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6. | CHAPTER VI
THE AGE OF MODERN CHEMISTRY |
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6. CHAPTER VI
THE AGE OF MODERN CHEMISTRY
§ 71. The Birth of Modern Chemistry.
Chemistry as distinct from Alchemy and iatro-chemistry commenced with Robert Boyle (see plate 15), who first clearly recognised that its aim is neither the transmutation of the metals nor the preparation of medicines, but the observation and generalisation of a certain class of phenomena; who denied the validity of the alchemistic view of the constitution of matter, and enunciated the definition of an element which has since reigned supreme in Chemistry; and who enriched the science with observations of the utmost importance. Boyle, however, was a man whose ideas were in advance of his times, and intervening between the iatro-chemical period and the Age of Modern Chemistry proper came the period of the Phlogistic Theory—a theory which had a certain affinity with the ideas of the alchemists.
§ 72. The Phlogiston Theory.
The phlogiston theory was mainly due to Georg Ernst Stahl (1660-1734), Becher (1635-1682) had attempted to revive the once universally accepted sulphur-mercury-salt theory of the alchemists in a somewhat modified form, by the assumption that all substances consist of three earths—the
PLATE 15. PORTRAIT OF ROBERT BOYLE
[Description: Portrait of Robert Boyle]§ 73. Boyle and the Definition of an Element.
Robert Boyle (1626-1691) had defined an element as a substance which could not be decomposed, but which could enter into combination with other elements giving compounds capable of decomposition into these original elements. Hence, the metals were classed among the elements, since they had defied all attempts to decompose them. Now, it must be noted that this definition is of a negative character, and, although it is convenient to term "elements" all substances which have so far defied decomposition, it is a matter of impossibility to decide what substances are true elements with absolute certainty; and the possibility, however faint, that gold and other metals are of a compound nature, and hence the possibility of preparing gold from the "base" metals or other substances, must always remain. This uncertainty regarding the elements appears to have generally been recognised by the new school of chemists, but this having been so, it is the more surprising that their criticism of alchemistic art was not less severe.
§ 74. The Stoichiometric Laws.
With the study of the relative weights in
- 1. "The Law of Constant Proportion"—The same chemical compound always contains the same elements, and there is a constant ratio between the weights of the constituent elements present.
- 2. "The Law of Multiple Proportions"—If two substances combine chemically in more than one proportion, the weights of the one which combine with a given weight of the other, stand in a simple rational ratio to one another.
- 3. "The Law of Combining Weights"—Substances combine either in the ratio of their combining numbers, or in simple rational multiples or submultiples of these numbers. (The weights of different substances which combine with a given weight of some particular substance, which is taken as the unit, are called the combining numbers of such substances with reference to this unit. The usual unit now chosen is 8 grammes of Oxygen.)2
As examples of these laws we may take the few following simple facts:—
- 1. Pure water is found always to consist of oxygen and hydrogen combined in the ratio of 1.008 parts by weight of the latter to 8 parts by weight of the former; and pure sulphur-dioxide, to take another example, is found always to consist of sulphur and oxygen combined in the ratio of 8.02 parts by weight of sulphur to 8 parts by weight of oxygen. (The Law of Constant Proportion.)
- 2. Another compound is known consisting only of oxygen and hydrogen, which, however, differs entirely in its properties from water. It is found always to consist of oxygen and hydrogen combined in the ratio of 1.008 parts by weight of the latter to 16 parts by weight of the former, i.e., in it a definite weight of hydrogen is combined with an amount of oxygen exactly twice that which is combined with the same weight of hydrogen in water. No definite compound has been discovered with a constitution intermediate between these two. Other compounds consisting only of sulphur and oxygen are also known. One of these (viz., sulphur-trioxide, or sulphuric anhydride) is found always to consist of sulphur and oxygen combined in the ratio of 5.35 parts by weight of sulphur to 8 parts by weight of oxygen. We see, therefore, that the weights of sulphur combined with a definite weight of oxygen in the two compounds called respectively "sulphur-dioxide" and "sulphur-trioxide," are in the proportion of 8.02 to 5.35, i.e., 3:2. Similar simple ratios are obtained in the case of all the other compounds. (The Law of Multiple Proportions.)
