CHEMISTRY II – ADVANCED PLACEMENT
2011-2012 SYLLABUS
COURSE OVERVIEW: AP Chemistry meets every day during the school year for a 90
minute block. Students receive a packet of work to complete over the summer that is
due the first day of school. This reinforces the fundamentals learned in Chemistry I. AP
Chemistry is a rigorous class that includes laboratory work at least once a week. This
class is designed to give high school students the same experience they would receive in a
first year college chemistry course. A major emphasis of this course is problem solving,
which must be practiced in both lab and daily in class work. Two full length AP practice
exams will be given during the 4th quarter and graded according to the AP scale in
preparation for the exam in May.
LABORATORY: Lab experience is essential to a thorough understanding of a concept in
any science class. For each experiment, students are required to submit a formal report
which includes a hypothesis, procedure, observations and data, calculations, sources of
error, and a conclusion. For several experiments students may be called on to present
any aspect of their report and lab experience to the rest of the class. This allows students
to critique each other and collaborate on concepts and make connections between
concepts with others.
REACTION PREDICTION SETS: Reaction prediction is a concept that is stressed in this
course. Reaction prediction is practiced daily in this class with warm ups after the second
unit and weekly problem sets which students turn in at the end of the week. I use
problems from old AP Exams as well as those found in several college textbooks. In
response to the change in format of Section II on the exam this year, students must also
answer two questions about each reaction (ex- precipitate color).
Unit 1: Chemical Fundamentals
Approximate number of days: 5
A.
General aim:
To describe the properties of matter, scientific matter, and chemical
calculations. Students should become familiar with the various pieces of lab
equipment, working with sig figs, metric system, naming compounds, the
mole concept
B.
Content:
1. Nomenclature
a. Inorganic nomenclature
b. Organic nomenclature
i. give examples of alkanes, alkenes, alkynes, aromatics
and aliphatics
ii. review structural formulas and functional groups
iii. review IUPAC nomenclature system
c. Transition Metals and Coordination chemistry - Complex
nomenclature
C.
Content:
1. English and metric systems
2. SI units and prefixes
D.
E.
3. Precision and accuracy
4. Fahrenheit, Celsius, and Kelvin temperature scales
5. Conversion factors
6. Density calculations
7. Classification of matter into subgroups
8. Properties of matter
9. Separation of mixtures
10. Significant figures – on AP test allowed +/- one figure (put 3 and
you will be ok most of the time)
Assignments: Organic HW sets 1 p1091 #24 thru 40 even,and 2 p1093 #5260 even, complex nomenclature practice sheet, organic test, reaction
prediction sets involving organic compounds for warm ups
Labs: synthesis and analysis of aspirin lab – also Lab Safety Rules and
procedures
Unit 2: Atomic Structure and the Periodic Table
Approximate number of days: 10
A.
General aim:
To gain an understanding of the development of atomic structure.
B.
Content:
1. Basic assumptions of Dalton’s atomic theory
2. J.J Thompson’s determination of charge-to-mass ratio
3. Millikan’s oil drop experiment
4. Rutherford’s nuclear atom
C.
General aim: To study nuclear particles, half life and radioactive decay.
D.
Content:
1. Characteristics of radiation
a. alpha particles
b. beta particles
c. positron production
d. electron capture
e. gamma radiation
2. Nuclear stability
a. zone of stability
b. magic numbers
3. Rate of decay
a. half-life
b. first-order process
4. Transformations
a. accelerators
b. synthesis of some transuranium elements
5. Detection
a. Geiger counter
b. scintillation counter
c. radiocarbon dating
6. Binding energy-mass defect
7. Nuclear fission
a. chain reaction
b. critical mass
8. Nuclear fusion
9. Nuclear reactors
E.
Assignments: Homework set p337 # 40 thru 50 even, other practice
problems and quizzes, test, periodic trends project
Unit 3:
A.
