Why does fluorine usually have an oxidation state of negative one in compounds?

Fluorine typically exhibits an oxidation state of −1 in compounds because it possesses the highest electronegativity of all chemical elements. This extreme ability to attract electrons means that fluorine does not give up its own electrons to other elements, which is why it is the only halogen that does not form compounds with positive oxidation states.1

Instead, fluorine strongly tends to gain an electron to achieve a stable octet configuration, effectively becoming a fluoride ion ($F^{-}$) in its interactions. This behavior is further supported by its high electron affinity and the strength of the bonds it forms with other elements, which contribute to the stability of its −1 oxidation state.12