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Proceedings of the Chemical Society, Vol. 22, No. 304 |
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Proceedings of the Chemical Society, London,
Volume 22,
Issue 304,
1906,
Page 29-56
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摘要:
Issued 9/2/06 PROCEEDINGS OF THE CHEMICAL SOCIETY. -VOl. 22. No.304. Thursday, February lst, 1906, at 8.30 p.m. Professor R. MELDOLA,F.R.S., President, in the Chair. Mr. J. B. Tillott was formally admitted a Fellow of the Society. Certificates were read for the first time in favour of Messrs. : Roderick Harold Capprr Birt, B.A., 54, Shooter’s .Hill Eoad, Blackheath, S.E. William Dickson, Bra some, Bridge of Weir. James Stuart Hills, 2-,Oxford Street, W. Brnest Ormerod, M.Sc., Ph.D., 8, Leopold Road, Wimbledon, S.W. John Henry West, 11, Sydney Street, Chelsea, S.W. Henry John Wiffcn, 17, Albany R )ad, Manor Park, E. Of the following papers, those marked * were read : *20. Hydroxylamine-ap-disulphonates (structural isomerides of hydroximinosulphates or hydroxylamine-PP-disulp honates).” By Tamemasa Haga. In a previous paper (Trccits., 1904, 85, 78 ; Proc., 1903, 19,28l), it was shown that Fremy’s mptasulpimzilates are hydroxylaminetri-suZphonates.Froin these salts there has now been obtained by hydrolysis a new series of salts which are structurally isomeric with %’remy’sIzeutraZ and basic sulphaxotates, now known to be hydroxp2-aminedisulphonates. The new salts are decomposed by sodium 30 amalgam, and are proved by the nature of this change, by their decomposition by concentrated potassium hydroxide solution, and by their hydrolysis, to be iiydroxyZamine-a/3-disulphonates7in coiitrast with the szclpikmotates, which are I~ydroxyZ~mine-pp-disul~?~oncctes, SO,K*ONH*SO,K and HON(SO,K),, respectively.This is believed to be the firsf indisputable case of the occurrence of fundamental structural isomerism among inorganic compounds. Sodium converts the new salts into sulphate and aminemonosulphonate; potassium hydroxide into the same products, together with nitrogen ; and acids transform them into sulphate and hydroxylamine. The new salts are practically all soluble in water and fairly stable; those prepared are principally the di- and tri-potassium salts, di- and tri-sodium salts, and the di-ammonium salt. -4It,ydroxyEccmine-a-monosulphonate seems incapable of existence; it would be, for example, a sulphate of potass-ium and amidogenium, H,NO*SO,*OK. DISCUSSION. Dr.DIVERSsaid that it follows somewhat unexpectedly from the author’s results that it is the presence of oxylic hydrogen and not aminic hydrogen in a hydroxylamine derivative or in hydroxy lamine itself which makes it easily oxidisable.For, whilst a hydroxylamine-a/3-disulphonate is not sensitive to oxidising agents, although it con-tains an atom of aminic hydrogen, a hydroxylamine-P/%disulphonate which contains none is readily oxidised to a peroxylaminesulphonate (I’rans., 1904, 85, 78; Proc., 1903, 19, 281) by virtue of the oxylic hydrogen atom, which is present in it but not in the up-salt. Apply-ing this deduction from facts to the case of the very sensitive hydroxyl- aminemonosulphonates, an explanation is found for the fact that these salts, when oxidised, as by cupric chloride or by cupric oxide in alkaline solution (Trans., 1889, 55, 760), give nitrous oxide but no hyponitrite, although when decomposed by potassium hydroxide alone they give much hyponitrite, together with sulphite.The production of hypo-nitrite by alkali alone is represented by 2(SO,K)HNi)H +4KHO= S(S0,K)KNOK + 4H,O =2S0,K2 + (NOK), + 4H,O. Its non-production, when cupric oxide is also present, is accounted for by the equation : H’Q N(S03K)K = OH, + N,O + SO,K, + SO,K,.*i-H*N*(SO,K) bK+ * Copper sulphate induces oxidation of a hydroxylaminemonosulphonate catalyti-cally, causing one-half of it to be reduced to aiiiinernonosulphonate in oxidising the other half in the way just formulated (compare I’~a?zs,1900, 77, 978). 31 It should therefore be taken into consideration, when determining the constitution of organic and other substitution derivatives of hydroxylamine, that indifference to oxidising agents is not evidence of the absence of nminic but of oxylic hydrogen. He also huggestetl, in explanation of the fact that a small part of a hydroxylamine-a,&disulphonate is much more difficult to hydrolyse than the rest, that the salt may polymerise to some extent during the heating and thus become resistant to hydrolysis.In reference to the circumstance that some of the author’s results had been anticipated by Raschig (Ber., 1906,39,245), and the question of dating communications having been raised by Professor McLeod, Pro- fessor ARMSTRONGexpressed the hope that no alteration in the existing practice would be made, and tbat nothing would be done to deprive authors of the liberty which they had so long enjoyed of correcting their papers up to &he moment of publication.It was most undesir- able that anything should be done to encourage discussions as to priority among authors. The public were gainers when, as in the present case, independent workers arrived at similar results. *21. “Studies in the camphane series. Part XXI. Benzene-diazo-tpsemicarbazinocamphor and its derivatives.” By Martin Onslow Forster. When a diazonium salt is added to an aqueous solution of camphoryl-t,b-semicarbazide nitrate, the corresponding derivative of benzenediaxo-CH-N*NH*N:N*C,H,~-semical.bazinocaroor,C, HI,< IC(OH)-NH.~O ,is pre-cipitated. Compounds of this class may be called diazo-$-semi-carbazines, and have been obtained from diazotised aniline, p-toluidine, p-anisidine, p-chloroaniline, p-bromoaniline, and the three nitroanilines ; they are characterised by the readiness with which dilute alkalis resolve them in to camphoryl-t,b-carbamide and the corresponding phenyl- azoimide.The author dissented from the views on coloured camphor derivatives expressed by Armstrong and Robert’son (Trans., 1905, 87, 1372). DISCUSSION. In replying to Dr. Forster, Prof. ARMSTRONGsaid that, beyond remarking that Stobbe’s results were in no way irreconcilable with his (the speaker’s) views as to the origin of colour, as he proposed to consider them on another occasion, he should not deal with them then ; nor would he continue the discussion on the relation of optical activity to structure in hydrazones, as this subject could not be dealt with properly in the time at disposal.He would confine his remarks to the compounds described by Dr. Forster. Of the two alternative formulae available for the semicarbazines, Dr. Forster had selected that containing the group *N*NH.N:NPh. Inasmuch as conipounds containing the group *N:NPh were at least yellow, he was of opinion that the formula selected did not represent the