Assertion: The electron affinity of chlorine is greater than that of fluorine.
Reason: Chlorine is more electronegative than fluorine.

Options

A. Both A and B true and R is the correct explanation A
B. Both A and R are true but R is not a correct explanation of A
C. A is true but R is false
D. A is false but R is true

Answer

To solve the question, we need to evaluate the assertion and the reason given in the statement.

### Step 1: Understand the Assertion
The assertion states that "The electron affinity of chlorine is greater than that of fluorine."

- **Electron Affinity**: This is the amount of energy released when an electron is added to a neutral atom in the gaseous state.
- Chlorine (Cl) has a higher electron affinity than fluorine (F) due to the size and electron repulsion effects. Chlorine, being larger than fluorine, can accommodate an additional electron more easily without significant repulsion compared to fluorine.

### Step 2: Understand the Reason
The reason states that "Chlorine is more electronegative than fluorine."

- **Electronegativity**: This is the tendency of an atom to attract electrons in a bond. Fluorine is actually the most electronegative element in the periodic table, with a higher electronegativity than chlorine. Therefore, this statement is false.

### Step 3: Conclusion
- The assertion is true: Chlorine does have a greater electron affinity than fluorine.
- The reason is false: Chlorine is not more electronegative than fluorine; in fact, fluorine is more electronegative.

### Final Answer
- The assertion is true, and the reason is false.