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Basic Structure of the AP
Chemistry Exam |
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185 minute exam divided
into a multiple choice section and a free response section. |
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 Multiple
Choice Section:
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 | 90 minutes to answer 75 questions |
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| May not use a calculator |
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| 50% of total score |
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Practice Multiple
Choice Exam With Answers |
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Free
Response Section:
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| 95 minutes
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| 50 % of total score |
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| Tables containing commonly used
chemistry equations are provided with each examination for students to
use when taking the free-response section. Calculators
permitted and necessary for part A of free response. |
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| Two parts: Part A: problems and
Part B: concepts |
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one required question will be lab-based
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| Three problems, and
three
response questions will be graded. The first problem will be an
equilibrium problem. One will be a lab based question and could be
in either part A or part B.. |
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Part A:
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55 Minutes for
part A |
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| May use calculator |
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All three problems will be scored
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Partial credit is given for work; Show Work; a point will be deducted
for serious error in sig figs. |
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Problems are divided into parts.
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The first problem will be an equilibrium problem and is required.
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| Standard Reduction Potentials, Periodic Table and Formula Chart are
provided |
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Part B:
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| 40 minutes for part B |
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| May not use calculators |
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| Periodic Table, Formula Chart & Standard Reduction Potentials are provided
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Part B; three questions will be scored.
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Question 4
is required and will entail predicting equations.
Predicting Reactions
Practice Problems
or
Practice Equations AP Style
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In the new question 4 format, all
students will write balanced chemical equations for three
different sets of reactants and will answer a short question about
each of the three reactions.
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multiple Parts, stress understanding and explaining concepts
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stay to the point
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answer using bullet, chart format, list, or outline
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TOPIC
OUTLINE
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The percentage after each topic indicates
the approximate proportion of questions on the examination that pertain to the
topic. The examination is constructed using the percentages as guidelines
for question distribution. |
I. Structure of Matter (20%)
A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and
physical means
3. Atomic number and mass number; isotopes
4. Electron energy levels: atomic spectra, quantum
numbers, atomic orbitals
5. Periodic relationships including, for example,
atomic radii, ionization energies, electron affinities, oxidation states
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent,
metallic, hydrogen bonding, van der Waals (including London dispersion forces)
b. Relationship to states,
structure, and properties of matter
c. Polarity of bonds,
electronegativities
2. Molecular models
a. Lewis structures
b. Valence bond: hybridization
of orbitals, resonance, sigma and pi bonds
c. VSEPR
3. Geometry of molecules and ions, structural isomerism
of simple organic molecules and coordination complexes; dipole moments of
molecules; relation of properties to structure
C. Nuclear chemistry: nuclear equations, half-lives, and radioactivity;
chemical applications |
II. States of Matter (20%)
A. Gases
1. Laws of ideal gases
a. Equation of state for an
ideal gas
b. Partial pressures
2. Kinetic-molecular theory
a. Interpretation of ideal gas
laws on the basis of this theory
b. Avogadro's hypothesis and
the mole concept
c. Dependence of kinetic energy
of molecules on temperature
d. Deviations from ideal gas
laws
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular
viewpoint
2. Phase diagrams of one-component systems
3. Changes of state, including critical points and
triple points
4. Structure of solids; lattice energies
C. Solutions
1. Types of solutions and factors affecting solubility
2. Methods of expressing concentration
3. Raoult's law and colligative properties (nonvolatile
solutes); osmosis
4. Non-ideal behavior (qualitative aspects) |
III. Reactions (35-40%)
A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Bronsted-Lowry,
and Lewis; coordination complexes; amphoterism
2. Precipitation reactions
3. Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in
oxidation-reduction
c. Electrochemistry:
electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials;
Nernst equation; prediction of the direction of redox reactions
B. Stoichiometry
1. Ionic and molecular species present in chemical
systems: net ionic equations
2. Balancing of equations including those for redox
reactions
3. Mass and volume relations with emphasis on the mole
concept, including empirical formulas and limiting reactants
C. Equilibrium
1. Concept of dynamic equilibrium, physical and
chemical; LeChatelier's principle; equilibrium constants
2. Quantitative treatment
a. Equilibrium constants for
gaseous reaction: Kc, Kp
b. Equilibrium constants for
reactions in solution
I.
Constants for acids and bases; pK; pH
II.
Solubility product constants and their application to precipitation and the
dissolution of slightly soluble compounds
III. Common
ion effect; buffers; hydrolysis
D. Kinetics
1. Concept of rate of reaction
2. Use of experimental data and graphical analysis to
determine reactant order, rate constants, and rate laws
3. Effect of temperature change on rates
4. Energy of activation; the role of catalysts
5. The relationship between the rate-determining step
and a mechanism
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of formation;
heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry
3. Second law: entropy; free energy of formation; free
energy of reaction; dependence of change in free energy on enthalpy and entropy
changes
4. Relationship of change in free energy to equilibrium
constants and electrode potentials |
IV. Descriptive Chemistry (10-15%)
A. Chemical reactivity and products of chemical reactions
B. Relationships in the periodic table
C. Introduction to organic chemistry: hydrocarbons and functional groups
(structure, nomenclature, chemical properties) |
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V. Laboratory (5-10%)
The AP Chemistry Examination includes some questions based on experiences and
skills students acquire in the laboratory:
1. making observations of chemical reactions and
substances
2. recording data
3. calculating and interpreting results based on the
quantitative data obtained
4. communicating effectively the results of
experimental work |
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TEST
TAKING TIPS
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Multiple
Choice: |
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Do not
spend too much time on difficult questions. |
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Go
through entire test and answer all the easy questions first. |
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When you come to a question that you can answer but
it will take considerable time, mark the question and come back to
it after you have gone through the entire test. |
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You are penalized for wrong answers so do not
randomly guess. |
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You can mark in your test booklet so elimination works
well. If you can eliminate several choices you may want to guess. |
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Free
Response: |
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Questions require you to apply and explain chemical concepts and solve
multiple step problems. |
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You do not have to answer in essay form and may save time
using one of the following methods: bullet format, chart format or
outline format. |
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Write your answers in the space provided and number your
answer clearly. |
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| There is a slight penalty for incorrect sig figs.
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COLLEGE
BOARDS TEST DESCRIPTION
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As
described in the new 2007, 2008 AP Chemistry Course Description, the
AP Chemistry Exam will have a new format beginning in May 2007. It
is important to note that the content covered by the exam will
not change. The weighting of the two major parts of the exam
will change slightly -- Sections I and II will each contribute 50
percent toward the final grade.
Section I (90 minutes) will not change and will still consist of 75
multiple-choice questions with broad coverage of chemistry topics.
However, there will be three primary changes in the format of
Section II of the 2007 exam. While these changes do not introduce
new content, students should be made aware of these changes before
taking the exam in May 2007.
The first change in Section II is that students will no longer be
asked to choose between alternative questions. All students will do
the same six questions: three problems, the first of which is an
equilibrium problem; question 4 (reactions); and two essay
questions.
A second change in Section II relates to question 4, which assesses
students' knowledge about chemical reactions. Currently students are
asked to write chemical equations for five of eight given sets of
reactants. In the new question 4 format, all students will write
balanced chemical equations for three different sets of
reactants and will answer a short question about each of the three
reactions.
The third change in Section II relates to the timing of Part A
(during which calculators are permitted) and Part B (when no
calculators are permitted). In Part A, students will have 55 minutes
to answer three problems; in Part B, students will have 40 minutes
to answer question 4 and questions 5 and 6, the two essay questions.
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