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Question: By oxidation of \({H_2}{O_2}\), we can obtain: A. \({O^{ - 2}}\) B. \(OH\) C. \(O_2^ - \) D....

By oxidation of H2O2{H_2}{O_2}, we can obtain:
A. O−2{O^{ - 2}}
B. OHOH
C. O2−O_2^ -
D. O2{O_2}

Explanation

Solution

We know that the chemical reaction in which a molecule, atom or ion loses electrons is referred to as the process of oxidation. In simpler terms, the process of oxidation is defined as the process of gaining the oxygen by any molecule or atom.

Complete step by step solution: Hydrogen peroxide is a chemical with formula H2O2{H_2}{O_2}. It is the simplest peroxide very unstable in nature. It is a very strong oxidising agent.
Hydrogen peroxide is a vital reagent. It has many applications. It is used as a mild antiseptic for the skin. It is also helping in cleaning of mouth as it helps in rinsing of mouth. It is used by farmers as it helps in growing mushrooms. It is also used in the kitchen as it helps in cleaning the dish maker. It can also act as a freshening agent as it helps to keep fruits fresh.
The oxidation of hydrogen peroxide i.e. H2O2{H_2}{O_2}leads to the formation of oxygen gas i.e. O2{O_2} . The reaction can be shown with the following chemical equation;
{H_2}{O_2} \to 2{H^ + } + {O_2} + 2{e^\\_}
It is clear that upon oxidation the hydrogen peroxide loses two electrons and leads to the formation of oxygen gas.
Hence, options (D)O2{O_2}, is the correct option.

Note: Both oxidation and reduction occur concurrently in a redox reaction. Using the oxidation states or the exchange of electrons, this reaction can be understood. The oxidation state describes the electrons obtained or lost during a reaction.