AP CHEMISTRY
MR. LINARES
SEMESTER ONE FINAL EXAM REVIEW
2012-2013
The first semester final exam will consist of a multiple-choice section and free-response
questions. The list below identifies topics that will appear on the exam. Use previous
homework problems, worksheets, and tests to prepare for your final. No calculators will
be used on the multiple choice section, they will only be allowed on the free response
section.
Chapter 2 – Atoms, Molecules and Ions (the structure of an atom)
 Name and write formulas of common ions and ionic compounds
The names of monatomic ions and polyatomic ions that you will need to know for
test are found in figure 2.11, page 54, and on page 60, tables 2.2 and 2.3
 Name the acids found on page 65….both in table 2.5 and in the text…(HNO3 etc)
 Name hydrates.
 Name and write formulas of covalent compounds (including hydrocarbons and
alcohols)
o Example:
Hydrocarbon*
Alcohol
Methane
CH4
methanol
CH3OH
Ethane
C2H6
ethanol
C2H5OH
Propane
C3H8
propanol
C3H7OH
*know that when combustion occurs with a hydrocarbon, it burns in air
and releases H2O & CO2
Chapter 3 – Mass Relationships in Chemical Reactions
 Molar conversions
 Using Avogadro’s number to find number of molecules, atoms, ions etc…from
molar mass
 Empirical formulas and Molecular formulas
 Percent Mass Composition
 Balancing equations
 Stoichiometry  Mole-Mole, Mole-Mass, Mass-Mass calculations
 Limiting reactants
 Excess Reactants
 Percent Yield
Chapter 4 – Reactions in Aqueous Solutions
 Define solutions and know its components
 Electrolytes and non-electrolytes
 Know what a hydration shell is and how it forms
 Net ionic equations
 Properties of acids and bases. Bronstead bases and acids. Hydronium ion
 Mono-, di-, and triprotic acids
 Acid-Base neutralization reactions
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Know the type of redox reactions and how to perform….
Examples…
Combination : S + O2  SO2
Decomposition: KClO3  KCl + O2 (unbalanced)
Combustion: CH4 + O2  CO2 + H2O (unbalanced)
Displacement (for H, metals and halogens): Zn + HCl  ZnCl2 + H2 (unbalanced)
Na + CaCl2  NR
Cl2 + KBr  Br2 + KCl (unbalanced)
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Solubility…definition and rules
Assigning oxidations numbers
Concentration of solutions (molarity)
Solution problems
Titrations
Chapter 5 - Gases
 All gas laws (including modified gas laws) from page 175-189, 192-196, and 203204
Chapter 6 - Thermochemistry
 Types of energy on page 224
 Endo- and exothermic reactions
 First and second law of thermodynamics
 Specific heat problems
 Hess’s law
Chapter 7 – Electronic Structure of Atoms
 Quantum numbers, electron orbitals and electron configurations and the periodic
table (page 286-301)
Chapter 8 – Periodic Properties of the Elements
 The five groups that elements are classified into on the periodic table (pages 318320)
 Trends in atomic radius, ionic radius, ionization energy, electronegativity (pages
323-335)
Chapter 9 – Chemical Bonding
 Covalent bonding and electronegativity (pages 366-372)
 Drawing Lewis Structures with formal charges and resonance structures (pages
372-379)
 Exceptions to the octet rule
 Bond enthalpy
Chapter 10 – Molecular Geometry
 Electron domain geometry and molecular geometry (along with bond angles and
hybridizations). Pi and sigma bonds (pages 400-428)