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Day 36: Introduction to Corrosion






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Day 36: Introduction to Corrosion. Importance of Corrosion What is Corrosion? Some theory. The four things that are required for corrosion Types of Corrosion. Environmental Degradation of Materials. Materials are “attacked” by their operating environment.
Day 36: Introduction to Corrosion

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Slide 1

Day 36: Introduction to Corrosion

  • Importance of Corrosion

  • What is Corrosion? Some theory.

  • The four things that are required for corrosion

  • Types of Corrosion

Slide 2

Environmental Degradation of Materials

  • Materials are “attacked” by their operating environment.

  • We will focus on the degradation of metals. This is called corrosion.

  • Some attention will be paid to polymers, but none to ceramics.

  • In metals, corrosion is produced by the loss of actual material, which leaves the piece as an ion in solution, and is carried away by an electrolyte.

  • Rust is a symptom of this problem in steel, but there can be corrosion without it.

Slide 3

Importance of Corrosion

  • The impact of corrosion on society is very significant.

From NACE:

Direct Costs of Corrosion:

Nearly 300 G$ in 1998. Clearly, they rise proportionally till today.

Between 3-5% of the Gross Domestic Product.

Slide 4

When Protective Coatings Break Down, things can get ugly.

From Corrosion Doctors web site

This obvious, up front relatively uniform corrosion is relatively benign. We see it for a long time before it hurts us. Not all corrosion is so nice.

Slide 5

Corrosion Disaster

Atlantic Southeast 529, 8-21-1995

Lead wool added for balancing

Cork stopper

Slide 6

A Corrosion Disaster

The Safety Board concludes that one of the four blades from the left

engine propeller separated in flight because a fatigue crack that originated from multiple corrosion pits in the taper bore surface of the blade spar propagated toward the outside of the blade, around both sides of the taper bore, then reached critical size. (See Section 1.16.1.)

Results of investigations conducted in two previous propeller blade

failures in 1994, one in Brazil with this model blade and the other in Canada with a similar model blade, indicated that corrosion was produced when entrapped moisture reacted with residual chlorine in a bleached cork used to retain the lead wool in the taper bore hole of the propeller.

Point: Corrosion is subtle and very hard to detect

Slide 7

So, What exactly is corrosion?

  • Corrosion is an irreversible interfacial reaction of a material (metal, ceramic, polymer) with its environment which results in consumption of the material or in dissolution into the material of a component of the environment.

  • Chemistry is at work. We are talking about a certain class of chemical reactions between a metal and the environment.

Slide 8

Example – The Daniell Cell

  • This example illustrates some of the basics of corrosion.

  • On the surface of the Zn bar we have the following

  • On the surface of the Cu bar we have the following

Note the current path. The salt bridge provides for ion exchange.

Slide 9

Dissimilar Metals have Galvanic Potential

Any voltage, even if small will produce corrosion damage over time.

Clearly dissimilar metals will create a corrosion cell. The anodic metal will be damaged.

Anodic

Cathodic

Slide 10

Please note the presence of stainless steel

  • Yes, under certain circumstances, stainless becomes active.

  • Factors: (These are bad for any metal!)

  • Low aeration in water

  • Low velocity water

  • Presence of Cl-. Chlorine is one of the worst offenders in promoting corrosion.

Slide 11

REDOX reactions

  • Here is a typical reduction reaction involving hydrogen ions in solution. Note that the H gains electrons.

  • Here is an oxidation reaction. Fe is the symbol for iron. Note that metal looses electrons.

Slide 12

These Reactions want to occur in Pairs

We are assuming that the Fe is surrounded by a weak acid in which H+ ions are abundant.

This acid is called an electrolyte. It provides a home for the dissolve Fe+2 ion.

Note that there has to be an internal movement of electrons through the Fe.

Slide 13

Where is the Cathode?

  • At the location at which hydrogen is being liberated, we have a local cathode, associated with what is called a hydrogen overvoltage.

  • Summary: What’s needed for Corrosion

    • An anode. This is where the damage occurs. Oxidation takes place.

    • A cathode. Here’s where the reduction reaction takes place.

    • An electrolyte. (Almost any moisture will do.)

    • A current path between the cathode and anode.

Slide 14

General Reactions

  • Anode: (Metal basically dissolves in the electrolyte.)

  • Cathode: (This is a very common reaction!)

Surfaces near high O2 concentration are cathodic!

Slide 15

Concentration Cell

Slide 16

Types of Corrosion

  • Uniform - common surface effect.

  • Galvanic - dissimilar metals.

  • Crevice corrosion.

  • Pitting.

  • Intragranular.

  • Errosion corrosion.

  • selective leaching. De-zincification of brass

  • Stress corrosion.

  • Hydrogen embrittlement

Slide 17

Uniform Corrosion

  • This one is common in steel that is unprotected by any surface coating. Most noticeable. Surface effect, leaving rust on the surface.

  • The good thing about this, if there is one, is that the corrosion is widely spread around.

  • The more dangerous forms of corrosion are:

  • Highly localized, concentrated.

  • Hidden.

Electrolyte?

Slide 18

Galvanic Corrosion

Steel screw in Mg

Steel screws and brass

Dissimilar metals, the damage occurs at the anode.

Slide 19

Crevice Corrosion

This is a concentration cell in action. Notice how the damage occurs in out of sight places.

Slide 20

Pitting

  • This is similar to crevice corrosion. It is based on low oxygen concentration at the bottom of the pit.

  • This is very common in materials that protect themselves with a passive layer, i.e. stainless. Also, aluminum.

Highly localized. Goes deep into the metal.

