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Proceedings of the Chemical Society, Vol. 26, No. 366 |
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Proceedings of the Chemical Society, London,
Volume 26,
Issue 366,
1910,
Page 17-39
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摘要:
"ssucd 12/2/10. PROCEEDINGS OF THE CHEMICAL SOCIETY. VOl. at3. No.366. Thursday, February 3rd, 1910, at 8.30 p.m., Professor HAROLDB. DIXON,F.R.S., President, in the Chair. Messrs. A. J. Ewins and H, T. Tizard were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs. : Herbert Edmund Clarke, 'B.Sc., 20, Grosvenor Road, Jesniond, Newcastle-on-Ty ne. William Jacob Jones, B.Sc., Queen's Terrace, Llanrwst. Frederick Charles Lewis, 20, Eskburn Road, Liverpool. Hubert Leslie Lucking, Ph.D., St. Mary's, West Heath Road, Hampstead, N.W. Of the following papers, those marked * were read : *24. '' Cupri-compounds : citrates, tartrates, acetates." By Spencer U.Pickering. The constitution suggested for the cupric carbonates has been con-firmed by a study of the citrates, of which eleven have been isolated or recognised.They are derived from the potassiocupric citrate, (C6H507)2KPC~,the copper becoming electronegative by union with two carbons, and also quadrivalent. The P-salt contains &POHOC*Cu"O*CO, (in which case it is alkaline), or CU"O~C*CU~~O*CO,,resulting from tho 18 union of potassium hydroxide or cupric oxide with the double citrate. More potash converts the :Cu'"O into :Cu"OHOK, the substance becoming violet, oxidising dextrose, and combining with cellulose. This is the y-salt. The a-salt is produced from the double salt and an alkaline carbonate, the elements of potassiocupric carbonate becom- ing added to the former.The double salt dissolves to form a /I-cupri-salt with (HO),C*Cu*"O*CO, : this obviates having to regard the former as a molecular compound. A similar explanation applies to the acetates. Hydroxides of the alkali metals with copper tartrate first form R neutral P-cupritartrate, cont,aining (HO),C*Cu1"O*C02, and also a :Cu'"O group between each pair of CHOH groups. Excess of alkali converts these into the :Cu'"OHOK groups of the y-salt. All y-salts decompose, giving cupric or cuprous oxides : a y-cupri-dextrose, with a :Cu"OHOK group between each pair of carbons, would explain the proportion of copper reduced by dextrose. DISCUSSION. 3lr. E. H. JEFFERSremarked that as regards the citrate known as Luff's salt, no other formula than the one now put forward by Mr.Pickering seemed to him to account for the strongly alkaline nature of that particular compound, Mr. TIZARDsaid he would like to know how copper acetate would ioniee if it really had the formula Mr. Pickering suggestod, namely : Qu:o CH,*CO, Mr. Pickerihg had said that solutions of copper acetate differed from those of otlier copper salts in having a deeper colour, and in depositing copper hydrate at high concentrations. But a deep colour was not an exclusive property of the acetate ; all copper salts of weak acids had a more or less deep colour in solution-the weaker the acid the deeper being tho colour. Again, the deposition of hydrate merely meant that hydrolysis of the salt was so great that at high concentrations the solution became supersaturated with regard to the hydrolytic product.He thought there was no reason why the ordinary formula for copper acetate should be given up. Sir W. RAMSAYsaid that three professedly new, but really old, forms of combination had been adduced by Mr. Pickering. First, linked I0 oxygen in U< 1, that me probably knew in hydrogen dioxide; I0 secondly, copper as tetrad, that we knew in '(real " potassium 19 cuprate, K,CuO,, a red substance; and lastly, copper in direct union with carbon, that was known in copper acetylide. The cupritartrates did not display the property of hydrogen dioxide, or of a cuprate, or of copper acetylide. saidMr. PICKERING that in the case of the carbonates it was evident that the only alternative to the copper atom being united to oxygen, as in compounds with electropositive copper, mas to leave it united with the carbon.That the cupricarbonates on electrolysis were found to contain an electronegative copper ion had been demonstrated by Wood and Jones, and the same had been proved as regards the cupritartrate by Masson and Steele. No novelty attached to the idea of copper being able to act as a tetrad, being electronegative or being directly united to carbon; but it was quite fallacious to argue that, because this latter form of union obtained in copper acetylide, which was explosive, all compounds exhibiting such a union must be explosive too. There were other reasons, quite apart from the union of the copper and carbon, to account for the explosiveness of copper acetylide.Similarly, it could not be argued that the group 0 13-43=C<& would be unstable, because I mas so; for the latter, in H-0 decomposing, formed an exceptionally stable substance, with a large evolution of heat, The formulae suggested for the acetates removed the difficulties presented of explaining the differences exhibited between th6se substances and ordinary copper salts. That suggested for the composition of cupridextrose (the existence of which could not be questioned) agreed exactly with the amount of copper yielded by it, and could not be discredited because it indicated the formation of formaldehyde; for, as a matter of fact, formic acid was, according to Clsus, one of the products of its decomposition and oxidation.