Question

For a reaction, \( NH_{4}NO_{2} \rightarrow N_{2} + 2H_{2}O \). Which from following phenomena is true regarding nitrogen?

• A. Oxidised
• B. Reduced
• C. Oxidised as well as reduced
• D. Neither oxidised nor reduced

Hint:

This is a comproportionation reaction where different oxidation states of the same element combine to form a single product.

Answer 1

The Correct Option is C

Step 1: Initial Oxidation States
In $NH_4NO_2$:
- In $NH_4^+$, Nitrogen is $-3$. - In $NO_2^-$, Nitrogen is $+3$.
Step 2: Final Oxidation State
In $N_2$ (elemental state), Nitrogen is $0$.
Step 3: Analysis
- $-3 \rightarrow 0$ (Increase in ON = Oxidation). - $+3 \rightarrow 0$ (Decrease in ON = Reduction).
Step 4: Conclusion
Since one nitrogen is oxidized and the other is reduced, nitrogen is both oxidized and reduced.
Final Answer:(C)