Mass Spectra and Isotopes: Francis W. Aston's Nobel Lecture on Atomic Weights and Isotopes, Lecture notes of Chemistry

Download Mass Spectra and Isotopes: Francis W. Aston's Nobel Lecture on Atomic Weights and Isotopes and more Lecture notes Chemistry in PDF only on Docsity! FRANCIS W. ASTON Mass spectra and isotopes Nobel Lecture, December 12, 1922 Dalton’s statement of the Atomic Theory, which has been of such incalcu- lable value in the development of chemistry, contained the postulate that "atoms of the same element are similar to one another, and equal in weight". The second part of this postulate cannot, in general, be tested by chemical methods, for numerical ratios are only to be obtained in such methods by the use of quantities of the element containing countless myriads of atoms. At the same time it is somewhat surprising, when we consider the complete absence of positive evidence in its support, that no theoretical doubts were publicly expressed until late in the nineteenth century. There are two methods by which the postulate can be tested experi- mentally, either by comparing the weights of the individual atoms, or al- ternatively by demonstrating that samples of an element can exist which though chemically identical yet have different atomic weights. The latter method, by which the existence of isotopes was first proved, has been fully dealt with in the previous lecture by Professor Soddy. The more direct method, with which this lecture is concerned, can be applied by means of the analysis of positive rays. The condition for the development of these rays is briefly ionization at low pressure in a strong electric field. Ionization, which may be due to col- lisions or radiation, means in its simplest case the detachment of one electron from a neutral atom. The two resulting fragments carry charges of electricity of equal quantity but of opposite sign. The negatively charged one is the electron, the atomic unit of negative electricity itself, and is the same what- ever the atom ionized. It is extremely light and therefore in the strong electric field rapidly attains a high velocity and becomes a cathode ray. The re- maining fragment is clearly dependent on the nature of the atom ionized. It is immensely more massive than the electron, for the mass of the lightest atom, that of hydrogen, is about 1,850 times that of the electron, and so will attain a much lower velocity under the action of the electric field. However, if the field is strong and the pressure so low that it does not collide with other atoms too frequently, it will ultimately attain a high speed in a direction 8 1 9 2 2 F . W . A S T O N opposite to that of the detached electron, and become a "positive ray". The simplest form of positive ray is therefore an atom of matter carrying a positive charge and endowed, as a result of falling through a high potential, with sufficient energy to make its presence detectable. Positive rays can be formed from molecules as well as atoms, so that it will at once be seen that any measurement of their mass will give us direct information as to the masses of atoms of elements and molecules of compounds, and that this information will refer to the atoms or molecules individually, not, as in chem- istry, to the mean of an immense aggregate. It is on this account that the accurate analysis of positive rays is of such importance. In the parabola method of analysis devised by Sir J. J. Thomson, the rays generated by means of an electric discharge, after reaching the surface of the cathode, enter a long and very fine metal tube. By this means a narrow beam of rays is produced which is subjected to deflection by electric and magnetic fields, and finally falls upon a screen of fluorescent material or a photographic plate. The fields are arranged so that the two deflections are at right angles to each other. If we call the displacement on the plate due to the electric field x and that due to the magnetic field y for any particle, (x, y) will be the rectangular coordinates of the point where it strikes the plate. Simple dynamics show that if the angle of deflection is small, for a particle of mass m , charge e and velocity V, the electric deflection x = k(Xe/mv2) and the magnetic deflection y = k’ ( He/mv) where X and H are the magnetic and electric fields, and k and k’ constants depending solely on the dimensions and form of the apparatus. Hence if both fields are on together, the locus of impact of all particles of the same e/m but varying velocity will be a parabola. Since e must be the electronic charge, or a simple multiple of it, measurement of the relative positions of the parabolas on the plate enables us to calculate the relative masses of the particles producing them, that is, the masses of the individual atoms. The fact that the streaks were definite, sharp parabolas, and not mere blurs, constituted the first direct proof that atoms of the same element were, even approximately, of equal mass. Many gases were examined by this method and some remarkable com- pounds, such as H2, discovered by its means. When in 1912 neon was in- troduced into the discharge tube, it was observed to exhibit an interesting peculiarity. This was that whereas all elements previously examined gave single, or apparently single, parabolas, that given by neon was definitely double. The brighter curve corresponded roughly to an atomic weight of 20, the fainter companion to one of 22, the atomic weight of neon being M A S S S P E C T R A A N D I S O T O P E S I I After emerging from the electric field the rays may be taken, to a first order of approximation, as radiating from a virtual source Z half-way through the field on the line S1S2. A group of these rays is now selected by means of the diaphragm D, and allowed to pass between the parallel poles of a magnet. For simplicity the poles are taken as circular, the field between them uniform and of such sign as to bend the rays in the opposite