Which of the following compounds exhibits hydrogen bonding?

• A. CO2
• B. CH4
• C. CCl4
• D. NH3

Answer: (D)

Verified step by step guidance

1. Understand what hydrogen bonding is: it is a special type of dipole-dipole interaction that occurs when hydrogen is directly bonded to highly electronegative atoms such as nitrogen (N), oxygen (O), or fluorine (F).
2. Examine each compound to see if it contains hydrogen atoms bonded to N, O, or F:
3. For CO2, the molecule is linear with carbon double bonded to oxygen atoms, but there are no hydrogen atoms present, so no hydrogen bonding.
4. For CH4 (methane), hydrogen atoms are bonded to carbon, which is not electronegative enough to create hydrogen bonding.
5. For CCl4 (carbon tetrachloride), there are no hydrogen atoms at all, so hydrogen bonding cannot occur.
6. For NH3 (ammonia), hydrogen atoms are bonded directly to nitrogen, which is highly electronegative, allowing for hydrogen bonding to occur.