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Which one of the following substances should exhibit hydrogen bonding in the liquid state?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
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Which of the following substances will exhibit hydrogen bonding between its molecules?
A
CH4
B
CO2
C
C2H6
D
NH3
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Understand what hydrogen bonding is: it is a special type of dipole-dipole interaction that occurs when hydrogen is covalently bonded to highly electronegative atoms such as nitrogen (N), oxygen (O), or fluorine (F).
Examine each substance to see if it contains hydrogen atoms bonded directly to N, O, or F, which is necessary for hydrogen bonding.
For CH4 (methane), hydrogen is bonded to carbon, which is not electronegative enough to create hydrogen bonding.
For CO2 (carbon dioxide), there are no hydrogen atoms present, so hydrogen bonding cannot occur.
For C2H6 (ethane), hydrogen atoms are bonded to carbon atoms, so no hydrogen bonding is possible; however, NH3 (ammonia) has hydrogen atoms bonded directly to nitrogen, which allows it to exhibit hydrogen bonding.
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