The document discusses the variety of minerals found in the Earth's crust, including both natural elements like gold and silver as well as natural compounds like bauxite and magnetite. It also covers the reactivity series of metals and how more reactive metals must be extracted from their ores using methods like heating with carbon or electrolysis, while less reactive metals can be found in purer form. A variety of everyday uses for common minerals are presented, along with the environmental impacts that can result from mining activities.

1. Form 3
-Ms Rachel-

2. 4.1
Variety of Minerals

3. Variety of Minerals
1. The Earth’s crust contains different
types of rocks that vary in colour,
shape, texture, structure and
formation.
2. All rocks contain compounds known
as minerals.
https://www.australiancurriculumlessons.com.au/2017/04/08/kind-rock-science-geology-lesson-year-8/

4. Variety of Minerals in the Earth’s crust
Minerals are elements or compounds which occur naturally in the earth’s crust and
have a specific chemical composition.
Minerals
Non-reactive
mineral
Natural elements
>Gold
>Silver
Reactive
mineral
Natural compounds
>Magnesium
>Zinc >Iron
>Aluminium
React with other elements
(oxygen, sulphur & carbon)
So that they become
chemically stable
Metal + Oxygen → Metal oxide
Metal + Oxygen + Carbon → Metal carbonate
Metal + Sulphur → Metal sulphide
Metal + Silicon+ Oxygen → Metal silicate
e.g. aluminium oxide, magnesium carbonate, iron
sulphide, calcium silicate, etc.

5. Variety of Minerals in the Earth’s crust
Minerals
Natural
elements
a) Gold 金
b) Silver 银
c) Platinum 白金
d) Mercury 水银
e) Diamond 钻石
Natural
compounds
a) Bauxite 铝土矿
b) Haematite 赤铁矿
c) Galena 方铅矿
d) Cassiterite 锡石
e) Magnetite 磁铁矿

6. Elements that Exists in Natural Compounds
Common name Systematic name Element combination
Bauxite (aluminium ore) 铝土矿 Aluminium oxide Aluminium, oxygen
Cassiterite (tin ore) 锡石 Tin (IV) oxide Tin, oxygen
Haematite (iron ore) 赤铁矿 Iron (III) oxide Iron, oxygen
Magnetite (Iron ore) 磁铁矿 Iron oxide Iron, oxygen
Pyrite (iron ore) 黄铁矿 Iron (II) sulphide Iron, sulphur
Galena (lead ore) 方铅矿 Lead (II) sulphide Lead, sulphur
Marble (limestone) 大理石(石灰石) Calcium carbonate Calcium, carbon, oxygen
Malachite (copper ore) 孔雀石 Copper (II) carbonate Copper, carbon, oxygen
Quartz (rock crystal) 石英 (水晶) Silicon dioxide Silicon, oxygen

7. Variety of Minerals in the Earth’s crust
Characteristics of minerals:
Very hard
used as knife
sharpening
stones
Soft
Can be cut
using a small
knife
Soluble in
water
Insoluble
in Water
Carbonate
minerals and
metal sulphides
will break down
when strongly
heated
Heat does not
affect metal
oxide minerals

8. Natural Mineral Uses in Daily Life
Aluminium oxide
- Sand paper
- Car and motorcycle parts
- High hardness
Silicon dioxide (Quartz)
- Make glass
- High melting point
- Inert against chemicals
Iron oxide
- Pigment in paint
- Red colour in nature
Magnesium carbonate
- Agent hand dryers for weightlifters,
rock climbers and gymnasts.
- Low solubility in water & hygroscopic
Silicates
- Electronic chips
- Have an electrical resistance
between conductors and insulators
Aluminium silicate (Kaolin)
- Crown tooth
- Hard
- Inert to acid
tending to
absorb moisture
from the air.

9. Natural Mineral Uses in Daily Life
Asbestos
- Firefighter suit
- High melting point
- Low thermal conductivity
Calcium carbonate
(Limestone)
- Neutralise an acid
- It is alkaline
Iron
- Manufacture of steel for
construction
Copper
- Electrical wire
- Good electrical conductor

10. 4.2
Reactivity Series
of Metal

11. Reactivity Series of Metals
1. Most metal minerals are natural compounds.
2. They tend to react with oxygen in the air to form metal oxide.
3. Temperature in the Earth’s crust > temperature of Earth’s surface, thus,
speeding up the chemical reactions between the metals with elements
(oxygen, carbon, sulphur) to form natural compounds minerals.
Reactive
Iron metal will rust when it is exposed to
oxygen in the air and rainwater. The brown
solid layer formed is the rust (metal oxide)
Non-reactive
Gold remains shiny though exposed to
air and water and does not react with
other elements
Metal + Oxygen → Metal Oxide
Metal + Oxygen → No Reaction

12. Potassium K
Sodium Na
Calcium Ca
Magnesium Mg
Aluminium Al
Carbon C
Zinc Zn
Hydrogen H
Ferum (Iron) Fe
Stanum (Tin) Sn
Plumbum (Lead) Pb
Copper Cu
Argentum (Silver) Ag
Aurum (Gold) Au
More
Reactive
Less
Reactive
Reactivity of
metal toward
oxygen
increases

13. Potassium K
Sodium Na
Calcium Ca
Magnesium Mg
Aluminium Al
Carbon C
Zinc Zn
Ferum (Iron) Fe
Stanum (Tin) Sn
Plumbum (Lead) Pb
Copper Cu
Argentum (Silver) Ag
Aurum (Gold) Au
Is heated to
supply oxygen
Prevent mixing
Reactivity of Metals towards Oxygen
http://spmchemistry.blog.onlinetuition.com.my/2012/12/series-of-reactivity-of-metals.html

