Multiple Choice
Which type of intermolecular force is primarily responsible for the high boiling point of water (H_2O)?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
Multiple Choice
Which of the following molecules can exhibit hydrogen bonding as a pure liquid?
A
NH3
B
CH4
C
CO2
D
C2H6
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 molecule to see if it contains N-H, O-H, or F-H bonds. For NH3 (ammonia), hydrogen is bonded to nitrogen, which is highly electronegative, so it can form hydrogen bonds.
For CH4 (methane), hydrogen is bonded to carbon, which is not electronegative enough to create hydrogen bonding, so CH4 cannot exhibit hydrogen bonding.
For CO2 (carbon dioxide), there are no hydrogen atoms present at all, so hydrogen bonding is not possible.
For C2H6 (ethane), hydrogen atoms are bonded to carbon atoms, similar to CH4, so it also cannot exhibit hydrogen bonding.
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