Principles of chemistry: a molecular approach
Gespeichert in:
| 1. Verfasser: | |
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| Format: | Buch |
| Sprache: | English |
| Veröffentlicht: |
Harlow, Essex
Pearson
[2016]
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| Ausgabe: | Third edition |
| Schlagworte: | |
| Online-Zugang: | Inhaltsverzeichnis |
| Beschreibung: | 833 Seiten, Seite A1-A46, G1-G15, C1-C2, I1-I33 Seiten Illustrationen, Diagramme (überwiegend farbig) |
| ISBN: | 9781292097282 1292097280 9780321971944 |
Internformat
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| 245 | 1 | 0 | |a Principles of chemistry |b a molecular approach |c Nivaldo J. Tro, Westmont College |
| 250 | |a Third edition | ||
| 264 | 1 | |a Harlow, Essex |b Pearson |c [2016] | |
| 264 | 4 | |c © 2016 | |
| 300 | |a 833 Seiten, Seite A1-A46, G1-G15, C1-C2, I1-I33 Seiten |b Illustrationen, Diagramme (überwiegend farbig) | ||
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Datensatz im Suchindex
| _version_ | 1804176434590121984 |
|---|---|
| adam_text | Contents
Preface 15
Matter, Measurement,
and Problem Solving 28
1.1 Atoms and Molecules 29
1.2 The Scientific Approach to Knowledge 31
1.3 The Classification of Matter 33
The States of Matter: Solid, Liquid, and Gas 33 Classifying
Matter According to Its Composition; Elements, Compounds,
and Mixtures 34
1.4 Physical and Chemical Changes and
Physical and Chemical Properties 35
1.5 Energy: A Fundamental Part of Physical and
Chemical Change 38
1.6 The Units of Measurement 39
The Standard Units 39 The Meter: A Measure of Length 40
The Kilogram: A Measure of Mass 40 The Second: A
Measure of Time 40 The Kelvin: A Measure of
Temperature 40 Prefix Multipliers 42 Derived Units: Volume
and Density 43 Volume 43 Density 44 Calculating
Density 44
1.7 The Reliability of a Measurement 45
Counting Significant Figures 47 Exact Numbers 48
Significant Figures in Calculations 49 Precision and
Accuracy 50
1.8
Atoms and Elements es
2.1 Imaging and Moving Individual Atoms 69
2.2 Modern Atomic Theory and the Laws
That Led to It 71
The Law of Conservation of Mass 71 The Law of Definite
Proportions 72 The Law of Multiple Proportions 73 John
Dalton and the Atomic Theory 74
2.3 The Discovery of the Electron 74
Cathode Rays 75 Millikan’s Oil Drop Experiment:
The Charge of the Electron 76
2.4 The Structure of the Atom 76
Solving Chemical Problems 51
Converting from One Unit to Another 51 General Problem-
Solving Strategy 53 Units Raised to a Power 55
Problems Involving an Equation 56
Chapter in Review 59
Key Terms 59 Key Concepts 59 Key Equations and
Relationships 60 Key Learning Objectives 60
Exercises 60
Problems by Topic 60 Cumulative Problems 64
Challenge Problems 65 Conceptual Problems 66
Questions for Group Work 67 Answers to Conceptual
Connections 67
2.5 Subatomic Particles: Protons, Neutrons, and
Electrons in Atoms 78
Elements: Defined by Their Numbers of Protons 79
Isotopes: When the Number of Neutrons Varies 80
Ions: Losing and Gaining Electrons 82
2.6 Finding Patterns: The Periodic Law and
the Periodic Table 83
Ions and the Periodic Table 85
2.7 Atomic Mass: The Average Mass of an
Element’s Atoms 87
2.8 Molar Mass: Counting Atoms by Weighing Them 88
The Mole: A Chemist’s “Dozen” 88 Converting between
Number of Moles and Number of Atoms 89 Converting
between Mass and Amount (Number of Moles) 90
Chapter in Review 94
Key Terms 94 Key Concepts 95 Key Equations and
Relationships 95 Key Learning Objectives 95
Exercises 96
Problems by Topic 96 Cumulative Problems 98
Challenge Problems 99 Conceptual Problems 100
Questions for Group Work loo Answers to Conceptual
Connections loi
5
6 Contents
Molecules, Compounds, and
Chemical Equations 102
3.1 Hydrogen, Oxygen, and Water 103
3.2 Chemical Bonds 105
