<p>Foreword xix</p> <p>Preface xxiii</p> <p>Editors’ Note xxvii</p> <p><b>Part I Fundamental Principles 1</b></p> <p><b>1 The Principle of Wave–Particle Duality: An Overview 3</b></p> <p>1.1 Introduction 3</p> <p>1.2 The Principle of Wave–Particle Duality of Light 4</p> <p>1.2.1 The Photoelectric Effect 4</p> <p>1.2.2 The Compton Effect 7</p> <p>1.2.3 A Note on Units 10</p> <p>1.3 The Principle of Wave–Particle Duality of Matter 11</p> <p>1.3.1 From Frequency Quantization in Classical Waves to Energy Quantization in Matter Waves: The Most Important General Consequence of Wave–Particle Duality of Matter 12</p> <p>1.3.2 The Problem of Atomic Stability under Collisions 13</p> <p>1.3.3 The Problem of Energy Scales: Why Are Atomic Energies on the Order of eV, While Nuclear Energies Are on the Order of MeV? 15</p> <p>1.3.4 The Stability of Atoms and Molecules Against External Electromagnetic Radiation 17</p> <p>1.3.5 The Problem of Length Scales: Why Are Atomic Sizes on the Order of Angstroms, While Nuclear Sizes Are on the Order of Fermis? 19</p> <p>1.3.6 The Stability of Atoms Against Their Own Radiation: Probabilistic Interpretation of Matter Waves 21</p> <p>1.3.7 How Do Atoms Radiate after All? Quantum Jumps from Higher to Lower Energy States and Atomic Spectra 22</p> <p>1.3.8 Quantized Energies and Atomic Spectra: The Case of Hydrogen 25</p> <p>1.3.9 Correct and Incorrect Pictures for the Motion of Electrons in Atoms: Revisiting the Case of Hydrogen 25</p> <p>1.3.10 The Fine Structure Constant and Numerical Calculations in Bohr’s Theory 29</p> <p>1.3.11 Numerical Calculations with Matter Waves: Practical Formulas and Physical Applications 31</p> <p>1.3.12 A Direct Confirmation of the Existence of Matter Waves: The Davisson–Germer Experiment 33</p> <p>1.3.13 The Double-Slit Experiment: Collapse of the Wavefunction Upon Measurement 34</p> <p>1.4 Dimensional Analysis and Quantum Physics 41</p> <p>1.4.1 The Fundamental Theorem and a Simple Application 41</p> <p>1.4.2 Blackbody Radiation Using Dimensional Analysis 44</p> <p>1.4.3 The Hydrogen Atom Using Dimensional Analysis 47</p> <p><b>2 The Schrödinger Equation and Its Statistical Interpretation 53</b></p> <p>2.1 Introduction 53</p> <p>2.2 The Schrödinger Equation 53</p> <p>2.2.1 The Schrödinger Equation for Free Particles 54</p> <p>2.2.2 The Schrödinger Equation in an External Potential 57</p> <p>2.2.3 Mathematical Intermission I: Linear Operators 58</p> <p>2.3 Statistical Interpretation of Quantum Mechanics 60</p> <p>2.3.1 The “Particle–Wave” Contradiction in Classical Mechanics 60</p> <p>2.3.2 Statistical Interpretation 61</p> <p>2.3.3 Why Did We Choose P(x) = |𝜓(x)|</p> <p>2 as the Probability Density? 