coloudess compounds. He was of opinion also that, although prepared by one method, Dr. Forster’s compounds were not all of one type, any more than 0-and p-nitrophenol and nitraniline were compounds of the same type as the corresponding bromophenols and bromanilines.It had long been admitted that the nitro-compounds referred to are at least partially composed of the isodynamic quinonoid forms ; the differences observed by Dr. Forster between his colourless and coloured com-pounds were precisely those observed on comparing the bromanilines with the nitranilines. Dr. LANDER1emarked that it was unlikely that ‘nitrogen compounds of this type would exhibit tautomerism. Pechmann had shown that the so-called ‘‘ virtually tautomeric ” mixed amidines were mixtures or ‘‘ solid solutions ” of structural isomerides, and further that the isomerism disappeared when the hydrocarbon residues were of different types, as in Dr.Forster’s compounds. Dr. LOWRYsaid that Dr. Forster appeared to have overlooked the fact that one of Stobbe’s compounds, the phenyldimethylfulgide (Ber., 1905, 38,3895) existed both in a yellow and in a colourless form, the two forms being convertible into one another in much the same way as the isomeric white and yellow oximes of the mesoxamide series studied by Dr. Whiteley (Trcms., 1903, 83, 24). Tbere was, therefore, the clearest possible evidence of the existence of dynamic isomerism in Stobbe’s series of compounds, and the argument that individual members of such a series must have the same constitution because pre- pared in the same way and exhibiting similar chemical properties was entirely fallacious. Dr. MORGANcited the case of the ortho-diazoimines as another example of a group of compounds the members of which seriecl differed considerably in colour although they were all prepared by the same general method and had similar properties.Diazoiminobenzene and its acyl derivatives were white or colourless substances. 2 :3-Diazo-iminonaphthalene was described as yellow, whereas 1 :8-diazoimino-naphthalene is brownish-red. In spite of this colour difference thero seemed to be no reason for suppoaing that these substances were differently constituted. Although three of Dr. Forster’s diazo-$-semicarbazines were nitro-compounds and possibly owed their colour to the presence of the nitro- groiip, yet it was very unlikely that the yellow p-anisyl derivative should be differently constituted to the white p-tolyl c )mp3und, inas- much as the former differed from the latter only in the substitution of methoxyl for methyl in the para-position to the diazo-complex.Dr. FORSTER,in reply, regretted that Dr. Lowry had misunderstood his attitude. He had not used ‘(the argument that individual members of such a series must have the same constitution because pre- pared in the same way and exhibiting similar chemictl properties.” His contention was, that in the absence of chemical distinctions among a series of compounds prepared alike, it was unsafe to say that the structural type of a colourless compound must differ from that of a coloured one merely because the substances differed in appearance. That was his reason for criticising the views of Professor Armstrong and Mr.Robertson regarding the structure of their camphorquinone-hydrazones, and nothing had been said that evening which impaired his conviction that to deduce a certain constitutional formula for a coloured substance solely from the assumption that the colour is due to the constitution ascribed is arguing in a circle, and therefore unacceptable. 6‘“22. The relations between absorption spectra and chemical constitution. Part I. The chemical reactivity of the carbonyl group.” By Alfred Walter Stewart and Edward Charles Cyril Baly. Attention has been drawn (Trans.,1904, 85, 1029, and 1905, 87, 766) to the relation which exists between tautomerism and the selective absorption which is shown by the spectra of derivatives of ethyl acetoacetate, whilst it has also been proved that the rates of addition of sodium hydrogen sulphite to ketones can be influenced by the introduction of a carboxgl radicle into the molecule, and that the effect thus produced is directly opposite to what one would expect if the hypothesis of steric hindrance held good (Trans., 1905, 87,185, and Proc., 1905, 21, 78).In the present piper, it is shown that these two phenomena are connected with one another, and the relation is indicated between the activity of the carbonyl group in certain ketones and their selective absorption. It is pointed out that in certain cases the phenomena of taatomerism furnish an explanation of the exceptional reactivity of the carbonyl group, as the passage from the enolic to the ketonic form would give rise to a carbonyl radicle, the condition of which may be considered as approximating to that of a nascent atom.This “ nascent carbonyl group ” would be more reactive than the normal carbmyl. But although in most instances tautornerism suffices to explain the phenomena, it breaks down in several cases, and to cover these a new and wider conception is re- 34 quired. From spectroscopic evidence it appears that in the a-diketones a vibration is going on which to il certain extent resembles that which was found in the case of ethyl acetoacetate and its derivatives. The nature of this vibration cannot be easily expressed in the ordinary structural formuh without the possibility of misconception, but it may be indicated somewhat as follows.The vibration is brought about by some change in the relations between the carbon and oxygen atoms, and it in some respects resembles the transition from the ketonic to the enolic form and back again. Using this analogy, we may postulate that the two extreme phases of the vibration can be re-represented by the formulae : -7:0-#’?