Ch.23 - Transition Metals and Coordination Chemistry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
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Brown 14th EditionCh.23 - Transition Metals and Coordination ChemistryProblema 43
Brown 14th EditionCh.23 - Transition Metals and Coordination ChemistryProblema 43Capitolo 23, Problema 43
Complete the exercises below. Determine if each of the following complexes exhibits geometric isomerism. If geometric isomers exist, determine how many there are. c. octahedral [Fe(o-phen)₂ Cl₂]⁺.
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Step 1: Understand the structure of the complex. The complex [Fe(o-phen)₂Cl₂]⁺ is an octahedral complex where 'o-phen' stands for 1,10-phenanthroline, a bidentate ligand, and there are two chloride ions as ligands.
Step 2: Identify the coordination number and geometry. The coordination number for this complex is 6, which is typical for octahedral complexes. The ligands are arranged around the central metal ion, Fe, in an octahedral geometry.
Step 3: Consider the arrangement of ligands. In an octahedral complex, geometric isomerism can occur if there are different types of ligands. Here, we have two bidentate o-phen ligands and two monodentate Cl⁻ ligands.
Step 4: Determine possible isomers. For octahedral complexes with the formula [M(A₂B₂)], where A and B are different ligands, geometric isomers can exist as 'cis' (adjacent) and 'trans' (opposite) forms. Apply this to [Fe(o-phen)₂Cl₂]⁺.
Step 5: Count the isomers. In this case, the complex can have two geometric isomers: one where the two Cl⁻ ligands are adjacent (cis) and one where they are opposite each other (trans).
Concetti chiave
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Geometric Isomerism
Geometric isomerism occurs when compounds have the same molecular formula and connectivity of atoms but differ in the spatial arrangement of those atoms. This type of isomerism is particularly relevant in coordination complexes, where ligands can occupy different positions around a central metal ion, leading to distinct isomers with different properties.
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02:02
Geometric Isomers
Octahedral Coordination Complexes
Octahedral coordination complexes consist of a central metal ion surrounded by six ligands arranged at the corners of an octahedron. The geometry allows for various ligand arrangements, which can lead to the formation of geometric isomers, such as cis and trans isomers, depending on the relative positions of the ligands.
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00:43Coordination Complexes Example
Ligand Types and Their Influence
The type of ligands attached to a metal center can significantly influence the possibility of geometric isomerism. Bidentate ligands, like o-phenanthroline (o-phen), can create more complex arrangements compared to monodentate ligands, affecting the number and types of isomers that can form in octahedral complexes.
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02:38Ligand Types
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