62</p> <p>2.3.4 Mathematical Intermission II: Basic Statistical Concepts 63</p> <p>2.3.4.1 Mean Value 63</p> <p>2.3.4.2 Standard Deviation (or Uncertainty) 65</p> <p>2.3.5 Position Measurements: Mean Value and Uncertainty 67</p> <p>2.4 Further Development of the Statistical Interpretation: The Mean-Value Formula 71</p> <p>2.4.1 The General Formula for the Mean Value 71</p> <p>2.4.2 The General Formula for Uncertainty 73</p> <p>2.5 Time Evolution of Wavefunctions and Superposition States 77</p> <p>2.5.1 Setting the Stage 77</p> <p>2.5.2 Solving the Schrödinger Equation. Separation of Variables 78</p> <p>2.5.3 The Time-Independent Schrödinger Equation as an Eigenvalue Equation: Zero-Uncertainty States and Superposition States 81</p> <p>2.5.4 Energy Quantization for Confined Motion: A Fundamental General Consequence of Schrödinger’s Equation 85</p> <p>2.5.5 The Role of Measurement in Quantum Mechanics: Collapse of the Wavefunction Upon Measurement 86</p> <p>2.5.6 Measurable Consequences of Time Evolution: Stationary and Nonstationary States 91</p> <p>2.6 Self-Consistency of the Statistical Interpretation and the Mathematical Structure of Quantum Mechanics 95</p> <p>2.6.1 Hermitian Operators 95</p> <p>2.6.2 Conservation of Probability 98</p> <p>2.6.3 Inner Product and Orthogonality 99</p> <p>2.6.4 Matrix Representation of Quantum Mechanical Operators 101</p> <p>2.7 Summary: Quantum Mechanics in a Nutshell 103</p> <p><b>3 The Uncertainty Principle 107</b></p> <p>3.1 Introduction 107</p> <p>3.2 The Position–Momentum Uncertainty Principle 108</p> <p>3.2.1 Mathematical Explanation of the Principle 108</p> <p>3.2.2 Physical Explanation of the Principle 109</p> <p>3.2.3 Quantum Resistance to Confinement. A Fundamental Consequence of the Position– omentum Uncertainty Principle 112</p> <p>3.3 The Time–Energy Uncertainty Principle 114</p> <p>3.4 The Uncertainty Principle in the Classical Limit 118</p> <p>3.5 General Investigation of the Uncertainty Principle 119</p> <p>3.5.1 Compatible and Incompatible Physical Quantities and the Generalized Uncertainty Relation 119</p> <p>3.5.2 Angular Momentum: A Different Kind of Vector 122</p> <p><b>Part II Simple Quantum Systems 127</b></p> <p><b>4 Square Potentials. I: Discrete Spectrum—Bound States 129</b></p> <p>4.1 Introduction 129</p> <p>4.2 Particle in a One-Dimensional Box: The Infinite Potential Well 132</p> <p>4.2.1 Solution of the Schrödinger Equation 132</p> <p>4.2.2 Discussion of the Results 134</p> <p>4.2.2.1 Dimensional Analysis of the Formula En = (ℏ2𝜋2∕2mL2)n2. Do We Need an Exact Solution to Predict the Energy Dependence on ℏ, m, and L? 135</p> <p>4.2.2.2 Dependence of the Ground-State Energy on ℏ, m, and L : The Classical Limit 136</p> <p>4.2.2.3 The Limit of Large Quantum Numbers and Quantum Discontinuities 137</p> <p>4.2.2.4 The Classical Limit of the Position Probability Density 138</p> <p>4.2.2.5 Eigenfunction Features: Mirror Symmetry and the Node Theorem 139</p> <p>4.2.2.6 Numerical Calculations in Practical Units 139</p> <p>4.3 The Square Potential Well 140</p> <p>4.3.1 Solution of the Schrödinger Equation 140</p> <p>4.3.2 Discussion of the Results 143</p> <p>4.3.2.1 Penetration into Classically Forbidden Regions 143</p> <p>4.3.2.2 Penetration in the Classical Limit 144</p> <p>4.3.2.3 The Physics and “Numerics” of the Parameter 𝜆 145</p> <p><b>5 Square Potentials. II: Continuous Spectrum—Scattering States 149</b></p> <p>5.1 Introduction 149</p> <p>5.2 The Square Potential Step: Reflection and Transmission 150</p> <p>5.2.1 Solution of the