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Proceedings of the Chemical Society, Vol. 30, No. 431 |
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Proceedings of the Chemical Society, London,
Volume 30,
Issue 431,
1914,
Page 165-194
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[Zssu~d12/6/14 PROCEEDINGS OF THE CHEMICAL SOCIETY. Vol. 30 No.431. May 25th, 1914. Extra Meeting, Professor W. H. PERKIN, Sc.D., LL.D., F.R.S., President, in the Chair. This meet,ing was held in the Theatre of the Royal Institution, by kind permission of the Managers. inThe PRESIDENT,opening the proceedings, said: We are assembled in this historic place to pay a tribute of respect to the honoured and revered name of Faraday, and, at the same time, to add another to the list of illustrious men who have served as Faraday lecturers in the past. I do not need to introduce Pro-fessor Arrhenius to such a gathering as this. Many of you know him personally, and all of you are aware of the great influence. which his brilliant and far-reaching generalisations have had on the development of modern science.I have therefore great pleasure on calling upon Professor Arrhenius to deliver t.lie Faraday Lecture. Professor ARRHENIUSthen delivered the Faraday Lecture, of which the following account is an abstract.$+ Most of my predecessors in this position, being mindful of the far-reaching importance of Faraday’s discoveries, have treated general questions connected with Faraday’s work, and bear-ing on our fundamenha1 conceptions of matter. It is most opportune for me that the chief investigation made by myself falls within the great domain of electrochemistry, which Faraday * Full Report, T., 1914, p. 1414. 166 enriched in a marvellous manner, especially by the discovery of his law, which is fundamental to all later work in this chapter of Science.The work on which I have to speak to you also concerns the constitution of matter. Solutions, especially those of salts, are of a peculiar character. Gay-Lussac, the most prominent physico- chemist of his time, paid special attention to solutions, and reached some conclusions which apparently are very modern. In his remarkable memoir of 1839, ‘‘ Consid6rations sur les forces chimiques,” he says: “As the effects of affinity do not change with temperature, whereas dissolution (solubility) is in a high degree dependent upon it, it is very difficult to avoid the assumption, that in dissolution as well as in evaporation, the product is essentially limited, at a given temperature, by the number of molecules which are able to exist in a certain volume of the solvent.They are separated from this, just as gaseous molecules are precipitated, by a lowering of temperature. . . . Dissolution is therefore in a high degree connected with evaporation, namely, in this respect, that both of them depend on the temperature and are subject to its variations. Hence they ought to show, if not a complete identity in their effects, at least a great analogy.” Here Gay-Lussac is a precursor of van’t Hoff, who, forty-five years later, developed in such a masterly manner the idea of the analogy between matter in the dissolved and in the gaseous state. In 1883 I investigated the electrical conductivity of different electrolytes, and came to the conclusion that the molecular con-ductivity increases with dilution, because the number of conductc ing molecules increases at the expense of the other, non-conducting, molecules.At infinite dilution all molecules of an electrolyte are conductors. This hypothesis led to the following chief conclusions. The molecular conductivity at infinite dilution is an additive property for all electrolytes, and not only within certain groups of electrolytes of similar composition, as maintained by Kohlrausch for the molecular conductivity of diluted electrolytes. According to the thermo-chemical data given by Berthelot and Thomsen, the stronger an acid is the greater is its molecular conductivity. The electrically conducting molecules are therefore the same as the chemically reacting molecules, the nature of which is charaterised by Williamson and Clausius.At infinite dilution all acids must therefore be of the same strength. In accordance with these ideas, the velocity of reaction caused by an acid is proportional to its number of electrically conducting molecules per unit volume. This assertion could only be verified qualitatively in some very few cases, because experimental determinations were wanting. The heat evolved on neutralising one equivalent of an acid consisting of only conducting molecules with a base of similar kind is always the same and equal to the heat produced when one equivalent of con-ducting molecules of water is transformed into one equivalent of non-conducting molecules. Theref ore the heat of neutralisation of strong acids with strong bases at higfi dilution, as in the experi- ments of Thomsen, when they are composed almost entirely of conducting molecules, is very nearly the same for all acids and bases in equivalent quantities.When a salt such as potassium ferrocyanide, K,C6N6F0, ths ions of which are 4K and C6N6Pe9 enters into a chemical reaction with another salt in aqueous solu-tion, there are formed only ferrocyanides and potassium salts, but not ferrous or ferric salts, because the result is always a rearrange- ment of the ions. Such were the conclusions drawn from a rather small number of experimental data, and I do not wonder that my colleagues refused to take notice of these ideas, which seemed absolutely in- compatible with the prevailing conceptions regarding the chemical nature of salts.Very soon after my memoir had appeared, Ostwald published measurements of the conductivity of thirty-four acids, and showed that the molecular conductivity of the acids is very nearly proportional to the velocity of reaction in catalytic pro-cesses (inversion of sucrose, hydrolysis of esters) caused by these acids. A little later he also proved that the relative strength of weak acids, as compared with that of strong acids, increases with dilution, so that all acids show a tendency to become of equal strength in infinite dilution. Both of these laws were predicted in my memoir of 1884. Then there were two different phenomena, ths molecular conductivity and the chemical activity of acids, which quantitatively led to the same conclusion. This was not, however, sufficient evidence to support the bold hypothesis that salts, including acids and bases, are to a great extent dissociated into their ions.Fortunately, I had not long to wait for further evidence. In 1886 van’t Hoff published his revolution- ising memoir on the analogy of dilute solutions to gases. There he showed that Raoult’s measurements on the freezing point of aqueous solutions pointed to the fact that the influence of one molecule of a salt, such as potassium chloride, in great dilution, was double that of a simple molecule (alcohol, ammonia). This fact was wholly analogous to the fact that some substances, for example, ammonium chloride and phosphorus pentachloride, in gaseous state per molecule exert a pressure which is double as great as that produced by common undissociated gases. According to the law of Avogadro, the latter circumstance could only be ex-plained by the hypothesis that the molecules of such substances as 168 ammonium chloride or phosphorus pentachloride are dissociated, when vaporised, into two molecules, namely, ammonia and hydrogen chloride or phosphorus trichloride and chlorine, respec- tively.The experimental proof of this hypothesis was also given by v. Pebal and v. Than in 1862 and 1864. From analogy to this experience, there seemed no other possibility open to explain the abnormal freezing point of solutions of potassium chloride than to suppose that the molecules of this salt were for the greater part dissociated into their ions K and C1.Thus Raoult’s measurements of the freezing point gave a means of deter- mining the degree of dissociation of a great number of substances, the aqueous solutions of which he had investigated. By the aid of the measurements of Kohlrausch, regarding the molecular con-ductivity of different substances, it was possible to make another independent determination of their degree of dissociation. The two methods gave values which agreed very well with each other when dilute solutions (generally 1 per cent.) were examined. A thorough examination by A. A. Noyes and Falk (J. Amer. Chenz.SOC.,1912, 34, 455) leads to the conclusion that for