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Proceedings of the Chemical Society, Vol. 6, No. 87 |
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Proceedings of the Chemical Society, London,
Volume 6,
Issue 87,
1890,
Page 139-156
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摘要:
Issued l&jll/J8i)O. PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 87. Session 1890-91. Titles of Papers received and printed in the Transactions during t’he recess. 68. “ Crystallographical relations of the derivatives of dibenzoyl-cinnamene.” By Alfred E. Tutton, Demonstrator in Chemistry at the Normal School of Science, South Kensington. 69. “Note on a compound from benzoin and acetone.” By Francis R. Japp, F.R.S., and Julius Raschen, Ph.D. 70. “Researches on normal and mixed diazoamides.” By Raphael Meldola, F.K.S., and F. W. Streatfeild, F.I.C. 71. “ Note on the action of nitric acid on dibrom-s-naphthol.” ByRaphael Meldola, F.R.S., and Frank Hughes. 72. ‘‘A new method for the estimation of nitrates and nitrites in water.” By R. Ormandy and J.B. Cohen, Ph.D., Owens College, Manchester. 73. ‘‘ A new mon~br~m~camphor.” By J. E. Marsh. 74. “Contributions to the knowledge of mu& acid. Part 11. Action of phosphorus pentachloride on muck acid.” By S.Ruhemann, Ph.D., M.A., and W. J. Elliott, B.A. 75. “Contributions to the knowledge of mucic acid. Part 111. Rgdromuconic acid.” By S. Ruhemann, Ph.D., M.A. 76. “Note on the reduction of aromatic amides.” By A. Hutchin-son, B.A., Scholar of Christ’s College, Cambridge. 140 77. “Some improved vacuum joints and taps.” By W. A. Shenstone. 78. “The production of camphor from turpentine.” By J. E. Marsh, B.A., and R. StockdaIe, B.A. 79. “p-Desylphenol.” By Francis R. Japp, F.R.S., and G. H, Wadsworth, Associate of the Normal School of Science.80. “ Paraxylenesulphonic acids.” By Gerald T. Moody, D.Sc., Demonstrator in the Chemical Department, City and Guilds of London Institute, Central Institution, and T. G. Nicholson. 81. “Action of phosphoric anhydride on fatty acids. Part 11.” By F. Stanley Kipping, Ph.D., D.Sc. 82. “An investigation of the conditions under which hydrogen peroxide is formed from ether. (Second Notice.)” By W. R. Dunstan and T. S. Dymond. November 6th, 1890. Dr. W. J. Russell, F.R.S., President in the Chair. Certificates were read for the first time in favour of Messrs. Gustavus Anthony Abrines, Waterport Street. Gibraltar ; William Baxter, Fordingbridge, Hants ; T. St. John Belbin, Bolton Mansions Hotel, South Kensington ; John Thomas Brierley, 249, Bolton Road, Chorley, Lancashire ; William J. Butcher, Emanuel College, Wands- worth Common ; William Waters Butler, Elmdon, SelIy Park, near Birmingham ; Frank Brownsword, Heaton Moor, Stockport ; M.Kelway Bamber, The Lodge, St. Waltham, Chelmsford ;Ernest Bentz, 147, Bishop Street, Alexandra Park, Manchester ;Arthur E. Barrows, Bloomfield Iron Works, Tipton, Staffordshire ; W. E. B. Blenkinsop, 15, Earlsfield Road, Wandsworth Common; Thomas Arthur Cheetham, 29, Park Road, Glasgow ; Arthur William Crosskey, Bentcliffe, Accrington ; Arthur William Cooke, 15, Belle Vue Terrace, Leeds ; Frederick Hudson Cox, 79, Angel1 Road, Brixton, S.W. ;William L. Dudley, Nashville, Tennesee, U.S.A. ; Thomas Edwards, Brewery House, Rhymney, Monmouthshire ; Walter N.Edwards, 4,Heme Hill Road, S.E. ; Thomas S. Goodwin, Montgomery Cottage, Newton, Glasgow ; Alfred Henry Green, Oaklands, Lowton, Newton-le-Willows ; William Mahowe Heller, St. Dunstan’s College, Catford, S.E. ; John C. Hewlett, Elmhurst, Beckenham, Kent ; Charles Terry Holloway, Apsley Villa, Lewisham High Road, S.E. ; John Richard Jackson, 51, Abbotsford Place, Glasgow ; John 141 Jackson, Tredegar Road, Rhymney ; Joseph Lunt, 5: South View, Rccleston Road, Ealing, W. ; George Griffiths Leason, Ashfield Cottage, Stoke-on-Trent ; Harry C. Myers, Strassburg, Germany ; William Mackeay, 2, Victoria Mansions, Wesfminster, S.W. ; Thomas Smith Murray, 7, Gayfield Square, Edinburgh ; William Reginald Ormandy, Park Road, Newton-le-Willows ; James Alexander Pond, Auckland, New Zealand ; Thomas Platts, 7, Victoria Street, London ; Henry Ramsen Redman, 10, The Gardens, Dulwich, S.E.; G.H. Robertson, 30, Hemstall Road, West Hampstead, N.W. ; Charles William Seccombe, Church Park, Witchurch, Tavistock ; Ernest Henry Sainter, 176, High Street, Redcar ; J. Napier Spence, 9, Headstone Terrace, Harrow ; Thomas Steel, Jarraville, Melbourne, Victoria ; John Joseph Sudborough, 111,Stratford Road, Birming- ham ; Charles Thomas Sprayne, Reinsgraben, Gottingen ; Francis Henry Tate, 9, Hackins Hey, Liverpool ; John Cundall Wood, 32, Frederick