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AUCHE 230 - Structure and Bonding (Elizabeth McGinitie)

Chemistry

Tác giả: Elizabeth McGinitie
Nhà xuất bản: University of Alberta - Augustana Faculty
Nguồn: LibreTexts
Giấy phép: CC BY-SA
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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01: Atomic Structure
1.01: The History of the Periodic Table
1.02: Electromagnetic Radiation
1.03: Quantum Theory
1.04: Atomic Spectra
1.05: The Bohr Atom
1.06: Two Ideas Leading to a New Quantum Mechanics
1.07: Wave Mechanics and Quantum Numbers
1.08: Electron Spin- A Fourth Quantum Number
1.09: Orbital Shapes and Energies
1.10: Electron Configurations
1.11: Electron Configurations for Transition Metal Elements
1.12: Magnetic Properties
1.13: Shielding and Effective Nuclear Charge
1.14: Slater's Rules
02: Simple Bonding Theory
2.01: Prelude to Chemical Bonding and Molecular Geometry
2.02: Ionic Bonding
2.03: Covalent Bonding
2.04: Electronegativity
2.05: Lewis Theory- An Overview
2.06: Writing Lewis Structures
2.07: Resonance
2.08: Exceptions to the Octet Rule
2.09: Shapes of Molecules
2.10: Multiple Bonds
2.11: Electronegativity and Atomic Size Effects
03: Molecular Symmetry
3.01: Symmetry Elements and Operations
3.02: Symmetry Elements
3.03: Molecular Point Groups
04: Molecular Orbital (MO) Theory
4.01: Formation of Molecular Orbitals from Atomic Orbitals
4.02: Molecular Orbitals from s Orbitals
4.03: Molecular Orbitals from p Orbitals
4.04: Molecular orbitals from d orbitals
4.05: Nonbonding Orbitals and Other Factors
4.06: Homonuclear Diatomic Molecules
4.07: Molecular Orbitals
4.08: Orbital Mixing
4.09: Diatomic Molecules of the First and Second Periods
4.10: Heteronuclear Diatomic Molecules
4.11: Orbital ionization energies
4.12: Polar bonds
4.13: Ionic Compounds and Molecular Orbitals
05: Acid-Base and Donor-Acceptor Chemistry
5.01: Acid-Base Models as Organizing Concepts
5.02: Arrhenius Concept
5.03: Brnsted-Lowry Concept
5.04: Rules of Thumb for thinking about the relationship between Molecular Structure and Brnsted Acidity and Basicity
5.05: The acid-base behavior of binary element hydrides is determined primarily by the element's electronegativity and secondarily by the element-hydrogen bond strength.
5.06: The Acidity of an Oxoacid is Determined by the Electronegativity and Oxidation State of the Oxoacid's Central Atom
5.07: Lewis Concept and Frontier Orbitals
5.08: The frontier orbital approach considers Lewis acid-base reactions in terms of the donation of electrons from the base's highest occupied orbital into the acid's lowest unoccupied orbital.
5.09: All other things being equal electron withdrawing groups tend to make Lewis acids stronger and bases weaker while electron donating groups tend to make Lewis bases stronger and acids weaker
5.10: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct.
5.11: Hard and Soft Acids and Bases
5.12: Hard-Hard and Soft-Soft preferences may be explained and quantified in terms of electrostatic and covalent and electronic stabilization on the stability of Lewis acid-base adducts
5.13: Quantitative Measures of Hardness Softness and Acid-Base Interactions from a Hard Soft Acid-Base Principle Perspective Involve Orbital Energies and or Apportioning Acid-Base Bonding in Terms of Electrostatic and Covalent Factors
06: Crystalline Solids
6.01: Crystalline and Amorphous Solids
6.02: The Solid State of Matter
6.03: Lattice Structures in Crystalline Solids