Question

Which of the following would show hydrogen bonding? (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (b) (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (d) HF

Short answer

Answer: All compounds (a) CH3OH, (c) CH3NH2, and (d) HF exhibit hydrogen bonding as they contain hydrogen atoms bonded to highly electronegative atoms (N, O, or F).

Step-by-step solution

Identify the hydrogen-bonding criteria

To exhibit hydrogen bonding, a compound must contain a hydrogen atom bonded to a highly electronegative atom (N, O, or F). We will now check each compound to see if it meets this criterion.

Analyze compound (a)

Compound (a) is \(\mathrm{CH}_{3} \mathrm{OH}\). We can see that there is a hydrogen atom bonded to an oxygen atom. Since oxygen is a highly electronegative atom, compound (a) meets the criteria for hydrogen bonding.

Analyze compound (b)

There is no compound (b) given in the exercise. We will move on to compound (c).

Analyze compound (c)

Compound (c) is \(\mathrm{CH}_{3} \mathrm{NH}_{2}\). In this compound, we can see that there is a hydrogen atom bonded to a nitrogen atom. Nitrogen is also a highly electronegative atom, so compound (c) meets the criteria for hydrogen bonding.

Analyze compound (d)

Compound (d) is \(\mathrm{HF}\). Here, we can see that there is a hydrogen atom bonded to a fluorine atom. Fluorine is a highly electronegative atom, which means compound (d) also meets the criteria for hydrogen bonding.

Conclude the answer

Based on our analysis, compounds (a) \(\mathrm{CH}_{3} \mathrm{OH}\), (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\), and (d) HF meet the criteria for hydrogen bonding as they contain hydrogen atoms bonded to highly electronegative atoms (N, O, or F).