AP Chemistry
AP Chemistry Overview
AP Chemistry meets daily for two semesters. Labs are included within this time period, with additional preparatory work completed before or after school. Also, AP Chemistry review sessions are on various AP topics.
Course Design
This course is designed to provide an experience similar to a first year college chemistry program. Chemistry concepts, mathematical problem solving skills and laboratory experiences are integrated using a variety of methods including hands on activities and technology. Students are required to have successfully completed a first year high school chemistry class as a prerequisite as well as Algebra II. This course builds on the concepts that were introduced in the first year of high school chemistry and integrates the concepts previously mastered with new material.
Teaching Strategies
· Encourage group work and study groups
· Allow time for hands on laboratory experiences with error analysis
· Require students to keep an organized lab notebook that parallels a first year college chemistry lab
· Vary presentations using lecture, demonstration, analogies, animations, student response system presentations, Power Points and other technology.
· Use a web blog to communicate with students other than class time
· Post schedules, links, lab instructions, keys to practice tests, class information on the class blog
Text
Chemistry The Central Science by Brown, LeMay, Bursten, Murphy, 11th edition, Prentice Hall, 2009.
Curricular Requirements:
C1 – Evidence of Curricular Requirement: Structure of Matter (Atomic theory and atomic structure, Chemical bonding)
C2 – Evidence of Curricular Requirement: States of Matter (Gases, Liquids and solids, Solutions)
C3 – Evidence of Curricular Requirement: Reactions (Reaction types, Stoichiometry, Equilibrium, Kinetics, Thermodynamics)
C4 – Evidence of Curricular Requirement: Descriptive Chemistry (Relationships in the periodic table)
C5 – Evidence of Curricular Requirement: Laboratory (Physical manipulations; Processes and procedures; observations and data manipulation; communication, group collaboration, and the laboratory report)
C6 – Evidence of Curricular Requirement: The course emphasizes chemical calculations and the mathematical formulation of principles
C7 – The course includes a laboratory component comparable to college-level chemistry laboratories.
A minimum of one double-period per week or its equivalent is spent engaged in laboratory work. A hands-on laboratory component is required. Each student should complete a lab notebook or portfolio of lab reports.
Unit One - Introduction to Chemistry, Atomic Theory, Matter, Formulas
Chapters: 1,2,3 Time: Week 1-2
Curricular Requirements – C1, C2, C5, C6, C7
Objectives:
· Review safety in the laboratory
· Calculate metric conversions
· Problem solving with dimensional analysis
· Error Calculations
· Standard Deviation
· Physical and Chemical Properties
· Significant Figures and Calculations
· Formulas
· Percent Composition, Empirical and Molecular Formulas
Activities:
· Summer assignment
· Lab - Calibration and measurement -90 minutes– C5
· Lab – Identify an Unknown from Physical Properties -150 minutes - C5
Unit Two - Stoichiometry and Reaction Types
Chapters: 3-4 Time: Weeks 3-5
Curricular Requirements: C3, C5, C6, C7
Objectives:
· Write and balance equations
· Mole concepts
· Calculate chemical quantities based in a chemical reaction and limiting reagents
· Complex Ions
· Identify types of reactions Predict products
· Write ionic and net equations
· Identify precipitate with solubility rules
· Redox reactions
· Introduction to applications of redox
Activities:
· Lab - Metathesis , 90 minutes
· Lab – Copper to Copper, 180 minutes
· Lab – Molecular models of complex ions, 60 minutes
· Lab –Iron compounds redox, 60 minutes
Unit Three – Kinetic Molecular Theory and Gases
Chapter 10 Time: Week 6
Curricular Requirements: C2, C5, C6, C7
Objectives:
· Review Boyles, Charles, Gay Lussac and combined laws
· Review Ideal gas laws and Avogadro’s Hypothesis
· Kinetic Molecular Theory
· Graham’s law of diffusion and effusion,
· Dalton’s law of partial pressure
· Using gas laws in chemical reactions
· Determining molar mass of gases
Activities:
· Determine the molar mass of a volatile liquid – 60 minutes
Unit Four – Thermochemistry
Chapters 5,19 Time: Weeks 7-9
Curricular Requirements: C3, C5, C6, C7
Objectives:
· The nature of energy and its relationship with chemical reactions
· Calorimetry problems, solving for Heat, Specific Heat, and Molar Heat
· Use Hess’s law to solve enthalpy problems
