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Solution Manual for Chemistry: An Atoms-Focused Approach (Second Edition) Second Edition

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ISBN-10 ‏ : ‎ 0393614050
ISBN-13 ‏ : ‎ 978-0393614053
Author: Natalie Foster; Rein V. Kirss; Thomas R. Gilbert

The Second Edition’s new co author, Stacey Lowery Bretz, uses visualization tools―based on Chemistry Education Research, and focused on the particulate nature of matter―to help students self assess what they know before, during, and after each chapter. Smartwork5 allows instructors to use this pedagogy as a diagnostic, and students receive hints and answer specific feedback within the text. New ChemTour Animations support visualization at a molecular level, and are integrated throughout the media package.

Chapter 1: Matter and Energy: An Atomic Perspective
1.1 Exploring the Particulate Nature of Matter
1.2 COAST: A Framework for Solving Problems
1.3 Classes and Properties of Matter
1.4 States of Matter
1.5 Forms of Energy
1.6 Formulas and Models
1.7 Expressing Experimental Results
1.8 Unit Conversions and Dimensional Analysis
1.9 Analyzing Experimental Results
Summary
Chapter 2: Atoms, Ions, and Molecules: The Building Blocks of Matter
2.1 When Projectiles Bounced Off Tissue Paper: The Rutherford Model of Atomic Structure
2.2 Nuclides and Their Symbols
2.3 Navigating the Periodic Table
2.4 The Masses of Atoms, Ions, and Molecules
2.5 Moles and Molar Masses
2.6 Mass Spectrometry: Determining Molecular Masses
Summary
Chapter 3: Atomic Structure: Explaining the Properties of Elements
3.1 Nature’s Fireworks and the Electromagnetic Spectrum
3.2 Atomic Spectra
3.3 Particles of Light: Quantum Theory
3.4 The Hydrogen Spectrum and the Bohr Model
3.5 Electrons as Waves
3.6 Quantum Numbers
3.7 The Sizes and Shapes of Atomic Orbitals
3.8 The Periodic Table and Filling Orbitals
3.9 Electron Configurations of Ions
3.10 The Sizes of Atoms and Ions
3.11 Ionization Energies and Photoelectron Spectroscopy
3.12 Electron Affinities
Summary
Chapter 4: Chemical Bonding: Understanding Climate Change
4.1 Chemical Bonds and Greenhouse Gases
4.2 Electronegativity, Unequal Sharing, and Polar Bonds
4.3 Naming Compounds and Writing Formulas
4.4 Lewis Symbols and Lewis Structures
4.5 Resonance
4.6 The Lengths and Strengths of Covalent Bonds
4.7 Formal Charge: Choosing among Lewis Structures
4.8 Exceptions to the Octet Rule
4.9 Vibrating Bonds and the Greenhouse Effect
Summary
Chapter 5: Bonding Theories: Explaining Molecular Geometry
5.1 Biological Activity and Molecular Shape
5.2 Valence-Shell Electron-Pair Repulsion Theory
5.3 Polar Bonds and Polar Molecules
5.4 Valence Bond Theory and Hybrid Orbitals
5.5 Molecules with Multiple “Central” Atoms
5.6 Chirality and Molecular Recognition
5.7 Molecular Orbital Theory
Summary
Chapter 6: Intermolecular Forces: Attractions between Particles
6.1 Intramolecular Forces versus Intermolecular Forces
6.2 London Dispersion Forces
6.3 Interactions Involving Polar Molecules
6.4 Trends in Solubility
6.5 Phase Diagrams: Intermolecular Forces at Work
6.6 Some Remarkable Properties of Water
Summary
Chapter 7: Stoichiometry: Mass Relationships and Chemical Reactions
7.1 Chemical Reactions and the Carbon Cycle
