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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 21.64
Chapter 21, Problem 21.64

What is the oxidation state of the metal in each of the complexes?
a. AgCl2–
b. [Cr(H2O)5Cl]2+
c. [Co(NCS)4]2–
d. [ZrF8]4–
e. [Fe(EDTA)(H2O)]–

Verified step by step guidance
1
Step 1: Understand the concept of oxidation state. The oxidation state is the charge of an atom if all bonds were ionic. It helps in determining the electron count of the metal in a complex.
Step 2: For each complex, identify the charge of the ligands and the overall charge of the complex. This will help in determining the oxidation state of the metal.
Step 3: For complex a, AgCl2–: Chloride (Cl–) has a charge of -1. With two chlorides, the total charge from ligands is -2. The overall charge of the complex is -1. Use the equation: oxidation state of Ag + (-2) = -1.
Step 4: For complex b, [Cr(H2O)5Cl]2+: Water (H2O) is neutral, and chloride (Cl–) has a charge of -1. The overall charge of the complex is +2. Use the equation: oxidation state of Cr + (-1) = +2.
Step 5: Repeat similar calculations for the remaining complexes: c. [Co(NCS)4]2–, d. [ZrF8]4–, and e. [Fe(EDTA)(H2O)]–, considering the charges of NCS–, F–, and EDTA4– respectively.

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Key Concepts

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

Oxidation State

The oxidation state, or oxidation number, is a measure of the degree of oxidation of an atom in a chemical compound. It indicates the number of electrons that an atom can gain, lose, or share when forming chemical bonds. Understanding oxidation states is crucial for determining the charge of metal ions in coordination complexes and helps in balancing redox reactions.
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Coordination Complexes

Coordination complexes consist of a central metal atom or ion bonded to surrounding molecules or ions, known as ligands. The nature of these ligands and their arrangement around the metal can influence the oxidation state of the metal. Analyzing the overall charge of the complex and the charges of the ligands is essential for calculating the oxidation state of the metal.
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Charge Balance

Charge balance is the principle that the total positive charge in a compound must equal the total negative charge. In coordination complexes, this involves summing the oxidation states of the metal and the charges of the ligands to ensure that the overall charge of the complex matches the given charge. This concept is fundamental for determining the oxidation state of the metal in various complexes.
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Related Practice
Textbook Question
In excess of NH3(aq), Zn2+ forms a complex ion, [Zn(NH3)4]2+ which has a formation constant Kf = 7.8 x 10^8. Calculate the concentration of Zn2+ in a solution prepared by adding 1.00 x 10^-2 mol Zn(NO3)2 to 1.00 L of 0.250 M NH3. (a) 7.9 x 10^-4 M(b) 2.8 x 10^-6 M(c) 3.9 x 10^-9 M(d) 6.4 x 10^-11 M
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Textbook Question

The oxalate ion is a bidentate ligand as indicated in Figure 21.8. Would you expect the carbonate ion to be a monodentate or bidentate ligand? Explain your reasoning.

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Textbook Question

Draw the structures of all possible diastereoisomers of an octahedral complex with the formula MA2B2C2. Which of the diastereoisomers, if any, can exist as enantiomers?

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Textbook Question

What is the electron configuration of Co2+ and how many unpaired electrons are in the free transition metal ion?

(a) [Ar]3d54s2; 5 unpaired electrons

(b) [Ar]3d54s2; 1 unpaired electron

(c) [Ar]3d7; 3 unpaired electrons

(d) [Ar]3d7; 1 unpaired electron

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Textbook Question

The [Cr(H2O)6]3+ ion is violet, and [Cr(CN)6]3- is yellow. Explain this difference using crystal field theory. Use the colors to order H2O and CN- in the spectrochemical series.

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