What oxidation state does fluorine always exhibit?

Fluorine always exhibits an oxidation state of -1 in compounds. This is due to its position on the periodic table as the most electronegative element, which means it has a strong tendency to gain electrons. When fluorine bonds with other elements, it typically accepts one electron, resulting in a stable electron configuration akin to that of the noble gases.

For example, in sodium fluoride (NaF), sodium donates one electron to fluorine, allowing fluorine to reach its desired electron configuration while exhibiting an oxidation state of -1. This behavior is consistent across all compounds involving fluorine, making -1 its definitive oxidation state.

The other options do not apply to fluorine in typical circumstances and reflect incorrect oxidation states due to either misinterpretation of its electronegativity or the nature of its chemical bonding.