7.2 Writing Balanced Chemical Equations
7.3 Stoichiometric Calculations
7.4 Limiting Reactants and Percent Yield
7.5 Percent Composition and Empirical Formulas
7.6 Comparing Empirical and Molecular Formulas
7.7 Combustion Analysis
Summary
Chapter 8: Reactions in Aqueous Solutions: Chemistry of the Hydrosphere
8.1 Solutions and Their Concentrations
8.2 Dilutions
8.3 Electrolytes and Nonelectrolytes
8.4 Acid–Base Reactions: Proton Transfer
8.5 Titrations
8.6 Precipitation Reactions
8.7 Oxidation–Reduction Reactions: Electron Transfer
Summary
Chapter 9: Properties of Gases: The Air We Breathe
9.1 An Invisible Necessity: The Properties of Gases
9.2 Effusion, Diffusion, and the Kinetic Molecular Theory of Gases
9.3 Atmospheric Pressure
9.4 Relating P, T, and V: The Gas Laws
9.5 The Combined Gas Law
9.6 Ideal Gases and the Ideal Gas Law
9.7 Densities of Gases
9.8 Gases in Chemical Reactions
9.9 Mixtures of Gases
9.10 Real Gases
Summary
Chapter 10: Thermochemistry: Energy Changes in Chemical Reactions
10.1 Energy as a Reactant or Product
10.2 Transferring Energy and Doing Work
10.3 Enthalpy and Enthalpy Changes
10.4 Heating Curves and Heat Capacity
10.5 Enthalpies of Reaction and Calorimetry
10.6 Hess’s Law and Standard Enthalpies of Reaction
10.7 Enthalpies of Reaction from Enthalpies of Formation and Bond Energies
10.8 Energy Changes When Substances Dissolve
10.9 More Applications of Thermochemistry
Summary
Chapter 11: Properties of Solutions: Their Concentrations and Colligative Properties
11.1 Osmosis: “Water, Water, Everywhere”
11.2 Osmotic Pressure and the van ’t Hoff Factor
11.3 Vapor Pressure
11.4 Solutions of Volatile Substances
11.5 More Colligative Properties of Solutions
11.6 Henry’s Law and the Solubility of Gases
Summary
Chapter 12: Thermodynamics: Why Chemical Reactions Happen
12.1 Spontaneous Processes
12.2 Entropy and the Second Law of Thermodynamics
12.3 Absolute Entropy and Molecular Structure
12.4 Applications of the Second Law
12.5 Calculating Entropy Changes
12.6 Free Energy
12.7 Temperature and Spontaneity
12.8 Driving the Human Engine: Coupled Reactions
Summary
Chapter 13: Chemical Kinetics: Clearing the Air
13.1 Cars and Air Quality
13.2 Reaction Rates
13.3 Effect of Concentration on Reaction Rate
13.4 Reaction Rates, Temperature, and the Arrhenius Equation
13.5 Reaction Mechanisms
13.6 Catalysts
Summary
Chapter 14: Chemical Equilibrium: Equal but Opposite Reaction Rates
14.1 The Dynamics of Chemical Equilibrium
14.2 Writing Equilibrium Constant Expressions
14.3 Relationships between Kc and Kp Values
14.4 Manipulating Equilibrium Constant Expressions
14.5 Equilibrium Constants and Reaction Quotients
14.6 Heterogeneous Equilibria
14.7 Le Châtelier’s Principle
14.8 Calculations Based on K
14.9 Equilibrium and Thermodynamics
14.10 Changing K with Changing Temperature
Summary
Chapter 15: Acid–Base Equilibria: Proton Transfer in Biological Systems
15.1 Acids and Bases: A Balancing Act
15.2 Acid Strength and Molecular Structure
15.3 Strong and Weak Bases
15.4 Conjugate Pairs
15.5 pH and the Autoionization of Water
15.6 Ka, Kb, and the Ionization of Weak Acids and Bases
15.7 Calculating the pH of Acidic and Basic Solutions
15.8 Polyprotic Acids
15.9 Acidic and Basic Salts
Summary
