01 matter-new2016

LESSONCONTENTS
2
1. What is matter?
2. Nature of matter : Structure of atom, molecules
3. Chemical elements and compounds
4. The three states of matter
5. Changes between states
copyright @ yuradia-MATA-2011

INTRODUCTION
3
 Physics is the study of both matter and energy,
in an attempt to understand how the physical
world around us works.
 Matter is what everything is made of. Matter
can be defined as anything that occupies space
and has mass.

INTRODUCTION
4
 Matter can be either a solid, liquid or gaseous state. Any
substance made from matter will take one one of these
form.
 However, substances can readily change states with the
addition or removal of energy.
 An example of this is water, which is at room
temperature is liquid, but becomes a solid (ice) when
cooled (energy removed) but also can become a gas
(steam) when heated (energy added).copyright @ yuradia-MATA-2011

WATER - MATTER
 CHANGE FROM ONE STATE TO
ANOTHER
 TEMPERATURE IS THE DOMINENT
FACTOR
 AT HIGH TEMPERATURE – GASES
 AT MODERATE TEMP. - LIQUID
 AT LOW TEMP. - SOLID ( ICE )
5 copyright @ yuradia-MATA-2011

ICE
WATER
GAS
HIGH TEMP
MODERATE TEMP
LOW TEMP

WHAT IS MATTER?
7
1. Matter - anything that occupies space and has
mass.
2. It includes everything around us ; the foot we
eat, the water we drink, the air we breathe, the
aircraft we fly, as well as the atmosphere.
3. Matter takes up space. So matter has volume.
Conservation of Matter
Matter cannot be created or destroyed, however we
can change the characteristics of matter.

Chemical nature of matter
8
1. When we break matter down into its
fundamental form we see that it is composed
of the basic building blocks of the universe.
2. Atom is the smallest unit that can exist. An
atom has a nucleus, consisting of protons and
neutrons, and layers of orbiting electrons.

9
3. Electron, protons and neutron are called sub-atomic
particles.

THE NUCLEUS
12
1. At the centre of the atom and contains protons and
neutrons.
2. Most of the mass of an atom comes from the
nucleus.
3. Protons and neutrons collectively known as
nucleons

ELECTRONS
13
 Electrons carry a negative charge of the same
magnitude as the proton.
 Electrons are arranged in energy levels or
shells around the nucleus.
 Valence electrons :
- how many electrons an atom has in its
outer
shell.
- determines the chemical behavior.
- The more valence electrons, the more
want for
the atom to get more electrons.

ELECTRONS
14
Valency :
 bonding capacity of an atom; usually equals the
number of unpaired electrons in the atoms
outermost shell.
 No. of bonds it can make with a monovalent
atom such as Hydrogen.
Monovalent
Bivalent
Trivalent
Tetravalent

Chemical Elements
15
 A chemical element, or element for short, is
a type of atom that is defined by its atomic
number;
 Atomic number is the number of protons in its
nucleus.
 The term is also used to refer to a pure
chemical substance composed of atoms with
the same number of protons.

Chemical Elements
16
 An element consists of only one kind of
atom.
 Common examples of elements are
hydrogen, nitrogen, and carbon.
 Chemical element can be found in the
PERIODIC TABLE. Scientifically, there are
92 naturally occurring element inside the
table. The rest are man made. A simple
Periodic Table gives information about
Proton No .copyright @ yuradia-MATA-2011

The Periodic Table of An Element

18
 Atomic number represented by the symbol Z.
 Atomic number uniquely identifies chemical elements.
 In an atom of neutral charge, the number of electrons
also equals the atomic number.
 Atomic number is closely related to the mass number
(A).
 The mass number (A), also called atomic mass
number or nucleon number, is the number of nucleons
(protons and neutrons) in a nucleus .copyright @ yuradia-MATA-2011

20
 Example :
 The difference between the mass number and
the atomic number gives the number of neutrons
(n) in a given nucleus: n=A−Z.
.

238
92
238
Mass number
(# of protons +
# of neutrons)
Atomic
Number
( # of protons)
Symbol of
element:
Uranium
HINTS!!
• Mass number is the larger number between the two numbers shown
•# of neutrons is the difference between the two numbers

ISOTOPES
 Carbon-12 and Carbon-13 are isotopes
12
6
13
6
Same atomic number
 Isotopes are atoms which have same atomic number, Z
but different mass number, A.

