Octahedral molecular geometry

In chemistry, octahedral molecular geometry, also called square bipyramidal,^[1] describes the shape of compounds with six atoms or groups of atoms or ligands symmetrically arranged around a central atom, defining the vertices of an octahedron. The octahedron has eight faces, hence the prefix octa. The octahedron is one of the Platonic solids, although octahedral molecules typically have an atom in their centre and no bonds between the ligand atoms. A perfect octahedron belongs to the point group O_h. Examples of octahedral compounds are sulfur hexafluoride SF₆ and molybdenum hexacarbonyl Mo(CO)₆. The term "octahedral" is used somewhat loosely by chemists, focusing on the geometry of the bonds to the central atom and not considering differences among the ligands themselves. For example, [Co(NH₃)₆]³⁺, which is not octahedral in the mathematical sense due to the orientation of the N−H bonds, is referred to as octahedral.^[2]

Octahedral molecular geometry
Examples	SF6, Mo(CO)6
Point group	Oh
Coordination number	6
Bond angle(s)	90°
μ (Polarity)	0

The concept of octahedral coordination geometry was developed by Alfred Werner to explain the stoichiometries and isomerism in coordination compounds. His insight allowed chemists to rationalize the number of isomers of coordination compounds. Octahedral transition-metal complexes containing amines and simple anions are often referred to as Werner-type complexes.

Structure of sulfur hexafluoride, an example of a molecule with the octahedral coordination geometry.

Isomerism in octahedral complexes

Main article: Stereochemistry

When two or more types of ligands (L^a, L^b, ...) are coordinated to an octahedral metal centre (M), 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 ML^a
₄L^b
₂, two isomers exist. These isomers of ML^a
₄L^b
₂ are cis, if the L^b ligands are mutually adjacent, and trans, if the L^b groups are situated 180° to each other. It was the analysis of such complexes that led Alfred Werner to the 1913 Nobel Prize–winning postulation of octahedral complexes.

• 
  cis-[CoCl₂(NH₃)₄]⁺
• 
  trans-[CoCl₂(NH₃)₄]⁺

Facial and meridional isomers

For ML^a
₃L^b
₃, two isomers are possible - a facial isomer (fac) in which each set of three identical ligands occupies one face of the octahedron surrounding the metal atom, so that any two of these three ligands are mutually cis, and a meridional isomer (mer) in which each set of three identical ligands occupies a plane passing through the metal atom.

• 
  fac-[CoCl₃(NH₃)₃]
• 
  mer-[CoCl₃(NH₃)₃]

Δ vs Λ isomers

Complexes with three bidentate ligands or two cis bidentate ligands can exist as enantiomeric pairs. Examples are shown below.

• 
  Λ-[Fe(ox)₃]³⁻
• 
  Δ-[Fe(ox)₃]³⁻
• 
  Λ-cis-[CoCl₂(en)₂]⁺
• 
  Δ-cis-[CoCl₂(en)₂]⁺

Other

For ML^a
₂L^b
₂L^c
₂, a total of five geometric isomers and six stereoisomers are possible.^[3]

1. One isomer in which all three pairs of identical ligands are trans
2. Three isomers in which one pair of identical ligands (L^a or L^b or L^c) is trans while the other two pairs of ligands are mutually cis.
3. Two enantiomeric pair in which all three pairs of identical ligands are cis. These are equivalent to the Δ vs Λ isomers mentioned above.

The number of possible isomers can reach 30 for an octahedral complex with six different ligands (in contrast, only two stereoisomers are possible for a tetrahedral complex with four different ligands). The following table lists all possible combinations for monodentate ligands:

Formula	Number of isomers	Number of enantiomeric pairs
ML6	1	0
MLa 5Lb	1	0
MLa 4Lb 2	2	0
MLa 4LbLc	2	0
MLa 3Lb 3	2	0
MLa 3Lb 2Lc	3	0
MLa 3LbLcLd	5	1
MLa 2Lb 2Lc 2	6	1
MLa 2Lb 2LcLd	8	2
MLa 2LbLcLdLe	15	6
MLaLbLcLdLeLf	30	15

Thus, all 15 diastereomers of ML^aL^bL^cL^dL^eL^f are chiral, whereas for ML^a
₂L^bL^cL^dL^e, six diastereomers are chiral and three are not (the ones where L^a are trans). One can see that octahedral coordination allows much greater complexity than the tetrahedron that dominates organic chemistry. The tetrahedron ML^aL^bL^cL^d exists as a single enantiomeric pair. To generate two diastereomers in an organic compound, at least two carbon centers are required.

Deviations from ideal symmetry

Jahn–Teller effect

Main article: Jahn–Teller effect

The term can also refer to octahedral influenced by the Jahn–Teller effect, which is a common phenomenon encountered in coordination chemistry. This reduces the symmetry of the molecule from O_h to D_4h and is known as a tetragonal distortion.