Ionic Bonds 105 Covalent Bonds 106
3.3 Representing Compounds: Chemical Formulas
and Molecular Models 106
Types of Chemical Formulas 106 Molecular Models 108
3.4 An Atomic-Level View of Elements and Compounds 108
3.5 Ionic Compounds: Formulas and Names 112
Writing Formulas for Ionic Compounds 113 Naming Ionic
Compounds 113 Naming Binary Ionic Compounds
Containing a Metal That Forms Only One Type of Cation 115
Naming Binary Ionic Compounds Containing a Metal That
Forms More Than One Kind of Cation 116 Naming Ionic
Compounds Containing Polyatomic Ions 117 Hydrated Ionic
Compounds 118
3.6 Molecular Compounds: Formulas and Names 119
Naming Molecular Compounds 119 Naming Acids 120
Naming Binary Acids 121 Naming Oxyacids 121
3.7 Formula Mass and the Mole Concept
for Compounds 122
Molar Mass of a Compound 123 Using Molar Mass
to Count Molecules by Weighing 123
3.8 Composition of Compounds 125
Conversion Factors from Chemical Formulas 127
3.9 Determining a Chemical Formula from
Experimental Data 128
Calculating Molecular Formulas for
Compounds 130 Combustion Analysis 131
3.10 Writing and Balancing Chemical Equations 133
Writing Balanced Chemical Equations 135
3.11 Organic Compounds 137
Chapter in Review 140
Key Terms 140 Key Concepts 140 Key Equations
and Relationships 141 Key Learning Objectives 142
Exercises 143
Problems by Topic 143 Cumulative Problems 146
Challenge Problems 147 Conceptual Problems 148
Questions for Group Work 148 Answers to Conceptual
Connections 148
Chemical Quantities and
Aqueous Reactions 150
4.1 Climate Change and the Combustion of Fossil Fuels 151
4.2 Reaction Stoichiometry: How Much
Carbon Dioxide? 153
Making Pizza: The Relationships Among Ingredients 153
Making Molecules: Mole-to-Mole Conversions 154
Making Molecules: Mass-to-Mass Conversions 154
4.3 Limiting Reactant, Theoretical Yield, and
Percent Yield 157
Limiting Reactant,Theoretical Yield, and Percent Yield
from Initial Reactant Masses 159
4.4 Solution Concentration and Solution Stoichiometry 163
Solution Concentration 164 Using Molarity in
Calculations 165 Solution Stoichiometry 169
4.5 Types of Aqueous Solutions and Solubility 170
Electrolyte and Nonelectrolyte Solutions 171 The Solubility
of Ionic Compounds 172
4.6 Precipitation Reactions 174
4.7 Representing Aqueous Reactions: Molecular, Ionic,
and Complete Ionic Equations 178
4.8 Acid-Base and Gas-Evolution Reactions 180
Acid-Base Reactions 180 Gas-Evolution Reactions 183
4.S Oxidation-Reduction Reactions 185
Oxidation States 187 Identifying Redox Reactions 189
Combustion Reactions 191
Chapter in Review 193
Key Terms 193 Key Concepts 193 Key Equations and
Relationships 194 Key Learning Objectives 194
Exercises 194
Problems by Topic 194 Cumulative Problems 198
Challenge Problems 199 Conceptual Problems 200
Questions for Group Work 201 Answers to Conceptual
Connections 201
Gases
5.1 Breathing: Putting Pressure to Work
5.2 Pressure: The Result of Molecular Collisions
Pressure Units 205
202
203
204
Contents 7
5.3 The Simple Gas Laws: Boyle’s Law, Charles’s Law,
andAvogadro’s Law 206
Boyle’s Law: Volume and Pressure 207 Charles’s Law:
Volume and Temperature 209 Avogadro’s Law: Volume and
Amount (in Moles) 211
5.4 The Ideal Gas Law 212
5.5 Applications of the Ideal Gas Law: Molar Volume,
Density, and Molar Mass of a Gas 214
Molar Volume at Standard Temperature and Pressure 215
Density of a Gas 215 Molar Mass of a Gas 217
5.6 Mixtures of Gases and Partial Pressures 218
Collecting Gases over Water 222
5.7 Gases in Chemical Reactions: Stoichiometry
Revisited 224
Molar Volume and Stoichiometry 226
5.8 Kinetic Molecular Theory: A Model for Gases 227
The Nature of Pressure 228 Boyle’s Law 228 Charles s
Law 228 Avogadro s Law 228 Dalton’s Law 228
Temperature and Molecular Velocities 229
5.9 Mean Free Path, Diffusion, and
