*?(OH)* YH' ?GH4. On boiling with fuming hydriodic acid, it isCGH,* CO CO CGH, converted quantitatively into tetraphenylenef urfuran. Acetic anhydride converts phenanthrone into /I-phenanth*glic ucetate, C,,Hg*O*C,H,O (m. p. 77-78'). When heated with methylic alcohol and sulphuric acid, phenanthrone yields metlqlic /Iphenunthrylic oxide, C14H9*O*UH, (m.p. 96-91"). When heated with ammonia it yields a mixture of P-p~e.nc~ntlbryZccn2~ne,C,,H,*NH, (ni.p. 139"), and P-diphenanthrylamine, (C,,H,),NH (m. p. 237"). With phenylhydrazine at 200° it interacts, 170 eliminating water and ammonia and yielding 2' :3'-diphenyZeneindoZe (m. p. 188-189"). 105. ''The yellow colouring principles of various tannin matters. IV." By A. G. Perkin, Cape sumach, the leaves of the Colpoon compressunt, is used in South Africa as a substitute for sumach (Rhus Co~icc~icc)under the name of "Pruim-bast." According to H. Procter (private communication) it contains 23 per cent. of a catechol tannin, Its dyeing property is due to the presence of a new glucoside, os?/rits.in, C27H30017,pale yellow needles, m.p. 185O, which is decomposed by acid into quercetin and glucose, C,7H,,0,7 +2H,O =Cj,,H,,07 +2C,Hl2O,. This is not identical with viola-quercetrin (Mandelin, J., 1883, 1369), C,2H,202, which exists in the YioZct ts.icoZorJoyensis, The tannin, obtained as an orange-coloured, transparent mass, is a glucoside yielding, with acid, an anhydride or phlobophane and a sugar. By fusion with alkali, protocatechuic acid is formed. A re-examination of gambier catechu (Ungui-icu Gambier) corroborated the statement of Lowe (Zeit.anal. Chem., 1874, 12, 127) that this contains quercetin. Acacia catechu not previously examined was found to contain the same colouring matter. The dyeing properties of a commercial sample of Venetian sumach (22.Cotinus) are due to myricetin and not quercetin a8 stated by Lome (loc. cit.). This result will be corroborated by the examination of a specially picked sample. Valonia (Quercus &gilops), divi-divi (Ca?sccZ@nuCoyiuria),myrabolans (Termincdicc chebukc), agarobilla (Cmsulpina breuifoliu), pomegranate rind (Puniccc yrccnatum), and gall-nuts (Quercus infectoriu), owe their tiactorial property to ellagic acid, and contain no member of the quercetin group. It is here pointed out that the plants examined hitherto contain, respectively, a tannin and colouring matter which yield on decomposition identical acids, and in some cases the same phenol.106. Ammonia and phenylhy drazine derivatives of ap-dibenzoylcin-namene (anhydracetophenonebenzil)." By Francis R. Japp, F.R.S., and Alfred Tingle, B.Sc. By oxidising dibenzoylcinnamenimide, C22H17N0-the first product of the action of ammonia on dibenzoylcinnamene-- with chromium trioxide, the authors have obtained a mixture of dibenxamide, benx- untide, and regenerated dibenxoylcinnamene. 171 By reducing dibenzoylcinnamenimide with zinc dust and acetic acid in the cold, A. Smith's tYiphenyZpyl.rhoZe, C6H5*1;1-EH , melting at C,H,* C C*C,H5 \/~H 140-141' (Trans,, 1890, 57,645), is formed. The authors discuss the various reactions of dibenzoyicinnamene and dibenzoylcinnamenimide, and ascribe to these compounds the formulae C6H,*C=CHI C6H,*C=CH NH It seems to be impossible to assign to dibenzoylcinnamenimide, for example, any other formula which will account for the formation of dibenzamide during oxidation.By the oxidation of triphenylpyrrholone-t he transformation pro- duct of dibenzoylcinnamenimide under the influence of heat-with chromium trioxide, the authors have obtained a compound which they regard as trzphe~yll~ydroxypyrrhoZone(m. p. 168") : or one of ihs possible tautomeric forms. Heated with caustic potash, this compound evolves ammonia, and yields a mixture of benzilic and benzoic acids. The authors have also studied the destructive distillation of the compound CZ8H,,N,(m. p. about 230°), obtained by Japp and Huntly (Trans., 1888, 53,184) by the action of phenylhydrazine on diben-zoylcinnamene.They find that it yields the 1:3 :4-triphen$pyraxole obtained by A. Smith (Annalen, 1896, 289, 332) by the destructive distillation of tetraphenyldihydro-1 :2-diazine. They point out that result renders it very improbable that the compoun,d C28H22N2 has the constitution of an anilidotriphenylpyrrhole, ascribed to it by Japp and Klingemann (Trans., 1890, 5'7, 671). 107. 66Derivativesof cotoin and phloretin." By A. G. Perkin and H.W. Martin. A study of the acetylisation of the diazobenzene derivatives of cotoin and phloretin. Cotoin, C14H1,0,, a constituent of coto-bark, is, according to Uiamician and Silber, a monomethyl ether of benzoylphloroglucinol, C,H,(OCH3)(OH),*~O-c6H5(Bey., 1894,%', 409).Cotoinuxobenxene, C14Hl,04*C,H5N,,forms orange-yellow needles, m. p. 183-1840. m.Cotoin-nzo-o-toluene, C,4Hl104*C~,*C,H4~2,p. 203-204", and cotoin-axop-toluene, m. p. 207--208", crystallise similarly. Biaoetyl-uxo-benzene cotoin, C1,H,O4(C,H,O),*CGH5~,,crystallises in scarlet needles, m. p. 155-156". As with the maclurin compound (Trans., 1897, 71, 186), the acetyl-groups could be determined by Liebermann's method. Pldoretin, C15H1405,occurs in the root bark of the apple tree as a glucoside phloridzin. According to Ciamician and Silber, it, has the constitution C,H,( OH), co*CH(CH,) 'C6H4 OH. Phlo?.etin-di.saxo-benzene, C15H1205(C6H5N2)2, needles, m. p. 254-256", phloi*etin-red disaxo-o-toluene, m.p. 250-25 lo, and phloretindisaxo-p-toluene,m. p. 250-251°, closely resemble the corresponding maclurin derivatives. Acetyl phloretindisuxobenxene, C15H,,0,(C,H,0)(C,H,N,), forms orange-red needles melting at 217-219". No higher acetyl derivative could be obtained. Comparing this result with those previously obtained with maclurin and phloroglucinoldisazobenzenes (Trans., 1.897,71, 186), it would thus appear that phloretin contains only three hydroxyl groups. From Ciamician and Silber's work there appears to be no doubt, however, as to the correctness of their constitution for phloretin (loc. cit.). Thus, all hydroxyls in the phloroglucinol nucleus of phloretin must in diazobenzenephloretin be in the ketonic form, a peculiarity which in some way is therefore due to the influence of the phloretol group. 108.IL Azobenzene derivatives of phloroglucinol." By A. G,Perkin. Though phloroglucinol is known to yield azo- and disazo-derivatives as phloroglucinol-p-azobenzene sulphonic acid, CGH,0,*K,*CGH4*S0,H (Stebbins, Am. Ciiem. SOC.J.,1880,2,240), and disazobenzenephloroglu- ainol, C,H*O,(N,*CGHs)2(Weselsky and Benedikt, Ber., 1879, 12,226), no trisszo-compounds have been previously obtained, though judging from its constitution the formation of such should be expected. ~l~loroglucinoltrisuzoben~ene,C6H30,(CGH5N2)3,fine needles possess- ing a green iridescence which do not melt below 300", is formed by addition of diazobenzene sulphate to a solut.ion of phloroglucinol in aqueous sodium carbonate.Its production is independent of the amount of diazobenzene sulphate employed. It contains no free hydroxyl groups, being insoluble in alkaline solutions. P~loroglucinol-o-trisu~oun~solis prepared from phloroglucinol and o-diazoanisol in either sodium carbonate or acetate solution. No corresponding disazo-compound could be obtained in this manner. It forms maroon coloured needles melting above 300°, insoluble in alka- line solutions. Pl~ZorogZucinoZ-disccxobenxene-m-ccxonit~obenzene,obtained from phloro- glucinol-disazobenzene and nz-diazonitrobenzene, forms dull red needles, In. p. 290O. It is proposed to study the reaction of other substituted diazoben- zenes with phloroglucinol under similar conditions. 109.The action of phosphorus pentachloride on fenchone.” By J. Addyman Gardner, M.A., and G. B.Cockburn,B.A. Fenchone is acted on at the ordinary temperature very much more slowly than camphor, and the products of the action are different, for on pouring into water to get rid of the excess of phosphorus penta- chloride and oxychloride, the authors obtained a crystalline compound of the formula C,,H,,ClPO(OH),, which they name chlorofenchone- phosphoric acid, and an oil consisting of unchanged fenchone and a substance containing chlorine, probably chlorofenchone. Chlorofenchone phosphonic acid is a white, crystalline solid, melting at 196’. It is very soluble in ether, alcohol, chloroform, and benzene, but more sparingly soluble in water.It is a dibnsic acid, and the sodium salt crystallises in white, needle-shaped crystals. The lead, barium, and copper salts are insoluble in water. The oil containing chlorine is at present under investigation. 110. “Ketolactonic acid and its homologues,” By C. H. G. Sprankling, B,Sc,, In 1882, Young (Trans., 1883,43,172) observed that when P-et,byl- acetosuccinic ether is slowly distilled, a little alcohol is liberat,e 1 and on hydrolysis of the distillate with hydrochloric acid a crystalline acid, C,H,,O,, is formed in addition to a-ethyl-P-acetopropionicacid and a small quantity of ethylsuccinic acid. The barium salt, Ba(C,H,O,),, is obtained by the action of barium carbonate; a cold solution of barium hydrate gives the salt of P-ethyl-acetosuccinic acid, whilst at 100’ barium carbonate is precipitated and the salt of a-ethyl-P-acetopropionic acid is formed.From its composition, method of formation and beliaviour it was concluded that the crystalline acid, to which the name ketolactonic YO,H7 C*Meacid mas given, has the constitution Et*yH 1 co--0 174 At Prof. Young's suggestion, these experiments have been repeated and a much larger yield of the crystalline acid has been obtained by prolonged heating of the P-ethylacetosuccinic ether before hydrolysis. The lower homologues of the acid have also been prepared in ft pure state from acetosuccinic ether and P-methylacetosuccinic ether re- spectively, and it has been found that by prolonged heating of p-iso- propylacetosuccinic ether and subsequent hydrolysis with hydrochloric acid a very small quantity of the higher homologue is formed.It is thus shown that the crystalline acid obtained by Young is the third member of a series to which the general name ketolactonic acid may conveniently be given. It will be necessary, however, to call the lowest member of the series ketolactonic acid, the others being named methyl, ethyl, isopropylketolactonic acid. Ketolactonic acid, C6H604 does not crystallise ;methyl-ketolactonic acid, like the ethyl compound, forms colourless crystals, m. p. 176"-The barium salts corresponding to those derived from the ethyl compound were prepared from ketolactonic acid and methyl-ketolactonic acid. The rate of action of sodacetoacetic ether on the brominated fatty ethereal salts, the rate of elimination of ethyl alcohol from the /3-alkyl- acetosuccinic ethers, and the rate of hydrolysis of the ethers differ greatly in the four cases examined, the rate in general diminishing rapidly with rise of molecular weight.The hydrolysis of the P-alkylacetosuccinic ethers may take place in two ways-(a) the acetyl group is replaced by hydrogen and an alkyl- succinic acid is formed; (b) carbon dioxide is evolved and an a-alkyl- P-acetopropionic acid formed. With the ethers investigated, the higher the molecular weight of the alkyl group the larger is the relative yield of the alkyl succinic acid. November 4th, 1897. Professor Dewar, F.R.S., President, in the Chair.Messrs. Harold W. Harrie, W. X.Lang, W. H. Barlow, and A. Y. C. Fenby were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Meesrs. Ernest George Annis, Health Office, Town Hall, Huddersfield ; William Ball, 54,Stretton Road, Leicester ;Richard Oxley Burland, J.P., Poolstock House, Wigan ; Alexander McLean Cameron, Day lesford, Victoria ; Owen Aly Clark, 12, Abbey Gate Street, Burg St. Edmunds; Alexander Clarkson, 2, Wnveney Crescent, Ballymena, Ireland ;Frank Uolling- ridge, B.Sc., Kenmore, Shepherd's Hill, Highgate, N. ; James Murray 175 Crofts, B.A ., Richleigh, Gloucester ; David Crole, Primrose Studios, Wellington Square, Chelsea, S.W. ; John Daniell, Council of Educa- tion Laboratory, Johannesburg, S.A.R.;Andrew James Dixon, Dapto, N.S.W. ; Robert Hamilton, 11, Ibrox Place, Glasgow ; John Harger, B.Sc., Ph.D., The Nook, St. James’s Nount, Liverpool; Charles Kelly, Oakmere, Hawarden, Cheshire; Tom Lemmey, B.A., Wellington College, Berks ; James Scott Maclaurin, D.Sc., Mount Eden, Auckland, N.Z. ; Allen Macmullen, 82, James Street, Dublin ; Edward Masters, The Aloes, Hinckley Road, Leicester ;John A. Mathews, 4, First Place, Brooklyn, N.Y. ; Philip George Gregory Moon, 129, Rosary Road, Thorpe, Norwich ; Joseph John Mooney, 34, Easter Road, Edinburgh ; James Charles Philip, B.Sc., Ph.D., 16~,Merton Road, Victoria Road, Kensington, W. ; Alexander Ferguson Reid, Stair Bridge, Stair, Ayrshire; Ernest Henry Roberts, Hollydale, Allfarth- ing Lane, Wandsworth, S.W.; Edward Sydney Simpson, 34, Pier Street, Perth, West Australia; Robert Francis Woodsmith, 