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The electron configuration is an abbreviated version of the orbital notation.

The orbital notation shows exactly where every electron is placed around the nucleus of the atom --> more specifically, what orbital and sublevel each electron is in and what the spin of the electron in an orbital is.

Remember the s sublevel only has 1 orbital and can hold 2 electrons with opposite spins.

the p sublevel has 3 orbitals each holding 2 electrons with a total of 6 electrons in the p sublevel.

the d sublevel has 5 orbitals each holding 2 electrons with a total of 10 electrons in the d sublevel.

the f sublevel has 7 orbitals each holding 2 electrons with a total of 14 electrons in the f sublevel.

n is the principal energy level (there are 7 maximum for a ground state electron)

l is the sublevel (there are 4 maximum for a ground state electron)

n l

1 1s2

2 2s2 2p6

3 3s2 3p6 3d10

4 4s2 4p6 4d10 4f14

5 5s2 5p6 5d10 5f14

6 6s2 6p6 6d10

7 7s2 7p6

Start with the first energy level, (the first row), and put a diagonal line through it then write it down: 1s2 Then go to the next energy level, (n = 2), and put a line through the 2s and write it down next to the 1s2: 1s2 2s2. Then finish the 2nd row by putting a line through the 2p and the 3s which is diagonally underneath it and write those down next to the 1s2 2s2: 1s2 2s2 2p6 3s2. Continue doing this until you have the entire electron configuration.

The order of electron configurations is:

1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

The orbital diagrams have the same order but you will see each orbital in the s, p, d, and f sublevels:

This is for Al, Si, P, and S.

Notice that you still draw every orbital in a sublevel (look at 3p in Al), even if you don't fill up that sublevel.

Also, notice Si: It has 2 electrons in the 3p. You don't pair them up in an orbital because there are only 2. You don't start pairing them up until you have 4, 5, or 6 electrons in the p sublevel.

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