Course Outcomes

COURSE OUTCOMES

AP CHEMISTRY

(SECONDARY)

(July 2013)

The AP Chemistry course presents a rigorous study of advanced chemistry topics. It is a course intended to be the equivalent of a university level general chemistry course. As such, the course is intended for highly motivated students in the upper secondary levels. Prerequisites for the course include successful completion of ten units of both Chemistry and Advanced Mathematics I (Algebra II) classes. These prerequisites may be waived for advanced students with the permission of the AP Chemistry instructor and the Director of Instruction or Director. Students are also expected to own a scientific calculator.

The course is divided into ten units based on the six Big Ideas outlined in the AP Chemistry Curriculum Framework. The Big Ideas are as follows:

•Big Idea 1: The chemical elements are fundamental building materials 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: 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: Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons.

•Big Idea 4: Rates of chemical reactions are determined by the details of molecular collisions.

•Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.

•Big Idea 6: 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.

*A schedule of suggested activities to support the Big Ideas can be found on pages 9-10

The Framework supports the Big Ideas by outlining 96 Learning Objectives. The ten Essential Units of the AP Chemistry course are designed to solidify these learning objectives by incorporating multiple Big Ideas and several Learning Objectives into each unit. Successful completion of this course will adequately prepare the student for the AP Chemistry examination as well as to continue the study of chemistry and related fields at the university level.

All ten Essential Units must be assessed for mastery. QSI’s philosophy of Mastery Learning requires every student to master each unit to an ‘A’ or a ‘B’ level. If a student does not sufficiently master a unit the first time, the student must restudy the material and be reassessed until mastery is achieved. Units are considered in progress (P) until mastery at the A or B level is acheived.

The AP Chemistry course is designed to assist students in the pursuit of active, inquiry-based learning and problem solving. Though using formulas and the recollection of facts are a natural part of the study of chemistry, this course focuses more on a conceptual understanding of chemical concepts and the development problem solving skills. Students are assisted in this pursuit through an inclusive hands-on laboratory component of the course. Each unit includes suggested laboratory assignments which will provide the student opportunities to practice laboratory skills, develop an appreciation for chemistry in practice, and solidify chemical concepts through application. The importance of laboratory component of the course cannot be overemphasized.

A solid foundation of chemical concepts and techniques is essential for success in AP Chemistry. Selective Unit One provides an opportunity for students to review and refine such foundational skills. Though these skills are crucial, time is short and a unit reviewing basic skills takes valuable class time. For this reason it is suggested that students intending to take AP Chemistry engage in Selective Unit One during the summer in preparation for the rigors of the upcoming school year. Performing a simple laboratory using household materials and writing a lab report prior to the school year is an excellent opportunity for students to prepare for AP Chemistry. Alternatively, Selective Unit One may be covered in the first week of class, but it is not recommended to spend more than one week on this unit.

Students in AP Chemistry should attend class for five periods of 48 minutes per week. Additional time for laboratory work, comprising of a two period block, should be scheduled to accommodate the completion of twenty experiments throughout the year. If these extended class periods are not available, students may need to attend school outside of regularly scheduled times, such as arriving at school early, staying at school late, or attending weekend sessions in order to accommodate the laboratory component of the course. A minimum of 25% of instructional time must be dedicated to hands-on laboratory experiences integrated throughout the course. A schedule of suggested laboratory experiments with the associated Science Practices from the AP Chemistry Curriculum Framework follows on page eight. The laboratory activities listed are recommended by the AP College Board, but other similar labs may be substituted.

Suggested Course Materials:

Textbook (required):

Zumdahl, Steven S. and Zumdahl, Susan A.,Chemistry.8th ed. Boston: Houghton Mifflin Company, 2010. ISBN 0-547-12532-1 (ZUM)

Laboratory Texts (required)

Vonderbrink, Ph.D., Sally A. Laboratory Experiments for Advanced Placement Chemistry, 2nd ed. Batavia, IL: Flinn Scientific, Inc. 2006. ISBN 978-1-933709-02-4 (Vonderbrink)

Hostage, David and Fossett, Martin, Laboratory Investigations for AP Chemistry, People’s Education Inc., New Jersey, 2006. ISBN 1-4138-0489-6 (Hostage)

Nelson, John and Kemp, Kenneth Chemistry the Central Science: Laboratory Experiments, 10thed, Pearson Prentice Hall 2006 ISBN 0-13-146479-5 (Nelson& Kemp)

Laboratory Notebook (required)

