Which of the following has the lowest melting point?

The combination of which of the following gives an ionic compound with maximum covalent character?

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:

Which of the following statements regarding the order of covalent character are correct?
$A. KF > KI ; LiF > KF$
$B. KF < KI ; LiF > KF$
$C. SnCl_4 > SnCl_2 ; CuCl > NaCl$
$D. LiF > KF ; CuCl < NaCl$
$E. KF < KI ; CuCl > NaCl$

Among the compounds $LiCl$,$RbCl$,$BeCl_2$,and $MgCl_2$,which compounds possess the highest and lowest ionic character,respectively?

Which of the following is in the increasing order of the ionic character?