|
1. |
Proceedings of the Chemical Society, Vol. 27, No. 388 |
|
Proceedings of the Chemical Society, London,
Volume 27,
Issue 388,
1911,
Page 147-176
Preview
|
PDF (1829KB)
|
|
摘要:
[Issued 13/6/11 PROCEEDINGS OF THB C H E M I C A L S 0 C I E T Y. VOl. 8. No.388. Thursday, June lst, 1911, at 8.30 pm.,Professor PERCYF. FRANKLAND,LL.D., F.R.S., President, in the Chair. Messrs. Ralph Roscoe Enfield, Victor John Harding, and Arthur A. Eldridge were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Mwrs. : Percy James Raymond, 20, Arboretum Road, Worcester. Ernest Vanstone, B.Sc., Gwynfe House, Mount Pleasant, Neath. Of the following papers, those marked * were read: "153. ''The dissociation pressures of the alkali bicarbonates. Part I. Sodium hydrogen carbonate," By Robert Martin Caven and Henry Julius Salomon Sand. The dissociation pressures of sodium carbonate monohydrate and of sodium hydrogen carbonate have been examined by meam of a specially dwigned tensimeter.Difficulty was experienced in the latter case, particularly from the formation of impermeable crusts on the bicarbonate. Satis-factory results were obtained only when the amount of bicarbonate employed was four or five hundred times that theoretically required 148 to evolve the necessary volume of gas at the. highest temperature reached in the experiments. It was found that the vapour pressure, in mm. of mercury, of sodium carbonate monohydrate can be represented with sufficient accuracy by t-he equation : log p= 10.825 -and that of sodium ’9, 3340hydrogen carbonate by the equation : log R= 11.8185--, 1’ From these equations the heat of dissociation of one gram-molecule of sodium carbonate monohydrate is calculated to be 13,800 calories, and that of two gram-molecules of sodium hydrogen carbonate to be 30,700 calories.The latter figure is in sufficient agreement with the number 29,700 calculated from thermochemical results given by de Forcrand (Compt. rend., 1909, 149,719). The pressures corresponding with the f our-phaae equilibrium- anhydrous sodium carbonate, sodium carbonate monohydrate, sodium hydrogen carbonatme, vapour-have also been calculated. “154. (6 The absorption spectra of cinchonine, quinine, and their isomerides.” By James Johnston Dobbie and Alexander Lauder. The authors have examined the absorption spectra, of cinchonine, quinine, and their isomerides, and find that each alkaloid gives tlwo distinct spectra, A and B, the band in B being more sharply defined and much more persistent than the band in A. The spectrum A is obtained when the alkaloid is dissolved in alcohol or in water containing not more than one equivalent of acid to one of the base; the spectrum B when it is dissolved in water containing at least two equivalents of acid to one of the base, The difference between the two spectra was shown to be associated with the fact that the nitrogen of the quinoline nucleus is tervalent in the former, but quinquevalent in the latter case.It was further shown that the spectrum A of cinchonine is prac- tically identical with the spectrum of quinoline in alcohol, and the spectrum B with the spectrum of quinoline salts in aqueous solution.This is explained by the circumstance that the whole of the molecule of the alkaloid, except the quinoline nucleus, is, according to the generally accepted view of the constitution of the alkaloid, com-pletely reduced, and reduced rings, as is well known, cause no selective absorption. The absorption spectra of the isomerides examined are indistin- guishable from those of cinchonine and quinine respectively. 149 *155. “The constituents of the bulb of Buphane disticha.” By Frank Tutin. Buphame aisticha, Herb., is a bulbous plant, indigenous to South Africa, and has long been known to possess toxic properties. The living, inner portions of the bulb contain an abundant amount of alkaloid, whilst the dry, outer layers are free from such a substance.An alcoholic extract of the inner portions of the bulb, when distilled with steam, yielded a small amount of an essential oil containing furfuraldehyde. The portion of the non-volatile product which was soluble in water yielded a small amount of acetovanillone (4-hydroxy-3-methoxyacetophenone), a quantity of chelidonic acid, and con-siderable amounts of copper and ladose. It also gave a mixture of alkaloids, the principal constituent of which is an amorphous, strongly basic product, designated buphanine, which possesses a physiological action similar to that of hyoscine. A weakly basic alkaloid, and one soluble in water, together with small amounts of narcissine, Cl6Hl7o4N, were also obtained. The weakly-basic alkaloid is a convulsant poison, whilst the base soluble in water resembles colchicine and narcissine in its action.Buphanine, on hydrolysis, is converted into a crystalline alkaloid, buphanitine, CBH2406N2,which melts at 240O. Buphanitine hydrochloride and methwdide were also prepared. The portion of the original extract which was insoluble in water consisted of amorphous products, together with pentatriacontane, a phytosterol, ipuranol, C,,H,80,(OH),, and a mixture of fatty acids, both free and combined. “156. The interaction of formic acid and cellulose.” By Charles Frederick Cross and Edward John Bevan. Derivatives of cellulose obhined by direct interaction with formic acid, and also in presence of catalysts, have been investi-gated, and the quantitative data as to composition and decomposi-tion (saponification both by alkalis and acids) are not reconcilable with the view that the products are simple Asters of a normal cellulose.Other modes of action of formic acid are known, and may explain the observed anomalies. The interaction of cellulose and simple hydroxy-compounds was described, particularly in the case of resorcinol, which yields a well crystallised product, the alkaline solutions of which are crimson. 150 The quantitative data accord with a C,, formula. This evidence, on the one hand, and the well known changes of the hexoms under the action of condensing acids on the other, were considered in relation to the interaction of formic acid and cellulose, in which more than one of the possible functions of the acid are involved.“157. (‘Configuration of the stereoisomeric dibromosuccinic acids.” (Preliminary note.) By Alex. McKenzie. Dibromosuccinic acid is formed by the action of bromine on fumaric acid, whilst maleic acid gives isodibromosuccinic acid, Although a large amount of research has been devoted to these dibromeacids, th4 question of their configuration had not been settled. Obviously, one of them must be resolvable into optically active components, and the other must be of the meso-type. The author finds that the iso-acid is the resolvable form. The author was led to examine this problem by a consideration of the Walden inversion, on the one hand, and of the following changes, which are recorded in the literature, on the other : I.H*fi*CO,H KMn0.i) YH(OH)*CO,H CO,H C*H C€I(OH)*CO,H-+ ( Fumaric acid. ) (Racemic acid. ) I +(by Br2) PHEr*CO,H (by water) $X(OH)*GO,H CHBr*CO,H -CH(OH)*CO,H (Dibromosuccinic acid. ) (mesoTartaric acid.) 11. H*$CO,H (by KMn04) vH(oH)*co,HK*C*CO,H CH( OH).CO,H -f (Maleic acid.) (mesoTartsric acid.) I +(by Br2) 7HBr*C02H (by water) 7H(OH)*C02H CHBr*C02H -CH(OH)*CO,H (isoDibromosuccinic acid. ) (Rscemic acid.) In the displacement of tEe halogen by the hydroxy-groups in these cases, it was conceivable that one had to deal with a change df configuration, or, in other words, with a process which was equivalent to a Walden inversion with optically inactive material. The other alternative was that the direct hydroxylation of fumaric and maleic acids with permanganate followed a stereochemical course of a different order from that followed by the direct addition of bromine.The experiments of the