Revisi Cepat SPM Chemistry Form 4 & 5

Penerbit Ilmu Bakti Sdn. Bhd
Coloured Graphical Notes

Chemistry

FORM

Suharfizza Senawi
Amimah Ayub (Guru Cemerlang)
Reena Sethu (Guru Cemerlang)

Penerbit Ilmu Bakti Sdn. BhdForm 4 Safety goggles Form 4
To prevent dust or
Chapter 1 Introduction to Chemistry splashes of chemicals
from getting into the eyes.
Personal protective equipments
Laboratory coat
Face mask To protect the body and
To protect the respiratory clothes from chemical
organs from chemicals in the spills.
form of powder or fumes.

Gloves
To protect the hands from
injuries, chemicals or
infections while handling
chemicals.

Laboratory shoes
To protect the feet from
injuries caused by chemical
spills, sharp objects or toxic
substances.

Safety equipment in the laboratory

Fume chamber Shower
To carry out experiments that release toxic vapours, To clean the
cause combustions or produce pungent smells. body when
accidents occur
on the body
parts.

Fire extinguisher Hand wash Eyewash
To extinguish fire To remove chemical substances, To clean the eyes
in the laboratory. oil, dirt and microorganisms when exposed to
from the hands. chemicals.

N1

Chapter 2 Matter and the Atomic Structure
The particle theory of matter

Matter

Element Compound
Penerbit Ilm Form 4
u Bakti Sdn. BhdSubstance that consists of only oneSubstance that consists of two or more
type of atom. different elements that are chemically
bonded together.
Atom Molecule

The smallest A neutral particle Molecule Ion
particle of an consists of two
element. or more similar A neutral particle Positively and
atoms which consists of two negatively charged
are chemically or more different particles which are
bonded together. atoms which chemically bonded
are chemically together by ionic
E.g.: Magnesium E.g.: Hydrogen gas bonded together. bond.
metal
E.g.: Nitrogen E.g.: Sodium
dioxide gas chloride

Mg Mg Mg Mg HH HH CI Na CI Na
Mg Mg Mg Mg Na CI Na CI
HH ONO CI Na CI Na
ONO

Subatomic particles

Electron Proton

Symbol e - Symbol p
-
Relative –1 Relative +1
charge + charge
+ ++
Relative 1 Relative 1
mass 1 840 -
- mass
- Neutron

Symbol n

Relative 0
charge

Nucleus - Relative 1
mass
Shell

N2

Contents

Graphical Notes N1 – N32 4.6 Elements in Period 3 51

4.7 Transition Elements 55
Penerbit Ilmu Bakti Sdn. Bhd
FORM 4 Summative Practice 4 58

Theme 1: The Importance of Chemistry Chapter Chemical Bond 60

Chapter Introduction to Chemistry 1 5

1 5.1 Basics of Compound Formation 60

1.1 Development in Chemistry Field 5.2 Ionic Bond 62

and Its Importance in Daily Life 1 5.3 Covalent Bond 66
1.2 Scientific Investigation in
5.4 Hydrogen Bond 69
Chemistry 2
1.3 Usage, Management and 5.5 Dative Bond 72

Handling of Apparatus and 5.6 Metallic Bond 73

Materials 4 5.7 Properties of Ionic Compounds
Summative Practice 1 7
and Covalent Compounds 74

Summative Practice 5 82

Theme 2: Fundamentals of Chemistry Theme 3: Interaction between Matter
Chapter Matter and the Atomic
Chapter Acid, Base and Salt 84
2 Structure 8
6

2.1 Basic Concepts of Matter 8 6.1 The Role of Water in Showing

2.2 Development of the Atomic Model 13 Acidic and Alkaline Properties 84

2.3 Atomic Structure 14 6.2 pH Value 88

2.4 Isotopes and their Uses 16 6.3 Strength of Acids and Alkalis 90

Summative Practice 2 19 6.4 Chemical Properties of Acids and

Alkalis 92

Chapter The Mole Concept, Chemical 6.5 Concentration of Aqueous

3 Formula and Equation 21 Solution 95

6.6 Standard Solution 101

3.1 Relative Atomic Mass and 6.7 Neutralisation 104

Relative Molecular Mass 21 6.8 Salts, Crystals and their Uses in

3.2 Mole Concept 23 Daily Life 107

3.3 Chemical Formula 27 6.9 Preparation of Salts 109

3.4 Chemical Equation 33 6.10 Effect of Heat on Salts 117

Summative Practice 3 36 6.11 Qualitative Analysis 123

Summative Practice 6 129

Chapter The Periodic Table of 7Chapter Rate of Reaction 132

4 Elements 38

4.1 Development of the Periodic 38 7.1 Determining Rate of Reaction 132

Table of Elements 39 7.2 Factors Affecting Rate of
4.2 Arrangement in the Periodic 40
42 Reactions 138
Table of Elements 48
4.3 Elements in Group 18 7.3 Application of Factors that Affect
4.4 Elements in Group 1
4.5 Elements in Group 17 the Rate of Reaction in Daily Life 145

7.4 Collision Theory 147

Summative Practice 7 151

Theme 4: Industrial Chemistry Theme 3: Heat

Chapter Manufactured Substances 3Chapter Thermochemistry 248
8 in Industry 154

8.1 Alloy and Its Importance 154 3.1 Heat Change in Reactions 248

8.2 Composition of Glass and Its 3.2 Heat of Reaction 251

Uses 158 3.3 Application of Exothermic and

8.3 Composition of Ceramic and Its Endothermic Reactions in Daily

Life 269
Penerbit Ilmu Bakti Sdn. BhdUses 160
Summative Practice 3 271
8.4 Composite Materials and their

