703 
AN ACCOUNT OF THE PROGRESS 
IN 
CHEMISTRY 
j/00******* ' ' IN 
THE YEAR 1886. 
BY ” / 
i 
H. CARRINGTON BOLTON. 
FROM THE SMITHSONIAN REPORT FOR 1886-’87. 
WASHINGTON: 
SMITHSONIAN INSTITUTION. 
1889. CHEMISTRY IN 1886. 
By H. Carrington Bolton, Ph. D., 
Professor of Chemistry in Trinity College, Hartford. 
GENERAL AND PHYSICAL. 
Nature and Origin of the Elements.—Mr. William Crookes, F. K. S., 
president of the chemical section of the British Association for the Ad- 
vancement of Science, gave an address at the Birmingham meeting in 
September, in which he undertook with great skill and learning to adapt 
the doctrine of evolution to the chemical elements. After glancing at 
the difficulty of defining an element he noticed the revolt of many phys- 
icists and chemists against the ordinary acceptation of the term. He 
next considered the improbability of their eternal self-existence or their 
origination by chance. He suggested as a remaining alternative their 
origin by a process of evolution, like that of the heavenly bodies accord- 
ing to Laplace. In this connection he remarks: “ This building up or 
evolution is above all things not fortuitous; the variation and devel- 
opment which we recognize in the universe run along certain fixed lines, 
which have beeu preconceived and foreordained. To the careless and 
hasty eye design and evolution seem antagonistic; the more careful in- 
quirer sees that evolution, steadily proceeding along an ascending scale 
of excellence, is the strongest argument in favor of a preconceived 
plan.” Mr. Crookes then shows that in the general array of the ele- 
ments, as known, a striking approximation is seen to that of the organic 
world, though he admits this apparent analogy must not be strained. 
He then reviews indirect evidences of the decomposition of the so- 
called elements, taking into consideration the light thrown upon this 
subject by Prout’s law and by the researches of Mr. Lockyer in solar 
spectroscopy. He also reviews the evidence drawn from the distribu- 
tion and collocation of the elements in the crust of our earth. He gives 
due consideration to Dr. Caruelly’s weighty argument in favor of the 
compound nature of the so-called elements from their analogy to the 
compound radicals.* 
* See Smithsonian Report for 1885, Chemistry. 388 
RECORD OF SCIENCE FOR 1880. 
A study of a special method of illustrating the periodic law, proposed 
by Prof. Emerson Reynolds, leads Mr. Crookes to a theory of the genesis 
of the elements. 
lie supposes in the very beginnings of time, before geological ages, 
the existence of a primordial matter, which he names protyle (it po and 6bj). 
He imagines a “ primal stage, before even the sun himself had consol- 
idated from the original protyle, when all was in an ultra-gaseous state, 
at a temperature inconceivably hotter than anything now existing in 
the visible universe; so high, indeed, that the chemical atoms could not 
have been formed, being still far above their dissociation points. In the 
course of time some process akin to cooling, probably internal, reduces 
the temperature of the cosmic protyle to a point at which the first step 
in granulation takes place—matter, as we know it, comes into existence, 
and atoms are formed. As soon as an atom is formed out of protyle It 
is a store of energy potential and kinetic. To obtain this energy the 
neighboring protyle must be refrigerated by it, and thereby the subse- 
quent formation of other atoms will be accelerated. But with atomic 
matter the various forms of energy which require matter £o render them 
evident begin to act; and amongst others that form of energy which 
has for one of its factors what we now call atomic weight. The easiest 
formed element, the one most nearly allied to the protyle in simplicity, 
is first born. Hydrogen (or perhaps helium), of all the known elements 
the one of simplest structure and lowest atomic weight, is the first to- 
come into being. For some time hydrogen would be the only form of 
matter (as we now know it) in existence, and between hydrogen and the 
next formed element there would be a considerable gap in time, during 
the latter part of which the element next in order of simplicity would 
be slowly approaching its birth point. Pending this period we may sup- 
pose that the evolutionary process, which soon was to determine the 
birth of a new element, would also determine its atomic weight, its af- 
finities, and its chemical position.” 
Space at our command forbids our following the author further in his 
sketch of the genesis of the elements. The application of radiant-mat- 
ter spectra to the theory is a weighty contribution to the ingenious 
argument so interestingly portrayed, and one which the author alone is 
qualified to advance. (Nature, xxxiv, 42.1.) 
Valency and the Electrical Charge on the Atom, by A. I\ Laurie.—The 
author points out the bearing of the facts of electrolysis on the true 
nature of valency. Helmholtz has shown that it follows from Faraday’s 
experiments on electrolysis, that while a monovalent atom carries to the 
electrode one charge of electricity, a divalent atom carries two charges 
of electricity; in other words, electrolysis proves that differences of 
valency mean differences in the electrical charge on the atom. The au- 
thor remarks that many elements vary in valency; copper, for instance, 
forms two very unlike series of compounds, one in which it is monova- CHEMISTRY. 
389 
lent, and one in which it is divalent; since, however, we may pass from 
cuprous to cupric compounds we are able to alter the electrical charge 
on the atom, increasing it by some simple multiple. He remarks fur- 
ther that in the case of the two copper chlorides their heat of forma- 
tion per chlorine atom is not very different. It is well known that the 
heat of formation of a salt approximates to the heat of formation as 
calculated from the electro-motive force developed when that salt is 
formed in a voltaic cell; hence from the heat of formation of the cuprous 
or cupric chloride, an approximate calculation can be made of the 
difference of electric potential between the copper atom and the chlo- 
rine atom in the two salts. But since the heat of formation per chlo- 
rine atom is nearly the same, the difference of potential is nearly the 
same in both salts; whence it follows that in doubling the electric 
charge on the copper atom the potential is not also doubled. This sig- 
nifies, then, that the capacity of the atom for electricity is increased at 
the same time. Laurie then suggests that the idea of atomic weight 
may perhaps be replaced by the idea of charges of electricity; that the 
atoms of the elements are of the same weight and probably of the same 
“stuff,” and that only two things condition the properties of the atom, 
namely, its electrical charge and its electrical potential. If this be ac- 
cepted MendelejefPs table becomes a statement of the periodic relation- 
ship between these. (Nature, xxxv, 131.) 
Water of Crystallization, by W. W. J. Nicol.—When a hydrated salt 
is dissolved does it retain its water of crystallization or does this latter 
cease to be distinguishable from the solvent water? Both views have 
been held by chemists, but the author shows that the science of thermo- 
chemistry clearly demonstrates that water of crystallization can not be 
attached to the salt in solution. The argument will be found in the 
original note. (Chem. News, liv, 53.) 
A Law of Solubility, by William Ackroyd.—The author announces as 
a new law of solubility the following: “A body will dissolve in a sol- 
vent to which it is allied more readily than in one to which it is highly 
dissimilar.” Thus organic bodies, generally speaking, require organic 
solvents, inorganic bodies inorganic solvents. Exceptions to the law 
are admitted by the author. (Chem. News, liv, 58.) 
Chemical Affinity and Solution.—In a paper before the Royal Society 
of Edinburgh, presented in 1878, W. Durham stated his opinion, based 
on the results of many experiments, that chemical combination, solu- 
tion, and suspension of solids, such as clay, in water, differ in degree 
ouly, and are manifestations of the same force; that there seems to be 
a regular gradation of chemical attraction from that exhibited in the 
suspension of clay in water up to that exhibited in the attraction of 
sulphuric acid for water, which we call chemical affinity. 
More recently Mr. E. Durham endeavored to show that the theory of RECORD OF SCIENCE FOR 1886. 
valeucy as usually held is incorrect in assuming chemical affinity to act 
in units or bonds, and insufficient to account for the various phenomena 
of varying atomicity, or valency, molecular compounds, crystallization, 
solution, alloys, etc., and that all these varied phenomena are simply 
due to the chemical affinity of the elementary atoms; the difficulties 
disappear if the idea of indivisible units of chemical affinity is aban- 
doned. This view is illustrated by reference to the compounds 11 Cl, 
NII3, and NH4CI. In MCI we have two monovalent elements combined 
and their chemical affinities completely neutralized or satisfied. In 
NII-, we have N considered as a trivalent element satisfied with three 
monovalent elements. Now these two completed or satisfied compounds 
combine with one another to form the third compound NH4C1. This is 
usually explained by regarding the N as acting with peutavalent force, 
and the compound is represented thus: 
Durham thinks this explanation most unreasonable and incredible, 
because it supposes that N, which has usually such a weak affinity for 
Cl, can nevertheless decompose the IIC1 into its constituent atoms, and 
fix the atom of Cl to itself. While on the other hand the Cl leaves the 
II, for which usually its affinity is so great, and unites itself to the N, 
for which usually its affinity is so small. Durham explains this action 
simply thus: The affinity of the Cl acts on all the four atoms of II, and 
the affinity of the N does the same; and thus the whole molecule is 
held together, and may be represented thus: 
Mr. Durham finds that chemists are apparently coming more and more 
to agree with his views, and quotes Pattison Muir’s “Principles of Chem- 
istry” to substantiate this. By reference to Thomsen’s researches in 
thermo chemistry, he obtains data which he regards as demonstrating 
the truth of his views on the subject of solution. lie regards solution 
as due to the affinities of the constituent elements of the body dissolved 
for the constituent elements of the solvent; thusNaCl dissolves in water 
on account of the affinity of the Na for the O and of the Cl for the II. 
These affinities are not strong enough to cause double decomposition, 391 
CHEMISTRY. 
and therefore an indefinite compound is formed, which we call a solu- 
tion. On examining the heat of formation of chlorides and of oxides 
(as obtained by Thomsen) he finds that that oxide (or chloride) which 
has the greatest heat of formation is the least soluble. Thus the heat 
of formation of the chlorides of Mg, Ca, Sr, Ba increases in the order 
of the metals as given; and the solubility of the chlorides of these 
metals decreases in the order given; again the heat of formation of the 
oxides increases in the order Ba, Sr, Ca, Mg, whereas the solubility of 
these oxides decreases in the same order. 
Mr. Durham contends that if his views be admitted, crystallization 
can be satisfactorily explained, and regular structure follows : 
In such a compound as BaCl2.6H20, the atoms of the molecule must 
be arranged somewhat in this way : 
His theory affords also a simple explanation of the freezing of water: 
In water attraction exists between the H2 of one molecule and the O of 
another, and vice versa; now, if the heat of the liquid be diminished suf- 
ficiently, that attraction will cause cohesion of the molecules, and will 
produce solid water or ice, the regular structure of which is caused by 
the symmetrical arrangement of the atoms. Hence the various condi- 
tions of matter, solid, liquid, and gaseous, may be due to the chemical 
affinity of the constituent atoms, modified in various ways by the kinetic 
energy of the system. 
These views are opposed to that which depicts chemical affinity as a 
sort of arbitrary force acting in units or bonds; on the contrary, affinity 
acts between all atoms of matter, whether of the same or different kinds, 
in varying degrees of intensity and quantity, producing combinations 
of more or less stability, graduating from the so-called mechanical mixt- 
ure of clay and water up to the irresolvable molecules of the perma- 
nent gas, condensing by its action the gas into the liquid, and the liquid 
into the solid. In short, there are no hard and fast lines in nature, but 
every phenomenon graduates by almost imperceptible degrees into an- 
other. (Nature, xxxm, 615.) 
A General Method for the Determination of Molecular Weights, by F. 
M. Raoult.—The author has previously shown that the molecular 
weights of organic bodies soluble iu water can be determined by the 
amount of reduction iu the temperature of its freezing point. Further 
investigations now enable him to generalize this method and to rnain- 392 
RECORD OF SCIENCE FOR 188G. 
tain that the molecular weights of all bodies, inorganic or organic, can 
be determined in like manner, provided the bodies are soluble in some 
liquid capable of assuming a solid state at a temperature ascertainable 
with accuracy. The menstruums employed are acetic acid, benzene, 
and water. The methods of procedure and of calculation will be found 
in the original paper. (Ann. Chim. Phys. [GJ, vm, 317.) 
On the Constitution of Acids, by W. A. Dixon.—The author proposes a 
theory explaining the fact that some acids form with the alkali metals 
alkaline hydrogen salts, whilst the similar salts of other acids are acid. 
He suggests that, as is the case with organic compounds, the hydrogen 
in inorganic acids exists in combination in two states, first, with oxygen 
as hydroxyl, and, second, with two oxygen atoms as oxyhydroxyl. He 
thinks that where both these exist in one acid the hydrogen of the oxy- 
hydroxyl is invariably replaced first, and therefore the principal acid 
function is in connection with oxyhydroxyl. Examples are taken from 
the acids of phosphorus; orthophosphoric acid is probably 
because the acid itself has strong acid properties; but these are imme- 
diately neutralized by the replacement of the hydrogen of the oxyhy- 
droxyl group by sodium, while the replacement of the hydrogen of one 
hydroxyl group gives a salt having an alkaline reaction. In like man- 
ner phosphorous acid may have the composition 1 
, and is dibasic; 
hypophosphorous acid is 
; and pyrophosphoric acid, 
Sulphuric acid may be 
and sulphurous 
forming acid and the second alkaline hydrogen salts with the alka- 
line metals. Uyposulphurous acid may be 
and is mono- 
basic. Nitric acid may be 
; metaphosphoric, 
, and 
chloric, 
(Phil. Mag. [3], xxi, 127.) 
The Re action* beticeen Metal* and Acid*, by Ilenry E. Armstrong.— 
In tbe course of a paper before the Chemical Hociety of London on the 
“ action of metals on acids,” in which experiments were described at- CHEMISTRY. 
393 
tempting to obtain evidence of definite compounds of metals in alloys 
by dissolving the alloys in a liquid capable of acting on both metals and 
determining the electromotive force between the alloy and a less pos- 
itive metal, the author made the following remarks: “ With reference to 
the action of metals on acids generally it is probably impossible for the 
chemist to pronounce definitely in favor either of the modern view that 
the metal directly displaces the hydrogen of the acid, or of the older 
view that the metal displaces the hydrogen from wafer, the resulting 
oxide and the acid then interacting to form a salt; the decision of this 
question must apparently depend upon the determination of the nature 
of the phenomena during electrolysis of an acid solution. If the acid 
alone be the electrolyte, then doubtless the modern view is the correct 
one; but if both water and acid are electrolyzed, and in proportions 
which vary according to the conditions, then both the old and new views 
of the nature of the action between a metal and the solution of an acid 
are correct, and the two kinds of change may go on side by side.” 
(Chem. News, liii, 212.) 
Chemical Behavior of Iron in the Magnetic Field, by Edward L Nich- 
ols.—When finely-divided iron is placed in a magnetic field of consid- 
erable intensity and exposed to the action of an acid, the chemical 
reaction differs in several respects from that which occurs under ordi 
nary circumstances. The cause of one such difference may be found in 
the fact that the solution of iron in the magnetic field is in a sense 
equivalent to its withdrawal by mechanical means to an infinite distance. 
Mechanical removal requires the expenditure of work, and the same 
thing is doubtless true of what might be called its chemical removal. 
In other words the number of units of heat produced by the chemical 
reaction should differ, within and without the field, by an amount equiv- 
alent to the work necessary to withdraw the iron to a position of zero 
potential. 
Experiments with aqua-regia and iron show that the speed of reaction 
is greater in the maguetic field than without and that the heat of chem- 
ical union is much greater. Under the influence of the magnet, aqua- 
regia and iron produce nitrous fumes, whereas when the influence of 
the magnet is removed only hydrogen is generated. 
When experimenting with iron and nitric acid, interesting effects of 
magnetism on the passivity of the iron were observed; five grams of 
powdered iron lay in%a beaker close above the poles of the electro-mag- 
net which was in circuit. Some cold nitric acid was poured upon tl»e 
iron, but the latter remained passive. Wishing to note the character of 
the reaction the author warmed the beaker slightly, then placed it upon 
the poles of the magnet and put a thermometer into the solution to get 
its temperature. The bulb of the thermometer touched the iron in 
stirring the acid, when the hitherto passive mixture burst almost ex- 
plosively into effervescence, and red nitrous fumes were liberated. 
Removal of the solution from the field of the magnet restored the pas- 394 
RECORD OF SCIENCE FOR 1#86. 
sivity of the iron, and the action iu a fewr seconds ceased entirely. 
When the beaker was brought back into the neighborhood of the mag- 
net a touch of a glass rod excited again the violent chemical action. 
Further reseafches are in progress. (Am. .1. Sci. xxxi, 272.) 
Density of Liquid Oxygen and of Liquid Nitrogen, by S. Wroblewski.— 
The author finds that liquid oxygen has a density of 0.6 at — 118°C. 
and of 1.24 at under a pressure of 0.02"*. The following table 
gives the constants for liquid nitrogen: 
Temperature. 
