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Chapter 23: Problem 69

Sketch the structure of the complex in each of the following compounds and give the full compound name: (a) cis- \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (b) \(\mathrm{Na}_{2}\left[\mathrm{Ru}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{5}\right]\) (c) trans- \(\mathrm{NH}_{4}\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\) (d) cis- \(\left[\mathrm{Ru}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]\)

Short Answer

Expert verified
\( \begin{array}{l} \textbf{(a)} \qquad \text{cis-Tetraamminecobalt(III) hexahydrate dinitrate} \\ \vspace{3pt} \textbf{(b)} \qquad \text{Sodium hexachlororuthenate(III) dihydrate} \\ \vspace{3pt} \textbf{(c)} \qquad \text{trans-Diaquabis(oxalato)cobaltate(III) tetrahydrate} \\ \vspace{3pt} \textbf{(d)} \qquad \text{cis-Dichlorobis(ethylenediamine)ruthenium(III)} \end{array} \)

Step by step solution

01

Identify the Metal and Ligands

The central metal ion in this complex is Cobalt (Co), and it is coordinated to four Ammonia (NH3) ligands and two Water (H2O) ligands.
02

Determine the Coordination Number and Geometry

The Coordination Number in this complex is 6, which is the sum of all ligands bonded to the central metal ion. The Coordination Geometry for Coordination Number 6 is typically Octahedral.
03

Sketch the Structure

In the cis isomer, the two Water (H2O) ligands are positioned adjacent to each other. The remaining four ligands occupied in the octahedral structure are Ammonia (NH3).
04

Compound Name

The full compound name is cis-Tetraamminecobalt(III) hexahydrate dinitrate. (b) Sketch the structure and give the full compound name for \(\mathrm{Na}_{2}\left[\mathrm{Ru}\left(\mathrm{H}_{2} \mathrm{O}\right)\mathrm{Cl}_{5}\right]\).
05

Identify the Metal and Ligands

The central metal ion in this complex is Ruthenium (Ru), and it is coordinated to one Water (H2O) ligand and five Chloride (Cl) ligands.
06

Determine the Coordination Number and Geometry

The Coordination Number in this complex is 6. The Coordination Geometry for Coordination Number 6 is typically Octahedral.
07

Sketch the Structure

The structure will have an octahedral arrangement, with one Water ligand and five Chloride ligands connected to the Ruthenium center.
08

Compound Name

The full compound name is Sodium hexachlororuthenate(III) dihydrate. (c) Sketch the structure and give the full compound name for trans- \(\mathrm{NH}_{4}\left[\mathrm{Co}\left(\mathrm{C}_{2}\mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\).
09

Identify the Metal and Ligands

The central metal ion in this complex is Cobalt (Co), and it is coordinated to two Oxalate (C2O4) ligands and two Water (H2O) ligands.
10

Determine the Coordination Number and Geometry

The Coordination Number in this complex is 6 since each Oxalate ligand occupies two coordination sites. The Coordination Geometry for Coordination Number 6 is typically Octahedral.
11

Sketch the Structure

In the trans isomer, the two Water (H2O) ligands are positioned opposite to each other. The remaining four ligands in the octahedral structure are occupied by two Oxalate (C2O4) ligands.
12

Compound Name

The full compound name is trans-Diaquabis(oxalato)cobaltate(III) tetrahydrate. (d) Sketch the structure and give the full compound name for cis- \(\left[\mathrm{Ru}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]\).
13

Identify the Metal and Ligands

The central metal ion in this complex is Ruthenium (Ru), and it is coordinated to two Ethylenediamine (en) ligands and two Chloride (Cl) ligands.
14

Determine the Coordination Number and Geometry

The Coordination Number in this complex is 6 since each Ethylenediamine ligand occupies two coordination sites. The Coordination Geometry for Coordination Number 6 is typically Octahedral.
15

Sketch the Structure

In the cis isomer, the two Chloride (Cl) ligands are positioned adjacent to each other. The remaining four ligands in the octahedral structure are occupied by two Ethylenediamine (en) ligands.
16

Compound Name

The full compound name is cis-Dichlorobis(ethylenediamine)ruthenium(III).

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Most popular questions from this chapter

The most important oxides of iron are magnetite, \(\mathrm{Fe}_{3} \mathrm{O}_{4},\) and hematite, \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (a) What are the oxidation states of iron in these compounds? (b) One of these iron oxides is ferrimagnetic, and the other is antiferromagnetic. Which iron oxide is likely to show which type of magnetism? Explain.

(a) A complex absorbs light in the range of \(200-300 \mathrm{nm} . \mathrm{Do}\) you expect it to have visible color? (b) A solution of a compound appears green. Does this observation necessarily mean that all colors of visible light other than green are absorbed by the solution? Explain. (c) What information is usually presented in a visible absorption spectrum of a compound? (d) What energy is associated with an absorption at \(440 \mathrm{nm}\) in \(\mathrm{kJ} / \mathrm{mol} ?\)

Oxyhemoglobin, with an \(\mathrm{O}_{2}\) bound to iron, is a low-spin \(\mathrm{Fe}(\mathrm{II})\) complex; deoxyhemoglobin, without the \(\mathrm{O}_{2}\) molecule, is a high-spin complex. (a) Assuming that the coordination environment about the metal is octahedral, how many unpaired electrons are centered on the metal ion in each case? (b) What ligand is coordinated to the iron in place of \(\mathrm{O}_{2}\) in deoxyhemoglobin? (c) Explain in a general way why the two forms of hemoglobin have different colors (hemoglobin is red, whereas deoxyhemoglobin has a bluish cast). (d) A 15 -minute exposure to air containing 400 ppm of CO causes about \(10 \%\) of the hemoglobin in the blood to be converted into the carbon monoxide complex, called carboxyhemoglobin. What does this suggest about the relative equilibrium constants for binding of carbon monoxide and \(\mathrm{O}_{2}\) to hemoglobin? (e) \(\mathrm{CO}\) is a strong-field ligand. What color might you expect carboxyhemoglobin to be?

Suppose that a transition-metal ion was in a lattice in which it was in contact with just two nearby anions, located on opposite sides of the metal. Diagram the splitting of the metal \(\bar{d}\) orbitals that would result from such a crystal field. Assuming a strong field, how many unpaired electrons would you expect for a metal ion with six \(d\) electrons? (Hint: Consider the linear axis to be the \(z\) -axis)

A four-coordinate complex \(\mathrm{MA}_{2} \mathrm{~B}_{2}\) is prepared and found to have two different isomers. Is it possible to determine from this information whether the complex is square planar or tetrahedral? If so, which is it?
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