Importance 162 Theme 4: Technology in Chemistry

Summative Practice 8 164

4Chapter Polymer 273

FORM 5 4.1 Polymer 273

Theme 1: Chemical Process 4.2 Natural Rubber 279

1Chapter Redox Equilibrium 166 4.3 Synthetic Rubber 287

Summative Practice 4 289

1.1 Oxidation and Reduction 166

1.2 Standard Electrode Potential 181 5Chapter Consumer and Industrial
Chemistry 290
1.3 Voltaic Cell 184

1.4 Electrolytic Cell 190

1.5 Extraction of Metal from Its 5.1 Oils and Fats 290

Ore 205 5.2 Cleaning Agents 292

1.6 Rusting 209 5.3 Food Additives 299

Summative Practice 1 213 5.4 Medicines and Cosmetics 301

5.5 Application of Nanotechnology

Theme 2: Organic Chemistry in Industry 306

Chapter Carbon Compound 216 5.6 Application of Green

2 Technology in Industrial Waste

2.1 Types of Carbon Compounds 216 Management 309

2.2 Homologous Series 218 Summative Practice 5 311

2.3 Chemical Properties and SPM Model Test 313

Interconversion between

Homologous Series 226

2.4 Isomers and Naming according Answers 330

to IUPAC Nomenclature 241

Summative Practice 2 246

1Chapter Theme 1: The Importance of Chemistry

Introduction to Chemistry

Penerbit Ilmu Bakti Sdn. Bhd1.1Development in Chemistry Field and Its Importance in CHAPTER 1 FORM 4
Daily Life

  1 Chemistry is the study of the composition of substances, basic form of matter
and interaction between matter.

  2 Chemical subtances are very important in our lives. Diagram 1.1 shows some
examples of chemicals found in daily life.

Circle Map

Internet Textbook

MEDICINE
• Antibiotics
• Antiseptics
• Vitamins
• Chemotherapy
• Analgesics

AGRICULTURE Examples of FOOD
• Herbicides chemicals in • Preservatives
• Pesticides • Colourings
• Fungicides daily life • Flavourings
• Fertilisers • Antioxidants
• Hormones INDUSTRIES • Stabilisers
• Paints
• Polymers
• Glass and ceramics
• Detergents
• Alloys

Reference book Library

Diagram 1.1 Examples of chemicals in daily life

1

 3 Some careers related to chemistry QUICK CHECK 1.1
are as follows:
(a) Chemist 1 What is chemistry?
(b) Pharmacologist 2 Give two examples of chemicals in
(c) Pharmacist
(d) Chemical engineer the following fields.
(e) Forensic scientist
(f) Toxicologist Field Chemicals
(g) Geochemist
(h) Chemistry teacher Medicine
Bakti Sdn. Bhd
CHAPTER 1 FORM 4 Food

Agriculture

Industry

3 List out five careers related to
chemistry.

1.2 Scientific Investigation
in Chemistry

Diagram 1.2 Chemistry-related careers   1 The scientific method is a systematic
approach used by scientists to

investigate phenomena.
 2 Steps in the scientific method are

as shown in Diagram 1.3.

Making an uMaking an Flow Map
observation inference Identifying the
Penerbit Ilm
problem

Making a Identifying Controlling
hypothesis variables variables

Planning an Collecting Interpreting
experiment data data

Making a Writing a
conclusion report

Diagram 1.3 Steps in the scientific method

Keywords • Variables – Pemboleh ubah
• Scientific method – Kaedah saintifik

2

Activity 3.2

Aim: by bubbling it into the water before
To determine the empirical formula of starting the heating process.
copper(II) oxide 10 Copper(II) oxide powder is heated with
a spirit lamp while the hydrogen gas is
CHAPTER 3 FORM 4 Apparatus: Bakti Sdn. Bhdstill continuously flowing.
Boiling tube, rubber stopper, rubber tube, 11 The heating process is stopped when
12 cm glass tube, 10 cm glass tube, spirit the black copper(II) oxide powder
lamp, retort stand and clamp, wooden block, turned completely brown.
electronic balance, spatula 12 The hydrogen gas is allowed to keep
flowing until the glass tube cools to
Materials: room temperature.
Water, copper(II) oxide powder, zinc 13 The glass tube that contains the brown
granules, 1.0 mol dm–3 hydrochloric acid, powder is removed. The water droplets
wooden splinter, cotton bud at the end of the glass tube is wiped off
using a cotton bud.
Procedure: 14 The glass tube with its content is
weighed and the mass is recorded.
12 cm Copper(II) 15 The heating, cooling and weighing
Rubber glass tube oxide powder process are repeated until a constant
tube mass is obtained.
Air hole Spirit 10 cm 16 The results are recorded in a table.
lamp glass tube
Dynamic Info
12 cm 1.0 mol dm–3
glass hydrochloric
tube acid
Zinc
Water granules This method can be used to determine
the empirical formula of other non-
Wooden block reactive metal oxides such as oxides of
tin and lead.
  1 A 12 cm glass tube is weighed using
the electronic balance and the mass is
recorded.
  2 Copper(II) oxide powder is filled into the
u Results:
glass tube. A wooden splinter is used to
Penerbit Ilm push the copper(II) oxide powder to the Description
middle section of the glass tube. Glass tube Mass (g)
  3 The mass of the glass tube with its content Glass tube + copper(II) oxide x
is weighed and the mass is recorded. Glass tube + copper y
  4 A boiling tube is filled with water until z
2
3 full.