electro-lytes consisting of two univalent ions the difference does not reach more than 2 per cent. if the solutions are 0.1 normal or less. The same is also valid for potassium sulphate and lead nitrate. For salts such as calcium chloride, calcium nitrate, magnesium chloride, etc., the deviation is much greater, the freezing-point method giving too high values. The deviation seems to have something to do with the hygroscopic nature of most of these salts. For copper sulphate and similar salts I have found that the said method gives too low values, which is due to the formation of double molecules, as Hittorf observed as early as 1859. The change of the molecular composition with dilution is seen from the simultaneous changel of the rate of migration.The chief point, however, is that salts (strong acids or bases included) consisting of two univalent ions give the molecular depression 2 x 1.85=3’7, salts of one bivalent ion with two univalent ions give 3 x 1.85=5*55, salts of one ter-valent ion with three univalent ions give 4 x 1*85=7*4, etc., whereas non-electrolytes give 1.85, all in extreme dilution. In extreme dilution the dissociation is complete. Further, it was possible to calculate the degree of dissociation from the strength of the catalytic action of the acids, and in 1889 I’showed that, within the limits of the errors of observation, the values found in this manner agree wholly with the values deduced from the magnitude of the electrical conductivity.Of the three methods of determining the degree of electrolytic dissociation, that founded on the measurement of the electrical con- ductivity has always been preferred to the other two. This choice 169 is chiefly based on practical reasons, because the method is applic- able to solutions in all solvents, and because it is possible to deter- mine the conductivity with an accuracy of about 0.2 per cent. up to the highest dilutions investigated-about 0*0001 normal. The high dilutions are just those by which the trustworthiness of the theory ought to be controlled. There was also a fourth fundamental fact in favour of the dis- sociation theory, namely, the additive properties of solutions of electrolytes. Certainly there are other additive properties valid also for non-dissociated substances; for example, the mass of a sub-stance is an absolutely additive property, because it is equal to the sum of the masses of the constituents. If we except the mass, however, the additive character is far less prominent for undisso- ciated molecules than for electrolytes.The additive properties of solutions of electrolytes have for a long time attracted the attention of physico-chemists, because they are so strongly pronounced. If the electrolytes are dissociated into their ions, it is quite clear that the properties of their solutions may be regarded as the sum of the properties of the solvent and of the ions. The additive property which is most familiar to the chemist, is the chemical reaction of solutions of electrolytes.All salts containing chlorine as ion give the reaction “ of chlorine,” as it is said, but it would be more exact to say “of the chlorine ion.” But chlorates containing the ion ClO,, perchlorates with the ion ClO,, the numerous chloro-salts of cobalt, platinum, iridium, etc., in which the chlorine is placed in the inner sphere, according to Werner, and all the salts of the chloro-substituted organic salts, do not give “the reaction of chlorine.” On these fair strong foundations: the freezing point, the elec- trical conductivity, the chemical reactions and other additive proper- ties of electrolytic solutions, as well as the strength of acids and bases, it was possible to erect a thoroughly solid building capable of sustaining attacks from without, and this building is the theory of electrolytic dissociation, first enunciated in 1887. As a general conclusion, it may be stated that the difficulties inherent to the theory of electrolytic dissociation have been over-come only within a very recent period, when the observed facts have been more closely examined. It is now our task to investigate the causes which interf\ere with the simple laws in more concen- trated solutions, and to find those other theoretical laws which govern these deviations.In presenting the Faraday Medal to Professor Arrhenius at the conclusion of the lecture, the PRESIDENTsaid : Professor Arrhenius, it is now my very pleasant duty to hand you the 1‘70 Faraday Medal, the highest honour the Society has to confer, and I should like to add an expression of our deep regard for you as an honoured member and our respect for you as a man of science.CHOOKES,Sir WILLIAM in proposing a vote of thanks to the lecturer, said : Mr. President, Ladies and Gentlemen,-With deep satisfaction I rise to propose a vote of thanks to our distinguished guest, and to offer our congratulations to him on his very interest- ing lecture. Professor Arrhenius has made his subject glow. He has drawn freely upon his vast stores of knowledge, and he invites us to share in the astonishing results of his researches. We are glad t’o welcome him in this country, where, indeed, he is already well known, and glad to felicitate him upon his command of our language, and on the fluency which is so marked a feature of his speech.We find it peculiarly fitting that the Faraday Lecture should be delivered by the Director of the Nobel Research Institute. There is perhaps no need for me to remind you of Professor Arrhenius’ scientific work. It is known to many how, more than a quarter of a century ago, he contributed to science one of its greatest generalisations, which he has now placed before you here, and which, after much strife, has taken its place as one of the corner-stones of chemistry. In early days I well remember the hostile objections. The hot controversies that raged reminded one of one of Ruskin’s whimsical sayings--that most matters of any consequence are not merely to be regarded from two points of view, but ar0 really three- or four-sided, or even polygonal, and “trotting round a polygon is stiff work for people who are in any way stiff in their opinions.” We can hardly listen to a Faraday Lecture without letting our thoughts dwell upon the great Faraday himself, and comparing him and his work with that of his eulogist, our illustrious guest.Faraday’s work, like that of Arrhenius, lay chiefly in the border- land of chemistry. He was the pioneer in the region of physical chemistry, which of late years has revealed such boundless stores of wealth. There is an obvious close connexion between his electro- chemical laws and Arrhenius’ theory of electrolytic dissociation.Faraday was a true epoch-maker, and a most striking example of the supreme value of those who cultivate science for its own sake without ulterior motives and without thought of the commercial value of their discoveries. How enormous is the value of Faraday’s work the world has not yet by any means realised, but if in later times an adequate appreciation of its far-reaching results comes to be written, I am almost tempted to suggest that its title might be Civilisation in the Making.” 171 Arrhenius has suggested to us how worlds may be made, and surely Faraday did more than any one single individual to show us how to civilise worlds when made. A further resemblance may be observed between our guest and Faraday, and that is the remarkable gift of clear exposition. Not many of those present, I suppose, ever heard Faraday lecture; but some of you know of his fame in exposition, and I can assure you from personal ex.perieiice that it has not in the slightest degree been exaggerated. Professor Arrhenius’ later work in immuno-chemistry, and his researches into the action of toxins and anti-toxins, have challenged the attention of the scientific world, and still more recently his investigations in cosmogony have startled staid scientific men. “Worlds in the Making” is a title bound to catch the mind’s eye, and those of you who have read the book, and the later volumes on the Life of the universe, will no doubt agree with me as to the absorbing interest of the subject, the cogency of the arguments, and the skill with which they are handled.The world is deeply in need of researchers both of the type of those whose genius is characterised by that fertility of resource in experi-mental ‘investigation exhibited by Faraday, and of the type of Arrhenius, whose gifts of intrepid speculation and imagination enable him to reveal new worlds of thought. Both