Nitrogen forms only NCl_3,whereas phosphorus | vedclass

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(A) Nitrogen belongs to the second period and has the electronic configuration $[He] 2s^2 2p^3$. It lacks $d$-orbitals in its valence shell,so it cann

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$P$ has $3d$ orbitals,while $N$ does not have $3d$ orbitals.

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(A) Nitrogen belongs to the second period and has the electronic configuration $[He] 2s^2 2p^3$. It lacks $d$-orbitals in its valence shell,so it cannot expand its octet to form $NCl_5$.Phosphorus belongs to the third period and has the electronic configuration $[Ne] 3s^2 3p^3$. It possesses vacant $3d$-orbitals,which allow it to undergo $sp^3d$ hybridization to form $PCl_5$ by expanding its octet.

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

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