AP Chemistry
Semester Two Study Guide
Unit One: General Chemistry Review
Unit Two: Organic Nomenclature
Unit Three: Reactions
Unit Four: Thermochemistry
Unit Five: Atomic Structure
Unit Six: Bonding
Unit Seven: Solids, Liquids and Gases
Unit Eight: Kinetics
Unit Nine: Equilibria
Unit Ten: Electrochemistry
Unit Eleven: Nuclear
Unit Twelve: Thermodynamics
*Labs*
Mr. Gray
Rockwood Summit High School
2010-2011
1
The Real A.P. Chem Test
Vs.
The Semester 2 Final
The Real AP Chem Test
The AP Chem Semester 2 Final
1. Exam time is 185 minutes
1. Exam time is 110 minutes
2. Section I is 90 minutes
75 MC questions
50% of test grade
no calculators
periodic table provided
no other reference sheets
2. Section I is 55 minutes
45 MC questions
50% of test grade
no calculators
periodic table provided
no other reference sheets
3. Section II is 95 minutes
6 FR questions
50% of test grade
3. Section II is 55 minutes
5 FR questions
50% of test grade
Part A (55 min.)
3 Problems with calculator
#1 equilibria
(20%)
#2 and #3 are unknown (40%)
Part A (30 min.)
3 Problems with calculator
#1 equilibria
(20%)
#2 kinetics
(20%)
#3 unknown
(20%)
Part B (40 min.)
3 Questions without calculator
#4 chemical equations (10%)
#5 and #6 are essays
(30%)
Part B (25 min.)
2 Questions without calculator
#4 chemical equations (10%)
#5 unknown
(30%)
Periodic table provided
Equation sheet provided
Reduction potentials provided
#2,3,5,or6 will be lab question
Periodic table provided
Equation sheet provided
Reduction potentials provided
2
The Composition of Your Semester 2 Final Exam
Unit
Questions
on Final
Topics
1. Math
a. Significant figure rules for multiplying,
dividing, adding and subtracting
b. Multiplication and division of scientific
notation WITHOUT a calculator
2. The Atom
a. aXz notation, ions, isotopes,
b. how to calculate atomic mass
1. General Chemistry Review
4
3. Nomenclature
a. Ionic, covalent, hydrate, and acids
4. Stoichiometry
a. Be fluent with the ENTIRE mole map
(especially gases and liquids)
b. Problems: limiting reactants, percent yields,
titrations, determining concentration of any
species in solution, percent composition,
obtaining empirical and/or molecular
formulas from given data
2. Organic Nomenclature
3. Reactions
1
5. Nomenclature
a. Hydrocarbon chains and functional groups
b. isomers
3
6. Reactions
a. Know all types of reactions
(EVERY EXAMPLE) on green sheet
b. Net ionic reactions and solubility rules
c. Know oxidation rules, how to identify redox
reactions and how to balance redox
reaction using half reaction method; know
what an activity series is and how to
read/use it
d. Know the 6 strong acids and 9 strong bases
(because they are ions in solution)
3
4. Thermochemistry
5. Atomic Structure
3
3
7. Thermochemistry
a. Know the 1st Law of Thermodynamics
b. Draw and interpret enthalpy diagrams for
exo-/endo- thermic reactions
c. Calculate enthalpy by: energy diagrams,
thermochemical equations (using
dimensional analysis), calorimetry, Hess’
Law, Enthalpies of formation (data tables),
bond enthalpies
d. Know how to calculate specific heat and
heat capacity
e. Problems: calorimetry of acid/base, hot
metal dropped in cool liquid
8. Electronic Structure of the Atom
a. Know something about the research of
Bohr, Rutherford, and Millikan and others
b. Basic wave calculations, parts and sequence
of electromagnetic spectrum
c. Explanation of line spectra, Planck’s formula
for quantizing energy (also Einstein’s energy
of electron), Bohr model of atom
d. Calculate transition energy in Hydrogen
e. Quantum numbers, orbital diagrams,
electron configurations and how they
correspond to periodic table (Aufbau,
Hund's, Pauli rules)
9. Periodic Table
a. Trends (atomic radii, ion size,
electronegativity, ionization energy,
electron affinity, metallic character)
6. Bonding
4
10. Bonding
a. Ionic, covalent, metallic, lattice energy,
coordinate covalent, characteristics of
multiple covalent bonds, bond polarity
(based on electronegativity)
b. Lewis structures, formal charges,
resonance, octet rule and exceptions
c. VSEPR Theory (molecular shapes), and
Valence Bond Theory (hybridization),
molecular polarity
4
11. IMF
a. Strengths of intermolecular forces and how
they relate to properties (b.p, m.p., surface
tension, viscosity, vapor pressure, etc)
b. Rank substances in order of their melting or
boiling points
c. Enthalpy of phase changes and graphs
d. Vapor pressure curves, cooling curves,
solubility curves and phase diagrams
7. Solids, Liquids, Gases
6
12. Gases
a. All gas laws, especially Ideal, Dalton,
Graham’s and Avogadro’s
b. Use Ideal gas law to solve for molar mass
and density
c. Kinetic Molecular Theory
d. Ideal vs. Non ideal gas
13. Solutions
a. Factors that affect solubility of solids,
liquids and gases
b. Units of concentration (molarity, molality,
mole fraction, percent mass,etc.)
