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(A) The bond order of $CO$ ($14$ electrons) is $3$.$NO^{+}$ ($14$ electrons),$CN^{-}$ ($14$ electrons),and $N_2$ ($14$ electrons) are isoelectronic wi

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$NO^{-}$

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(A) The bond order of $CO$ ($14$ electrons) is $3$.$NO^{+}$ ($14$ electrons),$CN^{-}$ ($14$ electrons),and $N_2$ ($14$ electrons) are isoelectronic with $CO$,so they all have a bond order of $3$.$NO^{-}$ has $16$ electrons. Using the molecular orbital configuration: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$.Bond order $= \frac{1}{2} (N_b - N_a) = \frac{1}{2} (10 - 6) = 2$.Thus,$NO^{-}$ has a bond order of $2$,which is different from $CO$.

The species having a bond order different from that in $CO$ is

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