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Explain why fluorine exhibits an oxidation state of -1 only while other element of the family exhibit oxidation of -1, +1 , +3, +5, +7
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because fluorine is the most electronegative element, so it can't exhibit any positive oxidation state
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Fluorine exhibits only -1 oxidation state because it does not have vacant d orbital , So it can't expand its oxidation state. Moreover, fluorine being highly electronegative can't show positive oxidation state.
The other highre members of group 17 have vacant d orbital. So , they are able to show variable oxidation state.
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