Here's why:
* Dipole-dipole interactions: Sulfur dioxide is a polar molecule. The sulfur atom is more electronegative than the oxygen atoms, leading to a partial positive charge on the sulfur atom and partial negative charges on the oxygen atoms. This creates a permanent dipole moment within the molecule, which allows for dipole-dipole attractions between neighboring SO2 molecules.
* London dispersion forces: These are present in all molecules, including SO2. They arise from temporary fluctuations in electron distribution, creating temporary dipoles that induce dipoles in neighboring molecules. These temporary attractions are weaker than dipole-dipole interactions but are still significant in contributing to the overall IMF strength.
Important note: While SO2 has a bent molecular geometry, it does not exhibit hydrogen bonding. Hydrogen bonding requires a hydrogen atom directly bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine. In SO2, the hydrogen atom is not directly bonded to any of these atoms.
