Final answer:
Propanol exhibits dipole-dipole interactions, hydrogen bonding, and London dispersion forces due to its polar nature and the presence of a hydrogen atom bonded to an electronegative oxygen atom.
Step-by-step explanation:
When identifying the intermolecular forces present in propanol (CH3CH2CH2OH), we consider both the molecular structure and the types of atoms involved. Propanol is a polar molecule due to the presence of an -OH (hydroxyl) group, which leads to an uneven distribution of electrons. This gives rise to dipole-dipole interactions, as there is a separation of charge within the molecule, resulting in a partial positive and a partial negative end that can interact with the opposites in nearby molecules.
Additionally, since propanol contains a hydrogen atom directly attached to an electronegative oxygen atom, it is capable of forming hydrogen bonds. Hydrogen bonding is a specific type of dipole-dipole interaction that is particularly strong and significantly influences the physical properties of a compound, such as its boiling point.
Although not specifically mentioned in the student's question, it's worth noting that all molecules also exhibit London dispersion forces (otherwise known as van der Waals forces), which are temporary dipole interactions that occur even in nonpolar molecules due to transient shifts in electron density.
Therefore, the correct intermolecular forces present in propanol are dipole-dipole interactions and hydrogen bonding, with London dispersion forces also playing a role to a lesser extent.