Chemical Bonds and Bond Energy by R. T. Sanderson

By R. T. Sanderson

Chemical Bond actual Chemistry sequence

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For this reason alone, we do not expect an electron freely to join a proton to form a neutron, despite the strong coulombic attraction between the opposite charges. Furthermore, we know 26 Atomic Structure 27 enough about nuclear energy to realize that destruction of a proton by absorption of an electron would also upset the very strong interactions among the nucleons which allow the close proximity of like-charged protons despite their mutual repulsions. One might then imagine an alternative arrangement of positive and negative charge that would minimize the energy without requiring actual coalescence of the charges.

Summary and Comments 25 (3) For binary compounds, an accurate method of calculating bond length as the sum of the radii of the two atoms, adjusted for partial charges. (4) A quantitative description of polar covalence. A polar covalent bond can be treated as a blend of nonpolar covalence and ionicity and its energy as the sum of separately calculated contributions, partial charges being indispensable in deter­ mining the blending coefficients. (5) Multiplicity factors that permit converting single bond energy to the bond energy of a multiple bond.

It must be pointed out that even if they are derived from meaningful values of τι, the proportionality constants C are only empirically determined. If the values 2. Significant Atomic Properties of the Chemical Elements Fig. 2-3 Relationship of homonuclear bond energy to rS product. 6 R. T. Sanderson, /. Inorg. Nucl Chem. 28, 1553 (1966). Or ύc = Atomic Properties 45 of C are assumed correct, or at the least, self-consistent, then of course the relationship Ε = CrS allows a semiexperimental determination of the electronega­ tivity, since both the radius and the bond energy are experimental quantities.

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