Question

Although the cis configuration is known for [ \(\mathrm{Pt}^{\left.(e n) \mathrm{Cl}_{2}\right] \text {, no }}\) trans form is known. (a) Explain why the trans compound is not possible. (b) Would \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) be more likely than en \(\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)\) to form the trans compound? Explain.

Short answer

The trans configuration is not possible for the given complex due to the chelate ring formed by the ethylenediamine (en) ligand, which restricts the movement and arrangement of other ligands. However, the ligand \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\), with a longer carbon chain between the nitrogen atoms, may be more likely to form a trans configuration because the increased flexibility may allow for the trans arrangement of other ligands such as the chlorides.

Step-by-step solution

Understand the structure of cis configuration

In the cis configuration of the given complex, the \(\mathrm{Pt}^{II}\) cation is bonded with two chloride ions (Cl-) and the ethylenediamine (en) ligand. The ethylenediamine ligand is a bidentate ligand, meaning it can bond to the central metal atom through two donor atoms. In this case, the nitrogen atoms (NH2) in en are the donor atoms and form a chelate ring together with the Pt atom.

Explain why trans configuration is not possible

In the trans configuration, the two chloride ions would be placed opposite each other instead of being adjacent as in the cis configuration. However, the presence of a chelate ring formed by the ethylenediamine ligand restricts the mobility between the ligands. The bidentate en ligand effectively "locks" the positions of the chloride ions, fixing them in the cis configuration. Therefore, the trans configuration cannot be formed.

Analyze the possibility of forming trans configuration with other ligands

To answer this question, let's consider the structure of the ligand \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\). This ligand also has two nitrogen donor atoms, but it has a longer carbon chain between them compared to the ethylenediamine (en) ligand. In this case, the longer ligand can potentially allow more flexibility, and the trans configuration may be achievable. To summarize, the original complex with ethylenediamine does not form a trans configuration due to the chelate ring, which restricts the movement and arrangement of other ligands. However, the ligand \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\), with a longer carbon chain between the nitrogen atoms, may be more likely to form a trans configuration because the increased flexibility may allow for the trans arrangement of other ligands such as the chlorides.

Key concepts

Cis-Trans Isomerism

Cis-trans isomerism is a fascinating concept in coordination chemistry. It refers to the spatial arrangement of ligands around a central metal atom in coordination complexes. This type of isomerism is particularly prominent in complexes that contain a square planar or octahedral geometry.

In the cis configuration, similar ligands are adjacent to each other, while in the trans configuration, they are opposite. This spatial difference can significantly alter the physical and chemical properties of the compounds. For example, in the case of the given complex \([\text{Pt(en)Cl}_2\text{]}\), the cis form exists because the chloride ions and the ethylenediamine (en) ligand stabilize in positions next to each other, forming a chelate ring.

Such spatial arrangements are not only interesting from a structural point of view but also critically influence reactivity, solubility, and biological activity. Understanding why a complex might favor either cis or trans configuration is crucial in synthetic chemistry and materials science.

Bidentate Ligands

Bidentate ligands are an essential element in coordination chemistry. They "bite" the central metal atom using two donor atoms to form stable rings, known as chelate rings. A common example of a bidentate ligand is ethylenediamine (en), which uses its two nitrogen atoms to anchor onto a central metal ion.

These ligands form a strong and stable attachment, minimizing the likelihood of dissociation. This is mainly due to the formation of the chelate ring, which is usually five or six membered and highly stable. The geometry and bond angles of the bidentate ligands contribute to the fixed positions of other ligands, often resulting in specific isomerism such as the observed cis configuration in the complex \([\text{Pt(en)Cl}_2\text{]}\).

Moreover, the introduction of bidentate ligands can lead to more rigid and structured complexes, which are easier to predict in terms of behavior and reactivity, making them invaluable in designing specific metal coordination compounds.

Chelate Effect

The chelate effect is a vital principle of coordination chemistry, referring to the improved stability of complexes formed with chelating ligands compared to those with monodentate ligands. It occurs when multidentate ligands form multiple bonds with a single central metal atom, creating a stronger and more stable complex.

In the case of the complex \([\text{Pt(en)Cl}_{2}\text{]}\), the ethylenediamine ligand acts as a chelating ligand by forming a single five-membered ring with the platinum. The stability of the chelate complex is due to entropic factors: replacing several monodentate ligands with one bidentate chelating ligand releases more water molecules, leading to increased disorder in the system and more stability.

The chelate effect is crucial in explaining why certain configurations, such as trans, may not form. In the presence of strong chelating ligands, any configuration that would disrupt the integrity of a chelate ring is less favored, as seen in the given exercise. Therefore, the cis configuration remains stable and dominant.