ISE Chemistry
Höfundur:
Julia Burdge (Útgáfa: 6)
Kaup valmöguleikar
Pulling from her experience of teaching general chemistry for many years, the author of the sixth edition of Chemistry offers a text that offers more in-depth explanation in areas where she knows students often encounter misunderstandings. The text is strengthened by its offering in ALEKS, featuring: • ALEKS Topics to assign as pre-requisite assignments to boost student confidence and help those lacking math skills.
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- McGraw-Hill Higher Education (International)
- 9781265647575
- 9781265122447
- ePub
- 6
- Julia Burdge
- English
- 2022-01-03
- 100
- 2
- 2
Kaflar
- Cover
- Title Page
- Copyright
- Dedication
- About the Author
- Brief Contents
- Contents
- Preface
- Acknowledgments
- 1 Chemistry: The Central Science
- 1.1 The Study of Chemistry
- • Chemistry You May Already Know
- ■ How Can I Enhance My Chances of Success in Chemistry Class?
- • The Scientific Method
- 1.2 Classification of Matter
- • States of Matter
- • Elements
- • Compounds
- • Mixtures
- 1.3 Scientific Measurement
- • SI Base Units
- • Mass
- • Temperature
- ■ Fahrenheit Temperature Scale
- • Derived Units: Volume and Density
- ■ Why Are Units So Important?
- 1.4 The Properties of Matter
- • Physical Properties
- • Chemical Properties
- • Extensive and Intensive Properties
- 1.5 Uncertainty in Measurement
- • Significant Figures
- • Calculations with Measured Numbers
- ■ What’s Significant About Significant Figures?
- • Accuracy and Precision
- 1.6 Using Units and Solving Problems
- • Conversion Factors
- • Dimensional Analysis—Tracking Units
- 2 Atoms, Molecules, and Ions
- 2.1 The Atomic Theory
- 2.2 The Structure of the Atom
- • Discovery of the Electron
- • Radioactivity
- • The Proton and the Nucleus
- • Nuclear Model of the Atom
- • The Neutron
- 2.3 Atomic Number, Mass Number, and Isotopes
- 2.4 The Periodic Table
- ■ Distribution of Elements on Earth
- 2.5 The Atomic Mass Scale and Average Atomic Mass
- 2.6 Ions and Ionic Compounds
- • Atomic Ions
- • Polyatomic Ions
- • Formulas of Ionic Compounds
- • Naming Ionic Compounds
- • Oxoanions
- • Hydrates
- 2.7 Molecules and Molecular Compounds
- • Molecular Formulas
- • Naming Molecular Compounds
- • Simple Acids
- • Oxoacids
- • Empirical Formulas of Molecular Substances
- 2.8 Compounds in Review
- 3 Stoichiometry: Ratios of Combination
- 3.1 Molecular and Formula Masses
- 3.2 Percent Composition of Compounds
- 3.3 Chemical Equations
- • Interpreting and Writing Chemical Equations
- • Balancing Chemical Equations
- ■ The Stoichiometry of Metabolism
- 3.4 The Mole and Molar Masses
- • The Mole
- • Determining Molar Mass
- • Interconverting Mass, Moles, and Numbers of Particles
- • Empirical Formula from Percent Composition
- 3.5 Combustion Analysis
- • Determination of Empirical Formula
- • Determination of Molecular Formula
- 3.6 Calculations with Balanced Chemical Equations
- • Moles of Reactants and Products
- • Mass of Reactants and Products
- 3.7 Limiting Reactants
- • Determining the Limiting Reactant
- Limiting Reactant Problems
- • Reaction Yield
- • Types of Chemical Reactions
- 4 Reactions in Aqueous Solutions
- 4.1 General Properties of Aqueous Solutions
- • Electrolytes and Nonelectrolytes
- • Strong Electrolytes and Weak Electrolytes
- • Identifying Electrolytes
- 4.2 Precipitation Reactions
- • Solubility Guidelines for Ionic Compounds in Water
- • Molecular Equations
- • Ionic Equations
- • Net Ionic Equations
- 4.3 Acid-Base Reactions
- • Strong Acids and Bases
- • Brønsted Acids and Bases
- • Acid-Base Neutralization
- 4.4 Oxidation-Reduction Reactions
- • Oxidation Numbers
- • Oxidation of Metals in Aqueous Solutions
- • Balancing Simple Redox Equations
- • Other Types of Redox Reactions
- 4.5 Concentration of Solutions
- • Molarity
- Preparing a Solution from a Solid
- • Dilution
- • Serial Dilution
- • Solution Stoichiometry
- ■ How Are Solution Concentrations Measured?