are revolu-tionaries and founders of new kingdoms. Both types are rare. Both are “world compellers,” and the world’s debt to them is incalculable. I think we may begin to look hopefully forward to a time of fuller recognition of scientific genius and deeper apprecia- tion of the value of scientific work, and certainly the British nation will not be found in the rear-guard in that desired advance.Once again let us offer our hearty thanks to Professor Arrhenius, and assure him of our genuine appreciation of his masterly ex-position of, I might almost say, a sensational chemical problem. Sir WILLIAM TILDEN, in seconding the vote of thanks, said: Ladies and Gentlemen,-I am one of those who cling tenaciously to the principle of submission to properly constituted authority. Consequently, when the President preferred a request that I should stand in this honourable position of seconding the vote of thanks to the Faraday Lecturer, which has been so eloquently proposed by the President of the Royal Society, I looked upon it as a com- mand, and concealed my own misgivings, feeling as I did that I could not be regarded as a representative of any body of chemical opinion on the present occasion.We are here to-day to celebrate the great name of Faraday. A celebration of the same kind has been held by the Chemical Society on, I think, ten previous occasions, and it would be impossible, as you realise, no doubt, for the Society effectively to carry out its wish except with the aid of our eminent colleagues. and friends who have visited us from abroad on all these previous occasions. We have had assistance from France, from Germany, from Italy, and from the United States. On the present occasion we have the great pleasure of welcoming among us, not for the first time-for his face and figure are familiar to everybody in London-we have the great pleasure of receiving here to-night and welcoming a representative of that great country which, I am almost tempted ta say, has done more-but at any rate has contributed not less- than any other country to the advancement especially of chemical science.It is only necessary to remember that Scandinavia has produced Scheele and Berzelius, beside many others whose names will doubt- less occur to you. I think you will agree with me that our friend who has just delivered the Faraday Lecture is a worthy successor to his great countrymen whose names I have just mentioned. I think the first qualification in a Faraday Lecturer must be that he has by his own work and his own researches contributed to the advancement of that department of science with which Faraday’s name is, and has always been, associated; and in this case that quality is presented eminently by the Faraday Lecturer. With regard to the theory of electrolytic dissociation, which has been the subject of the discourse this evening, my experience, perhaps, is very much that of a good many others, and probably the majority, in this room.When it first began to be discussed seriously, close upon twenty years ago, I confess I was among those who were strongly hostile. But I felt, as time went on, that I had to lay before my students-for I was a teacher in those days-at any rate an exposition of .what> other people believed in regard to this department od the theory of chemistry; and it was my experience that by merely presenting those views, so new and so unacceptable as they were to me at that time, I gradually got to feel that they were inevitable, and that they were absolutely necessary.One was forced to consider all the pros and cons, and ultimately I was led to a conviction of the very valuable character of the theory that I was then expounding. Of course, the theory of electrolytic dissociation, like every other theory which h-as become established in the fabric of theoretical chemistry, must pass through, has passed through, and will continue to pass through the same kind of experience as other theories. It has met, first of all, strong opposition and violent criticism, but it has ultimately been accepted, and all that remains is to clear away the few comparatively small difficulties.173 At the same time, I always feel, and I hope most teachers feel, that every theory which we accept is bound to be modified more or less as time goes on. If not actually abolished, it will at any rate be modified very considerably in favour of something which is more comprehensive, and perhaps illuminated by a large number of new facts at present unknown to us. I need scarcely say that I thank the President for allowing me the distinguished honour of standing here on this occasion, and I support most cordially the proposition which has been laid before the meeting by the President of the Royal Society. The CHAIRMANhaving put the vote to the meeting, it was carried with acclamation.Professor A'RRHENIUS,in acknowledging the vote of thanks, said : Amongst learned societies, the Chemical Society was one of the very first which lent me support and gave me encouragement. It has therefore been a great pleasure and favour to me to come back to London on repeated occasions and speak to and see my many dear friends in this Society. Every time I returned I felt that your kindness and friendliness towards me had increased. To-day it has reached its maximum, when you have conferred upon me the greatest honour you can give. I cannot express my deep feelings of gratitude towards the Society as I would wish, and I must confine myself to saying that you have my warmest and deepest thanks. Thursday, June 4th, 1914, at 8.30 p.m., Professor W.H. PERKIN, LL.D., F.R.S., President, in the Chair. The PRESIDENTreferred to the loss sustained by the Society through the death of: Elected. Died. Sir Joseph Vilson Swan.................. Jnne 31x1,1865. May 27th, 1914. Mr. D. R. Keller was formally admitted a Fellow of the Chemical Society. A certificate was read for the first time in favour of Mr. George von Kaufmann, jun., Christ's College, Cambridge. Of the following papers, those marked * were read: 174 “153. “The influence of nitro-groups on the reactivity of substituents in the benzene nucleus.” By James Kenner.* The influence mentioned in the title was referred to two distinct functions exercised by nitro-groups. One of these, which is shared with other meta-directive groupings, consists in the conferment of a certain degree of mobility on substituents in ortho-or para-positions, and was explained in terms of Flurscheim’s views.The other enables the substituent, thus rendered mobile, to take part in react.ions, in spite of the steric influences to which it is exposed. This function is exercised most powerfully by the nitro-group, and was correlated with another property characteristic of nitro-groups, namely, the power to form additive compounds. , An alternative theory, proposed by Borsche (Annalen, 1311, 386,356; 1913, 402, 81), was also discussed. With the assistance of Mr. R. Curtis, and in connexion with the views developed above, the action of hydrazine hydrate on methyl 2-chloro-3 : 5-dinitrobenzoate was studied and shown to lead at once to the formation of 5: 7-dinitro-3-keto-1: 3dihydro- indazole, without admitting of the isolation of the intermediate hydrazine derivative.In the case of phenylhydrazine, the main product was 5 : 7-dinitro-3-keto-2-phenyl-l: 3-dihtydroindazoZe, ac-companied by a small proportion of 2 : 4-dinitro-6-carbometh.ozy-hydruzobenzene, and another compound of unknown constitution. The indazole derivatives named gave rise to quinonoid sodiunz salts, whilst, by the action of phosphoryl chloride at 180°, 3: 5: 7-trichloroindazole and 3 : 5 : 7-trichJoro-2-phen~lindazole were pro-duced, the nits-o-groups attached to the benzene nucleus having suffered displacement by chlorine atoms.DISCUSSION. Dr. FLURSCHEIMwelcomed Dr. Kenner’s paper as an interest-ing contribution .on the problem of benzene substitution, It appeared that, generally, chemical reactivity was governed by the nature of the affinity of the atoms involved (polar factor), by the amount of that affinity (quantitative factor), and by considerations of space (steric factor). Dr. Kenner had taken the last two factors into consideration, and he had been able to embrace a considerable number of facts. At the same time, the polar factor could, of course, not always be neglected. For the mobility, for instance, of a nitro-group in 1: 3 : 5-trinitrobenzene (Lobry de Bruyn), of fluorine in m-fluoronitrobenzene (Hollenian), or of the 1-bromine in 1:2 :4:6-tetrabromobenzene (Jackson and Calvert), * This paper \\-as read at the meeting on May 21st, 1914.175 it even appeared that the polar factor was alone responsible; in other words, even when a sufficient amount of affinity was avail- able for it, a substituent might easily be detached from thel nucleus when both exhibited strong electropolarity of the same kind, so that the nature of their affinity was not conducive to mutual saturation (compare Ber., 1906, 39, 2016). Undoubtedly, the problem of the replacement of one benzene substituent by another was more complex than that of the mere substitution of hydrogen, and he was glad that Dr. Kenner had brought the subject before the meeting. Professor J. T. HEWITTreferred to the work of Borsche and Bahr (A?zizaJen,1913, 402, Sl), which shows that in the apparently symmetrical 4 : 6-dichloro-1: 3-dinitrobenzene, one halogen atom is more mobile than the other.This might be explained if the pro- ducts with amines, etc., assumed a quinonoid configuration; for if the 6-chlorine atom had reacted, and quinonoid structure were established between positions 6 and 1, the linking between the carbon atoms 3 and 4 must of necessity be a single one. Dr. KENNERagreed that his views might need amplification in order to become applicable to all the observed cases of mobility, and cited, as an example, the formation of the trichloroindazoles mentioned above. In his opinion, recent work on the metallic ketyls lent strong support to the view that colour was connected with the presence of residual affinity, and therefore to Hantzsch’s formula for the nitroanilines.He drew attention to another apparent fallacy in the views expressed by Borsche and Bahr, and suggested an alternative explanation of the results obtained by these workers. “154, Studies in the succinic acid series. Part I. The chlorides of succinic and methylsnccinic acids, and their constitution.” By George Francis Morrell. Since succinyl chloride gave with ammonia a 90 per cent. yield of as-succinamide, and with benzene and aluminium chloride a similar amount of succinophenone, Auger (Ann. Chim. Phys., 1891, [vi], 22, 326) concluded that it was a mixture of two isomerides. Meyer and Marx (Ber., 1908, 41, 2459) found that it gave with alcohols only the normal esters, and suggested a theory of tautomerism.In the present investigation, succinyl and methyl- succinyl chlorides have been prepared, and a consideration of their physical properties and anomalous behaviour with ammonia and substituted ammonias is held to disprove Auger’s theory, and to lend no support to the tautomerism theory. Succinyl chloride, for 176 example, was found to be a crystalline solid, melting sharply at +ZOO, and boiling at 87-88O/18 mm. Whether the first or last portions of the distillate were taken, it gave with aniline nothing but the s-anilide (m. p. 230O); with methylamine, only a 15 per cent;. yield of the s-dimethylamide; and with ammonia, almost entirely the as-amide.It is concluded that these acid chlorides are definite chemical individuals, and that there is no satisfactory evideace whatever for assigning to them any other constitution than that of normal acid chlorides, COCl~CHz*CHz*COC1. The formation of asymmetric products probably takes the follow- ing course, for example, with ammonia : YH,*COCI cH,*COCIICH,*COCl +NH,4 CH,*C(OH):NH + yH,---CO YH,---CO CH,.C(:NH)>' +CH,*C(NH,),>o. "155. ('The dilution limits of inflammability of gaseous mixtures. Part I. The determination of dilution limits. Part 11. The lower limits for hydrogen, methane and carbon monoxide in air." By Hubert Frank Coward. and Brank Brinsley. The smallest amount of hydrogen in an inflammable mixture of hydrogen and air has been variously stated as low as 4.5 and as high as 10 per cent.Similarly, the values given for the greatest amount of hydrogen in an inflammable mixture of hydrogen and air are as low as 55 per cent. and as high as 80 per cent. The hydrogen-oxygen mixtures show similar want of accord in the results of previous workers. A partial explanation exists in Clowes' observation that in certain weak mixtures a flame may be propagated upwards, but not downwards. A re-examination of the inflammability of weak gaseous mixtures has been started, based on the definition that, a mixture at a defined temperature and pressure is inflammable per se if, and only if, it will propagate flame indefinitely, the temperature and pressure of the unburnt gases being constant.The flame observed in many weak mixtures travels more slowly than the convection current set up by the, flame, so that the criterion of inflammability is the observed travel of a flame upwards through a vertical vessel of sufficiently great dimensions to avoid appreciable cooling influence by the walls and to'provide a sufficient length for observation of the flame to leave no doubt as to its capacity for indefinite self-propagation. 177 The experiments of previous observers do not satisfy this criterion, and the critical experiments of the authors have been carried out in vessels, one having a capacity of 170 litres, another a length of 4.5 metres. With all three gases used, the flames in certain weak mixtures have been observed to start as vortex rings, which rose, expanded, and ultimately broke into a general self- propagating inflammation, or were extinguished. The lower limits of inflammability of mixtures of each of the three gases with air saturated with aqueous vapour at 17O to 18O were: Hydrogen .....................4’1 per ceut. hlethaiie ..................... Carbon monoxide.. .......... 5.3 12.5 ,, ,, DISCUSSION. Professor BONEdrew attention to the great importance of accurate information concerning the behaviour of gaseous mixtures at, or near the lower explosion limits, and congratulated the authors on both their experimental demonstration and the beautiful photo- graphs which they had exhibited.He agreed in principle with the authors’ definition of “inflammability,” but pointed out the necessity of distinguishing between “ignitability ” and “in-flammability.” The phenomenon of ignition was very complicated, and was probably not a purely thermal one, as Professor W. M. Thornton had recently shown in an important communication to the Royal Society on the electrical ignition of gaseous mixtures, from which it appeared probable that ionisation was a factor pre- cedent to the actual combustion. Dr. SCOTTsuggested that the mixtures of hydrogen with oxygen and with air might be made more luminous by using weighed quantities of sodium, which would give the required quantities of hydrogen in contact with the water.The brilliant yellow of the flame would probably enable much more detail to be visible to the eye and to be recorded on the photographic plate. Dr. E. RIDEALasked whether there was any indication of a dark wave preceding the luminous cap which travelled up the tube. The dark wave caused by local compression of the gas could be conveniently photographed by a method which he had used with great success in the case of rifle bullets travelling through different gases. The bullet in its course is made to traverse two copper gauze disks placed close to one another; by this means contact is made between the two disks, which are connected to the out- sides of the Leyden jars of a Wimshurst machine. The primary spark follows a short time after contact is made, and if there is a photographic plate opposite to the spark-gap of the Wimshurst, 178 the bulletl, passing between the spark and the plate, throws its shadow on the latter.In front of the photograph of the bullet io always observable a parabolic-like curve, being a cross-section of the paraboloid-shaped mass of compressed .air partly dragged and partly pushed forward by the bullet in its flight. The line on the plate is caused by the fact that the compressed air has a different refractive index to that surrounding it. Different gases gave curves of the same order, but different' constants. In the present case, during combustion one might expect local differences of pressure, indications of which could be obtained by an adaptation of the foregoing method.Dr. COWARDagreed with Professor Bone that it was desirable to distinguish between inflammability and ignitability. A large flame might be developed in a mixture when an electric spark was passed or a jet of flame introduced into it, although the inflamma- tion would not be capable of indefinik self-propagation. This mixture would therefore not be inflammable per se, but a possibly dangerous