The normal boiling point for HBr is higher than the normal boiling point for HCl.This can be explained by A) larger dipole-dipole forces for HBr. B) larger dispersion forces for HBr. C) larger hydrogen-bond forces for HBr. D) larger dipole-dipole forces, larger dispersion forces, and larger hydrogen-bond forces for HBr.

Question

Quizplus · Accepted Answer

The correct explanation involves dispersion forces. The molecules in question are HBr and HCl. HBr has a larger molecular mass compared to HCl, which leads to larger dispersion forces due to the increased number of electrons and thus a larger electron cloud that can be more easily polarized. This results in a higher boiling point for HBr. The other types of intermolecular forces mentioned (dipole-dipole and hydrogen bonding) do not differ significantly between these two molecules because both are diatomic molecules with similar electronegativity differences and neither forms hydrogen bonds in the conventional sense.

The Normal Boiling Point for H Br Is Higher

The Normal Boiling Point for HBr Is Higher