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.