Which of the following compounds would have the highest boiling point?

• A. NH_3
• B. CH_4
• C. CO_2
• D. H_2O

Answer: (D)

Verified step by step guidance

1. Identify the types of intermolecular forces present in each compound: NH_3, CH_4, CO_2, and H_2O. These forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
2. Recognize that hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms like nitrogen (N), oxygen (O), or fluorine (F).
3. Analyze each compound: NH_3 has N-H bonds and can form hydrogen bonds; CH_4 is nonpolar and only exhibits London dispersion forces; CO_2 is linear and nonpolar, so it also only has London dispersion forces; H_2O has O-H bonds and can form strong hydrogen bonds.
4. Understand that stronger intermolecular forces lead to higher boiling points because more energy is required to separate the molecules during the phase change from liquid to gas.
5. Conclude that since H_2O can form the strongest hydrogen bonds among the given compounds, it will have the highest boiling point.