*25. ‘I The constitution of basic salts.” By Spencer U.Pickering. Additional evidence of the individuality of the five basic salts formed by the action of lime on copper sulphate was given, and it was shown that whilst the lower members are true basic salts, the higher members contain electronegative copper, and show all the properties of cupri-compounds ; they also contain calcium oxide and calcium sulphate. The extreme members of the series are simply cuprates of calcium. A simple scheme was suggested which seems to give a full explanation of the constitution and various properties of the compounds. Iron appears to form analogous compounds, namely, ferrates, with the metal in the electronegative condition.20 “26. ‘‘The constituents of red clover flowers.” By Frederick Belding Power and Arthur Henry Salway, The flowers of the common red clover (Frifoliumpratense, Linnb), which are used to some extent medicinally, have been subjected to a complete chemical examination. A quantity of the alcoholic extract, representing 37.1 kilograms of the dried flowers, when distilled with steam yielded 10.5 grams, or 0.028 per cent., of essential oil. This essential oil, which contained furfuraldehyde, possessed the following constants : d 20°/20 =0.9476; a,,+4OO’ in a I-dcm. tube. The portion of the alcoholic extract which was soluble in water contained a large amount of sugar, which yielded d-phenylglucosazone (m.p. 205O), but from the aqueous liquid the following definite sub- stances were isolated : salicylic and p-coumaric acids ; isorhamnetin, C,,H,,07 (m. p. 295O), which was probably present in the form of a glucoside; a number of new phenolic substances : pmtol, OH *C,,H,O,*O*CH, (m. p. 253O), which apparently is a hydroxymethoxyflavone ;pate?tsot, Cl,H90,(OH), (m. p. 210O) ;a yellow compound, Cl6Hl,O1 (m.p. %Go) ; a substance, C,,H,O,(OH), (m. p. 225O); a substance, CI4Hl2o6(m. p. 214’) ; also the following new glucosides : trifolin, C,,H,,O,,,H,O (m. p. 260°), which yields on hydrolysis a yellow colouring matter, trifolitim, Cl,H,,O, (m. p. 275O), and rhamnose ;isotrifolin, C,,H,,O,, (m. p. 250°), and a glucoside of quercitin, melting at 235’.The portion of the alcoholic extract which was insoluble in water con-sisted chiefly of resinous material, but from it the following compounds were obtained : myricyl alcohol, C,,H,,*OH ; heptacosane, C27H56, and hentriacontane, CslH6,; sitosterol, C,7H,60 (m. p. 135-136’ ; -34.4’) ; a new dihydric alcohol, trifolianol, C,,H,,O,(OH), (m. p. 295O); a mixture of fatty acids, and a small amount of pratol, ClsHl2O4,the latter having evidently been present in the resin in the form of a glucoside. “27. ‘&The influence of radium emanation on equilibrium in a gaseous system.” By Francis Lawry Usher. A quantitative study of the pressure changes following the intro- duction of radium emanation into ammonia and mixtures of nitrogen and hydrogen, coupled with analysis of the resulting mixture of gases, lead to the following conclusions : (1) Ammonia is decomposed rapidly at the ordinary temperature, and solid ammonia less rapidly at -190’.21 (2)This deconiposition is nearly irreversible, and re-combination of nitrogen and hydrogen was not observed to take place to a greater extent than 0.86 per cent. (3) At the ordinary temperature the decomposition follows approxi- mately the course of a unimolecular homogeneous reaction when cor- recting factors for the decay of the emanation, and alteration of its efficiency with time, are introduced. (4)The maximum effect observed was the decomposition of 134,300 molecules of ammonia per atom of emanation.The energy required to produce this effect is about one per cent. of the energy actually expended during its production. (5) If the ratio of ammonia to emanation molecules does not exceed 10,000 to 1, the statement that each atom in disintegrating produces the same effect is not strictly true, on account of the waste involved when the system is rich in emanation. (6) All experiments with gases in glass vessels in presence of the emanation are complicated by the fact that gas is driven into the glass, and can only be recovered by heating strongly in a vacuum. *28. 44 isoQuinoline derivatives. Part IV. Ortho-dihydroxy-bases. The conversion of 1-keto-6:7-dimethoxy-2-alkyltetrahydroiso-quinolines into 3 :4-dihy droxyphenylethylalkylnmines." By Frank Lee Pyman.A number of ortho-dihydroxy-bases have been prepared by the action of hot concentrated hydrochloric acid under pressure on certain 6 :7-dimethoxyisoquinoline derivatives described in the previous papers of this series. None of those in which the isoquinoline ring was preserved had any marked physiological action, but the 1-keto- 6 :7-dimethoxy-2-alkyltetrahydroisoquinolines gave rise to 3 :4-dihydroxyphen ylethylalkylamines, bases of very considerable pressor properties. DISCUSSION. Dr. HEWITTsuggested that the anhydride obtained from dihydroxy- dihydroisoquinoline methiodide by the action of a1kalis possibly possessed a quinonoid instead of a phenol-betaine structure. Substances of undoubted phenol-betaine constitution behaved as the phenoxides of powerful bases, dissolving in water to give alkaline solutions (for example, the anhydride of o-hydroxyphenyltrimethylammonium hydroxide : Griess, Ber., 1880, 13,246).Further, A. E. Dunstan, J. J. Fox, and J. T. Hewitt had shown that the coloured methiodides of hydroxy-and amino-substituted acridines (hydroxy- or amino-group in the para-position to the meso- carbon atom) yield nearly coloudess carbinol bases, which when heated give intensely coloured