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Chemistry
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1.1 An Introduction to Chemistry and the Scientific Method
1.1.1 An Introduction to Chemistry
1.1.2 The Scientific Method
1.2 Properties of Matter
1.2.1 States of Matter
1.2.2 A Word About Laboratory Safety
1.2.3 CIA Demonstration: Differences in Density Due to Temperature
1.2.4 Properties of Matter
1.3 Scientific Measurement
1.3.1 The Measurement of Matter
1.3.2 Precision and Accuracy
1.3.3 CIA Demonstration: Precision and Accuracy with Glassware
1.3.4 Significant Figures
1.3.5 Dimensional Analysis
1.4 Mathematics of Chemistry
1.4.1 Scientific (Exponential) Notation
1.4.2 Common Mathematical Functions
2.1 Early Atomic Theory
2.1.1 Early Discoveries and the Atom
2.1.2 Understanding Electrons
2.1.3 Understanding the Nucleus
2.2 Atomic Structure
2.2.1 Mass Spectrometry: Determining Atomic Masses
2.2.2 Examining Atomic Structure
2.2.3 CIA Demonstration: Flame Colors
2.3 The Periodic Table
2.3.1 Creating the Periodic Table
2.4 Chemical Nomenclature
2.4.1 Describing Chemical Formulas
2.4.2 Naming Chemical Compounds
2.4.3 Organic Nomenclature
3.1 Chemical Equations
3.1.1 An Introduction to Chemical Reactions and Equations
3.1.2 CIA Demonstration: Magnesium and Dry Ice
3.1.3 Balancing Chemical Equations
3.2 The Mole
3.2.1 The Mole and Avogadro's Number
3.2.2 Introducing Conversions of Masses, Moles, and Number of Particles
3.3 Solving Problems Involving Mass/Mole Relationships
3.3.1 Finding Empirical and Molecular Formulas
3.3.2 Stoichiometry and Chemical Equations
3.3.3 Finding Limiting Reagents
3.3.4 CIA Demonstration: Self-Inflating Hydrogen Balloons
3.3.5 Theoretical Yield and Percent Yield
3.3.6 A Problem Using the Combined Concepts of Stoichiometry
4.1 An Introduction to Solutions
4.1.1 Properties of Solutions
4.1.2 CIA Demonstration: The Electric Pickle
4.1.3 Concentrations of Solutions
4.1.4 Factors Determining Solubility
4.2 Reactions Involving Solutions
4.2.1 Precipitation Reactions
4.2.2 Acid-Base Reactions
4.2.3 Oxidation-Reduction Reactions
4.3 Stoichiometry Problems in Solutions
4.3.1 Acid-Base Titrations
4.3.2 Solving Titration Problems
4.3.3 Gravimetric Analysis
5.1 Gases and Gas Laws
5.1.1 Properties of Gases
5.1.2 Boyle's Law
5.1.3 Charles's Law
5.1.4 The Combined Gas Law
5.1.5 Avogadro's Law
5.1.6 CIA Demonstration: The Potato Cannon
5.2 The Ideal Gas Law and Kinetic-Molecular Theory of Gases
5.2.1 The Ideal Gas Law
5.2.2 Partial Pressure and Dalton's Law
5.2.3 Applications of the Gas Laws
5.2.4 The Kinetic-Molecular Theory of Gases
5.2.5 CIA Demonstration: The Ammonia Fountain
5.3 Molecular Motion of Gases
5.3.1 Molecular Speeds
5.3.2 Effusion and Diffusion
5.4 Behavior of Real Gases
5.4.1 Comparing Real and Ideal Gases
6.1 An Introduction to Energy
6.1.1 The Nature of Energy
6.1.2 Energy, Calories, and Nutrition
6.1.3 The First Law of Thermodynamics
6.1.4 Work
6.1.5 Heat
6.1.6 CIA Demonstration: Cool Fire
6.2 Enthalpy
6.2.1 Heats of Reaction: Enthalpy
6.2.2 CIA Demonstration: The Thermite Reaction
6.3 Calorimetry
6.3.1 Constant Pressure Calorimetry
6.3.2 Bomb Calorimetry (Constant Volume)
6.4 Hess's Law and Enthalpies of Formation
6.4.1 Hess's Law
6.4.2 Enthalpies of Formation
7.1 Electromagnetic Radiation and the Idea of Quantum
7.1.1 The Wave Nature of Light
7.1.2 Absorption and Emission