-00 -c:o I. 11. The convarsion of I into I1would give rise to the ‘(nascent carbonyl group,” just as the change of the enolic into the ketonic form does. Further, the experimental evidence available shows that some such relation does actually exist between the carbonyl groups of benzo-quinoae, and the grea.t reactivity of the quinones can be thus explained.It is proposed to term the general phenomenon “iso-rropesis” and to call “isorropic ” those radicles the activity of which is thus produced. *23. ‘‘The relation between absorption spectra and chemical constitution. Part 11. The quinones and a-diketones.” By Edward Charles Cyril Baly and Alfred Walter Stewart. In the preceding communication, it was shown that in the abeorp- tion spectrum of ethyl pyruvate an absorption band is developed in a different region and at a different dilution from the bands given by the substances having a labile hydrogen atom (Baly and Desch, Trans., 1904, 85,1029 ; 1905,87,766). This band was shown to be due to the two carbonyl groups in juxtaposition to one another ; when two such carbonyl groups are present in the molecule, a new type of oscillation is induced, resulting in the absorption of light of a much longer wave-length than is absorbed by the process of enol-keto-tautomerism.For this new type of oscillation, the name iso-rropesis was proposed. In the present paper it was shown that this isorropesis in a-diketones results in the absorption of light in the visible blue region, so that the substances are intensely yellow. This is evidenced by camphorquinons and diacetyl. An analogous condition in the close proximity of the carbonyl groups occurs in benzoquinone. It is shown that quinone develops the same absorption 35 band as do diacetyl and camphorquinone. The process of isorropesis occurs therefore in benzoquinone exactly as in the case of the a-diketones and is the origin of the yellow colour of this substance.The same is found to be true in the case of p-xyloquinone, tolu-quinone, a-naphthaquinone, acenaphthenequinone, and phennnthra-quinone. There is little doubt, therefore, that the yellow colour of the quinones is due to the isorropesis between the carbonyl groups in juxtaposition. These ohservations strongly support Armstrong's theory that the colour of certain benzene derivatives is due to the quinonoid linking, for they show that the colour is caused, not directly by this linking, but by the isorropesis between the unsatu- rated atoms where this linking exists. "24. ''The relation between absorption spectra and chemical con-stitution.Part 111. The nitranilines and the nitrophenols. " By Edward Charles Cyril Baly, Walter Henry Edwards, and Alfred Walter Stewart. In this paper are described the absorption spectra of compounds having the quinonoid linking and containing a nitrogen atom in place of one or both of the quinone oxygen atoms. By a comparison of the absorption spectra of the nitranilines with those of their hydrochlorides, it is shown that the free substances must exist in the quinonoid form, and that, as they show the same absorption band as benzoquinone and the a-dilretones, a similar process of isorropesis takes place between the unsaturated nitrogen atoms as between the oxygen atoms of benzo- quinone and the a-diketones.Similar arguments are found to hold good for the nitrophenols and for nitrosophenol. By these observa- tions the principle developed in the preceding papers that the colour of the quinones is due to the oscillation or isorropesis between the oxygen atoms is extended to those quinonoid compounds containing nitrogen atoms in the place of one or both of the oxygen atoms. DISCUSSION. Prof. ARMSTRONGsaid that Mr. Baly had put aside entirely the view which had long been held that ketonic interactions were conditioned by the combination of various substances with the carbonyl group and had adopted an entirely intra-molecular view of change, whether chemical or physical. He, however, was inclined to advocate the view that the changes were inter-molecular.He also still adhered to the opinion that three absorbing centres were required to produce visible colour, i.e., that iodoform, not methylene iodide, might be taken as typical of coloured substances, From this point 36 of view, the colour of compounds such as diacetyl might be accounted for on the assumption that polymeric molecules were present, formed by the association, through the residual affinity OF the oxygen atoms, of the ketonic gr -ups, e.g. : CH,-C-C'CH,.. 00 65 CH;?, E*CH, This explanation might perhaps apply also to metanitrophenol and metanitraniline. He remarked subsequently that the blue colour of water might be accounted for from t.his point of view but not by Mr. Baly's hypothesis. In reply to Prof.Armstrong, Mr. BALYpointed out that the absorption spectrum of acetone and ethyl acetoacetate in aqueous solution shows that the tautomeric process is much decreased by the action of the solvent. Similarly, in the case of henzoquinone, the absorption band due to isorropesis exhibited in alcoholic solution entirely disappears when the substance is examined in aqueous solution, its place being taken by two bands in the ultra-violet region. These facts, due no doubt to the formation of hydrates, are strong evidence against the suggestion made by Prof. Armstrong that the colour of diacetyl is due to a complex of two molecules of this substance. "25. '' The action of light on benzaldehydephenylhydrazone." By Frederick Daniel Chattaway.Fischer, who first prepared the ordinary stable a-modification of benzaldehydephenylhydrazone (Annalen, 1878,190,135), noted that it reddened when exposed to the air, and this observation was confirmed by Biltz (Zeit.physikal. C?Lem., 1899, 30, 527), and Reutt and Pawlewski (Bull. Acad. Sci.Cracoui, 1903, 503), who added that the reddening takes place on exposure to light, and disappears when the compound is heated or placed in the dark. The author has extended these observations, and shows that the presence or absence of air does not affect the coloration which is brought about by the violet and blue portions of the spectruni only. The changes of colour are probably clue to a reversible isomeric change from the hydrazino- to the azo-c' onfigurat ion, 37 The colour produced in benzaldehydephenylhydrazone when it has reached its maximum exactly equals in shade and intensity that of azobenzene itself.This explanation of the colour change is supported by the behaviour of benzaldehydediphenylhydrazoneand benxaldehyde -benzylphenylhydrazone, which are not capable of undergoing this type of change, and which are not altered in colour by light. This intramolecular rearrangement caused by light and accompanied by colour change leads to the suggestion that the fading of organic colouring matters in sunlight may in some cases at least be due to a similar reversible isomeric change. DISCUSSION. Dr. WADE,who asked whether the author had noticed the produc- tion of the coloured modification of the hydrazone at the moment of its formation, more especially in benzene solution, stated that he had experienced great difficulty in obtaining a colourless product when the reacting substances were dissolved in this solvent.Mr. W. ROBERTSONpointed out that according to the Hantzsch- Werner hypothesis two stereoisomerides are possible ; in the case, however, of the benzaldehydephenylhydrazones, three isomeric modi- fications are known and it is highly probable that all three possess different constitutions. The significance of the colour of the sub- stituted benzaldehydephenylhydrazones when taken in conjunction with the red unstable ‘‘ benzylidenephenylhydrazine” mas explained and the opinion expressed that the nitrobenzaldehydephenylhydr-azones were, in reality, stable azo-compounds.26. 