Oxygen exhibits positive oxidation state in its compounds with

Options

A. chlorine
B. fluorine
C. xenon
D. platinum

Explanation

To determine when oxygen exhibits a positive oxidation state in its compounds, we need to analyze its electronegativity in relation to other elements. Here’s a step-by-step solution:

### Step 1: Understand Oxidation States
Oxidation state refers to the degree of oxidation of an atom in a compound. An atom can have a positive, negative, or zero oxidation state depending on its bonding with other atoms.

### Step 2: Identify Electronegativity
Electronegativity is the tendency of an atom to attract electrons in a bond. The more electronegative an atom, the more it pulls electrons towards itself.

### Step 3: Compare Electronegativity of Oxygen
Oxygen has an electronegativity of 3.44 on the Pauling scale. We need to compare this with the electronegativities of the elements in the options provided:
- Chlorine (Cl) has an electronegativity of 3.16.
- Fluorine (F) has an electronegativity of 4.0.
- Xenon (Xe) has an electronegativity of 2.6.
- Platinum (Pt) has an electronegativity of 2.2.

### Step 4: Determine Conditions for Positive Oxidation State
Oxygen will exhibit a positive oxidation state when it bonds with an element that has a higher electronegativity than itself. This is because the more electronegative element will attract the shared electrons more strongly, resulting in oxygen losing some of its electron density.

### Step 5: Analyze Each Option
- **Option A: Chlorine** - Chlorine is less electronegative than oxygen, so oxygen cannot exhibit a positive oxidation state here.
- **Option B: Fluorine** - Fluorine is more electronegative than oxygen, so in compounds with fluorine, oxygen will exhibit a positive oxidation state.
- **Option C: Xenon** - Xenon is less electronegative than oxygen, so oxygen cannot exhibit a positive oxidation state here.
- **Option D: Platinum** - Platinum is also less electronegative than oxygen, so oxygen cannot exhibit a positive oxidation state here.

### Conclusion
The only element from the options provided that allows oxygen to exhibit a positive oxidation state is **Fluorine (Option B)**.

### Final Answer
Oxygen exhibits a positive oxidation state in its compounds with **Fluorine**.

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