Question

Determine if each of the following metal complexes is chiral and therefore has an optical isomer: (a) square planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right],(\mathbf{b})\) octahedral \(\left[\mathrm{Ni}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},(\mathbf{c})\) octahe- dral \(\operatorname{cis}-\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{ClBr}\right]\)

Short answer

The three metal complexes were analyzed for chirality by examining their structure and checking for symmetry elements. The results are as follows: (a) square planar [Pd(en)(CN)₂] is achiral, (b) octahedral [Ni(en)(NH₃)₄]²⁺ is achiral, and (c) octahedral cis-[V(en)₂ClBr] is chiral, therefore having an optical isomer.

Step-by-step solution

Identify the metal complex geometries

Three geometries of the metal complexes are given: square planar, octahedral, and cis-octahedral. The geometry will give us insights into the spatial arrangement of the ligands which may produce chirality.

Analyze the geometry of [Pd(en)(CN)₂]

The square planar coordination geometry has the metal ion at the center and the four ligands are at the corners of a square on the same plane. In this case, Pd is the central metal ion, coordinated to ethylenediamine (en) and two cyanide (CN) ligands. The structure can be represented as follows: en Pd CN CN Since there is a plane of symmetry in the molecule (the plane of the paper itself), this metal complex is not chiral.

Analyze the geometry of [Ni(en)(NH₃)₄]²⁺

The octahedral coordination geometry consists of a central metal ion surrounded by six ligands arranged in an octahedron. In this case, Ni is the central metal ion, coordinated to one ethylenediamine (en) and four ammonia (NH₃) ligands. The structure can be represented as follows: NH₃ en NH₃ NH₃ Ni NH₃ If we consider this structure carefully, we can identify a plane of symmetry along the ligands (en) and two of the NH₃ ligands. This indicates that the metal complex is not chiral.

Analyze the geometry of cis-[V(en)₂ClBr]

The cis-octahedron coordination geometry also consists of a central metal ion surrounded by six ligands arranged in an octahedron, but with specific arrangements. In this case, V is the central metal ion, coordinated to two ethylenediamine (en) ligands, one chloride (Cl), and one bromide (Br) ligand, in a cis configuration. Cis configuration means that the two en ligands are adjacent to each other. The structure can be represented as follows: Cl en V en Br Since this complex does not have any plane of symmetry or inversion center, this metal complex is chiral.

Conclusion

On analyzing each metal complex, we can conclude that: (a) square planar [Pd(en)(CN)₂] is achiral. (b) octahedral [Ni(en)(NH₃)₄]²⁺ is achiral. (c) octahedral cis-[V(en)₂ClBr] is chiral and therefore has an optical isomer.

Key concepts

Optical Isomerism

Optical isomerism, a fascinating aspect of stereochemistry, is the property of certain molecules and complexes to exist in forms which are non-superimposable mirror images of one another, much like a person's left and right hands. These non-superimposable mirror images are known as 'enantiomers'. Enantiomers of a molecule or complex have identical physical and chemical properties except for the direction in which they rotate plane-polarized light. This is called optical activity, and a substance that displays this property is said to be 'optically active'.

To determine if a metal complex shows optical isomerism, we must look for elements of symmetry. If a complex lacks symmetry elements such as a plane or center of symmetry, it can be chiral and, consequently, demonstrate optical isomerism. For instance, the cis-[V(en)₂ClBr] complex has no symmetry elements and thus is chiral, capable of existing as two enantiomers. These enantiomers will rotate the plane of polarized light in opposite directions, giving them optical activity.

Coordination Compounds

Coordination compounds, also known as coordination complexes, are molecules that consist of a central metal atom or ion bonded covalently to a set of molecules or ions known as ligands. The ligands are species that can donate a pair of electrons to the metal atom, establishing the coordinate bond. The charges, if any, on the coordination complex result from the charges of the central metal ion and the total charge of the ligands attached to it.

The number of ligands attached to the metal center is termed the 'coordination number', and it plays a crucial role in determining the geometry of the complex. Coordination compounds can exhibit a variety of colors, magnetic properties, and reactivities, which makes them interesting subjects in chemistry and of immense importance in biological systems, catalysis, and materials science.

Metal Complex Geometries

The arrangement of ligands around the central metal ion in a coordination compound is described by the complex's geometry. Some typical geometries include linear, square planar, tetrahedral, and octahedral. Each geometry includes its specific spatial arrangement which influences the compound's properties and reactivity.

For example, the square planar geometry, usually observed with coordination number 4, can be found in certain metal complexes like the [Pd(en)(CN)₂] mentioned earlier. The square planar arrangement often leads to differentiated positions known as 'cis' (adjacent) and 'trans' (opposite) for the ligands. An octahedral geometry, corresponding to a coordination number of 6, has more possibilities for variation. It can lead to 'cis' and 'trans' forms, as well as 'facial' (fac) and 'meridional' (mer) isomers, depending on the relative positions of identical ligands. The specific spatial arrangements of ligands in these geometries are central to the concept of chirality in complexes, as the lack of symmetry required for optical activity depends heavily on geometry.