anhydrides. Dr. PYMANreplied that the compound in question had the charac- teristic properties of phenol-betaines mentioned by Decker and Dunant (Annulem, 1908, 358, 296); amongst others, that of forming the methoxy-derivative of the isoquinolinium iodide when heated with methyl iodide.29. ‘* The action of chlorine on phenylcarbamide.” By Frederick Daniel Chattaway and Newcomb Kinney Chaney. Since each of the three hydrogen atoms attached to nitrogen in the compound can be exchanged for halogen, which can also pass into the nucleus, the action of chlorine on phenylcarbamide is a complicated one. The isolation of the various iJT-chloro -derivatives is rendered difficult, and in some cases impracticable, by the circumstance that the conditions under which the group *CO*NHClis stable bring about the transformation of the group *NCl*C,H,. Owing to the group *Cc)*NHCLbreaking down with liberation of nitrogen in presence of alkali bicarbonates, chlorination has to be effected in acid solution, and consequently 1V-chloro-derivatives containing the unsubstituted phenyl residue, although undoubtedly formed, have not been isolated in a pure state. Anaccount was given of the preparation and properties of a large number of the theoretically possible iV-chloro-derivatives of p-chloro-, 2 : 4-dichloro-, and 2 :4 :6-trichloro-phenylcarbamide.30. ‘‘ Halogen derivatives of malonanilide, ethyl malonanilate, and malonanilic acid.” By Frederick Daniel Chattaway and Frederick Alfred Mason. The halogen derivatives of malouanilide and of ethyl malonanilat e are produced together when ethyl malonate in some excess is heated for a short time with the corresponding aniline, and can easily be separated owing to the sparing solubility of the anilides in all ordinary solvents.The balogen substituted malonanilic acids are obtained by hydro-lysing the corresponding siibstituted rrialonanilic esters, When heated they decompose quantitatively into carbon dioxide and the similarly substituted acetanilides, thus, for example : C,H,C13*NH*CO*CH,*C0,HCO, + C, H,Cl,*NH*CO*CH,.= The compounds containing cblorine and bromine in tho 4-,2 :4, and 2 :4 :6-positions were described. 31. A natural substantive dyestuff.” By Arthur George Perkin. 6‘ The material known as the “red dura” of the Soudan consists of the leaf sheaths and stem of a variety of the Andropogon sorghum or Great Millet.’? In dyeing property it cIosely resembles sanderswood (Pterocarpus santalinus), giving with unmordanted wool a dull red shade, but this is rendered more permanent when a chromium or copper mordant is employed.The colouring matter, C,,H,,O,, which, owing to its similarity to santalin, is called dura-santalin, forms a scarlet, crystalline powder, soluble in a1 kalis with a violet-red color- ation. On fusion with alkali it yields phloroglucinol and p-hydroxy- benzoic acid, 32. “Reactivity of the halogens in organic compounds. Part IV. Interaction of bromoacetic, a-bromopropionic, and a-bromo- butyric acids and their sodium salts with silver salts in aqueous solution. Catalytic action of silver halides.” By George Senter. The reactions in question are mainly bimolecular, but are com-plicated by various disturbing causes.The results of the kinetic experiments with silver nitrate at 26’ are summarised in the accom- panying table, in which the numbers in the second and fifth lines represent the velocity-coefficients. In order to reduce them to a concentration of one mol. per litre, they must be multiplied by 600. CH,Br’CO,H. CHMeBr’C0,H. CHEtBr’C0,H. O.OOOC055 0-00055 0.0025 PI [loo1 C4501 CH,Br*CO,Na. CHMeBr’C0,Na. CHEtBr’C0,Na. 0-000016 0.0025 0’0060 131 C4501 [1100] The numbers in brackets give the relative reactivities of the compounds, referred to the slowest as unity. The silver bromide precipitated in the course of the reactions exerts a powerful accelerating influence on the velocity. Even 1/1000 molar silver bromide (mainly present in the insoluble form) may double the speed of a reaction. Silver iodide exerts a similar catalytic influence on t,he reaction between silver nitrate and methyl iodide in aqueous solution.These observations appear to account for some hitherto unexplained results obtained by previous observers. Nitric acid and benzenesulphonic acid greatly retard the rate of reaction between silver nitrate and bromopropionic acid ;lactic acid has a much smaller effect. The rate of reaction is not greatly affected by replacing half the solvent water by alcohol and by acetone respectively . 24 33. Strychnine, berberine, and allied alkaloids.” By William Henry Perkin, jun., and Robert Robinson. The constitution of strychnine and brucine and their derivatives was discussed in detail, and a modification of the usually accepted formula of berberine was suggested.34. ‘‘Al-Nonylenic acid.” By Victor John Harding and Charles Weizmann. Adescription was given of the methods of preparation of A1-nonylenic acid, its derivatives, and means of identification. 35. “The constitution of the amidines. A new method for determining molecular symmetry.” By Julius Berend Cohen and Joseph Harshall, H. v. Pechmann (Bey., 1895, 28, 869) stated that the amidines obtained (I)from benzanilide imidochloride and p-toluidine, and (11) from benzoyl-p-toluidide imidochloride and aniline, were identical, and that on ethylation a mixture of two ethyl derivatives was produced, corresponding with the replacement of the H* by C2H5in the two formulae : NPh: CPh*&*C,H, C,H,*N :CPh*N&Ph.