Final answer:
CH3OH (methanol) exhibits hydrogen bonding, dipole-dipole interactions, and London dispersion forces, due to the presence of a hydroxyl group and the polar bonds within the molecule. Ionic bonding is not present in this molecular substance.
Step-by-step explanation:
Intermolecular Forces in CH3OH (Methanol)
The types of intermolecular forces present in CH3OH(l), which is methanol in the liquid state, include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Methanol can engage in hydrogen bonding because it has a hydrogen atom bonded to an oxygen atom, which is one of the most electronegative elements. Dipole-dipole interactions are present because methanol possesses permanent dipole moments due to the polar bonds between carbon and oxygen, as well as oxygen and hydrogen. Finally, London dispersion forces exist in all molecular substances, including methanol, due to temporary, instantaneous dipoles that occur as electrons move around the nucleus. Therefore, the correct answers are: A) Hydrogen bonding, B) Dipole-dipole interactions, and C) London dispersion forces. Ionic bonding (D) is not present in CH3OH, as it is a molecular compound, not an ionic compound.