89, Bwrtholomew Close, E.C.; Frederick William Steel, Tamunua, Navua River, Fiji; Michael Edmund Stephens, Avenue House, Finchley, N. ; George Stubbs, Arnside, Hertford Road, East Finchley, N.; Edward Howard Tripp, Ph.D., Kent House, Blackheath Hill, S.E. ; John Scriven Turner, 20, Bury Street, Bloomsbury, W.C. ; Framjee Khurshedjee Viccajee, Hyderabad, Deccan, India ; Percy John Tinter, Wesley College, Sheffield ; Arthur James White, Whinsfield, Barrow- in-Furness. Sir WILLIAM then took the Chair, and of the following CROOKES papers those marked * were read :-“111. (‘On the properties of liquid fluorine.” By Professors Moissan and Dewar.The nearest approach to the properties of the mythical alkahest or universal solvent of the alchemist is to be met with in fluorine. The transparent vessels in which it can be manipulated have to be made of some fluoride like fluor-spar, and such vessels are equally difficult to construct and ill-adapted for chemical manipulation. Modern research has, however, revealed the fact that the most powerful chemical affinities are completely suspended by allowing substances to come into contact at very low temperatures, and it appeared possible that even fluorine, which has the most powerful chemical activity of all the elements, might be manipulated in glass vessels under such conditions, In a paper communicated to this Society entitled “The Lique- faction of Air and Research at Low Temperatures” (Proc., 1895, 176 11, 221) speaking of fluorine, the author remarked, "This is the only widely-distributed element that has not been liquefied.Some years ago, Wallach and Hensler pointed out that an examination of the boiling points of substituted halogen organic compounds led 'to the conclusion that, although the atomic weight of fluorine is nineteen times that of hydrogen, yet it must in the free state approach hydrogen in volatility. This view is confirmed by the specific refractive index, which Gladstone showed was rather lower than hydrogen. If the chemical energy of fluorine at low temperatures is abolished like that of other active substances, then some kind of glass or other trans- parent material not so brittle as calcium fluoride could be employed in the form of a tube, and its liquefaction achieved by the use of hydrogen as a cooling agent." The inference that fluorine approached hydrogen in volatility was deduced by Wallach and Hensler from a consideration of the boiling points of the fluorine derivatives of the benzene series.The following table :-I. Be~mue. Boilingpoint. Differ-ence. Toluene. Boiliiig point. Differ-ence. CGH6 ............ C6H,CH, ........... CGH5F1 ........ p-C6H4F1.CH, ...... CGH,Cl.. .......... 132'1 p-C6H4Cl* CH,. ..... 160°1 Aniline. ....CGH5NH2 p-C6H,F1*NH, . . 7830\ lS7"\ 40 430 Benzene. ..............CcH6 .........p-CGH,F12 '*') ""I 80 84" p-C,H4C1*NH2..230°J p-C,H,Cl, ......... 172OJ shows that the substitution of 1 atom of hydrogen in these compounds by fluorine only causes an increase of the boiling point of from 4" to 5", whereas chlorine causes an increase of from 45" to 50". Such a relatively large ratio as 1 to 10 in the increment of boiling poihts suggests a great difference in the volatility of the elements fluorine and chlorine in the free state. A further examination of the properties of fluorine compounds, however, showed that the volatility of fluorine was not likely to approach that of hydrogen. This mill be apparent from the following table :- 177 11. Boiling Boilingpoint point Methane. (absolute). Difference. Ethane.(absolute). Differcnco. CH, ......... 110") C,H, ...... 184'1 90" 58" CH3F1 ...... 200" C,H,Fl.. . 242") 50" 44"1CH,Cl ........ 250" C,H,CI ... 2863 CH, ......... 110" C*H,. ..... 110"~ 149"= 4 x 37" 241"= 4 x 60" CFJ, ......... 259" C*Cl,...... 35 io Aldehyde. R.p. (C.) Kenzaldehy de. 13.p. (C.)C,H,COH 179" --11° -18" CH3COFl ... 10") C,H,COFl 161" 41" 38" CH,COCl ... 51' CGHSCOCl. 199" where it is seen that the substitution of hydrogen by fluorine in methane and ethane raises the boiling point by 90" and 60" respectively, and that the ratio of the increments of boiling point in corresponding fluorine and chlorine compounds is now not greater than 1 :2. The boiling point of methyl fluoride was calculated from the critical point and vapour pressure of this substance as recorded by Professor Collie (Trans., 1889, 55, 110).It will be noted as a curious fact that the substitution of fluorine in the aldehyde radicle causes a lowering of the boiling point and not an increase, and that the difference in boiling point between the chlorine and fluorine substitution body in either series is always between 40" and 50". These considera- tions induced the hope that liquid air might give the command of a sufficiently low temperature for the liquefaction of fluorine, and that glass vessels might be used to collect the liquid. This view was sup- ported by a consideration of the melting points of the halogensland the corresponding critical points deduced by following the suggestions of Clarke (Am.Chem. Xoc. J.,1896, 18, 618), as to these relations. Thus the absolute melting points of chlorine, bromine, and iodine are respec- tively 171", 267", and 388", and, assuming the same mean difference in melting point extended to fluorine, then its melting point would be 64" absolute. Now the critical points of chlorine and bromine are about 2Q times the absolute melting points, thus giving 149" absolute, or -125", as the probable critical point of fluorine. This critical value is only a few degrees lower thaq oxygen, and from this calculation the authors were entitled to assume that the position of fluorine as regards volatility would be somewhere between that of oxygen and nitrogen. 178 The following research was conducted in the Chemical Laboratory of the Royal Institution, to which Professor Moissan brought the appa- ratus for the production of gaseous fluorine with which his name mill always be identified, and the authors had the invaluable assistance of Messrs.Lebeau, Lennox, and Heath in the conduct of the experiments. Fluorine was prepared by the electrolysis of potassium fluoride in solution in anhydrous hydrofluoric acid. The fluorine gas was freed from vapours of hydrofluoric acid by being passed through a serpentine of platinum cooled by a mixture of solid carbonic acid and alcohol. Two platinum tubes filled with perfectly dry sodium fluoride completed the purification. The apparatus used for liquefying the gas consisted of a small cylinder of thin glass, to the upper part of which was fused a platinum tube.This latter contained in its axis another smaller tube, likewise of platinum. The gas to be liquefied enters by the annular space, passes through the glass envelope, and escapes through the small inner tube. The glass envelope was fused to the platinum tube by which the fluorine was supplied. The glass cylinder being cooled down to the temperature of boiling liquid oxygen (-183O), the current of fluorine gas passed through the bulb without becoming liquid. At this low temperature, however, the gas has lost its chemical activity, and no longer attacks the glass. On lowering the temperature of the liquid oxygen by exhaustion, a yellow liquid is seen collecting in the glass envelope, while gas no longer escapes from the apparatus.At this moment the tube by which the gas had been escaping is stopped, so as to prevent air from entering and liquefying, and the glass bulb soon becomes full of a clear yellow liquid, possessed of great mobility. The colour of this liquid is the same as that of fluorine gas when examined in a stratum one metre thick. Fluorine thus becomcs liquid, according to this experiment, at about -l85O. When the bulb containing the liquid fluorine is lifted above the surface of the liquid oxygen, the yellow liquid begins to boil with an abundant disengagement of gas, having all the energetic reactions of fluorine. Silicon, boron, carbon, sulphur, phosphorus, and reduced iron, cooled in liquid oxygen and then placed in an atmosphere of fluorine, did not become incandescent.At this low temperature, fluorine did not dis- place iodine from iodides. However, its chemical energy is still suffi- ciently great to decompose benzene or oil of turpentine with in- candescence. It would thus seem that the powerful affinity of fluorine for hydrogen is the last to disappear. The authors have noticed on some occasions that a current of fluorine gas passed into liquid oxygen gives a flocculent precipitate of a white colour, which quickly settles 179 to the bottom. If this mixture is shaken and thrown on a filter, the substance can be collected. It possesses the curious property of de- flagrating with violence as soon as the temperature rises.A new apparatus (Fig. 1) was constructed similar to that already described (that is to say, a glass bulb, E, fused to a platinum tube, A, which contained another similar smaller tube, D) but having each of the platinum tubes, B and C, fitted with a screw valve, in such a man- ner that at any moment communication-either with the outer air or with the current of fluorine-could be interrupted. This little apparatus was placed in a cylindrical glass vacuum vessel containing liquid oxygen, connected with a vacuum pump and manometer. On repeating the former experiment with freshly prepared liquid air, instead of oxygen, fluorine easily becomes liquid at -190' C. With liquid oxygen as refrigerant, the liquefaction of fluorine takes place at a temperature corresponding to the evaporation of the oxygen under a pressure of 437 mm.of mercury. From these two experiments it results that the boiling point of fluorine is very close to -187'. This number is identical with Olszewski's boiling point of argon, so that this seems to be the first ex-ample of two gaseous elements boiling at the same temperature. It is a justifiable inference from the boiling point that the critical point must be about -120°, and thus, in all probability, the critical pres- sure is about 40 atmospheres, or less than half that of the critical pressure of chlorine, which is 84 atmospheres. This would make the critical constant for fluorine 4 as cont.rasted with chlorine, which has the value 5.The following table gives the boiling points of the halogens : Absolute Differ-temperature. ence. Fluorine.. .......... s70} 153" Chlorine............ '*''1 970 Bromine............ 337' Iodine .............. 460' When the little glass bulb was three-quarters full of liquid fluorine, both the valves were closed, and then a good air pump caused the liquid oxygen serving as refrigerant to boil rapidly at a pressure of 2.5 cm. Under these conditions, a temperature of -210' is reached, yet the fluorine did not show any sign of solidification, but retained its characteristic mobility. In future experiments it will be interesting to try the rapid ebullition of the liquid fluorine itself. During the repetition of this experiment, a slight accident occurred.The screw of one of the valves becoming worn, allowed air to leak into the exhausted bulb. This air was immediately liquefied, and in a few moments two distinct layers of liquid were seen ; the upper, colourless layer consisted of liquid air ; the lower one, of a pale yellow colour, being fluorine. To prevent the possible ingress of any air, the fluorine was intro- duced in its liquid state into a glass tube, the end of which was then sealed before the blow-pipe. The sealed tube, containing the liquid fluorine, was kept for a long time at -210" by the rapid evaporation of a large quantity of liquid air, but it gave no trace of a solid body. To determine the density of liquid fluorine, it was brought into contact with a number of bodies whose density is known, comparing their behaviour at the same time in liquid oxygen, which has about the same boiling point and density.By taking groups of bodies whose densities are very close to each other, it is easy to see which sink and which float in the liquid. This well-known though indirect method was the most suitable for these delicate experiments. The authors first satisfied themselves that the fluorine had no action on the materials used. To effect this, a crystal of ammonium thiocyanate (density= 1.31) was placed in a glass tube surrounded with boiling liquid air to the bottom of the tube, a current of fluorine gas was introduced by means of a platinum jet. The fluorine was rapidly liquefied, and the am- monium thiocyanate wa.s not attacked.The same experiment was repeated with a fragment of ebonite (d = 1-15),of caoutchouc (d = 0*99), of wood (d= 0*96),of amber (d = 1-11>,and of methyl oxalate (a?