Choose the correct statement with respect to the bond length of CO and `CO^+` :

Options

A. The bond length in CO is 1.128 A and `CO^+` is 1.115 A because during conversion of CO to `CO^+`, electron is removed from anti bonding orbital.
B. The bond length in CO is 1.115 A and `CO^+` is 1.128 A because during conversion of CO to `CO^+` electron is removed from bonding orbital.
C. During conversion of CO to `CO^+` bond length does not vary because bond order remain same.
D. The bond length in CO is 1.115 A and `CO^+` is 1.1284 because bond order decreases during conversion of CO to `CO^+` .

Answer

A

Explanation

Because of the greater difference in electronegativity between C and O, the energy of the molecular orbitals in CO are in the following order,
`sigma_(1s)^(2) sigma_(1s)^(*2) sigma_(2s)^(2) [pi_(2p_(y))^(2) = pi_(2p_(x))^(2)] sigma_(2p_(x))^(2), sigma_(2s)^(*2)`
Bond order in `CO = 1/2(10-4)=3`

When CO is converted to `CO^+`, one electron is removed from antibonding molecular orbitals. Hence, the bond order in `CO^+` is greater than CO.