Pressure iu 
atmospheres. 
Density re- 
ferred to water 
at 4° C. 
Coefficient of 
dilatation. 
—146. 6 
38.45 • 
0. 4552 
—153. 7 
30. 65 
0. 5842 
0. 0311 
— 193.0 
1.00 
0.83 
0.007536 
—202.0 
0. 105 
0.866 
0.004619 
Hence the atomic volume of oxygen is less than 14, and that of nitro- 
gen is near 15.5. 
The density of liquid air at —146.6° 0. and 45 atmospheres is equal 
to 0.6. (Comptes Rendus, cu, 1010.) 
INORGANIC. 
Itedeterminations of atomic weights. 
Element. 
Atomic 
weight. 
Authority. 
Reference. 
Uranium 
239. 02 
Liebig's Annalen, CCXXXII.299. 
Liebig’s Aunalen, ccxxxn,324. 
Do. 
Cobalt 
58.74 
Nickel 
58.56 
Platinum 
194. 57 
Z. anal. G'h., xxv (II). 
Comptes Rendus, cii, 1291. 
Ann. Chem., ccxxxiii. 
Germanium 
72. 32 
Lecoq de Boisbaudran. 
Antimony 
120. 69 
Tungsten (0 = 15.96). 
184.04 
Wwidell 
Am. Chem. j., VIII, 280. 
Austriutn, a new Element.—Dr. E. Linnemaun, professor of chemistry 
at Prague, died in April, 1886. Among his papers was found a letter 
addressed to the Vienna Academy of Sciences, announcing the discov- 
ery of a new element, which he called austrium, Aus. Dr. Linnemaun 
obtained the new metal from orthite of Arendal; its spectrum shows 
two violet lines; the wave lengths were found to be, for Aus. a, A = 416.5, 
and for Aus. /?, A=403.0. Prof. F. Lippich, of Prague, who presented 
Dr. Linnemann’s paper to the Vienna Academy, called attention to 
the fact that three not yet identified lines (A=415.56, A=416.08, and 
A=416.47) are shown in Angstrom’s atlas of the normal spectrum of 
the sun iu the neighborhood of the Aus. a line; the last of them might CHEMISTRY. 
395 
be supposed to be coincident with the Aus. a line (A=416.5). (Nature, 
XXXIV, 59, 1886.) 
Germanium, a new Element, by Clemens Winkler.—In the summer of 
1885 a rieli silver ore of uncommon appearance was found in the Him- 
melfuerst mine near Freiberg. It was recognized as a new mineral 
species by Prof. A. Weisbacb, and named by him “ argyrodite.” Th. 
Richter subjected the mineral to a preliminary examination with the 
blow pipe, and found it to consist essentially of silver and sulphur. In 
addition to these, he also detected the presence of a small quantity of 
mercury, which is remarkable and interesting from the fact that this 
metal had never before been found in the Freiberg ores. 
In the analyses made, Winkler found that the mercury did not amount 
to more than 0.21 per cent. According to the purity of the material the 
silver varied from 73 to 75 per cent., and the sulphur from 17 to 18 per 
cent. Small quantities of iron and traces of arsenic were also found. 
Though the analysis was often and carefully repeated there was always 
a loss of 6 to 7 per cent, without it beiug possible by the ordinary 
methods of qualitative analysis to discover the missing body. 
After several weeks of tedious search Winkler found that argyrodite 
contains a new element, very similar to antimony, but still very distinct 
from the same, which he named Germanium. The detection of this ele- 
ment was very difficult, because the argyrodite was accompanied by 
minerals containing arsenic and antimony, which, on account of their 
similar behavior, and a total lack of a sharp method for separation, 
caused much difficulty. 
Argyrodite, when heated with exclusion of air, preferably in a current 
of hydrogen, gives a black, crystalline, quite volatile, readily fusible 
sublimate, which melts to reddish-brown drops. In addition to mercury 
sulphite it consists essentially of germanium sulphide. Germautum sul- 
phide is a sulpho-acid; it is readily soluble in ammonium sulphide, and 
when reprecipitated by hydrochloric acid, in a perfectly pure plate, it 
forms a snow-white precipitate, which is instantly soluble in ammonium 
hydrate. In the presence of antimony or arsenic the precipitate is 
always tinged more or less yellow. 
On heating in a current of air or in nitric acid, germanium sulphide 
is converted into a white oxide, which Is not volatile at a red heat. It 
is soluble in potassium hydrate, and the alkaline solution, when acidified 
with sulphuretted hydrogen, gives the characteristic white precipitate. 
Too great dilution prevents or retards the precipitation. 
The oxide, like the sulphide, is reduced by hydrogen, the latter with 
greater difficulty on account of its volatility. The element has a gray 
color, and perfect metallic luster. It melts at a point somewhat below 
silver, say about 900°, and crystallizes in octahedra, which are very 
brittle. Its specific gravity is 5,469 at 20°.4. It is insoluble in hydro- 
chloric acid, readily dissolved by aqua-regia, is converted into a white 396 
RECORD OF SCIENCE FOR 1886. 
oxide by nitric acid and into a soluble sulphate by concentrated sul- 
phuric acid. Its atomic weight is 72.32, and it proves to be Mendele- 
jefFs ekasilicium. It forms two oxides, GeO and Ge02, two correspond- 
ing sulphides, and two chlorides, both of which are thin colorless fuming 
liquids. (J. Prakt. Chem., 1880, passim.) 
Atomic Weight of Antimony.—>-Alfred Popper, of the University of 
Graz, has made very careful determinations of the atomic weight of 
antimony, and obtains a mean of 120.69, which is an entire unit more 
than J. 1*. Cooke’s result, 119.60. He can find no source of error either 
in Cooke’s determinations or in his own, and suggests that the possible 
presence of germanium may solve the question. (Ann. Chem.,ccxxxiii.) 
On some Probable New Elements, by Alexander Pringle.—The author 
states that he obtained the material on which he worked from his own 
lauded property, situated upon the river Tweed, county of Selkirk, 
Scotland. He examined some gravel and other material forming the 
debris of an ancient glacier, which he “imagines” to be the ancient 
soil of the very ancient mountains in that geologic formation. He de- 
scribes more or less fully no less than six probable new elements; 
polymnestum is a metal of rather dark color, with an equivalent of 
about 74, and forming four oxides of various colors; erebodium is as 
black as charcoal and has an equivalent of 95.4; gadenium has an equiv- 
alent of 43.0 and forms two oxides ; Itesperisium is a non-metallic ele- 
ment having an equivalent of 45.2, and a red color and a metallic luster 
like a sunset sky. Two other nameless elements are briefly claimed by 
he author. (Chein. News, liv, j67.) 
Dysprosium, a new Element, by Lecoq de Boisbaudran.—In October, 
1878, announced a new earth, which he called philippium, 
but early in 1880 he recognized that it was identical with holmium, 
previously studied by Soret and by Cleve. Later in the same year, 
however, Delafontaine abandoned this view, because he determined that 
philippium had no absorption spectra. Lecoq de Boisbaudran has suc- 
ceeded by several hundred fractional treatments in separating holmium 
into two bodies, for the first of which he proposes to preserve the name 
holmium, and the second he names dysprosium (SuaitpoatroS = hard to 
get at). The new holmium has for characteristic absorption bands 040.4 
and 530.3, and .the bands of dysprosium are 753 ami 451.5. The author 
has encountered extraordinary difficulties in the separation of holmium, 
erbium, terbium, and dysprosium, and the scarcity of material greatly 
retards the laborious investigation. (Comptes Iiendus, cn, 1003 and 
1005.) 
New Elements in Oadolinite and Samar skite detected Spectroscopically, 
by William Crookes.—Finding that Lecoq de Boisbaudran is pursuing 
the spectroscopic study of the rare earths in the same track as himself, CHEMISTRY. 
397 
and publishing notes of phenomena already known to Mr. Crookes, the 
latter gives in this paper a preliminary notice and summary of his 
studies, although in an unfinished state. Mr. Crookes holds with other 
chemists the opinion that didymium is not a simple body, but has been 
unable to split it up into the green praseodymium and rose-red neo- 
dymium announced in 1S85 by Dr. Auer von Welsbach. Mr. Crookes 
thinks didymium will prove to be more complex than this indicates. 
The author, referring to his note-book under date March 3,1880, finds 
the statement that the “ big blue line (A 451.5) is still unclaimed,” and 
this blue line proves to be characteristic of dysprosium discovered by 
Lecoq de Boisbaudran. 
As a result of the spectroscopic examination of the fractionated 
earths fromsamarskite and from gadoliuite the author concludes that the 
earth hitherto called yttria is a highly complex body, capable of being 
dissociated into several simpler substances, each of which gives a phos- 
phorescent spectrum of great simplicity, consisting, for the most part, 
of only one line. The author admits that a hitherto unrecognized band 
in the spectrum, by absorption or phosphorescence, is not of itself defi- 
nite proof of a new element, but if supported by chemical facts, such 
as he details, there is sufficient primafacie evidence that a new element 
is present. Until, however, the new earths are separated in sufficient 
purity to enable their atomic weights to be approximately determined, 
and their chemical and physical properties observed, Mr. Crookes thinks 
it prudent to regard them as elements on probation. He gives in tab- 
ular form a list of these probationary elements, designating them by 
the initial letters of the minerals (or bodies) didymium, samarskite, 
and gadolinite, from which they are respectively derived, and by the 
addition to the initials of Greek letters. The table also gives the mean 
wave lengths of absorption lines in the phosphorescent spectra, and 
other data. 
.Table of Probationary Elements. 
Position of lines in the spectrum. 
Scale of 
spectro- 
scope. 
Mean wave 
length of 
line or band. 
A* 
Provis- 
ional 
name. 
Probability. 
Absorption bands in violet and 
\ 8.270° 
443 
5096 
D<x 
New. 
blue 
Bright lines in— 
$ 8.828 
475 
4432 
S/S 
Do. 
Violet 
8. 515 
456 
4809 
Sy 
Ytterbium. 
Deep blue 
8.931 
482 
4304 
G a 
New. 
Greenish blue (mean of a 
close pair). 
9.650 
545 
3367 
0 ji 
Gadolinium. 
Green 
9.812 
564 
3144 
Gy 
Gd 
New. 
Citron 
9. 890 
574 
3035 
Do. 
Yellow 
10. 050 
597 
2806 
Ge 
Do. 
Orange 
10. 129 
609 
2693 
S8 
Do. 
Red 
10. 185 
619 
2611 
GC 
Do. 
Deep red 
10. 338 
647 
2389 
G?/ 
Do. 398 
RECORD OF SCIENCE FOR 1886. 
Concerning the “ radiant-matter test ” for these phosphorescing bodies 
Mr. Crookes says it proves itself every day more and more valuable as 
one of the most far-searching and trustworthy tools ever placed in the 
hands of the experimental chemist. It is an exquisitely delicate test, 
capable of being applied to bodies which have been approximately sep- 
arated, but not yet completely isolated, by chemical means; its delicacy 
is unsurpassed even in the region of spectrum analysis; its economy 
is great inasmuch as the test.involves no destruction of the specimen; 
its convenience is such that any giveq test is always available for 
future reference, and the quantity of material is limited solely by the 
power of the human eye to see the body under examination. Beyond 
all these in importance is its trustworthiness, and during the five years 
this test has been in daily use in his laboratory Mr. Crookes has found it 
well-nigh infallible. Anomalies and apparent contradictions have arisen, 
but a little more experiment has shown that the anomalies were but 
finger-posts pointing to fresh paths of discovery, and the contradictions 
were due to erroneous interpretation of the facts. (Chem. News, liv, 
13.) 
On the Atomic Weight of the Oxide of Gadolinium, by A. E. Norden- 
skj^ld.—The author signifies by “oxide of gadolinium” the mixture 
of oxides of yttrium, erbium, and ytterbium first discovered in the 
gadolinite of Ytterby. He shows that this mixture of three isomorphous 
oxides, even when derived from totally different minerals found in local- 
ities far apart from one another, possesses a constant atomic weight, viz, 
about 262. The atomic weights of the three constituents vary greatly— 
Oxide of yttrium 227.2 
Oxide of erbium 380. 
£>xide of ytterbinm 392. 
taking 0=16 and calculating as R»03. 
The fact here demonstrated is one altogether new in chemistry and 
confirms in a remarkable way the views announced by William Crookes 
in his address to the B. A. A. S. on the genesis of the elements. It 
would appear that the work of these savants on the rare earths, so called, 
will result in revolutionizing views of chemists concerning the elements, 
so called. (Comptes Hendus, cm, 795.) 
Isolation of Fluorine by Electrolysis of Anhydrous Hydrofluoric Acid, 
by II. Moissan.—The preparation of Huorine in its elementary state is 
a problem which has long defied the efforts of chemists; the classical 
experiments of Davy, Gore, G. J. Knox, Pfaundler, Baudrimont, and 
others did not yield results satisfactory to all, and the alleged discovery 
of Prat was soon after experimentally refuted by Cillis. At the meeting 
of the French Academy of Sciences, held June 28, Monsieur II. Moissan 
described the results obtained by electrolyzing anhydrous hydrofluoric 
acid, and cautiously stated that fluorine was in all probability isolated; 
this memoir was followed by another on July 19, and soon after by a CHEMISTRY. 
399 
third, which finally removed all doubts as to the nature of the gas 
separated in the experiments. 
Moissan prepared anhydrous hydrofluoric acid after the method of 
Fremy, taking great precautions to eliminate water. This acid was 
placed in a platinum U-tube, cooled to —50° C. and submitted to the 
action of an electric current from fifty Bunsen cells. Under these con- 
ditions hydrogen was set free.at the negative pole, and at the positive 
pole a gas was obtained in a continuous current and having the follow- 
ing properties: In the presence of mercury it is completely absorbed, 
with formation of mercury fluoride of a light yellow color; the gas 
decomposes water, liberating ozone; phosphorus is ignited by it; sul- 
phur is heated, melting rapidly; carbon seems to be without action; 
melted potassium chloride is attacked with an escape of chlorine ; crys- 
talline silicon, purified by treatment with nitric and hydrofluoric acids, 
takes fire in contact with this gas and burns brilliantly,forming silicon 
fluoride. The electrode of platiu-iridium forming the positive pole is 
strongly corroded, while that of the negative pole is untouched. 
Moissan pointed out that the simplest explanation of these reactions 
is that they are due to elementary fluorine, but he deferred decision 
until he could show that the phenomena were not due to hydrogen per- 
fluoride or to a mixture of ozone and hydrofluoric acid. 
In the second memoir Moissan details the precautions observed in pre- 
paring the anhydrous hydrofluoric acid and gives additional data con- 
cerning the behavior of the gas. The anhydrous acid is made by heating 
to redness in a platinum vessel very carefully dried double fluoride of 
potassium and hydrogen (HF KF), the liquid being condensed in a re- 
ceiver cooled with a mixture of ice and salt. The anhydrous acid boils 
at 19°.5, is very hygroscopic, and fumes abundantly in moist air. For 
electrolysis the acid was cooled with chloride of methyl to —23°, and a 
current of twenty Bunsen cells sufficed. Absolutely anhydrous hydro- 
fluoric acid will not conduct electricity, therefore a small quantity of 
fused double fluoride of potassium .and hydrogen is added. 
The gas liberated at the not only attacks silicon in the 
cold, but adamantine boron as well. 
Sulphur takes fire in the gas, as do arsenic and antimony. The 
metals are attacked with less energy ; organic bodies, however, are vio- 
lently attacked; alcohol, ether, benzene, petroleum, etc., take fire on 
contact. 
When the experiment has lasted several hours and the gases are no 
longer separated by liquid hydrofluoric acid in the bend of the tube, 
the gases II and F recombine in the cold with violent detonation. 
In the third memoir the author shows that the same gas can be ob- 
tained by the electrolysis of carefully dried and fused double fluoride 
of hydrogen and potassium. The temperature maintained is 110°. 
He .also describes experiments showing conclusively that the gas in 
question is free fluorine; under certain conditions the gas was absorbed 400 
RECORD OF SCIENCE FOR 1886. 
by a weighed amount of iron, and a weight of iron fluoride was obtained 
sensibly corresponding to the weight of the hydrogen liberated. 
The isolation of fluorine by M. Moissan was regarded by the French 
Academy of Sciences as of such prime importance that the subject was 
referred to a committee for examination. This committee reported 
through its chairman, M: Debray (on the 8th of November), that they 
found Moissan’s experiments and statements satisfactory in all respects, 
and that the isolation of the element was undoubtedly an accomplished 
fact. (Comptes Kendus, Oil, 1543, CHI, 202, 250, and 850.) 
