1     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 The Origins of Atoms and Elements     

2  Measurement, Problem Solving, and the Mole Concept
2.1  The Metric Mix-up: A $125 Million Unit Error
2.2  The Reliability of a Measurement
2.3  Density
2.4  Energy and Its Units
2.5  Converting between Units
2.6   Problem-Solving Strategies  
2.7   Solving Problems Involving Equations
2.8   Atoms and the Mole: How Many Particles?

3    The Quantum-Mechanical Model of the Atom    
3.1   Schrödinger’s Cat
3.2   The Nature of Light    
3.3   Atomic Spectroscopy and the Bohr Model    
3.4   The Wave Nature of Matter: The de Broglie Wavelength, the Uncertainty Principle, and Indeterminacy    
3.5   Quantum Mechanics and the Atom    
3.6   The Shapes of Atomic Orbitals

4   Periodic Properties of the Elements    
4.1 Aluminum: Low-Density Atoms Result in Low-Density Metal
4.2 Finding Patterns: The Periodic Law and the Periodic Table    
4.3 Electron Configurations: How Electrons Occupy Orbitals    
4.4 Electron Configurations, Valence Electrons, and the Periodic Table    
4.5 How the Electron Configuration of an Element Relates to Its Properties
4.6 Periodic Trends in the Size of Atoms and Effective Nuclear Charge    
4.7 Ions: Electron Configurations, Magnetic Properties, Ionic Radii, and Ionization Energy

4.8    Electron Affinities and Metallic Character  

5   Molecules and Compounds     
5.1 Hydrogen, Oxygen, and Water
5.2 Types of Chemical Bonds
5.3   Representing Compounds: Chemical Formulas and Molecular Models
5.4   The Lewis Model: Representing Valence Electrons with Dots    
5.5   Ionic Bonding: The Lewis Model and Lattice Energies
5.6   Ionic Compounds: Formulas and Names
5.7     Covalent Bonding: Simple Lewis Structures
5.8   Molecular Compounds: Formulas and Names    
5.9   Formula Mass and the Mole Concept for Compounds  

5.10   Composition of Compounds    
5.11   Determining a Chemical Formula from Experimental Data    
5.12   Organic Compounds

6     Chemical Bonding I: Drawing Lewis Structures and Determining Molecular Shapes    
6.1   Morphine: A Molecular Imposter
6.2   Electronegativity and Bond Polarity
6.3   Writing Lewis Structures for Molecular Compounds and Polyatomic Ions     
6.4     Resonance and Formal Charge
6.5   Exceptions to the Octet Rule: Odd-Electron Species, Incomplete Octets, and Expanded Octets    
6.6   Bond Energies and Bond Lengths
6.7   VSEPR Theory: The Five Basic Shapes    
6.8   VSEPR Theory: The Effect of Lone Pairs    
6.9   VSEPR Theory: Predicting Molecular Geometries

6.10   Molecular Shape and Polarity

7        Chemical Bonding II: Valence Bond Theory and Molecular Orbital Theory
7.1 Oxygen: A Magnetic Liquid
7.2     Valence Bond Theory: Orbital Overlap as a Chemical Bond    
7.3     Valence Bond Theory: Hybridization of Atomic Orbitals    
7.4    Molecular Orbital Theory: Electron Delocalization

7.5     Molecular Orbital Theory: Polyatomic Molecules    
7.6     Bonding in Metals and Semiconductors

8      Chemical Reactions and Chemical Quantities
8.1      Climate Change and the Combustion of Fossil Fuels
8.2      Chemical Change
8.3   Writing and Balancing Chemical Equations    
8.4   Reaction Stoichiometry: How Much Carbon Dioxide?

8.5   Limiting Reactant, Theoretical Yield, and Percent Yield    
8.6    Three Examples of Chemical Reactions: Combustion, Alkali Metals, and Halogens

9     Introduction to Solutions and Aqueous Reactions
9.1        Molecular Gastronomy
9.2        Solution Concentration
9.3   Solution Stoichiometry    
9.4     Types of Aqueous Solutions and Solubility

9.5        Precipitation Reactions    
9.6        Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations    
9.7   Acid–Base Reactions
9.8      Gas-Evolution Reactions    
9.9      Oxidation–Reduction Reactions    

