Question

Why does fluorine exhibit only −1 oxidation state in all of its compounds?

Answer 1

1. Fluorine is the most electronegative element and has a strong tendency to gain exactly one electron to complete its valence shell.
2. It has no vacant d-orbitals in its valence shell to expand its octet.
3. Fluorine cannot show positive oxidation states because it cannot share or lose electrons beyond the one it gains.
4. Hence, fluorine always exhibits only the −1 oxidation state in all its compounds.
5. Other halogens show multiple oxidation states due to available d-orbitals and less electronegativity