Schrödinger Equation and Calculation of the Reflection Coefficient 150</p> <p>5.2.2 Discussion of the Results 153</p> <p>5.2.2.1 The Phenomenon of Classically Forbidden Reflection 153</p> <p>5.2.2.2 Transmission Coefficient in the “Classical Limit” of High Energies 154</p> <p>5.2.2.3 The Reflection Coefficient Depends neither on Planck’s Constant nor on the Mass of the Particle: Analysis of a Paradox 154</p> <p>5.2.2.4 An Argument from Dimensional Analysis 155</p> <p>5.3 Rectangular Potential Barrier: Tunneling Effect 156</p> <p>5.3.1 Solution of the Schrödinger Equation 156</p> <p>5.3.2 Discussion of the Results 158</p> <p>5.3.2.1 Crossing a Classically Forbidden Region: The Tunneling Effect 158</p> <p>5.3.2.2 Exponential Sensitivity of the Tunneling Effect to the Energy of the Particle 159</p> <p>5.3.2.3 A Simple Approximate Expression for the Transmission Coefficient 160</p> <p>5.3.2.4 Exponential Sensitivity of the Tunneling Effect to the Mass of the Particle 162</p> <p>5.3.2.5 A Practical Formula for T 163</p> <p><b>6 The Harmonic Oscillator 167</b></p> <p>6.1 Introduction 167</p> <p>6.2 Solution of the Schrödinger Equation 169</p> <p>6.3 Discussion of the Results 177</p> <p>6.3.1 Shape of Wavefunctions. Mirror Symmetry and the Node Theorem 178</p> <p>6.3.2 Shape of Eigenfunctions for Large n: The Classical Limit 179</p> <p>6.3.3 The Extreme Anticlassical Limit of the Ground State 180</p> <p>6.3.4 Penetration into Classically Forbidden Regions: What Fraction of Its “Lifetime” Does the Particle “Spend” in the Classically Forbidden Region? 181</p> <p>6.3.5 A Quantum Oscillator Never Rests: Zero-Point Energy 182</p> <p>6.3.6 Equidistant Eigenvalues and Emission of Radiation from a Quantum Harmonic Oscillator 184</p> <p>6.4 A Plausible Question: Can We Use the Polynomial Method to Solve Potentials Other than the Harmonic Oscillator? 187</p> <p><b>7 The Polynomial Method: Systematic Theory and Applications 191</b></p> <p>7.1 Introduction: The Power-Series Method 191</p> <p>7.2 Sufficient Conditions for the Existence of Polynomial Solutions: Bidimensional Equations 194</p> <p>7.3 The Polynomial Method in Action: Exact Solution of the Kratzer and Morse Potentials 197</p> <p>7.4 Mathematical Afterword 202</p> <p><b>8 The Hydrogen Atom. I: Spherically Symmetric Solutions 207</b></p> <p>8.1 Introduction 207</p> <p>8.2 Solving the Schrödinger Equation for the Spherically Symmetric Eigenfunctions 209</p> <p>8.2.1 A Final Comment: The System of Atomic Units 216</p> <p>8.3 Discussion of the Results 217</p> <p>8.3.1 Checking the Classical Limit ℏ → 0 or m → ∞ for the Ground State of the Hydrogen Atom 217</p> <p>8.3.2 Energy Quantization and Atomic Stability 217</p> <p>8.3.3 The Size of the Atom and the Uncertainty Principle: The Mystery of Atomic Stability from Another Perspective 218</p> <p>8.3.4 Atomic Incompressibility and the Uncertainty Principle 221</p> <p>8.3.5 More on the Ground State of the Atom. Mean and Most Probable Distance of the Electron from the Nucleus 221</p> <p>8.3.6 Revisiting the Notion of “Atomic Radius”: How Probable is It to Find the Electron Within the “Volume” that the Atom Supposedly Occupies? 