10   Thermochemistry    
10.1    On Fire, But Not Consumed
10.2    The Nature of Energy: Key Definitions
10.3    The First Law of Thermodynamics: There Is No Free Lunch    
10.4     Quantifying Heat and Work    
10.5     Measuring ΔE for Chemical Reactions: Constant-Volume Calorimetry    
10.6     Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
10.7     Measuring ΔH for Chemical Reactions: Constant-Pressure Calorimetry
10.8     Relationships Involving ΔHrxn    
10.9     Determining Enthalpies of Reaction from Bond Energies
10.10   Determining Enthalpies of Reaction from Standard Enthalpies of Formation
10.11   Lattice Energies for Ionic Compounds    

11        Gases    
11.1     Supersonic Skydiving and the Risk of Decompression
11.2     Pressure: The Result of Particle Collisions    
11.3    The Simple Gas Laws: Boyle’s Law, Charles’s Law, and Avogadro’s Law    
11.4    The Ideal Gas Law    
11.5    Applications of the Ideal Gas Law: Molar Volume, Density, and Molar Mass of a Gas
11.6    Mixtures of Gases and Partial Pressures    
11.7    A Particulate Model for Gases: Kinetic Molecular Theory    
11.8    Temperature and Molecular Velocities
11.9    Mean Free Path, Diffusion, and Effusion of Gases    
11.10  Gases in Chemical Reactions: Stoichiometry Revisited
11.11  Real Gases: The Effects of Size and Intermolecular Forces    

12       Liquids, Solids, and Intermolecular Forces    
12.1    Structure Determines Properties    
12.2    Solids, Liquids, and Gases: A Molecular Comparison    
12.3    Intermolecular Forces: The Forces That Hold Condensed States Together    
12.4    Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action    
12.5    Vaporization and Vapor Pressure    
12.6    Sublimation and Fusion    
12.7    Heating Curve for Water    
12.8    Water: An Extraordinary Substance    

13   Phase Diagrams and Crystalline Solids
13.1    Sliding Glaciers
13.2    Phase Diagrams
13.3    Crystalline Solids: Determining Their Structure by X-Ray Crystallography    
13.4    Crystalline Solids: Unit Cells and Basic Structures    
13.5    Crystalline Solids: The Fundamental Types    
13.6    The Structures of Ionic Solids
13.7    Network Covalent Atomic Solids: Carbon and Silicates    

14   Solutions    
14.1    Antifreeze in Frogs
14.2    Types of Solutions and Solubility    
14.3    Energetics of Solution Formation
14.4    Solution Equilibrium and Factors Affecting Solubility    
14.5    Expressing Solution Concentration    
14.6    Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation, and Osmotic Pressure    
14.7    Colligative Properties of Strong Electrolyte Solutions

15   Chemical Kinetics    
15.1    Catching Lizards    
15.2    Rates of Reaction and the Particulate Nature of Matter

15.3    Defining and Measuring the Rate of a Chemical Reaction    
15.4    The Rate Law: The Effect of Concentration on Reaction Rate    
15.5    The Integrated Rate Law: The Dependence of Concentration on Time    
15.6    The Effect of Temperature on Reaction Rate    
15.7    Reaction Mechanisms

15.8    Catalysis    

16   Chemical Equilibrium    
16.1    Fetal Hemoglobin and Equilibrium    
16.2    The Concept of Dynamic Equilibrium    
16.3    The Equilibrium Constant (K)    
16.4    Expressing the Equilibrium Constant in Terms of Pressure    
16.5    Heterogeneous Equilibria: Reactions Involving Solids and Liquids    
16.6    Calculating the Equilibrium Constant from Measured Equilibrium Concentrations    
16.7    The Reaction Quotient: Predicting the Direction of Change    
16.8    Finding Equilibrium Concentrations    
16.9    Le Ch®telier’s Principle: How a System at Equilibrium Responds to Disturbances    

17   Acids and Bases    
17.1    Batman’s Basic Blunder    
17.2    The Nature of Acids and Bases    
17.3    Definitions of Acids and Bases    
17.4    Acid Strength and Molecular Structure
17.5    Acid Strength and the Acid Ionization Constant (Ka)    
17.6    Autoionization of Water and pH
17.7    Finding the [H3O+] and pH of Strong and Weak Acid Solutions    
17.8    Finding the [OH-] and pH of Strong and Weak Base Solutions    
17.9   The Acid–Base Properties of Ions and Salts    
17.10  Polyprotic Acids    
17.11  Lewis Acids and Bases    

