Hydrofluoric acid (HF) exhibits hydrogen bonding as its primary type of intermolecular force. This occurs because HF molecules have a highly polar covalent bond between hydrogen and fluorine, resulting in a significant dipole moment.
Additionally, HF molecules can interact through dipole-dipole interactions due to this polarity. These forces arise because the positive end of one polar molecule is attracted to the negative end of another.
In summary, the intermolecular forces present in HF are:
- Hydrogen bonding: The strong attractive force between hydrogen atoms bonded to electronegative atoms (like fluorine).
- Dipole-dipole interactions: The attraction between the positive end of one polar molecule and the negative end of another.
The presence of these strong intermolecular forces gives HF unique properties, such as a relatively high boiling point compared to other hydrogen halides.