1. Some metals react with;
Reaction of Metals
Some metals react with;
Water – producing metal hydroxides and hydrogen
Acids – producing metal salts and hydrogen
Air – producing metal oxides
Reaction of Metals

2. Reactions of Metals
Reaction of Metals

3. Rusting
Rusting

4. Reactivity Series
In the reactivity series of metals, the most reactive metals are put at the top and the least reactive at the bottom
The reactivity series can be determined by looking at the relative reactivity of metals with air, water and acids
Reactivity Series

5. Reactivity Series
Reactivity Series

6. Reactivity Series
Reactivity Series

7. Displacement Reactions
A more reactive metal can displace a less reactive metal from its compound
Non-metal elements carbon and hydrogen can also displace less reactive metals form oxides of those compounds
Displacement Reactions

8. Displacement Reactions

9. Reduction using carbon
Some unreactive metals are found in their natural state (e.g. gold)
Often metals are found as metal oxides
To extract the metal, the oxygen must be removed from the metal oxide
This is called reduction
Metals below carbon in the reactivity series can be extracted by heating with carbon
Reduction using carbon

10. Reduction using carbon

11. Reduction using carbon

12. Iron can be extracted from iron ore in the blast furnace
The raw materials are iron ore, coke (carbon), and limestone
Hot air is used to convert carbon to carbon monoxide
Carbon monoxide reduces iron oxide to iron
Limestone reacts with impurities (e.g. sand) to produce molten slag
The Blast Furnace

13. The Blast Furnace
The Blast Furnace

14. Removing impurities
Removing impurities

15. The Blast Furnace
The Blast Furnace

16. Electrolysis
Metals above carbon in the reactivity series are extracted using electrolysis
Electrolysis is the process of splitting up compounds using electricity
Electrolysis only works if the substance is molten or dissolved (so the ions are free to move)
Positively charged ions (cations) move to the cathode, negatively charged ions (anions) move to the anode
Electrolysis

17. Electrolysis
Electrolysis

18. Electrolysis
Electrolysis

19. Purifying copper
Purifying copper

20. Electrolysis of Aluminium Oxide

21. Electrolysis of Sodium Chloride
Sodium Chloride (common salt) is found in the sea and in underground deposits
Electrolysis of sodium chloride solution produces chlorine at the anode, hydrogen at the cathode and sodium hydroxide solutions
Chlorine bleaches damp litmus paper
Each product has important uses
Electrolysis of Sodium Chloride

22. Electrolysis of Sodium Chloride

23. Wordsearch
Wordsearch

24. Quiz
Quiz