author are in favour of the latter view. Further, since the oxidation of fumaric and maleic acids by permanganate does not apparently lead to the formation of a mixture of r-and meso-tartlaric acids, it appears likely that a cliange of configuration takes place during the addition of bromine. isoDibromosuccinic acid was prepared by the action of bromine on maleic acid in the presence of ether. The experimental condi- tions may be regulated so that practically no fumaric acid is produced, and the course of action depends to a remarkable degree on the quality of the ether used.The oxonium complex, 2:;>0<”,:, described by Tschelinzeff, is possibly produced as an intermediate phase. The ease with which the bromine in the iso-acid is displaced renders the resolution a difficult one. A partial resolution was, however, effected by means of morphine, using methyl alcohol as solvent. Morphine (21 grams, 1 mol.) wm dissolved in warm methyl alcohol (290 c.c.), and, when the temperature of the solution was 460, 19 grams (1 mol.) of the iso-acid were added in one instalment. The solution of the acid was immediately followed by the separation of glassy crystals of a morphine salt. After twenty-four hours at about 15O, the crystals (22 grams) were removed. So far, it has not been found practical to crystallise further the salt which separates under these conditions.The resulting acid was strongly hvorotatory, giving [Q]D -100s70 for c= 8.6 in ethyl a,cetate solution. The mother liquor, from which the morphine salt had been removed, gave a dextrorotatory acid. 6.5 Grams of the acid with [a],,-100-7O were then treated with a solution of 7.1 grams of morphine in 100 C.C. of methyl alcohol. The resulting crystals (9.5 grams) gave an acid with [a], -114.5’ for c=7’4 in ethyl acetate solution. The latter acid (2.5 grams) was again acted on by a solution of 2.8 grams of morphine in 80 C.C. of methyl alcohol. The yield of salt was 3.5 grams, and the acid from this gave the value -118O for c =8-47in ethyl acetate solution.So far, there is no evidence to show that this acid is the pure Z-isomeride, and the work is being continued with the view of obtaining the latter. DISCUSSION. The PRESIDENTpointed out that the great interest attaching to Dr. McKenzie’s investigation was that he had definitely fixed the Walden inversion as takizig place in the passage from fumaric to dibromossuccinic acid and in that from maleic to isodibromosuccinic acid respectively. In previously investigated IValden changes it was always uncertain whether the inversion took place in the introduction of the halogen or in its removal. Although in the present case the inversion took place in inactive material, it appeared to him that it was actually brought about by the presence of asymmetric groupings within the molecules concerned.Thus if, according to accepted views, the double linking in fumaric acid were opened up, for example, by the addition of two atoms of bromine, the normal result must be the formation of a, racemic ccmpound, and if instead a meso-compound were produced it must depend on an atom of bromine and an atom of hydrogen exchanging places in one of the, two halves of the molecule. Such an inter- change could, according to accepted views on asymmetlry, only be effected under the directing influence of asymmetric matter itself, as towards symmetric matter the two alternative groupings were in every respect equivalent. Such asymmetric directive influence appeared to him to be available iu the present instance as soon as one atom of bromine had become attached, for the resulting asm-vu metric grouping Ho2C--C-H would influence the configuration of I\Br the asymmetric grouping built up in the other half of themolecule, when the second atom of bromine became attached, with the result, as appeared from the author’s experiments, that instead of the grouping : i/Br , there was obtained I/HH-C-CO,H Br-U-CO2H The same reasoning applied to the formation of the racemic isodibromosuccinic acid from maIeic acid. One was naturally led to inquire as to what asymmetric agency directed the transformation of one enartiomorph into the other in the case of the ordinary Walden inversions, and he wished to suggest that an asymmetric grouping which might exert such a directive influence was to be found in the probable combinations (by association or otherwise) of molecules of the optically active compound undergoing the halogenation of hydroxy- or amino-groups or the hydrolysis or amidation of halogen groups (these being the reactions in which the inversion had been found to take place).This hypothesis was in accord with the observations of Emil Fischer that optically active acids and their esters or their glycines often behaved differently, and again that different bases had different effects in respect of inversive action when used for the hydrolysis of optically active halogen compounds.Such different bases might be expected to alter profoundly the condition of association or of other state of combination in which the halogen compounds might exist, besides altering the nature of the asymmetric grouping which was influencing the asymmetric group actually undergoing hydr ol ys is. 153 This hypothesis also indicated the pmsibility of a single enanti+ morph (or the preponderance of one enantiomorph) emerging from a remtion in which an asymmetric grouping was, during a reaction, temporarily transformed into an unsaturated one. Dr. SENTER,with reference to the President’s suggestion that the intermediate formation of birnolecular compounds might play a part in the Walden inversion, said that he had recently obtained evidence of the formation of such a compound, namely, CH,Br-CO,*CH,*CD,Na, in the hydrolytic decomposition of sodium bromoacetate.The final product, glycollic acid, was formed both by the hydrolysis of this compound and by the direct hydrolytic decomposition of sodium bromoacetate, in proportions depending on the dilution and tem-perature. As regards the further explanation of the formation of active compounds based on the assumption of the successive addition of bromine atoms at a double bond, it would be interesting to know if there was any direct evidence of such a mode of addition. The available evidence appeared to show that free oxygen, and also hydrogen, always combined as whole molecules, with subsequent rearrangement, but other elements, including the halogens, might behave differently in this respect.168. The influence of conjugated linkings on general absorptive ‘6 power. Part 11. Some open-chain and cyclic compounds.” By Cecil Reginald Crymble, Alfred Walter Stewart, Robert Wright, and Florence Williamson Ilea. In continuation of the previous work on this subject, an examin& tion has been made of the absorption spectra of isomeric substances ccntaining double bonds in different positions in the molecule. Eighteen spectra have been compared in the case of isomeric substances, and it has been found that in every case the conjugation of double linkings increases the general absorptive power of the compound. This influence is specially marked in the cam of two other substances, namely, crotonic acid and allylacetic acid ;for here, although the former compound contains fewer atoms and has the same number of double bonds, yet its absorptive power is very much more marked than that of the latter, in which the double bonds are not conjugated with each other.An attempt has been made to detect the influence on general absorption of two unsatur- ated groups placed far apart in a chain, but near together in space; the results, however, have not been positive. 154 159. Lb New derivatives of aminolauronic acid." By John Weir. In the course of a research, the objects of which were: (1) the preparation of the camphor analogue of indigo, and (2) the preparation of a diaminocamphor, NH,*C,H,,*NH,, the following new compounds have been obtained.