Multiple Choice
Which of the following best explains why water (H_2O) has a much higher boiling point than would otherwise be predicted?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
Multiple Choice
Which of the following represents the intermolecular forces present in CO₂?
A
Dipole-dipole forces only
B
London dispersion forces only
C
London dispersion and dipole-dipole forces
D
Hydrogen bonding only
Verified step by step guidance1
Step 1: Identify the molecular structure and polarity of CO₂. Carbon dioxide (CO₂) is a linear molecule with two polar C=O bonds arranged symmetrically.
Step 2: Determine the overall molecular polarity. Because the molecule is linear and symmetrical, the dipole moments of the two C=O bonds cancel each other out, making CO₂ a nonpolar molecule.
Step 3: Understand the types of intermolecular forces. Dipole-dipole forces occur between polar molecules, hydrogen bonding occurs when H is bonded to N, O, or F, and London dispersion forces (also called induced dipole-induced dipole forces) occur in all molecules but are the only forces in nonpolar molecules.
Step 4: Since CO₂ is nonpolar, it does not exhibit dipole-dipole forces or hydrogen bonding. Therefore, the only intermolecular forces present are London dispersion forces.
Step 5: Conclude that the correct representation of intermolecular forces in CO₂ is 'London dispersion forces only.'
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