First issue is the incorrect formula for copper(I) iodide. $\ce{Cu2I2}$ is a common moiety in dicopper(I) iodide complexes (C.N. 4) with various ligands, but the correct formula unit for copper(I) iodide is $\ce{CuI}.$ Unlike mercury(I) iodide with $\ce{Hg2I2}$ formula unit depicting $\ce{Hg2^2+}$ moiety, there are no $\ce{Cu-Cu}$ linkages in copper(I) iodide.
Second, assigning states of aggregation would help to identify spectator ions and write net ionic equation \eqref{a-rxn-r2}. For simplicity, copper(I) iodide assumed to exist as precipitate due to its low solubility, and iodine as soluble compound due to formation of triiodide ion with potassium iodide $(\ce{KI3(aq)})$:
$$
\begin{align}
\ce{\overset{+2}{Cu}SO4(aq) + K\overset{-1}{I}(aq) &-> K2SO4(aq) + \overset{+1}{Cu}I(s) + \overset{0}{I}_2(aq)}\label{a-rxn-r1} \tag{R1} \\
\ce{\overset{+2}{Cu}^2+(aq) + \overset{-1}{I}^-(aq) &-> \overset{+1}{Cu}I(s) + \overset{0}{I}_2(aq)}\label{a-rxn-r2} \tag{R2}
\end{align}
$$
Third problem is improper half-reactions which contain non-existing chemicals in solution such as $\ce{I}$ or $\ce{S^6+}$. It also looks like you are mixing up dissociation and redox reactions, which is unnecessary at this point once you've came up with the net ionic equation. Correct half-reactions and balanced net ionic equations are as follows (states of aggregation which have already served their purpose are omitted for clarity):
$$
\begin{align}
\ce{\overset{+2}{Cu}^2+ + I- + e- &-> \overset{+1}{Cu}I} &|\times 2 \tag{red} \\
\ce{2\overset{-1}{I}^- &-> \overset{0}{I}_2 + 2 e-} & \tag{ox} \\
\hline
\ce{2 Cu^2+ + 4 I- &-> 2 CuI + I2} \tag{redox}
\end{align}
$$
To complete the full balanced reaction you need to add spectator ions — potassium and sulfate — with corresponding coefficients:
$$\ce{2 CuSO4(aq) + 4 KI(aq) -> 2 K2SO4(aq) + 2 CuI(s) + I2(aq)}\label{a-rxn-r3}\tag{R3}$$