Among the compounds LiCl,RbCl,BeCl_2,and MgCl | vedclass

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(B) According to $Fajans'$ rule,the ionic character of a compound depends on the polarizing power of the cation.Smaller cations with higher charge hav

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$RbCl$ and $BeCl_2$

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(B) According to $Fajans'$ rule,the ionic character of a compound depends on the polarizing power of the cation.Smaller cations with higher charge have higher polarizing power,leading to greater covalent character and lower ionic character.Larger cations with lower charge have lower polarizing power,leading to greater ionic character.Comparing the cations: $Rb^+$ (largest,$+1$ charge) has the least polarizing power,making $RbCl$ the most ionic.$Be^{2+}$ (smallest,$+2$ charge) has the highest polarizing power,making $BeCl_2$ the least ionic.Therefore,$RbCl$ has the highest ionic character and $BeCl_2$ has the lowest ionic character.

Among the compounds $LiCl$,$RbCl$,$BeCl_2$,and $MgCl_2$,which compounds possess the highest and lowest ionic character,respectively?

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