Final answer:
HCl molecules interact through London dispersion forces and dipole-dipole interactions but not through hydrogen bonding because the H is not bonded to an atom that allows for this stronger interaction, like O, N, or F.
Step-by-step explanation:
Hydrogen chloride (HCl) molecules interact with other like molecules through two types of intermolecular forces: London dispersion forces and dipole-dipole interactions. These are types of van der Waals forces. HCl is a polar molecule due to the considerable electronegativity difference between hydrogen and chlorine.
Therefore, there are dipole-dipole attractions between the positive end of one HCl molecule and the negative end of another. Additionally, all molecules, including HCl, exhibit London dispersion forces, which are due to the formation of instantaneous dipole moments that occur because of fluctuations in the electron distribution within molecules.
HCl does not engage in hydrogen bonding because hydrogen is not bonded to one of the highly electronegative atoms (O, N, or F) that are necessary to form a hydrogen bond. As a result, HCl molecules can interact through dispersion and dipole forces but not hydrogen bonding.