24: Chemistry of Coordination Chemistry
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1
Chapter 1: Introduction: Matter and Measurement
1.1: The Study of Chemistry
1.2: Classification of Matter
1.3: Properties of Matter
1.4: Units of Measurement
1.5: Uncertainty in Measurement
1.6: Dimensional Analysis
1.E: Matter and Measurement (Exercises)
1.S: Matter and Measurement (Summary)
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Chapter 2: Atoms, Molecules, and Ions
2.1: The Atomic Theory of Matter
2.2: The Discovery of Atomic Structure
2.3: The Modern View of Atomic Structure
2.4: Atomic Mass
2.5: The Periodic Table
2.6: Molecules and Molecular Compounds
2.7: Ions and Ionic Compounds
2.8: Naming Inorganic Compounds
2.9: Some Simple Organic Compounds
2.E: Atoms, Molecules, and Ions (Exercises)
2.S: Atoms, Molecules, and Ions (Summary)
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Chapter 3: Stoichiometry: Chemical Formulas and Equations
3.1: Chemical Equations
3.2: Some Simple Patterns of Chemical Reactivity
3.3: Formula Masses
3.4: Avogadro's Number and the Mole
3.5: Empirical Formulas from Analysis
3.6: Quantitative Information from Balanced Equations
3.7: Limiting Reactants
3.E: Stoichiometry (Exercises)
3.S: Stoichiometry (Summary)
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Chapter 4: Reactions in Aqueous Solution
4.1: General Properties of Aqueous Solutions
4.2: Precipitation Reactions
4.3: Acid-Base Reactions
4.4: Oxidation-Reduction Reactions
4.5: Concentration of Solutions
4.6: Solution Stoichiometry and Chemical Analysis
4.E: Reactions in Aqueous Solution (Exercises)
4.S: Reactions in Aqueous Solution (Summary)
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Chapter 5: Thermochemistry
5.1: The Nature of Energy
5.2: The First Law of Thermodynamics
5.3: Enthalpy
5.4: Enthalpy of Reaction
5.5: Calorimetry
5.6: Hess's Law
5.7: Enthalpies of Formation
5.8: Foods and Fuels
5.E: Thermochemistry (Exercises)
5.S: Thermochemistry (Summary)
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Chapter 6: Electronic Structure of Atoms
6.1: The Wave Nature of Light
6.2: Quantized Energy and Photons
6.3: Line Spectra and the Bohr Model
6.4: The Wave Behavior of Matter
6.5: Quantum Mechanics and Atomic Orbitals
6.6: 3D Representation of Orbitals
6.7: Many-Electron Atoms
6.8: Electron Configurations
6.9: Electron Configurations and the Periodic Table
6.E: Electronic Structure of Atoms (Exercises)
6.S: Electronic Structure of Atoms (Summary)
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Chapter 7: Periodic Properties of the Elements
7.1: Development of the Periodic Table
7.2: Effective Nuclear Charge
7.3: Sizes of Atoms and Ions
7.4: Ionization Energy
7.5: Electron Affinities
7.6: Metals, Nonmetals, and Metalloids
7.7: Group Trends for the Active Metals
7.8: Group Trends for Selected Nonmetals
7.E: Periodic Properties of the Elements (Exercises)
7.S: Periodic Properties of the Elements (Summary)
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Chapter 8: Basic Concepts of Chemical Bonding
8.1: Chemical Bonds, Lewis Symbols, and the Octet Rule
8.2: Ionic Bonding
8.3: Covalent Bonding
8.4: Bond Polarity and Electronegativity
8.5: Drawing Lewis Structures
8.6: Resonance Structures
8.7: Exceptions to the Octet Rule
8.8: Strength of Covalent Bonds
8.E: Basic Concepts of Chemical Bonding (Exercises)
8.S: Basic Concepts of Chemical Bonding (Summary)
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Chapter 9: Molecular Geometry and Bonding Theories
9.1: Molecular Shapes
9.2: The VSEPR Model
9.3: Molecular Shape and Molecular Polarity
9.4: Covalent Bonding and Orbital Overlap
9.5: Hybrid Orbitals
