Answer:
Option B
Explanation:
To identify the magnetic nature we need to check the molecular orbital configuration. If all orbitals are fully occupied, species is diamagnetic while when one or more molecular orbitals is/are singly occupied , species is paramagnetic
(a) NO(7+8=15)−σ1s2,σ∗1s2,σ2s2,σ∗2s2,π2p2x
=π2p2y,π2p2z,π∗2p1x =π∗2p0y
One unpaired electron is present.
Hence , it is paramagnetic
(b) CO(6+8=14)−σ1s2,σ∗1s2,σ2s2,σ∗2s2,π2p2x
=π2p2y,σ2p2z
No unpaired electron is present
Hence , it is diamagenetic
(c) O2(8+8=16)−σ1s2,σ∗1s2,σ2s2,σ∗2s2,σ2p2z,π2p2x
=π2p2x,π∗2p1x =π∗2p1y
Two unpaired electrons are present. Hence it is paramagnetic
(d) B2(5+5)−σ1s2,σ∗1s2,σ2s2,σ∗2s2,π2p1x
=π2p2x,π∗2p1x
=π2p1y
Two unpaired electrond are present. Hence it is paramagnetic