Corrosion Galvanic Corrosion
Corrosion
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For the hazard, see corrosive. Materials failure modes | Buckling | Corrosion | Creep | Fatigue | Fouling | Fracture | Impact | Mechanical overload | Thermal shock | Wear | Yielding | This box: view · talk · edit |
Corrosion is the disintegration of an engineered material into its constituent atoms due to chemical reactions with its surroundings. In the most common use of the word, this means electrochemical oxidation of metals in reaction with an oxidant such as oxygen. Formation of an oxide of iron due to oxidation of the iron atoms in solid solution is a well-known example of electrochemical corrosion, commonly known as rusting. This type of damage typically produces oxide(s) and/or salt(s) of the original metal. Corrosion can also refer to other materials than metals, such as ceramics or polymers, although in this context, the term degradation is more common.
In other words, corrosion is the wearing away of metals due to a chemical reaction.
Many structural alloys corrode merely from exposure to moisture in the air, but the process can be strongly affected by exposure to certain substances (see below). Corrosion can be concentrated locally to form a pit or crack, or it can extend across a wide area more or less uniformly corroding the surface. Because corrosion is a diffusion controlled process, it occurs on exposed surfaces. As a result, methods to reduce the activity of the exposed surface, such as passivation and chromate-conversion, can increase a material 's corrosion resistance. However, some corrosion mechanisms are less visible and less predictable.
Rust, the most familiar example of corrosion.
Volcanic gases have sped the corrosion of this abandoned mining machinery.
Corrosion on exposed metal. Contents[hide] * 1 Galvanic corrosion * 1.1 Galvanic series * 2 Resistance to corrosion * 2.1 Intrinsic chemistry * 2.2
From Wikipedia, the free encyclopedia
Jump to: navigation, search
For the hazard, see corrosive. Materials failure modes | Buckling | Corrosion | Creep | Fatigue | Fouling | Fracture | Impact | Mechanical overload | Thermal shock | Wear | Yielding | This box: view · talk · edit |
Corrosion is the disintegration of an engineered material into its constituent atoms due to chemical reactions with its surroundings. In the most common use of the word, this means electrochemical oxidation of metals in reaction with an oxidant such as oxygen. Formation of an oxide of iron due to oxidation of the iron atoms in solid solution is a well-known example of electrochemical corrosion, commonly known as rusting. This type of damage typically produces oxide(s) and/or salt(s) of the original metal. Corrosion can also refer to other materials than metals, such as ceramics or polymers, although in this context, the term degradation is more common.
In other words, corrosion is the wearing away of metals due to a chemical reaction.
Many structural alloys corrode merely from exposure to moisture in the air, but the process can be strongly affected by exposure to certain substances (see below). Corrosion can be concentrated locally to form a pit or crack, or it can extend across a wide area more or less uniformly corroding the surface. Because corrosion is a diffusion controlled process, it occurs on exposed surfaces. As a result, methods to reduce the activity of the exposed surface, such as passivation and chromate-conversion, can increase a material 's corrosion resistance. However, some corrosion mechanisms are less visible and less predictable.
Rust, the most familiar example of corrosion.
Volcanic gases have sped the corrosion of this abandoned mining machinery.
Corrosion on exposed metal. Contents[hide] * 1 Galvanic corrosion * 1.1 Galvanic series * 2 Resistance to corrosion * 2.1 Intrinsic chemistry * 2.2
References: 3. ^ A.K. Varshneya. Fundamentals of inorganic glasses. Society of Glass Technology, Sheffield, 682pp. (2006). 4 5. ^ Corrosion of Glass, Ceramics and Ceramic Superconductors. Edited by: D.E. Clark, B.K. Zoitos, William Andrew Publishing/Noyes, 672pp. (1992). 6 * Jones, Denny (1996). Principles and Prevention of Corrosion (2nd edition ed.). Upper Saddle River, New Jersey: Prentice Hall. ISBN 0-13-359993-0. * Working Safely with Corrosive Chemicals * A comprehensive 3.4-Mb pdf handbook "Corrosion Prevention and Control", 2006, 296 pages, US DoD, here * How do you remove and prevent flash rust on stainless steel? Article about the preventions of flash rust