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

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(B) According to $Fajans'$ rule,the ionic character of a compound depends on the polarizing power of the cation. As the size of the cation increases,i

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. 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 ($Li^+$,$Be^{2+}$,$Mg^{2+}$,$Rb^+$),$Rb^+$ has the largest size,resulting in the greatest ionic character for $RbCl$. Conversely,$Be^{2+}$ has the smallest size and highest charge density,giving it the highest polarizing power,which results in the least ionic (most covalent) character for $BeCl_2$. Therefore,the compound with the greatest ionic character is $RbCl$ and the one with the least ionic character is $BeCl_2$. Hence,option $B$ is correct.

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

Similar Questions

Which of the following orders is incorrect?

Assertion $(A)$: Covalent character follows $NaCl < MgCl_2 < BeCl_2 < LiCl$.
Reason $(R)$: According to Fajan's rules,covalent character of ionic compounds increases with decrease in size of cation.

The correct order of increasing ionic character is:

Which of the following molecules is the most covalent?

Which compound has the lowest melting point?

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