7.1.3 CIA Demonstration: Luminol
7.1.4 The Ultraviolet Catastrophe
7.1.5 The Photoelectric Effect
7.1.6 The Bohr Model
7.1.7 The Heisenberg Uncertainty Principle
7.2 Quantum Mechanics
7.2.1 The Wave Nature of Matter
7.2.2 Radial Solutions to the Schrödinger Equation
7.2.3 Angular Solutions to the Schrödinger Equation
7.3 Atomic Orbitals
7.3.1 Atomic Orbital Size
7.3.2 Atomic Orbital Shapes and Quantum Numbers
7.3.3 Atomic Orbital Energy
8.1 Electron Spin and the Pauli Exclusion Principle
8.1.1 Understanding Electron Spin
8.1.2 Electron Shielding
8.1.3 Electron Configurations through Neon
8.1.4 Electron Configurations beyond Neon
8.1.5 Periodic Relationships
8.2 Periodicity
8.2.1 Periods and Atomic Size
8.2.2 Ionization Energy
8.2.3 Electron Affinity
8.2.4 An Introduction to Electronegativity
8.3 Group Trends
8.3.1 Hydrogen, Alkali Metals and Alkaline Earth Metals
8.3.2 Transition Metals and Nonmetals
9.1 Valence Electrons and Chemical Bonding
9.1.1 Valence Electrons and Chemical Bonding
9.1.2 Ionic Bonds
9.1.3 CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds
9.2 Lewis Dot Structures
9.2.1 Lewis Dot Structures for Covalent Bonds
9.2.2 Predicting Lewis Dot Structures
9.3 Resonance Structures and Formal Charge
9.3.1 Resonance Structures
9.3.2 Formal Charge
9.3.3 Electronegativity, Formal Charge, and Resonance
9.4 Bond Properties
9.4.1 Bond Properties
9.4.2 Using Bond Dissociation Energies
10.1 Molecular Geometry and the VSEPR Theory
10.1.1 Valence-Shell Electron-Pair Repulsion Theory
10.1.2 Molecular Shapes for Steric Numbers 2-4
10.1.3 Molecular Shapes for Steric Numbers 5 & 6
10.1.4 Predicting Molecular Characteristics Using VSEPR Theory
10.2 Valence Bond Theory and Molecular Orbital Theory
10.2.1 Valence Bond Theory
10.2.2 An Introduction to Hybrid Orbitals
10.2.3 Pi Bonds
10.2.4 Molecular Orbital Theory
10.2.5 Applications of the Molecular Orbital Theory
10.2.6 Beyond Homonuclear Diatomics
10.2.7 CIA Demonstration: The Paramagnetism of Oxygen
11.1 Looking In-Depth at Redox Reactions
11.1.1 Oxidation Numbers
11.1.2 Balancing Redox Reactions by the Oxidation Number Method
11.1.3 Balancing Redox Reactions Using the Half-Reaction Method
11.1.4 The Activity Series of the Elements
11.1.5 CIA Demonstration: The Reaction between Al and Br2
12.1 Intermolecular Forces
12.1.1 An Introduction to Intermolecular Forces and States of Matter
12.1.2 Intermolecular Forces
12.2 Physical Properties of Liquids
12.2.1 Properties of Liquids
12.2.2 CIA Demonstration: Boiling Water at Reduced Pressure
12.2.3 Vapor Pressure and Boiling Point
12.2.4 Molecular Structure and Boiling Point
12.2.5 Phase Diagrams
12.2.6 CIA Demonstration: Boiling Water in a Paper Cup
12.3 Solid State: Structure and Bonding
12.3.1 Types of Solids
12.3.2 CIA Demonstration: The Conductivity of Molten Salts
12.3.3 Crystal Structure
12.3.4 Calculating Atomic Mass and Radius from a Unit Cell
12.3.5 Crystal Packing
12.4 Ceramics
12.4.1 Ceramics and Glass
12.4.2 CIA Demonstration: Superconductivity
13.1 Characterizing Solutions
13.1.1 Types of Solutions
13.1.2 Molarity and the Mole Fraction
13.1.3 Molality
13.1.4 Energy and the Solution Process
13.2 Effects of Temperature and Pressure on Solubility
13.2.1 Temperature Change and Solubility
13.2.2 Extractions
13.2.3 Pressure Change and Solubility
13.3 Colligative Properties
13.3.1 Vapor Pressure Lowering
