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Assuming the electron is in the lowest states and the atom is neutrally charged, it will fill an orbital before extending the next one.

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

H and He fill 1s as it holds two electrons.

Li and Be fill 2s as it holds two electrons.

B, C, N, O, F, and Ne will fill the 2p orbital as it holds 6 electrons (2p1, 2p2, and 2p3 orbitals).

However, nitrogen will have one electron in each 2p1, 2p2, and 2p3 orbitals as an electron will not go two to an orbital until each orbital is filled.

Neon completes the 2p orbital and is very stable (considered an inert gas--electrons are neither attracted nor want to leave the completed 2p orbital). Fluorine is the most electronegative element, as it wants to rip any electron it can to fill its 2p orbital.

All noble gasses (right most on the Periodic Table) will complete a p-orbital.

Periods 3-12 will fill a d-orbital.

Lanthanoids and actinoids will fill the f-orbitals.

So, for instance, Calcium (Ca) has an atomic number 20. You look up Ca on the periodic table.

As it comes after He, it will have a 1p orbital filled.

As it comes after Be, it will have a 2s orbital filled.

As it comes after Ne, it will have a 2p orbital filled.

And Ca will have a 3s orbital filled.

Therefore, you note that Ca has electrons in the following orbitals: 1s, 2s, 2p, 3s.

Another example is Fluorine (F), which would be: 1s, 2s, 2p1(2), 2p2(2), 2p3(1) where the parenthetical numbers note the number of electrons in each orbital.

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