A New Gaseous Body, Phosphorus Oxyfluoride, by H. Moissan.—The 
new compound PF3O2 lias an experimental density, which oscillates 
between 3.68 and 3.75. It is instantly absorbed by anhydrous alcohol, 
by solutions of chromic acid, or by the alkalies. The existence of this 
compound renders impossible the experiment indicated by Davy, who 
proposed to isolate fluorine by burning phosphorus lluoride in an at- 
mosphere of oxygen inclosed in a vessel of Huor spar. Fluorine has the 
curious property of tending always to form ternary or quaternary addi- 
tion products. (Comptes Rendus, cir, May 31,1886.) 
The Combustion of Carbonic Oxide and Hydrogen, by Harold B. Dixon.— 
The author in 1880 published the fact that a mixture of carefully dried 
carbonic oxide and oxygen would not explode when electric sparks were 
passed through it, but that by the addition of a minute trace of water 
or volatile body containing hydrogen the mixture became inflammable. 
To account for this fact the author has more recently put forward the 
hypothesis that the steam acts as the part of a carrier of oxygen, and 
that it undergoes reduction and successive re formation. Discussion 
has arisen* as to the mode in which steam exerts its influence, and the 
author herein gives his reasons for maintaining his hypothesis. 
Experiments were made with small quantities of various gases added 
to the non-inflammable mixture of dry carbon monoxide and oxygen, and 
the electric spark passed. In all cases where a gas containing hydrogen 
was introduced the mixture exploded; otherwise, not. Steam, therefore, 
and bodies which form steam under the conditions of the ex|>eriment, 
are alone able to determine the explosion, and it is evident that steam 
does not act as a mere third body, but in virtue of its own peculiar 
chemical properties. 
Moritz Traube rejected Mr. Dixon’s explanation of the phenomena 
under consideration, claiming that carbon monoxide does not decom- 
pose steam at high temperatures, but the author shows that it has been 
amply proved by different experiments, notably by Naumann and Pistor 
(Berichte d. chem. Ges., 1885, 2894) that the re action mentioned does 
take place. Mr. Dixon also gives exi>erimental data for refuting Traube’s 
view that hydrogen peroxide acts as the carrier of oxygen. 
* See Report ou Chemistry in Smithsonian Report for 1885, p. 651. CHEMISTRY. 
401 
In a note following Mr. Dixon’s paper, Professor Armstrong suggests 
that in a mixture of carbon monoxide and oxygen, the former is oxidized 
and the latter hydrogenized simultaneously by the steam present, a 
view which Mr. Dixon remarks is not opposed to any of the observed 
facts. The explanation offered by Professor Armstrong involves the 
simultaneous occurrence of two re-actions, which Mr. Dixon regards as 
taking place successively. (J. Chem. Soc. [London], 1886, 94.) 
On the Combustion of Cyanogen, by Harold B. Dixon.—The author has 
examined the conditions under which a mixture of cyanogen and oxygen 
gases explodes, and comes to the conclusion that the explosion depends 
solely upon the nature of the spark itself. The spark from a Holtz 
machine failed entirely to explode dry mixtures of these gases. The 
induction spark failed to explode the mixture in the eudiometer, where 
the wires were 0.25 to lmni apart; but the explosion was violent in the 
tubes when the wires were 1 to 3mm apart, and this was the case where the 
gases were moist. He then compared the explosion rate of this mixture 
with that of carbon monoxide and oxygen, using for the purpose a tube 
10 feet long and recording the time on a pendulum chronograph. The 
velocities obtained were as follows in meters per second : Cyanogen and 
oxygen, dried with phosphoric anhydride, 813; dried with KHO, 
808; saturated with moisture at 15° C., 752. Carbon monoxide and 
oxygen dried with phosphoric anhydride, 36; dried with H2SO4,110; 
saturated with moisture at 10° C., 175; at 35° C., 244; and at 60°, 317. 
It is notable that in the latter case the rate of explosion increases 
rapidly by the addition of moisture, while with the cyanogen moisture 
produces an opposite effect. When a platinum wire is heated to dull 
redness in the mixture of cyanogen and oxygen, the coil cooled without 
result when the circuit was opened; but when raised to full redness it 
glowed brightly for half a minute after the current was broken, and 
orange fumes appeared iu the tube. On opening the tube it was found 
that about three-fourths of the cyanogen had been converted into car- 
bon dioxide, and one-fourth into carbon monoxide. (J. Chem. Soc., 
xlix, 384.) 
Preparation of Hydrogen Dioxide, by James Kennedy.—Tlie author 
points out the difficulty of removing the barium chloride by means of 
silver sulphate when preparing hydrogen dioxide by Regnault’s method, 
and the uncertainties of Fownes’s method, and proposes the following, 
for which he claims simplicity and economy. 
Place any convenient quantity of tribasic phosphoric acid in a shal- 
low porcelain vessel immersed in a freezing mixture (ice and salt), and 
when the temperature has fallen to 40° F. or below, saturate with per- 
oxide of barium previously made into moderately thick paste with dis- 
tilled water; when completely saturated filter through pure filter paper. 
Certain precautions are to be observed in this process in order to in- 402 
RECORD OF SCIENCE FOR 1886. 
sure success. The use of a shallow vessel to allow a large contact surface 
with the freezing mixture; the BaOj must be added very slowly to pre- 
vent too great a rise in temperature, and stirred constantly. The Ila()2 
should be added until the mixture shows a slight alkaline reaction to 
insure the complete precipitation of BallPO*, as this compound is solu- 
ble in acids. The solution is freed from dissolved barium by addition 
of diluted sulphuric acid, and the insoluble precipitate removed by til- 
tration. 
In order to prevent the decomposition of the II202, the temperature 
should not be allowed to rise above 40° or 45° F. The reaction in this 
process is explained in the following equation: Ba024-H3P04=BaHP04 
+Bf(V 
The solution obtained is sufficiently concentrated for most purposes to 
which it is applied, and is much stronger than much of that found in 
commerce. (Pharm. News, vi, 148.) 
Hydroyen Peroxide and Us Estimation, by Maurice de Thierry.-—Since 
its discovery by Thenard in 1818, hydrogen peroxide has remained a 
mere chemical curiosity, but it has recently acquired industrial impor- 
tance. It is now used not only for restoring blackened oil paintings, but 
a large quantity is consumed in bleaching ostrich feathers, silk, and hair. 
When pure, peroxide of hydrogen has a density of 1.454, but the com- 
mercial product is much weaker; its activity being dependent on its con- 
centration the author has devised a method for determining the value 
of samples. The method is based on the decomposition by manganese 
dioxide and is conveniently carried out by means of the simple appara- 
tus figured in the original memoir. (Comptes Rendus, cn, (ill.) 
Hydrates of Sulphuric Acid.—At the January meeting of the Russian 
Chemical Society Professor Mendelejeff communicated some results of 
his investigations into the thermic effects of dilution of sulphuric acid 
with water. The maximum evolution of heat, and the maximum contrac- 
tion of 100 parts of the solution both correspond to the solution contain- 
ing from 05 to 75 per cent, of n2S04, which is very near the hydrate 
H6S06=S(0H)6. Together with some other observations this leads the 
author to the conclusion that there exist at least five more or less con- 
stant hydrates of sulphuric acid, viz, II2S04, II4S05, IIGS06, and two 
more containing a large ainonntof water, as IT2S04-f 100 IT20. (Nature, 
xxxm, 591.) 
Decomposition of Ammonia by Electrolysis, by the Rev. A. Irving.— 
The author electrolyzes a concentrated solution of sodium chloride, 
with which is mixed about one tenth its volume of the strongest solu- 
tion of ammonia. The solution is placed in an ordinary three-tubed 
voltameter of Hofmann’s form, into which carbon pencils are introduced 
(with the aid of corks), to obviate the action of nascent chlorine on plati- 
num were this metal used for the electrodes.. With four to six Buuseu CHEMISTRY. 
403 
or Grove cells a considerable volume of nitrogen and hydrogen is lib- 
erated in the separate tubes in a few minutes. The re-action may be 
thus represented: 
The HC1 is of course fixed by the free ammonia. The experiment is 
suitable for the lecture table. (Chein. News, liy, 16.) 
Electrolytic Aluminium.—L. Senet has devised a new process for ob- 
taining aluminium, as well as copper, silver, etc., by electrolysis. He 
exposes a saturated solution of sulphate of alumina, separated from a 
solution of chloride of sodium by a porous vessel, to a current of 6 or 
7 volts and 4 amperes. The double chloride of aluminium and sodium 
is decomposed, and the aluminium is deposited upon the negative elec- 
trode. (Cosmos, August 10, 1885.) 
Researches on Titanium and its Compounds, by Otto Freiherr von der 
Pfordten—First Part.—The results of this lengthy investigation are 
thus summarized by the author : 
(1) Pure sulphuretted hydrogen can be prepared by drying the gas 
over phosphorus pentoxide and passing it through chromous chloride, 
which removes the oxygen. 
(2) The hydrogen evolved in the usual way by zinc and acid contains 
no oxygen. 
(3) With titanium and some other elements having a great affinity 
for oxygen the sulphides can best be obtained by the action of sul- 
phuretted hydrogen ou the chloride. The action of sulphuretted hy- 
drogen on the oxide does not give pure products. 
(1) At a low temperature sulphuretted hydrogen reduces tetrachlo. 
ride of titanium to the dichloride, and at a higher temperature another 
compound forms, probably a sulpho-chloride. 
(5) On the other hand, at a red heat, a pure crystalline disulphide is 
obtained, derived from the product first formed. 
(6) Disulphide of titanium is oxidized by carbonic acid gas free from 
oxygen. (The only known case of a metallic sulphide decomposing 
carbon dioxide.) 
(7) Disulphide of titanium in nitrogen is changed to sesquisulphide. 
Hydrogen effects the same at a high heat in glass. 
(8) The same is reduced by hydrogen in a highly-heated platinum 
tube to mouosulphide. 404 
RECORD OF SCIENCE FOR 1886. 
(9) The properties of the three sulphides are fully described and 
compared. (Am. Chem., ccxxxiv, 257.) 
Occurrence of Titanium in Eruptive Rocks and Clays.—The work done 
in the division of chemistry and physics of the IJ. S. Geological Survey 
during the year 1884-’85 forms Bulletin No. 27 of the series issued by 
the Survey. The chemical papers include one on topaz from Stoneham, 
Maine, by F. W. Clarke, the chief chemist, a method of separating 
titanium and aluminium, by F. A. Gooch, a method of filtration, by the 
same author, and a number of miscellaneous analyses of minerals, 
rocks, soils, ores, and water. Analyses of several eruptive rooks and 
of clays show a considerable percentage of titanium : 
Rock. 
Per cent. 
TiO,. 
Hornblende-andesite, from Hague Volcano, Bogosloff Inland, Alaska 
Eruptive rock from New Mexico 
1.24 
0.92 
2. <J7 
2.7<» 
0. 79 
0. (',4 
0. 45 
Another specimen from New Mexico 
Basalt, from New Mexico 
Clay, Henry County, Illinois 
Another sample from Illinois 
Clay from Dodgeville, Wisconsin. .. 
A Xeic Oxide of Zirconium and its Utility in the Determination of this 
Element, Bailey.—By the action of hydrogen peroxide on zirconium 
sulphate the author obtained a white bulky precipitate, which proved to 
have the formula Zr2()5. This is a perfectly stable and definite body, 
less readily soluble in dilute sulphuric acid than Zr()2, and of positive 
utility in analytical determinations. Hydrogen peroxide does not pre- 
cipitate iron, aluminium, titanium, niobium, tantalum, tin, nor silicon, 
and the zirconium can be separated from all or any of these. With a 
moderately concentrated solution of hydrogen peroxide the precipita- 
tion is complete. (J. Chetn. Soc., xlix, 149.) 
Researchen on Uranium, by Clemens Zimmermann; Third Paper, pub- 
lished after the author’s death by George Alibegoff and Gerhard 
Kriiss.—A careful examination of the reactions of the oxide of uran- 
ium, U3U8, has led the author to the conclusion that the oxide U205 of 
Peligot is a mixture, and that a body having this composition does not 
exist. Peligot’s results were based on the behavior of U3Og when ig 
nited in the air. Zimmermann finds that U308 ignited in the air loses 
varying quantities of oxygen, but if ignited in an indifferent gas, like N 
or COj, the uranic oxide is gradually and completely con verted into U02. 
U308 is only absolutely stable when ignited in a current of oxygen. 
The color of the U308 varies with the method of preparation, and there- 
fore can not be used to control its purity. CHEMISTRY. 
405 
Determinations of the atomic weight of the element, conducted in 
several ways, lead to the value 239.02. (Ann. Chem., ccxxxii, 273.) 
New Compounds of Vanadium, by J. T. Brierley.—By mixing a blue 
solution of hypovanadium sulphate with a colorless one of an alkaline 
metavanadate the author has obtained the following series of new com- 
pounds: 
A soluble sodium salt, 2V204, V205, 2Na20 -f- 13H20. 
A soluble potassium salt, 2V204, V206, 2K20-f-CH20. 
An insoluble potassium salt, 2V204, 4V2Os, 5K20 + H20. 
A soluble ammonium salt, 2V204, 2V.206, (NH4)20 + 14H2 O. 
An insoluble ammonium salt, 2V204, 4V205, 3(NH4)2 0+6 H20. 
The first named crystallizes well in hexagonal plates of considerable 
size, and black color. The last named is a precipitate insoluble in hot 
water. (Ann. Chem., ccxxxii, 359.) 
j\7on-existence of Silver Subcliloride, by Spencer B. Newbury.—The 
author has obtained the product called silver subchloride (Ag2Cl?) by 
the three methods of Cavillier, Wetzlar, and Wohler, and after careful 
examination and analysis, finds that there is no evidence whatever of 
the existence of such a compound, and believes the substances supposed 
to be silver subchloride are nothing but simple mixtures of silver and 
silver chloride. He also rejects the existence of the silver subcitrate 
obtained by Wohler and von Bibra, claiming that the loss of weight on 
heating silver citrate in hydrogen, the formation of carbon dioxide, and 
residue of metallic silver indicate the decomposition of citric acid and 
separation of silver rather than the formation of silver subcitrate. 
(Am. Chem. J., viii, 196.) 
On Berthollet18 Fulminating Silver, by F. Raschig.—Although this 
substance was discovered by Berthollet nearly one hundred years ago, 
it has not been since closely studied, and its constitution has been un- 
certain. Berthollet obtained it by the action of ammonia on silver ox- 
ide. Raschig prepares it as follows: A solution of silver nitrate is pre- 
cipitated with sodium hydroxide, and the silver oxide is washed by 
decantation in the beaker and then transferred to a small flask. For 
each gram of silver nitrate used 2 c. c. of ail ammonia solution, contain- 
ing 25 per cent, of KEJ3, is added to the oxide, which dissolves easily 
with very slight residue. The solution of fulminating silver thus ob- 
tained is divided into several portions, and each dish is covered with 
a wratcli glass and allowed to stand sixteen to twenty hours. The 
ammonia evaporates, leaving the fulminating silver as a black crystal- 
line mass. After washing it was analyzed by digesting with very di- 
lute sulphuric acid, which usually leaves a residue of metallic silver. 
The dissolved silver was precipitated with hydrochloric acid, and the 
ammonia determined in the filtrate as platinic chloride. The results 406 
RECORD OF SCIENCE FOR 1886. 
of sixteen analyses gave ratios appioximating three atoms of silver to 
one of nitrogen, which gives the formula NAg;). 
The substance was also prepared by warming the ammonia solution 
of the silver oxide on a water bath, and by precipitating it with alcohol, 
and these samples gave the same results on analysis. Berthollet’s ful- 
minating silver explodes with a very slight concussion when dry, and 
even when moist must be handled with precaution. The explosive 
character of each sample analyzed was determined. It dissolves in 
potassium cyanide solution almost immediately, probably giving the re- 
action : 
NAg3 4- 3KCy + 311,0 = NH:i + 3KOO + 3AgCy 
(Liebig’s Annalen, ccxxxm, 93.) 
Compounds of the Nitrates of the Alkalies icith Nitrate of Silver, by A. 
Ditte.—The author describes the preparation and characteristics of 
the following double salts: AgN03,KN03; AgN()3, libN03; NII4N03, 
AgN03; and shows that with sodium and lithium analogous double 
salts are difficult to obtain in definite compounds. No less than twelve 
reasons are presented for dividing the alkaline group of metals into two 
sections, one embracing K, Rb, Cs, NH4; and the other, Li and Na. 
(Ann. Cliim. Phys. [6], vm, 418.) 
