1. Chapter: 3 (9-13-18_Notes) 3.2 Changes in matter
MAIN IDEA: Matter can undergo chemical and physical changes.

2. Heterogeneous Mixtures
Chapter - 3 Concept Map:
Examples:
Compounds
Elements
Chemical changes
Mixtures
Pure Substances
Physical changes
Matter
Homogeneous Mixtures
Heterogeneous Mixtures

3. 3 physical changes: Solid Liquid Gaseous
How many changes of the substance, H2O is shown in this photo?
3 physical changes:
Solid
Liquid
Gaseous

4. Changes in matter Physical change: Chemical change:
A change in which matter may look or behave differently but no new substance is formed
A change in which new substances are formed

5. Organize the following as physical or chemical change
Lighting up a match
Color change on leaves
condensation
Sugar crystal formation
Cooking eggs
Bubbling soda drink
Rusting of iron
Chopping a carrot

6. Organize the following as physical or chemical change
Physical change:
Chemical change:
Color change on leaves
Cooking eggs
Sugar crystal formation
Bubbling soda drink
condensation
Lighting up a match
Chopping a carrot
Rusting of iron

7. Changes in matter Physical change: Chemical change:
A change in which matter may look or behave differently but no new substance is formed
A change in which new substances are formed
Ex:
chopping/cutting
distillation
Freezing
Evaporation
Crystallization
Melting
Vaporization
Ex:
Cooking
Combustion (burning)
Rust formation

8. Evidence of chemical reactions
Example
Color change
Rust formation on iron (reddish)
Change in temperature
Baking soda mixed with water
Precipitate (solid) formation
Curdling of milk results in clumping
Production of new gas
Photosynthesis reaction results in oxygen synthesis
Change in smell
Rotting food

9. Law of Mass Conservation Mass reactants = Mass products
When a chemical reactions takes place inside a closed system, matter is neither created or destroyed.
OR,
When a chemical reactions takes place inside a closed system, mass of reactants equals the mass of the products.
Mass reactants = Mass products

10. How to write chemical equations for reactions
Each element (type of atom) has a chemical symbol.
So, each substance has a chemical formula that tells you’re the number of each type of element (atom) it contains.
Subscripts indicate number of atoms of each element in each substance
A number in front of the substance indicates the moles (parts) of the substance that is present in the reaction. (Every element is multiplied by this number)
A plus sign is used to show multiple reactants or products
An arrow indicated the direction of the reaction (points to products)
EXAMPLE:
Magnesium
Magnesium oxide
Oxygen gas + Mg
MgO O
Unbalanced
2 Mg
2 MgO O
Balanced
2( XY) = 2X and 2Y
2.Mg and 2.Oxygen

11. LAB6: Mass measurement Instructions
New gas in side balloon
Products
Deflated balloon
Baking soda
Vinegar
Reactants = vinegar + Baking soda
Products = gas + new liquid
Flask and balloon only
AFTER
Reaction= products
BEFORE
Combining reactants = reactants
Mass = M3
Mass = M1
Mass = M2
Mass of Reactants only = M2 – M1
Mass of products only = M3 – M1

12. Matter - Properties & Changes
Chapter - 3
Matter - Properties & Changes
3.1 Properties of matter ( Text Book p70-75)
MAIN IDEA: Most common substances have diverse chemical and physical properties and exist as solids liquids or gases.
3.2 Changes in matter (Text Book p76-79)
MAIN IDEA: Matter can undergo chemical and physical changes
3.3 Mixtures of matter (Text Book p80-83)
MAIN IDEA: Most everyday matter occurs as mixtures – combinations of two or more substances.
3.4 Elements & compounds (Text Book p84-91)
MAIN IDEA : A compound is a combination of two or more substances