As we stated earlier, the periodic law influences the electron arrangements of the elements and the electron orbital diagrams are the visual representation of electrons within orbitals. Now we're going to say here we have what are called degenerate orbitals. These are electrons in the same set of orbitals having same energy and they're filled using Hans rule. Now Hans rule says that these degenerate orbitals are first half filled before being totally filled.
So if we take a look here, we have our sublevel or subshell can hold a maximum of two electrons. It has one orbital. Within that orbital we have two electrons. One spins up, one spins down. So that would mean that the sublevel has a maximum of two electrons. For P sublevel we have 3 orbitals. Following Hun's rule we would half fill them first. So we go up, up, up. Each orbital we know can hold a maximum of two electrons, so we come back around, down, down, down. So the P sublevel holds a maximum of 6 electrons.
For D we have 5 orbitals. Here. Hans Rule says we have filled them first. Since they're all D set of orbitals, they all have similar energy. So then we come back around down, down, down, down, down for a total of 10 electrons. And then finally the F sublevel has seven of these orbitals. Half fill them again according to Hun's rule. So only half of them, according to Han's rule, come back around to totally fill them in. When we do that, we get a total of 14 electrons.
So just remember, periodic law influences the electron arrangement of elements, and it's these orbital diagrams that depict the visual representation of electron within any given orbital based on sub shell level or subshell letter. So just keep that in mind. S can hold a maximum of two electrons, P can hold up to 6D, can hold up to 10, and F can hold up to 14.