Multiple Choice
Which type of intermolecular force is the strongest in a sample of solid MgCl_2?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
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Which of the following molecules exhibits hydrogen bonding?
A
C2H6
B
CO2
C
CH4
D
NH3
Verified step by step guidance1
Understand the concept of hydrogen bonding: Hydrogen bonding occurs when a hydrogen atom is covalently bonded to a highly electronegative atom such as nitrogen (N), oxygen (O), or fluorine (F), and this hydrogen is attracted to a lone pair of electrons on another electronegative atom in a nearby molecule.
Examine each molecule to identify if it contains hydrogen atoms bonded to N, O, or F:
C2H6 (ethane) has hydrogen atoms bonded only to carbon, which is not electronegative enough to cause hydrogen bonding.
CO2 (carbon dioxide) has no hydrogen atoms at all, so it cannot exhibit hydrogen bonding.
CH4 (methane) has hydrogen atoms bonded to carbon, similar to C2H6, so it also cannot exhibit hydrogen bonding.
NH3 (ammonia) has hydrogen atoms bonded directly to nitrogen, which is highly electronegative and has lone pairs, making it capable of hydrogen bonding.
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