`AlCl_(3)` is a Less acidic than `BCl_(3)`.True or False

Answer

To determine whether the statement "AlCl₃ is less acidic than BCl₃" is true or false, we need to analyze the acidity of both compounds.

### Step-by-Step Solution:

1. **Understanding Acidity**:
- Acidity in Lewis acid terms refers to the ability of a compound to accept an electron pair. The stronger the ability to accept an electron pair, the stronger the Lewis acid.

2. **Analyzing BCl₃**:
- BCl₃ (Boron trichloride) is a Lewis acid. Boron has an incomplete octet and can accept an electron pair. The boron atom uses its 2p orbital for bonding, which is smaller in size compared to aluminum's 3p orbital. This smaller size allows boron to effectively accept electron pairs, making BCl₃ a stronger Lewis acid.

3. **Analyzing AlCl₃**:
- AlCl₃ (Aluminum chloride) is also a Lewis acid. However, aluminum uses its 3p orbital for bonding, which is larger than the 2p orbital of boron. The larger size of the aluminum atom makes it less effective at accepting electron pairs compared to boron.

4. **Comparing Acidity**:
- Since BCl₃ has a stronger ability to accept electron pairs due to the smaller size of boron compared to aluminum, it is classified as a stronger Lewis acid than AlCl₃.

5. **Conclusion**:
- Therefore, the statement "AlCl₃ is less acidic than BCl₃" is **True**.

### Final Answer:
True, AlCl₃ is less acidic than BCl₃.