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Electrons in the same atom differ because they can have different quantum numbers

Further explanation

Atoms consist of sub-particles: electrons, protons, and neutrons

The proton is positively charged (+1), the electron is negatively charged (-1). and neutrons not charged (neutral)

The electron configuration shows the energy level in the atom

The further away from the core, the higher the energy level

In the electron configuration we follow 3 rules:

  • 1. Aufbau: Electrons occupy orbitals of the lowest energy
  • 2 Hund: electrons fill orbitals with the same energy level
  • 3. Pauli: no electrons have the same 4 quantum numbers

Each orbital consists of 4 quantum numbers

  • n: the principal
  • l: the angular momentum / azimuthal
  • ml: the magnetic
  • ms: the electron-spin

From Pauli's rule, an electron can have 3 same but different quantum numbers in ms (quantum spin)

For example in the 1s orbital, then the quantum value of the 2 electrons that occupy the orbital:

  • first electron: n = 1, l = 0, ml = 0, ms = +1/2
  • second electron: n = 1, l = 0, ml = 0, ms = -1/2

Therefore, in one orbital it is not allowed to fill more than 2 electrons because the quantum numbers will be the same

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