Metal ions like `Ag^(+),Cu^(2+)` etc. act as

Options

A. Bronsted acids
B. Bronsted bases
C. Lewis acids
D. Lewis bases

Answer

To solve the question regarding how metal ions like `Ag^(+)` and `Cu^(2+)` act, we will analyze their behavior based on the definitions of Bronsted and Lewis acids and bases.

### Step-by-Step Solution:

1. **Understanding Metal Ions**:
- Metal ions such as `Ag^(+)` and `Cu^(2+)` are positively charged ions. This means they have lost electrons compared to their neutral atoms.

2. **Identifying Electron Configuration**:
- For `Cu`, the atomic number is 29. The electron configuration of neutral copper (Cu) is:
\[ \text{Cu: } 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^1, 3d^{10} \]
- When copper loses two electrons to become `Cu^(2+)`, the electron configuration becomes:
\[ \text{Cu}^{2+}: 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^9 \]
- This shows that there is a vacancy in the 3d subshell.

3. **Analyzing Silver Ion**:
- For `Ag`, the atomic number is 47. The electron configuration of neutral silver (Ag) is:
\[ \text{Ag: } 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^{10}, 4p^1 \]
- When silver loses one electron to become `Ag^(+)`, the electron configuration becomes:
\[ \text{Ag}^+: 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^{10} \]
- In this case, there are no vacancies in the d subshell.

4. **Defining Lewis Acids and Bases**:
- According to Lewis theory, a Lewis acid is defined as an electron pair acceptor, while a Lewis base is an electron pair donor.
- Since `Cu^(2+)` has a vacancy in its electron configuration, it can accept an electron pair, classifying it as a Lewis acid.
- `Ag^(+)`, while it does not have a vacancy, can still act as a Lewis acid due to its positive charge, which can attract electron pairs.

5. **Conclusion**:
- Both `Ag^(+)` and `Cu^(2+)` can act as Lewis acids because they can accept electron pairs. Therefore, the correct answer is that metal ions like `Ag^(+)` and `Cu^(2+)` act as Lewis acids.

### Final Answer:
**Metal ions like `Ag^(+)` and `Cu^(2+)` act as Lewis acids.**