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:

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

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

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

Physical Change Chemical Change H2 O2 H2O

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

Separation of Mixtures

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

% 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

Density mass (g) volume (ml) (density)= Specific Gravity (substance) (water) =Sp. Gr.= (water)=1.00 g/ml @ 25oC

K=oC+273.15

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)