Assertion :- Bond Dissociation energy is `F_(2) gt Cl_(2)`
Reason:- `Cl_(2)` have more electronic repulsion than `F_(2)`.

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.
C. If Assertion is True, but the Reason is False.
D. If both Assertion & Reason are false

Answer

To analyze the assertion and reason provided in the question, we will break down the concepts of bond dissociation energy and electronic repulsion in diatomic molecules, specifically focusing on fluorine (F₂) and chlorine (Cl₂).

### Step-by-Step Solution:

1. **Understanding Bond Dissociation Energy (BDE)**:
- Bond dissociation energy is the energy required to break a bond between two atoms in a molecule. Generally, a higher bond dissociation energy indicates a stronger bond.

2. **Comparing F₂ and Cl₂**:
- The assertion states that the bond dissociation energy of F₂ is greater than that of Cl₂ (F₂ > Cl₂). This assertion is incorrect. In reality, Cl₂ has a higher bond dissociation energy than F₂.

3. **Reason for the Difference**:
- The reason provided states that Cl₂ has more electronic repulsion than F₂. This is also incorrect. In fact, due to the smaller size of the fluorine atom, there is greater inter-electronic repulsion in F₂ compared to Cl₂.

4. **Analyzing Electronic Repulsion**:
- In F₂, the two fluorine atoms are closer together because of their smaller atomic size, leading to significant repulsion between the non-bonding electrons. This increased repulsion weakens the bond, resulting in a lower bond dissociation energy.
- Conversely, Cl₂ has larger atomic size, which means the electrons are farther apart, resulting in less repulsion and a stronger bond.

5. **Conclusion**:
- Both the assertion and the reason are incorrect. The bond dissociation energy of Cl₂ is greater than that of F₂, and Cl₂ has less electronic repulsion than F₂.

### Final Answer:
Both the assertion and the reason are incorrect. Therefore, the correct option is D.

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