Which of the following pair of compounds will have three ${\mathrm{sp}}^2$-hybrid orbitals?

Formula To Predict Hybridization of Central Atom$\mathrm{Number} \mathrm{of} \mathrm{Hybrid} \mathrm{orbitals}=\frac{1}{2}( \mathrm{No}. \mathrm{of} \mathrm{valence} \mathrm{electrons} \mathrm{in} \mathrm{valence} \mathrm{shell}+\mathrm{No}. \mathrm{of} \mathrm{monovalent} \mathrm{atoms} \mathrm{surrounding}-\mathrm{Charge} \mathrm{on} \mathrm{cation} + \mathrm{Charge} \mathrm{on} \mathrm{anion})$$$\begin{gathered} {\mathrm{SO}}_2\text{ : trigonal planar ; three }{\mathrm{sp}}^2\text{-hybrid orbitals } \\ {\mathrm{CH}}_4\text{ : tetrahedral ; four }{\mathrm{sp}}^3\text{-hybrid orbitals } \\ {\mathrm{SO}}_3\text{ : Trigonal planar ; three }{\mathrm{sp}}^2\text{-hybrid orbitals } \\ {\mathrm{C}}_2{\mathrm{H}}_4\text{ : Trigonal planar; three }{\mathrm{sp}}^2\text{-hybrid orbitals } \\ {\mathrm{BF}}_3\text{ : Trigonal planar ; three }{\mathrm{sp}}^2\text{-hybrid orbitals } \\ {\mathrm{SF}}_4\text{ : Irregular tetrahedral ; five }{\mathrm{sp}}^3\mathrm{d}\text{-hybrid orbitals } \\ {\mathrm{I}}_3^{-}\text{: near five }{\mathrm{sp}}^3\mathrm{d}\text{-hybrid orbitals } \end{gathered}$$