  5 The boiling tube is closed with a rubber Calculation:
stopper that is connected to another
12 cm glass tube. The boiling tube is Element Cu O
clamped to a retort stand. Mass (g) z–x y–z
  6 Some zinc granules is placed into Number of z–x y–z
another boiling tube. Then, 1.0 mol moles (mol) 64 16
dm–3 hydrochloric acid is added into Mole ratio
1 a b
the boiling tube until 3 full.
Discussion:
  7 The boiling tube is closed with a rubber   1 The black colour of copper(II) oxide turns
stopper that is connected to a 10 cm
glass tube. The boiling tube is clamped brown indicating that the copper(II)
to another retort stand. oxide has changed to copper.
  8 The glass tube that contains copper(II)   2 The following precautionary steps are
oxide powder is connected to the taken in this activity:
boiling tubes. (a) Dry hydrogen gas is passed
  9 Hydrogen gas is flowed for 10 seconds
through the combustion tube for

32

10 seconds to remove all air in the (c) The process of heating, cooling
combustion tube. The mixture of and weighing is repeated until a
hydrogen and oxygen can cause constant mass is obtained to ensure
an explosion when lighted. all copper(II) oxide has changed to
(b) The flow of hydrogen gas must copper.
be continuous throughout the
experiment to prevent hot copper Conclusion:
from reacting with oxygen to form The empirical formula of copper oxide is
copper(II) oxide again. CuaOb.
Penerbit Ilmu Bakti Sdn. Bhd
QUICK CHECK 3.3 The following information can be CHAPTER 3 FORM 4

obtained from the equation:

[RAM: H = 1, C = 12, O = 16, S = 32, Zn = 65] (a) The reactants are sodium, Na

HOTS Evaluating (b) and oxygen gas, sOo2d. ium oxide,
The product is
1 A compound consists of 9.75 g of
zinc, 4.8 g of sulphur and 9.6 g of (c) NFoau2Or m. ol of Na react with one
oxygen. Find the empirical formula
of the compound.
2 Hydrocarbon X contains 2.64 g of ompfhoNylsaoic2fOaOl.s2ttaoteporof deaucche two mol
carbon and 0.44 g of hydrogen. The reactant
relative molecular mass of hydrocarbon   5 The
X is 98. Determine the empirical
and product is written as follows:

formula and molecular formula. (a) (s) for solid

3 The empirical formula of pentanoic (b) (l) for liquid

amcaidssisiCs 31H16O6,. If the relative molecular (c) (aq) for aqueous solution
what is the molecular
(d) (g) for gas

formula of pentanoic acid? Dynamic Info

3.4 Chemical Equation Some symbols commonly used in
chemical equations:
  1 Chemical equation is an equation • → = produces
written using symbols and chemical • = reversible reaction
formulae. • ↑ = gas is produced
• ↓ = precipitate is formed
  2 A chemical reaction can be • Δ = heating
represented by a chemical equation.
 6 Diagram 3.3 shows the steps in
  3 The following basic information can writing a chemical equation.
be obtained from a chemical equation:
(a) Thereactantsthatwereinvolved Flow Map
(b) The products that are produced
(c) The number of moles of Write the Determine Balance the
reactants and products correct the number of
(d) The physical state of each of chemical atoms for each
the chemical substances formula number element by
for each of atoms adjusting the
  4 For example, sodium reacts with reactant for each coefficients
oxygen gas to form sodium oxide. element. in front of
The chemical equation for the and the chemical
reaction is as follows: product. formulae.
4Na(s) + O2(g) → 2Na2O(s)
Diagram 3.3 Steps to write a chemical equation

33

 7 The chemical equation can be (b) Explain the equation
interpreted qualitatively and qualitatively:
quantitatively. For example:
Solid sodium reacts with
2Na(s) + 2H2O(2l)N→aOH(aq) + H2(g) liquid water to form aqueous
sodium hydroxide solution
(a) Explain the equation and hydrogen gas.
quantitatively:
 8 The quantity of reactants and
2 mol of Na reacts with 2 mol products can be calculated using
oanf dH12OmtoolfoofrmH22. mol of NaOH stoichiometric from the given
numerical information.
CHAPTER 3 FORM 4 Bakti Sdn. Bhd
EXAMPLE

  1 The equation below shows the reaction between magnesium and sulphuric acid.

Mg(s) + H2SO4(aq) → MgSO4(aq) + H2(g)
Calculate the volume of hydrogen gas at STP when 12.0 g of magnesium reacts with

excess sulphuric acid.
[RAM: Mg = 24; 1 mole of gas occupies 22.4 dm3 at STP]

Number of moles of Mg = 12 = 0.5 mol
24

From the equation, 1 mol of Mg produces 1 mol of H2.
0.5 × 1
Therefore, 0.5 mol of Mg produces 1 = 0.5 mol of H2.

Volume of H2 at STP = 0.5 × 22.4 = 11.2 dm3

  2 An experiment is conducted to investigate the reaction between magnesium
and hydrochloric acid. 800 cm3 of hydrogen gas is collected in a syringe at room
u
conditions. Calculate the maximum mass of magnesium needed to produce
Penerbit Ilm hydrogen gas in the syringe.
[RAM: Mg = 24; 1 mole of gas occupies 24.0 dm3 at room conditions]
The chemical equation is Mg + 2HCl → MgCl2 + H2
0.8
Number of moles of H2 = 24 = 0.033 mol

From the equation, 1 mol of Mg produces 1 mol of H2.
0.033 × 1
Therefore, 1 = 0.033 mol of Mg produces 0.033 mol of H2.

Mass of Mg = 0.033 × 24 = 0.8 g

  3 The following chemical equation shows the reaction between iron and bromine.

2Fe(s) + 3Br2(g) → 2FeBr3(s)

2.8 g of iron burns completely in bromine. What is the mass of the product?
[RAM: Fe = 56, Br = 80]

Number of moles of Fe = 2.8 = 0.05 mol
56

From the equation, 2 mol of Fe produces 2 mol of FeBr3.
0.05 × 2
Therefore, 0.05 mol of Fe produces 2 = 0.05 mol of FeBr3.

Mass of FeBr3 = 0.05 × [56 + 3(80)] = 0.05 × 296 = 14.8 g

34

5Chapter Theme 2: Fundamentals of Chemistry

Chemical Bond

CHAPTER 5 FORM 4 5.1 Basics of Compound Bakti Sdn. Bhd  3 Atoms of noble gases are inert which
Formation means they do not share, release
or donate electrons with other
Stability of Noble Gases elements or between themselves.

