Final answer:
Hydrogen bonding is correctly described as a weak electrostatic attraction between a hydrogen atom bonded to an electronegative atom and a lone pair of electrons on a neighboring molecule. It's stronger than typical dipole-dipole interactions but much weaker than a covalent bond.
Step-by-step explanation:
The description of hydrogen bonding that best fits is C) Weak electrostatic attraction between hydrogen and electronegative atoms. Hydrogen bonding is an intermolecular or sometimes intramolecular attractive force where a hydrogen atom, covalently bonded to a small, highly electronegative atom such as oxygen, nitrogen, or fluorine, is attracted to a lone pair of electrons on a neighboring molecule.
This enables the formation of a special type of dipole-dipole interaction that is stronger than other dipole interactions, but still far weaker than a covalent bond, being approximately only 5% as strong as a typical covalent bond.