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(A) The total number of electrons in $CN^-$ is $6 + 7 + 1 = 14$.The total number of electrons in $CO$ is $6 + 8 = 14$.The total number of electrons in

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Bond order = $3$ and isoelectronic

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(A) The total number of electrons in $CN^-$ is $6 + 7 + 1 = 14$.The total number of electrons in $CO$ is $6 + 8 = 14$.The total number of electrons in $NO^+$ is $7 + 8 - 1 = 14$.Since all these species have $14$ electrons,they are isoelectronic.According to Molecular Orbital Theory,the bond order for a $14$-electron species is calculated as: $	ext{Bond Order} = \frac{1}{2}(N_b - N_a) = \frac{1}{2}(10 - 4) = 3$.Therefore,all these species have a bond order of $3$ and are isoelectronic.

What is the common feature among the species $CN^-$,$CO$,and $NO^+$?

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