Assertion (A): `CIF` is more reactive than `F_(2)`.
Reason (R ): The F-F bons is weaker than CIF bond.

Options

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

Explanation

To solve the question, we need to analyze both the assertion (A) and the reason (R) provided.

### Step-by-Step Solution:

1. **Understanding the Assertion (A)**:
- The assertion states that `ClF` (Chlorine Fluoride) is more reactive than `F2` (Fluorine gas).
- Reactivity in halogens can be influenced by bond strength. Generally, weaker bonds lead to higher reactivity.

2. **Analyzing the Reason (R)**:
- The reason states that the F-F bond is weaker than the Cl-F bond.
- To evaluate this, we need to compare the bond strengths of F-F and Cl-F.
- The F-F bond in `F2` is indeed strong due to effective orbital overlap between two identical fluorine atoms, while the Cl-F bond has some degree of ionic character due to the difference in electronegativity.

3. **Evaluating the Strength of Bonds**:
- The F-F bond is one of the strongest single bonds among diatomic molecules because of the small size of fluorine, which allows for effective overlap.
- The Cl-F bond, while strong, is not as strong as the F-F bond. However, the assertion that ClF is more reactive than F2 can still hold true.

4. **Conclusion**:
- The assertion (A) is correct: `ClF` is indeed more reactive than `F2`.
- The reason (R) is incorrect: The F-F bond is stronger than the Cl-F bond, which does not support the assertion.
- Therefore, the correct answer is that the assertion is correct, but the reason is wrong.

### Final Answer:
- Assertion (A) is correct.
- Reason (R) is incorrect.
- The answer is option C: Assertion is correct, Reason is incorrect.