Fluorine exhibit only – 1 oxidation state whereas other halogens exhibit +ve oxidation states also. Explain why ?

Explanation

To explain why fluorine exhibits only a -1 oxidation state while other halogens can exhibit positive oxidation states, we can break down the explanation into several steps:

### Step 1: Understanding Oxidation States
- **Oxidation state** refers to the degree of oxidation (loss of electrons) of an atom in a compound. It can be positive or negative depending on whether an atom loses or gains electrons.

### Step 2: Fluorine's Electronegativity
- Fluorine is the most electronegative element in the periodic table. This means it has a strong tendency to attract electrons towards itself. As a result, fluorine typically gains one electron to achieve a stable electron configuration, resulting in a -1 oxidation state.

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