direction to the foregoing electric field. If θ and ϕ be the angles (taken algebraically) through which the selected beam of rays is bent by passing through fields of strength X and H, then and (1) (2) where I, L are the lengths of the paths of the rays in the fields. Eq. (I) is only true for small angles, but exact enough for practice. It follows that over the small range of θ selected by the diaphragm, θ v2 and V are constant for all rays of given e/m, therefore o, and o, so that when the velocity varies in a group of rays of given e/m. This equation appears correct within practical limits for large circular pole-pieces. Referred to axes OX, OY the focus is at r cos Y sin or r, so that to a first-order approximation, whatever the fields, so long as the position of the diaphragm is fixed, the foci will all lie on the straight line ZF drawn through Z parallel to OX. For purposes of construction, G the image of Z in OY is a convenient reference point, ϕ, being here equal to 4 '. It is clear that a photographic plate, indicated by the thick line, will be in fair focus for values of e/m over a range large enough for accurate com- parison of masses. Since it is a close analogue of the ordinary spectrograph and gives a <<spectrum>> depending upon mass alone, the instrument is called a <<mass spectrographs and the spectrum it produces a <<mass spectrum>>. Fig. 2 shows a number of typical mass spectra obtained by this means. The numbers above the lines indicate the masses they correspond to, on the 12 1922 F. W.ASTON scale O = 16. It will be noticed that the displacement to the right with increasing mass is roughly linear. The measurements of mass made are not absolute, but relative to lines which correspond to known masses. Such lines due to hydrogen, carbon, oxygen, and their compounds are generally pres- ent as impurities or purposely added, for pure gases are not suitable for the smooth working of the discharge tube. The two principal groups of these reference lines are the CI group due to C (12), CH (13), CH2 (14), CH3 (15), CH4 or O(16), and the C2 group (24 to 30) containing the very strong line C2H 4 or CO (28). These groups will be seen in several of the spectra reproduced, and they give, with the CO, line (44), a very good scale of reference. It must be remembered that the ratio of mass to charge is the real quantity measured by the position of the lines. Many of the particles are capable of carrying more than one charge. A particle carrying two charges will appear as having half its real mass, one carrying three charges as if its mass was one- third, and so on: Lines due to these are called lines of the second and third order. Lines of high order are particularly valuable in extending our scale M A S S S P E C T R A A N D I S O T O P E S 13 of reference. When neon was introduced into the apparatus, four new lines made their appearance at 10, 11, 20, and 22. The first pair are second-order lines and are fainter than the other two. All four are well placed for direct comparison with the standard lines, and a series of consistent measurements showed that to within about one part in a thousand the atomic weights of the isotopes composing neon are 20 and 22 respectively. Ten per cent of the latter would bring the mean atomic weight to the accepted value of 20.20, and the relative intensity of the lines agrees well with this proportion. The isotopic constitution of neon was therefore settled beyond all doubt. Spectrum I on the plate shows the first-order lines of neon and some of the reference lines with which they were compared. The element chlorine was naturally the next to be analysed, and the ex- planation of its fractional atomic weight was obvious from the first plate taken. Its mass spectrum is characterized by four strong first-order lines at 35, 36, 37, 38. There is no sign whatever of any line at 35.46. The simplest explanation of the group is to suppose that the lines 35 and 37 are due to the isotopic chlorines, and lines 36 and 38 to their corresponding hydrochloric acids. The elementary nature of lines 35 and 37 is also indicated by the second-order lines at 17.5, 18.5, and also, when phosgene was used, by the appearance of lines at 63, 65, due to CO35CI and CO37CI. Later it was found possible to obtain the spectrum of negatively charged rays. These rays are formed by a normal positively charged ray picking up two electrons. On the negative spectrum of chlorine only two lines, 35 and 37, can be seen, so that the lines at 36 and 38 cannot be due to isotopes of the element. These results, taken with many others which cannot be stated here in detail, show that chlorine is a complex element, and that its isotopes are of atomic weight 35 and 37. Spectra II, III, and IV show the results with chlorine taken with different magnetic field strengths. The mass spectrum of argon shows an exceedingly bright line at 40, with second-order line at 20, and third-order line at 135. The last is particularly well placed between known reference lines, and its measurement showed that the triply charged atom causing it, had a mass 40 very exactly. Now the accepted atomic weight of argon is less than 40, so the presence of a lighter isotope was suggested. This was found at 36, and has now been fully substantiated; its presence to the extent of about 3 per cent is sufficient to account for the mean atomic weight obtained by density determinations. The elements hydrogen and helium present peculiar difficulties, since their lines are so far removed from the ordinary reference scale, but, as the lines 16 1 9 2 2 F . W . A S T O N Table of elements and isotopes. Element Atomic Atomic number weight Minimum number of isotopes Masses of isotopes in order of intensity H 1 He 2 Li 3 Be 4 B 5 C 6 N 7 0 8 F 9 Ne 10 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 A 18 K 19 Ca 20 Fe 26 Ni 28 Zn 30 As 33 Se 34 Br 35 Kr 36 Rb 37 Sn 50 Sb 51 I 53 X 54 Cs 55 132.81 Hg 80 200.6 1.008 3.99 6.94 9.1 10.9 12.00 14.01 16.00 19.00 20.20 23.00 24.32 26.96 28.3 31.04 32.06 35.46 39.88 39.10 40.07 55.84 58.68 65.37 74.96 79.2 79.92 82.92 85.45 118.7 121.77 126.92 130.2 1 1 2 1 2 1 1 1 1 2 1 3 1 2 1 1 2 2 2 ( 1 ) (4) 1 6 2 6 7(8) 2 I 7(9) 1.008 4 7, 6 9 11, 10 12 14 16 19 20,22 23 24,25,26 27 28,29,(30) 31 32 35,37 40,36 39,41 40, 44 56,(54)? 