(10−5)=2.5,and paramagnetic due to one unpaired electron. O2−(17e−s):
1s2σ*1s2σ2s2σ*2s2σ2pz2π2px2=π2py2π*2px2=π*2py1
Bond order =
1
2
(10−7)=1.5 and paramagnetic due to one unpaired electron. Therefore,both O2+ and O2− are paramagnetic and O2+ have higher bond order than O2− Also, O2− is less stable.