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Chapter 21: Problem 47

Draw all geometrical and linkage isomers of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{NO}_{2}\right)_{2}\)

Short Answer

Expert verified
There are a total of four isomers for the complex \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{NO}_{2}\right)_{2}\), considering both geometrical and linkage isomers. These include: 1. cis-isomer with both NO2- ligands attached through nitrogen. 2. cis-isomer with both NO2- ligands attached through oxygen. 3. trans-isomer with both NO2- ligands attached through nitrogen. 4. trans-isomer with both NO2- ligands attached through oxygen.

Step by step solution

01

Understand Geometrical and Linkage Isomers

Geometrical isomers are those isomers which differ in the arrangement(spatial orientation) of their ligands around the central metal atom. In the case of octahedral complexes, these isomers can arise due to the difference in the position of two ligands: - cis-isomers: the two similar ligands are adjacent to each other - trans-isomers: the two similar ligands are opposite to each other Linkage isomers are those isomers which differ in the point of attachment of their ligands to the central metal atom. They can arise if a ligand can bind to the metal center in more than one way, such as the NO2- ligand that can bind to the metal center through the nitrogen (N-NO2) or through the oxygen (O-NO2).
02

Identifying the Ligands and Possible attachments

Here, we have two types of ligands: 1. Ammonia (NH3) - it binds to the central metal atom through nitrogen. 2. Nitrite (NO2-) - it can bind to the central metal atom through nitrogen or oxygen. The complex has an octahedral configuration with 4 NH3 and 2 NO2- ligands.
03

Identifying Geometrical Isomers

For geometrical isomers, we need to determine the possible arrangements of the two NO2- ligands. There are two possibilities for this complex based on the positioning of NO2- ligands: 1. cis-isomer: The two NO2- ligands are adjacent to each other (90° angle between them) 2. trans-isomer: The two NO2- ligands are opposite to each other (180° angle between them)
04

Identifying Linkage Isomers

Since NO2- ligand can bind through nitrogen or oxygen, there are two possible linkage arrangements: 1. Both NO2- ligands bind through nitrogen (N-NO2) 2. Both NO2- ligands bind through oxygen (O-NO2)
05

Drawing All Possible Isomers

Now that we have identified all the possible geometrical and linkage configurations, we can draw all isomers: 1. cis-isomer with both NO2- ligands attached through nitrogen. 2. cis-isomer with both NO2- ligands attached through oxygen. 3. trans-isomer with both NO2- ligands attached through nitrogen. 4. trans-isomer with both NO2- ligands attached through oxygen. Considering both geometrical and linkage isomers, there are a total of four possible isomers for the complex \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{NO}_{2}\right)_{2}\).

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Most popular questions from this chapter

When concentrated hydrochloric acid is added to a red solution containing the \(\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) complex ion, the solution turns blue as the tetrahedral \(\mathrm{CoCl}_{4}^{2-}\) complex ion forms. Explain this color change.

The compound cisplatin, Pt \(\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2},\) has been studied extensively as an antitumor agent. The reaction for the synthesis of cisplatin is: $\mathrm{K}_{2} \mathrm{PtCl}_{4}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow \mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}(s)+2 \mathrm{KCl}(a q)$ Write the electron configuration for platinum ion in cisplatin. Most \(d^{8}\) transition metal ions exhibit square planar geometry. With this and the name in mind, draw the structure of cisplatin.

Consider the complex ions $\mathrm{Co}\left(\mathrm{NH}_{3}\right) 6^{3+}, \mathrm{Co}(\mathrm{CN})_{6}^{3-},\( and \)\mathrm{CoF}_{6}^{3-} .$ The wavelengths of absorbed electromagnetic radiation for these compounds (in no specific order) are \(770 \mathrm{nm},\) \(440 \mathrm{nm},\) and 290 $\mathrm{nm} .$ Match the complex ion to the wave- length of absorbed electromagnetic radiation.

Write electron configurations for the following transition metals and their ions. a. \(\mathrm{Co}, \mathrm{Co}^{2+}, \mathrm{Co}^{3+}\) b. \(\mathrm{Pt}, \mathrm{Pt}^{2+}, \mathrm{Pt}^{4+}\) c. \(\mathrm{Fe}, \mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}\)

Both \(\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) and \(\mathrm{Ni}(\mathrm{SCN})_{4}^{2-}\) have four ligands. The first is paramagnetic, and the second is diamagnetic. Are the complex ions tetrahedral or square planar? Explain.
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