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 2p_z² π2p_x² = π 2p_y²π ^*2p_x¹

O₂^- (17): σ1s² σ ^*1s² σ 2s² σ ^*2s² σ 2p_z² π2p_x² = π 2p_y²π ^*2p_x²= π^*2p_y¹

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.