Decomposition of Potassium Chlorate, by Frank L. Teed.—In a previ- 
ous paper the author arrived at the conclusion that the decomposition 
of potassium chlorate by heat was represented by the equation : 
lOKClOa = GKCIO, -f 4KC1 + 30, 
but later experiments lead him to believe that the following is more 
nearly correct: 
22KClO3=14K01O4 + 8KC1 +50, 
A majority of the author’s results fall within the limits calculated 
from these two equations. When the chlorate is heated with manganese 
dioxide it decomposes apparently without formation of perchlorate. 
In the discussion which followed the reading of this paper at the 
Chemical Society of London, l)r. Percy Frankland said experiments 
made in the South Kensington laboratory had lead to the equation: 
8KC103=5KC104 + 3KC1 + 20, 
(Cliem. News, Lin, 56.) 
For a further discussion of this subject see article by E. J. Maumen£ 
in Client. News, liii, 145. 
The Solray Process of Manufacturing “ Soda”—In our reports for 1883 
and 1884 we chronicled the decline of the Leblanc process and the iise 
of the so called “ ammonia process ” of manufacturing soda; we now CHEMISTRY. 
407 
note the establishment of a manufactory of carbonate of soda by the 
latter process in the United States. 
Solvay & Co. have established extensive works for conducting the 
process with which their name is connected in Belgium, France, Ger- 
many, ltussia, and Austria; and a company of gentlemen, which has 
secured the right to work under all the Solvay patents, has erected 
works at Geddes, near Syracuse, ISTew York State. These works pro- 
duced in 1885 14,651,500 kilos, of 98 per cent, carbonate of soda, and 
the production for 1886, with increased facilities, is estimated to reach 
30,000,000 kilos. 
The purity of the product is shown by the following analysis of the 
brand known as “ Pure Soda 
Analysis of “ Pure Soda.” 
Per cent. 
Iron and aluminum oxides 
025 
Silica 
025 
Carbonate of lime 
404 
Carbonate of magnesia 
175 
Chloride of sodium 
904 
Carbonate of soda 
93.730 
100. 203 
This product, being very pure, is especially adapted for glass making, 
soap making, paper making, scouring textile fabrics, and all the innu- 
merable uses to which this adjunct of civilization is continually put. 
The product of all the works making soda under the Solvay patents 
is over 220,000 tons per annum, and new establishments are rising in 
several localities. 
Composition of a Crystalline Scale formed, in the Ammonia-Soda Process, 
by George W. Leighton.—The crystalline scale, formed on the inner 
surface of an iron tank, in which vapors consisting of ammonia, carbon 
dioxide, and small quantities of hydrogen sulphide are passed through 
brine holding in solution the chlorides of sodium, magnesium, and cal- 
cium, with a small amount of calcium sulphate, has been examined. It 
has the appearance of a boiler scale, from one to two inches thick, with 
a vitreous luster and greenish-gray color, although sometimes black on 
the surface. The scale is usually covered with crystal planes, which 
prove to be the terminations of prisms (probably monoclinic). Analysis 
gave results corresponding closely to the formula: MgC J3, Na2C03, 
NaCl; and impurities consisting chieliy of OaC03. This is not a mixt- 
ure, but an interesting triple salt analogous to some mineral species. 
(Proc. Am. Acad. Arts and Sci., xxii, 158.) 
ORGANIC CHEMISTRY. 
On the Formation of So called closed Chains, by Prof. Victor Meyer.— 
Carbon atoms possess the marked peculiarity of combining to form 
molecules iu so-called ckaius, a property giving rise to the multiplicity 408 
RECORD OF SCIENCE FOR 1886. 
of organic bodies. In stearoue no less than thirty five carbon atoms 
unite to form a chain, which may be indicated thus: 
h3 /h2\ o /ha h3 
c_l c jl6_c-VcJie-c 
A limit to the extent of open-chain structure can not be predicted, 
but the case is very different' when closed chains are considered. 
While closed chains of three, four, live, and six links or atoms are 
numerous, the problem of forming rings having a greater number of 
links has been scarcely attacked by chemists. If bodies like anthracene 
and acridine, having double rings of the benzene type, be excepted, only 
two substauces are known having seven links in the molecular ring. 
These are: 
and 
Carbazostyril. 
Suberone. 
Tlie author has begun the study of the construction of rings having 
a number of liuks greater than six, and some of the results are as fol- 
lows: 
Sodium sulphide acts on iodide of methylene in accordance with the 
equation: 
CU2I2+ Na28=2NalH-CH,S 
But A. W. Hofmann has shown that the molecular weight of CH28 is 
three times as great as thus indicated, and Meyer formulates this as 
follows: C3n6S3 or 
a study of the body formed in the re-action 
C2TT4Br2+Jira2S=2XaBr+C2n4S 
the author arrives at the couclusiou it should be formulated thus: CHEMISTRY. 
409 
which is an exampleof a closed chain of nine links. Further researches 
led the author to the discovery of a body having the following consti- 
tution: 
which is the first example of a closed chain of twelve links. These 
bodies are quite unstable, as indeed might be anticipated from their 
complex structure. (Naturwiss. Rundschau, i, 2, 1886.) 
Products of the Manufacture of Gas from Petroleum, by Henry E. Arm- 
strong and A. K. Miller.—This paper gives results of an investigation 
which the authors have conducted during several years, on the decom- 
position and genesis of hydrocarbons at high temperatures; their main 
object has been to throw light on the nature of the changes resulting 
from the decomposition of petroleum hydrocarbons at high temperatures. 
The authors have thus far recognized among the products of the manu- 
facture of oil-gas the following hydrocarbons: 
(a) Paraffines, only in traces. 
(b) Pseudolefines, or saturated hydrocarbons of the series CnH2n, such 
as occur in Russian petroleum; present in relatively small amount.. 
(c) Olefines, viz, ethylene, propylene, normal amylene, hexylene, and 
lieptylene; higher homologues being absent. 
(d) Pseudacetylenes, viz, crotonylene (dimethylenethane) and iso 
allylethylene. 
(e) Beuzenoid hydrocarbons, viz, benzene, toluene, the three isomeric 
diinethylbenzenes, the two trimethylbenzenes (pseudocumene and mesi- 
tylene), and naphthalene. (J. Chem. Soc. [London], 188G, p. 74.) 
Some Organic Substances of High Refractive Power, by H. G. Madan.— 
The author finds that naphthyl-phenyl-ketone has a refractive index of 
1.6G6, which is even higher than that of carbon disulphide (1.63). Its 
dispersive power is almost exactly that of carbon disulphide. 
Metaciunamene has a refractive index of 1.593; monobromonaplitha- 
lene has a refractive index of 1.6G2, and the author thinks it may prove 
a valuable substitute for carbon disulphide for filling prisms, as it is 
much less volatile and inflammable. Mr. Madan mentions as a great 
desideratum a substance having all the excellent qualities of Canada 
balsam—colorless, neutral, permanent in the air, becoming fluid when 
moderately heated, but hard and tough when cold, and with a refractive 
index of at least 1.G6. Such a substance would be invaluable for mount- 
ing microscopic objects. (Phil. Mag. [5], xxi, 245.) 
A Convenient Method of Preparing Organic Compounds of Fluorine, by 
O. Wallach.—The author finds that organic bodies containing fluorine 410 
RECORD OF SCIENCE FOR 1886. 
can be readily obtained by the action of aqueous hydrofluoric acid on 
diazoamido compounds. He describes fluorbenzene (C6H5F1) boiling 
at 84° to 85°, parafluortoluene boiling at 11G° to 117°, flnornitroben- 
zene, fluoranilin, and other bodies. It appears that the replacement of 
hydrogen by fluorine changes very little the boiling points of the bodies, 
but greatly increases their speciflc gravities. (Ann. Chem., ccxxx v, 255.) 
On Platoso-Oxalic Acid, by II. G. Soderbanm.—Doebereiner formerly 
obtained, by the action of oxalic acid upon the sodium salt of platinum 
dioxide, a salt of a copper-red color, which he regarded as platiuous 
oxalate. Souchay and Lenssen assign it the formula PtNa2C40()-4-411*0- 
This salt has much analogy with the platinum sulphites, since the solu- 
tion gives neither the reactions of platinum nor those of oxalic acid. 
We may therefore regard this compound as the sodium salt of platoso- 
oxalic acid, which has been isolated. 
The salts of platoso oxalic acid are very remarkable, because they 
occur in isomeric or rather polymeric forms. 
For the preparation of the sodium salt sodium chloro-platinate is 
heated with an equal weight of sodium hydrate. The residue is treated 
with water, which dissolves out sodium chloride, leaving a yellow pow- 
der, Na20, 3Pt()2,(»II20. More of it is obtained by the addition of hydro 
chloric acid to the solution of sodium chloride, avoiding excess. It is 
washed with cold water and washed with one and a half parts of crys- 
talline oxalic acid. Carbonic acid escapes, and there is obtained a solu- 
tion of an intense blue color, from which cold slender brown needles of 
a metallic luster are deposited. This salt is collected upon a filter and 
repeatedly washed with boiling water. There filters first a yellow solu- 
tion, then a greenish or blue one, and lastly a solution of a reddish- 
brown. From the last liquid the mass of the sodium salt is deposited 
on cooling, crystallized in capillary needles of a coppery luster. The 
lirst solution after some time deposits lemon-yellow prisms of an isomeric 
salt. The intermediate solutions deposit mixtures of the two salts. 
Both salts yield with silver nitrate a yellowish-white precipitate of 
microscopic crystals of the silver salt of platoso-oxalic acid. On decom- 
posing this silver salt with the calculated proportion of hydrochloric 
acid we obtain an indigo blue solution, containing platoso-oxalic acid. 
We may obtain the salts of the acid either by the double decomposition 
of the sodium salts or by neutralizing the free acid with bases or car- 
bonates. With the brown sodium salt there are obtained salts of a 
brown, greenish, or blue color; but with the yellow salt we obtain iso* 
meric yellow or orange salts. The free acid generally gives salts of the 
former class,*, e., of a dark color, but by repeated crystallizations yellow 
salts may be obtained. Several metals belonging to the zinc group form 
dark-colored salts most readily; others, for instance silver, yield yellow 
salts, and others again form with equal ease either dark or yellow salts. 
The tri- and tetra-atomic metals give both dark and yellow salts, but of CHEMISTRY. 
411 
a different composition. The dark salts are in general less soluble; 
their density is lower and they often contain a smaller number of mole- 
cules of crystalline water. The difference between the two classes of 
salts does not depend on the water of crystallization, because both dark 
and yellow anhydrous salts have been obtained, and because there exist 
both yellow and dark salts containing the same number of molecules of 
crystalline water. 
The salts of platosooxalic acid are in general sparingly soluble in cold 
dilute acids; they are insoluble in alcohol. In hot water some of them 
dissolve readily; others are sparingly soluble. Most of them contain 
crystalline water, which they lose in part or entirely at 100°. They 
bear the temperature of 110° to 115° (though the ammonium salt is 
decomposed at 100°); but a little above this temperature they begin to 
decompose. If suddenly heated they are decomposed with detonation. 
Platoso oxalic acid, PtC408H2 +2H20, the preparation of which has 
been described above, gives, when its solution has been evaporated in 
a vacuum, a red crystalline mass of a metallic luster. It dissolves 
readily in water with an indigo-blue color, but this color changes to 
yellow on heating or diluting with water. Yet the blue color returns on 
cooling or on concentration. 
There are two potassium salts, a brown one forming copper-colored 
needles of specific gravity 3.01, and a yellow one in hexagonal prisms 
of specific gravity 3.03. Both contain the same number of molecules 
of crystalline water. With the ammonium salts the case is similar. 
The dark sodium salt forms slender needles containing 4 molecules of 
crystalline water, whilst the yellow salt forms prisms with 5 molecules 
of crystalline water. There are three isomeric calcium salts: the brown 
one, with 6£H20; the ytf-yellow salt, with 4H20, losing one molecule water 
at 100°; and the ;/-yellow salt, with 8H20, losing at 100° 5H20. There 
are also three strontium salts: a, dark, contains 3£H2() and loses £H20 
at 100°; /?, also dark, contains 0£H2O, and loses 3H20 at 100°; and 
y, yellow, contains only 3 molecules of crystalline water and undergoes 
no change at 100°. 
These researches were made in the laboratory of Prof. P. T. Clbve. 
(Bull. Soc. Chim., 1880, 188.) 
Iodo aldehyde is obtained by P. Chautard by acting on an aqueous 
solution of aldehyde with a mixture of iodic acid and iodine. 
5(C2H40) + 41 + I03H = 5(C2H3IO) + 3H20 
Iodo aldehyde forms an oily, volatile, non-inflammable, colorless, 
limpid liquid, blackening rapidly on exposure to light. It decomposes 
at 80° C., but in solution may be heated to high temperatures without 
change. It acts as a strong caustic, attacking eyes and respiratory 
organs. Its density is 2.14 at 20°. It is soluble in all proportions in 
alcohol, ether, benzene, chloroform, etc. It combines readily with ani- 
line and other ammonia derivatives. (Comptes Rendus, cn, 118.) 412 
RECORD OF SCIENCE FOR 1886. 
Synthesis of Conine, by A. Ladenburg.—Conine, the volatile alkaloid 
which forms the poisonous principle of hemlock (conium maculatum), 
was discovered iu 1827 by Giesecke, but was first obtained in a pure 
state in 1831 by Geiger. It has been often studied by chemists, nota- 
bly by Ortigosa, Blyth, Wertheim, and Kekule and von Planta; the 
two latter gave it the formula C8Hi5N, but it is now known to beCnHnN’. 
It forms a colorless, oily liquid of pungent odor, specific gravity = 0.89; 
boiling point 166° to 168°. It is easily soluble in alcohol and ether, 
sparingly iu water, and forms crystalline deliquescent salts. It is an 
active poison. This natural alkaloid has been formed synthetically by 
Ladenburgin the manner to be described. Hu go Sell iff, in 1871, thought 
he had effected this synthesis by the action of alcoholic ammonia on 
normal butyric aldehyde and subjecting the product to dry distillation, 
but the base thus obtained proved to be paraconine, an isomeric form. 
Ladenburg’s researches on the pyridine bases had already yielded 
him interesting results. The synthesis of piperidine was noted in our 
report for the year 1884. On the 25th of February he read a paper be- 
fore the German Chemical Society entitled “ Experiments on the Syn- 
thesis of Conine,” in which he announced the preparation of a base 
very closely resembling this alkaloid, and in October he presented de- 
tails of this remarkably interesting synthesis, and proofs of the iden- 
tity of the artificial and natural substances. The process is as follows: 
Paraldehyde and a-picoline are heated for ten hours in closed tubes 
to a temperature of 250° to 200°. The allylpyridine thus obtained was 
separated from the unchanged picoline, purified and fractioned until it 
distilled at 187°.o to 192°.5. The exact nature of this body was care- 
fully established by many tests. The a allylpyridine was then sub- 
mitted in alcoholic solution to the reducing action of sodium, w hereby 
a-propylpiperidine was obtained. The hydrochloride of this base, 
when purified, melted at 203° to 205°, and crystallized in silky-white 
needles. 
The base separated from this salt boiled at 100° to 107° and proved 
to have the greatest resemblance to conine. After a very careful study 
of its toxic and optical properties the author satisfied himself of the 
absolute identity of this dextro—a-propylpiperidine and conine, 
C3II7. C5H10. HX. (Ber. d. chem. Ges., XIX, 439 and 2578.) 
New Synthesis of an Inactive Borneol, by J. Bouchanlat and J. La- 
font.—Berthelot accomplished the synthesis of the camphor of Borneo 
by treating camphor with potassium alcohol ate, and Baubigny by the 
direct addition of hydrogen. The authors effect the transformation of 
terebeue, or inactive cam phene, C,0Ui6, through the medium of an organic 
acid into an ether of borneol, which by saponification yields a borneol 
having no influence ou polarized light. With the exception of its in- 
active optical properties, the new body is identical with borneol. 
(Comptes liendus, oil, 171.) CHEMISTRY. 
413 
Synthesis of Ammonium Cyanide by Electricity, by A. Figuier.—By 
passing a current of silent electricity through a mixture of one volume 
ofmethaneand two volumes of nitrogen, cyauide of ammonium is formed 
and noticeable by its odor. 
CH4+ N2 = CK lNH4. 
The product was collected and its identity established. (Comptes Ren- 
dus, cn, C94.) 
