Final answer:
Hydrogen bonds are indeed weaker than the covalent bonds within a water molecule. These intermolecular forces are significant for water's physical properties, but lack the strength of the direct atomic electron-sharing found in covalent bonds.
Step-by-step explanation:
The statement, "Hydrogen bonds are weaker than the bond that holds hydrogen to oxygen in a water molecule," is True. Hydrogen bonds are a type of weak intermolecular force that occurs when a hydrogen atom, which is already covalently bonded to a highly electronegative atom such as oxygen, is attracted to an electronegative atom in another molecule. Covalent bonds, such as the bond between hydrogen and oxygen in water, are much stronger because they involve the sharing of electron pairs between atoms.
In a water molecule, each water molecule can form up to four hydrogen bonds with neighboring molecules, which contribute to water's unique properties, such as its high boiling point and surface tension. Despite being weaker than the covalent bonds within the water molecule, these hydrogen bonds are strong enough to give water its cohesive and adhesive characteristics.