14. Magnesium Mg Burns with a very bright white flame Solid white
Aluminium Al Burns with a white flame Solid white
Zinc Zn Burns with a bright flame Solid yellow (hot), solid white (cool)
Ferum (Iron) Fe Glows brightly Solid brown
Plumbum (Lead) Sn Glows dimly Solid brown (hot), solid yellow (cool)
Reactivity of Metals towards Oxygen
Metal + Oxygen → Metal oxide
Magnesium + Oxygen → Magnesium oxide
Aluminium + Oxygen → Aluminium oxide
Zinc + Oxygen → Zinc oxide
Iron + Oxygen → Iron oxide
Lead + Oxygen → Lead oxide
Reactivity of
metal toward
oxygen
increases
Reactivity can be determined by the
brightness of the flame during reaction

15. The Position of Carbon and Hydrogen
in the Reactivity Series of Metal
1. Carbon and hydrogen are two non-metal elements that often
combine with oxygen elements to form oxide compounds e.g.
carbon dioxide (𝑪𝑶 𝟐) and water (𝑯 𝟐 𝑶).
2. They are also reactive to oxygen. So, they have been
incorporated into the reactivity series of metals toward oxygen.
Carbon + Oxygen → Carbon dioxide
Hydrogen + Oxygen → Water

16. Mixture Observation
Copper (II) oxide carbon A flame spreads to the whole mixture. A brown residue is formed.
Zinc oxide carbon A glow spreads to the whole mixture. A grey residue is formed.
Aluminium oxide carbon No change Aluminium oxide + carbon → No reaction
C is more reactive
than Zn & Cu but
less reactive than Al
Potassium K
Sodium Na
Calcium Ca
Magnesium Mg
Aluminium Al
Carbon C
Zinc Zn
Ferum (Iron) Fe
Stanum (Tin) Sn
Plumbum (Lead) Pb
Copper Cu
Argentum (Silver) Ag
Aurum (Gold) Au
Carbon cannot
displace oxygen from
aluminium oxide
Carbon can displace
oxygen from copper
oxide and zinc oxide
Copper (II) oxide + carbon → Copper + Carbon dioxide
Zinc oxide + carbon → Zinc + Carbon dioxide
The Position of Carbon in the Reactivity Series of Metal
http://onelearningsolution.blogspot.com/2015/02/33-reactivity-series-of-metals-and-its.html

17. Mixture Observation
Copper (II) oxide hydrogen Black powder glow brightly and turns brown. Water droplets form on the tube.
Iron (III) oxide hydrogen Reddish-brown powder glow dimly and turns to shiny grey. Water droplets are formed.
Zinc oxide hydrogen No change Zinc oxide + hydrogen → No reaction
H is more reactive
than Fe & Cu but less
reactive than Zn
Potassium K
Sodium Na
Calcium Ca
Magnesium Mg
Aluminium Al
Carbon C
Zinc Zn
Hydrogren H
Ferum (Iron) Fe
Stanum (Tin) Sn
Plumbum (Lead) Pb
Copper Cu
Argentum (Silver) Ag
Aurum (Gold) Au
Hydrogen cannot
displace oxygen from
zinc oxide
Hydrogen can displace
oxygen from copper
oxide and iron oxide
Copper (II) oxide + hydrogen→ Copper + Water
Iron (III) oxide + hydrogen → Iron + Water
The Position of Hydrogen in the Reactivity Series of Metal
https://slideplayer.com/slide/10819066/

18. 4.3
Extraction of
Metals from its Ore

19. Extraction of Metals from its Ore
Pure metal is very useful for humans. Pure metals need to be extracted
from their mineral’s ore.
• Metals that are more reactive than carbon in reactivity series
• K, Na, Ca, Mg, Al
Electrolysis of molten ores by
using carbon electrodes
• Metals that are more reactive than carbon in reactivity series
• Zn, Fe, Sn, Fe, Pb
Heating of ores with carbon (coke)
in blast furnace
• Metals that are very less reactive
• Cu, Hg
Heating metal sulphide
in the air
• Metals that are non-reactive existed as natural element
minerals in the Earth’s crust
• Ag, Au
Do not need to be extracted but
purification to remove the impurities

20. Extraction of Metal by
Heating of Ores with Carbon

21. Extraction of Iron from Iron ores (haematite)
https://secondaryscience4all.wordpress.com/2014/07/21/iron-extraction-blast-furnace/

22. Impact and Importance of Mining Activities
Mudflows Water pollution Landslide
https://www.shutterstock.com/search/mudflow http://mizzima.com/article/two-killed-landslide-jade-mining-area
https://mozambiqueminingpost.com/2016/10/13/africa-mining-vs-environment-south-africa-has-failed-to-protect-locals-from-gold-mine-pollution-harvard-report/
Unplanned mining, mining in large quantities, deforestation &
chemical waste of mining impact to life.

23. Importance of Mining Activities
Create job opportunities Infrastructure
development
Development new settlements
such as metro cities
High-tech equipment raw materials Intensify R&D

24. CREDITS: This presentation template was created by Slidesgo,
including icons by Flaticon, infographics & images by Freepik
and illustrations by Stories
Thanks!
https://www.facebook.com/brilliantA.edu/
mybrilliant_a
011-1509 3232
PT3 & SPM Online Tuition