Textbook Question
Look at the location in the periodic table of elements A, B, C, and D. What is the electron configuration of the transition metal in each of the following ions?
(a) A2+
(b) B+
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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 21.131b
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.131bChapter 21, Problem 21.131b
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.
(b) If NiCl2L2 is paramagnetic and Ni(NCS)2L2 is diamagnetic, which of the two complexes is tetrahedral and which is square planar?
Verified step by step guidance1
Understand the terms: Paramagnetic substances have unpaired electrons, while diamagnetic substances have all electrons paired.
Recall that square planar complexes often result in low-spin configurations, leading to paired electrons, while tetrahedral complexes are usually high-spin, resulting in unpaired electrons.
Consider the electronic configuration of Nickel(II), which is [Ar] 3d^8.
In a square planar geometry, the d-orbitals split such that the electrons pair up, leading to a diamagnetic complex.
In a tetrahedral geometry, the d-orbitals split differently, often resulting in unpaired electrons, leading to a paramagnetic complex.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Coordination Geometry
Coordination geometry refers to the spatial arrangement of ligands around a central metal atom in a complex. Nickel(II) complexes can adopt different geometries, such as square planar or tetrahedral, depending on the number and type of ligands coordinated to the metal. The geometry influences the electronic properties and reactivity of the complex.
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02:40
Molecular Geometry of Coordination Complexes
Magnetism in Coordination Complexes
The magnetic properties of coordination complexes are determined by the presence of unpaired electrons. A paramagnetic complex has unpaired electrons, resulting in a net magnetic moment, while a diamagnetic complex has all electrons paired, leading to no net magnetic moment. Understanding these properties helps in predicting the geometry of the complexes based on their magnetic behavior.
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00:43Coordination Complexes Example
Ligand Field Theory
Ligand field theory explains how the arrangement of ligands around a metal ion affects its electronic structure and energy levels. In square planar complexes, the d-orbitals split in a way that can stabilize unpaired electrons, leading to paramagnetism, while tetrahedral complexes have a different splitting pattern that can lead to diamagnetism. This theory is crucial for understanding the electronic configurations of metal complexes.
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02:40Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
Related Practice
Textbook Question
Predict the number of unpaired electrons for each of the following.
(c) Mn3+
(d) Cr2+
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Textbook Question
Cobalt(III) trifluoroacetylacetonate, Co(tfac)3, is a sixcoordinate, octahedral metal chelate in which three planar, bidentate tfac ligands are attached to a central Co atom:
(b) Diastereoisomers A and B have dipole moments of 6.5 D and 3.8 D, respectively. Which of your diastereoisomers is A and which is B?
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Textbook Question
What is the systematic name for each of the following ions?
(c) [Co(CO3)3]3-
(d) [Pt(en)2(SCN)2]2+
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Textbook Question
For each of the following complexes, draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons.
(b) [MnCl4]2- (tetrahedral)
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Textbook Question
For each of the following complexes, describe the bonding using valence bond theory. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(b) [Ag(NH3)2]+
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