molecular orbital

For example, the ground state energy level, 1s, splits into two molecular orbitals.

Molecular orbitals are said to be degenerate if they have the same energy.

The same analysis can be carried out for the molecular orbitals of cyclobutene.

It was a method for calculating the electronic energy and the molecular orbitals.

Group theory is also useful in studying the symmetry of molecular orbitals.

So, molecular orbitals are formed between the two atoms.

Six of these remaining electrons fill molecular orbitals "in the usual fashion".

Overlap is necessary for the formation of molecular orbitals.

Electronic structure describes the occupation of a molecule's molecular orbitals.

Molecular orbitals can either stabilize, destabilize, or have no effect on, the molecule.

This increased stability is due to the unique properties of aromatic molecular orbitals.

Molecular orbitals and vibrational frequencies are among the properties displayed.

A solid creates a large number of closely spaced molecular orbitals, which appear as a band.

The occupied molecular orbitals on the top are the 2 t orbitals.

Molecular orbitals allow chemists to apply quantum mechanics to study molecules.

Different molecular orbitals have different spatial distribution of the electron density.

However, the molecular orbitals of O are actually more complex than Lewis structures seem to suggest.

It is not incorrect to think of electrons in atomic or molecular orbitals as planets orbiting the Sun.

This in turn allows for a reduced band gap as the excited state molecular orbitals are delocalized.

Then, throughout the reaction, the symmetry of molecular orbitals with respect to this element must be conserved.

Specifically, the external magnetic field induces currents of the electrons in molecular orbitals.

In quantum chemistry, a complete active space is a type of classification of molecular orbitals.

Instead, multiconfiguration is achieved by using orthogonal molecular orbitals.

This delocalization "collapses" the molecular orbitals to a point that they absorb all light in the visible region.

The photochromic parts and metal parts are so close that they can affect each other's molecular orbitals.