This document discusses matter and substances. It describes the kinetic theory of matter and states of matter. It explains that all matter is made up of atoms, which contain protons, electrons, and neutrons. The periodic table arranges elements based on proton number and displays their properties. Substances can be made of atoms, molecules, or ions, which determines their physical properties like melting point and electrical conductivity. Metals have properties like shine, malleability, and conductivity, while non-metals have dull surfaces and are brittle. Purification methods like filtration, crystallization, and distillation are used to obtain pure substances. Substances are important in daily life, and their properties allow them to be processed for different uses.

1. Chapter 4
Matter and Substances

2. 4.1 Changes In Matter
Kinetic Theory of Matter
The theory states that:
- Matter is made up of tiny and discrete
particles
- The particles are always moving in
random motion
- The moving energy is called the kinetic
energy of particles
- The kinetic energy of particles depends
on the temperature of matter

3. States of Matter

4. Changes in state of matter
Sublimation
Sublimation

5. 4.2 Structure of atom
Every substances is made up of atoms.
2. There are three types of subatomic
particles: proton, electron and neutron.
1.
(e, negatively charged)
(p, positively charged)
(n, neutral/ no charged)

6. 4.3 Proton number and Nucleon
number
Proton number is the number of proton in an
atom.
 Nucleon number is the total number of
protons and neutrons in an atom.

The number of nucleon = neutrons number +
proton number
• Symbol of element.
For example, Aluminium (Al)
Proton number
(always smaller number)
Nucleon number
13
27
Al
Name of element

7. How to determine the charges of
particles
Particles
A
Number of
protons
6
Number of
electrons
8
B
C
10
11
9
11
a) Positively charged particles: B ( more proton number)
b) Negatively charged particles: A (more electron number)
c) Particle that has no charge (neutral): C (proton = electro

8. Isotopes
Isotopes of certain elements contains the
same number of protons but a different
number of neutrons in their atoms.
 For example, hydrogen


9. 4.4 Periodic table
•Elements are arranged according to their proton number (increases)
•Divided into metals, non-metals and semimetals
•Elements in the same group have same chemical properties

10. Importance of periodic table
Helps us to determine the properties
of elements.
 Can be used to forecast the properties
and uses of particular element.


11. 4.5 Properties of Substances
ATOMS
MOLECULES
IONS
•Substances made up of
atoms only.
•The smallest particle.
Substance made up of
molecules only (two or
more atoms).
•Substance made up of
ions only.
•Contain charged particle
•In solid (except mercury)
•Conduct electricity
•High boiling/melting point
•In solid, liquid or gas
•Cannot conduct
electricity
•Low boiling/melting point
•In solid
•Cannot conduct electricity
except in molten or
aqueous states
•High boiling/melting point
ALUMINIUM
Oxygen gas
Aluminiu
m
Water
Sodium chloride (NaCl)

12. Physical properties of substance made
up of atoms, molecules and ions
Section A: Melting
point.
Type of
substance
Melting
point
Lead
ATOM
High
Sulphur
Lead/sulphur/
Lead(II)bromide
Substance
s
MOLECULE Low
Lead (II)
Bromide
ION
High
•High melting point = strong forces of
attraction
•Low melting point = weak forces of
attraction

13. Section B: Electrical conductivity
SUBSTANCE
ELECTRICAL CONDUCTIVITY
SOLID
MOLTEN
LEAD
Can
Can
SULPHUR
Cannot
Cannot
LEAD(II)BROMID Cannot
E
Can
For ionic substance, lead(II)bromide:
•Does not conduct electricity in solid becaus
- ions cannot move freely
•Conducts electricity in molten because
- ions can move freely

14. 4.6 Properties of Metals and NonMetals
A) Surface condition
Metals: copper
Shiny surface
Dull
Non-metals: carbon

15. B) Malleability
•Non-metal: Brittle
• the lump of carbon shatters
•Metal :Malleable
• iron wire changes shape

16. C) Tensile
strength
Nichrome/
nylon
Nichrome (metal)
needed
more weights to
break
Nylon (non-metal)
needed
less weight to
break
Metals have higher tensile strength than non-metals