58,60 64,66,68,70 75 80,78,76,82,77,74 79,81 84,86,82,83,80,78 85,87 120,118,116,124,119,117,122,(121) 121, 123 127 129,132,131,134,136,128,130,(126), (124) 133 (197-200),202,204 Numbers in brackets are provisional only. M A S S S P E C T R A A N D I S O T O P E S 17 but with the lighter elements the divergence from the whole number rule is extremely small. This enables the most sweeping simplifications to be made in our ideas of mass. The original hypothesis of Prout, put forward in 1815, that all atoms were themselves built of atoms of protyle, a hypothetical element which he tried to identify with hydrogen, is now reestablished, with the modification that the primordial atoms are of two kinds: protons and elec- trons, the atoms of positive and negative electricity. The Rutherford-Bohr atom consists essentially of a positively charged central nucleus around which revolve planetary electrons at distances great compared with the dimensions of the nucleus itself. As has been stated, the chemical properties of an element depend solely on its atomic number, which is the charge on its nucleus expressed in terms of the unit charge, e. A neutral atom of an element of atomic number N has a nucleus consisting of K + N protons and K electrons, and around this nucleus revolve N electrons. The weight of an electron on the scale we are using is 0.0005, so that it may be neglected. The weight of this atom will therefore be K + N, so that if no restrictions are placed on the value of K any number of isotopes are possible. A statistical study of the results given above shows that the natural restrictions can be stated in the form of rules as follows: In the nucleus of an atom there is never less than one electron to every two protons. There is no known exception to this law. It is the expresssion of the fact that if an element has an atomic number N the atomic weight of its lightest isotope cannot be less than 2N. Worded as above, the ambiguity in the case of hydrogen is avoided. True atomic weights corresponding exactly to 2N are known in the majority of the lighter elements up to 36A. Among the heavier elements the difference between the weight of the lightest isotope and the value 2N tends to increase with the atomic weight; in the cases of mercury it amounts to 37 units. The corresponding divergence of the mean atomic weights from the value 2N has of course been noticed from the be- ginning of the idea of atomic number. The number of isotopes of an element and their range of atomic weight appear to have definite limits - Since the atomic number only depends on the net positive charge in the nucleus, there is no arithmetical reason why an element should not have any number of isotopes. So far the largest number appears to be 9 in the case of xenon, which also shows the maximum difference between its lightest and heaviest isotopes, 18 1922 F. W.ASTON 12 units. The greatest proportional difference calculated on the lighter weight is recorded in the case of lithium, where it amounts to one-sixth. It is about one-tenth in the cases of boron, neon, argon, selenium, krypton, and xenon. No element of odd atomic number has more than two isotopes. The number of electrons in the nucleus tends to be even - This rule expresses the fact that in the majority of cases even atomic number is associated with even atomic weight, and odd with odd. If we consider the three groups of elements, the halogens, the inert gases and the alkali metals, this tendency is very strongly marked. Of the halogens - odd atomic numbers - all 6 (+ 1 ?) atomic weights are odd. Of the inert gases - even atomic numbers - 13 (+2?) are even and 3 odd. Of the alkali metals - odd atomic numbers - 7 are odd and 1 even. In the cases of elements of other groups the prepon- derance, though not so large, is still very marked. Beryllium and nitrogen are the only elements yet discovered to consist entirely of atoms whose nuclei contain an odd number of electrons. If we take the natural numbers 1 to 40, we find that those not represented by known atomic weights are 2, 3, 5, 8, 13, (17), (18), 21, (33), 34, (38). It is rather remarkable that these gaps, with the exception of the four in parentheses, are represented by a simple mathematical series of which any term is the sum of the two previous terms. In consequence of the whole- number rule there is now no logical difficulty in regarding protons and electrons as the bricks out of which atoms have been constructed. An atom of atomic weight m is turned into one of atomic weight m + 1 by the addi- tion of a proton plus an electron. If both enter the nucleus, the new element will be an isotope of the old one, for the nuclear charge has not been altered. On the other hand, if the proton alone enters the nucleus and the electron remains outside, an element of next higher atomic number will be formed. If both these new configurations are possible, they will represent elements of the same atomic weight but with different chemical properties. Such elements are called "isobases". It will be observed that the principal atomic species of argon and calcium are isobases, each having a weight 40. In the same manner no less than four seleniums form isobasic pairs with kryptons. In all such pairs known with certainty to exist, the elements concerned have even atomic numbers and even atomic weights, also one member of each pair is an inert gas. The whole-number rule is not to be supposed as mathematically exact, for al- though the atoms of all elements are made up of the same electrical units their masses will be affected slightly by the way in which these unit charges