Question

Give the formula and name of a square-planar complex of \(\mathrm{Pt}^{2+}\) with one nitrite ion \(\left(\mathrm{NO}_{2}^{-}, \text {which binds to } \mathrm{Pt}^{2+}\right.\) through \(\mathbf{N}\) ), one chloride ion, and two ammonia molecules as ligands. Are isomers possible? If so, draw the structure of each isomer, and tell what type of isomerism is observed.

Short answer

The complex is \( [\mathrm{Pt}(\mathrm{NO}_2^-)(\mathrm{Cl}^-)(\mathrm{NH}_3)_2] \). Isomers possible: cis and trans geometric isomers.

Step-by-step solution

Identify the central metal and the charge

The central metal is platinum, denoted by \( \mathrm{Pt}^{2+} \). It has a charge of +2.

Identify the ligands

The ligands are one nitrite ion \( (\mathrm{NO}_2^-) \), one chloride ion \( \mathrm{Cl}^- \), and two ammonia molecules \( \mathrm{NH}_3 \).

Construct the formula of the complex

In a square-planar complex, the ligands are arranged around the central metal. The formula of the complex is \( [\mathrm{Pt}(\mathrm{NO}_2^-)(\mathrm{Cl}^-)(\mathrm{NH}_3)_2] \).

Check for possible isomers

Square planar complexes can exhibit geometric isomerism. In this case, the nitrite and chloride ions can occupy different positions relative to each other.

Draw and describe the isomers

Two possible isomers are **cis** and **trans**. In the **cis** isomer, the \( \mathrm{NO}_2^- \) and \( \mathrm{Cl}^- \) ligands are adjacent to each other. In the **trans** isomer, they are opposite each other. Geometric isomerism is the type observed here.

Key concepts

Geometric Isomerism

Geometric isomerism is a fascinating phenomenon found mainly in coordination chemistry. It occurs when the arrangement of the atoms or groups in a compound differs in space, yet the overall composition remains the same. This is not a change in connectivity as with constitutional isomers, but rather a variation in the 3D orientation.
For square-planar complexes, such as the ones involving platinum (Pt), geometric isomerism is quite common. These complexes allow the same set of atoms to be positioned differently around the central metal ion. This results in distinct isomers, usually termed as "cis" and "trans." These configurations can impact the physical and chemical properties drastically even though they share the same chemical formula.

Coordination Chemistry

Coordination chemistry delves into the study of compounds, which are formed when a central metal atom binds to surrounding ligands. These central atoms, often transition metals such as platinum, can hold onto ligands due to their vacant d-orbitals.
Typically, the central metal forms coordinate covalent bonds with these ligands. Such interactions often result in a variety of shapes and configurations, one commonly being the square-planar structure. The nature of these bonds and the resulting structures describe how the metal interacts with its environment, influencing the stability and reactivity of the complex.

Ligands

Ligands are molecules or ions that bond to a central metal atom. They are key players in forming coordination complexes. These entities can be negatively charged ions, like nitrite (NO\(_2^-\)), or neutral molecules, like ammonia (NH\(_3\)).
Each ligand donates at least one pair of electrons to the metal, forming a coordinate covalent bond. Ligands can vary greatly in size, charge, and the number of bonding sites they possess — referred to as their denticity. In the square-planar platinum complex, the nitrite, chloride, and ammonia ligands each have unique properties that influence how they interact with the metal.

Cis-Trans Isomerism

Cis-trans isomerism is a common type of geometric isomerism specific to certain compounds, including square-planar complexes. In the context of the platinum complex, this type of isomerism is evident when ligands are located either adjacent to each other (cis) or directly across from one another (trans).
In the cis configuration, the nitrite and chloride ions sit next to each other, while in the trans configuration, they are on opposite sides. This spatial difference can lead to differing chemical and physical properties, despite having the same formula. Understanding these isomers helps predict how the complex will react under different conditions.