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.
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
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
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
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
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
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
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)
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
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
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