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?

Similar Questions

Which of the following substances has the least covalent character?

Polarisability of halide ions increases in the order:

Which of the following statements regarding the order of covalent character are correct?
$A. KF > KI ; LiF > KF$
$B. KF < KI ; LiF > KF$
$C. SnCl_4 > SnCl_2 ; CuCl > NaCl$
$D. LiF > KF ; CuCl < NaCl$
$E. KF < KI ; CuCl > NaCl$

Which of the following diagrams shows the correct change in the ionic character of the given compounds according to Fajans' rule?

Out of the following,which one has the highest value of covalent character?

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