Identify the incorrect statement from the following:

Core Logic

(1) Phosphorus and Arsenic possess vacant d-orbitals. They can act as π$\pi$-acceptor ligands, forming dπ-dπ$d\pi-d\pi$ backbonds with transition metals. (Correct) (2) Nitrogen (Period 2) does NOT possess vacant d-orbitals in its valence shell. Oxygen also does not have d-orbitals. Therefore, Nitrogen cannot form a dπ-pπ$d\pi-p\pi$ bond with oxygen. (Incorrect) (3) Nitrogen forms strong pπ-pπ$p\pi-p\pi$ multiple bonds with itself (e.g., in N ≡ N$N \equiv N$). (Correct) (4) Phosphorus, arsenic, and antimony exhibit catenation (e.g., P₄$P_4$), although to a lesser extent than carbon. (Correct)

Step 1: Final Conclusion

Statement (2) is incorrect because nitrogen lacks d-orbitals.

Pattern Recognition

Period 2 elements (Li, Be, B, C, N, O, F) NEVER form dπ-pπ$d\pi-p\pi$ bonds using their own d-orbitals because they do not have accessible 2d orbitals.

Chapter Mix

Class 12 Chemistry: The p-Block Elements Class 11 Chemistry: Chemical Bonding and Molecular Structure