Textbook Question
Based on effective nuclear charge (Zeff), which ion is the strongest oxidizing agent?
(a) Cu2+
(b) Ni2+
(c) Fe2+
(d) Mn2+
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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 21.116
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.116Chapter 21, Problem 21.116
Although Cl- is a weak-field ligand and CN- is a strong field ligand, [CrCl6]3- and [Cr(CN)6]3- exhibit approximately the same amount of paramagnetism. Explain.
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Identify the oxidation state of chromium in both complexes. Chromium is in the +3 oxidation state in both [CrCl_6]^{3-} and [Cr(CN)_6]^{3-}.
Determine the electron configuration of the Cr^{3+} ion. Chromium has an atomic number of 24, so its electron configuration is [Ar] 3d^5 4s^1. For Cr^{3+}, remove three electrons, resulting in [Ar] 3d^3.
Consider the effect of ligand field strength on the d-orbitals. Cl^- is a weak-field ligand, leading to a high-spin complex, while CN^- is a strong-field ligand, typically leading to a low-spin complex.
Analyze the number of unpaired electrons. In both complexes, the Cr^{3+} ion has three unpaired electrons in the 3d orbitals, resulting in similar paramagnetic properties.
Conclude that despite the difference in ligand field strength, the number of unpaired electrons remains the same in both complexes, explaining the similar paramagnetism.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ligand Field Theory
Ligand Field Theory explains how the presence of ligands around a central metal ion affects its electronic structure and the energy levels of its d-orbitals. Strong-field ligands, like CN<sup>-</sup>, cause a larger splitting of d-orbitals compared to weak-field ligands, like Cl<sup>-</sup>. This theory helps in understanding the magnetic properties of coordination complexes based on the arrangement and strength of the ligands.
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02:40
Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
Paramagnetism
Paramagnetism is a form of magnetism that occurs in materials with unpaired electrons. In coordination complexes, the number of unpaired electrons determines the degree of paramagnetism. Both [CrCl<sub>6</sub>]<sup>3-</sup> and [Cr(CN)<sub>6</sub>]<sup>3-</sup> can exhibit similar levels of paramagnetism if they have the same number of unpaired electrons, despite the differences in ligand strength.
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01:33Paramagnetism and Diamagnetism
Crystal Field Splitting
Crystal Field Splitting refers to the energy difference between the split d-orbitals in a transition metal complex due to the presence of ligands. In octahedral complexes, the d-orbitals split into two sets: t<sub>2g</sub> and e<sub>g</sub>. The extent of this splitting influences the electron configuration and, consequently, the magnetic properties of the complex, which can lead to similar paramagnetic behavior in complexes with different ligands.
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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.
Related Practice
Textbook Question
The glycinate anion, gly-= NH2CH2CO2 -, bonds to metal ions through the N atom and one of the O atoms. Using to represent gly-, sketch the structures of the four stereoisomers of Co(gly)3.
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Textbook Question
What role does EDTA4- play as a trace additive to mayonnaise? Would the glycinate ion (H2NCH2CH2NH2) be an effective substitute for EDTA4-?
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Textbook Question
Which of the following complexes are paramagnetic?
(a) [Mn(CN)6]3-
(b) [Zn(NH3)4]2+ (tetrahedral)
(c) [Fe(CN)6]4-
(d) [FeF6]4-
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Textbook Question
Based on the wavelength of maximum absorption of the cobalt complexes, arrange the following ligands in a spectrochemical series from weakest-field to strongest-field ligand.
(a) Cl- < NCS- < H2O < NH3
(b) Cl- < NCS- < H2O < NH3
(c) H2O < Cl- < NH3 < NCS-
(d) Cl- < H2O < NCS- < NH3
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Textbook Question
What hybrid orbitals are used by the metal ion and how many unpaired electrons are present the complex ion [VCl4]- with tetrahedral geometry?
(a) sp3; 2 unpaired electrons
(b) sp3; 3 unpaired electrons
(c) sp3d2; 3 unpaired electrons
(d) sp3d2; 4 unpaired electrons
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