UNIT 3:
Properties of Matter
.
Unit Objectives
1. Define matter and give several examples and non-examples.
2. Explain what a substance is and be able to identify several examples of matter as either
being or not being a substance.
3. Explain the difference between chemical and physical properties of matter and label
several properties as one or the other.
4. Explain the difference between intensive and extensive properties of matter and label
several properties as one or the other.
5. Describe the solid state of matter in terms on shape, volume, compressibility and atomic
or molecular arrangement.
6. Describe the liquid state of matter in terms of shape, volume, compressibility and
atomic or molecular arrangement.
7. Describe the gaseous state of matter in terms of shape, volume, compressibility and
atomic or molecular arrangement.
8. Identify the state of several samples of matter by observing various properties.
9. Explain the differences and similarities between elements and compounds and give
examples of each.
10. Explain what is meant by a chemical mixture and how a mixture is different from a
compound.
11. Explain the differences and similarities between homogeneous and heterogeneous
mixtures and categorize mixtures as one or the other based on observed properties.
12. Define a solution and state the type of mixture that it is.
13. Using a types of matter flow chart categorize samples of matter based on physical and
chemical properties.
14. Categorize types of matter from atomic and molecular particle diagrams.
15. Draw atomic and molecular particle diagrams that fit each type of matter.
16. Describe and perform the process of filtration to separate appropriate mixtures.
17. Describe the type(s) of mixtures that can and cannot be separated using filtration.
18. Describe and perform the process of evaporation to separate appropriate mixtures.
19. Describe the type(s) of mixtures that can and cannot be separated using evaporation.
20. Describe and perform the process of distillation to separate appropriate mixtures.
21. Describe the type(s) of mixtures that can and cannot be separated using distillation.
22. Explain the differences and similarities between distillation and fractional distillation in
terms of types of mixtures that each can separate.
23. Describe and perform the process of chromatography to separate appropriate mixtures.
24. Describe the type(s) of mixtures that can and cannot be separated using
chromatography.
25. Explain the difference between an chemical change and a physical change and give
several examples of each.
26. Given a chemical reaction equation identify the reactants and products.
Notes 1: Properties of Matter – What is matter?
Lesson Objectives:
1. Define matter and give several examples and non-examples.
2. Explain what a substance is and be able to identify several examples of matter as either
being or not being a substance.
3. Explain the difference between chemical and physical properties of matter and label
several properties as one or the other.
4. Explain the difference between intensive and extensive properties of matter and label
several properties as one or the other.
 Chemistry is the study of the composition (make-up) of matter and the changes that it
undergoes (how it reacts).
 Matter is anything that has mass and occupies volume (or takes up space)
o Give three examples and three non-examples of matter
Matter
Not Matter
 A substance is any sample of matter that has a uniform
and definite composition.
o A substance will always be either a pure element
or pure compound.
o Examples : CO2 , He, Aluminum, Salt (NaCl),
Two Types of Properties of Matter (Chemical and Physical)
 Physical Properties – A trait or characteristic of a substance that can be observed
without changing its composition.
 Examples:
Malleability – Able to
be bent or shaped
without breaking –
Most metals are
malleable
_Color_
_Hardness_
Mass
Malleability
Brittle – Opposit of
malleable – easily
breaks
There are TWO DIFFERENT types of PHYSICAL PROPERTIES.
 Extensive Physical Properties
o Depends on the amount of matter in a sample
o Examples include mass, volume, length and shape
 Intensive Physical Properties
o Do Not depend on the amount of matter
o Depends on the type of matter in a sample
o Examples include color, taste, hardness, density, and boiling point.
 Chemical Properties - Properties that can only be determined by changing the identity
of the substance.
o Measure how the substance reacts in the presence of the other chemicals
o Examples:
 Blood turns red when exposed to oxygen
 Metals react with acids
 Paper burns
Complete the Guided Practice : Properties of Matter
Notes 2: States of Matter
Three states of matter that are common – Solid, Liquid and Gas
SOLIDS

Have definite shape and volume

Shape does not depend on the shape of its container

Not compressible (squeeze with pressure)

Very little space between particles (molecules or atoms)

Particles arranged in regular repeating patterns.

Examples:
o Ice, Coal, Rock, Wood
LIQUIDS

Have indefinite shape – Takes the shape of the container.

Has a definite or fixed volume – Occupies a fixed space

Some space between atomic or molecular particles

Atomic or molecular particles randomly arranged and are able
to flow over one-another.