13.3.2 Boiling Point Elevation and Freezing Point Depression
13.3.3 Boiling Point Elevation Problem
13.3.4 Osmosis
13.3.5 Colligative Properties of Ionic Solutions
13.4 Colloids
13.4.1 Colloid Formation and Flocculation
13.4.2 CIA Demonstration: The Tyndall Effect
14.1 Reaction Rates
14.1.1 An Introduction to Reaction Rates
14.1.2 Rate Laws: How the Reaction Rate Depends on Concentration
14.1.3 Determining the Form of a Rate Law
14.2 Orders of Reaction
14.2.1 First-Order Reactions
14.2.2 Second-Order Reactions
14.2.3 A Kinetics Problem
14.3 Temperature and Rates
14.3.1 The Collision Model
14.3.2 The Arrhenius Equation
14.3.3 Using the Arrhenius Equation
14.4 Reaction Mechanisms
14.4.1 Defining the Molecularity of a Reaction
14.4.2 Determining the Rate Laws of Elementary Reactions
14.4.3 Calculating the Rate Laws of Multistep Reactions
14.4.4 Steady State Kinetics
14.5 Catalysts
14.5.1 Catalysts and Types of Catalysts
14.5.2 A Word About Laboratory Safety
14.5.3 CIA Demonstration: Elephant Snot
14.5.4 CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate
14.5.5 CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone
15.1 Principles of Chemical Equilibrium
15.1.1 The Concept of Equilibrium
15.1.2 The Law of Mass Action and Types of Equilibrium
15.1.3 Converting Between Kc and Kp
15.2 Using Equilibrium Constants
15.2.1 Approaching Chemical Equilibrium
15.2.2 Predicting the Direction of a Reaction
15.2.3 Strategies for Solving Equilibrium Problems
15.2.4 Solving Problems Far from Equilibrium
15.2.5 An Equilibrium Problem Using the Quadratic Equation
15.3 Shifting Chemical Equilibrium
15.3.1 Le Châtelier's Principle
15.3.2 The Effect of Changing Amounts on Equilibrium
15.3.3 The Effect of Pressure and Volume on Equilibrium
15.3.4 The Effects of Temperature and Catalysts on Equilibrium
15.3.5 CIA Demonstration: NO2/N2O4
15.3.6 CIA Demonstration: Shifting the Equilibrium of FeSCN2+
16.1 Acid-Base Concepts
16.1.1 Arrhenius/Brønsted-Lowry Definitions of Acids and Bases
16.1.2 Hydronium, Hydroxide, and the pH Scale
16.2 Acid and Base Strengths
16.2.1 Strong Acids and Bases
16.2.2 CIA Demonstration: Natural Acid-Base Indicators
16.2.3 Weak Acids
16.2.4 Weak Bases
16.2.5 Lewis Acids and Bases
16.2.6 Trends in Acid and Base Strengths
16.3 Polyprotic Acids
16.3.1 Examining Polyprotic Acids
16.4 Acid-Base Properties of Salts
16.4.1 Acid-Base Properties of Salt Solutions
17.1 Reactions of Acids and Bases
17.1.1 Strong Acid-Strong Base and Weak Acid-Strong Base Reactions
17.1.2 Strong Acid-Weak Base and Weak Acid-Weak Base Reactions
17.1.3 The Common Ion Effect
17.2 Buffers
17.2.1 An Introduction to Buffers
17.2.2 CIA Demonstration: Buffers in Action
17.2.3 Acidic Buffers
17.2.4 Basic Buffers
17.2.5 The Henderson-Hasselbalch Equation
17.3 Acid-Base Titration
17.3.1 Strong Acid-Strong Base Titration
17.3.2 CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration
17.3.3 Weak Acid-Strong Base Titration
17.3.4 Polyprotic Acid-Strong Base Titration
17.3.5 Weak Base-Strong Acid Titration
17.3.6 Acid-Base Indicators
17.4 Solubility Equilibria
17.4.1 The Solubility Product Constant
17.4.2 CIA Demonstration: Silver Chloride and Ammonia
17.4.3 Solubility and the Common Ion Effect
17.4.4 Fractional Precipitation
17.4.5 The Effects of pH on Solubility
17.5 Complex Ion Equilibria
17.5.1 The Formation of Complex Ions
