Here are some common methods used to separate mixtures: 1. Sifting - Used to separate mixtures where components differ in size, such as separating sand and gravel. The smaller particles pass through the mesh, while larger ones are retained. 2. Magnetic separation - Used to separate mixtures where one component is magnetic, such as separating iron filings from sand. A magnet attracts and retains the magnetic component. 3. Filtration - Used to separate mixtures where components differ in physical state, such as separating solids from liquids. The liquid passes through the filter, while solids are retained. 4. Centrifugation - Used to separate mixtures where components differ in density, such as separating cream from milk. Spin

1. Prepared by:
Mrs. Eden C. Sanchez
SHS Teacher

2. The Particulate Nature of Matter
 Atoms—the particles that make up all matter—vary in
their subatomic composition.
 The number and arrangement of an atom's particles
(neutrons, protons, and electrons) determines the
properties of the atom.
 The behavior and interactions of atoms and molecules
within a substance determine its physical state.
 Greek philosopher Leucippus and his student
Democritus were the first to propose the idea of atom
about 440 B.C

3. States of Matter
 Gases, liquids, and especially solids surround us and
give form to our world. Chemistry at its most
fundamental level is about atoms and the forces that
act between them to form larger structural units. Let
us see how these macroscopic properties of matter
depend on the microscopic particles of which it is
composed.
 Gases, liquids and solids are all made up of atoms,
molecules, and/or ions, but the behaviors of these
particles differ in the three phases.

4.  The molecular units of crystalline solids tend to be
highly ordered, with each unit occupying a fixed
position with respect to the others.
 In liquids, the molecules are able to slip around each
other, introducing an element of disorder and creating
some void spaces that decrease the density.
 Gases present a picture of almost total disorder, with
practically no restrictions on where any one molecule
can be.

5. Note that:
Particles in a:
 gas are well separated with no regular arrangement.
 liquid are close together with no regular arrangement.
 solid are tightly packed, usually in a regular pattern.
Particles in a:
 gas vibrate and move freely at high speeds.
 liquid vibrate, move about, and slide past each other.
 solid vibrate (jiggle) but generally do not move from
place to place.

6. Differences in Particle Properties of the Three
Phases of Matter
Property Solid Liquid Gas
Arrangement
of Particles
Particles are
tightly packed
with ordered
arrangement
Particles have a
disordered
arrangement
Particles have
totally
disordered
arrangement
Relative
Spacing
between
Particles
Particles are
close to one
another
Particles are
slightly close to
one another
Particles are far
apart
Relative
Motion of
Particles
Particles are
essentially in
fixed position
Particles are free
to move, relative
to other particles
Particles have
complete
freedom of
motion

7.  Liquids and solids are often referred to as condensed
phases because the particles are very close together.

8. Seatwork: Complete the data for the differences
in the three phases of matter.
Property Solid Liquid Gas
Compressibility
Density
Volume
Shape
Diffusion
Expansion

9. Differences in Particle Properties of the Three
Phases of Matter
Property Solid Liquid Gas
Compressibility Low
compressibility
Low
compressibility
Highly
compressible
Density high high Very low
Volume Retains own
volume
Definite volume Indefinite, fills
the container
Shape Retains own
shape
Assumes shape
of container
Assumes shape
of container
Diffusion Extremely slow slow rapid
Expansion Low expansion
on heating
Low expansion
on heating
High expansion
on heating

10. Some Characteristics of Gases, Liquids and Solids and
the Microscopic Explanation for the Behavior
Gas Liquid Solid
assumes the shape
and volume of its
container
particles can move
past one another
assumes the shape of the
part of the container
which it occupies
particles can move/slide
past one another
retains a fixed volume
and shape
rigid - particles locked
into place
compressible
lots of free space
between particles
not easily compressible
little free space between
particles
not easily compressible
little free space between
particles
flows easily
particles can move
past one another
flows easily
particles can move/slide
past one another
does not flow easily
rigid - particles cannot
move/slide past one
another

12. Identify the state of matter being described
1. It assumes the shape and volume of the entire
container it occupies
2. It has low density and high compressibility
3. It assumes the shape of the part of the container
which it occupies
4. The particles are very far apart with no regular
arrangement
5. The particles vibrate in place

13. Properties of Matter
 Can you categorize each image whether it is an
example of physical or chemical change?

15. Activity:
Categorize the following property of matter as
physical or chemical.
Color, texture, odor, size, volume, density, hardness,
melting point, boiling point, electrical and thermal
conductivities, change in state, albedo, angular
momentum, flammability, heat of combustion, toxicity,
oxidation, radioactivity, area, brittleness, capacitance,
concentration, ductility, viscosity, freezing pt.,
elasticity, length, mass, and solubility

