1. Alexander Crumpton Fuqua
Chemistry Review
Alexander
Crumpton
Fuqua

2. Found on the periodic table
Elements
Pure substances
Found on the periodic table
Na, Li, Be, B, Fe, Au, etc…
Compounds Pure substance Chemically bound Separate through chemical reactions 2 or more elements H20, NaCl, CO2, Fe2O3
Mixtures 2 or more substances Physically combined Easily separated Filter, evaporate, sift

3. Types of Mixtures Homogeneous Mixture Heterogeneous Mixture
Also called a solution
Can not see the different parts
Evenly mixed
Air, steel, bronze, saltwater
Heterogeneous Mixture
Can identify all the parts mixed in
Salad, Trail mix, granite, sand, Italian dressing, chicken soup

4. Metalloids Sit on the staircase Semi-conductors Share characteristics
Metals
Magnetic
Shiny/luster
Reactive
Malleable
Left of the staircase
Ductile
Good conductors of heat and electricity
Non-Metals
Dull
Brittle
Right of the stair case
Poor Conductors
Reactive with others
Metalloids Sit on the staircase Semi-conductors Share characteristics

5. Periodic Table Arranged according to increasing atomic number
Group 1: Alkali Metals
Most reactive metals
Group 2: Alkaline Earth Metals
Reactive metals, but less than group 1
Group 3-12: Transition Elements
Most varied properties
Most familiar elements
Group 17: Halogens
Most reactive NON-METAL
Group 18: Noble Gases/Inert Gases
Least/Non-reactive group of elements
Found in elemental form in nature
Bonding Families USUALLY
Group 1  Group 17
Group 2 Group 16
Group 13 Group 15
Group 14 Group 14
Groups/Families Share Characteristics
1-92 Natural Elements
93 or higher- Synthetic Elements

6. Chemical vs. Physical Properties
Chemical Properties
Can only observe by changing the object to something else, a new kind of matter
Reacting with oxygen
Burning
Rusting
Apple turning brown
Reacting with Acids
Physical Properties
Can be observed WITHOUT making it something NEW
Can observe with the 5 Senses
Shape
Density
Solubility
Odor
Melting Point
Boiling Point
Color

7. Chemical vs. Physical Change
Chemical Change
New substance is created
Properties different from original
How you know a change has occurred:
Color change
Temperature change
Formation of a precipitate
Formation of a gas
Physical Change
Change in size, shape or form
No new substance is created

8. Endothermic vs. Exothermic Reactions
Endothermic Reactions:
Takes in energy (heat)
Examples:
Melting
Evaporating
Cooking
Exothermic Reactions:
Gives off energy (heat) to the surroundings
Examples:
Combustion
Composting
Candle Flame

9. Law of Conservation of Matter (Mass)
Matter is not created or destroyed in ordinary chemical and physical changes
Open System
Matter is lost to the surrounding environment
i.e. mixing baking soda and peroxide in an open beaker, allowing gas to escape…
Closed System
Matter is not lost to the surrounding environments
i.e. catching the smoke and ashes to measure out the final weight of the products…

10. Balancing Equations 2 H2O  2 H2O + 1 O2
Write out Elements in equations
Count # of atoms present
Start at the left, change coefficients (NEVER SUBSCRIPTS) in order to balance
Continue balancing from left to right
2 H2O  2 H2O + 1 O2

11. Some Chemical reactions occur in more than one step
Some Chemical reactions occur in more than one step. A 2 step reaction is shown Step 1: 2 PO2  PO3 + PO 30 grams x grams 7.62 grams Assuming all PO3 produced in step 1 completely reacts in step 2, approximately how many grams of CO2 are produced in step 2? Step 2: PO3 + CO  PO2 + CO x grams 5.09 grams 10 grams y grams

12. Some Chemical reactions occur in more than one step
Some Chemical reactions occur in more than one step. A 2 step reaction is shown Step 1: 2 PO2  PO3 + PO 10 grams x grams 4.83 grams Assuming all PO3 produced in step 1 completely reacts in step 2, approximately how many grams of CO2 are produced in step 2? Step 2: PO3 + CO  PO2 + CO x grams 7.29 grams 5 grams y grams