AP Chemistry Syllabi/Prospectus
2015-2016
Mr. Niedenzu
AP/IB Exam Policy:
As you are aware, CMS pays the exam fee for students to take AP and IB exams
Students must take the AP exam or take a teacher made exam at the end of the year that will count as 20% of
their final grade
Overview: The AP Chemistry course meets daily for one 90 minute period. Labs are conducted during the week on
alternating days. This course is designed to provide a solid, first-year college chemistry experience, both conceptually and in
the laboratory. The labs serve to supplement the learning in the lecture section of the course. Problem-solving skills, both
on paper and in the lab, are emphasized. There are weekly labs and during the last quarter three full practice AP tests are
taken and graded according to AP grading scale.
Laboratory: Students are required to submit a complete report for each lab experiment, including a hypothesis, procedure,
observations/data, calculations, sources of error, and a conclusion. All reports are kept in a lab notebook. The students are
also called upon to make a presentation to the class about their hypotheses, calculations, and conclusions – in this way
students can collaborate on the objectives and design of an experiment, and assist each other in reaching conclusions, and
gain insights into variance and sources of error. Lab descriptions are listed at end of syllabus after the resources.
Reaction sets: Are no longer part of the AP exam specifically but a good knowledge thereof is essential to answer some
questions.
Class rules
Students need to have access to the internet to access my website and other resources we will use during the year.
Cell phone use is not allowed during the school day – if I see it or hear it, it will be confiscated and turned in to the front
office.
No food is allowed in class. Only clear, colorless water bottles containing water will be permitted.
Cheating will not be tolerated.
Late work will have a letter grade deduction for each day late (unless there is some extenuating circumstance).
Behavior issues will be dealt with “in house” – the administration has many other things to deal with and I will handle these
issues as they arise. Also, be forewarned, I DO call parents at home and at work, and I will call you at home if you have been
absent or are absent to check on things.
Required materials:
materials for taking notes
scientific or graphing calculator
graph paper
colored pencils
Absences: I will follow the CMS guidelines on absences, please recheck your handbook on this.
If you are absent and want to stay current – email me immediately at school
kurt.niedenzu@cms.k12.nc.us
I will respond immediately!!!
Lab safety:
All students will undergo a review of lab safety rules and have to sign (along with the parents) that they have read the safety
rules, watched the safety video, know where all the safety equipment in the room is located and the proper way to use it.
Homework:
I do not assign a lot of homework at once – the problems I do assign are carefully selected – some of the assignments are
already on my web page, some will have answers with the questions.
Assignments/quizzes:
BEWARE: I will give short quizzes in class almost every day!!! I do give retakes on these if needed.
Missed assignments:
CMS allows you 5 days to schedule a time/due date to turn in missed assignments – remember it is your duty to take care of
this!
Grades:
I operate on the point system and generally most classes will have over 1000 points accumulated for each quarter.
Assignments will be listed as either formal (70% of the quarter grade) or informal (30% of the quarter grade) I will follow CMS
guidelines on grade distribution which this year is on a ten point scale where 100-90 is an A, 89-80 is a B, 79-70 is a C, 69-60 is
a D, below 60 is an F. Point distribution is as follows:
Quizzes: anywhere from 5 – 20 points
Homework: from 10 – 20 points
Lab reports: from 20 – 50 points
Tests: from 30 – 70 points
We will go over lab report format in class – be aware that this area is usually where many student’s grades suffer because
they do not turn in reports on time! In general you will have a week to turn in reports after the lab is done.
Tutoring:
The chemistry department will have weekly scheduled tutoring availability – the schedule will be given to you during the first
week of school. In the fall I have limited availability for tutoring due to coaching responsibilities. In the winter and spring I
will be available after school each day for help. Before school is an option this year since I have first block planning all year.
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
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)
D.
Assignments: Organic HW sets 1 p1091 #24 thru 40 even,and 2 p1093 #52-60 even, complex nomenclature
practice sheet, organic test, complex nomenclature qz, old reaction prediction sets involving organic
compounds;
E.