Chemical Stoichiometry
Approximate number of days: 10
General aim:
To calculate quantities of materials reacted or produced in chemical
reactions. Students will also apply the periodic law to chemical reactivity
in predicting products along with discussing the activity series of the
elements, distinguish between metals and nonmetals, use the properties of
metals and nonmetals to predict reaction products including using the
activity series to predict single replacement reactions. Also use the periodic
table to predict common oxidation states.
B.
Content:
1. Mole concept
2. Percent composition
3. Determination of the empirical and molecular formula for a
compound
4. Write and balance equations for:
a. combustion reactions
b. synthesis reactions
c. decomposition reactions
d. single replacement reactions
e. double replacement reactions
f. begin practicing reaction predictions – 3 given, have to do all
three, balance and answer other questions on them – used to
pick 5 of 8 with no balancing or other questions
5. Mass-mass calculations
6. Calculations involving a limiting reagent
7. Calculation of percent yield
C.
Assignments: homework sets 1 page 124 # 34 – 58 even, set 2 page 125 #
60 – 96 even (a,b only), test, first sets of reaction prediction
D.
Labs: formula of hydrate lab (copper sulfate), molar ratio lab
Unit 4:Electronic structure and Periodicity(see also stoichiometry general aim)
Approximate number of days: 6
A.
General aim:
To describe the electronic arrangement within an element and to
account for the periodicity of elements. Students should be able to name
the major subatomic particles in an atom, types of radioactive emissions,
discuss the Bohr model and the other models, work problems involving
quantum numbers and energies of electron transitions, the various Rules
and Principles, shapes of orbitals, basics of the periodic law, work problems
involving nuclear binding energy and half-life, balance nuclear equations
B.
C.
Unit 5:
A.
B.
Content:
1. Electromagnetic radiation: wavelength, frequency, velocity
2. Planck’s constant: energy and frequency
3. Dual nature of light
4. Bohr model
5. Heisenberg’s uncertainty principle
6. Electron probability distribution
7. Quantum numbers and electron orbitals
8. Paramagnetic vs. diamagnetic
9. Shapes of probability charge clouds for s, p, d, f orbitals
10. Pauli’s exclusion principle
11. Wave mechanical model
12. Aufbau principle
13. Hund’s rule
14. Electron configurations and dot diagrams for atoms
15. IUPAC periodic table
16. Effective nuclear charge and shielding
17. Periodic trends in ionization energy, electron affinity, atomic and
ionic radius
18. Properties of elements by their periodic table group
19. Lanthanide contraction
20. Colors- solutions/flame tests/precipitates/elements, especially
transition metal salts
Assignments: flame test demo, homework set 1 page 338 # 52,60,62
64,66, 68-80 even, set 2 page 340 #86-96 even; test
Chemical Bonding
Approximate number of days: 15
General aim:
To characterize chemical compounds according to the type of
bonding and the structure of molecules. Students should be able to draw
Lewis structures, use electronegativity to predict bond types, distinguish
between polar and nonpolar, ude bonding principles to determine
oxidation states, draw resonance structures, assign formal charge, compare
VB theory to MO theory, use VSEPR, draw MO diagrams and identify
hybridization.
Content:
1. Types of chemical bonds
a. why an ionic bond forms
b. why a covalent bond forms
c. electronegativity
d. polar bonds, dipole moment
2. Ionic bonds
a. electron configurations
b. formulas
c. lattice energy
3. Covalent bonds
a. localized electron-pair model
C.
D.
Unit 6:
A.
B.
C.
D.
Unit 7:
A.
B.
i. bond energy
ii. Lewis structures
iii. octet rule and exceptions
iv. molecular geometry, VSEPR, sigma and pi bonds
v. formal charge
b. shortcomings of valence bond theory: resonance
c. molecular orbital model
i. bond order
ii. delocalization of orbitals
4.
