Domanda del libro di testo
In octahedral complexes, the choice between high-spin and low-spin electron configurations arises only for d4 - d7 complexes. Explain.
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Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblema 103
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblema 103Capitolo 21, Problema 103
Use a sketch to explain why the dxy and dx2-y2 orbitals have different energies in an octahedral complex. Which of the two orbitals has higher energy?
Guida verificata passo dopo passo1
Step 1: Understand the geometry of an octahedral complex. In an octahedral complex, a central metal atom is surrounded by six ligands positioned at the corners of an octahedron. This arrangement leads to specific interactions between the metal's d orbitals and the ligands.
Step 2: Recall the five d orbitals: d_{xy}, d_{yz}, d_{zx}, d_{x^2-y^2}, and d_{z^2}. In a free atom, these orbitals are degenerate, meaning they have the same energy. However, in an octahedral complex, the presence of ligands causes a splitting of these energy levels.
Step 3: Consider the orientation of the d orbitals. The d_{xy} orbital lies in the xy-plane, while the d_{x^2-y^2} orbital also lies in the xy-plane but has lobes along the x and y axes. In an octahedral complex, ligands approach along the x, y, and z axes.
Step 4: Analyze the interaction with ligands. The d_{x^2-y^2} orbital has lobes that point directly towards the ligands along the x and y axes, leading to greater repulsion and higher energy. In contrast, the d_{xy} orbital's lobes are oriented between the axes, resulting in less direct interaction with the ligands and lower energy.
Step 5: Conclude which orbital has higher energy. Due to the direct interaction with the ligands, the d_{x^2-y^2} orbital experiences greater repulsion and thus has higher energy compared to the d_{xy} orbital in an octahedral complex.
Concetti chiave
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Crystal Field Theory
Crystal Field Theory (CFT) explains how the arrangement of ligands around a central metal ion affects the energy levels of its d-orbitals. In an octahedral complex, the ligands approach the metal ion along the axes, leading to a splitting of the d-orbitals into two energy levels: the lower-energy t2g set and the higher-energy eg set. This theory helps in understanding the electronic structure and stability of coordination complexes.
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01:18
The study of ligand-metal interactions helped to form Ligand Field Theory which combines CFT with MO Theory.
d-Orbital Splitting in Octahedral Fields
In an octahedral field, the five d-orbitals split into two groups due to the electrostatic interactions with surrounding ligands. The dxy and dx2-y2 orbitals are part of the eg set, which is higher in energy compared to the t2g set. The dx2-y2 orbital, oriented along the axes, experiences greater repulsion from the ligands than the dxy orbital, which is oriented between the axes, resulting in different energy levels.
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03:04The crystal field splitting pattern for octahedral complexes has the d orbitals on or along the axes as having the higher energy.
Ligand Field Strength
Ligand field strength refers to the ability of ligands to influence the energy levels of d-orbitals in a metal complex. Strong field ligands cause greater splitting of the d-orbitals, while weak field ligands result in smaller splitting. In the context of the dxy and dx2-y2 orbitals, the ligand field strength determines the extent of energy difference between these orbitals, with the dx2-y2 typically having higher energy due to its direct alignment with the ligands.
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02:40Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
Pratica correlata
Domanda del libro di testo
The reaction of the octahedral complex Co(NH3)3(NO2)3 with HCl yields a complex [Co(NH3)3(H2O)Cl2]+ in which the two chloride ligands are trans to one another.
(a) Draw the two possible stereoisomers of the starting material [Co(NH3)3(NO2)3]. (All three NO2- ligands are bonded to Co through the N atom.)
(b) Assuming that the NH3 groups remain in place, which of the two starting isomers could give rise to the observed product?
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Domanda del libro di testo
Consider the octahedral complex [Co(en)(dien)Cl]2+, where dien = H2NCH2CH2NHCH2CH2NH2, which can be abbreivated
(a) The dien (diethylenetriamine) ligand is a tridentate ligand. Explain what is meant by 'tridentate' and why dien can act as a tridentate ligand.
(b) Draw all possible stereoisomers of [Co(en)(dien)Cl]2+ (dien is a flexible ligand). Which stereoisomers are chiral, and which are achiral?
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Domanda del libro di testo
Tris(2-aminoethyl)amine, abbreviated tren, is the tetradentate ligand N(CH2CH2NH2)3. Using to represent each of the three NCH2CH2NH2 segments of the ligand, sketch all possible isomers of the octahedral complex [Co(tren)BrCl]+.
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