Mr. Emrick
Northwestern High School
AP Chemistry/CITC Chemistry through Clark State Community College
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 2013, 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 five (5) semester units of college credit.
Class starts at 7:15 and unless you have prior permission, you will be counted tardy after that time.
2012-2013 Syllabus – 2nd Semester
Topic
Intermolecular
Forces
Solutions
Subtopics
Objectives
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Types of Forces
Boiling Points
Heat of Fusion
Heat of Vaporization
Vapor Pressure
Phase Diagrams
Solid State
Describe the types of intermolecular forces and apply this to properties
of solutions, solids and liquids by:

Defining and giving examples of the intermolecular forces;

Using the structure of a compound to determine its most relevant
intermolecular force and applying this to making predictions of
physical properties;

Describing the types of and performing calculations involving
crystal structures of solids.
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Types of Solutions
Expressing Concentrations
Solubility and Structure
Solubility of Solids and
Temperature
Solubility of Gases and
Temperature
Solubility of Gases and
Pressure
Colligative Properties of
Solutions
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Chemical
Kinetics
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Reaction Rates
Order of Reactions
Differentiated Rate Laws
Integrated Rate Laws
Half-Life of Reactions
Factors Affecting Reaction
Rates
Activation Energy, Ea
Reaction Mechanisms
Catalysis
Describe how to make various types solutions and perform calculations
involving their colligative properties by:

Defining molarity, molality, mole fraction and mass percent types
of solutions;

Utilizing these definitions in performing calculations of vapor
pressure, freezing point depression, boiling point elevation, and
osmotic pressure.
Perform calculations involving reaction rates and determine reaction
orders by:

Using rate data to determine reaction order and to write its rate
law and determine the rate constant.

Applying the integrated rate laws.

Defining and calculating activation energies and the catalysis
concept;

Defining and applying concept of rate limiting step in reaction
mechanism
Textbook
Chapters
Power
Points
Problem
Sets
Chapter
10
Unit 8:
Lectures
23 - 25
Problem
Sets 23 25
Chapter
11
Unit 9:
Lectures
26 - 28
Problem
Sets:
26 - 28
Unit 11:
Lectures
34 and
35
Problem
Sets:
34 and 35
Chapter
12
Associated Labs
Lab 13 - Chromatography
Lab 14 – Molar Mass by
Freezing Point Depression
Lab 21 – Determination of a
Rate Law
2012-2013 - AP Chemistry Syllabus - 2nd Semester (cont.)
Topic
Subtopics


Chemical
Equilibrium
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Acids, Bases,
Salts, Ksp
Equilibrium Constants (Keq,
Kc, and Kp)
Calculating Equilibrium
Constants
Manipulating Keq
The Reaction Quotient (Q)
Le Chatelier’s Principle
Gibbs Free Energy and
Equilibrium
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Defining Acids and Bases
Conjugate Pairs
The Strength of Acids and
Bases
Autoionization of Water
Ka and Kb
pH
Polyprotic Acids
Acid/Base Reactions
pH and Soluble Salts
Common Ion Effect
Buffered Solutions
Solubility and pH
Complex Ion Formation

Acid Base Titrations
Objectives
Calculate equilibrium constants, equilibrium concentrations and apply
Le Chatelier's principle by:

Calculating equilibrium constants from concentration data and
rate constants;

Calculating equilibrium concentrations from initial concentrations
and equilibrium constants;

Applying Le Chatelier principle to equilibrium situations.
Discuss and apply thermodynamic principles to calculations involving
free energy, entropy, enthalpy, and equilibrium by:

Demonstrating the connections between entropy and equilibrium;
entropy and probability.

Using standard molar entropy values to calculate the standard
molar entropy of reaction.

Stating and explaining the 3 laws of thermodynamics.

Calculating and applying standard free energy changes for
reactions from entropy and enthalpy changes and from standard
free energies of formation.

Calculating free energy changes of reactions in non-standard
states, using Q.

Relating free energy to equilibrium and the equilibrium constant
both in words and equations.
Calculate pH of solutions of strong and weak acids and bases and
buffers by:

Calculating pH of strong acids and bases;

Applying equilibrium analysis to calculating pH of weak acids and
bases;

Applying Le Chatelier principle to solutions of buffers;

Calculating pH of buffer solutions using Henderson-Hasselbach
equation.
Perform calculations involving solubility equilibria and calculate
equilibrium concentrations of situations involving common ion effect
by:

Applying equilibrium analysis to calculate equilibrium constants
(Ksp) of sparingly soluble salts;

Utilizing Ksp values to determine concentrations of ions at
equilibrium and in situations involving the common ion effect;

Applying Ksp and other equilibrium analyses to determine effect of
complex ion formation on concentrations at equilibrium.
Textbook
Chapters
Chapters
13 and 16
Power
Points
Unit 5:
Lectures
15, 16,
and 17
Problem
Sets
Problem
Sets:
15, 16,
and 17
Problems
from
Textbook
Associated Labs



