Rank the following compounds in order of decreasing boiling point: sodium bromide (nabr), carbon tetrafluoride (cf4), and chloroform (chcl3) rank from highest to lowest boiling point. to rank items as equivalent, overlap them.

     Highest to lowest boiling point is

NaBr > CHCl3 > CF4

NaBr - ionic

CHCl3 - dipole - dipole

CF4 - dispersion force

If Intermolecular forces are strong then the molecule will have greater boiling point as it requires more energy to break the bond between molecules and convert them from liquid to gas.

As NaBr is an ionic compound(Na is a metal and Br is non metal).

Hence it has the strongest intermoleuclar force of attraction and it will have the highest boiling point.

CHCl3 and CF4 are covalent compounds.

But CHCl3 is polar covalent compound hence it  has higher boiling point than CF4.

CF4 is non polar covalent compound [due to the regular or symmetrical structure of CF4,where C-F bond is polar but the CF4 molecule as a whole is not polar as the polarity cancels out due to equal pulling of electrons by F towards all sides]

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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