Forms of Corrosion

Corrosion - corroded metalCorrosion 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.

Forms of Corrosion

During metal corrosion, the areas over which the anodic and cathodic reactions occur can vary greatly. Corrosion can come in different forms and grow at different rates. This results in various forms of corrosion such as uniform attack, pitting, and crevice corrosion. The problem is that many forms of corrosion exist and each is caused by different reasons and undergoes different mechanisms. Moreover, each form of corrosion has its own special mechanism, which can be quite complex in some cases. This is especially problematic when two or more types of corrosion take place simultaneously.

In the following section, we will briefly describe the most common forms of corrosion. They are basically divided into two subcategories: general (uniform) and localized form of corrosion.

  • General Corrosion. General corrosion, also known as uniform corrosion, is a form of corrosion that affects the entire surface of the metal, whereas other forms affect a specific spot or portion. This type of corrosion is commonly observed in pure metals which are metallurgical and compositionally uniform. It is a very slow reaction that is fairly evenly distributed over the entire metal surface exposed to any circulating water. The fact that it affects a fairly large area of the metal makes it much easier to detect, and hence much less severe than localized corrosion. The problem with general corrosion is that it results in a large volume of oxides that tend to attach themselves to the heat transfer surfaces and affect the efficiency of the system.
  • Localized Corrosion. In localized corrosion there is an intense at tack at localized sites on the surface of a component while the rest of the surface is corroding at much lower rate. Localized corrosion takes place when corrosion works with other destructive processes such as stress, fatigue, erosion, and other forms of chemical attack.

forms of corrosion

General Corrosion

General corrosion, also known as uniform corrosion, is a form of corrosion that affects the entire surface of the metal, whereas other forms affect a specific spot or portion. It is the most common form of corrosion. This type of corrosion is commonly observed in pure metals which are metallurgical and compositionally uniform. Weathering steels, magnesium alloys, zinc alloys, and copper alloys are examples of materials that typically exhibit general corrosion. Passive materials, such as stainless steels, aluminum alloys, or nickelchromium alloys are generally subject to localized corrosion.

It is a very slow reaction that is fairly evenly distributed over the entire metal surface exposed to any circulating water. The fact that it affects a fairly large area of the metal makes it much easier to detect, and hence much less severe than localized corrosion. The problem with general corrosion is that it results in a large volume of oxides that tend to attach themselves to the heat transfer surfaces and affect the efficiency of the system.

General Corrosion – Protection

Some standard methods associated with material selection that protect against general corrosion include:

  • The use of corrosion-resistant materials such as stainless steel and nickel, chromium, and molybdenum alloys.
  • The use of protective coatings such as paints and epoxies.
  • The application of metallic and nonmetallic coatings or linings to the surface which protects against corrosion, but allows the material to retain its structural strength (for example, a carbon steel pressure vessel with stainless steel cladding as a liner).

Localized Corrosion

In localized corrosion there is an intense at tack at localized sites on the surface of a component while the rest of the surface is corroding at much lower rate. Localized corrosion takes place when corrosion works with other destructive processes such as stress, fatigue, erosion, and other forms of chemical attack. Localized corrosion mechanisms can cause more damage than any one of those destructive processes individually. Localized corrosion can further classified as pitting corrosion, galvanic corrosion, crevice corrosion, selective corrosion, erosion corrosion, intergranular corrosion, chloride stress corrosion and stress corrosion cracking (SCC). Passive materials, such as stainless steels, aluminum alloys, or nickelchromium alloys are generally subject to localized corrosion.

Pitting Corrosion

Pitting, 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

Crevice Corrosion

Crevice corrosion refers to the localized corrosion that occurs at the crevice or gap between two or more joining metals. Crevice corrosion is a type of pitting corrosion that occurs specifically within the low flow region of a crevice. This type of attack is usually associated with small volumes of stagnant solution caused by holes, gaskets surface, lap joints, surface deposits, and crevice under bolt and rivets heads. The damage takes place due to the difference in constituents’ concentration, mainly oxygen, in the surfaces involved. Crevice corrosion can progress very rapidly (tens to hundreds of times faster than the normal rate of general corrosion in the same given solution).

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

  • Crevice corrosion may be prevented by using welded instead of riveted or bolted joints
  • 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

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.

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.

Erosion Corrosion

Erosion corrosion is the cumulative damage induced by electrochemical corrosion reactions and mechanical effects from relative motion between the electrolyte and the corroding surface. Erosion can also occur in combination with other forms of degradation, such as corrosion. This is referred to as erosion-corrosion. Erosion corrosion is a material degradation process due to the combined effect of corrosion and wear. Nearly all flowing or turbulent corrosive media can cause erosion corrosion. The mechanism can be described as follows:

  • mechanical erosion of the material, or protective (or passive) oxide layer on its surface,
  • enhanced corrosion of the material, if the corrosion rate of the material depends on the thickness of the oxide layer.

Erosion corrosion is found in the systems such as piping, valves, pumps, nozzles, heat exchangers and turbines. Wear is a mechanical material degradation process occurring on rubbing or impacting surfaces, while corrosion involves chemical or electrochemical reactions of the material. Corrosion may accelerate wear and wear may accelerate corrosion.

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.

References:

Materials Science:

  1. U.S. Department of Energy, Material Science. DOE Fundamentals Handbook, Volume 1 and 2. January 1993.
  2. U.S. Department of Energy, Material Science. DOE Fundamentals Handbook, Volume 2 and 2. January 1993.
  3. William D. Callister, David G. Rethwisch. Materials Science and Engineering: An Introduction 9th Edition, Wiley; 9 edition (December 4, 2013), ISBN-13: 978-1118324578.
  4. Eberhart, Mark (2003). Why Things Break: Understanding the World by the Way It Comes Apart. Harmony. ISBN 978-1-4000-4760-4.
  5. Gaskell, David R. (1995). Introduction to the Thermodynamics of Materials (4th ed.). Taylor and Francis Publishing. ISBN 978-1-56032-992-3.
  6. González-Viñas, W. & Mancini, H.L. (2004). An Introduction to Materials Science. Princeton University Press. ISBN 978-0-691-07097-1.
  7. Ashby, Michael; Hugh Shercliff; David Cebon (2007). Materials: engineering, science, processing and design (1st ed.). Butterworth-Heinemann. ISBN 978-0-7506-8391-3.
  8. J. R. Lamarsh, A. J. Baratta, Introduction to Nuclear Engineering, 3d ed., Prentice-Hall, 2001, ISBN: 0-201-82498-1.

See above:
Corrosion