(1) Carboxymethy Zaminoluuronic acid,CO, H*C8Hl4*NH*CH, CO,H, a crystalline solid, melting at 183-184', and having [u]F in water +45.7". (2) N-Anhydrocurboxyrnothylnminolauronicacid, C,Hl,<F:ON*CH,*CO,H, rz crystalline solid, melt8ing at 142-143", and having [u]F in water -22.ZC,in alcohol -11*6O, and in benzene -22.2". co NMep an orange-(3) Anhydromethylaminolccuronicmid, C,H14< I coloured wax. (4) Be.nxoyZamino2auronic acid, CO,H*C,H,,*NHBz, a crystalline solid, melting at 204", and having [a]1: in alcohol -18.4'. (5) HethyZ benzoylaminolaulaonate, a crystalline solid, melting at 88-89', and haviag [a]F in alcohol -28.9". acid, C8€€14<~o(6) N-Annhyd~.obenxoyZ~minolauronic hBz' a crystalline solid, melting at 71-72', and having [u]yin alcohol -69.1'.The two main objects of the work were not realised. 160. ('The triazo-group. Part XVIJI. P-Triazoethylamine," By Xartin Onslow Forster and Sidney Herbert Newman. &TriuzoethyZacmine,N,*CH,*CH,-NH,, obtained from the product of heating @-bromoethylamine hydrobromide with sodium azide, is a oolourless oil, which distils at 63-5O/50 mm., and has D16 1.0488. It is reduced to ethylenediamine by stannous chloride in hydro- chloric acid. The hydrochloride, with the benzoyl, p-tohene- s*idphonyZ,phthatyl, and p-nitrob enzylidene derivatives, have been prepared, together with the carbamide, phenylcarbamide, and pF,enyZt hi0car6 amide. Unlike the corresponding halogen derivativm, P-triamthylamine is not converted into dimethyleneimine by the action of the alkalis, thus offering an unusual contrast, between the azoimide complez and the halogen atoms.155 161. The interaction of metallic oxides and phosphoryl chloride, done and in the presence of certain organic compounds.” By Henry Bassett, jun., and Hugh Btott Taylor. Several metallic oxides read readily with phosphoryl chloride to give well defined double compounds. The following have been obtained : Ca0,2POCl3;Ca0,3POC13;Mg0,2POC13;Mg0,3POCl3 ; Mn0,3POC13;Zn0,3POC13. These compounds crystallise well, but are very sensitive to moisture, for which reason they are difficult to obtain quite pure. All the other oxides investigated (COO, CdO, ClitO, Cu,O, HgO, A&,O,, FqO,) react more or less readily with phosphoryl chloride, but in them cases large quantities of the metallic chlorides are formed.The mechanism of this chloride formation was discussed, and rmons and experiments were brought forwaxd which favour the view that it is preceded by the formation of an additive compound of the oxide and phosphoryl chloride. The double compounds of metallic oxides md phosphoryl chloride yield a series of well crystallised derivatives with acetone, ether, and various esters, for example, Ca0,P203@1,,2Me,C0 ; Mg0,P,0,C1,,2CH3*C0,E t ;MnO,PzOsC1,,2CH3*CO2Et. These organic derivatives are qu 2leasily obtained by dissolving the appropriate oxide in a solution of phosphoryl chloride in acetone, ethyl acetate, eh.Hydrogen chloride is liberated owing to the action of traces of moisture with formation of these derivatives of the compound P,O,Cl,. Their ready formation supports the view that this compound is one of the first products of the action of moisture on phosphoryl chloride. 162. ‘‘Acopper derivative of quinol.” By Hugh Vernon Thompson. An invsstigation into the effect of organic oxidising agenh on copper showed that a solution of pbenzoquinone in ethyl acetate containing traces of acetic acid readily attacks copper. The first product of I;he reaction is normal copper acetate, Cu(CpH604),H20,whilst after prolonged immersion the copper becomesi coated with a crystalline deposit varying in colour from orangered to brick-brown, and the solution also turns a red colour.Subsequent work showed that the deposit could be obtained in crystalline pelletg of a deep porbwine colour by dissolving a little p-benquinone in 30 C.C. of ethyl acetate to which 4 to 5 drops (about 0.07 gram) of glacial acetic acid had been added; in this 1.56 solution thin copper foil is placed so as to be only partly immersed, and the, temperature kept at 10-15° for one or two days. The sub- stance cannot be purified by ordinary means owing to its insolubility or instability in common solvents; the mean value calculated from a series of analyses gave C=30.61; H=3-57; Cu=33.16 per cent., corresponding with an empirical formula, C,H,04Cu. Since the initial product in the reaction is copper acetate, it is probable that the red deposit is a molecular compound containing copper acetate, in which case the molecular formula must be at least twice the empirical formula, namely, C,,H,,O,Cu,.If we assume that this is the correct molecular formula, the composition can be expressed as: (a) C,H130, J cuo,cu (c4H1304) or (6) CGHG02Cu:(;lu(C,HG04),2Ha0. That the substance is a molecular compound of hydrated copper acetate and a copper derivative of quinol follows from the facts that decomposition by glacial acetic acid in ether gives quinol and the salt Cu(C4H604),H20,and that on gently heating the compound in an atmosphere of carbon dioxide pbenzoquinone and water are liberated, leaving a residue of metallic copper and anhydrous copper acetate.The compound can be obtained in small amounts by other methods, but the quinol derivative has not yet been isolated from the copper acetate. Nitric acid reacts with this compound to give a yellow, crystalline substance, which is either a mixture of copper picrate and copper oxalate of approximately constant composition, or a molecular compound of the two salts of the composition : 2[ (C,H207N,),cu,5H,O1,7(C~O4~,H~O)4 163. “The action of salt solutions and of sea-water on iron at various temperatures.” By John Albert Newton Friend and Joseph Hallam Brown. The authors exposed thin plates of pure iron to the corrosive action of various concentrations of common salt and of sea-water at different temperatures.Below 13O it was found that dilute solutions exert a more corrosive action than distilled water at the same temperature; above 13O, on the other hand, they exert it lees corrosive action. At 13O the corrosive action is practically the same for dilute solutions of common saIt, for ordinary sea-water, and for distilled water. This temperature is therefore styled by the authors the “ Inversion Temperature.” 157 164. ‘‘Some derivatives of gelsemine.” By Charles Watson Xoore. Gelsemine, CzoH,,OzN,, is stable towards alkali hydroxides and reducing agents. By treatment with oxidising agents, on the other hand, the molecule is decomposed, and no definite products have been obtained by this means. On boiling gelsemine with concentrated hydrochloric acid for some hours, three new bases are formed, wEich have been designated as apogelsemine, isoapogelsernine, and chloro-isoapoqetsemine.Of these, apogelsemine, CzoH24O3N2, is the chief product of the reaction, and although it cannot be crystdlised, it yields well characterised, crystalline derivatives. Chloro-isoapogelsemine, C,,Hz,02N2C1, and its hydrolytic product, isoapogelsemine, C20Hz40,Nz, are only formed in relatively small amount&. Both these bases crystallise readily, and they, and several of their derivatives, have been characterised. It has also been observed that when gelsemifie methyl hydroxide is heated at 200° in aqueous solution, the expected gelsemethine is not produced, the methyl hydroxide losing methyl alcohol with regeneration of gelsemine.165. ‘(Syntheses with phenol derivatives containing a mobile nitro-group. Part IV. Quinone-imides, asymmetric quaternary ammonium compounds, and asymmetric carbinols. ” By Raphael Xeldola and Harold Kuntzen. Setting out from the iminazoles obtained by the action of primary amines on trinitroacetylaminophenol, it was shown that