 1 Elements naturally combine with  4 This is because atoms of noble gases
each other to form compounds. have achieved a stable duplet or
This is because the compounds octet electron arrangement.
formed are more stable than the
free elements. Stable Duplet and Octet Electron
Arrangements
 2 However, noble gases (Group 18)
are chemically unreactive and exist   1 Noble gases are stable due to their
as monoatomic gases in nature. electron arrangement.

He Ne Ar Kr

2 2.8 u 2.8.8 2.8.18.8

Duplet Octet
Penerbit Ilm
Diagram 5.1 Electron arrangement of noble gases

 2 Based on Diagram 5.1, it can be  5 Because of this, the energy of the
observed that helium, He has two electrons is very low and so, it is
electrons in its outermost shell difficult for the atoms to release
(valence shell). This is called a stable or receive electrons.
duplet electron arrangement.
Octet Rule
 3 The maximum number of electrons
that can be filled in the first shell  1 In order to achieve the stable octet
is two. Therefore, it is considered as electron arrangement, atoms in the
full. other main group in the Periodic
Table of Elements will react with
 4 For other noble gases (Ne, Ar, Kr, Xe one another in various ways.
and Rn), the valence shell contains
eight electrons. Thus, they have  2 The octet rule is what makes atoms
achieved a stable octet electron have a tendency to achieve the stable
arrangement. octet electron arrangement.

Keywords • Inert – Lengai • Valence shell – Petala valens
• Stability – Kestabilan

60

 3 However, if the outermost shell is the ➤
first shell, the maximum number of
electrons that can be filled is two. Na + Cl
Hence, the stable duplet electron
arrangement is achieved. 2.8.1 2.8.7
–
 4 The duplet electron arrangement +
is as stable as the octet electron Na Cl
Penerbit Ilmu Bakti Sdn. Bhd arrangement since there is no shell CHAPTER 5 FORM 4
occupied with electrons other than 2.8 2.8.8
the first shell. This is also said to
obey the octet rule. Diagram 5.2 Sodium atom transfers an electron
to chlorine atom to achieve stable octet electron
Scan the QR code or visit
https://youtu.be/XGZIIwtIzyg to arrangement
watch a video in order to learn
more about duplet and octet  5 A covalent bond is formed when
electron arrangement. a non-metal atom combines with
another non-metal atom. Both
For educational purposes only atoms will share their electrons to
form a bond.
Chemical Bonds
 1 There are two ways for atoms of an  6 For example, the formation of
chlorine gas:
element to achieve the stable duplet
or octet electron arrangement: Cl + Cl
(a) Transfer of electrons
(b) Sharing of electrons 2.8.7 2.8.7
 2 Those two ways will lead to the
formation of two types of chemical Cl Cl
bonds:
(a) Ionic bond 2.8.8 2.8.8
(b) Covalent bond
Diagram 5.3 Two chlorine atoms share a pair
Dynamic Info of electrons to achieve stable octet electron

The formation of chemical bonds only arrangement
involves the valence electrons.
QUICK CHECK 5.1
 3 An ionic bond is formed between a
metal and a non-metal atoms. The 1 State two types of chemical bonds.
metal atom transfers electrons to 2 Why noble gases do not form
the non-metal atom.
compounds?
 4 For example, the formation of
sodium chloride compound:

61

CHAPTER 5 FORM 4 5.2 Ionic Bond Bakti Sdn. BhdFormation of Ions

u 1 Ionic bond is a type of chemical  1 Ion is a charged particle that is
bond that is generated between formed when an atom accepts or
two oppositely charged ions by loses its electrons.
transfer of electrons between the
atoms.  2 Thus, an ion is an atom or a group
of atoms that carries a positive
 2 Ionic bonds are always formed or negative charge. For instance:
between metal and non-metal Magnesium ion, Mg2+, hydrogen
atoms. ion, H+, iodide ion, I– and nitrate

 3 In an ionic bond, the metal  3 iAonn,eNutOra3l–.particle means it has an
atom releases electrons to form a equal number of protons (+) and
positively-charged ion called cation electrons (–). Therefore, the total
while the non-metal atom receives charge of the particle is zero.
the electrons to form a negatively-
charged ion called anion. Formation of cations (positively-

 4 The compound formed is called charged ions)
ionic compound.
 1 Cations are formed by metal atoms.
 5 Diagram 5.4 shows an example of an  2 Metal atoms from Groups 1, 2 and
ionic compound formed between a
sodium ion, Na+ and a chloride ion, 13 in the Periodic Table of Elements
Cl–. have 1, 2 and 3 valence electrons
respectively.
–  3 They form cations by releasing
+ the valence electrons in order to
achieve the stable octet electron
Na Cl arrangement.
 4 When the protons in the nucleus of
Diagram 5.4 Ionic bond between sodium ion, Na+ an atom outnumber the electrons
and chloride ion, Cl– after the valence electrons are
Penerbit Ilm released, a positive ion is formed.

EXAMPLE +
  1 Formation of a cation with a charge of +1 K

Releases 1 electron
K

Number of protons = 19 Number of protons = 19
Number of electrons = 19 Number of electrons = 18
Charge = +1 (positive)
Charge = 0 (neutral)

K → K+ + e–
A neutral potassium atom loses an electron to form a potassium ion (cation) with the

charge of +1.

62

6.9 Preparation of Salts

Soluble and Insoluble Salts

 1 Salts are ionic compounds. So, most salts can dissolve (soluble) in water. However,
some salts are insoluble in water.

 2 Table 6.10 shows the solubility of different types of salts in water.
Penerbit Ilmu Bakti Sdn. Bhd
Table 6.10 Solubility of salts in water

Salts Solubility in water CHAPTER 6 FORM 4
Sodium, potassium and ammonium salts
Nitrate salts All are soluble
Carbonate salts
All are soluble
Chloride salts
All are insoluble except
Sulphate salts • PASoomdtamiussominuimcuamrcbacorabnroabtnoean,taNet,aeK2,C2(CONO3H34)2CO3
•
•

All are soluble except
• Silver chloride, AgCl
• Lead(II) chloride, PbCl2

All are soluble except
• BCLeaaarlciduiu(mImI) sssuuullpplphhhaaattetee,, ,BPCabaSSSOOO444
•
•

NOTE: ianscloealdd(wII)atcehrlobruidt es,oPlubbClle2,
Lead halides such lead(II) bromide, PbBr2 and lead(II) iodide,
PbI2 are insoluble in hot water.

