MKS@Chemistry Module Form 4 Complete Set

Mohd Faisol Mansor

[email protected]

TABLE OF CONTENTS

CHAPTER 1 : INTRODUCTION TO CHEMISTRY Page 1

CHAPTER 2 : THE STRUCTURE OF THE ATOM Page 5

CHAPTER 3 : CHEMICAL FORMULAE & EQUATIONS Page 22

CHAPTER 4 : PERIODIC TABLE OF ELEMENTS Page 54

CHAPTER 5 : CHEMICAL BONDS Page 79

CHAPTER 6 : ELECTROCHEMISTRY Page 100

CHAPTER 7 : ACIDS & BASES Page 130

CHAPTER 8 : SALTS Page 148

CHAPTER 9 : MANUFACTURED SUBTSANCES Page 175
: IN INDUSTRY

mohd faisol mansor/chemistry form 4/chapter 1

CHAPTER 1

INTRODUCTION TO CHEMISTRY

Chemistry Uses of Chemical Careers

Is the study of the Salt (NaCl) Doctor
composition, Vinegar (CH3COOH) Chemical Engineer
Tiles/Cement (CaCO3)
structure, properties Geologist
& interactions of Biochemist
matter. Pharmacist

Chemical Industry Contribution of Chemical
Industries
Petroleum
Food  Financial
 Job opportunity
Chemical Substance  Development of
Electronic
Agriculture country

Scientific Method : systematic method used to solve problems in Science.

Making Making Identifying Making
Observation Inference Problem Hypothesis

Collecting Planning an Controlling Identifying
Data Experiment Variables Variables

Interpreting Making Writing
Data Conclusion Report

1

mohd faisol mansor/chemistry form 4/chapter 1

PERIODIC TABLE OF THE ELEMENTS

2

mohd faisol mansor/chemistry form 4/chapter 1

Classify each of the following element into their group.

Hydrogen, H Oxygen, O Zinc, Zn
Chlorine, Cl Potassium, K Silver, Ag
Sodium, Na Carbon, C Phosphorus, P
Magnesium, Mg Sulphur, S Fluorine, F
Aluminium, Al Lithium, Li Barium, Ba
Copper, Cu Bromine, Br Lead, Pb
Neon, Ne Argon, Ar Calcium, Ca
Helium, He Iron, Fe Iodine, I

Metal Atom Nonmetal Atom

3

mohd faisol mansor/chemistry form 4/chapter 1

Classify each of the following element/compound into their group.

Sodium chloride, NaCl Hydrogen gas, H2
Chlorine gas, Cl2 Lead(II) oxide, PbO
Aluminium oxide, Al2O3 Silver bromide, AgBr
Carbon dioxide, CO2 Naphthalene, C10H8
Sugar, C6H12O6 Copper(II) iodide, CuI2
Oxygen gas, O2 Magnesium oxide, MgO
Zinc chloride, ZnCl2 Methane, CH4
Ethanol, C2H6O Water, H2O

Ionic Compound Molecule

(Metal Atom + Nonmetal Atom) (Nonmetal Atom + Nonmetal Atom)

4

mohd faisol mansor/chemistry form 4/chapter 2

CHAPTER 2

THE STRUCTURE OF THE ATOM

Element

Matter Substance that Compound
consists of only one
Anything that Substance that contains
occupies space & has type of atom. two or more elements
that are chemically
mass. bonded together.

Type of Particles Kinetic Theory of Matter Physical State
Atom
 Matter is made up of  Solid
Molecule tiny & discrete particle.  Liquid
Ion  Gas
 Particle vibrate, moving
Atom & collide with each other. Subatomic Particles

Smallest particle of  Particles move randomly. Electron
an element that can  There are forces between Proton
take place in chemical Neutron
the particle. Stronger the
reaction. forces, particle close to
each other.
Ion  Higher the temperature,
higher the kinetic energy
Is a positive charged of particle.
or negative charged
Molecule Diffusion
particle.
A group of two or Is a random movement
more atoms which are between different
particles from high
chemically bonded
together. concentration to lower
concentration.