Effusion of Gases 231
5.10 Real Gases: The Effects of Size and Intermolecular
Forces 233
The Effect of the Finite Volume of Gas Particles 233 The Effect
of Intermolecular Forces 234 Van der Waals Equation 235
Chapter in Review 236
Key Terms 236 Key Concepts 236 Key Equations and
Relationships 237 Key Learning Objectives 237
Exercises 238
Problems by Topic 238 Cumulative Problems 241
Challenge Problems 243 Conceptual Problems 244
Questions for Group Work 244 Answers to Conceptual
Connections 245
Thermochemistry 246
6.1 Chemical Hand Warmers 247
6.2 The Nature of Energy: Key Definitions 248
Units of Energy 250
6.3 The First Law of Thermodynamics: There Is
No Free Lunch 251
Internal Energy 251
6.4 Quantifying Heat and Work 256
Heat 256 Thermal Energy Transfer 258 Work:
Pressure-Volume Work 260
6.5 Measuring AE for Chemical Reactions: Constant-
Volume Calorimetry 261
6.6 Enthalpy: The Heat Evolved in a Chemical Reaction at
Constant Pressure 264
Exothermic and Endothermic Processes: A Molecular
View 266 Stoichiometry Involving AH: Thermochemical
Equations 267
6.7 Constant-Pressure Calorimetry: Measuring AHm 268
6.8 Hess’s Law and Other Relationships
Involving AH^n 270
6.9 Enthalpies of Reaction from Standard
Heats of Formation 273
Standard States and Standard Enthalpy Changes 273
Calculating the Standard Enthalpy Change for a Reaction 275
Chapter in Review 279
Key Terms 279 Key Concepts 279 Key Equations and
Relationships 280 Key Learning Objectives 280
Exercises 281
Problems by Topic 281 Cumulative Problems 284
Challenge Problems 285 Conceptual Problems 286
Questions for Group Work 286 Answers to Conceptual
Connections 287
The Quantum-Mechanical Model
of the Atom 288
7.1 Schrodinger’s Cat 290
7.2 The Nature of Light 290
The Wave Nature of Light 291 The Electromagnetic
Spectrum 293 Interference and Diffraction 294 The
Particle Nature of Light 296
7.3 Atomic Spectroscopy and the Bohr Model 299
7.4 The Wave Nature of Matter: The de Broglie Wavelength,
the Uncertainty Principle, and Indeterminacy 301
The de Broglie Wavelength 302 The Uncertainty
Principle 303 Indeterminacy and Probability Distribution
Maps 305
8 Contents
Trends in First Ionization Energy 351 Exceptions to Trends in
First Ionization Energy 354 Trends in Second and
Successive Ionization Energies 354
S.S Electron Affinities and Metallic Character 355
Electron Affinity 355 Metallic Character 356
Chapter in Review 360
Key Terms 360 Key Concepts 360 Key Equations and
Relationships 361 Key Learning Objectives 361
Exercises 361
Problems by Topic 361 Cumulative Problems 363
Challenge Problems 364 Conceptual Problems 364
Questions for Group Work 365 Answers to Conceptual
Connections 365
7.5 Quantum Mechanics and the Atom 307
Solutions to the Schrödinger Equation for the Hydrogen
Atom 307 Atomic Spectroscopy Explained 311
7.6 The Shapes of Atomic Orbitals 313
s Orbitals (/=0) 314 p Orbitals (1=1) 316 d Orbitals
(1=2)317 f Orbitals (/=3) 318 The Phase of
Orbitals 318 The Shapes of Atoms 318
Chapter in Review 319
Key Terms 319 Key Concepts 320 Key Equations and
Relationships 320 Key Learning Objectives 321
Exercises 321
Problems by Topic 321 Cumulative Problems 322
Challenge Problems 323 Conceptual Problems 324
Questions for Group Work 324 Answers to Conceptual
Connections 325
! i Periodic Properties of
the Elements 326
8.1 Nerve Signal Transmission 327
8.2 The Development of the Periodic Table 328
8.3 Electron Configurations: How Electrons
Occupy Orbitals 329
Electron Spin and the Pauli Exclusion Principle 330
Sublevel Energy Splitting in Multielectron Atoms 330
Electron Spatial Distributions and Sublevel Splitting 332
Electron Configurations for Multielectron Atoms 334
8.4 Electron Configurations, Valence Electrons, and the
Periodic Table 337
Orbital Blocks in the Periodic Table 338 Writing an
