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Title: Map: Inorganic Chemistry (LibreTexts)
Webpages: 384
Applicable Restrictions: Noncommercial
All licenses found:
- Undeclared: 68% (261 pages)
- CC BY-NC 4.0: 12.2% (47 pages)
- CC BY-SA 4.0: 10.2% (39 pages)
- CC BY 4.0: 4.2% (16 pages)
- CC BY-NC-SA 4.0: 2.9% (11 pages)
- CC BY-NC 3.0: 2.1% (8 pages)
- CC BY-NC-SA 3.0: 0.5% (2 pages)
By Page
- Map: Inorganic Chemistry (LibreTexts) — Undeclared
- Front Matter — Undeclared
- 1: Introduction to Inorganic Chemistry — Undeclared
- 2: Atomic Structure — Undeclared
- 3: Simple Bonding Theory — Undeclared
- 4: Symmetry and Group Theory — Undeclared
- 5: Molecular Orbitals — CC BY-SA 4.0
- 6: Acid-Base and Donor-Acceptor Chemistry — Undeclared
- 6.1: Acid-Base Models as Organizing Concepts — Undeclared
- 6.2: Arrhenius Concept — Undeclared
- 6.3: Brønsted-Lowry Concept — Undeclared
- 6.3.1: Brønsted-Lowry Concept — CC BY 4.0
- 6.3.2: Rules of Thumb for thinking about the relationship between Molecular Structure and Brønsted Acidity and Basicity* — Undeclared
- 6.3.3: The acid-base behavior of binary element hydrides is determined primarily by the element's electronegativity and secondarily by the element-hydrogen bond strength.* — Undeclared
- 6.3.4: Brønsted-Lowry Superacids and the Hammett Acidity Function — Undeclared
- 6.3.5: Thermodynamics of Solution-Phase Brønsted Acidity and Basicity — CC BY-NC 4.0
- 6.3.6: Thermodynamics of Gas Phase Brønsted Acidity and Basicity — CC BY-NC 4.0
- 6.3.7: The Acidity of an Oxoacid is Determined by the Electronegativity and Oxidation State of the Oxoacid's Central Atom* — CC BY-NC-SA 3.0
- 6.3.8: High Charge-to-Size Ratio Metal Ions Act as Brønsted Acids in Water — CC BY-NC-SA 4.0
- 6.3.9: The Solvent System Acid Base Concept — CC BY-NC 4.0
- 6.3.10: Acid-Base Chemistry in Amphoteric Solvents and the Solvent Leveling Effect — CC BY-NC 4.0
- 6.3.11: Non-nucleophilic Brønsted-Lowry Superbases — CC BY-NC 4.0
- 6.4: Lewis Concept and Frontier Orbitals — CC BY-NC 4.0
- 6.4.1: 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. — Undeclared
- 6.4.2: 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 — Undeclared
- 6.4.3: The electronic spectra of charge transfer complexes illustrate the impact of frontier orbital interactions on the electronic structure of Lewis-Acid base adducts — CC BY-NC 4.0
- 6.4.4: 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. — Undeclared
- 6.4.5: 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. — Undeclared
- 6.4.6: 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 — Undeclared
- 6.4.7: Bulky groups weaken the strength of Lewis acids and bases because they introduce steric strain into the resulting acid-base adduct. — Undeclared
- 6.4.8: Frustrated Lewis pair chemistry uses Lewis acid and base sites within a molecule that are sterically restricted from forming an adduct with each other. — CC BY-NC 4.0
- 6.5: Intermolecular Forces — Undeclared
- 6.6: Hard and Soft Acids and Bases — Undeclared
- 6.6.1: 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 — CC BY-NC 4.0
- 6.6.2: 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 — CC BY-NC 4.0
- 6.7: Problems — Undeclared
- 7: The Crystalline Solid State — Undeclared
- 7.1: Molecular Orbitals and Band Structure — CC BY-SA 4.0
- 7.1.1: Prelude to Electronic Properties of Materials - Superconductors and Semiconductors — CC BY-SA 4.0
- 7.1.2: Metal-Insulator Transitions — CC BY-SA 4.0
- 7.1.3: Periodic Trends- Metals, Semiconductors, and Insulators — CC BY-SA 4.0
- 7.1.4: Semiconductors- Band Gaps, Colors, Conductivity and Doping — CC BY-SA 4.0
- 7.1.5: Semiconductor p-n Junctions — CC BY-SA 4.0
- 7.1.6: Diodes, LEDs and Solar Cells — CC BY-SA 4.0
- 7.1.7: Amorphous Semiconductors — CC BY-SA 4.0
- 7.1.8: Discussion Questions — CC BY-SA 4.0
- 7.1.9: Problems — CC BY-SA 4.0
- 7.1.10: References — CC BY-SA 4.0
- 7.2: Formulas and Structures of Solids — Undeclared
- 7.3: Superconductivity — Undeclared