222</p> <p>8.3.7 An Apparent Paradox: After All, Where Is It Most Likely to Find the Electron? Near the Nucleus or One Bohr Radius Away from It? 223</p> <p>8.3.8 What Fraction of Its Time Does the Electron Spend in the Classically Forbidden Region of the Atom? 223</p> <p>8.3.9 Is the Bohr Theory for the Hydrogen Atom Really Wrong? Comparison with Quantum Mechanics 225</p> <p>8.4 What Is the Electron Doing in the Hydrogen Atom after All? A First Discussion on the Basic Questions of Quantum Mechanics 226</p> <p><b>9 The Hydrogen Atom. II: Solutions with Angular Dependence 231</b></p> <p>9.1 Introduction 231</p> <p>9.2 The Schrödinger Equation in an Arbitrary Central Potential: Separation of Variables 232</p> <p>9.2.1 Separation of Radial from Angular Variables 232</p> <p>9.2.2 The Radial Schrödinger Equation: Physical Interpretation of the Centrifugal Term and Connection to the Angular Equation 235</p> <p>9.2.3 Solution of the Angular Equation: Eigenvalues and Eigenfunctions of Angular Momentum 237</p> <p>9.2.3.1 Solving the Equation for Φ 238</p> <p>9.2.3.2 Solving the Equation for Θ 239</p> <p>9.2.4 Summary of Results for an Arbitrary Central Potential 243</p> <p>9.3 The Hydrogen Atom 246</p> <p>9.3.1 Solution of the Radial Equation for the Coulomb Potential 246</p> <p>9.3.2 Explicit Construction of the First Few Eigenfunctions 249</p> <p>9.3.2.1 n = 1 : The Ground State 250</p> <p>9.3.2.2 n = 2 : The First Excited States 250</p> <p>9.3.3 Discussion of the Results 254</p> <p>9.3.3.1 The Energy-Level Diagram 254</p> <p>9.3.3.2 Degeneracy of the Energy Spectrum for a Coulomb Potential: Rotational and Accidental Degeneracy 255</p> <p>9.3.3.3 Removal of Rotational and Hydrogenic Degeneracy 257</p> <p>9.3.3.4 The Ground State is Always Nondegenerate and Has the Full Symmetry of the Problem 257</p> <p>9.3.3.5 Spectroscopic Notation for Atomic States 258</p> <p>9.3.3.6 The “Concept” of the Orbital: s and p Orbitals 258</p> <p>9.3.3.7 Quantum Angular Momentum: A Rather Strange Vector 261</p> <p>9.3.3.8 Allowed and Forbidden Transitions in the Hydrogen Atom: Conservation of Angular Momentum and Selection Rules 263</p> <p><b>10 Atoms in a Magnetic Field and the Emergence of Spin 267</b></p> <p>10.1 Introduction 267</p> <p>10.2 Atomic Electrons as Microscopic Magnets: Magnetic Moment and Angular Momentum 270</p> <p>10.3 The Zeeman Effect and the Evidence for the Existence of Spin 274</p> <p>10.4 The Stern–Gerlach Experiment: Unequivocal Experimental Confirmation of the Existence of Spin 278</p> <p>10.4.1 Preliminary Investigation: A Plausible Theoretical Description of Spin 278</p> <p>10.4.2 The Experiment and Its Results 280</p> <p>10.5 What is Spin? 284</p> <p>10.5.1 Spin is No Self-Rotation 284</p> <p>10.5.2 How is Spin Described Quantum Mechanically? 