Corrosion is the gradual destruction of a material, usually a metal, by chemical or electrochemical reaction with its environment. In engineering, corrosion matters because it can weaken bridges, pipes, ships, tanks, aircraft, and fasteners long before they visibly fail. Different corrosion patterns reveal different causes, so identifying the type helps engineers choose the correct inspection and protection method.
Saltwater, moisture, oxygen, acids, temperature, and contact between dissimilar metals can all increase corrosion risk.
Most metal corrosion is electrochemical, meaning one area of the metal acts as an anode where metal atoms lose electrons, while another area acts as a cathode where a reduction reaction consumes electrons. An electrolyte such as water containing dissolved salts allows ions to move, completing the corrosion cell. Uniform corrosion spreads over a surface, while localized forms such as pitting, crevice corrosion, galvanic corrosion, and stress corrosion cracking can cause severe damage in small regions.
Engineers reduce corrosion by choosing compatible materials, applying coatings, controlling the environment, using inhibitors, and adding sacrificial anodes or impressed current cathodic protection.
Key Facts
- Anodic metal loss: M -> M^n+ + ne-
- Common oxygen reduction in neutral water: O2 + 2H2O + 4e- -> 4OH-
- Uniform corrosion rate can be estimated by corrosion rate = thickness loss / time
- Galvanic corrosion occurs when dissimilar metals are electrically connected in an electrolyte, with the more active metal acting as the anode.
- Pitting corrosion is dangerous because a small surface opening can hide deep metal loss and high local current density.
- Cathodic protection works by forcing the structure to behave as a cathode, often using a sacrificial anode such as zinc or magnesium.
Vocabulary
- Anode
- The region of a metal surface where oxidation occurs and metal atoms leave the solid as ions.
- Cathode
- The region of a metal surface where reduction occurs and electrons are consumed.
- Electrolyte
- A conductive liquid such as saltwater that allows ions to move between anodic and cathodic regions.
- Galvanic Series
- A ranking of metals and alloys by their tendency to corrode when electrically connected in a specific environment.
- Passivation
- The formation of a thin protective oxide film that slows further corrosion of a metal surface.
Common Mistakes to Avoid
- Assuming stainless steel cannot corrode, which is wrong because stainless steel can pit or suffer crevice corrosion if its passive film breaks down in chloride-rich environments.
- Treating all rust as uniform corrosion, which is wrong because localized forms such as pitting or crevice corrosion can cause deep penetration with little visible surface damage.
- Ignoring electrical contact between different metals, which is wrong because a galvanic couple can make the more active metal corrode much faster in the presence of an electrolyte.
- Using a coating without sealing edges, scratches, and bolt holes, which is wrong because exposed defects can become small anodic sites with concentrated corrosion current.
Practice Questions
- 1 A steel plate loses 0.45 mm of thickness over 3.0 years due to uniform corrosion. What is the average corrosion rate in mm/year?
- 2 A zinc coating has an available sacrificial thickness of 80 micrometers and corrodes at 5 micrometers per year in service. Estimate the coating life in years before the sacrificial layer is consumed.
- 3 A stainless steel bolt is tightened through an aluminum plate and exposed to seawater. Explain which corrosion type is likely, which metal is more at risk, and one design change that would reduce the problem.