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Introductory Chemistry - 1st Canadian Edition: End-of-Chapter Material

Introductory Chemistry - 1st Canadian Edition
End-of-Chapter Material
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table of contents
  1. Cover
  2. Title Page
  3. Copyright
  4. Table Of Contents
  5. Acknowledgments
  6. Dedication
  7. About BCcampus Open Education
  8. Chapter 1. What is Chemistry
    1. Some Basic Definitions
    2. Chemistry as a Science
  9. Chapter 2. Measurements
    1. Expressing Numbers
    2. Significant Figures
    3. Converting Units
    4. Other Units: Temperature and Density
    5. Expressing Units
    6. End-of-Chapter Material
  10. Chapter 3. Atoms, Molecules, and Ions
    1. Acids
    2. Ions and Ionic Compounds
    3. Masses of Atoms and Molecules
    4. Molecules and Chemical Nomenclature
    5. Atomic Theory
    6. End-of-Chapter Material
  11. Chapter 4. Chemical Reactions and Equations
    1. The Chemical Equation
    2. Types of Chemical Reactions: Single- and Double-Displacement Reactions
    3. Ionic Equations: A Closer Look
    4. Composition, Decomposition, and Combustion Reactions
    5. Oxidation-Reduction Reactions
    6. Neutralization Reactions
    7. End-of-Chapter Material
  12. Chapter 5. Stoichiometry and the Mole
    1. Stoichiometry
    2. The Mole
    3. Mole-Mass and Mass-Mass Calculations
    4. Limiting Reagents
    5. The Mole in Chemical Reactions
    6. Yields
    7. End-of-Chapter Material
  13. Chapter 6. Gases
    1. Pressure
    2. Gas Laws
    3. Other Gas Laws
    4. The Ideal Gas Law and Some Applications
    5. Gas Mixtures
    6. Kinetic Molecular Theory of Gases
    7. Molecular Effusion and Diffusion
    8. Real Gases
    9. End-of-Chapter Material
  14. Chapter 7. Energy and Chemistry
    1. Formation Reactions
    2. Energy
    3. Stoichiometry Calculations Using Enthalpy
    4. Enthalpy and Chemical Reactions
    5. Work and Heat
    6. Hess’s Law
    7. End-of-Chapter Material
  15. Chapter 8. Electronic Structure
    1. Light
    2. Quantum Numbers for Electrons
    3. Organization of Electrons in Atoms
    4. Electronic Structure and the Periodic Table
    5. Periodic Trends
    6. End-of-Chapter Material
  16. Chapter 9. Chemical Bonds
    1. Lewis Electron Dot Diagrams
    2. Electron Transfer: Ionic Bonds
    3. Covalent Bonds
    4. Other Aspects of Covalent Bonds
    5. Violations of the Octet Rule
    6. Molecular Shapes and Polarity
    7. Valence Bond Theory and Hybrid Orbitals
    8. Molecular Orbitals
    9. End-of-Chapter Material
  17. Chapter 10. Solids and Liquids
    1. Properties of Liquids
    2. Solids
    3. Phase Transitions: Melting, Boiling, and Subliming
    4. Intermolecular Forces
    5. End-of-Chapter Material
  18. Chapter 11. Solutions
    1. Colligative Properties of Solutions
    2. Concentrations as Conversion Factors
    3. Quantitative Units of Concentration
    4. Colligative Properties of Ionic Solutes
    5. Some Definitions
    6. Dilutions and Concentrations
    7. End-of-Chapter Material
  19. Chapter 12. Acids and Bases
    1. Acid-Base Titrations
    2. Strong and Weak Acids and Bases and Their Salts
    3. Brønsted-Lowry Acids and Bases
    4. Arrhenius Acids and Bases
    5. Autoionization of Water
    6. Buffers
    7. The pH Scale
    8. End-of-Chapter Material
  20. Chapter 13. Chemical Equilibrium
    1. Chemical Equilibrium
    2. The Equilibrium Constant
    3. Shifting Equilibria: Le Chatelier’s Principle
    4. Calculating Equilibrium Constant Values
    5. Some Special Types of Equilibria
    6. End-of-Chapter Material
  21. Chapter 14. Oxidation and Reduction
    1. Oxidation-Reduction Reactions
    2. Balancing Redox Reactions
    3. Applications of Redox Reactions: Voltaic Cells
    4. Electrolysis
    5. End-of-Chapter Material
  22. Chapter 15. Nuclear Chemistry
    1. Units of Radioactivity
    2. Uses of Radioactive Isotopes
    3. Half-Life
    4. Radioactivity
    5. Nuclear Energy
    6. End-of-Chapter Material
  23. Chapter 16. Organic Chemistry
    1. Hydrocarbons
    2. Branched Hydrocarbons
    3. Alkyl Halides and Alcohols
    4. Other Oxygen-Containing Functional Groups
    5. Other Functional Groups
    6. Polymers
    7. End-of-Chapter Material
  24. Chapter 17. Kinetics
    1. Factors that Affect the Rate of Reactions
    2. Reaction Rates
    3. Rate Laws
    4. Concentration–Time Relationships: Integrated Rate Laws
    5. Activation Energy and the Arrhenius Equation
    6. Reaction Mechanisms
    7. Catalysis
    8. End-of-Chapter Material
  25. Chapter 18. Chemical Thermodynamics
    1. Spontaneous Change
    2. Entropy and the Second Law of Thermodynamics
    3. Measuring Entropy and Entropy Changes
    4. Gibbs Free Energy
    5. Spontaneity: Free Energy and Temperature
    6. Free Energy under Nonstandard Conditions
    7. End-of-Chapter Material
  26. Appendix A: Periodic Table of the Elements
  27. Appendix B: Selected Acid Dissociation Constants at 25°C
  28. Appendix C: Solubility Constants for Compounds at 25°C
  29. Appendix D: Standard Thermodynamic Quantities for Chemical Substances at 25°C
  30. Appendix E: Standard Reduction Potentials by Value
  31. Glossary
  32. About the Authors
  33. Versioning History

