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Proceedings of the Chemical Society, Vol. 16, No. 221 |
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Proceedings of the Chemical Society, London,
Volume 16,
Issue 221,
1900,
Page 65-76
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PAGES MISSING FROM 1 TO 64 Tssued 22/3/1900 PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE XECRETARZES. Vol. 16. No.221. March Sth, 1900. Extra Meeting. Professor TRORPE,F.R.S., President, in the Chair. Professor WARINUTON,F.R.S., delivered a Lecture on Recent‘I Researches on Nitrification.” During recent years, the chief investigations on the character and properties of the nitrifying organisms have been carried out in Winogradsky’s laboratory in St. Petersburg, none having been exe- cnted in this country. Formerly, investigators had been unable to obtain pure cultures of the organisms ;their chemical characters had, however, been studied, as their capacity for growth in a purely mineral solution allowed of their separation from most of the other organisms in the soil.It had been found that the process of nitrifi-cation consisted of two distinct pieces of chemical work, effected by two agents, which could be separated from each other ; by the first (the nitrous organism), ammonia was converted into a nitrite ; by the second (the nitric organism), the nitrite was oxidised to nitrate, These facts were first ascertained at Rothanisted. To isolate the nitrous organism from soil, Winogradsky commences by a series of cultures in an inorganic solution containing an ammonium salt and the ash constituents of plant food. From this solution, cultivations on solid media are started. For some years, silica jelly was employed, but Omhliansky now prefers plates of magnesia-gypsum saturated with the mineral solution already men- tioned.To isolate the nitric organism, the preliminary cultures are made in a solution containing sodium nitrite and ash constituents. As a solid medium, purified agar, with nitrite and ash constituents, is made use of. The fermentable constituents of the agar have been previously removed by Beyerinck’s method. Winogradsky has examined soils from many parts of the world. He finds but one nitrous and one nitric organism in any soil. The nitric organism is everywhere the same species. The nitrous organism may vary. In Europe, N. Africa, and parts of Asia, the same species occurs, with variations in size, and in tendency to adopt a zoeglcea or motile condition; the latter condition displays the great,er chemical energy.The nitrous organism from Java is a dis-tinct species, having an extraordinarily long flagellum. The organism from S. America and Australia is generically different ; it is a giant coccus. A few other investigators have described different nitrifying organisms, but the evidence adduced has in some cases proved erroneous, and is in other cases as yet insufficient to warrant its acceptance. Winogradsky had proved by quantitative experiments that the nitrous organism derives its carbon from carbonic acid ;the nitric organism possesses the same power. As both organisms flourish in darkness, the energy necessary for the construction of organic matter out of carbon dioxide and water is apparently derived from the oxida- tion, respectively, of ammonia or a nitrite.Later experiments have shown that the carbonic acid is, in every case, probably taken from a supercarbonate. The nutrition of the bacteria which exist with the nitrifying organisms in a mineral solution requires further study. Stutzer states that his hypomicrobium grows in a mineral solution, and needs carbonic acid for its nutrition, yet possesses no nitrifying power ;its source of energy requires explanation. The refusal of the nitrifying organisms to grow on gelatin, and on most organic media, is well known. Winogradsky and Omhliansky have lately studied the influence of various kinds of organic matter on the nitrifying process. The presence of 0.5 of glucose in 1000 of liquid is sufficient to retard the action of both the nitrous and nitric organism, while about 2 per 1000 entirely prevents nitrifica- tion, Glucose has thus as great an influence upon the nitrifying organisms as phenol has on ordinary bacteria.Of simpler forms of organic matter, as sodium acetate, a much larger quantity is required to hinder nitrification. The influence of ammonia in preventing the action of the nitric organism is very remarkable ; 5 parts per million was sufficient to retard its action, and 150 parts per million prevented it altogether, a proportion which is comparable with an effective dose of mercuric chloride. It seems, however, probable that an increase in the quan- tity and energy of the