Chloride ions find their way into the pits, exacerbating the situation.

Slide 21

Stress Corrosion

  • Sometimes called stress corrosion cracking.

  • Ingredients: (1) tensile stress in the metal (2) corrosive (electrolyte) environment.

  • Accelerators: presence of Chloride ion and high temp.

  • Victims: Stainless steel is unsafe in water above 50C and over a few ppm of chloride, if any tension exists. Others: mild steel in alkaline environment, copper alloys in ammonia env.

  • The anode is the stresses region.

Slide 22

SCC in Stainless Steel

Failure is along grain boundaries.

Slide 23

Intergranular Corrosion

  • This is a segue from the previous. It is closely related.

  • Again, stainless steel is the ideal victim here. The problem is triggered by improper heating, and often this comes with welding. Carbides of chromium form in the grain boundary regions.

  • The chromium is tied up in the carbides. It can’t protect by forming the passive layer.

  • PLUS, there is a dissimilarity in metals producing a small but definite galvanic corrosion.

Slide 24

More intergranular

  • Exfoliation corrosion in Aluminum that has been heavily worked, such as in extrusion.

  • Corrosion products start to build up in between the long elongated grains, separating them and leadin to increased corrosion propagation through the metal.

Slide 25

Selective Leaching

  • Another example of microstructural corrosion.

  • In an alloy system, one phase may be anodic with respect to another phase.

  • Example: dezincification of brass.

  • Example: graphitization of cast iron.

Slide 26

Erosion Corrosion

  • This is caused by the impingement of a high velocity turbulent flow on a surface.

  • The flow is often multi-phase. This means there can be entrained solid particles, or even gas bubbles, as in cavitation of a propeller.

  • The flow will carry away any protective layer that was intended to protect the material, and even abrade the flow surface.

Slide 27

Hydrogen Embrittlement

  • This is not exactly galvanic corrosion, but it definitely is a form of environmental attack.

  • Hydrogen atoms diffuse into the metal from outside. Deep in the metal, they combine to form H2 gas or combine with C, if present to form CH4.

  • The pressure in this internal pockets of gas is enough to initiate cracking.

  • The metal is already seeing a lot of tensile stress.

  • Normally ductile high strength metals, particularly steels, are not so ductile anymore because of these internal cracks.

Slide 28

Where does the Hydrogen come from?

  • Arc welding can a source. Hydrogen might be released from the electrode.

  • Galvanic corrosion can produce hydrogen in a reduction reaction.

  • Sour gas wells

  • Hydrogen storage (You just don’t use high strength steel!)

Slide 29

Corrosion Protection

  • Protection of the Anode. (Passivation)

  • Reduce the activity of the cathode and or electrolyte. (Polarization)

  • Sacrificial Anodes

  • Impressed Voltages

Slide 30

Passivation of the anode

  • We have two examples already. Stainless and aluminum.

  • A thin oxide layer forms on the surface and isolates the metal from the environment.

  • Zn, Mg, Cu and Ti are also capable of passivation under normal conditions of operation.

  • Steel will also passivate in the presence of an alkaline environment, such as rebar in concrete.

  • Corrosion inhibitors. Some of these, such as the chromates, are capable of coating a steel and passivating it.

  • Coatings, paints, etc.

Slide 31

Polarization

  • This is an effect which reduces the actual chemical potential driving the cell. If the thermodynamic force driving the ion into solution is reduced, this is polarization.

  • Easy example. By lowering the electrolyte temperature, we find that it is usually less corrosive. Diffusion of ions is slowed.

  • Inhibitors are chemicals which slow corrosion. Some of them do this by promoting the polarization of the cathode.

Slide 32

Sacrificial Anodes

  • Galvanization of Steel

  • Dip steel sheet in molten zinc. Get a pretty thin coating.

  • Zinc will be anode. Steel exposed by crack is the cathode. Since we have a huge anode having to be served by a small cathode, corrosion rate will be slow.

Tiny cathode (steel)

Large area anode (zinc)

An example of a favorable area ratio. Bad deal: huge cathode, tiny anode

Slide 33

Another Example

  • Zinc is attached to the steel hull of the vessel.

Attachment points

Slide 35

Sacrificial Anode for a Pipeline

Slide 36

Impressed Voltage

By imposing a voltage which causes electrons to flow towards the object to be protected, we make it less anodic and protect it from corrosion damage.

Slide 38

Polymer Degradation

  • Swelling and Dissolution (Solvents)

  • Bond Rupture

    • Radiation (UV and higher)

    • Chemical Reaction Effects (Oxygen and Ozone)

    • Thermal Effects

Slide 39

http://inside.mines.edu/~dwu/classes/CH351/links/images/Foxtrot%20comic%20UVbull.gif

Slide 40

UV Degradation

  • Exposure to UV can result in deterioration of appearance and mechanical properties.

  • UV photons have sufficient energy to break carbon-carbon bonds

  • UV + Oxygen is photooxidation

  • The property degradation is due to

    • Chain scission (reduction in molecular weight)

    • Crosslinking (loss of ductility)

    • Induced Crystallization

http://en.wikipedia.org/wiki/UV_degradation

Slide 41

Free Radical oxidation of UHMWPE tibial implant. Could happen in vivo or in vitro. Vitamin E has been tried to deal with the free radicals.

http://www.informaworld.com/smpp/260129486-71745926/ftinterface~content=a906724758~fulltext=713240928

Slide 42

http://media.iupac.org/publications/pac/1972/pdf/3001x0135.pdf

Slide 43

http://media.iupac.org/publications/pac/1972/pdf/3001x0135.pdf


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