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Chemistry in Quantitative Language: Fundamentals of General Chemistry Calculations 2nd Revised edition [Pehme köide]

(Senior Materials Scientist, NIKE Inc)
  • Formaat: Paperback / softback, 528 pages, kõrgus x laius x paksus: 245x171x24 mm, kaal: 980 g, 33 line drawings
  • Ilmumisaeg: 12-Oct-2021
  • Kirjastus: Oxford University Press
  • ISBN-10: 0198867786
  • ISBN-13: 9780198867784
Teised raamatud teemal:
Chemistry in Quantitative Language: Fundamentals of General Chemistry Calculations 2nd Revised editionSuurem pilt
  • Formaat: Paperback / softback, 528 pages, kõrgus x laius x paksus: 245x171x24 mm, kaal: 980 g, 33 line drawings
  • Ilmumisaeg: 12-Oct-2021
  • Kirjastus: Oxford University Press
  • ISBN-10: 0198867786
  • ISBN-13: 9780198867784
Teised raamatud teemal:
Püsilink: https://www.kriso.ee/db/9780198867784.html
Märksõnad:
Problem-solving is one of the most challenging aspects students encounter in general chemistry courses, leading to frustration and failure. Consequently, many students become less motivated to take additional chemistry courses after the first year.

This book tackles this issue head on and provides innovative, intuitive, and systematic strategies to tackle any type of calculations encountered in chemistry. The material begins with the basic theories, equations, and concepts of the underlying chemistry, followed by worked examples with carefully
explained step-by-step solutions to showcase the ways in which the problems can be presented.

The second edition contains additional problems at the end of each chapter with varying degrees of difficulty, and many of the original examples have been revised.

Arvustused

Review from previous edition This book provides students with innovative, intuitive and systematic strategies to master problem-solving in chemistry... A valuable guide to solving chemcial equations, and calculations based on chemical equations. * Paul Yates, Chemistry World * A good supplement for any general chemistry course. It differs from the normal book in that the descriptive commentary is kept to a minimum, while the numerical problem-solving pieces are kept simple and methodical. Recommended. * Choice *

