Fluorine oxidises water to oxygen whereas chlorine & bromine react with water to form corresponding $\mathrm{HX} \& \mathrm{HOX}$ acids.

$$\begin{gathered} 2{\mathrm{F}}_2+2{\mathrm{H}}_2\mathrm{O}\stackrel{}{\to }4\mathrm{HF}+{\mathrm{O}}_2 \\ {\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{O}\stackrel{}{\to }\mathrm{HCl}+\mathrm{HOCl} \end{gathered}$$

The reaction of ${\mathrm{I}}_2$ with water is nonspontaneous. In fact ${\mathrm{I}}^{–}$ can be oxidised by oxygen in acidic medium. It is why the ${\mathrm{I}}^{–}$ in nature is not present in that much amount as other halides are present in nature.