(1.) (11.) If7here the bases differed in character, however, the amidines obtained by the two methods were still identical, but methylation produced only one methyl derivative, indicating a fixed structure for the original amidine. Tbe present investigation was undertaken to determine whether the introduction of optically active groups into the amidine would offer a more delicate means of distinguishing between the products of the two reactions in the event of their being indistinguishable by other means. I-Menthylamine mas used in the earlier experiments as the active base, and the other bases taken were aniline, the three tolu- idines, and ethylamine. The several amidines mere prepared by the two methods, and it was found that they were in each case abso-lutely identical as regards specific rotation and other physical properties.Furthermore, by ethylation it mas shown that the amidines mere in no case mixtures, but definite compounds in which the mobile hydrogen atom was attached to the less basic group, Finally, an amidine was prepared in which the two bases used, namely, d-and I-bornylamine, were enantiomorphous. In this case it 25 was found that the product was inactive, showing that it is probably a mixture of the two amidines in equal quantities. The ethylation product was also inactive. Attempts to resolve the simple amidine and the ethyl derivative into active constituents by fractional crystal- lisation of the d-camphorsul phonate were unsuccessful.36. “The half-life period of radium; a correction.” By Robert Whytlaw Qray and Sir William Ramsay, K.C.B. The half-life period of radium deduced from the volume of emanation yielded by 1 gram of the element in radioactive equi-librium was erroneously given as 1258 years (Tram., 1909, 95, 1082). The correct value oE this constant, calculated from the published experimental data, is 1744 years. 37. ‘(The absorption spectra of dinaphthanthracene and its hexa- hydro-derivative compared with the absorption spectra of its isomerides.” By Annie Homer and John Edward Purvis. The results of this investigation are : (1) the spectroscopic evidence supports the proposition that the hydrocarbon, C22H14(m.p. 267*5O), is a dinaphthanthracene compound, and that its hydride, C22H20,no longer contains an anthracene linking. (2) Hartenstein’s substance is not a dihydrodinaphthan thracene, but a dinaphthanthracene isomeric with both the dinaphthanthracene compound (m. p. 2675O) and picene. (3) The origin of tbe differences in the absorption bands of the above four compounds may be explained by a consideration of the differences in the anthracene linkings and in the angular or linear linkings of the rings. 38. ‘(Apparatus for demonstrating the electrolysis of hydrochloric acid.” By Augustns Edward Dixon and John Taylor. The electrolysis is performed in a large, vertical U-tube, into the limbs of which two arc-light carbon rods are plunged.From near the top of each limb, a short delivery tube passes off horizontally; by means of these tubes the electrolytic gases are led into the measuring vessel, which contains concentrated sulphuric acid. The latter vessel consists of a three-limbed tube of special construction, one of the limbs serving to control the pressure, while the other two receive and measure the hydrogen and the chlorine. A method was described for staining the sulphuric acid, and thus 26 rendering visible, at a greater distance than usual, the collection of the gases. The construction of the apparatus is such as to preclude leakage of the electrolyte, and to admit of ready access for the purpose of cleaning. 39. The relation between reactivity and chemical constitution of certain halogen compounds.” By Hans Thacher Clarke. The reactivity towards alcoholic pyridine OF the halogens (X) in a series of compounds of the type X*CH,*R has been studied, the group (R) being varied in each case.It was shown that the reactivity of the halogen is controlled by the residual affinity of the atom or group (R), and a dynamic formula for the carboxyl group was suggested. 40. (‘The action of lithium and calcium on organic halides.” By James Frederick Spencer and Gwynnedd Mary Price. Calcium and lithium react with organic halides on heating in a manner analogous to that observed in the interaction of magnesium and organic halogen derivatives (2kcm., 19OS, 93,6s). In the case of calcium, the reaction proceeds along two lines, as indicated by the equations : R*X+Ca =R-CaX ; 2R.X +Ca=CaX, +R*R.The compounds R*CaX are decomposed readily by water, giving the parent substances of the original halide : 2R*CaX+2H,O =2R.H +CaX, +Ca(OH),. In ethereal solution, calcium reacta similarly to magnesium in the Grignard reaction. The yield of the products in these reactions rarelyexceeds 40 per cent. of the theoretical amount. Lithium reacts much more readily than calcium on organic halides, with the produc- tion of lithium substitution products of the parent substance of the original halogen compound : R*X+2Li =LiX +R-Li. The lithium derivatives are very unstable, and are immediately decomposed by water, yielding the parent substance of the halide used : R*Li+H,O =R-H+LiOH.A second action takes place along with the formation of the lithium hydrocarbon, namely, the formation of compounds containing twice as many carbon atoms as the halide compound taken : 2R.X +2Li =2LiX +R*R. The yields obtained in these reactions are generally very good, and vary from 80 per cent, of aniline in the case of m-chloroaniline to 8 per cent. of octane from sec.-octyl iodide. 