Synthesis of Mellitic Acid and of other Benzo-carbonic Acids by Elec- 
trolyzing Water with Carbon Electrodes, by A. Bartoli and G. Papasogli.— 
By the electrolysis of distilled water with electrodes of pure carbon and 
a battery having an electromotive force equal to 1,200 Daniells, the 
authors obtaiued a black insoluble deposit (mellogen) and a very acid 
liquid which was found to contain mellitic, pyromellitic, hydromellitic, 
and hydropyromellitic acids. During the electrolysis carbon monoxide 
and dioxide with very little oxygen were evolved. Mellogen purified 
by precipitation from the aqueous solution by hydrochloric acid forms 
an amorphous, neutral, black, and friable body, insoluble iu alcohols 
and soluble in water, to which it imparts an intensely black color. Mel- 
logen dried at 140° has the composition CnH204, and has some aualogy 
with Brodie’s graphitic acid CnH405, but the two bodies are not iden- 
tical. Oxidizing agents convert it into benzo-carbonic acids. (Anuales 
Chirn. Phys. [6], vii, 349 and 364.) 
Products of the Electrolysis of a Solution of Ammonia with Coke Elec- 
trodes, by A. Millot.—A solution of ammonia containing 50 per cent, was 
electrolyzed with electrodes of coke purified by chloriue, and the chief 
products are an azulmic matter (which the author is still studying), urea, 
ammelide, biuret, and guanidine. The urea and guanidine probably 
arise from action of nascent carbon dioxide on ammonia with elimina- 
tion of water. Biuret is probably formed by the action of carbon diox- 
ide on guanidine, and ammelide from the action of this gas upon biuret 
with the co-operation of urea. Cyanuric acid was sought but not found. 
These results differ from those of Bartoli and Papasogli, who added salt 
to the ammouiacal solution to render it a better conductor, and the nas- 
cent chlorine resulting destroyed the above-mentioned products. 
(Comptes Rendus, cm, 153.) 
Identity of Cadaverine with Pentamethylendiamine, by A. Ladenburg.— 
Brieger in the course of his remarkable researches on ptomaines isolated 
from a cadaver a base having the formula C5n14N2, and which he named 
cadaverine. This base was also discovered in decomposing fish. 
Brieger, noting the resemblance in properties between cadaverine and 
pentamethylendiamine, sent a small specimen of the former to Laden- 
burg for investigation. The latter chemist found the reactions of the 
two bodies similar iu all respects except in their behavior with mercuriQ 414 
RECORD OF SCIENCE FOR 188<>. 
chloride; but he succeeded iu transforming cadaverine into piperidine 
by a known process and thus fully established the identity of the two 
bodies. (Ber. d. chem. Ges., xix, 2585.) 
On the Constitution of Levulose and Dextrose, by Heinrich Kiliani.— 
According to the author, levulose is a ketone alcohol, and has the con- 
stitution 
This result was arrived at by studying the behavior of levulose with 
hydrocyanic acid. 
The question whether dextrose is an aldehyde or an anhydride is not 
entirely settled, but the probable constitution is 
(Ber. d. chem. Ges., xix, 767 and 1128.) 
Chlorophyll and the Reduction of Carbonic Acid by Plants, by C. Timi- 
riazeff.—On subjecting an alcoholic solution of chlorophyll to nascent 
hydrogen (by means of zinc and acetic acid) the chlorophyll is reduced, 
and forms in dilute solutions a straw-yellow substance and in concen- 
trated solutions a substance of brown-red color. This substance has a 
well defined spectrum, in which the band in the red portion character- 
istic of chlorophyll is wanting. The most important property of this 
reduced chlorophyll is its rapid oxidation on exposure to air, with re- 
production of green chlorophyll. The author terms this new substauce 
protochlorophylliue, or, more briefly, protophylline. 
Solutions of protophylline can bo preserved only in glass tubes her- 
metically sealed. If a solution of protophylline be sealed up in a tills; 
together with carbonic acid and preserved in total darkness it retains 
indefinitely its color and characteristic spectrum, but on exposure to 
sunlight the solution turns green. The author remarks that in the 
absence of quantitative details he can not claim that this proves the 
reduction of carbonic acid by protochlorophylliue in the presence of CHEMISTRY. 
415 
sunlight, but he can not find any other explanation of the facts. He 
thinks that there is evidence of the existence of nrotophylline in living 
plants. He also finds that by pushing the reducing action of nascent 
hydrogen further another and colorless substance is obtained, which is 
now under examination. (Comptes Rendus, cn, (587.) 
Acetophenone, a new Hypnotic.—Acetophenone, also called acetylben- 
zene, C6H5. CO . CH3, has been found to possess valuable hypnotic 
properties. It is as yet only a laboratory product, but there should be 
no great difficulties in manufacturing it on a commercial scale. It is 
commonly obtained by distilling a mixture of calcium benzoate and cal- 
cium acetate, though many other methods are named in hand-books. It 
forms at ordinary temperatures a clear, colorless liquid, having a per- 
sistent characteristic odor; at a lower temperature it forms large flaky 
crystals, melting at 20°.5 C. Dr. Dujardin-Beaumetz, who has discov- 
ered its hypnotic properties, recommends it for simple insomnia, and 
says its use is not followed by disagreeable after-symptoms, such as 
nausea, headache, etc. He proposes for this substance the trade-name 
“ hypnone.” (Bull. Gen6rale de Therapeutique, 188C.) 
On Thionaphthenes, by Victor Meyer.—The author states that the first 
thiophene of the naphthalene series, which he names thionaphthene, has 
been obtained in his laboratory by A. Biedermauu. It has the consti- 
tution 
The author has obtained thionaphthene itself by the action of phos- 
phide of sulphur on cumaroue, the analogies of which are shown by 
the following schemes: 
Cumarone. 
Thionaphthene. 
(Ber. d. chem. Ges., xix, 1432 mid 1015.) 416 
RECORD OF SCIENCE FOR 1886. 
On Penthiophene and its Derivatives, by Karl Krekeler.—The existence 
of a body analogous to thiophene, but having live carbon atoms and 
oueof sulphur in a closed chain, has been foreseen by Victor Meyer and 
others. The author obtained a methyl derivative by acting on a methyl- 
glutaric acid with sulphide of phosphorus, this acid being derived from 
Imvulinic acid, a substance on which the author has lately experimented 
much. The body has the formula 
/3-methyl pen thiophene. 
This substance forms a colorless oily liquid, boiling at 134° C.; its spe- 
cific gravity = 0.9938 at 19° C. It gives the Laubenheiiuer color-test 
and other colored reactions. (Ber. d. chem. Ges., xix, 3266.) 
Thiocumarine and its Derivatives, by Fred. Tiemann.—By the action 
of phosphorus pentasulphide on cumarine the author obtained a sulpho- 
compound having the constitution 
Thiocumarine. 
This crystallizes in golden needles, easily soluble in alcohol, ether, and 
benzene, insoluble in water, and molting at 101°. By reacting on this 
body with hydroxylamine he obtained cumaroxime in loug while nee- 
dles, melting at 131°. In appropriate ways the following compounds 
were obtained: Cumaroximethyl ether, dihydrocumaroxime, and a 
plieuy 1-hydrazine derivative of cumarine. (Ber. d. chem. Ges., xix, 
1661.) 
Benzoic Sulphinide, or no-called “ Saccharine.”—I)r. Ira Bern sen, assisted 
by C. Fahlberg, in the year 1879, when engaged in researches originating 
with the former, discovered a substance which lie named benzoic sulpbi- 
uide. This body, which may also lie called anhydrosulphaminebenz tic 
acid, was obtained by the oxidation of orthotoluenesalphainide, and in 
the original paper (by R. and F.) is thus described: “Benzoic sulphi- 
nide is difficultly soluble in cold water. It is much more soluble in hot 
water, and can be obtained iu crystalliue form from its aqueous sola- CHEMISTRY. 
417 
tion. It crystallizes in short, thick prismatic forms, which are not well 
developed. Alcohol and ether dissolve it very easily. It fuses at 220° 
(uncorr.j, but undergoes at the same time partial decomposition. It 
possesses a very marked sweet taste, being much sweeter than cane sugar. 
The taste is perfectly pure. The minutest quantity of the substance, if 
placed upon the tip of the tongue, causes a sensation of pleasant sweet- 
ness throughout the entire cavity of the mouth. As stated above, the 
substance is soluble only to a slight extent in cold water, but if a few 
drops of the cold aqueous solution be placed in an ordinary goblet full 
of water, the latter then tastes like the sweetest sirup. Its presence 
can hence easily be detected in the dilutest solutions by the taste. 
Orthonitrobenzoic acid has this same property, but the sweetness is by 
no means so intense as in the case of benzoic sulphinide.” (Am. Chem. 
J., 1, 430.) 
On the 2d of February, 1886, Dr. Ivan Lewinstein read a paper before 
the Society of Chemical Industry on “ Saccharine,” in which he gives 
sole credit of the discovery of this sweet substance to Dr. Remsen’s 
assistant. The process of preparing it is the same, though he prefers 
for it the name benzoyl-sulphouie-imide, or the trade-name “saccharine.” 
The constitution of this body is thus shown: 
Dr. Lewinstein gives the following account of the properties and pros- 
pective uses of this substance: 
Saccharine presents the appearance of a white powder, and crystal- 
lizes from its aqueous solution in thick short prisms, which are with 
difficulty soluble in cold water, but more easily in warm. Alcohol, 
ether, glucose, glycerole, etc., are good solvents of saccharine. It melts 
at 200° 0., with partial decomposition; its taste in diluted solutions is 
intensely sweet, so much so that one part will give a very sweet taste 
to 10,000 parts of water. Saccharine forms salts, all of which possess 
a powerful saccharine taste; it is endowed with moderately strong an- 
tiseptic properties, and is not decomposed in the human system, but 
eliminated from the body without undergoing any change. It is about 
two hundred and thirty times sweeter than the best cane or beet root 
sugar. According to Dr. Stutzser, of Bonn, who has carefully inves- 
tigated the physiological properties of this substance, saccharine, taken 
into the stomach in the quantities in which it has to be added to food 
as a sweetening material, has no injurious effect whatever on the human 
system. Stutzser has given to dogs about 5 grams a day, without ob- 
serving any ill effects in them, and when we consider that 5 grams are 
equal in sweetening power to rather more than pounds of sugar, a 
quantity far larger than any one would like to consume in a day, his 
view seems amply corroborated by this fact alone; but, in addition to 
this, patients suffering from diabetes have now been treated for several 
months in one of the principal hospitals in Berlin, as I am informed, 
without their feeling the least inconvenience by its use. Physicians 
must be glad to find in saccharine a substance, by means of which di- 418 
RECORD OF SCIENCE FOR 188H. 
abetic persons may enjoy food which has hitherto not been admissible 
in their case. Saccharine does not belong to the class of carbohydrates, 
and does not possess nutritious properties. The use of saccharine will 
therefore, as indicated by its properties, be not merely as a probable 
substitute for sugar, but it may even be applied to medicinal purpose 
where sugar is not permissible. The inventor was fully aware that in 
order to supply a perfect substitute for cane or beet root sugar, some- 
thing else, viz, a similar substance, was needed for confectioner) and 
similar purposes, besides sweetening properties, and he has also en- 
deavored to solve this problem. Dr. Fahlberg combines glucose with 
starch sugar, a substance very similar to cane or beet root sugar, but 
inferior to these in sweetening properties, with saccharine, and thus 
obtains a compound which he calls “ dextro-saceharine,” which, as far 
as the taste is concerned, is scarcely distinguishable from the, best sugar. 
The quantity of saccharine used is in tin* proportion of one part to from 
1,000 to 2,000 parts of glucose. Now, since the price of saccharine is at 
present about 50* a pound, we shall find that even at this price such a 
mixture would be very considerably cheaper than real sugar, but we 
must bear in mind the fact that there is great likelihood of the process 
of manufacture of saccharine being considerably cheapened. 
It will then be evident not only that saccharine is a most interesting 
compound, but that it may also be destined to become an article of pri- 
mary commercial importance. The future must decide as to the rev- 
olutions it may bring about in the coal-tar industry, in the cultivation 
of the soil now devoted to growing canes or beets, and in the sugar in- 
dustry generally and other industries connected with it; but as great 
and important commercial interests are in question, it is highly advisa- 
ble to look well into this matter, and not allow’ our foreign competitors 
iu this and other markets to secure for themselves exclusively the ben- 
efit which this discovery may confer. There are in commerce small balls 
made from starch, to which has been added .05 per cent, of saccharine, 
of which one is sufficient to impart a very sweet taste, very similar to 
that of the best sugar, to a huge cup of black coffee. 
Investigations on the Sulphinides, by Dr. Ira Ilemsen.—The benzoic 
sulphinide described in the preceding note has been further studied by 
the author. By the substitution of the ethoxyl group for hydrogen 
paraethoxybenzoic sulphinide was obtained, crystallizing in fine white 
needles, melting at 257° to 258°. This derivative has not the sweet 
taste characteristic of the benzoic sulphinide. Another derivative, parn- 
brombenzoic sulphinide, crystallizing in long needles and subliming in 
feathery flakes at about 200°, has a remarkirlile taste. When first placed 
upon the tongue its taste is extremely sweet, fully as much so as that 
of benzoic sulphinide, a single small crystal being able to sweeten half 
a liter of water. After the sweet taste has passed an equally bitter taste 
takes its place, reminding one in its extreme bitterness of strychnine. 
This peculiarity can not be due to the presence of two substances of 
different degrees of solubility, since the purest specimens have this 
property. (Am. Chem. J., vm, 223.) 
Paranitrobenzoic Sulphinide, etc., by W. A. Noyes.—This body crys- 
tallizes iu small leaflets and in fine needles, fusing at 2011°. It is dillp CHEMISTRY. 
419 
cultly soluble in cold water and (together with its salts) has an intensely 
bitter taste. Its structure is as follows: 
Para-amidobenzoic sulpliinide, on the other hand, has an intensely sweet 
taste. Its solution, even when very dilute, shows a dark-blue fluor- 
escence. The author describes its salts with potassium, barium, and 
silver. (Am. Chem. J., vm, 167.) 
On Wrightine, by H. Warnecke.—This alkaloid, first isolated by Sten- 
house in 1864, from the seeds of Wrightia antidysenterica, an apocyna- 
ceous tree from India. It is the. first known solid base occurring in 
nature which is free from oxygen. If a trace of this base, dissolved in 
chloroform, is evaporated to dryness in a porcelain capsule, the residue 
covered with 2 to 3 c. c. of water and strong sulphuric acid is added in a 
slender stream, a golden-yellow color spreads from the bottom of the 
capsule through the whole liquid, and turns to a green on standing for 
twelve hours. If 1 milligram of the alkaloid is rubbed up in a watch- 
glass with five drops of strong sulphuric acid and let stand exposed to 
the air for two hours, the liquid which was at first colorless, turns yellow- 
ish green and finally a pale violet. If the above mixture is at once ex- 
posed in the neck of a flask to the steam of boiling water the mass turns 
dark green, and passes into deep blue on contact with a little water. 
(Ber. d. chem. Ges., xix.) 
Chemical Aspects of Future Food Supply.—The chemical section of 
.the American Association for the Advancement of Science, at the meet- 
ing in Buffalo, August, 1886, was numerously attended. The president 
of the section, Dr. Harvey W. Wiley, addressed the members on “The 
Economical Aspects of Agricultural Chemistry.” His concluding sen- 
tences on the Future Food Supply are as follows: “Since, with a proper 
economy, the natural supplies of potash and phosphoric acid, as we 
have seen, may be made to do duty over and over again, and last in- 
definitely, the economist who looks to the welfare of the future need 
have no fear of the failure of these resources of the growing plant. Iu- 
deed, it may be said that the available quantities of them may be in- 
creased by a wise practice of agriculture, based on the teachings 
of agricultural chemistry. But with the increase of population comes 
an increased demand for food, and therefore the stores of available 
nitrogen must be enlarged to supply the demands of the increased 
agricultural product. It is certain, that with the now analytical 
methods, and the new questions raised by the investigations of which 
I have spoken, many series of experiments will be undertaken, the 420 
RECORD OF SCIENCE FOR 1H86. 
outcome of which will definitely settle the question of the entrance 
of free nitrogen into vegetable tissues. If this question be answered 
affirmatively, agricultural science will not place bounds to the possible 
production of foods. If the nitrifying process does go on within the 
cells of plants, and if living organisms do fix free nitrogen in the soil in 
a form in which at least a portion of it may be nitrified, we may ex- 
pect to see the quantities of combined nitrogen increase pari pasmi 
with the needs of plant life. Thus, intensive culture may leave the 
gardens and spread over the fields, and the quantities of food suitable 
for the sustenance of the human race be enormously increased. In con- 
templating the agricultural economies of the future, however, it must not 
be forgotten that a certain degree of warmth is as necessary to plant 
development as potash, phosphoric acid, and nitrogen. If it be true, 
therefore, that the earth is gradually cooling, there may come a time 
when a cosmic athermancy may cause* the famine which scientific agri- 
culture will have prevented. Fortunately however for the human race 
the cereals, the best single article of food, are peculiarly suitable to a 
cold climate. Barley is cultivated in Iceland, and oatmeal feeds the 
best brain and muscle of the world in the high latitudes of Europe. It 
is probably true that all life, vegetable and animal, had its origin in the 
boreal circumpolar regions. Life has already been pushed half-way to 
the equator, and slowly but surely the armies of ice advance their lines. 
