Which of the following is//are basic hydride?

Options

A. `HCl`
B. `NH_(3)`
C. `H_(2)S`
D. `PH_(3)`

Explanation

To determine which of the given compounds are basic hydrides, we need to analyze each option based on their chemical properties and their position in the periodic table.

### Step-by-Step Solution:

1. **Identify the Options**: The options provided are NH3 (ammonia), PH3 (phosphine), H2S (hydrogen sulfide), and HCl (hydrochloric acid).

2. **Understand Basic Hydrides**: Basic hydrides are compounds that can donate a pair of electrons (act as Lewis bases) and typically have a lone pair of electrons on the central atom.

3. **Analyze Each Compound**:
- **NH3 (Ammonia)**:
- NH3 has one lone pair of electrons on nitrogen.
- It can accept protons (H+) and thus acts as a base.
- **Conclusion**: NH3 is a basic hydride.

- **PH3 (Phosphine)**:
- PH3 also has one lone pair of electrons on phosphorus.
- It can act as a base, though it is weaker than NH3.
- **Conclusion**: PH3 is a basic hydride.

- **H2S (Hydrogen Sulfide)**:
- H2S has two lone pairs on sulfur.
- It is known to be acidic in nature, as it can donate protons.
- **Conclusion**: H2S is not a basic hydride.

- **HCl (Hydrochloric Acid)**:
- HCl is a strong acid and does not have a lone pair to donate.
- It donates protons readily and does not act as a base.
- **Conclusion**: HCl is not a basic hydride.

4. **Final Conclusion**: Based on the analysis, the basic hydrides among the options are NH3 and PH3.

### Answer:
The basic hydrides from the given options are **NH3 and PH3**.

---