= 1.15). It is of importance, in the experiments just mentioned, that the various materiaIs used should be first kept at. a temperature of -190" for some little time before coming in contact with liquid fluorine. In one of the experiments a piece of caoutchouc, having been insuffi- ciently cooled, took fire on the surface of the liquid, and burnt com-pletely away with a brilliant flame without leaving any residue of carbon. The piece of caoutchouc ran about the surface of the liquid like sodium on water, giving a very intense light.The density experiment was carried out in the following manner :-In a glass tube closed at one end, and of which the lower part had been slightly drawn out, fragments of the five substances just men- tioned were placed. The tube was then plunged to a third of its length into boiling liquid air. When it was all reduced to a tempern-ture of about -290' the fluorine gas was carefully introduced. This soon liquefied, and the wood and the caoutchouc floated easily on the surface of the pale yellow liquid. On the other hand, the methyl oxalate and ebonite remained at the bottom, while the amber 181 rose and fell in the liquid, appearing to be of the same density. The apparatus was shaken several times, and the quantity of liquid fluorine increased, but the results were the same.The authors thus arrive at the conclusion from these experiments that the density of liquid fluorine is about 1-14. Another point which appears to be of interest is the following. The fragment of amber floating in the fluorine was very difficult to distinguish, which would seem to indicate that the index of refraction of liquid fluorine is in any case greater than that of liquid air or oxygen, although it is not likely to be so high as that of amber itself. Fluorine was liquefied in a thick-walled glass tube which had been previously graduated, and the tube sealed. On cooling the tube and its contents to --210°, a contraction of ?=th in the volume of the liquid fluorine took place.A similar tube was left alone in a vacuum vessel full of liquid air. An hour and a half afterwards, the tube still being in liquid air, the fluorine had not changed in appearance. But shortly afterwards, when the air had all evaporated, a violent detonation occurred ;the sealed tube and the double beaker in which it had been placed were smashed and reduced to powder. Different samples of liquid fluorine examined with the spectroscope through a thickness of about 2~cm. showed no specific absorption-bands in the visible spectrum. Liquid fluorine placed between the poles of a powerful electro- magnet does not show any magnetic phenomena. These experiments are the more decisive, as comparative ones with liquid oxygen were made at the same time, The capillary constant of fluorine is smaller than that of liquid oxygen.A capillary tube, plunged successively in fluorine, oxygen, alcohol, and water, gave the following figures : Height of liquid fluorine ............... 3.5 mm. 9) ,, oxygen ............... 5.0 ,, 9, alcohol........................ 14.0 ,, 9) water ........................ 22.0 ,, Liquid fluorine placed in cz glass tube surrounded with liquid air (temperature about -190" C.) had a slow current of hydrogen gas directed on to its surface by means of a fine platinum jet. There was immediate combustion with the production of flame. The experiment was repeated by dipping the platinum jet well below the surface of the liquid. At this temperature complete combination still took place, with a con-siderable evolution of light and heat.Oil of turpentine, in the solid state, is attacked by liquid fluorine. To perform this experiment a little oil of turpentine was placed at the bottom of a glass tube surrounded with boiling liquid air. As soon as 182 a small quantity of fluorine was liquefied on the surface of the solid, combination took place with explosive force, a brilliant flash of light, and deposition of carbon. After each explosion, the current of fluorine gas was kept up slowly, a fresh quantity of liquid fluorine was formed, and the detonations succeeded each other at intervals of from 6-7 minutes. Finally, after a longer interval of about 9 minutes, the quantity of fluorine formed was sufficient to cause, at the moment of the reaction, the complete destruction of the apparatus.In several of these experiments a little liquid fluorine accidentally fell on the floor ; the wood instantly took fire. The action of liquid oxygen has been studied with more care, since the authors observed that by passing a current of fluorine through liquid oxygen, a detonating body could be produced. If a current of fluorine is directed to the surface of liquid oxygen in a glass tube, the temperature being about -190°, the fluorine dis- solves in all proportions, imparting a yellowish colour, and giving the liquid a graded tint from the upper to the lower part ; the bottom of the tube is hardly coloured. If on the contrary, the fluorine gas is introduced at the bottom of the liquid oxygen, the yellow colour is produced at the bottom and diffuses slowly to t8he upper layers.This phenomenon indicates that the densities of liquid fluorine and oxygen are very near each other. When the temperature of the mixture of liquid oxygen and fluorine is allowed to rise slowly, the oxygen evaporates first. The liquid becomes more and more concen- trated as regards fluorine, and finally the latter begins to boil in its turn. In fact, at the commencement of this boiling the gas coming off will light a match which has only n, red-hot point, and will not make lamp-black or silicon red-hot ; but, on the other hand, the gas coming off at the end of the experiment will instantly cause these two latter bodies to burst into flame.When the glass bulb is com- pletely empty and its temperature is rising, a distinct disengagement of heat is suddenly noticed, and the interior of the glass loses its polish. This rise in temperature is due to the fluorine gas attacking the glass. In this experiment, using perfectly dry oxygen, no pre-cipitate is produced. If, on the contrary, oxygen is used which has been some hours in contact with the air, the detonating substance mentioned in previous experiments is produced. The body which is produced by the action of fluorine on oxygen containing in suspension minute crystals of ice seems to be a hydrate of fluorine, decomposing, with detonation, by a simple rise of tem-perature. This view must, however, be taken as conjecture, until the real composition is ascertained.A small quantity of water at the bottom of a glass tube being cooled down to -190°, liquid fluorine formed on the surface of the ice as a mobile liquid without showing 183 any chemical action, and evaporated on the temperature rising. AS soon as the apparatus became warmer the remaining gaseous fluorine attacked the ice with great energy, causing a strong smell of ozone. A globule of mercury was treated in the same way as the water described above. The surface remaining very brilliant, the liquid fluorine surrounded it without causing any diminution of metallic lustre. On allowing the temperature to rise, the fluorine began to boil, and the liquid disappeared completely, without any attack of the mercury.The experiments seem to warrant the following conclusions. Fluorine gas is easily liquefied at the temperature of boiling atmospheric air. The boiling point of liquid fluorine is -187’. It is soluble in all proportions in liquid oxygen and in liquid air. It does not solidify at -210O. Its density is 1.14, its capillarity is less than that of liquid oxygen; it has no absorption spectrum, and it is not magnetic. Finally, at -190” it has no action on dry oxygen, water, or mer- cury, but it reacts, with incandescence, on hydrogen and oil of turpen-tine. Future experiments must decide whether cooling below -200’ can suspend the powerful chemical action of liquid fluorine on hydrogen and hydrocarbons. One of the most important questions for future investigation is the specific refractive and dispersive indices of the fluid.Davy, in his paper on the substances produced in different chemical processes on fluor-spar (I‘M.2?7*ans.,1813, 278), says, “Dr. Wollaston has found that the fluoric combinations have very low powers of refracting light, and particularly the pure fluoric acid ; so that the refracting powers of fluorine will probably be found lower than those of any other substance, and it appears to possess higher acidifying and saturating powers than either oxygen or chlorine.” Gladstone has shown that the specific atomic refraction of the com- bined element does not exceed 0.9, taking the Lorentz formula, and that the atomic dispersion diminishes instead of increasing for short wave-lengths.Further, he found that the other halogen substitution compounds gave atomic refractions nearly agreeing with the same substances in the free state. It has been found that liquid gases give the same atomic refraction as the gaseous body, so that the refractive index of liquid fluorine may be at once deduced provided it be- haves like chlorine, bromine, or iodine. Taking 0.9 as the atomic refraction, the value would be, according to the Gladstone formula, 1,054,and the Lorentz, 1.081. Both values are far lower than those of liquid oxygen or air, 1-226 and 1.205 respectively. The general appearance of the liquid and the experiment with amber described above lead to the conclusion that liquid fluorine must have a refractive index much higher than that calculated.If the 184 refractive index is as great as 1.41, then the atomic refraction (Lorentz) will be 4.13, but if it is only about 1.192, then the atomic refraction will be 2. On both assumptions the atomicarefraction of liquid fluorine is much greater than the value 0.9 found by Gladstone. Should the smaller value 2 turn out to be the correct one then the in- ference might be fairly drawn that the critical constant was also about 3, or nearly the value for oxygen. This view would make the critical pres- sure of fluorine about the same as that of oxygen, or 50 atmospheres. Prom this it would follow that, unlike chlorine, bromine, and iodine, which have the same atomic refraction in combination and in the free state, fluorine has a different value in the one state as compared to the other.In this respect it would appear to resemble oxygen, whose atomic refraction in combination may be only three-fourths of what it is in Ihe free state. This view is confirmed by an examination of the atomic volume of fluorine. The other members of the halogen series have approximately the same atomic volume in combination as in the free state. Now, the atomic volume of fluorine in fluorbenzene is 11.5, or about half the atomic volume of chlorine, or taking chloro- benzene as standard, with chlorine as 22.7, then the atomic volume would be 10. The value for the free element appears to be 16.6, and the number deduced from liquid hydrofluoric acid about 15.Many metallic fluorides have relatively small atomic volumes. Thus the fluorides of cadmium, lithium, calcium, magnesium, and aluminium have an atomic volume just about half of that of the corresponding chloride. This difference is, however, easily explained if fluorine in the combined state has only half the atomic volume of chlorine. Dr. Thorpe’s value for the atomic volume of fluorine, deduced from a study of the chloride and fluoride of arsenic, is 9.2, or free fluorine at its boiling point ought to have a density of 2, provided it behaved like the other halogens. This density for the free element is much too high, the experimental value being about 1.14. Such changes in atomic volume again suggest a resemblance with oxygen, and would lead to the inference that the refractive constants must also differ in the free and combined states.These interesting pro- blems must, however, be left for future investigation. DISCUSSION. Dr. PERKINsaid he felt muchinterested in the paper, because of the remarkable magnetic rotation of combined fluorine, for example, in fluortenzene. When one atom of hydrogen in benzene is displaced by chlorine, the rotation is considerably increased. The substitution of bromine causes a still higher rotation, and that of iodine the highest. On the other hand, the substitutioc of fluorine reduces the magnetic rotation. He had suggested that this might be accounted for if fluorine were paramagnetic, because its megnetic rotation would then be the reverse of that of carbon and hydrogen.This, however, does not seem to be a probable explanation, since it is now found that liquid fluorine is not paramagnetic. It is possible that this element may have different values depending on whether it is free or com-bined. The nitro-group (NO,) influences magnetic rotation much in the same way as fluorine. Dr. GLADSTONEremarked on the importance of Professor Dewar’s communication, the most interesting portion to him being that on the optical properties of the liquid fluorine. The specific refraction oE that element had been calculated by him and his brother from fluorbenzene and from many salts, crystallised or in solution, with the invariable result that it was exceedingly