MKS@Chemistry Module Form 4 Complete Set

mohd faisol mansor/chemistry form 4/chapter 8

Table of Salts

Complete the table below.

Metal ion Sulphate salt Chloride salt Nitrate salt Carbonate salt

(SO42-) (Cl-) (NO3-) (CO32-)

K+ K2SO4 KCl KNO3 K2CO3

Na+

Ca2+

Mg2+

Al3+

Zn2+

Fe2+

Sn2+

Pb2+

Cu2+

Ag+

NH4+

Ba2+

Based on the table above, mark the insoluble salt.

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mohd faisol mansor/chemistry form 4/chapter 8

SOLUBLE & INSOLUBLE SALTS

SALT SOLUBLE INSOLUBLE

K+ , Na+ , NH4+ All soluble none

Nitrate salts All nitrate salts none
(NO3- )

Chloride salts All chloride salts Lead (II) chloride,
(Cl-) PbCl2
Silver chloride, AgCl
Mercury chloride,
HgCl

Sulphate salts All sulphate salts Lead (II) sulphate
(SO42-) Calcium sulphate
Barium sulphate

Carbonate Sodium carbonate, All others carbonate
salts (CO32-) Na2CO3 salts
Potassium carbonate,
K2CO3 All oxide salts
Ammonium carbonate,
(NH4)2CO3 All hydroxide salts

Oxide salts Sodium oxide, Na2O
(O2-) Potassium oxide, K2O
Calcium oxide, CaO

(slightly soluble)

Hydroxide salts Sodium hydroxide, NaOH
(OH-) Potassium hydroxide, KOH
Calcium hydroxide,
Ca(OH)2

(slightly soluble)

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mohd faisol mansor/chemistry form 4/chapter 8

Preparation and Purification of Soluble Salts

Soluble salt can be prepared by the following ways:

1. Reaction between acid and alkali - preparation for

sodium, potassium and ammonium salts only.

Eg: HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

[write the step of preparation of the salts on the diagram]

Burette Evaporating dish
HCl solution
NaCl solution

NaOH solution

NaCl crystal salt

NaCl salt crystal
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mohd faisol mansor/chemistry form 4/chapter 8

Preparation and Purification of Soluble Salts

Soluble salt can be prepared by the following ways:

1. Reaction between acid and metal oxide

Eg: HNO3(aq) + MgO(s) Mg(NO3)2 (aq) + H2O(l)

2. Reaction between acid and metal

Eg: H2SO4(aq) + Zn (s) ZnSO4(aq) + H2 (g)

3. Reaction between acid and metal carbonate

Eg: HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l)

[write the step of preparation of the salts on the diagram]

Copper(II) nitrate
Solution + excess

CuO

heat heat

Copper(II) nitrate Evaporating Dish
solution
152
Copper(II) nitrate solution
& crystal salt

Cu(NO3)2 crystal salt

mohd faisol mansor/chemistry form 4/chapter 8

Crystallization Physical characteristic of
crystals
is a process to crystallize
the soluble salts. Fixed geometrical shapes
such as a cuboids,
Recrystallization rhombic or prism

process will carried out in Flat surface, straight edges
order to get pure and and sharp angles.
more defined crystal

Same shapes for same
substance but differ in

sizes

Fixes angle between two
neighbouring surfaces.

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mohd faisol mansor/chemistry form 4/chapter 8

Preparation of insoluble salts
An insoluble salt is prepared through precipitation method.

Aqueous solution of two soluble salts are mixed to form
insoluble and soluble salt:

[write the general equation of preparation insoluble salt]

The reaction is called double decomposition.
Two solutions contain ions that make up the insoluble salts.
Eg: Preparation of lead(II) iodide salt by using lead(II)

nitrate solution and potassium iodide solution.

[write the balance chemical equation]

Double Decomposition

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mohd faisol mansor/chemistry form 4/chapter 8

Chemical and Ionic Equation
Chemical and ionic equation can be written for all reaction

That used to prepare salts.

