Complete Solutions Manual for Chemistry and Chemical Reactivity, 11th Edition by John C. Kotz, Paul M. Treichel, John Townsend , 9780357851401. Full chapters included Chapter 1 to 25. 1. Basic Concepts of Chemistry. 2. Atoms, Molecules and Ions. 3. Chemical Reactions. 4. Stoichiometry: Quantitative...
Chapter 1: Basic Concepts of Chemistry ............................................................................................. 1
Chapter 1R: Let’s Review .................................................................................................................. 15
Chapter 2: Atoms, Molecules, and Ions............................................................................................. 36
Chapter 3: Chemical Reactions .......................................................................................................... 88
Chapter 4: Stoichiometry: Quantitative Information about Chemical Reactions ......................... 119
E
Chapter 5: Principles of Chemical Reactivity: Energy and Chemical Reactions.......................... 184
C
Chapter 6: The Structure of Atoms .................................................................................................. 231
Chapter 7: The Structure of Atoms and Periodic Trends ............................................................... 256
N
Chapter 8: Bonding and Molecular Structure.................................................................................. 283
LE
Chapter 9: Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals.... 328
Chapter 10: Gases & Their Properties ............................................................................................. 356
EL
Chapter 11: Intermolecular Forces and Liquids .............................................................................. 398
Chapter 12: The Solid State ............................................................................................................. 418
Chapter 13: Solutions and Their Behavior. ..................................................................................... 448
C
Chapter 14: Chemical Kinetics The Rates of Chemical Reactions................................................ 492
EX
Chapter 15: Principles of Chemical Reactivity: Equilibria ............................................................ 533
Chapter 16: Principles of Chemical Reactivity: The Chemistry of Acids and Bases ................... 569
ED
Chapter 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria ............... 612
Chapter 18: Thermodynamics-Entropy and Free Energy............................................................... 671
Chapter 19: Principles of Chemical Reactivity: Electron Transfer Reactions .............................. 713
M
Chapter 20: Nuclear Chemistry........................................................................................................ 763
Chapter 21: The Chemistry of the Main Group Elements.............................................................. 789
Chapter 22: The Chemistry of the Transition Elements ................................................................. 833
Chapter 23 Carbon: Not Just Another Element............................................................................... 861
Chapter 24 Biochemistry .................................................................................................................. 901
Chapter 25 Environmental Chemistry Earth’s Environment, Energy, and Sustainability............ 919
iii
,Solution and Answer Guide
Kotz Treichel Townsend Treichel, Chemistry and Chemical Reactivity 11e, 978-0-357-85140-1,
Chapter 1: Basic Concepts of Chemistry
TABLE OF CONTENTS
Applying Chemical Principles ........................................................................................................... 1
Practicing Skills ................................................................................................................................... 1
E
General Questions ............................................................................................................................... 7
C
Applying Chemical Principles
N
CO2 in the Oceans
LE
1.1.1. Name of CO2: carbon dioxide
1.1.2. Symbols for metals mentioned in the article:
EL
calcium, Ca; copper, Cu; manganese, Mn; iron, Fe
1.1.3. Most dense metal: Cu (8960 kg/m 3) Least dense metal: Ca (1550 kg/m3)
C
Data taken from www.ptable.com
EX
1.1.4. CaCO3 (calcium carbonate) contains Ca (calcium), C (carbon), and O (oxygen).
ED
Practicing Skills
Nature of Science
M
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.
1
, Solution and Answer Guide: Kotz Treichel Townsend Treichel, Chemistry and Chemical Reactivity 11e,
978-0-357-85140-1, Chapter 1: Basic Concepts of Chemistry
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.
1.5. Practices of Green Chemistry described:
E
• Synthetic methods to maximize incorporation of all materials
C
• Synthetic methods to generate substances with little or no toxicity
• Raw materials should be renewable
N
• Energy requirements recognized for environmental and economic impact minimized
1.6. Practices of Green Chemistry described:
• Raw materials (plant-based materials) renewable
LE
EL
• Energy saved
• Synthesis uses products with low or no toxicity (water and plant-based materials)
•
C
Synthetic methods to generate substances with little or no toxicity
EX
Matter: Elements and Atoms, Compounds and Molecules
1.7. The names of each of the elements:
ED
(a) N nitrogen (c) Br bromine (e) Li lithium
(b) Ca calcium (d) I iodine (f) Fe iron – from the
Latin ferrium
M
1.8. The names of each of the elements:
(a) Cr chromium (c) Mg Magnesium – (e) Ar argon
often confused
with manganese
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