1. The following slides should help you with your revision, but should not be your only form of revision.
Remember to use your notes, a textbook, websites and Past Papers to help you. You can also ask a chemistry teacher for help too.

2. Complete the Summary of Reactions of Metals
Reacts with O2
Reacts with H2O
Reacts with Acid
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Dangerously Reactive forms metal oxide.
Reacts with cold water to form metal hydroxide + H2
Reacts explosively
Reacts form metal salt + H2O
Reacts with steam to form metal hydroxide + H2

3. Complete the Summary of Reactions of Metals
Reacts with O2
Reacts with H2O
Reacts with Acid
Tin
Lead
Hydrogen
Copper
Mercury
Silver
Gold
Platinum
Slowly forms metal oxide on heating
No reaction
No reaction
No Reaction

4. Revise the Reactivity Series
Metal Rhyme
Potassium Please
Sodium Send
Lithium Little
Calcium Charlie
Magnesium McLean
Aluminium A
Zinc Zebra
Iron If
Tin The
Lead Lazy
Hydrogen Horse
Copper Can’t
Mercury Munch
Silver Soft
Gold Grass
Platinum Properly.

5. Complete the summary of the Extraction of Metals…..Breaking Compounds
Metal Oxide
To Breakdown Oxide
Potassium oxide
Sodium oxide
Lithium oxide
Calcium oxide
Magnesium oxide
Aluminium oxide
Zinc oxide
Iron oxide
Tin oxide
Lead oxide
Copper oxide
Electrolysis of molten ore
Heat with reducing agent: C/CO/ CO2/ H2

6. What’s happening in the extraction of metals reactions?
To reduce a metal oxide to its metal requires the same amount of energy as the metal released to form the bonds in the oxide, since the same bonds are being broken as were made.
Metal oxides low in the activity series require only small amounts of energy to break the bonds, heat alone. This is because the oxides didn’t readily form in the first place; the metal is more stable on its own.
………………………………………………………..……………………..continued

7. What’s happening in the extraction of metals reactions?
Metal oxides high in the activity series require lots of energy to break the bonds, heat and electricity. This is because the oxides formed readily; the metals are more stable as oxides than as metals on their own.
Metals in the middle of the Activity Series tend to need coaxing both to form the oxide and to breakdown the oxide. Carbon, carbon monoxide or hydrogen can be used to help coax the metal oxide in the middle of the Activity Series to breakdown to form their metal.

8. What is Corrosion?
A chemical reaction which involves the surface of a metal changing from an element to a compound.

9. What is Rusting?
The special name given to the corrosion of iron.

10. What is required for corrosion?
Water and oxygen to be in contact with the surface of the metal.

11. What is the test for rust?
Ferroxyl indicator turns blue.

12. Name the two types of protection against corrosion
Physical protection
Sacrificial protection

13. Give 4 examples of physical protection
Painting
Greasing or oiling
Coating with plastic
Coating with other metals

14. What is required for sacrificial protection of a metal?
A more reactive metal is attached to the metal to prevent it from corroding

15. Mains electricity Batteries ( More accurately …cells)
To make many household appliances work a supply of electricity is needed, name the two forms the supply normally comes in?
Mains electricity
Batteries ( More accurately …cells)

16. What happens in an electrical wire when electricity is passed along?
There is a flow of electrons along the wire.

17. How can the voltage in electrochemical cell be made as large as possible?
The further apart the metals are from each other in the Electrochemical Series ( Check the Data Book!!) the greater the voltage produced.

18. Which pair of metals would give the largest volume?
Mercury and silver
Aluminium and magnesium
Zinc and iron
Lead and Calcium

19. What is the purpose of the electrolyte in an electrochemical cell?
The purpose of the electrolyte in the cell is to complete the circuit by enabling ions to carry the charge in the internal circuit.

20. What is the definition of an electrolyte?
An electrolyte is a solution or paste which allows electricity to move through it.

21. What types of solutions make good electrolytes?
Ionic solutions.

22. Why do ionic solutions make good electrolytes?
Ionic solutions make good electrolytes because the ions are free to move.

23. Which direction do electrons flow in an electrochemical cell?
Electrons always flow from the metal higher to the metal lower in the Electrochemical Series, via the external circuit.

24. What is the definition of a displacement reaction?
A more reactive metal will displace a less reactive metal from a solution of its ions.

25. Complete the Results for these Displacement Reactions:
Solution
Metal
Sodium
sulphate
Zinc sulphate
Copper sulphate
Silver nitrate Mg no
Yes Sn Cu
Conclusion:
A more reactive metal displaces a less reactive metal from a solution of its ions.

26. Zinc is added to copper (II) sulphate solution, what happens?Zn
Zn Zn
Cu2+ SO Zn2+ SO42-
SO42- Cu SO Zn2+
Cu2+ SO Cu SO42- Cu
Brown solid (Cu ) appears. Zn atoms go into solution,
blue colour becomes paler.

27. What is the definition of an alloy?
An alloy is a mixture of metals or of metals with non-metals.