1. The Classification of Matter
Unit I-1
Hebden 49-52

2. Substances Can be homogeneous Can be heterogeneous
Two or more phases
Gravel, cookies
Can be homogeneous
Only one phase
Air, water, salt water, a piece of iron

3. Mixture
More than one Pure Substance physically mixed together

4. Solution A mixture that looks like a pure substance.
Particles of all substances are completely mixed together

5. Solutions: Homogenous Mixtures
A solute is the substance to be dissolved
The solvent is the one doing the dissolving
Universal solvent- generally thought of as water

6. Solutions

7. WHAT IS? Identify the solvent and solute 100 mL of water
0.1 g of sugar

8. Solid Solutions -Alloys
Made by melting different metals and mixing them together
Examples of Alloys are:
Steel (iron, carbon and other elements like Cr and Mo)
Brass (copper and zinc)
Bronze (copper and tin)

9. Solid Solutions -Alloys
Amalgams – special type of alloy that combines Mercury with other metals [old dental work]
Titanium alloys (used to make high-end bike parts & frames)

10. Solid Solutions -Alloys

11. Suspension
Particles are large enough to make it cloudy.

12. Mechanical Mixture
You can see particles of different substances

13. Pure Substances Matter with a unique set of properties
Can be an element or a compound

14. Elements are composed of ATOMS
Atoms of different elements have different masses
is a pure substance that can not be broken down further by chemical means

15. Element
A Pure Substance made up of
ONE kind of atom
Its symbol can be found on the
Periodic Table

16. Metals and Non-Metals
An element can either be a metal or a non-metal

17. Non-Metals Generally gases or dull, brittle solids at room temperature
Bromine is the only liquid
Conduct heat and electricity poorly

18. Non-Metals

19. Metals shiny and solid at room temperature
Exception Mercury [only liquid]
Conduct heat and electricity
Ductile and malleable

20. Metals

21. Compound
A Pure Substance made up of two or more kinds of atoms.

22. Law of Definite
Proportions

23. Compounds
Every compound has its own chemical formula
Water is H20

24. Compound Water
Hydrogen
Water
Oxygen

25. Compounds
Contain symbols of different elements
H2SO4
NaCl
C2H5OH
C3H8

26. Compounds
NOTE: The properties of compounds are always different than the properties of their elements!

27. Ionic Compounds
An Ionic Compound is made up a metal and a non-metal or has Polyatomic Ions in it.
Polyatomic ions are ions made up of more than one kind of atom
They can be found on your ion table (back of Periodic Table)
Some Examples:
SO42- (sulphate), CO32- (carbonate)

28. Ionic Compounds Some example of IONIC compounds are: NaCl MgBr2 Al2O3
K2SO4

29. Covalent Compounds
A Covalent Compound is made up of a two non-metals or is a hydrocarbon
Some example of COVALENT compounds are:
CO2 , PBr3 , CCl4 , C8H18 , XeF6 , C4H9OH