Definition: Free radicals are unstable molecules that can react chemically with other substances in the body, releasing energy in the process known as oxidation or redox reactions. Definition: 1. Oxidation: This is a chemical reaction by which atoms lose electrons. Free radicals involve more stable molecules and do not undergo oxidative breakdown. When they react with other molecules, they generate heat or light in the process called oxidation. 2. Redox: The term "redox" refers to two different chemical processes that are mutually exclusive but not independent. Oxidation involves an electron being transferred from one atom (e.g., hydrogen atoms) to another (e.g., oxygen). Redox reactions can be characterized by how the electrons are involved in the oxidation process. In summary, free radicals do not undergo oxidative breakdown and generate energy when they react with other substances; instead, they release heat or light in this process. The term "oxidation" is often used to describe chemical changes that involve a loss of electrons, while "redox reactions" refer to these chemical processes that can be distinguished by how the electrons are involved. For example, oxygen and hydrogen react to form water (O2 + H2O), releasing heat as electricity or light. This reaction is an example of oxidation because it involves a single electron transfer from one atom to another, which creates energy in the process. The energy released during this reaction can be used for various purposes. In contrast, the chemical process "reducing" oxygen into water (2O + 4H2O) does not involve any loss of electrons; instead, it involves a net gain of four electrons from the hydrogen atom and three electrons from the oxygen atom. This is an example of redox because it involves two different processes: oxidation and reduction.
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