Textbook Question
Predict the number of unpaired electrons for each of the following.
(c) Mn3+
(d) Cr2+
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
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- 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
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- 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 21.126b
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.126bChapter 21, Problem 21.126b
Give a valence bond description of the bonding in each of the following complexes. 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) [NiBr4]2- (tetrahedral)
Verified step by step guidance1
Step 1: Determine the oxidation state of the metal ion in the complex. For [NiBr_4]^{2-}, the oxidation state of Ni is +2.
Step 2: Write the electron configuration for the free Ni^{2+} ion. Nickel (Ni) has an atomic number of 28, so its electron configuration is [Ar] 3d^8 4s^2. For Ni^{2+}, remove two electrons from the 4s orbital, resulting in [Ar] 3d^8.
Step 3: Draw the orbital diagram for the free Ni^{2+} ion. The 3d orbitals will have 8 electrons, with two unpaired electrons in the 3d orbitals.
Step 4: Determine the hybridization of the metal ion in the complex. In a tetrahedral complex like [NiBr_4]^{2-}, the metal ion uses sp^3 hybrid orbitals for bonding.
Step 5: Indicate the number of unpaired electrons in the complex. Since the 3d orbitals of Ni^{2+} have two unpaired electrons, the complex will also have two unpaired electrons.>
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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. In this theory, the strength of the bond is determined by the extent of overlap between the orbitals. For transition metals, VBT also considers hybridization, where atomic orbitals mix to form new hybrid orbitals that can accommodate bonding with ligands.
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Valence Shell Electron Pair Repulsion Theory
Hybridization
Hybridization is the process of combining atomic orbitals to create new hybrid orbitals that are suitable for bonding. In the case of the tetrahedral complex [NiBr4]²⁻, nickel undergoes sp³ hybridization, resulting in four equivalent hybrid orbitals that can form bonds with the four bromide ligands. This concept is crucial for predicting the geometry and bonding properties of coordination complexes.
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00:51Hybridization
Unpaired Electrons and Magnetic Properties
Unpaired electrons in an atom or ion contribute to its magnetic properties. In transition metal complexes, the number of unpaired electrons can indicate whether the complex is paramagnetic (having unpaired electrons) or diamagnetic (all electrons paired). For [NiBr4]²⁻, analyzing the electron configuration of the nickel ion and the resulting hybridization helps determine the number of unpaired electrons and the complex's overall magnetic behavior.
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Related Practice
Textbook Question
Two first-series transition metals have three unpaired electrons in complex ions of the type [MCl4]2-.
(a) What are the oxidation state and the identity of M in these complexes?
(b) Draw valence bond orbital diagrams for the two possible ions.
(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which ion is more likely to exist?
<QUESTION REFERENCES FIGURE 21.6>
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?
Textbook Question
Assign a systematic name to each of the following ions.
(c) [Fe(H2O)5NCS]2+
(d) [Cr(NH3)2(C2O4)2]-
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Textbook Question
Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures.
(c) [Cu(H2O)4Cl2]+
(d) Ru(NH3)3I3
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+