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. Both Statement I and Statement II are correct, Statement II is the correct explanation of Statement I
B. Both Statement I and Statement II are correct, Statement II is not the correct explanation of Statement I
C. Statement I is correct, Statement II is the incorrect
D. Statement I is incorrect, Statement II is the correct

Explanation

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

### Step-by-Step Solution:

1. **Understanding the Assertion (A)**:
- The assertion states that \( \text{Pb}^{+4} \) compounds are stronger oxidizing agents than \( \text{Sn}^{+4} \) compounds.
- To evaluate this, we need to consider the stability of the oxidation states of lead (Pb) and tin (Sn).

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