5

mohd faisol mansor/chemistry form 4/chapter 2

+ Atom, Molecule & Ion

Atom Atom Molecule (ELEMENT)

+ Molecule (COMPOUND)

Atom Atom + - Ionic Compound

++ -

Cation Anion

Example: Formation of WATER Water Molecule

+

Oxygen Atom Hydrogen Atom

A Glass of Water

6

mohd faisol mansor/chemistry form 4/chapter 2

Diffusion in Solid: Test tube is filled with a hot jelly and copper(II) sulphate crystal.

Difussion Rate:

Reason:

Diffusion in Liquid: A beaker is filled with water & potassium manganate (VII).

Difussion Rate:

Reason:

Diffusion in Gas: A gas jar is filled with few drop of bromine liquid.

Difussion Rate:

Reason:

7

mohd faisol mansor/chemistry form 4/chapter 2

States Particles Forces between Particles Motion
Arrangement particles

SOLID Held together Vibrate and rotate at
very strong fixed position

Packed closely in
orderly manner

LIQUID Strong but weaker Vibrate, rotate and
than solid move through liquid &
collide against each
Packed closely not in
orderly arrangement other

GAS weak Vibrate, rotate and
move freely
Far apart from each
other Gas

Solid Liquid Shape :

Shape : Shape : Ability to be
compressed:
Ability to be Ability to be
compressed: compressed:

8

mohd faisol mansor/chemistry form 4/chapter 2

Change in the State of Matter

Changes in the Heat Energy

9

mohd faisol mansor/chemistry form 4/chapter 2

Heating of Naphthalene Cooling of Naphthalene

1. Why is solid naphthalene, C10H8 not heated directly with Bunsen burner?
2. Why is water bath used to heat the naphthalene?
3. During the cooling of naphthalene, explain why

a) the boiling tube must place in a conical flask?

b) the naphthalene must stirred continuously?

4. What happens to the temperature of naphthalene during
a) melting? Give a reason.

b) freezing? Give a reason.

5. The melting point of sugar is 184oC. The melting point of sugar cannot be
determined using same apparatus. Why? What apparatus can be used
instead?

10

mohd faisol mansor/chemistry form 4/chapter 2

The Heating Curve of Naphthalene
Temperature (oC)

D

B C
A

Melting Point Physical State Time (min)

Is the temperature at AB = Why the temperature
which a solid changes into BC = increase from A to B?
CD =
a liquid at a particular When solid is heated,
pressure. heat energy is

________________.
This cause particles to
_________ kinetic energy
and vibrate __________.

Why the temperature Also known as Why the temperature
remains constant at BC? latent heat of increase from C to D?

Heat energy ___________ fusion. When liquid is heated,
by the particles is used to heat energy is

overcome the force ________________.
between the particles so This cause particles to
_________ kinetic energy
that the solid turn into and move __________.
liquid.

* label the melting point of the naphthalene in the diagram above as MP.
11

mohd faisol mansor/chemistry form 4/chapter 2

The Cooling Curve of Naphthalene
Temperature (oC)
E

FG

Freezing Point Physical State H

Is the temperature at EF = Time (min)
which a liquid changes FG =
into a solid at a particular GH = Why the temperature
decrease from E to F?
pressure.
When liquid is cooled,
heat energy is

________________.
This cause particles to
_________ kinetic energy
and move __________.

Why the temperature How to avoid supercooling? Why the temperature
remains constant at FG? decrease from G to H?

Heat energy ___________ When solid is cooled,
to the surroundings is heat energy is

exactly same as the heat ________________.
energy released by This cause particles to
particle to form the _________ kinetic energy
and vibrate __________.
forces to become a solid.

* label the freezing point of the naphthalene in the diagram above as FP.
12

mohd faisol mansor/chemistry form 4/chapter 2

The Atomic Structure

[Draw the atomic model & briefly explain]

(1) John Dalton
(1766 – 1844)

(2) J.J. Thomson (3) Ernest Rutherford
(1856 – 1940) (1871 - 1937)

(5) James Chadwick
(1891 - 1974)

(4) Neils Bohr
(1885 - 1962)

13

mohd faisol mansor/chemistry form 4/chapter 2

Subatomic Particles of an Atom

NUCLEUS PROTON NEUTRON
Proton + Neutron
Symbol : p Symbol : n
NUCLEON NUMBER = Relative electric Relative electric

Proton + Number of charge : +1 charge : 0
Relative mass: 1 Relative mass: 1
Number Neutron
NEUTRAL ATOM ELECTRON
Atom Q has a proton number Number of proton
of 11 and a nucleon number of Symbol : e
is equal to the Relative electric
23. How many protons, number of electron.
electrons and neutrons are charge : -1
Relative mass: 0.0005
present in the atom?
Definition
Nucleon number is
the total number of
proton and neutrons

in its atom.

