This document discusses reactivity of metals and minerals. It begins by describing the different types of minerals found in rocks and ores, including natural elements like gold and compounds like limestone. It then explains how the reactivity of metals can be determined by observing their reactions with oxygen and other substances. Experiments are described to determine the position of carbon and hydrogen in the reactivity series by observing whether they can displace metals from metal oxides when heated. The document concludes that understanding the reactivity series is important for extracting metals from their ores.

1. Chapter 4
REACTIVITY OF METALS

2.  MINERALS IN THE EARTH CRUST
 Each type of ore is different in terms of colour, structure, shape and texture
because the ores contain different minerals.
 NATURAL ELEMENTS
 NON REACTIVE ELEMENTS
 DOESN’T COMBINE WITH OTHER ELEMENTS
 EXAMPLES : GOLD (AURUM) AND SILVER ( ARGENTUM)
 NATURAL COMPOUNDS
 COMBINATION OF TWO OR MORE ELEMENTS
 COMBINATION BETWEEN METAL ELEMENTS AND NON-METALS ELEMENTS
1. MINERALS

3. 1.Sedimentary rock
limestone, sand stone
2. Igneous rock
Granite,basalt,
3. Metamorphic rock
Marble, gneiss
EXAMPLE OF ROCK

4. Earth’s crust  rock  mineral
Natural elements
(gold)
Natural compound
Bauxite ( Al, O )

5. Gold, diamond, silver
Diamond contain 100% atom
carbon
Gold=100% atom gold
Silver= 100% atom of silver
ELEMENTS MINERALS
(MINERAL BENTUK ELEMENTS)

6. Rock : lime stone
Contained mineral
 calcium carbonate [compound], calcite
Elements contained in calcium carbonate are
calcium,oxygen and carbon
NATURAL COMPOUND

7. = NOT elements
But Compound
Elements in Quartz are Silicon
and Oxygen
QUARTZ

8. MINERAL IN GRANITE(ROCK)

10. CAN BE DETERMINED BY MINERAL
Hardness
Resistance against erosion and scratches
Example - diamond has the highest hardness
Solubility in water
Whether mineral dissolves in water or not
Effects of heat
Whether minerals decomposed (breakdown into simpler
substances/elements) upon heating
CHARACTERISTICS OF MINERALS

11. Common name Scientific name Combination of
elements
Diamond Diamond carbon
Gold Gold Gold
Silver Silver Silver
NATURAL ELEMENTS

12. Common name Scientific name Combination of
elements
Hematite (Iron
ore)
Ferum(III) oxide Ferum(iron),oxygen
Pyrite Ferum (II) sulphide Ferum, sulphur
Cassiterite
(Tin Ore)
Stanum (IV) oxide Stanum,oxygen
EXAMPLES OF NATURAL COMPOUNDS

13. Bauxite
 elements of aluminium and oxygen
Quartz
element of silicon and oxygen
Galena
element lead and sulphur
EXAMPLES OF COMPOUNDS AND THEIR ELEMENTS

14. Common name Scientific name Combination of
elements
Lime stone Calcium
carbonate
Calcium, carbon
,oxygen
Sand stone Silicon dioxide Silicon,
oxygen
ELEMENTS OF LIME STONE

15.  Limestone is a natural compound
 Formed from the combination of calcium, carbon and oxygen.
 Also known as CALCIUM CARBONATE
 Properties of Limestone
 Insoluble in water
 Decomposed upon heating to form CALCIUM OXIDE and CARBON DIOXIDE IS RELEASED.
 = HEATED
 Reacts with dilute acid to form SALT, WATER AND CARBON DIOXIDE.
LIMESTONE
CALCIUM CARBONATE CALCIUM OXIDE + CARBON DIOXIDE
CALCIUM CARBONATE +DILUTE ACID SALT + WATER + CARBON DIOXIDE

16. Limewater shown CLOUDY
because Carbon dioxide
(CO2) is released
HEATING OF LIMESTONE ( CALCIUM CARBONATE)
■ Calcium oxide is
produced upon heating

17. After mixed hydrochloric
acid:
lime water turns
cloudy/chalky/milky
Because carbon dioxide
gas released
REACTION BETWEEN LIMESTONE AND DILUTE ACID

18. OBSERVATION
transparent
transparent
cloudy
cloudy

19. WORD EQUATIONS
REACTION BETWEEN CALCIUM CARBONATE WITH
DILUTE ACID
CALCIUM CARBONATE + DILUTE SULPHURIC ACID CALCIUM SULPHATE + WATER + CARBON DIOXIDE
CALCIUM CARBONATE + DILUTE HYDROCHLORIC ACID CALCIUM CHLORIDE + WATER + CARBON DIOXIDE
CALCIUM CARBONATE + DILUTE NITRIC ACID CALCIUM NITRATE + WATER + CARBON DIOXIDE

20. METALS AND NON-METALS
NATURAL ELEMENTS

21.  Metal reacts with non metals to form a more stable compounds
 The rate of reaction is different of each metals
 This is because some metals are reactive and some are less reactive
 A more reactive metal such as potassium is more reactive than ferum because
potassium reacts readily with other metals compare to ferum.
 A more reactive metal doesn’t need heat to react, some need to be heated to react
with other elements
 In fig 4.3, potassium has the highest reactivity compare to other elements, whereas,
Aurum or gold is a non reactive metal.
REACTIVITY SERIES OF METALS
REACTIVE METALS
NON REACTIVE