small.In the last list of the specific refractions of the elements (Yvoc. R.X.,1897, 60,141) it is given at only 0.031, which is not a third of the next lowest in the list. Its specific dispersion is also low, and it has the additional peculiarity of giving a reversed spectrum. Now Prof. Uewar finds that liquid fluorine has about the same refractive index as that of amber ;this is known to be 1.55 or thereabouts. As the specific gravity of the fluorine is stated to have been 1.14, we can easily calculate the specific refraction, viz., 0.482. This figure, instead of being the lowest in the list of elements, is nearly the highest, there being only six with higher values. It is true that in some cases the specific refraction of an element in the free state differs somewhat From that deduced from its compounds.Fluorine would naturally be compared with the three halogens, chlorine, bromine, and iodine. Liquid chlorine bas a specific refraction of about 0.27 ;in combination 0.28. Bromine has a specific refraction of about 0.20 ;in combination 0.21. Iodine vapour has a specific refraction of about 0.19 ; in combination 0.21. The free element, therefore, does not differ widely in specific refraction from the same element when in com- bination; and in each case is the smaller and not the greater of the two. A certain analogy does exist between fluorine and sulphur or phosphorus. These two when melted have high specific refractions, sulphur being 0.50, and phosphorus 0.59 ;these high figures are gene- rally much reduced when the elements are in combination, but the extent of this reduction is by no means comparable with what would appear to be the case with fluorine.Although Professor Dewar’s method is correct in principle, Dr. Gladstone expressed a strong hope that accurate determinations would be made by one or other of the more direct methods. Dr. THORPEsaid, in reference to the allusion by the President to his determination of the specific molecularvolume of fluorine as far back as 1880,that too much stress could not be laid upon the particular value viz., 9.2, which he then obtained. It was deduced from a study of the specific gravity and thermal expansion of arsenic fluoride, a substance which is not easy to obtain pure, and which is not altogether without action on glass, especially at temperatures approaching the boiling point. It, moreover, presupposes that arsenic fluoride has a molecular consti- fiient analogous to that of arsenic chloride.Such an assumption is probable, but having regard to the remarkable complexity of many fluorine compounds, as, for example, hydrogen fluoride itself, when corn pared with the corresponding chlorine compounds, the supposition can- not, at present, be regarded as more than probable. The particular value obtained, however, clearly indicated the order of the magnitude, as shown by its substantial agreement with the other values quoted by the author. With respect to the question raised by Dr.Gladstone, he might say that the peculiar behaviour of glass when immersed in arsenic fluoride mas significant, and suggested a method by which the refractivity of liquid fluorine in the free state might be ascertained with a fair ap- proximation to accuracy, viz., on the same principle as that adopted by the authors in determining the relative density of liquid fluorine- that is, by immersing solid> of known refractivity in the liquid, and observing which became invisible. Arsenic fluoride is a highly re- fractive liquid, and some specimens of glass threads and tubes become almost invisible when immersed in it. Professor DEWAR,in reply, observed that he did not intend to convey the impression that, because amber in liquid fluorine might be difficult to define clearly, it necessarily followed that the refractive index mould turn out to reach 1-55, as Dr.Gladstone seemed to infer. His present impression was that it exceeded that of liquid air, but he could go no further. No doubt the next time Professor Moissan and he had the opportunity of continuing the experiment, a direct deter- mination of the refractive index would be made. *112. “The liquefaction of air and the detection of impurities.” By Professor Dewar. In a paper on “ The relative behaviour of chemically prepared, and of atmospheric nitrogen,” read before the Society in the year 1894, it was stated that all samples of nitrogen and oxygen properly purified, are, when liquefied, clear transparent liquids, so that the solid matter which always separates when air or nitrogen or oxygen is liquefied on the large scale consists of impurities.Ordinary air, containing 4 parts of carbonic acid per 10,000 parts gave a turbid liquid from the solidification of the carbonic acid; and oxygen containing traces of APPARATUS OF FLUORINE.FOR LIQUEFACTION c PIG. 1. Apparalus for Ihe e-xaminafion oPthe least condensibie portion of Air. II II 2 I_ FIG. 2. 189 chlorine behaved in a similar manner. With the object of ascer-taining the proportion of any gas in air that is not condensable at about -210’ C. under atmospheric pressure, or is not soluble in liquid air under the same conditions, the following apparatus has been devised.A cylindrical bulb of a capacity of 101 c.c., marked B in figure, had a capillary tube sealed into it terminating in a three-way stopcock, as shown at E. The parts marked C and D consist of soda-lime and sulphuric acid tubes for removing carbonic acid and water. The stand marked G holds the large vacuum test tube into which B is inserted which holds the liquid air maintained under continuous exhaustion. As this low temperature had to be kept steady for from one to two hours, while at the same time the bulb B had to be completely covered with liquid air, it was necessary to arrange some means of keeping up the liquid air supply without disturbing the apparatus. The plan adopted is shown at H, which is a valve arrangement which can be so regulated as to suck liquid air from the large vacuum vessel A and discharge it continuously along a pipe into the vacuum test tube G, the latter being kept under good exhaustion. In working the apparatus, the tube I is connected to c?, gasometer containing 10 cubic feet of air, so that the volume of air condensed in each experiment may be observed.This was generally from 24 to 3 cubic feet. If there is a very small proportion of some substance not liyuefi-able or soluble in liquid air, then we should expect the vessel B would not fill up completely into the capillary tube. This is, however, exactly what does take place. After 40 minutes’ cooling, the vessel B and the cool part of the tube were filled with liquid. In this experi- ment some 80 litres of air were condensed, and any accumu-lated uncondensed matter must have been concentrated in the upper part of the capillary tube which had a volume of 0.5 C.C.Under the conditions, therefore, the material looked for must be less than 1 part by volume in 180,000 of air. To test the working with an uncondensable gas added to air, a volume of 10 cubic feet was taken in the gasholder and to that 500 C.C. of hydrogen were added. This is in the proportion of less than 1 in 500. Even after two hours’ cooling, the tube B could only be filled four- fifths. In order to prove that the gas accumulated in the upper part of B was hydrogen, the three-way stopcock at E was turned, and the temperature allowed to rise so that the gas was expelled from the evaporation of the liquid air and collected over mercury as shown at F.The gas thus collected was easily combustible and consisted chiefly of hydrogen. The amount of hydrogen was then reduced to 1 part in 1-,000 of air, and it wa,s found that after one and a quarter hour’s cooling the bulb B had filled to within a half C.C. of the capillary tube. A new sample of air containing 1 part of hydro- 190 gen in 10,000 of air filled the bulb B completely as if it were ordinary air. It appears from these experiments that 1 part of hydrogen in 1,000 of air is just detectable by this plan of working. As the 80 litres of air condensed contained some 80 C.C. of hydrogen, it appears that 100 C.C. of liquid air at from -200’ to -210’ C.had dissolved nearly all this gas; in fact, that 20 C.C. of hydrogen at the low temperature is dissolved in 100 C.C. of liquid air. In the paper on “ The liquefaction of air andresearch at low temperatures” (Proc., 1895, 11,221), it was shown that if hydrogen containing a small percentage of oxygen were employed for the purpose of getting a hydrogen jet, the liquid collected from it was oxygen, containing, however, so much hydrogen dissolved in it that the gas coming off for a time was explosive. In order to press this inquiry a little further, some natural gas known to contain a different constituent like helium suggested itself as being worthy of trial. Lord Rayleigh’s results of the examination of the gas from the King’s Well at Bath showed that it contained 1.2 part of helium per 1,000 volumes, so that it seemed admirably adapted for such experiments. The author has to express his thanks to the Corporation of Bath for giving permission to collect samples of the gas.The sample of gas from the Bath Spring was treated exactly in the same way as the hydrogen mixtures described above. During the liquefaction there was a marked difference in the appearance of the liquefied gas, for while the hydrogen and air mixtures gave a clear, transparent liquid, the product from the Bath gas was turbid, and the precipitate by transmitted light looked yellow-brown. This solid turns out to be of organic oiigin, probably of the petroleuni order of com-pounds. It has a very marked aromatic smell resembling such bodies.The trace of material left, gave, after treatment with concentrated nitric acid, the smell of nitrobenzene; and as its detection cannot be explained by the presence of any material of the kind in the vessels used in collecting, it must be assumed to be a normal constituent of the Bath gas. A further quantity of the Bath gas must be collected in order to confirm the presence of such bodies and to definitely make out their nature. Another peculiarity of the liquid is that, on examining it with the spectroscope, even through a thickness of 2 inches, no trace of the characteristic oxygen absorption spectrum could be detected. In all attempts to make nitrogen for liquefaction on the large scale, oxygen could always be detected in the liquid with the greatest ease by means of its absorption spectrum.After the cooling had continued for 1 hour the gas ceased to flow into the condensing vessel, and some 20 C.C. at the upper part of the glass cylinder B was filled with a gas that had not undergone liquefaction or solution. About 70 litres of the Bath gas were condensed, certainly the largest 191 quantity of this gas ever subjected to chemical examination. This was boiled off just as the hydrogen was treated in the experiments de- scribed above, and as, by accident, too much nitrogen had volatilised along with the gas, oxygen was added and the mixture sparked over alkali to get rid of the excess of nitrogen. During the sparking, the helium lines were well marked (along with others the origin of which must be-settled later), and a vacuum tube filled with the product of the sparking gave a splendid spectrum of the gas.The sample of gas directly collected from the liquid nitrogen cont’ained about 50 per cent. of helium. It is therefore possible to separate helium from a gas when it is only present to the extent of one-thousandth part by liquefaction in the manner described. From this it would appear that helium is less soluble in liquid nitrogen than hydrogen is in liquid air, and is of greater volatility than either of the constituents of air, as Professor Olszewski found (Bull. Ac. Crac., 1896, 297) by direct experiment on a pure sample of the gas sent to Cracow by Professor Kamsay with the object of liquefaction.In the author’s lecture (Proc. Roy. Inst., 1896), entitled I‘ New researches on liquid air,” the following observation occurs : ‘‘The exceptionally small refractive value observed by Lord Rayleigh in the case of helium shows that the critical pressure o€ this bocly is proportionately high. It would therefore be more difficult to liquefy than a substance having about the same critical temperature but possessing a lower critical pressure than hydrogen.” Now that it has been shown by Professor Moissan and the author that two substances like fluorine and argon, differing by 2 units in molecular weight, boil at nearly the same temperature, it seems reasonable to extend the analogy to the case of hydrogen and helium where the same difference occurs, and to suggest that they also probably have about the same volatility.If the sample of un-condensed gas resulting from the first liquefaction of the Bath gas were again treated in the same way, a much more concentrated specimen of helium could be obtained. Provided helium were wanted on a large scale, then a liquid air apparatus similar to that in use at the Royal Institution transported to Bath and worked with the gas from the King’s Well could be made to yield a good supply. With n modified form of apparatus, it will be possible to collect any residuary gas from the use, not of 3 cubic feet of air or Bath gas, but from hundreds of cubic feet of such products. This investigation will be continued with new samples, in order to see if the composition of the gases changes and to isolate the hydrocarbons. The author has to thank Mr.Lennox and Mr. Heath for able assis- tance in carrying out the experiments. 