27 41. ‘‘The change of cobaltous into cobaltic nitrite.” By Tsnneo Suzuki. In I S60, dark brownish-red crystals of very basic cobaltic nitrite were obtained by Lang, when he evaporated the solution left on mixing molecular yiiantities of cobalt sulphate and barium nitrite. Some years later, Hampe found that this crystalline, very soluble substance also contained cobaltous nitrite.It has now been quantitatively investigated. A straw-yellow silver salt and a potassium hydroxycobaltous hydroxycobaltinitrite have also been prepared. The composition of the silver salt is expressed by Ag,Co,’”(NO,),(OH),, from which it follows that a double atom of cobalticum in this salt is combined, half as bydroxide and half as nitrite, with silver nitrite. Lang’s product, very soluble in water and alkaline to litmus, appears to correspond in composition with the silver salt, but to have cobaltous hydroxide and hydroxynitrite combined with the cobaltic bydroxide, tbus : ~[CO,”CO,”’(NO,),( OH),,Co”( NO,)(OH) J,2C0”(0H)2,34H,O = Co1:’Coi’’( N0,),o(OH)1,,34H,O.Of the change undergone by cobaltous nitrite, the primary product is probably Co4”Co~”(N02),,(0H),, as shown by the following equation : GCo”(NO,), + 2H,O = 2N0 + 3Co”(N0,),,Co,”’(N02)~(OH)3,Co”(N0,)(OH), which then, by cumulative resolution, yields Lang’s crystals and a salt in solution, probably Co,”Co,”’(NO,),(OH),, analogous to the silver salt. 42. ‘(The solubility of potassium snlphate in concentrated aqueous solutions of non-electrolytes.” By John Jacob Fox and Arthur Josiah Hoffmeister Gauge. The solubility of potassium sulphate at 25O in aqueous solutions of ethyl alcohol, ethylene glycol, glycerol, mannitol, sucrose, acetone, pyridine, and chloral hydrate was determined. It was observed that as the number of hydroxyl groups in the molecule of the non-electrolyte was increased, the precipitating effect on the potassium sulphate was decreased.The results were discussed from the point, of view of the hydration of the non-electrolyte, and of the possible hydration of the ions derived from potassium sulpbate. Jones and Getman’s results as to the relative hydration of the non-electrolytes (Amer. Chenz. J., 1904, 32, 308) were shown to be inadequate to account for the depression of solubility in the various solutions. 28 43. (( The triazo-group. Part XII. Derivatives of para-triazobenz-aldehyde.” By Martin Onslow Forster and Hilda Mary Jndd, In the hope of explaining the peculiar change undergone by the potassium derivative of p-hydroxypheny lazoimide when a solution in alcohol or water is boiled, condensation products of p-triazobenz-aldehyde with hydroxylamine, phenylhydrazine, p-aminophenol, and camphoryl-+-semicarbazide were studied, and the isomerism of the y-trirtzobenzaldoximes was investigated.BLOCKS OF DIAGRAMS. The Council has decided to dispose of all the blocks of diagrams, etc., which have appeared in the Journal or Proceedings prior to the year 1904, and Fellows are notified that they may obtain the blocks illustrating their own papers by applying to the Assistant Secretary before February 28th, 1910. A small charge will be made to cover cost of looking out the blocks, and postage. At the next Ordinary Scientific Meeting on Thursday, February 17th, 1910, at 8.30 p.m., Sir Edward Thorpe, F.R.S., will deliver tbe Julius Thomsen Memorial Lecture, and the following papers will be communicated : “The absorption spectra of the vapours of pyridine and some of its derivatives at different temperatures and pressures.” By J.E. Purvis. (‘Absorption spectra and melting-point curves of aromatic diazo- amines.” By C. Smith and C. H. Watts. Synthesis of dl-narcotine (enoscopine). Preliminary note.” By W. H. Perkin, jun., and R. Robinson. Isomeric chromous chlorides.” By W. A. Knight and Miss E. M. Rich. ‘(The chromous chlorides.” By W. A. Knight. 29 CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names 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, February 17th, 1910. Adams, Percival Frederick, 81, Rock Avenue, Gillingham, Kent. Lecturer. Inter. B.Sc. (London). Science Lecturer under the Kent Education Committee at the Technical Institute, Gillingham. The chief reason for which admission to the Society is desired is that use may be made of the Society’s publications and library. T. Martin Lowry. A. N. Fitzgerald. H. R. Redman. I?. F. Ferrnoi*. Sidney Harvey. Auchinleck, Gilbert Grahame, Basseterre, St. Kitts, B.W. Indies. Science Master, St. Kitts-Nevis Grammar School. B.Sc. of McGill University, Montreal, Canada. Science Master, St. Kitts-Nevis Grammar School, from June lst, 1908, to present date.Subsequently appointed Superintendent of Agriculture to Government of Grenada, w.I. J. Wallace Walker. Francis Watts. H. A. Tempany. John R. Bouell. E. Gillmun. Banisker, Fred, The Grammar School, Doncaster. Master at the Doncaster Grammar School. B.Sc. Second Class Honours in Chemistry, University of Wales. Formerly Master at the Grammar School, St. Anne’s-on-Sea. Desirous of keeping in touch with the latest developments of Chemistry. P. G. Mander. Allan Baguley. Kennedy J. P. Orton. C. Iz. Young. H. 0. Jones. V,J.Jarrard. R. Henry Jones. W. E. S. Turner. Kenneth S. Catdwell. 