Which of the following statements is correct ?

Options

A. Hydrides of group 13 act as Lewis acids.
B. Hydrides of group 14 are electron deficient hydrides.
C. Hydrides of group 14 act as Lewis acids.
D. Hydrides of group 15 act as Lewis bases.

Explanation

To determine which statements about hydrides are correct, we can analyze the properties of different types of hydrides based on their electron configurations and bonding characteristics.

### Step-by-Step Solution:

1. **Identify Types of Hydrides**:
- Hydrides can be classified into three categories: electron deficient, electron precise, and electron rich hydrides.

2. **Electron Deficient Hydrides**:
- These hydrides have a central atom that does not complete its octet even after forming bonds with hydrogen. An example is BH3 (Boron Hydride).
- Since they are electron deficient, they can accept electrons and act as Lewis acids.

3. **Electron Precise Hydrides**:
- These hydrides have a central atom with a complete octet and do not have any tendency to accept or donate electrons. An example is CH4 (Methane).
- They do not act as Lewis acids or bases because their electron configuration is stable.

4. **Electron Rich Hydrides**:
- These hydrides have a central atom that has more than eight electrons in its valence shell, often due to lone pairs. An example is NH3 (Ammonia).
- They can donate electrons and act as Lewis bases because they have available lone pairs.

5. **Conclusion**:
- Based on the analysis:
- Electron deficient hydrides (like BH3) act as Lewis acids.
- Electron precise hydrides (like CH4) do not act as Lewis acids or bases.
- Electron rich hydrides (like NH3) act as Lewis bases.
- Therefore, statements regarding the behavior of these hydrides can be confirmed as correct.