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Hund's rule basically states that for a subshell with multiple orbitals, then you fill each orbital with one electron first before you fill a single orbital with two electrons. So for example, when you're filling in the p-orbitals, you fill up the px-, py-, and pz-orbitals with one electron each before you fill up the px-orbital with two electrons. The spin numbers are paired when you're filling up the separate orbitals with one electron.
Hund's rule is filling out orbitals with single same spin electrons before you pair them up in the same orbital. Pauli exclusion principle relates to 2 electrons in the same orbitals must have opposite spins.
I'm not sure if I completely understand the question but what I know about Hund's rule is that every orbital in a sublevel is singly occupied before any orbital is doubly occupied. All of the electrons in singly occupied orbitals have the same spin (to maximize total spin).
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