The Periodic Tables of Mendeleev
- Mendeleev's publications reveal several different forms of his Periodic Table
- There are many ways of arranging the elements to give Tables of different appearance but they must all follow Mendeleev's System
In this second celebratory article on Mendeleev, we witness how he corrected the atomic weights of In, Ce and U, and thus constructed the remarkable Periodic Table of 1871. Michael Laing
The giant Periodic Table on the Wall of the Bureau of Weights and Measures in St Petersburg
© Gordon Woods
What is important is that the Periodic Tables of 1869 and of 1871 are totally different in appearance.1 Figure 1 shows his Table of 1869. The elements are ordered on atomic weight with 'Groups' running horizontally, eg Li, Na, K, Rb and Cs. H stands alone. The elements In, Ce and Ur are positioned according to their wrong atomic weights; and there are gaps for the yet-to-be discovered elements with atomic weights of 45, 68 and 70. Here Mendeleev is certain. But he has problems with the heavy metals. Hg and Au are wrongly placed, as are Tl and Pb. It is the robust +1 and +2 oxidation states of these latter two elements that prompted him to put them below Cs and Ba respectively.
A change in layout
By 1871, the layout had changed to vertical Groups, and the elements In, Ce, and U are in their corrected positions.2(see Fig 2). There are gaps for elements of atomic weights 44, 68 and 72, and 100 (to become technetium in 1940). Now the vertical Groups contain two families linked by a common oxidation state, eg Group II - Be, Mg, Zn, Cd and Hg, and Ca, Sr and Ba. This is different from the arrangement of 1869 where the family Be to Cd is distant from Ca to Ba. We also notice that the elements Cu, Ag and Au are duplicated in Group I and Group VIII, bracketed in Group I. Hg is now correctly placed below Cd, and Au is below Ag. The atomic weights of Os and Ir are marked with '?'. Chemically they are correctly placed below Ru and Rh - it is their atomic weights that are in doubt.
By 1886 the three missing elements Sc, Ga and Ge had been found, and the inert gases were isolated in the 1890s. The Periodic System now showed its power and flexibility. It allowed the incorporation of these new mysterious gaseous elements as Group 0, after Group VII, the halogens, and before Group I. This is shown in Fig 3, a Table from the 1905 edition of Mendeleev's textbook, Osnovy ximii.3
The Group of inert gases is nicely separated to the left. There is a well-defined gap for an element of atomic weight 99, and a series of gaps for elements that will eventually become the lanthanides. (Mendeleev in a footnote to this Table comments on the difficulty that he has with placing those few which have been unequivocally identified.) The radioactive elements Rd, Th and U are correctly placed, with gaps for missing elements in horizontal row 12. Cu, Ag, and Au are still duplicated. There is a feeling of complete certainty all the way through to row 8, and again for the series Au to Bi in row 11. However, Mendeleev also offers a 'Groups horizontal' Table, shown as Fig 4.
Fig 2 The 1871 Table
We see here the Group 0 gases duplicated at top and bottom. The atomic weights in each vertical column increase down, and if the Table is rotated 90 degrees, it looks very much like a typical post-1950 Table, except that the atomic weights now increase from right to left, egthe series Ar, K, Ca to Se, Br and Kr. This arrangement with a continuous series in a column makes it obvious that the series Os to Bi is related to Ru to Sb and to Fe to As. Fe, Co, Ni head Group VIII (misprinted VII). He to Ne and Ne to Ar are labelled 'Typical Elements'. Here are two arrangements that seem to be totally different, both from the discoverer of the Periodic Law, but both follow the System.4
A closer look at the Table in Fig 4 shows that Ar = 38 has a superscript, as also does Ni = 59 and J (iodine) = 127. In the accompanying text Mendeleev says that these figures must be the correct atomic weights to fit into the System because these elements must obey the Periodic Law. He has a major philosophical problem and is in a scientific dilemma. In fact, the atomic weights (which he will not accept) had been accurately determined and showed that the orders Ar/K, Co/Ni, Te/J should be reversed (!) contrary to any chemical criteria. Only with the discovery of atomic number, the neutron and isotopes (many years after the death of Mendeleev) was this difficulty overcome.
The numbered rows in Fig 3 (and on the memorial Table in St Petersburg) are exactly that - rows, the Russian term ryadi. The numbering of Periods in our current Periodic Table is based upon the principal quantum number, n, and is accepted internationally. This did not exist when Mendeleev chose his labels. His rows (ryadi) 6 and 7 (in Fig 3 and the St Petersburg Table) correspond to today's Period 5, except for Kr included and Xe omitted. In 1871 (Fig 2) he used the term Typical Elements for the line Li to F, and Second Period (rows 3 and 4) for (Cu) to Br, Rb to Ag, with our Groups 7 and 1 in the middle of the series. This use of Period was gone from the 1905 and 1934 Tables.
Fig 3 A 1905 version of the Table
Many Tables but one System
One must not be blinkered and believe that there is only one perfect Periodic Table. This is not true. There are many ways of arranging the elements to give Tables of different appearance6-8- but all arrangements must obey the System of chemically similar elements being adjacent, either vertically or horizontally. Mendeleev shows this quite clearly, see Fig 3 and Fig 4. He was quite satisfied with both of these two alternative arrangements, otherwise he would not have published them in his book.
Fig 4 A 'Groups horizontal' version, 1905
In fact there exist two rough drafts of his first 'System of the Elements'.9 In one, the elements are ordered on atomic weight increasing upwards, while in the second they are ordered on atomic weight increasing down-
wards (Fig 5). This draft manuscript ultimately became in 1869 his first published Periodic Table.
Michael Laing is emeritus professor of inorganic chemistry, University of Natal, RSA. He can be contacted at 61 Baines Road, Durban 4001, Republic of South Africa (e-mail: email@example.com).
1. B. V. Nekrasov, Osnovy obshchei ximii, Vol 1, p 215-216. Moscow: Izdastyelstvo ximiya, 1969.
2. M. Laing, Educ. Chem., 2006, 43(1), 22.
3. D. Mendeleev, Osnovy ximii, Vol 1, 10th edn, p XXXIV and XXXV. Moscow: Gosudarstvennoe Nauchno Izdastyelstvo, 1931.
4. M. Laing, Educ. Chem., 2004, 41(1), 28.
5. M. Laing, Foundations of Chem., 2005, 7, 203.
6. E. Scerri, Educ. Chem., 2005, 42(65), 135.
7. P. J. Stewart, Educ. Chem., 2004, 41(6), 156.
8. P. G. Nelson, Educ. Chem., 1995, 32(6), 149; ibid,1987, 24(6), 171.
9. V. A. Krotikov, J. Chem. Educ., 1960, 37, 625.