Question

Sketch all of the isomers of \(\left[\mathrm{CoCl}_{2}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} .\) Label the cis chloro and trans chloro isomers.

Short answer

The complex has two geometrical isomers: one 'cis-chloro' with the two Cl adjacent, and one 'trans-chloro' with the two Cl opposite each other.

Step-by-step solution

Understanding the Complex

Recognize that the complex ion \(\left[\mathrm{CoCl}_{2}(\mathrm{en})(\mathrm{NH}_{3})_{2}\right]^{+}\) consists of a central cobalt ion (Co) with two chloride anions (Cl), an ethylenediamine (en) which acts as a bidentate ligand, and two ammonia molecules (NH3). The cobalt has a coordination number of 6, making the geometry octahedral.

Drawing the Geometrical Isomers

For the octahedral complex, there are two possible geometrical isomers: cis and trans. Draw the 'cis' isomer by placing the two chloride anions adjacent to each other, and the 'trans' isomer by placing the chloride anions opposite each other. In both cases, the ethylenediamine (en) will occupy two positions directly opposite each other due to its bidentate nature, and the remaining two positions are occupied by the ammonia molecules.

Labeling the Isomers

After drawing the structures, label the isomer with the chloro ligands adjacent as the 'cis-chloro' isomer and the one with the chloro ligands opposite each other as the 'trans-chloro' isomer.

Key concepts

Coordination Chemistry

Coordination chemistry involves the study of compounds formed between metal ions and various organic or inorganic ligands. In these compounds, known as coordination complexes, a central metal atom or ion is surrounded by a set of molecules or ions called ligands. These ligands donate pairs of electrons to the metal, creating a very specific arrangement depending on the number of electron-pairs donated, which is described as the coordination number of the metal. The stability and reactivity of these complexes largely depend on the nature of the ligands and the geometry of the complex.

In coordination complexes, ligands can be monodentate, donating one pair of electrons to the metal; bidentate, donating two; or even polydentate, forming several bonds to the metal ion. The coordination number and the types of ligands are crucial in defining the properties and possible applications of coordination compounds, which range from catalysis to the vibrant colors in inorganic pigments.

Octahedral Complex

An octahedral complex is a type of coordination compound where the central metal ion is surrounded by six ligands positioned at the corners of an octahedron. This geometry is one of the most common and important in coordination chemistry, particularly when the central atom has a coordination number of six. The octahedral shape emerges because it provides an energetically favorable arrangement where repulsions between the electron pairs in the ligand-metal bonds are minimized.

Within the octahedral arrangement, ligands can occupy positions along the x, y, and z axes, leading to distinct spatial configurations. Understanding these geometries is vital for predicting the properties of these complexes such as their magnetic behavior, reactivity, and even color. Importantly, octahedral complexes often exhibit isomerism, where the same atoms are connected in different ways, leading to isomers with distinct properties.

Cis-Trans Isomerism

Cis-trans isomerism, a form of stereoisomerism, is particularly relevant in octahedral complexes of coordination chemistry. It occurs when two identical ligands can be arranged differently around the central metal ion to form two distinct isomers. The 'cis' isomer has the two identical ligands adjacent to each other, at a 90-degree angle, while the 'trans' isomer has the two identical ligands opposite each other, separated by a 180-degree angle.

These isomers can have completely different physical and chemical properties. For example, 'cisplatin' is a widely used anti-cancer drug, while its 'trans' counterpart is not therapeutically useful. Understanding and identifying the 'cis' and 'trans' forms is crucial in coordination chemistry since the specific arrangement of ligands can significantly influence the activity and function of the coordination complex. In summarizing, paying attention to the ligand arrangement in octahedral complexes enhances our understanding of their behavior and applications in various fields, including medicine and materials science.