AP Chemistry (REA) - The Best Test Prep for the Advanced Placement Exam

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Overview



REA … Real review, Real practice, Real results.
 
Get the college credits you deserve.
 
AP CHEMISTRY, New 10th Edition
Completely aligned with today’s AP exam
 
Are you prepared to excel on the AP exam? 
* Set up a study schedule by following our results-driven timeline
* Take the first practice test to discover what you know and what you
   should know
* Use REA's advice to ready yourself for proper study and success
 
Practice for real
* Create the closest experience to test-day conditions with 6 full-length practice tests
* Chart your progress with full and detailed explanations of all answers
* Boost your confidence with test-taking strategies and experienced advice
 
Sharpen your knowledge and skills
* The book’s full review features coverage of all AP Chemistry main topic areas, such as solutions, stoichiometry, kinetics, and thermodynamics, as well as all subject areas found on the official exam, including the structure of matter, the states of matter, chemical reactions, and descriptive chemistry.
* Smart and friendly lessons reinforce necessary skills
* Key tutorials enhance specific abilities needed on the test
* Targeted drills increase comprehension and help organize study
 
Ideal for Classroom, Family, or Solo Test Preparation!
 
REA has provided advanced preparation for generations of advanced students who have excelled on important tests and in life. REA’s AP study guides are teacher-recommended and written by experts who have mastered the course and the test.
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Product Details

  • ISBN-13: 9780738602219
  • Publisher: Research & Education Association
  • Publication date: 3/15/2006
  • Series: Test Preps
  • Edition description: Ninth
  • Edition number: 9
  • Pages: 528
  • Age range: 16 - 17 Years
  • Product dimensions: 6.80 (w) x 9.80 (h) x 1.60 (d)

Read an Excerpt

THE AP CHEMISTRY EXAM

ABOUT THE EXAMINATION
The Advanced Placement Chemistry Examination is offered each May at participating schools and testing centers throughout the world. The Advanced Placement Program is designed to allow high school students to pursue college-level studies while attending high school. Participating colleges, in turn, grant credit and/or advanced placement to students who do well on the examinations.
The Advanced Placement Chemistry course is designed to be the equivalent of a college introductory chemistry course, often taken by chemistry majors in their first year of college. Since the test covers a broad range of topics, no student is expected to answer all of the questions correctly. (Consequently, it is important for students to not feel defeated when confronting a question that appears unanswerable.)
The examination follows the outline, published by the College Board, that appears below. The exam is divided into two, 90 minute sections. The first section is composed of 75 multiple-choice questions designed to test recall of a broad range of concepts and calculations. The score students earn on the multiple-choice test composes 45% of the total score. Calculators are not permitted on the multiple choice portion of the exam, although simple arithmetic may be needed to answer some questions.
The second section is a free-response exam and constitutes 55% of the final grade. Calculators are allowed on Part A, during which the student has 40-minutes to complete two problems. Calculators are not allowed on Part B, during which students have 50 minutes to complete chemical reaction questions and three essay questions. Most hand-held calculators are allowed in the examination. However, calculators with typewriter-style (QWERTY) keypads are not allowed. If you are unsure if your calculator is permitted, check with your teachers or Educational Testing Services.
A detailed outline of the topics on the examination and specific strategies for both portions of the Advanced Placement Chemistry examination follow.

DETAILED OUTLINE OF THE EXAMINATION
The following is an outline of the general breadth of topics that The College Board identifies as being on the AP Chemistry Examination.

I. Structure of Matter (20% of the AP test)
A. Atomic theory and structure
1. Evidence for atomic theory
2. Atomic mass
3. Atomic number, mass number; isotopes
4. Electron energy levels, quantum numbers, atomic orbitals
5. Periodic relationships: atomic radii, ionization energy, electron affinity, oxidation states.
B. Chemical Bonding
1. Binding forces a.Types of forces: ionic, covalent, network covalent, metallic, hydrogen bonding, van der Waals.
b.Relationships to states, structure, and properties of matter.
c.Polarity of bonds, electronegativities.
2. Molecular Models a.Lewis structures b.Hybridization of orbitals, resonance, sigma and pi bonds.
c.VESPR
3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination compounds; 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% of the AP test)
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 theory b. Avogadros hypothesis and the mole concept c. Dependence of kinetic energy on temperature d. Deviations in the ideal gas laws
B. Liquids and Solids
1. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams
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. Raoults law and colligative properties; osmosis
4. Behavior of non-ideal solutions

