Identify the incorrect statement from the following :

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 2s² 2p³ and that of oxygen is 2s² 2p⁴ . 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 N₂ ). Statement (2) is correct because ph