Assertion `:` `-I` effect of `Cl` atom is greater than `F` atom.
Reason `:` `Cl` atom has more elctronegativity than F atom.

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 Assertiion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False

Answer

To solve the question regarding the assertion and reason about the -I effect of Cl and F atoms, we can break down the solution into clear steps:

### Step 1: Understand the Assertion
The assertion states that the -I (negative inductive) effect of the chlorine (Cl) atom is greater than that of the fluorine (F) atom.

### Step 2: Understand the Reason
The reason provided states that the chlorine atom has more electronegativity than the fluorine atom.

### Step 3: Analyze the -I Effect
The -I effect is the ability of an atom or group to withdraw electron density from a neighboring atom through sigma bonds. This effect is generally stronger in more electronegative atoms.

### Step 4: Compare Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons. In the case of halogens:
- Fluorine (F) is the most electronegative element in the periodic table.
- Chlorine (Cl) is less electronegative than fluorine.

### Step 5: Conclusion on the Assertion
Since fluorine is more electronegative than chlorine, it has a stronger -I effect. Therefore, the assertion that the -I effect of Cl is greater than that of F is **false**.

### Step 6: Conclusion on the Reason
The reason states that Cl has more electronegativity than F, which is also **false** because F is indeed more electronegative than Cl.

### Final Conclusion
Both the assertion and the reason are false.