16. Properties of Matter
 Physical Property – characteristic that can be
observed or measured without changing the identity
or composition of the substance.
 Examples: Color, texture, odor, size, volume, density,
hardness, melting point, boiling point, electrical and
thermal conductivities, change in state
 Some physical properties of a substance depend on the
condition such as pressure and temperature, under
which they are measured. Example is ice, liquid water
and steam

17. Common Physical Properties
 Albedo – reflecting power of a surface
 Angular momentum – amount of rotation of an object
 Area- amount of two dimensional surface in a plane
 Brittleness – tendency of a material to break under
stress
 Boiling point – temperature where a liquid forms
vapor
 Capacitance – ability of an object to store an electrical
charge
 Color- hue of an object as perceived by humans

18.  Concentration – amount of one substance in a mixture
 Density – mass per unit volume of a substance
 Ductility – ability of a substance to be stretched into a wire
 Elasticity – tendency of a material to return to its former
shape
 Electrical conductivity – a material’s ability to conduct
electricity
 Freezing point – temperature where a liquid solidifies
 Hardness – how resistant solid matter is to external force
 Length – longest dimension of an object

19.  Luster – the way light interacts with the surface of a
crystal, mineral or rock
 Malleability – ability to form a thin sheet by
hammering or rolling a material
 Mass – amount of an object, an object’s resistance to
being accelerated
 Melting point – temperature where a solid changes to a
liquid
 Smell- scent or odor of a substance
 Solubility – ability of a substance to dissolve

20.  Temperature – numerical measure of heat and cold
 Thermal conductivity – property of a material to
conduct heat
 Viscosity – resistance to flow
 Volume- space that a substance occupies
 Phase changes
 Physical properties are very important because these
help chemists in identifying substances

21.  Example: A clear, colorless liquid observed to a boil at
1000C and freeze at 00C
How can a chemist determine whether a colorless
gas is hydrogen or oxygen?
 Chemical Property – ability of a substance to
undergo changes to transform into a different
substance. It describes how a substance reacts with
another substance

22.  Examples: oxidation, flammability
 When a charcoal burns in the presence of oxygen in
the air to become a new substance, the physical
properties of the original substance disappear. A new
set of physical properties for the new substance is then
observed
 Internal qualities of a substance must be altered to
determine its chemical properties

23.  Flammability – how easily something will burn or ignite.
Information about flammability is used in building codes,
fire codes, insurance requirements, and storing, handling
and transporting highly flammable materials
 Heat of combustion – amount of energy that is released as
heat when a substance is burned with oxygen. Example:
calorie
 Toxicity – how much a substance can damage an animal,
plant, cell, organ or other organism is its toxicity. Materials
with toxicity include lead, chlorine gas, hydrofluoric acid
and mercury

24.  Oxidation – this is what takes place by gaining oxygen,
losing hydrogen or losing electrons, results in the
oxidation number of a substance being changed.
 Radioactivity – emission of radiation from an atom
with an unstable nucleus

25. Extensive & Intensive Properties
 Based on the effect of the amount of matter
 Extensive properties – depend on the amount of
matter present
 Examples: volume, mass, size, weight, length
 Intensive properties – do not depend on the amount
of matter present, depend on the kind of matter in a
sample
 Example: color, odor, density, boiling point, state of
matter, melting point, luster, hardness, ductility and
malleability

26. Physical and Chemical Change
 If the change in a substance alters the form but not the
composition of that substance, the change is then
called a physical change.
 Examples: when ice is heated, when salt dissolves in
water
 Chemical change or chemical reaction can only be
observed when the substance undergoes a change in
composition.
 Example: when a compound is formed between two or
more element

27.  The substances that transform or undergo chemical
reaction are called reactants.
 The substances that are formed are called products.
 Common signs of chemical change:
1. Bubbles of gas appear
2. Precipitate forms
3. An unexpected color change occurs
4. Gain or release of energy (heat or light)

28. Read each scenario. Decide whether a physical or
chemical change has occurred and give evidence for your
decision.
1. The student cuts a slice off the loaf and spreads
butter on it.
2. Your friend decides to toast a piece of bread, but
leaves it in the toaster too long. The bread is black
and the kitchen is full of smoke
3. You forgot to dry the bread knife when you washed
it, a reddish brown spots appeared on it.
4. A straight piece of wire is coiled to form a spring.
5. A piece of charcoal is crushed to a powder.

