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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

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),

Matter Not Matter

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: _Color_ _Hardness_

Mass Malleability

Malleability – Able to

be bent or shaped

without breaking –

Most metals are

malleable

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 Liquid Gas

Shape

(definite or indefinite)

Volume

(definite or indefinite)

Compressibility

(Compressible or

Incompressible)

Nature of atomic or

molecular particles

(Sketch and describe)

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

separated

Description of the process Diagram

Solid from

liquid in a

heterogeneous

mixture.

The mixture is poured into a funnel lined with

filter paper

Solids remain in the filter paper and can be

dried and recovered for later use.

Liquid passes through the paper and can be

recovered for later use.

Brewing coffee

Evaporation Solid is

separated

from a

homogeneous

mixture with a

The solution is heated to slowly evaporate the

liquid.

The solid stays behind.

The liquid is not recovered

liquid

(solution)

Distillation A

homogeneous

mixture of

liquids is

separated into

its

components.

The solution is heated in a flask until the liquid

boils.

Different liquids boil at different temperatures

The vapor produced passes into the condenser

where it is collected and condenses back into a

liquid.

The pure liquid (distillate) is collected in the

flask

Distillation of crude oil produces a variety of petroleum products including gasoline and home heating oil.

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

Chemical reaction equation

CH4 + 2O2 CO2 + 2H2O

What you start with What you end up

with