Explanation

(c)
In nitrogen $d$-orbitals are absent, so it does not form $NCl_{5}$. Thus,$NCl_{5}$ does not exist but $PCl_{5}$ does.
$Pb^{2 +}$ is more stable than $Pb^{4 +}$, due to inert pair effect.
In carbonate ion$\$($CO_{3}^{2 -}$ ) all the three $C - O$ bonds are identical due to resonance.
[image:11_image19.emf]
$O_{2}^{+}$(8+8-1=15)=$\sigma 1s^{2},\sigma*1s^{2},\ \sigma 2s^{2},\ \sigma*2s^{2},\ \sigma 2p_{s}^{2},\ \pi 2p_{y}^{2} \approx \pi 2p_{z}^{2},\begin{matrix}
* \\
\pi
\end{matrix}2p_{y}^{1}$
NO (7+8=15)
Hence, bo0th $O_{2}^{+}$ and $NO$ contains one unpaired electrons, so paramagnetic.