NEET2026ChemistryChapterActual
Due to its small size, high electronegativity, and the absence of d-orbitals in its valence shell, nitrogen exhibits anomalous properties compared to the heavier elements of Group 15. Which of the following statements regarding the bonding capabilities of Group 15 elements is correct?
Options
- ABismuth readily forms diatomic molecules ( Bi₂ ) in the solid state due to highly effective p - p overlapping.
- BNitrogen can act as a -acceptor ligand with transition metals by utilizing d - d bonding.
- CPhosphorus can form compounds such as R₃P=CH₂ by utilizing its d-orbitals to form d - p bonds.
- DThe maximum covalency of nitrogen is strictly limited to three because it possesses only three half-filled p-o
Correct answer
C. Phosphorus can form compounds such as R₃P=CH₂ by utilizing its d-orbitals to form d - p bonds.
Step-by-step solution
Heavier elements of Group 15, such as bismuth, do not form effective p - p bonds because their atomic orbitals are large and diffuse, resulting in poor overlap. Thus, bismuth does not readily form diatomic molecules with p - p bonds. Nitrogen lacks d-orbitals in its valence shell, so it cannot participate in d - d or d - p bonding. It acts as a -acceptor ligand using its ^ * antibonding orbitals, not d-orbitals. Phosphorus and other heavier elements of Group 15 possess vacant d-orbitals in their valence shell. They