Instructor Solutions Manual
Chemistry & Chemical Reactivity
TENTH EDITION
John C. Kotz
State University of New York
College at Oneonta
Paul M. Treichel
University of Wisconsin – Madison
John R. Townsend
West Chester University of Pennsylvania
David A. Treichel
Nebraska Wesleyan University
Prepared by
Alton J. Banks
North Carolina State University - Raleigh
Australia • Brazil • Mexico • Singapore • United Kingdom • United States
, Table of Contents
Chapter 1: Basic Concepts of Chemistry ..........................................................................1
Let’s Review- The Tools of Quantitative Chemistry....................................13
Chapter 2: Atoms, Molecules and Ions ...........................................................................32
Chapter 3: Chemical Reactions.......................................................................................77
Chapter 4: Stoichiometry: Quantitative Information about Chemical Reactions .........104
Chapter 5: Principles of Chemical Reactivity: Energy and Chemical Reactions .........158
Chapter 6: The Structure of Atoms ...............................................................................204
Chapter 7: The Structure of Atoms and Periodic Trends ..............................................227
Chapter 8: Bonding and Molecular Structure ...............................................................254
Chapter 9: Orbital Hybridization and Molecular Orbitals ............................................292
Chapter 10: Gases & Their Properties ..........................................................................317
Chapter 11: Intermolecular Forces and Liquids............................................................359
Chapter 12: The Solid State..........................................................................................379
Chapter 13: Solutions and Their Behavior ...................................................................407
Chapter 14: Chemical Kinetics: The Rates of Chemical Reactions .............................447
Chapter 15: Principles of Chemical Reactivity: Equilibria...........................................488
Chapter 16: Principles of Chemical Reactivity:The Chemistry of Acids and Bases ....524
Chapter 17: Principles of Chemical Reactivity:Other Aspects of Aqueous Equilibria 566
Chapter 18: Thermodynamics-Entropy and Free Energy .............................................627
Chapter 19: Principles of Chemical Reactivity: Electron Transfer Reactions ..............670
Chapter 20: Environmental Chemistry: Environment, Energy, & Sustainability.........719
Chapter 21: The Chemistry of the Main Group Elements ............................................742
Chapter 22: The Chemistry of the Transition Elements ...............................................781
Chapter 23: Carbon: Not Just Another Element ...........................................................808
Chapter 24: Biochemistry .............................................................................................842
Chapter 25: Nuclear Chemistry ....................................................................................857
, Chapter 1
Basic Concepts of Chemistry
Applying Chemical Principles
CO2 in the Oceans
1.1.1.Name of CO2: carbon dioxide
1.1.2. Symbols for metals mentioned in the article:
calcium, Ca; copper, Cu; manganese, Mn; iron, Fe
1.1.3. Most dense metal: Cu (8920 kg/m3) Least dense metal: Ca (1550 kg/m3)
Data taken from www.ptable.com
1.1.4. CaCO3 (calcium carbonate) contains Ca, C, and O.
PRACTICING SKILLS
Nature of Science
1.1. (a) Proposal that pressure increases with decreased volume—hypothesis
(b) Over time experiments indicate that pressure and volume are inversely proportional—law
(c) Proposal that more molecules colliding per given area results in increased pressure--
theory
1.2. Categorize as hypothesis, theory, or law: Hypothesis--a tentative explanation or prediction in
accord with current knowledge.
Green Chemistry
1.3. Sustainable development means meeting today’s needs while ensuring that future
generations will be able to meet theirs.
1.4. Green chemistry refers to practices that reduce waste products during chemical processes,
use materials wisely, use renewable materials, generate substances with the lowest possible
toxicity, and conserve energy as well as materials.
