The species having bond order different from that in `CO` is

Options

A. `NO^(-)`
B. `NO^(+)`
C. `CN^(-)`
D. `N_(2).`

Answer

A

Explanation

The molecular orbital electronic configuration of all the species along their bond order is given as follows :
`CO : KK[sigma_(2s)]^(2)[sigma_(2py)^(**)]^(2)[pi_(2px)]^(2)[pi_(2py)]^(2)[sigma_(2py)]^(2),B.O. = 3.0`
`NO^(-)KK[sigma_(2s)]^(2)[sigma_(2s)^(**)]^(2)[pi_(2px)]^(2)[pi_(2pz)]^(2)[sigma_(2px)^(**)]^(2),B.O.=2.0`
`NO^(+),KK[sigma_(2s)]^(2)[sigma_(2s)^(**)]^(2)[pi_(2px)]^(2)[pi_(2py)]^(2)[sigma_(2py)^(**)],B.O.=3.0`
`CN^(-):KK[sigma_(2s)]^(2)[sigma_(2s)^(**)]^(2)[pi_(2px)]^(2)[pi_(2py)]^(2)[sigma_(2pz)^(**)]^(2),B.O.=3.0`
`N_(2):KK[sigma_(2s)]^(2)[sigma_(2px)^(**)]^(2)[pi_(2px)]^(2)[pi_(2py)]^(2)[sigma_(2pz)]^(2),B.O.=3.0`
Except for `NO^(-)` ion, all others have B.O. equal to 3.0