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.
(c) [Co(NCS)4]2- (tetrahedral)
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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 21.127b
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.127bChapter 21, Problem 21.127b
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]+
Verified step by step guidance1
Identify the central metal ion in the complex. In this case, it is Ag^+.
Determine the electron configuration of the free metal ion, Ag^+. Silver (Ag) has an atomic number of 47, so its electron configuration is [Kr] 4d^10 5s^1. As Ag^+ loses one electron, the configuration becomes [Kr] 4d^10.
Draw the orbital diagram for the free metal ion, Ag^+. Since Ag^+ has a filled 4d subshell, all 4d orbitals are paired, and there are no unpaired electrons.
Consider the ligands and their effect on the metal ion. NH3 is a neutral ligand and acts as a Lewis base, donating a pair of electrons to the metal ion. In [Ag(NH3)2]^+, the Ag^+ ion forms two coordinate covalent bonds with NH3 ligands.
Determine the hybridization of the metal ion in the complex. For [Ag(NH3)2]^+, the Ag^+ ion uses sp hybrid orbitals to accommodate the two pairs of electrons from the NH3 ligands, resulting in a linear geometry around the metal ion.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Valence Bond Theory
Valence Bond Theory (VBT) explains how atoms bond by overlapping their atomic orbitals to form covalent bonds. It emphasizes the role of hybridization, where atomic orbitals mix to create new hybrid orbitals that can accommodate electron pairs. This theory helps in understanding the geometry and bonding characteristics of complexes, such as how the shape of [Ag(NH3)2]+ is determined by the hybridization of the silver ion.
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Valence Shell Electron Pair Repulsion Theory
Hybridization
Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of [Ag(NH3)2]+, the silver ion undergoes hybridization to form dsp2 hybrid orbitals, which allows it to bond with two ammonia ligands. Understanding hybridization is crucial for predicting the geometry and bond angles in coordination complexes.
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Unpaired Electrons
Unpaired electrons are electrons that are alone in an orbital and are crucial for determining the magnetic properties of a complex. In [Ag(NH3)2]+, the silver ion has a specific electron configuration that can lead to the presence of unpaired electrons, affecting its reactivity and interaction with ligands. Identifying the number of unpaired electrons is essential for understanding the electronic structure and bonding behavior of the metal ion in the complex.
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Related Practice
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
Spinach contains a lot of iron but is not a good source of dietary iron because nearly all the iron is tied up in the oxalate complex [Fe(C2O4)3]3-.
(c) Draw a crystal field energy-level diagram for [Fe(C2O4)3]3-, and predict the number of unpaired electrons. (C2O42- is a weak-field bidentate ligand.)
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Textbook Question
Predict the number of unpaired electrons for each of the following.
(c) Mn3+
(d) Cr2+
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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.
(b) If NiCl2L2 is paramagnetic and Ni(NCS)2L2 is diamagnetic, which of the two complexes is tetrahedral and which is square planar?
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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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