arrange the compounds below in decreasing order of the ionic character of the bonds in them. that is, pick 1 for the compound with the most ionic bonds, pick 2 for the compound with the next most ionic bonds, and so on.

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# Brief Explanations:
Ionic character is determined by the difference in electronegativity between the atoms in a compound. The greater the electronegativity difference, the more ionic the bond.
- $Cl_2$ is a non - polar covalent compound (electronegativity difference $= 0$), so it has the least ionic character ($4$).
- $SCl_4$ is a covalent compound. The electronegativity difference between $S$ ($2.58$) and $Cl$ ($3.16$) is relatively small.
- For ionic compounds $LiCl$ and $CsCl$, we use the trend in electronegativity of metals. Electronegativity of $Li=0.98$, $Cs = 0.79$, and $Cl = 3.16$. The electronegativity difference for $LiCl$ is $|3.16 - 0.98|=2.18$, and for $CsCl$ is $|3.16 - 0.79| = 2.37$. But due to the smaller size of $Li^+$ compared to $Cs^+$,  according to Fajan's rules, $LiCl$ has more covalent character than $CsCl$. So $CsCl$ ($2$) has more ionic character than $LiCl$ ($3$).

# Answer:
$Cl_2$ ($4$) $<$ $SCl_4$ ($3$) $<$ $LiCl$ ($2$) $<$ $CsCl$ ($1$)

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