Street, Sunderland ; George Henry Wadsworfh, 3, Southfield Square, Lamb Lane, Bradford; Sidney Wood, 5, Woodview, Bradford, Yorks ; George Young, 5, Colinton Road, Edinburgh.The following papers were read :-83. “The magnetic rotation of saline solutions.” By W. H. Perkin, Ph.D., F.R.S. On account of the remarkable results given by solutions of the halhydrides and their compounds with ammonia and organic bases when examined as to their mqpetic rotatory power (cf. Chern. SOC. Trans., 1889, 740), it became important to study the solutions of metallic salts in a similar manner, and although the work which has been done in this direction is incomplete, and may occupy some time yet, the results, as far as they go, are of interest, especially in rela- tion to the question of the condition of substances in solution. The substances which have been examined up to the present are chiefly chlorides, bromides, iodides, nitrates, a nitrite, sulphates and phos- phates, also hydroxides of the alkali metals.In the following comparisons, the values taken for the halogens aye those found for them in their compounds with the alcohol radicles, i.e., C1 = 1.733, Br = 3.562, I = 7.757. Those for the metals are deduced from the rotations of their nitrates, because in the case of ammonium nitrate it was found that this salt gave a rotation which was practically normal, and the salts of the metals have been found to behave in a similar manner to those of ammonium. Should there be any errors in these calculated values of the metals they will be but 142 small, and therefore will not materially influence the character of any deductions that may be made from the rotation of their compounds.They are Na = 0.558, K = 0.809, Li = 0.398, Ca = 0.691, Bfg = 0.57'7. The solutions examined were for t,he most part either saturated or supersaturated; in the case of sodium iodide, lithium nitrate and sodium hydroxide, two st~engths, varying considerably from each other, were taken, but the results were found to be practically the same. In the case of lithium chloride, which forms much stronger solutions than any of the other chlorides, bromides or iodides examined, the rotation increased on dilution, as in the case of hydrogen chloride. LiCl + 3.213 mol. OH, gave 4.166 mol. rot. 9,,, + 7,411 ,) 4.559 ,, ,, + 11.760 ,, ?> 4.697 9, At present, this is the only salt known the rotatory power of which changes with the amount of water used, and probably, like hydrogen chloride, it will be found to give a stationary value before the above dilution of 11.760 mols.of water is reached ; but further experiments must be made to establish the facts of the case. In two instances the effect of varying tenperature was tried. A solution of sodium bromide was examined at 16" and 78.5" ; in this case there was a small reduction in the molecular rotation at the higher temperature of 0.105 ; with a solution of potassium iodide, cxamined at 16.6" and 84.4", there was also a small diminution at the higher temperature, but only of 0.024. Substances, especially if they have high rotations, give a slightly lower rotation at higher tempera- tures like the above than at lower temperatures: so that, allowing for errors of observation, these results indicate that practically little or no change in the nature of the solutions took place when they passed from one temperature to another.The following tables show- the calculated and found rotations of the substances examined and their relationship to each other :-Ealoid Compounds. Calculated. Found. Ratio. NaCl .... 2,291 5.068 1:2-212 KCl.. .-.. 2.542 5.377 1:2.115 LiCl.. . . .. 2.131 4.697 1:2.204 CaCl, .... 4.157 9.085 1: 2.185 MgCl, E.. . 4.043 9103 1 : 2.252 143 Calculated. Found. Ratio. NaBr .... 4.110 9.030 1: 2.197 KBr...... 4.372 9.222 1: 2.110 NaT.. .... S.31.5 18-867 1: 2.269 KI ...... 8.566 18.690 1: 2.182 It mill be seen that the rotations of these salts, when in aqueous solution, are practically 2.2 times greater than the calculated values for the dry substance; they are even greater than those of the analogous ammonium compounds, the calculated values for which now given differ by 1 from those previously published, which were incorrect. Calculated. Bound. Ratio. NHdCI.. .. 3.3305 6.096 1 : 1.844 NH4Br ... 5.134 10.196 1 : 1.985 NHJ ..... 9.329 19.996 1:2.144 A solution containing equimolecular proportions of NaI and NaOH gave a rotation for NaI = 18.454, or 0.413 lower than that given by hhe iodide alone. Hydroxides of Allinli .Metals.Calculated. Found. Ratio. NaOH.. .. 1.006 2.433 1:2.418 KOH.. ... 