The oxidation state of oxygen in peroxides, such as H2O2, Na2O2, and BaO2, is -1, contrasting with the typical oxidation state of -2 in other compounds. This distinction is crucial because the molecular structure of peroxides includes an O-O bond, which differentiates them from simple oxides. Therefore, H2O2 and Na2O2 cannot be simplified to HO and NaO, as they represent fundamentally different chemical entities. Understanding this concept is essential for accurate chemical nomenclature and bonding analysis.
PREREQUISITESChemistry students, educators, and professionals interested in oxidation states, molecular structures, and the unique properties of peroxide compounds.
I see thanksBvU said:Basically because they are different molecules. The O-O presence is essential.