Fluorine does not exhibit positive oxidation states because 

Options

A. it is the most electronegative element
B. of absence of d-orbitals in its valency shell
C. it is the element with highest EA
D. of it's high ionisation energy

Answer

### Step-by-Step Solution:

1. **Understanding Oxidation States**:
- Oxidation states indicate the degree of oxidation (loss of electrons) of an atom in a compound. Positive oxidation states occur when an atom loses electrons.

2. **Properties of Fluorine**:
- Fluorine is the lightest halogen and is known to be the most electronegative element in the periodic table. This means it has a strong tendency to attract electrons towards itself.

3. **Electronegativity and Positive Oxidation States**:
- For an element to exhibit a positive oxidation state, it must be able to lose electrons. However, since fluorine is the most electronegative element, it tends to gain electrons rather than lose them.

4. **Absence of D Orbitals**:
- Fluorine does not have d orbitals in its valence shell. The absence of these orbitals means that it cannot accommodate additional electrons or participate in bonding that would allow it to exhibit positive oxidation states.

5. **Comparison with Other Elements**:
- Other elements in the periodic table can exhibit positive oxidation states because they can lose electrons more easily, especially those with available d orbitals that can stabilize the positive charge.

6. **Conclusion**:
- Therefore, the primary reason fluorine does not exhibit positive oxidation states is that it is the most electronegative element, which makes it more favorable for fluorine to gain electrons rather than lose them.

### Final Answer:
Fluorine does not exhibit positive oxidation states because it is the most electronegative element.

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