17.5.2 Amphoteric Metal Hydroxides
18.1 Acid Strength in Organic Molecules
18.1.1 An Introduction to Reactivity
18.1.2 Bond Strengths
18.1.3 Inductive Effects
18.1.4 Hybridization Effects
18.1.5 Resonance Effects
18.1.6 Solvent Effects: Acid Dissociation versus Proton Affinity
18.2 Base Strength in Organic Molecules
18.2.1 A Review of Relationship between Acids and Conjugate Bases
18.2.2 Strengths of Organic Bases
18.2.3 Solvent Effects on Organic Base Strength
18.3 Lewis Acid and Base Reactions
18.3.1 Lewis Acids and the Formation of Acid-Base Adducts
18.3.2 Oxides as Lewis Acids
18.4 Introduction to Electrophiles and Nucleophiles
18.4.1 Nucleophilic Substitution at sp3 Carbon
18.4.2 Nucleophilic Substitution at sp2 Carbon
18.4.3 Elimination Reactions
18.4.4 CIA Demonstration: Slime
19.1 An Introduction to Thermodynamics
19.1.1 Spontaneous Processes
19.2 Entropy
19.2.1 Entropy and the Second Law of Thermodynamics
19.2.2 Entropy and Temperature
19.3 Gibbs Free Energy and Free Energy Change
19.3.1 Gibbs Free Energy
19.3.2 Standard Free Energy Changes of Formation
19.4 Using Free Energy
19.4.1 Enthalpy and Entropy Contributions to K
19.4.2 The Temperature Dependence of K
19.4.3 Free Energy Away from Equilibrium
20.1 Principles of Electrochemistry
20.1.1 Reviewing Oxidation-Reduction Reactions
20.2 Galvanic Cells
20.2.1 Electrochemical Cells
20.2.2 Electromotive Force
20.2.3 Standard Reduction Potentials
20.2.4 Using Standard Reduction Potentials
20.2.5 The Nernst Equation
20.2.6 Electrochemical Determinants of Equilibria
20.3 Batteries
20.3.1 Batteries
20.3.2 CIA Demonstration: The Fruit-Powered Clock
20.4 Corrosion
20.4.1 Corrosion and the Prevention of Corrosion
20.5 Electrolysis and Electrolytic Cells
20.5.1 Electrolytic Cells
20.5.2 The Stoichiometry of Electrolysis
21.1 Radioactivity
21.1.1 The Nature of Radioactivity
21.1.2 The Stability of Atomic Nuclei
21.1.3 Binding Energy
21.2 Rates of Disintegration
21.2.1 Rates of Disintegration Reactions
21.2.2 Radiochemical Dating
21.3 Nuclear Fission and Fusion
21.3.1 Nuclear Fission
21.3.2 Nuclear Fusion
21.3.3 Applications of Nuclear Chemistry
22.1 An Introduction to Metals
22.1.1 Metallurgical Processes
22.1.2 Band Theory of Conductivity
22.1.3 Intrinsic Semiconductors
22.1.4 Doped Semiconductors
22.2 Physical and Chemical Processes of Metals
22.2.1 The Alkali Metals
22.2.2 The Alkaline Earth Metals
22.2.3 Aluminum
22.2.4 CIA Demonstration: The Reaction between Al and Br2
23.1 Examining Transition Metals
23.1.1 Properties of Transition Metals
23.1.2 CIA Demonstration: Copper One-Pot Reactions
23.2 Coordination Compounds
23.2.1 Complexes and Ligands
23.2.2 Naming Coordination Compounds
23.2.3 Structures of Coordination Compounds and Isomers
23.3 Bonding in Coordination Compounds
23.3.1 Color and Transition Metals
23.3.2 Crystal Field Theory
23.3.3 Ligand Field Theory
23.3.4 Magnetic Properties and Spin
24.1 An Introduction to Nonmetals and Hydrogen
24.1.1 General Properties of Nonmetals
24.1.2 Hydrogen
24.2 Group 14: Carbon and Silicon
24.2.1 General Properties of Carbon
24.2.2 Silicon
24.3 Group 15: Nitrogen and Phosphorus
24.3.1 Nitrogen
24.3.2 Phosphorus
24.4 Group 16: Oxygen and Sulfur
24.4.1 Oxygen
24.4.2 CIA Demonstration: Creating Acid Rain
24.4.3 Sulfur
24.5 Group 17: The Halogens
24.5.1 Halogens
24.5.2 Aqueous Halogen Compounds
24.6 Group 18: The Noble Gases