Example: Formation of precipitate Barium Sulphate, BaSO4.

1. Chemical Equation:

BaCl2 (aq) + Na2SO4 (aq) BaSO4(s) + 2NaCl (aq)

2. Ionic Equation:

Ionic equation shows the ions take part in the reaction.

Exercise

1. Change each of the following word equations to a balanced
chemical equation.

a) Sulphuric acid + zinc zinc sulphate + hydrogen gas.

b) Silver nitrate + potassium iodide silver iodide + potassium
nitrate

c) Nitric acid + chromium(III) hydroxide chromium(III) nitrate
+ water

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mohd faisol mansor/chemistry form 4/chapter 8

2. Complete the following equations.
a) HCl (aq) + NiO (s)
b) HNO3 (aq) + Ca(OH)2 (aq)
c) H2SO4 (aq) + MgCO3 (s)

3. Write an ionic equation for each reaction between the following
pairs of substances.
a) Sulphuric acid, H2SO4 and barium hydroxide, Ba(OH)2 solution

b) Ammonium chloride, NH4Cl solution and silver nitrate, AgNO3
solution.

c) Lead(II) nitrate, Pb(NO3)2 solution and copper(II) sulphate,
CuSO4 solution.

d) Iron(III) oxide, Fe2O3 and hydrochloric acid, HCl.

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mohd faisol mansor/chemistry form 4/chapter 8

Constructing Ionic Equation using the Continuous Variation Method

12 34 56 78

Continuous variation method can be used to construct ionic
equation for the formation of insoluble salts.

Fixed volume of a reactant A is react with varying volumes
of a reactant B to determine the mole ratio of reactant A

that react completely with reactant B.

If x mol of reactant A with y mole of reactant B, than the
empirical formula for insoluble salt is A x B y.

Example: Fe2(CO3)3 (s)
2Fe3+ (aq) + 3CO32- (aq)

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mohd faisol mansor/chemistry form 4/chapter 8

158

mohd faisol mansor/chemistry form 4/chapter 8

Example
1. 6.0 cm3 of 0.2 mol dm-3 Xn+ solution reacts completely with 4.0

cm3 of 0.1 mol dm-3 Ym- solution to form a salt XmYn. Write the
ionic equation and hence determine the empirical formula of
the salt reaction.

2. 18.0 cm3 of 0.1 mol dm-3 solution of Px+ ions reacts completely
with 9.0 cm3 of 0.1 mol dm-3 solution of Qy- ions to form a salt
PyQx. Write the ionic equation and hence determine the
empirical formula of the salt in this reaction.

159

mohd faisol mansor/chemistry form 4/chapter 8

Solving Problem Involving Calculation of Quantities of Reactants or
Product in Stoichiometric Reactions

Since the quantities of chemicals involved in a reaction are in term
of moles, the quantities of chemicals (volume, mass and number of

particles) must be converted to moles in calculation regarding
quantities of reactant and products.

Exercise

1. Calculate the number of moles of aluminium sulphate

produced by the reaction of 0.2 mole of sulphuric acid with

excess aluminium oxide. [0.067 mol]

2. 2.0 g of sodium hydroxide reacts with excess sulphuric acid.

What is the mass of sodium sulphate produces

[RAM: H,1 ; O,16 ; Na,23 ; S,32] [ 3.55 g]

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mohd faisol mansor/chemistry form 4/chapter 8

3. What the volume of carbon dioxide gas evolved at s.t.p when

2.1 g of magnesium carbonate reacts with excess nitric acid.