30 Berens, Herbert Arthur, Sidney Sussex College, Cambridge. Exhibitioner. Taking Natural Science Tripos (Part 11.) in Chemistry in 19 11.Taking up Manufacturing Chemistry. H. 0. Jones. A. E. Bellars. Charles T. Heycock. W. J. Pope. H. 0. Hale. Canton, Howard, ‘* Lionsdale,” 2, Gloucester Road, Regent’s Park, N.W. Student of Dentistry and Medicine. Sttldent of Chemistry (In- organic? Organic, and Analytical) for 5 years. Ernest J. Parry. Hugh Candy. John C. Umney. Frank E. Teston. JVaZter Hibbert. Child, Arthur James, Oaklands, Edgware. Student of Chemistry. Studying as B.Sc. Honours Student at University College, London. Have studied 3 years under Sir William Kamsay. E. de Barry Barnett. N. T. M. Wilsmore. H. Thacher Clarke. P. May. Edward C. Cyril Bdy. J. Norman Collie. Samuel Smiles. Cocks,Reginald Henry, 14, Norbiton Avenue, Kingston Hill, Surrey. Science Master.Student at Oxford University, 1898-1902. Honours in Chemistry (M. L4.).Science Master, Kingston Grammar School, 1903-1909. Lecturer in Chemistry, Kingston-on-Thames Polytechnic, 1909. W. W. Fisher. N. V. Sidgwick. T. S. Moore. A. F. Walden. G. H. J. Adlam. Cooper, Leonard Harry, 524, Fulham Palace Road, Fulham, S.W. Analytical Chemist. Assistant to Mr. W. J. Dibdin, F.I.C., F.C.S., ctc. Author of t,he paper : ‘‘Colorimetric Estimation of Bromine and Iodine in the presence of Cblorine.” This paper will be read at the March meeting of the Society of Public Analysts. W. J. Dibdin. J. C. Crocker. J. L. White. J. Le mkowitsch. J. B. Coleman. J. Augustus Yoelcker. 31 Coventry, Bernard Okes, 24, Bolingbroke Grove, Wandsworth Common, S.W.; also Dehra Dun, U.P., India. Deputy Conservator of Forests and Imperial Forest Chemist, Imperial Forest Service, India. The candidate has been deputed by the Government of lndia to study Chemistry with the object of qualifying for a post OF Forest Chemist in India. Since appointed Imperial Forest Chemist from October 24th, 1909. Harold Hartley. N. V. Sidgwick. D. H. Nagel. Allan F. Walden. R. W. Sindall. Gumming,Alexander Charles, 3 9, Viewforth, Edinburgh. Lecturer and Assistant in Chemistry in the University of Edinburgh. D.Sc. (Melbourne). Studied under Prof. Orme Blasson, and carried out chemical research under Profs. Masson, James Walker, Richard Abegg, and Sir William Ramsay.Have published papers in Trans. Chem. SOC.,Proc. Royal Society, Fmns. Faraday Soc., and elsewhere. Orme Masson. James Walker. William Ramsay. Leonard Dobbin. Sydney A. Kay. Emslie, Benjamin Leslie, Glengairo, Oakville, Ontario (Office : 1105, Temple Buildings, Toronto). Agricultural Chemist and Manager in Canada of the educational propaganda work of the German Potash Syndicate. Holder of Diploma in Agriculture of Glasgow Agricultural College, and of Professional A ssociateship of the Surveyors’ Institution, London ; Member of the Royal Society of Arts, London; Fellow of the North British Academy of Arts ; Member of the Society of Chemical Industry (Toronto Section) ; Member of the American Chemical Society. Formerly held position as Agricultural Chemist in the hea 1 offices of the German Potash Syndicate at Stassfurt, Germany.Author of ‘‘The Stassfurt Potash Sitlts,” pnblished in the Joui-nd of the Society of Chemical Industry, under date of April 30th, 1909. Author of “Artificial Fertilisers : their Nature and Use,” first published in The Farmers’ Advocate, of London, Canada, during February and March, 1908. Translator of “ On the Assimilation of the Elements of Nutrition by Plants during Different Periods of their Growth,” being researches of the Ducal Agricultural Experiment 32 Station, Barnburg, Anhalt, Germany, and published by Vinton & Co., Ltd., London, E.C., in 1906. W. R. Lang. W. H. Ellis. W. Lash Miller. James McCutcheon. R. A. Bewy. Everest, Arthur Ernest, Clifton House, Shrewsbury. Priestley Research Scholar, University of Birmingham.B.Sc., Birmingham. Priestley Research Scholar, 1908-09, and 1909-10. Percy F. Frankland. Thos. J. Murray. Alex. Findlay. C. K. Tinkler. Hamilton McCombie. Thomas H. Pope. Forster, Aquila, 156, Coatsworth Road, Gateshead-on-Tyne. Prize Demonstrator in Chemistry at Armstrong College, Newcastle- on-Tyne. Bachelor in Science, Durham University. Author of “Note on Benzyl Ethyl Ether,” in Proceedings of the Durham University Philosophical Society. P. Phillips Bedson. F. C. Garrett. J. A. Smythe. S. Hoare Collins. Herbert Blair. Handley, John, P.O. Box 247, New Liskeard, Ontario, Canada. Mining Engineer and Assayer. 1897 : Part I and I1 Diploma in Agriculture, Cambridge.1907 : Elected Associate Member Canadian SOC. Civil Engineers; Member Canadian Mining Institute. 1897-1907 : Assistant, and in charge, Assaying and various engineering works in Canada. 1907 to present time in private practice as Engineer and Assayer. T.B. Wood. M. J. R. Dunstan. R. A. Berry. John Golding. J. F. BZuckshaw. Hayhurst, Walter, Tremellen Street, Accrington. Teacher. B.Sc. (Manchester University). Chief Science 1,ecturer and Demonstrator in the Pannal Ash College, Harrogate. Actively engaged in Chemical research. Jas. Grant. L. G. Radcliffe. Stanley J. Peachep. l? 8. Xinnatt. Fred. G. Richards. E. L.Bheccd. 