Examkrackers MCAT Chemistry / Edition 4

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Overview

198 full color pages covering all topics in MCAT inorganic chemistry, including an index and seven 30-minute MCAT practice exams with answers and explanations(161 questions), 168 additional MCAT practice questions also with answers and explanations.
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Product Details

  • ISBN-13: 9781893858282
  • Publisher: Osote Publishing
  • Publication date: 2/1/2003
  • Series: Examkrackers
  • Edition description: Fourth Edition
  • Edition number: 4
  • Pages: 212
  • Product dimensions: 8.52 (w) x 10.96 (h) x 0.43 (d)

Read an Excerpt

There are three definitions of an acid that you must know for the MCAT: Arrhenius, Bronsted-Lowry, and Lewis. These definitions are given here in the order in which they were created. An Arrhenius acid is anything that produces hydrogen ions in aqueous solution, and an Arrhenius base is anything that produces hydroxide ions in aqueous solution. This definition covers only aqueous solutions. Bronsted and Lowry redefined acids as anything that donates a proton, and bases as anything that accepts a proton. Finally, the Lewis definition is the most general, defining an acid as anything that accepts a pair of electrons, and a base as anything that donates a pair of electrons. The Lewis definition includes all the acids and bases in the Bronsted-Lowry and more. Lewis acids include molecules that have an incomplete octet of electrons around the central atom, like AlCl3 and BF3. They also include all simple cations except the alkali and the heavier alkaline earth metal cations. The smaller the cation and the higher the charge, the stronger the acid strength. Fe3+ is a common example of a Lewis acid. Molecules that are acidic only in the Lewis sense are not generally called acids unless they are referred to explicitly as Lewis acids.
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Table of Contents

Table of Contents
Lecture 1: Atoms, Molecules, and Quantum Mechanics 1
1-1 Atoms 1
1-2 Elements 2
1-3 The Periodic Table 3
1-4 Characteristics Within Groups 4
1-5 Ions 6
1-6 SI Units and Prefixes 10
1-7 Molecules 10
1-8 Naming Inorganic Compounds 12
1-9 Chemical Reactions and Equations 12
1-10 Chemical Yield 13
1-11 Fundamental Reaction Types 13
1-12 Reaction Symbols 14
1-13 Bonding in Solids 14
1-14 Quantum Mechanics 16
1-15 Quantum Numbers 16
1-16 The Heisenberg Uncertainty Principle 17
1-17 Energy Level of Electrons 17
Lecture 2: Gases, Kinetics, and Chemical Equilibrium 23
2-1 Gases 23
2-2 Kinetic Molecular Theory 24
2-3 Real Gases 27
2-4 Chemical Kinetics 29
2-5 The Collision Theory 29
2-6 Equations for Reaction Rates 30
2-7 Determining the Rate Law by Experiment 31
2-8 Recognizing Reaction Orders 32
2-9 Rates of Reversible Reactions 33
2-10 Catalysis 34
2-11 Effects of Solvent on Rate 36
2-12 Equilibrium 38
2-13 The Partial Pressure Equilibrium Constant 39
2-14 The Reaction Quotient 39
2-15 Le Châtelier’s Principle 40
Lecture 3: Thermodynamics 45
3-1 Thermodynamics 45
3-2 State Functions 45
3-3 Heat 46
3-4 Work 48
3-5 The First Law of Thermodynamics 49
3-6 Heat Engines 49
3-7 Thermodynamic Functions 53
3-8 Internal Energy 53
3-9 Temperature 54
3-10 Pressure 55
3-11 Enthalpy 55
3-12 Entropy 59
3-13 Gibbs Free Energy 61
Lecture 4: Solutions 65
4-1 Solutions 65
4-2 Colloids 66
4-3 More Solutions 66
4-4 Units of Concentration 67
4-5 Solution Formation 70
4-6 Vapor Pressure 71
4-7 Solubility 75
4-8 Solubility Guidelines 76
4-9 Solubility Factors 77
Lecture 5: Heat Capacity, Phase Change, and Colligative Properties 79
5-1 Phases 79
5-2 Heat Capacity 80
5-3 Calorimeters 81
5-4 Phase Changes 83
5-5 Phase Diagrams 84
5-6 Colligative Properties 88
Lecture 6: Acids and Bases 93
6-1 Definitions 93
6-2 How Molecular Structure Affects Acid Strength 96
6-3 Hydrides 97
6-4 Equilibrium Constants for Acid-Base Reactions 99
6-5 Finding the pH 100
6-6 Salts 101
6-7 Titrations 103
6-8 More Titrations and Buffered Solutions 103
6-9 Indicators and the End Point 105
6-10 Polyprotic Titrations 106
Lecture 7: Electrochemistry 109
7-1 Oxidation-Reduction 109
7-2 Oxidation States 109
7-3 Oxidation-Reduction Titrations 111
7-4 Potentials 113
7-5 Balancing Redox Reactions 114
7-6 The Galvanic Cell 114
7-7 IUPAC Conventions 116
7-8 Free Energy and Chemical Energy 117
7-9 More Cells 120
30-Minute In-class Exams 125
In-Class Exam for Lecture 1 125
In-Class Exam for Lecture 2 131
In-Class Exam for Lecture 3 137
In-Class Exam for Lecture 4 143
In-Class Exam for Lecture 5 149
In-Class Exam for Lecture 6 155
In-Class Exam for Lecture 7 161
Answers & Explanations to In-Class Exams 167
Answers and Scaled Score Conversion for In-Class Exams 168
Explanations to In-Class Exam for Lecture 1 169
Explanations to In-Class Exam for Lecture 2 170
Explanations to In-Class Exam for Lecture 3 172
Explanations to In-Class Exam for Lecture 4 174
Explanations to In-Class Exam for Lecture 5 176
Explanations to In-Class Exam for Lecture 6 178
Explanations to In-Class Exam for Lecture 7 179
Answers & Explanations to Questions in the Lectures 181
Answers to Questions in the Lectures 182
Explanations to Questions in Lecture 1 183
Explanations to Questions in Lecture 2 184
Explanations to Questions in Lecture 3 186
Explanations to Questions in Lecture 4 188
Explanations to Questions in Lecture 5 190
Explanations to Questions in Lecture 6 192
Explanations to Questions in Lecture 7 193
Index 197
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