By Professor Dr. Boris K. Vainshtein, Professor Dr. Vladimir M. Fridkin, Professor Dr. Vladimir L. Indenbom (auth.)
Structureof Crystals describes the appropriate and genuine atomic constitution of crystals in addition to the digital constructions. the basics of chemical bonding among atoms are given, and the geometric representations within the concept of crystal constitution and crystal chemistry, in addition to the lattice power, are thought of. the real sessions of crystal buildings in inorganic compounds in addition to the constructions of polymers, liquid crystals, organic crystals, and macromolecules are handled. This version is complemented with fresh facts on many sorts of crystal buildings - e.g., the constitution of fullerenes, high-temperature superconductors, minerals, and liquid crystals.
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Extra info for Modern Crystallography 2: Structure of Crystals
In the former, the twoelectron orbitals are all used up, but there are also electrons residing outside them. The bond in these compounds is comparatively weak. Electron-deficient compounds (typical examples are boranes) do not have a sufficient number of electrons to form two-electron orbitals, but here, too, covalent interaction is still possible. 5 Molecular-Orbital (MO) Method This is the basic method in modern quantum chemistry. , are single centered. One can, however, proceed from a more general assumption and consider the orbitals of one electron in the field of all the nuc1ei making up the molecule (or crystal) - multicenter single-electronfunctions - and then take into account the interaction of such orbitals.
The energy of the ionic component is approximately 30· AiN kcal/mol. 8,9]). In this approach the electronegativity Xis expressed as one-half of the sum of the ionization potential and the attractive energy X = (1+ + r)j2. 19) can be correlated by a certain normalization. 20) which contains the corresponding values for cations and anions. According to Fig. 13. Electron density of a' NaCI crystal. 10] 22 1. 18. The physical characteristic describing the ionic contribution to the bond is the effective charge of the ion Z'.
We emphasize once more that the scheme of superposition of the radial functions (Fig. 14) indicates only the site ofthe overlapping ofthe orbitals. The picture of ionization and cation-anion contacts is schematized in Fig. 15. On p(r) maps obtained by X-ray analysis (Figs. 13, 14), the "border" of the Cl atom corresponds to the site of the overlapping of the maxima of the radial functions, while the region of low p(r) lies between the outer shells of the ions Na + and CI- and is determined by the values of t\Na (Fig.