Lýsing:
The Atoms First approach provides a consistent and logical method for teaching general chemistry. This approach starts with the fundamental building block of matter, the atom, and uses it as the stepping stone to understanding more complex chemistry topics. Once mastery of the nature of atoms and electrons is achieved, the formation and properties of compounds are developed. Only after the study of matter and the atom will students have sufficient background to fully engage in topics such as stoichiometry, kinetics, equilibrium, and thermodynamics.
Thus, the Atoms First approach empowers instructors to present the most complete and compelling story of general chemistry. Far from a simple re-ordering of topics, this is a book that will truly meet the needs of the growing atoms-first market. The third edition continues to build on the innovative success of the first and second editions. Changes to this edition include specific refinements intended to augment the student-centered pedagogical features that continue to make this book effective and popular both with professors, and with their students.
Annað
- Höfundar: Julia Burdge, Jason Overby
- Útgáfa:4
- Útgáfudagur: 2020-01-07
- Hægt að prenta út 2 bls.
- Hægt að afrita 2 bls.
- Format:ePub
- ISBN 13: 9781260590371
- Print ISBN: 9781260571349
- ISBN 10: 1260590372
Efnisyfirlit
- Cover Page
- Useful Table
- Periodic Table
- List of Element
- Title Page
- Copyright
- Dedication
- About the Author
- Contents in Brief
- Contents
- List of Applications
- Preface
- Connect
- Instructor and Student Resources
- Acknowledgments
- Halftitle Page
- 1 CHEMISTRY: THE SCIENCE OF CHANGE
- 1.1 The Study of Chemistry
- Chemistry You May Already Know
- The Scientific Method
- Thinking Outside the Box: Tips for Success in Chemistry Class
- 1.2 Scientific Measurement
- SI Base Units
- Mass
- Temperature
- Derived Units: Volume and Density
- Environmental Aspects: Global Climate Change
- 1.3 Uncertainty in Measurement
- Significant Figures
- Calculations with Measured Numbers
- Accuracy and Precision
- 1.4 Using Units and Solving Problems
- Conversion Factors
- Dimensional Analysis—Tracking Units
- 1.5 Classification of Matter
- States of Matter
- Mixtures
- Thinking Outside the Box: How Many States of Matter Are There?
- 1.6 The Properties of Matter
- Physical Properties
- Chemical Properties
- Extensive and Intensive Properties
- 2 ATOMS AND THE PERIODIC TABLE
- 2.1 Atoms First
- 2.2 Subatomic Particles and Atomic Structure
- Discovery of the Electron
- Radioactivity
- The Proton and the Nuclear Model of the Atom
- The Neutron
- 2.3 Atomic Number, Mass Number, and Isotopes
- 2.4 Nuclear Stability
- Patterns of Nuclear Stability
- 2.5 Average Atomic Mass
- Thinking Outside the Box: Measuring Atomic Mass
- 2.6 The Periodic Table
- Environmental Aspects: Isolated Atoms and Stratospheric Ozone Depletion
- 2.7 The Mole and Molar Mass
- The Mole
- Molar Mass
- Interconverting Mass, Moles, and Numbers of Atoms
- 3 QUANTUM THEORY AND THE ELECTRONIC STRUCTURE OF ATOMS
- 3.1 Energy and Energy Changes
- Forms of Energy
- Units of Energy
- 3.2 The Nature of Light
- Properties of Waves
- The Electromagnetic Spectrum
- The Double-Slit Experiment
- Environmental Aspects: Solar Energy
- 3.3 Quantum Theory
- Quantization of Energy
- Photons and the Photoelectric Effect
- Thinking Outside the Box: Everyday Occurrences of the Photoelectric Effect
- 3.4 Bohr’s Theory of the Hydrogen Atom
- Atomic Line Spectra
- The Line Spectrum of Hydrogen
- 3.5 Wave Properties of Matter
- The de Broglie Hypothesis
- Diffraction of Electrons
- 3.6 Quantum Mechanics
- The Uncertainty Principle
- The Schrödinger Equation
- The Quantum Mechanical Description of the Hydrogen Atom
- 3.7 Quantum Numbers
- Principal Quantum Number (n)
- Angular Momentum Quantum Number (ℓ)
- Magnetic Quantum Number (mℓ)
- Electron Spin Quantum Number (ms)
- 3.8 Atomic Orbitals
- s Orbitals
- p Orbitals
- d Orbitals and Other Higher-Energy Orbitals
- Energies of Orbitals
- 4 PERIODIC TRENDS OF THE ELEMENTS
- 4.1 Development of the Periodic Table
- 4.2 Electron Configurations
- Energies of Atomic Orbitals in Many-Electron Systems
- The Pauli Exclusion Principle
- The Aufbau Principle
- Hund’s Rule
- General Rules for Writing Electron Configurations
- Thinking Outside the Box: How Do We Know that ns Orbitals Fill Before (n – 1) d Orbitals?
