The hybridization of sulfur in ${\mathrm{SO}}_2$ is;

${\mathrm{SO}}_2$ hybridization involves the hybridization of two $3\mathrm{p}$ orbitals and one 3s orbital. Two-hybrid orbitals have unpaired electrons, whereas one hybrid orbital has a Ione pair. The $3\mathrm{ }\mathrm{d}$ and $3\mathrm{p}$ orbitals stay unchanged and form pi bonds. ${\mathrm{SO}}_2$ molecule geometry is thought to be V-shaped or bent. Sulfur dioxide's electron geometry, on the other hand, is shaped like a trigonal planar. The three pairs of bonding electrons form a 119-degree angle. Two double pairs are linked together, as well as one lone pair, giving it a bent form.)