In case of nitrogen, NCl3 is possible but not NCl5 while in case of phosphorus, PCl3 as well as PCl5 are possible. It is due to

Question

In case of nitrogen, NCl3 is possible but not NCl5 while in case of phosphorus, PCl3 as well as PCl5 are possible. It is due to (A) availability of vacant d orbitals in P but not inN (B) lower electronegativity of P than N (C) lower tendency of H-bond formation in P thanN (D) occurrence ofP in solid while N in gaseous state at room temperature.

Tardigrade Admin · Accepted Answer

7N= 1s2 2s2 2p3; 15P = 1s2 2s2 2p6 3s2 3p3 In phosphorous the 3J-orbitals are available. Hence phosphorus can form pentahalides also but nitrogen cannot form pentahalide due to absence of d-orbitals.

Q. In case of nitrogen, $NC l_{3}$ is possible but not $NC l_{5}$ while in case of phosphorus, $PC l_{3}$ as well as $PC l_{5}$ are possible. It is due to

availability of vacant d orbitals in P but not inN

lower electronegativity of P than N

lower tendency of H-bond formation in P thanN

occurrence ofP in solid while N in gaseous state at room temperature.

$_{7} N = 1 s^{2} 2 s^{2} 2 p^{3};_{15} P = 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$
In phosphorous the $3 J$ -orbitals are available. Hence phosphorus can form pentahalides also but nitrogen cannot form pentahalide due to absence of d-orbitals.

Q. In case of nitrogen, NCl3​ is possible but not NCl5​ while in case of phosphorus, PCl3​ as well as PCl5​ are possible. It is due to