Assertion. `PbI_(4)` is a stable than `PbCl_(4)`.
Reason. Iodide ion stabilizes higher oxidation state.

Options

A. If both assertion and reason are true, and reason is the true explanation of the assertion.
B. If both assertion and reason are true, but reason not is the true explanation of the assertion.
C. If assertion is true, but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the question regarding the stability of \( \text{PbI}_4 \) compared to \( \text{PbCl}_4 \) and the reasoning behind it, we can break it down into a step-by-step analysis:

### Step 1: Analyze the Assertion
The assertion states that \( \text{PbI}_4 \) is more stable than \( \text{PbCl}_4 \). To evaluate this, we need to consider the properties of lead(IV) iodide and lead(IV) chloride.

**Hint:** Consider the nature of the halides involved and their ability to stabilize different oxidation states of lead.

### Step 2: Analyze the Reason
The reason provided is that the iodide ion stabilizes higher oxidation states. To understand this, we should look at the electronegativity of iodine compared to chlorine. Iodine has a lower electronegativity than chlorine, which affects its ability to stabilize the oxidation state of lead.

**Hint:** Compare the electronegativities of iodine and chlorine and how they influence the stability of lead in higher oxidation states.

### Step 3: Compare the Stability of \( \text{PbI}_4 \) and \( \text{PbCl}_4 \)
Lead(IV) iodide (\( \text{PbI}_4 \)) is known to be less stable than lead(IV) chloride (\( \text{PbCl}_4 \)). The larger size and lower electronegativity of the iodide ion lead to a weaker bond with lead in the +4 oxidation state, making \( \text{PbI}_4 \) more prone to reduction to \( \text{Pb}^{2+} \).

**Hint:** Think about how the size and charge of the halide ions affect the bond strength and stability of the lead compounds.

### Step 4: Conclusion on Assertion and Reason
Since \( \text{PbI}_4 \) is actually less stable than \( \text{PbCl}_4 \), the assertion is false. Additionally, the reason that iodide stabilizes higher oxidation states is also incorrect, as lower electronegativity does not favor stabilization of higher oxidation states.

**Hint:** Summarize your findings to conclude whether both the assertion and reason are true or false.

### Final Answer
Both the assertion and the reason are false. Therefore, the correct conclusion is that \( \text{PbI}_4 \) is not more stable than \( \text{PbCl}_4 \), and the iodide ion does not stabilize higher oxidation states effectively.