Textbook Question
Ammonia, NH₃, is very soluble in water (51.8 g/L at 20 °C and 760 mmHg).Show how NH₃ can hydrogen bond to water.
12. Liquids, Solids, and Intermolecular Forces
Intermolecular Forces (Simplified)
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Which of these molecules exhibit the most number of different intermolecular forces?
A
B
C
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Identify the types of intermolecular forces: The main types of intermolecular forces are London dispersion forces, dipole-dipole interactions, and hydrogen bonding.
Analyze the first molecule (propane): Propane (C3H8) is a nonpolar molecule, so it primarily exhibits London dispersion forces.
Analyze the second molecule (formaldehyde): Formaldehyde (CH2O) is a polar molecule due to the difference in electronegativity between carbon and oxygen, leading to dipole-dipole interactions. It also has London dispersion forces.
Consider hydrogen bonding: For hydrogen bonding to occur, a molecule must have a hydrogen atom attached to a highly electronegative atom (N, O, or F). Neither propane nor formaldehyde can form hydrogen bonds.
Compare the molecules: Propane exhibits only London dispersion forces, while formaldehyde exhibits both London dispersion forces and dipole-dipole interactions. Therefore, formaldehyde exhibits more types of intermolecular forces.
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