Materials

CRUDs in Power Plants

In nuclear engineering, “CRUD” is a technical term for corrosion and wear products (rust particles, etc.) in the coolant that become radioactive when exposed to radiation. The term is actually an acronym for Chalk River Unidentified Deposits, originally found on the cladding, or outer coating, of fuel rods in the Canadian reactor for which it was named. CRUD may be defined as deposited or suspended circulating corrosion products, principally metal oxides, formed by the reaction of water with piping materials. According to the ICRP, CRUD formed in the power plants is the major source of operator radiation exposure.

Besides these radiological aspects CRUDs can have a number of adverse effects on the plant and its components. These can include the following:

• Mechanical fouling of equipment.
• Increase in the pressure drop across the core

The power plant must be designed to minimize corrosion and deposition. This design includes efficient removal of corrosion products, the purification system, design and arrange equipment to mnimize crud deposition, and select coolant chemistry to reduce corrosion.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Protection from Corrosion

As was written, the problem of metallic corrosion is significant. In economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions. Therefore, various treatments are used to slow corrosion damage to metallic objects which are exposed to the weather, salt water, acids, or other hostile environments. Since there are many forms of corrosion, there are many ways to stop or mitigate corrosion. In every case, it depends on material to be protected and also on the environment, in which the material is used. Metals may be protected from corrosion by using a metal in an environment in which it is immune, by making a physical barrier between the metal and its environment, by means of an electric current, or by changing the environment.

Anodization

Anodization is an electrolytic passivation process used to increase the thickness of the natural oxide layer on the surface of metal parts. A limited number of metals, such as stainless steels, can achieve passivity. The process is called anodizing because the part to be treated forms the anode electrode of an electrolytic cell. Aluminium alloys are usually anodized to increase corrosion resistance and to allow dyeing (colouring).

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Protection from Corrosion

As was written, the problem of metallic corrosion is significant. In economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions. Therefore, various treatments are used to slow corrosion damage to metallic objects which are exposed to the weather, salt water, acids, or other hostile environments. Since there are many forms of corrosion, there are many ways to stop or mitigate corrosion. In every case, it depends on material to be protected and also on the environment, in which the material is used. Metals may be protected from corrosion by using a metal in an environment in which it is immune, by making a physical barrier between the metal and its environment, by means of an electric current, or by changing the environment.

Cathodic Protection

Cathodic protection is a very effective way of protection from corrosion based on the use of a material that is more anodic than the metal to be protected. The protected metal is electrically connected to another metal that is more reactive in the particular environment. The metal which is less corrosive resistant becomes anode and metal with more corrosive resistance become cathode. The corrosion of the less corrosive resistance is usually increased and attack on more resistant material is decreased. A difference in electrical potential exists between the different metals and serves as the driving force for electrical current flow through the corrodant or electrolyte. Cathodic protection systems are most commonly used to protect buried or submerged metal structures from corrosion, such as steel pipelines and tanks. Magnesium, zinc, and aluminum alloys are common sacrificial anodes. Magnesium anodes are most commonly used for buried soil applications. Zinc is most often used for freshwater and saltwater marine applications. Aluminum alloys are most often used for offshore structures.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Most metals are not thermodynamically stable in the metallic form; they want to corrode and revert to the more stable forms that are normally found in ores, such as oxides. Corrosion can also occur in materials other than metals, such as ceramics or polymers, although in this context, the term “degradation” is more common. Ceramic materials are relatively resistant to deterioration, which usually occurs at elevated temperatures or in rather extreme environments. The process is frequently also called corrosion. For polymers, mechanisms and consequences differ from those for metals and ceramics, and the term degradation is most frequently used. Corrosion degrades the useful properties of materials and structures including strength, appearance and permeability to liquids and gases.

Corrosion is electrochemical in nature because the corrosive chemical reactions involve a transfer of charge. The chemistry of corrosion is quite complex but it may be considered essentially as an electrochemical phenomenon. The metal ions go into solution causing the metal to become negatively charged with respect to the electrolyte. The difference in the charge causes a potential to develop and produces a voltage between the electrolyte and the metal.

Corrosion, as a natural and persistent process, also involves unintended deterioration of metals sometimes with disastrous outcomes. How big is the corrosion problem? The problem of metallic corrosion is significant. In economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions.

Corrosion is of primary concern in nuclear reactor plants. Corrosion occurs continuously throughout the reactor plant, and every metal is subject to it. Even though this corrosion cannot be eliminated, it can be controlled.

