Student Selected Solutions Manual for Introductory Chemistry

Table of Contents

1. The Chemical World
   • 1.1 Sand and Water
   • 1.2 Chemicals Compose Ordinary Things
   • 1.3 The Scientific Method: How Chemists Think
   • 1.4 Analyzing and Interpreting Data
   • 1.5 A Beginning Chemist: How to Succeed
2. Measurement and Problem Solving
   • 2.1 The Metric Mix-up: A $125 Million Unit Error
   • 2.2 Scientific Notation: Writing Large and Small Numbers
   • 2.3 Significant Figures: Writing Numbers to Reflect Precision
   • 2.4 Significant Figures in Calculations
   • 2.5 The Basic Units of Measurement
   • 2.6 Problem Solving and Unit Conversion
   • 2.7 Solving Multistep Unit Conversion Problems
   • 2.8 Unit Conversion in Both the Numerator and Denominator
   • 2.9 Units Raised to a Power
   • 2.10 Density
   • 2.11 Numerical Problem-Solving Strategies and the Solution Map
3. Matter and Energy
   • 3.1 In Your Room
   • 3.2 What Is Matter?
   • 3.3 Classifying Matter According to Its State: Solid, Liquid, and Gas
   • 3.4 Classifying Matter According to Its Composition: Elements, Compounds, and Mixtures
   • 3.5 Differences in Matter: Physical and Chemical Properties
   • 3.6 Changes in Matter: Physical and Chemical Changes
   • 3.7 Conservation of Mass: There Is No New Matter
   • 3.8 Energy
   • 3.9 Energy and Chemical and Physical Change
   • 3.10 Temperature: Random Motion of Molecules and Atoms
   • 3.11 Temperature Changes: Heat Capacity
   • 3.12 Energy and Heat Capacity Calculations
4. Atoms and Elements
   • 4.1 Experiencing Atoms at Tiburon
   • 4.2 Indivisible: The Atomic Theory
   • 4.3 The Nuclear Atom
   • 4.4 The Properties of Protons, Neutrons, and Electrons
   • 4.5 Elements: Defined by Their Numbers of Protons
   • 4.6 Looking for Patterns: The Periodic Law and the Periodic Table
   • 4.7 Ions: Losing and Gaining Electrons
   • 4.8 Isotopes: When the Number of Neutrons Varies
   • 4.9 Atomic Mass: The Average Mass of an Element’s Atoms
5. Molecules and Compounds
   • 5.1 Sugar and Salt
   • 5.2 Compounds Display Constant Composition
   • 5.3 Chemical Formulas: How to Represent Compounds
   • 5.4 A Molecular View of Elements and Compounds
   • 5.5 Writing Formulas for Ionic Compounds
   • 5.6 Nomenclature: Naming Compounds
   • 5.7 Naming Ionic Compounds
   • 5.8 Naming Molecular Compounds
   • 5.9 Naming Acids
   • 5.10 Nomenclature Summary
   • 5.11 Formula Mass: The Mass of a Molecule or Formula Unit
6. Chemical Composition
   • 6.1 How Much Sodium?