Definition
Proton number is the
number of protons in

its atom.

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mohd faisol mansor/chemistry form 4/chapter 2

Symbol of Elements

Element Symbol Element Symbol Element Symbol Element Symbol

Hydrogen Carbon Sodium Sulphur

Helium Nitrogen Magnesium Chlorine
Lithium Oxygen Aluminium Argon
Beryllium Fluorine
Silicon Potassium

Boron Neon Phosphorus Calcium

2131Na A fluorine atom has 9 protons and
10 neutrons. What is the proton
Also represented number and nucleon number of
by sodium-23 the atom? Represent the atom in
the form of .

Bromine-80 has 45 neutrons.

What are the proton number

and nucleon number of the

atom? Represent the atom

in the form of .

15

mohd faisol mansor/chemistry form 4/chapter 2

ISOTOPES Element Nucleon Proton No. of No. of
Number Number Neutron Electron
Atoms of the same Hydrogen-1
element has same Hydrogen-2 1 8 6
proton number but Hydrogen-3
different number of Carbon-12 35 17
Carbon-13
neutron Carbon-14
Oxygen-16
Why isotopes element Oxygen-17
has similar chemical Oxygen-18
Chlorine-35
properties? Chlorine-37
Bromine-80
Bromine-81

To determine the To determine
rate of absorption the age of
artifact.
of fertilisers by
plants.

USES OF To detect leaks in
ISOTOPES underground

petroleum pipe.

To detect the
location of a
tumor in the brain.

To treat
cancer.

16

mohd faisol mansor/chemistry form 4/chapter 2

The Electronic Structure of an Atom

Maximum number For atoms with The last shell filled
of electron filled in more than 20 with electrons
electrons, the third known as the
the shell: shell can filled up outermost
to 18 electrons. occupied shell.
1st = 2 electrons
2nd = 8 electrons
3rd = 8 electrons
4th = 8 electrons

Valence Electrons Electron Write the electron
Configuration arrangement for
Electrons in the potassium & state the
outermost Chlorine has valence electrons.
proton number 17.
occupied shell.

17

mohd faisol mansor/chemistry form 4/chapter 2

Element Proton Number of Electron Electronic Structure
Hydrogen Number Electron Configuration

1 & Valence
Electron

E.C =

V.E =

Helium 2

Lithium 3

Beryllium 4

Boron 5

Carbon 6

Nitrogen 7

18

mohd faisol mansor/chemistry form 4/chapter 2

Element Proton Number of Electron Electronic Structure
Number Electron Configuration

& Valence
Electron

Oxygen 8

Fluorine 9

Neon 10

Sodium 11

Magnesium 12

Aluminium 13

19

mohd faisol mansor/chemistry form 4/chapter 2

Element Proton Number of Electron Electronic Structure
Number Electron Configuration &

Valence
Electron

Silicon 14

Phosphorus 15

Sulphur 16

Chlorine 17

Argon 18

20

mohd faisol mansor/chemistry form 4/chapter 2

Element Proton Number of Electron Electronic Structure
Number Electron Configuration &

Valence
Electron

Potassium 19

Calcium 20

21

mohd faisol mansor/chemistry form 4/chapter 3

CHAPTER 3

CHEMICAL FORMULAE & EQUATIONS

Relative Atomic Mass Relative Molecular Mass Relative Formula Mass

Average mass of Average mass of Average mass of
one atom of an one molecule one formula unit
1/12 x mass of an
element 1/12 x mass of an atom of carbon-12
1/12 x mass of an atom of carbon-12
atom of carbon-12

Example 2) The relative atomic mass of helium,
nitrogen and sulphur is 4, 14, and 32
1) Element mercury is 20 times respectively.
heavier than helium. Determine a) How many times is one atom of
the relative atomic mass of sulphur heavier than one atom of
element mercury if the relative helium.
atomic mass of helium is 4.

b) Calculate the number of atoms of
helium that have the same mass as two
atoms of nitrogen.

