The fundamental principles of physics: from atom to molecule
Starting from the fundamental constituents of matter, this book provides a more precise idea of what an atom or a molecule is by using theories which reproduce the experimental behaviour of matter. Aware of the comprehension difficulties that quantum theory can raise in the minds of students, the bo...
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| Main Authors: | , |
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| Format: | Book |
| Language: | English |
| Published: |
Newcastle upon Tyne
Cambridge Scholars Publishing
2022
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| Subjects: | |
| Online Access: | Inhaltsverzeichnis |
| Summary: | Starting from the fundamental constituents of matter, this book provides a more precise idea of what an atom or a molecule is by using theories which reproduce the experimental behaviour of matter. Aware of the comprehension difficulties that quantum theory can raise in the minds of students, the book insists on the importance of the physical principles which underlie it, such as the Coulomb relationship, the particle-wave duality, the notion of indeterminism, presence probability and the virial theorem. |
| Physical Description: | xii, 500 Seiten Illustrationen, Diagramme |
| ISBN: | 9781527585546 |
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| 520 | 3 | |a Starting from the fundamental constituents of matter, this book provides a more precise idea of what an atom or a molecule is by using theories which reproduce the experimental behaviour of matter. Aware of the comprehension difficulties that quantum theory can raise in the minds of students, the book insists on the importance of the physical principles which underlie it, such as the Coulomb relationship, the particle-wave duality, the notion of indeterminism, presence probability and the virial theorem. | |
| 653 | 0 | |a Optics with Atomic, Molecular and Plasma Physics | |
| 653 | 0 | |a Biochemistry / Biophysics | |
| 653 | 0 | |a Physical and Theoretical Chemistry | |
| 700 | 1 | |a Henri-Rousseau, Olivier |d ca. 20./21. Jh. |e Verfasser |0 (DE-588)1276814909 |4 aut | |
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Contents Preface. x Foreword. xi Chapter 1. 1 The Constituents of Matter 1-І. The Macroscopic and Microscopic Domains.1 1. The macroscopic and microscopic ratio: the mole N.2 2. The value of N.2 I-П. Highlighting the Complexity of Atoms. 6 1. Experiment. 6 2. Measuring the electron charge. . 7 3. Measuring the electron mass: the J. J. Thomson experiment. 8 4. Determining the electron q/m ratio. 10 5. The nucleus. 14 I-Ш. Chemical Elements. 26 1. Definitions. 26 2. Experimental determination of the mass of elements. 29 I-IV. Periodic Classification of Elements (Descriptive). 33 1. Description.33 2. Period and number of
electrons.34 3. Radioactivity. 36 I-V. Tutorial for Chapter 1. 43 T-I-1. The Avogadro number. 43 T-I-2. The mass spectrometer. 45 T-I-3. Sub-atomic particles.51 T-I-4. Radioactivity.53 T-I-5. Periodic classification. 58 Chapter II. 60 The Wave-Like and Corpuscular Nature of Light II-L Some Reminders about the Wave-Like Nature of Light 60 1. Vibration wave function Ψ.61 2. Period T of a vibrational movement. 61 3. Frequency v.62
