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In redox reactions, some substances receive or accept electrons, and some give or donate. The species that donates the electrons is known as a reducing agent, and the species that accepts them is known as an oxidizing agent or oxidizer. In simple words, an oxidizer is a chemical species that oxidizes another chemical species by receiving electrons from it. Some common oxidizers are oxygen, ozone, fluorine, chlorine, hydrogen peroxide, etc.

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An oxidizing agent is a substance which supplies oxygen or any other electronegative element. In other words, it is a substance which removes hydrogen or any other electropositive element. In a chemical reaction, an oxidising agent, after carrying out oxidation, is itself reduced. Oxidising agents are also called oxidants or can be referred to as oxidizers. The oxidation state of oxidising agents decreases as they are reduced in an oxidation-reduction reaction. Oxidising agents are electron acceptors.

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Oxidising agents or oxidizers may contribute to combustion. Therefore the symbol for an oxidant or oxidising agent is a circle with flames on top of it. Oxidizers are considered dangerous, which is why they have a hazard symbol. Given below is the symbol of an oxidizer:

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If the number of electrons lost is equal to the number of electrons gained, then the two half-reactions are simply added to get the overall equation for the redox reaction. But, if the number of electrons lost during the oxidation half-reaction is different from the number of electrons gained during the reduction half-reaction, the two half-reactions are multiplied by a suitable integer.

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Learn more about an oxidizing agent as we go through its definition. Also, learn how we can identify it. Its properties, applications, and some examples are also discussed here.

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For example, during the oxidation of sodium by chlorine, the number of electrons lost by each sodium atom is one, while those gained by each chlorine molecule are two. Therefore the oxidation half-reaction is multiplied by 2 and then added to the reduction half equation to get the equation for the overall redox reaction.

We can say redox reactions can be considered as the sum of two half-reactions; one is oxidation half-reaction, and the other is reduction half-reaction. To explain these half-reactions, let us take an example of the oxidation of sodium by chlorine to form sodium chloride.

In these reactions, electrons are transferred from one substance. Thus, redox reactions may also be referred to as electron transfer reactions. The substance which loses electrons is called a reducing agent, and the other which accepts the electrons is called an oxidising agent.