Mr. Emrick
AP Chemistry/CITC Chemistry through Clark State Community College
Northwestern High School
2012-2013 School Year
Introduction:
The Advance Placement (AP) Chemistry/ CITC Chemistry through Clark State Community College course at Northwestern High School is a first-year college chemistry course taught on campus here at Northwestern High School. The students in this class have two options upon successful completion of the course. In May of 2011, students may take the AP Chemistry exam provided by the College Board Testing Services (approximately $80). The test is scored by the College Board and the score is sent to the colleges or universities indicated by the individual student. College credit may be awarded, at the discretion of the college or university, for a good score on the test. The students may also enroll at Clark State Community College and, at minimal cost and upon successful completion of the course, receive college credit. Class starts at 7:15 and unless you have prior permission, you will be counted tardy after that time.
2012-2013 Syllabus - 1 st Semester
Textbook
Chapters
Power Points
Problem
Sets
Associated
Labs
Topic
Measurements in Chemistry
Atomic Theory and Basic
Nomenclature and
Stoichiometry
Subtopics
Units
Significant
Figures
Objectives
Perform basic calculations related to laboratory measurement by:

Utilizing the correct metric units and convert these values to other units.
 Applying the rules for significant figures to calculation involving measurements.
 Defining and applying the terms, accuracy and precision, to laboratory measurements.
History of Atomic
Theory
Isotopes
Atomic Masses
Empirical and
Molecular
Formulas
Waves
Light
Electronic
Structure
Quantum
Numbers
The Orbital
Electron
Configuration
Atomic and Ionic
Radii
Ionization Energy
Electron Affinity
Electronegativity
Nomenclature
Stoichiometry
Describe atomic and molecular structure on various levels by:

Describing and explaining Dalton's atomic theory and its predictions.

Listing the subatomic particles and their properties.
 Describe the evidence for Quantum Theory and its implications; be familiar with quantum numbers.
Define the chemical mole and perform gram to mole and mole to gram conversions by:
 Applying the mole concept in the following situations: stoichiometric calculations,
 determining empirical and molecular formulas.
Predicting atomic structure and physical/chemical properties of elements using the periodic table.
Explain the reasoning behind the development of the periodic table by:
 Utilizing the periodic table to predict charges of monatomic ions, formulas of ionic compounds, electron configurations of atoms and ions.

Demonstrating knowledge of basic chemical and physical properties of the main group elements by group.
 Making predictions of relative properties of elements utilizing periodic trends.
Utilize chemical equations to describe and explain chemical reactivity by:
 Writing balanced chemical equations.
 Performing calculations using the mole concept in a variety of applications.
Chapter 1
Chapters 2, 3, and 7
Significant
Figures
Unit 1:
Lectures 1, 2,
3, 4, and 5
None All
Problem
Sets:
1, 2, 3, 4, and 5.
Problems from
Textbook
Lab 1
Determination of the
Chemical
Formula of
Magnesium
Oxide
Lab 2
Determination of the Formula of a Hydrate
Lab 3
Analytical
Gravimetric
Determination:
Percentage of
Phosphate in
Plant Food

2012-2013 AP Chemistry Syllabus - 1 st Semester (cont.)
Topic
Chemical
Bonding
Aqueous
Solutions and
Chemical
Reactions
Subtopics
Octet Rule
Ionic Bonding
Lattice Energy
Covalent Bonding
Lewis Diagrams
Exception to the
Octet Rule
Formal Charge
Bond Energy and
Bond Length
Resonance
Structures
Molecular Shapes
VSEPR Theory
Valence Bond
Theory
Hybrid Orbital
Theory
Multiple Bonds
Polar and Non-
Polar molecules
Electrolytic
Solutions
Solubility
Precipitation
Reactions
Redox Reactions
Oxidations
Numbers
Redox Reactions in
Acid and Basic
Solutions
The Activity Series
Halogen
Displacement
Reactions
Hydrogen
Displacement
Reactions
Disproportionation
Reactions
Synthesis Reactions
Decomposition
Reactions
Combustion
Reactions
Objectives
Determine molecular geometry from formulas of compounds by:
 Determining the number of valence electrons in molecules and polyatomic ions from their formulas using the periodic table.
 Drawing Lewis structures of molecules and polyatomic ions from their formulas.
 Determining the shapes of molecules and polyatomic ions from Lewis structures and models utilizing VSEPR concepts.
Explain and apply bonding theories by:
 Describing Valence-Bond Theory and its limitations.

Knowing the relationship between the various molecular geometries and hybridized orbitals.
 Describing the evidence for and the basic concepts of Molecular Orbital Theory and its implications.
 Utilizing MO theory to make predictions of magnetic properties and stability of small molecules/ions.
Utilize chemical equations to describe and explain chemical reactivity by:

Writing balanced chemical equations.

Writing ionic equations and predicting reaction outcomes for precipitation and acid-base reactions.
 Balancing oxidation-reduction reactions.

Performing calculations using the mole concept in a variety of applications.
Textbook
Chapters
Chapters 7, 8, and 9
Chapters 3 and
4
Power Points
Unit 3:
Lectures 10,
11, and 12
Problem
Sets
Associated
Labs
Unit 2:
Lectures 6, 7,
8, and 9
MO Theory
Power Point
Problem
Sets:
6, 7, 8, and 9
Problems from
Textbook
Line Spectra of Hydrogen
Problem
Sets:
10, 11, and 12
Problems from
Textbook
Lab 4
Mass – Mole
Relationship in a chemical
Reaction:
Precipitation of
Calcium
Carbonate
Lab 5
Standardization of Potassium
Permanganate
Solution Using a Primary
Standard, and
Determination of the
Concentration of Hydrogen
Peroxide in a
Solution

2012-2013 - AP Chemistry Syllabus - 1 st Semester (cont.)
Topic
Thermodynamics
Subtopics
Enthalpy
Calorimetry
Hess’s Law
Enthalpy of
Formation
Bond Energy
Entropy
Free Energy
Objectives
Explain and apply the first 2 laws of thermodynamics by:
 Describing and explaining the implications of the First Law of
Thermodynamics.
 Describing and explaining the implications of the Second Law of
Thermodynamics in terms of phase changes and chemical reactions.

