Assertion (A) :` Pb^(+4)` compounds are stronger oxidiising agents than ` Sn^(4+)` compounds .
Reason (R): The higher oxidation states for group `14` elements are more stable for the heavier members of the group due to inert pair effect .

Options

A. Statement-1 is Ture, Statement-2 is True, Statement-2 is a correct explanation for Statement-1.
B. Statement-1 is True, Statement-2 is Ture, Statement-2 is NOT a correct explanation for Statement-1
C. Statement-1 is Ture, Statement-2 is False
D. Statement-1 is Flase, Statement-2 is True

Explanation

To solve the assertion and reason question, we will analyze both the assertion (A) and the reason (R) step by step.

### Step 1: Analyze the Assertion (A)
The assertion states that Pb^(4+) compounds are stronger oxidizing agents than Sn^(4+) compounds.

- **Understanding Oxidizing Agents**: An oxidizing agent is a substance that can accept electrons and is reduced in the process. The strength of an oxidizing agent is often related to the stability of its higher oxidation state.
- **Lead (Pb) vs. Tin (Sn)**: Lead in the +4 oxidation state (Pb^(4+)) is less stable compared to its +2 oxidation state (Pb^(2+)). This instability makes Pb^(4+) a stronger oxidizing agent because it tends to be reduced to Pb^(2+).
- **Tin (Sn)**: On the other hand, Sn^(4+) is relatively more stable than Sn^(2+). This means that Sn^(4+) is less likely to act as an oxidizing agent compared to Pb^(4+).

**Conclusion for Assertion**: The assertion is correct; Pb^(4+) compounds are indeed stronger oxidizing agents than Sn^(4+) compounds.

### Step 2: Analyze the Reason (R)
The reason states that the higher oxidation states for group 14 elements are more stable for the heavier members of the group due to the inert pair effect.

- **Inert Pair Effect**: The inert pair effect refers to the tendency of the outermost s-electrons to remain non-bonding in heavier elements of a group. As we move down group 14 from carbon to lead, the +2 oxidation state becomes more stable compared to the +4 oxidation state due to this effect.
- **Application to Pb and Sn**: For heavier elements like lead, the +2 oxidation state is favored, making the +4 state less stable. Conversely, for tin, the +4 state is relatively more stable compared to lead's +4 state.

**Conclusion for Reason**: The reason is incorrect; higher oxidation states are not more stable for heavier members due to the inert pair effect. In fact, the +2 state is more stable for heavier elements.

### Final Conclusion
- **Assertion (A)**: True
- **Reason (R)**: False

### Summary
The assertion is correct while the reason is incorrect. Therefore, the statement "Pb^(4+) compounds are stronger oxidizing agents than Sn^(4+) compounds" is true, but the reasoning provided does not support this assertion.

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