- 4.3 Electron Configurations and the Modern Periodic Table
- 4.4 Effective Nuclear Charge
- 4.5 Periodic Trends in Properties of Elements
- Atomic Radius
- Ionization Energy
- Electron Affinity
- Metallic Character
- 4.6 Electron Configuration of Ions
- Ions of Main Group Elements
- Ions of d-Block Elements
- 4.7 Ionic Radius
- Comparing Ionic Radius with Atomic Radius
- Isoelectronic Series
- Environmental Aspects: Lead in the Water in Flint, Michigan
- Thinking Outside the Box: Mistaking Strontium for Calcium
- 5 IONIC AND COVALENT COMPOUNDS
- 5.1 Compounds
- 5.2 Lewis Dot Symbols
- 5.3 Ionic Compounds and Bonding
- 5.4 Naming Ions and Ionic Compounds
- Formulas of Ionic Compounds
- Naming Ionic Compounds
- 5.5 Covalent Bonding and Molecules
- Molecules
- Molecular Formulas
- Empirical Formulas
- 5.6 Naming Molecular Compounds
- Specifying Numbers of Atoms
- Compounds Containing Hydrogen
- Organic Compounds
- Environmental Aspects: CFC Nomenclature
- Thinking Outside the Box: Functional Groups
- 5.7 Covalent Bonding in Ionic Species
- Polyatomic Ions
- Oxoacids
- Hydrates
- Familiar Inorganic Compounds
- 5.8 Molecular and Formula Masses
- 5.9 Percent Composition of Compounds
- 5.10 Molar Mass
- Interconverting Mass, Moles, and Numbers of Particles
- Determination of Empirical Formula and Molecular Formula from Percent Composition
- 6 REPRESENTING MOLECULES
- 6.1 The Octet Rule
- Lewis Structures
- Multiple Bonds
- 6.2 Electronegativity and Polarity
- Electronegativity
- Dipole Moment, Partial Charges, and Percent Ionic Character
- 6.3 Drawing Lewis Structures
- 6.4 Lewis Structures and Formal Charge
- 6.5 Resonance
- 6.6 Exceptions to the Octet Rule
- Incomplete Octets
- Odd Numbers of Electrons
- Thinking Outside the Box: Species with Unpaired Electrons
- Environmental Aspects: Tropospheric Ozone
- Expanded Octets
- 7 MOLECULAR GEOMETRY, INTERMOLECULAR FORCES, AND BONDING THEORIES
- 7.1 Molecular Geometry
- The VSEPR Model
- Electron-Domain Geometry and Molecular Geometry
- Deviation from Ideal Bond Angles
- Geometry of Molecules with More Than One Central Atom
- 7.2 Molecular Geometry and Polarity
- Environmental Aspects: Polarity and The Greenhouse Effect
- 7.3 Intermolecular Forces
- Dipole-Dipole Interactions
- Hydrogen Bonding
- Dispersion Forces
- Ion-Dipole Interactions
- 7.4 Valence Bond Theory
- 7.5 Hybridization of Atomic Orbitals
- Hybridization of s and p Orbitals
- Hybridization of s, p, and d Orbitals
- 7.6 Hybridization in Molecules Containing Multiple Bonds
- 7.7 Molecular Orbital Theory
- Bonding and Antibonding Molecular Orbitals
- σ Molecular Orbitals
- Thinking Outside the Box: Phases
- Bond Order
- π Molecular Orbitals
- Molecular Orbital Diagrams
- Thinking Outside the Box: Molecular Orbitals in Heteronuclear Diatomic Species
- 7.8 Bonding Theories and Descriptions of Molecules with Delocalized Bonding
- 8 CHEMICAL REACTIONS
- 8.1 Chemical Equations
- Interpreting and Writing Chemical Equations
- Balancing Chemical Equations
- Patterns of Chemical Reactivity
- 8.2 Combustion Analysis
- Determination of Empirical Formula
- 8.3 Calculations with Balanced Chemical Equations
- Moles of Reactants and Products
- Mass of Reactants and Products
- 8.4 Limiting Reactants
- Determining the Limiting Reactant
- Reaction Yield
- Atom Economy