 

Protection from Corrosion

As was written, the problem of metallic corrosion is significant. In economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions. Therefore, various treatments are used to slow corrosion damage to metallic objects which are exposed to the weather, salt water, acids, or other hostile environments. Since there are many forms of corrosion, there are many ways to stop or mitigate corrosion. In every case, it depends on material to be protected and also on the environment, in which the material is used. Metals may be protected from corrosion by using a metal in an environment in which it is immune, by making a physical barrier between the metal and its environment, by means of an electric current, or by changing the environment.

• Material Selection. Perhaps the most common and easiest way of preventing corrosion is through the judicious selection of materials once the corrosion environment has been characterized. Some ferrous and many non-ferrous metals and alloys are widely used in corrosive environments. In all cases, it strongly depends on certain environment and other conditions. Here, cost may be a significant factor. It is not always economically feasible to employ the material that provides the optimum corrosion resistance.
• Anti-corrosion Surface Treatment. A coating provides protection by forming a physical barrier between the metallic substrate and an aqueous corrosive environment. Coatings protect metallic structures from corrosion by both inhibition and barrier effects. The barrier effect depends on the adhesion to the under-layer but also the non-conducting properties of the coating. Penetration of water or ions is a major cause for loss of the barrier, which may lead to delamination of the coating and under-film corrosion. Plating, painting, and the application of enamel are the most common anti-corrosion treatments.
• Anodization. Anodization is an electrolytic passivation process used to increase the thickness of the natural oxide layer on the surface of metal parts. A limited number of metals, such as stainless steels, can achieve passivity. The process is called anodizing because the part to be treated forms the anode electrode of an electrolytic cell. Aluminium alloys are usually anodized to increase corrosion resistance and to allow dyeing (colouring).
• Cathodic Protection. Cathodic protection is a very effective way of protection from corrosion based on the use of a material that is more anodic than the metal to be protected. The protected metal is electrically connected to another metal that is more reactive in the particular environment. The metal which is less corrosive resistant becomes anode and metal with more corrosive resistance become cathode. The corrosion of the less corrosive resistance is usually increased and attack on more resistant material is decreased. A difference in electrical potential exists between the different metals and serves as the driving force for electrical current flow through the corrodant or electrolyte. Cathodic protection systems are most commonly used to protect buried or submerged metal structures from corrosion, such as steel pipelines and tanks. Magnesium, zinc, and aluminum alloys are common sacrificial anodes. Magnesium anodes are most commonly used for buried soil applications. Zinc is most often used for freshwater and saltwater marine applications. Aluminum alloys are most often used for offshore structures.
• Corrosion Inhibitors. If the environment is controlled (especially in recirculating systems), corrosion inhibitors can often be added to it. These chemicals form an electrically insulating or chemically impermeable coating on exposed metal surfaces, to suppress electrochemical reactions. Corrosion inhibitors are chemicals that, when added in relatively low concentrations to the environment, reduces the rate of a corrosive process. Which substance that acts like inhibitors depends on both the corrosive environment as well as the alloy. Inhibitors are normally used in closed systems such as automobile radiators and steam boilers. An example of this principle is the use of antifreeze in cars. The effectiveness of an inhibitor depends on several different mechanisms. Some reacts with the chemically active species in the solution while other react with the corroding surface and interfere with the corrosive reaction, or form a thin protective coating. For example, oxygen is generally removed by reductive inhibitors such as amines and hydrazines. In this example, hydrazine converts oxygen, a common corrosive agent, to water, which is generally benign. Many inhibitors are also toxic and are therefore not suitable to use in  all applications. Another limitation of inhibitors is that they generally lose the effectiveness when the temperature and concentration of the environment increases.

Corrosion-resistant Alloys

Corrosion-resistant alloys, as their name indicates, are alloys with enhanced corrosion resistance. Some ferrous and many non-ferrous metals and alloys are widely used in corrosive environments. In all cases, it strongly depends on certain environment and other conditions. Corrosion-resistant alloys are used for water piping and many chemical and industrial applications. In case of ferrous alloys, we are talking about stainless steels and to some extent about cast irons. But some non-ferrous corrosion-resistant alloys exhibit remarkable corrosion resistance nad therefore they may be used for many special purposes. There are two main reasons why nonferrous materials are preferred over steels and stainless steels for many of these applications. For example, many of the non-ferrous metals and alloys possess much higher resistance to corrosion than available alloy steels and stainless steel grades. Second, a high strength-to-weight ratio or high thermal and electrical conductivity may provide a distinct advantage over a ferrous alloy.