24.6.1 Properties of Noble Gases
25.1 Hydrocarbons
25.1.1 Alkanes
25.1.2 Alkenes and Alkynes
25.1.3 Isomers
25.1.4 Aromatic Hydrocarbons
25.2 The Functional Groups
25.2.1 Alcohols, Ethers, and Amines
25.2.2 Carbonyl-Containing Functional Groups
25.3 Organic Polymers
25.3.1 Organic Polymers
25.3.2 CIA Demonstration: The Synthesis of Nylon
26.1 Biological Molecules
26.1.1 Proteins
26.1.2 Nucleic Acids
26.1.3 Carbohydrates
26.1.4 Lipids
27.1 Laboratory Techniques
27.1.1 CIA Demonstration: Laboratory Safety
27.1.2 CIA Demonstration: Chromatography
27.1.3 CIA Demonstration: Distillation
27.1.4 CIA Demonstration: Pipetting
27.1.5 CIA Demonstration: Dilutions
27.1.6 CIA Demonstration: Titrations
27.1.7 CIA Demonstration: Extractions
27.1.8 CIA Demonstration: Filtrations
27.1.9 CIA Demonstration: Weighing on an Analytical Balance
27.1.10 CIA Demonstration: Recrystallization
Dean Harman
University of Virginia
Dean Harman is a professor of chemistry at the University of Virginia, where he has been honored with several teaching awards. He heads the Harman Research Group, which specializes in the novel organic transformations made possible by electron-rich metal centers such as Os(II), RE(I), and W(0). Prof. Harman holds a Ph.D. from Stanford University.
Gordon Yee
Virginia Tech
Gordon Yee is an associate professor of chemistry at Virginia Tech in Blacksburg, VA. He received his Ph.D. from Stanford University and completed postdoctoral work at DuPont. A widely published author, Professor Yee studies molecule-based magnetism.
Tarek Sammakia
University of Colorado at Boulder
Tarek Sammakia is a Professor of Chemistry at the University of Colorado at Boulder where he teaches organic chemistry to undergraduate and graduate students. He received his Ph.D. from Yale University and carried out postdoctoral research at Harvard University. He has received several national awards for his work in synthetic and mechanistic organic chemistry.
TestPrep
60-day access$17.95
A fast way to prepare for a final exam!
Thinkwell has identified the topics that are most commonly found on a final exam. Take a quick test to find out which topics you need to work on and watch only those videos. If you have a limited time to prepare for a final, this is for you!
Online subscription is not required. Workbooks or CDs are not available.
Thinkwell's Chemistry TestPrep with Dean Harman, Gordon Yee and Tarek Sammakia helps you get ready for your finals with no wasted time! Thinkwell's Chemistry TestPrep helps you get right to work on the exact topics you need help with. Focus only on what you need and be ready for your exam in less than 5 hours!
Diagnostic Tests
Time is tight during exam season, so we'll help you get going by offering a Pre-study Prep Test that tells you exactly which topics you need to review. Once you've studied the recommended topics, there's a Practice Final that checks to make sure you're up to speed and ready to ace your final. There's no wasted time with Thinkwell's Chemistry TestPrep!
Comprehensive Video Tutorials
We've built Thinkwell's Chemistry TestPrep around carefully selected multimedia tutorials that provide a quick and concise review of Chemistry. Thinkwell's tutorials offer a more engaging, more effective way for you to learn. Watch one Thinkwell video lecture and you'll understand why Thinkwell works better.
