(A): Fluorine does not form oxyacids
(R): Electronegativity of fluorine is higher than that of oxygen.

Options

A. Both A & R are true, R is the correct explanation of A
B. Both A & R are true, R is not correct explanation of A
C. A is true, R is false
D. A is false, R is true

Answer

To analyze the assertion and reason provided in the question, we can break down the information step by step.

### Step 1: Understand the Assertion
**Assertion (A):** Fluorine does not form oxyacids.
- Oxyacids are acids that contain oxygen, hydrogen, and another element (in this case, a halogen). For example, chloric acid (HClO3) is an oxyacid where chlorine is the halogen.

### Step 2: Understand the Reason
**Reason (R):** Electronegativity of fluorine is higher than that of oxygen.
- Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. Fluorine has the highest electronegativity in the periodic table (approximately 4.0), while oxygen has a lower electronegativity (approximately 3.5).

### Step 3: Analyze the Relationship between A and R
- In oxyacids, the halogen typically has a positive oxidation state, while oxygen has a negative oxidation state.
- Since fluorine is the most electronegative element, it tends to attract electrons more strongly than oxygen. This means that fluorine cannot easily exist in a positive oxidation state, which is necessary for the formation of oxyacids. Instead, it tends to form negative oxidation states.

### Step 4: Conclusion
- Since fluorine cannot exist in a positive oxidation state due to its high electronegativity, it does not form oxyacids. Therefore, both the assertion and the reason are true, and the reason correctly explains the assertion.

### Final Answer
Both the assertion (A) and the reason (R) are true, and the reason (R) correctly explains the assertion (A).