Passivation

There are metals, that exhibit a passivity to corrosion. Passivity is the characteristic of a metal exhibited when that metal does not become active in the corrosion reaction. Passivation is natural process of the buildup of a stable, tenacious layer of metal oxide or protective barrier on the surface of the metal that acts as a barrier separating the metal surface from the environment. Passivity decreases or stops the corrosion process because of the formation of the layer. Fortunately, from an engineering standpoint, the metals most susceptible to this kind of behavior are the common engineering and structural materials, including iron, nickel, silicon, chromium, titanium, and alloys containing these metals.

For example, stainless steel owes its corrosion-resistant properties to the formation of a self-healing passive surface film. For passivation to occur and remain stable, the Fe-Cr alloy must have a minimum chromium content of about 10.5% by weight, above which passivity can occur and below which it is impossible. Once the surface is cleaned and the bulk composition of the stainless steel is exposed to air, the passive film forms immediately.

Aluminium is highly corrosion resistant in many environments because it also passivates. If damaged, the protective film normally re-forms very rapidly. However, a change in the character of the environment (e.g., alteration in the concentration of the active corrosive species) may cause a passivated material to revert to an active state. Generally, at high temperatures (in water, corrosion limits the use of aluminium to temperatures near 100°C), the relative low strength and poor corrosion properties of aluminium make it unsuitable as a structural material.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Protection from Corrosion

As was written, the problem of metallic corrosion is significant. In economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions. Therefore, various treatments are used to slow corrosion damage to metallic objects which are exposed to the weather, salt water, acids, or other hostile environments. Since there are many forms of corrosion, there are many ways to stop or mitigate corrosion. In every case, it depends on material to be protected and also on the environment, in which the material is used. Metals may be protected from corrosion by using a metal in an environment in which it is immune, by making a physical barrier between the metal and its environment, by means of an electric current, or by changing the environment.

Anti-corrosion Surface Treatment

A coating provides protection by forming a physical barrier between the metallic substrate and an aqueous corrosive environment. Coatings protect metallic structures from corrosion by both inhibition and barrier effects. The barrier effect depends on the adhesion to the under-layer but also the non-conducting properties of the coating. Penetration of water or ions is a major cause for loss of the barrier, which may lead to delamination of the coating and under-film corrosion. Plating, painting, and the application of enamel are the most common anti-corrosion treatments.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Intergranular Corrosion – Weld Decay

Intergranular corrosion (IGC) is preferential corrosion along the grain boundaries of a material. for some alloys and in specific environments. This type of corrosion is especially prevalent in some stainless steels. In stainless steels, intergranular corrosion may occur as a consequence of the precipitation of chromium carbides (Cr₂₃C₆) or intermetallic phases.

The resistance of these metallic alloys to the chemical effects of corrosive  agents is based on passivation. For passivation to occur and remain stable, the Fe-Cr alloy must have a minimum chromium content of about 10.5% by weight, above which passivity can occur and below which it is impossible. But the chromium carbides may precipitate in the grain boundaries, which result in depletion of chromium in the zones close to the grain boundaries due to the diffusion rate of chromium that is slow. The chromium-depleted zones become less corrosion resistant than the rest of the matrix. In a corrosive environment the depleted areas may be activated and corrosion will occur in very narrow areas between the grains.

Intergranular corrosion is an especially severe problem in the welding of stainless steels, when it is often termed weld decay. Also a stainless steel, which has been heat-treated in a way that produces grain boundary precipitates and adjacent chromium depleted zones, it is sensitised. Stainless steels can be stabilized against this behavior by addition of titanium, niobium, or tantalum, which form titanium carbide, niobium carbide and tantalum carbide preferentially to chromium carbide, by lowering the content of carbon in the steel and in case of welding also in the filler metal under 0.02%, or by heating the entire part above 1000 °C and quenching it in water, leading to dissolution of the chromium carbide in the grains and then preventing its precipitation.

There are two special cases of intergranular corrosion, but these mechanisms are treated separately:

• Stress corrosion cracking. Intergranular corrosion induced by environmental stresses is termed stress corrosion cracking.
• Chloride stress corrosion cracking. Intergranular corrosion induced by combined action of environmental stresses and chlorine is termed chloride stress corrosion cracking.