Electron Configuration for an Element from Its Position in
the Periodic Table 339 The Transition and InnerTransition
Elements 340
8.5 The Explanatory Power of the Quantum-Mechanical
Model 341
8.6 Periodic Trends in the Size of Atoms and Effective
Nuclear Charge 342
Effective Nuclear Charge 344 Atomic Radii and the
Transition Elements 345
8.7 Ions: Electron Configurations, Magnetic Properties,
Ionic Radii, and Ionization Energy 347
Electron Configurations and Magnetic Properties of
Ions 347 Ionic Radii 348 Ionization Energy 351
Chemical Bonding I:
The Lewis Model see
9.1 Bonding Models and AIDS Drugs 368
9.2 Types of Chemical Bonds 368
9.3 Representing Valence Electrons with Dots 370
9.4 Ionic Bonding: Lewis Symbols and
Lattice Energies 371
Ionic Bonding and Electron Transfer 371 Lattice Energy:
The Rest of the Story 372 Trends in Lattice Energies: Ion
Size 373 Trends in Lattice Energies: Ion Charge 373 Ionic
Bonding: Models and Reality 374
9.5 Covalent Bonding: Lewis Structures 375
Single Covalent Bonds 375 Double and Triple Covalent
Bonds 376 Covalent Bonding: Models and Reality 376
9.6 Electronegativity and Bond Polarity 377
Electronegativity 378 Bond Polarity, Dipole Moment, and
Percent Ionic Character 379
9.7 Lewis Structures of Molecular Compounds and
Polyatomic Ions 382
Writing Lewis Structures for Molecular Compounds 382
Writing Lewis Structures for Polyatomic Ions 383
9.8 Resonance and Formal Charge 384
Resonance 384 Formal Charge 386
9.9 Exceptions to the Octet Rule: Odd-Electron Species,
Incomplete Octets, and Expanded Octets 389
Odd-Electron Species 389 Incomplete Octets 389
Expanded Octets 390
Contents 9
10.8 Molecular Orbital Theory: Electron Delocalization 435
Linear Combination of Atomic Orbitals (LCAO) 436
Period Two Homonuclear Diatomic Molecules 439
Chapter in Review 446
Key Terms 446 Key Concepts 446 Key Equations and
Relationships 447 Key Learning Objectives 447
Exercises 447
Problems by Topic 447 Cumulative Problems 450
Challenge Problems 452 Conceptual Problems 452
Questions for Group Work 453 Answers to Conceptual
Connections 453
9.10 Bond Energies and Bond Lengths 391
Bond Energy 392 Using Average Bond Energies to Estimate
Enthalpy Changes for Reactions 393 Bond Lengths 395
9.11 Bonding in Metals: The Electron Sea Model 396
Chapter in Review 398
Key Terms 398 Key Concepts 398 Key Equations and
Relationships 399 Key Learning Objectives 399
Exercises 399
Problems by Topic 399 Cumulative Problems 401
Challenge Problems 402 Conceptual Problems 403
Questions for Group Work 403 Answers to Conceptual
Connections 403
]; Chemical Bonding II:
Molecular Shapes, Valence
Bond Theory, and Molecular
Orbital Theory ^
10.1 Artificial Sweeteners: Fooled by Molecular Shape 405
10.2 VSEPR Theory: The Five Basic Shapes 406
Two Electron Groups: Linear Geometry 407 Three Electron
Groups: Trigonal Planar Geometry 407 Four Electron
Groups: Tetrahedral Geometry 407 Five Electron Groups:
Trigonal Bipyramidal Geometry 408 Six Electron Groups:
Octahedral Geometry 409
10.3 VSEPR Theory: The Effect of Lone Pairs 410
Four Electron Groups with Lone Pairs 410 Five Electron
Groups with Lone Pairs 412 Six Electron Groups with
Lone Pairs 413
10.4 VSEPR Theory: Predicting Molecular Geometries 414
Representing Molecular Geometries on Paper 417
Predicting the Shapes of Larger Molecules 417
10.5 Molecular Shape and Polarity 418
10.6 Valence Bond Theory: Orbital Overlap as a
Chemical Bond 421
10.7 Valence Bond Theory: Hybridization of
Atomic Orbitals 423
$p3 Hybridization 425 sp2 Hybridization and Double
Bonds 426 sp Hybridization and Triple Bonds 430 sp3d
and sp3d2 Hybridization 431 Writing Hybridization and
Bonding Schemes 433
iMl Liquids, Solids, and
Intermolecular Forces 454
11.1 Water, No Gravity 455
11.2 Solids, Liquids, and Gases: A Molecular
