Which type of intermolecular force is primarily responsible for the higher boiling point of water (H2O) compared to methane (CH4)?

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

Answer: (C)

Verified step by step guidance

1. Identify the types of intermolecular forces present in both water (H\_2O) and methane (CH\_4).
2. Recognize that methane is a nonpolar molecule, so the primary intermolecular forces it experiences are London dispersion forces.
3. Understand that water is a polar molecule with an oxygen atom bonded to hydrogen atoms, which allows it to form hydrogen bonds, a special and strong type of dipole-dipole interaction.
4. Compare the strength of hydrogen bonding in water to the weaker London dispersion forces in methane, noting that stronger intermolecular forces lead to higher boiling points.
5. Conclude that hydrogen bonding is primarily responsible for the higher boiling point of water compared to methane.