vi Contents 4. Angular frequency ω. 62 5. Wavelength λ. 62 6. Wavenumber υ. 63 7. Light interferences. 63 II -II. The Corpuscular Aspect of Light.72 1. Experiment. 72 2. The photoelectric effect: theoretical explanation. 73 3. Quantitative measurement of thephotoelectric effect. 74 II-IV. Tutorial for Chapter II. 77 T-II-1. The wave-like nature of light. 77 T-II-2. The corpuscular nature of light. 82 Chapter III.86 The Corpuscular and Wave-Like Nature of Matter III-L The Davisson and Germer Experiment. 87 III-II. The Jönsson Experiment (1961). 89 III-ΠΙ. The Möllenstedt Experiment (1955). 90 III-IV. The Meaning of the Square of the Amplitude. 92 III-V. Tutorial for Chapter III. 93
Τ-ΠΙ-1. de Broglie’s wavelength. 93 T-III-2. The photoelectric effect.95 Chapter IV. 97 Evidence of the Quantization of Energy in the Hydrogen Atom IV-I. The Franck-Hertz Experiment. 98 1. Experimental device. 98 2. How the experimental device works in the absence of gas. 99 3. How the experimental device works in the presence of gas. 99 4. Interpretation of the Franck-Hertz experiment.100 IV-II. The Emission Spectrum of Atomic Hydrogen. 102 1. Obtaining an emission spectrum. 102 2. Obtaining an empirical formula. 104 3. Generalization to other series. 106 4. Intuitive interpretation of Balmer’s formula. 109 IV-III. The Absorption Spectrum of Atomic Hydrogen. 112 1. The absorption spectrum. 112 2. Particularity of the absorption spectrum. 112 3. The Boltzmann distribution law. 113 IV-IV. Generalization to Hydrogenic Atoms. 115 IV-V. Tutorial for Chapter
IV. 116 T-IV-1. The Franck-Hertz experiment. 116
The Fundamental Principles of Physics vii T-IV-2. Atomic spectra. 120 Chapter V. 135 The Semi-Classical Model of the Hydrogen Atom V-Լ BOHR’s Model of Hydrogenic Atoms. 135 1. Principles. 137 2. Potential energy.137 3. Kinetic energy.138 4. Orbital angular momentum.138 5. Quantization of the angular momentum. 139 4. Total energy.139 5. Atomic radius. 141 6. Graphical representation. 142 7. The electronic transition hypothesis. 143 V -II. Perfecting BOHR’s Model. 146 V -III. Tutorial for Chapter V. 147 Chapter VI. 154 The Quantum Model of the Hydrogen Atom V I-I. Theoretical Explanation of Energy Quantization: The Potential
Well. 154 1. Comparing the electron in the atom to a stationary wave. 154 1. A wave equation. 157 2. A compact form of the Schrôdinger equation. 159 3 Solving the Schrôdinger equation for a particle in a potential well. 161 4. Heisenberg’s uncertainty principle. 170 5. Eigenvalues and mean values of an operator.172 6. Fluctuation of mean values. 176 VI-II. Schrodinger’s Model of the Hydrogen Atom. 180 1. Comparison between the 1 -D and З-D problem. 180 2. The З-D Schrôdinger equation. 180 3. Spherical polar. 181 4. Schrôdinger. 182 5. Wave fimctions: solutions of the Schrôdinger equation. 186 6. Operator and wave function notation. 190 7. The mean value of an operator. 192 8. Graphical representation of wave functions: the atomic orbitals (AOs). 197 9. The orbital momentum and its relationship with the quantum numbers 1 and
m. 207
viii Contents 10. The 4th quantum number: spin.209 VI-ΠΙ. Extension of the Model to Polyelectronic Atoms.215 1. General principles. 215 2. Electronic structures and periodic classification.221 3. The periodicity of physicochemical properties enlightened by electronic configurations. 224 VI -IV. Tutorial for Chapter VI. 237 T-VI-1. The one-dimensional atomic model. 237 T-VI-2. Applications of the potential well model.240 T-VI-3: Extension to three dimensions: the hydrogen atom and hydrogenic atoms. 245 ChapterVII.252 The Chemical Bond VII-Լ The Chemical Bond According to Lewis. 252 1. The chemical bond: principles.252 2. Lewis’s rule. 253 3. Bonding and non-bonding doublets. 254 4. Exceptions to the Lewis rule. 256 5. Formal charges. 257 6. Failures of the Lewis method. 259
