Provide the structure of the $SO_{2}$ molecule and calculate the formal charge on each atom.

(N/A) The $SO_{2}$ molecule has a bent structure with $sp^{2}$ hybridization at the sulfur atom.
$1$. The Lewis structure involves a double bond between $S$ and one $O$ atom,and a single bond between $S$ and the other $O$ atom,with a lone pair on the $S$ atom.
$2$. Formal charge formula: $FC = V - L - \frac{1}{2}B$,where $V$ is valence electrons,$L$ is lone pair electrons,and $B$ is bonding electrons.
$3$. For the central $S$ atom: $V=6, L=2, B=6$. $FC = 6 - 2 - \frac{1}{2}(6) = +1$.
$4$. For the double-bonded $O$ atom: $V=6, L=4, B=4$. $FC = 6 - 4 - \frac{1}{2}(4) = 0$.
$5$. For the single-bonded $O$ atom: $V=6, L=6, B=2$. $FC = 6 - 6 - \frac{1}{2}(2) = -1$.