33 Hughea, Herbert Hillier, 22, Ranelagh Road, Tottenham, N.Science Master (at Tottenham Grammar School). B.Sc. of London University; Chemistry taken at Final. Student of Chemistry at Stafford Technical School, and Mason Univ. Coll., Birmingham. Science Master (including Chemistry) for last six years. R. Henry Jones. Arthur Adams. A. 16. Coles. AlZarn Baguley.IT. Slutes. Price. Jaques, Arthur, 23, St. Oswin’s Avenue, Cullercoats, Northumberland. Student of Chemistry. B.Sc. (Dunelm). Published articles in Chem. ATews, Vol. 88 (295) ; Vol. 90 (107); Vol. 96 (77). Late Lecturer in Chemistry and Demonstrator in Physics, Magee College, Londonderry ;late Fellow of Armstrong College, Newcastle-on-Tyne. Have done two years’ research work in Electrochemistry under Professor Abegg, Breslau.Wish to take in the Journal and use the Library. P. Phillips Bedson. S. Hoare Collins. F. C. Garrett. Herbert Elair. J. A. Smythe. John Watson. Jenkins, Leslie Charles W., 31, Eastcombe Avenue, Charlton, Kent. English representative for Hard and Foreign wood importers. Studying Analytical Chemistry under Prof. Raphael Meldoln. Specially working in dyeing moods, etc. Special investigation with reference to alloys, and general analytical work. Thos. R. Duggan. B. S. Bull. R. Meldola. A. E. Bell. A. Harrison. Krall, Hans, Trinity College, Dublin. Student. Senior Moderator (Experimental Science), B.A. (T. C. D.), 1‘308. Science Master, Rathmines College, 1908-09. Research Student, University Chemical Laboratory, T. C. D. (since 1909).Sydney Young. Wm. C. Ramsden. Emil A. Werner. Wm. Caldwell. James H. Yollok. Lavender, John Herbert, 27, Parade Street, Barrow-in-Furness. Assistant Analyst, Vickers, Sons Sr; Maxim, Naval Construction Works; also Lecturer in Chemistry and Metallurgy at Technical 34 School, Barrow-in-Furness. Late Staff ordshire County Council Scholar in Metallurgy at Birmingham University, 1906-09. Formerly Demonstrator in Chemistry and Physics in West Bromwich Science School, and afterwards in the Municipal Secondary School. 3rd Sta,ge Inorganic Chemistry and 3rd Stage Metallurgy (Board of Education Examinations). Pull Technological Certificate, Iron and Steel Manufacture (City and Guilds Examinations). Thomas Turner. T. Slater Price. R. Lloyd Whiteley.Alex. Findlay. V.J.Lancastev. Lewis, Samuel Judd. 124, Newington Causeway, S.E. Analytical and Consulting Chemist. Most important contributions to scientific literature are a Doktor Dissertation, and some half-dozen papers on Zirconium. Also a few papers to Pharmaceutical litera- ture. B.Sc. (Lond.), F.I.C., Ph.C., Ph.D. (Tubingen). Have held appointment for 8 years as Analytical and Industrial Chemist. Now practising as Analytical and Consulting Chemist. J. Norman Collie. William Ramsay. A. (2. Bloxam. Arthur R. Ling. Samuel Smiles. Marcan, Alexander, Royal Mint, Bangkok, Siam. Chief Assayer, Royal Mint, Bangkok, Siam. Sssociate of the Institute of Chemistry. R. Meldola. S. B. Schryver. M. 0. Porster. William A.Tilden. W. Gowland. Meanwell, Charles Wright, 15, Woodlands Crescent, Aluswell Hill Road, N. Analytical Chemist at Messrs. Thos. De La Rue & Co., Ltd., 110, Bun- hill Row, E.C. School training at Middle Class Schools, Cooper Street, E.C., under Prof. F. S. Barff. Three years’ training at “ Young ” Chair of Technical Chemistry, Anderson’s College, Gltlsgow, under Prof. E. J. Mills, F.R.S. (1879-1881). Joint paper with Prof. Mills on ‘‘ The Action of Oxides on Salts. Part I11 ” (JowrnaZ qf the Chenaical Xocietp, Nov., 1881.) Two short notes contributed to ‘‘ Handbook of the London Geological Field Class,” 1891. Silver Medallist at examination of City and Guilds of London, 1881, on Oils, Colours, etc. Intermediate Examination for B.Sc., London, with Honours in Chemistry, 1888.Twenty-eight years as Chemist with 35 Messrs. De La Rue & Co., 21 of which under Dr. Hugo iVIiiller, F.R.S. Elected F.I.C., 1887. Hugo Muller. Edmund J. Mills. Evelyn de la Rue. A. G. Perkin. W. J. Cousin?. Murch, Douglas Wilshin, Selby House, Victoria Road, Wednesbury, S. Staffs. Chemist at Messrs. Chance & Hunt, Limited, Training: Manchester School of Technology ; Messrs. Crace Calvert & Thornson, Analytical and Consulting Chemists, Manchester ; University College, Liverpool (Languages). Experience : Assistant Chemist at Messrs. Lever Bros., Ltd. (5 years); Chemist at Messrs. Bowman, Thompson & Co., Ltd. (8 years); Chemist at Messrs. Brunner, Mond & Co., Ltd.(2 years); Chemist at Messrs. Chance & Hunt, Ltd. (7 years). William Thomson. Edward Jackson. Fredc. H. Bowman. Francis Henry Tate. F. E. Bowman. Alfred C. flryw. Neal,George Williams, 8, Little Park Gardens, Enfield. Lecturer in Chemistry and Mathematics at the Hackney Pupil Teachers’ Centre, London, N.E. Bachelor of Science (Lond.). Lecturer in Chemistry at Hackney Pupil Teachers’ Centre, and at Kingsland Science aud Art Centre. I am anxious to have access to the Society’s publications, and to be acquainted with the results of recent Chemical Research. W. H. Collier. Frank E. Weston. I€. R. Ellis. Alfred Hyder. 1,V. 11.Ratelife. Nicholson, Philip Brady, 2, Silverwood Terrace, Thrybergh, Rotherham. Analytical Chemist to Messrs.Simon-Carves, Ltd., Silverwood Colliery, Rotherham. Seven years Assistant Chemist, Messrs. Walter Scott, Ltd., Leeds Steel Works. Five years, studied Chemistry and Metallurgy at the Leeda School oE Science. Two years and a-half, Analytical Chemist to Ne3srs. Simon-Carves Bye-product Coke Oven Construction and Working Co. Ltd., Silverwood Colliery, Rotherham. R. Wells Varley. Samuel Psrrish. Harry W. Dixon. JK Sudderick Bmhs. Oswcsld F. Kirby. 