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Which of the following pairs of species has identical value of bond order?

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{NO}^{+}, N_{2}

CO

and

N_{2}^{+}

{CN}^{-}, O_{2}^{+}

N_{2}

and

O_{2}^{+}

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detailed solution

Correct option is A

Valence electrons of $N_{2} = 10$ Electronic Configuration $(σ 2 s)^{2} (σ * 2 s)^{2} {(π 2 p_{x})}^{2} {(π 2 p_{y})}^{2} {(σ 2 p_{z})}^{2}$

Bond order $= (8 - 2) / 2 = 3$

Valence electrons of ${NO}^{+} = 10 (σ 2 s)^{2} (σ * 2 s)^{2} {(π 2 p_{x})}^{2} {(π 2 p_{y})}^{2} {(σ 2 p_{z})}^{2}$

Bond order $= (8 - 2) / 2 = 3$

Valence electrons of $CO = 10$ ; Same as ${NO}^{+}$

Valence electrons of ${CN}^{-} = 10;$ Same as ${NO}^{+}$

Valence electrons of $N_{2}^{-} = 11$ Bond order $= (9 - 2) / 2 = 3.5$

Valence electrons of $O_{2}^{+} = 11$ Electronic configuration $(σ 2 s)^{2} (σ * 2 s)^{2} {(σ 2 p_{z})}^{2} {(π 2 p_{x})}^{2} {(π 2 p_{y})}^{2} {(π * 2 p_{x})}^{1}$

Bond order $= (8 - 3) / 2 = 2.5$

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