Q32Short answer
Using molecular orbital theory, compare the bond energy and magnetic + – character of O2 and O2 species.
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(i) According to molecular orbital theory electronic configurations of + – O2 and O2 species are as follows : O2 : (1s) (* 1s ) (2s) (* 2s ) (2pz) (2px2 , 2p2y ) (* 2px1 ) + 2 2 2 2 2 O2 : (1s) (* 1s ) (2s) (* 2s ) (2pz) (2p2x ,2p2y ) (* 2px2 , * 2py1) – 2 2 2 2 2 + 10 − 5 5 Bond order of O2 = = = 2.5 2 2 10 − 7 3 – Bond order of O2 = = = 1.5 2 2 + – Higher bond order of O2 shows that it is more stable than O2 . Both the species have unpaired electrons. So both are paramagnetic in nature.