Can you rank the following molecules in order of increasing boiling point: NaF (salt), H2S, HF, CO2?

CO₂ < H₂S < HF < NaF

Nonpolar Molecules (Symmetrical distribution of charge)=London Dispersion (weakest IMF's, lowest boiling point); Polar Molecules (Asymmetrical distribution of charge)=Dipole-Dipole Forces; Molecules with H-F, H-O, or H-N (because of big EN)=Hydrogen Bonding; Saltwater (ionic compound and water)=Ion-Dipole Forces (strongest IMF's, highest boiling point). CO2 is nonpolar (symmetrical distribution of charge), so it has London forces. H2S is a polar molecule (asymmetrical distribution of charge) without H-F, H-O, or H-N, so it has dipole-dipole forces. HF has F-H in its structure, so it has hydrogen bonding. NaF is an ionic compound, so it has ion-ion opposite attractions. In order, London forces are weakest, dipole-dipole forces are stronger, hydrogen bonds are even stronger than dipole-dipole, and ion-ion forces are strongest.*##**##*