According to the Molecular orbital theory, diatomic oxygen should have σ(adsbygoogle = window.adsbygoogle || []).push({}); _{2px}(internuclear axis) and [itex]\pi[/itex]_{2py}and [itex]\pi[/itex]_{2pz}orbitals filled with two unpaired electrons, one at antibonding [itex]\pi[/itex]_{2py}and the other at antibonding [itex]\pi[/itex]_{2pz}. And of course, the 2s bonding and antibonding orbitals as well.

According to the molecular orbital theory, does this imply that diatomic oxygen possesses three "bonds" and one set of unpaired electrons, opposed to the double bond (sigma pi) implied by the valence bond theory?

Thank you.

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# Sigma and Pi Bonds for Diatomic Oxygen Molecule

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