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Inorganic Chemistry

This is the textbook for Inorganic and Advanced Inorganic Chemistry classes for the fall semester of 2022.

Chemistry

Tác giả: Hass et al.
Nhà xuất bản: St. Mary's College
Nguồn: LibreTexts
Ngôn ngữ: EN
Danh mục: Khoa học cơ bản

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01: Introduction to Inorganic Chemistry
1.01: What is Inorganic Chemistry
1.02: Inorganic vs Organic Chemistry
1.03: History of Inorganic Chemistry
1.04: Perspectives
1.05: Practice problems
02: Atomic Structure
2.01: Historical Development of Atomic Theory
2.1.01: The Periodic Table
2.1.02: Discovery of Subatomic Particles and the Bohr Atom
2.02: The Schrodinger equation particle in a box and atomic wavefunctions
2.2.01: Particle in a Box
2.2.02: Quantum Numbers and Atomic Wave Functions
2.2.03: Aufbau Principle
2.2.04: Shielding
2.03: Periodic Properties of Atoms
2.3.01: Ionization energy
2.3.02: Electron Affinity
2.3.03: Covalent and Ionic Radii
2.04: Problems (do we want this here)
03: Simple Bonding Theory
3.01: Lewis Electron-Dot Diagrams
3.1.01: Resonance
3.1.02: Breaking the octet rule with higher electron counts (hypervalent atoms)
3.1.03: Formal Charge
3.1.04: Lewis Fails to Predict Unusual Cases - Boron and Beryllium
3.02: Valence Shell Electron-Pair Repulsion
3.2.01: Lone Pair Repulsion
3.2.02: Multiple Bonds
3.2.03: Electronegativity and Atomic Size Effects
3.2.04: Ligand Close Packing
3.03: Molecular Polarity
3.04: Hydrogen Bonding
3.05: Problems (do we want this here)
04: Acid-Base and Donor-Acceptor Chemistry
4.01: Acid-Base Models as Organizing Concepts
4.02: Arrhenius Concept
4.03: Brnsted-Lowry Concept
4.3.01: Brnsted-Lowry Concept
4.3.02: Rules of Thumb for thinking about the relationship between Molecular Structure and Brnsted Acidity and Basicity
4.3.03: The acid-base behavior of binary element hydrides is determined primarily by the element's electronegativity and secondarily by the element-hydrogen bond strength.
4.3.04: Brnsted-Lowry Superacids and the Hammett Acidity Function
4.3.05: Thermodynamics of Solution-Phase Brnsted Acidity and Basicity
4.3.06: Thermodynamics of Gas Phase Brnsted Acidity and Basicity
4.3.07: The Acidity of an Oxoacid is Determined by the Electronegativity and Oxidation State of the Oxoacid's Central Atom
4.3.08: High Charge-to-Size Ratio Metal Ions Act as Brnsted Acids in Water
4.3.09: The Solvent System Acid Base Concept
4.3.10: Acid-Base Chemistry in Amphoteric Solvents and the Solvent Leveling Effect
4.3.11: Non-nucleophilic Brnsted-Lowry Superbases
4.04: Lewis Concept and Frontier Orbitals
4.4.01: 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.
4.4.02: 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
4.4.03: The electronic spectra of charge transfer complexes illustrate the impact of frontier orbital interactions on the electronic structure of Lewis-Acid base adducts.
4.4.04: Substances' solution phase Lewis Basicity towards a given acid may be estimated using the enthalphy change for dissociation of its adduct with a reference acid of similar hardness.
4.4.05: In the boron triflouride affinity scale the enthalphy change on formation of an adduct between the base and boron triflouride is taken as a measure of Lewis basicity.
4.4.06: Lewis base strength may also be estimated by measuring structural or energy changes on formation of a Lewis acid-base complex as illustrated by efforts to spectroscopically assess of the strengths of halogen bonds
4.4.07: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct.
4.4.08: Frustrated Lewis pair chemistry uses Lewis acid and base sites within a molecule that are sterically restricted from forming an adduct with each other.
4.05: Intermolecular Forces
4.5.01: Host-Guest Chemistry and - stacking interactions