imin-azolium iodides (I) can be obtained by heating the iminazoles with alkyl iodides, the resulting compounds being hydrolysable with the formation of the iminazolium hydroxides (11). The latter, on heating, lose water, and pass into quinone-imides (111), and on solution in alkali are transformed into the isomeric carbinols (IT): NO, N*X NO, N-X NO, N-X I I.p OA/\ ,C-Y \/\/ -+ \/\/”NO, N NO, N NO, N Z/\ iI Z/\OH 158 It was pointed out that compounds of the types I and I1 contain an asymmetric nitrogen atom of tho form O:N a b c, and should therefore be resolvable into optically active antipodes.The carbinol form (IV) also contains an asymmetric carbon atom, and should be resolvable. As the carbinols and iminazolium hydroxides are interconvertible, the interesting possibility is thus offered of transferring oplical activity from a, nitrogen to a carbon atom. Type I11 represents a new class of quinone-imide derivatives, for which the authors propose the name of imirzuaolones. The carbinols (IV) are named, in accordance with precedent, iminazolols. Several compounds of each series were described.186. (( Note on EL colour change in P-paranitrophenol brought about by sunlight.” By Thomas Vigond Barker. pNitropheno1 yields two modifications which have been examined crystallographically by the author (Zeitsch. Kryst. Min., 1907, 44, 159). The two modifications possess great similarity in the values of their prism angles; that they are quite distinct, however, follows from the observed transformation of one into the other on heating under the microscope. The transition temperature, if one really exists, has not been accurately determined, but the author’s observations would seem to point to a temperature of 63O, for a saturated toluene solution yields crystals of either modification according as the temperature is above or below 63O.That modifi- cation which appears at high temperatures will henceforth be termed a the other P. The a-modification is almmt colourless, being of a very pale lemon-yellow tint. The P-modification, on the other hand, is of a pronounced yellow colour; but on allowing it to remain for some time the crystals were found tlo acquire gradually a red tinge on the surface. The a-crystals, on the other hand, preserved their original tint. Experiments were theref ore made under varying conditions, and it was soon found that the red coloration appears only when the crystals are exposed to sunlight. The brighter the light the quicker is the change; in dull weather crystals may be exposed for many days without any appreciable change, whilst on a bright day the red coloration is apparent after an hour or so.Absolutely no change takes place if the crystal be kept in the dark. A tube which has been kept wrapped up in black paper presents no trace of chmge, even after a lapse of seven years. It was at first thought that the coloration might possibly be due to the formation of an ammonium salt. That this is not the caw 159 is proved by the fact that the change proceeds in a desiccator over sulphuric acid, and again when the desiccator is filled with hydrogen or carbon dioxide. The change, although quickly enough detected by the eye, must in reality be a very slow process, since crystals after some months’ exposure still present a yellow nucleus, and it is likely that the red material acts as a protection against further change by absorbing the aictinic rays.It b very remarkable that the a-modification is wholly unacted- on. Of this there can be no doubt, as the following will show. Solutions in water at the ordinary temperature yield crystals, the great majority of which are those of the P-modification, but, in addition, some crystals of the a-modification also appear. Owing to the similarity in habit, it is often impossible without an actual measurement on the goniometer to distinguish between crystals of the two modifications. The whole of one crop thus obtained was collected into a tube, and exposed to sunlight for some time; all the crystals with the exception of two turned red after a few hours.The action was allowed to proceed for a few months; but even after this prolonged treatment the two crystals still failed to show the slightest trace of change. They were there fore taken out, and measured on the goniometer, and proved to be crystals of the a-modification. A few of the red crystals selected at random proved on measurement to be those of the P-modification. Commercial p-nitrophenol consists of a mixture of both kinds of crystals, and on examination it will generally be found that some are red whilst others are not. The former are those of the &modification. Cases of colour change have previously been observed, but as far as the author is aware, no case has previously been discovered in which the change is restricted to one crystalline modification.At prAsent the usually accepted view with regard to polymorphous modifications is that the difference in crystalline form is not due to a difference in the chemical molecule, but rather in the different mode of packing of the molecules. The above remarkable difference of behaviour, however, of the two ‘‘polymorphous ” modifications of pnitrophenol would seem to argue for a difference in chemical structure; it is difEcult to see how a mere difference in the arrangement of the same chemical molecules should render one crystal structure immune to the action of actinic rays. It is therefore suggested that the chemical structures of the a-and R-modifications of p-nitroghenol ar0 different. 160 167.'' The sensitiveness of pentamminenitrosocobalt salts to light." By Oskar Krafft Heinrich Burger, In purifying the red variety of pentamminenitrosocobalt nitrate (Sand and Gender, Ber., 1903, 36,2083; Annden, 1903, 329, 194) by cryst,allisation from water, it was notided that the deep red solution is sensitive Lo light, and is slowly decomposed with the formation of nitric oxide and a green flocculent precipitate of cobaltous hydroxide. This decomposition cannot well be explained but by the assttmption that the red salt changes under the influence of light into thc black isoinoride considered, by Sand and Gender, to contain bivalent cobalt, and that the latter is then decomposed by the water. The reactiori may be represented by the equation : C%(NZoZ) (NH3)10(N03)4 + H2,0 = Co(OH), + 2NO + 4NH,NO, + 6NH,.If the solutioii is kept acid during the decomposition, the same quantity of gas is developed, but no precipitate is formed, the cobalt remaining in soiution as cobaltous salt. A similar decomposition is observed when a solution of the red salt is heated for some time. The development of gas is the same, but instead of the green, flocculent hydroxide a more compact, black cobaltous oxide is formed. That the decomposition in light is really due to the rays of light, and not to those of heat, is shown conclusively by the fact that the more refrangible end of the spectrum only produces ths reaction. A determination of the solubility in water of the red nitrate showed that one part of the salt dissolves in about twenty-five parts of water.For the purpose of identifying the gas evolved in the reaction, a few C.C. of an acidified solution of the red nitrate were placed on top of the mercury in a eudiometer, and subjected for several hours to the action of direct sunlight. It was found advan-tageous to have the solution acidified, because otherwise the gas bubbles become attached to the flocculent precipitate, and do not separate easily. The acid merely serves to prevent the formation of cobaltous hydroxide, otherwise the reaction proceeds in exactly the same way. The slow liberation of gas was the only sign of the change taking place. No variation of colour could be observed, as the colour of the red cobaltic nitrate in solution is almost the &me as that of a cobaltous salt.The gm evolved was proved to be nitric oxide. The following short account of a series of experiments Will givean idea of the velocity of the reaction. Four flat porcelain dishes of about 8 cm. diameter were charged with 10 C.C. each of a solution containing 1.620 grams of the red nitrate per 100 C.C. They were all exposed at the same time to direct sunlight (the sun being close to the zenith), and successively withdrawn at intervals of five minutes. The precipitate formed was colIected in the dark, the filtrate evaporated with sulphuric acid, and the cobalt’ sulphate weighed. 