285</p> <p>10.5.3 What Spin Really Is 291</p> <p>10.6 Time Evolution of Spin in a Magnetic Field 292</p> <p>10.7 Total Angular Momentum of Atoms: Addition of Angular Momenta 295</p> <p>10.7.1 The Eigenvalues 295</p> <p>10.7.2 The Eigenfunctions 300</p> <p><b>11 Identical Particles and the Pauli Principle 305</b></p> <p>11.1 Introduction 305</p> <p>11.2 The Principle of Indistinguishability of Identical Particles in Quantum Mechanics 305</p> <p>11.3 Indistinguishability of Identical Particles and the Pauli Principle 306</p> <p>11.4 The Role of Spin: Complete Formulation of the Pauli Principle 307</p> <p>11.5 The Pauli Exclusion Principle 310</p> <p>11.6 Which Particles Are Fermions and Which Are Bosons 314</p> <p>11.7 Exchange Degeneracy: The Problem and Its Solution 317</p> <p><b>Part III Quantum Mechanics in Action: The Structure of Matter 321</b></p> <p><b>12 Atoms: The Periodic Table of the Elements 323</b></p> <p>12.1 Introduction 323</p> <p>12.2 Arrangement of Energy Levels in Many-Electron Atoms: The Screening Effect 324</p> <p>12.3 Quantum Mechanical Explanation of the Periodic Table: The “Small Periodic Table” 327</p> <p>12.3.1 Populating the Energy Levels: The Shell Model 328</p> <p>12.3.2 An Interesting “Detail”: The Pauli Principle and Atomic Magnetism 329</p> <p>12.3.3 Quantum Mechanical Explanation of Valence and Directionality of Chemical Bonds 331</p> <p>12.3.4 Quantum Mechanical Explanation of Chemical Periodicity: The Third Row of the Periodic Table 332</p> <p>12.3.5 Ionization Energy and Its Role in Chemical Behavior 334</p> <p>12.3.6 Examples 338</p> <p>12.4 Approximate Calculations in Atoms: Perturbation Theory and the Variational Method 341</p> <p>12.4.1 Perturbation Theory 342</p> <p>12.4.2 Variational Method 346</p> <p><b>13 Molecules. I: Elementary Theory of the Chemical Bond 351</b></p> <p>13.1 Introduction 351</p> <p>13.2 The Double-Well Model of Chemical Bonding 352</p> <p>13.2.1 The Symmetric Double Well 352</p> <p>13.2.2 The Asymmetric Double Well 356</p> <p>13.3 Examples of Simple Molecules 360</p> <p>13.3.1 The Hydrogen Molecule H2 360</p> <p>13.3.2 The Helium “Molecule” He2 363</p> <p>13.3.3 The Lithium Molecule Li2 364</p> <p>13.3.4 The Oxygen Molecule O2 364</p> <p>13.3.5 The Nitrogen Molecule N2 366</p> <p>13.3.6 The Water Molecule H2O 367</p> <p>13.3.7 Hydrogen Bonds: From the Water Molecule to Biomolecules 370</p> <p>13.3.8 The Ammonia Molecule NH3 373</p> <p>13.4 Molecular Spectra 377</p> <p>13.4.1 Rotational Spectrum 378</p> <p>13.4.2 Vibrational Spectrum 382</p> <p>13.4.3 The Vibrational–Rotational Spectrum 385</p> <p><b>14 Molecules. II: The Chemistry of Carbon 393</b></p> <p>14.1 Introduction 393</p> <p>14.2 Hybridization: The First Basic Deviation from the Elementary Theory of the Chemical Bond 393</p> <p>14.2.1 The CH4 Molecule According to the Elementary Theory: An Erroneous Prediction 393</p> <p>14.2.2 Hybridized Orbitals and the CH4 Molecule 395</p> <p>14.2.3 Total and Partial Hybridization 401</p> <p>14.2.4 The Need for Partial Hybridization: The Molecules C2H4, C2H2, and C2H6 404</p> <p>14.2.5 Application of Hybridization Theory to Conjugated Hydrocarbons 408</p> <p>14.2.6 Energy Balance of Hybridization and Application to Inorganic Molecules 409</p> <p>14.3 Delocalization: The Second Basic Deviation from the Elementary Theory of the Chemical Bond 414</p> <p>14.3.1 A Closer Look at the Benzene Molecule 414</p> <p>14.3.2 