Examples:
o Water, milk, oil
GASES

Takes on both the shape and volume of its container

Nature of atomic or molecular particles
o A lot of space between particles
o Move with fast, random motion.
States of Matter
Summarize the properties of matter in the table below
Solid
Shape
(definite or indefinite)
Volume
(definite or indefinite)
Compressibility
(Compressible or
Incompressible)
Nature of atomic or
molecular particles
(Sketch and describe)
Liquid
Gas
Notes 3: Types of Matter
 Matter is separated into two categories – Pure Substances and Mixtures
 Each of the two categories is further separated into two additional sub-categories
Pure Substances – 2 Types – Elements and Compounds
Elements
 The simplest form of matter
 Smallest particles are just one type of atom
 Cannot be broken down by physical nor chemical
means.
 Organized on the Periodic Table of Elements
 Examples: Silver (Ag) Carbon (C), Hydrogen (H)
Compounds
 Atoms of two or more different elements chemically bonded.
 Smallest particles are molecules of multiple atoms.
 Cannot be broken down by physical means (like boiling, freezing)
 Can be broken down by chemical reactions
o H2O can be split into hydrogen and oxygen by a chemical
process called electrolysis
 Examples: H2O, CO2, NaCl, CO (Note this is different than Co)
Mixtures – 2 Types – Heterogeneous and Homogeneous
 Any mixture is a physical blend of two or more pure
substances
 NO chemical reaction occurs when the substances are
mixed.
 NO new substance is formed.
 Can be separated by physical means
Homogeneous Mixtures
 The prefix homo- means same
 The composition of a homogeneous mixture is
uniform throughout.
 There are no observable differences in the
sample.
 Koolade – no matter where you put the straw
your sip tastes the same.
 Examples: Corn oil, Salt Water, Air (mixture of gases),
Heterogeneous Mixtures
 The prefix hetero – means different
 The composition of the matter is observably
different in different places – Non-uniform.
 Examples: Chocolate chip cookie, Vegetable soup,
Soil, Tossed salad
Particle Diagrams
 Often samples of matter are represented by particle diagrams to show the nature of the
smallest particles for each category of matter.
 Examples:
o A pure element in the gaseous state of matter could exist as
individual atoms.
o A pure compound in the gaseous state of matter could exist is pairs
of atoms bonded
o The following particle diagram would be a homogeneous mixture
of two different pure elements.
Complete the Guided Practice: Categorizing Matter
Notes 4: Separating Mixtures
 Mixtures of pure substances can be separated using various methods.
 The type of mixture determines the method that is used.
Filtration
What is being
Description of the process
Diagram
separated
Solid from
liquid in a
 The mixture is poured into a funnel lined with
filter paper
heterogeneous  Solids remain in the filter paper and can be
mixture.
dried and recovered for later use.
 Liquid passes through the paper and can be
recovered for later use.
Evaporation
Solid is
separated
 The solution is heated to slowly evaporate the
liquid.
from a
 The solid stays behind.
homogeneous
 The liquid is not recovered
mixture with a
Brewing coffee
liquid
(solution)
Distillation
A
homogeneous
 The solution is heated in a flask until the liquid
boils.
mixture of
 Different liquids boil at different temperatures
liquids is
 The vapor produced passes into the condenser
separated into
where it is collected and condenses back into a Distillation of crude oil produces
a variety of petroleum products
liquid.
including gasoline and home
 The pure liquid (distillate) is collected in the
heating oil.
its
components.
flask
Chromatography Separation of
mixtures of
pigments in
dyes and inks.
 A sample of the mixture is put on a piece of
special chromatography paper.
 The end of the paper is dipped in a pure liquid
solvent like water or alcohol.
 The liquid flows up the paper by capillary
action.
 As the liquid flows up the paper, the mixture
of pigments is dissolved at different amounts
and therefore move up the paper at different
rates.
Notes 5: Changes in Matter
 Matter can undergo many types of changes.
 Changes in matter are categorized into Physical Changes and Chemical Changes.
Physical Changes
 A change in the form of the matter
 Does not change the chemical composition of the
sample of matter.
 Relatively easy to reverse
o E.g ice to water then back to ice
 Examples
o Crushing or grinding
o Changes in state like boiling water into a gas.
o Tearing or breaking
Chemical Changes
 A change that results in producing a new
substance or new substances.
 The new substance(s) has different
composition and different properties than
the original substance(s)
 Relatively difficult to reverse.
o Burning paper to produce CO2 can’t easily be turned back into paper.
 The following are indicators that a chemical change MAY have taken place
o Change in color.
o Production of a new odor or aroma.
o Generating a gas
o Input or release of energy
 Examples:
o Cooking almost anything
o Rusting or corrosion
o Combustion or burning of anything
Chemical Reactions
 When a chemical change occurs it is referred to as a chemical reaction.
 Chemical reactions are represented by using reaction equations.
 The left side of the chemical reaction equation are the substance(s) that exist BEFORE the
reaction begins and are called the reactants.
 The right side of the reaction equation are the substance(s) that exist after the reaction is
completed and are called the products.
Math equation
5 + 3
=
8
What you start with
What you end up
with
Chemical reaction equation
CH4 + 2O2  CO2 + 2H2O