VII-II. The Chemical Bond According to Molecular Orbital (MO) Theory. 260 1. Principles. 262 2. Graphical representations of molecular orbitals. 270 3. Energy level diagrams. 279 4. Interference principles. 280 5. Extension to polyelectronic molecules. 282 6. Molecular orbitals and physical properties of diatomic molecules. 301 7. MOs and heteronuclear diatomic molecules.303 8. Other heteronuclear diatomic molecules.306 9. Properties of diatomic molecules in light of the fundamental principles of physics. 310 10. Qualitative prediction of the evolution of the properties of diatomic molecules. 315 VII-ΠΙ. Theories Dealing with Molecular Geometry. 345 1. The VSEPR method (Valence Shell Electronic Pair Repulsions). 346 2. The theory of hybridization of atomic orbitals. 352
The Fundamental Principles of Physics ix ѴП-ІѴ. Extended Systems and the Hückel Leao Method: Principles. 398 1. The Hamiltonian. 399 2. Energy of state i. 399 3. Molecular state. 399 4. Molecular energy. 400 5. Variational method. 400 6. Applications. 402 VI I-V. Tutorial For Chapter VII. 416 T-VII-1. The Lewis method. 416 T-VII-2. The theory of molecular orbitals for diatomic molecules. 424 T-VII-3. Molecular geometry and the VSEPR method. 429 T-VII-4. Molecular geometry and the hybridization of atomic orbitals. 451 T-VII-5. The hybridization of atomic orbitals and transition metal complexes. 462 T-VII-6. Extended systems. 466 Chapter VIII. 478 Chemical Reactivity and Molecular
Orbitals: Electrocyclic Reactions ѴШ-Լ Electrocyclic Reactions. 479 VIII-II. Woodward-Hoffmann’s Selection Rules. 480 1. Neutral molecules. 480 2. Ionic molecules. 485 Conclusion. 490 Acknowledgements. 492 Index. 493 |
| adam_txt |
Contents Preface. x Foreword. xi Chapter 1. 1 The Constituents of Matter 1-І. The Macroscopic and Microscopic Domains.1 1. The macroscopic and microscopic ratio: the mole N.2 2. The value of N.2 I-П. Highlighting the Complexity of Atoms. 6 1. Experiment. 6 2. Measuring the electron charge. . 7 3. Measuring the electron mass: the J. J. Thomson experiment. 8 4. Determining the electron q/m ratio. 10 5. The nucleus. 14 I-Ш. Chemical Elements. 26 1. Definitions. 26 2. Experimental determination of the mass of elements. 29 I-IV. Periodic Classification of Elements (Descriptive). 33 1. Description.33 2. Period and number of
electrons.34 3. Radioactivity. 36 I-V. Tutorial for Chapter 1. 43 T-I-1. The Avogadro number. 43 T-I-2. The mass spectrometer. 45 T-I-3. Sub-atomic particles.51 T-I-4. Radioactivity.53 T-I-5. Periodic classification. 58 Chapter II. 60 The Wave-Like and Corpuscular Nature of Light II-L Some Reminders about the Wave-Like Nature of Light 60 1. Vibration wave function Ψ.61 2. Period T of a vibrational movement. 61 3. Frequency v.62
vi Contents 4. Angular frequency ω. 62 5. Wavelength λ. 62 6. Wavenumber υ. 63 7. Light interferences. 63 II -II. The Corpuscular Aspect of Light.72 1. Experiment. 72 2. The photoelectric effect: theoretical explanation. 73 3. Quantitative measurement of thephotoelectric effect. 74 II-IV. Tutorial for Chapter II. 77 T-II-1. The wave-like nature of light. 77 T-II-2. The corpuscular nature of light. 82 Chapter III.86 The Corpuscular and Wave-Like Nature of Matter III-L The Davisson and Germer Experiment. 87 III-II. The Jönsson Experiment (1961). 89 III-ΠΙ. The Möllenstedt Experiment (1955). 90 III-IV. The Meaning of the Square of the Amplitude. 92 III-V. Tutorial for Chapter III. 93
