Shanxian Chemical
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Hydrogen Peroxide Oxidizing or Reducing Agent
On the Redox Properties of Hydrogen Peroxide
Hydrogen peroxide often exhibits unique redox properties in chemical reactions. It can be used as both an oxidizing agent and a reducing agent, depending on the specific situation and object of the reaction.
When encountering reducing substances, hydrogen peroxide mostly exhibits its oxidation properties. Because the oxidation state of oxygen in its molecule is -1 valence, it is in the intermediate valence state, and it tends to be lower oxidation state -2 valence, so it is easy to obtain electrons and oxidize other substances. If it reacts with ferrous ions, ferrous ions are oxidized to iron ions, and oxygen in hydrogen peroxide gains electrons and decreases to -2 valence, generating water. In this process, hydrogen peroxide exerts an oxidizing force and is reduced by itself, showing its ability as an oxidizing agent.
However, if it is a strong oxidizing agent, hydrogen peroxide can also be used as a reducing agent. At this time, its oxygen atoms can lose electrons, and the oxidation state is increased to 0 valence, generating oxygen. For example, when reacted with an acidic potassium permanganate solution, potassium permanganate has strong oxidation properties. Hydrogen peroxide supplies electrons in it, and itself is oxidized, showing the properties of a reducing agent.
In summary, the redox properties of hydrogen peroxide are not static and depend on the redox capacity of other substances in the reaction system. In chemical research and practical applications, this property can be clearly used in various reactions to maximize its effectiveness.
Hydrogen peroxide often exhibits unique redox properties in chemical reactions. It can be used as both an oxidizing agent and a reducing agent, depending on the specific situation and object of the reaction.
When encountering reducing substances, hydrogen peroxide mostly exhibits its oxidation properties. Because the oxidation state of oxygen in its molecule is -1 valence, it is in the intermediate valence state, and it tends to be lower oxidation state -2 valence, so it is easy to obtain electrons and oxidize other substances. If it reacts with ferrous ions, ferrous ions are oxidized to iron ions, and oxygen in hydrogen peroxide gains electrons and decreases to -2 valence, generating water. In this process, hydrogen peroxide exerts an oxidizing force and is reduced by itself, showing its ability as an oxidizing agent.
However, if it is a strong oxidizing agent, hydrogen peroxide can also be used as a reducing agent. At this time, its oxygen atoms can lose electrons, and the oxidation state is increased to 0 valence, generating oxygen. For example, when reacted with an acidic potassium permanganate solution, potassium permanganate has strong oxidation properties. Hydrogen peroxide supplies electrons in it, and itself is oxidized, showing the properties of a reducing agent.
In summary, the redox properties of hydrogen peroxide are not static and depend on the redox capacity of other substances in the reaction system. In chemical research and practical applications, this property can be clearly used in various reactions to maximize its effectiveness.
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