The document discusses the reactivity series of metals and their reactions with water, acids, and oxygen. It explains that more reactive metals like sodium exist in compounds rather than as elements in the Earth's crust, due to their reactivity. The reactivity series is determined by comparing the relative abilities of different substances like metals and carbon to attract oxygen. Carbon is found to be more reactive than zinc but less reactive than aluminum based on its ability to remove oxygen from their oxides when heated together.

1. SCIENCE FORM 4
CHAPTER 5:
ENERGY AND
CHEMICAL
CHANGES

2. 5.3 THE REACTIVITY SERIES
OF METALS
•Why do gold, silver and platinum exist as
elements in the Earth’s crust and whereas
metals such as sodium and potassium do
not exist as elements in the Earth’s crust?
•Some metals are more reactive than
others.
•Different metals show different
reactivity with water, acids and oxygen.

3. • The reactions involving metals:
(i) Reaction of reactive metal with water to
produce alkali and hydrogen.
Metal + Water Metal hydroxide (Alkali)
+ Hydrogen
Example:
Sodium (natrium) + water sodium hydroxide
+ hydrogen

4. (I) REACTION OF REACTIVE METAL
WITH WATER TO PRODUCE ALKALI
AND HYDROGEN.
• https://www.youtube.com/watch?v=jI__JY7pqOM
• Comparing Li, Na and K
• https://www.youtube.com/watch?v=YRPuDQtB_5Y
Sodium in water explosion -Chemical Reaction
• https://www.youtube.com/watch?v=QQF61CFOySw
LITHIUM, POTASSIUM, SODIUM (NCSS – old version)
https://www.youtube.com/watch?v=Yj70bUtXd4Q
Reaction of calcium, magnesium, zinc with water

6. (ii) Reaction of reactive metal with dilute
acid to produce a salt and hydrogen.
metal + acid Salt + hydrogen
Example:
magnesium + hydrochloric acid
magnesium chloride + hydrogen

7. (II) REACTION OF REACTIVE METAL
WITH DILUTE ACID TO PRODUCE A
SALT AND HYDROGEN.
• https://www.youtube.com/watch?v=l0U7VDSxGHk
• Reaction of Mg, Al, Zn, Copper and Iron with HCl
• https://www.youtube.com/watch?v=SeKsLi_6WkY&l
ist=PLC10F4535D849964F&index=211
MAGNESIUM with hydrochloric acid

8. (iii) Reaction of metal with oxygen to form
metal oxide
Metal + Oxygen Metal oxide
Example:
Magnesium + oxygen magnesium oxide
sodium potassium

12. (III) REACTION OF METAL WITH
OXYGEN TO FORM METAL OXIDE
• https://www.youtube.com/watch?v=hQyJIxiSvUA
• Reaction of different metal powder with Oxygen
• https://www.youtube.com/watch?v=GWGIjd0cHUk
• Burning metal powders (Zn, Al, Mg, Fe) +
Thermochromism

13. SCIENCE MODULE CHAPTER 5
• https://www.youtube.com/watch?v=dmcfsEEogxs
SODIUM
https://www.youtube.com/watch?v=hjB96do_fRw&list
=PLC10F4535D849964F&index=31
CALCIUM

14. EXPERIMENT P.106 = P.107
Reaction of sodium and calcium with water

15. Reacts very actively with water
Reacts actively with water

16. EXPERIMENT PAGE 108
EXPERIMENT 5.2
REACTION OF METALS WITH ACID

18. OBSERVATION
• https://www.youtube.com/watch?v=q72nsOFSj-0
• Calcium and HCl
• https://www.youtube.com/watch?v=l0U7VDSxGHk
• Reaction of Mg, Al, Zn, Copper and Iron with HCl

19. 4MB/4MC/4MD – CORRECTION !!!
Reacts very actively
Reacts actively
Reacts less actively

20. EXPERIMENT PAGE 109
REACTION OF METALS WITH OXYGEN
https://www.youtube.com/watch?v=JHLvU
BRLDxM

24. OBSERVATION

25. DISCUSSION

26. CONCLUSION

27. EXPERIMENT P. 113

28. PROCEDURE
• https://www.youtube.com/watch?v=VamGz6S0Lk4
• Reducing Metal Oxides using Carbon
• https://www.youtube.com/watch?v=E5HsEKne1TE
• Lead oxide reduction

29. OBSERVATION

31. COPPER OXIDE  COPPER + CARBON DIOXIDE

32. IRON OXIDE  IRON + CARBON DIOXIDE

33. LEAD OXIDE  LEAD + CARBON DIOXIDE

34. ZINC OXIDE  ZINC + CARBON DIOXIDE

35. ALUMINIUM OXIDE  ??

36. DISCUSSION

39. CONCLUSION

40. • Based on their reactivity with oxygen, metals and
carbon (non-metal) can be arranged in a reactivity
series as follows:
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Copper
Silver
Gold
Potato
Soup
Can
Make
All
Cruel
Zoos
In
The
Land
Change
So
Good

41. THE POSITION OF CARBON IN THE
REACTIVITY SERIES
• The position of carbon in the reactivity series is
determined by comparing its attraction for oxygen with
other metals.
• When carbon is heated with a metal oxide, carbon can
remove oxygen from the metal oxide if carbon is more
reactive than the metal.
• Example,
When zinc oxide are heated with carbon, the oxygen in
the zinc oxide is removed by carbon. Therefore, carbon
is more reactive than zinc.

42. • When carbon is heated with aluminium
oxide, the carbon cannot remove oxygen
from aluminium oxide.
• This means that carbon is more reactive
than zinc but less reactive than aluminium.
• Therefore, carbon is positioned between
aluminium and zinc in the reactivity series.

43. CHAPTER 5: ENERGY AND CHEMICAL CHANGES QUIZ
5. Which of the following metals can be
extracted from their ores by heating their
oxides with carbon?
I. Tin
II. Iron
III. Zinc
A. I and II only
B. I and III only
C. II and III only
D. I, II and III

44. CHAPTER 5: ENERGY AND CHEMICAL CHANGES
QUIZ
6. Lead can be obtained by heating a mixture of lead
oxide and carbon. This reaction takes place because
carbon
A. is a fuel
B. acts as a catalyst
C. is more reactive than lead
D. is a non-metal whereas lead is a metal