AP Chemistry 1st Semester Exam Review Sheet
The textbook section in which each objective is covered is in ( ), followed by practice
problems, also in ( ), from the end of that chapter. Complete the work for the
objectives on notebook paper as follows: Write definitions where appropriate, solve
the practice problems, showing all work necessary to get the answer. Most of the
practice problems were homework problems this semester. Completing the work
for the review sheet will earn you extra credit on your exam (up to 5 points)
Review Stuff (Chapters 1-3): Be able to -1. Distinguish between physical and chemical properties of matter (1.3) (#21)
2. Calculate density (1.4) (#29)
3. Use significant figures correctly in calculations (1.5) (#37,41)
4. Figure out the number of subatomic particles in isotopes (2.3) (#23,27)
5. Identify the elements that exist as diatomic molecules (2.6)
6. Distinguish between an ionic compounds, molecular compounds, acids, and salts from
their formula (2.6-2.8) (#65)
7. Name and write formulas for compounds (2.6-2.8) (#71a-d,73a-d,75,77)
8. Distinguish between an empirical and molecular formula (2.6) (#49)
9. Interpret particulate level drawings (3.1,3.2) (#1,3,4)
10. Calculate the empirical formula of a compound (3.5) (#45)
11. Do combustion analysis problems (3.5) (#55)
12. Do stoichiometry, including limiting reagent problems (3.6,3.7) (#61,77)
13. Do percent yield problems (3.7) (#83)
Reactions (Chapter 4): Be able to—
1. Distinguish between strong, weak, and non-electrolytes (4.1) (#1,2,35,37)
2. Know the solubility of the following ions: nitrates, alkali metals, ammonium ion
(4.2)
3. Predict the products of precipitation reactions, and write as net ionic equations
(4.2) (#26)
4. Distinguish between strong and weak acids and bases (4.3)
5. Write acid/base neutralization reactions (net ionic) (4.3) (#39,40)
6. Identify oxidation numbers (4.4) (#49)
7. Identify the following for redox reactions: the species being oxidized or reduced
(4.4) (#51)
8. Calculate ion molarities (4.5) (#69,71)
9. Calculate the molarity of an acid or base from titration data (4.6) (#81)
Other Reaction stuff (from packets I gave you): Be able to—
1. Predict the products of the following types of synthesis reactions, and write as net
ionic equations: metallic oxides + water, nonmetallic oxides + water
Practice: a) drops of dinitrogen trioxide are added to distilled water
b) powdered barium oxide is mixed with water
2. Predict the products of the following types of decomposition reactions, and write
as net ionic equations: metallic carbonate decomposition, carbonic acid
decomposition
Practice: a) solid ammonium carbonate is heated
b) carbonic acid →
Thermochemistry (Chapter 5): Be able to—
1. distinguish between an open, closed, and isolated system (5.1)
2. use the First Law of Thermodynamics equation (U = q + w) (5.2) (#25)
3. do stoichiometric calculations involving enthalpy quantities (5.4) (#43)
4. calculate quantities involving “coffee cup” constant pressure calorimetry (5.5)
(53,55)
5. calculate heat quantities using a bomb calorimeter (5.5) (#57,59)
6. use Hess’s Law to calculate enthalpy changes (ΔH) for reactions (5.6) (#63,65)
7. calculate enthalpy changes for reactions (ΔH) using standard enthalpies of
formation (5.7) (#71,75)
Thermodynamics (chapter 19): Be able to –
1. recognize processes associated with increases and decreases in entropy
(19.2,19.3) (#37,43)
2. calculate ∆G° and ∆S° from their energies of formation (19.4,19.5) (#53d,61d)
3. use the equation for Gibbs free energy change to predict the spontaneity of a
chemical reaction (19.5) (#57,69)
4. know the conditions associated with entropy and enthalpy that lead to
spontaneous or nonspontaneous processes(19.6) (#65)
5. Interpret particulate drawings associated with thermodynamics (19.6) (#4)
Atomic Structure (Chapter 6): Be able to—
1. use the following equations: c= x  and E = h (6.1,6.2) (#19,25)
2. know the number and types of atomic orbitals in an atom, and where they can be
located (6.5) (#71)
3. write electron configurations for atoms or ions following the Aufbau Principle,
Hund’s Rule, and the Pauli Exclusion Principle (6.7-6.9) (#75)
Periodic Properties of the Elements (Chapter 7): Be able to –
1. Understand trends in, and rank elements in order of; atomic size, ionic size,
ionization energy, or metallic character (7.3,7.4,7.6) (#41,43,55)
Chemical Bonding (Chapter 8): Be able to –
1. know how the lattice energy of an ionic compound is affected by the size and
charge of the ions in the lattice (8.2) (#24)
2. write plausible Lewis structures for neutral molecules and polyatomic ions
(8.3,8.5-8.7) (#47,63)
3. calculate formal charges (8.5) (#51)
4. use bond energies to determine the ΔH of a reaction (8.8) (#71)
Molecular Geometry and Bonding Theories (chapter 9): Be able to -1. Predict the electron group and molecular geometry of a molecule (9.1-9.3) (#25)
2. Determine if molecules are polar or nonpolar based on their molecular geometry
(9.1-9.3) (#41)
3. Describe and predict the hybridization of atomic orbitals (9.4,9.5) (#51)
4. Identify the σ and π bonds in bonding schemes (9.6) (#57)
Gases (Chapter 10): Be able to –
1. Use the following gas laws: Combined Gas Law, The Ideal Gas Law, Dalton’s
(10.3-10.6) (#26,39,51,59,63)
2. Use the Ideal Gas Law together with stoichiometry to calculate gas amounts in a
reaction not at STP (10.5) (#57)
3. Use the Kinetic Molecular Theory to explain properties of gases (10.7,10.8)
(#9,81,82)
4. Know and understand the conditions that lead to gases exhibiting non-ideal
behavior (10.9) (#91)
Liquids, Solids, and Intermolecular Forces (chapter 11,12): Be able to –
1. Interpret particulate drawings of liquids (11.1) (#1)
2. Predict properties of liquids based on the nature of their intermolecular forces
(11.2-11.3,11.5) (#17,26,35,51)
3. Calculate the heat associated with phase changes combined with temperature
changes (11.4) (#45)
4. Classify solids based on their bonding/intermolecular forces and understand how
differences in bonding relate to physical properties (12.1,12.3-12.7)
(#11,13,63,65)
Physical Properties of Solutions (chapter 13): Be able to –
1. Predict if a solutions is likely to form between a solute and solvent based on
intermolecular forces (13.1-13.3) (#7,15,33)
2. Distinguish between saturated, supersaturated, and unsaturated solutions (13.2)
(#23,25)
3. Describe the effects of temperature and pressure on the solubility of gases (13.3)
(#35,37)
4. Express solution concentration in molarity and mole fraction (13.4)
(#43,49a+c,53)