AP Syllabus
TEXT
Chemistry, Matter and Change by Steven S. Zumdahl. 9th Edition, McGraw-Hill, 2015.
ISBN 9781133611097.
GENERAL INTRODUCTION
AP Chemistry is a two-semester course which provides an in-depth overview of chemical concepts and is intended to be the equivalent of a general chemistry course taken the first year of college. It is a fast paced course requiring outside class study time. There will also be projects requiring research time outside of class. It is intended to be more vigorous than ordinary Chemistry courses and is intended to prepare students for their AP Chemistry College Board exam in May. The course is structured around the six Big Ideas as outlined by the College Board.
REQUIRED MATERIALS
Graphing calculator, 3 subject Notebook, headphones, pens, pencils, lab safety googles (optional)
LABS
The labs completed require following or developing processes and procedures, taking observations, and data manipulation. See lab list provided for lab details. Students communicate and collaborate in lab groups; however, each student writes a laboratory report in a lab notebook for every lab they perform. A minimum of 25% of student contact time will be spent doing hands-on laboratory activities.
COURSE DESIGN
Big Idea 1:
Structure of Matter – the chemical elements are fundamental building blocks of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions.
Big Idea 2:
Properties of Matter - Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them.
Big Idea 3:
Chemical Reactions - Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons.
Big Idea 4:
Rates of Chemical Reactions - Rates of chemical reactions are determined by details of the molecular collisions.
Big Idea 5:
Thermodynamics - The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
Big Idea 6:
Equilibrium - Any bond or intermolecular attraction that can be formed can be broken.
These two processes are in a dynamic competition, sensitive to initial conditions and external perturbations.
THE 10 PARTS OF A LAB REPORT
A specific format will be given to the student for each lab. Students must follow that format and label all sections very clearly. AP Chemistry lab reports are much longer and more in depth than the ones completed in the first year chemistry course. Therefore, it is important that students don’t procrastinate when doing pre-lab and post-lab work. Late labs will not be accepted. Labs not completed in class must be done at lunch or before/after school by appointment.
Pre-Lab Work
Pre-lab work is to be completed and turned in on the day the lab is performed.
1. Title
The title should be descriptive. For example, “pH Titration Lab” is a descriptive title and “Experiment 5” is not a descriptive title.
2. Date
This is the date the student performed the lab.
3. Purpose
A purpose is a statement summarizing the objective of the lab.
4. Procedure Outline
Students need to write an outline of the procedure. They should use bulleted statements or outline format to make it easy to read. If a student is doing a guided inquiry lab, they may be required to write a full procedure that they develop.
5. Pre-Lab Questions
Students will be given questions to answer before the experiment is performed. They will need to completely answer each question while incorporating the question into the answer. It is important to produce a good record of lab work.
6. Data Tables
Students will need to create any data tables or charts necessary for data collection in the lab.
During the Lab
7. Data
Students will record all their data directly in their lab notebook. Do not use a separate “data” sheet. Students will label all data clearly and include proper units of measurement. This section should be extremely organized and clear.
Post-Lab Work
8. Calculations and Graphs
Students should show how calculations are carried out. Graphs need to be titled, axes need to be labeled, and units need to be shown on the axis. To receive credit for any graphs, they must be at least a quarter page in size.
9. Conclusions
This will vary from lab to lab. Students will usually be given a prompt on what to write, but it is expected that all conclusions will be reasoned and succinct.
10. Post Lab Error Analysis Questions
Follow the same procedure as for Pre-Lab Questions.
THE LAB NOTEBOOK
A record of lab work is an important document, which will show the quality of the lab work that students have performed.