1.257 2,658 1: 2.114 Here, again, a remarkable increase of rotation is obtained, quite as great, or even larger in one case, than with the halogen salts. Potassium hydroxide in alcoholic solution gives a somewhat lower number than the above for its aqueous solution; but it is possible that some of the potassium in this instance may be in combination as alcoholate, and this may account for the difference. Xulphates. Calculated. Found. Difference. NaHSO, .... 2.419 2.525 0.106 N%SO,. ..... 2.513 2.877 0.364 Li2SOI....... 2.099 2.379 0.280 In this table ths difference is given instead of the ratio, and it will be seen that it is but small compared with the foregoing, but it increases with the number of atoms of metal.144 Phosphates. Calculated. Found. DiEerence. Nt~HzP04.... 3.328 3.481 0.153 Na,HP04 .... 3.678 4.076 0.398 Na,P04.. .... 4.036 5.079 1.043 As in the case of the sulphates, the rotat'ion increases beyond the calculated with the number of atoms of metal; in the last case the difference is considerable. Potassium Nitrite.-This salt is interesting, because it allows of a comparison being made between it and potassium nitrate which can be placed side by side with a similar comparison between isobutyl nitrite and nitrate. Difference. KN02. ........... "g43 }0.408.KNO, ............ 1-535 C4HgNOz.. ....... 5'510 }9.330.CJ&J?O, ......... 5.180 From this it is seen that in both cases the nitrites give larger rota- tions than the nitrates, and the differences do not vary very greatly. though sufficient to show that the rohtion of potassium nitrat,e undergoes some change when that salt is in solution.Nitrates. NaN0,. .............. 1.284 KNO, ................ 1.535 LiN0,. ............... 1.124 Ca(NO& ............. 2143 Mg(NOJ2. ............ 2.029 It has been assumed that the solutions of the nitrates give prac- tically normal results, and the values of the metals have been deduced from them: the reasons for this have already been given; it may be added that of all the salts examined the nitrates give the lowest numbers for the metals. Nevertheless, experiments are in progress to test the validity of this method of determining the values of the metals.In considering the numbers given in this communication, it is well to remember that, owing to the method employed in calculating the results obtained from solutions, all experimental errors fall upon the numbers obtained for the dissolved substance, and consequently will also influence the differences found in comparing the results, as in the tables given above. When the solutions contain large percent- ages of dissolved substance the errors are but small, but when the 143 percentages are small the errors naturally increase ; on this account it will be difficult to get good results with compounds that are sparingly soluble in water.It is very difficult to understand why the haloid acids, their Ralts and also caustic alkalis should give such extremely large rotations when in aqueous solution. If dissociation takes place, there does not seem to be any reason why any very considerable change of rotation should occur ;but whatever the cause, the change evidently indicates some very important difference existing between dissolved and undis- solved substances of these classes. DTSCUSSIOF. Dr. GLADSTONEremarked that similar excessive values mere ob-tained on determining the refractive powers of solutions of metallic chlorides, &c., although the differecce between the calculated and observed values were much smaller than in the case of Dr. Perkin’s measurements.It was all-important to determine the difference in the behaviour t.0 light of a substance in its solid state and when in solution; but this was difficult, as few solids were uniaxial : as an example of the difference he mentioned that in the case of the sodium chloride the solid has a rcfraction of 14.4,while that of the dissolved substance is 15.3. Mr. PICKERINGsaid that Dr. Perkin’s results must have a very im- portant, bearing on the question of the nature of solutions. When salts caused a double depression of the freezing point, the physicists held it to be due to dissociation into ions; but here was a case of a similar ef‘fect which cannot well be attributed to dissociation. As far as can be seen, dissociation mould not double the rotation, still less would it make it more than double, and, even if it could be held to do 0, such an explanation would be inadmissible in the case of saturated solutions, for in such solations the physicists themselves held that there is little or no dissociation. Professor RAMSAYthought that the abnormal results may not be entirely connected with dissociation into ions : the optical phenomena were probably much more complex ; it was conceivable that the sepa- rated atoms might be much more powerfully affected in a magnetic field than when combined. 