Why fluorine does not exhibit any positive oxidation state?

Explanation

Electronic configuration of `F` is `1s^(2)2s^(2)2p^(5)`. `F` has only one unpair electorn. As `F` is the highest electronegative element, the possibility of sharing its electron with more electronegative element than itself is not there, hence it cannot show an oxidation state of `+1` . further, due to absence of d-orbitals in its valence shell, the paired electrons present in `2s` or `2p` electrons cannot be unpaired, hence `F` does not shown `+3,+5` or `+7` oxidation state too. Thus, fluorine does not exhibt any positive oxidation state.