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
E.
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
Assignments: Homework set p337 # 40 thru 50 even, other practice problems and quizzes, test
Unit 3: Chemical Stoichiometry
Approximate number of days: 10
A.
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 (note new format on AP test for this year!!) – 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: % of Sulfate lab (gravimetric analysis), formula of hydrate lab (copper sulfate), molar ratio lab (single
replacement with copper sulfate solution and solid iron)
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.
Content:
C.
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
Unit 5: Chemical Bonding
Approximate number of days: 15
A.
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
B.
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
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
C.
Assignments:
Molecular model labs,
synthesis and analysis of alum lab, homework sets # 22-90
even (due various days, a and b only on those that have more two questions) p. 403-406, quizzes, test
D.
Labs: .Molecular model labs, synthesis and analysis of alum lab
Unit 6: Gases
A.
B.
C.
D.
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, Dumas method lab (molar mass of gas), R constant lab using decomposition
of potassium chlorate
Unit 7: Liquids and Solids
Approximate number of days: 7
A.
General aim:
To describe the intermolecular forces responsible for properties of liquids and solids and the
process of changing from one state to another.
B.
Content:
1. Intermolecular forces
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
C.
D.
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: Spec 20 lab and chromatography labs using column chromatography (use Beer’s law)
Unit 8: Thermochemistry/Thermodynamics
Approximate number of days: 10
A.
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
B.
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: Specific heat lab, heat of neutralization lab, 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, heat of neutralization lab
Unit 9: Solutions
Approximate number of days: 8
A.
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
B.
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
Calculations involving concentration of solutions
a. standard solutions
b. dilution of solutions
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: Freezing pt. depression lab, qualitative analysis lab, Reaction sets given each week during the
year on Mondays – due Friday (use old ones from AP tests and others); 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)
3.
C.
D.
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.
Assignments: Iodine clock reaction lab; 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
D.
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. 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
C.
Assignments: daily mini quizzes using Zumdahl’s red Equilibrium book
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
C.
D.
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
Assignments: we will be using the Zumdahl “redbook” to 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
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 of iodoform lab, Creating Danielle cells and concentration cells lab
Teaching Resources
Text: Steven Zumdahl and Susan Zumdahl, Chemistry, 6th edition (2003) ISBN 0-618-22156-5
Houghton Mifflin Company
222 Berkeley Street, Boston, MA 02116-3764
AP Chemistry workbook – Peter Demmin and David Hostage – Multiple-Choice & Free Response Questions in Preparation For
The AP Chemistry Examination, 5th Edition (2005)
D&S Marketing Systems, Inc.
1205 38th Street
Brooklyn, NY 11218
AP Chemistry workbook – John Moore and Richard Langley – 5 Steps to a 5 AP Chemistry, 1st edition (2004) ISBN 0-07141275-1
McGraw-Hill
Two Penn Plaza
New York, NY 10121-2298
AP Chemistry lab book – David Hostage and Martin Fossett, Laboratory Investigations AP Chemistry, 1 st edition (2006) ISBN
1-4138-0489-6
The People’s Publishing Group, Inc.
299 Market Street
Saddle Brook, New Jersey 07663
Multimedia – AP Chemistry Teacher’s Tools, www.FraneMedia.com 2nd edition 2005
PO Box 254
Pennington, NJ 08534-0254
Multimedia – AP Chemistry Neo/Lab Virtual Lab Software, www.neosci.com
PO Box 22729
Rochester, NY 14692-2729
Multimedia – www.apexvs.com
Apex Learning, Inc. (2006)
Chemistry AP Labs:
NOTE: all labs are hands on unless otherwise noted
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)
Determination of the Molecular Mass of a Volatile Liquid
Using the “Dumas” method, students will determine the molar mass of a small sample of a
volatile liquid. (1.5 hours – expect poor results on this one)
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 FeSCN 2+
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 hour)
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
7. synthesis of a coordination compound and its chemical analysis
8. separation by chromatography
(this lab can take up to 5 days to do, approximately 6 – 7 hours)