84.(‘Note on normal and isopropylparatoluidine.” By E. Hori and H. F. Morley. Desiring to distinguish with certainty between normal and iso- propy lparatoluidine, the authors have prepared the pure substances and several of their derivatives.146 The normal compound boils at 3;30-2:33"; its density at 20" is 0,9243 gram per c.c., and at the boiling point 0.7543: hence its molecular specific volume is 197.53 (theory 199.3) ; its molecular refractive energy is 82.5 (theory 79.3). Isopropylparatoluidine boils at 219-221 (mcorr.) ; its density at 20" is 0.9226 gram per c.c., and at the boiling point 0.7466: hence its molecular specific volume is 199.57; its molecular refractive energy is 81.4. The isopropylnitrosamine is a crystalline solid, whereas the iso- meride is an oil. The normal and iso-compound form oxalates differing in solubility and stability. 85. '' The action of light on ether in presence of oxygen and water." By Arthur Richardson.In a recent paper by Professor Dunstan and Mr. Dymond (Chem. Xoc. I'mns., 1890, 574) it is stated that hydrogen peroxide is not formed when puye ether is exposed to light in contact with air and water, and these authors consider that the formation of this substance is due t,o the impurities contained in the ether, which can be removed by treatment with potassium bichromate or iodhydric acid. The author describes experiments made with ether which had been purified by some of the methods described by Dunstan and Dymond ; he finds that hydrogen peroxide is formed in the liquid in every case after exposure to light in contact with moist air or oxygen, but not in the dark at the ordinary temperature.The methods employed to prepare and purify the ether are described in full in the paper ; they were as follows :-(1.) Commercial "pure '' ether, from which the alcohol had been removed bj repeated shaking with water, was afterwards agitated with potassium bichromate. (2.) Ether obtained by the action of pure sulphuric acid on pure alcohol was shaken with potash solution and with water, and one portion was treated with potassium bichromate, another with iodhydric acid. (3.) The liquid from (2) was collected after exposure to light and again agitated with potassium bichromate. (4.) Ether prepared from an entirely different sample of pure alcohol and pure sulphuric acid was treated as before with potassium bichromate ; it was distilled after being allowed to stand over calcium chloride and then over metallic sodium.The ether boiled constantly at 34.6" at 760 mm. pressure corr. to 0". 147 The ether prepared by these methods was placed in colourless bottles, and air or oxygen was passed into the space above thc liquid before the stoppers were inserted. Some experiments were made on the influence of temperature in bringing about the formation o€hydrogen peroxide ; it was found that ether and moist oxygen exposed to a t4emperature of 75-88" in the dark contained, after four days, considerable quantities of this sub-stance ; similar results were obhained when ether and oxygen were heated to 60" €or a period of' 40 hours. Ether uapour and moist oxygen gave piactically no peroxide when so heated.It was found, however, that liquid ether keptl at 0" contained hydrogen peroxide after exposure to light for four days. Hence it appeays that when special precautions are taken to ensure the presence of oxygeu over the ether, hjdrogen peroxide is formed at oydinary temperatures, and evcii at 0" in the light, but not in the dark ; it is, liowcver, formcd in absence of light at about 60". Professor DUNWANsaid t81iat Mr, Uymond and he had made their experiments on the conditions necessary for the formation of hydrogen peroxide from ether, because there was no evidence that previous workers had eniployed the pure substance. They had been unable to detect hydrogen peroxide in ethep that had been exposed at a low texperature to the electric light and diffused daylight.For the detection of hydrogen peroxide, reliance had been placed on the characteristic chroniic reaction which they had proved to be capa- ble of indicating 0.0003 gram of the substance. Dr. Richardson, who meanwhile had purified ether by the method employed by the speaker, and still adhered to some of his original statements, aserted that he had detected hydrogen peroxide in ether exposed at a low temperature to white light by means of titanium oxide, but it appeared that he had failed to obtain the chromic reaction. The suggestions which Dr. Richardson