Which of the following halogens does not exhi | vedclass

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(D) Fluorine $(F)$ is the most electronegative element in the periodic table.Due to its high electronegativity and the absence of $d$-orbitals in its

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$F$

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(D) Fluorine $(F)$ is the most electronegative element in the periodic table.Due to its high electronegativity and the absence of $d$-orbitals in its valence shell,it cannot expand its octet or share electrons in a way that results in a positive oxidation state.Therefore,fluorine always exhibits an oxidation state of $-1$ in its compounds.In contrast,other halogens like chlorine $(Cl)$,bromine $(Br)$,and iodine $(I)$ possess vacant $d$-orbitals and lower electronegativity,allowing them to exhibit positive oxidation states such as $+1, +3, +5$,and $+7$.

Which of the following halogens does not exhibit a positive oxidation state in its compounds?

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