Identify the species that is oxidized and the species that is reduced in this reaction. Also, identify the oxidizing agent and the reducing agent.

Given the equation of the reaction below:

3Cl₂(g) + 2Al(s) → 6Cl⁻(aq) + 2Al³⁺(aq)

The oxidized species is aluminum, Al, as its oxidation number increases from zero to +3. Al therefore, acts as the reducing agent.

Also, the reduced species is chlorine gas, Cl₂, as its oxidation number decreases from zero to -1. Therefore, Cl, is the reducing agent.

Note: the question is incomplete. a related question is given as follows; Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron transfer reaction. 3Cl2 + 2Al → 6Cl - + 2Al3+ species oxidized:

Explanation:

An oxidation is a process in which there is a loss of electrons whereas  reduction is a process involving the gain of electrons. A redox reaction is a reaction in which oxidation and reduction processes occur concurrently and to the same extent.

In a redox reaction reaction, the substance which is oxidized serves as the reducing agent by donating electrons to the substance which is reduced. On the other hand, the substance which is reduced serves as the oxidizing agent by accepting the electrons donated by the substance which is oxidized. In oxidation, the oxidation number of the substance oxidized increases, whereas in reduction, the oxidation number of the substance decreases.

For example, given the equation of the reaction below:

3Cl₂(g) + 2Al(s) → 6Cl⁻(aq) + 2Al³⁺(aq)

The oxidized species is aluminum, Al, as its oxidation number increases from zero to +3. Al therefore, acts as the reducing agent.

Also, the reduced species is chlorine gas, Cl₂, as its oxidation number decreases from zero to -1. Therefore, Cl, is the reducing agent.

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