Lecture 10: Crevice Corrosion and Pitting

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The Nature of Metal/Environment

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Crevice corrosion:

Localised corrosion resulting from the formation of a concentration cell in a crevice formed between a metal and nonmetal, or between two metal surfaces.

Two prerequisites:

Case 7.1

Case 7.2

Case 7.3

Case 7.4

In 1981, it was reported that one of the most serious problems in the US nuclear industry was "denting" (localised attack) of Inconel 600 tubing because of the corrosion in crevices between the tubes and carbon steel support plates.

With about 60 steam generators affected, the COST of rectifying the known problems was estimated to be US$6000 million.

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The Mechanisms of Crevice Corrosion

The Fontana and Greene Model

Stage 1

corrosion occurs as normal both inside and outside the crevice:

anodic reaction: M=>Mn+ + ne

cathodic reaction: O2+2H2O +4e=4OH-

The positively charged metallic ions are electrostatically counterbalanced by OH-

Stage 2

at this stage, the cathodic reaction inside the crevice consumed most of the oxygen available.

Inside the Crevice Outside the Crevice
O2 depleted O2 readily available
Anodic reaction cathodic reaction

Stage 3

Inside the Crevice Outside the Crevice
O2 depleted O2 readily available
Anodic reaction cathodic reaction
High [Mn+] concentration High [OH-] concentration
Overall positive Overall negative
High [Cl-] concentration Normal [Cl-] concentration

Cl- and OH- diffuse into the crevice to maintain a minimum potential energy.
=>Metal chloride is formed. Hydrolysis of metal chloride lowers pH=>

MCln + nH2O = M(OH)n + nHCl

Stage 4

Inside the Crevice Outside the Crevice
Low pH Normal pH
High [Cl-] concentration Normal [Cl-] concentration
High [Mn+] concentration Low [Mn+] concentration

More Mn+ ions attrack more Cl- leads to lower pH inside crevice
=> accelerate metal dissolution=>More Mn+ ions produced =>attrack more Cl- =>lower pH
=> autocatalytic process

For stainless steel, it is the dissolution and hydrolysis of Cr that leads to the fall in pH:

Cr3+ + 3H2O = Cr(OH)3 + 3H+

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PITTING CORROSION

Definition:

Extremely localised attack that results in holes in metals.

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Characteristics of pitting:

(1) difficult to detect

(2) difficult to measure/compare

(3) difficult to predict

(4) vicious

(5) shape of pits

(6) growth of pits

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Mechanism of pitting

Propagation mechanism same as crevice corrosion:

concentration cell causes local acidification within pit.

autocatalytic nature

Initiation of pitting is different from crevice:

Crevice requires physical crevice - a gap between two surfaces

Pitting has no geometrical requirement

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Differential Aeration Caused Pitting

Pitting underneath a water droplet

(a) initiation period:

general/uniform corrosion

Fe = Fe2+ + 2e

(b) the center of the water droplet is depleted in O2.

Concentration cell causes separation of anode and cathode:

centre of droplet: anode

edge of droplet: cathode

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Summary

Pitting corrosion is one of the most damaging forms of corrosion. It may be initiated by metallurgical factor or environmental factor or both. Once initiated, the propagation is autocatalytic (self-accelerating) in nature. Crevice corrosion is caused by the presence of a physical gap (crevice) between two surfaces that leads to the set up of differential aeration cell. Inside the crevice, anodic reaction is also self-accelerating (autocatalytic) in nature. The processes inside the creive is essentially the same as the propagation of pitting. Stainless steels and alloys are particularly susceptible to pitting and crevice corrosion.

Reading Assignments

To reinforce learnings in this lecture read pages 162-172 (textbook)
To prepare yourself for the
next lecture read pages 172-177 (textbook)

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