Comparison 456
Changes between States 458
11.3 Intermolecular Forces: The Forces That Hold
Condensed States Together 458
Dispersion Force 459 Dipole-Dipole Force 461
Hydrogen Bonding 463 Ion-Dipole Force 465
11.4 Intermolecular Forces in Action: Surface Tension,
Viscosity, and Capillary Action 466
Surface Tension 467 Viscosity 467 Capillary Action 468
11.5 Vaporization and Vapor Pressure 468
The Process of Vaporization 468 The Energetics of
Vaporization 469 Heat of Vaporization 470 Vapor
Pressure and Dynamic Equilibrium 471 Temperature
Dependence of Vapor Pressure and Boiling Point 473 The
Clausius-Clapeyron Equation 474 The Critical Point: The
Transition to an Unusual State of Matter 476
11.6 Sublimation and Fusion 477
Sublimation 477 Fusion 478 Energetics of Melting and
Freezing 478
11.7 Heating Curve for Water 479
11.8 Phase Diagrams 480
The Major Features of a Phase Diagram 480 Regions 480
Lines 481 The Triple Point 481 The Critical Point 481
Navigation within a Phase Diagram 482
10
Contents
12.7 Colligative Properties of Strang Electrolyte
Solutions 533
Strong Electrolytes and Vapor Pressure 534
Chapter in Review 536
Key Terms 536 Key Concepts 536 Key Equations and
Relationships 537 Key Learning Objectives 537
Exercises 538
Problems by Topic 538 Cumulative Problems 540
Challenge Problems 542 Conceptual Problems 542
Questions for Group Work 543 Answers to Conceptual
Connections 543
11.9 Water: An Extraordinary Substance 482
11.10 Crystalline Solids; Unit Cells and Basic Structures 483
Closest-Packed Structures 487
11.11 Crystalline Solids: The Fundamental Types 489
Molecular Solids 490 Ionic Solids 490 Atomic
Solids 491
11.12 Crystalline Solids: Band Theory 493
Chapter in Review 495
Key Terms 495 Key Concepts 495 Key Equations and
Relationships 496 Key Learning Objectives 497
Exercises 497
Problems by Topic 497 Cumulative Problems 501
Challenge Problems 502 Conceptual
Problems 502 Questions for Group Work 503 Answers
to Conceptual Connections 503
i- ..
Solutions 504
12.1 Thirsty Solutions: Why You Should Not Drink
Seawater 505
12.2 Types of Solutions and Solubility 507
Nature’s Tendency toward Mixing: Entropy 507 The Effect
of Intermolecular Forces 508
12.3 Energetics of Solution Formation 511
Aqueous Solutions and Heats of Hydration 512
12.4 Solution Equilibrium and Factors Affecting
Solubility 515
The Temperature Dependence of the Solubility of
Solids 515 Factors Affecting the Solubility of Gases in
Water 516
12.5 Expressing Solution Concentration 518
Molarity 519 Molality 520 Parts by Mass and Parts by
Volume 520 Mole Fraction and Mole Percent 521
12.6 Colligative Properties: Vapor Pressure Lowering,
Freezing Point Depression, Boiling Point Elevation,
and Osmotic Pressure 523
Vapor Pressure Lowering 524 Vapor Pressures of Solutions
Containing a Volatile (Nonelectrolyte) Solute 527 Freezing
Point Depression and Boiling Point Elevation 528
Osmosis 531
: Chemical Kinetics 544
13.1 Catching Lizards 545
13.2 The Rate of a Chemical Reaction 546
13.3 The Rate Law: The Effect of Concentration on
Reaction Rate 549
Determining the Order of a Reaction 551 Reaction Order
for Multiple Reactants 552
13.4 The Integrated Rate Law: The Dependence of
Concentration on Time 555
The Half-Life of a Reaction 559
13.5 The Effect of Temperature on Reaction Rate 562
Arrhenius Plots: Experimental Measurements of
the Frequency Factor and the Activation Energy 564
The Collision Model: A Closer Look at the Frequency
Factor 567
13.6 Reaction Mechanisms 568
Rate Laws for Elementary Steps 568 Rate-Determining
Steps and Overall Reaction Rate Laws 569 Mechanisms
with a Fast Initial Step 570
13.7 Catalysis 572
Homogeneous and Heterogeneous
Catalysis 573 Enzymes: Biological Catalysts 574
Chapter in Review 577
Key Terms 577 Key Concepts 577 Key Equations and
