Multiple Choice
According to molecular orbital theory, overlap of two p atomic orbitals produces which type of molecular orbitals?
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12. Molecular Shapes & Valence Bond Theory
Molecular Orbital Theory
Multiple Choice
Which of the following correctly describes the molecular orbital energy diagram for the diatomic molecule H_2?
A
Both electrons are unpaired and occupy separate atomic orbitals.
B
Two electrons occupy the bonding sigma_{1s} orbital, and the antibonding sigma_{1s}^* orbital remains empty.
C
Both electrons occupy the antibonding sigma_{1s}^* orbital.
D
One electron occupies the bonding sigma_{1s} orbital, and one electron occupies the antibonding sigma_{1s}^* orbital.
Verified step by step guidance1
Recall that the hydrogen molecule (H_2) consists of two hydrogen atoms, each contributing one 1s electron, for a total of two electrons.
Understand that when atomic orbitals combine to form molecular orbitals, the 1s orbitals combine to form a lower-energy bonding orbital (\(\sigma\)_{1s}) and a higher-energy antibonding orbital (\(\sigma\)_{1s}^*).
Apply the Aufbau principle to fill the molecular orbitals: electrons fill the lowest energy orbitals first, so both electrons will occupy the bonding \(\sigma\)_{1s} orbital before any occupy the antibonding \(\sigma\)_{1s}^* orbital.
Recognize that electrons tend to pair up with opposite spins in the same orbital, so the two electrons in the \(\sigma\)_{1s} bonding orbital will be paired.
Conclude that the correct molecular orbital configuration for H_2 is two electrons paired in the bonding \(\sigma\)_{1s} orbital, with the antibonding \(\sigma\)_{1s}^* orbital remaining empty.
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