192 DISCUSSION. Sir WILLIANCROOKESsaid that a few days ago he received from Professor Dewar a tube containing some of the gas at atmospheric pres- sure. A small quantity was let into a new and completely exhausted spectrum tube, which was then re-exhausted and filled several times. On exhausting to 5 mm. pressure and passing an induction spark it showed the nitrogen spectrum brilliantly, and on intercalating a con-denser the yellow helium line was visible, but too faint to be measure- able in the large spectroscope.To remove the nitrogen, 47 C.C. were mixed in an eudiometer with an equal volume of oxygen, and sparked for about 8 hours, absorption of the products being effected by strong potash solution over the mercury. When contraction had ceased, the residual oxygen was absorbed by passing pyrogallol into the potash. The unabsorbed gas amounted to 25 C.C. This gas, dried over phos- phoric anhydride, was examined in a new spectrum tube, end on. (Tube shown in action.) It gave the heliuni line (wave-length 5875.87) brilliantly, together with the other helium lines. No argon lines could be seen. “113. “The absorption of hydrogen by palladium at high temperatures and pressures.” By Professor Dewar. One of the author’s earliest papers was entitled ‘‘The motion of n palladium plate during the formation of Graham’s hydrogenium,” The explanation of the motion together with a record of other experiments can be found in the Proc.Roy. SOC.Edin., 1868, 6, 504. A subsequent investigation by the author into the physical constants of hydrogenium appeared in the Trans. Roy. Xoc. Edin,, 1876, 2’7, 167, and had reference to the specific gravity, specific heat, and coefficient of expansion of the occluded hydrogen. These observations led to the conclusion that the specific gravity was inde- pendent of the amount of condensed gas, and had a mean value of 0.62. The specific heat, relatively to palladium, of the condensed hydrogen appeared to vary inversely as the quantity occluded, but taken relatively to successive charges was nearly constant, having the value 3.4,which is identical with that of gaseous hydrogen at constant pressure.The coefficient of cubical expansion of the alloy is about twice that of palladium, and that of the hydrogen in its compressed state not more than three times that of mercury. A later communication was made to the Philosophical Society of Cambridge (Proc., 1878,3, 207) dealingwith the thermo electric relations and electric conductivity of hydrogenium. It was shown that the potential difference of a junction of hydrogenium- palladium is at ordinary temperature nearly equal to that of an iron- copper junction, and that it increases with the temperature according to the general parabolic law ; the rate of the increase being, however, greater than iron-copper and subject to a regular variation on account of successive heatings. The formation of thermo-electric piles, and of neutral points in a wire of this substance, along with the continuous formation of thermo-electric currents through the application of a hydrogen flame mere explained.Experiments on electric resistance proved that it increases directly with the amount of hydrogen condensed in the palladium. Subsequent investigators have dealt more elaborately with the many problems suggested by hydrogenised palladium, but so far the essential facts referred to above have been confirmed. In the course of the early observations the following experiment is recorded as illustrating the absorption of hydrogen by palladium at a red heat.Take a strip of thin sheet palladium, 4 or 5 cm. loug, and about 5 mm. in breadth, clamp it firmly by the end in a suit'able support, so that the strip is free to vibrate, and insert it edgeways in the middle of a hydrogen flame, burning from a nozzle about 1 mm. in diameter. If the palladium be now depressed into the inner dark cone it immediately begins to vibrate, producing a low, musical note, If the flame be extinguished by stopping the current of hydrogen for an instant, on allowing the gas to flow, the vibration cominences again, and may be kept up without any actual flame. The motion in this position in the flame is due to the absorption of hydrogen on the cool side next the inner cone, with its attendant increase of length, producing a bending of the sheet, into the hot portion of the flame, where the hydrogen is instantly expelled from :he palladium, which is forced to return to its original position from its natural elasticity.It is now knomn that no absorption of hydrogen at atmospheric pres- sure by palladium takes place above 145' C., so that the cause of motion must originate at a comparatively low temperature. The question arises, Can palladium, under any condition of pressure, absorb hydrogen at a red heat in quantity at all comparable to what it can do at lower temperatures 1 If free hydrogen and palladium-hydrogen are compared as regards volatility, the one boils at 30' (abs.), the other at 420' (abs.), very much like two isomeric forms of the same substance.This ratio of 1:14 given (and certainly the ratio could not be made greater than 1:16, since the absolute boiling points may be taken as in the ratio of their respective critical points) we thus arrive at a hypo thetical palIadium-hydrogen critical point of 640' (abs.) or 366' C, An almost exact parallel may be drawn between 194 palladium-hydrogen in its relation to free hydrogen and iridium oxide in its relation to free oxygen. Thus liquid oxygen boils at 90' (abs.) and the tension of dissociation of iridium oxide is 1 atmo-sphere at 1423" (abs.). The ratio of the absolute boiling points of liquid oxygen and the oxygen of iridium oxide are therefore as 1 :15.9, which is almost the same value as that found above for the rela- tive volatilities ef hydrogen and palladium, In either case, the ratio of the absolute boiling points of the respective substances may be taken as approximately representing the ratio of the latent heats of transition of state.It might then be possible that palladium no longer absorbed hydrogen under any condition of pressure. The present experiments mere undertaken with the view of answering this question. The diagram (3) hhows the general arrangement of the appa-ratus most suitable for examining the behaviour of the metals like palladium, sodium, potassium, &c., towards hydrogen at high tempera- tures and pressures. A rod of palladium A weighing about 119 gms., kindly placed at my disposal by Mr.George Matthey, F.R.S., was placed in a strong steel cylinder D having.an accurately fitting conical joint,. As lithle extra space as possible was left in the cylinder, which was heated in a bath of fusible metal E. The vessel-was connected with the manometer B by a strong copper tube, Rnd the latter was similarly joined to a compressed gas cylinder €3 containing hydrogen. The apparatus, without the palladium, must be carefully tested at high pressures and temperatures. There must be no trace of a leak. An extra stop- cock at C enabled the hydrogen accumulated in the apparatus to be blown off suddenly when required, aftor the hydrogen cylinder stop- cock mas shut off. Before commencing the experiments at high temperatures, it is well to charge the apparatus to a pressure of 90 atmospheres with hydrogen and then blow off the gas and measure it.In this way the volume of hydrogen that is absorbed for every diminu- tion of the pressure of hydrogen is known. In the first experi-ments a pressure of 20 atmospheres of hydrogen in the apparatus corres- ponded to 780 c.C. of gas, measured at atmospheric pressure. When the fusible metal bath was heated to 420' and hydrogen at a pressure of 80 atmospheres introduced at starting, it fell to a pressure of 60 atmospheres in 24 minutes. Blowing off the gas instantly to get rid of accumulated impurities and again applying a pressure of 80 atmospheres of hydrogen, the pressure was reduced to 60 atmospheres in 6 minutes. When the same operations were repeated a third time, the diminution of pressure by 20 atmospheres took 16 minutes, and a fourth opera- tion required 28 minutes.In all, therefore, upwards of 3,000 C.C. of hydrogen were absorbed in less than an hour. If the palladium could be seen at about a low red heat, then during the rapid absorption of the hydrogen as described in the last experiment, the temperature must rise very considerably, and the metal, during the operation, must actually appear to grow much brighter. Calculating from the tensions of the gas, the evolutioii of heat at 300' must be about 4698 gram- units of heat per gram of hydrogen absorbed. The reverse action would take place on reducing the pressure of hydrogen in the charged palladium, After the four charges the pressure remained constant at 80 atmospheres, no more hydrogen being absorbed.The hydrogen gas outside the palladium was now suddenly blown off, the stopcock shut, and the pressure allowed to rise from the escape of gas absorbed by the palladium. In this way it was noted that a pressure of 40 atmos-pheres was reached in half an hour. The whole amount of gas that had been absorbed by the metal was found, on measurement, to be 2,980 C.C. After the first charge of hydrogen the steel cylinder mas opened and the palladium examined. It was found to have n deep rent in it extending along nearly the whole length of the rod. During the occlusion of the hydrogen the volume of the metal is increased by one-tenth, so that in the passage OF hydrogen in and out of the metal enormous strains must be produced.As the volume of the original metal is a little less than 10 c.c., it may be taken that above 300 times its volume of hydrogen had been absorbed at the tempera- ture of 420" and under a pressure of 80 atmospheres. The free space in the manometer and connections was now diminished, so that a pressure of 20 atmospheres corresponded to a volume of 300 C.C. OF hydrogen instead of 780 C.C.as above. The palladium was saturated at 360" C. under a pressure of 80 atmospheres in the manner described above, except that a very much larger number of charges of hydrogen had to be employed. After saturation, the pressure of hydrogen was slowly reduced to 25 atmospheres : it rose to 30 atmospheres from gas passing outwards from the metal, now heated up to 500" C., and finally reached 100 atmospheres; on cooling to 400' the pressure diminished from reabsorption of the hydrogen.On blowing off the gas between 400' C. and 500' C. 1,400 C.C. of free and 3,300 C.C. of combined hydrogen were found. A rod of palladium, in this way, can be quickly charged with hydrogen at about 300" C. or 400' C., and as it is only the pure gas that is occluded, this process may be used as a. rapid means of getting pure hydrogen in quantity for experimental purposes. In the next experiment, the palladium was heated to 500" C. before any hydrogen under pressure was applied. ATo absorption was observed till the pressure of hydrogen reached 60 atmospheres.On charging as before at pressures between SO atmospheres and 60 atmospheres, the metal was found to absorb 1,900 C.C. of gas. The experiment was repeated, with the difference that the charging pressure of hydrogen 197 was raised to between 120 atmospheres and 100 atmospheres, and it was found that the palladium had now occluded 3,700 C.C. of hydrogen. Thus it appears from these experiments that at 500' C. palladium can still occlude 300 times its volume of hydrogen under a pressure of 120 atmospheres. The observations on the tension of hydrogen in palladium by Troost and Hautefeuille showed that, for the same temperature, the values became constant and independent of the amount of occluded gas, only when the volume of hydrogen absorbed lay between 200 and 600 times that of the metal.Any other proportions gave variable tensions for the same temperature. The fact that 300 volumes can still be occluded at 500' C. seems to show that palladium and hydrogen, under such conditions, still follow the same laws of ab-sorption as at lower temperatures. Nothing analogous to a critical point, where no combination takes place between the metal and hydrogen, has been reached. Hoitsema published an important paper on palladium-hydrogen ten- sions in the Archives Neerlccndaises, 1896, 30, 44. In this memoir, Hoitsema gives also a series of observations on the same subject made by Roozeboom. Taking the tensions given by the latter (simply because the curve seems more regular) for the horizontal portions of the dis- sociation curves at different temperatures, and calculating a Willard Gibbs' formula, from the following data, viz., 20' C.pressure 7 mm. ; 100' C. pressure 205 xnm. ; 170' C. pressure 1467 mm., the expression results (where T is the absolute temperature) 1983.4log. p = 7.00338 --+0.237'8 log. T. T From this it follows that the latent heat of dissociation of the palla- dium-hydrogen per atom of hydrogen in gram-units is 4561 +0.2378 T. This would seem to show the latent heat of dissociation increases instead of diminishing with temperature. In other words, the heat of combination should be rather greater at higher temperatures, instead of diminishing as it must do if a point where no occlusion takes place were being approached.Thus theory and experiment would seem to agree. The best and safest method for the experimental study of the rela- tions of hydrogen and palladium at high temperatures and pressures would be to investigate the change of electrical resistance in a heated wire of the metal when subjected to different hydrogen pres- sures. The problem is, no doubt, more complicated, still interesting results must follow from such an investigation. Some of the electrical properties of hydrogen and palladium at low temperatures have been determined by Professor Fleming and the author, and the results will appear in future publications bearing on the subject. 