Chem 230: Essential Inorganic Chemistry
- Page ID
- 550592
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- Front Matter
- This page introduces the LibreTexts Project, a non-profit initiative that offers free, openly licensed educational resources to enhance accessibility for students and educators. It emphasizes collaborative development and sharing of educational materials to lower textbook costs and improve the educational experience overall.
- 1: Atomic Properties and Periodicity
- This page discusses key concepts in quantum mechanics, focusing on atomic orbitals' shapes, energies, and quantum numbers. It explains their role in determining ground state electron configurations and influences on elemental properties. The organization of the periodic table by characteristics like atomic radius and ionization energy is highlighted, alongside the significance of effective nuclear charge (Zeff) in elucidating periodic trends and exceptions in elemental behavior.
- 2: Bonding Theory Overview
- This page discusses covalent bonding concepts, emphasizing Lewis electron dot diagrams, valence electrons, and their influence on molecular geometry, including lone pairs and multiple bonds. It also addresses metallic bonding, crystal structures of metals and ionic compounds, and the significance of charge and size in ionic bonding. Additionally, key theories like VSEPR and molecular orbital theory are introduced.
- 3: Oxidation and Reduction of Elements
- This page provides an overview of redox reactions, emphasizing the simultaneous processes of oxidation and reduction. It covers balancing these reactions via the ion-electron method and explores electrochemical cells, detailing the roles of anodes and cathodes. Standard reduction potentials, thermodynamics relating to electrical work and free energy, and diagrams like Latimer, Frost, and Pourbaix for summarizing redox properties are introduced.
- 4: Inorganic Acids and Bases
- This page provides an overview of the Brønsted-Lowry acid-base theory, defining acids as \(H^+\) donors and bases as \(H^+\) acceptors, while also introducing conjugate acid-base pairs. It examines trends in different types of acids and metal hydroxide solubility. Moreover, it delves into Lewis acids and bases, highlighting their relationship with Brønsted acids and discussing the acidity of metal ions in water, along with the hard-soft classification of these acids and bases.
- 5: Coordination Chemistry Introduction
- This page covers complex ions and ligands, focusing on their interaction with central metal ions. It classifies ligands as monodentate or chelating, explains coordination number, and introduces Crystal Field Theory (CFT) to analyze color and magnetism in transition-metal complexes. Key topics include crystal field splitting energy, thermodynamics of ligand interactions, stability constants for ligand exchange, and isomerism in complex ions.
- 5.1: Ligands
- 5.2: Electron Configuration of Gas-Phase Metal Ions
- 5.3: Crystal Field Theory, d orbital splitting in presence of ligands
- 5.4: Crystal Field Electron Configuration
- 5.5: Crystal Field Stabilization Energy
- 5.6: Thermodynamic and Structure Consequences of d orbital splitting
- 5.7: Ligand Exchange Reactions and Affinity Determination
- 5.8: Ligand Binding Thermodynamics and the Chelate Effect
- 5.9: Hard and Soft Ligands and Metal Ions
- 5.10: Potential Isomers of Complex Ions
- 6: Molecular Orbital Theory
- This page covers color prediction in coordination complexes through Crystal Field Theory (CFT) and its industrial applications. It explains symmetry operations, molecular shapes, and point group assignments, along with molecular orbital diagrams, particularly highlighting the complexities in BF₃. Additionally, it introduces ligand field theory, differentiating between strong and weak field ligands and discussing the spectrochemical series for ligands and metal ions.
- 6.1: Overview of Colors from Transition Metal Ions
- 6.2: Symmetry and Symmetry Operations
- 6.3: Molecule Shapes (Point Groups)
- 6.4: Point Group Assignment
- 6.5: Overview of Classifying Bonding Orbitals in a Molecule
- 6.6: MO Diagram Construction of CO2
- 6.7: MO Diagram Construction of H2O
- 6.8: MO Diagram Construction of NH3
- 6.9: MO Construction of BF3
- 6.10: Lewis Acid-Base Dative Bond and MO Diagrams
- 6.11: MO Diagram for bonding in [M(NH3)6]n+
- 6.12: MO Diagram for bonding in [M(H2O)6]n+
- 6.13: Spectrochemical Series for Ligands
- 6.14: Spectrochemical Series for Metal ions
- 7: Why is Carbon Monoxide Poisonous?
- This page covers π-acid ligands, especially carbon monoxide, in coordination chemistry, highlighting CO's strong field ligand properties due to π backbonding despite being a poor base. It introduces Ligand Field Theory (LFT) as an advancement of Crystal Field Theory, emphasizing molecular orbital interactions.
- 7.1: Pi-Acid Ligands
- 7.2: [Fe(CO)6]2+ MO Diagram
- 7.3: Revisit Octahedral Metal Ion Electron Configurations
- 7.4: Magnetic Moments for Spin State Determination
- 7.5: LFSE/CFSE Calculations Again
- 7.6: Spectrochemical Series of Ligands (Again)
- 7.7: Exchange Inertness of d3, d4(LS), d5(LS), d6(LS), and d8(SQP)
- 7.8: O2 Reduction, since CO displaces O2
- 7.9: Bonding in Carbonmonoxy-myoglobin [Fe(CO)]2+
- 7.10: Active Site of Cytochrome c Oxidase
- 7.11: Cyanide is also a poison (affinity data)
- 7.12: Cyanide is also a poison (spectrocopic data)
- 8: What Happens "Above The Arrow" in Organic Chemistry
- This page covers metal-π system ligands and their reactivity in comparison to spectator ligands, along with the 18-electron rule for predicting stable organometallic complexes. It also details various organometallic reactions, highlighting the Suzuki-Miyaura coupling as a key metal-catalyzed reaction for creating carbon-carbon bonds crucial for organic synthesis.
- 9: Why is Cisplatin "King of the Chemotherapeutic Drugs?"
- This page explores the Jahn-Teller effect causing geometric distortion in molecular systems, particularly in octahedral and tetrahedral complexes, leading to energy changes. It addresses spin states in coordination compounds, influenced by ligand and crystal field theories, and discusses the trans effect. Additionally, it highlights cisplatin as a significant platinum-based chemotherapy drug, noting its importance and effectiveness in cancer treatment.
- Back Matter
- This page discusses creating glossary entries for a textbook, detailing essential components like words, definitions, images, and resource links. It emphasizes the need for clarity and case sensitivity in definitions, illustrated with a genetics example. The page also suggests using coding functions to improve the glossary's layout and presentation.