Answer:
Fluorine has no d-orbitals (2d
orbitals) and there is no scope for any electron promotion. Therefore, fluorine
can show only oxidation state of - 1 in its compounds. However, the other members
of the family have vacant d-orbitals to which electron promotion can readily
take place from the p and s orbitals present in the same shell. As a result,
these elements can show variable oxidation states \[(-1,\,+1,\,+3,\,+5\,\,\text{and}\,+7)\]
in their compounds.
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