Experiment 6.4

Aim: Apparatus:
To study the solubility of nitrate, sulphate, Test tubes, glass rod, spatula, test tube rack
carbonate and chloride salts
Materials:
Problem statement: Nitrate, sulphate, carbonate and chloride
Are all salts soluble in water? salts, distilled water

Hypothesis: Procedure:
Some salts are soluble in water while some  1 5.0 cm3 of distilled water is poured into
are insoluble in water.
five different test tubes.
Variables:  2 0.2 g of copper(II) nitrate, magnesium
(a) Manipulated: Types of salts
(b) Responding: Solubility of salts in water nitrate, zinc nitrate, lead(II) nitrate and
(c) Fixed: Quantity of salts, volume and calcium nitrate are added into each
test tube respectively using a spatula.
temperature of water

Keywords • Insoluble salt – Garam tak terlarutkan
• Soluble salt – Garam terlarutkan

109

 3 The test tubes are shaken to mix the mixture and the observation is recorded.
 4 The experiment is repeated by referring to the following table to replace the nitrate

salts.

Results:

Type of salt Formula of salts Solubility in water

CHAPTER 6 FORM 4 Nitrate CPbu((NNOO33))22,, CMag(N(NOO3)32)2, Zn(NO3)2,Bakti Sdn. Bhd Soluble
Sulphate CuSO4, MgSO4, ZnSO4
Chloride PbSO4, BaSO4 Soluble
Carbonate CuCl2, MgCl2, ZnCl2 Insoluble
PbCl2, AgCl Soluble
Na2CO3, K2CO3, (NH4)2CO3 Insoluble
CuCO3, MgCO3, ZnCO3 Soluble
Insoluble

Conclusion:
Some salts are soluble in water and some are insoluble in water.

Preparation of Soluble Salts Tree Map
Diagram 6.19 shows the preparation of soluble salts.

Soluble salts

u
Penerbit Ilm
• Sodium salts Other salts
• Potassium salts
• Ammonium salts

Preparation Preparation

Acid + alkali → salt + water • Acid + reactive metal → salt + hydrogen gas
(Neutralisation) • Acid + metal oxide → salt + water
• Acid + metal carbonate → salt + water + carbon dioxide gas

Diagram 6.19 Preparation of soluble salts

There are two things to be considered when preparing a salt:
1 What are the chemicals used?
2 How to separate the salt from the other substance?
110

AAccttivivitityy66.3.6

Aim: (B) Preparation of the salt
To prepare a soluble salt through the
reaction of an acid and an alkali Glass rod
Apparatus:
Pipette, bulb, burette, retort stand with Salt Sodium
clamps, conical flask, beaker, white tile, solution xxxxxxxxxxxxxxxxxxxx Cooled salt chloride
tripod stand, glass rod, wire gauze, Bunsen crystals
burner, spatula, filter funnel, filter paper Heat solution
Materials:
1.0 mol dm–3 hydrochloric acid, 1.0 mol dm–3
sodium hydroxide solution, phenolphthalein
solution
Procedure:
(A) Determine the volume of acid for

neutralisation

Burette
Penerbit Ilmu Bakti Sdn. Bhd Sodium Distilled Filter CHAPTER 6 FORM 4
chloride water paper
crystals Sodium chloride
crystals

 1 The experiment is repeated by adding
the calculated volume of 1.0 mol dm–3
hydrochloric acid to 25.0 cm3 of 1.0 mol
dm–3 sodium hydroxide solution in a
beaker without the phenolphthalein
solution.
Retort 1.0 mol dm–3  2 The colourless solution in the beaker is
stand hydrochloric acid evaporated to form a saturated solution

25.0 cm3 of 1.0 mol dm–3  3 T( h43e of water is evaporated). down
sodium hydroxide solution saturated solution is cooled
+ phenolphthalein indicator to allow crystallisation to occur.
 4 The white crystals formed is filtered, then
 1 A burette is filled with 1.0 mol dm–3 rinsed with a little distilled water and
hydrochloric acid and the initial burette dried between filter papers.
reading is recorded.
(C) Recrystallisation of the salt
 2 25.0 cm3 of 1.0 mol dm–3 sodium hydroxide  1 The impure sodium chloride crystals is
solution is drew up using a pipette and
transferred into a conical flask. placed in a beaker.
 2 A little distilled water is added just
 3 2 to 3 drops of phenolphthalein solution
are added into the conical flask and the enough to cover the crystals. The mixture
initial colour of the solution is recorded. is heated while stirring and more distilled
water is added slowly until all the crystals
 4 The conical flask is placed below the are dissolved.
burette and put a white tile under it.  3 The solution is filtered into a clean
conical flask to remove impurities.
 5 The titration is started by adding the  4 The filtrate is heated to obtain a saturated
hydrochloric acid into the conical flask solution.
while swirling the flask gently.  5 The saturated solution is allowed to
cool down to room temperature for
 6 The titration is stopped when the colour crystallisation to occur.
of the solution changes from light pink  6 The crystals is filtered, then rinsed with
to colourless. The final burette reading a little distilled water and dried between
is recorded. filter papers.

  7 The volume of 1.0 mol dm–3 hydrochloric
acid used is calculated.

Dynamic Info

Recrystallisation is a procedure to purify salt.

111

Uses of Ceramics
Table 8.3 shows the uses of ceramics.