9.6: Multiple Bonds
9.7: Molecular Orbitals
9.8: Second-Row Diatomic Molecules
9.E: Exercises
9.S: Molecular Geometry and Bonding Theories (Summary)
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Chapter 10: Gases
10.1: Characteristics of Gases
10.2: Pressure
10.3: The Gas Laws
10.4: The Ideal Gas Equation
10.5: Further Applications of the Ideal-Gas Equations
10.6: Gas Mixtures and Partial Pressures
10.7: Kinetic-Molecular Theory
10.8: Molecular Effusion and Diffusion
10.9: Real Gases - Deviations from Ideal Behavior
10.E: Exercises
10.S: Gases (Summary)
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Chapter 11: Liquids and Intermolecular Forces
11.1: A Molecular Comparison of Gases, Liquids, and Solids
11.2: Intermolecular Forces
11.3: Some Properties of Liquids
11.4: Phase Changes
11.5: Vapor Pressure
11.6: Phase Diagrams
11.7: Structure of Solids
11.8: Bonding in Solids
11.E: Liquids and Intermolecular Forces (Exercises)
11.S: Liquids and Intermolecular Forces (Summary)
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Chapter 12: Solids and Modern Materials
12.1: Classes of Materials
12.2: Materials for Structure
12.3: Materials for Medicine
12.4: Materials for Electronics
12.5: Materials for Optics
12.6: Materials for Nanotechnology
12.E: Solids and Modern Materials (Exercises)
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Chapter 13: Properties of Solutions
13.1: The Solution Process
13.2: Saturated Solutions and Solubility
13.3: Factors Affecting Solubility
13.4: Ways of Expressing Concentration
13.5: Colligative Properties
13.6: Colloids
13.E: Properties of Solutions (Exercises)
13.S: Properties of Solutions (Summary)
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Chapter 14: Chemical Kinetics
14.1: Factors that Affect Reaction Rates
14.2: Reaction Rates
14.3: Concentration and Rates (Differential Rate Laws)
14.4: The Change of Concentration with Time (Integrated Rate Laws)
14.5: Temperature and Rate
14.6: Reaction Mechanisms
14.7: Catalysis
14.E: Exercises
14.S: Chemical Kinetics (Summary)
• 15
Chapter 15: Chemical Equilibrium
15.1: The Concept of Equilibrium
15.2: The Equilibrium Constant
15.3: Interpreting & Working with Equilibrium Constants
15.4: Heterogeneous Equilibria
15.5: Calculating Equilibrium Constants
15.6: Applications of Equilibrium Constants
15.7: Le Châtelier's Principle
15.E: Exercises
15.S: Chemical Equilibrium (Summary)
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Chapter 16: Acid–Base Equilibria
16.1: Acids and Bases: A Brief Review
16.2: Brønsted–Lowry Acids and Bases
16.3: The Autoionization of Water
16.4: The pH Scale
16.5: Strong Acids and Bases
16.6: Weak Acids
16.7: Weak Bases
16.8: Relationship Between KaKa and KbKb
16.9: Acid-Base Properties of Salt Solutions
16.10: Acid-Base Behavior and Chemical Structure
16.11: Lewis Acids and Bases
16.E: Acid–Base Equilibria (Exercises)
16.S: Acid–Base Equilibria (Summary)
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Chapter 17: Additional Aspects of Aqueous Equilibria
17.1: The Common-Ion Effect
17.2: Buffered Solutions
17.3: Acid-Base Titrations
17.4: Solubility Equilibria
17.5: Factors that Affect Solubility
17.6: Precipitation and Separation of Ions
17.7: Qualitative Analysis for Metallic Elements
17.E: Additional Aspects of Aqueous Equilibria (Exercises)
17.S: Additional Aspects of Aqueous Equilibria (Summary)
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Chapter 18: Chemistry of the Environment
18.1: Earth's Atmosphere
18.2: Outer Regions of the Atmosphere
18.3: Ozone in the Upper Atmostphere
18.4: Chemistry of the Troposphere
18.5: The World Ocean
18.6: Fresh Water
18.7: Green Chemistry
