To form a molecule with a trigonal bipyramidal electron geometry, we need to mix atomic orbitals that will result in five hybrid orbitals for bonding. There should be three equatorial orbitals and two axial orbitals for this molecular geometry.
To achieve this, an s orbital (which is spherical and has one orientation) can be mixed with three p orbitals (each of which have two orientations and are perpendicular to each other in space), and one d orbital (which has multiple orientations).
When one s, three p, and one d orbitals mix together, they form a set of five sp3d hybrid orbitals. These orbitals arrange themselves in a trigonal bipyramidal geometry, as it allows them to minimize electron-electron repulsion and have the most stable arrangement.
In summary, mixing one s, three p, and one d orbitals creates five hybrid orbitals (sp3d) that have a trigonal bipyramidal electron geometry.
To form a molecule with a trigonal bipyramidal electron geometry, what set of pure atomic orbitals must be mixed?
The answer is one s, three p, and one d. How do you figure this out?
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