Relative Molecular Mass (RMM)/Relative Formula Mass (RFM) can
be calculated by adding up the Relative Atomic Mass (RAM).

+-

Water, H2O Sodium Chloride, NaCl
RMM = RFM =

22

mohd faisol mansor/chemistry form 4/chapter 3

Example Atom, Molecule & Ion

1. Calculate relative molecular mass of the following element or compound.

a) Oxygen gas, O2 b) Chlorine gas, Cl2

c) Carbon dioxide, CO2 d) Ammonia, NH3

e) Iodine gas, I2 f) Sulphur dioxide, SO2

g) Sugar, C6H12O6 h) Ethanol, C2H6O

2. Calculate relative formula mass of the following compound.

a) Magnesium oxide, MgO b) Potassium iodide, KI

c) Calcium carbonate, CaCO3 d) Copper(II) nitrate, Cu(NO3)2

e) Aluminium oxide, Al2O3 f) Zinc Sulphate, ZnSO4

g) Hydrated magnesium sulphate, h) Hydrated copper(II) sulphate,
MgSO4.7H2O CuSO4.5H2O

23

mohd faisol mansor/chemistry form 4/chapter 3

The Mole, Number of Particles, Mass & Volume of Substances.

NUMBER OF MASS OF
PARTICLES SUBSTANCES
One mole of The mass of one
substance contains mole of the
6.02 x 1023 particles. substance equal to
the mass of 6.02 x
1023 particles.

Avogadro Constant MOLE Molar Mass
NA = 6.02 x 1023 Amount of substance = RAM/RMM/RFM
that contains as many
mole = no of particles particles as the number mole = Mass
NA of atoms in exactly 12 g Molar Mass

of carbon-12

No of particles Mass = mole x MM
= mole x NA

VOLUME OF GAS Molar Volume
One mole of any gas 1) Room Condition
always has the same
= 24 dm3 mol -1
volume under the 2) At S.T.P
same temperature &
= 22.4 dm3 mol -1
pressure.
mole = Volume
Unit conversion Molar Volume
1 dm3 = 1000 cm3

Volume = mole x MV

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mohd faisol mansor/chemistry form 4/chapter 3

Example 1

1. A closed glass bottle contains 0.5 mol of oxygen gas, O2.
a) How many oxygen molecules, O2 are there in the bottle?

b) How many oxygen atoms are there in the bottle?

2. Find the number of moles of hydrogen gas, H2 containing
a) 3.01 x 1024 hydrogen molecule, H2

b) 6.02 x 1023 hydrogen atoms.

3. Find the number of moles of molecules in a sample containing 9.03 x 1023
molecules of carbon dioxide, CO2.

4. A sample contains 6.02 x 1025 molecule of water. How many moles of water
are there in the sample?

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mohd faisol mansor/chemistry form 4/chapter 3

5. A container contains 1.806 x 1023 oxygen molecules, O2. A sample of 0.5 mol
of oxygen gas, O2 is added to the container. How many molecules are there
altogether in the container?

6. Calcium is needed for the formation of bones and teeth. How many calcium
ions are there in a serving of cereal that contains 0.007 mol of calcium ions?

7. A beaker contains 0.1 mol of zinc chloride, ZnCl2
a) Calculate the number of moles of chloride ions in the beaker.
b) Find the total number of ions in the beaker.

26

mohd faisol mansor/chemistry form 4/chapter 3

Example 2

1. What is the mass of
a) 0.1 mol of magnesium? [RAM: Mg, 24]

b) 2.408 x 1023 atoms of magnesium? [RAM: Mg, 24 ; NA = 6.02 x 1023]

2. How many moles of molecules are there in 16 g of sulphur dioxide gas, SO2?
[RAM: O, 16 ; S, 32]

3. How many chloride ions are there in 27.2 g of zinc chloride, ZnCl2?
[RAM: Cl, 35.5 ; Zn, 65 ; NA = 6.02 x 1023]

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mohd faisol mansor/chemistry form 4/chapter 3

