Explain why fluorine always exhibit an oxidation state of -1 ?

Explanation

(i) The electronic configuration of fluorine is `1s^(2) 2s^(2) 2p_(x)^(2) 2p_(y)^(2)2p_(z)^(1)`.
(ii) To attain the noble gas configuration it gains one electrons and exhibits -1 oxidation state.
(iii) Fluorine is most electronegative atom so does not exhibit positive oxidation state.
(iv) Since it cannot expand its octet due to non availability of d-orbitals.