Central Falls AP Chemistry Course Syllabus
Instructor: Carl Africo
Introduction:
This course is similar in content to a high-level first year college chemistry course. In many aspects I will teach it as a college course would be taught. I hope that this experience will help prepare you for the realities of college; I want you to leave this course with at least as much knowledge of the chemistry subject matter and laboratory procedures that a college freshman would attain through his course work in that subject. You should also leave it with study, research, and organizational skills that will serve you well in college.
It is my intent to design this course to be as fulfilling for you as possible. You must put a lot of effort into the course; but, you will hopefully come away from it with deep satisfaction.
Class Times:
The AP chemistry class will meet for 70 minutes daily four days a week with one 90 minute day once a week for the entire school year. They will be 3 mandatory Saturday sessions and tutoring is available from 6:30am to 7:45 am on Mondays and Fridays.
Text: Brown, Theodore; Lemay, Eugene; Bursten, Bruce; and Catherine Murphy. Chemistry: The Central Science, Twelfth Edition.
Grading System:
Exams 25%
Labs / CIM Task 25%
Quizzes / Abstracts 20%
HW/CW 10%
Blogs / lab journals 10%
Group Participation 10%
Grading:
An examination will be given at the completion of every two chapters in the textbook. All examinations will consist entirely of multiple choice questions and free response questions. Each exam will primarily contain material covered since the previous exam. I will attempt to design the examinations to prepare you for the AP exam. Remember, chemistry, unlike many subjects, is cumulative. We often use concepts learned in earlier units of the course
Quizzes will be given on Fridays and will include problems and questions similar to the ones we have been working on in class during the week. They may also include questions about the experiment(s) done that week.
Homework / Class work:
You will generally have one to two hours of homework every day. Homework will include reading assignments, problems, preparing for labs, writing lab reports, and studying for quizzes and exams.
You will be given a set of homework problems for each chapter. These problems should be regarded as the minimum problem assignment. You are encouraged to attempt to do any additional problems. The more problems that you attempt to do the better prepared you will be in the course. As noted earlier, homework will not be collected but it will be checked periodically. We will discuss problems in class.
A word of warning!! There is a great temptation to neglect to do the homework. If you cannot assume this responsibility then you should not be in this class. You will not be successful and will only be a burden to others. There is no way that you can gain any real value from the class if you do not do the work outside of the class. You must be prepared to give this commitment to the class.
Grouping and Group work:
Within the first couple weeks of the course students are grouped in pairs. These groupings constitute lab partners, but are also used during classroom instruction. Partners are allowed to help each other during many class activities (obviously excluding formal assessments). Further, when activities will benefit from a larger group two pairs will work together. Throughout all of this work these pairs are held to accountable as a team which pair assessments and labs being used to link grades to provide motivation for mutual support. First among these group assignments is a problem of the day, which are generally drawn from past AP multiple choice questions. Students respond to these questions as a pair in a single notebook which is collected and scored weekly. Responses must include an answer choice, reason, and, if necessary a correction based on a brief class discussion.
Fall Semester
Chapter 1 Introduction: Matter and Measurement
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
1.1 The Study of Chemistry
1.2 Classification of Matter
1.3 Properties of Matter
1.4 Units of Measurement
1.5 Uncertainty in Measurement
1.6 Dimensional Analysis
Chapter 2 Atoms, Molecules, and Ions
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.
2.1 The Atomic Theory of Matter
2.2 The Discovery of Atomic Structure
2.3 The Modern View of Atomic Structure
2.4 Atomic Weights
2.5 The Periodic Table
2.6 Molecules and Molecular Compounds
2.7 Ions and Ionic Compounds
2.8 Naming Inorganic Compounds
2.9 Some Simple Organic Compounds
Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
3.1 Chemical Equations
3.2 Some Simple Patterns of Chemical Reactivity
3.2 Formula Weights
3.4 Avogadro’s Number and the Mole
3.5 Empirical Formulas from Analysis
3.6 Quantitative Information from Balanced Equations
3.7 Limiting Reactants
Chapter 4 Aqueous Reactions and Solution Stoichiometry
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.