· Relate free energy, entropy and enthalpy to the spontaneity of a system
· Calculate free energy, entropy and enthalpy
· Be able to predict and explain whether reactions will occur
Activities:
· Lab – virtual lab – heat
http://www.chm.davidson.edu/ChemistryApplets/calorimetry/HeatofSolutionofAmmoniumNitrate.html
· Lab – Heat of neutralization, 150 minutes
Unit Five – Kinetics
Chapter 14 Time: Weeks 10-12
Curricular Requirements: C3, C5, C6, C7
Objectives:
· Reaction rates
· Factors that influence rate
· Collision theory
· Differential and integrated rate laws
· Determining order
· Half lives
· Interpreting reaction mechanisms based on rate law
· Role of catalysts
Activities:
· Lab – Dry lab – half life and order – small scale, 60 minutes
· Lab – Acid Catalyzed Iodination of Acetone, 60 minutes
Unit Six – Equilibrium, Aqueous Equilibrium
Chapter 15, 16, 17 Time: Weeks 13-17
Curricular Requirements: C3, C5, C6, C7
Objectives:
· Be able to write equilibrium expressions for reactions
· Calculate Keq and Kp
· Apply LeChatelier’s principle to predict changes in equilibrium
· Calculate equilibrium concentrations of reactants and products
· Calculate solubility equilibria concentrations
· Calculate Ksp
· Calculate using a common ion
· Use experiment ion product to predict precipitation
Activities:
· Student Response System – interactive practice, 60 minutes
· Online Trackstar on Equilibrium topics and virtual lab, 60 minutes
· Lab – LeChatelier’s Principle, 90 minutes
· Lab – Determination of the Solubility Product Constant for a Sparingly Soluble Salt, 180 minutes
REVIEW AND MIDTERMS…………………………….Week 18
Spring Semester
Unit Seven – Acids and Bases
Chapter 16-17 Time: Weeks 1-4
Curricular Requirements: C3, C5, C6, C7
Objectives:
· Explain Arrhenius, Bronsted – Lowry , Lewis theories
· Characteristics of acids and bases
· Acid and base anhydrides
· Relate acid base strength to dissociation equilibrium
· Calculate pH, pOH, pK of strong and weak acids and bases
· Be able to interpret titration graphs
Activities:
· Lab – Determination of the Dissociation Constant of a Weak Acid, 180 minutes
· Lab – Hydrolysis of salts and pH of buffer solutions, 180 minutes
· Virtual Lab – Buffers – 90 minutes
http://www.chem.ubc.ca/courseware/121_virtual_lab/123.html
http://www.chemcollective.org/vlab/vlab.php
Unit Eight– Atomic Structure, Periodicity and Bonding
Chapter 7-9 Time: Weeks 5-8
Curricular Requirements: C1, C4, C5, C6, C7
Objectives:
· Understand the basics of the quantum mechanical model
· Write electron designations for atoms and determine quantum numbers for electrons
· Understand the organization of the periodic table and trends
· Make predictions of properties and chemical behavior using the periodic table
· Draw Lewis structures and apply formal charge
· Determine shapes and polarity of molecules
· Understand resonance and determine molecules with resonance
· Understand hybridization and bond energies
Activities:
· Lab – Atomic Spectra and Atomic Structure, 150 minutes
· Lab – Molecular models, 120 minutes
· Lab – Qualitative Analysis – Group 1 cations, 180 minutes
· Virtual Lab – Qualitative Analysis http://www.dartmouth.edu/~chemlab/info/resources/qual/soluble.SolubleAppletC.html
Unit Nine–Solutions, Liquids, Solids, Colligative Properties
Chapter 11 - 13 Time: Weeks 9-10
Curricular Requirements: C2, C5, C6, C7
Objectives:
· Calculate and perform the different methods of measuring concentration.
· Describe and identify different types of solutions
· Explain factors affecting solubility
· Explain how colligative properties of solutions affect properties. Be able to calculate the effects.
· Explain the various types of intermolecular forces, and the types of molecules or compounds they affect. What are the resultant properties of the compounds involved including metallic bonding, ionic bonding, and network solids?
· Relate intermolecular forces to vapor pressure and boiling point.
· Draw and interpret phase change diagrams.
Activities:
· Lab – Colligative Properties: Freezing-Point Depression and Molar Mass, 150 minutes
Unit Ten– Electrochemistry
Chapter 20 Time: Week 11-13
Curricular Requirements: C3, C5, C6, C7
Objectives:
· Distinguish between electrolytic and galvanic cells
· Relate maximum cell potential to the free energy difference between reactants and products
· Calculate amounts and equilibrium constants
Activities:
· Electrochemistry introductory packet, 120 minutes
AP Practice and Exam, and Special Topics
Time: Weeks 14-18
LuAnn Pierce
Lassiter High School
Blog: http://lhsblogs.typepad.com/pierce/