10 C.C. of the original solution contained 0.1620 gram of nitrate. 10 C.C.contained after 5 minutes’ exposure 0.0988 ,, 9, Jf?, 7, 9, 2, 10 ,, 0.0828 ,, J, 7, ¶¶ 9) 9, J?,, 15 ,, 0,0704 ,, 9, 9, 77 2, 20 9, ,, 0.0698 ?, 9, It is evident that the reaction slows down id9 the solution becomes more dilu,te, and the soluble products of the reaction (ammonia and ammonium nitrate) accamulate in the solution. The spectrum of the red solution shows only general absorption of the more refrangible part from the green onwards. As would be expected, only those rays that are absorbed will produce decomposi- tion. Solutions of the red nitrate of equal strength were exposed to sunlight covered with red, yellow, green, and blue glasses respec- tively. After several days’ expmswre, the solution under the red and yellow glass did not show any sign of decomposition, that under the green filter only a slight one, whereas the solution under the blue glass WM decomposed to a considerable extent.It wm suggested that the solution of the red nitrate might be used with advantage for the construction of a chemical photometer. 188. ‘‘Lecture experiment to illustrate dust exploaiona. The surface meas of certain finely-divided combustible solids.” By William Robert Lang and Hoges Lloyd. The following experiment serves as an illustration of the liability to explosion of the dust from starch and from coal when mixed with air. A glass cylinder, about seven feet long and four inches wide and open at both ends, is set up vertically, wires from an induction-coil being led through glass tubes into the middle of the chamber.Lycopodium, starch, and coal-dust, when allowed to fall into the tube and a spark passed through the mixture, ignite with explosive violence, the combustion being propagated throughout the length of the tube, ad the flames issuing a considerable distance from either end. Direct application of a, lighted taper produces the same result. With the view of arriving at some approximate idea of the total aurface of the combustible matter exposed to the air in such cases, the dimensions of the particles of the substaces employed were 162 ascertained by a microscopic examination, and the surfamazea per 100 grams of each calculated. In like manner, “pyrophoric carbon ” and pyrophoric iron were examined, and similar calcula- tions made.The results may be summasised w follows: Mean Total diameter of surface area for particles in 100 gramsSubstance. millime tres. of substance. Lycopodium .................................... 0 -028 20.92 square metres. Maize starch ................................ 0.0122 32-78 9, ?, Coal dust : {;: fimneedium .................. 0.012 33.33 )I 9, .................. 0.0016 250.00 ,,‘‘Pyrophoric carbon ” ..................... 0‘00125 332.00 ,, ,, ,,Pyrophoric iron ..............:.............. 0.0054 16-08 9, ¶# 169. The constitution of berberine.” By Charles Kenneth Tinkler. From an examination of the ultrwklet absorption spectra of berberine and its simple derivatives, evidence hzm been obt)ained of the existence of two modifications of the alkaloid in the did state.Berberine crystallised from water gives spectra in aqueous, alcoholic, and also in chloroform solution, which are identical with those of the berberine salts, and from this agreement the substance would appear to have an ammonium-base constitution it5 represented by formula (I) (compare Perkin, T~w~s.,1910, 97,321) : A solution of the substance containing alkali, however, gives spectra which agree closely with those of Freund and Beck’s methyl-dihydroberberine, and the same spectra itre given by a chloroform and an ethereal solution of berberinal, the substance precipitated by the addition of sodium hydroxide to an aqueous solution of berberinium hydroxide. This agreement cah only be explained by assigning to berberinal the carbinol formula (11),and the name berberinol is suggested for this substance: The transformation of berberinol into berberinium hydroxide is readily followed by means of the spectrmcope.Spectroscopic evidence wm also obtained in support of the view that the products of decompwition of berberinol by exctxm of alkali am dihydroberberine and oxyberberine. Since both modifications of the alkaloid can be obtained in 163 solution in chloroform, it appears that both the ammonium base and the carbinol exist in the solid state. In this respect berberine differs from the other substances that have been investigated in connexion with the carbind-ammonium base aldehydeamine isomerism, in which cases evidence of the existence of the carbinol form alone in the solid state has been obtained.170. Triketohydrindene hydrate. Part IV. Hydrindantin and its analogues.” By Siegfried Buhemana. Hydrindantin hw been shown to yield a red solution with sodium carbonate and a blue solution with sodium hydroxide (Trans., 1911, 99, 792). An examination of these shows that the red salt is a salt of hydrindantin, and the blue sodium compound is a chromo-salt of the hydrolytic product of hydrindantin, namely, hydroxy- diketohydrindene, C,H4<gg>CH*OH. This substance, which ia to be regarded as the analogue of dialuric acid, could not be obtained pure, because it is readily oxidised to hydrindantin. Owing to the close resemblance of hydrindantin to alloxantin, the violet barium ooinpound which this substance yields with baryta is to be regarded as a chromo-salt of dialuric acid, instead of alloxantin, The author also considers that isatide is an analogue of alloxantin, and that, therefore, it must be represented thus: ?RH4;->CE*O*C(OH)<C,H,*NHbo NH*CO (compare Heller, Ber., 1904, 37, 946). Further, it was found that dialuric acid does not unite with triketohydrindene hydrate to form an analogue of alloxantin, but that the acid reduces the triketone to hydrindantin.This substance is also produced from oximino- diketohydrindene, C,H,<g>C:NOH, by means of concentrated hydriodic acid; on using stannous chloride, instead of hydriodic acid, the analogue of uramil, namely, diketohydrindamine, c,H,<~~>cH~NH,, is formed.171. Aminoqnerce t in. ’’ (Preliminary note .) By Edwin Roy Watson. An aminoquercetim has been obtained from qnercetin by mm- pletely methylating to protect the moIecule, nitrating, reducing, and demethylating. 164 Nitropentamethylpuercetin, C,,H,O,(OMe),*NO,, prepared by dissolving pentamethylquercetin in cold nitric acid (D 1*4),crystal-lises from acetone in bright yellow, needle-shaped crystals, melting at 202-2crBo. Ami~opentarrLet?