1s 2s 2p 3s 3p 4s 3d 4p
Why do electron configurations have 3d orbitals out of order from the rest?
Here we break down how radial and angular nodes create a situation where 3d orbitals experience a greater repulsion from other electrons than 4s electrons do. This is in spite of the fact that 4s have a further average distance from the nucleus.
The end result is that 4s and 3d orbital states have similar energies and this creates scenarios where the lowest energy configuration depends on a myriad of factors (nuclear charge, quantum spin pairing, etc.)
This also can help explain why some of the exceptions to Aufbau are seen such as Cr being a 4s1 3d5 instead of 4s2 3d 4.
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