4.1 General Properties of Aqueous Solutions
4.2 Precipitation Reactions
4.3 Acid-Base Reactions
4.4 Oxidation-Reduction Reactions
4.5 Concentrations of Solutions
4.6 Solution Stoichiometry and Chemical Analysis
Chapter 5 Thermochemistry
Big Idea 5: The Laws of Thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
5.1 The Nature of Energy
5.2 The First Law of Thermodynamics
5.3 Enthalpy
5.4 Enthalpies of Reaction
5.5 Calorimetry
5.6 Hess’s Law
5.7 Enthalpies of Formation
5.8 Foods and Fuels
Chapter 6 Electronic Structure of Atoms
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.
6.1 The Wave Nature of Light
6.2 Quantized Energy and Photons
6.3 Line Spectra and the Bohr Model
6.4 The Wave Behavior of Matter
6.5 Quantum Mechanics and Atomic Orbitals
6.6 Representations of Orbitals
6.7 Many-Electron Atoms
6.8 Electron Configurations
6.9 Electron Configurations and the Periodic Table
Chapter 7 Periodic Properties of the Elements
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
7.1 Development of the Periodic Table
7.2 Effective Nuclear Charge
7.3 Sizes of Atoms and Ions
7.4 Ionization Energy
7.5 Electron Affinities
7.6 Metals, Nonmetals, and Metalloids
7.7 Group Trends for the Active Metals
7.8 Group Trends for Selected Nonmetals
Chapter 8 Basic Concepts of Chemical Bonding
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule
8.2 Ionic Bonding
8.3 Covalent Bonding
8.4 Bond Polarity and Electronegativity
8.5 Drawing Lewis Structures
8.6 Resonance Structures
8.7 Exceptions to the Octet Rule
8.8 Strengths of Covalent Bonds
Chapter 9 Molecular Geometry and Bonding Theories
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
9.1 Molecular Shapes
9.2 The VSEPR Model
9.3 Molecular Shape and Molecular Polarity
9.4 Covalent Bonding and Orbital Overlap
9.5 Hybrid Orbitals
9.6 Multiple Bonds
9.7 Molecular Orbitals
9.8 Second-Row Diatomic Molecules
Chapter 10 Gases
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
10.1 Characteristics of Gases
10.2 Pressure
10.3 The Gas Laws
10.4 The Ideal-Gas Equation
10.5 Further Application of the Ideal-Gas Equation
10.6 Gas Mixtures and Partial Pressures
10.7 Kinetic-Molecular Theory
10.8 Molecular Effusion and Diffusion
10.9 Real Gases: Deviations from Ideal Gas Behavior
Chapter 11 Intermolecular Forces, Liquids, and Solids
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
11.1 A Molecular Comparison of Gases, Liquids, and Solids
11.2 Intermolecular Forces
11.3 Some Properties of Liquids
11.4 Phase Changes
11.5 Vapor Pressure
11.6 Phase Diagrams
11.7 Structure of Solids
11.8 Bonding in Solids
Chapter 13 Properties of Solutions
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
13.1 The Solution Process
13.2 Saturated Solutions and Solubility
13.3 Factors Affecting Solubility
13.4 Ways of Expressing Concentration
13.5 Colligative Properties
13.6 Colloids
Spring Semester
Chapter 14 Chemical Kinetics
Big Idea 4: Rates of Chemical Reactions are determined by the details of the molecular collisions
14.1 Factors that Affect Reaction Rates
14.2 Reaction Rates
14.3 The Rate Law: The Effect of Concentration on Rate
14.4 The Change of Concentration with Time
14.5 Temperature and Rate
14.6 Reaction Mechanisms
14.7 Catalysis
Chapter 15 Chemical Equilibrium
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.
15.1 The Concept of Equilibrium
15.2 The Equilibrium Constant
15.3 Interpreting and Working with Equilibrium Constants
15.4 Heterogeneous Equilibria
15.5 Calculating Equilibrium Constants
15.6 Applications of Equilibrium Constants
15.7 Le Châtelier’s Principle
Chapter 16 Acid-Base Equilibrium
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.