Stress Corrosion Cracking – SCC

One of the most serious metallurgical problems and one that is a major concern in the nuclear industry is stress-corrosion cracking (SCC). Stress-corrosion cracking results from the combined action of an applied tensile stress and a corrosive environment, both influences are necessary. SCC is a type of intergranular attack corrosion that occurs at the grain boundaries under tensile stress. It tends to propagate as stress opens cracks that are subject to corrosion, which are then corroded further, weakening the metal by further cracking. The cracks can follow intergranular or transgranular paths, and there is often a tendency for crack branching. Failure behavior is characteristic of that for a brittle material, even though the metal alloy is intrinsically ductile. SCC can lead to unexpected sudden failure of normally ductile metal alloys subjected to a tensile stress, especially at elevated temperature. SCC is highly chemically specific in that certain alloys are likely to undergo SCC only when exposed to a small number of chemical environments.

See also: Stress Corrosion Cracking

The most effective means of preventing SCC in reactor systems are:

• designing properly
• reducing stress
• removing critical environmental species such as hydroxides, chlorides, and oxygen
• avoiding stagnant areas and crevices in heat exchangers where chloride and hydroxide might become concentrated.

Chloride Stress Corrosion Cracking

Chloride stress corrosion occurs in austenitic stainless steels under tensile stress in the presence of oxygen, chloride ions, and high temperature. It is one of the most important forms of stress corrosion that concerns the nuclear industry. Austenitic stainless steels contain between 16 and 25% Cr and can also contain nitrogen in solution, both of which contribute to their relatively high uniform corrosion resistance. One type of corrosion which can attack austenitic stainless steel is chloride stress corrosion.

The three conditions that must be present for chloride stress corrosion to occur are as follows:

• Chloride ions are present in the environment
• Dissolved oxygen is present in the environment
• Metal is under tensile stress

Chloride stress corrosion involves selective attack of the metal along grain boundaries. The resistance of these metallic alloys to the chemical effects of corrosive  agents is based on passivation. For passivation to occur and remain stable, the Fe-Cr alloy must have a minimum chromium content of about 10.5% by weight, above which passivity can occur and below which it is impossible. But the chromium carbides may precipitate in the grain boundaries, which result in depletion of chromium in the zones close to the grain boundaries due to the diffusion rate of chromium that is slow. The chromium-depleted zones become less corrosion resistant than the rest of the matrix. In a corrosive environment the depleted areas may be activated and corrosion will occur in very narrow areas between the grains.

It has been found that this is closely associated with certain heat treatments resulting from welding. This can be minimized considerably by proper annealing processes. This form of corrosion is controlled by maintaining low chloride ion and oxygen content in the environment and use of low carbon steels. Ferritic stainless steels are chosen for their resistance to stress corrosion cracking, which makes them an attractive alternative to austenitic stainless steels in applications where chloride-induced SCC is prevalent.

See above:
Corrosion

Chloride stress corrosion occurs in austenitic stainless steels under tensile stress in the presence of oxygen, chloride ions, and high temperature. It is one of the most important forms of stress corrosion that concerns the nuclear industry. Austenitic stainless steels contain between 16 and 25% Cr and can also contain nitrogen in solution, both of which contribute to their relatively high uniform corrosion resistance. One type of corrosion which can attack austenitic stainless steel is chloride stress corrosion.

The three conditions that must be present for chloride stress corrosion to occur are as follows:

• Chloride ions are present in the environment
• Dissolved oxygen is present in the environment
• Metal is under tensile stress

Chloride stress corrosion involves selective attack of the metal along grain boundaries. The resistance of these metallic alloys to the chemical effects of corrosive  agents is based on passivation. For passivation to occur and remain stable, the Fe-Cr alloy must have a minimum chromium content of about 10.5% by weight, above which passivity can occur and below which it is impossible. But the chromium carbides may precipitate in the grain boundaries, which result in depletion of chromium in the zones close to the grain boundaries due to the diffusion rate of chromium that is slow. The chromium-depleted zones become less corrosion resistant than the rest of the matrix. In a corrosive environment the depleted areas may be activated and corrosion will occur in very narrow areas between the grains.

