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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