- 4.6 Aqueous Reactions and Chemical Analysis
- • Gravimetric Analysis
- • Acid-Base Titrations
- • Redox Titration
- 5 Thermochemistry
- 5.1 Energy and Energy Changes
- • Forms of Energy
- • Energy Changes in Chemical Reactions
- • Units of Energy
- 5.2 Introduction to Thermodynamics
- • States and State Functions
- • The First Law of Thermodynamics
- • Work and Heat
- 5.3 Enthalpy
- • Reactions Carried Out at Constant Volume or at Constant Pressure
- • Enthalpy and Enthalpy Changes
- • Thermochemical Equations
- 5.4 Calorimetry
- • Specific Heat and Heat Capacity
- • Constant-Pressure Calorimetry
- Determination of ΔH°rxn by Constant-Pressure Calorimetry
- ■ Heat Capacity and Hypothermia
- • Constant-Volume Calorimetry
- Determination of Specific Heat by Constant-Pressure Calorimetry
- ■ What if the Heat Capacity of the Calorimeter Isn’t Negligible?
- 5.5 Hess’s Law
- 5.6 Standard Enthalpies of Formation
- 6 Quantum Theory and the Electronic Structure of Atoms
- 6.1 The Nature of Light
- • Properties of Waves
- • The Electromagnetic Spectrum
- • The Double-Slit Experiment
- 6.2 Quantum Theory
- • Quantization of Energy
- ■ Laser Pointers
- • Photons and the Photoelectric Effect
- ■ Where Have I Encountered the Photoelectric Effect?
- 6.3 Bohr’s Theory of the Hydrogen Atom
- • Atomic Line Spectra
- • The Line Spectrum of Hydrogen
- Emission Spectrum of Hydrogen
- ■ Lasers
- 6.4 Wave Properties of Matter
- • The de Broglie Hypothesis
- • Diffraction of Electrons
- 6.5 Quantum Mechanics
- • The Uncertainty Principle
- • The Schrödinger Equation
- • The Quantum Mechanical Description of the Hydrogen Atom
- 6.6 Quantum Numbers
- • Principal Quantum Number (n)
- • Angular Momentum Quantum Number (ℓ)
- • Magnetic Quantum Number (mℓ)
- • Electron Spin Quantum Number (ms)
- 6.7 Atomic Orbitals
- • s Orbitals
- • p Orbitals
- • d Orbitals and Other Higher-Energy Orbitals
- • Energies of Orbitals
- 6.8 Electron Configuration
- • Energies of Atomic Orbitals in Many-Electron Systems
- • The Pauli Exclusion Principle
- • The Aufbau Principle
- • Hund’s Rule
- • General Rules for Writing Electron Configurations
- 6.9 Electron Configurations and the Periodic Table
- 7 Electron Configuration and the Periodic Table
- 7.1 Development of the Periodic Table
- ■ The Chemical Elements of Life
- 7.2 The Modern Periodic Table
- • Classification of Elements
- • Representing Free Elements in Chemical Equations
- 7.3 Effective Nuclear Charge
- 7.4 Periodic Trends in Properties of Elements
- • Atomic Radius
- • Ionization Energy
- • Electron Affinity
- • Metallic Character
- • Explaining Periodic Trends
- 7.5 Electron Configuration of Ions
- • Ions of Main Group Elements
- • Ions of d-Block Elements
- 7.6 Ionic Radius
- • Comparing Ionic Radius with Atomic Radius
- • Isoelectronic Series
- 7.7 Periodic Trends in Chemical Properties of the Main Group Elements
- • General Trends in Chemical Properties
- • Properties of the Active Metals
- • Properties of Other Main Group Elements
- • Comparison of Group 1 and Group 11 Elements
- ■ Salt Substitutes
- • Variation in Properties of Oxides Within a Period
- 8 Chemical Bonding I: Basic Concepts
- 8.1 Lewis Dot Symbols
- 8.2 Ionic Bonding
- • Lattice Energy
- • The Born-Haber Cycle
- Born-Haber Cycle
- 8.3 Covalent Bonding
- • Lewis Structures
- • Multiple Bonds
- • Comparison of Ionic and Covalent Compounds
- 8.4 Electronegativity and Polarity
- • Electronegativity
- • Dipole Moment, Partial Charges, and Percent Ionic Character
- 8.5 Drawing Lewis Structures
- 8.6 Lewis Structures and Formal Charge
- 8.7 Resonance
- 8.8 Exceptions to the Octet Rule
- • Incomplete Octets
- • Odd Numbers of Electrons
- ■ The Power of Radicals
- • Expanded Octets
- ■ Which Is More Important: Formal Charge or the Octet Rule?
