To determine the intermolecular forces present in ethanol (
), we need to consider the following types of forces:1. **Hydrogen Bonds**: Ethanol has an -OH group, which can form hydrogen bonds. The hydrogen atom attached to the oxygen can act as a hydrogen bond donor, and the lone pairs on the oxygen atom can act as hydrogen bond acceptors.2. **Dipole-Dipole Attractions**: Ethanol is a polar molecule due to the presence of the -OH group, leading to dipole-dipole interactions between molecules.3. **London Dispersion Forces**: All molecules, including ethanol, exhibit London dispersion forces (also known as van der Waals forces). These are weak intermolecular forces that arise from temporary dipoles induced in atoms or molecules.Given these points, the correct answer should include all three types of intermolecular forces: hydrogen bonds, dipole-dipole attractions, and London dispersion forces.Therefore, the correct answer is:B. Hydrogen-bonds, dipole-dipole attractions, London dispersion forces