COURSE OUTLINE
Unit 1: Chemistry Fundamentals
Topics Covered:
1. Scientific Method
BI 1.D.1:a
2. Classification Matter
a. pure substances vs mixtures
1.A.1:b
b. law of definite proportions
1.A.1:c
c. law of multiple proportions
1.A.1:d
d. chemical and physical changes
3.C.1:b, 3.C.1:c, 5.D:2
3. Nomenclature and formula of binary compounds
1.E.2:b
4. Polyatomic ions and other compounds
1.E.2:b
5. Determination of atomic masses
1.A.1:a
6. Mole concept
1.A.3:b, 1.A.3:c, 1.A.3:d, 1.E.2:b
7. Percent composition
1.A.2:a
8. Empirical and molecular formula
1.A.2:b
9. Writing chemical equations and drawn representations
1.E.1:a, 1.E.1:c, 3.C.1:a
10. Balancing chemical equations
1.A.3:a, 1.E.2:c, 1.E.2:d, 3.A.1:a
11. Applying mole concept to chemical equations (Stoich)
1.A.3:a, 1.E.1:b
12. Determine limiting reagent, theoretical and % yield
3.A.2:a
Labs:
Math & Measurement in Science
LO 1.3; SP 2, 5
*Guided Inquiry: Physical and Chemical Properties
LO 1.17, 1.18; SP 1, 3, 4, 6
Stoichiometry Lab
LO 1.1, 3.3, 3.4; SP 2, 5
Unit 2: Types of Chemical Equations
Topics Covered:
1. Electrolytes and properties of water
2.A.3:h
2. Molarity and preparation of solutions
1.D.3:c, 2.A.3:i, 2.A.3:j
3. Precipitation reactions and solubility rules
6.C.3:d
4. Acid Base reactions and formation of a salt by
1.E.2:f, 3.A.2:c
titration
5. Balancing redox
3.B.3:a, 3.B.3:b, 3.B.3:c, 3.B.3:d
6. Simple redox titrations
1.E.2:f
7. Gravimetric Calculations
1.E.2:e
Labs:
pH Titration Lab
LO 1.2; SP 2, 5
Bleach Lab
LO 1.18, 3.8, 3.9; SP 2, 5
Activity: Online Redox Titration Activity [CR3c]
LO 3.9; SP 1
Unit 3: Net Ionic Equations
Topics Covered:
1. Redox and Single Replacement Reactions
3.A.1, 3.B.3:e, 3.C.1:d
2. Double Replacement Reactions
3.A.1, 3.C.1:d
3. Combustion Reactions
3.A.1, 3.B.3:e
4. Addition Reactions
3.A.1, 3.B.1:a
5. Decomposition Reactions
3.A.1, 3.B.1:a, 3.C.1:d
Labs:
Copper Reactions Lab
LO 1.4, 3.1, 3.2, 3.5, 3.6, 3.10; SP 6
Unit 4: Gas Laws
Topics Covered:
1. Measurement of gases
2. General gas laws - Boyle, Charles, Combined and Ideal
2.A.2:a, 2.A.2:c
3. Dalton's Law of partial pressure
2.A.2:b
4. Molar volume of gases and Stoichiometry
3.A.2:b
5. Graham’s Law
6. Kinetic Molecular Theory
2.A.2:d, 5.A.1
7. Real Gases and deviation from ideal gas law
2.A.2:e, 2.A.2:f, 2.A.2:g, 2.B.2:c, 2.B.2:d
Demonstration:
Graham’s Law Demonstration
LO 2.6; SP 1, 6
Labs:
Molecular Mass of a Volatile Liquid
LO 2.4, 2.5, 5.2; SP 2, 5
Unit 5: Thermochemistry
Topics Covered:
1. Law of conservation of energy, work, and internal energy
5.B.1, 5.E.2:a
2. Endothermic and exothermic reactions
3.C.2, 5.B.3:e, 5.B.3:f
3. Potential energy diagrams
3.C.2, 5.C.2:c, 5.C.2:d, 5.C.2:e
4. Calorimetry, heat capacity and specific heat
5.A.2, 5.B.2, 5.B.3:a, 5.B.3:b, 5.B.4
5. Hess's law
5.B.3:a
6. Heat of formation/combustion
5.C.2:g
7. Bond Energies
2.C.1:d, 5.C.1, 5.C.2:a, 5.C.2:b
