`Mg^(2+)` is .......... Than `Al^(3+)`

Options

A. stronger Lewis acid
B. stronger Lewis base
C. weaker Lewis acid
D. weaker Lewis base

Explanation

To determine the relationship between `Mg^(2+)` and `Al^(3+)` in terms of Lewis acidity, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Lewis Acids and Bases**:
- Lewis acids are defined as species that are electron-deficient and can accept electron pairs.
- Lewis bases are species that are electron-rich and can donate electron pairs.

2. **Analyzing the Charges**:
- `Mg^(2+)` has a +2 charge, meaning it has lost 2 electrons.
- `Al^(3+)` has a +3 charge, meaning it has lost 3 electrons.

3. **Comparing Electron Deficiency**:
- Since `Al^(3+)` has a higher positive charge (+3) compared to `Mg^(2+)` (+2), it is more electron-deficient.
- The greater the positive charge, the stronger the Lewis acid, as it has a higher tendency to accept electrons.

4. **Conclusion**:
- Since `Al^(3+)` is more electron-deficient than `Mg^(2+)`, it is a stronger Lewis acid.
- Therefore, `Mg^(2+)` is a weaker Lewis acid compared to `Al^(3+)`.

5. **Final Answer**:
- The correct statement is: `Mg^(2+)` is a weaker Lewis acid than `Al^(3+)`.