Multiple Choice
Which of the following molecules would exhibit the strongest dipole-dipole interactions?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
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Which of the following substances exhibits hydrogen bonding as its strongest intermolecular force?
A
H2O
B
CO2
C
CH4
D
CCl4
Verified step by step guidance1
Identify the key requirement for hydrogen bonding: a hydrogen atom must be directly bonded to a highly electronegative atom such as nitrogen (N), oxygen (O), or fluorine (F).
Examine each substance to see if it contains hydrogen atoms bonded to N, O, or F: H2O has hydrogen atoms bonded to oxygen; CO2 has no hydrogen atoms; CH4 has hydrogen atoms bonded to carbon; CCl4 has no hydrogen atoms.
Recall that hydrogen bonding is a special, strong type of dipole-dipole interaction that occurs only when hydrogen is bonded to N, O, or F, making H2O capable of hydrogen bonding.
Understand that CO2 and CCl4 are nonpolar molecules with only London dispersion forces as their strongest intermolecular force, and CH4, although it has hydrogen, does not have hydrogen bonded to N, O, or F, so it cannot form hydrogen bonds.
Conclude that among the given substances, H2O exhibits hydrogen bonding as its strongest intermolecular force.
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