nitric organism enables it to bear a some-what greater quantity of ammonia. It appears from careful trials that the nitrifying organisms are without action upon nitrogenous organic matter ;even methylamine is unaffected by them.For nitrification of organic matter to take place, the aid of other organisms is necessary to decompose it and bring the nitrogen into the form of ammonia. The behaviour of the nitrifying organisms towards organic matter and ammonia is of great practical importance. The lecture was illustrated by lantern slides, and by a number of specimens of pure cultures on solid media, sent by Professor Wino- gradsky from St. Petersburg. The principal publications referred to will be found in Tyans. Chenz. Xoc., 1891, 59,484;Archives des Sciences biologiques, 1and '7; Cent.Bakt., 1899, 2, 653 ;Mitt, Lnndw. Institute Breslcm, 1,75 ; 2, 197 ; Compt. rend., 1899, 128,566. On the motion of Sir W. T. THISTLETOWDYER,seconded by Dr. HUGOMULLER,a vote of thanks was pitssecl to Professor Waring- ton for his lecture. March 15th, 1900. Professor THORPE,F.R.Y., President, in the Chair. Nessrs. A. H. Bennett, A. W. Harvey, and H. W. Cook were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs, Heinrich Rowland Beringer, 11, Dolcoath Road, Camborne ; John Richard Brooke, 20, Aberdeen Park, Highbury, N.; Arthur Brand Chater, 65, Queen Street, Brisbane ; Nicholas Cullinan, ftisca, Illonmouthshire ; John Cussons, 4, Mount Pleasant, Portmadoc ; William Donald, Saltcoats, Ayrshire ;Frederic Richard Ellis, 15, Elton Road, Bishopston, Bristol ; Thomas FitzGibbon, 1, Clyde Cottages, Ilford ; James Herbert Hagnes, 73, Brynland Avenue, Bishopston, Bristol; Thomas Ltmb Lockhart, Johannesburg, Transvaal.The following letter, addressed to the President, has been received from Professor van't Hoff, in acknowledgment of the congratulations sent to him by the Officers and Council on the occasion of the celebra- tion, in December last, of the completion of the 25th year of his Doctorate : CHARLOTTENBURG,20th Februccry, 1900. MY DEAR COLLEAGUE, Still engaged in answering the congratulations I received on the occasion of my Jubilee, I now come again to those from the Chemical Society of London, which reached me through the kind intervention of you and Professor Dunstan.1 pray that you will convey my feelings of gratitude to the Society, which has so recently admitted me as one of its Foreign Uembers. I am, yours truly, J. H. VAN’T HOFF. Of the following papers, those iiiarked * were read. *43. “The vapour densities of dried mercury and mercurous chloride.” By H.Brereton Baker, M.A. The vapour density of ammonium chloride has already been shown to be normal when carefully purified and dried (Tw~as.,1894, 65, 615; 1898, 73, 425), pointing to the fact that moisture is necessary for the dissociation of this substance. Experiments have been tried with purified and dried mercurous chloride with the view of finding out if it behaved in a similar way when vaporised.The determina- tions were made with a specially devised modification of Victor Xeyer’s apparatus in an atmosphere of nitrogen at 448’. The mean of five determinations gives a vapour density of 217.4. h determina-tion of the vapour deusity of the undried substance in the same apparatus gave 118.4. Dried mercurous chloride did not give gold amalgam when gold was heated in its vapour. Under the same conditions, the gold amalgam was obtained with the incompletely dried chloride. Very dry mercuroos chloride therefore would seem to have the formula Hg,Cl, at 448’. Similar experiments were made with carefully purified and dried mercury at 448’. The mean of three determinations in an atmo-sphere of nitrogen was 108.1, so thzt the molecule of dried mercury is probably monatomic at this temperature.DISCUSSION. 31r. D. HOWARDsaid that prolonged experience in the sublimation of large quantities of mercurous chloride had shown that the presence of vapour of water seemed to determine the corrosive action of the vapour on iron, and that the behaviour of the vapour of the chloride in the coin- paratively imperfect dryness obtainable on a large scale, suggested n, true sublimation rather than dissociation. Professor DEWARremarked that it might interest the Society to know that Lord Rayleigh had recently found liquid air to be an effective desiccating agent as compared with phosphorus pentoxide, and that shortly the results of new determinations of the density of hydrogen thus dried would be communicated to the Royal Society.Professor MCLEODpointed out that it would be interesting to know the quantity of water which would be sufficient to cause the complete dissociation of the heated mercurous chloride, for if the quantity were known it might be possible to ascertain the mechanism of the change. *44.