Discussion Forum



1)

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 in N

B) lower electronegativity of P than N

C) lower tendency of H-bond formation in P than N

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

Answer:

Option A

Explanation:

$_{7}N = 1s^{2} 2s^{2} 2p^{3}; _{15}P =1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{3}$

In phosphorous the 3d-orbitals are available. Hence phosphorus can form pentahalides also but nitrogen cannot form pentahalide due to absence of d-orbitals