[ RAM: C,12;O,16;Mg,24; s.t.p = 22.4 dm3] [ 560 cm3]

4. What is the mass of magnesium required to react with 20 cm3 of
2.0 mol dm3 hydrochloric acid to produce 120 cm3 of hydrogen
at temperature? [RAM: Mg,24 ; 1 mol = 24 dm3 at room temp.]
[ 0.12 g]

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mohd faisol mansor/chemistry form 4/chapter 8

Qualitative Analysis of Salts

General procedure of qualitative analysis

Observations on the physical Action of heat on salts Tests for cations and Confirmatory tests for
properties of salts anions cations and anions

Colour & Solubility of the Salt

GREEN PALE GREEN BROWN YELLOW/BROWN

 Iron(II) Sulphate, FeSO4 [depend on concentration]
 Iron(II) Nitrate, Fe(NO3)2
 Iron(II) Chloride, FeCl2  Iron(III) Sulphate, Fe2(SO4)3
 Iron(III) Nitrate, Fe(NO3)3
 Iron(III) Chloride, FeCl3

REDDISH-BROWN INSOLUBLE GREEN INSOLUBLE

 Iron(III) Oxide, Fe2O3  Copper(II) Carbonate, CuCO3

BLUE BLUE BLACK INSOLUBLE

 Copper(II) Sulphate, CuSO4  Copper(II) Oxide, CuO
 Copper(II) Nitrate, Cu(NO3)2
 Copper(II) Chloride, CuCl2

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mohd faisol mansor/chemistry form 4/chapter 8

Colour & Solubility of the Salt

WHITE COLOURLESS WHITE INSOLUBLE

 Potassium Oxide, K2O  Magnesium Oxide, MgO
 Sodium Oxide, Na2O  Aluminium Oxide, Al2O3
 Calcium Oxide, CaO

WHITE [cold] YELLOW [cold]

INSOLUBLE INSOLUBLE

YELLOW [hot] BROWN [hot]

 Zinc Oxide, ZnO  Lead(II) Oxide, PbO

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mohd faisol mansor/chemistry form 4/chapter 8

Gas test

Oxygen gas hydrogen gas

Wooden splinter

Oxygen gas, O2 Hydrogen gas, H2

Carbon dioxide gas sulphur dioxide gas

Carbon dioxide Sulphur dioxide

HCl acid HCl acid
Sodium Sulphite, Na2SO3
Sodium Carbonate,
Na2CO3 Glass rod dipped into ammonia gas
concentrated HCl acid
chlorine gas White fumes
Ammonia gas, NH3
Red litmus paper
164
Chlorine gas, Cl2

mohd faisol mansor/chemistry form 4/chapter 8

EFFECT OF HEAT ON SALTS

Carbonate salts

Sodium carbonate & potassium carbonate are very stable. They do
not decompose on heating.

Carbonate Salt Heating Metal Oxide + Carbon dioxide

Heating

Carbonate salts residue
[ white ] [ white ]

Salts Chemical Equation
1. Calcium carbonate
2. Magnesium carbonate
3. Aluminium carbonate

Heating

Carbonate salts residue
[ white ] [ yellow – hot ]
[ white – cold ]
Salts
1. Zinc carbonate Chemical Equation

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mohd faisol mansor/chemistry form 4/chapter 8

Carbonate Salt Heating Metal Oxide + Carbon dioxide

Heating

Carbonate salts residue
[ brown ] [ brown ]

Salts Chemical Equation
1. Iron(III) carbonate

Heating

Carbonate salts residue
[ green ] [ black ]

Salts Chemical Equation
1. Copper(II) carbonate

Heating

Carbonate salts residue
[ white ] [ brown – hot ]
[ yellow – cold ]
Salts
1. Lead(II) carbonate Chemical Equation

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mohd faisol mansor/chemistry form 4/chapter 8

Carbonate Salt Heating Metal + Carbon dioxide + Oxygen gas

Heating

Carbonate salts residue
[ white ] [ grey ]

Salts Chemical Equation
1. Mercury(II) carbonate

Heating

Carbonate salts residue
[ white ] [ shiny grey ]

