Hydride of certain non - metallic element X is amphoteric in nature. It also reacts with sodium hydride as well with metallic sodium to liberate dihydrogen gas. The element X can be

Options

A. Nitrogen
B. Carbon
C. Oxygen
D. Sulphur

Answer

To solve the problem, we need to identify the non-metallic element X whose hydride is amphoteric in nature and reacts with sodium hydride and metallic sodium to liberate dihydrogen gas.

### Step-by-Step Solution:

1. **Understanding Amphoteric Nature**:
- An amphoteric substance can act as both an acid and a base. We need to find a hydride of a non-metal that exhibits this behavior.

2. **Identifying Possible Elements**:
- The options provided are nitrogen, carbon, oxygen, and sulfur. We need to evaluate the hydrides of these elements to see which one is amphoteric.

3. **Evaluating Hydrides**:
- **Nitrogen (NH₃)**: Ammonia is primarily a base and does not show amphoteric behavior.
- **Carbon (CH₄)**: Methane is a non-polar molecule and does not exhibit amphoteric properties.
- **Oxygen (H₂O)**: Water is known to be amphoteric. It can act as an acid (donating H⁺) and as a base (accepting H⁺).
- **Sulfur (H₂S)**: Hydrogen sulfide behaves mainly as an acid and does not show amphoteric properties.

4. **Reactions with Sodium Hydride and Sodium**:
- Water (H₂O) reacts with sodium hydride (NaH) to produce sodium hydroxide (NaOH) and hydrogen gas (H₂):
\[ 2 \text{NaH} + 2 \text{H}_2\text{O} \rightarrow 2 \text{NaOH} + \text{H}_2 \]
- Water also reacts with metallic sodium (Na) to produce sodium hydroxide and liberate hydrogen gas:
\[ 2 \text{Na} + 2 \text{H}_2\text{O} \rightarrow 2 \text{NaOH} + \text{H}_2 \]

5. **Conclusion**:
- Based on the evaluations, the non-metallic element X is **Oxygen**. Its hydride (water) is amphoteric and reacts with both sodium hydride and metallic sodium to liberate dihydrogen gas.

### Final Answer:
The element X can be **Oxygen**.