The march of the human race equatorwards is a forced march, even if it 
be no more than a millimeter in a millennium. Some time in the remote 
future the last man will reach the equator. There, with the mocking 
disk of the sun in the zenith, denying him warmth, flat-headed and 
pinched as to every feature, he will gulp his last mite of albuminoids in 
his oatmeal, and close his struggle against an indurate hospitality.” 
(Economical Aspects of Agricultural Chemistry, an Address by II. \V. 
Wiley. Cambridge, 1008.) 
Recent Prog rex* in the Coal-Tar Industry.—Under the above title Sir 
Henry E. Roscoe delivered a most valuable and interesting discourse 
at the Koval Institution on April 10, 1880. He refers the numerous 
products, whether dye-stuffs, perfumes, antipyretic medicines, or sweet 
principles to two great classes of hydrocarbons, the paraffinoid and the 
benzenoid hydrocarbons. The first is the foundation of the fats, and 
the second of the essences or aromatic bodies. Petroleum is the source 
of the first class and coal tar of the second. The following tables give 
an interesting view of the marvellous products of coal and their relative 
amounts. 
I. Products of distillation of 1 ton of Lancashire coal: 
10,000 cnbic feet gas. 
30 to 25 gallons ammouiacal liquor (5° Tw.). 
12 gallons of coal-tar 139.2 pounds, specific gravity, 1.16). 
13 hundredweight of coke. CHEMISTRY. 
421 
II. Products of 12 gallons of gas-tar: 
1.10 pounds benzene '(= 1.10 pounds aniline) 
0.90 pound toluene (=0.77 pound toluidine) 
= 0.62 pound magenta. 
1.5 ponuds phenol proper (=1.2 pounds Aurin). 
2.44 pounds solvent naphtlia (three xylenes). 
2.40 pounds heavy naphtha. 
6.30 pounds naphthalene (=5.25 pounds cr-naphthylamine, 7.11 vertnilline 
scarlet RRR, or 9.50 pounds naphthol yellow). 
17.0 pounds creosote. 
14.0 pounds heavy oil. 
0.46 pound anthracene (=2.25 alizarine 20 per cent.). 
69.6 pounds pitch. 
III. Dyeing power of colors from 1 ton of Lancashire coal: 
Pounds. 
Dye-stuff. 
Dye yards of 
flannel 27 
inches wide. 
0.6-23 
Magenta 
500 
[or, 1. *23 
Methylviolet .... 
1,000 ] 
9. 50 
Naplithol yellow. 
3,800 
[or, 7.11 
Vermiliiue 
2,560 ] 
1.2. 
Aurin 
120 
2.25 
Alizarin 
*255 
* Printers’ cloth. 
The distinguished lecturer illustrated the tinctorial power of the coal- 
tar products by exhibiting a party-colored flag showing the exact 
amount of color obtainable from 1 pound of Lancashire coal; this flag 
was made up as follows: 
Inches. 
Magenta flannel 8 x 27 
Violet flannel 24 x 27 
Yellow flannel 61 x27 
Orange flannel 1. 9 x 27 
Turkey-red flannel 4 x27 
The colors chosen are only a few amoDg the numerous list of deriva 
tives. This list comprises at present the following: 
1G distinct yellows. 
12 oranges. 
30 reds. 
15 blues. 
7 greens. 
9 violets. 
Several browns. 
Several blacks. 
Derived from benzene, to 
luene phenols, xylene, 
n a p h t h al e n e, anthra- 
cene. 
The coal-tar antipyretic medicines next engaged the lecturer’s atten- 
tion. Professor Dewar discovered in 1881 that quinoline belongs to the 422 
RECORD OF SCIENCE FOR 1880. 
aromatic series,and first observed that certain pyridine suits act as feb 
ri luges; so he may be called the father of antipyretic medicines. Of 
these, kairine was discovered by Prof. O. Fischer in 1881, and its feb- 
rifuge properties were first noticed by Professor Filehne, of Erlangen. 
It is actually ethyl-tetraoxy quinoline, and has the constitution 
Antipyrine, the second of these febrifuges, was discovered by Dr. L. 
Kuorr, of Erlangen, and its physiological properties were studied by 
Professor Filehne. It has the following constitution: 
orCnHwy20. For the preparation of these bodies and their physio- 
logical effects, as well as for brief notices of cumarine and vauilliue, we 
refer to the original address. (Nature, xxxiv, pp. Ill and 133.) 
/Statistics of the Coal Tar Color Industry.— In a paper on the scientific 
development of the coal-tar color industry, by Prof. K. Meldola, before 
the Society of Arts, he gives some statistics showing the magnitude of 
the industry under discussion. In Germany a factory of about the third 
magnitude consumes at present 500 to GOO tons of aniline per annum. 
The Badische Company employ twenty-five hundred laborers and olli 
cials, and the Hoechst Color Works (formerly Meister, Lucius & Binn- 
ing) employ sixteen hundred men and fifty-four chemists. In these 
large establishments they manufacture not only aniline, but alizarine, 
acids, alkalies, and all the necessary chemicals. 
The probable consumption of alizarine by British dye-works in 18SG 
amounted to G,900 tons (of 10 per cent, paste), of which perhaps G5 
per cent, was manufactured in Germany. The author points out that 
although historically the industry is indebted to English discoveries, 
commercially the control is leaving England for Germany. (Nature, 
XXXIV, 324.) 
NOTES. 
Gadolinium is the name definitely given by Marignac to the metal Yor, 
which he discovered in 1880. The provisional name was abandoned at 
the suggestion of Lecoq de Boisbaudran. This is not to be confounded 
with the same word as used by Xordensk jdld. 
Ammonio permanganate of silver, as well as the analogous compounds 
of copper, cadmium, nickel, zinc, and magnesium are new compound* CHEMISTRY. 
423 
obtained by J. Klobb. They are all explosive wnen ueated or struck 
by a hammer. (Comptes Reudus, cm, 384.) 
The decomposition of chlorine water in sunlightis shown by A.Popper 
to yield, besides the usually admitted oxygen and hypochloric acid, 
chloric acid itself, aud he shows that this was not formed by the treat- 
ment to which the liquid was subjected for analytical purposes. (Ann. 
Chem., ccxxxi.) 
Phosphorus tetroxide,P2G4, has been obtained by Thorpe and Tutton. 
It forms when phosphorus is burned in a limited supply of dry air. It 
occurs as transparent, highly lustrous, very deliquescent crystals, which 
do not fuse at 100°, and do volatilize at 180°. On solution in water 
they form pliosphoroso-phosphoric acid, previously discovered by Salzer. 
For reactions of this oxide and other details see original paper. (J. 
Chem, Soc., Trans. 188G, 833.) 
The thickness of the air layer adhering to glass has been carefully 
measured by Otto Schumann and found to be somewhat less than 
0.000007cm. O. E. Meyer estimates the diameter of molecules at 
0.000000005<>ni; the air layer is therefore more than one thousand times 
as large as the diameter of molecules. (Wiedemann’s Auualen, xxvn, 
91, ’86.) 
Attention is called by Arthur G. Bloxam to the solubility of sulphur 
in alcohol, a fact not generally noted in text-books. By slowly cooling 
a solution of sulphur in hot alcohol he obtained brilliantly transparent 
crystals up to half an inch in length, and so white as easily to be mis- 
taken for niter. Chemists using rubber corks in distilling alcohol should 
bear in mind this solubility of sulphur as a possible source of impurity. 
(Chem. News, Lin, 181.) 
Tyrotoxicon is the name given to a highly poisonous ptomaine dis- 
covered by Dr. Victor C. Vaughan in cheese. Its occurrence in poison- 
ous ice-cream has also been demonstrated by Dr. Vaughan, who pre- 
sented a paper on the subject to the Michigan State Board of Health, 
July 13, 1886. 
Lecoq de Boisbaudrau remarks the fluorescence of manganese sul- 
phate when mixed with a large amount of calcium sulphate and subjected 
to electrical action in a vacuum. Sulphate of manganese alone does not 
fluoresce under these conditions. (Comptes Rendus, cm, 468.) 
Caesium and rubidium nitrites, according to Tli. Rosenblatt, form 
with cobalt nitrite crystalline double salts, which are the least soluble 
compounds of these alkaline metals yet discovered. Caesio cobaltic- 
nirrite requires 20,100 parts of water at 17° C., and the rubidium salt 
19,800 parts for solution. Thallium forms similar compound. (Ber. d. 
chem. Ges , xix, 2531.) 
The oxides of gold have been critically studied by Gerhard Kriiss, who 
finds there are three only: Au2Oi, Au202, and Au2Ot. All attempts to 
obtain lower or higher oxides were futile. (Ber. d. chem. Ges., xix, 
2541.) 424 
RECORD OE SCIENCE FOR 1886. 
I oil i lie is reported by «J. A. Wanklyn to exist in a tree state in the 
mineral water of the Woodhall Spa, near Lincoln. Sufficient is present 
to impart a brown color to the water and to give the usual reaction with 
carbon disulphide. The spa has long been known as useful iu skin 
diseases (Cliem. News, Liv, 300.) 
The complete synthesis of pyrrol has been accomplished by Ciamician 
and Silber; the steps in the transformation from succinimide to pyrrol 
are as follows: Succinimide, bichlormalei'nimide, perchloride of tetra- 
chlorpyrrol, tetrachlorpyrrol, tetrajod pyrrol, pyrrol. (Ber. <1. chem. 
Ges., xix, 3027.) 
Combinationsof acetamide with metallic chlorides have been described 
by G. Andr6, notably with cupric chloride, cadmium chloride, the chlo- 
rides of nickel and cobalt, and mercuric chloride. These bodies are 
crystalline, and decompose at a moderately low temperature. (Comptes 
Remlus, on, 115.) 
Prof. A. Michaelis, of Aachen, continues his extended researches on 
compounds of the elements of the nitrogen group with radicals of the 
aromatic series. In Liebig’s Anualen, Vol. ccxxxin, in union with A. 
Reese, he describes several compounds of antimony with phenyl and 
its derivatives, and in union with Paetow he describes compounds of 
arsenic with benzyl. 
Calcined magnesia, showing peculiar behavior with reagents, is sup- 
posed by George Stillingtleet Johnson to contain rare earths. (Chem. 
News, liv, 88.) 
The mosandraof I)r. J. Lawrence Smith has been examined by Lecoq 
de Boisbaudran, samples being furnished by Dr. Marion, of Louisville, 
and found to consist chiefly of terbia and Ya. (Chem. News, liii, 103.) 
Sozolic acid, or orthoxypheuylsulphurous acid, discovered by M. Ser- 
rant, is a more powerful antiseptic than salicylic or phenic acids. The 
corresponding para compound has no antiseptic properties. The author 
claims for sozolic acid great benefits to medicine and surgery. (Comptes 
Keudus, Cll, 1079.) 
A summary of all that is known concerning samarium and its com- 
pounds has been published by P. T. Cleve, of (Jpsala. The subject is 
treated under the heads history, separation, mode of occurrence, atomic 
weight, sj>ectrum, oxides, and the numerous salts. (Chem. News, liii, 
30 et seq.) 
Cerium, yttrium, and glucinum, according to Dr. J. II. Stroliecker, 
occur iu extraordinary quantities in the clays of Hainstadt. One of 
the clays analyzed contained as high as 13.4 per cent, cerium hydrox- 
ide. The author’s analytical methods and his statements have met 
severe criticisms on the part of several chemists, but he insists on 
their accuracy. (J. f prakt. Chemie, 1880.) 
Glycyphylliu is a crystalline substance, which Dr. Edward H. Ren- 
nie extracted from the leaves of Smilax glycyphylla, a plant common 
in New South Wales. Crystallized from water it has the formula CHEMISTRY. 
425 
C21H2409+4£H20. On boiling with dilute sulphuric acid it decom- 
poses into pliloretiu and isodulcite, and is therefore closely allied to 
phlorizin. (J. Chem. Soc., Trans. 1886, 857.) 
According to Dr. F. W. Dafert, starch obtained from Panicutn candi 
dim yields with iodine a reddish brown color instead of the usual blue 
coloration. (Biedertnann’s Centralblatt, 1886.) 
The formation of ferrates can be conveniently exhibited in a lecture 
by a method described by C. L. Bloxam. Place a fragment of potas- 
sium hydroxide ill a solution of ferric chloride, add a few drops of bro- 
mine, and heat gently. The resulting dark brown mass dissolves in 
water, yielding a fine red solution, which may be kept many hours 
without decomposition. By boiling ferric chloride with bleaching pow- 
der a similar red solution of calcium ferrate can be obtained. (Chem. 
News, Liy, 43.) 
A new alloy of aluminium and tin (100A1 : lOSn), having a specific 
gravity of 2.85, is recommended by M. Bourbowze for all instruments 
requiring lightness. It can be soldered as easily as brass, and resists 
reagents almost as well as aluminium itself. (Comptes Rendus, oil, 
June 7, 1886.) 
The third annual convention of the Association of Official Agricul- 
tural Chemists was held August 26 and 27, in Washington, D. C., under 
the presidency of Dr. Harvey VV. Wiley. The members adopted official 
methods for determining phosphoric acid and moisture and for potash, 
but agreed not to select any single method for the determination of 
nitrogen as official. Details of the methods adopted and other papers 
of value will be found in the proceedings, published as Bulletin 12 of 
the Division of Chemistry, Department of Agriculture. 
The Berichteof the German Chemical Society in Berlin grows apace; 
the volumes for 1885 contain 3,516 pages of contributions and 1,033 
pages of abstracts, making a total of 4,549 pages. The society has 
ordered for 1886 an edition of 3,600 copies. 
The Tokyo Chemical Society (of Japan), organized in 1878 by the 
graduates of the Tokyo University, has eighty-six members. The offi- 
cers for 1886 are as follows: President, J. Sakurai; vice-presidents, T. 
Isouo, M. Kuliara, N. Matsui, J. Takayama, G. Nakasawa; secretary, 
T. Uyeda; treasurers, T. Isido and T. Takamatsu. The members are 
exclusive.y Japanese (no foreigners). They meet twice a month and 
publish a journal in Japanese entitled Tokyo Kagakkai Kaishi, edited 
by J. Sakurai. The eighth annual meeting was held April 10, 1886, at 
the botanical garden of the Imperial University, Tokyo, and several 
interesting addresses and papers were read. 
The Chemical Society of London now numbers fourteen hundred and 
fifty-nine fellows, thirty-one of these being honorary foreign members. 
During the year 1885-’86 one hundred and four papers were read to the 
society, a larger number than for several years past. The income for 
the year named amounted to £3,743. A subject catalogue of the library 426 
RECORD OF SCIENCE FOR 188G. 
was recently published. The president for the current year is Dr. Hugo 
Miiller, F. B. 8., and the first vice-president is William Crookes, F. It. S 
The twelve principal chemical societies of the world have nearly nine 
thousand members, distributed as shown in the following table (from 
H. C. Bolton’s Address to X. Y. Academy of Sciences, March 15, 1880): 
Deutsche cheruische Gesellschaft zu Berlin 2, 
Society of Chemical Industry (England) 2,40J 
Chemical Society of Londou 1,500 
8oci6t6 chimique de Paris 560 
Institute of Chemistry of Great Britain and Ireland 430 
American Chemical Society 250 
Society of Public Analysts (Englaud) lsO 
Chemical Society of St. Petersburg 100 
Associazioue chimico-farmaceuf ica Horentina *200 
Chemical Society of Tokio, Japan HI 
Chemical Society of Washington, D. C 48 
Association of Official Agricultural Chemists (IJuitod States of America) 17 
Total 8,7H1 
The centenary of the death of Schoele was commemorated on May 21, 
1880, at the little town of Koping, Sweden, where he passed the last 
ten years of his life. 
The prodigious activity in all departments of science obtaining in 
Germany is well illustrated by statistics of the meeting of “deutscher 
Natnrforsclier und Aerzte” held a* Berlin in September, 1880. At this 
meeting no less than 5,051 persons took part, including 2,221 members, 
I, associates, 1,490 women. Nearly every quarter of the globe was 
represented. North America by 42 persons, Japan by 10, India by 2, 
Egypt by 4, Australia by 4, aud the Cape of Good Hope by 2. In the 80 
sections into which the association is divided 522 lectures and 155 
experimental demonstrations were held in 131 sessions. And those in 
attendance were invited to join 48 excursions. 