18   Aqueous Ionic Equilibrium    
18.1    The Danger of Antifreeze    
18.2    Buffers: Solutions That Resist pH Change    
18.3    Buffer Effectiveness: Buffer Range and Buffer Capacity    
18.4    Titrations and pH Curves    
18.5    Solubility Equilibria and the Solubility Product Constant    
18.6    Precipitation    
18.7    Complex Ion Equilibria    

19   Free Energy and Thermodynamics    
19.1    Energy Spreads Out    
19.2    Spontaneous and Nonspontaneous Processes    
19.3    Entropy and the Second Law of Thermodynamics
19.4    Predicting Entropy and Entropy Changes for Chemical Reactions
19.5    Heat Transfer and Entropy Changes of the Surroundings    
19.6    Gibbs Free Energy    
19.7    Free Energy Changes in Chemical Reactions: Calculating     
19.8    Free Energy Changes for Nonstandard States: The Relationship between  and
19.9    Free Energy and Equilibrium: Relating  to the Equilibrium Constant (K)    

20       Electrochemistry    
20.1    Lightning and Batteries
20.2    Balancing Oxidation–Reduction Equations    
20.3    Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
20.4    Standard Electrode Potentials
20.5    Cell Potential, Free Energy, and the Equilibrium Constant    
20.6    Cell Potential and Concentration
20.7    Batteries: Using Chemistry to Generate Electricity    
20.8    Electrolysis: Driving Nonspontaneous Chemical Reactions with Electricity
20.9    Corrosion: Undesirable Redox Reactions    

21       Radioactivity and Nuclear Chemistry    
21.1    Diagnosing Appendicitis    
21.2    The Discovery of Radioactivity    
21.3    Types of Radioactivity
21.4    The Valley of Stability: Predicting the Type of Radioactivity
21.5    Detecting Radioactivity    
21.6    The Kinetics of Radioactive Decay and Radiometric Dating
21.7    The Discovery of Fission: The Atomic Bomb and Nuclear Power    
21.8    Converting Mass to Energy: Mass Defect and Nuclear Binding Energy    
21.9    Nuclear Fusion: The Power of the Sun    
21.10  Nuclear Transmutation and Transuranium Elements    
21.11  The Effects of Radiation on Life    
21.12  Radioactivity in Medicine and Other Applications    

22   Organic Chemistry    
22.1    Fragrances and Odors    
22.2    Carbon: Why It Is Unique
22.3    Hydrocarbons: Compounds Containing Only Carbon and Hydrogen
22.4    Alkanes: Saturated Hydrocarbons    
22.5    Alkenes and Alkynes    
22.6    Hydrocarbon Reactions
22.7    Aromatic Hydrocarbons
22.8    Functional Groups    
22.9    Alcohols    
22.10  Aldehydes and Ketones
22.11  Carboxylic Acids and Esters
22.12  Ethers    
22.13  Amines    
22.14  Polymers    

23   Transition Metals and Coordination Compounds    
23.1    The Colors of Rubies and Emeralds    
23.2    Properties of Transition Metals
23.3    Coordination Compounds
23.4    Structure and Isomerization    
23.5    Bonding in Coordination Compounds
23.6    Applications of Coordination Compounds

Appendices    
Appendix I    The Units of Measurement
Appendix II     Significant Figures
Appendix III Common Mathematical Operations in Chemistry    
A Scientific Notation    
B Logarithms    
C Quadratic Equations    
D Graphs    
Appendix IV    Useful Data    
A Atomic Colors    
B Standard Thermodynamic Quantities for Selected Substances at 25 °C    
C Aqueous Equilibrium Constants at 25 °C    
D Standard Reduction Half-Cell Potentials at 25 °C    
E Vapor Pressure of Water at various Temperatures    
Appendix V    Answers to Selected Exercises    
Appendix VI    Answers to In-Chapter Practice Problems    