- 7.4: Bonding in Ionic Crystals — Undeclared
- 7.5: Imperfections in Solids — Undeclared
- 7.6: Silicates — Undeclared
- 7.7: Thermodynamics of Ionic Crystal Formation — Undeclared
- 7.P: Problems — Undeclared
- 7.1: Molecular Orbitals and Band Structure — CC BY-SA 4.0
- 8: Chemistry of the Main Group Elements — Undeclared
- 8.1: General Trends in Main Group Chemistry — Undeclared
- 8.1.1: The Periodic Table is an Organizing Concept in Main Group Chemistry — Undeclared
- 8.1.1.1: The metal-nonmetal-metalloid distinction and the metal-nonmetal "line" are useful for thinking about trends in elements' physical properties — Undeclared
- 8.1.1.2: There are qualitative differences in the chemistry of the elements in the first two rows and those in the rest of the periodic table — Undeclared
- 8.1.2: Electronegativity increases and radius decreases towards the upper left of the periodic table, with electron withdrawing substituents, and with oxidation state — Undeclared
- 8.1.3: Ionization energy roughly increases towards the upper left of the periodic table but is also influenced by orbital energy and pairing energy effects — Undeclared
- 8.1.4: As may be seen from considering element's redox diagrams, main group elements (aside from the noble gases) generally are more oxidizing towards the upper left of the periodic table and more reducing towards the lower right of the periodic table — Undeclared
- 8.1.4.1: Latimer Diagrams summarize elements' redox properties on a single line — CC BY 4.0
- 8.1.4.2: Frost Diagrams show how stable element's redox states are relative to the free element — Undeclared
- 8.1.4.3: Pourbaix Diagrams are Redox Phase Diagrams that Summarize the most stable form of an element at a given pH and solution potential — Undeclared
- 8.1.1: The Periodic Table is an Organizing Concept in Main Group Chemistry — Undeclared
- 8.2: What are the main group elements and why should anyone care about them? — Undeclared
- 8.3: Group 1, The Alkali Metals — Undeclared
- 8.4: Hydrogen — Undeclared
- 8.5: Group 2, The Alkaline Earth Metals — Undeclared
- 8.6: Group 13 (and a note on the post-transition metals) — Undeclared
- 8.7: Group 14 — Undeclared
- 8.7.1: The Group 14 Elements and the many Allotropes of Carbon — Undeclared
- 8.7.2: Inorganic Compounds of the Group 14 Elements — Undeclared
- 8.7.3: Chemistry of Carbon (Z=6) — Undeclared
- 8.7.4: Chemistry of Silicon (Z=14) — Undeclared
- 8.7.5: Chemistry of Germanium (Z=32) — Undeclared
- 8.7.6: Chemistry of Tin (Z=50) — Undeclared
- 8.7.7: Chemistry of Lead (Z=82) — Undeclared
- 8.8: Group 15 — Undeclared
- 8.9: The Nitrogen Family — Undeclared
- 8.9.1: General Properties and Reactions — Undeclared
- 8.9.2: Chemistry of Nitrogen (Z=7) — Undeclared
- 8.9.3: Chemistry of Phosphorus (Z=15) — Undeclared
- 8.9.4: Chemistry of Arsenic (Z=33) — Undeclared
- 8.9.5: Chemistry of Antimony (Z=51) — Undeclared
- 8.9.6: Chemistry of Bismuth (Z=83) — Undeclared
- 8.9.7: Chemistry of Moscovium (Z=115) — Undeclared
- 8.10: Group 16 — Undeclared
- 8.11: The Oxygen Family (The Chalcogens) — Undeclared
- 8.11.1: General Properties and Reactions — Undeclared
- 8.11.2: Chemistry of Oxygen (Z=8) — Undeclared
- 8.11.3: Chemistry of Sulfur (Z=16) — Undeclared
- 8.11.4: Chemistry of Selenium (Z=34) — Undeclared
- 8.11.5: Chemistry of Tellurium (Z=52) — Undeclared
- 8.11.6: Chemistry of Polonium (Z=84) — Undeclared
- 8.11.7: Chemistry of Livermorium (Z=116) — Undeclared
- 8.12: Group 17 (The Halogens) — Undeclared
- 8.13: The Halogens — Undeclared
- 8.13.1: Physical Properties of the Halogens — Undeclared
- 8.13.2: Chemical Properties of the Halogens — Undeclared
- 8.13.2.1: Halide Ions as Reducing Agents — Undeclared
- 8.13.2.2: Halogens as Oxidizing Agents — Undeclared
- 8.13.2.3: Interhalogens — Undeclared
- 8.13.2.4: More Reactions of Halogens — Undeclared
- 8.13.2.5: Oxidizing Ability of the Group 17 Elements — Undeclared
- 8.13.2.6: Testing for Halide Ions — Undeclared
- 8.13.2.7: The Acidity of the Hydrogen Halides — Undeclared
