I see thanksBvU said:Basically because they are different molecules. The O-O presence is essential.
The oxidation state of oxygen in peroxides is typically -1.
In most compounds, oxygen has an oxidation state of -2. However, in peroxides, the oxygen atoms are bonded to each other, resulting in an overall oxidation state of -1 for each oxygen atom.
Yes, the oxidation state of oxygen in peroxides can change depending on the reaction. For example, in the decomposition of hydrogen peroxide, the oxygen atoms have an oxidation state of -1, but in the formation of water and oxygen gas, the oxygen atoms have an oxidation state of -2.
Some common examples of peroxides include hydrogen peroxide (H2O2), sodium peroxide (Na2O2), and calcium peroxide (CaO2).
The oxidation state of oxygen in peroxides is important because it helps determine the reactivity and stability of the compound. Peroxides are often used as oxidizing agents in various chemical reactions, and their oxidation state plays a crucial role in these reactions.