Amongst LiCl,RbCl,BeCl_{2},and MgCl_{2},the c | vedclass

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(B) According to Fajan's rule,the ionic character of a bond depends on the polarizing power of the cation.Greater size of the cation and smaller charg

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$RbCl$ and $BeCl_{2}$

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(B) According to Fajan's rule,the ionic character of a bond depends on the polarizing power of the cation.Greater size of the cation and smaller charge on the cation lead to less polarization,resulting in more ionic character.Comparing the cations: $Rb^+$ is the largest with a $+1$ charge,making $RbCl$ the most ionic.$Be^{2+}$ is the smallest with a $+2$ charge,leading to the highest polarization and the least ionic (most covalent) character.Therefore,$RbCl$ has the greatest ionic character and $BeCl_{2}$ has the least ionic character.

Amongst $LiCl$,$RbCl$,$BeCl_{2}$,and $MgCl_{2}$,the compounds with the greatest and the least ionic character,respectively,are

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