Question

Identify the oxidized substance, the reduced substance, the oxidizing agent, and the reducing agent in the redox reaction. Mg(s)+Cl2(g)⟶Mg2+(aq)+2Cl−(aq) Mg(s)+Cl2(g)⟶Mg2+(aq)+2Cl−(aq) Which substance gets oxidized? MgMg Cl−Cl− Mg2+Mg2+ Cl2Cl2 Which substance gets reduced? Cl2Cl2 Mg2+Mg2+ MgMg Cl−Cl− What is the oxidizing agent? Mg2+Mg2+ Cl−Cl− MgMg Cl2Cl2 What is the reducing agent? Cl2Cl2 MgMg Cl−Cl− Mg2+

Answer 1

Answer: oxidizing agent: $Cl_2$

reducing agent: $Mg$

Explanation:

Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

$Mg(s)+Cl_2(g)\rightarrow Mg^{2+}(aq)+2Cl^-(aq)$

On reactant side:

Oxidation state of magnesium = 0

Oxidation state of chlorine = 0

On product side:

Oxidation state of magnesium = +2

Oxidation state of chlorine = -1

The oxidation state of chlorine reduces from 0 to -1, it is getting reduced. The substance which gets reduced, oxidize others and called as oxidizing agent.

The oxidation state of magnesium increases from 0 to +2. Thus, it is getting oxidized. The substance which gets oxidized, reduces others and called as reducing agent.