It has been found that this is closely associated with certain heat treatments resulting from welding. This can be minimized considerably by proper annealing processes. This form of corrosion is controlled by maintaining low chloride ion and oxygen content in the environment and use of low carbon steels. Ferritic stainless steels are chosen for their resistance to stress corrosion cracking, which makes them an attractive alternative to austenitic stainless steels in applications where chloride-induced SCC is prevalent.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Galvanic Corrosion

Galvanic corrosion occurs when two dissimilar metals are immersed in a conductive solution in presence of some potential difference and there is a flow of electron between the metals. It may also take place with one metal with heterogeneities (dissimilarities) (for example, impurity inclusions, grains of different sizes, difference in composition of grains, or differences in mechanical stress). The metal which is less corrosive resistant becomes anode and metal with more corrosive resistance become cathode. The corrosion of the less corrosive resistance is usually increased and attack on more resistant material is decreased. A difference in electrical potential exists between the different metals and serves as the driving force for electrical current flow through the corrodant or electrolyte.

Galvanic corrosion occurs only if the following conditions are met:

• Two different metals must be present
• The two metals must be in contact, or an electrically conductive path between the two must be present
• There must be an electrically conductive path for the ions to move from the “anode” to the “cathode”

If any of these conditions is not satisfied, galvanic corrosion is not likely to take place.

Galvanic corrosion only causes deterioration of one of the metals. The stronger, more noble one is cathodic (positive) and protected. This is the mechanism of galvanic anodes, which are the main component of a galvanic cathodic protection (CP) system used to protect buried or submerged metal structures from corrosion. In some instances, galvanic corrosion can be helpful.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Selective Leaching – Selective Corrosion

Selective leaching or selective corrosion is the removal of one element from a solid alloy by corrosion process. The most common example is the dezincification of brass, in which zinc is selectively leached from a copper–zinc brass alloy. This process produces a weakened porous copper structure. The selective removal of zinc can be in a uniform manner or localized scale.

However, many alloys are subject to selective leaching under certain conditions. Similar process occurs in other alloy systems in which aluminum, iron, cobalt, chromium, and other elements are removed. Elements in an alloy that are more resistant to the environment remain behind. Two mechanisms are involved:

• Two metals in an alloy are dissolved; one metal redeposits on the surface of the surviving elements.
• One metal is selectively dissolved, leaving the other metals behind.

The first system is involved in the dezincification of brasses, and the second system is involved when molybdenum is removed from nickel alloys in molten sodium hydroxide.

See above:
Corrosion

Corrosion is the deterioration of a material due to chemical interaction with its environment. It is natural process in which metals convert its structure into a more chemically-stable form such as oxides, hydroxides, or sulfides. The consequences of corrosion are all too common. Familiar examples include the rusting of automotive body panels and pipings and many tools. Corrosion is usually a negative phenomenon, since it is associated with mechanical failure of an object. Metal atoms are removed from a structural element until it fails, or oxides build up inside a pipe until it is plugged. All metals and alloys are subject to corrosion. Even the noble metals, such as gold, are subject to corrosive attack in some environments.

Pitting Corrosion

Pitting corrosion, characterized by sharply defined holes, is one of the most insidious forms of corrosion. They ordinarily penetrate from the top of a horizontal surface downward in a nearly vertical direction. It is supposed that gravity causes the pits to grow downward. Pitting corrosion can cause failure by perforation while producing only a small weight loss on the metal. This perforation can be difficult to detect and its growth rapid, leading to unexpected loss of function of the component. Pitting corrosion has also been associated with both crevice and galvanic corrosion. Metal deposition (copper ions plated on a steel surface) can also create sites for pitting attack.

Causes of pitting corrosion include:

• Local inhomogeneity on the metal surface
• Local loss of passivity
• Mechanical or chemical rupture of a protective oxide coating
• Galvanic corrosion from a relatively distant cathode

With corrosion-resistant alloys, such as stainless steels, the most common cause of pitting corrosion is highly localized destruction of passivity by contact with moisture that contains halide ions, particularly chlorides. However, alloying with about 2% molybdenum enhances their resistance significantly. Chloride-induced pitting of stainless steels usually results in undercutting, producing enlarged subsurface cavities or caverns.

Pitting Corrosion – Protection

Pitting corrosion is a hazard due to the possible rapid penetration of the metal with little overall loss of mass. Pitting corrosion is minimized by:

• Avoiding stagnant conditions
• Using the correct metals and alloys that are less susceptible to the corrosion
• Avoiding agents in the medium that cause pitting
• Designing the system and components such that no crevices are present

See above:
Corrosion