Assertion: `Pb^(4+)`can be reduced easily to `Pb^(2+)`.
Reason: `Pb^(2+)` is paramagnetic.

Options

A. If both (A) and (R) are correct and (R) is correct explanation of (A)
B. If both (A) and (R) are correct and (R) is correct explanation of (A)
C. If (A) is correct , but (R) is incorrect
D. If (A) is incrorect byt (R) is incroroect .

Explanation

To solve the assertion-reason question, we need to analyze both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that `Pb^(4+)` can be reduced easily to `Pb^(2+)`.
- This reduction is primarily influenced by the inert pair effect, which refers to the tendency of the outermost s-electrons to remain paired and not participate in bonding as we move down the group in the periodic table.

2. **Analyzing the Stability of Oxidation States**:
- Lead (Pb) can exist in multiple oxidation states, with `Pb^(4+)` being less stable compared to `Pb^(2+)`.
- The `Pb^(2+)` state is more stable due to the inert pair effect, making it easier for `Pb^(4+)` to be reduced to `Pb^(2+)`.

3. **Conclusion on Assertion**:
- Since `Pb^(4+)` can indeed be reduced to `Pb^(2+)` easily due to the inert pair effect, the assertion is **correct**.

4. **Understanding the Reason**:
- The reason states that `Pb^(2+)` is paramagnetic.
- To determine if `Pb^(2+)` is paramagnetic, we need to check its electron configuration and the presence of unpaired electrons.

5. **Electron Configuration of Lead**:
- The electron configuration of lead (Pb) is `[Xe] 4f14 5d10 6s2 6p2`.
- When lead loses two electrons to form `Pb^(2+)`, it loses the two 6p electrons, resulting in the configuration `[Xe] 4f14 5d10 6s2`.

6. **Determining Magnetic Properties**:
- In `Pb^(2+)`, there are no unpaired electrons in the 6s or 6p orbitals, indicating that it is **diamagnetic**.
- Since `Pb^(2+)` does not have unpaired electrons, the reason is **incorrect**.

7. **Final Conclusion**:
- The assertion is correct, while the reason is incorrect. Therefore, the correct answer is that the assertion is true, but the reason is false.

### Final Answer:
- Assertion: True
- Reason: False