c. Colligative properties (vapor pressure,
freezing point, boiling point, osmotic
pressure, Raoult’s law)
8. Kinetics
5
14. Kinetics
a. General knowledge about rates and rate
laws (4 things that increase rate, initial rate
law method and integrated rate laws)
b. Know how to verify the plausibility of a
mechanism based on the rate determining
step (RDS)
c. Collision theory and transition state theory,
activated complex, stability, catalysts and
intermediates
5
9. Equilibria
10. Electrochemistry
6
4
15. Basic Equilibrium Concepts
a. Write equilibrium constant expressions for
homo- and hetero- geneous equilibria
b. Use the Reaction Quotient, Q, to determine
if at equilibrium or the direction a system
will shift to reach equilibrium
c. LeChatelier’s principle (what will shift an
equilibrium and which way will it go)
d. ICEBOX problems
16. Acid-Base Equilibria
a. Compare and contrast 3 acid-base theories
b. Determine acid/base strength based on
molecular structure or Ka/Kb value
c. Determine if a salt will hydrolyze to make
solution acidic or basic and write the
equation for the process
d. Be familiar with pH, know all the “square of
pHun” calculations
e. Solve ICEBox problems with common ion
effect, buffers, weak acids and bases
f. Calculate pH and concentrations of acids
and bases during all parts of a titration,
calculate the equivalence point using
MaVa=MbVb
17. Solubility
a. Write solubility equations, calculate Ksp,
solubility, and molar solubility
b. Know how to use selective ion precipitation
as a tool to separate ions; calculate which
ion will precipitate first and what % remains
when second ion precipitates
18. Redox and Voltaic Cells
a. Assign oxidation numbers and balance
redox equations and half reactions
b. Draw and label voltaic cells
c. Use standard reduction potentials to
calculate Ecell
19. Ecell and Spontaneity
a. Relate Ecell to G and Kc; predict spontaneity
of a cell
b. Use Nernst equation to calculate Ecell at
non-standard conditions
c. Electrolytic cells (sketch and label; calculate
how much solid will form from given
amperage and time)
6
11. Nuclear
12. Thermodynamics
2
4
20. Nuclear
a. Types of radioactive emissions (which
particles are involved and how they form)
b. Write balanced nuclear equations for
emission/fission/fusion processes, know aXz
notation for each particle
c. Use belt of stability to predict stability or
type of decay that will occur
d. Calculate half life or amount of parent
material remaining after several half lives
21. Enthalpy, Entropy and Free Energy
a. Know endothermic/exothermic reactions
and their H signs; exothermic reactions
are favored in our universe
b. Know the main 3 things that increase
entropy, S; increases in entropy are
favored in our universe
c. Know Gibbs’ free energy equation to use
enthalpy and entropy to determine if and
when a process is spontaneous; know
when temperature plays a role in
spontaneity
d. Calculate the crossover temperature
e. Relate G to Kc
13. Labs – Concepts from any lab we have performed in General, Honors, or AP Chemistry could
appear in any question.
a. Be familiar with proper lab and safety techniques, common errors and outcomes of all labs
we did (volumetric glassware, aspirin/gravimetric analysis, emp/mol formulas, titrations,
calorimetry/heat of neutralization, molar mass of volatile liquid, chromatography,
spectrophotometry/Beer's law, heat of vaporization, molecular mass of unknown liquid),
kinetics of a reaction, calculating Kc using a spectrophotometer, acid-base titrations,
calculating Ksp, making voltaic cells
7
Things You Should Have Memorized
1. Element names and symbols
2. Polyatomic ion names, formulas, and charges
3. All Reaction types
4. Solubility rules
5. All VSEPR shapes and angles
6. Mole map
7. Organic functional groups (names and general formula for identification)
8. Organic hydrocarbon chain prefixes (meth, eth, prop, but, etc.)
9. 6 Strong acid names and formulas
10. 9 Strong base names and formulas
11. Parts of the EMS in order from low to high energy
12. Every type of IMF and their relative strengths
13. Periodic Trends
14. Colors of common flame tests and precipitates
8
9
10