The sole oxidation state of fluorine, consistently -1, stems from its electronic configuration and the lack of d orbitals. As the most electronegative element, fluorine readily accepts an electron to achieve a stable, complete valence shell (octet).
Fluorine's electronic configuration is \(1s^2 2s^2 2p^5\). Its valence shell needs one electron to fill the 2p orbital. The absence of d orbitals prevents fluorine from expanding its valence shell, a capability that allows other elements to exhibit varying oxidation states.
Consequently, fluorine exclusively displays a -1 oxidation state because it cannot share or donate electrons to form positive oxidation states, a direct result of its d orbital deficiency.
Factors
Impact on Oxidation State
Electronegativity
High
d Orbitals
Absent
Size
Small
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