Starter 1. The following metals were reacted with water. Put them in order of reactivity, with the least reactive metal first. Lithium, potassium, calcium,

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Presentation transcript:

Starter 1. The following metals were reacted with water. Put them in order of reactivity, with the least reactive metal first. Lithium, potassium, calcium, sodium, magnesium. Magnesium, calcium, lithium, sodium and potassium. 2. Write the three general equations for metals reacting with oxygen, acids and water.

Aim: To discuss how metals can be extracted from their natural compounds (called ores) by the following processes: Heating metal oxide Heating metal oxide with carbon Electrolysis of the metal oxide

Extracting Metals from their Ores Unreactive metals such as gold and silver are found uncombined in the earth’s crust. (due to their unreactivity) Most other metals are found combined in ores. Ores are naturally-occurring compounds of metals. To obtain the pure metal a process of EXTRACTION is used. This involves separating the metals from the other elements with which they have combined.

The first metals to be discovered were the least reactive ones: gold and silver. This is because the less reactive the metal, the easier it is to extract from its ore. Some metals can be obtained from their metals oxides by: 1. Heating metal oxide 2. Heating metal oxide with carbon 3. Electrolysis of the metal oxide

1. Extracting the Metal from the Metal Oxide by Heating Glowing splint Pyrex test tube Compound Observation Copper oxide Silver oxide No change Silver metal formed, glowing splint relit

Conclusion; Oxides of more reactive metals are more difficult to decompose (breakdown). Oxides of metals below copper in the reactivity series decompose when heated to give the metal and oxygen. Metal oxide  Metal + Oxygen Silveroxide  silver + oxygen 2(Ag+)2O2-(s)  4Ag(s) + O2(g) Ag+ + e-  Ag REDUCTION

2. Extracting the Metal from the Metal Oxide by Heating with Carbon Pyrex test tube Metal oxide + carbon powder Heat Compound Observation Copper oxide Magnesium oxide Brown powder formed No change

Conclusion: Metals below aluminium in the reactivity series can be extracted from their oxides by heating with carbon. The carbon and oxygen join to give carbon dioxide. Metal oxide + carbon Metal + carbon dioxide

3. Extracting the Metal from the Metal Oxide by Electrolysis The most reactive metals are extracted by electrolysis of their molten ores. Metal oxide  Metal The positive metal ions are attracted to the negative electrode where it accepts electrons. The metal ion in the compound gains electrons. The extraction of the metal from its ore is an example of reduction.