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Ch.21 - Transition Elements and Coordination Chemistry
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.84a
Chapter 21, Problem 21.84a

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?

Verified step by step guidance
1
Step 1: Understand the concept of constitutional isomers. Constitutional isomers are compounds with the same molecular formula but different connectivity of atoms. In coordination chemistry, this can involve different arrangements of ligands around the central metal atom.
Step 2: Identify the formula and name for each structure. Examine each structure to determine the ligands attached to the ruthenium(II) center and their arrangement. Use IUPAC naming conventions for coordination compounds to name each structure.
Step 3: Determine which structures are linkage isomers. Linkage isomers occur when a ligand can coordinate to the metal center through different atoms. Look for ligands that can bind through multiple atoms, such as NO2- (which can bind through nitrogen or oxygen).
Step 4: Identify which structures are ionization isomers. Ionization isomers occur when a ligand inside the coordination sphere can exchange places with an anion or neutral molecule outside the coordination sphere. Compare the structures to see if any such exchanges have occurred.
Step 5: Summarize your findings. List the formula and name for each structure, identify the linkage isomers, and identify the ionization isomers based on your analysis.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Coordination Compounds

Coordination compounds consist of a central metal atom or ion bonded to surrounding molecules or ions called ligands. The arrangement and types of ligands can lead to different structural forms, known as isomers. Understanding the basic structure of coordination compounds is essential for identifying and naming the various isomers presented in the question.
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Isomerism in Coordination Compounds

Isomerism in coordination compounds occurs when two or more compounds have the same formula but different arrangements of atoms. Linkage isomers arise when a ligand can attach to the metal in different ways, while ionization isomers differ in the ions that are present in solution. Recognizing these types of isomerism is crucial for answering parts (b) and (c) of the question.
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Nomenclature of Coordination Compounds

The nomenclature of coordination compounds follows specific rules set by the International Union of Pure and Applied Chemistry (IUPAC). This includes naming the ligands, indicating their number, and specifying the oxidation state of the metal. Properly applying these rules is necessary to accurately provide the names and formulas for the structures in part (a) of the question.
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Related Practice
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. 

(a) [AuCl4]2 (square planar)

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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>

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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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Textbook Question

There are two possible [M(OH)4]- complexes of first-series transition metals that have three unpaired electrons.

(a) What are the oxidation state and the identity of M in these complexes?

(b) Using orbital diagrams, give a valence bond description of the bonding in each complex.

(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which [M(OH)4]- complex is more likely to exist? 

<QUESTION REFERENCES FIGURE 21.6>-

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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.

(a) [Pt(NH3)4]2+ (square planar)

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