Distorted octahedral geometry

Some molecules, such as XeF₆ or IF⁻
₆, have a lone pair that distorts the symmetry of the molecule from O_h to C_3v.^[4][5] The specific geometry is known as a monocapped octahedron, since it is derived from the octahedron by placing the lone pair over the centre of one triangular face of the octahedron as a "cap" (and shifting the positions of the other six atoms to accommodate it).^[6] These both represent a divergence from the geometry predicted by VSEPR, which for AX₆E₁ predicts a pentagonal pyramidal shape.

Bioctahedral structures

Pairs of octahedra can be fused in a way that preserves the octahedral coordination geometry by replacing terminal ligands with bridging ligands. Two motifs for fusing octahedra are common: edge-sharing and face-sharing. Edge- and face-shared bioctahedra have the formulas [M₂L₈(μ-L)]₂ and M₂L₆(μ-L)₃, respectively. Polymeric versions of the same linking pattern give the stoichiometries [ML₂(μ-L)₂]_∞ and [M(μ-L)₃]_∞, respectively.

The sharing of an edge or a face of an octahedron gives a structure called bioctahedral. Many metal pentahalide and pentaalkoxide compounds exist in solution and the solid with bioctahedral structures. One example is niobium pentachloride. Metal tetrahalides often exist as polymers with edge-sharing octahedra. Zirconium tetrachloride is an example.^[7] Compounds with face-sharing octahedral chains include MoBr₃, RuBr₃, and TlBr₃.

• 
  Ball-and-stick model of niobium pentachloride, a bioctahedral coordination compound.
• 
  Ball-and-stick model of zirconium tetrachloride, an inorganic polymer based on edge-sharing octahedra.
• 
  Ball-and-stick model of molybdenum(III) bromide, an inorganic polymer based on face-sharing octahedra.
• 
  View almost down the chain of titanium(III) iodide highlighting the eclipsing of the halide ligands in such face-sharing octahedra.

Trigonal prismatic geometry

Main article: trigonal prismatic molecular geometry

"Trigonal prism" redirects here. For the three-sided prism, see Triangular prism.

For compounds with the formula MX₆, the chief alternative to octahedral geometry is a trigonal prismatic geometry, which has symmetry D_3h. In this geometry, the six ligands are also equivalent. There are also distorted trigonal prisms, with C_3v 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-orbital energies

Main article: Ligand field theory

For a free ion, e.g. gaseous Ni²⁺ or Mo⁰, the energy of the d-orbitals are equal in energy; that is, they are "degenerate". In an octahedral complex, this degeneracy is lifted. The energy of the d_z² and d_x²−y², the so-called e_g set, which are aimed directly at the ligands are destabilized. On the other hand, the energy of the d_xz, d_xy, and d_yz orbitals, the so-called t_2g set, are stabilized. The labels t_2g and e_g 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 Δ_o, which varies according to the number and nature of the ligands. If the symmetry of the complex is lower than octahedral, the e_g and t_2g levels can split further. For example, the t_2g and e_g sets split further in trans-ML^a
₄L^b
₂.

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 Δ_o and absorb light at longer wavelengths.

Reactions

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 changes 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 an anation. The reverse reaction, water replacing an anionic ligand, is called aquation. For example, the [CoCl(NH₃)₅]²⁺ slowly yields [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.

See also

• Octahedral clusters
• AXE method
• Molecular geometry

References

1. "Trigonal bipyramidal molecular shape @ Chemistry Dictionary & Glossary". glossary.periodni.com. Retrieved 2022-07-03.
2. Von Zelewsky, A. (1995). Stereochemistry of Coordination Compounds. Chichester: John Wiley. ISBN 0-471-95599-X.
3. Miessler, G. L.; Tarr, D. A. (1999). Inorganic Chemistry (2nd ed.). Prentice-Hall. p. 290. ISBN 0-13-841891-8.
4. Crawford, T. Daniel; Springer, Kristen W.; Schaefer, Henry F. (1994). "A contribution to the understanding of the structure of xenon hexafluoride". Journal of Chemical Physics. 102 (8): 3307–3311. Bibcode:1995JChPh.102.3307C. doi:10.1063/1.468642.
5. Mahjoub, Ali R.; Seppelt, Konrad (1991). "The Structure of IF⁻
   ₆". Angewandte Chemie International Edition. 30 (3): 323–324. doi:10.1002/anie.199103231.
6. Winter, Mark (2015). "VSEPR and more than six electron pairs". University of Sheffield: Department of Chemistry. Retrieved 25 September 2018. the structure of XeF₆ is based upon a distorted octahedron, probably towards a monocapped octahedron
7. Wells, A.F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 0-19-855370-6.

External links

• Example of octahedral geometry at 3dCHEM.com
• Indiana University Molecular Structure Center
• Point Group Symmetry Examples