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
Now that we have defined chemical and physical properties of matter, we can use that to help us classify it.
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 (mechanical 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 (mechanical mixture) – Uneven distribution of substances. (Very impure)
- You can see the different parts.
Examples:
Milk
Blood

12. Mixtures
Homogeneous Mixture (solution) – 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. Special Types of Heterogeneous Mixtures
Colloid – substance microscopically dispersed evenly throughout another substance
e.g. Whipped cream, butter, paint
Suspension - mixture containing solid particles that are sufficiently large for eventually settling out
e.g. Italian dressing, dust in air, oil and water

14. Examples of Mixtures
gas in gas: The atmosphere is a mixture of gases, mostly nitrogen and oxygen.
liquid in liquid :Wine is a mixture of mostly ethanol and water.
solid in solid: Alloys, such as brass, are made up of a mixture of metals.
gas in liquid: Soft drinks, such as cola, are mixtures of mainly carbon dioxide gas and water.
solid in liquid: Sea Water is a mixture of salts dissolved in water.
solid in gas: Smoke is mixture of tiny solid particles in atmospheric gases.

15. A FEW METHODS FOR SEPARATING MIXTURES
Distillation – process of separating a mixture by differences in boiling point
Filtration – process of separating a solid and a liquid

16. Crystallization : when 2 materials crystallize at different temperatures then we condense the mixture to extract the component which crystallizes first
Magnetism – separating magnetic from non-magnetic metals

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

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

19. 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.

20. 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

21. 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