4. What is the mass of carbon that contains 6.02 x 1023 carbon atoms?

5. What is the mass of
a) 0.01 mol of ammonia gas, NH3?
b) 6.02 x 1024 nitrogen molecules, N2?

6. How many moles of molecules are there in 2.8 g of carbon monoxide, CO?

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mohd faisol mansor/chemistry form 4/chapter 3

Example 3

1. What is the volume of 1.2 mol of ammonia gas, NH3 at STP?
[Molar volume: 22.4 dm3 mol-1]

2. How many moles of ammonia gas, NH3 are present in 600 cm3 of the gas
measured at room conditions? [molar volume: 24 dm3 mol-1]

3. Calculate the volume of the following gases.
a) 0.3 mol of oxygen gas, O2, at room condition.

b) 4 mol of helium gas measured at STP.

4. Calculate the number of moles of 48 dm3 of chlorine gas, Cl2, at room
condition.

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mohd faisol mansor/chemistry form 4/chapter 3

Example 4

1. What is the volume of 12.8 g of oxygen gas, O2, in cm3, at STP?
[RAM: O, 16 ; Molar volume: 22.4 dm3 mol-1]

2. How many molecules of carbon dioxide, CO2, are produced when 120 cm3 of
the gas is released during chemical reaction between an acid and a
carbonate at room conditions?
[Molar volume: 24 dm3 mol-1 ; NA = 6.02 x 1023]

3. What is the mass of 0.6 dm3 of chlorine gas, Cl2 at room condition?
[RAM: Cl, 35.5 ; Molar volume = 24 dm3 mol-1]

4. 3 dm3 of an unknown gas has a mass of 6.0 g at room conditions. Find the
molar mass of the gas.

30

mohd faisol mansor/chemistry form 4/chapter 3

CHEMICAL FORMULAE Magnesium Nitrate Water

A representation Mg(NO3)2 H2O
of a chemical
substance using [state the number of particles consist in the substance above]
letters and
Compound Molecular Empirical n
subscript numbers. Formula Formula 2

Empirical Formula Water H2O CH2
The simplest Ethene

number ratio of Glucose C6H12O6
atoms in the
compound.

Molecular Formula = (Empirical Formula)n

Molecular Formula RMM of Molecular Formula
RMM of Empirical Formula = n
The actual number
of atoms that are The empirical formula of a compound
is CH2. Its relative molecular mass is 42.
present in the
compound. Find its molecular formula.

[RAM: H, 1 ; C, 12]

Copper(II) Oxide

Magnesium Oxide

31

mohd faisol mansor/chemistry form 4/chapter 3

To determine Empirical Formulae of Magnesium Oxide

1. Why is the magnesium ribbon cleaned with
sand paper before used?

2. Name the white fumes produced.
3. State the reason:

a) covering the crucible with its lid as soon as
the magnesium start burning.

b) raising the lid of the crucible at intervals
during heating.

c) heating, cooling & weighing are repeated
until constant mass is obtained.

4. Why is it important not to let any white fumes
escape from the crucible?

To determine Empirical Formulae of Copper(II) Oxide

1. Why do we start off with copper(II) oxide instead of allowing copper to react with
oxygen in the air in this experiment?

2. How do you test that the air in the tube has been removed completely?
3. Explain what will happen if we burn excess hydrogen gas without removing the air

completely in combustion tube?
4. Why we need to continue the flow of hydrogen gas after the heating of copper(II)

oxide?
5. Why do we need to repeat heating, cooling and weighing until constant mass is

obtained?

32

mohd faisol mansor/chemistry form 4/chapter 3

Example 1

a) A sample of aluminium oxide contains 1.08 g of aluminium and 0.96 g of
oxygen. What is the empirical formula of this compound? [RAM: O, 16 ; Al, 27]

Element Al O
Mass of Element (g)

Number of Mole

Ratio of Mole
Simplest Ratio

Empirical Formula of Aluminium Oxide =

b) 0.20 g of calcium reacts with fluorine to give 0.39 g of calcium fluoride. Find
the empirical formula of the calcium fluoride produced. [RAM: F, 19 ; Ca, 40]

