Final answer:
Hydrogen bonding consists of a hydrogen atom 'sandwiched' between two very electronegative atoms. It is an intermolecular attractive force that is weaker than a covalent bond, but stronger than other dipole-dipole interactions. An example of hydrogen bonding is the attraction between hydrogen atoms and lone pairs on oxygen atoms in a water molecule.
Step-by-step explanation:
A hydrogen bond is an intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule. Hydrogen bonds are very strong compared to other dipole-dipole interactions, but still much weaker than a covalent bond. For example, in a water molecule (H₂O), the hydrogen atoms are attracted to the lone pairs on the oxygen atom, forming hydrogen bonds.