Isomerism
a. Geometric isomers
b. Stereoisomers
Assignments: Molecular model lab,
synthesis and analysis of alum
lab, homework sets # 22-90 even (a and b only on those that have more
than two questions) p. 403-406, quizzes, test
Labs: .Molecular model labs, synthesis and analysis of alum lab
Gases
Approximate number of days: 8
General aim:
To investigate the laws and models that describe the properties and
behavior of gases. Students should know the kinetic-molecular theory,
intermolecular forces, units used in gas law problems, interpret phase
diagrams and solubility curves along with working out gas law problems
Content:
1. Measuring pressure: units, manometers and barometers
2. Gas laws: Boyle, Charles, Guy Lussac, Avogadro, Ideal, Dalton,
Graham
3. Gas stoichiometry
a. STP
b. molar volume
c. mass-volume calculations
4. Kinetic-molecular theory
a. explain properties of gases
b. define temperature
5. Real gases
a. deviation from ideal behavior
b. van der Waals correction
Assignments: homework sets 1,2,3 (set 1 p. 233 32-46 even, set 2 48-60
even, set 3 64-80 even) gas test; old AP essay questions
Labs: Molar volume of gas lab
Liquids and Solids
Approximate number of days: 7
General aim:
To describe the intermolecular forces responsible for properties of
liquids and solids and the process of changing from one state to another.
Content:
1. Intermolecular forces
C.
D.
Unit 8:
A.
B.
a. dipole-dipole forces
b. hydrogen bonding
c. London dispersion forces
2. Properties of the liquid state
a. surface tension
b. capillary action
c. viscosity
d. vapor pressure
3. Types of solids
a. amorphous
b. crystalline cubic forms, close-packed forms
4. Determination of crystal structure
5. Bonding in metals
a. electron-sea model
b. band model
6. Network atomic solids
a. properties of carbon and silicon
b. semiconductors
7. Comparison of types of solids and properties
8. Changes of state
a. specific heat
b. freezing point
c. boiling point
d. heat of fusion
e. heat of vaporization
9. Heating curve
10. Phase diagrams
a. water
b. carbon dioxide
Assignments: homework sets page p. 500 – 505, # 36 – 90 even over
several days; test; magnet demo; old AP essay questions; sodium
polyacrylate demo (“waterlok”)
Lab: Beer’s Law lab using a Spec 20
Thermochemistry/Thermodynamics
Approximate number of days: 10
General aim:
To relate the fundamental aspects of the energy changes that
accompany chemical reactions. Students should be able to solve problems
involving Hess’s law, heat problems, calorimetry problems and
interconvert with electro and equilibrium problems
Content:
1. Concept of energy
a. potential energy, kinetic energy
b. first law of thermodynamics
c. heat
d. work
e. state functions
f. system and surroundings
g. endothermic and exothermic reactions
h. internal energy of a system
2. Calorimetry
a. use of a calorimeter
b. heat capacity
c. energy released as heat
3. Enthalpy change for a chemical reaction
a. Hess’s law
b. standard enthalpies of formation
c. heat of reaction, e.g., heat of combustion
C.
General aim:
To predict whether or not a process is spontaneous, based on
properties of the reactants and products.
D.
Content:
1. Second law of thermodynamics
2. Spontaneity of process determined by entropy calculations
3. ∆Gsurroundings = -∆Hsystem / T
4. Calculation of ∆G for a process from standard free energies of
formation
5. ∆G = ∆H - T∆S
6. Predicting spontaneity from ∆G
7. Calculation of ∆G at conditions other than standard temperature
8. Predicting spontaneity from sign notation of enthalpy and entropy
9. Calculation of Keq from ∆G
E.
Assignments: old AP essays, homework set 1 p. 819 #20-50 even, set 2 p.
282 #34-62 even, quizzes, test
F.
Lab: Specific heat lab, Determination of the Thermodynamic Principles of
the Dissolution of Borax lab
Unit 9:
A.
B.
Solutions
Approximate number of days: 8
General aim:
To investigate the properties of solutions. Students should also be
able to work out problems involving different concentration units,
interpret solubility curves, work out problems involving colligative
properties
Content:
1. Solution composition: mass percent, molarity, molality, normality,
mole fraction
2. Nature of solutions
a. water as a solvent
b. strong and weak electrolytes
c. concentration expressed as molarity
d. solubility rules for salts in water
3. Calculations involving concentration of solutions
a. standard solutions
b. dilution of solutions
C.