   • 6.2 Counting Nails by the Pound
   • 6.3 Counting Atoms by the Gram
   • 6.4 Counting Molecules by the Gram
   • 6.5 Chemical Formulas as Conversion Factors
   • 6.6 Mass Percent Composition of Compounds
   • 6.7 Mass Percent Composition from a Chemical Formula
   • 6.8 Calculating Empirical Formulas for Compounds
   • 6.9 Calculating Molecular Formulas for Compounds
7. Chemical Reactions
   • 7.1 Grade School Volcanoes, Automobiles, and Laundry Detergents
   • 7.2 Evidence of a Chemical Reaction
   • 7.3 The Chemical Equation
   • 7.4 How to Write Balanced Chemical Equations
   • 7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water
   • 7.6 Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid
   • 7.7 Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations
   • 7.8 Acid—Base and Gas Evolution Reactions
   • 7.9 Oxidation—Reduction Reactions
   • 7.10 Classifying Chemical Reactions
8. Quantities in Chemical Reactions
   • 8.1 Climate Change: Too Much Carbon Dioxide
   • 8.2 Making Pancakes: Relationships between Ingredients
   • 8.3 Making Molecules: Mole-to-Mole Conversions
   • 8.4 Making Molecules: Mass-to-Mass Conversions
   • 8.5 More Pancakes: Limiting Reactant, Theoretical Yield, and Percent Yield
   • 8.6 Limiting Reactant[JJ2] , Theoretical Yield, and Percent Yield from Initial Masses of Reactants
   • 8.7 Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction
9. Electrons in Atoms and the Periodic Table
   • 9.1 Blimps, Balloons, and Models of the Atom
   • 9.2 Light: Electromagnetic Radiation
   • 9.3 The Electromagnetic Spectrum
   • 9.4 The Bohr Model: Atoms with Orbits
   • 9.5 The Quantum-Mechanical Model: Atoms with Orbitals
   • 9.6 Quantum-Mechanical Orbitals and Electron Configurations
   • 9.7 Electron Configurations and the Periodic Table
   • 9.8 The Explanatory Power of the Quantum-Mechanical Model
   • 9.9 Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
10. Chemical Bonding
    • 10.1 Bonding Models and AIDS Drugs
    • 10.2 Representing Valence Electrons with Dots
    • 10.3 Lewis Structures of Ionic Compounds: Electrons Transferred
    • 10.4 Covalent Lewis Structures: Electrons Shared
    • 10.5 Writing Lewis Structures for Covalent Compounds
    • 10.6 Resonance: Equivalent Lewis Structures for the Same Molecule
    • 10.7 Predicting the Shapes of Molecules
    • 10.8 Electronegativity and Polarity: Why Oil and Water Don’t Mix
11. Gases
    • 11.1 Extra-Long Straws
    • 11.2 Kinetic Molecular Theory: A Model for Gases
    • 11.3 Pressure: The Result of Constant Molecular Collisions
    • 11.4 Boyle’s Law: Pressure and Volume
    • 11.5 Charles’s Law: Volume and Temperature
    • 11.6 The Combined Gas Law: Pressure, Volume, and Temperature
    • 11.7 Avogadro’s Law: Volume and Moles
    • 11.8 The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
    • 11.9 Mixtures of Gases
    • 11.10 Gases in Chemical Reactions
12. Liquids, Solids, and Intermolecular Forces
    • 12.1 Spherical Water
    • 12.2 Properties of Liquids and Solids
    • 12.3 Intermolecular Forces in Action: Surface Tension and Viscosity
    • 12.4 Evaporation and Condensation
    • 12.5 Melting, Freezing, and Sublimation
    • 12.6 Types of Intermolecular Forces: Dispersion, Dipole—Dipole, Hydrogen Bonding, and Ion—Dipole
    • 12.7 Types of Crystalline Solids: Molecular, Ionic, and Atomic
    • 12.8 Water: A Remarkable Molecule
13. Solutions
    • 13.1 Tragedy in Cameroon
    • 13.2 Solutions: Homogeneous Mixtures
    • 13.3 Solutions of Solids Dissolved in Water: How to Make Rock Candy
    • 13.4 Solutions of Gases in Water: How Soda Pop Gets Its Fizz