16.1 Acids and Bases: A Brief Review
16.2 Brønsted-Lowry Acids and Bases
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Strong Acids and Bases
16.6 Weak Acids
16.7 Weak Bases
16.8 Relationship between Ka and Kb
16.9 Acid-Base Properties of Salt Solutions
16.10 Acid-Base Behavior and Chemical Structure
16.11 Lewis Acids and Bases
Chapter 17 Additional Aspects of Aqueous Equilibria
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.
17.1 The Common-Ion Effect
17.2 Buffered Solutions
17.3 Acid-Base Titrations
17.4 Solubility Equilibria
17.5 Factors that Affect Solubility
17.6 Precipitation and Separation of Ions
17.7 Qualitative Analysis of Metallic Elements
Chapter 19 Chemical Thermodynamics
Big Idea 5: The Laws of Thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
19.1 Spontaneous Processes
19.2 Entropy and the Second Law of Thermodynamics
19.3 The Molecular Interpretation of Entropy
19.4 Entropy Changes in Chemical Reactions
19.5 Gibbs Free Energy
19.6 Free Energy and Temperature
19.7 Free Energy and the Equilibrium Constant
Chapter 20 Electrochemistry
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
20.1 Oxidation States and Oxidation-Reduction Reactions
20.2 Balancing Oxidation-Reduction Equations
20.3 Voltaic Cells
20.4 Cell EMF under Standard Conditions
20.5 Free Energy and Redox Reactions
20.6 Cell EMF under Nonstandard Conditions
20.7 Batteries and Fuel Cells
20.8 Electrolysis
Chapter 21 Nuclear Chemistry
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 4: Rates of Chemical Reactions are determined by the details of the molecular collisions
21.1 Radioactivity
21.2 Patterns of Nuclear Stability
21.3 Nuclear Transmutations
21.4 Rates of Radioactive Decay
21.5 Detection of Radioactivity
21.6 Energy Changes in Nuclear Reactions
21.7 Nuclear Power: Fission
21.8 Nuclear Power: Fusion
21.9 Radiation in the Environment and Living Systems
Tentative Schedule 2013-2014
Topic
# of Days
Introduction: Matter and Measurement
8
Atoms, Molecules, and Ions
8
Stoichiometry: Calculations with Chemical Formulas and Equations
7
Chapters 1 – 3 Test
1
Aqueous Reactions and Solution Stoichiometry
7
Thermochemistry
9
Electron Structure of Atoms
6
Chapters 4 – 6 Test
1
Periodic Properties of the Elements
9
Basic Concepts of Chemical Bonding
5
Molecular Geometry and Bonding Theories
5
Chapters 7 – 9 Test
1
Gases
8
Intermolecular Forces, Liquids, and Solids
6
Properties of Solutions
6
Chapters 10 – 13 Test
1
Final Exam Review
1
Final Exam (First Semester)
1
Chemical Kinetics
9
Chemical Equilibrium
9
Acid-Base Equilibria
12
Chapters 14 – 16 Test
1
Additional Aspects of Aqueous Equilibria
7
Chemical Thermodynamics
6
Electrochemistry
11
Chapters 17 – 20 Test
1
Nuclear Chemistry
4
AP Chemistry Test Review
10
AP Chemistry Test
1
Individual Chemical Laboratory Research
15
Final Exam Review
2
Final Exam (Second Semester)
1
The Laboratory:
Chemistry is an experimental science and, as such, the laboratory will be the focus of much of our efforts in the class. We will generally work on experiments at least two days each week. You are expected to be fully prepared for each experiment. Be familiar with the experiment before coming to class. Every student will be expected to maintain a lab notebook. All laboratory results are expected to be written in this notebook as the experiment is performed.