Relationships 578 Key Learning Objectives 578
Contents 11
Finding Equilibrium Concentrations When We Are Given the
Equilibrium Constant and Initial Concentrations or
Pressures 606 Simplifying Approximations in Working
Equilibrium Problems 6io
14.9 Le Chatelier’s Principle: How a System at
Equilibrium Responds to Disturbances 614
The Effect of a Concentration Change on Equilibrium 614
The Effect of a Volume (or Pressure) Change on
Equilibrium 616 The Effect of a Temperature Change on
Equilibrium 617
Chapter in Review 619
Key Terms 619 Key Concepts 620 Key Equations and
Relationships 620 Key Learning Objectives 621
Exercises 578
Problems by Topic 578 Cumulative Problems 583
Challenge Problems 585 Conceptual Problems 586
Questions for Group Work 587 Answers to Conceptual
Connections 587
ill Chemical Equilibrium sss
14.1 Fetal Hemoglobin and Equilibrium 589
14.2 The Concept of Dynamic Equilibrium 591
14.3 The Equilibrium Constant (K) 592
Expressing Equilibrium Constants for Chemical
Reactions 593 The Significance of the Equilibrium
Constant 594 Relationships between the Equilibrium
Constant and the Chemical Equation 595
14.4 Expressing the Equilibrium Constant in Terms
of Pressure 597
Units of K 598
14.5 Heterogeneous Equilibria: Reactions Involving
Solids and Liquids 599
14.6 Calculating the Equilibrium Constant from
Measured Equilibrium Concentrations 600
14.7 The Reaction Quotient: Predicting the Direction
of Change 603
14.8 Finding Equilibrium Concentrations 605
Finding Equilibrium Concentrations When We Are Given the
Equilibrium Constant and All but One of the Equilibrium
Concentrations of the Reactants and Products 605
Exercises 621
Problems by Topic 621 Cumulative Problems 625
Challenge Problems 626 Conceptual Problems 626
Questions for Group Work 627 Answers to Conceptual
Connections 627
Acids and Bases 628
15.1 Heartburn 629
15.2 The Nature of Acids and Bases 630
15.3 Definitions of Acids and Bases 631
The Arrhenius Definition 632 The Bransted-Lowry
Definition 632
15.4 Acid Strength and the Acid Ionization
Constant (Ka) 634
Strong Acids 634 Weak Acids 635 The Acid Ionization
Constant (Ka) 636
15.5 Autoionization of Water and pH 637
The pH Scale: A Way to Quantify Acidity and Basicity 639
pOH and Other p Scales 641
15.6 Finding the [H30+] and pH of Strong and
Weak Acid Solutions 642
Strong Acids 642 Weak Acids 642 Polyprotic
Acids 646 Percent Ionization of a Weak Acid 648
15.7 Base Solutions 650
Strong Bases 650 Weak Bases 650 Finding the [OH-]
and pH of Basic Solutions 652
12 Contents
15.8 The Acid-Base Properties of Ions and Salts 653
Anions as Weak Bases 654 Cations as Weak Acids 657
Classifying Salt Solutions as Acidic, Basic, or Neutral 658
15.9 Acid Strength and Molecular Structure 660
Binary Acids 660 Oxyacids 661
15.10 Lewis Acids and Bases 662
Molecules That Act as Lewis Acids 663 Cations That Act
as Lewis Acids 664
Chapter in Review 665
Key Terms 665 Key Concepts 665 Key Equations and
Relationships 666 Key Learning Objectives 666
Exercises 666
Problems by Topic 666 Cumulative Problems 669
Challenge Problems 670 Conceptual Problems 671
Questions for Group Work 671 Answers to Conceptual
Connections 671
jj Aqueous Ionic Equilibrium m
16.1 The Danger of Antifreeze 673
16.2 Buffers: Solutions That Resist pH Change 674
Calculating the pH of a Buffer Solution 676
The Henderson-Hasselbalch Equation 677 Calculating pH
Changes in a Buffer Solution 680 The Stoichiometry
Calculation 680 The Equilibrium Calculation 681 Buffers
Containing a Base and Its Conjugate Acid 683
16.3 Buffer Effectiveness: Buffer Range and
Buffer Capacity 685
Relative Amounts of Acid and Base 685 Absolute
Concentrations of the Acid and Conjugate
Base 685 Buffer Range 686 Buffer Capacity 687
16.4 Titrations and pH Curves 688
The Titration of a Strong Acid with a Strong Base 689