End-of-Chapter Material

Additional Exercises

  1. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the boiling of water, including the proper phase labels.
  2. Chemical equations can also be used to represent physical processes. Write a chemical reaction for the freezing of water, including the proper phase labels.
  3. Explain why 4Na(s) + 2Cl2(g) → 4NaCl(s) should not be considered a proper chemical equation.
  4. Explain why H2(g) + ½O2(g) → H2O(ℓ) should not be considered a proper chemical equation.
  5. Does the chemical reaction represented by 3Zn(s) + 2Al(NO3)3(aq) → 3Zn(NO3)2(aq) + 2Al(s) proceed as written? Why or why not?
  6. Does the chemical reaction represented by 2Au(s) + 2HNO3(aq) → 2AuNO3(aq) + H2(g) proceed as written? Gold is a relatively useful metal for certain applications, such as jewellery and electronics. Does your answer suggest why this is so?
  7. Explain what is wrong with the double-replacement reaction
    NaCl(aq) + KBr(aq) → NaK(aq) + ClBr(aq).
  8. Predict the products of and balance the double-replacement reaction Ag2SO4(aq) + SrCl2(aq) → ?
  9. Write the complete and net ionic equations for the double-replacement reaction
    BaCl2(aq) + Ag2SO4(aq) → ?
  10. Write the complete and net ionic equations for the double-replacement reaction
    Ag2SO4(aq) + SrCl2(aq) → ?
  11. Identify the spectator ions in the reaction NaCl(aq) + KBr(aq) → NaBr(aq) + KCl(aq). What is the net ionic equation?
  12. Complete the reaction 3H2SO4(aq) + 2Al(OH)3(s) → ? and identify the spectator ions. What is the net ionic equation?
  13. Can a reaction be a composition reaction and a redox reaction at the same time? Give an example to support your answer.
  14. Can a reaction be a combustion reaction and a redox reaction at the same time? Give an example to support your answer.
  15. Can a reaction be a decomposition reaction and a redox reaction at the same time? Give an example to support your answer.
  16. Can a reaction be a combustion reaction and a double-replacement reaction at the same time? Give an example to support your answer.
  17. Why is CH4 not normally considered an acid?
  18. Methyl alcohol has the formula CH3OH. Why would methyl alcohol not normally be considered a base?
  19. What are the oxidation numbers of the nitrogen atoms in these substances?
    1. N2
    2. NH3
    3. NO
    4. N2O
    5. NO2
    6. N2O4
    7. N2O5
    8. NaNO3
  20. What are the oxidation numbers of the sulfur atoms in these substances?
    1. SF6
    2. Na2SO4
    3. K2SO3
    4. SO3
    5. SO2
    6. S8
    7. Na2S
  21. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in 2CuCl(aq) → CuCl2(aq) + Cu(s) and indicate the initial and final oxidation numbers of that element.
  22. Disproportion is a type of redox reaction in which the same substance is both oxidized and reduced. Identify the element that is disproportionating in
    3Cl2(g) + 6OH−(aq) → 5Cl−(aq) + ClO3−(aq) + 3H2O(ℓ) and indicate the initial and final oxidation numbers of that element.

Answers

  1. H2O(ℓ) → H2O(g)
  1. The coefficients are not in their lowest whole-number ratio.
  1. No; zinc is lower in the activity series than aluminum.
  1. In the products, the cation is pairing with the cation, and the anion is pairing with the anion.
  1. Complete ionic equation: Ba2+(aq) + 2Cl−(aq) + 2Ag+(aq) + SO42−(aq) → BaSO4(s) + 2AgCl(s)
    Net ionic equation: The net ionic equation is the same as the complete ionic equation.
  1. Each ion is a spectator ion; there is no overall net ionic equation.
  1. Yes; H2 + Cl2 → 2HCl (answers will vary)
  1. Yes; 2HCl → H2 + Cl2 (answers will vary)
  1. It does not increase the H+ ion concentration; it is not a compound of H+.
    1. 0
    2. −3
    3. +2
    4. +1
    5. +4
    6. +4
    7. +5
    8. +5
  1. Copper is disproportionating. Initially, its oxidation number is +1; in the products, its oxidation numbers are +2 and 0, respectively.

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Chapter 5. Stoichiometry and the Mole
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Copyright © 2014

                                by Jessie A. Key

            Introductory Chemistry - 1st Canadian Edition by Jessie A. Key is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.
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