Laboratory reports are due for every lab group consisting of two people. It is highly suggested that lab partners alternate the writing of the reports, although both people should be involved in its production. You will be required to submit two types of laboratory reports: formal and in formal (abstract). The primary reason for having two types is to allow us to do as many experiments as possible. Formal laboratory reports require a great deal of time and effort to write; therefore, you will be able to submit an informal report for several experiments a grading period. The type of report required for each experiment will be marked on your tentative assignment schedule for the unit.
Formal Laboratory Report
Include a title page.
Title of Experiment
Names: Date:
AP Chemistry
The laboratory report will include the following sections (in this order): I. Purpose
II. Materials
III. Procedure
IV. Data /Results (including graphs)
V. Analysis Questions
VI. Conclusion
Abstract Laboratory Report Format
Title Page
Purpose
Results / Data Sheets
Conclusion
Lab
LABS
1
Lab Safety and introduction to materials and procedures
2
Tools and Measurement in the Lab: Calibration and Accuracy – students design protocols to test the accuracy and calibrate basic laboratory equipment such as balances, thermometers, and graduated cylinders.
Examination of Solutions, Hydration, and Electrolytes
- This activity is centered around an interactive simulation hosted by the University of Colorado at Boulder and introduces students to basic solution concepts (http://phet.colorado.edu/en/simulation/sugar-and-salt-solutions)
3
Determination of Mole Relationships in a Chemical Reaction
- Conforms to AP recommended procedure 9
4
Determination of Percent Water in a Compound
- Conforms to AP recommended procedures 2 and 16
5
Determination of the Empirical Formula of a Compound
- Conforms to AP recommended procedure 1
6
Determination of Concentration by Oxidation-Reduction Titration of H2O2
- Conforms to AP recommended procedure 8
7
Determination of an Electrochemical Series
- Conforms to AP recommended procedure 20
8
Measurements Using Electrochemical Cells and Electroplating
- Conforms to AP recommended procedure 21
9
Determination of Enthalpy Change Associated with a Reaction
- Conforms to AP recommended procedure 13
10
Determination of the Rate of a Reaction, Its Order and Its Activation Energy
- Conforms to AP recommended procedure 12
Examination of reaction kinetics under various conditions of concentration and temperature
- This virtual lab allows students to use a simulation from the University of Colorado at Boulder (located at http://phet.colorado.edu/en/simulation/reactions-and-rates to study the kinetic profiles of various reactions under various conditions
11
Examination of Equilibrium
- This activity uses a simulation from the University of Colorado at Boulder (located at http://phet.colorado.edu/en/simulation/reversible-reactions) to examine concepts of equilibria and how relevant parameters can be manipulated
12
Colorimetric or Spechtrophotometric Analysis & Determination of Keq
- Conforms to AP recommended procedures 10 and 17
13
Standardization of NaOH
- Conforms to AP recommended procedure 6
14
Acid-Base Titration
- Conforms to AP recommended procedure 7
15
Determination of Appropriate Indicators
- Conforms to AP recommended procedure 11
16
Preparation of Buffers
- Conforms to AP recommended procedure 19
17
Virtual – located at http://www.chm.davidson.edu/vce/CoordChem/index.html, this activity will allow students to virtually synthesize and analyze a coordination compound
- Conforms to AP recommended procedure 15
18
Determining the Molar Volume of a Gas
- Conforms to AP recommended procedure 5
19
Examination of Molecular Geometry
- This virtual lab is designed to provide students with experience observing and predicting molecular geometries. It is based on a simulation from the University of Colorado at Boulder located at http://phet.colorado.edu/en/simulation/molecule-shapes
20
Determination of Molar Mass by Vapor Density
- Conforms to AP recommended procedure 3
21
Establishing Patterns of Solubility through a series of reactions
- This lab is designed to reinforce students’ understanding of net ionic equations, predicting reaction products and identifying an unknown through its chemical properties
22
Determination of Molar Mass by Freezing Point Depression
- Conforms to AP recommended procedure 4
23
Synthesis of Aspirin (Lab kit and protocol from Flinn Scientific)
- Conforms to AP recommended procedure 22
Total Hours
34.5 Class hours
Instructor: Carl Africo
Introduction:
This course is similar in content to a high-level first year college chemistry course. In many aspects I will teach it as a college course would be taught. I hope that this experience will help prepare you for the realities of college; I want you to leave this course with at least as much knowledge of the chemistry subject matter and laboratory procedures that a college freshman would attain through his course work in that subject. You should also leave it with study, research, and organizational skills that will serve you well in college.
