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

Introductory Chemistry - 1st Canadian Edition
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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. Cycloalkanes are named based on the number of C atoms in them, just like regular alkanes, but with the prefix cyclo– on the name. What are the names of the three smallest cycloalkanes?
  2. Cycloalkenes are named similarly to cycloalkanes (see Exercise 1). What are the names of the cycloalkenes with five, six, and seven C atoms?
  3. Draw the bond-line structure of all noncyclic alkanes with only four C atoms.
  4. Draw the bond-line structure of all noncyclic alkanes with only five C atoms.
  5. Cyclic alkanes can also have substituent groups on the ring. Draw the bond-line structure of all cyclic alkanes with only four C atoms.
  6. Cyclic alkanes can also have substituent groups on the ring. Draw the bond-line structure of all cyclic alkanes with only five C atoms.
  7. Draw and name all possible isomers of pentene.
  8. Draw and name all possible normal (that is, straight-chain) isomers of heptyne.
  9. Polyunsaturated alkenes have more than one C–C double bond. Draw the carbon backbone of all possible noncyclic polyunsaturated alkenes with four C atoms and two double bonds. What are the complete molecular formulas for each possible molecule?
  10. Draw the carbon backbone of all possible five-carbon cyclic alkenes with two double bonds, assuming no substituents on the ring.
  11. If a hydrocarbon is combined with enough halogen, all the H atoms will eventually be substituted with that halogen atom. Write the balanced chemical reaction between ethane and excess chlorine.
  12. If a hydrocarbon is combined with enough halogen, all the H atoms will eventually be substituted with that halogen atom. Write the balanced chemical reaction between butane and excess bromine.
  13. Molecules with multiple double bonds can also participate in addition reactions. Draw the structure of the product when butadiene, CH2=CH–CH=CH2, reacts with chlorine.
  14. Draw the structure of the product when allene, CH2=C=CH2, reacts with bromine.
  15. What is the maximum number of methyl groups that can be on a propane backbone before the molecule cannot be named as a propane compound?
  16. Explain why cycloethane cannot exist as a real molecule.
  17. In the gasoline industry, what is called isooctane is actually 2,2,4-trimethylpentane. Draw the structure of isooctane.
  18. Isooctane (see Exercise 17) is an isomer of what straight-chain alkane?
  19. The actual name for the explosive TNT is 2,4,6-trinitrotoluene. If the structure of TNT is as shown below, propose the structure of the parent compound toluene.

    \chemfig{-[:-90]*6(-(-O_2N)=-(-NO_2)=-(-NO_2)=)}

  20. Phenol is hydroxybenzene, the simplest aromatic alcohol. Picric acid is an explosive derivative of phenol whose formal name is 2,4,6-trinitrophenol. With reference to Exercise 19, draw the structure of picric acid.
  21. Draw the structures of all possible straight-chain isomers of bromopentane.
  22. Draw the structures of all the possible isomers of butanol. Include branched isomers.
  23. What is the final product of the double elimination of HCl from 1,1-dichloroethane?
  24. Draw the structure of the final product of the double elimination of 1,3-dibromopropane.
  25. Draw the structure of and name the alcohol whose double elimination would yield the same product as in Exercise 23. Name the molecule as a hydroxyl-substituted compound.
  26. Draw the structure of and name the alcohol whose double elimination would yield the same product as in Exercise 24. Name the molecule as a hydroxyl-substituted compound.
  27. Draw the smallest molecule that can have a separate aldehyde and carboxylic acid group.
  28. Name the functional group(s) in the following structure:

    \chemfig{*6(-=(*5(-(--[:0]NH_2)--(=O)-))-=-(-HO)=)}

  29. Ethyl acetate is a common ingredient in nail-polish remover because it is a good solvent. Draw the structure of ethyl acetate.
  30. A lactone is an ester that has its ester functional group in a ring. Draw the structure of the smallest possible lactone. (It is called acetolactone, which might give you a hint about its structure.)
  31. Draw the structure of diethyl ether, once used as an anaesthetic.
  32. The smallest cyclic ether is called an epoxide. Draw its structure.
  33. Write the chemical reaction of HCl with trimethylamine.
  34. Putrescine and cadaverine are molecules with two amine groups on the opposite ends of a butane backbone and a pentane backbone, respectively. They are both emitted by rotting corpses. Draw their structures and determine their molecular formulas.
  35. With four monomers, draw two possible structures of a copolymer composed of ethylene and propylene.
  36. With four monomers, draw two possible structures of a copolymer composed of ethylene and styrene.
  37. Draw the silicone that can be made from this monomer:

    \chemfig{[:90]*6((-[:-90]Si?[a]-[:-90])-----(-[:-90]Si?[a,2]-[:-90]([:-60]*6(-----))))}

  38. One of the ingredients in the original Silly Putty was a silicone polymer with two methyl groups on each Si atom. Draw this silicone.

