MCQ
Amongst $LiCl, BeCl_2, MgCl_2$ and $RbCl$ the compounds with greatest and least ionic character, respectively are
- A$LiCl$ and $RbCl$
- ✓$RbCl$ and $BeCl_2$
- C$RbCl$ and $MgCl_2$
- D$MgCl_2$ and $BeCl_2$
✓
Answer
Correct option: B.
$RbCl$ and $BeCl_2$
b
as the size of the cation increases ionic character increases,so among the given chlorides the Rb is having larger sine and the element having least size is Be. So, the compound having more ionic character is $\mathrm{RbCl}$.
as the size of the cation increases ionic character increases,so among the given chlorides the Rb is having larger sine and the element having least size is Be. So, the compound having more ionic character is $\mathrm{RbCl}$.
The compound having more ionic character is $\mathrm{BeCl}_{2}$. Hence option $\mathrm{B}$ is correct.
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