Labs:
*Guided Inquiry: Hess’ Law Lab
LO 3.11, 5.3-5.5, 5.7, 5.8; SP 2, 5, 3, 4, 6
Activity: Online Heating and Cooling Curve Simulations
LO 5.6 & SP 1
Unit 6: Atomic Structure and Periodicity
Topics Covered:
1. Electron configuration and the Aufbau principle
1.B.2:a
2. Valence electrons and Lewis dot structures
1.B.2:c
3. Periodic trends
1.B.1:b, 1.B.1:c, 1.B.2:b, 1.B.2:d, 1.C.1:c, 1.D.1:b, 2.C.1:a, 2.C.1:b
4. Table arrangement based on electronic properties
1.C.1:a, 1.C.1:b, 1.C.1:d
5. Properties of light and study of waves
1.C.2:e, 1.D.3:a, 5.E.4:b
6. Atomic spectra of hydrogen and energy levels
1.B.1:d, 1.B.1:e, 1.D.3:b
7. Quantum mechanical model
1.C.2:d
8. Quantum theory and electron orbitals
1.C.2:c
9. Orbital shape and energies
1.C.2:b
10. Spectroscopy
1.D.2:a, 1.D.2:b, 1.D.2:c, 1.D.3:b
Labs:
Spectroscopy Lab
LO 1.5, 1.6, 1.7, 1.8, 1.14, 1.15; SP 1, 6
Activity: Periodic Table Dry Lab
LO 1.9, 1.10, 1.11, 1.12, 1.13; SP 1, 5, 6
Unit 7: Chemical Bonding
Topics Covered:
1. Lewis Dot structures
2.C.4:a
2. Resonance structures and formal charge
2.C.4:c, 2.C.4:d, 2.C.4:e
3. Bond polarity and dipole moments
2.C.1:c, 2.C.1:e, 2.C.1:f
4. VSPER models and molecular shape
2.C.4:b, 2.C.4:e, 2.C.4:f
5. Polarity of molecules
2.C.1:e
6. Lattice energies
1.B.1:a, 1.C.2:a, 2.C.1:d (1-2), 2.C.2:a, 2.C.2:b, 2.D.1:b
7. Hybridization
2.C.4:g
8. Molecular orbitals and diagrams
2.C.4:h, 2.C.4:i
Labs: CR5b & CR6
*Guided Inquiry: Bonding Lab
LO 2.1, 2.17, 2.19, 2.20, 5.1, 5.10; SP 1, 3, 4
*Guided Inquiry: Investigation of Solids
LO 2.22-2.32; SP 1, 3, 4, 6
Activity: Atomic Theory Dry Lab
LO 2.21 & SP 1, 6
Unit 8: Liquids, Solids, and Solutions
Topics Covered:
1. Structure and bonding
a. metals, network, and molecular
2.A.1:a, 2.A.1:d, 2.C.3, 2.D.1:a, 2.D.2:a, 2.D.1:b, 2.D.3, 2.D.4
b. ionic, hydrogen, London, van der Waals
2.A.1:b, 2.B.1:a, 2.B.1:b, 2.B.1:c,
2.B.2:a, 2.B.2:b, 2.B.2:c, 2.B.2:d,
2.B.3:a, 5.D:1
2. Vapor pressure and changes in state
3. Heating and Cooling Curves
2.A.1:e, 5.B.3:c, 5.B.3:d
4. Composition of solutions
2.A.1:c, 2.A.3:b, 2.A.3:c, 2.B.3:b
5. Colloids and Suspensions
2.A.3:a, 2.A.3:b, 2.A.3:g
6. Separation Techniques
2.A.3:e, 2.A.3:f
7. Effect on Biological Systems
2.B.3:e, 2.D.3, 5.E.4:c
Demonstration:
Evaporation of Liquids
LO 2.11, 2.18, 5.9, 5.12; SP 1, 6
Labs:
*Guided Inquiry: Solution Preparation Lab
LO 2.8, LO 2.9, 2.14, 2.15; SP 1-4
Vapor Pressure of Liquids Lab
LO 2.3, 2.12, 2.13, 2.16; SP 2, 5, 6
Activity: Effect on biological systems [CR4]
Unit 9: Kinetics
Topics Covered:
1. Rates of reactions
4.A.1:a
2. Factors that affect rates of reactions/collision theory
4.A.1:b, 4.A.1:c, 4.D.1, 4.D.2
3. Reaction Pathways
4.B.3:a, 4.B.3:b
4. Rate equation determination
4.A.2:a
a. rate constants
4.A.3
b. mechanisms
4.B.1, 4.C.1, 4.C.2, 4.C.3
c. method of initial rates
4.A.2:c
d. integrated rate laws
4.A.2:b, 4.A.3:d