flame might be formed in it; the initial impetus of the spark was not rapidly dissipated. The authors had seen such flames in mixtures just below the dilution limit which were nearly 30 cm. wide, and travelled 60, 90, or even 120 cm. from their source. Dr. Scott's suggestion for rendering the hydrogen flames more luminous would be useful for photographic purposes; up to the present, the authors had desired to se0.and record the appearance of flame in pure mixtures, and for that reason to avoid the presence of spray or dust particles. "156. LL The thermal decomposition of methyl alcohol." By William Arthur Bone and Hamilton Davies. The authors find that methyl alcohol vapour decomposes on heatr ing principally in two ways, namely: (1) An essentially low-temperature decomposition into, primarily, steam and a residue, :CH,, which has a fugitive free existence, CH,*OH =:CH2+H,O. (2) The normal high-temperature decomposition primarily into f omaldehyde and hydrogen, the formaldehyde then decomposing into carbon monoxide and hydrogen, CH,*OH =CH20+ H,.co + H, Thus, at 650°, 20 to 25 per cent. of the methyl alcohol decom- poses according to (I), the remainder according to (2), the R,C: 179 formed during (1) combining with part of the H, produced during (2), forming methane. At 1000°, more than 95 per cent. of the methyl alcohol decom- poses according to (a), the remainder according to (1). At neither temperature is there any separation of carbon, nor could any acetylene be detected in the products. 157. ‘‘A comparative study of the absorption spectra of some compounds of phosphorus, arsenic, antimony, and bismuth.” (Preliminary note.) By Cecil Reginald Crymble. In accordance with the rule connecting valency and absorption (T., 1912, 101,266), it has been found that solutions of compounds of the above elements absorb ultra-violet light, the extent of the absorption varying greatly with the nature of the compound.If the chlorides ECl, are compared, the limit of general absorp- tion is displaced towards the visible on passing from phosphorus trichloride to bismuth trichloride, and in the latter compound an absorption band makes its appearance in Bi/1000 solution with a head at 2850. The pentachlorides of phosphorus and antimony have been ex-amined, and they possess much greater absorptive power than the corresponding trichlorides. The limit of the general absorption of antimony trichloride and the absorption band of bismuth chloride are displaced towards the visible on formation of the complex salts ECl3,nMC1. Like sulphat,es and selenates, the highly oxidised phosphates and arsenates are quite diactinic ;antimonates and arsenites show slight absorption; and, as is known, bismuthic acid is a red powder.The grouping P:O in the phosphorus oxy-acids is devoid of absorptive power, and phosphoryl chloride is almost diactinic. The investigations are being extended to the fourth group of elements, especially to tin and lead; and from the variations in the absorptive power of solutions of stannic chloride, which occur on keeping, it is hoped to gain some information on the constitu- tion of these salts. ‘I158. The reactions of a-amino-P-hydroxy-compoundsas cyclic structures.” By James Colquhoun Irvine and Alexander Walker Fgfe. The behaviour of /3-hydroxy-a&diphenylethylamine towards methylating agents has been studied in order to ascertain if com-pounds in which a secondary hydroxyl group and a primary amino- 180 group are attached to neiglibouring carbon atoms are capable of reacting in accordance with a cyclic formula.By the action of silver oxide and methyl iodide on the amine, a dimethyl derivative melting at 135-137O was obtained. As this compound contained no normal methoxyl group, yet nevertheless failed to form a methiodide, a hydrochloride, or a platinichloride, it is regarded as the anhydride of /3-hydroxy-a/3-diphenylet?byldimethylammoniant hydroxide (I). In the absence of salttforming properties, and in its capacity to combine with silver iodide, the compound resembles the alkyl glucosamines, for which a cyclic structure has already been suggested.On the other hand, direct methylation of 0-hydroxy-a/3-diphenyl- ethylamine by means of methyl iodide gave successively B-hydroxy-a/3-diphenylethylmethylamine,/3-hydroxy-a~-diphenylethyldimet?ayl-ainiiae (11),and the corresponding methiodide. The properties of these substituted amines are perfectly regular in that they form salts and platinichlorides, from which it may be concluded that the normal open-chain structure may be applied to them. The following formulze are consequently ascribed to the isomeric coin- pounds isolated : C,H,-yH-Q C,H,*TH*OH C,H,*CH*NHMe2 C,H,*CH*N Me, u.1 (11.1 The constitution assigned to B-h ydrox y-afl-diphen yle th yldimethyl- amine (11) was confirmed by the conversion of the compound into 8-methoxy-ap-diphe izyle th,yldim ethylamine, OMe*CHPh*CHPh*NMe,, which, in turn, reacted with nitrous acid to give hydrobenzoin methyl ether.The same methoxy-amine resulted from the methyl- ation of /3-methoxy-a/3-dip?benylet?~ylamine,both by the silver oxide reaction and by the agency of methyl iodide, the compound in the former case being isolated as the methiodide combined with one molecule of silver iodide. The results of the investigation are applied to the constitutioii of the alkyl glucosamines, and the capacity of these coinpounds to combine simultaneously with alkyl haloids and with silver haloids is explained on the assumption that the addition takes place through the oxygen atom of the ring.159. Ionic equilibria across semi-permeable membranes.” By Frederick George Donnan and Arthur John Allmand. Experiinents have been made on the distribution of potassium chloride between two compartments separated by a copper ferro- 181 cyanide membrane, one compartment containing potassium f erro-cyanide. The higher concentration of potassium chloride in the solution free from ferrocyanide, and the quantitative relation of this unequal distribution to the concentration of chloride and ferro- cyanide, have been established. The results agree, in general, with the view of such membrane- equilibria proposed by Donnan. A discussion of the distribution data and the measurements of electromotive force appears to show that, at all events in the case of a copper ferrocyanide membrane and potassium ferrocyanide solutions, the phenomena are quantita- tively not so simple as supposed in the theory mentioned.160. 6L The effect of ring-formation on viscosity.” By Ferdinand Bernard Thole. The opinion previously put forward that ring-formation is accompanied by an increase in viscosity has been confirmed by a comparison of the viscosities of a considerable number of cyclic compounds (carbocyclic and heterocyclic rings containing from two to seven atoms) with those of corresponding open-chain analogues. The chemical types of the latter have been carefully chosen to correspond with those of the cyclic compounds, since the results of some previous investigators with other physical properties have been confused by illegitimate comparisons. Viscosity has been found to fall in line with certain other physical properties in showing an anomaly which varies steadily as the complexity of the ring increases, and giving no change of direction on passing the five-membered ring-system.161. nb Action of monochloroacetic acid on thiocarbamide and monoalkylated thiocarbamides.” By Prafulla Chandra RQyand Francis V. Fernandes. By the action of monochloroacetic acid on thiocarbamide in aqueous solution, the latter evidently tautomerises, and gives rise to f ormamidinethiolacetic acid, NH,*C(:NH)*S*CH,*CO,H. If, however, acetone is used as a solvent, the corresponding hydro- chloride of the base is obtained.Similar hydrochlorides are yielded by the action of nionochloroacetic acid on mono-substituted tliiocarbamicles in acetone solution ; thus, the hydrochlorides of rri ethylf ormamidine- and ally1f ormamidiize-t~,iolacetic acids have been prepared. 182 162. ‘(Action of Grignard reagents on acid amidea.” By Alex. McKenzie, Geoffrey Martin, and Harold Gordon Rule. In continuation of former work (McKenzie and Wren, T., 1908, 93, 310; 97, 473; Wren, T., 1909, 95, 1583, 1593), the authors have examined the action of Grignard reagents on several acid amides. In those cases where a ketol was isolated as one of the products, the yield was small. A mixture of benzoin and a&dihydroxy-aflP-triphenylethane is produced by the action of magnesium phenyl bromide on mandelopiperidide.The formation of benzoylbenzylcarbinol from a-hydroxy-P-phenylpropionamideis accompanied by the formation of ap-dihydroxy-aay-triphenyl-propane. d-Benzoylbenzylcarbinol undergoes racemisation at the ordinary temperature when a few drops of sodium. ethoxide are added to its alcoholic solution. This change is, however, much slower than that undergone by E-benzoin under similar conditions; the value for the rotation of a 5 per cent. solution falls to about onehalf of the original after 481 hours have elapsed. 