had made to explain why hydrogen peroxide had nub been formed in their experiments were quite untmA.de. At least d litresof air were in contact with the exposed ether.There could be no doubt as to the purity of the ether they had used. The slight greenish tint of the bottles was shown riot to be detrimental by the circumstance that hydrogen peroxide was produced from specimens of impure ether contained in them. They had emplojed the electric light partly because they had failed to obtain results with diffused sunlight in London, and partly because they wished to ascertain whether pure ether was affected by violet rays acting at a low tempe-rature. They had recently obtained evideiice which seemed to show 148 that certain specimens of nnpurified ether could form hydrogen per- oxide even in the dark. The whole purport of Dr. Richardson's first paper on this subject was to prove that when hydrogen peroxide is formed from moist ether, the water and not the ether is oxidised.They had opposed this view as they were in possession of good evidence that the ether is oxidised. It now appeared that Dr. Richardson had abandoned his former view, alfhough he still con- tended that hydrogen peroxide could be formed from water and oxygen alone in the presence of light. But they had also failed to confirm this statement. No evidence could be obtained of the presence of hydrogen peroxide in acidulated water which had been exposed to intense sunlight or to the electric light (cf. Chem. SOC. Trans., 1890, 988). They were also unable to confirm the statement that pure ether yields hydrogen peroxide when heated with air and water to 50-60". Mi*.DYMOXD said that Dr. Richardson had not stated whether he had tested his ether for the impurities which are known to be invariably present, some of which may be produced durinq the process of purification employed, and which arc particularly difficult to remove, viz., aldehyde and ethylene. In his previous paper, Dr. Richardson had stated that after hydrogen peroxide had been pro- duced in ether, the ether remained unaltered. Did he adhere to that statement now that he had convinced himself that the ether was concerned in the production of the peroxide? In the experiments made by Professor Dunstan and himself, it was always noticed that when peroxide of hydrogen was produced from ether, the ether afterwards contained aldehyde, acetic acid and other substances.Mr. GROVES,referring to Dr. Richardson's statement that he had found that pure dry ether was acted On when exposed with oxygen, said that this result was contrary to recent experience as to the influence of water in promoting chemical change ; it was difficult to conceive how hydrogen peroxide could be produced in such a case. Mr. PICKERINGinquired why so minute an amount of peroxide was obtained ; if pure ether afforded hydrogen peroxide when oxidised, it was to be expected that the action would continue, and that a larger proportion would result. Dr. PERKINsaid that the alcohol was best removed from ether by means of phosphoric anhydride. Dr. JAPPmentioned that Professor Frankland had always used this substance in purifying the ether used in preparing zinc methide ; and Professors RAMSAYand DUNSTAN subsequently stated that they had employed it with good results. Dr.RICHARDSON,in reply, stated that he did not see that Professor Dunstan's ether had any claim to greater purity than that used by him- self. On the contrary, the fact that Professor Dunstan's ether distilled 149 only within + degree showed tlhat it was not so pure as that used by him, which distilled within -?s degree. The ether used by the speaker was found to be without action on potassium iodide in the dark after contact with the solution for two weeks. With regard to the remarks made on the quality of the bottles used, it appeared to him that the fact that methylated ether was found to contain H202after exposure to light.in greenish glass bottles, did not shorn that the formation of this body was in this case brought about by light at aII, for, as Professor Dunstan had just pointed out, impure ether which had been kept iu the dark wag found to contain this substance. He did not see that the absence of H202in Dunstan’s ether could be accounted for by the use of the electric light, for Professor Dunstan states (Chern. Soc. Trans., 1890, 579) that in one series ether was exposed for two months to much sunlight during August and September, the temperature ranging between 15-25’, but, under these circumstances, no H,02was formed. The speaker would like to point out that in all except the last sample oi ether he had obtained