198 The author is indebted to Mr. Robert Lennox for able assistance in the conduct of the experiments.DISCUSSION. Mr. R. J. FRISWELLasked whether the President had made any measurements of the tensile strength of the steel. He was astonished to hear of the metal standing 100 atmospheres at over 500’ C. He was asking for information, as he had been unable to obtain any data as to the strength of metals near a red heat, a point at which it must be rapidly falling away. The matter was of great interest for experi- menters using autoclaves. Engineers did not seem to have done any work on tensile strength at points above the temperatures usual in steam boilers. Prof. DEWAR,in reply to Mr. Friswell, agreed that no engineering formuls existed. The experiments were dangerous, but one had to take the risk.The metal used was Whitworth compressed steel, and the vessel was made by drilling out a solid mass. He had no data as to tensile strength, the results were desired and the risk taken. 114. “On some yellow vegetable colouring matters.” By A. G. Perkin. The Rhus rhodanthema, a tree growing to the height of 70 or 80 feet, is indigenous to northern New South Wales. The colouring matter C,,H,,O, is indentical with fisetin. A glucoside of fisetin, C36H,o0,6(C =60.18 ;H =4-45>, colourless needles, m. p. 2 15-217’, is also present ;it is decomposed with difficulty by boiling dilute acids. This closely resembles fustin, C,8H46023or C36H26014 (C =63.34 ; H =3*81),m. p. 217-219’, the fisetin glucoside of R. Cotinus (Schmid, Ber., 1886, 19, 1753), but differs from it in percentage composition.Its decomposition with acid would be closely expressed by the equa- tion C,,H,,O,, +2H20=2C,,H,,06 + C6H1406,if rhamnose or glucose are liberated by this reaction. Gallic acid was also isolated, evidently as a decomposition product of gallotannic acid contained in the wood. Berberis ortuensis, a plant resembling Berber6 vulgaris, flourishes in Cyprus. It was found to contain berberine, but no colouring matter of the mordant yellow class. The perianths surrounding the seeds of Rumex obtusqolius contain a trace of quercetin, which is interesting, as in many roots of this species methylanthraquinone derivatives also exist. It is also pointed out that the leaves and green stems of madder (Rubia tinctoh) contain a yellow colouring matter which will be examined, 115.“Naphthylureas.” By George Young,Ph.D., and Ernest Clark. The mononaphthylureas may be prepared by the action of potassium cyanate on the hydrochloride of the corresponding naphthylamine. In consequence of the rapid conversion of the mononaphthylureas into the symmetrica.1 di-naphthylureas which takes place on heating, even below the melting points of the former, the true melting points have escaped the observation of previous authors. a-Naphthylurea melts at 213-214’, at which temperature it is converted into di-a-naphthylurea, melting at 284-2S6’. P-Naphthylurea melts at 21 3-215’, and immediately forms di-P-naphthylurea, melting at 289-290’.Acetyl-a-naphthylurea, m. p. 214 -215” ; benzoyl-a-naphthylurea, m. p. 2-13-243*5’ ; acetyl-/3-naphthylurea, m. p. 202-203s50 ; benzoyl-P-naphthylurea, m. p. 219-220”. 116 “Benzoylphenylsemicarbazide.” Preliminary notice. By George Young, Ph.D., and Henry Annable. In a previous communication presented to the Society (Trans., 189’7, 71, 200), attention was drawn to the disagreement between the melting points of benzoylphenylsemicarbazide, 202-203’, as observed by Michaelis and Schmidt (Bey., 1887, 20, 1713), and 210-211” as observed by Widman (Bey.,1893, 26,945). It described the prepara- tion and examination of this substance-melting at 202-203’-and suggested the possible existence of two benzoylphenylsemicarbazides both having the constitutional formula, C,R,N(COC6H,)*NH*CO*NH,. Shortly after the publication of this paper;; Dr.Widman had the courtesy to submit a sample of his preparation for comparison. This sample had been observed by Dr. Widman to melt at 210-21 2’ ;the authors found it to melt at 211-212’. Their thermometer agreed therefore with Dr. Widman’s. A comparison of the properties of the two preparations led to exceedingly interesting results. Widmm’s benzoylphenylsemicarbazide seemed to be almost, if not quite, insoluble in boiling benzene, the melting point remaining unaffected. The authors’ benzoylphenylsemicarbazide was fairly soluble in boiling benzene, crystallising out again on cooling. Mere recry stallisation from benzene did not affect the substance, but prolonged boiling with benzene caused a gradual rise of the melting point.On the other hand, the substance was easily soluble in boiling water and crystallised out on cooling unchanged, whereas Dr. Widman’s pre- paration dissolved in boiling water with difficulty and crystallised out on cooling, with the melting point considerably lowered. These results induced the authors to undertake a thorough investigation of the formation and properties of benzoylphenylsemicarbazide. They have 200 been able to determine that the action of benzoyl chloride on phenyl- semicarbazide produces under different conditions three distinct forms of benzoylphenylsemicarbazide. These three forms melt respectively at 202-203", 205-206" and 210-211".They are each capable of conversion into either of the other two. They exhibit different and characteristic crystalline structures under the microscope. They possess different solubilities and densities. The form of highest meiting point seems incapable of solution without undergoing at least partial change into one or other of the lower melting forms, but pure solutions of these latter may be easily prepared. These solutions have no action on polarised light. The authors are at present engaged in examining the physical properties of these substances and in extend- ing the investigation to a number of other closely related compounds, in the hope of being able to determine whether they are capable of existence in two or more modifications.117. '(Sulphocamphylicacid.'' By W. H. Perkin, jun, In a previous communication (Proc., 1895, 11,23) it was shown that when the potassium salt of sulphocamphylic acid is treated with phos- phorus pentabromide, the sulphobromide, C,H,,(SO,Br) CO,H, is pro-duced, and from this substance by elimination of sulphur dioxide an acid of the formula C,H,,Br-CO,H was obtained, which, as it gives P-camphylic acid, C,Hl1CO,H, on treatment with alcoholic potash, may be called 6romodihydro-P-camphylicacid. During the course of further experiments, the corresponding cam-phylic suZphochZoride, C,H,,(SO,Cl)CO,H, has been obtained by treating the potassium salt of sulphocarnphylic acid at 0" with phosphorus pentachloride. This substance melts at 168-170°, and at the same time slowly undergoes decomposition with evolution of sulphur dioxide and formation of chZoi.dihydro-P-cccmphyZicacid, a crystalline substance which melts at 105-106".Like the corresponding bromo-compound, it is decomposed by boiling with alcoholic potash, with elimination .of hydrogen chloride and forma- tion of P-camphylic acid. In the last communication on sulphocamphylic acid (Proc., 1896, 12, 189) it was stated that, when /I-camphylic acid was treated with phosphorus trichloride, and the product distilled under reduced pres- sure, the chloride of an acid melting at 130' is obtained which was called iso-P-camphylic acid, because at the time it was thought that this acid might prove to be isomeric with P-camphylic acid.It has since been found that the reaction does not proceed in this way, but that the following much more remarkable change takes place. When the chloride of P-csmphylic acid is distilled, there is, as already men- 201 tioned, some decomposition and charring, and during this distillation the chloride is yeduced almost completely to the chloride of an acid, C,H,,O,, which on investigation has been found to be identical with isolauronolic acid, the acid which Koenigs and Hoerlin (Bey., 1893, 26,813), and the author (Proc., 1893,9, 109) obtained by the elimina- tion of sulphuric acid from sulphocamphylic acid. This same isolauronolic acid (together with a liquid acid, which is possibly an isomeride) is obtained when P-camphylic acid is reduced with sodium amalgam under certain conditions, and quite lately it has also been obtained in large quantity by fusing sulphocamphylic acid with soda in a cast-iron pot.When fused in a nickel dish with caustic soda, sulphocamphylic acid yields a mixture of a-and j3-camphylic acids, C,H,,02, but when an iron pot is used, the iron acts as a reducing agent, and the product, which is found to contain quantities of ferric oxide, on treatment in the usual way yields large quantities of isolauronolic acid, C,H,,O,. Isolauronolic acid is, as Koenigs and Meyer (Bey., 1894, 27, 3466) showed, readily oxidised to isolauronic acid, CgH120:I,a ketonic acid which gives a well characterised oxime and a semicarbazide. On reduction with sodium amalgam, the author finds that isolauronic acid is readily converted into dihydvoisoluuronic acid, C,H,,O, (m.p. 8S0), a result differing somewhat from that of Eoenigs and Meyer, who obtained in this way a lactone, C9H1402,melting at 47-50°, together with a substance melting at 80--81°, which they consider to be a mixture of two acids, C,H,,O, and C,Hl,O,. The author has further studied the action of oxidising agents on isolauronic acid, and finds that, under certain conditions, this acid is split up into dimethylsuccinic acid, COOH. C(CH,),* CH,*COOH and a ketonic acid, C,H,,O,, which melts at 51'. This ketonic acid on oxidation is converted into aa-dimethylglutaric acid, CO,H* C(CH,),*CH,*CH,*CO,H, and it therefore evidently has andthe constitution CH3*CO*C(CH3),*CH,*CH2*C0,H,is identical with the acid previously obtained (Proc., 1896, 12, 190), by oxidising P-camphylic acid.A careful study of the results obtained in this long series of ex- periments on sulphocamphylic acid and the acids derived from it, seems to the author to clearly indicate that the constitutions of isolauronolic and isolauronic acids are most probably represented by the following formuis. 202 CH3 CH, CH3 I \/ I CH2--U-------C102H CO-c-Isolauronolic acid. Isolauronic acid. As sulphocamphylic acid on heating is resolved into isolauronolic acid and sulphuric acid, and on the other hand, isolauronolic acid, as was indicated in a previous communication (Proc., 1893, 9, 109) and has since been proved, when heated with sulphuric acid at 90°, is again converted into sulphocamphylic acid, it follows that the determination of the constitution of isolauronolic acid will throw most important light on the formula of sulphocamphylic acid, and on the remarkable changes which take place during the formation of this sulpho-acid Erom camphoric acid.The discussion of these points and of their bearing on the consti- tution of camphoric acid, the author must reserve for a detailed description of his experiments, which he hopes soon to be able to lay before the Society. ADDITIONS TO THE LIBRARY. I. By Puwhase. Brande, W. T. Outlines of Geology; being the substance of a course of lectures delivered in the theatre of the Royal Institution in the year 1816.Pp. vii+ 144. London 1817. Friihling und Schulz. Anleitung zur untersuchung der fur die Zucker-Induetrie in betracht kommenden Rohmaterialien, Producte, Nnbenproducte und* Hulfssubstanzen. Fiinfte, umgearbeitete und vermehrte auflage herausgegeben von Dr. R. Friihling. Pp. xvi +465. Braunschweig 1897. Hirsch, B., und Siedler, P. Die fabrikation der Kiinstlichen Mineralwasser und anderer moussirender Getranke. Dritte, neu bearbeitete auflage. Pp. xii + 393. Braunschweig 1897. Hixon, H. W. Notes on Lead and Copper Smelting and Copper Converting. Pp. viii + 116. New Pork and London 1897. Jett>el, W. Die Zundwaaren-Fabrikation nach dem Heutigen Standpunkte. Pp. viii + 255. Wien, Pest, Leipaig 1897. Lehmann, K.B., und Neumann, Rudolf. Atlas und Grundriss der Bakteriologie und lehrbuch der speciellen bakteriologischen diagnostik. 