Which of the following substances has the strongest intermolecular forces?

• A. N2 (nitrogen)
• B. CO2 (carbon dioxide)
• C. H2O (water)
• D. CH4 (methane)

Answer: (C)

Verified step by step guidance

1. Identify the types of intermolecular forces present in each substance: N\_2, CO\_2, H\_2O, and CH\_4. These forces can include London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
2. Recognize that N\_2 and CO\_2 are nonpolar molecules, so their intermolecular forces are primarily London dispersion forces, which are generally weaker.
3. Note that CH\_4 is also nonpolar, so it mainly exhibits London dispersion forces as well.
4. Understand that H\_2O is a polar molecule with a bent shape, allowing it to form hydrogen bonds, which are a special and much stronger type of dipole-dipole interaction.
5. Conclude that because hydrogen bonding is stronger than London dispersion forces and regular dipole-dipole interactions, H\_2O has the strongest intermolecular forces among the given substances.