D.
4. Calculations involving reactions in solutions
5. Heat of solution
a. lattice energy
b. hydration energy
6. Factors that affect solubility
a. structure of solute and solvent
b. pressure
c. temperature
7. Factors that affect vapor pressure
a. concentration
b. solute-solvent interactions
8. Colligative properties
a. freezing point depression, boiling point elevation, electrolytes
b. osmosis
c. applications
d. van’t Hoff factor
Assignments: homework sets 1 p. 181 #20 – 66 even, set 2 p. 547 # 12-70
even; test
Labs: Freezing pt. depression lab, qualitative analysis lab (identification of 6
unknown cations)
Unit 10: Chemical Kinetics
Approximate number of days: 7
A.
General aim:
To measure, alter, and predict the rates of chemical reactions.
B.
Content:
1. Reaction rates
a. definitions and units
b. instantaneous rates from plot of concentrations versus tie
c. factors that affect rate: concentration, temperature, catalyst
d. potential energy diagram for a reaction
2. Integrated rate law
a. equations relating concentration and time
b. reaction order determined form the plot needed to give a
straight line
c. determination of overall order
3. Reaction mechanism
a. molecularity
b. rate-determining step
c. distinguishing between catalyst and intermediates in
mechanism
4. Collision model
a. activation energy: Arrhenius equation
b. molecular orientations
5. Catalysts: homogeneous and heterogeneous
6. Half-life (first order for common nuclear)
C.
D.
Assignments: old AP essay test (focus on finding rate law and rate constant
when given a table of experimental values); methylene blue demo,
homework p. 598 #22-60 even, quizzes, test
Lab: Iodine clock reaction lab, bromate clock reaction lab, thiosulfate lab
Unit 11: Chemical Equilibrium, Part I
Approximate number of days: 7
A.
General aim:
To investigate the characteristics of chemical equilibrium. Students
should be able to solve equilibrium problems involving gases and solutions,
understand the meaning of Q and K, understand LeChatelier’s principle to
predict shifts; how temperature, pressure, concentration, catalysts affect or
do not affect equilibrium
B.
Content:
1. System at equilibrium
a. rates of forward and reverse reactions
b. composition of equilibrium mixture
c. law of mass action
d. equilibrium expression
e. equilibrium constant
2. Calculation of concentrations that characterize a given equilibrium
position
a. homogeneous equilibria
b. heterogeneous equilibria
c. Kc and Kp
3. Applications of K
a. to predict extent of reaction
b. to calculate equilibrium concentrations given initial
concentrations
4. Le Chatelier’s principle
a. change in concentration
b. change in pressure
c. change in temperature
C. Assignments: LeChatelier’s principle lab with copper chloride (can tell shift by
color changing greener or bluer), daily mini test assignments using Zumdahl’s
Equilibrium book (red)
D. Lab: LeChatelier’s principle lab with copper chloride (can tell shift by color
changing greener or bluer), Ksp of magnesium oxalate lab by titrating with
standardized potassium permanganate
Unit 12: Equilibrium, Part 2 - Acids and Bases
Approximate number of days: 10
A.
General aim:
To apply chemical equilibrium principles to the interactions of acids
and bases.
B.
Content:
1. Acid-base models
a. Arrhenius
b. Bronsted-Lowry
C.
c. Lewis
2. Equilibrium constants and acid strengths
3. Calculation of H for weak and strong acids and bases
4. Dissociation of water
a. Kw
b. amphoterism
5. Hydrolysis of salt solutions
a. Kh
b. equilibrium expression
6. Acidic and basic oxides
Assignments: quizzes at the end of each class
Unit 13: Equilibrium, Part 3- Aqueous Equilibria Approximate number of days: 10
A.
General aim:
To make aqueous equilibria calculations involving buffers, solubility
products, and complex ions.
