AP Chemistry

Period 5 Instructor: Dr. Brian Campbell

Room 10

Textbook

Zumdahl, Steven S. and Zumdahl, Susan A., Chemistry. Eighth Edition.

2010. Houghton-Mifflin.

Lab Manual

Wentworth, R.A.D. Experiments in General Chemistry. Sixth Edition. 2000.

Houghton-Mifflin.

Randall, J., et.al. Advanced Chemistry with Vernier. Second Edition. 2007.

Vernier Software and Technology

Class Goals

The student who takes AP Chemistry will be exposed to the advanced study

of chemistry as it pertains to the following areas:

- Structure of Matter

- States of Matter

- Chemical Reactions

- Descriptive Chemistry

- Laboratory Exercises

This course will emphasize scientific problem solving, chemical calculations,

and mathematical formulation of chemical principles. The laboratories are

like those conducted in a freshman level collegiate class. Students will

physically manipulate equipment and materials, collect data and use it to

form conclusions and verify hypotheses. Students will be required to keep a

bound laboratory notebook and submit written reports of all their labs.

Students are required to take the AP Chemistry Examination in May.

Individual students may obtain college credit if they score well enough on

this exam. However, many students have found the experience of taking this

course to be quite valuable in preparing them for college chemistry even if

they did not pass the AP Chemistry Exam.

The class will meet for 60 minutes every day, five days per week. Students

should expect to devote an average of 2 periods per week to laboratory

exercises. (Some labs will require more than two periods and others less.)

Grading

Grades will be determined on the following items.

Homework – 20%

Labs – 40%

Quizzes – 40%

Homework: At the end of lecture there will be problems assigned from

the textbook, which will be due the following day. At the end of a unit there

will be a homework assignment with multiple choice and free response

questions as well.

Labs: Lab reports will be due two days following the conclusion of a

lab. Late lab reports will only be accepted with a substantial penalty. Each

report will be written in ink (no pencil!) in a bound lab book. All lab exercises

will be conducted in groups of 2 or 3 students. Each report will have the

following items.

- Title of the lab

- Objectives of the lab

- A hypothesis

- Pre-lab questions

- Any relevant data

- Any required calculations and post-lab questions

- A statement of errors

- A final statement of conclusions

Quizzes: There will be a quiz consisting of 10 multiple choice questions

and two free response questions at the end of each unit. One of the free

response questions will concern the unit content, and the other will involve

either nomenclature or chemical equations. There will be instruction on the

type of equations within each unit. The quizzes are designed to be completed

in one class period.

Quarter Grades are assigned as follows: (New in 2012 – 2013)

A 100% - 90%

B 89% - 80%

C 79% - 70%

D 69% - 60%

F 59% - 0%

Course Outline (Subject to change)

Chapters 1 and 2 will be covered in the summer assignment.

Chapter 1 – Chemical Foundations

- Dimensional analysis

- Uncertainty

- Significant figures

- Lab – Measurements of Mass and Volume

Chapter 2 – Atoms, Ions, and Molecules

- Atomic theory

- Writing formulas

- Nomenclature

- Lab – Isotopes and Mass Spectroscopy

Unit 1 - Stoichiometry

Chapter 3 – Stoichiometry

- Atomic mass

- Moles and molar mass

- Empirical and molecular formulas

- Balancing chemical equations

- Stoichiometric calculations

- Limiting Reactant

- Percent Yield

- Lab – Empirical Formula of an Oxide and Determination of an

Unknown Compound

- Nomenclature – Ionic and Covalent

Unit 2 - Gases

Chapter 5 – Gases

- Pressure

- Gas laws

- Ideal gas law

- Gas stoichiometry

- Dalton’s law of partial pressures

- Kinetic molecular theory of gases

- Graham’s law of effusion

- Real gases and the van der Waal’s equation

- Lab – Boyle’s Law and the Empty Space in Air

- Nomenclature – Acids and salts

Unit 3 – Atomic Structure

Chapter 7 – Atomic Structure and Periodicity

- Electromagnetic radiation

- Atomic spectra

- Bohr’s model

- Quantum theory and quantum numbers

- Atomic orbitals

- Electron configurations

- Periodic table

- Periodic trends

- Lab – Solubilities Within a Family and Absorption Spectrum of

Cobalt (II) Chloride

- Nomenclature – Oxidation numbers

Unit 4 – Bonding and Intermolecular Forces

Chapters 8, 9, and 23 – Chemical Bonding and Organic Chemistry

- Types of chemical bonds

- Lewis structures

- Exceptions to the octet rule

- Resonance

- Polarity of bonds and compounds

- VSEPR model

- Hybridization (Chapter 9)

