oxidereduction

Oxidation-reduction, often shortened to redox, is a fundamental type of chemical reaction involving the transfer of electrons between chemical species. This transfer results in a change in the oxidation states of the participating atoms. Oxidation is defined as the loss of electrons by a species, leading to an increase in its oxidation state. Conversely, reduction is defined as the gain of electrons by a species, resulting in a decrease in its oxidation state. These two processes always occur simultaneously; one species cannot be oxidized without another species being reduced.

In a redox reaction, the species that loses electrons and becomes oxidized is called the reducing agent, as it causes the reduction of another species. The species that gains electrons and becomes reduced is called the oxidizing agent, as it causes the oxidation of another species. Common examples of redox reactions include combustion, corrosion (like rusting of iron), and cellular respiration. Electrochemistry is a field that heavily relies on redox reactions, with applications in batteries and electrolysis. Understanding redox is crucial in various scientific disciplines, including chemistry, biology, and environmental science, as it governs many natural and industrial processes.