Using molecular orbital theory, compare the bond energy and magnetic character of O+2 and O-2 species.
The Molecular Orbital configuration of O2+ and O-2 is given below:
O2+ (15): σ1s2 σ *1s2 σ 2s2 σ *2s2 σ 2pz2 π2px2 = π 2py2π *2px1
O2- (17): σ1s2 σ *1s2 σ 2s2 σ *2s2 σ 2pz2 π2px2 = π 2py2π *2px2= π*2py1
Bond order for O2+
Bond order for O-2 
According to Molecular Orbital Theory, the greater the bond order greater is the bond energy.
Thus, O2+ is more stable than O-2.
Both of the ions have unpaired electrons. Thus, they will be paramagnetic in nature.
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