Structure & Reactivity
TM7. Geometry in Transition Metal Complexes
If you have studied Lewis structures, then you know that the number of lone pairs and atoms around a specific atoms tells you the geometry at that specific atom. Something very similar is true in coordination complexes, but it's slightly simpler. In transition metal complexes, the lone pairs on the metal do not contribute to its overall geometry. All that matters is the number of ligands attached to the metal.
In coordination complexes, the number of ligands determines the geometry.
As a result, there is a pretty straightforward correlation between coordination number (the number of ligands) and geometry.
# ligands | geometry |
2 | linear |
3 | trigonal planar |
4 | tetrahedral; sometimes square planar |
5 | trigonal bipyramidal; sometimes square pyramidal |
6 | octahedral |
There are two exceptions to that straightforward rule. There are two possble geometries for coordination number four, and two possible geometries for coordination number five. How do we know which will happen?
For coordination number five, we really can't make an easy prediction. In terms of the angles between ligands, these two possible geometries are really pretty close to each other, so the distinction is subtle. If you call everything that's five-coordinate a trigonal bipyramidal geometry, you will be in the right ballpark.
Coordination number four is a different story; we do have some predictive ability here. However, there are two different factors that come into play, so there are still some subtle cases.
The first factor is sterics or crowding. In a tetrahedron, the four ligands would be 109 degrees away from each other. In square planar geometry, the four ligands are only 90 degrees away from each other. A tetrahedral geometry is less crowded, and that makes it fairly common.
In order for a square planar geometry to form, there has to be some factor that offsets the steric preference for tetrahedral geometry. There is an electronic destabilization that can happen in tetrahedral geometry. It can happen in square planar geometry, too, but is not quite so bad when there are eight electrons on the metal. As a result, square planar geometry is most common when the metal has eight electrons.
See a more in-depth discussion of coordination complexes in a later course.
This site is written and maintained by Chris P. Schaller, Ph.D., College of Saint Benedict / Saint John's University (with contributions from other authors as noted). It is freely available for educational use.
Structure & Reactivity in Organic, Biological and Inorganic Chemistry by Chris Schaller is licensed under a Creative Commons Attribution-NonCommercial 3.0 Unported License.
Send corrections to cschaller@csbsju.edu
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