Question

Bond order of N2+ N2, N2-

Answer 1

Bond Order=1/2[ nb-Na]
where 
nb= Number of electrons in bonding moleclar orbitals.
na=Number of Electrons in anti bonding molecular orbitals

Bond order Of N2:
Total number of electrons=14
Electronic Configuration σ1s²  σ*1s²  σ2s²  σ*2s²  π2py²  [π2pz²  σ2px² ]
Therefore,
Bond Order=10-4/2=6/2=3
So nitrogen molecule has triple bond.

Bond Order of N2⁺:
Total number of electrons:13
Electronic Configuration=:σ1s²  σ*1s²  σ2s²  σ*2s²  π 2py² [π2pz²  σ2px1 ]
Bond Order=[9-4]/2=5/2=2.5

Bond order of N2⁻:
Total number of electrons =15
Bond order=10-5/2=2.5

Answer 2

Answer:

Explanation:

Bond Order=1/2[ nb-Na]

where 

nb= Number of electrons in bonding moleclar orbitals.

na=Number of Electrons in anti bonding molecular orbitals

Bond order Of N2:

Total number of electrons=14

Electronic Configuration σ1s²  σ*1s²  σ2s²  σ*2s²  π2py²  [π2pz²  σ2px² ]

Therefore,

Bond Order=10-4/2=6/2=3

So nitrogen molecule has triple bond.

Bond Order of N2⁺:

Total number of electrons:13

Electronic Configuration=:σ1s²  σ*1s²  σ2s²  σ*2s²  π 2py² [π2pz²  σ2px1 ]

Bond Order=[9-4]/2=5/2=2.5

Bond order of N2⁻:

Total number of electrons =15

Bond order=10-5/2=2.5