In case of nitrogen, NCI₃ is possible but not NCl₅ while in case of phosphorous, PCl₃ as well as PCl₅ are possible. It is due to

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lower tendency of H-bond formation in P than N.

availability of vacant d orbitals in P but not in N.

occurrence of P in solid while N in gaseous state at room temperature.

lower electronegativity of P than N.

answer is A.

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Detailed Solution

Both N and P are members of group-15 of the periodic table. N is the first member and has an electronic configuration $1 s^{2} 2 s^{2} 2 p^{3} .$ It forms a maximum of three bonds because its valency is 3. It has no vacant d orbitals, so it cannot extend its valency.

P is the second member of group 15 and its valance shell electronic configuration is $3 s^{2} 3 p^{3} .$ Its valency is 3, hence forms three bonds with neighboring atoms. But as P has vacant 3d orbitals, it can extend its valency. For instance, in PCl₃ (showing valency 3 of phosphorus) and PCl₅ (showing valency 5 of phosphorus).

Hence phosphorous can form pentahalides but nitrogen can not form pentahalides

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