In F-, H-, Cl-, Br- , which has smallest radius? And why...

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Solution

As radius depends on effective nuclear charge and effective nuclear charge is the property by which nucleus attracts the electrons and decreases the size. In the case of hydrogen anion the only anion with electron to proton ratio (e/p) =2, as the nuclear charge is less comparable to number of electrons there is more repulsion because nuclear attraction is not good so the electron cloud will expand largely to overcome, resulting in the expansion of ion. While in fluorine ion there is not such increase in size from fluorine..It's a special case when Increase in H to H- size is much larger. Trend in ionic size : F(ion)<Cl(ion)<Br(ion)<H(ion)<I(ion)..

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