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Chapter 19: Problem 66

Ethylenediamine (en) is a bidentate ligand, and the ligand diethylenetriamine (dien) is the tridentate analog of en, \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NHCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) (the donor atoms are in color). Draw the Lewis structure of dien and all possible geometric isomers of \(\left[\mathrm{Co}(\mathrm{dien})_{2}\right]^{3+} .\)

Short Answer

Expert verified
\(\left[\mathrm{Co}( ext{dien})_2\right]^{3+}\) can form fac and mer isomers due to the spatial orientation of dien ligands.

Step by step solution

01

Understanding the Structure of Diethylenetriamine (dien)

Diethylenetriamine, abbreviated as dien, is a tridentate ligand, which means it can coordinate to a metal ion through three donor atoms. The formula for dien is \( \mathrm{NH}_{2}\mathrm{CH}_{2}\mathrm{CH}_{2}\mathrm{NHCH}_{2}\mathrm{CH}_{2}\mathrm{NH}_{2} \), where the nitrogen atoms act as the donor atoms. We begin by drawing the Lewis structure, emphasizing the nitrogen atoms for clarity.
02

Drawing the Lewis Structure of dien

To draw the Lewis structure of dien:1. Start with the central amine group (\( \mathrm{NH} \)).2. Connect each nitrogen atom to its adjacent carbon atom (\( \mathrm{CH}_2\)).3. Ensure each \( \mathrm{NH}_2 \) group is connected to carbon, and there are ethylene (\( \mathrm{CH}_2\mathrm{CH}_2 \)) linkers between the nitrogen atoms. The structure is linear with alternating carbon and nitrogen atoms and lone pairs on each nitrogen.
03

Understand Coordination

\(\left[\mathrm{Co}( ext{dien})_2\right]^{3+}\) complex has cobalt as a central metal ion, with two dien ligands. Each dien coordinates with cobalt through its three nitrogen donor atoms. This coordination results in a total of 6 nitrogen atoms forming bonds with cobalt, filling the coordination sphere.
04

Identifying Possible Geometric Isomers

Geometric isomers occur when the spatial arrangement of atoms leads to different structures. For \(\left[\mathrm{Co}( ext{dien})_2\right]^{3+}\), each of the two dien ligands can have different spatial arrangements around the cobalt ion, leading to isomeric configurations.
05

Drawing the Geometric Isomers

For \(\left[\mathrm{Co}( ext{dien})_2\right]^{3+}\), potential geometric isomers include:- **Facial (fac) isomer:** All three donor atoms of one dien ligand are adjacent to each other, forming triangular facial coordination.- **Meridional (mer) isomer:** Two donor atoms from one dien ligand and one donor atom from the other are adjacent, creating a 'meridian' shape through the octahedral complex.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ligand Coordination
Ligand coordination is a key concept in understanding coordination compounds, where molecules or ions form bonds with a central metal atom or ion. Diethylenetriamine (dien) is an excellent example of a tridentate ligand. This means it can attach to the metal through three coordination sites, which, in this case, are nitrogen atoms. Each nitrogen atom in dien donates a pair of electrons to form a coordinate bond with cobalt, which is the central metal ion in \( [\text{Co}(\text{dien})_2]^{3+} \).
  • Tridentate ligands like dien are useful because their multiple coordination sites can create stable metal complexes.
  • This tridentate nature allows for more complex spatial arrangements, leading to different isomers.
  • The formation of these coordinate bonds results in a fully occupied coordination sphere around the metal center, influencing the geometry and stability of the compound.
Understanding how ligands like dien coordinate with metals helps in predicting the resulting structure and properties of coordination compounds.
Geometric Isomers
Geometric isomers in coordination chemistry refer to isomers that have the same molecular formula but different spatial arrangements of atoms, which result in distinct molecules. In the context of \( [\text{Co}(\text{dien})_2]^{3+} \), each dien ligand has three nitrogen atoms that can bind to the cobalt ion. This setup allows for different geometric configurations.
  • **Facial Isomer (fac):** All three donor atoms from one dien ligand are next to each other, forming a triangle on one face of the octahedral structure.
  • **Meridional Isomer (mer):** The donor atoms are arranged so that one from one ligand and two from the other are adjacent, creating a continuous plane cutting through the complex.
These isomers differ in how the ligands and their donor sites are spatially related to each other around the central metal ion. Identifying geometric isomers is important because they can have different chemical and physical properties, affecting their behavior in various chemical processes.
Lewis Structure
The Lewis structure is a diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. When drawing the Lewis structure for diethylenetriamine (dien), several steps need to be observed:
  • Start with the central nitrogen atom and proceed to connect it to adjacent carbon atoms, forming the principal backbone.
  • Each nitrogen atom should have a pair of lone electrons visible, as these are crucial for coordinating with a metal ion.
  • The resulting structure is linear with alternating nitrogen and carbon atoms, depicting the tridentate nature of dien.
The Lewis structure provides a clear visualization of how dien might interact in coordination complexes, particularly which atoms serve as electron pair donors to the central metal ion. This representation is fundamental in predicting the molecule's geometry and reactivity.
Organic Ligand
An organic ligand is a molecule primarily composed of carbon and hydrogen atoms, although it may include other elements like nitrogen. Diethylenetriamine (dien) is an example of an organic ligand with nitrogen as a donor atom. Organic ligands are crucial in forming coordination complexes due to their walk of offering lone electron pairs to bond with metal ions.
  • **Diverse Structures:** Organic ligands can have various structures and can be simple or complex, affecting how they interact with metal centers.
  • **Functional Groups:** Their diverse functional groups, like amine groups in dien, are responsible for electron donation and dictate their ligating behavior.
  • **Versatility in Reactions:** Organic ligands are versatile in participating in complex reactions, serving as key elements in catalysis and enzyme mimetics.
By understanding how organic ligands like dien function and interact with metals, chemists can design specific coordination compounds with desired properties and applications.

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Most popular questions from this chapter

Recently, researchers found a low-spin tetrahedral complex of cobalt(III) in which the ligands are large hydrocarbon groups bonded to the metal through carbon atoms. Construct a crystal field energy-level diagram containing the metal \(d\) electrons of this complex. How many unpaired electrons are expected in this complex?

The complex \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) has five unpaired electrons, whereas \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{4-}\) has only one. Using the ligand field model, depict the electron configuration for each ion. What can you conclude about the effects of the different ligands on the magnitude of \(\Delta ?\)

The ion \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) is a weak Br酶nsted-Lowry acid in water. Write the equilibrium for this process. Discuss the number of unpaired electrons in the \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) ion and the iron product of the equilibrium reaction. Is it possible to determine the number of unpaired electrons without an experiment?

Write the formula for each of the following coordination compounds. (a) a coordination compound containing two complex ions of \(\mathrm{Co}(\mathrm{III}),\) one with six \(\mathrm{CN}^{-}\) ions and the other with three ethylenediamine molecules (you may use the abbreviation "en" for the ethylenediamine molecule) (b) a coordination compound of platinum(II) nitrate, in which four ammonia molecules are coordinated to the transition-metal ion (c) the sodium salt of the complex formed from \(\mathrm{Rh}(\mathrm{III})\), five \(\mathrm{Cl}^{-}\) ions, and one water molecule

In each part, explain why one element has the higher first ionization energy. (a) \(\mathrm{Ti}\) or \(\mathrm{Mn}\) (b) \(\mathrm{V}\) or \(\mathrm{Ta}\) (c) \(\mathrm{Ru}\) or \(\mathrm{Rh}\) (d) \(\mathrm{Mo}\) or \(\mathrm{Os}\)
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