|2. Understanding Corrosion|
2.2 Corrosion Components
No metal would corrode, until it has four essential constituents which
constitute a corrosion cell. The following are the four essential
(1) Anode: It is the site
where oxidation occurs. An anodic reaction is accompanied by loss of
electrons. Typical anodic reactions are given below
Fe Fe2+ + 2e
Al Al3+ + 3e
Zn Zn2+ + 2e
Mg Mg2+ + 2e
(2) Cathode: It is the site where reduction takes place. The electrons released at the anode travel to the cathode by a metallic path where they react with the ions in the electrolyte and cause reduction of the positive ions. The cathodic reaction is accompanied by a gain of electrons. Following are the major cathodic reactinos in corrosion of metals in aqueous solution.
2H+ + e H2
O2 + 4H+ + 4e 2H2O (in acid solution)
2H2O + O2 + 4e 4OH- (in neutral solution)
(3) Electrolyte: It provides a conductive medium for passage of ions which act as charge carriers, like Fe2+ ions, which carry a positive charge and flow from anode to cathode.
(4) Metallic path: It provides the flow of electrons from the anode to cathode. All metals provide the electron path.
All the above four components are shown in the figure below. The flow of electric current is also shown.