It is my intent to design this course to be as fulfilling for you as possible. You must put a lot of effort into the course; but, you will hopefully come away from it with deep satisfaction.
Class Times:
The AP chemistry class will meet for 70 minutes daily four days a week with one 90 minute day once a week for the entire school year. They will be 3 mandatory Saturday sessions and tutoring is available from 6:30am to 7:45 am on Mondays and Fridays.
Text: Brown, Theodore; Lemay, Eugene; Bursten, Bruce; and Catherine Murphy. Chemistry: The Central Science, Twelfth Edition.
Grading System:
Exams 25%
Labs / CIM Task 25%
Quizzes / Abstracts 20%
HW/CW 10%
Blogs / lab journals 10%
Group Participation 10%
Grading:
An examination will be given at the completion of every two chapters in the textbook. All examinations will consist entirely of multiple choice questions and free response questions. Each exam will primarily contain material covered since the previous exam. I will attempt to design the examinations to prepare you for the AP exam. Remember, chemistry, unlike many subjects, is cumulative. We often use concepts learned in earlier units of the course
Quizzes will be given on Fridays and will include problems and questions similar to the ones we have been working on in class during the week. They may also include questions about the experiment(s) done that week.
Homework / Class work:
You will generally have one to two hours of homework every day. Homework will include reading assignments, problems, preparing for labs, writing lab reports, and studying for quizzes and exams.
You will be given a set of homework problems for each chapter. These problems should be regarded as the minimum problem assignment. You are encouraged to attempt to do any additional problems. The more problems that you attempt to do the better prepared you will be in the course. As noted earlier, homework will not be collected but it will be checked periodically. We will discuss problems in class.
A word of warning!! There is a great temptation to neglect to do the homework. If you cannot assume this responsibility then you should not be in this class. You will not be successful and will only be a burden to others. There is no way that you can gain any real value from the class if you do not do the work outside of the class. You must be prepared to give this commitment to the class.
Grouping and Group work:
Within the first couple weeks of the course students are grouped in pairs. These groupings constitute lab partners, but are also used during classroom instruction. Partners are allowed to help each other during many class activities (obviously excluding formal assessments). Further, when activities will benefit from a larger group two pairs will work together. Throughout all of this work these pairs are held to accountable as a team which pair assessments and labs being used to link grades to provide motivation for mutual support. First among these group assignments is a problem of the day, which are generally drawn from past AP multiple choice questions. Students respond to these questions as a pair in a single notebook which is collected and scored weekly. Responses must include an answer choice, reason, and, if necessary a correction based on a brief class discussion.
Fall Semester
Chapter 1 Introduction: Matter and Measurement
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
1.1 The Study of Chemistry
1.2 Classification of Matter
1.3 Properties of Matter
1.4 Units of Measurement
1.5 Uncertainty in Measurement
1.6 Dimensional Analysis
Chapter 2 Atoms, Molecules, and Ions
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.
2.1 The Atomic Theory of Matter
2.2 The Discovery of Atomic Structure
2.3 The Modern View of Atomic Structure
2.4 Atomic Weights
2.5 The Periodic Table
2.6 Molecules and Molecular Compounds
2.7 Ions and Ionic Compounds
2.8 Naming Inorganic Compounds
2.9 Some Simple Organic Compounds
Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
3.1 Chemical Equations
3.2 Some Simple Patterns of Chemical Reactivity
3.2 Formula Weights
3.4 Avogadro’s Number and the Mole
3.5 Empirical Formulas from Analysis
3.6 Quantitative Information from Balanced Equations
3.7 Limiting Reactants
Chapter 4 Aqueous Reactions and Solution Stoichiometry
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.
