1. Metals

2. Learning Objectives Order metals in order of reactivity Relate extraction method to reactivity Write word/symbol equations for reduction of metal ores with carbon

3. Iron Hematite (iron oxide, Fe 2 O 3 ) Magnetite Magnetite (iron oxide Fe 3 O 4 )

4. Put the metals in order of reactivity MetalReaction with dilute acid Reaction with water Reaction with oxygen A Some reactionSlow reactionBurns brightly B No reaction Reacts slowly C No reaction D Violent reactionSlow reactionBurns brightly E Reasonable reaction Reacts with steam only Reacts slowly

5. Displacement reactions Mg Magnesium SO 4 Cu Copper sulphate The magnesium DISPLACES the copper from copper sulphate SO 4 Mg Magnesium sulphate Cu Copper A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound.

6. Displacement reactions A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound. E.g. if you drop some magnesium into copper sulphate a reaction will happen because magnesium is more reactive than copper, so the reaction is: Magnesium + copper sulphate copper + magnesium sulphate However, if you drop some copper into magnesium sulphate NOTHING will happen.

7. Extraction methods Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Copper Silver Gold Platinum Metals ABOVE CARBON, because of their high reactivity, are extracted by ELECTROLYSIS Metals BELOW CARBON are extracted by heating them with carbon in a BLAST FURNACE These LOW REACTIVITY metals don’t need to be extracted because they are SO unreactive you’ll find them on their own, NATIVE (not in a metal oxide) N.B. Cu can sometimes be found native Increasing reactivity

8. Reduction with carbon Zinc, iron, tin, lead and copper can all be extracted from their ores by SMELTING. Metal ore (usually an OXIDE) is heated to a high temperature with carbon. Carbon competes with the metal for the oxygen and DISPLACES it. This is a REDOX process, the carbon is OXIDISED (gains oxygen) at the same time the metal ore is REDUCED (loses oxygen)

9. Equations Copper oxide + carbon  carbon dioxide + copper (CuO) 2CuO + C  CO 2 + 2Cu Iron oxide + carbon  carbon dioxide + iron (Fe 2 O 3 ) 2Fe 2 O 3 + 3C  3CO 2 + 4Fe

10. Summary: Extracting metals 1)What is an ore? 2)In what form are metals usually found in the Earth? 3)How do you get a metal out of a metal oxide? 4)What is this type of reaction called? Type of metalExtraction processExamples High reactivity (i.e anything above carbon) Middle reactivity (i.e. anything below carbon) Low reactivity