Covalent Character of Ionic Bonds and Polar Character of Covalent Bond

${\mathrm{AlCl}}_3$ is an electron deficient compound but ${\mathrm{AlF}}_3$ is not. This is because

Assertion $\left(\mathrm{A}\right):$ Covalent character follows: $\mathrm{NaCl}<{\mathrm{MgCl}}_2<{\mathrm{BeCl}}_2<\mathrm{LiCl}$
Reason $\left(\mathrm{R}\right):$ According to Fajan's rules, covalent character of ionic compounds increases with decrease in size of cation.

Which of the following compounds is polar ?

Which of the alkaline earth metal halides given below is essentially covalent in nature?

Amongst $\mathrm{LiCl}, \mathrm{RbCl}, {\mathrm{BeCl}}_2 \text{and} {\mathrm{MgCl}}_2$, the compounds with the greatest and the least ionic character, respectively, are.

The most polarisable ion among the following is.

Choose the correct statement with reference to water and hydrogen peroxide. 

The electronic configuration ${\mathrm{Hg}}^{2+}$is _____.

Polarising action of ${\mathrm{Cd}}^{2+}$on anion is stronger than that of ${\mathrm{Ca}}^{2+}$because

Statement-I. $\mathrm{LiCl}$ is covalent whereas $\mathrm{NaCl}$ is ionic.

Statement-2. Greater the size of the cation, greater is its polarising power.

Incorrect option among the following is :

What is the correct order of decreasing polarisability of the following ions?

${\mathrm{Cl}}^{-}, {\mathrm{Br}}^{-}, {\mathrm{l}}^{-}, {\mathrm{F}}^{-}$

What will be the correct sequence of increasing covalent character ?

Predict the correct order of ionic radius.

Which option represents correct order of increasing covalent character of chlorides?

$\mathrm{ }\mathrm{C}-\mathrm{C}\mathrm{l}$ bond enthalpy is greater than $\mathrm{C}\mathrm{ }–\mathrm{I}$ bond, because:

The sequence of the polarizability of ${\mathrm{I}}^{–},\mathrm{ }\mathrm{B}{\mathrm{r}}^{–},\mathrm{ }\mathrm{C}{\mathrm{l}}^{–}and\mathrm{ }{\mathrm{F}}^{–}$ ions is

The solubility of $\mathrm{CsF}$ is more than $\mathrm{CsI}$. Which of the following factor satisfy this statement?