Abstract
To better understand why hypervalent F, O, N, C, and B compounds are rarely stable, we carried out a systematic study of 28 systems, including anionic, cationic, and neutral molecules, held together by covalent, hypervalent, and noncovalent bonds. Molecular geometries, frequencies, atomic charges, electrostatic potentials, energy and electron densities, Mayer bond orders, local stretching force constants, and bond strength orders (BSOs) were derived from high accuracy CCSD(T) calculations and utilized to compare the strength and nature of hypervalent bonds with other types of bonds. All hypervalent molecules studied in this work were found to be either first-order transition states or unstable to dissociation, with F3- and OF3- as the only exceptions. For several systems, we found that a weak noncovalent bonded complex is more stable than a hypervalent one, due to the high energetic cost to accommodate an extra ligand, which can surpass the stability gained by 3c-4e bonding.
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