To solve this problem, we need to understand the oxidation states of Group 16 elements.$\newline$Group 16 elements include oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).$\newline$The common oxidation states for these elements are -2, +2, +4, and +6.$\newline$Let's analyze each element:$\newline$• Oxygen (O) commonly exhibits a -2 oxidation state in most of its compounds.$\newline$• Sulfur (S), selenium (Se), and tellurium (Te) can exhibit -2 oxidation states, especially in their binary compounds with hydrogen.$\newline$• Polonium (Po), however, is less likely to exhibit a -2 oxidation state.$\newline$This is because polonium is a metal and prefers to exhibit positive oxidation states, such as +2 and +4.$\newline$Therefore, among the Group 16 elements, polonium (Po) does NOT show a -2 oxidation state.$\newline$This corresponds to Option 2.