4b The union of chlorine and hydrogen.” By Charles Hutchens Burgess and David Leonard Chapman. The authors have investigpted the dependence of the character of the induction period on the conditions. The results obtained increased the difficulty of explaining the phenomenon in question by the theory of an intermediate compound. They also iidicated that the effect must be due to some retarding impurity. The impurity was found to be a gaseous compound resulting from the interaction of chlorine and ammonia. An inhibitive compound can also be formed by the action of chlorine on compounds capable of yielding ammonia on oxidation. When such substances are present in the actinometer, the retarding impurity can be gradually formed for considerable periods of time, so that the mixture after it has been previously induced can again become inert when it is allowed to remain in the dark.If the gases and the water contained in the actinometer are carefully purified from all ammoniacal impurity, no induction period can be observed even after the actinometer has stood for weeks in the dark. Ammonia (chlorine-substituted ammoni;L) retards the actiofi between chlorine and formaldehyde in the light. Its inhibitive effect is, how-ever, much less in this case. No difference could be detected in the absorption coefficients of mixtures in equal volumes of air and chlorine and of hydrogen and chlorine.The energy which brings about the combination of hydrogen and chlorine is therefore probably derived from the light absorbed by the chlorine in virtue of its optical properties. 27. ‘(Note on the molecular weight of epinephrine.” By George Barger and Arthur James Ewins. Abel and Taveau have recently (J.Biol. Chern., 1905, 1, 1) objected to the formula C,H1,03N = 183 for epinephrine (adrenaline), the active principle of the adrenal gland. They prefer the formula 2(C,,H,,O3N,$H,O) = 408, and criticise the molecular weight deter- minations of previous investigators, arguing that the use of acetic acid is “entirely inadmissible,” since the substance cannot be re- covered unchanged from the solution. Von Fiirth (Monatsh., 1903, 24, 261) has shown that at least part of the substance can be obtained crystalline by ammonia after evaporating the acetic acid in a vacuum, and the authors have confirmed this observation.That the loss of epinephrine is extremely small in acetic acid solution was shown by Dr. H. H. Dale, who, using a physiological method indicated by Elliott (J,PhysioZ., 1905, 32, 447), finds it possible to estimate epinephrine with an accuracy of about 5 per cent. This physiological method also Eerved as a criterion for the purity of the epinephrine employed, the mo ,t active specimen obtained by repeated fractional precipitation with sodium carbonate and ammonia being selected. The microscopic method of molecular weight determination (T?*ans., 1905, 87, 1756) was employed, with glacial acetic acid and with benzaldehpde, at a temperature of 90’.(I) 0.0732 gram in 2.00 grams of acetic acid was intermediate between 0.19 and 0,214 gram-molecule of benzil per 1000 grams of solvent. 31= 172-1 93. (TI) 0.1016 gram in 2.00 grams of acetic acid was intermediate between 0-166 and 0.18 gram-molecule of acetanilide per 1000 grams of solvent. M = 180-194. (111) 0.0732 gram in 2.00 grams of acetic acid was intermediate between 0.205 and 0.21 gram-molecule of bend per 1000 grams of solvent. M = 174-179. (IV) 0,0732 gram in 2.00 grams of benzaldehyde was intermediate between 0.21 and 0.22 gram-molecule of bend per 1000 grams of solvent. M = 167-174. The mean of all these values is 179. The epinephrine solutions in Experiments I1 and 111 were heated to 90’ €or ten minutes (the time during which the capillary tubes were heated), then diluted with water, nearly neutralised, and made up to 1 in 10,000, On comparison with a solution of the same strength, made by dissolving the solid epinephrine in the minimum quantity of hydrochloric acid, Dr.Dale could not trace any loss of physiological activity. The value obtained by Jowett (Trans., 1904, 85, 194) in a very dilute glacial acetic acid solution by the freezing-point method was 135, and by Bertrand (Compt. mad., 1904, 139, 502) was 174.3. It wodd appear, therefore, that Abel’s formula should be abandoned. 28. “The critical temperature and value of of some carbon compounds.” By James Campbell Brown.The critical temperatures of a number of organic alcohols, acids, esters, and aromatic hydrocarbons are determined. The latent heats of the repurified substances have been redetermined, and the values of ML*the constant -0 are calculated for a number of these compounds for which this constant could not be given (Trans., 1903, 83, 987, and Trans., 1905,87, 265). Two or three of the boiling points are given more correctly for the purified substances. MLThe value of 0rises very slightly with the increase of OH, in the aliphatic alcohols, acids, and esters, but is very constant for the aromatic hydrocarbons. 29. ‘l Slow oxidations in the presence of moisture.’’ By Norman Smith. Experiments have been carried out to determine whether the oxida- tion of ammonia at the ordinary temperature in the presence of air and * ML= molecular heat of vaporisstion, 0=absolute temperature of the boiling point.40 water could be brought about (1) by catalysis, (2) by induced oxidation. The catalysts used were ferric oxide, stannic oxide, manganese dioxide, lead peroxide, and platinum. Stannic oxide and manganese dioxide produced both nitrite and nitrate from the ammonia (0.05 milligram of nitrate for 5 grams of oxide used); ferric oxide and lead peroxide gave only small amounts of nitrite and nitrate (0.01 milligram of nitrate), whilst platinum appeared to be without action. With platinum heated to a temperature just below dull redness, however, a very dilute solution of ammonia or ammonium salts was readily oxidised in presence of air.In the presence of copper or tin undergoing oxida- tion in air, ammonia mas readily oxidised to nitrite and nitrate ; zinc in some experiments gave positive, and in others negative, results, whilst ferrous and manganous hydroxides showed only traces of nitrite or nitrate. In the cases where the formation of nitrate was brought about by induced oxidation, the amount of nitrate produced was much greater than with catalysts. The experiments were extended to the case of nitrogen. No evidence of oxidation of nitrogen by catalysts was obtained. In the presence of substances undergoing oxidation, the metals zinc, iron, and magnesium only among a large number of substances investigated gave ammonia, nitrite, or nitrate.These results were shown to be probably due to traces of nitride in the metals. Water was evaporated in air under various conditions and it mas shown that in no case was ammonium nitrite produced (compare Schonbein, J.pr. CJAem., 1861, 84, 215, and others) if the following sources of error were avoided :(a)traces of nitrite in the air, (b) nitrites produced in the burning of flames, (c) presence of ammonium com- pounds or albuminoid matter in the water, (d) traces of nitride in the metals. No hydrogen peroxide was produced in the evaporation of water under various conditions, except in presence of certain metals such as zinc, which undergo rapid oxidation at the same time. 30. Fischer’s salt and its decomposition by heat.” By Prsfulla Chandra RBy.Fischer’s salt as ordinarily prepared seems to correspond to the formula Co2(NO2),,6KN0,,3H2O. It is, however, invariably con-taminated with appreciable traces of an oxide of cobalt. The method of Rosenheim and Koppel evidently does not yield a purer product as claimed by them, The salt when heated in a vacuum decomposes according to the following equation : CO,(NO,)~,~KNO~,~H~O=CO,O, + 6N0 + 3KN0, + 3KN02+ 3H20. 