An element that never has a positive oxidation state in any of its compounds is

Options

A. O
B. N
C. Cl
D. F

Explanation

To determine which element never has a positive oxidation state in any of its compounds, we can analyze the given options: O (Oxygen), N (Nitrogen), C (Carbon), L (likely Chlorine), and F (Fluorine).

### Step-by-Step Solution:

1. **Understand Oxidation States**: Oxidation states (or oxidation numbers) indicate the degree of oxidation of an atom in a compound. An oxidation state can be positive, negative, or zero.

2. **Analyze Each Element**:
- **Oxygen (O)**: Typically has a -2 oxidation state in compounds but can also exhibit a positive oxidation state in certain compounds (e.g., in peroxides or with fluorine).
- **Nitrogen (N)**: Can have multiple oxidation states ranging from -3 to +5, depending on the compound.
- **Carbon (C)**: Can exhibit oxidation states from -4 to +4, depending on its bonding.
- **Chlorine (Cl)**: Can have oxidation states ranging from -1 to +7, depending on the compound.
- **Fluorine (F)**: Is the most electronegative element and always has a -1 oxidation state in compounds. It never exhibits a positive oxidation state.

3. **Identify the Element**: Among the options, Fluorine (F) is unique because it never has a positive oxidation state in any of its compounds due to its high electronegativity.

4. **Conclusion**: Therefore, the element that never has a positive oxidation state in any of its compounds is **Fluorine (F)**.

### Final Answer:
**Fluorine (F)**

---