NEET Chemistry Question (2026) — Solution

Step-by-step solution

Nitrogen and oxygen both belong to the second period of the periodic table. The valence shell electronic configuration of nitrogen is 2s^ 2 2p^ 3 and that of oxygen is 2s^ 2 2p^ 4 . Since the principal quantum number is n=2 for both elements, they do not have vacant d-orbitals in their valence shells. Therefore, nitrogen cannot form d -p bonds with oxygen. They can only form p -p multiple bonds. Statement (1) is correct as nitrogen forms p -p multiple bonds with itself (e.g., in N_ 2 ). Statement (2) is correct because phosphorus and arsenic have vacant d-orbitals and can act as -acceptor ligands, forming d -d back-bonds with the filled d-orbitals of transition metals. Statement (3) is correct as phosphorus, arsenic, and antimony exhibit the property of catenation. Thus, the incorrect statement is (4). Answer: Nitrogen can form d -p bond with oxygen.