Within oxygen difluoride, $\text{OF}_2$, fluorine has an oxidation number of $-1$. $\text{OF}_2$ reacts with sulfur dioxide in accordance with the equation below. $\text{OF}_2 + \text{SO}_2 \rightarrow \text{SO}_3 + \text{F}_2$ What is oxidised and what is reduced in this reaction?
- Afluorine oxidised; oxygen in OF$_2$ oxidised; sulfur reduced
- Bfluorine oxidised; oxygen in OF$_2$ reduced; sulfur oxidised
- Cfluorine reduced; oxygen in OF$_2$ oxidised; sulfur reduced
- Dfluorine reduced; oxygen in OF$_2$ reduced; sulfur oxidised