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In which of the following ionization processes, the bond order has increased and the magnetic behaviour has changed?

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C_{2} \to C_{2}^{+}

NO \to {NO}^{+}

O_{2} \to O_{2}^{+}

N_{2} \to N_{2}^{+}

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detailed solution

Correct option is B

The order of increasing energy of molecular orbitals is

$(σ 2 s) (σ^{*} 2 s) (π 2 p_{x}) (π 2 p_{y}) (σ 2 p_{z}) (π^{*} 2 p_{x}) (π^{*} 2 p_{y}) (σ^{*} 2 p_{z})$

The valence electrons in $C_{2}, NO, O_{2}$ and $N_{2}$ are 8, 11, 12 and 10, respectively. The given criteria is satisfied only by $NO$ . Its configuration is

$(σ 2 s)^{2} (σ * 2 s)^{2} {(π 2 p_{x})}^{2} {(π 2 p_{y})}^{2} {(σ 2 p_{2})}^{2} {(π^{*} 2 p_{x})}^{1}$

In converting $NO to NO +$ , the electron is removed from antibonding molecular orbital and the resultant ion possesses no unpaired of electrons.

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