"NaBr, MgF"_2 and "Ca"_3("PO"_4)_2 are all ionic compounds with strong ionic attractions.
The attractions are smallest in "NaBr" (only +1 ions), stronger in "MgF"_2 ( +1 and +2 ions) and strongest in "Ca"_3("PO"_4)_2 (+2 and +3 ions).
The remaining compounds are all covalent.
"H"_2 — Lowest boiling point because it has low molecular mass and weak London dispersion forces of attraction.
"H"_2"S" — Higher molecular mass and higher London dispersion forces. The "S-H" bonds are almost nonpolar, so the dipole-dipole forces are quite weak.
"HCl" — Polar bond, so stronger dipole-dipole forces.
"CCl"_4 — Nonpolar molecule, but more atoms and high molecular mass. ∴ Strong London dispersion forces.
"H"_2"O" — Strong hydrogen bonds between the molecules.
Thus, the predicted order of boiling points is
"H"_2 < "H"_2"S < HCl < CCl"_4 < "H"_2"O" < "NaBr < MgF"_2 < "Ca"_3("PO"_4)_2