Molecules and compounds
23
1. When atoms bond together they form a
molecule.
2. There are a few molecules that exist as single
atoms.
3. Example : Helium (He), argon (Ar) and
water (H2O).
4. When atoms bonds together to form a
molecule, they share electrons.

smallest particles of an element or compound
which can exist independently.
Example: Oxygen molecules (O2)
MOLECULES
Breaks into
2 oxygen
atoms

COMPOUND
• substances that are made when the atoms of two or
more different elements joined together chemically
• can be broken down into other substances
1 Hydrogen atom 2 Oxygen atoms
Breaks into
Example: Water (H2O)

The Molecule of Water

27
Chemical Compound
 If 2 or more different atoms are combined, a
chemically different substance is formed,
which is called a compound.
eg : H2O, HCL
A chemical compound is a chemical
substance consisting of two or more
different chemically bonded chemical
elements

28
Chemical Compound
Chemical compound can be :
 Ionic compound
 covalent compound

29
Chemical Compound
Covalent compound :
• bonds are formed via sharing electron
• These electrons are from the outer shell of an atom.
Ionic compound :
• valence electron moves from one atom to outer shell
of another atom.
• Atoms will become charged particles – ions
 +ve ions : cations – loss 1 or more electrons
 -ve ions : anions – gain 1 or more electrons
Notes : ionic compound will form ionic bonding &
covalent compound will form a
covalent bondingcopyright @ yuradia-MATA-2011

Covalent Bond
30
 Covalent bonding is a form of chemical
bonding that is characterized by the sharing of
pairs of electrons between atoms.
 Forms between atoms when they share
electrons.

Ionic Bond
 Ionic bonds are a type of chemical bond based on electrostatic
forces between two oppositely-charged ions.
 Example :

MIXTURE
 Mixture are of pure substances.
 Has the properties of the different
substances that make it up.
 Mixtures melt at a range of temperatures
and are easy to separate.

THE THREE STATES OF MATTER

Flow ability:
•Cannot flow
•Cannot be
compressed
Energy
content:
Low
Volume:
Fixed
Shape:
Fixed
Particles
arrangement:
Close to each
other
SOLID

SOLID
35
The properties of a solid
i. greatest density (heaviest) because the
particles are closest together.
ii. cannot flow freely like gases or liquids
because the particles are strongly held in
fixed positions.
iii. have fixed surface and volume (at a
particular temperature) because of the
strong particle attraction.

SOLID
36
The properties of a solid
iv. difficult to compress because there is no
real “empty” space between the particles.
v. will expand a little on heating but nothing
like as much as liquids because of the
greater particle attraction restricting the
expansion (contract on cooling). The
expansion is caused by the increased
strength of particle vibration.

Flow ability:
•Can flow
•Difficult to
compress
Energy
content:
Average
Volume:
Fixed
Shape:
Follows
container
Particles
arrangement:
Loosely
arranged
LIQUID

LIQUID
38
THE PROPERTIES OF A LIQUID
i. have a much greater density than gases
(heavier) because the particles are much closer
together.
ii. flow freely despite the forces of attraction
between the particles but liquids are not as fluid
as gases.
iii. have a surface, and a fixed volume (at a
particular temperature) because of the increased
particle attraction, but the shape is not fixed and
is merely that of the container itself.

LIQUID
39
THE PROPERTIES OF A LIQUID
iv. not readily compressed because of the lack of
empty space between the particles.
v. will expand on heating (contract on cooling) but
nothing like as much as gases because of the
greater particle attraction restricting the
expansion.
vi. When heated, the liquid particles gain kinetic
energy and hit the sides of the container more
frequently, and more significantly, they hit with a
greater force,so in a sealed container the
pressure produced can be considerable.copyright @ yuradia-MATA-2011

Flow ability:
•Can flow
•Easy to
compress
Energy
content:
High
Volume:
Not Fixed
Shape:
Follows
container
Particles
arrangement:
Very Loosely
arranged
GAS

GASEOUS
41
THE PROPERTIES OF A GAS
i. have a low density (light) because the particles
are so spaced out in the container (density =
Mass ÷Volume).
ii. flow freely because there are no effective forces
of attraction between the particles.
iii. have no surface, and no fixed shape or volume,
and because of lack of particle attraction, they
spread out and fill any container.
iv. readily compressed because of the empty space
between the particles.

GASEOUS
42
THE PROPERTIES OF A GAS
iv. If the container volume can change, gases readily expand
on heating because of the lack of particle attraction, and
readily contract on cooling. On heating, gas particles gain
kinetic energy and hit the sides of the container more
frequently, and more significantly, they hit with a greater
force. Depending on the container situation, either or both
of the pressure or volume will increase (reverse on
cooling).
v. The natural rapid and random movement of the particles
means that gases readily spread or diffuse. Diffusion is
fastest in gases where there is more space for them to
move and the rate of diffusion increases with increase
temperature.

CHANGES BETWEENSTATES

Physical vs. Chemical Changes
48
 Physical changes are about energy and states of
matter.
 Chemical changes happen on a molecular level.
 Example when you step on a can, you have forced a
physical change. The shape of the object has changed.
It wasn't a change in the state of matter.
 When you melt an ice cube you have also forced a
physical change (adding energy) .That caused a
change in the state of matter. You can cause physical
changes with forces like motion, temperature, and
pressure.

49
 Chemical changes happen on a much smaller scale.
Example changes in colour .
 Most chemical changes happen between molecules
and are unseen. When iron (Fe) rusts you can see it
happen over a long period of time. The actual
molecules have changed their structure (the iron
oxidized).
 Melting a sugar cube is a physical change because the
substance is still sugar.
 Burning a sugar cube is a chemical change. The
energy of the fire has broken down the chemical
bonds.

01 matter-new2016

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