- 3. From the data given in (1) above we can fix the combining
number of hydrogen as 1.008, that of
sulphur as 8.02. Now, compounds are known containing sulphur and hydrogen, and, in each case, the weight of sulphur combined with 1.008 grammes of hydrogen is found always to be either 8.02 grammes or some multiple or submultiple of this quantity. Thus, in the simplest compound of this sort, containing only hydrogen and sulphur (viz., sulphuretted-hydrogen or hydrogen sulphide), 1.008 grammes of hydrogen is found always to be combined with 16.04 grammes of sulphur, i.e., exactly twice the above quantity. (The Law of Combining Weights.)99
Berthollet (1748-1822) denied the truth of the law of constant proportion, and a controversy ensued between this chemist and Proust (1755-1826), who undertook a research to settle the question, the results of which were in entire agreement with the law, and were regarded as completely substantiating it.
§ 75. Dalton's Atomic Theory.
At the beginning of the nineteenth century, John Dalton (see plate 15{sic should be 16}) put forward his Atomic Theory in explanation of these facts. This theory assumes (1) that all matter is made up of small indivisible and indestructible particles, called "atoms"; (2) that all atoms are not alike, there being as many different sorts of atoms as there are elements; (3) that the atoms constituting any one element are exactly alike and are of definite weight; and (4) that compounds are produced by the combination of different atoms. Now, it is at once evident that if matter be so constituted, the stoichiometric laws must necessarily follow. For the smallest particle of any definite compound (now called a "molecule") must consist of a definite assemblage of different atoms, and these
PLATE 16.
PORTRAIT OF JOHN DALTON
[by Worthington, after Allen]
[Description: Portrait of John Dalton]
§ 76. The Determination of the Atomic Weights of the Elements.
With the acceptance of Dalton's Atomic Theory, it became necessary to determine the atomic weights of the various elements, i.e., not the absolute atomic weights, but the relative weights of the various atoms with reference to one of them as unit.4
We cannot in this place enter upon a discussion of the various difficulties, both of an experimental and theoretical nature, which were involved in this problem, save to remark that the correct atomic weights could be arrived at only with the acceptance of Avogadro's Hypothesis. This hypothesis, which is to the effect that equal volumes of different gases measured at the same temperature and pressure contain an equal number of gaseous molecules, was put forward in explanation of a number of facts connected with the physical behaviour of gases; but its importance was for some time unrecognised, owing to the fact that the distinction between atoms and molecules was not yet clearly drawn. A list of those chemical substances at present recognised as "elements," together with their atomic weights, will be found on pp. 106, 107.
§ 77. Prout's Hypothesis.
It was observed by a chemist of the name of Prout, that, the atomic weight of hydrogen being taken
It is highly probable that what is true of the elements investigated by Dr. Aston is true of the remainder. It appears, therefore, that the irregularities presented by the atomic weights of the ordinary elements, which have so much puzzled men of science in the past, are due to the fact that these elements are, in many cases, mixtures. As concerns hydrogen, it is only reasonable to suppose that the close packing of electrically charged particles should give rise to a slight decrease in their total mass, so that the atomic weights of other elements referred to H = 1 should be slightly less than whole numbers, or, what is the same thing, that the atomic weight of hydrogen referred to O = 16 should be slightly more than unity.
§ 78. The "Periodic Law".
