Question

Consider the statements. (A) \( \text{N} - \text{N} > \text{P} - \text{P} \) (Bond energy of single bond)
(B) All oxidation states of N lying between \(+1\) and \(+4\) tend to disproportionate in acidic medium.
(C) Maximum covalency of nitrogen is 4
(D) Nitrogen can form \(d\pi - p\pi\) bond with itself and other elements.
(E) Nitrogen has maximum density in its group due to its small size
The incorrect statements are:

• A. A, B \& D
• B. A, D \& E
• C. B, C \& E
• D. A, C \& E

Answer 1

The Correct Option is B

Concept:
Nitrogen shows anomalous behavior in Group 15 due to its small size, high electronegativity, and absence of vacant d-orbitals. These properties influence bond strength, oxidation states, and bonding behavior. Step 1: Analyze Statement (A). \[ \text{Bond energy: } \text{N-N} < \text{P-P} \] Due to lone pair repulsion in nitrogen, N–N bond is weaker than P–P. Hence, (A) is incorrect. Step 2: Analyze Statement (B). Oxidation states between \(+1\) and \(+4\) in nitrogen tend to disproportionate: \[ \text{Example: } HNO_2 \rightarrow NO + NO_3^- \] Thus, (B) is correct. Step 3: Analyze Statement (C). Nitrogen has no vacant d-orbitals: \[ \text{Maximum covalency of N = 4} \] Thus, (C) is correct. Step 4: Analyze Statement (D). Nitrogen cannot form \(d\pi - p\pi\) bonds because it lacks d-orbitals. Thus, (D) is incorrect. Step 5: Analyze Statement (E). Nitrogen has the least density in its group due to small size and gaseous nature. Thus, (E) is incorrect. Step 6: Final selection. Incorrect statements: \[ A,\; D,\; E \] \[ \boxed{\text{Option (2)}} \]