22.  Metal reacts with oxygen to form METAL OXIDE
 The rate of reaction is different of each metal (based on the reactivity series)
 Heat energy and/maybe light energy will be produced
 Non-reactive metals such as silver, gold and platinum do not react with oxygen
 Reactive metals such as potassium and sodium will react with oxygen even without the
presence of heat
 Other metals react with oxygen need heating.
 To supply oxygen to the reaction, POTASSIUM MANGANATE (VII) CRYSTAL is heated.
 Precautions when carrying out this experiment
 Do not mix the metal fillings with potassium manganate (VII) crystal – mixture will cause explosion
 Don’t look directly at the flame of burning reactive metal (such as magnesium) – it can damage
your eyes
 Asbestos paper and glass are dangerous, handle them with extra caution.
REACTION BETWEEN METAL AND OXYGEN
METAL + OXYGEN METAL OXIDE

23. EXPERIMENT

24. METAL OBSERVATION
RATE OF REACTION COLOUR OF FLAME COLOUR OF
PRODUCTS/RESIDUE
MAGNESIUM Metal burns very quickly and
brightly
Bright white flame Solid white
Magnesium oxide
ALUMINIUM Metal burns quickly and brightly Bright white flame Solid white
Aluminium oxide
ZINC Metal burns slowly Bright green blue flame Solid yellow-hot
Solid white – cold
Zinc oxide
IRON Metal glows brightly Bright yellow Solid brown
Iron oxide
LEAD Metal glows dimly No flame (glow) Solid brown – hot
Solid yellow – cold
Lead oxide
OBSERVATION

25. REACTION BETWEEN METAL AND OXYGEN
CONCLUSION
Burns very fast with oxygen

26.  Page 133
QUESTIONS AND ANSWERS
Magnesium oxide

27.  Carbon is a non-metal
 Carbon reacts with oxygen to form carbon dioxide
 The position of carbon in the reactivity series can be determined by the reaction of
carbon with other metals
 When a mixture of carbon and metal oxide is heated strongly,
 REACTION WILL OCCUR if carbon is MORE REACTIVE than metal (CARBON WILL REMOVE METAL
FROM ITS METAL OXIDE)
 NO REACTION will occur if Carbon is LESS REACTIVE than the metal
POSITION OF CARBON IN THE REACTIVITY SERIES IN
METALS
CARBON + METAL OXIDE METAL + CARBON DIOXIDE

28.  1.mixture of carbon and zinc oxide
 Repeated by:-
 Carbon and aluminium oxide
 Carbon and lead oxide
DETERMINING THE POSITION OF CARBON IN THE
REACTIVITY SERIES OF METALS

29. Aluminium Oxide + Carbon  NO REACTION
CARBON + ALUMINIUM OXIDE

30. BEFORE HEATING
Aluminium oxide
carbon

31. AFTER HEATING … NO REACTION
Aluminium oxide carbon
CARBON CANNOT REMOVE ALUMINIUM FROM ALUMINIUM OXIDE BECAUSE ALUMINIUM IS MORE REACTIVE
THAN CARBON ( CARBON IS LESS REACTIVE THAN ALUMINIUM)

32. ZINC OXIDE + CARBON  ZINC + CARBON DIOXIDE
CARBON + ZINC OXIDE

33. LEAD OXIDE + CARBON  LEAD + CARBON DIOXIDE
CARBON + LEAD OXIDE

34. BEFORE
Lead oxide carbon

35.  LEAD
CARBON DIOXIDE
 CARBON CAN REMOVE OXIDE FROM LEAD OXIDE BECAUSE CARBON IS MORE REACTIVE
THAN LEAD.
AFTER

36. RESULTS
MIXTURE OBSERVATION INFERENCE
ZINC OXIDE + CARBON MIXTURE GLOWS BRIGHTLY CARBON IS MORE REACTIVE THAN
ZINC
ALUMINIUM OXIDE + CARBON NO REACTION CARBON IS LESS REACTIVE THAN
ALUMINIUM
LEAD (II) OXIDE + CARBON MIXTURE GLOWS CARBON IS MORE REACTIVE THAN
LEAD
Aluminium, carbon, zinc, copper

37. CARBON
POSITION OF CARBON IN THE REACTIVITY OF METALS

38.  Hydrogen is a non-metal
 The position of hydrogen in the reactivity series of metal is also determined by its
ability to remove oxygen from metal oxide.
 If HYDROGEN is MORE REACTIVE than the metal, HYDROGEN WILL REMOVE OXYGEN
from the METAL OXIDE.
 HYDROGEN
POSITION OF HYDROGEN IN THE REACTIVITY SERIES

39. APPARATUS SET-UP TO DETERMINE THE POSITION OF
HYDROGEN IN THE REACTIVITY SERIES OF METALS

40. RESULTS

41. Aluminium Oxide + Hydrogen NO REACTION
Zinc Oxide + Hydrogen  NO REACTION
Iron oxide + Hydrogen  IRON + WATER
Copper oxide + Hydrogen COPPER + WATER
WORD EQUATIONS

42.  Most metals in metal ores exist in the form of metal oxides, metal sulphides and metal
carbonates
 Extraction of metals involve in the reducing of metal ores to metal or obtaining metal
from their ores
 Position of metals in the reactivity series will determine the suitable method for the
extraction of metals
 Carbon is widely used to extract iron, tin, zinc and lead from their ores because carbon
is more reactive than these metals.
 CARBON IS KNOWN AS REDUCING AGENT
EXTRACTION OF METALS FROM THEIR ORES

43.  THANK YOU AND GOOD LUCK
 IF YOU HAVE DONE YOUR VERY BEST, YOUR BEST IS ENOUGH!
 TCER P