B.
Content:
1. Common ion effect
a. acid dissociation equilibrium
b. buffered solutions
c. solubility of ionic solids
2. Buffered solutions
a. characteristics
b. calculation of pH
c. Henderson-Hasselbach equation (use whenever you can!)
d. buffer capacity
3. Titration curves
a. strong acid-strong base
b. weak acid-strong base
c. strong acid-weak base
d. polyprotic acids
e. indicators
4. Solubility product
a. calculation of Ksp given salt solubility
b. calculation of salt solubility given Ksp
c. calculation of salt solubility in solution containing a common
ion
d. selective precipitation
5. Complex ions
a. equilibrium principles
b. effect on the solubility of a salt
C.
Assignments: we will be using the Zumdahl “redbook” to go through four
subunits on equilibrium and we will be answering all the mini test in each
chapter along with unit tests at the end of each chapter; unit 1 test on
general equilibrium, unit 2 test on acid-base equilibrium, unit 3 test on
buffers and titrations, unit 4 test on Ksp; old AP essay questions, quizzes,
test
D.
Lab: spec-20 Ksp lab, Ka lab with pH meters
GREEN CRYSTAL LAB – after equilibrium we will take about 6 days to do the crystal lab
which covers at least 8 of the lab components on the AP requirement list (see description
in lab section)
Unit 14: Electrochemistry
Approximate number of days: 7
A.
General aim:
To consider the theoretical basis of oxidation-reduction reactions.
B.
Content:
1. Oxidation-reduction equations
a. half reactions
b. oxidizing agent and reducing agent
c. balanced net equation
2. Electrochemical cell
a. sketch and label
b. anode-oxidation
c. cathode-reduction
d. cell potential
e. examples of common galvanic cells
3. Electrolytic cell
a. sketch and label
b. predicting products of reactions at anode and cathode
4. Standard electrode potentials
a. relative to potential of standard hydrogen electrode
b. comparison of strength of oxidizing agents
c. Nernst equation for nonstandard conditions
d. predict direction of spontaneous change
5. Cell voltage used to determine ∆G
6. Cell voltage used to determine Keq
7. Faraday’s laws of electrolysis
8. Applications of electrolysis
9. Stoichiometric calculations
a. equivalent weight
b. normality of oxidizing and reducing agents
C.
Assignments: homework p. 868 # 16 – 80 even (over various days), voltaic
cell demo, voltaic cell simulations, electrolysis demo, old AP essays, quizzes,
test
D.
Lab: electrolytic synthesis lab, concentration cells lab
Teaching Resources
Text: Steven Zumdahl and Susan Zumdahl, Chemistry, 6th edition (2003) ISBN 0-61822156-5
Houghton Mifflin Company
222 Berkeley Street, Boston, MA 02116-3764
Problem Sets- G. Gilbert Long and Forrest C. Hentz- Problem Exercises for General
Chemistry, 3rd edition (1986) ISBN 0-471-82840-8
John Wiley & Sons, Inc.
New York, NY
AP Chemistry lab book – David Hostage and Martin Fossett, Laboratory Investigations
AP Chemistry, 1st edition (2006) ISBN 1-4138-0489-6
The People’s Publishing Group, Inc.
299 Market Street
Saddle Brook, New Jersey 07663
Chemistry AP Labs:
NOTE: all labs are hands on & full participation is expected.
Determining the Heat Capacity of an unknown metal
Using the concept of the conservation of energy, students will determine the heat
capacity of an
unknown metal by heating a weighed sample, then placing it into a weighed amount of
water in a
calorimeter and recoding the temperature change. (1 hour)
Finding the Formula of a Hydrate
Students will heat a weighed sample of a hydrate. Using the mass of the anhydrous
sample, students will determine the moles of water and moles of anhydrous compound.