1 Atomic Structure and Isotopes
1(8)
1.1 Atomic Theory
1(1)
1.2 The Structure of the Atom
2(2)
1.3 Isotopes
4(1)
1.4 Relative Atomic Mass
5(2)
1.5 Problems
7(2)
2 Formula and Molecular Mass
9(4)
2.1 Formula Mass
9(1)
2.2 Molecular Mass
9(1)
2.3 Molar Mass
10(1)
2.4 Problems
11(2)
3 The Mole and Avogadro's Number
13(6)
3.1 The Mole and Avogadro's Number (Na)
13(1)
3.2 The Mole and Molar Mass
13(1)
3.3 Calculating the Number of Moles
13(5)
3.4 Problems
18(1)
4 Formulas of Compounds and Percent Composition
19(12)
4.1 Percent Composition
19(3)
4.2 Types of Chemical Formula
22(3)
4.3 Empirical Formula from Combustion Analysis
25(2)
4.4 Molecular Formula
27(2)
4.5 Problems
29(2)
5 Chemical Formulas and Nomenclature
31(12)
5.1 General Background
31(1)
5.2 Chemical Formula
32(1)
5.3 Oxidation Numbers
32(2)
5.4 Writing the Formulas of Compounds
34(3)
5.5 Nomenclature of Inorganic Compounds
37(3)
5.6 Problems
40(3)
6 Chemical Equations
43(7)
6.1 Writing Chemical Equations
43(1)
6.2 Balancing Chemical Equations
43(3)
6.3 Types of Chemical Reactions
46(2)
6.4 Problems
48(2)
7 Stoichiometry
50(14)
7.1 Reaction Stoichiometry
50(1)
7.2 Information From a Balanced Equation
50(1)
7.3 Types of Stoichiometric Problem
50(7)
7.4 Limiting Reagents
57(2)
7.5 Reaction Yields: Theoretical, Actual, and Percent Yields
59(1)
7.6 Problems
60(4)
8 Structure of the Atom
64(17)
8.1 Electronic Structure of the Atom
64(1)
8.2 Electromagnetic Radiation
64(2)
8.3 The Nature of Matter and Quantum Theory
66(1)
8.4 The Hydrogen Atom
67(3)
8.5 The Quantum-Mechanical Description of the Hydrogen Atom
70(1)
8.6 Quantum Mechanics and Atomic Orbitals
71(4)
8.7 Electronic Configuration of Multielectron Atoms
75(3)
8.8 Problems
78(3)
9 Chemical Bonding 1: Basic Concepts
81(21)
9.1 Introduction: Types of Chemical Bonds
81(1)
9.2 Lewis Dot Symbols
81(2)
9.3 Ionic Bonding: Formation of Ionic Compounds
83(3)
9.4 Covalent Bonding: Lewis Structures for Molecules
86(1)
9.5 Covalent Bonding: Writing Lewis Structures
86(2)
9.6 Resonance and Formal Charge
88(3)
9.7 Exceptions to the Octet Rule
91(2)
9.8 Polar Covalent Bonds: Bond Polarity and Electronegativity
93(5)
9.9 Problems
98(4)
10 Chemical Bonding 2: Modern Theories of Chemical Bonding
102(27)
10.1 VSPER Theory: Molecular Geometry and the Shapes of Molecules
102(1)
10.2 VSEPR Theory: Predicting Electron Group Geometry and Molecular Shape with the VSEPR Model
103(4)
10.3 VSEPR Theory: Predicting Molecular Shape and Polarity
107(3)
10.4 Valence Bond Theory
110(1)
10.5 Valence Bond Theory: Types of Overlap
111(1)
10.6 Hybridization
112(7)
10.7 Limitations of Valence Bond Theory
119(1)
10.8 Molecular Orbital Theory
120(5)
10.9 Problems
125(4)
11 Gas Laws
129(23)
11.1 Standard Temperature and Pressure
129(1)
11.2 Boyle's Law: Volume vs Pressure
129(1)
11.3 Charles's Law: Volume vs Temperature
130(2)
11.4 The Combined Gas Law
132(2)
11.5 Gay-Lussac's Law and Reactions Involving Gases
134(2)
11.6 Avogadro's Law
136(1)
11.7 The Ideal Gas Law
137(2)
11.8 Density and Molecular Mass of a Gas
139(1)
11.9 Molar Volume of an Ideal Gas
140(2)
11.10 Dalton's Law of Partial Pressure
142(1)
11.11 Partial Pressure and Mole Fraction
143(1)
11.12 Real Gases and Deviation from the Gas Laws
144(2)
11.13 Graham's Law of Diffusion
146(2)
11.14 Problems
148(4)
12 Liquids and Solids
152(25)
12.1 The Liquid State
152(1)
12.2 Vapor Pressure and the Clausius--Clapeyron Equation
152(3)
12.3 The Solid State
155(1)
12.4 The Crystal System
156(3)
12.5 Calculations Involving Unit Cell Dimensions
159(6)
12.6 Ionic Crystal Structure
165(2)
12.7 The Radius Ratio Rule for Ionic Compounds
167(4)
12.8 Determination of Crystal Structure by X-Ray Diffraction
171(3)
12.9 Problems
174(3)
13 Solution Chemistry
177(22)
13.1 Solution and Solubility
177(1)
13.2 Concentration of Solutions
178(10)
13.3 Solving Solubility Problems
188(3)
13.4 Effect of Temperature on Solubility
191(1)
13.5 Solubility Curves
191(2)
13.6 Effect of Pressure on Solubility
193(1)
13.7 Problems
194(5)
14 Volumetric Analysis
199(15)
14.1 Introduction
199(1)
14.2 Applications of Titration
199(1)
14.3 Calculations Involving Acid-Base Titration
200(6)
14.4 Back Titrations
206(4)
14.5 Kjeldahl Nitrogen Determination
210(2)
14.6 Problems
212(2)
15 Ideal Solutions and Colligative Properties
214(14)
15.1 Colligative Properties
214(1)
15.2 Vapor Pressure and Raoult's Law
214(3)
15.3 Elevation of Boiling Point
217(3)
15.4 Depression of Freezing Point
220(2)
15.5 Osmosis and Osmotic Pressure
222(3)
15.6 Problems
225(3)
16 Chemical Kinetics
228(27)
16.1 Rates of Reaction
228(1)
16.2 Measurement of Reaction Rates
228(5)
16.3 Reaction Rates and Stoichiometry
233(1)
16.4 Collision Theory of Reaction Rates
234(1)
16.5 Rate Laws and the Order of Reactions
235(1)
16.6 Experimental Determination of Rate Law Using Initial Rates
236(4)
16.7 The Integrated Rate Equation
240(6)
16.8 Half-Life of a Reaction