A remarkable property of the atomic weights was discovered, in the sixties, independently by Lothar Meyer and Mendeléeff. They found that the elements could be arranged in rows in the order of their atomic weights so that similar elements would be found in the same columns. A modernised form of the Periodic Table will be found on pp. 106, 107. It will be noticed, for example, that the "alkali" metals, Lithium, Sodium, Rubidium and Cæsium, which
0 | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 |
[Hydrogen H=1°008]a |
Hydrogen H=1°008 |
|||||||
Helium He=4°00 |
Lithium Li=6°94 |
Glucinum Gl=9°1 |
Boron B=10°9 |
Carbon C=12°005 |
Nitrogen N=14.008 |
Oxygen O=16°00 |
Flourine F=19°0 |
|
Neon Ne=20°2 |
Sodium Na=23°00 |
Magnesium Mg=24°32 |
Aluminium Al=27°1 |
Silicon Si=28°3 |
Phosphorus P=31°04 |
Sulphur S=32°06 |
Chlorine Cl=35°46 |
|
Argon A=39°9' |
Potassiumb K=39°10 |
Calcium Ca=40°07 |
Scandium Sc=45°1 |
Titanium Ti=48°1 |
Vanadium V=51°0 |
Chromium Cr=52°0 |
Manganese Mn=54°93 |
Iron Fe=55°84c Cobalt Co=58°97 Nickel Ni=58°68 |
Copper Cu=63°57 |
Zinc Zn=65°37 |
Gallium Ga=70°1 |
Germanium Ge=72°5 |
Arsenic As=74°96 |
Selenium Se=79°2 |
Bromine Br=79°92 |
||
Krypton Kr=82°92 |
Rubidium Rb=85°45 |
Strontium Sr=87°63 |
Yttrium Y=89°33 |
Zirconium Zr=90°6 |
Columbium Cb=93°1 |
Molybdenum Mo=96°0 |
? | Ruthenium Ru=101°7 Rhodium Rh=102°9 Palladium Pd=106°7 |
Silver Ag=107°88 |
Cadmium Cd=112°40 |
Indium In=114°8 |
Tin Sn=118°7 |
Antimony Sb=120°2 |
Tellurium Te=127°5 |
Iodined I (orJ)- 126°92 |
||
Xenon Xe=130°2 |
Cæsium Cs=132°81 |
Barium Ba=137°37 |
Lanthanum La=139°0 |
Ceriume Ce=140°25 |
? | ? | ? | ? |
? | ? | ? | ? | ? | ? | ? | ||
? | ? | ? | ? | ? | Tantalum Ta=181°5 |
Tungsten W=184°0 |
? | Osmium Os=190°9 Iridium Ir=193°1 Platinum Pt=195°2 |
Gold Au=197°2 |
Mercury Hg=200°6 |
Thallium Tl=204°0 |
Lead Pb=207°20 |
Bismuth Bi=208°0 |
Polonium |
? | ||
Emanation (Niton)222°0 |
? | Radium Ra=226°0 |
Actinium ? |
Thorium Th=232°15 |
Ekatantalum ? |
Uranium U=238°2 |
? | ? |
NOTES.
There are several somewhat different forms of this Periodic Table. This is one of the simplest, but it lacks certain advantages of some of the more complicated forms. The atomic weights given are those of the International Atomic Weights Committee for 1920-1. They are calculated on the basis. Oxygen = 16. The number of decimal places given in each case indicates the degree of accuracy with which each atomic weight has been determined. The letter or letters underneath the name of each element is the symbol by which it is invariably designated by chemists.
The number above each column indicates the valency which the elements of each group exhibit towards oxygen. Many of the elements are exceptional in this respect.
[a] The exact position of Hydrogen is in dispute.
[b] The positions of Argon and Potassium have been inverted in order that these elements may fall in the right columns with the elements they resemble; [d] 50 also have the positions of Tellurium and Iodine.
[c] The whole of "Group 8" forms an exception to the Table.
[e] There are a number of ill-defined rare earth metals with atomic weights lying between those of Cerium and Tantalum. They all appear to resemble the elements of "Group 3," so that their positions in the Table cannot be decided with accuracy.
resemble one another very closely, fall in Column 1; the "alkaline earth" metals occur together in Column 2; though in each case these are accompanied by certain elements with somewhat different properties. Much the same holds good in the case of the other columns of this Table; there is manifested a remarkable regularity, with certain still more remarkable divergences (see notes appended to Table on pp. 106, 107). This regularity exhibited by the "elements" is of considerable importance, since it shows that, in general, the properties of the "elements" are periodic functions of their atomic weights; and, together with certain other remarkable properties of the "elements," distinguishes them sharply from the "compounds." It may be concluded with tolerable certainty, therefore, that if the "elements" are in reality of a compound nature, they are all, in general, compounds of a like nature distinct from that of other compounds.
