Final answer:
Hydrogen fluoride (HF) exhibits hydrogen bonding as its predominant intermolecular force due to fluorine's high electronegativity and the polarized nature of the HF bond.
Step-by-step explanation:
The predominant intermolecular force in hydrogen fluoride (HF) is hydrogen bonding. This type of force occurs because fluorine is highly electronegative, making the HF bond exceptionally polarized and resulting in a significant partial positive charge on the hydrogen and a partial negative charge on the fluorine atom. The molecular structure of HF facilitates the formation of strong hydrogen bonds between the positively charged hydrogen atom of one molecule and the lone pair of electrons on the fluorine atom of another molecule, this interaction is stronger than in other hydrogen halides due to fluorine's electronegativity and small size.