In which of the following oxidation state of oxygen is +2.

Options

A. `H_2O`
B. `H_2O_2`
C. `O_2F_2`
D. `OF_2`

Answer

To determine in which compound the oxidation state of oxygen is +2, we will analyze each of the given options step by step.

### Step 1: Analyze Water (H2O)
1. **Identify oxidation states**: In H2O, hydrogen (H) has an oxidation state of +1.
2. **Set up the equation**: Let the oxidation state of oxygen be \(X\). The overall charge of the molecule is 0.
\[ 2(+1) + X = 0 \]
3. **Solve for \(X\)**:
\[ 2 + X = 0 \implies X = -2 \]
4. **Conclusion**: The oxidation state of oxygen in H2O is -2.

### Step 2: Analyze Hydrogen Peroxide (H2O2)
1. **Identify oxidation states**: In H2O2, hydrogen (H) again has an oxidation state of +1.
2. **Set up the equation**: Let the oxidation state of oxygen be \(X\). The overall charge of the molecule is 0.
\[ 2(+1) + 2X = 0 \]
3. **Solve for \(X\)**:
\[ 2 + 2X = 0 \implies 2X = -2 \implies X = -1 \]
4. **Conclusion**: The oxidation state of oxygen in H2O2 is -1.

### Step 3: Analyze Dioxygen Difluoride (O2F2)
1. **Identify oxidation states**: In O2F2, fluorine (F) has an oxidation state of -1.
2. **Set up the equation**: Let the oxidation state of oxygen be \(X\). The overall charge of the molecule is 0.
\[ 2X + 2(-1) = 0 \]
3. **Solve for \(X\)**:
\[ 2X - 2 = 0 \implies 2X = 2 \implies X = +1 \]
4. **Conclusion**: The oxidation state of oxygen in O2F2 is +1.

### Step 4: Analyze Oxygen Difluoride (OF2)
1. **Identify oxidation states**: In OF2, fluorine (F) has an oxidation state of -1.
2. **Set up the equation**: Let the oxidation state of oxygen be \(X\). The overall charge of the molecule is 0.
\[ X + 2(-1) = 0 \]
3. **Solve for \(X\)**:
\[ X - 2 = 0 \implies X = +2 \]
4. **Conclusion**: The oxidation state of oxygen in OF2 is +2.

### Final Answer
The oxidation state of oxygen that is +2 is found in **OF2**.