246(2)
16.9 Reaction Rates and Temperature: The Arrhenius Equation
248(2)
16.10 Problems
250(5)
17 Chemical Equilibrium
255(21)
17.1 Reversible and Irreversible Reactions
255(1)
17.2 The Equilibrium Constant
255(4)
17.3 The Reaction Quotient
259(1)
17.4 Predicting the Direction of Reaction
259(1)
17.5 Position of Equilibrium
260(1)
17.6 Homogeneous vs Heterogeneous Equilibria
261(1)
17.7 Calculating Equilibrium Constants
262(1)
17.8 Calculating Equilibrium Concentrations from K
263(5)
17.9 Qualitative Treatment of Equilibrium: Le Chatelier's Principle
268(5)
17.10 Problems
273(3)
18 Ionic Equilibria and pH
276(37)
18.1 The Ionization of Water
276(1)
18.2 Definition of Acidity and Basicity
276(1)
18.3 The pH of a Solution
277(1)
18.4 The pOH of a Solution
278(2)
18.5 The Acid Ionization Constant, Ka
280(1)
18.6 Calculating pH and Equilibrium Concentrations in Solutions of Weak Acids
280(3)
18.7 Percent Dissociation of Weak Acids
283(2)
18.8 The Base Dissociation Constant, Kb
285(1)
18.9 Relationship Between Ka and Kb
286(2)
18.10 Salt Hydrolysis: Acid--Basis Properties of Salts
288(4)
18.11 The Common Ion Effect
292(1)
18.12 Buffers and pH of Buffer Solutions
293(5)
18.13 Polyprotic Acids and Bases
298(3)
18.14 More Acid--Base Titration
301(2)
18.15 pH Titration Curves
303(5)
18.16 Problems
308(5)
19 Solubility and Complex-Ion Equilibria
313(12)
19.1 Solubility Equilibria
313(1)
19.2 The Solubility Product Principle
313(1)
19.3 Determining Ksp from Molar Solubility
314(2)
19.4 Calculating Molar Solubility from Ksp
316(2)
19.5 Ksp and Precipitation
318(2)
19.6 Complex-Ion Equilibria
320(3)
19.7 Problems
323(2)
20 Thermochemistry
325(19)
20.1 Introduction
325(1)
20.2 Calorimetry and Heat Capacity
325(2)
20.3 Enthalpy
327(4)
20.4 Hess's Law of Heat Summation
331(2)
20.5 Lattice Energy and the Born-Haber Cycle
333(2)
20.6 Bond Energies and Enthalpy
335(3)
20.7 Problems
338(6)
21 Chemical Thermodynamics
344(21)
21.1 Definition of Terms
344(1)
21.2 The First Law of Thermodynamics
344(1)
21.3 Expansion Work
345(3)
21.4 Entropy
348(1)
21.5 The Second Law of Thermodynamics
348(1)
21.6 Calculation of Entropy Changes in Chemical Reactions
348(4)
21.7 Free Energy
352(1)
21.8 The Standard Free Energy Change
352(3)
21.9 Enthalpy and Entropy Changes during a Phase Change
355(1)
21.10 Free Energy and the Equilibrium Constant
356(2)
21.11 Variation of ΔG0 and Equilibrium Constant with Temperature
358(3)
21.12 Problems
361(4)
22 Oxidation and Reduction Reactions
365(24)
22.1 Introduction
365(1)
22.2 Oxidation and Reduction in Terms of Electron Transfer
365(1)
22.3 Oxidation Numbers (ON)
366(2)
22.4 Oxidation and Reduction in Terms of Oxidation Number
368(1)
22.5 Disproportionation Reactions
369(1)
22.6 Oxidizing and Reducing Agents
369(2)
22.7 Half-Cell Reactions
371(1)
22.8 Balancing Redox Equations
372(9)
22.9 Oxidation-Reduction Titration
381(4)
22.10 Problems
385(4)
23 Fundamentals of Electrochemistry
389(23)
23.1 Galvanic Cells
389(1)
23.2 The Cell Potential
389(1)
23.3 Standard Electrode Potential
390(1)
23.4 The Electrochemical Series (ECS)
391(1)
23.5 Applications of Electrode Potential
391(2)
23.6 Cell Diagrams
393(1)
23.7 Calculating from Electrode Potential
394(2)
23.8 Relationship of the Standard Electrode Potential, the Gibbs Free Energy, and the Equilibrium Constant
396(3)
23.9 Dependence of Cell Potential on Concentration (the Nernst Equation)
399(3)
23.10 Electrolysis
402(1)
23.11 Faraday's Laws of Electrolysis
402(6)
23.12 Problems
408(4)
24 Radioactivity and Nuclear Reactions
412(15)
24.1 Definitions
412(1)
24.2 Radioactive Decay and Nuclear Equations
412(3)
24.3 Nuclear Transmutations
415(1)
24.4 Rates of Radioactive Decay and Half-Life
416(3)
24.5 Energy of Nuclear Reactions
419(4)
24.6 Problems
423(4)
Appendix A
427(18)
A.1 Essential mathematics
427(1)
A.2 Significant figures and mathematical operations
428(1)
A.3 Scientific notation and exponents
429(3)
A.4 Logarithms
432(2)
A.5 Algebraic equations
434(11)
Appendix B
445(12)
B.1 Systems of measurement
445(1)
B.2 Measurement of mass, length, and time
446(1)
B.3 Temperature
447(1)
B.4 Derived units
448(1)
B.5 Density and specific gravity
449(2)
B.6 Dimensional analysis and conversion factors
451(6)
Solutions 457(38)
Index 495
Dr. Christopher Oriakhi works at NIKE Inc as a senior scientist where he is actively involved in materials chemistry R&D, technology innovation management, and new product development. Prior to NIKE, Chris was a Senior Member of Technical Staff at Hewlett-Packard for 15+ years, a Senior Principal Engineer at Bloom Energy in Silicon Valley, and a Senior Technical Director at FUJIFILM in New Castle, Delaware. In addition, Chris has lectured chemistry courses at universities in Nigeria, Canada, and United States. He is a member of the American Chemical Society, Materials Research Society and a fellow of the Royal Society of Chemistry.