AP Chemistry Syllabus
Honors Chemistry II and AP Chemistry Syllabus
Teacher: E. Reagan
emily.reagan@caswell.k12.nc.us
YOUR AP EXAM IS MONDAY May 4th 2015
Primary Text:
Chemistry, 9th Edition, Zumdahl and Zumdahl
Cracking the AP Chemistry Exam, 2012 Edition: Princeton Review: Books. ISBN 037542721X
Supplementary Print Resources:
Chemistry A Guided Inquiry, Richard S. Moog, John J. Farrell
Principal Online Resources:
Chem Team Main Menu
SAS in Schools
Unitedstreaming Video Site
Course Overview
The course is taught in two semesters of 90 days each. The first semester is called Honors Chemistry II, and the second is AP Chemistry. Each day’s class consists of a 90-minute block. Laboratory work is completed during one to three lab periods, depending on each lab’s complexity. The purpose pf AP Chemistry is tp provide a college level course in chemistry and to prepare the student to seek credit and/or appropriate placement in college chemistry courses. Emphasis is placed on depth of understanding of a topic, rather than skimming the topic. The day before tests are spend in study groups and all homework is due by this day as well as reading logs.
Structure of the Course
AP Chemistry is built around six big ideas and seven science practices. The big ideas are:
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 details of the 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.
Science Practice 1: The student can use representations and models to communicate scientific phenomena and solve scientific problems.
Science Practice 2: The student can use mathematics appropriately.
Science Practice 3: The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP course.
Science Practice 4: The student can plan and implement data collection strategies in relation to a particular scientific question.
Science Practice 5: The student can perform data analysis and evaluation of evidence.
Science Practice 6: The student can work with scientific explanations and theories.
Science Practice 7: The student is able to connect and relate knowledge across various scales, concepts, and representations in and across domains.
The following is an overview of the course and the correlation between Zumdahl and AP Topics as well as the order in which the topics will be covered through the year:
|Chapter in Zumdahl |AP Chemistry Topic Correlation |
|1. Chemical Foundation |None - Review |
|2. Atoms, Molecules, and Ions |Atomic Theory and Structure BI1 BI2 |
|3. Stoichiometry |Stoichiometry BI3 |
|4. Solution Stoichiometry and Chemical Analysis |Reaction types and Stoichiometry BI3 |
|5. Gases |Gases BI1 BI2 |
|22. Organic Chemistry |Descriptive Chemistry |
|7. Atomic Structure and Periodicity |Atomic Theory and Structure BI1 BI2 |
|14. Acids and Bases |Equilibrium BI6 |
|15. Application of Aqueous Equilibria |Equilibrium BI6 |
|8. Ionic Bonding |Chemical Bonding BI1 BI2 |
|9. Covalent Bonging |Chemical Bonding BI1 BI2 |
|10. Liquids and Solids |Chemical Bonding BI1 BI2 |
|6. Thermochemistry |Thermodynamics BI5 |
|17. Spontaneity, Entropy, and Energy |Thermodynamics BI5 |
|13. Chemical Equilibrium |Equilibrium BI6 |
|12. Chemical Kinetics |Kinetics BI4 |
|18. Electrochemistry |Reaction Types BI3 |
Teaching Strategies
As this is a second year course, students are expected to have a sound prior understanding of the basics of the following concepts:
• Nomenclature and equation writing and balancing
• Molar relationships
• Atomic structure, including electronic structure
• History of atomic theory
• Periodicity
• Gas laws
• Solutions
These topics are revisited during AP, but are covered more quickly. Classes consist of problem solving, discussion of chemical concepts, laboratory work, lecture, and some demonstrations. Quizzes are given biweekly, homework is assigned by chapter, and chapter tests are given at the end of each chapter. For chapter tests, I use questions from Zumdahl’s 6th Edition Test Bank, Princeton Review’s Cracking the AP Chemistry Test, released AP Test questions.
Students work in pairs on most labs. A few labs are geared for individual work. Each student is required to keep a permanently bound lab notebook, containing lab reports for each lab, including purpose, procedure, data, calculations, percent error, percent yield, where appropriate, and possible sources of error. These are graded after each lab. Students have a free exchange of ideas and techniques during lab classes. A few labs take the form of problems to be solved when students are given limited information and must develop lab procedures and carry them out to solve the problems. A few labs will last more than 1 class period and will require students to come to class at other times during the day to check on their experiment or record data.
Grading
Tests 50%, Labs 30%, Quizzes 10%, Homework/Class work 10%
The following is an outline of the topics and chapters covered and the order of coverage for each topic.