203 Teil I. Atlas, mit 558 farbigen abbildungen auf 63 tafeln und C. 70 bildern im text. Teil 11. Text, Pp. vii + 448. Munchen 1896. Mace, E. Trait6 pratique de Bactbiologie. Troisieme Bdition mise au courant des travaux les plus recents avec 185 figures dans le texte. Premiere partie. Pp. i + 704. Paris 1897. Menschutkin, N. Analytical Chemistry. Translated from the third German edition by James Locke. Pp. xii + 512. London 1896. Moissan, Henri. Le Four Electrique. Pp. vi + 385. Paris 1897. Moldenhauer, F. Grundriss der Mineralogie fur Lohere Lehran- stalten. Pp. xviii + 263. Karlsruhe 1838. Planck, Max.Vorlesungen uber Thermodynamik, mit f unf figuren in text. Pp. vi + 248. Leipzig 1897. 11. Donations. Clowes, F., and Coleman, J. B. Quantitative Chemical Analysis. Fourth edition. Pp. xxiv + 583. London 1897. From the Authors. Fletcher, Thomas. The Commercial UEes of Coal Gas. Pp. 104. London 1897. From the Author. Harcourt, A. G. Vernon, and Madan, H. G. Exercises in Practical Chemistry. Fifth edition revised by H. G. Madan. Pp. xvi+598. Oxford 1897. From H. G. Madan, Esq. Hewitt, J. T. Organic Chemical Manipulation. Pp. xi + 260, 63 illustrations. London 1897. From the Author. Mawe, J. Instructions for the Management of the Blow-Pipe, and Chemical Tests. 3rd edition. Pp. 71. London 1822. From C. E. Franck, Esq. Mendelkeff, D.The Principles of Chemistry, translated from the Russian (6th edition) by G. Kamensky. Edited by T. A. Lawson. Vol. I.,pp. xviii+621 ; vol. II., pp. 518. London 1897. From the Editor. Newth, G. S. A Text-book of Inorganic Chemistry. 5th edition. Pp. xv + 669. London 1897. From the Author. Sykes, W. J. The principles and practice of Brewing. Pp. xriii + 511. With plate and numerous illustrations. London 1897. From the Author. Walke, Willoughby. Lectures on Explosives. A course of lectures prepared especially as a manual and guide in the laboratory of the U.S. Artillery School. Pp. xvi -I-435. 2nd edition. New York 1897. From the Author. Wilson, G. Inorganic Chemistry. New edition revised and en- larged by H. G. Madan. Pp. V-I-535. London 1897.From 33. G. Madan, Bsq. Williams, R. P. Elements of Chemistry. Pp. vi + 412. Boston 1897. From the Publishers. Gabba, L. Manuale del Chimico e dell’ industriale. Pp. xvi + 442. Seconda edizione. (Manuali Hoepli.) Milano 1898. Ghersi, I. Leghe Metalliche ed Amalgame. Pp. xii + 431 con 15 incisioni. (Manuali Hoepli). Milano 1898. Vender, V. La Fabbricazione dell’ Acido Solforico. Pp. v + 312 con 107 incisioni. (Manuali Hoepli). Milano 1897. From the Publishers. Allen, Matthew. Outlines of a Course of Lectures on Chemical Philosophy. Pp. x + 70. London 1819. Bergman, Torberni. Sciagraphia Regni Mineralis Secundum Prim cipia Proxima Digesti. Editio prima Italica. Pp. 160. Florentiae 1783. Davy, Humphrey. Outlines of a Course of Lectures on Chemical Philosophy, Pp.54, and Sadler, John. An Explanation of the Terms used in Chemistry. Pp. 22. London 1804. Dundonald, Earl of. A Treatise showing the Intimate Connection that subsists between Agriculture and Chemistry. Pp. vii + 252. London 1795. Fourcroy, A. F. klhmens d’histoire naturelle et de Chimie. Cin-quibme 6dition. Vols. 1 and 5. Paris. Oliver, William. A Practical Dissertation on Bath Waters. Pp. 136. London 1707. From S. G. Rosenblum, Esq. Pamphlets. Baker, R. T., and Smith, H. G. On the Presence of a True Manna on a (( Blue Grass,” Andropogon annukatus, Forsk. (Read before the Royal Society of N.S. Wales.) From the Authors. Head, J. On Charging Open-hearth Furnaces by Machinery. Pp. 26. Reprint from the Journal of the Iron and Steel Institute, 1897.From the Author. Head, J. The Coal Industry of the South-eastern States of North America. Excerpt from the Transactions of the Federated Institution of Mining Engineers, 1897. From the Author. Jones, L. J.W. Ferric Sulphate in Mine Waters, and its action on metals. Pp. 9. Read before the Colorado Scientific Society, June 5, 1897. From the Author. Latham, P. W. On the Synthesis and Molecular Construction of the Dead and Living Proteid. Pp. 28. Cambridge 1897. From the Publishers. Long, J. H. On the Speed of Reduction of Ferric Alum by Sugar. Chicago 1897. From the Author. Wardle, Sir Thomas, and Bell, P. Carter. On the Adulteratiop of 205 Silk by Chemical Weighting. Pp.43. Read before the Society of Chemical Industry, April, 1897. From the Authors. Wood, T. W. The Assay of Bullion, and Ellis, T. Flower. A Brief Account of the Malay Tin Industry. Chemical and Metal- lurgical Society of Johannesburg. February, 1897. From T. J. McKillop, Esq. At the next Meeting, on Thursday, November 18th, the following Papers will be received. The authors of those marked with an asterisk have announced their intention of being present. * “ On the decomposition of carnphoric acid by fusion with potash or soda.” By A. W. Crossley, M.Sc., Ph.D., and W. H. Perkin, jun., F.R.S. ‘‘ Experiments on the synthesis of camphoric acid.” By IT-H. Bentley, B.Sc., and W. H. Perkin, jun., F.R.S. * “ The action of magnesium on cupric sulphate solution.” ByFrank Clowes, D.Sc., and R.M. Caven, B.Sc. * “ Properties and relationships of dihydroxytartaric acid.” ByH. J. H. Fenton, M.A. LIBRARY. The attention of Fellows is called to the change of the hours during which the Library is open for consultation. The Library is open for consultation and the issue of books from 10a.m. to 6 p.m. (Saturdays 10 a.m. to 4 p.m.) and on the evenings of meetings from 7 p.m. to 9 p.m. CERTIFICATES OF CANDIDATES FOR ELECTION. N.B.-The name: of those who sign from ‘‘ General Knowledge ” are printed in italics. The following Candidates have been proposed for election, A ballot will be held on Thursday, December 2nd. Annis, Ernest George, Health Office, Town Hall, Huddersfield. Physician and Surgeon (M.R.C.S.Eng., L.R.C.P. Lond., L.S.A. Lond., D.P.H., R..C.S. & P.). Medical Officer of Health and General Chemical Adviser to the Town Council of County Borough of Hudders-field. Henry E. Roscoe. S. G. Rawson. Arthur P. Luff. Frank Scudder. Thos. Stevenson. Henry Kenwood. Ball, John,Ph.D., A.R.S.M. 18, Redshaw Street, Derby. Engineer. Has studied Chemistry and Metallurgy for four years at the Royal College of Science, London, the Royal Saxon Mining Academy, Freiberg, and the University of Zurich. During a portion of the above time was engaged in research. Author of a paper dealing with the rate of solution of zinc in acids, Pvoc. C.X., December 3rd, 1896;“Assaying at the Royal Saxon School of Mines,” Milzing Journal, October, 1895 ;also ‘‘The Serpentine and Associated Rocks of Davos,” Zurich, 1897.Whitworth Scholar. De la Beche Medallist of the Royal School of Mines, London. T. E. Thorpe. W. C. Roberts-Austen. W. Palmer Wynne. A. Howard. William A. Tilden. Ball, William, 54, Stretton Road, Leicester. Science Teacher. Teacher of Chemistry (Theoretical and Practical) for last eight years. For last six years, Teacher of Chemistry at the Alderman Newton’s School, Leicester. E. J. Cox. Lewis Ough. R. E. S. Richardson. W. W. Fisher. John WuJttS. 20’1 Beadle, Alec. Alf’red, Beadonwell, Belvedere, Kent. Electro-Chemistry. Two years’ course Electricity at Faraday House, Charing Cross ;six months’ course Analytical Inorganic Chemistry, under Mr.C. J. Wilson; three and a half years Assistant to Mr. James Swinburne, carrying on work of Chemical and Electro- chemical nature. Chns. Fred. Cross. Charles J. Wilson. Clayton Beadle. James Swinburne. Dugald Clerk. James Dewar. Otto Hehner. Edward Bevan. Burland, Richard Oxley, J.P., Poolstock House, Wigan. Manufacturing Chemist. Taken Certificates South Kensington. Member Society Chemical Industry. Manufacturing Chemist twenty years, Sulphate of Iron, Oxide of Iron, Oil, Paints, &c. E. H. Saniter. Arthur H. Tuer. Wm. Jas. Orsman. Arthuy Ccwey. Charles A. Kohn. Cameron, Alexander McLean, Daylesford, Victoria. Director and Science Teacher School of Mines three years. Edin-burgh University.Matriculated 1880, and attended usual courses of Chemistry, Botany, and Natural History for three years ;also during same period attended the Chemical Laboratory of the Public Analyst to the City, J. Falconer King, and Extramural Lecturer; obtained Certificate of Merit. Melbourne University, 1891, obtained Certificate for Metallurgy (including Assaying). Government of Victoria, 1893, obtained highest grade Certificate for Chemistry, Metallurgy, and Assaying, with Honours in each, and the Education Department’s Scholars hips. J. Dennant. J. Falconer King. Orme Masson. C. R.Blackett. A. W.Craig.Clark, Owen Aly, 12, Abbeygate Street, Bury St. Edmunds. Chemist. Associate Pharmaceutical Society Great Britain. Ana-lytical and Consulting Chemist to Greene, King and Co., Limited, Westgate Brewery, Bury St.Edmunds. Analytical and Consulting Chemist to tha Norwich Property Owners’ Association, Frank Browne. Fredk. Johnson. W. Watsop Will. Thomas Tyrer, Arthur E. Barclay. Clarkson, Alexander, 2, Waveney Crescent, Ball ymena, Ireland. Analytical Chemist. The Antrim Iron Ore Co., Ltd., Belfast. Seven years’ experience as an Analytical Chemist. Two years as a Student;, and 5 years as Assistant Chemist in the Laby’s Parkhead Forge, Glasgow, and L.S. Co. Ltd., Mothermell. R. R. Tatlock. A. Humboldt Sexton. John A. Craw. Geo. Ritchie. €1.W. Dickinson. Collingridge, Frank, ‘6 Kenmore,” Shepherd’s Hill, Highgate, London, N. Chemical Research Student.Bachelor of Science (London, 1895) Chemistry, Physics, Mathematics. Associate of Institute of Chemistry (1896). William Ramsay. N. T. M. Wilsmore. Morris W. Travers. J. Norman Collie. J. Wallace Walker. A. M. Kellas. Crofts, James Murray, ‘(Ric hleigh,” Gloucester. Research Student of Emmanuel College. B.A. Emmanuel College, Cambridge. First Class Nat. Sciences Tripos Part I.;2nd. Class Nat. Sciences Tripos, Part 11. (Chemistry and Physiology). Inter. Science (London) : Scholar of Emmanuel College. G. D. Liveing. W. J. Sell. H. J. H. Fenton. M. M. Pattison Muir. S. Ruhemann. R. S. Morrell. George Embrey. Crole, David, Primrose Studios, Wellington Square, Chelsea, S.W. Author. Carried out researches in India, &c., in the Chemistry of Tea ;read a paper on that subject before the Society of Arts this year, and also written a technical work on “Tea.” Have been a Student under, or worked in, the Laboratories of Professors Drinkwater, Page, Bayne, &c.James Bayne. Frederic Jas. M. Page. Hubert E. Lindley. H. Wilson Hake. N. Kelway Bamber. Daniell, John, Council of Education Laboratory, Johannesburg, S.A.R. Lecturer in Chemistry and Assaying to Witwatersrand School of Metallurgy. For 18 years Head Chemist and Head Assayer to Messrs. Nevill, Druce & Co., Llanelly, S. Wales. Lecturer in Chemistry 209 etc., at Llanelly under 5.and A. Department. Now Director of the Witwatersrand School of Metallurgy. Robert Wallace. Iionel. M Jones. John R.Morgan. J. Falconer King. George Beilby. Dixon, Andrew James, Dapto, N.S.W. Head Chemist and Assayer to the Smelting Company of Australia. Three years a student at the Glasgow and West of Scotland Technical College with Profs. Mills and Dittmar. Passed as an Associate of the Institute of Chemistry in 1891, and became a Fellow in 1896. Studied Metallurgy for 1 year at the Royal School of Mines. Worked 3$ years as analyst with W. A. Dixon in Sydney. At present Head Chemist and Assayer to the Smelting Company of Australia. Will. A, Dixon. William M. Hamlet. Alexander Orr. Henry G. Smitb. A. J. Bersnsan. Guttmann, Oscar, Assoc. M. Inst. C.E.,F.I.G., 12, Mark Lane, London, E.C., and 18, Aberdare Gardens, N.W. Consulting Engineer, engaged in the management and erection of explosives and chemical works for the last 23 years, author of various books and contribntions to periodicals on explosives and other matters, member of council of the Society of Chemical Industry, etc., etc., Otto Hehner.John A. R. Newlands. John Heron. Rudolph Messel. Arthur R. Ling. C. A. Mitchell. El. E. R. Newlands. Hamilton, Robert, 11, Ibrox Place, Glasgom. Science Teacher. Bellahouston Academy, Govan, Glasgow. Eight years Teacher of Chemistry and Physiography in above school. Certificated by Science and Art Department in Inorganic Chemistry (first Honours), Organic Chemistry, Physiography, Magnetism and Electricity, Geology, Mathematics (Glasgow University). R. R. Tatlock. James Craig.Hugh Manners. James Robson. William Ralsi&a. Thomas Grog. John Wm. Biggart. Rarger, John, The Nook, St. James’ Mount, Liverpool. I studied three years at University College, Liverpool, and took degree of B.Sc. with Honours in Chemistry in Victoria. Worked for 210 eighteen months at Heidelberg University, a.nd took degree of Ph.l). Research on Succinic Acid Derivatives. Worked with Professor P. E. Frankland at Mason College, for one year, as Priestley Research Scholar-Research on Tartaric Acid Derivatives. I am an Associate of Institute of Chemistry of Great Britain al;d Ireland. J. Campbell Brown. Charles A. Kohn. R. E. Kenyon. Andrew Turnbull. W. R. Innes. Horseman, James Walter, 5, South Parade, Chelsea, London, S.W.Demonstrator to Drs. Moritz aud Morris, of 72, Chancery Lane. Intermediate Science, London. Two years’ study at University College of North Wales, Bangor. One and half year’s study at University College, London. Private Assistant to Professor Ramsay before hold- ing present post. William Ramsay. John Shields. Morris W. Travers. N. T. M. Wilsmore. J. Norman Collie. Geo. W. MacDonald. Kelly, Charles, Oakmere, Hawarden, Chester. Science Teacher. 