4.1 General Properties of Aqueous Solutions
4.2 Precipitation Reactions
4.3 Acid-Base Reactions
4.4 Oxidation-Reduction Reactions
4.5 Concentrations of Solutions
4.6 Solution Stoichiometry and Chemical Analysis
Chapter 5 Thermochemistry
Big Idea 5: The Laws of Thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
5.1 The Nature of Energy
5.2 The First Law of Thermodynamics
5.3 Enthalpy
5.4 Enthalpies of Reaction
5.5 Calorimetry
5.6 Hess’s Law
5.7 Enthalpies of Formation
5.8 Foods and Fuels
Chapter 6 Electronic Structure of Atoms
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.
6.1 The Wave Nature of Light
6.2 Quantized Energy and Photons
6.3 Line Spectra and the Bohr Model
6.4 The Wave Behavior of Matter
6.5 Quantum Mechanics and Atomic Orbitals
6.6 Representations of Orbitals
6.7 Many-Electron Atoms
6.8 Electron Configurations
6.9 Electron Configurations and the Periodic Table
Chapter 7 Periodic Properties of the Elements
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
7.1 Development of the Periodic Table
7.2 Effective Nuclear Charge
7.3 Sizes of Atoms and Ions
7.4 Ionization Energy
7.5 Electron Affinities
7.6 Metals, Nonmetals, and Metalloids
7.7 Group Trends for the Active Metals
7.8 Group Trends for Selected Nonmetals
Chapter 8 Basic Concepts of Chemical Bonding
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule
8.2 Ionic Bonding
8.3 Covalent Bonding
8.4 Bond Polarity and Electronegativity
8.5 Drawing Lewis Structures
8.6 Resonance Structures
8.7 Exceptions to the Octet Rule
8.8 Strengths of Covalent Bonds
Chapter 9 Molecular Geometry and Bonding Theories
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
9.1 Molecular Shapes
9.2 The VSEPR Model
9.3 Molecular Shape and Molecular Polarity
9.4 Covalent Bonding and Orbital Overlap
9.5 Hybrid Orbitals
9.6 Multiple Bonds
9.7 Molecular Orbitals
9.8 Second-Row Diatomic Molecules
Chapter 10 Gases
Big Idea 2: Chemical and physical properties of materials can be explained by structure and arrangement of atoms, ions, or molecules and the forces between them.
10.1 Characteristics of Gases
10.2 Pressure
10.3 The Gas Laws
10.4 The Ideal-Gas Equation
10.5 Further Application of the Ideal-Gas Equation
10.6 Gas Mixtures and Partial Pressures
10.7 Kinetic-Molecular Theory
10.8 Molecular Effusion and Diffusion
10.9 Real Gases: Deviations from Ideal Gas Behavior
Chapter 11 Intermolecular Forces, Liquids, and Solids
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
11.1 A Molecular Comparison of Gases, Liquids, and Solids
11.2 Intermolecular Forces
11.3 Some Properties of Liquids
11.4 Phase Changes
11.5 Vapor Pressure
11.6 Phase Diagrams
11.7 Structure of Solids
11.8 Bonding in Solids
Chapter 13 Properties of Solutions
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
13.1 The Solution Process
13.2 Saturated Solutions and Solubility
13.3 Factors Affecting Solubility
13.4 Ways of Expressing Concentration
13.5 Colligative Properties
13.6 Colloids
Spring Semester
Chapter 14 Chemical Kinetics
Big Idea 4: Rates of Chemical Reactions are determined by the details of the molecular collisions
14.1 Factors that Affect Reaction Rates
14.2 Reaction Rates
14.3 The Rate Law: The Effect of Concentration on Rate
14.4 The Change of Concentration with Time
14.5 Temperature and Rate
14.6 Reaction Mechanisms
14.7 Catalysis
Chapter 15 Chemical Equilibrium
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.
15.1 The Concept of Equilibrium
15.2 The Equilibrium Constant
15.3 Interpreting and Working with Equilibrium Constants
15.4 Heterogeneous Equilibria
15.5 Calculating Equilibrium Constants
15.6 Applications of Equilibrium Constants
15.7 Le Châtelier’s Principle
Chapter 16 Acid-Base Equilibrium
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.