163. (( Synthetic hydrocarbons allied to the terpenes.” By Walter Norman Haworth and Alexander Walker Fgfe. The method used by Blaise (Compt. rend., 1901, 133, 1217) for the production of ketones from nitriles has been applied in the synthesis of three hydroaromatic ketones of the cyclohexene series.These were converted into optically active and inactive carbinols and hydrocarbons analogous to the members of the terpene group. The alteration in the rotation values due to the synthetic changes has been carefully studied, as have also the spectrochemical properties. The compounds described are interest- ing examples of ‘‘multiple disturbance ” of con jugation, and show the expected diminution of exaltation in accordance with the views OF Auwers and Eisenlohr. 164. ‘(Asymmetric tervalent nitrogen.” (Preliminary note.) By Tom Sidney Moore. The cause of the failure of the attempts that have been made to obtain optically active compounds owing their asymmetry to the presence of tervalent nitrogen atoms attached to three different groups is probably the rapid racemisation of the substances investi- gated, which havr, all been of the type N-/ab \c.183 Compounds of the type N-/a\ b-N and N--/a\ N, in which a, b, \C/ \@' and c are three different divalent groups or chains, of which at least one is unsymmetrical with regard to the two nitrogen atoms, should exist in two enantiomorphic forms. Racemisation might be expected to be slow, or even non-existent, in compounds of the first type, and it might be slow enough in compounds of the second type to allow of the demonstration of isomerism. Experi-ments on the preparation of suitable compounds of the first type are now in progress; of the second type several examples are known, and one of these has been examined. The compound chosen was 2-p-sulphophenyl-2 : 3-dihydro-1 :2 :4-naphthaisotm'azine, which was prepared according to the general method given by Meldola and Forster (T., 1891, 59, 678), and found tobe very similar in properties to the phenyl derivative described by them.The two possible forms would be : The following results were obtained with a specimen of the brucine salt of this compound after it had been twice recrystal- lised from alcohol. (1) The brucine salt was treated at Oo with excess of N-sodium hydroxide, and the resulting aqueous solution extracted with chloroform until it was free from brucine (three extractions).In four such experiments hhe resulting alkaline solution of the sodium salt showed a small but definite dextrorotation, which decayed with time, until after a few hours the solution was optic- ally inactive. The values for the initial specific rotation of the sodium salt were between + [3*5O]and + [1*7O]. Parallel experi- ments with the acid itself gave, as one expected, inactive solutions. In other experiments with the brucine salt, where only the equivalent quantity of sodium hydroxide was used, the solution .of the sodium salt was inactive; this agrees with the experience of Mills and Bain (T., 1910, 97, 1866; 1914, 105, 64), who found that excess of alkali hindered the racemisation of their compounds.(2) The brucine salt, when added to chloroform, first dissolves completely, and then deposits some of the acid, this process not being complete for some hours. One such solution was allowed to remain overnight, and its rotatory power was measured after 184 filtration. It was then kept for three days in a closed vesseI (during which period no further acid was deposited), and its rota- tory power again measured. The angles observed were -0*15* and -0’22O respectively. This change of rotatory power with time indicates that the brucine salt contained an excess of the dextro-acid, which racemised gradually on keeping. Mr. J. J. Manley very’kindly estimated the sulphur in a speci- ment of the acid recovered from the brucine salt.Found, S =9-65, C,,H,,O,N,S requires S =9.44 per cent. The author is proceeding with a detailed examination of this and similar compounds; in the meantime, t’he results given above offer definite evidence of asymmetry in tervalent nitrogen atoms attached to three separate groups. 165. (‘The alkaloids of Daphnandra micrantha.” By Frank Lee Pyman. The alkaloids of the bark of the Queensland plant, Daphnandra micrantha, Benth., have been investigated, and three new crystal-line bases, daphnandrine, C3,H3,06N2,daphnoline, CaHsO6N2 (or C3,Hx0,N,), and rnicrant hine, C36H3206N2,have been isolated and characterised. 166. (( The relation between the absorption spectra and the constitn- tion of certain isoquinoline alkaloids and of the alkaloids of ipecacuanha.” By James Johnston Dobbie and John Jacob Fox.It was shown that cmtain isoquinoline alkaloids, including tetra- hydroberberine, laudanosine, corydaline, the salts of cryptopine and protopine, which possess similar spectra, are all characterised by the presence of unreduced nuclei derived from catechol. When the spectra of one molecule of these alkaloids are compared with the spectra of two molecules of creosol (4-hydroxy-3-methoxy-toluene), they are seen to have their band in the same position. In these, as in cases previously described (T., 1911, 99, 1254; 1912, 101, 77; 1913, 103,1193), the reduced part of the molecule has very little influence on the spectrum. It was also shown that the band of the spectrum of morphine, which contains one catechol nucleus, only differs from that of creosol in being somewhat narrower.Emetine and cephaeline give the same spectrum as the above- mentioned alkaloids, and therefore in all probability also contain catechol nuclei, a conclusion which is in harmony with the facts of their constitution, so far as these are) known (Carr and Pyman, P., 1913, 29, 226; 1914, 30,157). 185 167. ‘‘ The interaction of benzoin and the chlorides of dibasic acids.” By Hamilton McCombie and John Wilfrid Parkes. The interaction of benzoin and dibasic acid chlorides was studied in the hope of obtaining compounds derived from one molecule of benzoin and one molecule of the acid chloride, which would prove to be derivatives of stilbenediol.The following acid chlorides were employed : carbonyl chloride, oxalyl chloride, phthalyl chloride, and camphoryl chloride. In all cases, however, even when excess of benzoin was employed, the only compounds that could be isolated were formed from two molecular proportions of benzoin and one of the acid chloride. In t’he case of oxalyl chloride, two different compounds were isolated, both possessing the formula C,,*,,O,. 168. ‘‘ The fractional distillation of petroleum.” By James McConnell Sanders. In the examination of crude petroleum, burning oil, or petrol by the distillation test, it is often desirable to determine the specific gravity of successive fractions; the rule of the New York Produce Exchange requires, for an oil to be considered as a “pure natural oil,” that it should exhibit a regular gradation in the densities of successive fractions. When the Engler method is used for fractionating an oil, or when the amount of sample available is small, the ordinary rapid methods of determining the specific gravities of the fractions cannot be conveniently used.The author described an apparatus whereby the gravity of successive fractions may be determined rapidly during the distillation, the fractions being removed in succession or mixed, and the gradual change of density dete’rmined as the distillation proceeds. From the data obtained, curves may be plotted showing the behaviour of an oil during close fractionation, or the effect of cracking at any stage.Some special difficulties found in the distillation of heavy asphaltic oils of Mexican origin were discussed, more especially in regard to the determination of water, and the carrying of the distillation to the “coking stage.” A special distillation flask was described, whereby these difficul- ties are overcome by means of an electrically deposited copper coating to the flask, an electrically heated and controlled still- head, and the subsequent removal of adhering water in the side- neck and condenser tubes by means of absolute alcohol, which is then treated with magnesium amalgam and the evolved hydrogen measured. 