17. D) Electrical conductivity
* Metals: the bulb
lights up with
copper rod
* METALS conduct
electricity
* Non-metals:
the bulb does
not lights up with
glass rod
* NON-METALS
do not conduct
electricity

18. E) Heat
conductivity
Type of
Example Time taken
materials
for the
thumbtack
to drop
off/second
s
METALS
Copper
rod
96
NONMETALS
Glass rod 130
•Metals: copper rod are good heat conductors
•Non-metals: glass rod are poor heat conductors

19. 4.6 Properties of Metals and Non-Metals
Comparison between metals and non-metals
METALS
Physical properties
NON-METALS
Shiny
Surface
Dull
Ductile
Ductility
Non-ductile/ brittle
Malleable
Malleability
Non-malleable
High
Low
Good
Melting and Boiling
point
Electrical conductivity
Good
Heat conductivity
Poor
High
Tensile strenght
Low
Non-conductive
except carbon

20. Uses of metals
Iron is
used in
making
cars
Copper is used
to make wires
Silver is
often used
to make
jewellery
Aluminium is
used to make
power lines

21. Uses of non-metals
Sulphur is
used to
make
matchstick
tips
Diamonds are
mostly used to
make
jewellery
Sulphur is
ingredient in
making paint

22. 4.7 Purification of Substances
1.
2.
Pure substances are substances that
contain only one type of substance.
- do not have any impurities
- for example,
* pure sugar only contains sugar
molecules
* pure water only contains water
molecules
Pure substances have fixed boiling and
melting point.
- for example,
* pure water boils at 100°C

23. Effect of impurities on the boiling point
of a pure liquid

•
The presence of impurities in a pure
substance can
a) increase its boiling point
b) decrease its freezing point
For example,
- when a salt is added to pure water,
water will be boil at a temperature
higher than 100°C

24. Title: Effect of impurities on the boiling
point of a pure liquid
(PEKA)
Aim: To study the effect of impurities on the
boiling
point.
 Hypothesis: The presence of salt increases the
boiling point of a pure liquid
 Variables:
manipulated variable
:
responding variable
:
constant variable :
 Materials: distilled water, table salt
 Apparatus: 100cm³beaker, wire gauze, tripod
stand, Bunsen burner,
thermomater


25. 
Procedure:
Salt
Distilled
water
1. Distilled water was filled into a
beaker until it is half full.
2. The water was heated until its
boils. The temperature was
recorded.
3. Two spatulas of table salt
were
added into the distilled water
and the mixture was heated
again.
4. The boiling point of the
mixture
of water and table salt were
recorded.

26. 
Results :
• Conclusion:
Boiling point of
distilled water (°C)
Absent
Present
• Analysis:
The presence of
table salt
100

27. Methods of purification
Purification is a process of removing impurities
from a substance.
 The methods are:
a) Filtration: process of separating solid from liquid

Mixture of solid
and liquid
Filter paper
Residue (solid)
Filtrate (liquid)

28. b) Crystallisation : process of forming crystals
from a liquid or gas
- production of salt from sea water
- production of pure solid copper(II)sulphate
from its solution
Substance in crystal form

29. c) Distillation: a process to obtain a pure liquid from
a solution of liquid mixture.
- production of distilled water
- petroleum fractions (fractional distillation)
Tap water flows to cool the vapour and
condense it into liquid
To make sure the
condenser
is fully filled with water
Porcelin chips:
To break up the
air bubbles

30. Fractional distillation

31. 4.8 Uses of various
substances
Humans need various types of substances
in daily life.
 With scientific knowledge and technology,
humans have used the properties of
substances to make their lives better.
 For example, pure metals which may not
be suitable for a particular purpose
because they are too heavy or rust easily.
- they can be processed into more suitable
substances.
- pure iron
steel (strong and does not
rust)


32. SCIENCE PROCESS SKILL
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 SPM ENHANCEMENT CORNER/
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