Table 8.3 Uses of ceramics

Use Example
Building materials Making bricks, cements and concretes, tiles, toilet bowls
Kitchenware Pots, plates, mugs
Decorative items Vases, potteries
Insulators Wall of nuclear reactors, engine parts, wall of furnaces
Electrical items Electric cables and plugs
Medical Dentures, bone implants, knee joint replacements
CHAPTER 8 FORM 4 Bakti Sdn. Bhd
Dynamic Info

The table below shows the properties of ceramics that make them suitable to be used as
building materials.

Building material u Property
Bricks • Available in large quantities
• Lighter than stones
Cement and concrete • Weatherproof
• Cheap
Tiles • Can withstand high temperature
Penerbit Ilm • Can be produced in large volumes
• Stronger binding material
• Can withstand compression
• Durable
• Waterproof
• Resistant to abrasion
• Durable

QUICK CHECK 8.3 8.4 Composite Materials
and their Importance
1 State three properties of ceramics.
2 Compare and contrast between  1 Composite material is the
combination of two or more non-
traditional ceramics and advanced homogenous materials (matrix and
ceramics. HOTS Analysing strengthening substances) that has
3 Explain with examples how different physical properties from
ceramics are beneficial in the the original materials.
medical field.
4 Why are ceramics suitable to be  2 The matrix substance surrounds and
used as kitchenware compared to binds the strengthening substance
pure metals? HOTS Analysing together to form a new material
(composite material).
Keywords

• Composite material – Bahan komposit • Matrix – Matriks • Strengthening – Pengukuhan

162

 3 Composite materials are the improved version of the original substances.
 4 Table 8.4 shows the five types of composite materials and their characteristics.

Table 8.4 Types, components, properties and uses of composite materials

Composite Component Property Use
material • Concrete (cement To build buildings,
• Stronger bridges
Reinforced and stone) • Does not rust
concrete • Steel • Able to withstand a Used in MRI
machines, Maglev
Superconductor • Copper(II) oxide stronger force trains, generators,
• Barium carbonate • Conducts electricity making computer
• Yttrium oxide parts
with no resistance To make helmets,
at a very low construction
temperature panels, pipes, water
Penerbit Ilmu Bakti Sdn. Bhd tanks, racquets CHAPTER 8 FORM 4
Fibre glass • Glass fibres • High tensile strength To make optical
• Polyester • Does not corrode lenses, car
• Can be moulded windshields
Photochromic • Silver chloride • Stronger
glass • Glass • Darkens when Used as
telecommunication
Optical fibre • Silica exposed to light cables, medical
• Sodium • Brightens when it is endoscopes

carbonate dark
• Calcium oxide • Able to transmit

digital data at a high
speed
• Flexible
• Thinner
• Chemically inert

QUICK CHECK 8.4 3 The diagram below shows an example
of a composite material, optical fibre.
1 List the components in a
superconductor and its properties.

2 The diagram below shows a pair of
spectacles made from a type of soda
lime glass.

Suggest a composite material that can
be used to improve the properties of The composite material is widely
the glass and explain. HOTS Creating
used in telecommunication.
Briefly describe its properties and
why it is suitable to be used in
telecommunication. HOTS Analysing

Keywords
• Reinforced concrete – Konkrit diperkukuhkan

163

2Chapter Theme 2: Organic Chemistry

Carbon Compound

2.1 Types of Carbon Compounds Bakti Sdn. Bhd

CHAPTER 2 FORM 5   1 Carbon compounds are compounds that contain the carbon element.
 2 Carbon compounds can be divided into two:

(a) Organic compounds – compounds found in or produced by living things
that contain carbon-hydrogen bonds. Some examples are petrol, sugar and
polyvinyl chloride (PVC).

(b) Inorganic compounds – compounds derived from mineral sources that
have no carbon-hydrogen bonds. The examples include carbon monoxide,
CO, carbon dioxide, CO2 and calcium carbonate, CaCO3.

 3 Further classification for organic compounds divides them into two groups, the
hydrocarbons and the non hydrocarbons. Diagram 2.1 shows the classification.

Tree Map

Organic compounds

Hydrocarbons Non hydrocarbons
Contain only C and Contain C and H atoms

H atoms and other elements
u
Penerbit Ilm
Saturated hydrocarbons Unsaturated hydrocarbons Alcohols Carboxylic
Hydrocarbons which Hydrocarbons which acids
contain only single
contain at least one double
covalent bonds between or triple covalent bonds
carbon atoms
between the carbon atoms

Alkane Alkene Alkyne
H H H H H H H H
| | | | | | | |
H—C—C—C—H H—C—C—C==C H—C≡ C—C—H
| | | | | | |
H H H H H H H
Single covalent bond Double covalent bond Triple covalent bond

Diagram 2.1 Classification of organic compounds

Sources and Uses of Hydrocarbons

 1 The main sources of hydrocarbons:

(a) Crude oil (b) Natural gas (c) Coal

Keywords • Alkyne – Alkuna
• Hydrocarbon – Hidrokarbon

216

 2 Crude oil and natural gas are formed from the decomposition of animals and
plants millions of years ago whereas coal is produced from dead wood.

 3 Table 2.1 shows the uses of hydrocarbons in daily life.

Table 2.1 Uses of hydrocarbons

Type of hydrocarbon Uses
Petroleum gas (propane, butane) Used in cooking gas, fireplaces and grills
Naphta Used in petrochemical industry
Petrol Used as fuel for cars
Kerosene Used as fuel for aeroplanes
Diesel Used as fuel for lorries and heavy vehicles
Lubricating oil Used as lubricants and candles
Fuel oil Used as fuel for power plants and ships
Bitumen Used as materials to pave roads
Penerbit Ilmu Bakti Sdn. Bhd
 4 After crude oil is extracted by drilling wells into underground reservoirs, it CHAPTER 2 FORM 5
needs to undergo fractional distillation and cracking process in petroleum
refinery.

 5 Fractional distillation is a process to separate the fractions of hydrocarbons in
petroleum at different temperatures according to their size.

 6 Cracking is a process in which heavy hydrocarbon molecules are broken up into
lighter molecules with the help of heat, pressure and a catalyst.