Chapter 16: Additional Aqueous Equilibria: Chemistry and the Oceans
16.1 Ocean Acidification: Equilibrium under Stress
16.2 The Common-Ion Effect
16.3 pH Buffers
16.4 Indicators and Acid—Base Titrations
16.5 Lewis Acids and Bases
16.6 Formation of Complex Ions
16.7 Hydrated Metal Ions as Acids
16.8 Solubility Equilibria
Summary
Chapter 17: Electrochemistry: The Quest for Clean Energy
17.1 Running on Electrons: Redox Chemistry Revisited
17.2 Electrochemical Cells
17.3 Standard Potentials
17.4 Chemical Energy and Electrical Work
17.5 A Reference Point: The Standard Hydrogen Electrode
17.6 The Effect of Concentration on Ecell
17.7 Relating Battery Capacity to Quantities of Reactants
17.8 Corrosion: Unwanted Electrochemical Reactions
17.9 Electrolytic Cells and Rechargeable Batteries
17.10 Fuel Cells
Summary
Chapter 18: The Solid State: A Particulate View
18.1 Stronger, Tougher, Harder
18.2 Structures of Metals
18.3 Alloys
18.4 Metallic Bonds and Conduction Bands
18.5 Semiconductors
18.6 Structures of Some Crystalline Nonmetals
18.7 Salt Crystals: Ionic Solids
18.8 Ceramics: Useful, Ancient Materials
18.9 X-ray Diffraction: How We Know Crystal Structures
Summary
Chapter 19: Organic Chemistry: Fuels, Pharmaceuticals, and Modern Materials
19.1 Carbon: The Stuff of Daily Life
19.2 Alkanes
19.3 Alkenes and Alkynes
19.4 Aromatic Compounds
19.5 Amines
19.6 Alcohols, Ethers, and Reformulated Gasoline
19.7 Aldehydes, Ketones, Carboxylic Acids, Esters, and Amides
19.8 A Brief Survey of Isomers
Summary
Chapter 20: Biochemistry: The Compounds of Life
20.1 Composition, Structure, and Function: Amino Acids
20.2 Protein Structure and Function
20.3 Carbohydrates
20.4 Lipids
20.5 Nucleotides and Nucleic Acids
20.6 From Biomolecules to Living Cells
Summary
Chapter 21: Nuclear Chemistry: The Risks and Benefits
21.1 Decay Modes of Radionuclides
21.2 Rates of Radioactive Decay
21.3 Energy Changes in Radioactive Decay
21.4 Making New Elements
21.5 Nuclear Fusion and the Origin of the Elements
21.6 Nuclear Fission
21.7 Measuring Radioactivity
21.8 Biological Effects of Radioactivity
21.9 Medical Applications of Radionuclides
Summary
Chapter 22: The Main Group Elements: Life and the Periodic Table
22.1 Main Group Elements and Human Health
22.2 Periodic Properties of Main Group Elements
22.3 Major Essential Elements
22.4 Trace and Ultratrace Essential Elements
22.5 Nonessential Elements
22.6 Elements for Diagnosis and Therapy
Summary
Chapter 23: Transition Metals: Biological and Medical Applications
23.1 Transition Metals in Biology: Complex Ions
23.2 Naming Complex Ions and Coordination Compounds
23.3 Polydentate Ligands and Chelation
23.4 Crystal Field Theory
23.5 Magnetism and Spin States
23.6 Isomerism in Coordination Compounds
23.7 Coordination Compounds in Biochemistry
23.8 Coordination Compounds in Medicine
Summary
Appendix 1: Mathematical Procedures
Appendix 2: SI Units and Conversion Factors
Appendix 3: The Elements and Their Properties
Appendix 4: Chemical Bonds and Thermodynamic Data
Appendix 5: Equilibrium Constants
Appendix 6: Standard Reduction Potentials
Appendix 7: Naming Organic Compounds
Glossary
Answers to Particulate Review, Concept Tests, and Practice Exercises
Answers to Selected End-of-Chapter Questions and Problems
Credits
Index