An Elementary Theory of Delocalization: The Free-Electron Model 417</p> <p>14.3.3 LCAO Theory for Conjugated Hydrocarbons. I: Cyclic Chains 418</p> <p>14.3.4 LCAO Theory for Conjugated Hydrocarbons. II: Linear Chains 424</p> <p>14.3.5 Delocalization on Carbon Chains: General Remarks 427</p> <p>14.3.6 Delocalization in Two-dimensional Arrays of p Orbitals: Graphene and Fullerenes 429</p> <p><b>15 Solids: Conductors, Semiconductors, Insulators 439</b></p> <p>15.1 Introduction 439</p> <p>15.2 Periodicity and Band Structure 439</p> <p>15.3 Band Structure and the “Mystery of Conductivity.” Conductors, Semiconductors, Insulators 441</p> <p>15.3.1 Failure of the Classical Theory 441</p> <p>15.3.2 The Quantum Explanation 443</p> <p>15.4 Crystal Momentum, Effective Mass, and Electron Mobility 447</p> <p>15.5 Fermi Energy and Density of States 453</p> <p>15.5.1 Fermi Energy in the Free-Electron Model 453</p> <p>15.5.2 Density of States in the Free-Electron Model 457</p> <p>15.5.3 Discussion of the Results: Sharing of Available Space by the Particles of a Fermi Gas 460</p> <p>15.5.4 A Classic Application: The “Anomaly” of the Electronic Specific Heat of Metals 463</p> <p><b>16 Matter and Light: The Interaction of Atoms with Electromagnetic Radiation 469</b></p> <p>16.1 Introduction 469</p> <p>16.2 The Four Fundamental Processes: Resonance, Scattering, Ionization, and Spontaneous Emission 471</p> <p>16.3 Quantitative Description of the Fundamental Processes: Transition Rate, Effective Cross Section, Mean Free Path 473</p> <p>16.3.1 Transition Rate: The Fundamental Concept 473</p> <p>16.3.2 Effective Cross Section and Mean Free Path 475</p> <p>16.3.3 Scattering Cross Section: An Instructive Example 476</p> <p>16.4 Matter and Light in Resonance. I: Theory 478</p> <p>16.4.1 Calculation of the Effective Cross Section: Fermi’s Rule 478</p> <p>16.4.2 Discussion of the Result: Order-of-Magnitude Estimates and Selection Rules 481</p> <p>16.4.3 Selection Rules: Allowed and Forbidden Transitions 483</p> <p>16.5 Matter and Light in Resonance. II: The Laser 487</p> <p>16.5.1 The Operation Principle: Population Inversion and the Threshold Condition 487</p> <p>16.5.2 Main Properties of Laser Light 491</p> <p>16.5.2.1 Phase Coherence 491</p> <p>16.5.2.2 Directionality 491</p> <p>16.5.2.3 Intensity 491</p> <p>16.5.2.4 Monochromaticity 492</p> <p>16.6 Spontaneous Emission 494</p> <p>16.7 Theory of Time-dependent Perturbations: Fermi’s Rule 499</p> <p>16.7.1 Approximate Calculation of Transition Probabilities Pn→m(t) for an Arbitrary “Transient” Perturbation V(t) 499</p> <p>16.7.2 The Atom Under the Influence of a Sinusoidal Perturbation: Fermi’s Rule for Resonance Transitions 503</p> <p>16.8 The Light Itself: Polarized Photons and Their Quantum Mechanical Description 511</p> <p>16.8.1 States of Linear and Circular Polarization for Photons 511</p> <p>16.8.2 Linear and Circular Polarizers 512</p> <p>16.8.3 Quantum Mechanical Description of Polarized Photons 513</p> <p>Online Supplement</p> <p>1 The Principle of Wave–Particle Duality: An Overview</p> <p>OS1.1 Review Quiz</p> <p>OS1.1 Determining Planck’s