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Octahedral molecular geometry


In chemistry, octahedral molecular geometry describes a molecular geometry in which 6 ligands are symmetrically arranged around a central atom in an octahedral geometry. All six ligands are chemically equivalent. The central atom is often a transition metal. The octahedron has eight faces (hence the prefix octa) and thus is one of the Platonic solids (although octahedral molecules typically have an atom in their centre, which the Platonic solids don't. A perfect octahedron belongs to the point group Oh. Examples of octahedral compounds are sulfur hexafluoride (SF6) and molybdenum hexacarbonyl. The term octahedral is used somewhat loosely: [Co(NH3)6]3+, which is not strictly octahedral in the mathematical sense due to the orientation of the N-H bonds, is referred to as octahedral.[1]

The concept of octahedral transition metal compounds was developed by Alfred Werner. His insight allowed chemists to understand much prior coordination chemistry. Octahedral transition-metal complexes containing amines and simple anions are often referred to Werner-type complexes.



When two or more types of ligands are coordinated to an octahedral metal centre, the complex can exist as isomers. The naming system for these isomers depends upon the number and arrangement of different ligands.

  • Cis and Trans

For MLa4Lb2, two isomers exist. These isomers of MLa4Lb2 are cis, if the Lb ligands are mutually adjacent, and trans, if the Lb groups are situated 180° to each other. It was the analysis of such complexes that lead Alfred Werner to the 1913 Nobel Prize winning postulation of octahedral complexes.

For MLa2Lb2Lc2, cis and trans isomers are also possible. All three types of ligands La, Lb and Lc may be trans, or one type may be trans while the other two are cis. This latter case gives two unique isomers (for a total of three).

  • Facial and Meridional

For MLa3Lb3, two isomers are possible - a facial isomer (fac) where the three identical ligands are mutually cis, and a meridional isomer (mer) where the three ligands are coplanar.

  • Chirality

More complicated complexes, with several different kinds of ligands or with bidentate ligands can also be chiral.

  • Other

The number of possible isomers can reach 30 for a complex with six different ligands. The following table lists all possible combinations for monodentate ligands:

Formula Number of isomers Number of enantiomeric pairs
ML6 1 0
MLa5Lb 1 0
MLa4Lb2 2 0
MLa3Lb3 2 0
MLa4LbLc 2 0
MLa3Lb2Lc 3 0
MLa2Lb2Lc2 6 1
MLa3LbLcLd 5 1
MLa2Lb2LcLd 8 2
MLa2LbLcLdLe 15 6
MLaLbLcLdLeLf 30 15

Thus, all 15 diastereomers of MLaLbLcLdLeLf are chiral, whereas for MLa2LbLcLdLe, six diastereomers are chiral and three are not: the ones where La are trans. One can see that octahedral coordination allows much greater complexity that the tetrahedron that dominates organic chemistry. The tetrahedron MLaLbLcLd exists as a single enatiomeric pair. To generate two diastereomers in an organic compound, at least two carbon centers are required.

Trigonal prismatic geometry

For compounds with the formula MX6, the chief alternative to octahedral geometry is a trigonal prismatic geometry, which has symmetry D3h. In this geometry, the six ligands are also equivalent. There are also distorted trigonal prisms, with C3v symmetry; a prominent example is W(CH3)6. The interconversion of Δ- and Λ-complexes, which is usually slow, is proposed to proceed via a trigonal prismatic intermediate, a process called the "Bailar twist." An alternative pathway for the racemization of these same complexes is the Ray-Dutt twist.

Splitting of d-orbitals in octahedral complexes

Main article: Ligand field theory

For a "free ion", e.g. gaseous Ni2+ or Mo0, the d-orbitals are equi-energetic, that is they are "degenerate." In an octahedral complex, this degeneracy is lifted. The dz2 and dx2-y2, the so-called eg set, which are aimed directly at the ligands are destabilized. On the other hand, the dxz, dxy, and dyz orbitals, the so-called t2g set, are not. The labels t2g and eg refer to irreducible representations, which describe the symmetry properties of these orbitals. The energy gap separating these two sets is the basis of Crystal Field Theory and the more comprehensive Ligand Field Theory. The loss of degeneracy upon the formation of an octahedral complex from a free ion is called "crystal field splitting" or "ligand field splitting." The energy gap is labeled Δo, which varies according to the nature of the ligands. If the symmetry of the complex is lower than octahedral, the eg and t2g levels can split further. For example, the t2g and eg sets split further in trans-MLa4Lb2.

Ligand strength has the following order for these electron donors: weak: iodine < bromine < fluorine < acetate < oxalate < water < pyridine < cyanide :strong

So called "weak field ligands" give rise to small Δo and absorb light at longer wavelengths.


Given that a virtually uncountable variety of octahedral complexes exist, it is not surprising that a wide variety of reactions have been described. These reactions can be classified as follows:

  • Ligand substitution reactions (via a variety of mechanisms)
  • Ligand addition reactions, including among many, protonation
  • Redox reactions (where electrons are gained or lost)
  • Rearrangements where the relative stereochemistry of the ligand change within the coordination sphere.

Many reactions of octahedral transition metal complexes occur in water. When an anionic ligand replaces a coordinated water molecule the reaction is called a anation. The reverse reaction, water replacing an anionic ligand, is called an "aquation reaction." For example, the [Co(NH3)5Cl]2+ slowly aquates to give [Co(NH3)5(H2O)]3+ in water, especially in the presence of acid or base. Addition of concentrated HCl converts the aquo complex back to the chloride, via an anation process.


  1. ^ von Zelewsky, A. "Stereochemistry of Coordination Compounds" John Wiley: Chichester, 1995. ISBN 047195599.

See also

This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Octahedral_molecular_geometry". A list of authors is available in Wikipedia.
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