with selected problems from the end of each chapter for review
CHAPTER 1
Chemical vs. physical changes # 13, 14
Classification of matter (elements, compounds, mixtures) # 1, 2, 7, 8
Describing states of matter Pg. 5 of text
# 11, 12 Extensive vs. intensive physical properties
CHAPTER 2
General set up of the periodic table and properties of the elements
# 29 - 32
Predicting charge of ions from location on the periodic table
Naming and writing formulas for ionic compounds and acids
Atomic number, mass number, isotope
Determining the # of p
+
, n
0
and e
-
for an atom
# 43, 44
# 47, 48, 53 - 58
# 15 – 18
# 15 - 18
Protons vs. neutrons vs. electrons # 14
General classifications of organic compounds, section 2.9 Read section 2.9; # 65, 66
CHAPTER 3
Balancing equations # 5 - 8
General forms of the various of chemical reactions
Product prediction
# 10 - 14
# 10 - 12
Limiting reactant and excess reactant problem solving # 69 - 74
Molecular formula problem solving # 45, 46
CHAPTER 4
Use of the activity series for metal and halogen single replacement reactions
Diatomic molecules (F
2
, Cl
2
, O
2
, etc.)
# 43 - 48
Know what elements are diatomic molecules in their free states

1

CHAPTER 4, continued
Molarity of Solutions
Properties of acids and bases
Use of solubility rules
Electrolytes v. nonelectrolytes
Strong and weak electrolytes
Writing formula unit, total ionic, net ionic equations
Determining the oxidation number of an element
Redox reactions - Recognize the oxidizing agent and reducing agent
General forms of the different types of chemical reactions
Classifying types of reactions
Product prediction for all types of reactions
# 51, 52
# 21 - 28
# 11 - 16
# 27, 28
# 27, 28
# 29 - 32
# 39 - 42
# 41, 42
# 15, 16, 29 – 32, 41 - 46
# 15, 16, 29 – 32, 41 - 46
# 15, 16, 29 – 32, 41 - 46
Identifying and naming strong and weak acids and bases # 23, 24
CHAPTER 5
Distinguish between potential and kinetic energy endothermic vs. exothermic reactions
The first law of thermodynamics
Study definitions
Study definitions
# 17, 18
# 22
Study definitions
Movement of energy in system/surroundings
Definitions: Joule, Specific Heat, calorie, Heat Capacity,
Standard enthalpy of formation
Calorimetry/applications of calorimetry
Calorimetry problem solving
Hess’s law problem solving
Read section 5.8
# 47, 48
# 57 - 62
2

Format:
39 multiple choice questions (1 point each)
4 classify the reaction type/product prediction/writing balanced net ionic equations (choose from 8) (4 points each)
2 problems (choose from 3) (10 points each)
You will be given a periodic table, necessary formulae and constants, the activity series and the solubility rules with your exam
Don’t forget to bring a #2 lead pencil and a calculator to the exam
No cell phones, please!
REACTIONS: Each equation is worth 4 points. One point will be deducted for any errors in the classification of the reaction type (Combination, Decomposition, Combustion, Single Displacement, Double
Replacement). One point will be deducted for any errors in the reactants. One point will be deducted for any errors in the products. Three points will be deducted if there are errors in both the reactants and the products.
This is the procedure used on AP exams.
PROBLEMS: Partial credit will be given in the same manner used during the year.
1.
Complete the problems suggested in this review packet
2.
Check your answers using the chapter answer keys you already have
3.
Complete the reaction prediction practice problems and check your answers
4.
Review your notes for those topics and skills for the problems you had difficulty with
5.
Ask questions during the final exam review in class
3