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The Pauli Exclusion principle states that in an atom, or molecule, no two electrons can have the same four quantum numbers since they cannot be at the same place at the same time with the same energy. Also, it states that an orbital can have a maximum of two electrons and electrons in the same orbital have to have opposite spins. The Hund's Rule states that all orbitals have to be filled by a one electron first before pairing them up with another electron.
The Pauli Exclusion Principle basically states that no more than 2 electrons can occupy a single orbital. Hund's Rule states that due to electron/electron repulsion, orbitals must be occupied by one electron before they can be occupied by a second electron.
Pauli's exclusion principle limits orbitals to only 2 electrons each (1 pair of electrons per orbital). Hund's rule states that an orbital must be occupied by one electron before it can be occupied by a second.
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