- Environmental Aspects: Green Chemistry Metrics
- 8.5 Periodic Trends in Reactivity of the Main Group Elements
- General Trends in Reactivity
- Hydrogen (1s1)
- Reactions of the Active Metals
- Reactions of Other Main Group Elements
- Comparison of Group 1 and Group 11 Elements
- 9 CHEMICAL REACTIONS IN AQUEOUS SOLUTIONS
- 9.1 General Properties of Aqueous Solutions
- Electrolytes and Nonelectrolytes
- Strong Electrolytes and Weak Electrolytes
- 9.2 Precipitation Reactions
- Solubility Guidelines for Ionic Compounds in Water
- Molecular Equations
- Ionic Equations
- Net Ionic Equations
- Environmental Aspects: Softening Hard Water
- 9.3 Acid-Base Reactions
- Strong Acids and Bases
- Brønsted Acids and Bases
- Acid-Base Neutralization
- 9.4 Oxidation-Reduction Reactions
- Oxidation Numbers
- Oxidation of Metals in Aqueous Solutions
- Balancing Simple Redox Equations
- Other Types of Redox Reactions
- 9.5 Concentration of Solutions
- Molarity
- Dilution
- Serial Dilution
- Thinking Outside the Box: Visible Spectrophotometry
- The pH Scale
- Solution Stoichiometry
- 9.6 Aqueous Reactions and Chemical Analysis
- Gravimetric Analysis
- Acid-Base Titrations
- 10 ENERGY CHANGES IN CHEMICAL REACTIONS
- 10.1 Energy and Energy Changes
- 10.2 Introduction to Thermodynamics
- States and State Functions
- The First Law of Thermodynamics
- Work and Heat
- 10.3 Enthalpy
- Reactions Carried Out at Constant Volume or at Constant Pressure
- Enthalpy and Enthalpy Changes
- Thermochemical Equations
- 10.4 Calorimetry
- Specific Heat and Heat Capacity
- Constant-Pressure Calorimetry
- Constant-Volume Calorimetry
- Thinking Outside the Box: Heat Capacity of Calorimeters
- Environmental Aspects: Energy Density and Specific Energy
- 10.5 Hess’s Law
- 10.6 Standard Enthalpies of Formation
- 10.7 Bond Enthalpy and the Stability of Covalent Molecules
- 10.8 Lattice Energy and the Stability of Ionic Solids
- The Born-Haber Cycle
- Comparison of Ionic and Covalent Compounds
- 11 GASES
- 11.1 Properties of Gases
- 11.2 The Kinetic Molecular Theory of Gases
- Molecular Speed
- Diffusion and Effusion
- 11.3 Gas Pressure
- Definition and Units of Pressure
- Calculation of Pressure
- Measurement of Pressure
- 11.4 The Gas Laws
- Boyle’s Law: The Pressure-Volume Relationship
- Charles’s and Gay-Lussac’s Law: The Temperature-Volume Relationship
- Avogadro’s Law: The Amount-Volume Relationship
- The Gas Laws and Kinetic Molecular Theory
- The Combined Gas Law: The Pressure-Temperature-Amount-Volume Relationship
- 11.5 The Ideal Gas Equation
- Applications of the Ideal Gas Equation
- Environmental Aspects: Lead in Gasoline
- 11.6 Real Gases
- Factors That Cause Deviation from Ideal Behavior
- The van der Waals Equation
- van der Waals Constants
- 11.7 Gas Mixtures
- Dalton’s Law of Partial Pressures
- Mole Fractions
- Thinking Outside the Box: Decompression Injury
- 11.8 Reactions with Gaseous Reactants and Products
- Calculating the Required Volume of a Gaseous Reactant
- Determining the Amount of Reactant Consumed Using Change in Pressure
- Using Partial Pressures to Solve Problems
- 12 LIQUIDS AND SOLIDS
- 12.1 The Condensed Phases
- 12.2 Properties of Liquids
- Surface Tension
- Viscosity
- Vapor Pressure of Liquids
- Boiling Point
- 12.3 Properties of Solids
- Melting Point
- Vapor Pressure of Solids
