Abstract
Of course the hydrogen atom, discussed at length in Chapter Eleven, is a one-electron system, but it is not the only one. The ions He+ and Li2+ for example also possess one electron. It is appropriate to consider all such systems together, because their properties are similar. In many-electron atoms the picture, regrettably, is more complex, as electron-electron repulsion terms must be included in any expression for electron energy. It is only for one-electron systems that the energy-degeneracy of orbitals within a particular shell is retained (Figure 12.1). Not only are orbitals of (say) the 3-shell of higher energy than those of the 2-shell, but the ‘size’ of orbitals of the same type increases with energy. We have used the expression
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Further Reading
A L Companion, Chemical Bonding, McGraw-Hill, New York, 1979.
J R Dyer, Applications of Absorption Spectroscopy of Organic Compounds, Prentice-Hall, New Jersey, 1965.
H B Gray, Chemical Bonds, Benjamin-Cummings, California, 1973.
W Heitler, Elementary Wave Mechanics, Oxford University Press, Oxford, 1969.
R McWeeney, Coulson’s Valence, Oxford University Press, Oxford, 1979.
J N Murrell, S F A Kettle, and J M Tedder, The Chemical Bond, Wiley, Chichester, 1978.
L Pauling, The Chemical Bond, Oxford University Press, Oxford, 1967.
H S Pickering, The Covalent Bond, Wykeham Publications, London, 1977.
D H Williams and I Fleming, Spectroscopic Methods in Organic Chemistry, McGraw-Hill, London, 1973.
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© 1982 D. A. Robinson and J. McK. Woollard
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Robinson, D.A., Woollard, J.M. (1982). Atomic Structure. In: Chemistry for Colleges and Schools. Palgrave, London. https://doi.org/10.1007/978-1-349-04540-2_12
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DOI: https://doi.org/10.1007/978-1-349-04540-2_12
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