My general understanding of Molecular Orbitals is as follows:(adsbygoogle = window.adsbygoogle || []).push({});

N atoms come together to form N molecular orbitals.

N/2 of the orbitals will be spatially asymmetric with symmetric spins.This corresponds to the antibonding orbital.

N/2 will be spatially symmetric with antisymmetric spins. This corresponds to the bonding orbital..

Each bonding orbital can contain a maximum of 2 electron with opposite spins.

Each antibonding orbital can either be empty or contain 1 electron since parallel spins in the same state are not allowed and with opposite spins the overall orbital would be symmetric which is not allowed for a fermion.

Excited electron can move to both higher energy bonding and antibonding orbitals as long as the Pauli Exclusion principle is not violated.

Is this the correct interpretation (particularly the last paragraph)?

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# Molecular Orbitals

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