Hayden-McNieil 100 Set Carbonless Duplicate Spiral Bound Laboratory Notebook ISBN 978-1429224543

Supplemental Materials: (Optional, but purchase of a single copy of each is highly recommended)

5 Steps to a 5 AP Chemistry, 2014-2015 Edition (5 Steps to a 5 on the Advanced Placement Examinations Series)by Richard H. Langley and John Moore (Jul 12, 2013) ISBN:978-0-07180373-1

Cracking the AP Chemistry Exam, 2013 Ed. The Princeton Review. ISBN 978-0-37542989-7

An outline of the 10 essential units and three selective units with suggested materials follows. These unit outcomes are normally engaged in the given order. Ten essential units comprise the complete course and must be assessed for mastery.

Essential Units:

E01 - Chemical Reactions: ZUM Chapters 3& 4

Essential unit one describes three types of chemical reactions; precipitation reactions, acid-base reactions and oxidation-reduction reactions. The student will write balanced chemical equations and solve stoichiometric problems using the mole concept for each type of reaction.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Counting by weighing
Balancing chemical equations
Determining molecular and empirical formulas
Limiting reagent and percent yield
The nature of aqueous solutions: strong & weak electrolytes
Composition of a solution
Describing reactions in solution
Stoichiometry of precipitation reactions
Types of chemical reactions

Precipitation reaction

Acid-base reactions

Oxidation-reduction reactions

QSI AP CHEMISTRY SEC CO

E02 - Gases & Thermochemistry: Chapters 5 & 6

Unit two introduces gas behavior according to the Kinetic Molecular Theory, gas stoichiometry, and thermochemical properties such as enthalpy, calorimetry, and specific heat. The student investigates gas behavior under changing conditions as well as how enthalpy (heat) can be transferred in systems.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Gas laws of Boyle, Charles and Avogadro
The Ideal Gas Law
Dalton’s Law of Partial Pressures
Kinetic Molecular Theory of Gases
Effusion & Diffusion
Real Gases
The Nature of Energy
Enthalpy & Calorimetry
Hess’s Law
Standard Enthalpies of formation

QSI AP CHEMISTRY SEC CO

E03 - Atomic Structure: Chapter 7

Unit three tracks the history of the development of the quantum mechanical model of the atom. Students relate electron behavior to atomic properties and periodic trends.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Electromagnetic radiation
Atomic spectrum of Hydrogen
The Bohr Model
Quantum Mechanical Model of the Atom
Orbital shapes and energies
Electron spin and the Pauli Principle
Polyelectronic Atoms
Aufbau Principle and the Periodic Table
Periodic Trends and Properties of a Group

QSI AP CHEMISTRY SEC CO

E04 - Bonding: Chapters 8 & 9

Columb’s Law is integral in explaining many chemical properties. Unit four relates Columb’s Law and electrostatic forces to the bonding of atoms and the shapes of molecules. The student compares categories of bonds, creates Lewis structures, employs the rules for making VSEPR models of atoms, and explores hybridized bonds. The student will also investigate molecular geometry.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Types of Bonding
Electronegativity
Bond Polarity and Dipole Moments
Electron Configurations and Sizes of Ions
Formation of Binary Ionic Compounds
Covalent Bonding
Localized Electron Bonding Model
Lewis Structures
Exceptions to the Octet Rule
Resonance
The VSEPR Model
Orbitals and Hybridization
Molecular Orbital Model
Homo-nuclear and Hetero-nuclear Diatomic Molecules
Combining Localized Electron and Molecular Orbital Models

QSI AP CHEMISTRY SEC CO

E05 - States of Matter: Chapters 10 & 11

Unit five introduces the student to forces which exist between molecules. The student relates properties of solids, liquids, and gases to the intermolecular forces existing within the sample. The student also investigates the properties of different states of matter.

Key Concepts

QSI AP CHEMISTRY SEC CO

Intermolecular Forces
The Liquid State
Structure and Types of Solids
Structure and Bonding in Metals
Network Atomic Solids: Carbon & Silicon
Molecular and Ionic Solids
Vapor Pressure and Change in State
Solution Composition
Factors affecting solubility
Vapor Pressure of Solutions and Osmotic Pressure
Colloids

QSI AP CHEMISTRY SEC CO

E06 - Kinetics: Chapter 12

Unitsix takes into account that to be useful, a chemical reaction must occur at a reasonable rate. The student calculates rate laws, examines the effect of catalysts on reaction rates, explores reaction mechanisms, and investigates factors which affect reaction rates.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Reaction Rates and Formation of Rate Laws
Integrated Rate Law
Reaction Mechanisms
Half Life
A Model for Chemical Kinetics
Catalysis

QSI AP CHEMISTRY SEC CO

E07 - Equilibrium: Chapters 13 & 14

Unit sevenpresents the student with the idea that although a system at equilibrium is macroscopically static, it is microscopically dynamic. The student uses a balanced chemical equation to determine the equilibrium constant for a reversible reactions. The student also predicts equilibrium shifts given various stresses to the system and examines equilibria of acids and bases. The student will finally investigate factors affecting equilibrium.