Constant from Everyday Observations</p> <p>2 The Schrödinger Equation and Its Statistical Interpretation</p> <p>OS2.1 Review Quiz</p> <p>OS2.2 Further Study of Hermitian Operators: The Concept of the Adjoint Operator</p> <p>OS2.3 Local Conservation of Probability: The Probability Current</p> <p>3 The Uncertainty Principle</p> <p>OS3.1 Review Quiz</p> <p>OS3.2 Commutator Algebra: Calculational Techniques</p> <p>OS3.3 The Generalized Uncertainty Principle</p> <p>OS3.4 Ehrenfest’s Theorem: Time Evolution of Mean Values and the Classical Limit</p> <p>4 Square Potentials. I: Discrete Spectrum—Bound States</p> <p>OS4.1 Review Quiz</p> <p>OS4.2 Square Well: A More Elegant Graphical Solution for Its Eigenvalues</p> <p>OS4.3 Deep and Shallow Wells: Approximate Analytic Expressions for Their Eigenvalues</p> <p>5 Square Potentials. II: Continuous Spectrum—Scattering States</p> <p>OS5.1 Review Quiz</p> <p>OS5.2 Quantum Mechanical Theory of Alpha Decay</p> <p>6 The Harmonic Oscillator</p> <p>OS6.1 Review Quiz</p> <p>OS6.2 Algebraic Solution of the Harmonic Oscillator: Creation and Annihilation Operators</p> <p>7 The Polynomial Method: Systematic Theory and Applications</p> <p>OS7.1 Review Quiz</p> <p>OS7.2 An Elementary Method for Discovering Exactly Solvable Potentials</p> <p>OS7.3 Classic Examples of Exactly Solvable Potentials: A Comprehensive List</p> <p>8 The Hydrogen Atom. I: Spherically Symmetric Solutions</p> <p>OS8.1 Review Quiz</p> <p>9 The Hydrogen Atom. II: Solutions with Angular Dependence</p> <p>OS9.1 Review Quiz</p> <p>OS9.2 Conservation of Angular Momentum in Central Potentials, and Its Consequences</p> <p>OS9.3 Solving the Associated Legendre Equation on Our Own</p> <p>10 Atoms in a Magnetic Field and the Emergence of Spin</p> <p>OS10.1 Review Quiz</p> <p>OS10.2 Algebraic Theory of Angular Momentum and Spin</p> <p>11 Identical Particles and the Pauli Principle</p> <p>OS11.1 Review Quiz</p> <p>OS11.2 Dirac’s Formalism: A Brief Introduction</p> <p>12 Atoms: The Periodic Table of the Elements</p> <p>OS12.1 Review Quiz</p> <p>OS12.2 Systematic Perturbation Theory: Application to the Stark Effect and Atomic Polarizability</p> <p>13 Molecules. I: Elementary Theory of the Chemical Bond</p> <p>OS13.1 Review Quiz</p> <p>14 Molecules. II: The Chemistry of Carbon</p> <p>OS14.1 Review Quiz</p> <p>OS14.2 The LCAO Method and Matrix Mechanics</p> <p>OS14.3 Extension of the LCAO Method for Nonzero Overlap</p> <p>15 Solids: Conductors, Semiconductors, Insulators</p> <p>OS15.1 Review Quiz</p> <p>OS15.2 Floquet’s Theorem: Mathematical Study of the Band Structure for an Arbitrary Periodic Potential V(x)</p> <p>OS15.3 Compressibility of Condensed Matter: The Bulk Modulus</p> <p>OS15.4 The Pauli Principle and Gravitational Collapse: The Chandrasekhar Limit</p> <p>16 Matter and Light: The Interaction of Atoms with Electromagnetic Radiation</p> <p>OS16.1 Review Quiz</p> <p>OS16.2 Resonance Transitions Beyond Fermi’s Rule: Rabi Oscillations</p> <p>OS16.3 Resonance Transitions at Radio Frequencies: Nuclear Magnetic Resonance (NMR)</p> <p>Appendix 519</p> <p>Bibliography 523</p> <p>Index 527</p>