29. 6. Chewing food to break it down into smaller particles
represent a _______ change, but the changing of starch
into sugars by enzymes in the digestive system
represents a _______ change.

30. Classification of Matter
Pure Substance & Mixture

31. Mixture
 Is a physical blend of two or more components, each of
which retains its own identity and properties
 The parts or components of a mixture are simply
mixed together physically and can usually be separated
 The properties of a mixture are a combination of the
different properties of the components
 Salt solution is a mixture

32. Pure Substance
 Refers to a matter that cannot be separated into
simpler components without chemical change.
 Physical change can alter the state of matter but not
the chemical identity of a pure substance.
 Pure substances have fixed characteristic elemental
compositions and properties
 Can be classified as elements or compounds

33. Elements and Compounds
 Element is the simplest type of substances with
unique physical and chemical properties. It consists of
only one kind of atom, and cannot be broken down
into simpler substance.
 There are 92 elements in nature and 26 have been
produced artificially.
 Elements are named after famous people/scientists,
planets, geographic location, and minerals.
 It is represented by chemical symbol

34. Names, Symbols and Selected Properties of
Some Common Elements
Names Symbol Properties
Aluminum Al Light, silvery metal
Barium Ba Silvery white metal
Carbon C Soft black solid
Hydrogen H Colorless gas
Magnesium Mg Silvery white,
ductile, light metal
Nickel Ni Silvery white,
ductile, malleable
metal

35.  A few chemical symbols are derived from the Latin or
Greek names of the elements
 Examples are: Copper, Gold, Iron. Silver, Lead,
Mercury, Potassium, Sodium, Tin
 Elements have three groups:
 Metals
 Nonmetals
 Metalloids

36. Properties of Metals & Nonmetals
Metals Nonmetals
Hard, dense, solid
(except Hg)
Some are gases, liquids or
solids; less dense; and
softer (except diamond)
Shiny and can be
polished
Dull, cannot be polished
(except diamond)
Malleable and ductile Brittle
Can conduct heat and
electricity
Insulators (except
graphite)

37. Properties of Metals & Nonmetals
Metals Nonmetals
Usually have high
melting points
Have low melting points
Have high tensile
strengths
Have low tensile
strengths
Have high densities Have low densities

38.  Metalloids are elements which possesses
characteristic of both metals non-metals. They are
also known as semimetals or amphoteric elements
 Examples: B, Si, Ge, As, Sb, Te and Po
 Ge and Si are used in transistor chips because of
their semiconducting property. They become more
electrically conductive as temperature increases.

40. Compound
 It is a substance which can be broken down into simple
substance by ordinary chemical means.
 It is made up of two or more different kind of elements
that are chemically combined with one another.
 It is represented by chemical formula.
 Examples: water, table salt, baking soda and sucrose
 Can be classified as organic and inorganic as to the
presence or absence of carbon
 It is either acid, base and neutral (salt)

41. Homogeneous and Heterogeneous
 Phase – describes the physical state of matter – solid,
liquid and gas
 When all parts of a chemical system have the same
properties and appearance, it is described as
homogeneous.
 A system is heterogeneous when it has non-uniform
appearance and different phases can be recognized.
This means when the system is divided into several
portions, different portions will have different
appearance and different compositions.

42. Homogeneous and Heterogeneous
 Homogeneous mixture is a mixture in which the
composition throughout the system is uniform.
 Example is seawater
 Heterogeneous mixture has one or more visible
boundaries among its components in which the
components are not evenly distributed throughout. It
has non uniform appearance and different phases can
be recognized.
 Examples: halo-halo, chicken macaroni soup

43. In your house, examine common household materials like
bleach, toothpaste, rubbing alcohol, cooking oil,
shampoo, etc. Read the labels and answer the table
below.
Household
Materials
Element or
Compound
Present
Chemical
Symbol/Formula
1.
2.
3.
4.
5.
6.
7.

44. Household
Materials
Element or
Compound
Present
Chemical
Symbol/Formula
8.
9.
10.

45. Classify the following materials as pure substance or a
mixture. If it is an example of a pure substance,
categorize it as element or a compound. If the sample
material is an example of mixture, categorize it further
as homogeneous or heterogeneous.
1. Softdrinks
2. Chocolate chips
3. Buko salad
4. Sugar
5. Soil
6. Aluminum foil
7. Black coffee

46. 8. Sugar solution
9. Air with smog
10. Alcohol
11. Stainless steel
12. Sand
13. Pure air
14. Chunky spaghetti sauce
15. Table salt

47. Methods of Separating
Mixtures