Consider the following experimental boiling points:
HF: 20°C
HCl: -85°C
HBr: -67°C
HI: -35°C
Which of the following statements is correct for this set of
compounds and supported by the data given? Select as many as
applicable; however, points will be deducted for incorrect
choices.
Select one or more:
HF has the highest boiling point because of hydrogen bonding.
The high boiling point of HF is due to dipole-dipole forces,
which are absent in the other three compounds.
The boiling point trend for HCl, HBr, and HI can mostly be
explained by the strength of dispersion forces.
The molecule with the strongest intermolecular forces is HI.
The molecule with the strongest intermolecular forces
is HF.
HF has the highest boiling point because it is the most
polarizable of the four compounds.