CHEM 1A03 Lecture Notes - Lecture 9: Iron(Iii) Oxide, Oxidizing Agent, Oxidation State

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: David Brock

Document Summary

Reduction is associated with producing metals from their compound. Red iron (iii) oxide is reduced by carbon monoxide to iron. Fe2o3(s) + 3co(g) (cid:314) 2 fe(s) + 3 co2(g) The production of tin and copper metals are other examples where a metal compound is reduced to the metal. Therefore, the substance that cause or promotes the reduction of metal compounds to an elemental metal is called reducing agent. The reactions of substances with oxygen e. g. corrosion, burning of wood, combustion is called oxidation reaction. This also include the conversion of metals to its compounds by nonmetal e. g. chlorine and bromine. A substance that promotes the oxidation of a metal to produce a metal compound is called an oxidizing agent. The oxidizing agents from above are oxygen, chlorine, and bromine. During a redox reaction, some substance must accept the electrons that another substance looses. Balancing redox equations using half- reactions (ion electron method)