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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
All textbooksTro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblem 79
Chapter 10, Problem 79

According to MO theory, which molecule or ion has the highest bond order? C2, C2+ , C2- According to MO theory, which molecule or ion has the highest bond energy? According to MO theory, which molecule or ion has the shortest bond length?

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1
Identify the molecular orbitals (MOs) for each species: C_2, C_2^+, and C_2^-.
Determine the electron configuration for each species using the MO diagram for diatomic carbon species.
Calculate the bond order for each species using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.
Compare the bond orders to determine which species has the highest bond order, as bond order is directly related to bond energy and inversely related to bond length.
Conclude that the species with the highest bond order will have the highest bond energy and the shortest bond length.

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