‘‘The preparation of pure hydrobromic acid.” By A. Scott. The author recommends the employment of sulphurous acid as a better and more convenient agent for preparing hydrobromic acid from bromine than amorphous phosphorus, even when purified from chlorides as Stas recommends. Almost all samples of phosphorus con- tain arsenic to a certain extent, and this, by the action of the bromine, becomes arsenious bromide which distils over with the hydrobromic acid, giving rise to arsenites and arsenates in the bromides prepared from acid madein this way.By distillation two or three times, the hydrobromic acid is easily separated from the sulphuric acid formed at the same time, but it is always safer to add a little barium bromide before the final distilla- tion, The purity of the acid was all that could be desired ;this was shown by preparing from it some pure potassium bromide and titrating it against pure silver with all Stas’s precautions, when its equivalent was found to be 119.099 (Ag= 10’7.93). Similar determinations with potassium bromide from hydrobromic acid prepared as recommended by Stas (Bzcvres, 1, 842) and by J.P. Cooke (Squibb’s process) (Pmc. Anaer. Acad., 1881, 17,31) gave 119.099 and 119,102 respec- tively. Stas’sown number (mean of 14 experiments) is 119.095. *45. u A new sulphide of arsenic.” By A. Scott. When phosphorus containing (as it almost always does) small quantities of arsenic is oxidised by nitric acid and the solution boiled down, at a certain degree of concentration the liquid becomes brown provided too much nitric acid has not been used. This brown colour, as has long been known, is due to the separation of metallic arsenic by the reducing action of the phosphorous acid present. If, before the concentration has been carried so far, the liquid be diluted and sulphur dioxide passed into it and then warmed, a yellow precipitate of arsenic trisulphide is obtained, caused by the reduction of the sul-phurous acid to hydrogen sulphide by the phosphorous acid.This reaction may be usel as a test for arsenates by adding a few drops of phosphorus trichloride to the solution, then some sulphurous acid, and warming, when the yellow precipitate is obtained at once. If, however, these substances be allowed to react at ordinary tem- peratures, a dark brown precipitate is obtained which consists almost entirely of a new arsenic sulphide having the formula As@. This may be freed from the sinail quantity of trisulphide usually formed at the same time by repeated treatment with ammonia solution into which a little hydrogen sulphide has been passed. This new sulphide is unattacked by ammonia, colourless ammonium sulphide, or carbon disulphide, but dissolves in yellow ammonium sulphide and is attackell by potash solution, giving a dark brown substance exactly like that obtained by Berzelius by the action of potash solution on realgar.*46. (6 The action of iodine on alkalies.” By R. L.Taylor. In the present paper, the author describes experiments using iodine in much stronger solutions-decinormal-sixty times the strength of the aqueous solution previously used by him (Menz. Lit. & Phil. SOC. -JIctnch.,lS97,41, VIII.). Using Schwicker’s method, he finds that if the requisite quantity (or more) of alkali is added to a decinormal solution of iodine and then a bicarbonate iinnzedichtely added, from 88 to 94 per cent.of the iodine is liberated, and therefore that amount of tlie iodine had reacted with the alkali to form hypoiodite and iodide. By allowing different short intervals to elapse between the mixing of the alkali and iodine and the addition of the bicarbonate, he finds that the hypoiodite decomposes with great rapidity even at the ordinary temperature. The stability of a hypoioclite, in fact, depends upon its dilution, and this accounts for the definite results obtainable with very dilute solutions and the previous failures to obtain satisfactory evidence of the formation of hypoiodite when strong solutions of iodine, or the solid itself, have been used. The iodine used was in solution in potassium iadide, the only effect of using varying amounts of which was to vary the amorint of alkali required to complete the reaction, as might indeed be surmised from the fact that the reaction is a reversible one.The author concludes that the action of iodine upon alkalies in the cold is always the same in the first instance, namely, the formation of hypoiodite and iodide, and that the hypoiodite decomposes more or less rapidly, according to the concentration, into iodate and iodide. *47. ‘‘ The interaction between sulphites and nitrites.” By Edward Divers and Tamemasa Haga. The interaction of a nitrite with