In a redox reaction, explain why the oxidizing agent undergoes reduction?
Reduction is defined as the gain of electrons. In order to function as an oxidizing AGENT, the agent must be reduced. Reducing AGENTS are oxidized in doing their job.
In a redox reaction, the oxidizing agent is the species that causes oxidation to occur to another substance, while itself undergoing reduction. This means that the oxidizing agent gains electrons during the reaction.
To understand why this happens, we need to consider the concept of electron transfer in redox reactions. Oxidation involves the loss of electrons, while reduction involves the gain of electrons.
When the oxidizing agent interacts with another species, it accepts electrons from that species, causing it to be reduced. This occurs because the oxidizing agent has a higher affinity for electrons compared to the other species involved in the redox reaction.
To determine why the oxidizing agent undergoes reduction, you can look at the reduction potential (E°) of the species involved in the reaction. Reduction potential is a measure of the tendency of a species to gain electrons. The species with the higher reduction potential will be the oxidizing agent, as it has a stronger tendency to accept electrons.
By examining the standard reduction potential tables, you can compare the values of different species and identify the oxidizing agent based on their relative reduction potentials.
In summary, the oxidizing agent undergoes reduction in a redox reaction because it has a greater tendency to gain electrons compared to the other species involved in the reaction.