All matter is particulate in nature. This simply means that matter is made up of tiny bit bits material known as particle.

1. All matter is particulate in nature. This
simply means that matter is made up of
tiny bit bits material known as particle.
THE PARTICLE NATURE OF MATTER

2. Matter is composed of particle and was
conceived by Democritus, a Greek
Philosopher.
Democritus named the particle atom from
the Greek word atomos, meaning
indivisible.

3. LOOP ACTIVITY

4. ACTIVITY 9.1
I. Objectives:
 describe the characteristics of a material
 Illustrate the particle making up the material
II. Materials
Aluminum foil
Pencil
Water
microscope

5. STATE OF MATTER AND THEIR
PROPERTIES
matter-anything that occupies space
and has mass
• Mass is the fundamental property of
matter.

6. STATE OF MATTER
• Solid
• Liquid and
• Gas
• Plasma
• Molecules, compared to atom is large particle formed
by the combination of two or more atoms.

7. ARRANGEMENT OF MOLECULES OF THE 3
STATES OF MATTER

8. THE KINETIC MOLECULAR THEORY
OF MATTER
• All matter, be it in solid, liquid, or gas
stated, are made up of tiny particles
known as atoms.
• Particles are in constant, random motion.
• Particles in motion have kinetic energy,
and their motion increases as they gain
energy.

9. • There is a transfer of energy between
particles (atoms molecules) as these
particles collide with each other.
• Collisions between these particles are
perfectly elastic.
• Molecular motion is greatest in gases,
less in liquids, and least in solids.

10. • Kinetic Molecular theory is very useful
in explaining why the states of matter
differ in movements and arrangement.
• Intramolecular forces-the attractive
forces that hold particles together.
• Intra-means “within”

11. • Intermolecular forces- forces of attraction,
inter- means “between” and “ among”.
• Intermolecular forces can hold together
identical particles such as water particles in
a drop of water, or two different types of
particles, such as carbon in graphite, and
the cellulose particles in paper.

12. PROPERTIES OF SOLID
1. Density
Density is the ratio of mass per unit volume. Solid
have greater density than liquids and gases.
2.Crystalline solids
The individual pieces of crystalline solids are called
crystals.
Crystalline solids is a solid whose atoms, ions, or
molecules are arranged in an orderly, geometric, 3
dimensional structure.

13. 3. Metallic solids
Metallic solids consist of positive metal ions
surrounded by a sea of mobile electrons.
4. Amorphous solids
Not all solids contain crystals. An amorphous
solid is one in which the particles are not
arranged in a regular,repeating pattern.
Amorphous means “without shape”
Ex. Glass, rubber, and plastic

14. PROPERTIES OF LIQUIDS
1. Fluidity
Fluidity is the ability to flow. Gases and liquids are classified
as fluids because they can flow.
2. Viscosity
Viscosity is a measure of the resistance of a liquid to flow.
The particles in liquid are close enough for attractive forces
to slow the movement as they flow past one another.
3. Temperature
When there is an increase in temperature, there is an
increase in the kinetic energy.

15. 4. Surface tension
Surface tension is the energy required to
increase the surface area of a liquid by a
given amount. It is a measure of the
inward pull by particles in the interior.
5.Capillary Action
There are two forces at work : cohesion
and adhesion.
Cohesion is the force of attraction between
identical molecules.

16. • Adhesion is the force of
attraction between different
molecules.
• The adhesive force between
the molecules and the silicon
dioxide in the glass is greater
than the cohesive forces
between the water molecules.
• If the narrow tube are used,
then the action is called
capillary action or capillary.

17. 6. Density
Liquids have densities that vary. The
density of a liquid with a constant
volume varies according to the weight.
The greater the weight, the higher the
density.

18. PROPERTIES OF GASES
1. Volume
Gases do not have definite volume. This means that a gas will fill
whatever volume is available. The space is where the molecules
move freely.
The volume of gas is measure using calibrated tube called
burrette.
2. Pressure
Gas molecules are in continuous motion and they frequently
strike the walls of their container.
The movement of the molecules exerts a force over the area
known as pressure.

20. The SI unit pressure is pascal (Pa) and the
instrument used to measure it is known as
barometer. Other units used are atmosphere
(atm) and torr.
3. Temperature
An important property of gas is temperature. It
is a measure of the average kinetic energy of
particles in matter. An increase in temperature
causes a gas to expand, thus increasing its
volume.

21. PLASMA- THE 4TH STATE OF
MATTER
• Plasma-It is a hot ionized gas that allows
both positive charged ion and a negative
charged electron to coexist.
• Plasma is strongly influenced by electric
and magnetic fields.
• 98% of matter in the universe is in
plasma state.
• -occurs in lightning volts, auroras, and
fluorescent light.

22. ARRANGEMENT OF MOLECULES FROM SOLID TO
PLASMA

23. OTHER STATES OF MATTER
• BOSE-EINSTEIN CONDENSATE (BEC)
represents the 5th state of matter beyond solid.
• BEC was predicted by Albert Einstein and
Satyendra Nath Bose, and the concept of BEC
in gas was realized by Eric Cornell and Carl
Wieman in 1995
• Scientist refrigerated particles called bosons in
a very low temperature.

24. • Cold boson merge to form a single
super particle that is more like a wave
than an ordinary speck of matter.
• BEC are fragile , and light travels very
slowly through them.
• BECs behave in a more orderly manner
than solids. Atoms in solids are locked
into roughly the same location with
regards to other atoms.

25. SIXTH STATE OF MATTER
• A new form of matter called fermionic
condensate was discovered by NASA-
supported researcher physicists, Deborah Jin –
lead scientist who produced the first fermionic
condensate in Dec. 2003.
• -by cooling a cloud of 500,00 potassium- 40
atoms to less than millionth of a degree above
absolute zero.
• Fermionic condensate and BECs are related.

26. LESSON 2

27. Explain physical changes in terms
of arrangement and motion of
atoms and molecules.
Use the particulate of matter to
explain melting, freezing,
evaporation, and condensation.
FOCUS
POINTS

28. PHASE CHANGES IN A WATER
CYCLE

29. PHASE CHANGES THAT
REQUIRE ENERGY

30. MELTING
• Solid to liquid

31. VAPORIZATION
• Vaporization- Is the process by
which liquid changes to gas or
vapor.
• Evaporation- when vaporization
occurs only on the surface of a
liquid.

32. EVAPORIZATION

33. SUBLIMATION- SOLID TO GAS

34. PHASE CHANGES THAT RELEASE
ENERGY

35. CONDENSATION
- Gas or a vapor become liquid

36. FREEZING
(Reverse of melting) Liquid to solid
The freezing point is the temperature
at which liquid is changed into
crystalline solid.

37. DEPOSITION
• -Process which gas or vapor change
into solid.
• When water vapor comes in contact
with a cold window glass in winter, it
forms a solid deposit on the window
glass cold frost.

38. Is a graph of pressure versus
temperature that shows in which
phase a substance exists under
different conditions of temperature
and pressure.
PHASE DIAGRAM

39. PHASE DIAGRAM