sulphurous acid or a sulphite, usually regarded as complicated, is really very simple. Nitrous acid, in the form of nitrous fumes, is entirely taken up by a solution of a pyro-sulphite with the production of a tmo-thirds normal hydroximido- sulphate, thus HONO + (KSO,)SO,K =HON(SO,K),. If the normal sulphite be used, the reaction is 3HONO + BK,SO, =2KN0, + OH, + HON(SO,K),.Sulphurous and nitrous acids themselves may be used to show the nature of this interaction, and to prove that neither the base of the nitrite nor the sulphite takes any part in the sulphonation. A sulphite does not act on a nitrite in presence of free alkali, and a pyrosulphite ceases to act when it has become the normal sulphite by its action upon the nitrite. The sulphonation of a nitrite requires always an acidic condition of the solution, and the authors maintain that, in every case, it is nitrous acid itself, rather than the nitrite taken, which suffers the sulphonation. Carbon dioxide or an acid carbonate causes a normal sulphite to act slowly upon a nitrite.The statements of Claus, Berglund, and Raschig, that an alkaline hydroxide is produced in the sulphonation of a nitrite, is disproved by the authors and shown to be due to a misconception of the facts observed. Sulphur dioxide, passed into a solution of sodium or potassium nitrite and hydroxide, converts the latter into normal sdphite before sulphonation begins ; pyrosulphite is then produced much faster than it can be consumed in sulphonating the nitrite, because of .the retarding influence of the normal sulphite still present ; and finally, when the quantity of the normal sulphite is sufficiently reduced, the pyrosulphite disappears faster than it is formed, leaving hydroximido- sulphate as the sole final product.If the normal carbonate be taken in place of the hydroxide, the sulphonation proceeds rapidly with the simultaneous production of acid carbonate and of sulphite over and above what is consumed in forming the hydroximidosulphste, so long as any normal carbonate remains. Finally, the sulphite and acid carbonate are used up with the sulphur dioxide in sulphonating the last portions of the nitrous acid. As it is nitrous acid itself which undergoes the sulphonation, the nitrite of any base should be capable of being used for the purpose, and the authors have tried with success, not only the nitrites of sodium and potassium, but also those of ammonium, calcium, barium, zinc, mercury (oiis), and silver, *48.‘‘ The sym-dipropyl-, sym-di-isopropyl-, and act’-propylisopropyl succinic acids.’’ By William A, Bone and C. H. G. Sprankling. In continuance of their investigations on the alkyl substituted succinic acids, the authors have prepared those which form the subject of the present communication, and show, contrary to the statement of Auwers (Anncden, 1898, 292, 164), that each exists in two stereoiso-meric, inactive forms. In the case of each acid, each stereoisomeride yields with acetyl 72 chloride its own anhydride (liquid) which with aniline yields a charac-teristic anilinic acid ;each isomeride, on being heated to a high tempera- ture with strong hydrochloric acid under pressure, is to a greater or less extent converted into the opposite form ; trans-acids are completely converted into cis-anhydrides on being heated with acetic anhydride fo 1709 The paper concludes with a discussion of the dissociation constants of the new acids in relationship to those of other alkyl-substituted succinic acids, special atten tion being drawn to the very great difference between the values for the trccns-and cis-s-diisopropyl acids.The chief properties of the acids may be thus tabulated : TIT~IIS. Cis. BI. 11. Dissocia nr. p.n1. p. Aiiilinic tion con Acid.tAcid. acid. stant. s-Dipropylsuccinic.,....,.... 152-3" 184-5" 0'025 121" 101-2" 0.049 c-Diiropropylsuccinic ,. . ... . 226 201-2 '0'0108 171 154-5 0.2300 aa,-PropylisoproI,ylsuccinic 192-4 147-9 0 0147 151-2 liquid 0 -0295 49.'(Manno-galactan and lx!vulo-mannan ; two new polysac-charides." By Julian L, Baker and Thomas H.Pope. The authors described two new complex carbohydrates, the one obtained from the Indian clearing nut (XtwpAnos potatorum), and the other from the ivory nut (Plqteleplms nzcccrocas.pa). As these carbo- hydrates are very stable, the authors have been limited almost entirely to a study of the products obtained by their hydrolysis, these being, for the clearing nut substance, galactose and mannose, and for the ivory nut carbohydrate, mannose and another sugar, which, although not isolated as such, exhibits the characters of Immlose. Having regard to the relative proportions of the different sugars obtained, the authors propose to call the first of these substances manno-galactan, and the other Imwlo-mannan.They give no colour reaction with iodine, nor could acetyl- or phenylhydrazine derivatives be obtained. Manno-gcckccctan.