(A): Oxygen exhibits positive oxidation states in some of its compounds
(R): In binary fluorides, fluorine is always more electronegative

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 statement and reason provided in the question, we will break it down step by step.

### Step 1: Understanding the Statement (A)
The statement (A) claims that "Oxygen exhibits positive oxidation states in some of its compounds."

- **Explanation**: Typically, oxygen has an oxidation state of -2 in most of its compounds. However, in certain compounds, particularly those involving highly electronegative elements like fluorine, oxygen can exhibit positive oxidation states.

### Step 2: Understanding the Reason (R)
The reason (R) states that "In binary fluorides, fluorine is always more electronegative."

- **Explanation**: Fluorine is the most electronegative element on the periodic table, with an electronegativity value of 4.0 on the Pauling scale. This means that in compounds where fluorine is present, it will attract electrons more strongly than oxygen, leading to a negative oxidation state for fluorine and a positive oxidation state for oxygen.

### Step 3: Examples of Oxygen's Positive Oxidation States
To illustrate the statement (A), we can consider specific examples:

- **OF2 (Oxygen Difluoride)**: In this compound, the oxidation state of oxygen is +2. This occurs because each fluorine atom has an oxidation state of -1, and the overall charge must balance to zero.

- **O2F2 (Dioxygen Difluoride)**: In this compound, the oxidation state of oxygen is +1. Again, each fluorine atom contributes -1, and the total must balance to zero.

### Step 4: Conclusion
Both the statement (A) and the reason (R) are true. The reason (R) correctly explains why oxygen can exhibit positive oxidation states in certain compounds, particularly in the presence of fluorine.

### Final Answer
Both A and R are true, and R is the correct explanation of A.

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