sufficient H20, after exposure to give the blue coloration with K2Cr207;in the last case, however, the time of exposure had been necessarily short, and the light exceedingly poor, so that the presence of H,O, could only be detected by the more delicate tests such as KI and H,TiO,.He was not surprised to learn that Professor Dunstan had failed to obtain H,O, on exposing H20to light, for in the formation of this body, under these conditions, many special pre- cautions must be observed, such as keeping the temperature low, &c., as he found that the H,02first formed was very readily decomposed. In reply to Professor Pickeriag, Dr. Richardson wished to point out that other products of decomposition were formed when ether was exposed to light, some of which might probably decompose the peroxide first formed; thus a specimen of ether which had been exposed with water and oxygen to light for 18 months contained no H202,the smell of the ether had changed, and black particles were seen floating in the liquid-this was a point which the author hoped to further investigate, however.86. “ Action of ammonia and methylamine on the oxylepidens.” By Felix Klingemann, Ph.D., and W. F. Laycock, Ph.D. This investigation was undertaken with the object of ascertaining whether the arialogy which was shown by Japp and Klingemann to prevail between the interact,ions of a/?-dibenzoylcinnamene and those of dibenzoylstilhene (Zinin’s ‘‘acicular oxyIepiden ”) was preserved in the behaviour of these compounds with ammonia and amines.The authors find that this is the case. 150 On heating dibenzoylstilbene with alcoholic ammonia at 200°, it is converted into a, mixture of two isomeric compounds of the formula CzsH2,N0: dibenzoy lstilbenimide, which crystallises from benzene in crusts of yellow, prismatic forms melting at 180-183", and corresponds with dibenzoylcinnamenimide; and tetraphenyl-pyrrholone, which crystallises in pale-yellow, square plates melting at .206-207", corresponding with triphenylpyrrholone, Dibenzoylstil-benimide is converted by heating at 310" into tetraphenylpyrrholone, just as di benzoylcinnamenimide is converted into triphenylpyrrho- lone. The constitution of tetraphenylpyrrholone is shown by the fact that it is also obtained by heating tetraphenylcrotolactone (Zinin's " tabular oxylepiden ") with alcoholic ammonia at 200" :-(C6H5)?,y-fi*C6H5 + NH, = (c6H5)27-z c6H5 + H2O.OC C*C6H5 oc C*C,H,\o/ 'dH Tetraphenylcrotolactone.Tetraphenylpyrrholone. By the action of nascent hydrogen (from sodium and boiling amyl alcohol) tetraphenylpyrrholone is converted into tetraphenyZpyrrho1-(C6H5)'27-?H*C6H5 idone, OC CHgC6H,, which crptallises from alcohol in slender, YH pale-brown needles melting at 237". When clibenzoylstilbene is heated with an alcoholic solution of metbylamine at 200°, it is converted, with eliminatlion of water, into (Ce&)z?-#*ce,H5 methyl tetraphen y lpyrrholone, OC C*C6H5, which crystallises\/N-CH, from hot alcohol in thin, faintly yellowish, asymmetric plates melting at 161".On the other hand, tetraphenylcrotolactone unites directly with methylamine at 150°, forming benzo~ltri~h.enyl~ropiomethylamide, (C&L)2F-#*CJ& (C6H,),7*9H*CGH5 which crys- oc C9C6H5+ NH2*CH3= CH,*NH.OC co*c6H5,\/0 tallises from glacial acetic acid in lustrous plates melting at 267". When this compound is distilled under reduced pressure, it parts with water and is converted into methyltetraphenylpyrrholone. The crystalline form of the compound thus obtained differed, however, from that of the same substance from dibenzoylstilbene, and the melting point was found at 158", instead of at 161" ; but the authors 151 attribute these differences to dimorphism, as in the case of the corre-corresponding tlriphenyl derivatives prepared by Japp and Klinge- mann.87. “ Condensation of acetone-phenanthraquinone.” By G. H. Wadsw orth. The author finds that by the dehydrating action of a mixture of concentrated sulphuric acid and absolute alcohol, acetone-phenanthra- quinone is converted into it compound of the formula C,,H,,O, = 2C,,Hla0, -3H,O. It crystallises from benzene in tufts of minute needles melting at 238” C. 88. “Contribiitions to the knowledge of mucic acid. Part IV. Action of phosphorus pentachloride on mucic acid.” By 8.Ruhemann, Ph.D., M.A., and S. F. Dufton, B.A., B.Sc. The aut,hors find that mucic acid is converted by the action of phosphorus pentachloride into a crystalline compound which, assuming CCl*CH*COOHdichloromuconic acid to be an acid of the formula ICC1.CH-COOH, CCI(P0 CL,).C H(OH)*COC1may be represented by the formula I OnCCl(POCl,)*CH(OB).COCl’ dissolving this substance in water