41 On this decomposition is based an accurate and expeditious method of aiialysing the compound. 31. Action of quinones on o-diamines, 0-nitroaniline, m-nitro- aniline, and 2-nitro-p-toluidine. A preliminary note.” By James Leicester. In a previous paper (Ber., 1890, 23, 2793; Abstr., 1890, 1445), it was shown that the action of o-nitroaniliue and 2-nitro-p-troluidine on benzoquinone, toluquinone, and naphthaquinone was the same in principle as that occurring in the case of aniline and benzoquinone.Quinonefluorin dines and quinonephenazine derivatives were obtained on reduction with ammonium sulphide (Proc., 1893, 9, 9.j. Homofluorindine, C,H,<~~~C,H2~~~>C,H4, has been now prepared from quinonehomofluorindine, by reduction with hydriodic acid (0. Fischer and E. Hepp, Ber., 1890, 33,2789, and Bw.,1888, 21, 683). Various salts of the base have been made. Quinone-a-methylphenazine, C,H20,<x>C,H,Me, has also been reduced in a similar way. Some of the salts dissolve in alcohol with a deep blue colour and have a red fluorescence; the slightest trace of ammonia changes the colour to bright red with a strong fluorescence.The absorption spectra of some of the compounds are under investi- gation with a view to the question of the origin of colour in organic compounds. Quinonephenotolazine, NC6HMe0,< Is>C,H, [N :N : Me= 2 :3 :51,I Nnaphthaquinonephenaeine, Cl,H402<&>C,H4, and a-naphthaquin-Nonetolazine, CIOH4O2<&>C6H3Me, are also being examined in a similar manner. 32. L6 Some oxidation products of the hydroxybenzoic acids. 11.” By Arthur George Perkin. When gallic acid dissolved in 76 per cent. sulphuric acid is oxidised by means of potassium persulphate, a colouring matter very similar to 42 ellaqic acid is produced. This substance, C,,H609, to which the name flavelZagic acid is assigned, is obtained in yellow needles (m.p. above 360O) and dissolves in alkalis with a greenish-yellow coloration, and gives an ucetyi! compound, CI4HO,(C,H,O), (colourless needles, m. p. 31 7-31 go), and a benxoyl derivative, CI,H0,(C7H,0), (prismatic needles, m. p. 287--3S9°). On distillation with zinc dust, it gives fluoi*ene,and on digestion with boiling potassium hydroxide solution is converted into a substance, C,3H,08(m. p. above 360°), the alkaline solution of which develops a bluish-violet colour on oxidation. It crystallises with lH20 in almost colourless needles, gives an acetpl compound, CI3H2O,(C2H30),(prismatic needles, m. p.232-234’), and a corresponding benxoyl derivative (m. p. 261-263”). The results indicate that this substance is hexahydroxydiphenylmethyEolid, OH OH and that flavellagic acid is hydroxyellagic acid. OH OH OH k’lavellagic acid. Ellngic acid. When gallic acid is oxidised in acetic acid by means of potassium persulphate and sulphuric acid, ellagic acid is formed, and this process is preferable to &hat in which concentrated sulphuric acid is employed as the solvent (Proc., 1905, 21, 185), owing to the simultaneous production in this case of a small quantity of flavellagic acid. These colouring matters could only be separated in the form of their benzoyl derivatives. 33. 6‘ Contributions to the chemistry of oxygen compounds. Part I. The compounds of tertiary phosphine oxides with acids and salts.” By Robert Howson Pickard and Joseph Kenyon.Tertiary phosphine oxides are easily prepared by the action of phosphorus oxychloride on organo-magnesium compounds. They com- bine with acids, metallic salts, and orga no-magnesium iodides, forming compounds having the general formule (R,PO),,H,X ;(R3PO),,M”X2; and (R3PO),,CH3MgI. The cornpounds described include some of those in which R is methyl, ethyl, propyl, phenyl, or benzyl, HX is 43 ferrocyanic, chloroauric, cobalticyanic, dichromic, camphoric, iodo- bismuthic,,or iodomercuric acids, and MX, is zinc chloride or iodide, cadmium iodide, mercuric or cobalt chlorides. Other compounds of the oxides which do not conform to these general formulae are those with hydrochloric, trichloroacetic, pyruvic, and chloroplatinic acids and cupric chlorides. The constitution of these compounds is best explained by Werner’s theory of oxonium compounds (Anncclen, 1902, 333,296).The oxides are very weak bases. Their aqueous solutions do not affect the birotation of dextrose, and their compounds with acids are hydrolysed to a large extent by water. 34. ‘(The rapid electro-analysis of metals. Preliminary note.’’ By Henry Julius Salomon Sand. A method for the rapid electro-deposition of metals for analysis and their separation by graded potential has been elaborated. Silver has thus been accurately separated from cdpper in about six minutes from boiling acetate solutions, more than half a gram being deposited without the use of an auxiliary electrode.Copper was separated from bismuth from a boiling tartrate solution (time: about eight minutes). An auxiliary electrode is necessary. The operation must be repeated once, as the first deposit contains traces of bismuth. Owing to the high stirring-efficiency of the electrodes, bismuth has been easily obtained in a perfectly adherent form from nitrate solutions, the time required being about ten minutes, with no auxiliary electrode. By treating the precipitation of bismuth as a separation from hydrogen, perfectly adherent metallic deposits have also been obtained from tartrate and acetate solutions (with the use of an auxiliary electrode). So far the deposition of the following metals has been studied and successfully carried out: copper with currents of ten amperes at about three volts, lead as peroxide, silver from boiling ammoniacal and acetate solutions, and bismuth.At the next Ordinary Meeting, on Thursday, February 15th, 1906, at 8.30 p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated : ‘‘ By A. Angel.