nonbonding

These complexes utilize either the triple bond or the nonbonding electrons on P.

The nonbonding electrons on sulfur are delocalized into the π-system.

The frontier orbitals are at a higher energy level than the bonding and nonbonding MOs.

Furthermore the t nonbonding metal orbitals are unaltered.

One of the three equatorial positions is occupied by a nonbonding lone pair of electrons.

When a nonbonding pair of electrons, a lone pair, occupies space, chirality can result.

Filling up these orbitals gives two stabilizing and two nonbonding orbitals.

These are called "bonding," "antibonding," and "nonbonding" MOs, respectively.

The molecules' bonding and nonbonding MOs should be filled and the antibonding MOs empty.

This segment is longer in other bonding animals (such as humans), and shorter in other nonbonding animals (such as chimpanzees).

Oxygen has 6 valence electrons and prefers to share two electrons in bonding with carbon, leaving the remaining 4 nonbonding electrons in 2 lone pairs.

The number of atoms bonded to a central atom plus the number of lone pairs of its nonbonding valence electrons is called its steric number.

These orbitals can be combined into two sp nonbonding orbitals, equivalent to each other, which can be compared to the lone pairs of VSEPR theory.

In mainstream chemistry close proximity of two nonbonding atoms leads to destabilizing steric repulsion but in QTAIM the observed hydrogen hydrogen interactions are in fact stabilizing.

Furthermore, the carbon atom in a carboxamide has a low lying LUMO that is capable of accepting electron density from the nonbonding lone pair on the nitrogen, weakening the carbon-oxygen bond.

Pauling also considered the nature of the interatomic forces in metals, and concluded that about half of the five d-orbitals in the transition metals are involved in bonding, with the remaining nonbonding d-orbitals being responsible for the magnetic properties.

Carbyne molecules are generally found to be in electronic doublet states: the nonbonding electrons on carbon are arranged as one radical (unpaired electron) and one electron pair, leaving a vacant atomic orbital, rather than being a tri-radical (the quartet state).

A bonding electron pair is involved in a sigma bond with an adjacent atom, and, being shared with that other atom, lies farther away from the central atom than does a nonbonding pair (lone pair), which is held close to the central atom by its positively-charged nucleus.