Which of the following has been arranged in order of increasing oxidation number of nitrogen?

Options

A. `NH_(3)ltN_(2)O_(5)ltNOltN_(2)`
B. `NO_(2)^(+) lt NO_(3)^(-) lt NO_2^(-) lt N_(3)^(-)`
C. `NH_(4)^(+) lt N_(2)H_(4) lt NH_(2)OH lt N_(2)O`
D. `NO_(2) lt NaN_(3) lt NH_(4)^(+) lt N_(2)O`

Answer

To determine the order of increasing oxidation number of nitrogen in the given compounds, we will analyze each option step by step.

### Step 1: Identify the oxidation states of nitrogen in each compound.

1. **For NH₃ (Ammonia)**:
- Hydrogen (H) has an oxidation state of +1.
- Let the oxidation state of nitrogen (N) be x.
- The equation becomes: x + 3(+1) = 0 → x + 3 = 0 → x = -3.
- Therefore, the oxidation state of nitrogen in NH₃ is **-3**.

2. **For N₂H₄ (Hydrazine)**:
- Hydrogen (H) has an oxidation state of +1.
- Let the oxidation state of nitrogen (N) be x.
- The equation becomes: 2x + 4(+1) = 0 → 2x + 4 = 0 → 2x = -4 → x = -2.
- Therefore, the oxidation state of nitrogen in N₂H₄ is **-2**.

3. **For NH₂OH (Hydroxylamine)**:
- Hydrogen (H) has an oxidation state of +1 and Oxygen (O) has -2.
- Let the oxidation state of nitrogen (N) be x.
- The equation becomes: x + 2(+1) + (-2) = 0 → x + 2 - 2 = 0 → x = -1.
- Therefore, the oxidation state of nitrogen in NH₂OH is **-1**.

4. **For N₂ (Dinitrogen)**:
- In its elemental form, nitrogen has an oxidation state of **0**.

### Step 2: Arrange the oxidation states in increasing order.

Now we have the oxidation states:
- NH₃: -3
- N₂H₄: -2
- NH₂OH: -1
- N₂: 0

Arranging these in increasing order:
- -3 (NH₃) < -2 (N₂H₄) < -1 (NH₂OH) < 0 (N₂)

### Conclusion

The correct order of increasing oxidation number of nitrogen is:
**-3 < -2 < -1 < 0**

Thus, the correct option is **C**.

---