(if you do copper sulfate 1.5 hours, if part of green crystal lab – making crystal 1.5 hours,
hydrate part will take parts of two periods for about 2 hours)
Finding the Ratio of Moles of Reactants in a Chemical Reaction
Students will mix a series of solutions, producing an exothermic reaction. Based on the
mixture that
produces the most heat, students can determine the stoichiometric ratio. (1.5 hours)
Synthesis and Analysis of an Alum
Students will synthesis potassium aluminum sulfate (or some other “alum”). Students will
then run several tests to determine the purity of the sample. (3.0 hours)
Determining the Molar Volume of a Gas
Students react a known mass of magnesium ribbon with an excess of concentrated
hydrochloric acid solution. They collect the hydrogen gas over water and calculate the
molar volume once they have accounted for the different factors that affect pressure. (1
hour)
Thermochemistry and Hess’s Law
Through a series of acid-base reactions, students will determine the heat of
neutralizations for each
reaction. From these values, they can then verify Hess’s Law. (1.5 hours)
Working with Molecular Models - Understanding the VSEPR Theory
Students will use kits to build models of various molecules in order to show the different
shapes.
Students should understand how lone pair electrons impact the shape of the molecule.
(1.5 hours)
Solving for the gas constant R
Using the vanderWaals equation and decomposing potassium chlorate to produce
oxygen gas you can solve for the gas constant R (1.5 hours – should get good results if
carefull)
Determination of the Molecular Mass by Freezing Point Depression
Using a computer simulation, students will investigate the effect of adding solutes to
solvents.
The van’t Hoff factor for electrolytes will be investigated. (1.5 hours)
Study of the Kinetics of a Reaction
Students will determine the order of an iodine clock reaction and observe what factors
affect the rate of a reaction. (1.5 hours)
Working with Molecular Models - Understanding Intermolecular Forces
Students will use kits to build models of various molecules in order to show the different
shapes.
Students should understand how the arrangement of the atoms in these molecules
determines whether or not the molecule is polar. (1.5 hours)
Determination of the Equilibrium Constant for the Formation of FeSCN2+
by Spectrophotometric Analysis
Using Beer’s Law, students will prepare a series of standards. Then a second set of
solutions are prepared in which concentrations of each reactant are varied. (1.5 hours –
other things can be used – thymol blue with different acid concentrations can be used)
Determination of the Dissociation Constant of a Weak Acid
Using a pH meter during an acid-base titration, students will determine the dissociation
constant of a weak monoprotic acid by titrating it against a strong base. (1.5 hours)
LeChatelier’s Principle - Studying Factors that Affect Equilibrium
Students will study the effect of temperature, concentration changes, and the effect of a
catalyst
on the position of a reaction. (1.5 hours – copper chloride is good for this one)
Acid-Base Titrations - Strong Acid with a Strong Base vs. Weak Acid with a Strong Base
Students will run a series of acid-base titrations using a pH meter in order to observe the
differences between a neutralization reaction between a strong acid with a strong base
versus a weak acid with a strong base. The concept of buffers will be introduced. (3.0
hours)
Working with Molecular Models - Study of Organic Functional Groups
Students will use kits to build models of simple organic functional groups such as alkanes,
alkenes, alcohols, and esters. (1 hour)
Synthesis and Analysis of Aspirin and an Ester
Students will synthesize aspirin and then analyze it for purity and will also produce an
ester. (Parts of three days, 3 hours)
Qualitative Analysis Lab
The students are given 6 cations to separate and run verification test on
(Mn,Cu,Ag,Fe,Al,Zn) and then are given an unknown sample of a combination of these
and are asked to identify using a qualitative analysis scheme. (Parts of four days, 5 – 6
hours total)
“Green Crystal Lab” - Synthesis and Analysis of a complex of an iron complex salt
This lab incorporates several of the labs suggested by the AP program, including the
following:
1. the determination of the formula of a compound
2. determination of the percentage of water in a hydrate
3. standardization of a solution using a primary standard (NaOH with KHP)
4. determination of concentration by acid-base titration, including a weak acid or weak
base
5. determination of concentration by oxidation-reduction titration (oxalate with
permanganate)
6. determination of mass and mole relationship in a chemical reaction