Pentavalence in phosphorous is more stable when compared to that of nitrogen even though they belong to same group is due to

Options

A. reactivity of phosphorous
B. inert nature of nitrogen
C. dissimilar electronic configuration
D. larger size of phosphorus atom.

Answer

C

Explanation

Electronic configuration of nitrogen atom is `1s^(2)2s^(2)2p^(3)`. Only three unpaired electrons of p orbital take part in bonding so trivalence is stable in this case. Since there is no d orbital in second orbit pentavalence is not stable. Electronic configuration of phosphorus atom `1s^(2)2s^(2)2p^(6)3s^(2)2p^(3)3d^(0)`. It can use three unpaired electrons of 3p orbital to exhibit trivalence and also can use 3d orbital to exhibit pentavalency `[1s^(2)2s^(2)2p^(6)3s^(1)3p^(3)3d^(1)]`.