What occurs during a redox reaction?

In a redox reaction, electrons are transferred from one species to another. This process is fundamental because it involves oxidation, where an atom or molecule loses electrons, and reduction, where another atom or molecule gains electrons. The exchange of electrons is what facilitates the change in oxidation states of the reacting species.

During oxidation, the species that loses electrons is oxidized, which usually results in an increase in oxidation state. Conversely, the species that gains those electrons is reduced, leading to a decrease in its oxidation state. This transfer is crucial in various chemical processes, including combustion, cellular respiration, and corrosion.

The notion that electrons are created in the reaction is incorrect, as electrons are conserved in chemical reactions; they do not just appear out of nowhere. The idea that only protons are exchanged is also misleading, as redox reactions specifically involve the transfer of electrons rather than protons, although protons may play a role in reactions when acids and bases are involved. Lastly, the statement that the reactants and products remain untouched misrepresents the nature of chemical reactions, which inherently involve changes to the substances involved. In a redox reaction, new products are formed from the reactants due to these electron transfer processes.