Nitrogen forms NCl_3 whereas phosphorus forms | vedclass

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(A) Nitrogen has an electronic configuration of $1s^2 2s^2 2p^3$. It lacks $d$-orbitals in its valence shell $(n=2)$,so it cannot expand its octet to

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$P$ has orbitals that can be used in bonding,but $N$ does not have $3d$ orbitals in its valence shell.

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(A) Nitrogen has an electronic configuration of $1s^2 2s^2 2p^3$. It lacks $d$-orbitals in its valence shell $(n=2)$,so it cannot expand its octet to form $NCl_5$.Phosphorus has an electronic configuration of $[Ne] 3s^2 3p^3$. It possesses vacant $3d$-orbitals,which allow it to undergo $sp^3d$ hybridization to form $PCl_5$.

Nitrogen forms $NCl_3$ whereas phosphorus forms both $PCl_3$ and $PCl_5$. Why?

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