Which type(s) of intermolecular forces are expected between molecules of hydrogen chloride (HCl)?

• A. London dispersion forces only
• B. Dipole-dipole forces and London dispersion forces
• C. Hydrogen bonding only
• D. Ionic bonding

Answer: (B)

Verified step by step guidance

1. Identify the types of atoms involved in the molecule HCl: hydrogen (H) and chlorine (Cl).
2. Determine the polarity of the HCl molecule by comparing electronegativities: chlorine is more electronegative than hydrogen, so the H-Cl bond is polar, creating a permanent dipole moment.
3. Recall that polar molecules exhibit dipole-dipole intermolecular forces due to the attraction between the positive end of one molecule and the negative end of another.
4. Recognize that all molecules, regardless of polarity, experience London dispersion forces (also called induced dipole-induced dipole forces) due to temporary fluctuations in electron distribution.
5. Conclude that HCl molecules exhibit both dipole-dipole forces (because of their polarity) and London dispersion forces (because all molecules have them), but not hydrogen bonding or ionic bonding.