Salts Chemical Equation
1. Silver carbonate

Heating residue
[ golden yellow ]
Carbonate salts
[ white ]

Salts Chemical Equation
1. Aurum(II) carbonate

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mohd faisol mansor/chemistry form 4/chapter 8

nitrate salts
Nitrate Salt Heating Metal Oxide + Oxygen gas + Nitrogen dioxide

Heating

nitrate salts residue
[ white ] [ white ]

Salts Chemical Equation
1. Calcium nitrate
2. Magnesium nitrate
3. Aluminium nitrate

Heating

nitrate salts residue
[ white ] [ yellow – hot ]
[ white – cold ]
Salts
1. Zinc nitrate Chemical Equation

168

mohd faisol mansor/chemistry form 4/chapter 8

Nitrate Salt Heating Metal Oxide + Oxygen gas + Nitrogen dioxide

Heating

nitrate salts residue
[ brown ] [ brown ]

Salts Chemical Equation
1. Iron(III) nitrate

Heating

nitrate salts residue
[ blue ] [ black ]

Salts Chemical Equation
1. Copper(II) nitrate

Heating

nitrate salts residue
[ white ] [ brown – hot ]
[ yellow – cold ]
Salts
1. Lead(II) nitrate Chemical Equation

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mohd faisol mansor/chemistry form 4/chapter 8

Nitrate Salt Heating Metal + Nitrogen dioxide + Oxygen gas

Heating

nitrate salts residue
[ white ] [ grey ]

Salts Chemical Equation
1. Mercury(II) nitrate

Heating

nitrate salts residue
[ white ] [ shiny grey ]

Salts Chemical Equation
1. Silver nitrate

Nitrate Salt Heating Metal nitrite + Oxygen gas

Heating

nitrate salts residue
[ white ] [ white ]

Salts Chemical Equation
1. Potassium nitrate
2. Sodium nitrate 170

mohd faisol mansor/chemistry form 4/chapter 8

TEST FOR ANIONS

Unknown aqueous salt solution Salt needed to be
dissolved into water

first to produce
aqueous salt
solution.

[ state the procedure ] [ state the procedure ] [ state the procedure ] [ state the procedure ]

OBSERVATION OBSERVATION OBSERVATION OBSERVATION

[ label the diagram ] [ label the diagram ] [ label the diagram ] [ label the diagram ]

Ionic Equation Ionic Equation Ionic Equation Ionic Equation

CONCLUSION CONCLUSION CONCLUSION CONCLUSION

[ state the anion ] [ state the anion ] [ state the anion ] [ state the anion ]
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mohd faisol mansor/chemistry form 4/chapter 8

TEST FOR CATIONS

Unknown aqueous salt solution Salt needed to be
Add NaOH drop by drop dissolved into water
(soluble salts) or in

dilute acid then
filtered (insoluble
salts) first to produce
aqueous salt solution.

No precipitate White precipitate Coloured precipitate
Green

Dissolve in excess NaOH Add NaOH drop by drop until excess Brown
Insoluble in excess NaOH Blue

* All coloured ions insoluble in excess NaOH

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mohd faisol mansor/chemistry form 4/chapter 8

TEST FOR CATIONS

Unknown aqueous salt solution Salt needed to be
Add NH3 drop by drop dissolved into water
(soluble salts) or in

dilute acid then
filtered (insoluble
salts) first to produce
aqueous salt solution.

