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Metals

Metals. Learning Objectives. Use reactivity data to determine a reactivity series Relate extraction method to reactivity of metals Write word/symbol equations for reduction of metal ores with carbon. Put the metals in order of reactivity. Displacement reactions. Magnesium. Copper sulphate.

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Metals

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  1. Metals

  2. LearningObjectives • Use reactivity data to determine a reactivity series • Relate extraction method to reactivity of metals • Write word/symbol equations for reduction of metal ores with carbon

  3. Put the metals in order of reactivity

  4. Displacement reactions Magnesium Copper sulphate Mg Cu SO4 The magnesium DISPLACES the copper from copper sulphate Mg SO4 Cu Magnesium sulphate Copper A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound.

  5. The Thermite reaction Fe O Al Aluminium Iron oxide Aluminium DISPLACES iron from iron oxide Simplified and NOT balanced equation

  6. Pie chart to show the elements present in the earth’s crust

  7. Most elements in the earth’s crust are found as compounds Compounds contain atoms of more than 1 element ---------- joined together. There are 2 types of chemical ---- IONIC bonds are formed between a metal + non metal. The metal atom TRANSFERS electrons to the non metal. COVALENT bonds are formed between non metals. The atoms SHARE electrons.

  8. Extraction methods 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 Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Copper Silver Gold Platinum Increasing reactivity

  9. Native metals Unreactive elements (Gold, silver and sometimes copper) do not need to be extracted as they are not chemically combined with any other elements.

  10. Iron Magnetite (iron oxide Fe3O4) Magnetite Hematite (iron oxide, Fe2O3)

  11. Metal ores • Minerals in rocks are not pure, but mixed with other substances. • To be useful the metal needs to be extracted from the rock. • A metal ore is a rock containing enough of the metal compound to make it economic to extract it. • This can vary over time as demand/ supplies/ value change.

  12. The Blast furnace Waste gases escape Raw materials added Coke (carbon to help reduce the iron oxide) Limestone (to remove acidic impurities) Iron ore Oxygen in the air reacts with carbon to make carbon monoxide that reduces the iron ore) Hot air Molten SLAG Molten IRON

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

  14. Equations From an oxide: Iron oxide + carbon carbon dioxide + iron (Fe2O3) 2Fe2O3 + 3C  3CO2 + 4Fe From a sulfide: Copper sulfide + oxygen  sulfur dioxide + copper oxide (CuS) 2CuS + 3O2 2SO2 + 2CuO Copper oxide + carbon  carbon dioxide + copper (CuO) 2CuO + C  CO2 + 2Cu

  15. Summary: Extracting metals • What is an ore? • In what form are metals usually found in the Earth? • How do you get a metal out of a metal oxide? • What is this type of reaction called?

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