33

mohd faisol mansor/chemistry form 4/chapter 3

c) Find the empirical formula of a compound that consists of 32.4% of sodium,
22.6% of sulphur and 45.0% of oxygen. [RAM: O, 16, Na, 23 ; S, 32]

d) 60 g of aluminium sulphide contains 38.4 g of sulphur. Find the empirical
formula of the compound. [RAM: Al, 27 ; S, 32]

34

mohd faisol mansor/chemistry form 4/chapter 3

Example 2

a) Butane has empirical formula of C2H5 and relative molecular mass of 58. Find
its molecular formula.

b) Ethanoic acid is an important ingredient of vinegar. The empirical formula of
this acid is CH2O. Given that its molar mass is 60 g mol-1, find its molecular
formula.

c) 6.24 g of element X combines with 1.28 g of oxygen to produce a compound
with an empirical formula of X2O. What is relative atomic mass of X?
[RAM: O, 16]

35

mohd faisol mansor/chemistry form 4/chapter 3

d) Element Y react with oxygen to produce a compound with molecular
formula YO3. Given that the mass of 1 mol of the compound is 80 g.
Determine the relative atomic mass of element Y.

e) Determine the percentage composition by mass of water in hydrated
copper(II) sulphate, CuSO4.5H2O. [RAM: H, 1 ; O, 16 ; S, 32 ; Cu, 64]

f) Due to its high nitrogen content, urea, CO(NH2)2 is commercially used as
fertilizers. Calculate the percentage composition by mass of nitrogen in urea,
CO(NH2)2. [RAM: H, 1 ; C, 12 ; N, 14 ;O, 16]

36

mohd faisol mansor/chemistry form 4/chapter 3

Metal Cation IONIC Ionic
Atom (+ve ion) COMPOUND Formulae

Nonmetal Anion
Atom (-ve ion)

Zinc Zn2+ Zinc Oxide Ionic
Zn O2- ZnO Formulae

Oxygen Silver Ionic
O Chloride Formulae

Silver

Chlorine

37

mohd faisol mansor/chemistry form 4/chapter 3

Charge Name of Cation Formula of Cation
1+
Hydrogen ion H+
2+ Lithium ion Li +
3+ Sodium ion Na +
K+
Potassium ion Ag +
Silver ion NH4 +
Ba 2+
Ammonium ion Ca 2+
Barium ion Mg 2+
Calcium ion Zn 2+
Cu 2+
Magnesium ion Fe 2+
Zinc ion Pb 2+
Al 3+
Copper(II) ion
Iron(II) ion Fe 3+
Lead(II) ion

Aluminium ion

Iron(III) ion

Charge Name of Anion Formula of Anion
1-
Hydroxide ion OH -
2- Chloride ion Cl -
3- Fluoride ion F-
Bromide ion Br -
I-
Iodide ion NO3 -
Nitrate ion O 2-
Oxide ion SO4 2-
Sulphate ion CO3 2-
Carbonate ion PO4 3-
Phosphate ion

38

mohd faisol mansor/chemistry form 4/chapter 3

Name of Cation Formula of Name of Cation Formula of
Cation Cation
Hydrogen ion Hydrogen ion
Lithium ion Formula of Magnesium ion Formula of
Sodium ion Anion Anion
Barium ion
Potassium ion Potassium ion
Silver ion
Iron(II) ion
Ammonium ion Ammonium ion
Barium ion
Calcium ion Zinc ion
Aluminium ion
Magnesium ion
Zinc ion Lithium ion
Iron(III) ion
Copper(II) ion Sodium ion
Iron(II) ion Calcium ion
Lead(II) ion Silver ion

Aluminium ion Copper(II) ion
Lead(II) ion
Iron(III) ion
Name of Anion
Name of Anion
Phosphate ion
Hydroxide ion Bromide ion
Chloride ion Oxide ion
Fluoride ion
Bromide ion Carbonate ion
Iodide ion
Iodide ion
Nitrate ion Chloride ion
Oxide ion Sulphate ion
Sulphate ion
Carbonate ion Nitrate ion
Phosphate ion Hydroxide ion

Fluoride ion

39

mohd faisol mansor/chemistry form 4/chapter 3

Name of Cation Formula of Name of Cation Formula of
Cation Cation
Hydrogen ion Hydrogen ion
Lithium ion Formula of Lithium ion Formula of
Sodium ion Anion Sodium ion Anion