Τ-ΠΙ-1. de Broglie’s wavelength. 93 T-III-2. The photoelectric effect.95 Chapter IV. 97 Evidence of the Quantization of Energy in the Hydrogen Atom IV-I. The Franck-Hertz Experiment. 98 1. Experimental device. 98 2. How the experimental device works in the absence of gas. 99 3. How the experimental device works in the presence of gas. 99 4. Interpretation of the Franck-Hertz experiment.100 IV-II. The Emission Spectrum of Atomic Hydrogen. 102 1. Obtaining an emission spectrum. 102 2. Obtaining an empirical formula. 104 3. Generalization to other series. 106 4. Intuitive interpretation of Balmer’s formula. 109 IV-III. The Absorption Spectrum of Atomic Hydrogen. 112 1. The absorption spectrum. 112 2. Particularity of the absorption spectrum. 112 3. The Boltzmann distribution law. 113 IV-IV. Generalization to Hydrogenic Atoms. 115 IV-V. Tutorial for Chapter
IV. 116 T-IV-1. The Franck-Hertz experiment. 116
The Fundamental Principles of Physics vii T-IV-2. Atomic spectra. 120 Chapter V. 135 The Semi-Classical Model of the Hydrogen Atom V-Լ BOHR’s Model of Hydrogenic Atoms. 135 1. Principles. 137 2. Potential energy.137 3. Kinetic energy.138 4. Orbital angular momentum.138 5. Quantization of the angular momentum. 139 4. Total energy.139 5. Atomic radius. 141 6. Graphical representation. 142 7. The electronic transition hypothesis. 143 V -II. Perfecting BOHR’s Model. 146 V -III. Tutorial for Chapter V. 147 Chapter VI. 154 The Quantum Model of the Hydrogen Atom V I-I. Theoretical Explanation of Energy Quantization: The Potential
Well. 154 1. Comparing the electron in the atom to a stationary wave. 154 1. A wave equation. 157 2. A compact form of the Schrôdinger equation. 159 3 Solving the Schrôdinger equation for a particle in a potential well. 161 4. Heisenberg’s uncertainty principle. 170 5. Eigenvalues and mean values of an operator.172 6. Fluctuation of mean values. 176 VI-II. Schrodinger’s Model of the Hydrogen Atom. 180 1. Comparison between the 1 -D and З-D problem. 180 2. The З-D Schrôdinger equation. 180 3. Spherical polar. 181 4. Schrôdinger. 182 5. Wave fimctions: solutions of the Schrôdinger equation. 186 6. Operator and wave function notation. 190 7. The mean value of an operator. 192 8. Graphical representation of wave functions: the atomic orbitals (AOs). 197 9. The orbital momentum and its relationship with the quantum numbers 1 and
m. 207
viii Contents 10. The 4th quantum number: spin.209 VI-ΠΙ. Extension of the Model to Polyelectronic Atoms.215 1. General principles. 215 2. Electronic structures and periodic classification.221 3. The periodicity of physicochemical properties enlightened by electronic configurations. 224 VI -IV. Tutorial for Chapter VI. 237 T-VI-1. The one-dimensional atomic model. 237 T-VI-2. Applications of the potential well model.240 T-VI-3: Extension to three dimensions: the hydrogen atom and hydrogenic atoms. 245 ChapterVII.252 The Chemical Bond VII-Լ The Chemical Bond According to Lewis. 252 1. The chemical bond: principles.252 2. Lewis’s rule. 253 3. Bonding and non-bonding doublets. 254 4. Exceptions to the Lewis rule. 256 5. Formal charges. 257 6. Failures of the Lewis method. 259
VII-II. The Chemical Bond According to Molecular Orbital (MO) Theory. 260 1. Principles. 262 2. Graphical representations of molecular orbitals. 270 3. Energy level diagrams. 279 4. Interference principles. 280 5. Extension to polyelectronic molecules. 282 6. Molecular orbitals and physical properties of diatomic molecules. 301 7. MOs and heteronuclear diatomic molecules.303 8. Other heteronuclear diatomic molecules.306 9. Properties of diatomic molecules in light of the fundamental principles of physics. 310 10. Qualitative prediction of the evolution of the properties of diatomic molecules. 315 VII-ΠΙ. Theories Dealing with Molecular Geometry. 345 1. The VSEPR method (Valence Shell Electronic Pair Repulsions). 346 2. The theory of hybridization of atomic orbitals. 352