5. Activation Energy and Boltzmann Distribution
4.B.2, 4.B.3:c
Demonstration:
Factors that Effect Rates of Reaction
LO 4.1, 4.8, 4.9; SP 1
Labs:
*Guided Inquiry: Determining Order of a Reaction
LO 1.16, 4.2, 4.3, 4.4; SP 2-6
Determining the Activation Energy of a Reaction
LO 4.5, 4.6; SP 2, 5
Activity: Online Kinetics Activity
LO 4.1; SP 1, 3, 6
Unit 10: General Equilibrium
Topics Covered:
1. Characteristics and conditions of chemical equilibrium
6.A.1, 6.A.3:a, 6.A.3:f
2. Equilibrium expression derived from rates
6.A.3:b
3. Factors that affect equilibrium
6.A.3:c
4. Le Chatlier's principle
6.A.3:b, 6.B.1, 6.B.2, 6.C.3:e, 6.C.3:f
5. The equilibrium constant
6.A.3:d, 6.A.3.e, 6.A.4
6. Solving equilibrium problems
6.A.2
Labs:
Determination of a Kc with Varied Initial Concentrations
LO 5.17, 6.1-6.10; SP 2, 5
Activity: Online Gas Phase Equilibrium Activity
LO 6.8, 6.9; SP 1, 6
Unit 11: Acids and Bases
Topics Covered:
1. Definition and nature of acids and bases
3.B.2, 6.C.1:c, 6.C.1:d, 6.C.1:e, 6.C.1:f
2. Kw and the pH scale
6.C.1:a, 6.C.1:b, 6.C.1:g
3. pH of strong and weak acids and bases
6.C.1:h
4. Polyprotic acids
6.C.1:n
5. pH of salts
6. Structure of Acids and Bases
Labs:
Determination of a Ka by Half Titration
LO 2.2, 3.7; SP 2, 5
Unit 12: Buffers, Ksp, and Titrations
Topics Covered:
1. Characteristics and capacity of buffers
6.C.2
2. Titrations and pH curves
6.C.1:i, 6.C.1:j, 6.C.1:k, 6.C.1:l, 6.C.1:m
3. Choosing Acid Base Indicators
4. pH and solubility
5. Ksp Calculations and Solubility Product
6.C.3:a, 6.C.3:b
Labs:
Types of Titrations
LO 6.11, 6.12, 6.13, 6.14, 6.15, 6.16, 6.17; SP 2, 5, 6
*Guided Inquiry: Preparation of a Buffer
LO 6.18, 6.19, 6.20; SP 2, 3, 4, 5
Molar Solubility and Determination of Ksp
LO 6.21, 6.22, 6.23, 6.24; SP 2, 5, 6
Unit 13: Thermodynamics
Topics Covered:
1. Laws of thermodynamics
2. Spontaneous process and entropy
5.E.1
3. Spontaneity, enthalpy, and free energy
5.E.2:c, 5.E.3
4. Free energy
5.E.2:d, 5.E.2:e, 5.E.2:f, 6.C.3:c, 6.D.1:a
5. Free energy and equilibrium
5.E.2, 6.D.1:b, 6.D.1:c, 6.D.1:d
6. Rate and Spontaneity
5.E.2:e, 5.E.5
Labs:
Solubility and Determination of ΔH°, ΔS°, ΔG° of Calcium Hydroxide
LO 5.12, 5.13, 5.14, 5.18, 6.25; SP
2, 5, 6
Unit 14: Electrochemistry
Topics Covered:
1. Balancing redox equations
3.B.3:a, 3.B.3:b, 3.B.3:c, 3.B.3:d
2. Electrochemical cells and voltage
3.C.3:a, 3.C.3:b, 3.C.3:c, 5.E.4:a
3. The Nernst equation
3.C.3:d
4. Spontaneous and non-spontaneous equations
3.C.3:e
5. Chemical applications
3.C.3:f
Demonstration:
Lead Storage Battery
LO 3.12, 3.13, 5.15; SP 1
Labs:
Voltaic Cell Lab
LO 3.12, 3.13, 5.16; SP 2, 5
AP Exam Review
1. Review of All Topics
1.A.2:c
2. 4 AP Style Review Exams
3. Mock AP
Labs:
The Green Crystal Lab
LO 1.2, 2.7, 2.10, 3.7, 3.8, 3.9, 5.11; SP 2, 5, 6
AP Chemistry Lab List
