Which of the following molecules can form hydrogen bonds...

Which of the following molecules can form hydrogen bonds with molecules of water? (a) methanol (CH $_{3} \mathrm{OH}$ ); (b) ethane $\left(\mathrm{CH}_{3} \mathrm{CH}_{3}\right) ;$ (c) dimethyl ether $\left(\mathrm{CH}_{3} \mathrm{OCH}_{3}\right)$ (d) acetic acid (CH $_{3} \mathrm{COOH}$ )

Key Concepts

Polarity and Functional Groups

The ability of a molecule to engage in hydrogen bonding is often linked to the presence of polar functional groups. The distribution of electrical charge within a molecule, due to differences in electronegativity among atoms, creates regions of partial positive and negative charges. Functional groups that include highly electronegative atoms not only contribute to the overall polarity of the molecule but also provide sites for hydrogen bonding, which is essential for interactions with water.

Hydrogen Bond Donors and Acceptors

Molecules capable of hydrogen bonding contain either hydrogen bond donors or acceptors. A hydrogen bond donor is typically a hydrogen atom attached directly to an electronegative atom, making the hydrogen partially positive and able to engage in bonding with other electronegative atoms. Conversely, a hydrogen bond acceptor is an electronegative atom with one or more lone pairs that can interact with a hydrogen from another molecule’s hydrogen bond donor. This dual capacity underlies many of the interactions in aqueous environments.

Hydrogen Bonding

Hydrogen bonding is a specific, strong type of dipole-dipole interaction that occurs when a hydrogen atom covalently bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine, is attracted to a lone pair of electrons on another electronegative atom. This interaction plays a critical role in determining the physical properties of substances and their solubility in water.

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