~yl~~ercetin,C,,H402~OMe),*NR2,prepared by reducing the nitro-compound with tin and alcoholic hydrochloric acid, crystallises from benzene in almost white, stout prisms, melting at 200-202°. Its hydrochloride crystdlises from dilute hydro-chloric acid in white, needle-sha-ped cryst'als, and its sdphate from dilute sulphuric acid also in white, needle-shaped crystals.An acetyl derivative crgstallises from alcohol and acetic wid in stout, white prisms, melting at about 223-226O. Amimoquercetin, C,,H,O,~OH),*NHz, is obtained in solution ;ts hydriodide on boiling either aminopentamethylquercetin or nitro- pentamethylquercetin with hydriodic acid (D 1.7). The free base is isolated in light yellow, needle-shaped crystals by decomposing its salts with pyridine and water. The hydrochloride, C,P, ,O,N,Ha, crystallises from dilute hydrochloric acid in yellow, fine needle- shaped crystals, the Ihydriodide from dilute hydriodic acid in orange- coloured warts, and the sulphate from dilute sulphuric acid in yellowish-brown warts.An acetyl derivative, crystallising from '&oh01 and acetic acid in white rhombs, melting at 151--1530, is obtained by acetylation of either aminoquercetin or ib salts; it is either the hex& or the hepta-acetyl derivative. Aminoquercetin dyes mordanted wool the following shades : brown on chrome, yellow-brown on alum, orange-red on tin, and brownish-black on iron. The shades are browner and deeper than corresponding dyeings with quercetin. In the course of this investigation, the following quercetin derivatives have also been prepared : Pemtamethy1puercetin hydrochloride, C20H,o0,,HC1, hydro-bromide, C,,H2,07,HBr, sdphate, C20Hz,07,HzS04, and nitrate, Cz,H,o07,HN0,.The first three of these oxonium salts are obtained in bright yellow, needle-shaped crystals on adding a concentrated solution of the corrssponding acid to a solution of pentamethylquercetin in glacial acetic acid, and the nitrate is obtained, also in bright yellow needles, by adding concentrated nitric acid to a solution of pentamethylquercetin in absolute alcohol. Il'mnztropentainethylquercetzr, C',,H20,(UMe),(N02)3, prepared by dissolving pentamethylquercetin in cold fuming nitric acid, is a canary-yellow substance, melting at 190--205°. Dibromopentameth~yluercetin, C,,5H*q02B~,(0Me),,prepared by 165 brominating pentamethylquercetin in glacial acetic acid solution, crystallk from alcohol or benzene in white, short prisms or leaflets arranged in sheavs, melting at 173-175O.Dibromopentamethylquercetin hydrob rornide, C,,H,,0,Br2,HBr, is obtained in bright yellow, needle-shaped crystals as an intermediate compound in the bromination of pentamethylquercetin. Dibromonitropentamethylpuercetin,C,,H,02Br2(OMe),-N02, pre-pared by dissolving dibromopentamethylquercetin in cold nitric acid (D 1*4), crystallises from alcohol or acetone in light yellow rhombs, melting at 173-175O. PentamethylquercPtindiazonium chboride, C,,HH,O2(0Me),=N2Cl,is obtained in bright yellow, needleshaped crystals on diazotising aminopentamebhylquercetin hydrochloride. Pentame thy1qu ercetindz‘aa onium sulpha t e separates in yellow, needleshaped crystals on adding dilute sulphuric acid to a cold saturated aqueous solution of the corresponding diazonium chloride.PentamethyZquercetinazo-P-.naphthot, C,,H,02(OMe),*N2~C,,H6*OH, prepared by mixing an alkaline solution of &naphthol and a solution of pentamethylquerceti~~diazoniumchloride, crystallises from glacial acetic acid in deep crimson, needle-shaped crystals, melting and decomposing at 211O. The amincwgroup in aminoquercetin is probably in the catechol nucleus in that position which is para- with respect to one of the hydroxyl groups and meta- to the other, but experiments are in hand to determine its position definitely. Experiments are also in progress to convert aminoquercetin into the corresponding hydroxy- quercetin, and from the. compounds now described to prepare other derivatives with dyeing properties. 172.‘( The reduction of nitroacenaphthene.’’ By Holland Crompton and Maggie Walker. The methods suggested by Quincke (Ber., 1888, 21, 1454) and by Graebe (Annulen, 1903, 327, 81) for the reduction of nitroace-naphthene are slow, and were not found to give good yields of aminoacenaphthene. Better results were obtained on using zinc dust and water as a reducing agent Nitroacenaphthene is mixed intimately with about five times its weight of zinc dwt, and sufficient water is added to form a thin paste. The mixture is heated for ten hours on a water-bath, then dried at about 60°, and extracted with light petroleum. The amincl acenaphtheno obtained on distilling off the solvent is slightly brown, 166 owing to the presence of a small quantity of a brown-coloured by-product, which has not been further examined. It can be purified by treatment with dilute sulphuric acid.It is best to crystallise out the sulphate, as this salt is more stable on exposure to air than is the free base. The yield in the above process is about 60 per cent. of the theoretical. 173. (‘Epicamphor : a new isomeride of camphor’.” (Preliminary note.) By Frederick Russell Lankshear and William Henry Perkin, jun. Two ketederivatives should be obtainable from camphane, namely : CH2*CH--CH2 CH,*CH--CO and CMe,I I I I CH,*CLMe-CO UH,*(!?Me--UH, Camphor. Epicamphor. and of these the second, for which the name epkamphor is proposed, has not yet been described.Owing to the interest attaching to this substance, one of the authors has for some years attempted to prepare it, but, until recently, without success. It may be obtained by the following series of reactions. Cmphorcarboxylic acid (I) is converted by reduction and subsequent elimination of water into bornylenecarboxylic acid (II), and the authors have observed that this. acid is converted by reduction with palladium and hydrogen quantitatively into camphaiiecarboxylic acid (111) (compare Bredt, Anmlen, 1909,366, 60). This saturated acid is readily brominated when its chloride is warmed with bromine on the steam-bath, and the bromclesjter obtained by pouring the bromcsacid chloride into alcohol is next digested with potassium acetate in acetic acid solution, After hydrolysis with alcoholic potassium hydroxide, the a-hydroxycamphanecarboxylic acid (IV) is oxidised by lead peroxide, permanganate, or also by chromic acid, and, in each cw, small yields of epicamphor are obtained.CH,*CH-C-CO,H II llYMe2CH,=CMe--CH CH2*CMe--bH2 (111.) 167 Epicamphor is readily volatile in steam, has the same odour as camphor, and is remarkably like this substance in almost all its propertiesi; it melts at about 165O, but this melting point, as well as the others mentioned in this paper, will be carefully revised when larger quantities of material are available. Found : C =78.3; H=10.5. C2,H,,0 requirea C=79.0; H’=10.4 per cent. Epicamphoroxime melts at about 102O, and has the sitme odour as camphoroxime, which melts at 119O.(Found, C=72-3; H=10-4; N=8*6. C,,H,,ON requires C-71.8; H=10*2; N=&-4per cent.) Epicarnphor~emicarLazone separates from benzene in flocks and from methyl alcohol in glistening needles, and melts at 225-227O with effervwcence, whereas cnmphorsemicazbazone melts at 236-238O. (Found, N =20.1. Cl1H1,ON, requires N =20.1 per cent.) The authors intend to prepare a number of derivatives of epicamphor with the object of comparing them with the correspond- ing derivativee of camphor. ADDITIONS TO THE LIBRARY. I. Donations. Blucher, H. Modern industrial chemistry. Translated by J. P. Millington. pp. xvi + 779. ill. London 191 1. (Refrence.) From the Publishers : The Gresham Publishing Company.Edge,John Harold. Notes on practical cotton finishing. pp. 103. ill. London 191 1. (Rccd. 9/5/11.) From the Author. Fowler, Gilbeyt John. An introduction to bacteriological and enzyme chemistry. pp. viii+ 328. ill. London 1911. (Recd. 26/5/11.) From the Author. Korner, Wilhdm. Uber die Bestimmung des chemischen Ortes bei den aromatischen Substanzen. (Ostmald’s Klassiker, No. 174.) Leipzig 1910. (Recd. 30/5/11.) From the Author. Ostwald, Wilhelm. Introduction to chemistry. Authorized transla- tion by William T.Hall and Robert S. Williams, pp. ix+ 368. ill. New York 1911. (Recd. 28/4/11,) From the Publishers : Messrs. John Wiley and Sons. 168 11. By Purchase. Bang, Ivar. Chemie und Biochemie der Lipoide.pp. xi+187. Wiesbaden 1911. (Recd. 17/5/11.) Hopkins, Cyril George. Soil fertility and permanent agriculture. pp. xxiii + 653. ill. Boston 1910. (Recd. 25/5/11 .) May, Percy. The chemistry of synthetic drugs. pp. xiiif289. London 19 11. (Recd. 25/5/11.) Roberts-Austen, Sii* William Chandler. An introduction to the study of metallurgy. 