Chemistry - CHEMICAL BONDING Question with Solution | TestHub

Electronic configurations and bond orders of O₂⁺, O₂⁻, and H₂⁻ are:

O₂⁺: $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\sigma }_{2p_z}{)}^2({\pi }_{2p_x}{)}^2({\pi }_{2p_y}{)}^2({\pi }_{2p_x}^{\ast }{)}^1$

Bond Order (B.O.) = $\frac{1}{2}[10-5]=2.5$

O₂⁻: $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^2({\sigma }_{2s}{)}^2({\sigma }_{2s}^{\ast }{)}^2({\sigma }_{2p_z}{)}^2({\pi }_{2p_x}{)}^2({\pi }_{2p_y}{)}^2({\pi }_{2p_x}^{\ast }{)}^2({\pi }_{2p_y}^{\ast }{)}^1$

Bond Order (B.O.) = $\frac{1}{2}[10-7]=1.5$

H₂⁻: $({\sigma }_{1s}{)}^2({\sigma }_{1s}^{\ast }{)}^1$

Bond Order (B.O.) = $\frac{1}{2}[2-1]=0.5$