1. Chemistry is the study of the properties and behavior of matter.
Physical material of the universe
Has mass
Occupies space

2. Properties of Matter
Physical properties: Measured without changing the substance (melting point, color)
Chemical properties: Describe how substances react to form different substances (hydrogen burns in oxygen)
Intensive properties: Do not depend on the amount of substance (melting point)
Extensive properties: Depend on the amount of substance (mass, volume)

3. States of Matter (macroscopic level)
Gas
No fixed volume or shape
compressible
Liquid
Volume independent of container, no fixed shape
Incompressible
Solid
Volume and shape independent of container
Incompressible, rigid

4. States of Matter (molecular level)
Gas
Molecules far apart,
Move at high speeds, collide often
Liquid
Molecules closer than those in gas,
Move rapidly but can slide over each other
Solid
Molecules packed closely in definite arrangements

5. Separation of Mixtures
Separation techniques exploit differences in properties of the components
Filtration: To remove solid from liquid
Distillation: To boil off one or more components
Chromatography: To exploit solubility of components

6. Elements & Compounds
An element is a substance made of one kind of atom.
Examples are oxygen and silicon.
A compound is a substance made of two or more elements.
Has different properties than those of the elements from which it is made.
Example is SiO2 (glass or sand).
Elements are combined in a specific proportion.

7. Compounds
A compound is a substance of 2 or more elements, chemically combined.
Plants make glucose.
Geologic processes make calcium carbonate.
Two types of compounds
Molecular compounds
Ionic compounds

8. Molecules
A molecule is a particle of matter made up of two or more atoms held together by SHARING of electrons. N2
Nitrogen
CO2
Carbon dioxide

9. Mixtures Mixtures are substances made of two or more parts.
Not combined chemically
Make-up or composition may vary (soil)
Parts of mixtures keep their original properties.
Parts can be separated by physical means.
Distillation, evaporation and filtering are examples of physical means.

10. Mixture vs. Compound Mixture Compound Composition* may vary.
Composition is constant.
Components** keep their original properties.
Properties are different than those of its components.
Components are not chemically combined.
Components are chemically combined.
Components can be separated by physical means.
Components usually require chemical means for separation.
*Composition = how something is made. (Compose = To make.)
**Component = a part
*** vary = differ

11. Properties of Mixtures
Can be made up of any number of compounds or elements.
Homogeneous mixture: All parts are alike.
Uniform
Any sample contains same amount of each component.
Milk and orange juice are examples.
Heterogeneous mixture: Not every part has the same composition.
Non-uniform
One sample may have more of one component than another sample.
Soil and garlic salt are examples.

12. Properties of Matter
Physical properties: Measured without changing the substance (melting point, color)
Chemical properties: Describe how substances react to form different substances (hydrogen burns in oxygen)
Intensive properties: Do not depend on the amount of substance (melting point)
Extensive properties: Depend on the amount of substance (mass, volume)

13. Classifying Substances
Element, Mixture or Compound?
Homogeneous or heterogeneous mixture?
Ionic or molecular compound?
Metal alloy (steel)
mixture
homogeneous
Tin
element
Brass
mixture (Cu,Zn)
Carbon dioxide (CO2)
compound
molecular
Calcium Carbonate (CaCO3)
ionic
Ammonia (NH3)
Cement
heterogeneous
Ink
Cola with ice

14. Periodic Table
The modern periodic table shows the position of the element is related to :
1. Atomic number AND
2. Arrangement of electrons in its energy levels

15. Periodic Table Organization
Nonmetals: Upper right corner plus hydrogen. 
Metals: 80 % of elements to left of zig-zag line. 
Metalloids: Have properties of both metals and nonmetals. They border the zig-zag line.  
Rare Earth Metals: Two rows of elements separated to make it more convenient size.
Period: Horizontal row of table  
Group: Vertical column of table

16. Groups Predict Properties
Alkali metals in Group I are the most reactive elements due to 1 valence electron
Halogens in Group 17 combine with metals to form salts
Noble gases in Group 18 are not reactive due to 8 valence electrons (2 for He)
Elements behave chemically like those closest to them on the table, particularly in same group.

17. Properties of Metals 1.Malleable (can be shaped without breaking)
2.Ductile (can be pulled into wire)
3.Have luster (are shiny)
4.Conduct electricity (Electrons are free to move.)
5.Have a low number of electrons in their outer energy levels ( 1 to 3)

18. Nonmetals No luster Not good conductors
Many valence electrons (4 or more)
Carbon: Component of living things
Entire branch of chemistry devoted compounds containing carbon: Organic Chemistry

19. Metalloids Along zig-zag line (not including Al)
Have properties of metals and non-metals
Often shiny like metals
Conduct heat and electricity
Common use is semiconductors, computer chips
Semiconductors conduct electricity when other elements are incorporated into them