non-bonding orbital technical
non-bonding molecular orbital technical

This state can be viewed as a chain of non-bonding orbitals.

The method is particularly efficient for alternant hydrocarbons in which the coefficients of the non-bonding orbitals involved are very easy to calculate.

Non-bonding orbitals are often designated by the letter n in molecular orbital diagrams and electron transition notations.

Non-bonding orbitals are the equivalent in molecular orbital theory of the lone pairs in Lewis structures.

The d, d and d orbitals remain non-bonding orbitals.

Although non-bonding orbitals are often similar to the atomic orbitals of their constituent atom, they do not need to be similar.

These are often divided into bonding orbitals, anti-bonding orbitals, and non-bonding orbitals.

The other three d orbitals in the basic model do not have significant interactions with the ligands and remain as three degenerate non-bonding orbitals.

The repulsive interaction should be proportional to the overlap integrals summed of non-bonding orbitals with exponential relationship:

In ordinary carbene, no π-MO-system is present, so the two non-bonding electrons can be placed in the two non-bonding orbitals on the carbon atom.

In coordination chemistry, a pi-donor ligand is a kind of ligand endowed with filled non-bonding orbitals that overlap with metal-based orbitals.

For transition metals, some classes of molecule tend to obey the 18-electron rule which corresponds to the utilization of valence-shell s, p and d orbitals to form bonding and non-bonding orbitals.

Electrons in non-bonding orbitals tend to be associated with atomic orbitals that do not interact positively or negatively with one another, and electrons in these orbitals neither contribute to nor detract from bond strength.

For example, there are two rigorously non-bonding orbitals that are occupied in the ground state of the hydrogen fluoride diatomic molecule; these molecular orbitals are localized on the fluorine atom and are composed of p-type atomic orbitals whose orientation is perpendicular to the internuclear axis.

Zigzag edges provide the edge localized state with non-bonding molecular orbitals near the Fermi energy.

Some orbitals (e.g. p and p orbitals from the fluorine in HF) may not have any other orbitals to combine with and become non-bonding molecular orbitals.

Non-Kekulé molecules with two formal radical centers (non-Kekulé diradicals) can be classified into non-disjoint and disjoint by the shape of their two non-bonding molecular orbitals (NBMOs).

This reduction of symmetry lifts the degeneracy of the two formerly non-bonding molecular orbitals, which by Hund's rule forces the two unpaired electrons into a new, weakly bonding orbital (and also creates a weakly antibonding orbital).