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Definition of corrosion
Corrosion is the oxidation of metals by certain substances (mostly water and oxygen) in the environment. A metal corrodes when it gives up its electrons and loses strength and elasticity. Some common examples of corrosion include rusting of iron, surface oxidation of aluminium, tarnishing of silver and verdigris on copper. Corrosion can be classified into two categories
• Dry corrosion where the metal is oxidised directly by atmospheric oxygen.
• Wet corrosion is when the presence of water and air accelerates the process of corrosion.
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The condition which rusting of irons occurs
For iron and for any other metal, any region of electrochemical corrosion must have
a) an anode where oxidation occurs
b) a cathode where reduction occurs
c) a meta path for electron and
d) an electrolyte.
The rusting of iron will be hastened by the following conditions
1. The presence of oxygen is large concentrations at the surface of iron which will accelerate the corrosion of another area with less oxygen if there is electrical contact between them. This helps to explain why corrosion pits in iron can be very deep. Since the bottom of the pit has less oxygen than the top, it will act as an anode and corrosion in the pit will be accelerated.
. Pure iron is more resistant to corrosion than impure iron. Electrochemical cells can occur if, for example, copper is present. Copper can serve as a cathode half-cell since its atoms are less readily oxidised than iron atoms. The electrons travel through the iron and the ions through a moisture film to complete the circuit.
. Iron corrodes more readily where ions in the metal lattice have been distorted by stress.
The rusting of iron
Corrosion prevention
There are two basic ways of protecting metal surfaces from corrosion physical protection and galvanic protection.
• Physical protection eg. Paint and lacquer. The paint and acquer acts as a physical barrier which stops oxygen and water from making contact with the metal.
• Galvanic protection eg Cathodic protection. Ther are two main types of cathodic protection presently in use.
1. Sacrificial anode. Steel pipes, tanks ans ships are protected
galvanically by attaching lumps of magnesium or zinc to the
steel. The more active metal is more readily oxidised and
behaes as a sacrificial anode, whilst the steel is cathodically
protected.
. Impressed current. Metals such as iron can be connected to
the negative pole of a power source such as a battery.
Electrons are pushed onto the iron which is then cathodically
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