How it works
A free metal ion's five d orbitals are equal in energy. Ligands around the ion push some of them higher than others. Each chart shows one arrangement of ligands, with blank lines for the levels.
Read the full guide
Square planar
Four ligands sit along the x and y axes. From the top the levels are dx²-y², then dxy, then dz², then dxz and dyz together at the bottom. The orbitals that point at the ligands are pushed up the most.
Octahedral and tetrahedral
With six ligands on the axes, dz² and dx²-y² form the upper level and dxy, dxz and dyz the lower. With four ligands at the corners of a tetrahedron the pattern turns over and the gap is smaller.
- The orbitals named z² and x²-y² point along the axes; the other three point between them.
- One level can hold two or three orbitals of equal energy.
Questions and answers
What is the order of the d orbitals in a square planar complex?
From highest energy to lowest: dx²-y², dxy, dz², then dxz and dyz at the same level. That is the order general chemistry texts draw.
Why do the d orbitals split in an octahedral field?
Two of them, dz² and dx²-y², point straight at the six ligands and are repelled most. The other three, dxy, dxz and dyz, lie between the ligands and stay lower. The gap between the two sets is written Δo.
How is tetrahedral splitting different from octahedral?
It is the other way up: dz² and dx²-y² are the lower set and dxy, dxz and dyz the upper. The gap is smaller too, about four ninths of the octahedral gap for the same metal and ligands.
Can I practice here for “label the d orbitals in the following d-orbital energy diagram of a square-planar complex”?
Yes, for practice. That sentence is the instruction of a labeling exercise. This chart is our own drawing and not a copy of any course figure. The order of the lower levels can differ between complexes, so follow your own text.