(A) Moleculer orbital configuration of
C2 (12 electrons)
=σ1s2σ1s2*σ2s2σ2s2*π2px2=π2py2∴Na=4Nb=8∴‌‌BO=‌[8−4]=2 Here no unpaired electron present, so it is diamagnetic.
Moleculer orbital configuration of
C2+(11 electrons)
‌=σ1s2σ1s2*σ2s2σ2s2*π2px2=π2py1‌∴‌‌Na=4‌Nb=7‌∴‌‌BO=‌[7−4]=1.5Here 1 unpaired electron present, so it is paramagnetic.
(B) Moleculer orbital configuration of
N2 (14 electrons)
‌=σ1s2σ1s2*σ2s2σ2s2*π2px2=π2py2σ2pz2‌∴Na=4‌Nb=10‌∴‌‌BO=‌[10−4]=3 Here no unpaired electron present, so it is diamagnetic.
Moleculer orbital configuration of
N2+(13 electrons)
=σ1s2σ1s2*σ2s2σ2s2*π2px2=π2py2σ2pz1∴Na=4Nb=9∴‌‌BO=‌[9−4]=2.5 Here 1 unpaired electron present, so it is paramagnetic.
(C) Moleculer orbital configuration of NO (15 electrons) is
σ1s2σ1s2*σ2s2σ2s2*σ2pz2π2pz2=π2py2π2px1*=π2py0* ∴Na=5 Nb=10 ∴‌‌BO=‌[10−5]=2.5 Here is 1 unpaired electron, So it is paramagnetic.
Moleculer orbital configuration of
NO+(14 electrons) is
σ1s2σ1s2*σ2s2σ2s2*σ2pz2π2pz2=π2py2π2px0*=π2py0* ∴Na=4Nb=10∴‌‌BO=‌[10−4]=3 Here is no unpaired electron, So it is diamagnetic.
(D) Molecular orbital configuration of
O2 ( 16 electrons) is
σ1s2σ1s2*σ2s2σ2s2*σ2pz2π2px2=π2py2π2px1*=π2py1* ‌∴Na=6‌Nb=10‌∴‌‌BO=‌[10−6]=2Here 2 unpaired electrons present, so it is paramagnetic.
Molecular orbital configuration of
O2+(15 electrons) is
‌σ1s2σ1s2*σ2s2σ2s2*σ2pz2π2px2=π2py2π2px1*=π2pyo*‌∴‌‌Nb=10‌Na=5‌∴‌‌BO=‌[10−5]=2.5Here 1 unpaired electrons present, so it is also paramagnetic.