Ch.21 - Transition Elements and Coordination Chemistry

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.21 - Transition Elements and Coordination Chemistry

Problem 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

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 EDTA^4– respectively.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

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.

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.

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.

Recommended video:

Guided course

01:53

Formal Charge

Related Practice

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.

137

views

Textbook Question

The glycinate anion, gly-= NH₂CH₂CO₂ ^-, bonds to metal ions through the N atom and one of the O atoms. Using to represent gly-, sketch the structures of the four stereoisomers of Co(gly)₃.

134

views

Textbook Question

What is the oxidation state of the metal in each of the complexes?

a. [Ni(CN)₅]^3–

b. Ni(CO)₄

c. [Co(en)₂(H₂O)Br]²⁺

d. [Cu(H₂O)₂(C₂O₄)₂]^2–

e. Co(NH₃)₃(NO₂)₃

views

Textbook Question

What role does EDTA^4-play as a trace additive to mayonnaise? Would the glycinate ion (H₂NCH₂CH₂NH₂) be an effective substitute for EDTA^4-?