Amongst LiCl,RbCl,BeCl_2,and MgCl_2,the compo | vedclass

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(B) According to Fajan's rule,the ionic character of a compound depends on the polarizability of the cation. As the size of the cation increases,its p

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$RbCl$ and $BeCl_2$

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(B) According to Fajan's rule,the ionic character of a compound depends on the polarizability of the cation. As the size of the cation increases,its polarizing power decreases,which leads to an increase in the ionic character of the bond. Among the given cations ($Li^+$,$Rb^+$,$Be^{2+}$,$Mg^{2+}$),$Rb^+$ has the largest ionic radius,resulting in the highest ionic character for $RbCl$. Conversely,$Be^{2+}$ has the smallest size and highest charge density,causing the greatest polarization of the chloride ion,which results in the least ionic (most covalent) character for $BeCl_2$. Therefore,the compound with the greatest ionic character is $RbCl$ and the compound with the least ionic character is $BeCl_2$.

Amongst $LiCl$,$RbCl$,$BeCl_2$,and $MgCl_2$,the compounds with the greatest and least ionic character respectively are:

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