and carefully concentrating the solution, large, colourless, yhombic crystals of the corresponding phosphodichloromuconic acid are obtained ; several salts of this acid are described, among others, one formed by the combination of 6NH3 with the acid.The phosphochloride is converted by the action of phosphorus pentachloride at 120” into dichloromucoiiyl chloride, hydrogen chloride and phosphorus oxychloride. The authors have succeeded in converting the isomeride of Bode’s dichloromuconic acid discovered by Ruhemann and Elliott (cj.Trans., 1890, 931) into Bode’s acid, by adding a small quantity of bromine tto the cold aqueous solution ; t’hey therefore conclude that the isomeric dichloromuconic acids are related to each other much as are maleic and f umaric acids. 89. “Halogens and the asymmetrical carbon atom.” By F. H. Easterfield. At the suggestion of Professor Emil Fischer, the author has endeavoured to prepare active haloid derivatives similar in constitu- tion to Le Bel’s optically active secondary nmyl iodide, CH3*CHI.CsH:, which at pressnt stands a!one as the only active compound in which B halogen is united to the asymmetric carbon atom. His results are negative. Thus active mandelic acid gave inactive phenylbromacetic acid when heated with bromhydric acid at a temperature not exceeding 50"; and no resolution of the acid into active constituents was effected by means of alkaloid salts.ADDITIONS TO THE LIBRA.RY. I. Donations. Manual of Pharniaceutical Testing, by B. S. Proctor. London 1890. From the Publishers. A Treatise on Practical Chemistry and Qualitative Analysis, by F. Clowes. 5th Edition. London lS90. From the Author. A Technological Dictionary of Insurance Chemistry, by W. A. Harris. Liverpool 1890. From the Author. Principles of General Organic Chemistry, by E. Hjelt. Trans-lated by J. B. Tingle. London 1890. Prom the Translator. Geological Survey of New South Wales :-Paleontology, No. 3. Geological and Palaontological Relations of the Coal and Plant-bearing Beds o€ the Palizeozoic mcl Mesozoic Age in Eastern Australia and Tasmania, by 0.Feistmant el. Palzontology, No. 4. The Fossil Fishes of the Hawkesbury Series at, Gosford, by A. S. Woodward. 4to. Sydney 1890. From the Director of the Survey. United States Geological Survey :-Eighth Annual Report (in 2 parts). 1886-7. 4to. Washing-ton 1889. Monographs, XV (2 parts). The Potomac or Younger Mesozoic Flora, by W. M. Fontaine. Monographs, XVI. The Palaeozoic Fishes of North America, by J. S. Newberry. 4to. Washington 1889. From the Director of the Survey. A Course of Chymistry, by N. Lemery. Translated from the French (2nd Edition) by W. Harris. London 1686. Trois Traitez de la philosophie naturelle, Eon encore imprimez.Ide S6cret livre du tres-ancien Philosophe Artephius, traitnnt cle 1'Art occulte de transmutation M6tdlique. Les figures hi6rogli- phiques de Nicolas Flame1 ainsi qu'il les a mises en la quatriesnie arche qu'il a bastie au Cimetibre des Innocents A Paris. Le vrais 153 livre du docte Synesius. Le tout traduit par P. Arnauld. Paris 1612. From T. Bolas, Esq. Qualitative Chemical Analysis of Inorganic Substances, by C. F. Juritz. Cape Town 1890. From the Author. The Organic Analysis of Potable Wa,teis, by J. A. Blair. London 1890. From the Publishers. Chemical Arithmetic. Part I. A collection of Tables for the use of Chemists and others, by W. Dittmar. Glasgow 1890. From the Publishers.Manual of Assaying Gold, Silver, Copper, and Lead Ores, by W. L. Brown. Revised and enlarged by A. B. Griffiths. London 1890. From the Publishers. Grundzuge der theoretischen Chemie, von L. Meper. Leipzig 1890. From the Author. Pamphlets. Report of the Field Experiments on Swedes with different Maiiures, proposed to members of bhe Royal Agricultural College Club ; byX.Kinch. Cirencester 1890. Prom the Author. Die Licht- und Warrnestrahlung verbrennender (he, yon R. VCLL Helmholtz. 4to. Berlin 1890. From the Author. Ueber Feuerbestattung, von F. Goppelsroeder. Miihlhausen i. Els. 1890. From the Author. Studier ofver Gadolinit, af G. W. Petersson. Stockholm 1890. Kemiska Studier ofver Nagra Hartser, af K. A. Vesteyberg. Upsala 1890.From the Author. Nitrogen, its Uses and Sources in Agriculture, by C. 211. Aikman. Glasgow 1890. From the Author. Sull’ influenza della qualit& delle Acque usate nulla trattura dei bozzoli, del E. Rotondi. Ronia 1890. From the Author. Results of Experiments at Rothamsted on the Growth of Legu-minous Crops for many years in succession on the same land, by J. H. Gilbert. (From the Agricultural Stmudent’s Gazette, N. S., vol. IV, 5 and 6). Cirencester 1890. From the Aut,hor. Gold from Pyrites and other Sulphides, by E. J. Hill. Dunedin 1890. From the Author. Production de vari&s chez les Saccharomyces, par E. C. Hansen (Extrait des Annales de Micrographie 11,5), 1890. Nouvelles recherches sur la circulation du Saccharomyces apiculatus dans la Nature, par E.C. Hansen (Extrait des Annales des Sciences Naturelles : Botanique, XI, :3). 