- 8.13.3: Chemistry of Fluorine (Z=9) — Undeclared
- 8.13.4: Chemistry of Chlorine (Z=17) — Undeclared
- 8.13.5: Chemistry of Bromine (Z=35) — Undeclared
- 8.13.6: Chemistry of Iodine (Z=53) — Undeclared
- 8.13.7: Chemistry of Astatine (Z=85) — Undeclared
- 8.14: The Noble Gases — Undeclared
- 8.14.1: History, usage, properties, and distribution of the elements — Undeclared
- 8.14.2: Properties of Nobel Gases — Undeclared
- 8.14.3: Chemistry of the Group 18 (Noble Gas) Elements — Undeclared
- 8.14.4: Reactions of Nobel Gases — Undeclared
- 8.14.5: Chemistry of Helium (Z=2) — Undeclared
- 8.14.6: Chemistry of Neon (Z=10) — Undeclared
- 8.14.7: Chemistry of Argon (Z=18) — Undeclared
- 8.14.8: Chemistry of Krypton (Z=36) — Undeclared
- 8.14.9: Chemistry of Radon (Z=86) — Undeclared
- 8.14.10: Chemistry of Xenon (Z=54) — Undeclared
- 8.P: Problems — Undeclared
- 8.1: General Trends in Main Group Chemistry — Undeclared
- 9: Coordination Chemistry I - Structure and Isomers — CC BY 4.0
- 10: Coordination Chemistry II - Bonding — CC BY-NC 4.0
- 10.1: Evidence for Electronic Structures — CC BY-NC 4.0
- 10.2: Bonding Theories — CC BY-NC 4.0
- 10.3: Ligand Field Theory — CC BY-NC 4.0
- 10.4: Angular Overlap — CC BY-NC 4.0
- 10.4.1: Sigma Bonding in the Angular Overlap Model — CC BY-NC 4.0
- 10.4.2: Pi Acceptors in the Angular Overlap Model — CC BY-NC 4.0
- 10.4.3: Pi Donors in the Angular Overlap Model — CC BY-NC 4.0
- 10.4.4: The Spectrochemical Series — CC BY-NC 4.0
- 10.4.5: The Magnitude of Parameters eσ, eπ and Δ — CC BY-NC 4.0
- 10.4.6: The Magnetochemical Series — CC BY-NC 4.0
- 10.5: The Jahn-Teller Effect — CC BY-NC 4.0
- 10.6: Four- and Six-Coordinate Preferences — CC BY-NC 4.0
- 10.7: Other Shapes — CC BY-NC 4.0
- 10.P: Problems — CC BY-NC 4.0
- 11: Coordination Chemistry III - Electronic Spectra — Undeclared
- 11.1: Absorption of Light — Undeclared
- 11.2: Quantum Numbers of Multielectron Atoms — CC BY 4.0
- 11.3: Electronic Spectra of Coordination Compounds — Undeclared
- 11.3.1: Selection Rules — Undeclared
- 11.3.2: Correlation Diagrams — Undeclared
- 11.3.3: Tanabe-Sugano Diagrams — Undeclared
- 11.3.4: Symmetry labels for split terms — Undeclared
- 11.3.5: Applications of Tanabe-Sugano Diagrams — Undeclared
- 11.3.6: Tetrahedral Complexes — Undeclared
- 11.3.7: Charge-Transfer Spectra — Undeclared
- 11.3.8: Applications of Charge-Transfer — Undeclared
- 12: Coordination Chemistry IV - Reactions and Mechanisms — Undeclared
- 12.1: Introduction to Reactions of Metal Complexes — CC BY-NC 3.0
- 12.2: Substitutions Reactions — Undeclared
- 12.3: Kinetics Hint at the Reaction Mechanism — CC BY-SA 4.0
- 12.3.1: Rate Law for Dissociative Mechanisms — CC BY-SA 4.0
- 12.3.2: Rate Laws for Interchange Mechanisms — CC BY-SA 4.0
- 12.3.3: Rate Law for Associative Mechanisms — CC BY-NC 3.0
- 12.3.4: Preassociation Complexes — CC BY-NC 3.0
- 12.3.5: Activation Parameters — CC BY-NC 3.0
- 12.3.6: Some Reasons for Differing Mechanisms — CC BY-NC 3.0
- 12.4: Experimental Evidence in Octahedral Substitutions — Undeclared
- 12.5: Stereochemistry of Octahedral Reactions — Undeclared
- 12.6: Substitutions in Square Planar Complexes — Undeclared
- 12.7: The Trans Effect — CC BY-NC 3.0
- 12.8: Redox Mechanisms — Undeclared
- 12.9: Reactions of Coordinated Ligands — Undeclared
- 13: Organometallic Chemistry — Undeclared
- 13.1: Introduction to Organometallic Chemistry — Undeclared
- 13.2: Nomenclature, Ligands, and Classification — Undeclared
- 13.3: Electron Counting in Organometallic Complexes — Undeclared
- 13.4: Survey of Organometallic Ligands — Undeclared
- 13.5: Bonding between Metal Atoms and Organic Pi Systems — Undeclared
- 13.6: Metal-Carbon Bonds — Undeclared
- 13.7: Characterization of Organometallic Complexes — CC BY-NC-SA 4.0
- 14: Organometallic Reactions and Catalysis — Undeclared
- 15: Parallels between Main Group and Organometallic Chemistry — Undeclared
- 16: Appendix — Undeclared
- Back Matter — Undeclared