169. ‘‘Hercuration of aromatic amines.” (Preliminary note.) By Gilbert T. Morgan and J. Campbell Elliott. The circumstance that aromatic compounds cont’aining metallic and metalloidal substituents are becoming increasingly important in therapeutics renders the conditions of f ormatioii of these pro- ducts a matter of considerable interest.The introduction into aromatic nuclei of arsenic, antimony, and similar metalloids involves reactions needing special precautions, and proceeding only slowly to completion. On the contrary, the mercuration of aromatic amines proceeds so rapidly and quantitatively that the process can be readily demonstrated as a lecture experiment. One gram of aniline is added to 6.6 grams of mercuric acetate dis- solved in 300 c.~. of cold methyl alcohol, and the solution boiled for two minutes. Another 6.6 grams of mercuric acetate dissolved in 300 C.C.of methyl alcohol are boiled for the same time, and serve for a control experiment. The two hot solutions are each poured into 300 C.C. of water containing 7.5 grams of potassium iodide. The conhrol solution of mercuric acetate gives immediately yellow mercuric iodide, changing almost instantaneously into the stable red modification. The solution to which the aniline has been added no longer contains mercuric ions, the whole of the mercury having become attached to the aromatic nucleus. It yields a yellowish-white precipitate of di-and tri-iodomercurianilines, which is quit’e distinct from the red precipitate obtained in the control experiment. m-Toluidine (1.1 gram) may be substituted for aniline in the foregoing experiment, with a similar result, the yellowish-white precipitate containing a mixture of di- and tri- iodomercuri-m-toluidines (compare Schrauth and Schoeller, Ber., 1912, 45, 2808).Other bases containing unsubstituted ortho- and para-positions behave in a similar manner. With methylaniline and dimethyl- aniline, similar proportions (2-3 molecules) of mercuric acetate are t.aken up, but the resulting yellowish-white, organic mercuri- iodides are discoloured by red and green oxidation products respec- tively. An analogous reaction occurs with diethylaniline, the amount of coloured by-product being less. Diphenylamine reacts with 5-6 molecular proportions of mercuric acetate, and yields a voluminous, white organo-mercuri-iodide.Aromatic bases, partdy substituted in their reactive ortho- and para-positions, are also readily mercurated, but the amount of mercuric acetate taken up diminishes as substitution increases. o-Toluidine and dimethyl-o- toluidine condense with two molecular proportions of mercuric acetate, and give white organo-mercuric iodides, but with the latter base the reaction proceeds very slowly. pToluidine reacts 18‘7 readily with one molecular proportion of mercuric acetate. Further treatment with more acetate leads to oxidation. Methyl-ptoluidine and dimethyl-ptoluidine behave similarly. a-Naphthylamine and p-naphthylamine condense, respectively, with one and two molecular proport,ions of mercuric acetate, and yield the corresponding organo-mercuric iodides (compare Brieger and Schulemann, J.pr. Chem., 1914, [ii], 89, 97). When the foregoing organo-mercuric iodides are left in contact with hydriodic acid, some of the organically combined mercury is removed in the form of mercuric iodide, but these compounds are not affected by neutral iodides. 170. ‘I The viscosities of mixtures of formamide with the alcohols.” By Solomon English and William Ernest Stephen Turner. In confirmation and extension of previous work (Merry and Turner, T., 1914, 105, 748), the viscosities of mixtures of form-amide with n-propyl, isobutyl, and isoamyl alcohols at 25O have been measured. It had prelviously been shown that with water, methyl alcohol and ethyl alcohol, the negative deviation of the observed from the calculated viscosity grew less in the order of the substances named, and it was now shown that the deviation becomes positive with n-propyl alcohol, although the viscosity curve does not attain a maximum, and that the isobutyl and isoamyl alcohol curves each contains a maximum point.The n-propyl alcohol curve is sinuous, and the sinuosity is developed in the two higher alcohols, so that they contain, not only a pronounced maxi- mum, but also a minimum, point. 171. Action of nitro-substituted aryl haloids on alkali thiosulphates and selenosnlphates.” By Douglas Frank Twiss. Various investigations have already shown that the alkyl haloids can react with the alkali thiosulphates, giving the corresponding alkali alkyl thiosulphates; but the few corresponding aryl thio- sulphates discovered hitherto have been prepared by less simple processes, usually depending on oxidation of a mixture of sodium thiosulphate and an aromatic substance.Unsubstituted aryl haloids fail to react with sodium thio-sulphab, but the 2 : 4-dinitro- and 2 :4 : 6-trinitro-phenyl haloids readily enter into action with not more than a semimolecular pro- portion of sodium thiosulphate, yielding, not the corresponding organic thiosulphate compounds, which appear to be capable of only transient existence, but the corresponding sulphides. In a similar manner, reaction with not more than a semimolecular pro- portion of potassium selenosulphate produces the corresponding selenides.When an excess of sodium thiosulphate is used with 4-chloro- or 4-bromo-1: 3-dinitrobenzene, the resulting 2 : 4-dinitrophenyl sulphide is not the only product, for the solution subsequently deposits 2 :4-dinitrophenyl disulphide. An excess of potassium selenosulphate yields almost exclusively 2 : 4-dinitrophenyl di-selenide. These results are explained by the primary formation of an unstable alkali aryl thiosulphate or selenosulphate which, in the presence of excess of aryl haloid, passes Into the corresponding sulphide or selenide, according t’o the equation (for the former case) NaRS20, +RHal +H20=NaHal +R2S+H2S0,, whilst with an excess of inorganic thiosulphate or selenosulphate the alkali aryl thiosulphate or selenosulphate produced subse-quently decomposes, as their aliphatic analogues readily do, yield- ing disulphide or diselenide.At the next Ordinary Scientific Meeting, on Thursday, June lSth, 1914, at 8.30 p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated : ‘‘ Nitrogenous constituents of hops.” By A. Chaston Chapman. “The isomerism of the oximes. Part IV. The constitution of the 1C’-methyl ethers of the aldoximes and the absorption spectra of oximes, their sodium salts and methyl ethers.” By 0. L. Brady. “The wet oxidation of metals. Part 111. The corrosion of lead.” By B. Lambert and H. E. Cullis. ‘I Studies in the camphane series. Part XXXV. Isomeric hydrazoximes of camphorquinone and some derivatives of amino-camphor.” By M.0. Forster and E. Kunz. “ The velocities of combination of sodium phenoxides with olefine oxides.” By D. R. Boyd and E. R. Marle. “Colouring matters contained as glucosides in the flowers of some Indian plants.” By A. G. Perkin and I. Shurlman. “A new chlorocamphor.” (Preliminary note.) By T. M. Lowry and V. Steele. “Ideal refractivities of gases.” By W. J. Jones and J. R. Partington. “The purification and physical properties of a-bromonaphth-alene’.” By M. Jones and A. Lapworth. ‘I Det’ermination of water in alcohol-water mixturm by the clouding points of mixtures with a-bromonaphthalene.” By M. Jones and A. Lapworth. 