(B) According to Fajan's rule,small cations with high charge have high polarizing power,leading to covalent character in ionic bonds.$Be^{2+}$ is a sm

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(B) According to Fajan's rule,small cations with high charge have high polarizing power,leading to covalent character in ionic bonds.$Be^{2+}$ is a small cation with a high charge density compared to $Na^+$,$Li^+$,and $Rb^+$.Therefore,$BeCl_2$ exhibits significant covalent character,whereas $NaCl$,$LiCl$,and $RbF$ are predominantly ionic compounds.

Class 11 Chemistry Chemical Bonding and Molecular Structure Polarisation and Fajan’s rule

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Which one of the following is a covalent molecule?

A
$NaCl$
B
$BeCl_2$
C
$LiCl$
D
$RbF$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Chemical Bonding and Molecular Structure

Subtopic

Polarisation and Fajan’s rule

The melting points of $(i)$ $BeCl_2$, $(ii)$ $CaCl_2$, and $(iii)$ $HgCl_2$ follow the order:

MediumWBJEE 2019

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Which of the following represents the correct solubility order?

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The bond between two non-metallic elements having maximum covalent character is ...........

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$STATEMENT-1$: Boron always forms covalent bonds.
Because
$STATEMENT-2$: The small size of $B^{3+}$ favors the formation of covalent bonds.

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Which of the following statements about $LiCl$ and $NaCl$ is correct?

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Which one of the following is a covalent molecule?

Similar Questions

The melting points of $(i)$ $BeCl_2$, $(ii)$ $CaCl_2$, and $(iii)$ $HgCl_2$ follow the order:

Which of the following represents the correct solubility order?

The bond between two non-metallic elements having maximum covalent character is ...........

$STATEMENT-1$: Boron always forms covalent bonds.Because$STATEMENT-2$: The small size of $B^{3+}$ favors the formation of covalent bonds.

Which of the following statements about $LiCl$ and $NaCl$ is correct?

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$STATEMENT-1$: Boron always forms covalent bonds.
Because
$STATEMENT-2$: The small size of $B^{3+}$ favors the formation of covalent bonds.