In the molecule sulfur dioxide (SO2), the bond between sulfur (S) and oxygen (O) is considered polar. This is due to the difference in electronegativity between the two atoms; oxygen is more electronegative than sulfur, which causes the electrons in the bond to be drawn closer to the oxygen atom. As a result, the bond has a dipole moment, meaning that there is a partial positive charge on the sulfur end and a partial negative charge on the oxygen end.
When we look at the geometry of SO2, it has a bent shape due to the presence of a lone pair of electrons on the sulfur atom. This bent geometry prevents the dipole moments from canceling each other out, which means that the molecule as a whole is polar. The asymmetric distribution of charges in the molecule leads to an overall dipole moment, confirming that SO2 is a polar molecule.