4.5.02: Hydrogen bonds may be considered as a special type of Lewis acid-base interaction in which a Lewis acid hydrogen ion is shared between Lewis bases
4.06: Hard and Soft Acids and Bases
4.6.01: 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
4.6.02: 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
4.07: Problems
05: Redox Stability and Redox Reactions
5.01: Prelude to Redox Stability and Redox Reactions
5.02: Balancing Redox Reactions
5.03: Electrochemical Potentials
5.04: Latimer and Frost Diagrams
5.05: Redox Reactions with Coupled Equilibria
5.06: Pourbaix Diagrams
5.07: Discussion Questions
5.08: Problems
5.09: References
06: The Crystalline Solid State
6.01: Molecular Orbitals and Band Structure
6.1.01: Prelude to Electronic Properties of Materials - Superconductors and Semiconductors
6.1.02: Metal-Insulator Transitions
6.1.03: Periodic Trends- Metals Semiconductors and Insulators
6.1.04: Semiconductors- Band Gaps Colors Conductivity and Doping
6.1.05: Semiconductor p-n Junctions
6.1.06: Diodes LEDs and Solar Cells
6.1.07: Amorphous Semiconductors
6.1.08: Discussion Questions
6.1.09: Problems
6.1.10: References
6.02: Formulas and Structures of Solids
6.2.01: The Solid State of Matter
6.2.02: Lattice Structures in Crystalline Solids
6.03: Superconductivity
6.3.01: Superconductors
6.04: Bonding in Ionic Crystals
6.05: Imperfections in Solids
6.5.01: Imperfections
6.06: Silicates
6.6.01: Silicon
6.07: Thermodynamics of Ionic Crystal Formation
6.7.01: Lattice Energy
6.7.02: Lattice Energy - The Born-Haber cycle
6.7.03: Lattice Enthalpies and Born Haber Cycles
6.7.04: The Born-Lande' equation
6.08: Problems
07: Symmetry and Group Theory
7.01: Symmetry Elements and Operations
7.02: Point Groups
7.2.01: Groups of Low and High Symmetry
7.2.02: Other Groups
7.03: Properties and Representations of Groups
7.3.01: Matrices
7.3.02: Representations of Point Groups
7.3.03: Character Tables
7.04: Examples and Applications of Symmetry
7.4.01: Chirality
7.4.02: Molecular Vibrations
7.05: Problems (under construction)
08: Molecular Orbitals
8.01: Formation of Molecular Orbitals from Atomic Orbitals
8.1.01: Molecular Orbitals from s Orbitals
8.1.02: Molecular Orbitals from p Orbitals
8.1.03: Molecular orbitals from d orbitals
8.1.04: Nonbonding Orbitals and Other Factors
8.02: Homonuclear Diatomic Molecules
8.2.01: Molecular Orbitals
8.2.02: Orbital Mixing
8.2.03: Diatomic Molecules of the First and Second Periods
8.2.04: Photoelectron Spectroscopy
8.03: Heteronuclear Diatomic Molecules
8.3.01: Polar bonds
8.3.02: Ionic Compounds and Molecular Orbitals
8.04: Larger (Polyatomic) Molecules
8.4.01: Bifluoride anion
8.4.02: Carbon Dioxide
8.4.03: HO
8.4.04: NH
8.4.05: CO (Revisted with Projection Operators)
8.4.06: BF
8.05: Problems
09: Coordination Chemistry I - Structure and Isomers
9.01: Prelude to Coordination Chemistry I - Structure and Isomers
9.02: History
9.03: Nomenclature and Ligands
9.04: Isomerism
9.05: Coordination Numbers and Structures
9.06: Coordination Frameworks
9.07: Problems
10: Coordination Chemistry II - Bonding
10.01: Evidence for Electronic Structures
10.1.01: Thermodynamic Data
10.1.02: Magnetic Susceptibility
10.1.03: Electronic Spectra
10.1.04: Coordination Number and Molecular Shapes
10.02: Bonding Theories
10.2.01: Crystal Field Theory
10.03: Ligand Field Theory
10.3.01: Ligand Field Theory - Molecular Orbitals for an Octahedral Complex
10.3.02: Orbital Splitting and Electron Spin
10.3.03: Ligand Field Stabilization Energy
10.3.04: Tetrahedral Complexes
10.3.05: Square-Planar Complexes
10.04: Angular Overlap
10.4.01: Sigma Bonding in the Angular Overlap Model
10.4.02: Pi Acceptors in the Angular Overlap Model
10.4.03: Pi Donors in the Angular Overlap Model
10.4.04: The Spectrochemical Series
10.4.05: The Magnitude of Parameters e e and
10.4.06: The Magnetochemical Series
10.05: The Jahn-Teller Effect
10.06: Four- and Six-Coordinate Preferences
10.07: Other Shapes
10.08: Problems