No precipitate White precipitate Coloured precipitate
Green

Dissolve in excess NH3 Add NH3 drop by drop until excess Brown
Insoluble in excess NH3 Blue

Dissolved in excess NH3

Dark blue solution
* Fe2+ & Fe3+ ions insoluble in excess NH3

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mohd faisol mansor/chemistry form 4/chapter 8

Confirmatory Test for Cation

Cation Procedure Observation
Fe 2+

Fe 3+

Pb 2+

NH4 +

Exercise

1. Identify the aqueous solutions based on the test and observation given.

Type Observation Answer

a. Potassium thiocyanate, Blood red solution formed.
KSCN, solution is added.

b. Potassium iodide, KI, solution Yellow precipitate is

is added. formed.

c. Ammonia solution, NH3, is Blue precipitate dissolve to

added until excess. form dark blue solution.

d. A little hydrochloric acid is Effervescene occur and

added. lime water turn into chalky.

e. A sulphuric acid, iron(II)

sulphate solution and Brown ring formed.
concentrated sulphuric acid

is added.

f. Ammonia solution is added White precipitate

until excess. dissolved.

K2CO3 ZnCl2 PbCl2 CuSO4 NaNO3 FeCl3

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mohd faisol mansor/chemistry form 4/chapter 9

CHAPTER 9

MANUFACTURED SUBSTANCES IN INDUSTRY

SULPHURIC ACID

The Uses of
Sulphuric Acid

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mohd faisol mansor/chemistry form 4/chapter 9

[ Cause by ]

[ Effect ] POLLUTION of [ Cause by ]
Sulphur DIOXIDE
Formation of Acid Rain

Burning of Sulphur

[ Explain the formation of acid rain & write the chemical equation ]

Burning of Sulphur Dioxide

[ Explain the formation of acid rain & write the chemical equation ]

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mohd faisol mansor/chemistry form 4/chapter 9

Effect of Acid Rain

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mohd faisol mansor/chemistry form 4/chapter 9

Industrial Process in the Manufacture of Sulphuric Acid

Contact Process

Burn in Stage 1
the air
[ write the chemical equation ]

Catalyst: Stage 2

Temp. : [ write the chemical equation ]
Pressure:

Dissolves in Stage 3 ( i )
concentrated H2SO4
[ write the chemical equation ]

Dilute with water Stage 3 ( ii )

[ write the chemical equation ]

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mohd faisol mansor/chemistry form 4/chapter 9

AMMONIA

[ Label the uses of ammonia ]

The Uses of
ammonia

179

mohd faisol mansor/chemistry form 4/chapter 9

Properties of
ammonia

Glass rod dipped into
concentrated HCl acid

White fumes
Ammonia gas, NH3

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mohd faisol mansor/chemistry form 4/chapter 9

Industrial Process in the Manufacture of Ammonia

Haber Process

1 part 3 parts

Catalyst chamber

Catalyst :
Temperature :

Pressure :

The unreacted [ Write the balance chemical equation ]
mixture will flowed
Condenser
back

[ state what happen in the condenser ]

[ state the final product ]

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mohd faisol mansor/chemistry form 4/chapter 9

Preparation of Ammonium Fertilisers in the laboratory

Ammonia fertilizers can be prepared by using neutralization reaction between acid and
ammonia solution.

Acid + Ammonia Ammonium salts H2SO4 + NH3 (NH4)2SO4

Eg: Preparation of ammonium sulphate salt

Burette Evaporating dish
H2SO4 acid solution
(NH4)2SO4 solution

Ammonia solution

(NH4)2SO4 crystal salt

(NH4)2SO4 crystal salt

182

mohd faisol mansor/chemistry form 4/chapter 9

Alloys

Pure metal is soft and not strong.
Atom of pure metal have similar shape and size.
The particles in pure metal are arranged layer by layer and

easily slide along between each other.

Physical
Properties
Of pure metal

Ductile

[ state the definition of the ductile and draw the particle arrangement ] malleable
[ state the definition of the malleable and draw the particle arrangement ]
183

mohd faisol mansor/chemistry form 4/chapter 9

alloys [ draw the particle arrangement of alloy ]

Alloy is a mixture of two or more elements
which is the major component is pure
metals.

Foreign elements either metal or
non-metal is added into pure metal.

The size of foreign elements either
smaller or bigger.

It will disrupt the orderly arrangement of
pure metal. Thus, the properties of pure
metals improved.

