Derivative of nitrogen (III) act as

Options

A. Oxidizing agent only
B. reducing agent only
C. both oxidizing and reducing agent
D. nitrating agent

Answer

To solve the question regarding the derivatives of nitrogen (III) and their behavior as oxidizing or reducing agents, we can break down the explanation into a step-by-step solution.

### Step-by-Step Solution:

1. **Understanding Nitrogen (III) Compounds**:
- Nitrogen (III) refers to compounds where nitrogen has an oxidation state of +3. An example of such a compound is nitrous acid (HNO2).

2. **Determining the Oxidation State**:
- In HNO2, we can determine the oxidation state of nitrogen by using the formula for oxidation states. The overall charge of the compound is neutral (0), and we can set up the equation:
\[ x + 2(-2) + 1 = 0 \]
Here, \(x\) is the oxidation state of nitrogen. Solving this gives:
\[ x - 4 + 1 = 0 \implies x - 3 = 0 \implies x = +3 \]

3. **Identifying Derivatives of Nitrogen**:
- Any compound that contains nitrogen in the +3 oxidation state is considered a derivative of nitrogen.

4. **Oxidation and Reduction**:
- The oxidation state of nitrogen can vary. The maximum oxidation state is +5 (as in nitric acid, HNO3) and the minimum is -3 (as in ammonia, NH3).
- Therefore, nitrogen in the +3 state can either be oxidized to +5 or reduced to -3.

5. **Behavior as Oxidizing and Reducing Agents**:
- If nitrogen in the +3 state is oxidized to +5, it acts as a reducing agent because it loses electrons.
- Conversely, if nitrogen in the +3 state is reduced to -3, it acts as an oxidizing agent because it gains electrons.
- Thus, nitrogen (III) derivatives can function as both oxidizing and reducing agents depending on the reaction conditions.

### Final Conclusion:
- Derivatives of nitrogen (III) can act as both oxidizing and reducing agents depending on whether they are oxidized to +5 or reduced to -3.