Question

Sketch all the possible stereoisomers of (a) tetrahedral \(\left[\mathrm{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\right]\), (b) square-planar \(\left[\mathrm{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\), (c) octa- hedral \(\left[\mathrm{Fe}(0 \text { -phen })_{2} \mathrm{Cl}_{2}\right]^{+}\)

Short answer

The possible stereoisomers for each complex are as follows: (a) Tetrahedral Complex: \(\left[\mathrm{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\mathrm{Cl}_{2}\right]\) - Only one stereoisomer possible, with no geometric or optical isomers. (b) Square-Planar Complex: \(\left[\mathrm{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\) - Two geometric isomers (cis and trans) possible, with no optical isomers. (c) Octahedral Complex: \(\left[\mathrm{Fe}(0 \text { -phen })_{2} \mathrm{Cl}_{2}\right]^{+}\) - Two geometric isomers (cis and trans) possible, each with two optical isomers due to enantiomeric pairs, resulting in a total of four stereoisomers.

Step-by-step solution

(a) Tetrahedral Complex: \(\left[\mathrm{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\mathrm{Cl}_{2}\right]\)

For the given tetrahedral complex \(\left[\mathrm{Cd}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\mathrm{Cl}_{2}\right]\), Cd has a coordination number of 4. The ligands can be placed at the 4 vertex positions of a tetrahedron surrounding the central metal atom Cd. Since all the ligands are not the same in this complex, we will determine the possible geometric isomers that you can obtain by changing the relative positions of the ligands. There is only one stereoisomer possible for this tetrahedral complex: 1. Two water ligands are located at two adjacent vertices, and two chlorine ligands occupy the other two vertices. No other geometric arrangements are equivalent, so there are no geometric isomers in this case. Moreover, there are no chiral centers, so no optical isomers are possible.

(b) Square-Planar Complex: \(\left[\mathrm{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\)

In the square-planar complex, \(\left[\mathrm{IrCl}_{2}\left(\mathrm{PH}_{3}\right)_{2}\right]^{-}\), the central metal atom Ir has a coordination number of 4. The ligands can be placed at the 4 corner positions of a square surrounding the central metal atom. We can identify the following geometric isomers for this complex: 1. Poisisomer (Cis-isomer): Two chlorine and two phosphine ligands are placed opposite to each other along the diagonal. 2. Trans-isomer: Two chlorine ligands occupy adjacent sites, and two phosphine ligands occupy the other two adjacent sites. No other geometric arrangements are possible. There are no chiral centers in this complex, so no optical isomers are possible.

(c) Octahedral Complex: \(\left[\mathrm{Fe}(0 \text { -phen })_{2} \mathrm{Cl}_{2}\right]^{+}\)

In the octahedral complex, \(\left[\mathrm{Fe}(0 \text { -phen })_{2} \mathrm{Cl}_{2}\right]^{+}\), the central metal atom Fe has a coordination number of 6. The ligands can be placed at the 6 vertices of an octahedron surrounding the central atom. We can identify the following geometric isomers for this complex: 1. Cis-isomer: Two chlorines are adjacent, and two bidentate (0 -phen) ligands occupy the equatorial plane. 2. Trans-isomer: Two chlorines are opposite to each other, and two bidentate (0 -phen) ligands occupy the equatorial plane. Since (0 -phen) is a chiral and bidentate ligand, these two geometric isomers can further give rise to additional optical isomers. So for each geometric isomer (cis and trans), we can have two optical isomers due to enantiomeric pairs. So in total, there are four stereoisomers possible for this octahedral complex.

Key concepts

Coordination Compounds

Coordination compounds are fascinating structures formed by a central metal atom or ion, surrounded by molecules or ions known as ligands. These ligands are attached to the metal atom through coordinate covalent bonds. This unique bonding gives rise to many complex geometries and properties. The coordination number, which indicates the number of ligand atoms bonded to the central atom, plays a crucial role in determining the shape of the compound.

Coordination compounds have various applications, including catalysts, biological systems, and pigments. Understanding their geometric and stereochemical properties helps us delve deeper into their functionality and potential uses. In the exercises, we explore different geometrical arrangements in coordination compounds, such as tetrahedral, square-planar, and octahedral configurations.

Tetrahedral Geometry

Tetrahedral geometry is a common shape for coordination compounds with a coordination number of 4. In this arrangement, the ligands form the vertices of a tetrahedron around the central metal atom.

For example, in the complex \( [\mathrm{Cd}(\mathrm{H}_{2}\mathrm{O})_{2}\mathrm{Cl}_{2}] \), two water and two chlorine ligands are symmetrically arranged. Since the ligands are different, careful consideration is required to determine if any isomers can occur. In this case, no geometric isomers exist as the arrangement is symmetrical and not chiral. Unlike some other geometries, tetrahedral complexes often lack the necessary asymmetry for optical isomerism.

Square-Planar Complex

Square-planar geometry is observed in certain transition metal complexes, particularly with coordination number 4. This structure resembles a flat square with the central metal atom at the center. In the case of the complex \( [\mathrm{IrCl}_{2}(\mathrm{PH}_{3})_{2}]^{-} \), the ligands, including two chlorine and two phosphine groups, can be arranged in distinct ways. The most notable geometric isomers are:

• Cis-isomer: Chlorines and phosphines across from each other diagonally.
• Trans-isomer: Chlorines and phosphines adjacent to each other.

Due to the plane symmetry, no optical isomers exist for this arrangement. The square-planar structure is crucial in certain metal-based drugs and catalysts.

Octahedral Complex

Octahedral geometry is prevalent in coordination compounds with a coordination number of 6. It features ligands at the vertices of an octahedron, bonding around the central metal atom.For example, the complex \( [\mathrm{Fe}(0\text{ -phen})_{2}\mathrm{Cl}_{2}]^{+} \) allows for a fascinating exploration of isomerism. There are geometric isomers, like:

• Cis-isomer: Chlorines adjacent to each other, while phenanthroline ligands are in the equatorial plane.
• Trans-isomer: Chlorines opposite each other.

Thanks to the chiral 0-phen ligands, each geometric isomer can also form two optical isomers, resulting in a total of four stereoisomers. This level of complexity enriches the study of such compounds, revealing potential applications in fields like pharmaceuticals and materials science.