A : Atomic size of F is smaller than that of Cl .
R : F- F bond is stronger than Cl-Cl bond .

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion , then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanation of the assertion , then mark (2)
C. If Assertion is true statement but Reason is false , then mark (3)
D. If both Assertion and Reason are false statements , then mark (4)

Answer

To solve the assertion-reason question, we will analyze both the assertion and the reason step by step.

### Step 1: Analyze the Assertion
**Assertion:** The atomic size of F is smaller than that of Cl.

- **Explanation:** Fluorine (F) and chlorine (Cl) are both members of Group 17 (the halogens) in the periodic table. As we move down a group in the periodic table, the atomic size increases due to the addition of electron shells. Therefore, since fluorine is above chlorine in the group, it has a smaller atomic radius. Thus, the assertion is **correct**.

### Step 2: Analyze the Reason
**Reason:** F-F bond is stronger than Cl-Cl bond.

- **Explanation:** The strength of a bond is influenced by the bond length and the atomic size of the atoms involved. Although fluorine has a smaller atomic size than chlorine, the F-F bond is actually weaker than the Cl-Cl bond. This is due to the high electronegativity of fluorine, which leads to significant repulsion between the lone pairs of electrons on the two fluorine atoms. As a result, the F-F bond is weaker than expected. Therefore, the reason is **incorrect**.

### Conclusion
- **Assertion:** Correct
- **Reason:** Incorrect

### Final Answer
The assertion is correct, but the reason is incorrect.

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