It is now some years since the late Sir William Crookes attempted to explain the periodicity of the properties of the elements on the theory that they have all been evolved by a conglomerating process from some primal stuff—the protyle—consisting of very small particles. He represented the action of this generative cause by means of a "figure of eight" spiral, along which the elements are placed at regular intervals, so that similar elements come underneath one another, as in Mendeléeff's table, though the grouping differs in some respects. The slope of the curve is supposed to represent the decline of some factor (e.g., temperature) conditioning the process, which process is assumed to be of a recurrent nature, like the swing of a pendulum After the completion of one swing
§ 79. The Corpuscular Theory of Matter.
We must now turn our attention to those recent views of the constitution of matter which originated to a great extent in the investigations of the passage of electricity through gases at very low pressures. It will be possible, however, on the present occasion, to give only the very briefest account of the subject; but a fuller treatment is rendered unnecessary by the fact that these and allied investigations and the theories to which they have given rise have been fully treated in several well-known works, by various authorities on the subject, which have appeared during the last few years. 7
When an electrical discharge is passed through a high-vacuum tube, invisible rays are emitted from the kathode, generally with the production of a greenish-yellow
§ 80. Proof that the Electrons are not Matter.
This eminent physicist, however, had shown mathematically that a charged particle moving with a very high velocity (approaching that of light)
"The corpuscle is, then, nothing but a disembodied, electrical charge, containing nothing material, as we have been accustomed to use that term. It is electricity, and nothing but electricity. With this new conception a new term was introduced, and, now, instead of speaking of the corpuscle we speak of the electron." 8 Applying this modification to the above view of the constitution of matter, we have what is called "the electronic theory," namely, that the
§ 81. The Electronic Theory of Matter.
Sir J. J. Thomson has elaborated this theory of the nature and constitution of matter; he has shown what systems of electrons would be stable, and has attempted to find therein the significance of Mendeléeff's generalisation and the explanation of valency. There can be no doubt that there is a considerable element of truth in the electronic theory of matter; the one characteristic property of matter, i.e., inertia, can be accounted for electrically. The fundamental difficulty is that the electrons are units of negative electricity, whereas matter is electrically neutral. Several theories have been put forward to surmount this difficulty. Certainly the electron is a constituent of matter; but is it the sole constituent? Recent research indicates that, as already pointed out, all atoms consist of two distinct portions, a massive central nucleus, whose net charge is positive, surrounded by a number of electrons, just sufficient to neutralize this charge. The point of greatest interest is that the indicated number of free electrons is exactly the number which expresses the position of the element in the Periodic Table, reckoning helium as 2, lithium as 3, and so on; and it would seem that the chemical properties of the elements are determined entirely by these electrons, and are, therefore, not, strictly speaking, periodic functions of their atomic weights, as was formerly thought (§ 78), but of their atomic numbers. The exact nature of the nuclei of the various atoms has yet to be
§ 82. The Etheric Theory of Matter.
The analysis of matter has been carried a step further. A philosophical view of the Cosmos involves the assumption of an absolutely continuous and homogeneous medium filling all space, for an absolute vacuum is unthinkable, and if it were supposed that the stuff filling all space is of an atomic structure, the question arises, What occupies the interstices between its atoms? This ubiquitous medium is termed by the scientists of to-day "the Ether of Space." Moreover, such a medium as the Ether is demanded by the phenomena of light. It appears, however, that the ether of space has another and a still more important function than the transmission of light: the idea that matter has its explanation therein has been developed by Sir Oliver Lodge. The evidence certainly points to the conclusion that matter is some sort of singularity in the ether, probably a stress centre. We have been too much accustomed to think of the ether as something excessively light and quite the reverse of massive or dense, in which it appears we have been wrong. Sir Oliver Lodge calculates that the density of the ether is far greater than that of the most dense forms of matter; not that matter is to be thought of as a rarefaction of the ether, for the ether within matter is as dense as that without. What we call matter, however, is not a continuous substance; it consists,
§ 83. Further Evidence of the Complexity of the Atoms.