    • 13.5 Specifying Solution Concentration: Mass Percent
    • 13.6 Specifying Solution Concentration: Molarity
    • 13.7 Solution Dilution
    • 13.8 Solution Stoichiometry
    • 13.9 Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter
    • 13.10 Osmosis: Why Drinking Saltwater Causes Dehydration
14. Acids and Bases
    • 14.1 Sour Patch Kids and International Spy Movies
    • 14.2 Acids: Properties and Examples
    • 14.3 Bases: Properties and Examples
    • 14.4 Molecular Definitions of Acids and Bases
    • 14.5 Reactions of Acids and Bases
    • 14.6 Acid—Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution
    • 14.7 Strong and Weak Acids and Bases
    • 14.8 Water: Acid and Base in One
    • 14.9 The pH and pOH Scales: Ways to Express Acidity and Basicity
    • 14.10 Buffers: Solutions That Resist pH Change
15. Chemical Equilibrium
    • 15.1 Life: Controlled Disequilibrium
    • 15.2 The Rate of a Chemical Reaction
    • 15.3 The Idea of Dynamic Chemical Equilibrium
    • 15.4 The Equilibrium Constant: A Measure of How Far a Reaction Goes
    • 15.5 Heterogeneous Equilibria: The Equilibrium Expression for Reactions Involving a Solid or a Liquid
    • 15.6 Calculating and Using Equilibrium Constants
    • 15.7 Disturbing a Reaction at Equilibrium: Le Châtelier’s Principle
    • 15.8 The Effect of a Concentration Change on Equilibrium
    • 15.9 The Effect of a Volume Change on Equilibrium
    • 15.10 The Effect of a Temperature Change on Equilibrium
    • 15.11 The Solubility-Product Constant
    • 15.12 The Path of a Reaction and the Effect of a Catalyst
16. Oxidation and Reduction
    • 16.1 The End of the Internal Combustion Engine?
    • 16.2 Oxidation and Reduction: Some Definitions
    • 16.3 Oxidation States: Electron Bookkeeping
    • 16.4 Balancing Redox Equations
    • 16.5 The Activity Series: Predicting Spontaneous Redox Reactions[JJ3]
    • 16.6 Batteries: Using Chemistry to Generate Electricity
    • 16.7 Electrolysis: Using Electricity to Do Chemistry
    • 16.8 Corrosion: Undesirable Redox Reactions
17. Radioactivity and Nuclear Chemistry
    • 17.1 Diagnosing Appendicitis
    • 17.2 The Discovery of Radioactivity
    • 17.3 Types of Radioactivity: Alpha, Beta, and Gamma Decay
    • 17.4 Detecting Radioactivity
    • 17.5 Natural Radioactivity and Half-Life
    • 17.6 Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Other Artifacts
    • 17.7 The Discovery of Fission and the Atomic Bomb
    • 17.8 Nuclear Power: Using Fission to Generate Electricity
    • 17.9 Nuclear Fusion: The Power of the Sun
    • 17.10 The Effects of Radiation on Life
    • 17.11 Radioactivity in Medicine
18. Organic Chemistry
    • 18.1 What Do I Smell?
    • 18.2 Vitalism: The Difference between Organic and Inorganic
    • 18.3 Carbon: A Versatile Atom
    • 18.4 Hydrocarbons: Compounds Containing Only Carbon and Hydrogen
    • 18.5 Alkanes: Saturated Hydrocarbons
    • 18.6 Isomers: Same Formula, Different Structure
    • 18.7 Naming Alkanes
    • 18.8 Alkenes and Alkynes
    • 18.9 Hydrocarbon Reactions
    • 18.10 Aromatic Hydrocarbons
    • 18.11 Functional Groups
    • 18.12 Alcohols
    • 18.13 Ethers
    • 18.14 Aldehydes and Ketones
    • 18.15 Carboxylic Acids and Esters
    • 18.16 Amines
    • 18.17 Polymers
19. Biochemistry
    • 19.1 The Human Genome Project
    • 19.2 The Cell and Its Main Chemical Components
    • 19.3 Carbohydrates: Sugar, Starch, and Fiber
    • 19.4 Lipids
    • 19.5 Proteins
    • 19.6 Protein Structure
    • 19.7 Nucleic Acids: Molecular Blueprints
    • 19.8 DNA Structure, DNA Replication, and Protein Synthesis