Aim of making
alloys

184

STEEL mohd faisol mansor/chemistry form 4/chapter 9

Uses of Alloys & Their Compositions
[ state the components, properties & uses of alloy ]
COPPER-NICKEL
DURALUMIN

Pure metal : 99% Iron BRASS
Foreign element : 1% Carbon

- Strong
- Hard
- Withstands corrosion

- To make bridge, vehicles,
building & train tracks

STAINLESS STEEL PEWTER
BRONZE

185

mohd faisol mansor/chemistry form 4/chapter 9

Synthetic Polymers

Polymers are long chains of molecules made from combination of monomers by
polymerisation process.

Two types of polymer:
i) Natural polymer
ii) Synthetic polymer

Polymer that occurs naturally made by living organisms.

Polymer Natural Polymer
RUBBER polymers CELLULOSE
Monomer Monomer

Polymer Polymer
PROTEIN FAT
Monomer Monomer

Polymer
STARCH
Monomer

Amino acid

Isoprene

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mohd faisol mansor/chemistry form 4/chapter 9

Polymer that are man-made polymer produced from
chemical compound through polymerisation.

Two types of polymerisation: Synthetic Polymer
i) Addition polymerisation polymers POLYPROPENE
ii) Condensation polymerisation Monomer

Polymer
POLYTHENE
Monomer

Polymer Polymer
NYLON POLYVINYL CHLORIDE (PVC)
Monomer Monomer

Polymer
PERSPEX
Monomer

187

mohd faisol mansor/chemistry form 4/chapter 9

Glass & ceramics

Main component of glass is silica & silicon dioxide, SiO2.

glass

Main
characteristics

188

mohd faisol mansor/chemistry form 4/chapter 9

Type of Glass

FUSED SILICA GLASS SODA-LIME GLASS
Method of Productions Method of Productions

Compositions Compositions

Properties Properties

- Very high melting point - Transparent
- Not easy to change its shape - Low melting point
- Does not easily expand or shrink - Easily shaped
- Easily broken
with changes of temperature - Cannot withstand heat & chemical
- Transparent to ultraviolet ray reaction

Uses Uses

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mohd faisol mansor/chemistry form 4/chapter 9

Type of Glass

BOROSILICATE GLASS LEAD CRYSTAL GLASS
Method of Productions Method of Productions

Compositions Compositions

Properties Properties

- Withstand heat & chemical reaction - Very transparent
- High melting point - Shiny
- Transparent to light & infrared ray - High density

but not to ultraviolet ray Uses

- Expand & shrink a little when

temperature changes

Uses

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mohd faisol mansor/chemistry form 4/chapter 9

Made from clay at very high temperature and the main
component is silicate.

ceramics

Common
properties

191

mohd faisol mansor/chemistry form 4/chapter 9

Uses of
ceramics

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mohd faisol mansor/chemistry form 4/chapter 9

Composite Materials

Produced from the combination of two or more different
compound such as alloys, metals, glass, ceramic & polymers.

USES OF COMPOSITE MATERIALS

REINFORCED CONCRETE SUPERCONDUCTOR
Compositions Compositions

Properties Properties
Uses Uses

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mohd faisol mansor/chemistry form 4/chapter 9

USES OF COMPOSITE MATERIALS

FIBRE GLASS FIBRE OPTICS
Compositions Compositions

Properties Properties
Uses Uses

“Success is not the key to happiness. Happiness is the key to success. 194
If you love what you are doing, you will be successful.”
- Albert Schweitzer -

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mohd faisol mansor/chemistry form 4/chapter 9

USES OF COMPOSITE MATERIALS

PHOTOCHROMIC GLASS CERAMIC GLASS
Compositions Compositions

Properties Properties
Uses Uses

“ There are no secrets to success. It is the result of
preparation, hard work, and learning from failure.”

- Colin Powell -

195