Interactive Exercises with Feedback
Each of Thinkwell's Chemistry TestPrep topics includes exercises with fully worked-out solutions and explanations. Practice and review as often as you like and be ready for your exam!
Review Notes and More
We include illustrated review notes, a glossary, transcripts of the video lectures, and links to relevant websites. These optional materials can be viewed online, and the notes and transcripts can be printed and kept for reference.
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Finals season is a breeze with Thinkwell's Chemistry TestPrep? It's a sure-fire way to make the grade!
1.1 TestPrep Topics
1.1.1 Balancing Chemical Equations
1.1.2 Introducing Conversions of Masses, Moles, and Number of Particles
1.1.3 Finding Empirical and Molecular Formulas
1.1.4 Stoichiometry and Chemical Equations
1.1.5 Finding Limiting Reagents
1.1.6 Theoretical Yield and Percent Yield
1.1.7 Concentrations of Solutions
1.1.8 Solving Titration Problems
1.1.9 Gravimetric Analysis
1.1.10 The Combined Gas Law
1.1.11 The Ideal Gas Law
1.1.12 Partial Pressure and Dalton's Law
1.1.13 Applications of the Gas Laws
1.1.14 Effusion and Diffusion
1.1.15 The First Law of Thermodynamics
1.1.16 Work
1.1.17 Heat
1.1.18 Heats of Reaction: Enthalpy
1.1.19 Constant Pressure Calorimetry
1.1.20 Hess's Law
1.1.21 Enthalpies of Formation
1.1.22 Valence Electrons and Chemical Bonding
1.1.23 Oxidation Numbers
1.1.24 Balancing Redox Reactions Using the Half-Reaction Method
1.1.25 Intermolecular Forces
1.1.26 Boiling Point Elevation and Freezing Point Depression
1.1.27 Converting Between Kc and Kp
1.1.28 Predicting the Direction of a Reaction
1.1.29 Strategies for Solving Equilibrium Problems
1.1.30 Solving Problems Far from Equilibrium
1.1.31 An Equilibrium Problem Using the Quadratic Equation
1.1.32 Le Châtelier's Principle
1.1.33 The Effect of Changing Amounts on Equilibrium
1.1.34 The Effect of Pressure and Volume on Equilibrium
1.1.35 The Effects of Temperature and Catalysts on Equilibrium
1.1.36 Strong Acid-Strong Base and Weak Acid-Strong Base Reactions
1.1.37 Strong Acid-Weak Base and Weak Acid-Weak Base Reactions
1.1.38 An Introduction to Buffers
1.1.39 Acidic Buffers
1.1.40 Basic Buffers
1.1.41 The Henderson-Hasselbalch Equation
1.1.42 Strong Acid-Strong Base Titration
1.1.43 Weak Acid-Strong Base Titration
1.1.44 Polyprotic Acid-Strong Base Titration
1.1.45 Weak Base-Strong Acid Titration
1.1.46 Acid-Base Indicators
1.1.47 The Solubility Product Constant
1.1.48 Solubility and the Common Ion Effect
1.1.49 Fractional Precipitation
1.1.50 The Effects of pH on Solubility
Dean Harman
University of Virginia
Dean Harman is a professor of chemistry at the University of Virginia, where he has been honored with several teaching awards. He heads the Harman Research Group, which specializes in the novel organic transformations made possible by electron-rich metal centers such as Os(II), RE(I), and W(0). Prof. Harman holds a Ph.D. from Stanford University.
Gordon Yee
Virginia Tech
Gordon Yee is an associate professor of chemistry at Virginia Tech in Blacksburg, VA. He received his Ph.D. from Stanford University and completed postdoctoral work at DuPont. A widely published author, Professor Yee studies molecule-based magnetism.
Tarek Sammakia
University of Colorado at Boulder
Tarek Sammakia is a Professor of Chemistry at the University of Colorado at Boulder where he teaches organic chemistry to undergraduate and graduate students. He received his Ph.D. from Yale University and carried out postdoctoral research at Harvard University. He has received several national awards for his work in synthetic and mechanistic organic chemistry.
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