Which of the following intermolecular forces is present in ammonia (NH_3)?

• A. London dispersion forces only
• B. Ion-dipole interactions
• C. Metallic bonding
• D. Hydrogen bonding

Answer: (D)

Verified step by step guidance

1. Identify the molecular structure of ammonia (NH_3). Ammonia consists of one nitrogen atom bonded to three hydrogen atoms, with a lone pair of electrons on the nitrogen.
2. Recall the types of intermolecular forces: London dispersion forces, dipole-dipole interactions, hydrogen bonding, ion-dipole interactions, and metallic bonding.
3. Determine if ammonia can exhibit hydrogen bonding. Hydrogen bonding occurs when hydrogen is directly bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine, and there is a lone pair on the electronegative atom.
4. Since NH_3 has hydrogen atoms bonded to nitrogen (a highly electronegative atom) and nitrogen has a lone pair, ammonia molecules can form hydrogen bonds with each other.
5. Conclude that the dominant intermolecular force in ammonia is hydrogen bonding, although London dispersion forces are also present but weaker; ion-dipole and metallic bonding do not apply here.