189 C ERTIFlCATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names of those who sign from ‘(General Knowledge ” are printed in italics.The following Candidates have been proposed for election. A ballot will be held on Thursday, June 18th, 1914. Aufllogoff, Nicholas Alexander, Thsrries Haven, Essex. Chief Chemist and Works Manager to London & Thames Haven Oil Wharves, Ltd., 101 Leadenhall St., E.C. Seven years Chemist-in-charge, Refinery European Petroleum Co. Four years Refioery Manager London 9r Thames Haven Oil Wharves, Ltd. Eleven years Chief Chemist to same Co. Boverton Redwood. Vivian B. Lewes. Robert Red wood. J. S. S. Brame. Bertrand Turner. Berry, Harry, The Northern College of Pharmacy, Burlington St., Manchester. Pharmaceutical Chemist. Lecturer in Chemistry and Physics at the Northern College.Formerly engaged in the assay laboratories of the University College Hospital, London. Student under Prof. Hewlett at Bacteriological Lab., King’s College, Strand, W. E. Gower Bryant. C, H. Hampshire. Henry Garoe tt. G. 7‘. V.N~wsholme. M. S. Pickering. G. Crewe Clmmbres. Boon, Alfred Archibald, Chemistry Department, Heriot Watt College, Edinburgh. Assistant Professor of Chemistry, Heriot Watt College, Edinburgh. D.Sc. (Edinburgh). Author of papers communicated to the Society. Examiner in Chemistry to the Pharmaceutical Society (North British Branch). D. S. Jerdan. Isidor Morris HeilbroD. Forsyth J. Wilson. A. Dctvidson. A. Scott Dodd. 190 Collins, Stanley Winter, 1, Tideswell Road, Putney, S.W. Lecturer in Chemistry at King's College, University of London.B.Sc. Hons. Chemistry, London ;Fellow of the Institute of Chemistry. John M. Thomson. W. D. Ralliburton. Herbert Jackson. Patrick H. Kirkaldg. Henry L. Smith. C'remer, Herbert William, Preston Lea, Faversham, Kent. Student Demonstrator in Chemistry, University of London, King's College. B.Sc. London (1st Class Hon.) in Chemistry. John M. Thomson. W. D. Halliburton. Herbert Jackson. W. B. Bottomley. Patrick H. Kirkaldy. P. A. Ellis Richards. Cutler, John Vernell, Rose Cottage, Farringdon Lane, Ribbleton, Preston; Associate Municipal School of Technology (Chemistry, 1908), Manchester. Previously Assistant Chemist, The Badische Go., Ltd., Manchester. Now Chemist to Messrs. Horrockses, Crewdson & Co.Ltd. (Preston). Reginald B. Brown. Stanley J. Peachey. Jul. Hubner. Edmund Knecht. F. S. Sinnatt. E. L. Rhead. Galstaun,Shanazar Galstaun, Abbotsholme, Derbyshire. Schoolmaster (Natural Science) (Chemislry principally). Honours B. A., Natural Sciences, Cambridge, 1913. W. J. S. Naunton. S. Ruhemann. H. J. H. Fenton. C. T.Heycock. IV. G. Gledhill. Gittins, James Mylam, South Lynn, Limes Road, Folkestone. Schoolmaster. B.Sc, Hons. Chem., 1906 ;M.Sc. (on Chemical Research), 1909 ;1906 to 1908 Research Assist. to Dr. J. J. Sudborough (Professor Chemistry, 1J.C.W., Aberystmgth) ; Investigator and Part Author of following works on Esterificstion : T., 1908, 93,210; 1909, 95,315. J. J. Sudborough. Norman Picton.T. Campbell James. Alex. Pindlay. E. R. Thomas. C. IL). Bury. 191 Henderson, Frederick George, 44, Dene View, Wallsend-on-Tg ne. Analytical Chemist. Chief Chemist to the Walker and Wallsend Union Gas Company; Consulting Chemist to the Central Refining Works Co. ; Formerly on’the Scientific Staff of J. & H. S. Pattinson, Rexol Ltd., the Aluminium Corporation, Ltd., the Tharsis Sulphur and Copper Co. J. T. Dunn. Ernest F. Hooper. N. H. Martin. F. N. Binks. F. W. Pittuck. F. C. Garrett. P.Phillips Bedson. Henri, Victor, Paris, 8 rue du Puits de 1’Ermite. Assistant, Director of the Physiological Laboratory at the Sorbonne Paris. William Ramsay. Henry E. Armstrong. George Senter. T. Martin Lowry. F. G. Dohnan. George Barger.Hinkel, Leonard Eric, ‘‘Bucklands,” Old Oak Road, Acton. Lecturer in Chemistry at Uuiversit-y of London, King’s College ; B.Sc. (1st Class HODS.),London; Fellow of the Institute of Chemistry John M. Thomson. Patrick H. Kirkaldy. Herbert Jackson. P. A. Ellis Richards. W. D. Halliburton. Arthur W. Crossley. Holt; Alfred, 32, Britain St., Bury, Lancs. Paper Mill Chemist. London University Matriculation Certificate ; Board of Education Certificate in Inorganic Chemistry, Stage Ill. (Theor. and Pract.) ;Organic Chemistry, Stage 11.(Theor. and Pract.) ; 1st Class Honours, Cotton Bleaching ; 2nd Class Honours, Cotton Dyeing; 1st Class Honours, Paper Manufacture (City and Guilds of London Institute) ;Silver Medallist, 1910. Geo.M. Normsn. Jul. Hubner. Harry Ingham. Edmund Knecht. William Bixon. Jennings, John Cyril, ‘‘Rosindell,” Firlop Road, Leytonstone, N.E. Analytical Chemist. Educated at East London College ; Studied Chemistry for Eight Years ;Student at Battersea Polytechnic ;Articled 192 to Leo Taylor, F.I.C., Public Analyst, for two years; Two and a-half years with large Firm of Oil Refiners and Distillers. At present holding position as Chief Assistant to Messrs. W. B. Dick & Co., London, Refiners and Distillers of Oils, Greases, and Turpentines. C. Smith. S. E. Davenport. R. P. Hodges. J. L. White. J. Wilson. Leighton, John Orron, 30, Albany Street, Hull. Analyst, Bankside Oil Mills, Seed-Crusbiag Mill. Pupil and Assistant with Harry Thompson, F.C.S.; in charge of the Laboratory, Bankside Oil Mills ; Specialising in Seed-Crushing, Oil and Agri-cultural work, and Investigating Manufacturing Processes in connec- tion with the Oil Industry. Harry Thompson. R. J. Yorter. Arnold R. Tankard. C. B. Newton. Thornas Luxbon. Machin, Robert Ernest, 5, Redcliffe Road, South Kensington. School Teacher. Graduate of London University ; now engaged upon a Post-Graduate Courre at Birkbeck College. George Senter. Fred Barrow. Geoffrey Xartin. G. W. Clough. Horace G. Stone. Pollock, Ernest Fergusm, Kirkland, Bonhil), Dumbartonshire Assistant in the Organic Chemistry Department of the University of Glasgow. Fellow of the Institute of Chemistry; Ph.l). (Jena); Associate of the Koyal Technical College, Glasgow. Papers published : “Contributions to the Chemistry of the Terpenes.Part VHI. Dihydrocamphene and Dihydrobornylene ” (with G. G. Henderson), T., 1910, 97, 1620; “ Ueber Methylcyclohexenone ” (with P. Rabe), Ber., 1912, 45, 2924. T. S. Patterson. Isidor M. Heilbron. Cecil H. Desch. G. G. Henderson. Forsyth J. Wilson. Jas. A. Russell Henderson. Rai, Hashmat, Chemical Buildings, Government Coltcge, Lahore (India). B.A., 1906; M.Sc., Physics, 1908; M.Sc., Chemistry, 1910, all of the 193 Punjab University. Assistant Professor of Chemistry, Govt. College, 1,ahore. F. G. Donnan. R. E. Slade. W. B. Tuck. J.N. Collie. Twine Masson. Roberts, Charles Edward, St, John’s Coll., Cambridge.Student, engaged in Chemical research. 1st Class Nat. Sci. Trip. Part I, ; 2nd Class Nat. Sci. Trip., Part 11. (Chemistry); 2nd Class Honours, London, B.Sc. (Chemistry). W. J. Pope. H. J. H. Fenton. W. H. Mills. Charles T. Heycock. F. E. E. Lamplougb. Robinson, Frederic, The Hollies, Mile End, Stockport, Cheshire. Chemist to MessrF. The Exors. of F. Robinson, Unicorn Brewery, Stockport. M.Sc. Tech, ; A.I.C. Research Student, Manchester University. Desirous of joining to keep in touch with chemical research Jas. Grant. H F. Coward. Edmund Knecht. Stanley .J. Peachey. F. S. Sinnatt. E. L. Rhead. Rowbottam, Walter Edward, 23, Darville Road, Stoke Newington, London. Analytical Chemigt. I studied Chemistry for 2 years at Hackney Technical Institute and pissed the Board of Education Examination on the Subject.For the past 3 pears I have bean articled pupil and assistant to Leo Taylor, Esq., F.I.C., C.C. Public Analyst for Hackney, Southend-on-Sea, etc. I rtm desirous of obtaining the Journal of the Society and availing myself of the privileges of Membership. 8. E. Ddvenport, V. Lefebure. Chas. A. Stamp. J. J. Fox. R. P. Hodges. Charles ,4. Keane. Thompson, Thomas William, Queen Elizabeth’s Grammar School, Gainsborough. Schoolmaster. Late Scholar of Jesus College, Cambridge. 2nd Class Natural Science Tripos, Pt. I., 1909. Science Master, Queen Elizabeth’s Grammar School, Faversham, 1909-19 12. Science Master, 194 Queen Elizabeth’s Grammar School, Gainsborough, since 1912.(B.A. 1909 ;M.A. 1913.) H. J. H. Fenton. F. E. E. Lamplough. S. Ruhemann. R. A. Scott Mach F. W. Dootson. w.H. Mills. White, Alfred John, ‘‘Hawes Down,” West W ickham, Kent. Schoolteacher. B.8c. (Lond.), and Student in Chemistry for 3 years at Birkbeck College. Am desirous of keeping abreast with recent work in Chemistry. George Senter. Geoffrey Martin. Fred Barrow. G. W. Clough. G. H. I1Iartin. The following Certificate bas been authorised by the Council for presentation to bdlot under Bye-Law I (3) : Chattopadhyay, Probodha Chundra, 90, Maniktala Main Road, Harrison Road P.O., Calcutta. Chemist, Bengal Chemical and Pharmaceutical Works, Limited, Calcutta. Worked as a Post-graduate strident in the Presidency College under Dr. P.C. RPy after taking tbe M.A. degree in Chemistry. Formerly in charge of the Pharmaceutical and Sulphuric Acid Manu- facture Departments of the Bengal Chemical and Pharmaceutical Works, Ltd., and at present in charge of the Research Laboratory and Perfumery Depts. of the said firm. Have designed some scientific apparatue, and have contributed original papers in the Journal of Society of Chemical Industry. P. C. R8y. J. B. Bhaduri. Jatindranath Sen. R. CLAY ASD SONS, LTD., BRUNSWICK ST., STAMFORD ST., S.E., AND BCXOAY, SCIFOLK.
ISSN:0369-8718
DOI:10.1039/PL9143000165
出版商:RSC
年代:1914
数据来源: RSC
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