There are also certain other facts which appear to demand such a modification of Dalton's Atomic Theory as is found in the Electronic Theory. One of the characteristics of the chemical elements is that each one gives a spectrum peculiar to itself. The spectrum of an element must, therefore, be due to its atoms, which in some way are able, at a sufficiently high temperature, to act upon the ether so as to produce vibrations of definite and characteristic wave-length. Now, in many cases the number of lines of definite wavelength
§ 84. Views of Wald and Ostwald.
Such modifications of the atomic theory as those we have briefly discussed above, although profoundly modifying, and, indeed, controverting the philosophical significance of Dalton's theory as originally formulated, leave its chemical significance practically unchanged. The atoms can be regarded no longer as the eternal, indissoluble gods of Nature that they were once supposed to be; thus, Materialism is deprived of what was thought to be its scientific basis.11 But the science of Chemistry is unaffected thereby; the atoms are not the ultimate units out of which material things are built, but the atoms cannot be decomposed by purely chemical means; the "elements" are not truly elemental, but they are chemical elements. However, the atomic theory has been subjected to a far more searching criticism. Wald argues that substances obey the law of definite
It should be noted, however, that if by the term "phlogiston" we were to understand energy and not some form of matter, most of the statements of the phlogistics would be true so far as they go.
In order that these laws may hold good, it is, of course, necessary that the substances are weighed under precisely similar conditions. To state these laws in a more absolute form, we can replace the term "weight" by "mass," or in preference, "inertia"; for the inertial of bodies are proportional to their weights, providing that they are weighed under precisely similar conditions. For a discussion of the exact significance of these terms "mass" and "inertia," the reader is referred to the present writer's Matter, Spirit and the Cosmos (Rider, 1910), Chapter I., "On the Doctrine of the Indestructibility of Matter."
The term "valency" is not altogether an easy one to define; we will, however, here do our best to make plain its significance. In a definite chemical compound we must assume that the atoms constituting each molecule are in some way bound together (though not, of course, rigidly), and we may speak of "bonds" or "links of affinity," taking care, however, not to interpret such terms too literally. Now, the number of "affinity links" which one atom can exert is not unlimited; indeed, according to the valency theory as first formulated, it is fixed and constant. It is this number which is called the "valency" of the element; but it is now known that the "valency" in most cases can vary between certain limits. Hydrogen, however, appears to be invariably univalent, and is therefore taken as the unit of valency. Thus, Carbon is quadrivalent in the methane-molecule, which consists of one atom of carbon combined with four atoms of hydrogen; and Oxygen is divalent in the water-molecule, which consists of one atom of oxygen combined with two atoms of hydrogen. Hence, we should expect to find one atom of carbon combining with two of oxygen, which is the case in the carbon-dioxide—(carbonic anhydride)—molecule. For a development of the thesis, so far as the compounds of carbon are concerned, that each specific "affinity link" corresponds in general to a definite and constant amount of energy, which is evolved as heat on disruption of the bond, the reader is referred to the present writer's monograph On the Calculation of Thermo-Chemical Constants (Arnold, 1909). The phenomena of valency find their explanation in modern views concerning the constitution of atoms (see § 81).
Since hydrogen is the lightest of all known substances, the unit, Hydrogen = 1, was at one time usually employed. However, it was seen to be more convenient to express the atomic weights in terms of the weight of the oxygen-atom, and the unit, Oxygen = 16 is now always employed. This value for the oxygen-atom was chosen so that the approximate atomic weights would in most cases remain unaltered by the change.
Hon. R. J. STRUTT: "On the Tendency of the Atomic Weights to approximate to Whole Numbers," Philosophical Magazine, [6], vol. i. (1901), pp. 311 et seq.
F W. ASTON: "Mass-spectra and Atomic Weights," Journal of the Chemical Society, vol. cix. (1921), pp. 677 et seq.
We have found Prof. Harry Jones' The Electrical Nature of Matter and Radioactivity (1906), Mr. Soddy's Radioactivity (1904), and Mr. Whetham's The Recent Development of Physical Science (1909) particularly interesting. Mention, of course, should also be made of the standard works of Prof. Sir J. J. Thomson and Prof. Rutherford.
For a critical examination of Materialism, the reader is referred to the present writer's Matter, Spirit and the Cosmos (Rider, 1910), especially Chapters I. and IV.