Calculating work done in pressure-volume situations.
 Defining enthalpy.
 Calculating specific and molar heat capacities and energy changes involving these quantities.
Define the chemical mole and perform gram to mole and mole to gram conversions by:
 Applying the mole concept in the following situations: stoichiometric calculations, determining empirical and molecular formulas.
Demonstrate understanding of Hess's Law and Gibbs free energy by:

*Calculating heats of reactions utilizing Hess's law and individual reaction steps, bond dissociation energies, or standard heats of formation.
 Defining entropy and Gibbs free energy.
 Making predictions as to whether a process is spontaneous based upon general enthalpy and entropy values.
Textbook
Chapters
Chapters 6 and
16
Power Points
Unit 4:
Lectures 13 and 14
Problem
Sets
Associated
Labs
Problem
Sets:
13 and 14
Problems from
Textbook
Computer Lab
13
Determining the Enthalpy of a Chemical
Reaction
Gases
Pressure
Gas Laws
Ideal Gas Law
Partial Pressures
Mole Fractions
Average KE of a
Gas
Average Speed of a Gas
Effusion
Diffusion
Real vs. Ideal
Gases
Describe and apply the various gas laws by:
 Describing the Boyle's Law, Charles' Law, Graham's Law, Avogadro's Law and the
Ideal Gas Law;
 Applying these laws in calculations of pressure, volume, temperature and mass of gases in changing situations;

Explaining the gas laws using the Kinetic Molecular Theory of Matter.
Chapter 5
Unit 6:
Lectures 18,
19, and 20
Problem
Sets:
18, 19, and 20
Problems from
Textbook
Lab 9
Determination of Molar Mass by Vapor
Density:
Finding the
Molar Mass of
Butane
Lab 10
Determining the Molar
Volume of a
Gas: Finding the Molar
Volume of
Oxygen in a
Reaction
Between
Bleach and
Hydrogen
Peroxide

2012-2013 - AP Chemistry Syllabus - 1 st Semester (cont.)
Topic
Nuclear
Chemistry
Subtopics
Modes of Nuclear
Decay
Configurations for Nuclear
Stability
Binding Energy
Nuclear Fission
Nuclear Fusion
Objectives
Demonstrate understanding of basic nuclear chemistry by
 Describing spontaneous nuclear reactions including balancing nuclear equations and calculating energy changes associated with nuclear reactions
 Listing & describing the 5 ways in which chemical and nuclear reactions differ.

Applying the concepts of nuclear chemistry to define and apply: the radioactive half-life concept of radioactive decay, nuclear transmutation &
 its purpose, and the uses of nuclear chemistry in electricity production, dating (geological, anthropological, archeological), medical diagnosis and basic research.
Using the band of stability to predict and explain what type of radioactivity
(if any) a particular isotope will emit.


Calculating mass defect and binding energies for formation of nuclei.
Describing nuclear fusion and nuclear fission, including the components of a nuclear reactor
Textbook
Chapters
Chapter 18
Power Points
Problem
Sets
Associated
Labs
Unit 13:
Lecture 36
Nuclear
Reactor Power
Point
Problem
Set:
36
Problems from
Textbook
To Be
Determined
Assessment:

Every Topic will have one or more worksheet(s) to practice and assess acquisition of skills and applications of knowledge. These will be reviewed one day after the completion of the topic and subtopics covered in the worksheets. There will be no grade for these worksheets but to pass quizzes and tests you must complete these worksheets prior to their review. Try putting something down in writing on every question on the worksheet. It is OK to miss questions and learn from your mistakes.
Not trying a question at all is not OK.

There will be at least 12 to 15 short, 30-minute quizzes. You will be given exactly 30 minutes to take the quiz. There will be no extended time for the quiz, so don’t ask.
The quiz will cover recently completed lectures. Each quiz is worth 10 points.

At the end of each Unit there will be a period long test. The test will begin promptly at 7:15 and will be collected at 8:15. You will be given exactly one hour to take the test. There will be no extended time for the test, so don’t ask. The tests will vary from 20 to 30 points.

You will be taking a mid-semester exam at the end of the 1 st quarter. The test will be given over two days and will begin at 7:15 and end at 8:15. You will be given exactly one hour each day to take the exam. There will be no extended time for the exam, so don’t ask. Each exam will be a combination of multiple choice (day 1) and free response questions (day 2) from the first quarter. The exam will be 50 points.

There will be a semester exam given before winter break. The exam will begin promptly at 7:15 and end at 8:45. The exam will be a combination of multiple choice and free response questions from the first semester. The exam will be 100 points.

There are two different types of lab reports. o Formal labs reports (one each quarter) are typed, are worth 50 points (5 points for each bullet), and will include:
 title page (experiment title, your name, your partner’s name, date of lab, date of report, instructor)
 abstract of lab at the bottom of the title page

 purpose of the lab
 introduction that relates purpose to chemistry concepts
 summary of procedure
 data tables
 calculations
 analysis of data and calculations including error analysis
 summary of results of analysis as related to purpose
 pre-lab questions with answers o Informal lab report (those not assigned as formal) are worth 20 points (4 points for each bullet) and will include:
 pre-lab questions with answers
 data table(s)
 calculations
 analysis
 summary

Your grade for each quarter will be based on percentage of total points earned. See your agenda for letter grade.