The following labs will be completed during the school year. Guided Inquiry Labs are indicated with an asterisk (*).
Lab: Math and Measurement in Science & Density of an Organic Liquid
Description: Students learn how to measure mass and volume with varied pieces of equipment and focus on the accuracy of those pieces of equipment in their calculation and determination of significant figures. Students also determine the identity of an unknown organic liquid using density determination.
*GUIDED INQUIRY Lab: Discovery of Physical and Chemical Properties
Description: Students are given the materials to conduct various procedures. They construct a procedure for each of the eight changes to be observed, have their procedures approved by the instructor, and then carry out the procedures. The data collected is used to develop a set of criteria for determining whether a given change is chemical or physical.
Lab: Stoichiometry Lab
Description: Students determine the correct mole ratio of reactants in an exothermic reaction by mixing different amounts of reactants and graphing temperature changes.
Lab: pH Titration Lab
Description: Students perform a titration and then determine the concentration of an HCl solution by using a potentiometric titration curve and finding the equivalence point. Data is graphed in a graphing program.
Lab: Bleach Lab
Description: Students perform redox titrations to determine the concentration of hypochlorite in household bleach.
Activity: Online Redox Titration Activity
Description: Utilizing an eduweb lab simulation, students have the opportunity to manipulate various factors that influence a redox titration.
Lab: Copper Reaction Lab
Description: Students perform a series of reactions, starting with copper and ending with copper. Students then calculate percent recovered.
Demonstration: Graham’s Law of Diffusion
Description: HCl and NH3 are placed in either end of a glass tube. Using distance traveled of each gas by looking at formation of NH4Cl ring, MM of HCl is calculated.
Lab: Molar Mass of a Volatile Liquid
Description: Students use the Dumas method for determination of the molar mass of an unknown volatile liquid.
Lab: Hess’s Law Lab
Description: Students perform a series of reactions and calculate enthalpy, proving Hess’s law.
Activity: Online Heating and Cooling Curve Simulations
Description: Utilizing the eduweb lab simulation website, students heat an unknown and graph its temperature as it cools, giving them the ability to calculate the energy released.
Lab: Spectrum and Spectroscopy Lab
Description: Students look at a series of emission spectra and determine the identity of an unknown. They will also receive and analyze IR and mass spectroscopy data.
Activity: Periodic Table Dry Lab
Description: Students graph values for atomic radius, electronegativity, and ionization energy to predict trends and explain the organization of the periodic table.