The first meeting of this association was held in 1821, in Leipzig, and 
was attended by 13 persons; surely small beginnings are not to be 
despised. 
NECROLOGY OF CHEMISTS, J88G. 
Robert Alexander, a young English chemist of much promise, was 
killed instantly during the disastrous earthquake in Charleston, South 
Caroliua, August 31, 1880. He was born March 18, 1803, near Birken- 
head, England. His chemical education was chiefly in the analytical 
laboratory of Mr. G. W. Wigner, Loudon. In January, 1880, he came 
to America, and in March went to Charleston, where he was engaged 
in developing a sanitary system when he met his death. 
James Apjohn died June 2, 1880, at the advanced age of ninety one. 
He held the chair of chemistry in the Royal College of Surgeons, Dub- 
* Estimated. Many chemist** are members of several societies; against this dupli- 
cation may be set those chemists not c mnected with societies. CHEMISTRY. 
427 
lin, from 1823 to 1850, and in the University from the latter date until 
1874. He published many original memoirs on general physics and 
chemistry, and long held a foremost place as a theoretic and practical 
chemist. 
H. A. Bayne, professor of chemistry at the Royal Military College, 
Kingston, Ontario, died in September. He was a native of Nova Scotia. 
After graduating at Dalhousie College, Halifax, he studied chemistry 
with Bunsen and with Dumas. He had occupied the chair of chemistry 
at Kingston only since 1879. 
Appolinaire Bouchardat, born in 180(3, died April 7, 1880. He 
held since 1852 the chair of physics and organic chemistry in the Col- 
lege of Pharmacy of Paris. His investigations were chiefly in the field of 
pharmaceutical chemistry. He edited the “Anuuaire de therapeu, 
tique” from 1841 to 1885, the “Repertoire de pharinacie ” from 1847 to 
1872, and other important works. He was a member of many learned 
societies. 
Carl Bulk died in July, in the forty-first year of his age. He was 
a teacher in the Gewerbeschule in Barmen, and chemist to the Barmen 
Color Manufactory (Farben-Industrie), which makes a specialty of ani- 
line dyes. Dr. Bulk was an original member of the German Chemical 
Society. 
Alexander Michailowitsch yon Butlerow died August 17, 
1880. He was born September 0, 1828, in the province of Kasan, was 
at first a pharmaceutist, and then studied in the universities of Kasan 
and of Moscow, lu 1854 he became professor of chemistry at Kasan- 
and in 1809 at the University of St. Petersburg, which chair he held at 
his death. His original researches were chiefly in organic chemistry, 
and gained for him a world-wide reputation. 
Henry Suckden Evans, born at Islington, England, in 1830, died in 
Montreal in 1880. He was president of the Pharmaceutical Society and 
chief analyst to the Dominion of Canada. His publications were chiefly 
in pharmaceutical chemistry. 
Gottlieb C. Faas, a student of chemistry residing in Birmingham, 
Alabama, was killed by a locomotive October 3, in Pennsylvania. 
Francesco Filippuzzi, of Padua, died July 22f 1880. He was born 
in 1824, and after receiving his education in Austria was appointed pro- 
fessor of chemistry at the University of Padua, where he organized prac- 
tical courses modeled on those of German universities. Though not 
eminent as an investigator he will long be remembered as a teacher by 
numerous grateful pupils. A fuller notice will be found in Ber. d. chem. 
Ges., xix, 2941. 
Charles Froebel died June 19, 1880. He was professor of ana- 
lytical chemistry in the New York College of Pharmacy from 1872 to 
18S2. 
Frederick Guthrie, born October 15, 1833, died October 21,1880. 
From 1801 to 1807 lie held the chair of chemistry and physics in the 428 
RECORD OF SCIENCE FOR 1HS6. 
Royal College, Mauritius, and since 18(5!) the chair of physics in the 
Royal School of Mines, London. His original contributions to both 
sciences were numerous and important, lie founded in 1873 the Phys- 
ical Society of London. Guthrie was also the author of several works 
on heat, electricity, and molecular physics. 
F£lix Leblanc died in Paris in May (!), 1880. He was for many 
years a co-laborer with Dumas, and at his death was connected with the 
ltlcole Centrale des Arts et Manufactures, in Paris. His studies on car- 
bon monoxide are noteworthy. He was vice-president of the Society 
for Encouragement of National Industries, and member of many learned 
societies. 
E. Linnemann, professor of chemistry at the University of Prague, 
died April 137,1880. He was born in 1841. For an account of his scien- 
tific labors see Her. d. chem. Ges., xix, 1149. 
Frederic Melsens died in Brussels April 20, 1880, aged seventy- 
two years. He was an active investigator in both inorganic and organic 
chemistry throughout his life. 
Moser yon Moosbruch, of Vienna, an agricultural chemist, died 
early in the year 1880. 
William Ripley Nichols died July 14, aged thirty-nine. He held 
the chair of general chemistry in the Massachusetts Institute of Tech- 
nology, of which he was a graduate. He was the author of several text- 
books, and had a high reputation as an expert chemist in matters per- 
taining to hygiene. 
Max Reimann died October 22, 1880. His investigations and writ- 
ings for twenty years were chiefly in the line of industrial chemistry. 
For a biographical sketch see Ber. d. chem. Ges., xix (1880). 
G. F. Heinrich Schroder, born in Munich, September 28,1810, died 
May 12,1885. A full biography will be found in Berichte der deutschen 
chemischen Gesellschaft, xvm, It., 843. 
Charles UpnAM Shepard, the well-known American mineralogist, 
died May 1, 188G, in his eighty-second year. His chemical work was 
chiefly in connection with minerals. A full notice will be found in the 
American Journal of Science, Vol. xxxi, 482 (June, 1880). 
Edward Solly dic'd April 2, 1880, in the sixty-seventh year of his 
age. He was a member of the Royal Society. 
Julius Adolph Stockhardt, the well-know n agricultural chemist, 
died at Tharandt, Saxony, June 1, in his seventy-seventh year. He 
was the originator of the agricultural experiment stations now so com- 
mon in Europe and elsewhere. His text-book, “Principles of Chem- 
istry,” did much to popularize the science. He was editor of many jour- 
nals devoted to scientific agriculture. For a fuller sketch of his life see 
Popular Science Monthly for June, 1881. 
Magnus Troilius died April 19, in Philadelphia, Pennsylvania. 
He was a graduate of the Royal School of Mines of Stockholm, and 
held for several years the position of chemist to the Midvale Steel CHEMISTRY. 
429 
Works. His “Notes oil the Chemistry of Iron” was published during 
the year. 
Martin Websky, born July 17, 1824, died November 26, 1886. 
Since 1874 he has been professor of mineralogy at the University of 
Berlin, being the successor of Gustav Bose. His chemical work has 
been chiefly in connection with mining and mineralogy. 
Clemens Zimmermann, instructor in chemistry at the University of 
Munich, died March 27, 1885. He was born March 4, 1856, in Munich, 
and was consequently only twenty-nine years of age. Dr. Zimmermann 
was one of the most active and promising young chemists of Germany. 
His researches on the atomic weight of uranium and in analytical chem- 
istry are classical. A full biography (with portrait) will be found in 
Berichte der deutschen chemischen Gesellschaft, xvui, B., 826. 
Otto Ziurek died May 11, 1886. He was born in Upper Silesia 
June 19,1821. His literary and practical works were chiefly in the field 
of pharmaceutical chemistry. (Ber. d. chein. Ges., xix, 1316.) 
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Braun, F. Uutersuchnngen liber die Losliclikeit fester Korper und d'e den Yorgang 
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Breslauer, M. Die chemische Beschaifeuheit der Luft in Brandenburg a. H. Ein 
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Buckeridge, H. L. Chemical Student’s Manual for the Lecture-Room and Lab- 
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Bulletin du laboratoire provincial de chimie agricole & Roulers. Bruges, 1886. 8vo. 
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Casali, A. II passato, il preseute e 1’ avvenire della chiinica: discorso inauguralo 
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Ragguagli sui lavori esegniti uel laboratorio chimico agrario di Bologna. 
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Catalogue (A) of the Library of the Chemical Society, arranged according to subjects, 
with indexes containing authors’ names and subjects. London, 1886. 8vo. 
Cavazzi, A. Azione dell’ idrogene fosforato gassoso sul triclornro di oro sciolto nell’ 
etere, nell’ alcool o nell’ acqua. Bologna, 1885. 8vo. 
Azioni del gas idrogene fosforato sopra 1’ acido solforico. Bologna, 1886. 4to. 
Azione del solfuro di carbonio sopra alcuni metalli. Bologna, 1886. 4to. 
Metodo per prepararo il protocloruro di raine; sopra tin miscuglio esplosivo. 
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Cazeneuve, P. La coloration des vins par les couleurs de la houille. Methodes 
analytiques et marcbe systdmatique pour reconnaitre la nature de la coloration. 
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Centenaire de Chevreul, 31 aottt 1886. Principaux travaux de Chevrenl. Paris, 
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31 aoftt 1886. Discours prononcds ati Musdum d’histoire naturelle. Paris, 1886. 
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Cesaro, G. M6moire sur la reproduction de quelques phosphates do for natnrels par 
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Elements of Chemical Physics. 4th edit. London, 1886. Roy. 8vo. 
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Select Methods in Chemical Analysis (chiefly Inorganic). 8econd edition, re- 
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Deutsche Cbemiker-Zeitung. Centralblatt fiir die chemische Praxis und otfentlicbe 
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Encyclopddie chimique, publid sous la direction de Frdmv. Paris, 1886. 8vo. 
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Tome vn : Cbimie organique. Fasc. 4. fathers, par Leidid. 
Tome viii. Chirnie organique. Fasc. 6. Section 1. Alcalis organiques aftifi- 
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Tome x : Applications de cbimie organique. Analyse chimique des vdgdtaux, 
par G. Dragendorff. Traduit par F. Schlagdenhauffeu, RECORD OF SCIlsNOE FOR 1886. 
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Neue chemische Untersuehung des Kochbruunens zu Wiesbadeu und Verglsi- 
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Gange, C. Lehrbuch der augewaudten Optik in der Chemie. Spectralanalyse, 
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GeREACH, G. Th. Ueber Alkohol und Gemische aus Alkohol und Wasser. Wies- 
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Godefroy, L. Recherches relatives a Faction du chlore sur un melange de dichromate 
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Goppelsroeder, Friedrich. Ueber die Darstelluug der Farbstoffe sowie iiber deren 
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Gossels, W. Die Nitrate des Tbier- und Pflanzenkorpers. Berlin, 1686. 
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Grandeau, H. De Faction de sulfate de potasse a temperature dlevde sur les phos- 
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Guareschi, I. Nuove ricercbe sulla naftalina: nota. Torino, 1885. 8vo. 
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Separazione del nichelio dal cobalto. Pisa, 1886. 8vo. 
Guerin, G Origine et transformations des matieres azotees cbez les etres vivants. 
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Gcillaume, E. Fabrication de l’amidon, description des diverses operations. Paris, 
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Gusenburger, H. Die Untersucbungen der Schmierole und Fette mit specieller 
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Haarmann, Rudolph. Ein Beitrag zur Kenntniss der Isozuckersaure. Inaug.-Diss. 
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Haller, M. Ueber einige Derivate des Metaamidoanthraobinons. Freiburg i. B., 
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Hagemann,G A Studier over nogle Molekulvoiumen. 1886. 8vo. 
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Das Verziunen, Verzinkcn, Vernickelu, Verstiihleu und das Ueberzieben von 
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Harz, Kurt. Ueber die Propylaldekyd uud deudrei isomeren Toluidinen eutstehen- 
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Ueber einige mikroscopiscb- cheinische Keactiouen. Miiuclien, 1886. 8vo. 
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Hedix, S. G. Om pyridinens platinabaser. Akad. afhandl. Lund, 1886. 4to. 
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Heixzerlikg, C. Abriss der cliemischen Technologic mit besomlerer Rilcksicht auf 
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Die Gefaliren uud Krankheiten in der ehemischen Industrie und die Mittel zu 
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Heinzkrling, C. Phosphorfabrication, Ziiudholzer und Explosivstoffe. Halle, 1886. 
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Helene, M. La poudre A canon et les nouveaux corps explosifs. 2®6dition. Paris, 
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Henrici, J. Kleiner Grnudriss der Elementar-Chemie. Leipzig, 1886. 8vo. . 
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Heusel, J. Eine neue Theorie der Lebeus-Chemie in typisclien Figuren vnran- 
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Hoff, H. J. van’t. Bijdrage tot de keuuis der inaktieve appelzuren van verschil- 
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Hommage a Monsieur Chevrenl A l’occasion deson centenaire. Paris, 1886. 4to. 
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Humjiel, .J.J. The Dyeing of Textile Fabrics. London, 1885. 12mo. 
Husband, H. A. Aids to the Analysis of Food and Drugs. London, 1885. 12mo. 
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Isbekt, A. Zur Kenntuiss des Acetessigiithers uud eiuiger seiner Abkouiuilinge. 
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Israel, A- Ueber den Propiopropionsaureiithylather. Jena, 188(i. CHEMISTRY, 
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Kahn, M. Ueber die Einwirkung von Normalbutylaldehyd auf Anilin bei Gegen- 
wart rauckender Salzsiiure. Erlangen, 1886. 8vo. 
Kaiser, A. Ueber Mononitroderivate der Para- und Metaacetamidbenzoesiiure sowie 
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Kees, Alfred. Ein Beitrag zur Kenntniss des Helicins. Inaug.-Diss. Berlin, 1886. 
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Kleyer, A. Die Cbemie in ilirer Gesamtbeit und die cbemisclie Technologic der 
Neuzeit. Bearbeitet nacb eigeuem System unter Mitwirkung der bewahrtesten 
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von Amin-und Hydrazinbaseu auf Acetessigester und seine Derivate. Erlangen, 
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Kollrepp, A. Ueber einige Derivate der beiden gechlorten Para-Nitrophenole. 
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2 vols. Heidelberg, 1886. 8vo. 
M6mo;re sur les volumes moliiculaires des liquides. Remarques sur un ind- 
moire de Bartoli public dans les Annales de cbimie et de physique, 6e sdrie, 
mars 1886. Avec un avant-propos expliquant pourquoi ce mdraoire n’est pas 
publid dans les memes annales, et contenaut quelques remarques concernant “ Les 
origines do l’alchiinie” de Berthelotet les “Beitriige zur Gescbichte der Cbemie” 
de H. Kopp. Heidelberg, 1886. 8vo. 
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XpupuTuv Trapu. re rolg Kal rolg veuripoig. ’Ev ’AOjjvmg, 1886. 
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RECORD OF SCIENCE FOR 1886. 
Kratzer, H. Chemische Unterricbts-Brhfe. Fllr das SelbBt-Studium Erwachseuer. 
Mit besonderer Beiilcksichtigung der neuosten Fortsobritte der Cbemie mid mi- 
ter Mitwirkung liervorragender Facbmiinner und Gelebrten herausgegeben. I. 
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II. Cursus: Die orgauischo Cbemie, oder die Cbemie der Kohlenstoft'verbin- 
duugen. Mit besonderer Beriieksichtigung der chomischou Teebnologie. Filter 
Mitwirkung dor Ilerren Landerer, Herrburger, W. A. Herrmann, Alwin Engel- 
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Wasserglas und Iufnsorienerde, deren Natur und Bedeutung flir Industrie, 
Technik und die Gewerbe. Wien, 1886. 
Kreusskr, II. Das Eisen, sein Vorkommen und seine Gowinnung. Weimar, 1886. 
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trage der k. k. Reichs-Kriegs-MiuisteriHms verfasst. Wieu, 1886. 8vo. 
Krohn, C. W. Ueber einige Derivate des MonochlorpHOudocumolH. Miiuchen, 188T>. 
8vo. 
Krukenberg, C. F. Compendio di analisi cbimico-medico. Trad. c. note di D. 
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belladonna und des Extractum belladonnm. Inaug.- Diss. Freiburg, 1886. 
Kurzgefasste Anleitung zur qualitativen chemischen Analyse. Giessen, 1886. 
Labat, A. Du degr6 de certitude de l’analyse des eaux. Paris, 1885. 8vo. 
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Landoi.t, H. Ueber die Zeitdauer der Reaction zwischen Jodsiiure und Schwetliger- 
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Lange, O. Ueber Methylderivatedes Pyridins. Ein Beitrag zur Kenntuiss der Pyri- 
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Langguth, F. O. Beitriige zur Kenntniss der Parabibromcyinolsulfonsiiuro. Frei- 
burg i. B.. 1886. 8vo. 
Langi.ebeht, J. Qutmica. Trad, de la tiltima edicion francesa por L. Elizage. 
