1. Matter-has mass and occupies space
Properties:
Chemical-exhibited by matter as it undergoes changes in composition
Physical-exhibited by matter without a change in composition.
Extensive-depends on the amount of matter
Intensive-independent of the amount of matter
Physical & Intensive:

2. Chemical Change-one or more substances are either used up
or formed and energy is absorbed or released.
Physical Change-change in physical properties without a change in
composition.
Energy-capacity to do work or transfer heat.
Kinetic Energy (KE)-motion
Potential Energy (PE)-position,
condition or composition.
Release of Energy Exothermic
Absorption of Energy- Endothermic

3. E=mc2 Law of Conservation of Matter-There is no
observable change in the quantity of matter during a chemical reaction or during a physical Change.
Law of Conservation of Energy-Energy cannot be created or destroyed in a chemical reaction or in a physical change. It can only be converted from one form to another.
E=mc2
Combined-The combined amount of matter and energy in the universe is fixed.
2Mg + O2-----> 2MgO

4. Chemical Changes
P4(s)+6Cl2(g)----->4PCl3(l)

5. Physical Change
Chemical Change H2 O2
H2O

6. 8C
10H 2O 4N
Law of Definite Proportions-Different samples of any pure
compound contain the same elements in the same proportions by mass

7. Separation of Mixtures

8. SI=International System of Units
Temperature = K (Kelvin)
Time = s (seconds)
Energy = J (Joule)

9. % Composition Parts of A (by mass) 100 parts mixture (by mass)
%A (mass)=
Mass A Mass mixture
49.5 grams of Carbon
100 grams of caffeine 8C
10H 2O 4N
49.5% C
5.15% H
16.5% O
28.9% N

10. Density mass (g) volume (ml) (density)= Specific Gravity (substance)
(water)
=Sp. Gr.=
(water)= oC

11. K=oC

12. Heat Transfer (Amount of heat in J) Specific Heat =
(mass of substance in g)(Temperature change in K/oC)
Specific Heat =
Heat Capacity= (Csp)(mass) units=(J/ oC)