Square pyramidal molecular geometry

Idealized structure of a compound with square pyramidal coordination geometry.
Structure of xenon oxytetrafluoride, an example of a molecule with the square pyramidal coordination geometry.

In molecular geometry, square based pyramidal geometry describes the shape of certain compounds with the formula ML5 where L is a ligand. If the ligand atoms were connected, the resulting shape would be that of a pyramid with a square base. The point group symmetry involved is of type C4v. The geometry is common for certain main group compounds that have a stereochemically active lone pair, as described by VSEPR theory. Certain compounds crystallize in both the trigonal bipyramidal and the square pyramidal structures, notably [Ni(CN)5]3−.[1]

As a transition state in Berry Pseudorotation

As a trigonal bipyramidal molecule undergoes Berry pseudorotation, it proceeds via an intermediary stage with the square planar geometry. Thus even though the geometry is rarely seen as the ground state, it is accessed by a low energy distortion from a trigonal bipyramid.

Pseudorotation also occurs in square pyramidal molecules. Molecules with this geometry, as opposed to trigonal bipyramidal, exhibit heavier vibration. The mechanism used is similar to the Berry mechanism.

Examples

Some molecular compounds that adopt square pyramidal geometry are XeOF4,[2] and various halogen pentafluorides (XF5, where X = Cl, Br, I).[3][4] Complexes of vanadium(IV), such as [VO(acac)2] are square pyramidal (acac = acetylacetonate, the deprotonated anion of acetylacetone (2,4-pentanedione)).

See also

References

  1. ↑ Spiro, Thomas G.; Terzis, Aristides; Raymond, Kenneth N. (1970). "Structure of Ni(CN)53−. Raman, infrared, and x-ray crystallographic evidence". Inorg. Chem. 9 (11): 2415. doi:10.1021/ic50093a006.
  2. ↑ "Square Pyramidal Molecular Geometry". VSEPR. http://www.up.ac.za/academic/chem/mol_geom/planpyr.htm
  3. ↑ "Square Pyramidal Geometry". http://intro.chem.okstate.edu/1314F97/Chapter9/5BP1LP.html
  4. ↑ G. L. Miessler and D. A. Tarr “Inorganic Chemistry” 3rd Ed, Pearson/Prentice Hall publisher, ISBN 0-13-035471-6.

External links

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