Correct option is (B) 2
Oxygen molecule (\(O_2\)): Each oxygen atom has 8 electrons. Hence, \(O_2\) molecule has a total of 16 electrons. The electronic configuration of \(O_2\) molecule therefore is:
\(O_2:(\sigma1s)^2(\sigma*1s)^2(\sigma2s)^2(\sigma∗2s)^2(\sigma2p_z)^2(\pi2p_x)^2=(\pi2p_y)^2(\pi∗2p_x)^1=(\pi∗2p_y)^1\)
As we can see from the above electronic configuration, there are two unpaired electrons in the antibonding molecular \(\pi\)-orbital which leads to oxygen exhibiting paramagnetic properties.
