Which of the following compounds has the strongest intermolecular forces?

• A. N2
• B. CH4
• C. CO2
• D. H2O

Answer: (D)

Verified step by step guidance

1. Identify the types of intermolecular forces present in each compound: N\_2, CH\_4, CO\_2, and H\_2O. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
2. Recognize that N\_2, CH\_4, and CO\_2 are nonpolar molecules, so their primary intermolecular forces are London dispersion forces, which are generally weaker.
3. Note 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.
4. Compare the strength of hydrogen bonding in H\_2O to the London dispersion forces in the other molecules, understanding that hydrogen bonding significantly increases intermolecular attraction.
5. Conclude that because hydrogen bonding is stronger than London dispersion forces, H\_2O has the strongest intermolecular forces among the given compounds.