‘‘The solubility Cuprous formate.” of triphenylmethane in organic liquids with which it forms crystalline compounds.” By H. Hartley and N. G. Thomas. ‘‘The spontaneous crystallisation of supersaturated solutions.” ByH. Hartley. “The preparation and properties of some new tropeines.” By H. A. D. Jowett and A. C. 0. Hann. “Studies in asymmetric synthesis.Part IV. The application of Grignard’e reaction for asymmetric syntheses.” By A. McKenzie. CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names of those who sign from ‘‘ General Knowledge ” are printed in itdics. The following Candidates have been proposed for election. A ballot will be held on Thursday, 15th February, 1906. Banner, George Ernest, ‘‘ Brooklyn,” Highfield Road, Rock Ferry, .Cheshire. Manager of Chemical Works, Bankhall, for Earnuel Banner & Co., Ltd. Have been a student under Messrs. A. Norman Tate & Co. for some time and engaged in chemical work for the last ten years, also during the last 1s months I have been manager of Chemical Works for Messrs. Samuel Banner & Co., Ltd., Liverpool.I wish to join the Society so as to be in closer touch with the subject and obtain the Journal. Francis Henry Tate. James Smith. Alfred Smetham. 7Vm. P. Thompson. Falter S, Xperflcer. Barker, Arthur Ernest, 3, York Road, Chorl ton-cum-Hardy, Manchester. Schoolmaster. A$ present studying at University College, London. B.Sc. (London), B.A. (London). I wish to be able to obtain informa-tion as to recent work, and to keep up to date, William Ramsay. Samuel Smiles. J. Norman Collie. A. W. Stewart. W. H. Edwards. 46 Bell, William Edward, 88, Monk’s Road, Lincoln. Chemist and Manager of Messrs. Tomlinson and Hayward’s Chemical Works, Lincoln and Warrington. Studied in the laboratory of Messrs.A. Norman Tate & Co., Liverpool. Engaged in the examination of Coal Tar Oils, Crude Glycerines, Tobaccos, Jic. I wish to obtain the latest chemical literature of the day. Francis Henry Tate. Alfred Shrubsole. F. Percy Watson. H. Broccdbent. V.Birhett. Blatchley, Charles Frederick Polwhele, Downside College, Bath. Science Master at Downside College, near Bath. Second Class Honours, Final Honour School of Natura,l Science (Chemistry), Oxford, B.A. (Desirous of having the Journal of the Society.) H. B. Baker. John Watts. Leonard G. Killby. R. de J.Fleming-Struthers. Andrea Angel. J. E. Marsh. Bogue, Thos. Going Stoney, 5, Kenilworth Square, Dublin. M.P.S.I. I am a Member of the Pharmaceutical SOC. of Ireland, and have studied chemistry in Trinity College under Professors Young and Werner, and also in Mr.Armstedt Ray’s laboratories. I am now chemist to Harvey & Co., Ltd., Wholesale Manufacturing Veterinary Chemists. Sydney Young. Wm. C. Ramsden. Emil A. Werner. J. Armstedt Ray. David S. Jardin. Braid, Arthur Forbes, Rose Mount, Dumbreck, Glasgow; and 29, Hampton Road, Forest Gate, London, E. Analytical Chemist. Five years with Messrs. Tatlock & Thomson. City Analysts, Qlasgow, 2 years as student and 3 as assistant. Work included analyses of Iron, Tin, Manganese, Copper, and other ores, Iron, Steel, Copper, Brass, and other metals and alloys. Natural and Artificial Manures, &c. Sugars and Molasses, Oils, Pats, and Waxes, Waters and Assaying. Five years Glasgow Technical College training.At present chemist to the Charing Cross, West End, and City Electricity Supply Co., Ltd. It. R. Tatlock. G. G. Henderson. R. T. Thomson. Thomas Gray. A. Humboldt Sexton. 47 Briggs, Richard Victor, Sirseah Research Station, Mozufferpore P.O., Bengal. Assistant, Sirseah Indigo Research Station. Assistant, five years, C. Rawson, Esq.,F.I.C., F.C.S., Consulting and Analytical Chemist, Bradford. Connected with the chemistry of indigo in India from 1900-05. Medallist Honours Grade, Wool Dyeing, City and Guilds Institute. Student at Bradford Technical College. Cyril Bergtheil. Walter M. Gardner. Robert S. Finlow. J. Walter Leather. D. Hooper. Caldwell, William, Mont-Cecil, Bloomfield, Belfast.Demonstrator, Physiological Department, Trinity College, Dublin. M.A., Royal University, Ireland. Sydney Young. A. Louis Robinson. Emil A. Werner. W. E. Adeney. Wm. Cecil Ramsden. Cecil H. Desch. Clarke, Reginald William Lane, 15, Torridon Road, Hither Green, London, S.E. Demonstrator and Assistant Lecturer, Goldsmiths' College, New Cross. Studied for three years at the City and Guilds of London Institute, Technical College, Finsbury. Holder of College Certificate in Chemistry. Associate of the Institute of Chemistry. I have conducted research work with Professor Meldola and Dr. Lapworth. R. Meldola. Arthur Lapm orth. John Castell- Evans. Arthur H. Coote. F. Henry Streatfeild. Conyngham, Wm. Boulton, 'Sandon,' Ballsbridge, Co.Dublin. Pharmaceutical Chemist. Member of the Pharmaceutical Society of Ireland. Past student of the Royal College of Science, Ireland. W. Palmer Wynne. Sydney Young. W. N. Hartley. Richard J.Noso. Peter MacEwan. E'rnil A. I.tTerner. James S. Ashe. WPLC. Rumsden. W.E. Adeney. Courtauld, Stephen Lewis, Rocking Place, Braintree. B.A., Cantab., Natural Science Tripos, 1904. Engaged in research in the Chemical Department of the Central Technical College, South Kensington. Charles T. Heycock. William A. Davis. Henry E. Armstrong. Willinm Robertson. Gerald T. Moody. Edward Horton. Durrans, Thomas Harold, 1, Cornwall Terrace, Regent’s Park, N.W. Student. Studying Chemistry, Physics, &c., at the Birkbeck College, Chancery Lane, for B.Sc., Lond., with the object of becoming a Manu-facturing Chemist.Member of the Paraday Society. John E. Mackenzie. Frank E. Weston. H. F. C. Goltz. F. Mollmo Perkin. Alex, McKenzie. Evans, Frederick Watkins, 3, Charlotte Street, Hull. Pharmaceutical Chemist. I have been 2 years at the London College of Chemistry, 323, Clapham Road, and having obtained my M.P.S. and Ph.C. desire to pursue further work in Organic Chemistry. John T. Griffiths. Henry Royal-Dawson. Thomas Luxtoa. T.A. flightscules. Robert J. Porter. David J. Willicms. Fierz, Hans Eduard, Ph.D., Clydach on Tawe, Glamorg., Wales. Chemist at the Blond Nickel Go., Ltd., Clydach. Three papers published together with M. 0. Forster, D.Sc., Ph.D., F.R.S., in the Journal of the Chemical Society. William A.Tilden. G. T.Morgan. M. 0. Forster. Chapman Jones. James C. Philip. Glover, Walter Hamis, 38, Ribblesdale Road, Streatham Park, S.W. Assistant in the Chemical Department, Central Technical College, S. Kensington. Student, 1898-1901, and Junior Demonstrator, 1901-1902, at the Technical College, Finsbury. Studied, 1902-1903, at Wurzburg University ; and 1903-1905 at Leipzig University under Prof. Hantzsch, and obtained degree of Ph.D. (Leipzig), July, 1905. Henry E. Armstrong. William A. Davis. T. Martin Lowry. William Arthur Lethbridge. Gerald T. Moody. John Vargaa Eyre. 49 Hayworth, William Prince, 119, Clapton Common, London, N.E. Senior Student in Chemical