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(D) The reducing power of halide ions depends on their ability to lose electrons,which is inversely proportional to the electronegativity of the corre

Vedclass · Accepted Answer

$I^{-}$

Vedclass · Answer

(D) The reducing power of halide ions depends on their ability to lose electrons,which is inversely proportional to the electronegativity of the corresponding halogen atom.As we move down the group from $F$ to $I$,the size of the halide ion increases,and the hold of the nucleus on the valence electrons decreases.Therefore,the ease of oxidation increases in the order: $F^{-} Thus,$I^{-}$ is the strongest reducing agent among the given options.

The strongest reducing agent among the given halide ions is:

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