- 8.9 Bond Enthalpy
- 9 Chemical Bonding II: Molecular Geometry and Bonding Theories
- 9.1 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
- ■ How Are Larger, More Complex Molecules Represented?
- 9.2 Molecular Geometry and Polarity
- ■ Can More Complex Molecules Contain Polar Bonds and Still Be Nonpolar?
- 9.3 Valence Bond Theory
- • Representing Electrons in Atomic Orbitals
- • Energetics and Directionality of Bonding
- 9.4 Hybridization of Atomic Orbitals
- • Hybridization of s and p Orbitals
- • Hybridization of s, p, and d Orbitals
- 9.5 Hybridization in Molecules Containing Multiple Bonds
- Formation of Pi Bonds in Ethylene and Acetylene
- 9.6 Molecular Orbital Theory
- • Bonding and Antibonding Molecular Orbitals
- • σ Molecular Orbitals
- • Bond Order
- • π Molecular Orbitals
- • Molecular Orbital Diagrams
- • Molecular Orbitals in Heteronuclear Diatomic Species
- 9.7 Bonding Theories and Descriptions of Molecules with Delocalized Bonding
- 10 Gases
- 10.1 Properties of Gases
- • Characteristics of Gases
- • Gas Pressure: Definition and Units
- • Calculation of Pressure
- • Measurement of Pressure
- 10.2 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 Combined Gas Law: The Pressure-Temperature-Amount-Volume Relationship
- 10.3 The Ideal Gas Equation
- • Deriving the Ideal Gas Equation from the Empirical Gas Laws
- • Applications of the Ideal Gas Equation
- 10.4 Reactions with Gaseous Reactants and Products
- • Calculating the Required Volume of a Gaseous Reactant
- • Determining the Amount of Reactant Consumed Using Change in Pressure
- • Predicting the Volume of a Gaseous Product
- 10.5 Gas Mixtures
- • Dalton’s Law of Partial Pressures
- • Mole Fractions
- • Using Partial Pressures to Solve Problems
- Molar Volume of a Gas
- ■ Hyperbaric Oxygen Therapy
- 10.6 The Kinetic Molecular Theory of Gases
- • Application to the Gas Laws
- • Molecular Speed
- • Diffusion and Effusion
- 10.7 Deviation from Ideal Behavior
- • Factors That Cause Deviation from Ideal Behavior
- • The van der Waals Equation
- ■ What’s Really the Difference Between Real Gases and Ideal Gases?
- 11 Intermolecular Forces and the Physical Properties of Liquids and Solids
- 11.1 Intermolecular Forces
- • Dipole-Dipole Interactions
- • Hydrogen Bonding
- ■ Sickle Cell Disease
- • Dispersion Forces
- • Ion-Dipole Interactions
- 11.2 Properties of Liquids
- • Surface Tension
- • Viscosity
- • Vapor Pressure
- 11.3 Crystal Structure
- • Unit Cells
- • Packing Spheres
- • Closest Packing
- 11.4 Types of Crystals
- • Ionic Crystals
- ■ How Do We Know the Structures of Crystals?
- • Covalent Crystals
- • Molecular Crystals
- • Metallic Crystals
- 11.5 Amorphous Solids
- 11.6 Phase Changes
- • Liquid-Vapor Phase Transition
- • Solid-Liquid Phase Transition
- • Solid-Vapor Phase Transition
- ■ The Dangers of Phase Changes
- 11.7 Phase Diagrams
- 12 Modern Materials
- 12.1 Polymers
- • Addition Polymers
- • Condensation Polymers
- ■ Electrically Conducting Polymers
- 12.2 Ceramics and Composite Materials
- • Ceramics
- • Composite Materials
- 12.3 Liquid Crystals
- 12.4 Biomedical Materials
- • Dental Implants
- • Soft Tissue Materials
- • Artificial Joints
- 12.5 Nanotechnology
- • Graphite, Buckyballs, and Nanotubes
- 12.6 Semiconductors
- 12.7 Superconductors
- 13 Physical Properties of Solutions
- 13.1 Types of Solutions
- 13.2 The Solution Process
- • Intermolecular Forces and Solubility
- • The Driving Force for Dissolution
- ■ Why Are Vitamins Referred to as Water Soluble and Fat Soluble?
- 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
- ■ Intravenous Fluids
- ■ Hemodialysis
- 13.6 Calculations Using Colligative Properties
- 13.7 Colloids
- 14 Chemical Kinetics
- 14.1 Reaction Rates
- • Average Reaction Rate
- • Instantaneous Rate
- • Stoichiometry and Reaction Rate
- 14.2 Dependence of Reaction Rate on Reactant Concentration
- • The Rate Law
- • Experimental Determination of the Rate Law
- 14.3 Dependence of Reactant Concentration on Time
- • First-Order Reactions
- • Second-Order Reactions
- 14.4 Dependence of Reaction Rate on Temperature
- • Collision Theory
- • The Arrhenius Equation
- 14.5 Reaction Mechanisms
- • Elementary Reactions
- • Rate-Determining Step
- • Experimental Support for Reaction Mechanisms
- • Identifying Plausible Reaction Mechanisms
- • Mechanisms with a Fast Initial Step
- 14.6 Catalysis
- • Heterogeneous Catalysis
- • Homogeneous Catalysis
- • Enzymes: Biological Catalysts
- ■ Catalysis and Hangovers
- 15 Chemical Equilibrium
- 15.1 The Concept of Equilibrium
- ■ How Do We Know That the Forward and Reverse Processes Are Ongoing in a System at Equilibrium?
- 15.2 The Equilibrium Constant
- • Calculating Equilibrium Constants
- • Magnitude of the Equilibrium Constant
- 15.3 Equilibrium Expressions
- • Heterogeneous Equilibria
- • Manipulating Equilibrium Expressions
- • Equilibrium Expressions Containing Only Gases
- 15.4 Using Equilibrium Expressions to Solve Problems
- • Predicting the Direction of a Reaction
- • Calculating Equilibrium Concentrations
- Equilibrium (ice) Tables
- 15.5 Factors That Affect Chemical Equilibrium
- • Addition or Removal of a Substance
- • Changes in Volume and Pressure
- • Changes in Temperature
- • Catalysis
- Le Châtelier’s Principle
- Effect of Volume Change
- ■ What Happens to the Units in Equilibrium Constants?
- ■ Hemoglobin Production at High Altitude
- 16 Acids and Bases
- 16.1 Brønsted Acids and Bases
- 16.2 The Acid-Base Properties of Water
- 16.3 The pH Scale
- ■ Antacids and the pH Balance in Your Stomach
- 16.4 Strong Acids and Bases
- • Strong Acids
- • Strong Bases
- 16.5 Weak Acids and Acid Ionization Constants
- • The Ionization Constant, Ka
- • Calculating pH from Ka
- Using Equilibrium Tables to Solve Problems
- • Percent Ionization
- • Using pH to Determine Ka
- 16.6 Weak Bases and Base Ionization Constants
- • The Ionization Constant, Kb
- • Calculating pH from Kb
- • Using pH to Determine Kb
- 16.7 Conjugate Acid-Base Pairs
- • The Strength of a Conjugate Acid or Base
- • The Relationship Between Ka and Kb of a Conjugate Acid-Base Pair
- 16.8 Diprotic and Polyprotic Acids
- 16.9 Molecular Structure and Acid Strength
- • Hydrohalic Acids
- • Oxoacids
- • Carboxylic Acids
- 16.10 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
- 16.11 Acid-Base Properties of Oxides and Hydroxides
- • Oxides of Metals and Nonmetals
- • Basic and Amphoteric Hydroxides
- 16.12 Lewis Acids and Bases
- 17 Acid-Base Equilibria and Solubility Equilibria
- 17.1 The Common Ion Effect
- 17.2 Buffer Solutions
- • Calculating the pH of a Buffer
- • Preparing a Buffer Solution with a Specific pH
- Buffer Solutions
- ■ Maintaining the pH of Blood
- 17.3 Acid-Base Titrations
- • Strong Acid–Strong Base Titrations
- • Weak Acid–Strong Base Titrations
- • Strong Acid–Weak Base Titrations
- • Acid-Base Indicators
- 17.4 Solubility Equilibria
- • Solubility Product Expression and Ksp
- • Calculations Involving Ksp and Solubility
- • Predicting Precipitation Reactions
- 17.5 Factors Affecting Solubility
- • The Common Ion Effect
- • pH
- Common Ion Effect
- • Complex Ion Formation
- 17.6 Separation of Ions Using Differences in Solubility
- • Fractional Precipitation
- • Qualitative Analysis of Metal Ions in Solution
- 18 Entropy, Free Energy, and Equilibrium
- 18.1 Spontaneous Processes
- 18.2 Entropy
- • A Qualitative Description of Entropy
- • A Quantitative Definition of Entropy
- 18.3 Entropy Changes in a System
- • Calculating ΔSsys
- • Standard Entropy, S°
- • Qualitatively Predicting the Sign of ΔS°sys
- Factors That Influence the Entropy of a System
- 18.4 Entropy Changes in the Universe
- • Calculating ΔSsurr
- • The Second Law of Thermodynamics
- • The Third Law of Thermodynamics
- 18.5 Predicting Spontaneity
- • Gibbs Free-Energy Change, ΔG
- • Standard Free-Energy Changes, ΔG°
- • Using ΔG and ΔG° to Solve Problems
- 18.6 Free Energy and Chemical Equilibrium
- • Relationship Between ΔG and ΔG°
- • Relationship Between ΔG° and K
- 18.7 Thermodynamics in Living Systems
- 19 Electrochemistry
- 19.1 Balancing Redox Reactions
- 19.2 Galvanic Cells
- Construction of a Galvanic Cell
- 19.3 Standard Reduction Potentials
- 19.4 Spontaneity of Redox Reactions Under Standard-State Conditions
- 19.5 Spontaneity of Redox Reactions Under Conditions Other than Standard State
- • The Nernst Equation
- • Concentration Cells
- ■ Biological 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
- • 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
- • Patterns of Nuclear Stability
- • Nuclear Binding Energy
- 20.3 Natural Radioactivity
- • Kinetics of Radioactive Decay
- • Dating Based on Radioactive Decay
- 20.4 Nuclear Transmutation
- 20.5 Nuclear Fission
- Nuclear Fission and Fusion
- 20.6 Nuclear Fusion
- 20.7 Uses of Isotopes
- • Chemical Analysis
- • Isotopes in Medicine
- 20.8 Biological Effects of Radiation
- ■ Radioactivity in Tobacco
- 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
- 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
- ■ The Coordination Chemistry of Oxygen Transport
- 23 Organic Chemistry
- 23.1 Why Carbon Is Different
- 23.2 Organic Compounds
- • Classes of Organic Compounds
- • Naming Organic Compounds
- ■ How Do We Name Molecules with More Than One Substituent?
- ■ How Do We Name Compounds with Specific Functional Groups?
- 23.3 Representing Organic Molecules
- • Condensed Structural Formulas
- • Kekulé Structures
- • Bond-Line Structures
- • Resonance
- 23.4 Isomerism
- • Constitutional Isomerism
- • Stereoisomerism
- ■ Plane-Polarized Light and 3-D Movies
- ■ Biological Activity of Enantiomers
- 23.5 Organic Reactions
- • Addition Reactions
- • Substitution Reactions
- ■ SN1 Reactions
- • Other Types of Organic Reactions
- ■ The Chemistry of Vision
- 23.6 Organic Polymers
- • Addition Polymers
- • Condensation Polymers
- • Biological Polymers
- 24 Metallurgy and the Chemistry of Metals (ONLINE ONLY)
- 24.1 Occurrence of Metals
- ■ The Importance of Molybdenum
- 24.2 Metallurgical Processes
- • Preparation of the Ore
- • Production of Metals
- • The Metallurgy of Iron
- • Steelmaking
- • Purification of Metals
- 24.3 Band Theory of Conductivity
- • Conductors
- • Semiconductors
- 24.4 Periodic Trends in Metallic Properties
- 24.5 The Alkali Metals
- 24.6 The Alkaline Earth Metals
- • Magnesium
- • Calcium
- 24.7 Aluminum
- 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
- 25.6 The Halogens
- • Preparation and General Properties of the Halogens
- • Compounds of the Halogens
- • Uses of the Halogens
- Appendixes
- 1 Mathematical Operations
- 2 Thermodynamic Data at 1 atm and 25°C
- 3 Solubility Product Constants at 25°C
- 4 Dissociation Constants for Weak Acids and Bases at 25°C
- Glossary
- Answers to Odd-Numbered Problems
- Index