Chapters
14 and15
Unit 10:
Lectures
29, 30,
31, 32,
and 33
Problem
Sets:
29, 30, 31,
32, and 33
Problems
from
Textbook
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Lab 7: The
Spectrophotometric
Analysis of the
Cobalt(II) Ion
Lab 8: Determining an
Equilibrium Constant
Lab 15: Qualitative
Analysis of Cations and
Anions
Lab 16: Preparation and
Properties of Buffered
Solutions
Lab 18: Determining the
pKa of Different Indicators
Lab 19: Standardization
of a Sodium Hydroxide
Solution Using a Primary
Standard
Lab 20: Determining
Concentration by
Acid/Base Titration:
Titration of Vinegar
2012-2013 - AP Chemistry Syllabus - 2nd Semester (cont.)
Topic
Subtopics
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
Electrochemistry
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Survey of
Elements
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Voltaic (Galvanic) Cells
Voltage
Standard Reduction
Potential
Standard Cell Potential
Spontaneous Redox
Reactions
Gibbs Free Energy
Nernst Equation
Concentration Cells
Electrolytic Cells
Representative
Elements: Groups 1A
Through 4A
Representative
Elements: Groups 5A
through 8A
Transition Metals and
Coordination Chemistry
Objectives
Describe galvanic and electrolytic cells and perform calculations involving
standard cell potential, free energy, equilibrium, and stoichiometry by:

Describing galvanic and electrolytic cells, including components of
each, half reactions and shorthand notation.

Using standard reduction potentials to calculate standard potentials of
cells, calculate standard free energy changes, equilibrium constants
and predict relative strengths of oxidizing/reducing agents.

Apply the Nernst equation to determine cell potentials, free energies
and reaction quotient (or vice versa) under non-standard conditions,
i.e. pH determinations.

Describing, in detail, important industrial examples of galvanic and
electrolytic cells including batteries, industrial process and prevention
of corrosion.

Calculating the amount of current needed or moles of product
produced in electrolytic applications.
Discuss the properties of main group elements in both descriptive and applied
situations by:

Describing and explaining why second period elements have properties
distinctive from other elements in the same groups focusing on the unique
chemistry of boron.

Describing the typical allotropes of the following elements, using their
structures to predict their general properties: carbon, silicon, nitrogen,
phosphorus, oxygen, sulfur.

Describe the existence and properties of typical compounds of carbon, silicon,
phosphorus and sulfur, including important industrial applications.

Relate the valence electron configurations of the main group elements to their
typical oxidation states in compounds.
Discuss the chemistry of the transition elements and explain color and bonding in
transition metal complexes utilizing valence bond theory and crystal field theory by:

Using the electron configurations of transition elements to predict their typical
oxidation states and the relative stabilities.

Describing the properties of important transition elements such as chromium,
iron and copper in their various oxidation states.

Stating and giving examples of the trends in the following properties of
transition elements: metallic, atomic radii and densities, ionization energies,
standard oxidation potentials.

Applying the terminology of coordination compounds and the typical
geometries, including the various ligand types to describe their structures and
properties.

Apply Valence Bond theory to explaining the bonding in coordination
complexes.

Use crystal field theory to explaining the color of complexes and their magnetic
properties by crystal field theory, including predicting the energy of
absorbance.
Textbook
Chapters
Chapter
17
Chapters
19, 20,
and 21
Power
Points
Unit 7:
Lecture
s 21
and 22
Problem
Sets
Problem
Sets:
21 and 22
Problems
from
Textbook
Problems
from
Textbook
Associated Labs



Lab 11: Determination
of an Electrochemical
Series
Lab 12: Measurements
Using Electrochemical
Cels
Lab 17: Synthesis and
Analysis of a
Coordination Compound
2012-2013 - AP Chemistry Syllabus – 2nd Semester (cont.)
Topic
Organic
Chemistry
Biochemistry
Subtopics




Naming Hydrocarbons
Functional Groups
Isomers
Polymers

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
Lipids
Carbohydrates
Proteins
Objectives
Describe and predict properties of various functional groups in organic
chemistry and name simple organic molecules by:

Describing organic molecules containing single bonds, double
bonds and triple bonds in terms of hybridization, geometry, bond
angles, and number of sigma and pi bonds.

Recognizing functional groups and using their structures to predict
physical properties and acid/base properties.

Identifying, naming and describing the shapes of alkanes,
cycloalkanes, alkenes, alkynes and simple aromatics; identifying
polymers.

Writing chemical equations for the major reactions of alkanes,
alkenes and simple aromatic compounds
Describe and predict properties and roles of various biochemicals by:

Describing the four stages in catabolism and the role of ATP.

Defining, recognizing structures & giving examples of: mono-, diand polysaccharides; lipids including fats, oils, steroids; amino
acids as polar, nonpolar, acidic and basic, the four common
nucleotides.

Defining terms specific to carbohydrates, describing the structure
and properties of important mono-, di- and polysaccharides.

Relating the physical properties of fatty acids to the # of carbon
atoms and the # of double bonds.

Describing & giving examples of the four levels of protein
structure, including the process by which amino acids combine to
form proteins.

Using enzyme terminology & the lock and key model to describe
enzyme action.

Using the structures of the nucleotides to explain the Watson Crick Model of DNA structure & how this structure is utilized in the
processes of replication, transcription and translation.
Textbook
Chapters
Power
Points
Problem
Sets
Problem
Set:27
Chapter
22
Chapter
22
Lecture
37
Problems
from
Textbook
Associated Labs

Lab 22: Synthesis,
Purification, and
Analysis of an Ester
Problems
from
Textbook
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.
2012-2013 - AP Chemistry Syllabus – 2nd Semester (cont.)
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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 1st 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 second 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.