Glossary
Credits
Index

• Key Concept Videos combine artwork from the textbook with both 2D and 3D animations to create a dynamic on-screen viewing and learning experience. These short videos include narration and brief live action clips of author Niva Tro explaining the key concept of each chapter of Chemistry: Structure and Properties.
• Interactive Worked Examples are digital versions of select worked examples from the text that make Tro’s unique problem-solving strategies interactive. In these digital versions, students are instructed how to break down problems using Tro’s “Sort, Strategize, Solve, and Check” technique. These problems are incorporated into MasteringChemistry as assignable activities. 
• Self-Assessment Quizzes at the end of each chapter are algorithmically coded into MasteringChemistry to allow students to practice the types of questions they would commonly see on the ACS or other exams.
• Interactive Simulations are assignable and cover difficult chemistry concepts. Written by leading authors in simulation development, these increase students’ understanding of chemistry and clearly illustrate topics such as stoichiometry, acid-base titration, and cause-and-effect relationships.
• PhET simulations are interactive applets that foster conceptual understanding and active learning, and are complimented by tutorials developed to make these powerful visuals assignable. Topics include acid-base solutions, balancing chemical equations, and molecular polarity.
• Pause and Predict Video Quizzes bring chemistry to life with lab demonstrations that illustrate key topics in general chemistry. Students predict the outcome of experiments as they watch the videos; multiple-choice questions challenge students to apply the concepts from videos to related scenarios.
• End-of-Chapter Questions are enhanced with feedback to provide scaffolded support so students can move between robust tutorials and answering end-of-chapter and test questions on their own. 

Note: If you are purchasing the standalone text or electronic version, MasteringChemistry does not come automatically packaged with the text. To purchase MasteringChemistry, please visit: www.masteringchemistry.com or you can purchase a package of the physical text + MasteringChemistry by searching the Pearson Higher Education website.  MasteringChemistry is not a self-paced technology and should only be purchased when required by an instructor.

• Emphasizing the particulate nature of matter and more specifically how structure affects properties, Dr. Tro consulted—on everything from content and organization to art and pedagogy—with a community of instructors who teach their general chemistry courses with an atoms-first approach
• Unlike in other atoms-first texts, the theme of structure affecting properties is carried throughout the entire book, including the topics commonly taught in the second half of the course, in order to consistently emphasize the theme and present topics in a logical progression. 
  • Art has also been carefully selected to best demonstrate visually the relationship between microscopic and macroscopic.
    
  • Over 250 instructors teaching with an atoms-first approach were involved in the development of the text including: 
    

• 2,000 students were also involved in development by class testing chapter and providing detailed reviews.
  
• 150 reviewers
• 75 class testers
• 50 focus group participants
  

• Conceptual Connections reinforce conceptual understanding of the most complex concepts in each chapter while the consistent step-by-step framework within the in-chapter worked examples encourages students to think logically through the problem-solving process.

• Each chapter includes several Conceptual Connections, in which students are asked to think about key concepts and solve problems without doing any math.

• Tro’s four-step “Sort, Strategize, Solve, and Check” approach helps students connect the concept of the problem to its solution by developing an explicit conceptual plan for each problem. This method helps students understand where to start when given a problem and to think through the solution rather than simply formula hunting based on the given information.
• Two- and three-column example formats help students to understand the logic and purpose of each step in the problem-solving process as well as the details of its implementation. Tro’s conceptual plans map out problems for students and, in many cases, also apply the same methodology to another problem in a side-by-side format.

• Why are some examples presented in two columns rather than three? Some topics can be covered with just one example (with the explanation in the left column and the worked-out example in the right column), while other topics are best covered by having two side-by-side examples (with the explanation in the left column and two side-by-side examples in the center and right column). Three-column examples typically show two similar but slightly different approaches to the same concept.

• Self-Assessment Quizzes are located at the end of each chapter. Tro's Self-Assessment Quizzes contain 10-15 multiple-choice questions that are similar to those found on the ACS exam on other standardized exams. Niva Tro actively participates on the ACS Exams Committee for Gen Chem !, Gen Chem II, and full year exams. The Self-Assessment Quizzes are also assignable in MasteringChemistry.

•  Multipart images include symbolic, macroscopic, and molecular perspectives that are fundamental to visualizing and understanding chemistry.  

• Tro’s multipart images help students see the relationship between the formulas they write down on paper (symbolic), the world they see around them (macroscopic), and the atoms and molecules that compose the world (molecular).
• Abundant molecular-level views show students the connection between everyday processes visible to the eye and the behavior of atoms and molecules. 
• Illustrations include extensive labels and annotations to direct student attention to key elements in the art and promote understanding of the processes depicted.