Which of the following statements about hydrogen bonds is true?

The statement that hydrogen bonds involve a hydrogen atom and a polar molecule is accurate because hydrogen bonds are a type of dipole-dipole interaction that occurs between molecules containing hydrogen atoms bonded to highly electronegative atoms, such as oxygen, nitrogen, or fluorine. In these cases, the hydrogen atom carries a partial positive charge due to its weak bond with the electronegative atom, while the other molecule has a region of partial negative charge. This polarity allows for the attraction between different molecules.

Hydrogen bonds are essential in many biological processes, such as the formation of DNA strands and the properties of water. For example, they contribute to the high boiling point of water, its surface tension, and its ability to dissolve many substances, thereby playing a crucial role in biological systems.

The incorrect options highlight common misconceptions about hydrogen bonds. For instance, they are not particularly strong or irreversible, as they can be easily broken and reformed, contributing to their dynamic nature in liquid environments. Additionally, hydrogen bonds do not occur exclusively between non-polar molecules; rather, they specifically require polar molecules where a hydrogen atom is bonded to an electronegative atom. Furthermore, they can indeed exist in both solid and liquid states, as seen in ice and liquid water