6th edition, revised and enlarged by F. W. Harbord. pp. xv + 478. ill. London 19 10. (Recd. 25/5/11.) Thiel, A. Der Stand der Indikatorenfrage. Zugleich ein Beitrag zur chemischen Theorie der Fstrbe. (Sammlung, Vol. XVI.) Stuttgart 1911. Tutton, AlJred Edwin Howard. Crystallography and practical mensurement. pp. xiv + 946. ill. London 1911. (Recd. 25/5/11.) Wehmer, C. Die Pflanzenstoffe.Chemische Bestandteile und Zusammensetzung der einzelnen Pflanzenarten, Rohstoff e und Produkte. pp. xvi + 937. Jena 191 1. (Recd. 17/5/11.) Werner, A. New ideas on inorganic chemistry. Translated by Edgar Percy Hedley. pp. xvi+ 268. London 1911. (Bed 25/5/11.) Zeitschrift fur angewandte Chemie, General Register. Jahrgiinge 1887 bis 1907. Edited by Berthold Rassow and Ernst Wovgang Muller. pp. iv + 609. Leipzig 1910. (Rqference.) 1x1. Pamphlets. Autenrieth, Wilhelm, and Tesdorpf, Theodor. U ber eine kolorimetrische Bestimmung des Traubenzuckers im Ham. (From the Miinch. med. Woch., 1910, 37.) Beck, Karl, and Stegmiiller, Ph. Uber die Loslichkeit von Bleisulfat und Bleichromat fur sich, in Gemischen und in Form von Olfarben in verdunnter Salzsaure, sowie uber das Gleichgewicht von Chromat und Bichromat in Losung.(From the Arb. K. Gesundh.-Arnt, 1910, 34.) Calliess, Franx W'ilhelrn. U ber Ephedrin und Pseudoephedrin. (From the Apoth. Zeit., 1910, 25.) Clacher, William. Some notes on animal charcoal. (From the Int. sugar J.,1910.) Comanducci, Exio. Tallochinina. pp. 7. Napoli 19 10. Coventry, Bernard. Report on the progress of agriculture in India for 1909-10. pp. 106. Calcutta 1911. Dibdin, William Joseph. Notes of lecture on mortar and cement. pp. 32. London 1911. 169 Fischel, Riclard. Der histochemische Nachweis der Peroxydase. (From the Wien. klin. JVoch., 1910,23.) Forssner, Gunnar. U ber die Einwirkung des Nahrungsfettes auf die Acetonkorperausscheidung.(From the Xkand. Archiv. Physiol., 1910,23.) Fouard, Eugone. L'etat colloidal de l'amidon et sa constitution physicochimique. pp. 147. Lava1 1911. Gaebel, Gustaw Otlo. Das Reischauersche Titrationsverfahren zur Bestimmung des Harnzuckers. (Prom the Apoth. Zed., 1910, 25.) Gazzetti, C., and Sarti, C. Intorno ad una reazione rossa del reattivo di Esbach. (From the Arch. farm. sperim. Xci., 1910, 9.) Uray, George. On the dissolved matter contained in rain water collected at Lincoln, New Zealand. (From the Canterbury Agyic. Coll. Mug.,1910). Hamalainen, Juho. U ber das Schicksal des Cineols (Eukalyptols) im Organismus. (From the Skand. Arch. Physiol., 1910, 24.) Hamalainen, Juho, and Sjostrom, Lennart. Uber den Umfang der Glykuronsaurepaarung bei enzymimmunisierten Kaninchen.(From the 87caud. Arch. Physiol., 1910, 24.) Henderson, Velyen E. Hemmung der Wirkung chemischer Muskelreize durch Anelektrolyte. (From the Zentr. Physiol., 1920, 24.) Javillier, M. Sur les silicotungstates de conicine, de sparthine et d'atropine. (From the Bull. Sci.Phara., 1910, 17.) Kinoshita, Tosaku. Uber das Auf treten und die quantitative Bestimmung des Trimethylamins im menschlichen Ham. (From the Zentr. physiol., 1910, 24.) Lauder, Alexander, and Fagan, T. W. The variation in the composition of milk. Fifth annual report. pp. 42. Edinburgh 1911. Loew, Oscar. U ber die physiologische Rolle der Kalziumsalze; (From the Munch.Med. Woch. 1910.) Uber die Wirkung von Strontiumsalzen auf Algen.(From Flora, 1911, 102.) Loew,Osaar, and Bokorny, Fh. Aktives Eiweiss und Tannin in Pflanzenzellen. (From Flora, 1911, 102.) Miculicich, Miroslnv. Uber den Einfluss von Elektrolyten und Anelektrolyten auf die Permeabilitat der roten Blutkorperchen. (From the Zentr. Phpiol., 1910, 24.) XOreau, B.Ana'lyse quan'titacive a"un mglange ae seJs, de recherche particulihment difficile. (From the Bull. Sci.Pharrn., 1910.) Pohl, Juliw. Experimenteller Beitrag zum Oxalsaurestoff wechsel. (From the Zeitsch. exp. Path., 1910, 8.) 170 THE FARADAY LECTURE. The Faraday Lecture, entitled, ‘(The Fundamental Properties of the Elements,” will be delivered by Professor Theodore W. Richards, of Harvard University, on Wednesday, June 14th, 1911, at 8 p.m.The Lecdure will be given, by the kind permission of the Managers, in the theatre of the Royal Institution, 21, A1bema.de Street, W. Admission will be by ticket only. Each Fellow of the Society is entitled to two ticketsi which may be obtained on application to the Assistant Secretary, Chemical Society, Burlington House, W. At the next Ordinary Scientific Meeting on Thursday, June lSth, 1911, at 8.30 pm., there will be a ballot for the election of Fellows, and the following papers will be communicated : “The alleged complexity of tellurium.” By A. G. Vernon Harcourt and 13. B. Baker. “The purification and properties of acetic acid.” By W. R. Bowfield and T. M. Lowry. “ Cupriglycollates.” By S. U. Pickering. “The solubility of carbon dioxide in beer.” By A.Findlay and B. Shen. “ An addition to the Buchner funnel.” By A. c‘. G.Egerton. “ Polymorphic phthalylhydrazides.” By F. D. Chattaway and D. F. S. Wunsch. “ The decomposition of hydrazides and hydrazones by heat.” By F. D. Chattaway, C. Cumming, and B. H. Wilsdon. “ Note on gum kino.” By J. L. Simonsen. “ The action of ammonia and amines on 2-phenyl-1 :3-benzoxazine 4-0110.’’ By A. W. Titherley and E. C. Hughes. “Electromotive forces in alcohol. Part I. Concentration cells with electrodes reversible to chlorine ions.” By A. Lapworth and J. R. Partington. “ Some oxidation products of the hydroxybenzoic acids. Part 111.” By A. G. Perkin. 171 CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT.N B.-The names of those who sign from ‘‘ General Knowledge I> are printed in italics. The following- Candidates have been proposed for election. A ballot mill be held on Thursday, June 15th, 1911. Atkine, Ernest Andrew, 71, East Hill, Wandsworth, S.W. Pharmaceutical Chemist. Have had one year’s experience as Student in Laboratory, and also have studied successfully for Minor and Major Pharmaceutical Qualifications. Am desirous of keeping up-to-date in my knowledge of pure Chemistry, more especially in its application to Pharmacy. James D. Kettle. Alsxarrder Scott. C. F. Baker. John W. Heath. C. Edwd. Sage. 8. Bosworth. Atkinson, Norman Ernest, Ash Cottage, Thornhill Lees, Dewsbury. Works manager. Six years Portland Cement Works’ Chemist.At present, Manager of Calcium Carbide Works. Walter M. Gardner. Walter F. Reid. A. Battye Knaggs. H. S. Raper. €lurker North. Blrtckhurst, Arthur Owen, ‘(Downing,” Broughton, Preston. Agricultural Demonstrator. I am desirous of keeping in touch with chemical developments. National Diploma in Agriculture (N.D.A.). A first-class Certificate granted by the Board of Education in the Advanced Agricultural Chemistry Section of the Agricultural Science Examination. Research work on manurial residues of crops for the Potash Syndicate, and in Black Scab of Potatoes for the Board of Agriculture. R. Henry Jones, John Robinson. Allan Baguley. Hurold B. Dixm, Ch. Weizmann. 172 Bradshaw, George Arthur, 28, Raymond Street, Bury, Lancs.Teacher of Chemistry, MSc. Degree in Chemistry, Victoria University of Manchester, 1908. 