Sulphur and rest of the elements of group `16` are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire `ns^2 np^6` configuration by sharing two electrons with the atoms of other elements and thus, exhibit `+2` oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the `p` and s-orbitals of the same shell. As a result, they can show `+4` and `+ 6` oxidation states.
Oxygen exhibits `+2` oxidation state in

Options

A. `H_2 O`
B. `OF_2`
C. `Cl_2 O`
D. `H_2 O_2`

Explanation

To determine in which compound oxygen exhibits a +2 oxidation state, we will analyze the oxidation states of oxygen in various compounds.

### Step-by-Step Solution:

1. **Analyze Water (H₂O)**:
- In water, hydrogen has an oxidation state of +1.
- The equation for the oxidation state of oxygen (O) can be set up as:
\[ 2(+1) + x = 0 \]
- This simplifies to:
\[ 2 + x = 0 \implies x = -2 \]
- Therefore, in H₂O, oxygen has an oxidation state of -2.

2. **Analyze Oxygen Difluoride (OF₂)**:
- Fluorine is the most electronegative element and has an oxidation state of -1.
- The equation for the oxidation state of oxygen can be set up as:
\[ 2(-1) + x = 0 \]
- This simplifies to:
\[ -2 + x = 0 \implies x = +2 \]
- Therefore, in OF₂, oxygen has an oxidation state of +2.

3. **Analyze Dichlorine Monoxide (Cl₂O)**:
- In this compound, oxygen is more electronegative than chlorine.
- The equation for the oxidation state of oxygen can be set up as:
\[ 2x + (-2) = 0 \]
- This simplifies to:
\[ 2x - 2 = 0 \implies 2x = 2 \implies x = +1 \]
- Therefore, in Cl₂O, oxygen has an oxidation state of -2.

4. **Analyze Hydrogen Peroxide (H₂O₂)**:
- In hydrogen peroxide, the oxidation state of hydrogen is +1.
- The equation for the oxidation state of oxygen can be set up as:
\[ 2(+1) + 2x = 0 \]
- This simplifies to:
\[ 2 + 2x = 0 \implies 2x = -2 \implies x = -1 \]
- Therefore, in H₂O₂, oxygen has an oxidation state of -1.

### Conclusion:
From the analysis, we find that oxygen exhibits a +2 oxidation state in **Oxygen Difluoride (OF₂)**.

### Final Answer:
Oxygen exhibits +2 oxidation state in **OF₂**.