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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

$RbCl$ and $BeCl_2$

Vedclass · Answer

(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

The covalent character of $CaCl_2, BaCl_2, SrCl_2$ and $MgCl_2$ follows the order:

Which of the following bonds is the most covalent?

Which compound has the lowest melting point?

Which of the following compounds exhibits covalent character?

The charge/size ratio of a cation determines its polarizing power. Which of the following sequences represents the increasing order of the polarizing power of the cations $K^+$,$Ca^{2+}$,$Mg^{2+}$,and $Be^{2+}$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module