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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. How many electrons does it take to make the mass of one proton?
  2. How many protons does it take to make the mass of a neutron?
  3. Dalton’s initial version of the modern atomic theory says that all atoms of the same element are the same. Is this actually correct? Why or why not?
  4. How are atoms of the same element the same? How are atoms of the same element different?
  5. Give complete atomic symbols for the three known isotopes of hydrogen.
  6. A rare isotope of helium has a single neutron in its nucleus. Write the complete atomic symbol of this isotope.
  7. Use its place on the periodic table to determine if indium, In, atomic number 49, is a metal or a nonmetal.
  8. Only a few atoms of astatine, At, atomic number 85, have been detected. On the basis of its position on the periodic table, would you expect it to be a metal or a nonmetal?
  9. Americium-241 is a crucial part of many smoke detectors. How many neutrons are present in its nucleus?
  10. Potassium-40 is a radioactive isotope of potassium that is present in the human body. How many neutrons are present in its nucleus?
  11. Determine the atomic mass of ruthenium from the given abundance and mass data.
    IsotopeAbundanceMass
    Ruthenium-965.54%95.907 u
    Ruthenium-981.87%97.905 u
    Ruthenium-9912.76%98.906 u
    Ruthenium-10012.60%99.904 u
    Ruthenium-10117.06%100.906 u
    Ruthenium-10231.55%101.904 u
    Ruthenium-10418.62%103.905 u
  12. Determine the atomic mass of tellurium from the given abundance and mass data.
    IsotopeAbundanceMass
    Tellurium-1200.09%119.904 u
    Tellurium-1222.55%121.903 u
    Tellurium-1230.89%122.904 u
    Tellurium-1244.74%123.903 u
    Tellurium-1257.07%124.904 u
    Tellurium-12618.84%125.903 u
    Tellurium-12831.74%127.904 u
    Tellurium-13034.08%129.906 u
  13. One atomic mass unit has a mass of 1.6605 × 10−24 g. What is the mass of one atom of sodium?
  14. One atomic mass unit has a mass of 1.6605 × 10−24 g. What is the mass of one atom of uranium?
  15. One atomic mass unit has a mass of 1.6605 × 10−24 g. What is the mass of one molecule of H2O?
  16. One atomic mass unit has a mass of 1.6605 × 10−24 g. What is the mass of one molecule of PF5?
  17. From their positions on the periodic table, will Cu and I form a molecular compound or an ionic compound?
  18. From their positions on the periodic table, will N and S form a molecular compound or an ionic compound?
  19. Mercury is an unusual element in that when it takes a 1+ charge as a cation, it always exists as the diatomic ion.
    1. Propose a formula for the mercury(I) ion.
    2. What is the formula of mercury(I) chloride?
  20. Propose a formula for hydrogen peroxide, a substance used as a bleaching agent. (Curiously, this compound does not behave as an acid, despite its formula. It behaves more like a classic nonmetal-nonmetal, molecular compound.)
  21. The uranyl cation has the formula UO22+. Propose formulas and names for the ionic compounds between the uranyl cation and F−, SO42−, and PO43−.
  22. The permanganate anion has the formula MnO4−. Propose formulas and names for the ionic compounds between the permanganate ion and K+, Ca2+, and Fe3+.

Answers

  1. About 1,800 electrons
  1. It is not strictly correct because of the existence of isotopes.
  1. H11, H12, and H13
  1. It is a metal.
  1. 146 neutrons
  1. 101.065 u
  1. 3.817 × 10−23 g
  1. 2.991 × 10−23 g
  1. ionic
    1. Hg22+
    2. Hg2Cl2
  1. uranyl fluoride, UO2F2; uranyl sulfate, UO2SO4; uranyl phosphate, (UO2)3(PO4)2

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Chapter 4. Chemical Reactions and Equations
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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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