Answers

  1. cyclopropane, cyclobutane, and cyclopentane
  1. Bond-line structure of all noncyclic alkanes with only four C atoms:

    \chemfig{-[:-30]-[:30]-[:-30]}\hspace{4em}\chemfig{-[:-90](-[:-150])-[:-30]}

  1. Bond-line structure of all cyclic alkanes with only four C atoms:

    \chemfig{*4(----)}\hspace{4em}\chemfig{*3(-(-)--)}

  1. Isomers of pentene:

        \begin{align*} \chemfig{=[:30]-[:-30]-[:30]-[:-30]}&\hspace{4em}\chemfig{-[:30]=[:-30]-[:30]-[:-30]} \\ \\ \chemfig{=[:30](-[:90])-[:-30]-[:30]}&\hspace{4em}\chemfig{-[:30](-[:90])=[:-30]-[:30]} \end{align*}

  1. Carbon backbone of all possible noncyclic polyunsaturated alkenes with four C atoms and two double bonds:

    \chemfig{H_2C=C=CH-[:-60]CH_3}\hspace{4em}\chemfig{H_2C=[:-60]HC-CH=[:-60]CH_2}

    Both molecular formulas are C4H6.

  1. C2H6 + 6Cl2 → C2Cl6 + 6HCl
  1. Structure of butadiene’s reaction with chlorine:

    \chemfig{H-(-[:90]Cl)(-[:-90]H)-(-[:90]Cl)(-[:-90]H)-(-[:90]Cl)(-[:-90]H)-(-[:90]Cl)(-[:-90]H)-H}

  1. two
  1. Structure of isooctane:

    \chemfig{-[:30](-[:90])(-[:150])-[:-30](-[:-90])-[:30]-[:-30]}

  1. Structure of toluene:

    \chemfig{-[:-90]*6(-=-=-=)}

  1. Straight-chain isomers of bromopentane:

    \chemfig{Br-[:30]-[:-30]-[:30]-[:-30]-[:30]}\hspace{4em}\chemfig{-[:30](-[:90]Br)-[:-30]-[:30]-[:-30]}\hspace{4em}\chemfig{-[:-30]-[:30](-[:90]Br)-[:-30]-[:30]}

  1. ethyne

        \begin{align*}\chemfig{HO-[:-60]--[:60]OH} &\hspace{2em} \chemfig{HO-[:-60](-[:-120]HO)-}\end{align*}

  1. The names are 1,2-dihydroxyethane and 1,1-dihydroxyethane, respectively.
  1. \chemfig{H-[:-30](=[:-90]O)-[:30](=[:90]O)-[:-30]OH}
  1. \chemfig{-[:30](=[:90]O)-[:-30]O-[:30]-[:-30]}
  1. \chemfig{-[:30]-[:-30]O-[:30]-[:-30]}
  1. (CH3)3N + HCl → (CH3)3NHCl
  1. (answers will vary)

    \begin{array}{c}\chemfig{-[@{left,0.5}]C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H)(-[:-90]CH_3)-C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H)(-[:-90]CH_3)-C(-[:90]H_2)-[@{right,0.5}]} \polymerdelim[delimiters={[]},height=25 pt]{left}{right} \\ \\ \chemfig{-[@{left,0.5}]C(-[:90]H_2)-C(-[:90]H)(-[:-90]CH_3)-C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H_2)-C(-[:90]H)(-[:-90]CH_3)-C(-[:90]H_2)-[@{right,0.5}]} \polymerdelim[delimiters={[]},height=25 pt]{left}{right} \end{array}

  1. \chemfig{-[@{left,0.5}]Si(-[:90])(-[:-90]([:-60]*6(-----)))-Si(-[:90]([:120]*6(-----)))(-[:-90])-[:0, 2.0]Si(-[:90])(-[:-90]([:-60]*6(-----)))-Si(-[:90]([:120]*6(-----)))(-[:-90])-[@{right,0.5}]} \polymerdelim[delimiters={[]},height=20 pt]{left}{right}

Annotate

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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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