Which of the following represents the correct order of ionic character?

Among the following,the maximum covalent character is shown by the compound:

Polarisability of halide ions increases in the order:

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

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

Given below are two statements:
Statement $I$: The correct order in terms of bond dissociation enthalpy is $Cl_{2} > Br_{2} > F_{2} > I_{2}$.
Statement $II$: The correct trend in the covalent character of the metal halides is $[SnCl_{4} > SnCl_{2}]$, $[PbCl_{4} > PbCl_{2}]$ and $[UF_{4} > UF_{6}]$.
In the light of the above statements, choose the correct answer from the options given below: