Chemistry: Structure and Properties, Global Edition

Name: Chemistry: Structure and Properties, Global Edition
Price: 4590 ISK
Availability: InStock
Author: Nivaldo J. Tro
ISBN: 9781292767192

Höfundur: Nivaldo J. Tro (Útgáfa: 3)

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For courses in 2-semester general chemistry. A focused atoms-first approach to learning chemistry With Chemistry: Structure and Properties, author Nivaldo Tro tells the story of chemistry with an atoms-first approach, emphasizing that matter is composed of particles and the structure of those particles determines the properties of matter. This relationship is the thread that weaves all of chemistry together and is applied to all aspects of the text.

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Útgefandi: Pearson International Content

ISBN: 9781292767192

Print ISBN: 9781292767178

Format: ePub

Útgáfa: 3

Höfundar: Nivaldo J. Tro

Tungumál: English

Útgefið: 2026-05-27

Prent takmörkun á líftíma: 100

Prent takmörkun: 2

Afritunar takmörkun: 2

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Cover
Cover
Front Matter
Title page
Copyright
About the Author
Brief Contents
Preface
Acknowledgments
Global Edition Acknowledgments
What’s New in This Edition
Contents
Contents
E: Essentials: Units, Measurement, and Problem Solving
Introduction: Essentials: Units, Measurement, and Problem Solving
E.1: The Metric Mix-up: A $125 Million Unit Error
E.2: The Units of Measurement
E.3: The Reliability of a Measurement
E.4: Significant Figures in Calculations
E.5: Density
E.6: Energy and Its Units
E.7: Converting between Units
E.8: Problem-Solving Strategies
E.9: Solving Problems Involving Equations
Chapter Summary: Essentials: Units, Measurement, and Problem Solving
Exercises: Essentials: Units, Measurement, and Problem Solving
1: Atoms
Introduction: Atoms
1.1: A Particulate View of the World: Structure Determines Properties
1.2: Classifying Matter: A Particulate View
1.3: The Scientific Approach to Knowledge
1.4: Early Ideas about the Building Blocks of Matter
1.5: Modern Atomic Theory and the Laws That Led to It
1.6: The Discovery of the Electron
1.7: The Structure of the Atom
1.8: Subatomic Particles: Protons, Neutrons, and Electrons
1.9: Atomic Mass: The Average Mass of an Element’s Atoms
1.10: Atoms and the Mole: How Many Particles?
1.11: The Origins of Atoms and Elements
Chapter Summary: Atoms
Exercises: Atoms
2: The Quantum-Mechanical Model of the Atom
Introduction: The Quantum-Mechanical Model of the Atom
2.1: Schrödinger’s Cat
2.2: The Nature of Light
2.3: Atomic Spectroscopy and the Bohr Model
2.4: The Wave Nature of Matter: The de Broglie Wavelength, the Uncertainty Principle, and Indeterminacy
2.5: Quantum Mechanics and the Atom
2.6: The Shapes of Atomic Orbitals
Chapter Summary: The Quantum-Mechanical Model of the Atom
Exercises: The Quantum-Mechanical Model of the Atom
3: Periodic Properties of the Elements
Introduction: Periodic Properties of the Elements
3.1: Aluminum: Low-Density Atoms Result in Low-Density Metal
3.2: The Periodic Law and the Periodic Table
3.3: Electron Configurations: How Electrons Occupy Orbitals
3.4: Electron Configurations, Valence Electrons, and the Periodic Table
3.5: Electron Configurations and Elemental Properties
3.6: Periodic Trends in Atomic Size and Effective Nuclear Charge
3.7: Ions: Electron Configurations, Magnetic Properties, Radii, and Ionization Energy
3.8: Electron Affinities and Metallic Character
3.9: Periodic Trends Summary
Chapter Summary: Periodic Properties of the Elements
Exercises: Periodic Properties of the Elements
4: Molecules and Compounds
Introduction: Molecules and Compounds
4.1: Hydrogen, Oxygen, and Water
4.2: Types of Chemical Bonds
4.3: Representing Compounds: Chemical Formulas and Molecular Models
4.4: The Lewis Model: Representing Valence Electrons with Dots
4.5: Ionic Bonding: The Lewis Model and Lattice Energies
4.6: Ionic Compounds: Formulas and Names
4.7: Covalent Bonding: Simple Lewis Structures
4.8: Molecular Compounds: Formulas and Names
4.9: Formula Mass and the Mole Concept for Compounds
4.10: Composition of Compounds
4.11: Determining a Chemical Formula from Experimental Data
4.12: Organic Compounds
Chapter Summary: Molecules and Compounds
Exercises: Molecules and Compounds
5: Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes
Introduction: Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes
5.1: Morphine: A Molecular Impostor
5.2: Electronegativity and Bond Polarity
5.3: Writing Lewis Structures for Molecular Compounds and Polyatomic Ions
5.4: Resonance and Formal Charge
5.5: Exceptions to the Octet Rule: Odd-Electron Species, Incomplete Octets, and Expanded Octets
5.6: Bond Energies and Bond Lengths
5.7: VSEPR Theory: The Five Basic Shapes
5.8: VSEPR Theory: The Effect of Lone Pairs
5.9: VSEPR Theory: Predicting Molecular Geometries
5.10: Molecular Shape and Polarity
Chapter Summary: Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes
Exercises: Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes
6: Chemical Bonding II: Valence Bond Theory and Molecular Orbital Theory
Introduction: Chemical Bonding II: Valence Bond Theory and Molecular Orbital Theory
6.1: Oxygen: A Magnetic Liquid
6.2: Valence Bond Theory: Orbital Overlap as a Chemical Bond
6.3: Valence Bond Theory: Hybridization of Atomic Orbitals
6.4: Molecular Orbital Theory: Electron Delocalization
6.5: Molecular Orbital Theory: Polyatomic Molecules
Chapter Summary: Chemical Bonding II: Valence Bond Theory and Molecular Orbital Theory
Exercises: Chemical Bonding II: Valence Bond Theory and Molecular Orbital Theory
7: Chemical Reactions and Chemical Quantities
Introduction: Chemical Reactions and Chemical Quantities
7.1: Climate Change and the Combustion of Fossil Fuels
7.2: Chemical and Physical Change
7.3: Writing and Balancing Chemical Equations
7.4: Reaction Stoichiometry: How Much Carbon Dioxide?
7.5: Stoichiometric Relationships: Limiting Reactant, Theoretical Yield, Percent Yield, and Reactant in Excess
7.6: Three Examples of Chemical Reactions: Combustion, Alkali Metals, and Halogens
Chapter Summary: Chemical Reactions and Chemical Quantities
Exercises: Chemical Reactions and Chemical Quantities
8: Introduction to Solutions and Aqueous Reactions
Introduction: Introduction to Solutions and Aqueous Reactions
8.1: Molecular Gastronomy
8.2: Solution Concentration
8.3: Solution Stoichiometry
8.4: Types of Aqueous Solutions and Solubility
8.5: Precipitation Reactions
8.6: Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
8.7: Acid–Base Reactions
8.8: Gas-Evolution Reactions
8.9: Oxidation–Reduction Reactions
Chapter Summary: Introduction to Solutions and Aqueous Reactions
Exercises: Introduction to Solutions and Aqueous Reactions
9: Thermochemistry
Introduction: Thermochemistry
9.1: Fire and Ice
9.2: The Nature of Energy: Key Definitions
9.3: The First Law of Thermodynamics: Nothing Is Free
9.4: Quantifying Heat and Work
9.5: Measuring ΔE for Chemical Reactions: Constant-Volume Calorimetry
9.6: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
9.7: Measuring ΔH for Chemical Reactions: Constant-Pressure Calorimetry
9.8: Relationships Involving ΔHrxn
9.9: Determining Enthalpies of Reaction from Bond Energies
9.10: Determining Enthalpies of Reaction from Standard Enthalpies of Formation
9.11: Lattice Energies for Ionic Compounds
Chapter in Review: Thermochemistry
Exercises: Thermochemistry
10: Gases
Introduction: Gases
10.1: Supersonic Skydiving and the Risk of Decompression
10.2: A Particulate Model for Gases: Kinetic Molecular Theory
10.3: Pressure: The Result of Particle Collisions
10.4: The Simple Gas Laws: Boyle’s Law, Charles’s Law, and Avogadro’s Law
10.5: The Ideal Gas Law
10.6: Applications of the Ideal Gas Law: Molar Volume, Density, and Molar Mass of a Gas
10.7: Mixtures of Gases and Partial Pressures
10.8: Temperature and Molecular Velocities
10.9: Mean Free Path, Diffusion, and Effusion of Gases
10.10: Gases in Chemical Reactions: Stoichiometry Revisited
10.11: Real Gases: The Effects of Size and Intermolecular Forces
Chapter Summary: Gases
Exercises: Gases
11: Liquids, Solids, and Intermolecular Forces
Introduction: Liquids, Solids, and Intermolecular Forces
11.1: Water, No Gravity
11.2: Solids, Liquids, and Gases: A Molecular Comparison
11.3: Intermolecular Forces: The Forces That Hold Condensed States Together
11.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
11.5: Vaporization and Vapor Pressure
11.6: Sublimation and Fusion
11.7: Heating Curve for Water
11.8: Phase Diagrams
11.9: Water: An Extraordinary Substance
Chapter Summary: Liquids, Solids, and Intermolecular Forces
Exercises: Liquids, Solids, and Intermolecular Forces
12: Crystalline Solids and Modern Materials
Introduction: Crystalline Solids and Modern Materials
12.1: Friday Night Experiments: The Discovery of Graphene
12.2: Crystalline Solids: Determining Their Structures by X-Ray Crystallography
12.3: Crystalline Solids: Unit Cells and Basic Structures
12.4: Crystalline Solids: The Fundamental Types
12.5: The Structures of Ionic Solids
12.6: Network Covalent Atomic Solids: Carbon and Silicates
12.7: Ceramics, Cement, and Glass
12.8: Semiconductors and Band Theory
12.9: Polymers and Plastics
Chapter Summary: Crystalline Solids and Modern Materials
Exercises: Crystalline Solids and Modern Materials
13: Solutions
Introduction: Solutions
13.1: Antifreeze in Frogs
13.2: Types of Solutions and Solubility
13.3: Energetics of Solution Formation
13.4: Solution Equilibrium and Factors Affecting Solubility
13.5: Expressing Solution Concentration
13.6: Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure
13.7: Colligative Properties of Strong Electrolyte Solutions
Chapter Summary: Solutions
Exercises: Solutions
14: Chemical Kinetics
Introduction: Chemical Kinetics
14.1: Catching Lizards
14.2: Rates of Reaction and the Particulate Nature of Matter
14.3: Defining and Measuring the Rate of a Chemical Reaction
14.4: The Rate Law: The Effect of Concentration on Reaction Rate
14.5: The Integrated Rate Law: The Dependence of Concentration on Time
14.6: The Effect of Temperature on Reaction Rate
14.7: Reaction Mechanisms
14.8: Catalysis
Chapter Summary: Chemical Kinetics
Exercises: Chemical Kinetics
15: Chemical Equilibrium
Introduction: Chemical Equilibrium
15.1: Fetal Hemoglobin and Equilibrium
15.2: The Concept of Dynamic Equilibrium
15.3: The Equilibrium Constant (K)
15.4: Expressing the Equilibrium Constant in Terms of Pressure
15.5: Heterogeneous Equilibria: Reactions Involving Solids and Liquids
15.6: Calculating the Equilibrium Constant from Measured Equilibrium Concentrations
15.7: The Reaction Quotient: Predicting the Direction of Change
15.8: Finding Equilibrium Concentrations
15.9: Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
Chapter Summary: Chemical Equilibrium
Exercises: Chemical Equilibrium
16: Acids and Bases
Introduction: Acids and Bases
16.1: Batman’s Basic Blunder
16.2: The Nature of Acids and Bases
16.3: Definitions of Acids and Bases
16.4: Acid Strength and Molecular Structure
16.5: Acid Strength and the Acid Ionization Constant (Ka)
16.6: Autoionization of Water and pH
16.7: Finding the [H3O+] and pH of Strong and Weak Acid Solutions
16.8: Finding the [OH−] and pH of Strong and Weak Base Solutions
16.9: The Acid–Base Properties of Ions and Salts
16.10: Polyprotic Acids
16.11: Lewis Acids and Bases
Chapter Summary: Acids and Bases
Exercises: Acids and Bases
17: Aqueous Ionic Equilibrium
Introduction: Aqueous Ionic Equilibrium
17.1: The Danger of Antifreeze
17.2: Buffers: Solutions That Resist pH Change
17.3: Buffer Effectiveness: Buffer Range and Buffer Capacity
17.4: Titrations and pH Curves
17.5: Solubility Equilibria and the Solubility Product Constant
17.6: Precipitation
17.7: Complex Ion Equilibria
Chapter Summary: Aqueous Ionic Equilibrium
Exercises: Aqueous Ionic Equilibrium
18: Free Energy and Thermodynamics
Introduction: Free Energy and Thermodynamics
18.1: Nature’s Heat Tax: You Can’t Win and You Can’t Break Even
18.2: Spontaneous and Nonspontaneous Processes
18.3: Entropy and the Second Law of Thermodynamics
18.4: Entropy Changes Associated with State Changes
18.5: Heat Transfer and Entropy Changes of the Surroundings
18.6: Gibbs Free Energy
18.7: Entropy Changes in Chemical Reactions: Calculating ΔSrxn°
18.8: Free Energy Changes in Chemical Reactions: Calculating ΔGrxn°
18.9: Free Energy Changes for Nonstandard States: The Relationship between ΔGrxn° and ΔGrxn
18.10: Free Energy and Equilibrium: Relating ΔGrxn° to the Equilibrium Constant (K)
Chapter Summary: Free Energy and Thermodynamics
Exercises: Free Energy and Thermodynamics
19: Electrochemistry
Introduction: Electrochemistry
19.1: Lightning and Batteries
19.2: Balancing Oxidation–Reduction Equations
19.3: Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
19.4: Standard Electrode Potentials
19.5: Cell Potential, Free Energy, and the Equilibrium Constant
19.6: Cell Potential and Concentration
19.7: Batteries: Using Chemistry to Generate Electricity
19.8: Electrolysis: Driving Nonspontaneous Chemical Reactions with Electricity
19.9: Corrosion: Undesirable Redox Reactions
Chapter Summary: Electrochemistry
Exercises: Electrochemistry
20: Radioactivity and Nuclear Chemistry
Introduction: Radioactivity and Nuclear Chemistry
20.1: Diagnosing Appendicitis
20.2: The Discovery of Radioactivity
20.3: Types of Radioactivity
20.4: The Valley of Stability: Predicting the Type of Radioactivity
20.5: Detecting Radioactivity
20.6: The Kinetics of Radioactive Decay and Radiometric Dating
20.7: The Discovery of Fission: The Atomic Bomb and Nuclear Power
20.8: Converting Mass to Energy: Mass Defect and Nuclear Binding Energy
20.9: Nuclear Fusion: The Power of the Sun
20.10: Nuclear Transmutation and Transuranium Elements
20.11: The Effects of Radiation on Life
20.12: Radioactivity in Medicine and Other Applications
Chapter Summary: Radioactivity and Nuclear Chemistry
Exercises: Radioactivity and Nuclear Chemistry
21: Organic Chemistry
Introduction: Organic Chemistry
21.1: Fragrances and Odors
21.2: Carbon: Why It Is Unique
21.3: Hydrocarbons: Compounds Containing Only Carbon and Hydrogen
21.4: Alkanes: Saturated Hydrocarbons
21.5: Alkenes and Alkynes
21.6: Hydrocarbon Reactions
21.7: Aromatic Hydrocarbons
21.8: Functional Groups
21.9: Alcohols
21.10: Aldehydes and Ketones
21.11: Carboxylic Acids and Esters
21.12: Ethers
21.13: Amines
Chapter Summary: Organic Chemistry
Exercises: Organic Chemistry
22: Transition Metals and Coordination Compounds
Introduction: Organic Chemistry
22.1: The Colors of Rubies and Emeralds
22.2: Properties of Transition Metals
22.3: Coordination Compounds
22.4: Structure and Isomerization
22.5: Bonding in Coordination Compounds
22.6: Applications of Coordination Compounds
Chapter Summary: Transition Metals and Coordination Compounds
Exercises: Transition Metals and Coordination Compounds
Backmatter
Appendix I: Common Mathematical Operations in Chemistry
Appendix II: Useful Data
Appendix III: Answers to Selected End-of-Chapter Problems
Appendix IV: Answers to In-Chapter Practice Problems
List of Elements with Their Symbols and Atomic Masses
Periodic Table
Conversion Factors and Relationships
Selected Key Equations
Math and Chemistry-Based Glossary
Credits
Glossary