Department, Technical College, Finsbury, E.C.Certificated Student in Chem. Dept., City and Guilds Tech. Coll., Finsbury, E.C. Senior Student and Junior Demonstrator in Chem. Dept. of above College. Intermediate Associate of Institute of Chemistry Exam. (Pass). Matriculate3 Student of London Uni- versity. R. Meldola. John Castell-Evans. Iiawrence Briant. F. Southerden. E. W. Bealey. Irving,Renry Carlyle, 14, Heath Hurst Road, Hampstead, N.W. Science Student. B.A. (Oxon.) in Chemistry ; Marcon Hall [1903]. Engaged in Rezearch Work at the Central Technical College, South Kensington. Henry E. Armstrong. William A. Davis. Gerctld T. Moody. William Robertson. Edward Horton. Jones,Llewellyn Thomas, Brenig View, Tregzron. Science Master, County School, Tregaron.Three years’ study Chemistry and Physics, University College of Wales, Aberystwyth. B.Sc., University of Wales. Two years Science Master, Tregaron County School. J. J. Sudborough. F. D. Chattaway. ‘I’.Campbell James. J. Alan Murray. J.P.Jlillington. Jones,William Henry Matthews, Leyden Villa, Chester. Deputy City Surveyor, Resident Engineer and Analyst in charge of the New Sewage Purification Works, Chester. Being the Analyst in charge of the Sewage Purification Works, and having to make Analyses of the Sewage in its Crude State, and during the various Stages of passing through the different Tanks and Filters before it enters the River Dee, and desiring to profit from the Study of the Publications and lectures of the Society, and to obtain, by visiting other similar works, that information on the subject essential for my purposes which would be more readily obtained if I wtjre a Member of the Chemical Society.Fredc. H. Bowinan. John Welsh. Edward Halliwell. W. A. Handcock. W. P. Lowe. Uenry IZ. Whitehead, 50 Le Rosaignol, Robert, 2, Cssarea Place, Jersey. Research Student. BSc. Hons. Chem. “The Velocity Reaction be- tween Potassium Ferricyanide and Potassium Iodide,” in conjunction with Prof. Donnan, Trams. Chem. SOC.,1908 ; “Rate of Decay of Thorium Emanation,” in conjunction with C. T. Gimingham,Phil. Mag., 1904. J. Norman Collie, N. T. M. Wilsmore. J. K. H. Inglis. Samuel Smiles. Edward C. Cyril Baly. McDowall, John, Girdstingwood, Kirkcudbright, Scotland.Analytical Chemist. One year study Heriot-Watt College (engineer- ing), four years’ study Edinburgh University (Chemistry) ; Foods and Drugs School of Medicine, Edinburgh. Chemist to Backus and Johnston, CO. At present Chemist to Henry J. Monson & Co., Upper Egypt. Frank Hughes. G. H. Gemmell. Alex. Crum Brown. Hugh Marshall. Leonard Dobbin. J. P. Longstaff. Martin, George Frederick Wesley, 14, Castle Park, Lancaster. Acting Chemist to Messrs. Maudsley and Son, Chemical Manufac- turers, Lancaster, and Organist of Parish Church. I have been a student of science for nine years, and am the inventor of a sheep dip approved by the Board of Agriculture. Former student at the Storey Institute, Lancaster.Have now a private laboratory where I take pupils, Being engaged in research work am anxious to keep in touch with progressive Chemical Science. Henry Eoss. Percy F. Frankland. Rowland Williams. Alex. Findlay. J. A. Storey. Alex. McKelnxie. Parfltt, Samuel, 33, Partridge Road, Cardiff. Deputy and Assistant Manager (Engineering Works, Dry Dock, etc.). Long and careful researches in Siderology and the practical application of improved chemical methods to retard the corrosions in ingot iron and like materials. F. Gwilym Treharne. Thomas Hughes. Llewellyn J. Davies. J. J. Berimye?-. R. FV. Atkinson. 51 Parkin, John, Blaith wai te, Carlisle. M.A., Trinity College, Cambridge. Botanist, interested in the chemical side. 1st Class Nat.Sci. Tripos, Pt. I, 1894. 1st Class Nat. Sci. Tripos, Pt. 11,1895 (Botany and Chemistry). Papers :--rr Carbo-hydrates of Monocotyledons,” Phil. Trans., R.S., Vol. 191, 1899 ; “ On a Reserve Carbohydrate which produces Mannose from the bulb of Lilium,” Proc. Canzb. Phil. Xoc., Vol. XI, 1901 ; ‘(India-rubber,” Circular, Roy. Bot. Gardeits, Ceylon, 1899. At present engaged in the study of the carbohydrates of plants. Horace T. Erown. J. E. Purvis. W. J. Sell. H. 0. Jones, George Dixon. Perkins, William Hughes, Harpiir Hill, Nr. Buxton. Demonstrator in Chemistry, The University, Leeds. 16.S~. (1st Class Honours), Manchester University, 1904. Arthur Smit hells. W. Lowson. J. B. Cohen. C. E. Whiteley.H. M. Dawson. Pitman, John Edmund, Hartley Univ. College, Southampton. A sst. Lecturer and Demonstrator in Chemistry, Hartley Univ. College. Studied chemistry for 3 years (1900-1903) at the Hartley Univ. College, Southamp ton. Appointed Demonstrator and A sst. Lecturer, 1903, in above College. Hold the B.Sc. degree (Lond.) with Honours in Chemistry. Joint author with Prof, Boyd of rr Note on Zeisel Reaction,” J.C.S., 1905. D. R. Boyd. Geo. Fredk. Phillips. A. Vernon Harcourt. W. T. L. Leeming. J. Brierley. C. F. Bahzr. Rogerson, Harold, 46, Bloomsbury St., Bedford Square, London, W.C. Research Chemist in the Wellcome Chemical Research Laboratories, London, E.C. B.Sc. (Manchester), 1904. MSc. (exam.), 1905. For one year worked with Dr.J.F. Thorpe, Ph.D., at the Victoria Univer- sity, Manchester, on ‘‘ Some Alkyl Derivatives of Glutaconic Acid ” and also “ Some Alkyl Derivatives of Aconitic Acid.” Frederick €3. Power. D. L. Chapman. Harold B. Dixon. Wm. A. Bone. W. H. Perkin, jun. J. F. Thorpe. Alfred Holt, jun. 52 Rowsell, Philip Foale, Nutbrook, Exmouth. Analytical and Manufacturing Chemist. Principal of Holman, Ham &, Co., Manufacturing Chemists, Exeter. Holder of Certificates in Chemistry under the Kensington Board and Pharmaceutical Society of Great Britain. Author of various articles, on antiquarian matters specially, and others. As a Chemist I desire admission to the Society for the use of Library and current literature as published by them.William T. Bayne. Albert Cooper. Harold W. Harrie. E. J. Jackman. Isuac 8. Scarf. Shrimpton, John Kirby, 23, Fountains Terrace, North Rd., Ripon. Chemist to Messrs. Robt. Kearsely & Co., varnish and colour makers, Ripon. I have studied at the South Western Polytechnic since 1901. I have held the post of Student Demonstrator during the session 1904-5, when I conducted several investigations in con junction with Professor J. B. Coleman. S. Skinner. W. E. Oakden. J. B. Coleman. F. H. Lowe. J. C. Crocker. Smith, Frank, 407,Church Rd., Smithills, Bolton. Science Master. Graduated in Science (Chemistry and Physics) at the Victoria University, Manchester (1903). Teaching chemistry at Bolton Municipal Secondary School.Lecturer in chemistry at Bolton P.T.’s Centre. Wishes to receive Society’s publications. Harold B. Dixon. Norman Smith. W. H. Perkin, jun. I>. L. Chapman. Wm. A. Bone. G. H. Bailey. Thornton, Percy Charles, 9, Cantwell Rd., Plumstead, S.E. Science