Abstract
Atoms may bind together according to the quantal structure of their single-electron energy shells. Electrons in the valence upper shells participate in the chemical bond, leaving behind a background of positive ions. The hole density of the ionic background is given, in its most general pair-wise form, by
where χ ia (r) = χ a (r - Ri is the a-th atomic-like orbital of the i-th ion placed at R i , c s ia are the coefficients of the s-th linear combination of atomic-like orbitals, and β s is the content of the chemical-bond orbital Φ s in the molecular-like orbital ψ s ; ψ s = α s ϕ s + β s Φ s , ϕ s = ∑ ia c s ia χ ia , α 2 s + β 2 s = 1. Averaging out the c s ia -coefficient in (1), and in virtue of the orthogonality of the eTa-matrix, one gets the ionic density
hence, the total number of electronic holes of the ionic background is given by
where z i is the nominal valence of the i-th atom. One can see that each ion participate in the chemical bond with an effective valence
smaller than the nominal valence z i ; and the same is true for each valence atomic-like orbital ia.
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Cune, L.C., Apostol, M. (2002). Atomic Clusters. In: Graja, A., Bułka, B.R., Kajzar, F. (eds) Molecular Low Dimensional and Nanostructured Materials for Advanced Applications. NATO Science Series, vol 59. Springer, Dordrecht. https://doi.org/10.1007/978-94-010-0349-0_21
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DOI: https://doi.org/10.1007/978-94-010-0349-0_21
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