1. The Structure of Matter: Matter is anything that has mass and takes up space.

2. The Particle Theory of Matter
All matter is made up of tiny particles that have empty space between them.
Different substances are made up of different kinds of particles.
Particles are in constant random motion.
The particles of a substance move faster as its temperature increases.
Particles attract each other.

3. STATES OF MATTER Matter exists in three states:
1. Solid – shape is definite
2. Liquid-shape is indefinite as it takes the shape of the container
3. Gas-shape is indefinite as it takes the shape of the container

4. Observing Matter
1. Qualitative observations- describe the properties of matter using the senses eg. Colour, taste, smell, state
2. Quantitative observations - describe the properties of matter using exact measurement eg. Length, mass, density, volume

5. Classification of Matter
One way chemists classify matter is based on its purity.

6. Classification of Matter
Pure Substance – Matter that has only 1 set of chemical and physical properties.
Example: Pure water always has the exact same chemical and physical properties under the same conditions.
If water ever tastes different then it isn’t pure water; it fits into our next category.

7. Classification of Matter
Mixture – Two or more pure substances mixed together. Each substance in the mixture retains its own set of chemical and physical properties.
Example: Copper and Zinc can be mixed together to produce brass.
Even though it may look different, it is still copper and zinc. Each metal retains its own properties like melting point.

8. Classification of Matter
Mixture – Two or more pure substances mixed together. Each substance in the mixture retains its own set of chemical and physical properties.
Unlike pure substances, mixtures can always be separated by physical means.
How could we separate the copper and zinc back out?

9. Mixtures
Mixture – Two or more pure substances mixed together. Each substance in the mixture retains its own set of chemical and physical properties.
If a sample of sand contains iron and salt, how could you separate them from the other minerals?

10. Mixtures Some mixtures are more pure than others.
Heterogeneous mixture – Uneven distribution of substances. (Very impure)
- You can see the different parts.
Examples:
Sand
Granite
Wood

11. Mixtures Some mixtures are more pure than others.
Heterogeneous mixture – Uneven distribution of substances. (Very impure)
- You can see the different parts.
Examples:
Milk
Blood

12. Mixtures
Homogeneous Mixture – Components are evenly mixed. (More pure than heterogeneous)
- Cannot see the parts.
Salt water contains salt and water, but are mixed all the way to the atomic level , but it can still be separated by physical means.
Seawater distillation plant

13. Pure Substances
Pure substances can also be divided into 2 categories: compounds and elements.

14. Pure Substances
Compound – Two or more elements chemically bonded together.
Examples:
Carbon Dioxide (CO2)
Water (H2O)
Salt (NaCl)
Sucrose (C12H22O11)

15. Pure Substances
Compounds have only 1 set of properties. They cannot be separated by any physical process.
- Can only be separated by a chemical reaction.
Water can be separated into Hydrogen and Oxygen by a process called Electrolysis.

16. Pure Substances
Elements – Substances made up of only one type of atom.
- Cannot be separated by any physical OR chemical process.
Examples:
Carbon
Helium
Gold

17. Heterogeneous Mixture
Matter
Can be separated physically
Cannot be separated physically
Mixture
Pure Substance
Cannot see the parts
Can be separated chemically
Can see the parts
Cannot be separated
Heterogeneous Mixture
Homogeneous Mixture
Compound
Element
Most impure
Most pure