Textbook Question
The Ni2+(aq) cation is green, but Zn2+(aq) is colorless. Explain.
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Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- 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 ChemistryProblem 21.121
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.121Chapter 21, Problem 21.121
Predict the crystal field energy-level diagram for a linear ML2 complex that has two ligands along the :
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Identify the geometry of the complex. In this case, the complex is described as linear with the formula ML2, indicating that the metal (M) is in the center with two ligands (L) aligned along the same axis.
Understand the coordination number and arrangement. For a linear ML2 complex, the coordination number is 2, which means there are two ligands directly coordinating with the metal ion.
Determine the splitting of the d-orbitals in the presence of the ligands. In a linear geometry, the d-orbitals split into different energy levels due to the electrostatic field created by the ligands. The d-orbitals along the axis of the ligands (d_z^2) will experience a different environment compared to those lying in the plane perpendicular to the axis (d_xy, d_xz, d_yz, d_x^2-y^2).
Predict the arrangement of the d-orbitals in terms of energy. In a linear complex, the d_z^2 orbital will have a higher energy due to direct interaction with the ligands along the z-axis. The other four d-orbitals (d_xy, d_xz, d_yz, d_x^2-y^2) will be lower in energy and are degenerate (having the same energy level) as they experience less direct interaction with the ligands.
Sketch the crystal field energy-level diagram based on the above predictions. Place the d_z^2 orbital at a higher energy level and group the other four d-orbitals together at a lower energy level, indicating their degeneracy and lesser interaction with the ligands.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Crystal Field Theory
Crystal Field Theory (CFT) explains how the arrangement of ligands around a central metal ion affects the energy levels of the d-orbitals. In a complex, ligands create an electric field that splits the degenerate d-orbitals into different energy levels, influencing the complex's stability, color, and magnetic properties.
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The study of ligand-metal interactions helped to form Ligand Field Theory which combines CFT with MO Theory.
Ligand Field Strength
Ligand field strength refers to the ability of a ligand to influence the splitting of d-orbitals in a metal complex. Strong field ligands cause a larger splitting of the d-orbitals, leading to different electronic configurations and properties compared to weak field ligands, which result in smaller splitting.
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02:40Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
Geometry of Coordination Complexes
The geometry of coordination complexes, such as linear, tetrahedral, or octahedral, determines the spatial arrangement of ligands around the metal center. In a linear ML2 complex, the ligands are positioned 180 degrees apart, which affects the d-orbital splitting pattern and the overall electronic structure of the complex.
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02:40Molecular Geometry of Coordination Complexes
Related Practice
Textbook Question
Draw the structure of all isomers of the octahedral complex [NbX2Cl4]- (X- = NCS-), and identify those that are linkage isomers.
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Textbook Question
Which of the following complexes can exist as enantiomers? Draw their structures.
(a) [Cr(en)3]3+
(b) cis-[Co(NH3)Cl]2+
(c) trans-[Co(en)2(NH3)Cl]2+
(d) [Pt(NH3)3Cl3]+
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Textbook Question
Predict the number of unpaired electrons for each of the following.
(a) Sc3+
(b) Co2+
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Textbook Question
Constitutional isomers of a ruthenium(II) coordination compound are shown below.
(a) Give the formula and name for structures 1-3.
(b) Which structures are linkage isomers?
(c) Which structures are ionization isomers?
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Textbook Question
Nickel(II) complexes with the formula NiX2L2, where X− is Cl− or N-bonded NCS− and L is the monodentate triphenylphosphine ligand P(C6H5)3, can be square planar or tetrahedral.
(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.
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