Question

The oxidation states of ‘N’ in \( \text{NH}_4^+ \), \( \text{NO}_2^- \), and \( \text{NO} \) are _______ , respectively.

• A. \( +2, -3, \) and \( +3 \)
• B. \( -3, +3, \) and \( +2 \)
• C. \( -3, +3, \) and \( -4 \)
• D. \( +4, -2, \) and \( +2 \)

Hint:

To determine the oxidation state of nitrogen in compounds, balance the oxidation states of the other atoms and apply the rule that the sum of oxidation states equals the charge of the molecule or ion.

Answer 1

The Correct Option is B

- In \( \text{NH}_4^+ \), the oxidation state of nitrogen is \( -3 \) since the total charge of the ammonium ion is \( +1 \), and each hydrogen has an oxidation state of \( +1 \).
- In \( \text{NO}_2^- \), the oxidation state of nitrogen is \( +3 \), as oxygen has an oxidation state of \( -2 \) and the total charge is \( -1 \).
- In \( \text{NO} \), the oxidation state of nitrogen is \( +2 \), as oxygen has an oxidation state of \( -2 \) and the molecule is neutral.
Thus, the oxidation states of nitrogen in \( \text{NH}_4^+ \), \( \text{NO}_2^- \), and \( \text{NO} \) are \( -3, +3, \) and \( +2 \), respectively. Final Answer: \[ \boxed{-3, +3, \text{ and } +2}. \]