The invisible dance of electrons that powers every living cell

Science · Published 29 October 2026 Swipe more like this →

In short: Every breath you take and every calorie you burn relies on a fundamental chemical exchange: the movement of electrons. These reactions are so essential to life that they occur naturally in all biological systems, governing everything from metabolism to the way our bodies process energy.

Redox is shorthand for oxidation-reduction, a process where two interdependent half-reactions occur simultaneously. In these reactions, one substance loses electrons—a process called oxidation—while another gains them, known as reduction. Because electrons are rarely shown in standard chemical equations, scientists use oxidation numbers to track which atoms are being oxidized and which are being reduced. A common mnemonic used to remember this is "OILRIG": Oxidation Is Loss, Reduction Is Gain. These reactions are essential for energy production and basic titrations. They represent a fundamental chemical exchange between two key players: oxidants and reductants.

The direction of this electron flow is not random; it is governed by reduction potential. This value measures a chemical species' tendency to gain electrons. The higher the reduction potential, the stronger that substance's power to pull electrons toward itself. For example, in a displacement reaction between zinc and copper, zinc has a lower reduction potential (-0.76 V) than copper (0.34 V). Consequently, zinc gives up two electrons to the copper cation, which acquires them and becomes reduced. This flow is an intrinsic property of the species involved. It can be viewed as a directional process where one substance acts as the donor while the other serves as the recipient.

While these reactions are foundational to industrial energy production and laboratory titrations, they are also critical for safety in green chemistry. Because redox reactions are inherent to biological systems, interference by harmful chemicals can lead to undesired consequences. To design safer chemicals and understand metabolic processes, scientists use tools like the Nernst equation to quantitatively describe how a chemical's intrinsic reduction potential is modulated by its specific environment. Understanding these mechanisms allows for the design of safer chemicals in green engineering. These processes are vital to numerous metabolic pathways found within living organisms.

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