Potassium ion Potassium ion 40
Silver ion Silver ion

Ammonium ion Ammonium ion
Barium ion Barium ion
Calcium ion Calcium ion

Magnesium ion Magnesium ion
Zinc ion Zinc ion

Copper(II) ion Copper(II) ion
Iron(II) ion Iron(II) ion
Lead(II) ion
Aluminium ion
Aluminium ion Iron(III) ion

Iron(III) ion Lead(II) ion

Name of Anion Name of Anion

Hydroxide ion Hydroxide ion
Chloride ion Chloride ion
Fluoride ion Fluoride ion
Bromide ion Bromide ion

Iodide ion Iodide ion
Nitrate ion Nitrate ion
Oxide ion Oxide ion
Sulphate ion Sulphate ion
Carbonate ion Carbonate ion
Phosphate ion Phosphate ion

mohd faisol mansor/chemistry form 4/chapter 3

Name of Cation Formula of Name of Cation Formula of
Cation Cation
Hydrogen ion Hydrogen ion
Lithium ion Formula of Lithium ion Formula of
Sodium ion Anion Sodium ion Anion

Potassium ion Potassium ion 41
Silver ion Silver ion

Ammonium ion Ammonium ion
Barium ion Barium ion
Calcium ion Calcium ion

Magnesium ion Magnesium ion
Zinc ion Zinc ion

Copper(II) ion Copper(II) ion
Iron(II) ion Iron(II) ion
Lead(II) ion
Aluminium ion
Aluminium ion Iron(III) ion

Iron(III) ion Lead(II) ion

Name of Anion Name of Anion

Hydroxide ion Hydroxide ion
Chloride ion Chloride ion
Fluoride ion Fluoride ion
Bromide ion Bromide ion

Iodide ion Iodide ion
Nitrate ion Nitrate ion
Oxide ion Oxide ion
Sulphate ion Sulphate ion
Carbonate ion Carbonate ion
Phosphate ion Phosphate ion

mohd faisol mansor/chemistry form 4/chapter 3

Example

Construct the chemical formula for each of the following ionic compound.