- Amorphous Solids
- Crystalline Solids
- Thinking Outside the Box: X-ray Diffraction
- 12.4 Types of Crystalline Solids
- Ionic Crystals
- Covalent Crystals
- Molecular Crystals
- Metallic Crystals
- 12.5 Phase Changes
- Liquid-Vapor
- Solid-Liquid
- Solid-Vapor
- Environmental Aspects: Water Vapor in the Atmosphere
- 12.6 Phase Diagrams
- 13 PHYSICAL PROPERTIES OF SOLUTIONS
- 13.1 Types of Solutions
- 13.2 A Molecular View of the Solution Process
- The Importance of Intermolecular Forces
- Energy and Entropy in Solution Formation
- 13.3 Concentration Units
- Molality
- Percent by Mass
- Comparison of Concentration Units
- 13.4 Factors That Affect Solubility
- Temperature
- Pressure
- 13.5 Colligative Properties
- Vapor-Pressure Lowering
- Boiling-Point Elevation
- Freezing-Point Depression
- Osmotic Pressure
- Electrolyte Solutions
- Thinking Outside the Box: Intravenous Fluids
- Thinking Outside the Box: Fluoride Poisoning
- 13.6 Calculations Using Colligative Properties
- 13.7 Colloids
- Environmental Aspects: EPS Foam Bans
- 14 CHEMICAL KINETICS
- 14.1 Reaction Rates
- 14.2 Collision Theory of Chemical Reactions
- 14.3 Measuring Reaction Progress and Expressing Reaction Rate
- Average Reaction Rate
- Instantaneous Rate
- Stoichiometry and Reaction Rate
- 14.4 Dependence of Reaction Rate on Reactant Concentration
- The Rate Law
- Experimental Determination of the Rate Law
- 14.5 Dependence of Reactant Concentration on Time
- First-Order Reactions
- Second-Order Reactions
- 14.6 Dependence of Reaction Rate on Temperature
- The Arrhenius Equation
- Thinking Outside the Box: Surface Area
- 14.7 Reaction Mechanisms
- Elementary Reactions
- Rate-Determining Step
- Mechanisms with a Fast First Step
- Experimental Support for Reaction Mechanisms
- 14.8 Catalysis
- Heterogeneous Catalysis
- Homogeneous Catalysis
- Enzymes: Biological Catalysts
- Environmental Aspects: Catalytic Converters
- 15 ENTROPY AND GIBBS ENERGY
- 15.1 Spontaneous Processes
- 15.2 Entropy
- A Qualitative Description of Entropy
- A Quantitative Definition of Entropy
- 15.3 Entropy Changes in a System
- Calculating ΔSsys
- Standard Entropy, S°
- Qualitatively Predicting the Sign of
- 15.4 Entropy Changes in the Universe
- Calculating ΔSsurr
- The Second Law of Thermodynamics
- Thinking Outside the Box: Thermodynamics and Living Systems
- Environmental Aspects: Thermodynamic Limits on Energy Conversion
- The Third Law of Thermodynamics
- 15.5 Predicting Spontaneity
- Gibbs Energy Change, ΔG
- Standard Gibbs Energy Changes, ΔG° 709
- Using ΔG and ΔG° to Solve Problems
- 15.6 Thermodynamics in Living Systems
- 16 CHEMICAL EQUILIBRIUM
- 16.1 The Concept of Equilibrium
- 16.2 The Equilibrium Constant
- Calculating Equilibrium Constants
- Magnitude of the Equilibrium Constant
- 16.3 Equilibrium Expressions
- Heterogeneous Equilibria
- Manipulating Equilibrium Expressions
- Gaseous Equilibria
- 16.4 Chemical Equilibrium and Gibbs Energy
- Using Q and K to Predict the Direction of Reaction
- Relationship Between ΔG and ΔG° 743
- Relationship Between ΔG° and K
- 16.5 Calculating Equilibrium Concentrations
- 16.6 Le Châtelier’s Principle: Factors That Affect Equilibrium
- Addition or Removal of a Substance
- Changes in Volume and Pressure
- Changes in Temperature
- Catalysis
- Environmental Aspects: Bioaccumulation of Toxins
