1: Intro, Review, and Effective Nuclear Charge
- Page ID
- 360772
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1.3: Simple Bonding Theory
- 1.1: Introduction to Inorganic Chemistry
- Welcome to Inorganic chemistry; The image shown here was created by graphics designer, John Megahan (https://johnmegahan.com/) in consultation with Anne McNeil (https://mcneilgroup.chem.lsa.umich.edu/diversity/)
- 1.2: Atomic Structure
- 1.2.1: Historical Development of Atomic Theory
- 1.2.1.1: The Periodic Table
- 1.2.1.2: Discovery of Subatomic Particles and the Bohr Atom
- 1.2.2: The Schrödinger equation, particle in a box, and atomic wavefunctions
- 1.2.2.1: Particle in a Box
- 1.2.2.2: Quantum Numbers and Atomic Wave Functions
- 1.2.2.3: Aufbau Principle
- 1.2.2.4: Shielding
- 1.2.3: Periodic Properties of Atoms
- 1.2.3.1: Ionization energy
- 1.2.3.2: Electron Affinity
- 1.2.3.3: Covalent and Ionic Radii
- 1.2.3.4: Hard and Soft Acids and Bases
- 1.2.3.4.1: 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
- 1.2.3.4.2: 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
- 1.3: Simple Bonding Theory
- 1.3.1: Lewis Electron-Dot Diagrams
- 1.3.1.1: Resonance
- 1.3.1.2: Breaking the octet rule with higher electron counts (hypervalent atoms)
- 1.3.1.3: Formal Charge
- 1.3.1.4: Lewis fails to predict unusual cases- Boron and Beryllium
- 1.3.2: Valence Shell Electron-Pair Repulsion
- 1.3.2.1: Lone Pair Repulsion
- 1.3.2.2: Multiple Bonds
- 1.3.2.3: Electronegativity and Atomic Size Effects
- 1.3.2.4: Ligand Close Packing
- 1.3.3: Molecular Polarity
- 1.3.4: Hydrogen Bonding
- 1.3.5: Valence Bond Theory
- 1.3.6: Hybrid Atomic Orbitals