Which intermolecular forces are present in a liquid sample of methanol (CH3OH)?

• A. Only hydrogen bonding
• B. London dispersion forces and dipole-dipole forces only
• C. Only London dispersion forces
• D. London dispersion forces, dipole-dipole forces, and hydrogen bonding

Answer: (D)

Verified step by step guidance

1. Identify the molecular structure of methanol (CH\_3OH), noting that it contains a hydroxyl group (-OH) attached to a methyl group (CH\_3).
2. Recognize that all molecules exhibit London dispersion forces due to temporary fluctuations in electron density, so methanol will have these forces.
3. Determine if methanol is polar: the presence of the electronegative oxygen atom bonded to hydrogen creates a permanent dipole, so methanol exhibits dipole-dipole interactions.
4. Check for hydrogen bonding: since methanol has an -OH group where hydrogen is directly bonded to oxygen (a highly electronegative atom), it can form hydrogen bonds with other methanol molecules.
5. Conclude that methanol exhibits all three intermolecular forces: London dispersion forces, dipole-dipole forces, and hydrogen bonding.