1883-93, Assistant Master ; 1833-96, Exhi-bitioner, Royal College of Science, London ; 1896 to present, Science Master. William A. Tilden. W. Palmer Wynne. Chapman Jones. Martin 0, Forster. James Bruce. Lemmey, Tom, Wellington College, Berks. Assistant Master. B.A. Oxon. Honours School of Natural Science (Chemistry).Second Science Master at Wellington College. H. Purefoy Fitzgerald, V. H. Veley. W. W. Fisher. E. W. T. Jones. John Watts. J. E. Marsh. Maclaurin, James Scott, Mount Eden, Auckland, N.Z. Analytical Chemist. Author of the following papers in the Tmns-actions of the Chemical Society : “The Dissolution of Gold in a Solution of Potassium Cyanide,” 1893 ; ‘‘The Action of Potassium Cyanide Solutions on New Zealand Gold and Silver,” 1895; “The Relative Weights of Gold and Silver dissolved by Potassium Cyanide 211 Solutions from Alloys of those Metals,” 1896 ; (‘Double Sulphides of Gold and other Metals,” 1896. B.Sc. 1891 ; First Class Honours 1892 ; D.Sc. 1897 ;all of New Zealand University. Science Scholar- ship of Royal Commission for 1851 Exhibition gained in 1895.Fred D. Brown. Henry E. Armstrong. J. A. Pond. A. Vernon Earcourt. James Mactear. Ckaude Vautin. D.A. Xutherland. Macmullen, Alan, 82, James Street, Dublin. Brewer at Messrs. A. Guinness, Son and Co., Ltd. Natural Science Scholar at Balliol College, Oxford. First Class in Chemistry, Natural Science School. Science Master at Wellington College, Berks. Is studying the science and practice of brewing. A. Vernon Hnrcourt. John Conroy. D. H. Nagel. Wm. Odling. W. W. Fisher. Mansford, Charles John Jodrell, B.A. London, Lady Manners Grammar School, Bakewell. Headmaster. Headmaster of Lady Manners Grammar School and Organised Science School. Engaged in teaching Chemistry since 1884. A.S. Waterfield. William G. Boul. R. -W. Buttemer. Samuel Rideal. G. E. Scott Smith. Masters, Edward, The Aloes, Hinckley Road, Leicester. Science Teacher. Associate of the Royal College of Science, London (in Chemistry). Now Teacher of Chemistry and Physics at Alderman Newton’s Higher Grade Science School, Leicester. William A. Tilden. G. S. Newth. Chapman Jones. W. Palmer Wynne. James Bruce. Mathews, John A., 4, First Place, Brooklyn, N.Y. Fellow in Chemistry, Columbia University, N.Y. Washington and Jefferson College (B.S. and M.S.) Three years Post-graduate in Columbia University (M.A.). Assistant in Assaying and Quantitative in Columbia, 1896-7 ;Fellow-Elect in Chemistry, 1897-8. Publica-tions in journals :-School of Mines Quarterly (1894), (‘Carborundum ”; J.Brner.Chem. Xoc. (1896), “Phthalimid ” ;J.Arne?.. Chem. SOC.(1896), (( Table of Factors” (with E. H. Miller) ; J. Amer. Chem. Xoc. (1897), 6‘ On the Ferrocyanides of Zn and Mn ” (with Dr. Miller) ; Lectured 212 to Brooklyn Institute of Arts and Sciences (1896). An extended Review and Bibliography (600 references) of the Metallic Ccwbides was recommended to the Smithsonian Institution for publication, and accepted by that Institution. It has not yet been published. The “ Committee on Indexing Chemical Literature ” of the American Asso-ciation for the Advancement of Science which thus approved and recom- mended my work consisted of H. Carrington Bolton, H. W. Wiley, Francis W.Clarke, A. R. Leeds, A. B. Prescott, and Alfred Tuckerman. Charles F. Chandler. Peter T. Ansten. Jas. S. C. Wells, H. T. VultB. James H. Stebbins, Jun. I’ILos. P. Tiltshire. 8.A. G‘oldschmidt. J. H. Wc~inwright. V. Coblentx. Wm. Jay Xchiefelin. Moon,Philip George Gregory, 139, Rosary Road, Thorpe, Norwich. Chemist in charge, British Gas Light Company, Norwich. Chemist to the British Gas Light Company. Formerly student for 3 years at the East London Technical College. Assistant Chemist for 3 years at Messrs. Martineau’s sugar refinery, London; 1st Honours and Medal, Inorganic Chemistry, South Keneingtoa, 1894. Sydney Steel. J. Theo. Hewitt. Francis Sutton. A. P. Laurie. Z? Xapier Xutton. Gwnccrd Dyer. Mooney, Joseph John, 34, Easter Road, Edinburgh.Surgeon and Apothecary. L.S.A. London, L.A.H. Dublin, worked for 6 months in the Pharmaceutical Laboratory of Owens College under Mr. Wm. Elborne, and for 6 months in the Laboratory of Mr. King, Edinburgh, City Analyst. Author of 6‘ Chemical Processes relating to Water, Air, Food, and Drugs.” In course of publication by Thin, Edinburgh. William Elborne. J. Falconer King. Eugen Blume. J. Watson Napier. 6.f1. Gemmell. Philip, James Charles, 16~,Merton Road, Victoria Road, Kensington, W. Student. Graduated B.Sc. at Aberdeen University, 1895 ; Ph.D. of Gottingen, 1897. Published in the Zeitschrgt fur physik. Chernie, September, 1897, article on ‘‘ Das dielectrische Verbalten flussiger Mischungen.” F.R. Japp. T. S. Murray. Henry E. Armstrong. F. Stanley Kipping. Gerald T. Moody. 213 Reid, Alexander Ferguson, Stair Bridge, Stair, Ayrsbire. Technical Chemist. (1) Some time Chemical Assistant to Hugh Dickie, B.A., LL.D., of Kilmarnock. (2) Three years in the labora- tories of Messrs. Wallace, Tatlock and Clark, City Analysts, Glasgow. (3) Studied Chemistry at the Glasgow and West of Scotland Technical College under Professor A. H. Sexton F.R.S.E., F.I.O., ;Professor G. G. Henderson, D.Sc., M.A., F.I.C., ; Professor A. Schloesser, Ph.D., M.Sc. F.I.C. (4) Five years Chemist to the Cassel Gold Extracting Company of Glasgow. (5) Nearly three years Chemist to Mr. Montgomerie, Stair, N.B. (6) Contributions to Chemical Literature :-Cheinical News, vol.57, p. 39, vol. 65, pp. 68, 125 ; vol. 66, p. 166 ; vol. 67, p. 159, &c. Zeitsc?w$t fu9-anulytische Chemie, vol. 33, part 4. Journal of the Chemical Society, 1892, p. 1027 (Abstracts). G. G. Henderson. Wm. Rintoul. Hora tio Balla nty ne. John Clark. R. R. Tatlock. John S. MacArthur. A. Humboldt Sexton. Roberts, Ernest Henry, Hollydale, Allfarthing Lane, Wandsworth, S.W. Chemist, Dairy Supply Company, Limited. Two and a half years Liverpool College of Chemistry, 7 years assistant to Dr. Bernard Dyer. Bernard Dyer. Sydney Steel, Otto Hehner. Edward Bevan. J,F. H. Gilbard. Cli,urles E. Cassal. Simpson, Edward Sydney, B.E. 34,Pier Street, Perth, West Australia. Government Mineralogist and Assayer. Student Mining School University of Sydney, 1892-1895 ; 1st Honours and Slade Prize for Chemistry, 1893 ; 1st Honours and Caird Scholarship for Chemistry, 1894 ; Bachelor of Engineering with Honours, 1895 ;Researches on Russell Process in 1895 ; Assistant Assayer and Acting Analyst, Mt. Morgan G.M.Co., 1896-97. A. Liversidge. J. A. Schofield. James Taylor. John C. H. Jfingccye. John M. Fltomson. Smith, Robert Francis Wood, 89, Bartholomew Close, E.C. Bacteriologist and Consulting Chemist. Special Chemistry Course (three years) at City Guilds Technical College at South Kensington. 214 Late private assistant to Prof. A. A. Kaultack at St. Bartholomew’s Hospital Path. Lab.; author of paper, ‘‘Vibrio Tonsillaris,” Centralblatf fiir Baktes*iologie,etc.Gerald T. Moody. F. Stanley Hipping. Julian L. Baker. R. C. T. Evans. Henry E. Armstrong. Arthur R. Ling. Southern, Thomas, Junr., 2, Cherry Mount, The Cliff, Higher Broughton, Manchester. Manufacturing Chemist. Studied Chemistry, 1883-1886, under Mr. Wilson, of Manchester Grammar School, and 1886 under Mr. G. H. Hurst, Analytical and Consulting Chemist, Manchester. Sub-sequently 2 years at Owens College, Manchester. Now Chemist to the Wheathill Chemical Works, Salford, where I have had inside manage- ment of the works and superintendence of various alterations and im- provements during the past 6 years. Member of the Society of Chemical Industry. Christopher Wilson. George H. Hurst. J. Carter Bell. George J.Allen. R.J.Flintof. Steel, Frederick William, Tamunua, Navua River, F.iji. Analytical Chemist. Student, Science and Art Dept., local (Glasgow and Greenock) Classes. Student under Prof. J. M. Milne, Ph.D., F.I.C. (St. Mungo’s College, Glasgow). Student under Prof W. Dittmar, LL.D., F.R.S. (G. dz W. S. Technical College). Three years Chemist to the Fiji Sugar Co., Ltd., and at present still holds this position. Thos. Steel. T. U. Walton. T. L. Patterson. John TVm. Biggart. Geo. Patterson. Stephens, Michael Edmund, -4venue House, Finchley. Writing Ink Manufacturer, partner in the firm of Henry C. Stephens of Aldersgate Street, The Candidate has had the Technical Manage- ment and direction of the laboratory and works for the past 11 years. James Dewar.Henry E. Armstrong. William Crookes. Henry C. Stephens. John A. R. Newlands. Boverton Redwood. E.Fmnkland. I;: A. Abet?. 215 Stubbs, George, Arnside, Hertford Road, East Finchley, N. A Student at the Royal College of Science, 1887-8. Analyst in the Government Laboratory, London. For seven years assistant teacher of Organic Chemistry at the Birkbeck Institution. T. E. Thorpe. R. Bannister. H. J. Helm. E. Grant Hooper. J. Woodward. C. Proctor. Tripp, Edward Howard, Kent House, Blackheath Hill, S.E. Ph.D. (Marburg). Four-and-a-half years’ study in Germany. Joint author with Prof. Zincke of an original investigation of ‘‘Ketobromides in the asym. Xylenol series,” Member of the “ Deutsche Whemische Gesellschaft,” Honorary Demonstrator at the Central Technical College, City and Guilds of London Institute.Thomas Tyrer. Wm. Martindale. Henry E. Armstrong. Aug. Schloesser. Rudo@h Messel. David Howard. Turner, John Scriven, 20, Bury Street, Bloomsbury, London, W.C. Assistant to J. Kear Colwell, Esq., Public Analyst, Clerkenwell Town Hall, Rosebery Avenue, London, E.C. Studied Chemistry at University College School under Temple Orme, Esq., and for two years in the laboratories of the Pharmaceutical Society under Professors W. R. Dunstan, F.R.S., F.I.C., and J. Attfield, F.R.S., F.I.C. For the past twelve months assistant to J. K. Colwell, F.I.C., Public Analyst for St. Giles’, Holborn and Clerkenwell. J. Kear Colwell. Wyndham R. Dunstan. John Attfield. J. iYoi*rnccnCollie.Cl~cwlesh’.Cccssccl. Viccajee, Framjee Khurshedjee, Hyderabad, Deccan (India), H.H. the Nizam’s State. Hyderabad Civil Service, H.H. the Nizam’s Mint. Studied Chemistry at the Nizarn’s College, Hyderabad, Deccan (India) (2 years’ course) served probation at the Assay Office, Bombay Mint, for about 12 months. In charge of Assay Work at H.H. the Nizam’s Mint (1894-96) ;went through a course of Metallurgy .and Assaying at the Koyal School of Mines (1896-97), London. W. C. Roberts-Austen. Henry C. Jenkins. Ernest A. Smith. F. W. Bayly. T.K. Rose. Vinter, Percy John, Wesley College, Sheffield. Schoolmaster. Second Class Science Tripos, 1893, Cambridge ; Chemistry one of the three subjects taken. Further work done in Organic preparations in the University Laboratories.Now Senior Science Master, Wesley College, Sheffield ; formerly Science Master, Blairlodge School, Scotland. S. 3'. Dufton. Alexander Scott. F. L. Overend. ?V. CccdetoN Williccms. G. T. W. Newsholnie. While, Arthur James, Whinsfield, Barrow-in-Furness. Analytical Chemist. First Class Metallurgy and Assaying School of Mines, London. Eighteen months Head Chemist to Barrow Hzmatite Steel Co. W. C. Roberts-Austen. F. W. Bayly. T. K. Rose. Ernest A. Smith. . Henry C. Jenkins. Young,Francis Samuel, Mile Hill School, London, N.W. Science Master, Mill Hill School; M.A. Oxon. Degree in Final Honour, School of Chemistry. Research with Dr. Ruhemann in 1894. Teacher and Lecturer on Chemistry at Mill Hill School, London, N.W., since 1894.V. H. 'Veley. W. W. Fisher. J. E. Mamh. John Watts. J. Addyman Gardner. S. Ruhemann. RICHARD CLAY AND SONS, LIMITED, LONDON AND BUNCAY.
ISSN:0369-8718
DOI:10.1039/PL8971300165
出版商:RSC
年代:1897
数据来源: RSC
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