a)Magnesium hydroxide b) Silver iodide c) Potassium Bromide

d) Zinc nitrate e) Sodium carbonate f) Aluminium oxide

g) Copper(II) iodide h) Iron(II) sulphate i) Magnesium oxide

j)Calcium carbonate l) Ammonium phosphate m) Sodium hydroxide

n) Zinc bromide o) Lead(II) nitrate p) copper(II) sulphate

42

mohd faisol mansor/chemistry form 4/chapter 3

Example

1. Write the formula of the following substances.

a) Potassium iodide = 1) Nitric acid =

b) Magnesium oxide = 2) Lead(II) iodide =

c) Carbon dioxide = 3) Copper(II) nitrate =

d) Copper(II) oxide = 4) Zinc sulphate =

e) Lead(II) bromide = 5) Iron(II) chloride =

f) Calcium chloride = 6) Iron(III) chloride =

g) Hydrochloric acid = 7) Chlorine gas =

h) Copper(II) sulphate = 8) Potasium nitrate =

i) Hydrogen gas = 9) Silver nitrate =

j) Water = 10) Magnesium bromide =

k) Sulphuric acid = 11) Zinc chloride =

l) Silver chloride = 12) Sodium hydroxide =

m) Potassium nitrate = 13) Ammonia =

n) Calcium carbonate = 14) Iron(II) sulphate =

o) Aluminium oxide = 15) Lead(II) oxide =

p) Oxygen gas = 16) Carbon monoxide =

q) Oleum = 17) Magnesium sulphate =

r) Ammonium sulphate = 18) Ammonium nitrate =

s) Sodium chloride = 19) Potassium hydroxide =

t) Zinc oxide = 20) Lithium oxide =

43

mohd faisol mansor/chemistry form 4/chapter 3

Example

1. Write the formula of the following substances.

a) Potassium iodide = 1) Nitric acid =

b) Magnesium oxide = 2) Lead(II) iodide =

c) Carbon dioxide = 3) Copper(II) nitrate =

d) Copper(II) oxide = 4) Zinc sulphate =

e) Lead(II) bromide = 5) Iron(II) chloride =

f) Calcium chloride = 6) Iron(III) chloride =

g) Hydrochloric acid = 7) Chlorine gas =

h) Copper(II) sulphate = 8) Potasium nitrate =

i) Hydrogen gas = 9) Silver nitrate =

j) Water = 10) Magnesium bromide =

k) Sulphuric acid = 11) Zinc chloride =

l) Silver chloride = 12) Sodium hydroxide =

m) Potassium nitrate = 13) Ammonia =

n) Calcium carbonate = 14) Iron(II) sulphate =

o) Aluminium oxide = 15) Lead(II) oxide =

p) Oxygen gas = 16) Carbon monoxide =

q) Oleum = 17) Magnesium sulphate =

r) Ammonium sulphate = 18) Ammonium nitrate =

s) Sodium chloride = 19) Potassium hydroxide =

t) Zinc oxide = 20) Lithium oxide =

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mohd faisol mansor/chemistry form 4/chapter 3

Example

1. Write the formula of the following substances.

a) Potassium iodide = 1) Nitric acid =

b) Magnesium oxide = 2) Lead(II) iodide =

c) Carbon dioxide = 3) Copper(II) nitrate =

d) Copper(II) oxide = 4) Zinc sulphate =

e) Lead(II) bromide = 5) Iron(II) chloride =

f) Calcium chloride = 6) Iron(III) chloride =

g) Hydrochloric acid = 7) Chlorine gas =

h) Copper(II) sulphate = 8) Potasium nitrate =

i) Hydrogen gas = 9) Silver nitrate =

j) Water = 10) Magnesium bromide =

k) Sulphuric acid = 11) Zinc chloride =

l) Silver chloride = 12) Sodium hydroxide =

m) Potassium nitrate = 13) Ammonia =

n) Calcium carbonate = 14) Iron(II) sulphate =

o) Aluminium oxide = 15) Lead(II) oxide =

p) Oxygen gas = 16) Carbon monoxide =

q) Oleum = 17) Magnesium sulphate =

r) Ammonium sulphate = 18) Ammonium nitrate =

s) Sodium chloride = 19) Potassium hydroxide =

t) Zinc oxide = 20) Lithium oxide =

45

mohd faisol mansor/chemistry form 4/chapter 3

Example

Name the following ionic compound by using their IUPAC name.

Ionic Name Ionic Name
Formula Formula

NaCl KI
MgO BaSO4
Cu(NO3)2 CaCO3
Al2O3 FeCl3
ZnCl2 LiOH
CuO FeSO4
AgNO3 NaOH
MgBr2
PbSO4 ZnO
PbI2

NaBr Br -
Bromide
Na +
Sodium

Sodium Bromide

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mohd faisol mansor/chemistry form 4/chapter 3

CHEMICAL EQUATIONS

a) Qualitative Aspect

K(S) + H2O(l) KOH(aq) + H2(g)

Reactant Product

Meaning: Solid Potassium react with water liquid to give
potassium hydroxide solution and hydrogen gas

p/s: 1) Able to classify reactant and product.
2) Able to balance the equation.

Example 1

For each equation, identify the reactant(s), product(s) and the state of each
of them. Then, balance the equation.

a) H2 (g) + O2 (g) H2O (l)

b) CuO (s) + HCl (aq) CuCl2 (aq) + H2O (l)

c) Cl2 (g) + NaBr (aq) NaCl (aq) + Br2 (l)

d) Mg (s) + HCl (aq) MgCl2 (aq) + H2 (g)

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mohd faisol mansor/chemistry form 4/chapter 3

Example 2

Write a balanced equation for each of the following reactions.

a) Carbon monoxide gas + oxygen gas Carbon dioxide gas

b) Hydrogen gas + nitrogen gas Ammonia gas

c) Aluminium + iron(III) oxide Aluminium oxide + iron

d) Ammonia gas react with oxygen gas to yield nitrogen monoxide gas and
water.

e) Silver nitrate solution is added to calcium chloride solution. Silver chloride
precipitate and calcium nitrate solution are produced.

f) When solid zinc carbonate is heated, it decomposes into zinc oxide powder
and carbon dioxide gas.

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