land and its resources bab 1
TRANSCRIPT
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Chapter 6
LAND AND ITSRESOURCES
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Minerals in the Earth’s Crust
1. Minerals are solid elements or chemical
compounds that are naturally present in
the Earth crust.
2. Examples of mineral are gold, quartz
(silicon dioxide), silver, limestone
(calcium carbonate) and tin ore.
3. Minerals exist in the form of element or
compound.
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Gold quartz
limestone
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4. Gold, silver,platinum and mercury are
examples of natural elements, which
means that they are found uncombinedwith another element.
5. Carbon and sulphur are two types of
non-metal mineral element that existnaturally.
6. Most minerals in the Earth crust exist in
the form of compounds especially oxide,carbonate, sulphide and silicate.
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Identifying the elements in natural
compounds
1. Minerals in the form of compounds
consist of combinations of a few types of
different element.
2. Minerals that are found as compounds
are made up of metallic elements
combined with non-metallic elements.
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Elements present in minerals that are found as
natural compounds
Naturalcompound
Mineral Elements
Oxide Haematite Iron, oxygen
Cassiterite Tin, oxygen
Calcite Calcium, carbon, oxygen
Carbonate Malachite Copper, carbon, oxygen
Iron pyrite Iron, sulphur
Sulphide Galena Lead, sulphur
Silicate China clay Aluminium, silicon, oxygen
Calcium
silicate
Calcium, silicon, oxygen
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Properties of minerals
Most minerals are still in existence and have not
changed in the Earth crust because minerals aregenerally hard and do not dissolve in water.
A. Hardness of minerals
i). We can determine a mineral’shardness by rubbing the mineralagainst objects such as nails, coins or a fingernail.
ii). Soft minerals are scratched easily.iii). Diamond is an example of the hardest
mineral.
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B. Solubility of minerals
i). Most of the minerals that exist in
the Earth’s crust as naturalcompounds are hard and do notdissolve in water.
C. Effect of heat on minerals
i). Mineral like metal oxide andsilicate normally do not
decompose when heated.ii). Some mineral like metal
carbonates and sulphides can be
easily decompose when heated.
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Effect of heat on metal carbonate
1. Metal carbonate change to their oxides and carbon
dioxide when burnt in air. The carbon dioxide gascauses limewater to turn cloudy.
heat
Metal carbonate metal oxide + carbon dioxide
Eg: heat
Zinc carbonate zinc oxide + carbon dioxide
Carbon dioxide that is released can be tested by using lime
water.
Lime water will turn cloudy in the presence of carbon dioxide.
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Effect of heat on metal sulphide
1. When heated, a metal sulphide breaks
down into a metal oxide and releasessulphur dioxide gas.
2. This gas changes the potassium
manganate (VII) solution from purple tocolourless.
heat
Metal sulphide + oxygen metal oxide + sulphur dioxideEg: heat
Iron sulphide + oxygen iron oxide + sulphur dioxide
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3. Sulphur dioxide is an acidic gas that can betested with
i). Acidic potassium manganate (VII) solution. This gas bleaches thepurple colour of the solution tocolourless.
ii). Acidic potassium dichromate(VI)solution. This gas changes the orange
–coloured solution to green.
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Arrangement of apparatus to study
characteristics of minerals
6 2 R ti B t M t l d N
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6.2 Reactions Between Metals and Non-
metals1. The two main groups of elements are metals and non-metals.
Example of metals : potassium, sodium, calcium, magnesium,aluminium,zinc, iron, lead,copper, gold, silver,mercury
Example of non-metal :
solid -sulphur, carbon
liquid -bromine
gaseous -oxygen,hydrogen,nitrogen,helium,chlorine
2. Most metals react with non-metals to form compounds.
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Reaction between metal with
oxygen and sulphur
1. Metals have shiny surfaces, and becomes dull
after some time. This happens because most
metal react with oxygen.
2. Metal react with oxygen and sulphur atdifferent rates.
3. The very reactive metals react with oxygen
and sulphur vigorously.(eg: Sodium and
potassium)
metal + oxygen metal oxide
metal + sulphur metal sulphide
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The reaction of metals with
oxygen
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The reaction of metals with sulphur
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6.3 Silicon Compounds
1. Silicon is the second most abundant elementin the Earth’s crust.
2. Silicon usually combines with other elementlike metal and oxygen to form a silicon
compounds.
3. Silica is silicon dioxide consisting of silicon andoxygen.(eg: sand and quartz)
4. Silicates are silicon compounds that are madeup of silicon,metal and oxygen.(eg: asbestos,mica, talc, clay)
Th ti f ili
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The properties of silicon
compounds
• Silica and silicate are stable compounds.
1. do not dissolve in water 2. do not react with acids
3. do not break down when
heated
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Uses of silicon compounds in daily
life
Sand - to make bricks, mortar,glasswareQuartz - is mixed with cement to make
concrete
Asbestos - as heat insulator in the form of sheet.