The Fundamental Principles of Physics ix ѴП-ІѴ. Extended Systems and the Hückel Leao Method: Principles. 398 1. The Hamiltonian. 399 2. Energy of state i. 399 3. Molecular state. 399 4. Molecular energy. 400 5. Variational method. 400 6. Applications. 402 VI I-V. Tutorial For Chapter VII. 416 T-VII-1. The Lewis method. 416 T-VII-2. The theory of molecular orbitals for diatomic molecules. 424 T-VII-3. Molecular geometry and the VSEPR method. 429 T-VII-4. Molecular geometry and the hybridization of atomic orbitals. 451 T-VII-5. The hybridization of atomic orbitals and transition metal complexes. 462 T-VII-6. Extended systems. 466 Chapter VIII. 478 Chemical Reactivity and Molecular
Orbitals: Electrocyclic Reactions ѴШ-Լ Electrocyclic Reactions. 479 VIII-II. Woodward-Hoffmann’s Selection Rules. 480 1. Neutral molecules. 480 2. Ionic molecules. 485 Conclusion. 490 Acknowledgements. 492 Index. 493 |
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| spelling | Blaise, Paul ca. 20./21. Jh. Verfasser (DE-588)1276814844 aut The fundamental principles of physics from atom to molecule by Paul Blaise and Olivier Henri-Rousseau Newcastle upon Tyne Cambridge Scholars Publishing 2022 xii, 500 Seiten Illustrationen, Diagramme txt rdacontent n rdamedia nc rdacarrier Starting from the fundamental constituents of matter, this book provides a more precise idea of what an atom or a molecule is by using theories which reproduce the experimental behaviour of matter. Aware of the comprehension difficulties that quantum theory can raise in the minds of students, the book insists on the importance of the physical principles which underlie it, such as the Coulomb relationship, the particle-wave duality, the notion of indeterminism, presence probability and the virial theorem. Optics with Atomic, Molecular and Plasma Physics Biochemistry / Biophysics Physical and Theoretical Chemistry Henri-Rousseau, Olivier ca. 20./21. Jh. Verfasser (DE-588)1276814909 aut Digitalisierung UB Bayreuth - ADAM Catalogue Enrichment application/pdf http://bvbr.bib-bvb.de:8991/F?func=service&doc_library=BVB01&local_base=BVB01&doc_number=033955572&sequence=000001&line_number=0001&func_code=DB_RECORDS&service_type=MEDIA Inhaltsverzeichnis |
| spellingShingle | Blaise, Paul ca. 20./21. Jh Henri-Rousseau, Olivier ca. 20./21. Jh The fundamental principles of physics from atom to molecule |
| title | The fundamental principles of physics from atom to molecule |
| title_auth | The fundamental principles of physics from atom to molecule |
| title_exact_search | The fundamental principles of physics from atom to molecule |
| title_exact_search_txtP | The fundamental principles of physics from atom to molecule |
| title_full | The fundamental principles of physics from atom to molecule by Paul Blaise and Olivier Henri-Rousseau |
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| title_full_unstemmed | The fundamental principles of physics from atom to molecule by Paul Blaise and Olivier Henri-Rousseau |
| title_short | The fundamental principles of physics |
| title_sort | the fundamental principles of physics from atom to molecule |
| title_sub | from atom to molecule |
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