Demonstrator under the Liverpool Education Committee. I w-as a Student for littlo more than 2 yeats in the Laboratory of University College (1902-1 904). \Vas appointed Student Demon- strator in Chemistry there, relinquishing this post to become Asst. Chemist in Royal Arsenal, Woolwich (1904-1905). William Ramsay. J. K. H. Inglis. J. Norman Collie. N. T. M. Wilsmore. Edward C. Cyril Baly. 53 Thorp,Arthur William, 210, Sherborne Road, Yeovil. Analytical Chemist. Assistant in the Laboratory of Mr.Walter Thorp, F.I.C. (Drug Analyst to the. Irish Local Government Board), for 7 years; Chemist to Aplin and Barrett, Ltd., for 3 years ; is a Member of the Society of Public Analysts. W. H. Hurtley. H. Droop Richmond. Walter Thorp. E. H. Miller. Otto Rosenheim. Ton kin, Ronald William, 37, Oakhill Road, Putney, S.W. Chief Chemist to the Imperial Tobacco Co., of York Road, St. Luke’s. Studied for 3 years at the Central Technical (City and Guilds of London) College, Kensington. Henry X. Armstrong. William A. Davis. Gerald T. Moody. William Robertson. Robert J. Caldwell. Walker, Franklin Wilfred, 39, Graham Rd., Acton Green, London, W. Dyers’ Chemist. First Class Certificates in Advanced Organic and Inorganic Chemistry ;First Class Honours in Wool, Silk, and Cotton Dyeing (City and Guilds of London), with Institute’s Silver Medal in each case.Formerly for 3 years Junior Assistant in Dyeing Dept., Yorks. College (now Univ. of Leeds), under lateprof. Hummel. Now Chemist to Messrs. Eastman & Son, Dyers and Cleaners, London. Author of paper on ‘‘ Bleaching and Stripping Agents,’’ Journ. Xoc. Dyers and Colourists, Jan. 1905. Wish to keep informed of recent Chemical Research. A. G. Green. Reginald B. Brown. A. G. Perkin. M. C. Lamb. F. E. Robertson. Warren, Richard Alfred, ‘‘Belle Vue,” Hallow Road, Worcester. A Brewer with Messrs. Hill, Evans & Co., Ltd., Vinegar Works, Worcester. Five years student of Chemistry at the Victoria Institute, Worcester.First Class Advanced and First Class, Stage 111,Practical Inorganic Chemistry, South Kensington. Cecil Cooke Duncan. G. Percy Bailey. J. Hector Barnes. Bernard Dyer. T.Xlater Price. 54 Watt, Henry Edgar, 19, Summerhill Road, Dartford, Kent. Chemist, Messrs. Burroughs, Wellcome JL Co., Dartford, Kent. Bachelor of Science (Honours in Chemistry, 1900) ; Master of Science, 1902, Durham-University, also Freire-Marreco Prizeman and Medallist and Johnston Chemical Research Scholar (Durham University). Associate of the Institute of Chemistry (Branch ‘‘ E ”). P. Phillips Bedson. S. Hoare Collins. F. C. Garrett. F. H. Lees. H. A. D. Jowett. Wechsler, Elkan, 59, Petherton Road, Canonbury, N. Demonstrator in Chemistry at the Goldsmiths’ College, New Cross, I studied at the City and Guilds Technical College, Finsbury, and at the Wiirzburg University, and have carried out researches under Professors R.Meldola and A. Hantzsch. I graduated at the Wiirzburg University, taking the Ph.D. degree. R. Meldola. Arthur Lapworth. John Castell-Evans. L. Eynon. F. Henry Streatfeild. Wheaton, Harold Joseph, 21, Chesterton Eoad, Cambridge. Chemical Engineer. I have taken the Chemistry course in connec- tion with Engineering at the Central Technical College, and have since held positions as Assistant Analyst in the Thames Conservancy and Kennicott Water Softener Co.’s Laboratories. Charles E. Groves. Gerald T. Moody. Henry E. Armstrong. William A.Davis. T. Martin Lowry. Willett, Herbert William Mills, The Cedars, Chislehurst. During term : Magdalen College, Oxford. Student of Chemistry at the University of Oxford. Henry A. Miers. D. H. Nagel. Harold Hartley. N. V. Sidgwick. H. B. Baker. Willstaetter, Richard, Zurich (V Bergstrasse 25). Ph.D. Professor of Chemistry, Polytechnicurn, Zurich. George Lunge. M. 0. Forster. T.V. H, Perkin, jun, Rudolf Lessing. William Ramsay. James Bewar. Raphael Meldola. 55 Wolfe, Ernest Edwin, Kinsale, Co. Cork, Jreland. Pharmaceutical Chemist. Member of Pharmaceutical Society, Ireland. Teacher of Practical and Theoretical Chemistry. J. Armstedt Ray. S. V. O’Connor. P. J. Fielding. David 8. Jardin. Francis Dickinson. Pates, John W-illiam, 7 I, North Street, Hugglescote, Nr.Leicester. Science Master, Market Bosworth Grammar School, Nr. Nuneaton. I have been through the course of Chemistry at the Royal College of Science, taking the final for the A.R.C.Sc. in that subject. Have passed the B.Sc. with Honours in Chemistry. As Science Master in the above School, I wish to keep well in touch with recent chemical work and investigations. Oxford Senior, First Class. College of Preceptors, 1st Class Honours (7th). Board of Education Exams. William A. Tilden. Chapman Jones. M. 0. Forster. James C. Philip. G. T.Morgan. The following Certificates have been authorised by the Council for presentation to Ballot under Rye-law I (3) : Grindley, Harry Sands, Urbana, Illinois. Professor of General Chemistry, State University-of Illinois.B.Sc., University of Illinois, 1888. D.Sc., Harvard University, 1894. Author and joint author of various publications in the German Chemical Society Proceedings, American Chemical Journal ; Journal of the American Chemical Society, U.S. Department of Agric. Bulletins, ‘‘ University Studies ” (University of Illinois publications). Sidney Calvert. Mace, William, Hope, King st on, Jamaica. Lecturer in Agricultural Science, Board of Agriculture, Jamaica, 1905, now (1906) Chemist, Amity Hall Sugar Factory, Ltd. Desire to be in touch with modern work and Chemical research. H. H. Cousins. Talbot, George Stanley, Ocean Island, c/o P.P. Co., 60a, Pitt Street, Sydney, N.S.W. Analytical Chemist.Student for three years and four months under the trining and instruction of W. A. Dixon, Esq., F.I.C., and Illessrs. 56 Dixon and Byrn, Analysts under the Public Health Act, N.S.W. For the last two year.3, and at present, Chief Analyst to the Pacific Phos- phate Go., Ltd., Sydney, N.S.W. Desire inembership to keep in touch with current chemical liternture. George A. Byrn. Will, A. Dixon. Andrew J. Dixon. Wastenays, Hardolph, Brisbane, Queensland. Analyst, Brisbane Board of Waterworks. Primary Chemical Train- ing, Demonstrator, Chemistry, 2 years, College of Pharmacy, Brisbane. Assistant Government Analyst, Q., under J. Brownlie Henderson, F.I.C., F.C.S. (seven years, February, 1897, to January, 1904). Analyst to Brisbane Board of Waterworks (January, 1904, to date).Paper before Royal Society, Q., August, 1905 (" Dcscript,ion of Enoggera Reservoir, Brisbane, and Methods of rendering it fit for a Town Supply 77 ). J. C. Briinnich. P. W. Jones. J. Brownlie Henderson. W. A. Hargreaves. R. CLAY AND SONS, LTD. BHEAD ST. HILL, B.L., AND BUNOAY, SUFFOLK.
ISSN:0369-8718
DOI:10.1039/PL9062200029
出版商:RSC
年代:1906
数据来源: RSC
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