Key Concepts:

QSI AP CHEMISTRY SEC CO

The Equilibrium Condition
Equilibrium Constant
Equilibrium Expression Involving Pressures
Heterogeneous Equilibria
Solving Equilibrium Problems
Le Châtelier’s Principle
Acid strength and the pH scale
Calculating pH of Strong and Weak Acids
Polyprotic Acids
Acid-Base Properties of Salts and Oxides
Effect of Structure on Acid-Base Properties
Lewis Acid-Base Model

QSI AP CHEMISTRY SEC CO

E08 - Applications of Equilibria: Chapter 15&16

Unit eight builds on acid-base concepts. The student calculates pH, designs buffer solutions, interprets titration curves, predicts solubility, and examines factors which affect solubility. The student also investigates acid-base equilibria and/or solubility of salts.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Common Ion Effect
Buffer Solutions and Buffer Capacity
Titrations and pH Curves
Acid-Base Indicators
Solubility Equilibria and Solubility Product
Precipitation and Qualitative Analysis
Complex Ion Equilibrium

QSI AP CHEMISTRY SEC CO

E09 - Thermodynamics and Electrochemistry: Chapters 17& 18

Unit nine introduces the laws of thermodynamics. The student applies the thermodynamic laws to determine if a reaction is favorable. The student also explores the basics of electrochemistry, including electrolytic and galvanic cells. The student investigates the principles of thermodynamics and electrochemistry.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Thermodynamically Favored Processes and Entropy
Second Law of Thermodynamics
Effect of Temperature on Spontaneity
Free Energy and Chemical Reactions
Entropy Changes in Chemical Reactions
Dependence of Free Energy on Pressure
Free Energy, Equilibrium and Work
Galvanic Cells
Standard Reduction Potential
Cell Potential, Electrical Work and Free Energy
Dependence of Cell Potential on Concentration
Batteries, Corrosion, and Electrolysis
Commercial Electrolytic Processes

QSI AP CHEMISTRY SEC CO

E10 - Organic and Biological Molecules: Chapter 22

Unit ten gives the student a basic introduction to organic chemistry. The student recognizes and names various organic molecules, including those with important biological significance, such as nucleic acids and proteins. The student also investigates the synthesis and purification of an organic compound.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Alkanes
Alkenes and Alkynes
Aromatic Hydrocarbons
Hydrocarbon Derivatives
Polymers and Natural Polymers

QSI AP CHEMISTRY SEC CO

Selective Units:

S01 - Chemical Foundations: Chapter 1&2

Selective Unit one reviews basic chemistry concepts with which the student should be familiar. As this is a review unit, it could be assigned as a summer assignment or be covered in the first week of class. The student reviews basic units of measurement including significant figure usage and dimensional analysis, the atom and its fundamental particles, the Periodic Table, and naming ionic and covalent molecules.

QSI AP CHEMISTRY SEC CO

Scientific Method
Units of Measurement, Uncertainty and Significant Figures
Dimensional Analysis
Classification of Matter
Dalton’s Atomic Theory
Molecules and Ions
Periodic Table and Naming Simple Compounds
Atomic masses
History of the atom

QSI AP CHEMISTRY SEC CO

S02 - Nuclear Chemistry: Chapter 19

Selective Unit two changes the focus from importance of the electron interaction to that of the nucleus of the atom. The student determines what makes a nucleus stable as well as quantifies the energy contained within the nucleus and how it can be used. The student also calculates half-lives and evaluates the potential dangers of nuclear radiation.

Key Concepts:

QSI AP CHEMISTRY SEC CO

Nuclear Stability and Radioactive Decay
Kinetics of Radioactive Decay
Nuclear Transformations
Detection and Uses of Radioactivity
Thermodynamic Stability of the Nucleus
Nuclear Fission and Fusion
Effects of Radiation

QSI AP CHEMISTRY SEC CO

S03 – End of Year Project

Unit Statement: Selective Unit three is an end of year project in which students should engage following completion of the AP Chemistry examination. The student finds a movie clip which contains an element of chemistry and researches the topic to determine if the clip contains fact or fiction. The student then writes a scientific research paper and presents findings in a multimedia presentation. This project was adapted from a project found online. A link to the original document can be found under Technology Resources below.