, Chapter 1 Basic Concepts of Chemistry
1.5. Practices of Green Chemistry described:
• Preventing waste
• Energy saved
• Synthetic methods to generate substances with little or no toxicity
• Raw materials (solid catalyst) should be renewable
• To a lesser extent—ALL the practices are used in the new process
1.6. Practices of Green Chemistry described:
• Raw materials (yeast) renewable
• Energy saved—processes run near room temperature and pressure
• Synthesis uses products with low or no toxicity (palm kernel or coconut oil) and not nitric
acid or produce a greenhouse gas
• Substances used to minimize hazards (no nitric acid)
• To a lesser extent—ALL the practices are used in the new process
Matter: Elements and Atoms, Compounds and Molecules
1.7. The name of each of the elements:
(a) C carbon (c) Cl chlorine (e) Mg magnesium—
typically
confused with
manganese (Mn)
(b) K potassium— (d) P phosphorus— (f) Ni nickel
from Latin, frequently
Kalium confused with
Potassium
1.8. The names of each of the elements:
(a) Mn manganese-- (c) Na sodium (e) Xe xenon
typically
confused with
magnesium (Mg)
(b) Cu copper (d) Br bromine (f) Fe iron
1.9. The symbol for each of the elements:
(a) barium Ba (c) chromium Cr (e) arsenic As
(b) titanium Ti (d) lead Pb (f) zinc Zn
2
Chemistry & Chemical Reactivity
TENTH EDITION
John C. Kotz
State University of New York
College at Oneonta
Paul M. Treichel
University of Wisconsin – Madison
John R. Townsend
West Chester University of Pennsylvania
David A. Treichel
Nebraska Wesleyan University
Prepared by
Alton J. Banks
North Carolina State University - Raleigh
Australia • Brazil • Mexico • Singapore • United Kingdom • United States
, Table of Contents
Chapter 1: Basic Concepts of Chemistry ..........................................................................1
Let’s Review- The Tools of Quantitative Chemistry....................................13
Chapter 2: Atoms, Molecules and Ions ...........................................................................32
Chapter 3: Chemical Reactions.......................................................................................77
Chapter 4: Stoichiometry: Quantitative Information about Chemical Reactions .........104
Chapter 5: Principles of Chemical Reactivity: Energy and Chemical Reactions .........158
Chapter 6: The Structure of Atoms ...............................................................................204
Chapter 7: The Structure of Atoms and Periodic Trends ..............................................227
Chapter 8: Bonding and Molecular Structure ...............................................................254
Chapter 9: Orbital Hybridization and Molecular Orbitals ............................................292
Chapter 10: Gases & Their Properties ..........................................................................317
Chapter 11: Intermolecular Forces and Liquids............................................................359
Chapter 12: The Solid State..........................................................................................379
Chapter 13: Solutions and Their Behavior ...................................................................407
Chapter 14: Chemical Kinetics: The Rates of Chemical Reactions .............................447
Chapter 15: Principles of Chemical Reactivity: Equilibria...........................................488
Chapter 16: Principles of Chemical Reactivity:The Chemistry of Acids and Bases ....524
Chapter 17: Principles of Chemical Reactivity:Other Aspects of Aqueous Equilibria 566
Chapter 18: Thermodynamics-Entropy and Free Energy .............................................627
Chapter 19: Principles of Chemical Reactivity: Electron Transfer Reactions ..............670
Chapter 20: Environmental Chemistry: Environment, Energy, & Sustainability.........719
Chapter 21: The Chemistry of the Main Group Elements ............................................742
Chapter 22: The Chemistry of the Transition Elements ...............................................781
Chapter 23: Carbon: Not Just Another Element ...........................................................808
Chapter 24: Biochemistry .............................................................................................842
Chapter 25: Nuclear Chemistry ....................................................................................857
, Chapter 1
Basic Concepts of Chemistry
Applying Chemical Principles
CO2 in the Oceans
1.1.1.Name of CO2: carbon dioxide
1.1.2. Symbols for metals mentioned in the article:
calcium, Ca; copper, Cu; manganese, Mn; iron, Fe
1.1.3. Most dense metal: Cu (8920 kg/m3) Least dense metal: Ca (1550 kg/m3)
Data taken from www.ptable.com
1.1.4. CaCO3 (calcium carbonate) contains Ca, C, and O.
PRACTICING SKILLS
Nature of Science
1.1. (a) Proposal that pressure increases with decreased volume—hypothesis
(b) Over time experiments indicate that pressure and volume are inversely proportional—law
(c) Proposal that more molecules colliding per given area results in increased pressure--
theory
1.2. Categorize as hypothesis, theory, or law: Hypothesis--a tentative explanation or prediction in
accord with current knowledge.
Green Chemistry
1.3. Sustainable development means meeting today’s needs while ensuring that future
generations will be able to meet theirs.
1.4. Green chemistry refers to practices that reduce waste products during chemical processes,
use materials wisely, use renewable materials, generate substances with the lowest possible
toxicity, and conserve energy as well as materials.
, Chapter 1 Basic Concepts of Chemistry
1.5. Practices of Green Chemistry described:
• Preventing waste
• Energy saved
• Synthetic methods to generate substances with little or no toxicity
• Raw materials (solid catalyst) should be renewable
• To a lesser extent—ALL the practices are used in the new process
1.6. Practices of Green Chemistry described:
• Raw materials (yeast) renewable
• Energy saved—processes run near room temperature and pressure
• Synthesis uses products with low or no toxicity (palm kernel or coconut oil) and not nitric
acid or produce a greenhouse gas
• Substances used to minimize hazards (no nitric acid)
• To a lesser extent—ALL the practices are used in the new process
Matter: Elements and Atoms, Compounds and Molecules
1.7. The name of each of the elements:
(a) C carbon (c) Cl chlorine (e) Mg magnesium—
typically
confused with
manganese (Mn)
(b) K potassium— (d) P phosphorus— (f) Ni nickel
from Latin, frequently
Kalium confused with
Potassium
1.8. The names of each of the elements:
(a) Mn manganese-- (c) Na sodium (e) Xe xenon
typically
confused with
magnesium (Mg)
(b) Cu copper (d) Br bromine (f) Fe iron
1.9. The symbol for each of the elements:
(a) barium Ba (c) chromium Cr (e) arsenic As
(b) titanium Ti (d) lead Pb (f) zinc Zn
2
