Multiple Choice
Which factor primarily determines the strength of dipole-dipole interactions between molecules?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
Multiple Choice
What is the strongest intermolecular force possible between molecules of ammonia (NH_3)?
A
Hydrogen bonding
B
Dipole-dipole interactions
C
Ion-dipole interactions
D
London dispersion forces
Verified step by step guidance1
Identify the types of intermolecular forces that can occur between molecules: London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ion-dipole interactions.
Examine the molecular structure of ammonia (NH_3). Note that nitrogen is highly electronegative and bonded to hydrogen atoms, creating a polar molecule with a significant dipole moment.
Determine if hydrogen bonding is possible by checking if hydrogen is directly bonded to a highly electronegative atom such as nitrogen, oxygen, or fluorine. In NH_3, hydrogen is bonded to nitrogen, which satisfies this condition.
Recognize that hydrogen bonding is a special, stronger type of dipole-dipole interaction that occurs when hydrogen is bonded to N, O, or F, making it stronger than regular dipole-dipole forces and London dispersion forces.
Conclude that the strongest intermolecular force in ammonia is hydrogen bonding because of the N-H bonds and the molecule's polarity.
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