*GUIDED INQUIRY Lab: Bonding Lab
Description: Students experimentally investigate ionic and molecular substances deducing properties of their bonds in the process.
*GUIDED INQUIRY Lab: Investigation of Solids
Description: Students investigate types of solids using various experimental techniques.
Activity: Atomic Theory Dry Lab
Description: Students make drawings of a series of molecules and from those drawings predict geometry, hybridization, and polarity.
Lab: Preparation of Solutions Lab
Description: Students make solutions of specified concentrations gravimetrically and by dilution. Solution concentrations will be checked for accuracy using a spectrophotometer.
Demonstration: Evaporation of Liquids
Description: Using a data collection device, the teacher will show the temperature curves of evaporation of various liquids and students must deduce the differences based on IMF’s.
Lab: Vapor Pressure of Liquids
Description: Students measure the vapor pressure of ethanol at different temperatures to determine ΔH.
Activity: Effect on biological systems
Description: Students examine a demonstration size model of DNA or an alpha helix, and use their fingers to identify which atoms / base pairs are particularly involved in hydrogen bonding within the molecule, causing the helical structure. Students then discuss how the increased UV light because of ozone depletion can cause chemical reactions and thus mutations and disruption of hydrogen bonding.
*GUIDED INQUIRY Lab: Determining the Rate Law of a Crystal Violet Reaction
Description: Using calorimetry and Beer’s law, students determine the order of a reaction and its rate law.
Lab: Determining the Activation Energy of the Crystal Violet Reaction
Description: Students use the same set up as in the crystal violet lab, but this time varying temperature to calculate the activation energy with the use of the Arrhenius equation.
Activity: Online Kinetics Activity
Description: Using a web based simulation students will study the elementary steps of a mechanism and how it relates to reaction rate and collision theory.
Lab: Determining Kc with Various Initial Concentrations
Description: Students use a spectrophotometer to determine the Kc of a series of reactions.
Activity: Online Gas Phase Equilibrium Activity
Description: In the online inquiry activity, students are able to manipulate the environment and produce stresses that verify the tendency of Le Chatelier’s principle.
Lab: Determining Ka by Half Titration
Description: Students do a titration in which ½ of the weak acid titrated is neutralized (aka midpoint) and then the Ka is determined.
*GUIDED INQUIRY Lab: Types of Titrations
Description: Students investigate titration curves by doing titrations of different combinations of weak and strong acids and bases.
*GUIDED INQUIRY Lab: Preparation of a Buffer
Description: Given a selection of chemicals, students prepare a buffer of a given pH.
Lab: Molar Solubility and Determination of Ksp
Description: Students find the Ksp of calcium hydroxide doing a potentiometric titration with the addition of methyl orange indicator for verification.
Lab: Solubility and Determination of ΔH°, ΔS°, ΔG° of Calcium Hydroxide
Description: Students collect and analyze data to determine ΔH°, ΔS°, and ΔG° of calcium hydroxide.
Lab: Voltaic Cell Lab
Description: Students find the reduction potentials of a series of reactions using voltaic cells/multi-meters and build their own reduction potential table. Dilutions will be made and the Nernst equation will also be tested.
Demonstration: Lead Storage Battery
Description: Students and teacher will build a battery to solidify knowledge of electrolytic cells in comparison to voltaic cells.
Lab: GREEN CRYSTAL LAB
Description: A series of labs completed over a 4-week period. Students work at their own pace in pairs. The goal of this lab is to determine the empirical formula of a ferro-oxalato crystal. It includes the following experiments:
Experiment 1: Synthesis of the crystal
Experiment 2: Standardization of KMnO4 by redox titration
Experiment 3: Determination of % oxalate in crystal by redox titration
Experiment 4: Standardization of NaOH by acid/base titration
Experiment 5: Determination of % K+ and Fe3+ by ion exchange chromatography and a double equivalence point titration
Experiment 6: Determination of the % water in the hydrated crystal