Question

Identify the incorrect statement.

• A. \( \text{PEt}_3 \) and \( \text{AsPh}_3 \) as ligands can form \( d\pi \)-\( d\pi \) bond with transition metals
• B. The \( \text{N} - \text{N} \) single bond is as strong as the \( \text{P} - \text{P} \) single bond
• C. Nitrogen has unique ability to form \( p\pi \)-\( p\pi \) multiple bonds with nitrogen, carbon and oxygen
• D. Nitrogen cannot form \( d\pi \)-\( p\pi \) bond as other heavier elements of its group

Answer 1

The Correct Option is B

Let's examine each statement:
1. PEt$_3$ and AsPh$_3$ can form d$\pi$-d$\pi$ bonds: PEt$_3$ (triethylphosphine) and AsPh$_3$ (triphenylarsine) are ligands that can act as $\pi$-acceptors. The phosphorus or arsenic atom in these ligands has empty d orbitals that can accept electron density from the filled d orbitals of transition metals, forming d$\pi$-d$\pi$ backbonds. This is a correct statement.
2. N-N single bond strength: The N-N single bond is considerably weaker than the P-P single bond. This weakness is due to the lone pair repulsion between the nitrogen atoms. The lone pairs on the relatively small nitrogen atoms are close enough to experience significant repulsion, weakening the N-N single bond. Phosphorus atoms are larger, and their lone pairs are further apart, resulting in less repulsion and a stronger P-P bond. Therefore, statement (2) is incorrect.
3. Nitrogen's p$\pi$-p$\pi$ multiple bonds: Nitrogen readily forms p$\pi$-p$\pi$ multiple bonds with itself (N$_2$), carbon (C$\equiv$N, CN), and oxygen (N=O). This is a key aspect of nitrogen chemistry and is a correct statement.
4. Nitrogen's d$\pi$-p$\pi$ bonding: Nitrogen does not have accessible d orbitals in its valence shell. Therefore, it cannot form d$\pi$-p$\pi$ bonds, unlike heavier elements in its group (phosphorus, arsenic, etc.) which have d orbitals available. This is a correct statement.