- Thinking Outside the Box: Biological Equilibria
- 17 ACIDS, BASES, AND SALTS
- 17.1 Brønsted Acids and Bases
- 17.2 Molecular Structure and Acid Strength
- Hydrohalic Acids
- Oxoacids
- Carboxylic Acids
- Thinking Outside the Box: Substituent Electronegativity and Acid Strength
- 17.3 The Acid-Base Properties of Water
- 17.4 The pH and pOH Scales
- 17.5 Strong Acids and Bases
- Strong Acids
- Strong Bases
- 17.6 Weak Acids and Acid Ionization Constants
- The Ionization Constant, Ka
- Calculating pH from Ka
- Percent Ionization
- Environmental Aspects: Acid Rain
- Using pH to Determine Ka
- 17.7 Weak Bases and Base Ionization Constants
- The Ionization Constant, Kb
- Calculating pH from Kb
- Using pH to Determine Kb
- 17.8 Conjugate Acid-Base Pairs
- The Strength of a Conjugate Acid or Base
- The Relationship Between Ka and Kb of a Conjugate Acid-Base Pair
- 17.9 Diprotic and Polyprotic Acids
- 17.10 Acid-Base Properties of Salt Solutions
- Basic Salt Solutions
- Acidic Salt Solutions
- Neutral Salt Solutions
- Salts in Which Both the Cation and the Anion Hydrolyze
- 17.11 Acid-Base Properties of Oxides and Hydroxides
- Oxides of Metals and Nonmetals
- Basic and Amphoteric Hydroxides
- 17.12 Lewis Acids and Bases
- 18 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
- 18.1 The Common Ion Effect
- 18.2 Buffer Solutions
- Calculating the pH of a Buffer
- Preparing a Buffer Solution with a Specific pH
- Environmental Aspects: Ocean Acidification
- 18.3 Acid-Base Titrations
- Strong Acid–Strong Base Titrations
- Weak Acid–Strong Base Titrations
- Strong Acid–Weak Base Titrations
- Acid-Base Indicators
- 18.4 Solubility Equilibria
- Solubility Product Expression and Ksp
- Calculations Involving Ksp and Solubility
- Predicting Precipitation Reactions
- 18.5 Factors Affecting Solubility
- The Common Ion Effect
- pH
- Complex Ion Formation
- Thinking Outside the Box: Equilibrium and Tooth Decay
- 18.6 Separation of Ions Using Differences in Solubility
- Fractional Precipitation
- Qualitative Analysis of Metal Ions in Solution
- 19 ELECTROCHEMISTRY
- 19.1 Balancing Redox Reactions
- 19.2 Galvanic Cells
- 19.3 Standard Reduction Potentials
- 19.4 Spontaneity of Redox Reactions Under Standard State Conditions
- Thinking Outside the Box: Amalgam Fillings and Dental Pain
- 19.5 Spontaneity of Redox Reactions Under Conditions Other Than Standard State
- The Nernst Equation
- Concentration Cells
- 19.6 Batteries
- Dry Cells and Alkaline Batteries
- Lead Storage Batteries
- Lithium-Ion Batteries
- Fuel Cells
- 19.7 Electrolysis
- Electrolysis of Molten Sodium Chloride
- Electrolysis of Water
- Environmental Aspects: Artificial Leaves as a Renewable Energy Source
- Electrolysis of an Aqueous Sodium Chloride Solution
- Quantitative Applications of Electrolysis
- 19.8 Corrosion
- 20 NUCLEAR CHEMISTRY
- 20.1 Nuclei and Nuclear Reactions
- 20.2 Nuclear Stability
- Types of Nuclear Decay
- Nuclear Binding Energy
- 20.3 Natural Radioactivity
- Kinetics of Radioactive Decay
- Dating Based on Radioactive Decay
- 20.4 Nuclear Transmutation
- 20.5 Nuclear Fission
- Environmental Aspects: Nuclear Power, Waste, and Recycling
- 20.6 Nuclear Fusion
- 20.7 Uses of Isotopes
- Chemical Analysis
- Thinking Outside the Box: Nuclear Medicine
- Isotopes in Medicine