1890. Ueber die Pilzstudien in der Zymotechnik, von E. C. Hansen (Abdrnck aus der Zeits. f. das gesammt Brauwesen). 1890. From the Author. 154 Wattles and Wattle-Barks, by J. H. Maiden. Sydney 1890. From the Author. Richesse de Vesous et Cannes B 1’Ile Maurice, par L. Ehrmann. SBries I et 11, 1888-90 (Extraits de la Revue Agricole). Maurice 1889-90. From the Author. The Chemical Constitution of some Colonial Fodder Plants and Woods, by C. F. Juritz. Wynberg 1890. Erom the Author. Address on Technical Education, by J. Philipson. Aberdeen 1830. From the Author. International Standards for the Analysis of Iron and Steel.Extracts from the work of the American Committee, by J. W. Langley. (From the Trans. of the American Inst. of Mining Engineers, October, 1890.) 11. By Purchase. La coloration artificielle des vins, par M. Monavon. Paris 1890. La glycogenie animale, par J. Seegen. Traduction par L. Hahn. Paris 1890. Cours de Minkralogie, par A. de Lapparent. 2me. Edition. Paris, 1890. Etudes cristallographiques, par A. Bravais. Paris 1866. The Study of Rocks, by F. Rutley. 4th Edition. London 1888. A System of Mineralogy. Descriptive Mineralogg, comprising the most recent Discoveries, by J. D. Dana, aided by G. J. Brush. 9th Edition. New York 1889. Tabellarische Uebersicht der Mineralien nach ihren krystallo-graphisch-chemischen Beziehungen geordnet, von P.Groth. 3te Aufl. Braunschweig 1889. Die mikroscopische Beschaff enheit der Mineralien und Gesteine, von F. Zirkel. Leipzig 1873. Die Paragenesis der Mineralien, von A. Breithaupt. Freiberg 1849. Lehrbuch der Mineralogie, von G. Tschermak. 3te Aufl. Wien 1889. Elementme der Mineralogie, begrundet von C. F. Naumann. 12te Aufl., bearbeitet von F. Zirkel. Leipzig 1885. Lehrbuch der chemischen und ph-pikalischen Geologie, von G. Bischof. Bde. 1-111 and Snppl. 1863-66 and 1871. Tafeln zur Bestimmuug der Mineralien, von F. Kobcll. 12te Aufl., bearbeitet von I(.Oebbeke. Munchcn 1884. 155 A meeting of the Research Fund Committee will be held in December. Fellows desiring grants are requested to forward their applications to the Secretaries.At the next meeting, on November 20th, there will be it ballot for the following candidates :-1. Branson Charles F., Kenley Lodge, Macaulay Road, Clapham Common. 2. Clark, D. G.,434, St. John’s Wood Park, N.W. 3. Caird, George, 20, Springfield, Dundee. 4. Colman, Wa’lter Henry, 41, Poynings Road, Junction Road, N. 5. Day, Charles Edwin, 1,Merchiston Bank Terrace, Edinburgh. 6. Edward, John Huchison, 117, Stockport, Road, Manchester. 7. Frost, Robert, St. James’s Chambers, Duke Street, S.W. 8. German, George, Huntingdon House, Ashby-de-la-Zouch. 9. Gordon, Colin, Millwall Club, West Ferry Road, Millwall. 10. Haslam, Arthur R., Ph.D., 64, Rathgar Road, Dublin. 11.Haydon, Frank, Ettrick, Putney Common, S.W. 12. Johnson, John Robert, 16, Oxford Street, Liverpool. 13. Jenkins, Wallace, 410, Glossop Road, Sheffield. 14. Kelly, Patrick, 43, Lennox Street, Dublin. 15. McKillopp, John, Pulan Brani, Singapore. 16. Marshall, Thomas Rhymer, 4, East Castle Road, Edinburgh. 17. McCubbin, William Alexander, Mill Bank House, West Derby, Liverpool. 18. Palmer, Arthur E., Ashley Mount, Tettenhall, Wolverhampton. 19. Parker, Thomas, ICI.I.C.E., Wolverhampton. 20. Parkes, Thomas, Grammar School, Stamford. 21. Redding, Richard James, Royal Laboratory, Woolwich Arsenal. 22. Seaton, Edward Cox, 35, George Street, Hanover Square. 23. Smith, Frederick, Johannesburg, Transvaal, South Africa.24. Stagg, William, 52, Seymour Road, Bristol. 25. Thoi-nley, John Brooks, Ivanhoe Terrace, Ashby-de-la-Zouch. 26. Wilson, James Mitchell, Hall Gate, Doncaster. 156 The following papers will be read :-“ The estimation of cane-sugar.” By (1. O’Sullivan, F.R.S., and F. W. Tompson. “ A new method of determining the specific volumes of liquids and of their saturated vapours.” By Professor S. Young. “ The molecular weights of metals when in solution.” By Messrs. Heycock and Neville. “ The spectra of blue and yellow cblorophyll with some observa- tions of leaf green.” By Professor Hartley, F.R.S. HAIiBISON AND SONS, PRINTERS IN ORDIBARY TO HER MAJESTY, ST. MARTIN’S LANE.
ISSN:0369-8718
DOI:10.1039/PL8900600139
出版商:RSC
年代:1890
数据来源: RSC
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