The Titration of a Weak Acid with a Strong Base 692
The Titration of a Weak Base with a Strong Acid 698
The Titration of a Polyprotic Acid 698 Indicators: pH-
Dependent Colors 699
16.5 Solubility Equilibria and the Solubility
Product Constant 701
Ksp and Molar Solubility 701 Ksp and Relative
Solubility 703 The Effect of a Common Ion on
Solubility 703 The Effect of pH on Solubility 705
16.6 Precipitation 706
16.7 Complex Ion Equilibria 707
Chapter in Review 710
Key Terms 710 Key Concepts 710 Key Equations and
Relationships 7io Key Learning Objectives 711
Exercises 711
Problems by Topic 711 Cumulative Problems 714
Challenge Problems 716 Conceptual Problems 716
Questions for Group Work 717 Answers to Conceptual
Connections 717
Free Energy and
Thermodynamics ?is
17.1 Nature s Heat Tax: You Can’t Win and You
Can’t Break Even 720
17.2 Spontaneous and Nonspontaneous Processes 721
17.3 Entropy and the Second Law of Thermodynamics 722
Entropy 723 The Entropy Change Associated with a
Change in State 728
17.4 Heat Transfer and Changes in the Entropy of the
Surroundings 729
The Temperature Dependence of ASsurr 730 Quantifying
Entropy Changes in the Surroundings 730
17.5 Gibbs Free Energy 732
The Effect of AH, AS, and T on Spontaneity 734
17.6 Entropy Changes in Chemical Reactions:
Calculating AS^n 735
Standard Molar Entropies (S°) and the Third Law of
Thermodynamics 736
17.7 Free Energy Changes in Chemical
Reactions: Calculating AG0™ 740
Calculating Free Energy Changes with
AG^n = AH°nn - TAS°n 740 Calculating AG°n with
Tabulated Values of Free Energies of Formation 741
Calculating AG°„n for a Stepwise Reaction from the
Changes in Free Energy for Each of the Steps 743 Why
Free Energy Is “Free” 744
17.8 Free Energy Changes for Nonstandard States:
The Relationship between AG™ and AG™ 745
The Free Energy Change of a Reaction Under Nonstandard
Conditions 746 Standard Conditions 746 Equilibrium
Conditions 747 Other Nonstandard Conditions 747
17.9 Free Energy and Equilibrium: Relating AG™ to the
Equilibrium Constant (K) 748
Contents 13
Chapter in Review 751
Key Terms 751 Key Concepts 752 Key Equations and
Relationships 752 Key Learning Objectives 753
Exercises 753
Problems by Topic 753 Cumulative Problems 756
Challenge Problems 757 Conceptual Problems 758
Questions for Group Work 758 Answers to Conceptual
Connections 759
Electrochemistry m
Electrochemistry m
18.1 Pulling the Plug on the Power Grid 761
18.2 Balancing Oxidation-Reduction Equations 762
18.3 Voltaic (or Galvanic) Cells: Generating Electricity from
Spontaneous Chemical Reactions 765
Electrochemical Cell Notation 767
18.4 Standard Electrode Potentials 768
Predicting the Spontaneous Direction of an Oxidation-
Reduction Reaction 773 Predicting Whether a Metal Will
Dissolve in Acid 775
18.5 Cell Potential, Free Energy, and
the Equilibrium Constant 775
The Relationship between AG° and E°c^ 776
The Relationship between £^el) and K 777
18.6 Cell Potential and Concentration 779
Concentration Cells 782
18.7 Batteries: Using Chemistry to Generate Electricity 783
Dry-Cell Batteries 783 Lead-Acid Storage Batteries 784
Other Rechargeable Batteries 784 Fuel Cells 785
18.8 Electrolysis: Driving Nonspontaneous Chemical
Reactions with Electricity 786
Stoichiometry of Electrolysis 789
18.9 Corrosion: Undesirable Redox Reactions 790
Preventing Corrosion 792
Chapter in Review 793
Key Terms 793 Key Concepts 793 Key Equations and
Relationships 794 Key Learning Objectives 795
Exercises 795
Problems by Topic 795 Cumulative Problems 798
Challenge Problems 799 Conceptual Problems 800
Questions for Group Work 800 Answers to Conceptual
Connections soi
i Radioactivity and Nuclear
Chemistry 802
19.1 Diagnosing Appendicitis 803
19.2 Types of Radioactivity 804
Alpha (a) Decay 805 Beta (/3) Decay 806 Gamma (7)