-The powdered clearing nuts are extracted with hot dilute aqueous alkali, and the filtered extract precipitated by means of Fehling's solution ;this yields an insoluble, blue, pasty, copper com- pound, which, after washing, is decomposed with acid, the addition of alcohol to the acid solution then causing the reprecipitation of the carbohydrate. The manno-galactan thus prepared, when dry, is a snow-white, amorphous substance, fairly soluble in cold water and more so in hot ; it dissolves readily in dilute caustic alkali solutions.Its composition corresponds with the formula C,H,,O,, and in dilute aqueous solution it has a specific rotation [aJDat 15”= + 74”. After acid hydrolysis [.ID has a value of about 58.S0, corresponding nearly with the proportion of two parts of galactose to one of niannose. This ratio is supported by the determination of the mucic acid yielded on oxidation with nitric acid. The dibenxoyl derivative, C6HS05Bz2,of the manno-galactan is amorphous and dissolves in benzene, alcohol, and acetic acid, but gives no definite melting point ;in a glacial acetic acid solution, its specific rotation [a], = + 23”. ~~vu~o-mc6nncm.-Asthis substance undergoes decomposition in contact with hot aqueous alkali, the extraction of the ivory nut turnings is carried out in the cold, the alkaline liquor being then pre- cipitated by means of Fehling’s solution.After separating and wash- ing the copper compound, it is decomposed with hydrochloric acid, and the filtered acid liquid, on standing, deposits a thick, white precipitate, which is soluble in hot water, but on boiling the solution, fhe insoluble iaevulo-mannan separatesout. Af terdrying, thelaevulo-mannan isobtained as a white, amorphous substance having the composition C,H,,O,, and its specific rotation in dilute alkali [alD= -44.1”. After hydrolysis with acid, [a], becomes + 9.5”; this corresponds nearly with the proportion 20 parts of mannose to 1 of lzvulose. Approximate determination of the mannose by the hydrazone method shows that at least 90 per cent.of the mixed sugars considis of mannose. The dibefixoyZ derivative, C6H8O5Bz2,prepared by the Baumann method, is an amorphous substance soluble in benzene, alcohol, and glacial acetic acid, which has in the last-named solvent a specific rotation [a ID= -74O. 50. ‘L Hydrolysis of semicarbazones.” By GCeorge Young, Ph.D., and Ernest Witham, B.A.,B.Sc. The publication by Kipping of a “note on the decomposition of semicarbazones ” (this vol., 63) necessitates a preliminary notice of an investigation on which the authors are engaged. Some time ago, they observed that hydrazodicarbamide gradually disappeared when boiled with water for some days, ammonia and carbon dioxide being evolved.By heating hydrazodicarbamide with water in a sealed tube, they were able to control the hydrolysis, and to obtain a solution ths properties of which showed that it contained the first product of hydrolysis, ammonium semicarbazidocarboxylate, NH2*CO*NH*NH*C02NH,. When an aqueous solution of this salt is heated in an open vessel, it rapidly dissociates into ammonia, carbon dioxide, and semicarbazide, the latter being then further hydrolysed. The authors have studied the hydrolysis of other similarly constitu- ted substances, amongst them benzalsemicarbazone. When boiled with water in a reflux apparatus, benzalsemicarbazone gradually acquires a yellow colour, due to the formation of benzalazine. Heated with water in a sealed tube, the benzalsemicarbazone dissolves to a colour-less solution, which yields benzalazine on boiling, or more quickly on addition of sulphuric acid.In both cases, carbon dioxide is evolved. The filtrate from the benzalazine yields a further quantity of that substance on shaking with benzaldehyde. The formation of benzalazine from benzalsemicarbazone when the latter is boiled with water takes place apparently according to the following scheme : CGH,*CH:N*NH*CO*NH,+ H2O = CGH,*CH:N*NH*CO,NH*. C,H,* CH:N*NH*CO,NH, = C,H,*CH:N*NH2+ CO, + NH,. 2 C,H;*CH:N*NH,= C,H,*CH:N*N:CH*C,H,+ N,H,. In the formation of the azine from benzylparatolylketone, quoted by Kipping, the process would doubtless be hastened by the presence of free acetic acid.The investigation is being extended to the corresponding thio-corn- pounds and to substituted hydrazodicarbamides. 51. (‘The dissociation constant of azoimide.” By Charles Alfred West, A.R.C.Sc. The dissociation constant of azoimide in aqueous solution was determined some years ago by Ostwald, but no details were ever published. The results obtained by the author agree closely with those of Ostwald, and show that azoimide as an acid approximates to acetic acid, The values of p, m, and k are as follows : ?’