III. Reactions (35-40% of the AP test)
A. Reaction types
1. Acid-base reactions, concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes, amphoterism.
2. Precipitations reactions
3. Oxidtion-reduction reactions a.Oxidation number b.The role of the electron in oxidation-reduction c.Electrochemistry: electrolytic and galvanic cells; Faradays 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 reactions
2. Balancing of equations, including oxidation-reduction 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; Le Chateliers principle; equilibrium constants
2. Quantitative treatment a.Equilibrium constants for gaseous reactions: Kp, Kc 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 dissolution of slightly soluble compounds iii. Common ion effect; buffers; hydrolysis
D. Kinetics
1. Concept of reaction rate
2. Use of experimental data and graphical analysis to determine reaction order, rate constants, and rate laws
3. Effect of temperature on reaction rates
4. Energy of activation; the role of catalysts
5. Relationship between the rate-determining step and mechanism of reaction
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of formation; heat of reaction; Hesss 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 of enthalpy and entropy changes
4. Relationship between change in free energy, equilibrium constants, and electrode potentials

IV. Descriptive Chemistry (10-15% of the AP test)
A. Chemical reactivity and products of chemical reactions
B. Relationships in the periodic table; horizontal, vertical, and diagonal with examples of alkali metals, alkaline earth metals, halogens, and the first series of transition metals
C. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)

V. Laboratory (5-10% of the AP test)
A. Making observations of chemical reactions
B. Recording data
C. Calculating and interpreting results based on observed quantitative data
D. Effectively communicating experimental results, including error analysis

Format, Scoring, and Strategies of Multiple Choice questions and Free Response Questions follows...

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Table of Contents

TABLE OF CONTENTS

About Our Author
Independent Study ScheduLe

Chapter 1

THE AP CHEMISTRY EXAM
  About the Examination
  Detailed Outline of Examination
  Multiple Choice Strategies
  Free Response Strategies

Chapter 2

ATOMIC THEORY AND STRUCTURE
  Evidence for Atomic Theory
  Atomic, Mass, Atom Number, isotopes
  Electrons
  Periodic Trends

Chapter 3

BONDING
  Bonds Between Atoms
  Molecular Models
  Attractions Between Molecules; Polarity
  Structure and Physical Properties

Chapter 4

NUCLEAR CHEMISTRY
  Nuclear Reactions and Equations
  Rate of Decay; Half-Life
  Nuclear Stability and Radioactivity

Chapter 5

GASES
  Ideal Gas Laws
  Kinetic Molecular Theory
  Deviations from Ideal Gas Laws

Chapter 6

LIQUIDS AND SOLIDS
  Phase Diagrams
  Phase Changes
  Properties of Liquids
  Properties of Solids

Chapter 7

SOLUTIONS
  Solubility
  Solution Concentrations
  Colligative Properties
  Nonideal Solutions

Chapter 8

TYPES OF REACTIONS
  Acid-Base Reactions
  Precipitations Reactions
  Oxidation-Reduction Reactions

Chapter 9

STOICHEOMETRY
  Balancing Chemical Equations
  Mole Conversions
  Stoicheometry Problems
  Limiting Reactants
  Empirical Formulas and Percent Composition

Chapter 10

EQUILIBRIUM
  Le Chatlier's Principal
  Equilibrium Constants
  Reaction Quotient, Q
  Equilibrium Constants for Gaseous Reactions
  Equilibrium Constants for Reactions in Solution
  Common Ion Effect
  Buffers

Chapter 11

KINETICS
  Reaction Rate
  Rate law and Reaction Order
  Kinetics and Equilibrium
  Temperature and Reaction Rates
  Activation Energy and Catalysts
  Reaction Mechanisms

Chapter 12

THERMODYNAMICS
  State Functions
  The First Law and Enthalpy
  The Second Law, Entropy, and Free Energy
  G°, K, and E°

Chapter 13

DESCRIPTIVE CHEMISTRY
  Products of Chemical Reactions
  Relationships in the Periodic Table
  Inorganic Compounds
  Organic Molecules

Chapter 14

LABORATORIES
  Lab safety
  Lab Measurements
  Example Problems for the Recommended Experiments

PRACTICE EXAMS

AP CHEMISTRY EXAM 1
  Answer Key
  Detailed Explanations of Answers
AP CHEMISTRY EXAM 2
  Answer Key
  Detailed Explanations of Answers

AP CHEMISTRY EXAM 3
  Answer Key
  Detailed Explanations of Answers
AP CHEMISTRY EXAM 4
  Answer Key
  Detailed Explanations of Answers
AP CHEMISTRY EXAM 5
  Answer Key
  Detailed Explanations of Answers
ANSWER SHEETS

GLOSSARY

INDEX

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