36 Palmer, Gilbert, 17, Wansbeck Gardens, West Hartlepool. Science Master. B.Sc. (Lond.), 1909 (Chemistry, Physics, and Mathematics). Engaged in teaching Chemistry since 1900 at ‘‘Organised Science School,” Technical College, West Hartlepool, and at Elwick Road School, West Hartlepool.James C. Philip. M. 0. Forster. G. T. Morgan. J. Archyll Jones. J. W. Patterson. Rattey, Clifford Glare, 37, Park Avenue, Sminton, near Manchester. Electro-Chemist. Four years Student of East London College (University of London). Six years Analyst to the Electrical Power Storage Co., Ltd., London (Accumulator Manufacturers). Present position : Head Chemist to the Chloride Electrical Storage Co., Ltd., Clifton Junction, Manchester (Accumulator Manufacturers). J. T. Hewitt. J. J. Fox, F. G. Pope. H. R.Le Xueur. Clarence Smith. F. W. Caton. Rees, John James Beaumont, Johannesburg College, S. Africa. Schoolmaster. B.Sc. London (Chemistry). Desirous to keep in touch with the latest researches in Chemistry. A. E. Dunstan.A. T. Cameron. W. H. Mills. F. Curxoiz .gritten. TV. Bradshaw Tuck. Russell, John, Oaklands,” Carsick Hill, Tom Lane, Sheffield. Science Master (Sheffield Central Secondary School). Honours Degree in Chemistry (Oxford). Engaged in teaching Chemistry, and desirous of keeping in touch with chemical literature. D. H. Nagel. N. Garrod Thomas. N. V. Sidgwick. T. S. Moore. Harold Hartley. Sen, Aswini Kumar, S1/2, Harrison Road, Calcutta, India. Dyer and Chemist. B.A. (Calcutta University : subjects of study being Chemistry, Physics, and Mathematics) ;B.Sc. Tech. (Victoria University, Manchester, in Applied Chemistry and Chemical Tech- nology); also holder of the Diploma of the Municipal School 37 of Technology, Mnnchesterer, in Applied Chemistry and Chemical Technology.Jas. Grant. 1,. G. Radcliffe. Stanley J. Peachey. F. S. Sinnat. E. I;. Rhead. Smith, Ernest William, 20, St. Bevan’s Road, Halifax. Head of the Pure and Applied Chemistry Department, Technical College, Halifax. Assistant Lecturer in Chemistry, Technical Schools, Hull, 1’303-05. Head o€ the Chemistry Department, Technical College, Halifax, 1905-present time. F. Stanley Kipping. Henry J. S. Sand. It,M Cavon. William Cranfield. R. Lyon. Southgate, Herbert William, 130, Horseferry Road, Westminster, S.W. Physics Lecturer, Westminster College, Horseferry Road, West- minster, S.W. R.Sc. (London). Engaged in Research Work on the Optical Properties of Organic Compounds. T. Martin Lowry.Edward C. Cyril Baly. George Senter. W. Bradshaw Tuck. Frank Lee Pyman. Stuart, Murray, 27, Chowringhee, Calcutta, India. Assistant Superintendent, Geological Survey of India. B.Sc., Birmingham, in Geology and Chemistry. February-May, 1905, Acting Chemist to the Birmingham Corporation Gas Works. Publications : ‘‘ Suitability of Sands in the Rajmahal Hills for Glass Manufacture,” “ Growth of Alunogen on a Meteorite,” Records Geol. Survey Imd., Vol. xxxvii, pt. 2, and “ China-Clay and Fireclay Deposits in the Rajmahal Hills,” Rec. Geol. XUT.Imd., Vol. xxxviii, pt. 2, etc. Percy F. Frankland. C. K. Tinkler. Alex. Findlay. Hamilton McCombie. Thos. J. Murray. EdgaT P.Hedley. Ward, Percy George, The Lodge, Preston Park, Brighton. Recently a Student of the Royal College of Science (Lond.); A.R.C.S. (Lond.) ;B.Sc.(Lond.). William A. Tilden. (3. T. Morgan. M. 0. Forster. J. C. Philip. Chapman Jones, 38 Wolfenden, Stuart Jardine Morris, The Grange, Sidcup, Kent. Student. Commenced the study of Chemistry some 5 years ago in the laboratory of a Fellow (Mr. P. R. Sanders), and since have followed up the subject at various Public Institutions. Specially interested in Electrochemistry, and wish to keep in touch with literature and latest work on the subject. Going to Cambridge in about a year’s time to take Science Tripos Course. Dr. Wolfenden, R past Fellow and well-known investigator in Physiological Chemistry (M. D. Cantab.). P. R.Sanders. J. Connah. Frank E.Weston. T.J. Cheater. Cecil H. Cribb, Francis G. H. Tcite. Young,John, Highfield, Stanley Road, Toddington, Middlesex. Analytical Chemist. Studied Chemistry for four years at the Glasgom and West of Scotland Technical College, and obtained the Diploma (A.G.T.C.). Passed the examinations for the Associateship of the Institute of Chemistry (A.T.C.). Employed as Assistant Chemist to Messrs. Thos. De La Rue & Co., Ltd., Manufacturing Stationers, etc. G. G. Henderson. William S. Denham. William Dickson. Evelyn de la Rue. Thomas Gray. A. Campion. James C. Imine. The following Certificates have been authorised by the Council for presentation to ballot under Bye-law I. (3) : Buchner,Eduard, Ph.D. (Munich). Breslau l., Burgstrasse 8.Professor at the University. Investigator of the fermentation without cells. Prof. Albert Ladenburg. Prof. Dr. Theodor Curtius Prof. Dr. Rich. Abegg. (Heidel berg). Horace T.Brown. Das, Tarak Nas, 31, Bhaironath, Benares City, India. Chemical Assistant of Dr. Arthur Richardson, Central Hindoo College, Benares. Passed B.Sc. Examination, Allahabad University, in 1907. Has been Assistant in Practical Chemistry for 3 years 39 in the Central Hindu College, Benares, under Dr. Arthur Richardson. Has done independent research on ‘‘ Reaction of Oxalates,” which appeared in the Chemical News of June 25, 1909. A. Sanyal. Bidh Bhushccn Dzttt. P.c. Bay. McBeath, John William, Kimberley, South Africa. Chemist, Kimberley Mine Hospital. Passed the Pharmaceutioal Society’s Exam.in 1878. Chemist to Sir Wm. Gray & Go., West Hartlepool, 16 years. Chief Assayer to A. Davison’s Executors, Kimberley, 1894 to 1898. Managing Partner of Albania Salt Works, Griqualand West, 1898 to 1901. F. J. Pooler. J. A. JViZkinso?~. Rau, Malur Srinivasa, M.A., M.D., B.Sc. (Edin.),D.P.H. (Cam-bridge). Bangalore, South India. Chemical Analyst and Bacteriologist to the Mysore Govt., Banga- lore. Chemical Analyst for the last 13 years in Bangalore ;formerly Professor of Chemistry, Doveton Protestant College, Madras. Worked in the Laboratories of the Vniversity of Edinburgh, University College, London, and of Mr. C. H. Cribb, Public Analyst, 136, Shaftesbury Avenue. William Ramsay. Cecil H. Cribb. Henry Kenwood. Edward Bevun.
ISSN:0369-8718
DOI:10.1039/PL9102600017
出版商:RSC
年代:1910
数据来源: RSC
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