Metallic corrosion is the damage of metal materials by the surrounding medium. Rust of metals is the most common form of corrosion. During corrosion, chemical or electrochemical multiphase reactions occur at the interface of metals, causing the metal to enter an oxidized (ionic) state. This significantly reduces the strength, plasticity, toughness and other mechanical properties of metal materials.
Corrosion is an electrochemical process in which metals react with the surrounding environment, and the resulting degradation causes the loss of material properties (such as mechanical strength, appearance, and impermeability to liquids and gases). The cause of corrosion is the energy difference between the metal and its natural ore. It takes energy to extract any metal from the ore. This "excess energy" drives corrosion because the metal will try to return to its natural state.
Electrochemically speaking, corrosion is the release of electrons. The process of releasing electrons is called an oxidation reaction or an anodic reaction. However, these electrons need to be consumed somewhere, so a reduction reaction or a cathodic reaction needs to occur.
Electrochemically speaking, corrosion is the release of electrons. The process of releasing electrons is called an oxidation reaction or an anodic reaction. However, these electrons need to be consumed somewhere, so a reduction reaction or cathodic reaction needs to occur.
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