Question

Which answer describes hydrogen bonding?

a. The attraction between hydrogen and lone electron pairs of a strongly electronegative molecule.
b. The attraction between hydrogen and the permanent dipole of a weakly electronegative molecule.
c. The attraction between hydrogen and a permanent dipole of a weakly electronegative molecule.
d. The attraction between hydrogen and an induced dipole of a strongly electronegative molecule.

Answer 1

Hydrogen bonding is the attraction between a hydrogen atom covalently bonded to a strongly electronegative atom and a lone pair of electrons on an atom in a neighboring molecule. It is a strong dipole interaction but much weaker than a covalent bond, constituting about 5% of its strength.

Step-by-step explanation:

The correct description of hydrogen bonding is option a: The attraction between a hydrogen atom and a lone pair of electrons on a strongly electronegative atom. Hydrogen bonds occur when a hydrogen atom that is covalently bonded to one of the three most electronegative elements (fluorine, oxygen, or nitrogen) is attracted to a lone pair of electrons on an atom in a neighboring molecule.

This type of intermolecular force is an exceptionally strong dipole interaction, although it is much weaker than a covalent bond. The hydrogen bond strength is approximately 5% of that found in a covalent bond, and this attraction is critical in determining the properties of water, among other substances.