1. Chapter 3
Matter

2. The Questions Why do is the sun hot?
Why does wood burn whereas rocks do not?
What is flame?
How does soap work?
Why does soda frizz when you open the bottle?

3. Matter
Define as the “stuff” of which the universe is composed, has two characteristics:
It has a mass and it occupies space.
Three states of matter:
Solid
Liquid
Gas

4. The Three States of Matter
Definition
Examples
Solid
Rigid, has a fixed shape and volume
Ice cube, diamond, iron bar
Liquid
Has a define volume but takes the shapes of its container
Gasoline, water, alcohol, blood
Gas
Has no fixed volume or shape; take the shape and volume of its container
Air, helium, oxygen

5. Physical and Chemical Properties and Changes
Physical properties
Characteristics that do not involve a change in a sample’s chemical makeup.
E.g Temperature, color, amount, melting point, solubility….
Chemical properties
Characteristic that do involve a change in chemical makeup
E.g rusting of iron, combustion etc…

6. Examples
Classify each of the following as a physical or a chemical property
The boiling point of a certain alcohol is 78oC
Diamond is very hard
Sugar ferments to form alcohol
A metal wire conducts an electric current

7. Physical Changes
Involves a change in one or more physical properties, but no change in the fundamental components that make up the substance
Solid  liquid  gas

8. Chemical Change
Involves a change in the fundamental components of the substances; a given changes into a new different substance or substances
Also called as chemical reactions
E.g Combustion of propane
Propane + oxygen gas  Carbon dioxide +water vapor

9. Example
Classify each of the following as a physical or a chemical change
Iron metal is melted
You make scrambled eggs
Wood burns in air
A rock broken into smaller pieces

10. 3.3 Elements and Compound Classify as a pure substance
Have a constant composition
Element is a substance that cannot be broken down into other substance by chemical method
Compound is a substance that composed of 2 or more elements or any substance that can be broken down into elements
element + element  compound
compound  element + elements + ….

11. 3.4 Mixtures and Pure Substances
Mixtures: formed when 2 or more substances are blended together in some random proportion
Individual substances do not undergo a chemical change
Homogeneous mixture (solution) has uniform properties throughout.
E.g – water-base solutions
Air: mixture of N2(g), O2(g)
Heterogeneous mixture has regions with different composition
E.g – Sand with sugar, water with gasoline, dust with air

12. Examples
Identify each of the following as a pure substance, a homogeneous mixture, or a heterogeneous mixture
Gasoline
Brass
Pure apple juice
Chocolate chip cookies

13. 3.5 Separation Mixtures Physical methods Gravity Suction
Distillation
Filtration
Gravity
Suction
Common separation
Homogeneous mixture
Heterogeneous mixture

14. Distillation Separate solid from liquid E.g – Separation of salt water
Volatile substance is readily separated through heating
Composition of each individual substance does not changed
E.g – Separation of salt water
If two solutions are volatile then distillation cannot be achieved

15. Filtration Used to remove impurities from solution
Impurities (larger solid particles) stay on the filter paper
Water goes through the paper
E.g – sand and seawater

16. Summary