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Larbal£trier, A. Les engrais chimiques et les matures fertilisantes d’originu 
min<?rale; emploi pratique des engrais chimiques. Paris, 1885. 18mo. 
Larsen, E. Ueber Paraxylylphenylketon und seine Ueberfiihrung in Betamethylan- 
tbracen. Freiburg i. B., 1886. 8vo. 
Lahsson, A. Nagot om den kemiska industrien i Sverige. llelsingborg, 1886. 8vo. 
LAszi.6, E. D. Chemische und mechanische Analyse ungarlandischer Tbone mit 
Riicksicht auf ihre industrielle Verwendbarkeit. Ungariscb und Deutsch. Buda- 
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Lawes, Sir J. B., aud J. H. Gilbert. On the Valuation of Unexhausted Manures. 
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Leclerc, A. Recherches sur la de l’ammoniaqne dans les sols funnis an 
sulfate d’ammoniaque. Nancy, 1885. 8vo. 
Ledebi'R, A. Die Metalle, llire Gewinunng and ihre Verarbeitnng allgemein fasslicb 
dargestellt. Mit 64 in den Text eingedruckten Holzschnitten. I. Liefernng. 
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Lederkr, L. Synthese von Pyrrolderivaten. Erlangen* 1886. 8vo. 
Leeds, Albert R. A Chemical, Biological, and Experimental Inquiry into the pro- 
posed future Water Supply of the City of Albany. New York, 1886. 8vo. 
Leemans, C. Papyri gr*ci uiusei antiqnarii publici Lugduni-Batavi. Regis augustis- 
simi jussn edidit, interpretationem latinam, adnotationem, indices et tabulas ad- 
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Tomas II contains: *• Papyrus X. Excerpta chemica," the earliest text on chemistry. 
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Liebkecht, A. Uel>er Nicotin. Kiel, 1886. 8vo. CHEMISTRY. 
439 
Liebkkich, O. Ueberden todtenRaum bei chemischeu Reactionen. Berlin (Mitth. 
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Liepmann, H. K. Die Mechanik der Lencipp-Deinocritischen Atome unter beson- 
derer Beriicksichtigung <ler Frage nach dem Ursprung der Bewegung derselben. 
Leipzig, 1886. 8vo. , 
Liils-BoDART. Conference et manipulations chiiniques. Paris, 1885. 12mo. 
Linnemann, E. Ueber ein nenes Leuchtgas-Sanerstoffgeblase und das Zirkonlicht. 
Wien, 1886. 8vo. 
List, Reinhold. Zur Condensation von Thiobarnstoff und Acetessigiither. Inaug.- 
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Liveing, G. D. Chemical Equilibrium the Result of the Dissipation of Energy. 
Cambridge & London, 1886. 8vo. 
Loew, P. Ueber Formaldehyd und dessen Condensation. Leipzig, 1886. 8vo. 
Lomas, J. Manual of the Alcali Trade, including the Manufacture of Sulphuric Acid, 
Sulphate of Soda, and Bleaehing Powder. Second edition, with additions. Lon- 
don, 1886. 
Loo, H. van. Ueber das Betadichinolylin. Miinchen, 1885. 8vo. 
Lotman, G. Handboek voor bet omlerzoek van grondstoffen en producten der suiker- 
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LOw, W, Ueber Terephtalaldehyd. Erlangen, 1886. 8vo. 
LOwig, C. Arsenikvergiftung und Mumifikaticn. Gerichtlich-cliemischo Abhand- 
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Lutoslawski, W. Das Gesetz der Beschleunigung der Esterbildung. Beitrag zur 
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Lutz, Erich. Ueber don Abbau der Myristinsiiure bis zur Laurinsaure. Inaug.- 
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Mahreniioltz, A. Die praktisch-cheraischen Uebungen an Landwirtschaftsschulen. 
Zum Gebrauch bei den analytischen Arbeiten im Laboratorium zusammengestellt. 
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Maindron, Ernest. L’oeuvre de Jean-Baptiste Dumas, avec une introduction par 
Schiitzenberger, accompagn6 d’un portrait de Dumas. Paris, 1886. 8vo. 
Malosse, Th. Calorim6trie et thermom6trie. Paris, 1886. 
Manuel de chimie inorgamque h l’usage des dlfeves du pensionnat des frbres des 6coles 
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Marchand, V. Le. Chimie de 1’unitA Etude comparative des mathdmatiques cos- 
miques par la science de l’arithm6tiqne naturelle. Caen, 1886. 8vo. 
Mascarenas, Eugenio, y Jaime Santoma. Estudio analltico de vinos catalanes. 
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Maschke, Leopold. Ein Beitrag zur Kenntniss des /J-Naphtylamins. Ueber einen 
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Masing, M. E. Elements der pharmaceutischen Chemie. Ein Leitfaden fiir den 
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Maumen£, E. Lemons sur la thdorie g6n6rale de Paction chimique, professdes it 
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Mautiiner und Suida. Zur Gewinnung von Indol aus Derivaten des Orthotoluidins. 
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Matbury, A. C. The Student’s Chemistry. Part I. Non-metallic Elements. Lon- 
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Mayer, A. Lehrbuch der Agriculturchemie in 40 Yorlesungen. Nebst Auhang: 
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Mays, K. Notiz iiber eine bequeme Bereitungsweise der neutralen Lackmuspa- 
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Mazzara, G. Ricerche snlla trasformazione del tirnol in carvacrol: nota. Torino, 
1886. 8vo. 
Mazzara, G., e G. Discalzo. Bromoderivati del timol, del timochinone e dell’ ossi- 
tim*l:u«ta. Teriae, 1886. 8v«. 440 
RECORD OF SCIENCE FOR 1886. 
Mazzara, G. e G. Possbtto. Supra il diamilossimetiltrifeuilmetano. Torino, 1885. 
Meads, S. 1*. Chemical Primer; an elementary work for use in high schools, acad- 
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Medicus, Ludw. Kurze Auleituug zur Gewichtsaualysc. Uebuugsbeispiele zum 
Gebraucho beirn Uuterricht in chemischen Laboratorien. 3. Autlage. Tiibingen, 
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Meissner, Franz. Ueber die beim Bcuetzen pulverformiger Kdrper auftretende 
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von O. Bach. 2. verbesserte Aullage. Leipzig, 1886. 8vo. 
Merck, W. Ueber Cocaiu. Kiel, 1886. 8vo. 
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Gottingen, 1886. 
Meusel, E. Die Quellkraft der Rhodanate und die Quellung als Ursache ferment- 
artiger Reaktionen. Gera, 1886. 8vo. 
Meyer, E. von. Uutersuchuugeu Uber Isatosiiure und Abkdmmlinge dene 1 ben. 
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Meyer, L. Ueber die ueuere Entwickolung der chemischen Atomlehre. Tiibingen, 
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Meyer, P. Ueber Amido- und Oxypheuanthreuchinoue. Bonu, 1886. 8vo. 
Meyer, R. Ueber die iutramolekuluren Uiulageruugeu indeuCymol-nnd Cumiureihc. 
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Milani, Antonio. Sulla preparazioue farmaceutica del nitrato d’ amile. Roiua, 
1885. 
Milani, G. La chimica in famiglia con cinquauta disegni originali di E. Mazzauti. 
Firenze, 1«86. 16mo. 
Miller, W. von, und II. Kilia ii. Kurzes Lehrbuch dei analytiseben Chemie. 
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Mills, E. J. Destructive Distillation, or the Paratliu, Coal Tar, Resin, Oil and 
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MOnkeuero, K. Eiuwirkung von Chlorameisensaureiither auf Nitrotoluideu. Inaug.- 
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Molisch, H. Zwei ueue Zuckerreactioneu. Wien, 1886. 8vo. 
Morley, II. Forster. Outlines of Organic Chemistry. Loudon, 1886. 8vo. 
M('iilberg, F. Der Kreislauf der StofFe auf der Erde. Basel, 1886. 8vo. 
Muir and Wilson. The Elements of Thermal Chemistry. London, 1885. 8vo. 
Munroe, Charles E. Index to the Literature of Explosives. Part I. Baltimore, 
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Muspratt. Tbeoretische, praktische und aualytische Chemie, in Anwenduug auf 
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Nicolaysen, Carl. Zur Kenutuiss des Phenylacridins. Freiburg i. B, 1885. 
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On tbe influence of fluctuatious of atmospheric pressure on the evolution of fire-damp. 
Report of experiments concerning this question carried on in tbe Archduke 
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Orme, Temple. Rudiments of Chemistry. London, 1886. 8vo. 
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Parmentier. Molybdeue, vanadium, et titane. Paris, 1886. 8vo. 
Parneli., E. A. The Life and Labors of John Mercer, the self-taught Chemical Phi- 
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Parone, S. Corso di nozioni fisico-chimiche e di materie prime. 2 vols. Torino, 
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Patiie, K. Ueber die Einwirkung von Brom auf die Pseudocumol (5) sulfonsaure 
in verdiinnter wasseriger Losuug und einige Derivate des Pseudocumols. Frei- 
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Paterno, E., e R. Nasini. Sulla determinazione del peso moleculare delle sostauze 
organiche per mezzo del puuto di congelameuto delle loro soluzioni. Roma, 1886. 
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Paucksch, H. Beitriige zur Kenntniss des Ortho- und Paraamidoathylbenzols 
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Pawlewski, Bronislaw. Sposoby oceniania wartosci naftv. Warszawa, 1885. 
Peale, Albert C. Lists and Analyses of the Mineral Springs of the United States. 
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Pendleton, J. H. Ueber Isomerie in der Thiophenreihe. Gottingen, 1886. 8vo. 
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Analyses des mat i feres fertilisantes et alimentaires. 2me Edition, revue et aug- 
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Peters, Hermann. Aus pharmaceutischer Vorzeit in Bild uud Wort. Berlin, 1886. 
Peyraud, H. Etudes expferimentales sur la composition de Fair de Vichy. Bordeaux, 
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Pfeiffer, E. Die Analyse der Milch. Anleitnng zur qualitativen und quautita- 
tiven Untersuchuug dieses Secretes fiir Chemiker, Pharmazeuten und Aertzte. 
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Pfungst, A. Ueber die Einwirkung der Nitroethane auf die chlorhydrine melir- 
werthiger Alkohole, Leipzig, 1886. 8vo. 
Phillips, S. E. Old or New Chemistry, which is fittest for survival ? And other 
essays in chemical philosophy. London, 1886. 
Phipson, T. L. Outlines of a New Atomic Theory. Fourth edition. London, 1886. 
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Pickel, M. Beitrag zur Kenntniss der Condensation der Phenylhydrazin. Erlangen, 
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Pinner, A. Repetitorium der organischen Chemie. 7. Aufl. Berlin, 1886. 8vo. 
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Posadsky, S. Practischc Modification der Pettenkofer-Nagorsky’schen Methode zur 
Bestimmung des Kohleusauregehalts dei Luit. Mit Tabellen : i. Der Bestimm- 
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der Barytlosung, und 11. Zur Reduction eines Gasvolumens auf 0° Temperatur 
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Proceedings of the Third Annual Convention of the Association of Official Agricult- 
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RECORD OF SCIENCE FOR 1886 
prrciiKTT, I. Qualitative Chemical Analyses (Inorganic and Organic). Part I. 
Elemeutary stage for schools and science classes. Leeds, 1886. 12rtio. 
Rammklsbeiig, C. F. Handbuch der Mineralchemie. Erganznngsheft aur 8. Auflage. 
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Diechemische Natnrder Mineralien. Svstematisch znsammengestellt. Berlin, 
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Leitfaden fiir die qnantitative chemische Analyse, bosomlers der Mineralien 
and Hiittenprodncte, dnrcli Bcispiele erliiutert. 4. nmgearbeitete Antlagn. Ber- 
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Ramsaukr, P. Petroleum. Oldenburg, 1886. 8vo. 
Raskk, Kart.. Znr chemischen Kenntniss des Embryo. Berlin, 1886. 
Rathke, A. Bibliothek fiir Zucker-Interessenten. Bandinndv. Magdeburg, 1886. 
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Recoura, A. Recherches sur les chlorures de chrome. Paris, 1886. 4to. 
Reese, A. Ueber aromatische Antimonverbindungen. Freiburg i. B., 1885. 8vo. 
Rkgodt, II. Notions de chimie applicables aux usages de la vie (programmes offl- 
ciels). 27e 6d. Paris, 1886. 12mo. 
Rkh, A. Ueber die Einfiihrung von Brom in Benzoesiiure und die Einwirkung von 
Natrium auf Metabrombenzoesaureiithylester. Darmstadt, 1886. 8vo. 
Remse.n, Ira. An Introduction to the Study of Chemistry. New York, 1886. 8vo. 
Einleitung in das Studium der Kohlenstoffverbindungen, oder Organische 
Chemie. Tiibingen, 1886. 
Rknk, F. Die Luffc. (Aus dem Handbuch der Hygiene.) Leipzig, 1886. 8vo. 
Renotte, F. Petite chimie agricole A la portae des cultivateurs. Entretieu familier 
sur la vie des plautes et sur la culture ratiounelle de la bctterave et 
sur les champs Louvain, 1886. 8vo. 
Reuss, W. Beitriige zur Kenntniss der salpetersauren Quecksilberoxydulsalze. 
Braunschweig, 1886. 8vo. 
Richards, Edgar. Principles and Methods of Soil Analysis. Bulletin No. 10, De- 
partment of Agriculture, Division of Chemistry. Washington, 1886. 8vo. 
Richards, Eli.en H. Food Materials and their Adulterations. Household Manuals 
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Richardson, A. On the Determination of the Vapor Pressure of Organic Alcohols 
and Acids and the Relations existing between the Vapor Pressures of Organic 
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Richter, V. v. Lehrbnch der anorganischcn Chemie. Mit 69 Holzschnitten und I 
Spectraltafel. 5. neu bearb. Auflage. Bonn, 1886. 8vo. 
Chemistry of the Carbon Compounds, or Organic Chemistry. Translated from 
• the fourth German edition by E. F. Smith. Philadelphia, 1886. 
Rischbieth, P. Ueber die Ratlinose oder den sogenaunten Plnszucker aus Melasso 
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Rivot. Docimasic; Trait6 d’analyse des substances minlrales. Tome v. Paris, 1886. 
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Rosa, A., ed E. Pf.rroncito. Relazione sull’ analiei chimica e biologies su alcune 
acque proposte per provedere di acqua potabile la cittA di Aosta. Aosta, 1886. 
16mo. 
Roscoe, Henry E. Lessons in Elementary Chemistry, Inorganic and Organic. New 
edition. London, 1886. 
Roscoe, H, und C. Schorlemmer. Kurzes Lehrbuch der Chemie nachden nenesten 
Ansichten der Wissenschaft. 8. Anfl. Braunschweig, 1886. 8vo. 
Rosenberg, J. Beitrage zur Kenntniss der Thiophengruppe. Anhang iiber die An- 
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Rydberg, J. R. Om de kemiska grundiimnenas periodiska system. Stockholm, 
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Sacc, F. Trabajos del laboratorio nacional de qufmica en Cochabamba. La Paz, 
1886. 12mo. 
Sadtler, S. P. Die Gewinnung des Theers and Ammoniakwassers. Uebersetzt und 
mit einem Anhange verseheu von G. Bornemaun. Leipzig, 1886. 8vo. 
Salmonowitz, S. Beitriige zur Kenntniss der Alkaloide des Aconitum lycoctonum. 
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Sanger, A. Ueber einige Aether und eine neue Bildungsweise der Unterphosplior- 
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Saucerotte. Petite cliimie des 6coles, simples notions sur les applications de cette 
science a Pindustrie, & l’agriculture, et & l’dconomie domestique. 6s Edition, 
revue et modifide. Paris, 1885. 18mo. 
Sbriziolo, M. Trattato teorico-pratico di tossicologia generale e speciale medico- 
clinico-legale. Napoli, 1885. 
Schafft, A. Uebersichtstafeln zum Unterricht in der anorganischen Chemie und 
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Schafs, A. Notes des aides-chimistes pour sncreries. St.-Trond, 1885. 8vo. 
Scheurer-Kestner. Nicolas Leblanc et sa sonde artificielle. (Conference de la 
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Schmid, Jacob. Ueber das Fisetin, den Farbstoff des Fisetholzes. Iuaug.-Diss. 
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Schmieder, Johannes. Ueber Bestandtheile des Polyporus. Inaug.-Diss. (Erlan- 
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Schmidt, E. Beitriige zur Kenntniss der isomeren Mono- und Dinitroderivate der 
unsymmetri8chon (a)-m-xylolsulfonsiiure. Freiburg i. B., 188 . 8\ o. 
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