Ray Emission 807 Positron Emission 807 Electron
Capture 807
19.3 The Valley of Stability: Predicting the Type of
Radioactivity 809
Magic Numbers 811 Radioactive Decay Series 811
19.4 The Kinetics of Radioactive Decay and
Radiometric Dating 811
The Integrated Rate Law 813 Radiocarbon Dating: Using
Radioactivity to Measure the Age of Fossils and
Artifacts 814 Uranium/Lead Dating 816
19.5 The Discovery of Fission: The Atomic Bomb and
Nuclear Power 817
Nuclear Power: Using Fission to Generate Electricity 819
19.6 Converting Mass to Energy: Mass Defect and
Nuclear Binding Energy 820
Mass Defect 821
19.7 Nuclear Fusion: The Power of the Sun 823
19.8 The Effects of Radiation on Life 824
Acute Radiation Damage 824 Increased Cancer Risk 824
Genetic Defects 824 Measuring Radiation Exposure 824
19.9 Radioactivity in Medicine 826
Diagnosis in Medicine 826 Radiotherapy in Medicine 827
Chapter in Review 828
Key Terms 828 Key Concepts 829 Key Equations and
Relationships 830 Key Learning Objectives 830
Exercises 830
Problems by Topic 830 Cumulative Problems 832
Challenge Problems 832 Conceptual Problems 833
Questions for Group Work 833 Answers to Conceptual
Connections 833
Appendix 1 A-l
Appendix 11 A-7
Appendix III A-17
Appendix IV A-42
Glossary G-l
Credits C-l
Index 1-1
|
| any_adam_object | 1 |
| author | Tro, Nivaldo J. 1963- |
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| discipline | Chemie / Pharmazie |
| edition | Third edition |
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| isbn | 9781292097282 1292097280 9780321971944 |
| language | English |
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| spelling | Tro, Nivaldo J. 1963- Verfasser (DE-588)17399847X aut Principles of chemistry a molecular approach Nivaldo J. Tro, Westmont College Third edition Harlow, Essex Pearson [2016] © 2016 833 Seiten, Seite A1-A46, G1-G15, C1-C2, I1-I33 Seiten Illustrationen, Diagramme (überwiegend farbig) txt rdacontent n rdamedia nc rdacarrier Chemistry, Physical and theoretical Textbooks Chemistry, Physical and theoretical Study and teaching (Higher) Chemie (DE-588)4009816-3 gnd rswk-swf 1\p (DE-588)4123623-3 Lehrbuch gnd-content Chemie (DE-588)4009816-3 s DE-604 Digitalisierung UB Regensburg - ADAM Catalogue Enrichment application/pdf http://bvbr.bib-bvb.de:8991/F?func=service&doc_library=BVB01&local_base=BVB01&doc_number=029085921&sequence=000001&line_number=0001&func_code=DB_RECORDS&service_type=MEDIA Inhaltsverzeichnis 1\p cgwrk 20201028 DE-101 https://d-nb.info/provenance/plan#cgwrk |
| spellingShingle | Tro, Nivaldo J. 1963- Principles of chemistry a molecular approach Chemistry, Physical and theoretical Textbooks Chemistry, Physical and theoretical Study and teaching (Higher) Chemie (DE-588)4009816-3 gnd |
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| title | Principles of chemistry a molecular approach |
| title_auth | Principles of chemistry a molecular approach |
| title_exact_search | Principles of chemistry a molecular approach |
| title_full | Principles of chemistry a molecular approach Nivaldo J. Tro, Westmont College |
| title_fullStr | Principles of chemistry a molecular approach Nivaldo J. Tro, Westmont College |
| title_full_unstemmed | Principles of chemistry a molecular approach Nivaldo J. Tro, Westmont College |
| title_short | Principles of chemistry |
| title_sort | principles of chemistry a molecular approach |
| title_sub | a molecular approach |
| topic | Chemistry, Physical and theoretical Textbooks Chemistry, Physical and theoretical Study and teaching (Higher) Chemie (DE-588)4009816-3 gnd |
| topic_facet | Chemistry, Physical and theoretical Textbooks Chemistry, Physical and theoretical Study and teaching (Higher) Chemie Lehrbuch |
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