Textbook Question
What is the systematic name for each of the following coordination compounds?
(a) Cs[FeCl4]
(b) [V(H2O)6](NO3)3
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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 & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
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McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.118a
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.118aChapter 21, Problem 21.118a
Draw a crystal field energy-level diagram, and predict the number of unpaired electrons for each of the following:
(a) [Mn(H2O)6]2+
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Identify the metal ion and its oxidation state. For [Mn(H2O)_6]^{2+}, manganese (Mn) is in the +2 oxidation state.
Determine the electron configuration of the Mn^{2+} ion. Manganese in its elemental form is [Ar] 3d^5 4s^2, so Mn^{2+} is [Ar] 3d^5.
Recognize that [Mn(H2O)_6]^{2+} is an octahedral complex, which means the 3d orbitals will split into two sets: t_{2g} (lower energy) and e_g (higher energy).
Distribute the 5 d-electrons of Mn^{2+} among the split d-orbitals according to Hund's rule, filling the lower energy t_{2g} orbitals first before pairing electrons in the higher energy e_g orbitals.
Count the number of unpaired electrons in the d-orbitals after distribution.
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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 its electronic structure and energy levels. It describes the splitting of d-orbitals in transition metal complexes due to the electrostatic interactions between the metal ion and surrounding ligands. This theory is crucial for predicting the magnetic properties and color of the complexes.
d-Orbital Splitting
In an octahedral field, the five d-orbitals split into two energy levels: the lower-energy t2g (dxy, dyz, dzx) and the higher-energy eg (dx2-y2, dz2) orbitals. The extent of this splitting depends on the nature of the ligands and their field strength. Understanding this splitting is essential for determining the electron configuration and the number of unpaired electrons in a complex.
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d Orbital Orientations
Unpaired Electrons and Magnetism
Unpaired electrons in an atom or ion contribute to its magnetic properties. A species with unpaired electrons exhibits paramagnetism, while those with all paired electrons are diamagnetic. In the context of transition metal complexes, the number of unpaired electrons can be predicted from the electron configuration after considering d-orbital splitting, which is vital for understanding the complex's behavior in a magnetic field.
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Related Practice
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
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
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
Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures.
(a) Pt(NH3)3Cl (square planar)
(b) [FeBr2Cl2(en)]-
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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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