Here's why:

* Molecular shape: SO2 has a bent or V-shaped geometry due to the presence of lone pairs on the sulfur atom. This shape results in an uneven distribution of electron density, creating a permanent dipole moment.

* Polarity: The sulfur-oxygen bonds are polar, with oxygen being more electronegative than sulfur. This polarity contributes to the overall dipole moment of the molecule.

* Dipole-dipole interactions: The positive end of one SO2 molecule is attracted to the negative end of another SO2 molecule, resulting in a dipole-dipole interaction.

Other forces present but weaker:

* London dispersion forces: These weak forces are present in all molecules due to temporary fluctuations in electron distribution. They are also present in SO2.

* Hydrogen bonding: SO2 does not participate in hydrogen bonding because it does not have a hydrogen atom directly bonded to a highly electronegative atom like oxygen or nitrogen.

Therefore, dipole-dipole interactions are the dominant intermolecular forces in SO2.