The correct option is A (a−r,t)
(b−q,t)
(c−q,t)
(d−p,s)
Bond order:
B.O=12(bonding e−−antibonding e−)
Magnetic nature:
Unpaired e−⇒ Paramagnetic
Paired e−⇒ Diamagnetic
For O2−2
total number of electron =18
Molecular configuration:
σ1s2,σ∗1s2,σ2s2,σ∗2s2,σ2p2z,
π(2p2x=2p2y),π∗(2p2x=2p2y)
B.O=12(10−8)=1
all electrons are paired so nature of O2−2 is diamagnetic.
For He+2
total number of electrons =3
Molecular configuration:
σ1s2,σ∗1s1
B.O=12(2−1)=0.5
Paramagnetic nature.
For CO
total number of electron =14
Molecular configuration:
σ1s2,σ∗1s2,σ2s2,π(2p2x=2p2y),σ2p2z,σ∗2s2
B.O=12(10−4)=3
Diamagnetic in nature.
For NO+
total number of electrons =14
Molecular configuration:
σ1s2,σ∗1s2,σ2s2,σ∗2s2,π(2p2x=2p2y),σ2p2z
B.O=12(10−4)=3
Diamagnetic in nature.