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Electrons, atoms, and molecules in inorganic chemistry : a worked examples approach /
"Electrons, Atoms, and Molecules in Inorganic Chemistry: A Worked Examples Approach builds from fundamental units into molecules, to provide the reader with a full understanding of inorganic chemistry concepts through worked examples and full color illustrations. The book uniquely discusses fai...
| Clasificación: | Libro Electrónico |
|---|---|
| Autores principales: | , |
| Formato: | Electrónico eBook |
| Idioma: | Inglés |
| Publicado: |
London :
Academic Press,
[2017]
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| Temas: | |
| Acceso en línea: | Texto completo |
Tabla de Contenidos:
- Front Cover; Electrons, Atoms, and Molecules in Inorganic Chemistry: A Worked Examples Approach; Copyright; Dedication; Contents; Preface; Chapter 1: Particle Wave Duality; 1.1. Cathode and Anode Rays; 1.2. Charge of the Electron; 1.3. Mass of Electron and Proton; 1.4. Rutherford's Atomic Model; 1.5. Quantum of Energy; 1.6. Hydrogen Atom Line-Emission Spectra; Electrons in Atoms Exist Only in Very Specific Energy States; 1.7. Bohr's Quantum Theory of the Hydrogen Atom; 1.8. The Bohr-Sommerfeld Model; 1.9. The Corpuscular Nature of Electrons, Photons, and Particles of Very Small Mass.
- 1.10. Relativity Theory: Mass and Energy, Momentum, and Wavelength Interdependence; 1.11. The Corpuscular Nature of Electromagnetic Waves; The Photoelectric Effect; The Compton Effect; 1.12. de Broglie's Considerations; 1.13. Werner Heisenberg's Uncertainty Principle, or the Principle of Indeterminacy; 1.14. The Probability of Finding an Electron and the Wave Function; 1.15. Atomic and Subatomic Particles; Elementary Particles; Suggestions for Further Reading; Chapter 2: Electrons in Atoms; 2.1. The Wave Function (the Schr�odinger Equation); 2.2. Properties of the wave function.
- 2.3. Schr�odinger Equation of the Hydrogen Atom; 2.4. Transformation of the Schr�odinger Equation From Cartesians to Spherical Polar Coordinates; 2.5. The Angular Equation; 2.6. The Phi-Equation; 2.7. The [theta]-Equation; 2.8. The Radial Equation; 2.9. The Final Solution for the Full Wave Function, [psi]nlm(R, [theta], [phi]); 2.10. The Orthonormal Properties of the Real Wave Functions; 2.11. The Quantum Numbers: n, l, and ml; The Principle Quantum Number, n; The Quantum Numbers l and Angular Momentum; The Angular Momentum Quantum Numbers, l and m; Picture and Represent Precisely ml Vectors of p- and d-Orbitals.
- 2.12. The Spin Quantum Number, s; 2.13. The Boundary Surface of s-Orbital; 2.14. The Boundary Surface of p-Orbitals; 2.15. The Boundary Surface of d-Orbitals; 2.16. Calculating the Most Probable Radius; 2.17. Calculating the Mean Radius of an Orbital; 2.18. The Structure of Many-Electron Atoms; 2.19. The Pauli Exclusion Principle; 2.20. Slater Determinant; 2.21. Penetration and Shielding; 2.22. The Building-Up Principle; 2.23. Term Structure for Polyelectron Atoms; 2.24. Term Wave Functions and Single Electron Wave Functions; 2.25. Spin-Orbital Coupling.
- 2.26. Spin-Orbital Coupling in External Magnetic Field; Suggestions for Further Reading; Chapter 3: Chemical Bonding; 3.1. Electronegativity and Electropositivity; 3.2. Electronegativity and Electropositivity Trends; 3.3. Molecular and Nonmolecular Compounds; 3.4. Types of Bonds; 3.5. Metallic Bonding and General Properties of Metals; Conductivity and Mobility of Electrons; Luster and Free Electron Irradiation; Malleability, Cohesive Force, Number of Valence Electrons; Theories of Bonding in Metals; Free Electron Theory; Bond Lengths; Crystal Structures of Metals (Metallic Structures).