In the compounds LiCl,RbCl,BeCl_2,and MgCl_2, | 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 ha

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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),$Li^+$ ($+1$ charge),$Mg^{2+}$ ($+2$ charge),and $Be^{2+}$ (smallest,$+2$ charge). $RbCl$ has the largest cation with the lowest charge,making it the most ionic. $BeCl_2$ has the smallest cation with the highest charge,making it the least ionic (most covalent). Therefore,the most ionic is $RbCl$ and the least ionic is $BeCl_2$.

In the compounds $LiCl$,$RbCl$,$BeCl_2$,and $MgCl_2$,which of the following are the most and least ionic in nature,respectively?

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