Prerequisites
Chemical Laboratory Safety
Chemical Laboratory Equipment
Requirements for Lab Manual
Chapter 1 Chemical Foundations
Relationships between measurements
Unit conversions within metric and between metric and English units
Accuracy and precision
Significant figures-rules and applications
Dimensional analysis
Density determinations, calculations, applications
Physical and chemical properties/changes
Temperature conversions
Assignments:
Read: Sections 1-9
Chapter 2 Atomic Theory, Atoms, Molecules, and Ions
Overview of the development of the atomic theory, including Dalton’s theory
Modern atomic theory of atomic structure
Isotopic symbols-students determine protons, electrons and neutrons from symbols
Calculating average atomic mass
Nomenclature review (ionic, covalent, and acid nomenclature rules)
Cation/anion formation and names
Properties of metals, nonmetals, and metalloids
Assignments:
Read: Sections 2-8
Chapter 19 Nuclear Chemistry
Band of stability
Nuclear particles and their properties
Writing and balancing nuclear equations
Half-life problems
Applications of Nuclear Chemistry
Chapter 3 Stoichiometry
Molar mass calculations
Percent composition problems
Empirical formula/molecular formula
Mass/mole/particle/volume conversions
Prediction of products of chemical reactions
Precipitation reactions
Writing and balancing equations from word equations
Complete molecular; Complete ionic; Net ionic
Stoichiometric calculations
Mole-mole; Mole-mass; Mass-mole; Mass-mass; Mass-volume; Percent yield
Assignments:
Read: Sections 1-9
Chapter 4 Solution Stoichiometry and Redox Reactions
Solubility rules
Polar and nonpolar molecules
Electrolytes
Molarity problems, Making dilutions
Titration calculations
Reaction Prediction and equation writing
Neutralization reactions
Recognizing redox reactions
Assigning oxidation numbers
Determining oxidized and reduced species in reactions
Writing redox half-reactions
Balancing redox reactions in acid and basic solutions
Definitions of acid, base, indicators, oxidation, reduction
Assignments:
Read: Sections 2-10
Chapter 22 Organic Chemistry
Nomenclature of the alkane, alkene, and alkyne series
Cis-Trans Isomerism
Basic functional groups
Alcohols, Esters, Carboxylic Acids
Aromatic hydrocarbons
Dehydration synthesis
Halogenated hydrocarbons
Preparation of aspirin and calculation of % yield
Assignments:
Read: Sections 1-4
Chapter 5 Gases
Kinetic Molecular Theory
Converting between pressure units
Avogadro’s Law
Ideal Gas Law
Boyle’s, Charles’, and Gay-Lussac’s Laws problems and applications
Graham’s Law
Determining molar mass from gas density
Assignments:
Read: Sections 1-6
Chapter 7 Atomic Structure and Periodicity
Periodicity of atomic trends (groups and periods)
Electron configurations and atomic properties
s, p, d, f orbitals and their positions on the periodic table
Valence electrons as a function of family
Noble gas core configurations
Assignments:
Read: Sections 1-8, 11-13
Chapter 14 Acids and Bases (covered 1st and 2nd semesters)
pH scale
Calculation of [H+], [OH-], pH, and pOH
Calculations based on experimental titration data
Assignments:
Read: Sections 14.1-14.7; 15.1-15.5
Sections of Chapters 8 - 10 Chemical Bonding
Types of chemical bonds
Electronegativity and bond polarity
VSEPR and Lewis Structures
Molecular geometry
Intermolecular forces and physical properties
Heating and cooling curves
Assignments:
Read: Sections 8.1-8.13; 9.1-9.2; 10.1; 10.8-10.9
Chapter 6 and 17 Thermochemistry and Thermodynamics
Law of Conservation of Energy
Potential and Kinetic Energy
Thermosicles Lab-preparation of a heating curve for H2O
Chemical energy
Delta E= q +w
Enthalpy calculations
Entropy
Delta H, Delta S, Delta G calculations
Q= m Cp D T calculations
Hess’s Law problems
Hess’s Law Lab
Delta Hf calculations
Spontaneity
Free Energy
Assignments:
Read: Sections 6.1-6.5; 16.1; 16.4-16.9
Chapter 13 Chemical Equilibrium
Writing equilibrium expressions
Calculation of equilibrium constants
Solving equilibrium problems Kp,Kc, Ksp
Le Chatelier’s Principle and applications
Predicting equilibrium shifts with changing conditions
Assignments:
Read: Sections 1-3; 5-7
Chapter 12 Chemical Kinetics
Reaction Rates
Rate Laws
Reaction Mechanisms
Lab-Determination of Rate of Decomposition of Crystal Violet
Assignments:
Read: Sections 1-8
Chapters 14 and 15 Acids and Bases
Acid-base theories; Arrhenius, Bronsted-Lowry, and Lewis
Strength of acids and bases
Acid-base titration curves
Solving acid-base problems pKa, pKb, pH, pOH
Acid-Base Titrations and analysis
Chapter 18 Electrochemistry
Galvanic cells
Cell Potential
Standard reduction potentials
Nernst equation
Assignments:
Read: Sections 1-7
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