18.E: Chemistry of the Environment (Exercises)
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Chapter 19: Chemical Thermodynamics
19.1: Spontaneous Processes
19.2: Entropy and the Second Law of Thermodynamics
19.3: The Molecular Interpretation of Entropy
19.4: Entropy Changes in Chemical Reactions
19.5: Gibbs Free Energy
19.6: Free Energy and Temperature
19.7: Free Energy and the Equilibrium Constant
19.E: Chemical Thermodynamics (Exercises)
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Chapter 20: Electrochemistry
20.1: Oxidation States & Redox Reactions
20.2: Balanced Oxidation-Reduction Equations
20.3: Voltaic Cells
20.4: Cell Potential Under Standard Conditions
20.5: Gibbs Energy and Redox Reactions
20.6: Cell Potential Under Nonstandard Conditions
20.7: Batteries and Fuel Cells
20.8: Corrosion
20.9: Electrolysis
20.E: Electrochemistry (Exercises)
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Chapter 21: Nuclear Chemistry
21.1: Radioactivity
21.2: Patterns of Nuclear Stability
21.3: Nuclear Transmutations
21.4: Rates of Radioactive Decay
21.6: Energy Changes in Nuclear Reactions
21.7: Nuclear Fission
21.8: Nuclear Fusion
21.9: Biological Effects of Radiation
21.E: Exercises
21.S: Nuclear Chemistry (Summary)
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Chapter 22: Chemistry of the Nonmetals
22.1: General Concepts: Periodic Trends and Reactions
22.2: Hydrogen
22.3: Group 18: Nobel Gases
22.4: Group 17: The Halogens
22.5: Oxygen
22.6: The Other Group 16 Elements: S, Se, Te, and Po
22.7: Nitrogen
22.8: The Other Group 15 Elements: P, AS, Sb, and Bi
22.9: Carbon
22.10: The Other Group 14 Elements: Si, Ge, Sn, and Pb
22.11: Boron
22.E: Chemistry of the Nonmetals (Exercises)
22.S: Chemistry of the Nonmetals (Summary)
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Chapter 23: Metals and Metallurgy
23.1: Occurance and Distribution of Metals
23.2: Pyrometallurgy
23.3: Hydrometallurgy
23.4: Electrometallurgy
23.5: Metallic Bonding
23.6: Alloys
23.7: Transition Metals
23.8: Chemistry of Selected Transition Metals
23.E: Metals and Metallurgy (Exercises)
• 24
Chapter 24: Chemistry of Coordination Chemistry
24.1: Metal Complexes
24.2: Ligands with more than one Donor Atom
24.3: Nomenclature of Coordination Chemistry
24.4: Isomerization
24.5: Color and Magnetism
24.6: Crystal Field Theory
24.E: Chemistry of Coordination Chemistry (Exercises)
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Chapter 25: Chemistry of Life: Organic and Biological Chemistry
25.1: General Characteristics of Organic Molecules
25.2: Introduction to Hydrocarbons
25.3: Alkanes
25.4: Unsaturated Hydrocarbons
25.5: Functional Groups
25.6: Compounds with a Carbonyl Group
25.7: Chirality in Organic Chemistry
25.8: Introduction to Biochemistry
25.9: Proteins
25.10: Carbohydrates
25.11: Nucleic Acids
25.E: Organic and Biological Chemistry (Exercises)
25.S: Organic and Biological Chemistry (Summary)
• Homework
1.E: Matter and Measurement (Exercises)
2.E: Atoms, Molecules, and Ions (Exercises)
3.E: Stoichiometry (Exercises)
4.E: Aqueous Reactions (Exercises)
5.E: Thermochemistry (Exercises)
6.E: Electronic Structure (Exercises)
7.E: Periodic Trends (Exercises)
8.E: Chemical Bonding Basics (Exercises)
9.E: Bonding Theories (Exercises)
10.E: Gases (Exercises)
11.E: Liquids and Intermolecular Forces (Exercises)
12.E. Solids and Modern Materials (Exercises)
13.E: Properties of Solutions (Exercises)
14.E: Kinetics (Exercises)
15.E: Chemical Equilibrium (Exercises)
16.E: Acid–Base Equilibria (Exercises)
17.E: Additional Aspects of Aqueous Equilibria (Exercises)
18.E: Chemistry of the Environment (Exercises)
19.E: Chemical Thermodynamics (Exercises)
20.E: Electrochemistry (Exercises)