 7 This process produces products such as methane gas, ethane gas, propane
gas and much more. Diagram 2.2 shows the fractional distillation process in
petroleum refinery.

Petroleum gas (< 40 °C)

Fractionating Petrol (40 – 75 °C)
tower Naphta (75 – 150 °C)
Kerosene (160 – 250 °C)
Crude oil vapours Diesel (125 – 300 °C)

Lubricating oil
(300 – 350 °C)

Fuel oil (350 – 500 °C)

Petroleum 400 °C Bitumen ( > 500 °C)
(Crude oil)

Furnace

Diagram 2.2 Fractional distillation process in petroleum refinery

Keywords • Petroleum refinery – Penapisan petroleum
• Cracking process – Proses peretakan

217

4Chapter Theme 4: Technology in Chemistry

Polymer

Penerbit Ilmu Bakti Sdn. Bhd4.1 Polymer

 1 Polymer is made of hundreds or thousands of molecules (monomers) that link

together to form a long chain molecule.
 2 Monomer is a small molecule used to synthesise polymers.
 3 The word “poly” means many and “mono” means one or single.
 4 Polymerisation reaction occurs when many small molecules (monomers) are

joined by covalent bonds.
 5 A group of atoms in a polymer is called repeating unit. For instance, the

jroeipneattoignegthuenritbiynfpoormlyeinthgecnoev(aploenlytthbeonned)sisto—fCoHrm2—tChHe 2p—o.lyTmheesre, repeating units CHAPTER 4 FORM 5
polythene.
 6 The repeating unit of polythene and a portion of the polymer are shown in

Diagram 4.1.

1 2 H H 1 2 H H H H H H H H

| | | | | | | | | |

—C—C— —C—C—C—C—C—C—C—C—

| | | | | | | | | |
H H n H H H H H H H n H

Repeating unit of polythene Polythene polymer

Diagram 4.1 Polythene

 7 Other examples of commonly used polymers are shown in Table 4.1 with their
monomers and repeating units.

Table 4.1 Commonly used polymers, their repeating units and monomers

Polymer Repeating units Monomers

­—CH2­—CH2­­—CH2­—­ CH2—­ 1 2 H H CH2=CH2
Polyethene (Polythene) Ethene
| |

—C—C—

| |

H H n

H H H H 1 2 H H CH3CH=CH2
Propene
| | | | | |

—C—C—C—C— —C—C——

| | | | | |

H CH3 H CH3 H CH3 n

Polypropene (PP)

—CH2—­ CH=CH—­ CH2—­  2—CH2­—CH=CH­—CH2­—n H H
Polybutadiene
C—C
H—C C—H

| |

H H

Butadiene

Keywords • Monomer – Monomer • Repeating unit – Unit berulang
• Polymer – Polimer

273

Polymer Repeating units Monomers

H H H H H H — CH2—­ C| H—n |
H2C=CH
| | | | | | | | | | | |
Styrene
—C—C—C—C—C—C—C—C—C—C—C—C—

| | | | | | | | | | | |

H H H H H H H H H H H H

Polystyrene (PS)

HH
H H H H H H H H H Bakti Sdn. Bhd H H H H| C| =C|
| H H | | H H | | H | | H H | |
C | | C—C | | C—C | C—C | | C—C —  CH2—CH=CH—CH2­—n— CH2—HC| —n | | |
|
| C=C | | C=C | | C | | C=C | | C=C C=C
H | | | | | | | H
H H H H H H H H H | |
H H H H H H
H

Polystyrene butadiene Styrene and butadiene

F F F F F F F F F F 1 2 F F CF2=CF2
Tetrafluoroethene
| | | | | | | | | | | |

—C—C—C—C—C—C—C—C—C—C— —C—C—

| | | | | | | | | | | |

F F F F F F F F F F F F n

Polytetrafluoroethene (Teflon)



CHAPTER 4 FORM 5  8 Polymers can be classified based on three aspects:

(a) Sourced from natural or synthetic materials

(b) Their properties – thermoplastic, thermoset, elastomer

(c) Polymerisation processes

Natural Polymers and Synthetic Polymers u

 1 In general, there are two main sources of polymer, which are natural polymers
and polymers that are made from synthetic materials.

 2 Due to the broad range of properties, both natural and synthetic polymers play
essential roles in daily life.

 3 Natural polymers such as protein, can be derived from variety of sources like
animals, plants and microorganisms.

 4 Table 4.2 shows some examples of natural polymers and their monomers.
Penerbit Ilm
Table 4.2 Natural polymers and their monomers

Natural polymer Monomer

Natural rubber Isoprene

Protein Amino acid
Starch Glucose

Cellulose Glucose
Gelatine Collagen

 5 Many common synthetic polymers are made from petroleum and other
hydrocarbons. For instance, chains of ethylene molecules can combine to form
an artificial polyethylene.

Keywords
• Synthetic polymer – Polimer sintetik

274

 6 Table 4.3 shows some examples of synthetic polymers and their monomers.

Table 4.3 Synthetic polymers and their monomers

Synthetic polymer Monomer
Polythene Ethene

Polypropene Propene (propylene)
Polyvinyl chloride Vinyl chloride (chloroethene)

Polystyrene Styrene
Polyamides (nylon) Amide
Penerbit Ilmu Bakti Sdn. Bhd
  7 One example of synthetic polymers is polyvinyl chloride or its common name,
PVC. It is the third most widely produced synthetic polymer in the world.

  8 PVC is a high strength thermoplastic material used in making pipes, cables,
medical devices and many more. Diagram 4.2 shows the uses of PVC in daily life.