Key Concepts:

Research
Scientific Writing
Oral presentation
Review of Chemistry Concepts

Schedule of suggested laboratory experiments(guided inquiry format is suggested for labs shaded in gray)

Unit # / Lab # / Name of Laboratory / Lab Manual / Associated Science Practices
E01 / 1 / Determination of Empirical Formula of Silver Oxide / Vonderbrink / 2,3,5,6,7
E01 / 2 / Analysis of Silver in an Alloy / Vonderbrink / 2,3,4,5,6
E01 / 3 / Gravimetric Analysis of a Metal Carbonate / Vonderbrink / 2,3,4,5,6
E01 / 4 / Analysis of Alum: AlK(SO4)2 ·12H2O / Vonderbrink / 2,3,4,5
E01
E02 / 5 / Finding the Ratio of Moles of Reactants in a Chemical Reaction / Vonderbrink / 1,2,3,4,5,6,7
E02 / 6 / Thermodynamics – Enthalpy of Reaction and Hess’s Law / Vonderbrink / 1,2,3,4,5,6,7
E02 / 8 / Determining the Molar Volume of a Gas / Vonderbrink / 1,2,3,4,5,6,7
E02 / - / Micromole Rockets / Chemmybear* / 2,3,4,5,6
E03 / 7 / An Activity Series / Vonderbrink / 1,4,5,6,7
E04 / 11 / Molecular Geometries of Covalent Molecules: Lewis Structures and the VSEPR Model / Nelson & Kemp / 1,5,6,7
E05 / 9 / Determination of the Molar Mass of Volatile Liquids / Vonderbrink / 1,2,3,4,5,6,7
E05 / 11 / Molar Mass By Freezing Point Depression / Vonderbrink / 2,3,4,5,6
E06 / 12 / Kinetics of a Reaction / Vonderbrink / 2,3,4,5,6,7
E06 / 13A / Kinetics: Differential and Integrated Rate Laws: Part A / Hostage / 1,2,3,4,5,6
E07 / 13 / The Determination of Keq for FeSCN2+ / Vonderbrink / 1,2,3,4,5,6,7
E07 / 14 / Determination of Ka for Weak Acids / Vonderbrink / 1,5,6,7
E07 / 15 / Acid-Base Titrations / Vonderbrink / 1,2,3,4,5,6,7
E08 / 16 / Selecting Indicators for Acid-Base Titrations / Vonderbrink / 1,2,3,4,5,6,7
E08 / 17 / Preparation and Properties of Buffer Solutions / Vonderbrink / 3,4,5,6
E08 / 18 / Determination of the Solubility Product of an Ionic Compound / Vonderbrink / 2,3,4,5,6
E09 / 22 / Electrochemical Cells / Vonderbrink / 2,3,4,5,6,7
E09 / 23 / Electrolysis / Vonderbrink / 1,2,3,4,5,6,7
E09 / 17 / Exploring Electrochemistry / Hostage / 1,2,3,4,5,6,7
E10 / 25 / Synthesis, Isolation, and Purification of an Ester / Vonderbrink / 1,2,3,4,5,6,7
S01 / 1 / Determination of the Empirical Formula of Silver Oxide / Vonderbrink / 2,3,5,6,7
S01 / 26 / Predicting the products of Chemical Reactions and Writing Chemical Equations / Vonderbrink / 1,2,3,4,5,6,7
S02 / 13B / Kinetics: Differential & Integrated Rate Laws: Part B / Hostage / 1,2,3,4,5,6,7

Schedule of possible activities which support the Big Ideas

Big Idea 1 – The Structure of Matter

›The student justifies, with evidence, the arrangement of the periodic table and applies periodic properties to chemical reactivity.

›The student is given several elements and pairs them by families or by period and are asked to rationalize the change in electronegativity of each group based on the electronic structure of the atom.

›The student uses a mass spectrometer printout of the relative masses of isotopes of an element to determine a) the percentages of the isotopes and (b) the average atomic mass of the element.

›The student graphs values for atomic radii, electronegativities, and ionization energies to predict trends and explain the organization of the periodic table.

Big Idea 2 - Properties of Matter - Characteristics, States, and Forces of Attraction.

›The student makes drawings of a series of molecules and from those drawings predicts geometry, hybridization, and polarity.