What is the oxidation state of oxygen in `O_2 F_2` ?

Options

A. `+1`
B. `+2`
C. `-2`
D. `-1`

Explanation

To find the oxidation state of oxygen in \( O_2F_2 \), we can follow these steps:

### Step 1: Assign Variables
Let the oxidation state of oxygen be \( x \). Since there are two oxygen atoms in \( O_2F_2 \), we can express the total oxidation state of oxygen as \( 2x \).

### Step 2: Determine the Oxidation State of Fluorine
Fluorine (F) is more electronegative than oxygen and typically has an oxidation state of \(-1\). In \( O_2F_2 \), there are two fluorine atoms, so the total contribution from fluorine is \( 2 \times (-1) = -2 \).

### Step 3: Set Up the Equation
Since the molecule \( O_2F_2 \) is neutral, the sum of the oxidation states must equal zero. Therefore, we can set up the following equation:

\[ 2x + (-2) = 0 \]

### Step 4: Solve for \( x \)
Now, we can solve for \( x \):

\[ 2x - 2 = 0 \]
\[ 2x = 2 \]
\[ x = \frac{2}{2} = 1 \]

### Conclusion
The oxidation state of oxygen in \( O_2F_2 \) is \( +1 \).