16.1 Acids and Bases: A Brief Review
16.2 Brønsted-Lowry Acids and Bases
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Strong Acids and Bases
16.6 Weak Acids
16.7 Weak Bases
16.8 Relationship between Ka and Kb
16.9 Acid-Base Properties of Salt Solutions
16.10 Acid-Base Behavior and Chemical Structure
16.11 Lewis Acids and Bases
Chapter 17 Additional Aspects of Aqueous Equilibria
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.
17.1 The Common-Ion Effect
17.2 Buffered Solutions
17.3 Acid-Base Titrations
17.4 Solubility Equilibria
17.5 Factors that Affect Solubility
17.6 Precipitation and Separation of Ions
17.7 Qualitative Analysis of Metallic Elements
Chapter 19 Chemical Thermodynamics
Big Idea 5: The Laws of Thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
19.1 Spontaneous Processes
19.2 Entropy and the Second Law of Thermodynamics
19.3 The Molecular Interpretation of Entropy
19.4 Entropy Changes in Chemical Reactions
19.5 Gibbs Free Energy
19.6 Free Energy and Temperature
19.7 Free Energy and the Equilibrium Constant
Chapter 20 Electrochemistry
Big Idea 3: Changes in matter involve the rearrangement and / or reorganization of atoms and / or the transfer of electrons
20.1 Oxidation States and Oxidation-Reduction Reactions
20.2 Balancing Oxidation-Reduction Equations
20.3 Voltaic Cells
20.4 Cell EMF under Standard Conditions
20.5 Free Energy and Redox Reactions
20.6 Cell EMF under Nonstandard Conditions
20.7 Batteries and Fuel Cells
20.8 Electrolysis
Chapter 21 Nuclear Chemistry
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 4: Rates of Chemical Reactions are determined by the details of the molecular collisions
21.1 Radioactivity
21.2 Patterns of Nuclear Stability
21.3 Nuclear Transmutations
21.4 Rates of Radioactive Decay
21.5 Detection of Radioactivity
21.6 Energy Changes in Nuclear Reactions
21.7 Nuclear Power: Fission
21.8 Nuclear Power: Fusion
21.9 Radiation in the Environment and Living Systems
Tentative Schedule 2013-2014
Topic
# of Days
Introduction: Matter and Measurement
8
Atoms, Molecules, and Ions
8
Stoichiometry: Calculations with Chemical Formulas and Equations
7
Chapters 1 – 3 Test
1
Aqueous Reactions and Solution Stoichiometry
7
Thermochemistry
9
Electron Structure of Atoms
6
Chapters 4 – 6 Test
1
Periodic Properties of the Elements
9
Basic Concepts of Chemical Bonding
5
Molecular Geometry and Bonding Theories
5
Chapters 7 – 9 Test
1
Gases
8
Intermolecular Forces, Liquids, and Solids
6
Properties of Solutions
6
Chapters 10 – 13 Test
1
Final Exam Review
1
Final Exam (First Semester)
1
Chemical Kinetics
9
Chemical Equilibrium
9
Acid-Base Equilibria
12
Chapters 14 – 16 Test
1
Additional Aspects of Aqueous Equilibria
7
Chemical Thermodynamics
6
Electrochemistry
11
Chapters 17 – 20 Test
1
Nuclear Chemistry
4
AP Chemistry Test Review
10
AP Chemistry Test
1
Individual Chemical Laboratory Research
15
Final Exam Review
2
Final Exam (Second Semester)
1
The Laboratory:
Chemistry is an experimental science and, as such, the laboratory will be the focus of much of our efforts in the class. We will generally work on experiments at least two days each week. You are expected to be fully prepared for each experiment. Be familiar with the experiment before coming to class. Every student will be expected to maintain a lab notebook. All laboratory results are expected to be written in this notebook as the experiment is performed.