. Pa ?N. It. 10 6.38 0-01397 0.0000198 100 15.98 0.0415 0~0000180 1000 45.97 0.1194 0*0000166 52. (( Racemisation occurring during the formation of benzylidene, benzoyl and acetyl derivatives of dextro-ac-tetrahydro+-naphthylamine.” By William Jackson Pope and Alfred William Harvey.On heating dextro-ac-tetrahydro-P-naphthylaminecarbonate (Proc., 1899, ‘15, 170) with benzaldehyde on the water-bath, a product is obtained which by fractional crystallisation is resolved into the inactive benzylideneDetrahydro-P-naphthylamine of Bamberger and Kitscheldt (Ber., 1890, 23,876) and benxyZide?aedextrotetrahydro-P-naphthylamine, C,,H,,*N:CHPh ;the new substance, which is accom- panied by about 20 parts of the isomeride, crystallises in aggregates of colourless needles melting at 5s-60°, and since it is more soluble than the inactive isomeride, the latter is a true racemic compound. The purest sample obtained of the active substance has [alD= -+27.6' in a 1 per cent.solution in alcohol. Benzoylation occurs readily on treating dextrotetrahydro-P-naph-thyI amine dex tro-a- bromocamphorsulphonat e by the Schot ten-Baumann method, but the product consists almost wholly of the inactive benzoyltetxahydro-@-naphthylamine of Bamberger and Muller (Ber., 1888, 21, SSO), and contains only a very small proportion of benxoyl-clextrotetruh~d~o-P-n~pl~tl~yZc~mine,C,,H,,*NH*COC,H, ; a larger yield of the latter substance is obtained by adding a solution of benzoic chloride in benzene to a solution of dextrotetrahydro-P-naphthylamine in benzene at 0". The active benzoyl derivative is isolated by f ractional cry stallisation from alcohol, being more soluble than its inactive isomeride, and forms less than 5 per cent.of the total pro- dnct. It crystallises in wool-like needles melting at 155-157", and the highest specific rotation observed was [a],,= +58" in solution in met one. On treating at Oo a solution of dextrotetrahydro-P-naphthylamine in benzene with acetyl chloride dissolved in benzene a mixture of Bamberger and Muller's inactive tetrahydroacenaphthalide with 2 or 3 per cent. of dextrotet~c-ch~d~oace~az~~~~hc~Z~de,C,,H,,:NH*COCH,, is obtained'; the active component is the more soluble, and may be iso- lated by fractional crystallisation from benzene. It forms long, colourless needles melting at 104-106°, and the highest specific rotation observed mas [uJ, = + 37" in a 2 per cent. solution in benzene. During the conversion of dextrotetrahydro-P-naphthylamineinto its benzylidene, benzoyl, or acetyl derivative, all but a very small1 proportion of the primary base undergoes racemlsation, and this racemisation apparently occurs prior to the formation of the final product, because the active derivatives are not racemised by heating at 100' either alone or in solution.Racemisation, as a result of operating upon an amido-group contiguous to an asymmetric carbon atom, does not seem to have been observed before, most of the cases, with rare exceptions, such as that of camphor (Kipping and Pope, Trans.,1897, 71, 956), being of substances in which a hydroxyl-group is attached to the asymmetric carbon atom, and in which the- possibility arises of change from an ''enolic " to a (( ketonic " form.It is important to note that in the present cases the whole of the material 76 i-, not racemised, indicating that the asymmetric carbon atom in the group ‘CH+2>C<EH, never becomes separately bound to only three CH2 atomic groups at any stage in the substitution. Work on these and analogous cases is being continued in the hope of obtaining inforniation respecting the mechanism of substitution in ti ivalent nitrogen compounds. ANNUAL GENERAL MEETING. BUNSEK MEMORIAL LECTURE. The Annual General Meeting of the Society, for the election of Oficers and other business, will be held on Thursday,March 29th, at 3 o’clock in the afternoon. At this meeting the Longstaff Medal will be presented to Professor W. H. Perkin, junr., F.R.S. In the evening, the Bunsen Memorial Lecture will be delivered by E. ROSCOE,Sir HENRY F.R.S., Vice-President The Chair mill be taken at 8.30. -4t the next ordinary meeting, on Thui sday, April 5th, the following paperh will be communicated by the authors. l‘ The liquefaction of a gas by ‘ self-cooling.’ d lecture experi-ment.” By G. S. Newth. kt Note on partially miscible aqueous inorganic solutions.” By G. S.Newtli. “The decomposition of chlorates. Part 11.” By W. H. Sodeau, B.Sc. RICFIARD CLAY AND Soh’s, LIUITLD, IOYDOh ANI) hLN(A\.
ISSN:0369-8718
DOI:10.1039/PL9001600065
出版商:RSC
年代:1900
数据来源: RSC
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