Construction Domestic Packaging Wires & cables CHAPTER 4 FORM 5

Automotive Medical Toys Clothing

Diagram 4.2 Uses of polyvinyl chloride (PVC)

  9 In general, polymer properties can  3 The strong hydrogen bonds between
be divided into three types: the thermoplastic molecules help
(a) Thermoplastic polymers to prevent from flowing under
(b) Thermosetting polymers moderate stress. This is what makes
(c) Elastomers polymers a thermoplastic material a practical
rubbery solid.
Thermoplastic polymers
 4 Commonexamplesofthermoplastics
 1 Thermoplastic is a rubbery solid are polyvinyl chloride (PVC), teflon,
material consists of polymers nylon, acrylic, polyester, polystyrene
linked by strong intermolecular and polypropylene.
interactions. However, these
intermolecular interactions do not  5 Diagram 4.3 shows the structure of
have real chemical interlinks. a thermoplastic.

 2 Thus, a thermoplastic responds Diagram 4.3 Thermoplastic polymer structure
to high temperature and pressure
where it forms a new shape that
can be reprocessed and reused.

Keywords • Thermoplastic – Termoplastik • Thermoset – Termoset
• Elastomer – Elastomer

275

Answers

FORM 4 (b) To carry out experiments that
release toxic vapours, cause
combustions or produce pungent
smells

(c) To extinguish fire in the laboratory
3 Hydrocarbons and organic solvents are

stored in a shady area which is far from
sunlight and sources of heat.

Summative Practice 1

1 C 2 D 3 D 4 B 5 C
6 A 7 D
ANSWERSPenerbit Ilm1Chapter Introduction to Chemistry
u
Bakti Sdn. BhdQuick Check 1.1

1 Chemistry is the study of the
composition of substances, basic form of
matter and interaction between matter.

2 Field Chemicals

Medicine Antibiotics, vitamins

Food Preservatives, colourings

Agriculture Fertilisers, pesticides 2Chapter Matter and the Atomic

Industry Paints, alloys Structure

3 Doctor, pharmacist, biotechnology Quick Check 2.1
researcher, biomedical engineer and
nanotechnology engineer 1 Matter is anything that occupies space

and has mass such as a book, air and

Quick Check 1.2 soil.

1 Scientific method is a systematic 2 (a) The constant temperature when a
approach used by scientists to
investigate phenomena. solid completely changes to become

2 The steps in the scientific method: a liquid at a specific pressure
1. Making an observation
2. Making an inference (b) The constant temperature when
3. Identifying the problem
4. Making a hypothesis a liquid changes to a solid at a
5. Identifying the variables
6. Controlling the variables specific pressure
7. Planning an experiment
8. Collecting data 3 (a) Melting (b) Molecule
9. Interpreting data
10. Making a conclusion (c) (i) (ii)
11. Writing a report
4 (a) (i)
(ii)


(b) Temperature (oC)

Quick Check 1.3 80

1 Safety goggles, face mask, gloves, Time (s)
laboratory coat and laboratory shoes
5 The heat lost to the surrounding is
2 (a) To wash and clean the eyes when exactly balanced by the heat energy
accidents occur on any part of the released as the particles attract one
another to form a solid.
eyes

330

Quick Check 2.2 (b) RMM of Na2CO3 = 2(23) + 12 + 3(16)

1 Protons, electrons and neutrons = 106
2 (a) X: Electron   Y: Nucleus
2 2X + 3(32) + 12(16) = 342

(b) Particle Proton Neutron  2X = 342 – 288

Relative charge +1 0 X = 54 = 27
2
3 (a) The mass of one aluminium atom
Relative mass 1 1 1
is 27 times greater than 12 mass of
Penerbit Ilmu Bakti Sdn. Bhd
Quick Check 2.3 one carbon-12 atom.

1 (a) Nucleon number of an element is (b) 27 = 3 times
9
the total number of protons and

neutrons in the nucleus of its atom. Quick Check 3.2

(b) Proton number is the number of 1 (a) 1.0 × 6.02 × 1023 = 6.02 × 1023 atoms

protons in the nucleus of an atom. (b) 0.5 × 6.02 × 1023 = 3.01 × 1023 ions

2 (a) 24 (b) 2.8.2 (c) 4.0×6.02×1023=2.408×1024molecules

3 35 – 17 = 18 2 (a) 4.5 × 6.02 × 1023 = 2.709 × 1024 atoms

4 (a) 2.4 (b) 0.4 × 6.02 × 1023 × 5 = 1.204 × 1024 atoms

(b) (i) 11 + 12 = 22 (ii) +1 (c) 6.0 × 6.02 × 1023 = 3.612 × 1024 atoms

(c) 1.62 × 1024
6.02 × 1023
3 (a) = 2.691 mol

C 4.5 × 1023
6.02 × 1023
(b) = 0.748 mol

Quick Check 2.4 4 (a) 31 = 0.775 mol
40
1 Isotopes are atoms of the same element
(b) 17.25 = 0.138 mol
with the same number of protons but 65 + 12 + 3(16)

different numbers of neutrons. (c) 23.45 = 0.135 mol
+ 32 +
2 1. Isotopes have the same number of 2(39) 4(16)

protons/proton number 5 (a) 45.22 = 1.884 mol
24
2. Isotopes have different number of

neutrons. (b) 0.46 = 0.019 mol
24
3. Isotopes have different nucleon

numbers. 5.4
22.4
3 (a) To estimate the age of artifacts (c) = 0.241 mol

(b) Relative atomic mass of C 0.45
22.4
= (99 × 12) + (1 × 13) = 12.01 (d) = 0.02 mol ANSWERS
100

Summative Practice 2 Quick Check 3.3

1 D 2 B 3 A 4 A 5 C 1
6 D 7 C 8 A 9 C 10 B
Element Zn S O

Mass (g) 9.75 4.8 9.6

3Chapter The Mole Concept, Chemical Number 9.75 = 0.15 4.8 = 0.15 9.6 = 0.60
of moles 65 32 16
Formula and Equation
Mole 0.15 0.15 0.6
Quick Check 3.1 ratio 0.15 = 1 0.15 = 1 0.15 = 4

1 (a) RMM of MgSO4 = 24 + 32 + 4(16) Therefore, the empirical formula is
= 120 ZnSO4.

331