21.E: Nuclear Chemistry (Exercises)
22.E: Chemistry of the Nonmetals (Exercises)
23.E: Metals and Metallurgy (Exercises)
24.E: Chemistry of Coordination Chemistry (Exercises)
25.E: Organic and Biological Chemistry (Exercises)
Transition metals are defined as those elements that have (or readily form) partially filled d orbitals. These include the d -block (groups 3–11) and f-block element elements. The variety of properties exhibited by transition metals is due to their complex valence shells. Unlike most main group metals where one oxidation state is normally observed, the valence shell structure of transition metals means that they usually occur in several different stable oxidation states. In addition, electron transitions in these elements can correspond with absorption of photons in the visible electromagnetic spectrum, leading to colored compounds. Because of these behaviors, transition metals exhibit a rich and fascinating chemistry.
24.1: Metal ComplexesA complex ion has a metal ion at its center with a number of other molecules or ions surrounding it. These can be considered to be attached to the central ion by coordinate (dative covalent) bonds (in some cases, the bonding is actually more complicated than that. The molecules or ions surrounding the central metal ion are called ligands. Simple ligands include water, ammonia and chloride ions. 24.2: Ligands with more than one Donor AtomLigands can be further characterized as monodentate, bidentate, tridentate etc. where the concept of teeth (dent) is introduced. Monodentate ligands bind through only one donor atom. Monodentate means "one-toothed." The halides, phosphines, ammonia and amines seen previously are monodentate ligands. Bidentate ligands bind through two donor sites. Bidentate means "two-toothed." It can bind to a metal via two donor atoms at once. 24.3: Nomenclature of Coordination ChemistryCoordination complexes have their own classes of isomers, different magnetic properties and colors, and various applications (photography, cancer treatment, etc), so it makes sense that they would have a naming system as well. 24.4: IsomerizationTwo compounds that have the same formula and the same connectivity do not always have the same shape. There are two reasons why this may happen. In one case, the molecule may be flexible, so that it can twist into different shapes via rotation around individual sigma bonds. This phenomenon is called conformation, and it is covered in a different chapter. The second case occurs when two molecules appear to be connected the same way on paper, but are connected in two different ways in three dimens 24.5: Color and MagnetismCrystal field theory, which assumes that metal–ligand interactions are only electrostatic in nature, explains many important properties of transition-metal complexes, including their colors, magnetism, structures, stability, and reactivity. 24.6: Crystal Field TheoryCrystal field theory treats interactions between the electrons on the metal and the ligands as a simple electrostatic effect. The presence of the ligands near the metal ion changes the energies of the metal d orbitals relative to their energies in the free ion. Both the color and the magnetic properties of a complex can be attributed to this crystal field splitting. The magnitude of the splitting depends on the nature of the ligands bonded to the metal. 24.E: Chemistry of Coordination Chemistry (Exercises)These are homework exercises to accompany the Textmap created for "Chemistry: The Central Science" by Brown et al.
Thumbnail: Structure of the \(trans-[CoCl_2(NH_3)_4]^+\) complex ion. Image used with permission (Public domain; Benjah-bmm27 ).