Using molecular orbital theory, compare the bond energy and magnetic character of 0+2 and O–2

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The molecular electronic configuration of O2 molecule is KK σ2s2σ*2s2σ2pz2π2px2π2py2π*2px1π*2py1 In O2? one electron will enter in π*2px orbital and bond order will be= 8 – 5/2=3/2 In O2+ one electron will be removed from π*2py orbital and bond order will be...
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The molecular electronic configuration of O2 molecule is KK σ2s2σ*2s2σ2pz2π2px2π2py2π*2px1π*2py1 In O2? one electron will enter in π*2px orbital and bond order will be= 8 – 5/2=3/2 In O2+ one electron will be removed from π*2py orbital and bond order will be =8 -3/2 =5/2 Therefore the bond energy of O2+ will be greater than bond energy of O2?(because O2+ is having higher bond order). Both are having unpaired electrons therefore they are paramagnetic. read less
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