Notice the energy change for an electron moving in two energy levels (from energy level 4 to energy level 2) compared to the energy change for an electron
moving in only one energy level (from energy level 3 to energy level 1). Why
doesn't the electron lose twice as much energy when it moves in two levels as it
loses when it moves only one energy level?
Hint: look at the diagram of energy levels.

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

the millers tale is the answer.