Pure silicon is used to make electronic chips.
Fibres made from silicon compounds are called optic
fibres.
Optic fibre are used- to replace copper wire tosend information, likesound data,video,etc.
- to observe internal organs
(in medical field)
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Uses of silicon compounds in daily life
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6.4 Calcium Compounds
1. Calcium is a reactive metal. Therefore it does
not exist in its pure form in nature.2. Calcium carbonate is an important calcium
compound.
3. Calcium carbonate is a compound of calcium,
oxygen and carbon.4. Limestone and marble are example of natural
calcium compounds.
5. Seashells, eggshells,bones are largely calcium
carbonate.6. The stalagmites and stalactites built up in
caves are eg.of calcium carbonate too.
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Stalactites and stalagmites
The properties of calcium
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The properties of calciumcarbonate
1. Calcium carbonate compound does not dissolves inwater.
2. Calcium carbonate react with acid to form salt, water and releases carbon dioxide.
Calcium carbonate + hydrocloric acid calcium chloride + carbon dioxide + water
3. Calcium carbonate decomposes to produce calciumoxide and release carbon dioxide when heated over a strong heat.
heated
Calcium carbonate calcium oxide + carbon dioxide
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4. Calcium oxide (quicklime) reacts with water to formsolid calcium hydroxide (slaked lime). A lot of heat is
released.
Calcium oxide + water calcium hydroxide + heat
5. Calcium hydroxide is an alkali. It dissolves in water
to become lime water which is used to test for the
presence of carbon dioxide gas.
Calcium hydroxide + carbon calcium carbonate + water
solution dioxide
F i f l i id d l i
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Formation of calcium oxide and calcium
hydroxide
6 5 N t l F l R d Th i
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6.5 Natural Fuel Resources and Their
Importance
1. Natural fuel resources found in the Earth crustinclude
a). petroleum b). coal
c). natural gas
2. Fuels are substances that burn to produceheat as a form of energy.
3. These fuel consist mainly of hydrocarbon,which are compounds made up of hydrogenand carbon.
4. Petroleum, coal and natural gas are calledfossil fuels because they are formed fromthe remains of living plants and animals thatlived millions of years ago.
F i f l d l
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Formation of natural gas and petroleum
1. Petroleum(crude oil) and natural gas areformed from the remains of tiny sea creatures
which were buried in sediments at the bottomof the ocean.
2. Sediments of these organisms changed intopetroleum after being subjected to hightemperature and pressure for a long period of time.
3. These remains were changed into a dark,sticky liquid called petroleum.
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4. Some may change into gas,
called natural gas.
5. Petroleum and natural gas are
found together, held in between
layers of non-porous rocks.
6. Crude petroleum contains many
types of hydrocarbons mixed
together.
7. Petroleum must be separated
into fractions before it can be
used by a process called fraction
distillation.
Petroleum and natural gas are
held in between layers of non-
porous rocks.
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The formation of coal
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The formation of coal
1. Millions of years ago, most of the land on Earth
was covered with dense forests and swamps.2. Coal is formed from the plants die, and have
been compressed by layers of earth on top of
it.
• High pressure and temperature that act on
these plants change them into coal.
4. People use coal for generating electricity,
cooking, lighting and running motors andtrains.
Fractional distillation
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Fractional distillation
1. In the oil and gas industry, fractional distillation
is carried out by heating unprocessedpetroleum in a furnace at 400°C in an oilrefinery.
2. In the furnace, the petroleum is heated until it isturned into vapour.
3. The vapour is then pump into a hugefractionating column and its begin to cool down
and changes into liquid.
4. Each and every petroleum fraction has its owncharacteristics and uses.
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5. The characteristics of the fraction or distillate is
related to its boiling point.
6. The higher the boiling point of a petroleumfraction:
a). the darker to its colour b). the higher is its viscosity
c). the more difficult it is to burn
d). the more soot its flames produce
7. All petroleum fractions do not dissolve inwater.
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Fractional distillation
cooking oil
Fuel for vehicles
For making plastic
Fuel for aircraft
For heavy vehicles
Lubricants for machines
Fuel oil for ships
As building material (tar) for road
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The contributions of the petroleum and the natural gas
industry to the economic development of Malaysia
1. The discovery of offshore oilfields in Sabah,Sarawak and Terengganu has madeMalaysia a net producer of petroleum.
2. Malaysia’s crude oil is of high quality, lightand low in sulphur content.
3. The petroleum industry provides the countrywith income in terms of taxes, royalties anddividends, and also provides us with a high
living standard and more job opportunities.
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The efficient ways of using natural
fuela). Fossil fuels are non-renewableresources.
b). They cannot be replaced and will not lastforever.
c). Therefore, we have to use them efficiently,such as by practising car pool, using publictransport and not wasting electricity.
d). Besides, we should practise the 3Rs whichmeans reduce, reuse and recycle petroleum products.