- Organic chemistry (Chapter 23)

- Lab – Molecular Models of Organic Compounds and From Oil of

Wintergreen to Salicylic Acid

- Nomenclature – Organic nomenclature and functional groups

Chapter 10 – Liquids and Solids

- Intermolecular forces

- Properties of liquids

- Properties of solids

- Types of solids

- Phase changes and phase diamgrams

- Lab – A Student’s View of Liquids and Solids

Unit 5 – Solutions (A portion of Chapter 10 regarding phase changes may be

included here.)

Chapter 4 – Types of Chemical Reactions and Solution Stoichiometry

- Aqueous solutions

- Molarity

- Solubility rules and precipitation reactions

- Solution stoichiometry

- Oxidation – reduction reactions

- Lab – Ionic Reactions in Aqueous Solution

Chapter 11 – Solutions

- The solution process

- Factor affecting solubility

- Molality, mole fraction, normality, and percent by mass

- Colligative properties

- Electrolytes and nonelectrolytes

- Colloids

- Lab – Molar Mass From Freezing Point Depression

- Equations – Double Replacement Reactions and Net Ionic

Equations

Unit 6 - Kinetics

Chapter 12 – Chemical Kinetics

- Reaction rates

- Rate laws

- Half-life

- Activation energy

- Reaction mechanisms

- Catalysts

- Lab – Iodine Clock Reaction

- Equations – Single Replacement Reactions

Unit 7 – General Equilibrium

Chapter 13 – Chemical Equilibrium

- Equilibrium expressions and constants

- Law of mass action

- Gas phase equilibrium

- Le Chatlier’s principle

- Reaction quotients

- Calculating equilibrium concentrations

- Lab – Le Chatelier’s Principle and Determining an Equilibrium

Constant

- Equations – Synthesis Reactions

Unit 8 – Acids and Bases

Chapter 14 – Acids and Bases

- Nature of acids and bases

- Strength of acids and bases

- Acid – base theories

- pH

- Acid – base equilibrium

- Lab – How Much Acetic Acid is in Vinegar and An Acid-Base

Titration Curve

- Equations – Anhydride Reactions

Unit 9 – Equilibrium Applications

Chapter 15 – Applications of Aqueous Equilibria

- Common ion effect

- Buffers

- Titrations

- Solubility equilibrium

- Fractional precipitation

- Qualitative Analysis

- Lab – Qualitative Analysis

- Equations – Decomposition Reactions

Unit 10 - Thermodynamics

Chapter 6 – Thermochemistry

- Energy and the 1st law of thermodynamics

- Enthalpy

- Calorimetry

- Hess’s Law

- Standard enthalpy of formation

- Lab – Thermochemistry and Hess’s Law

- Equations – Combustion Reactions

Chapter 16 – Spontaneity, Entropy and Free Energy

- Spontaneous processes

- Second and third laws of thermodynamics

- Entropy

- Free energy

- Equilibrium effects

- Lab – Spontaneity

Unit 11 – Electrochemistry (A portion of Chapter 4 may be covered here)

Chapter 17 – Electrochemistry

- Galvanic cells

- Standard reduction potentials

- Nernst equation

- Concentration effects

- Equilibrium effects

- Faraday’s laws

- Lab – Electrochemistry

- Equations – Redox Reactions

Unit 12 – Transition Metal Chemistry and Nuclear Chemistry

Chapter 20 – Transition Metals and Coordination Chemistry

- Properties of transition metals

- Coordination compounds

- Ligands

- Isomerism in coordination compounds

- Crystal field theory

- Lab – Thermochemistry of Complex Ions

- Equations – Complex Ion Reactions

Chapter 21 – The Nucleus: A Chemist’s View

- Nuclear stability and radioactivity

- Kinetics of radioactive decay

- Nuclear equations

- Fission and fusion

- Lab – Radioactivity of Potassium Chloride

AP Exam – May 6, 2013