- 20.8 Biological Effects of Radiation
- 21 Environmental Chemistry
- 21.1 Earth’s Atmosphere
- 21.2 Phenomena in the Outer Layers of the Atmosphere
- Aurora Borealis and Aurora Australis
- The Mystery Glow of Space Shuttles
- 21.3 Depletion of Ozone in the Stratosphere
- Polar Ozone Holes
- 21.4 Volcanoes
- 21.5 The Greenhouse Effect
- 21.6 Acid Rain
- 21.7 Photochemical Smog
- 21.8 Indoor Pollution
- The Risk from Radon
- Carbon Dioxide and Carbon Monoxide
- Formaldehyde
- 22 COORDINATION CHEMISTRY
- 22.1 Coordination Compounds
- Properties of Transition Metals
- Ligands
- Nomenclature of Coordination Compounds
- Thinking Outside the Box: Chelation Therapy
- 22.2 Structure of Coordination Compounds
- 22.3 Bonding in Coordination Compounds: Crystal Field Theory
- Crystal Field Splitting in Octahedral Complexes
- Color
- Magnetic Properties
- Tetrahedral and Square-Planar Complexes
- 22.4 Reactions of Coordination Compounds
- 22.5 Applications of Coordination Compounds
- 23 ORGANIC CHEMISTRY
- 23.1 Why Carbon Is Different
- 23.2 Classes of Organic Compounds
- Basic Nomenclature
- Molecules with Multiple Substituents
- Molecules with Specific Functional Groups
- 23.3 Representing Organic Molecules
- Condensed Structural Formulas
- Kekulé Structures
- Bond-Line Structures
- Resonance
- 23.4 Isomerism
- Constitutional Isomerism
- Stereoisomerism
- Thinking Outside the Box: Thalidomide Analogues
- 23.5 Organic Reactions
- Addition Reactions
- Substitution Reactions
- Other Types of Organic Reactions
- 23.6 Organic Polymers
- Addition Polymers
- Condensation Polymers
- Biological Polymers
- 24 MODERN MATERIALS
- 24.1 Polymers
- Addition Polymers
- Condensation Polymers
- Thinking Outside the Box: Electrically Conducting Polymers
- 24.2 Ceramics and Composite Materials
- Ceramics
- Composite Materials
- 24.3 Liquid Crystals
- 24.4 Biomedical Materials
- Dental Implants
- Soft Tissue Materials
- Artificial Joints
- 24.5 Nanotechnology
- Graphite, Buckyballs, and Nanotubes
- 24.6 Semiconductors
- 24.7 Superconductors
- 25 NONMETALLIC ELEMENTS AND THEIR COMPOUNDS (ONLINE ONLY)
- 25.1 General Properties of Nonmetals
- 25.2 Hydrogen
- Binary Hydrides
- Isotopes of Hydrogen
- Hydrogenation
- The Hydrogen Economy
- 25.3 Carbon
- 25.4 Nitrogen and Phosphorus
- Nitrogen
- Phosphorus
- 25.5 Oxygen and Sulfur
- Oxygen
- Sulfur
- Thinking Outside the Box: Arsenic
- 25.6 The Halogens
- Preparation and General Properties of the Halogens
- Compounds of the Halogens
- Uses of the Halogens
- 26 METALLURGY AND THE CHEMISTRY OF METALS (Online Only)
- 26.1 Occurrence of Metals
- 26.2 Metallurgical Processes
- Preparation of the Ore
- Production of Metals
- The Metallurgy of Iron
- Steelmaking
- Purification of Metals
- Thinking Outside the Box: Copper
- 26.3 Band Theory of Conductivity
- Conductors
- Semiconductors
- 26.4 Periodic Trends in Metallic Properties
- 26.5 The Alkali Metals
- 26.6 The Alkaline Earth Metals
- Magnesium
- Calcium
- 26.7 Aluminum
- Appendix 1 Mathematical Operations A-1
- Appendix 2 Thermodynamic Data at 1 atm and 25°C A-6
- Appendix 3 Solubility Product Constants at 25°C A-13
- Appendix 4 Dissociation Constants for Weak Acids and Bases at 25°C A-15
- Glossary G-1
- Answers to Odd-Numbered Problems AP-1
- Index I-1
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