BITSAT 2018 Paper

O2 : σ 1s2 , σ* 1s2 , σ2s2 , σ* 2s2 , σ 2pz2 , π2px2,π2py2 , π*2px1,π*2py1
Bond order =

10−6

2

= 2
(two unpaired electrons in antibonding molecularorbital)
O2+ : σ1s2 , σ*1s2 , σ2s2 , σ*2s2 , σ2pz2 , π2px62,π2py2 , π*2px1,π*2py0
Bond order =

10−5

2

= 2.5
(One unpaired electron in antibonding molecularorbital)
Hence O2 as well as O2+ both are paramagnetic,
and bond order of O2+ is greater than that of O2