1908-9 Science Master, The College, Kilkenny, Ireland. Since 1909 Chemistry Master, the High School, West Leeds. Harry Ingham. Harold B. Dixon. Geo. M. Norman. E. C. Edgar. Ch. Weizmann. Cooke, Charles Ernest, 35, Sebert Koad, Forest Gate, Essex. Representative of Messrs. J. and R. Griffin, Ltd., Manufacturing Chemists, Kingsway, London. Studied Chemistry at Royal College of Science and at the Kartley University College, Southampton. In 1908 wits Science Master at the Grammar School, Shoreham, Sussex. Chas. W. Truelove. M. 0. Forster. D. R. Boyd. G. T. Morgan. W. Godden. Clarke, Arthur Frederick, 12, Pork Avenue, Gillingham, Kent.Teacher and Lecturer at Gillingham Technical Institute. Desirous of coming in touch with current scientific literature. R. C. Farmer. H. R. Redman. W. H. Gibson. Robert Robertson E.G. Cou;zens. Cowling, Thomas, Easingwold, Yorks. Teacher. For three years Chemical Student, University College, Nottingham. Hold First-class Certificates in Advanced Chemistry from Board of Education. Interested in Chemical research. Frederick Cowling. A. H. Salway. John Thomas Fox. F. Tutin. Harold Bog arson. Datta,Ganesh, Dora Ismail Khan, N. W.F.P., India. Barrister-at-law and Advocate, Chief Court, Lyallpur. B.A. (Punjab Univ.) ;M.R.A.C. (Cirencester, England), etc. Graduated in Arts at the University of the Punjab, India, in 1904.Obtained Honours Diploma OF Membership at the Royal Agricultural College, England, in April, 1909, after nearly three years' study. Subsequently studied science and practice of dairying at different institutions in England. 173 Am landowner, manager of my farm8, and interested in promoting scientific agriculture. E. F. Harrison. Ruchi Ram Sahni. P. D. Sabherwkl. Hari Prasad. Puran Singh. Demuth, Rudolph , 68, Salushury Road, London, N.W. Chemical Technologist. Studied at University of Marburg and Imperial Polytechnicurn, Charlottenburg. I was engaged by the Cape Government in experimental work connected with Rinderpest- epidemic, especially in regard to the production of chemical anti septics and disinfectants for use in connexion with that and other infectious diseases of cattle.I have also been engaged in Agricultural and Horticultural researches of a chemical nature. In the field of Hygiene I have worked and produced useful apparati-now universally in use, etc., etc. Peter NacEwan. Alfred Gordon Salamon. Thos. Tyrer. J. Lewkomitsch. George T,Holloway. Gardner, Edgar Harold, 34, Salisbury Avenue, Colchester. Schoolmaster. Student of Chemistry with the idea of becoming a teacher of the subject. Inter. B.Sc. (Lond.). Engaged with Mr. Neville on Stereoisomeric research for some time. H. A. D. Neville. Will. T. Boone. A. W. Nunn. H. P. Wilson. A. E. Barker. Ghose, Joges Chandra, Bhagalpur, Eehar, India. Professor of Chemistry, T.N.J.College, Bhagalpur. M. A. in Chemistry, Class 11. ;worked for two years in the Presidency College Chemical Laboratory under Dr. P. C. Rby, D.Sc., Ph.D., and Mr. Cunningbam, M.A., F.C.S., A.R.C.S.I. Lecturing on Chemistry for four years. Atul Chandra Ganguli. PunchGmalz Neogi, Y.c. Rky. Chuni La1 Rose. Bidhu Bhushan Dutt. Jatindranath Sen. Gonville, Cyril Herbert Koszelski, F.R.B.S. (London),‘‘Milton,” Queen’s Koad, Buckhurst Hill, or 63, The Broadway, Stratford, Essex. Colouring Specialist ;Joint Inventor of a new chemical process for making Caramel. Technical Chemist. Have done considerable work 174 both in the Study of Chemistry and its Practical Application in Manufacture. Worked out and invented an improved process for Caramel and also for priming Beers, etc.Studied Chemistry both privately and publicly, :he latter at Sir John Cad Institute, and the Chemistry of Brewing under Mr. Ling and under Dr. Harden for Micro-biology. John Heron. Arthur R. Ling. Charles A. Keane. Arthur Harden. H. Burrows. F. R. Holloman. Goold, Rowland Lewis, 5, Corporation Street, Birmingham. Registered Patent Agent (by Examination). Associate of the Institution of Electrical Engineers. I am a Patent Agent practising in the firm of Lewis Wm. Goold. In the department of my business relating to Chemical Science I have been engaged in the investigation of principles and analogies in the Chemistry of new manufactures tendered as subject for Letters Patent. I now have the responsible conduct .of practically all the more important and more technical of the chemical and cognate matters with which my firm from time to time has to deal.I desire admission to the Society in order that I may follow more closely the progress of Chemical Science. W. R. Bousfield. Douglas F. Twiss. T. Slater Price. Arthur Colef ax. E. A. Tyler. Joseph,Edward Lionel, 96, Victoria Street, S.W. Managing Director of Ozonair, Limited. Consulting Engineer. Member of the Institution of Electrical Engineers. Inventor and Patentee of about 100 Inventions and Processes connected with Ozone in its various applications, etc., etc. Leonard Temple Thorne. William A. Tilden. W. H. Simmons. J.C. Cain. W. Gordon Carey. Linenbroker, Henry Edmund, 100, Harrow Road, Paddington.Wholesale Chemical Manufacturer. Principal of ’‘ The Imperieux Laboratories.” Intent to advance in Chemical Science. Author of ‘‘ Blue Book Recipes on Scientific Colouring ” ; Author of “Das Brevier der Haarfarben Chemie.” Contributor to various periodicals. John T. Furnell. William A. Colebourn. Frank E. Weston. w.H. CdieT. J, Cruickehnnk Smith, 175 Ling, Herbert JameB, Hankow, China. Chemist (Director Hankow Disp., Ltd.). Pharmacist. Investiga-tions include Chinese Wood Oil, Chinese Bean Oil, Rhubarb, etc. Desirous of keeping in touch with modern research upon these nubjects. E.J. Millard. Thomas Tyler. John C. Eewlett. Peter ittacEwan. E.E.Robing. Merriman, Richard William, 244, Victoria Park Road, South Hackney.Demonstrator in Chemistry, Guy’s Hospital Medical School. M.A. Cambridge, Natural Science Tripos, Parts I and 11. Joint Author with Dr. S. Ruhemann of (a)‘‘ Ths Action of Phenylpropiolyl Chloride on Ketonic Compounds” (Trans., 1905, 87, 1384); (b) “Tetrazoline. Part I11” (Trans., 1905, 87,1768). Joint Author with Dr. J. Wade of “The Correction of the Specific Gravity of LiqUidg for the Buoyancy of Air” (Trans., 1909,95,2174). S. Ruhemann. J. T. Hewitt. John Wade, F. G. Pope. Horace Finnemore. Paul, Felix Gabriel, M.R.A.S.E., No. 64, 38th Street,, Rangoon, Burma; Superintendent of Land Records, Burma; at present on leave in England. Calcutta University Entrance Examination ; Clerkship Examination of Burma ; Higher Survey Examination for the appoint- ment of Land Records officers in Burma.Has experience in the investigation of Chemical Science, especially in connexion with agri- cultural and other lands in Burma, and the treatment and classification of soils as a Survey and Revenue assessment officer under the British Government for several years. E. Towyn Jones. Clarence A. Seyler. J. A. Hatfield. E. A. Tyler. John Williams Bevan. Pitt, Leonard Ison, 109,Abbott Road, Bromley, London, E. Schoolmaster. Studied Science for four years at the East London College, and obtained First Class Hons. in Chemistry at the London B.Sc. Examination in Oct. ’08. Science Master at Stamford School since May ’09. J. T. Hewitt. Clarence Smith. F. G.Pope. A. D. Mitchell. F. S. Long. 176 Walton, Willam Keighley,‘‘ Beechwood,” Upper Rushton Road, Thornbury, Bradford. Analytical Chemist. Since 1903 with I?. W. Richardson, F.I.C., City Analyst, Bradford, and West Riding County Analyst, Yorkshire, as chief assistant. Joint author of paper on “Analysis of Camphorated Oil for Camphor Substitutes,” Analyst, 1908. Later as Research Chemist to Messrs. Richardson and Jaff6, Analysts, Bradford. Conjoint autbor with Mr. Richardson of paper on “Composition oE Turkey Red Oil,” shortly to be read. F. W. Richardson. George H. Martin. A, Jaff4. GeoErey A. Bracewell. Walter a. Gardner. The folloming Certificate has been authorised by the Council for presentation to Ballot, under Bye-law 1. (3). Gallsworthy, Benjamin, Thilawa, Rangoon.Oil Refiner. At present Chief Refiner to the British Burma Petroleum Co. ;previously Chemist to the Indo Burma Petroleum Go., Ltd., and for many years engaged in Chemical work in the Indian Leather Industries. H. V. -Mitchell. J. T.Hewitt. R CLAY AND SON<, L’rD., I\RllNJWICK ST., SPAXFORU h’l’., 4 E., AND BUNUAI, SUFI’ULK.
ISSN:0369-8718
DOI:10.1039/PL9112700147
出版商:RSC
年代:1911
数据来源: RSC
|
|