Question

The anomalous behavior of Nitrogen is due to_________.

• A. Ease Of Multiple Bond Formation
• B. Small Size And High Electronegativity.
• C. Non-availability Of D-orbitals In The Valence Shell.
• D. All Of These.

Answer 1

The correct option is D

All Of These.

1. Group 15 element-Nitrogen has an electronic configuration $2{\mathrm{s}}^2,2{\mathrm{s}}^2,2{\mathrm{p}}^3.$ It has three or five valence electrons because it can bond in outer 2p or 2s orbitals.
2. Molecular nitrogen is stable because it can form strong π bonds.
3. Nitrogen can also form triple bonds stronger than double bonds. because lone pair to lone pair repulsion is minimized.
4. Unlike the elements in group 15, nitrogen shows anomalous behavior due to Nitrogen's high electronegativity.

Hence, Option(D) is correct option.