Laboratory reports are due for every lab group consisting of two people. It is highly suggested that lab partners alternate the writing of the reports, although both people should be involved in its production. You will be required to submit two types of laboratory reports: formal and in formal (abstract). The primary reason for having two types is to allow us to do as many experiments as possible. Formal laboratory reports require a great deal of time and effort to write; therefore, you will be able to submit an informal report for several experiments a grading period. The type of report required for each experiment will be marked on your tentative assignment schedule for the unit.
Formal Laboratory Report
Include a title page.
Title of Experiment
Names: Date:
AP Chemistry
The laboratory report will include the following sections (in this order): I. Purpose
II. Materials
III. Procedure
IV. Data /Results (including graphs)
V. Analysis Questions
VI. Conclusion
Abstract Laboratory Report Format
Title Page
Purpose
Results / Data Sheets
Conclusion
Lab
LABS
1
Lab Safety and introduction to materials and procedures
2
Tools and Measurement in the Lab: Calibration and Accuracy – students design protocols to test the accuracy and calibrate basic laboratory equipment such as balances, thermometers, and graduated cylinders.
Examination of Solutions, Hydration, and Electrolytes
- This activity is centered around an interactive simulation hosted by the University of Colorado at Boulder and introduces students to basic solution concepts (http://phet.colorado.edu/en/simulation/sugar-and-salt-solutions)
3
Determination of Mole Relationships in a Chemical Reaction
- Conforms to AP recommended procedure 9
4
Determination of Percent Water in a Compound
- Conforms to AP recommended procedures 2 and 16
5
Determination of the Empirical Formula of a Compound
- Conforms to AP recommended procedure 1
6
Determination of Concentration by Oxidation-Reduction Titration of H2O2
- Conforms to AP recommended procedure 8
7
Determination of an Electrochemical Series
- Conforms to AP recommended procedure 20
8
Measurements Using Electrochemical Cells and Electroplating
- Conforms to AP recommended procedure 21
9
Determination of Enthalpy Change Associated with a Reaction
- Conforms to AP recommended procedure 13
10
Determination of the Rate of a Reaction, Its Order and Its Activation Energy
- Conforms to AP recommended procedure 12
Examination of reaction kinetics under various conditions of concentration and temperature
- This virtual lab allows students to use a simulation from the University of Colorado at Boulder (located at http://phet.colorado.edu/en/simulation/reactions-and-rates to study the kinetic profiles of various reactions under various conditions
11
Examination of Equilibrium
- This activity uses a simulation from the University of Colorado at Boulder (located at http://phet.colorado.edu/en/simulation/reversible-reactions) to examine concepts of equilibria and how relevant parameters can be manipulated
12
Colorimetric or Spechtrophotometric Analysis & Determination of Keq
- Conforms to AP recommended procedures 10 and 17
13
Standardization of NaOH
- Conforms to AP recommended procedure 6
14
Acid-Base Titration
- Conforms to AP recommended procedure 7
15
Determination of Appropriate Indicators
- Conforms to AP recommended procedure 11
16
Preparation of Buffers
- Conforms to AP recommended procedure 19
17
Virtual – located at http://www.chm.davidson.edu/vce/CoordChem/index.html, this activity will allow students to virtually synthesize and analyze a coordination compound
- Conforms to AP recommended procedure 15
18
Determining the Molar Volume of a Gas
- Conforms to AP recommended procedure 5
19
Examination of Molecular Geometry
- This virtual lab is designed to provide students with experience observing and predicting molecular geometries. It is based on a simulation from the University of Colorado at Boulder located at http://phet.colorado.edu/en/simulation/molecule-shapes
20
Determination of Molar Mass by Vapor Density
- Conforms to AP recommended procedure 3
21
Establishing Patterns of Solubility through a series of reactions
- This lab is designed to reinforce students’ understanding of net ionic equations, predicting reaction products and identifying an unknown through its chemical properties
22
Determination of Molar Mass by Freezing Point Depression
- Conforms to AP recommended procedure 4
23
Synthesis of Aspirin (Lab kit and protocol from Flinn Scientific)
- Conforms to AP recommended procedure 22
Total Hours
34.5 Class hours