Which of the following pairs of species have the same bond order, but one is diamagnetic and the other is paramagnetic?

Step-by-step solution

The bond order (BO) and magnetic nature of the given species are evaluated using Molecular Orbital Theory: 1) O ₂²⁻ (18 e^- ): BO = 1, diamagnetic. F ₂ (18 e^- ): BO = 1, diamagnetic. Both have the same BO and both are diamagnetic. 2) O ₂^+ (15 e^- ): BO = 2.5, paramagnetic. N ₂^- (15 e^- ): BO = 2.5, paramagnetic. Both have the same BO and both are paramagnetic. 3) O ₂ (16 e^- ): BO = 2, paramagnetic (due to two unpaired electrons in ^ * 2p orbitals). C ₂ (12 e^- ): BO = 2, diamagnetic (all electrons are paired in