Rule |
Description |
|
1) |
Pauli exclusion principle* |
No two electrons may have the same set of quantum
numbers |
2) |
selecting n |
(For any particular l) the lower the value
of n, the lower the energy. |
3) |
selecting l |
(For any particular n) the lower the value
of l the lower the energy. |
4) |
selecting ml |
In filling ml, initially they all
have the same energy value. |
5) |
selecting ms |
Initially ms either + or − have
the same energy |
6) |
Hund's rule |
If either ml or m
s could be changed to the next electron, ml
changes before ms. |
1) |
For the principal quantum number, n: |
n = 1 or 2 or 3 or 4 .... i.e. an
even positive integer. |
2) |
For the subsidiary quantum number, l: |
0 =< l =< n-1 |
3) |
For the magnetic quantum number, ml
: |
-l =< ml =<
+l |
4) |
For the spin quantum number, ms
: |
ms = +1/2 or -1/2 |
* electrons must also always obey the Pauli exclusion principle.
Click here to see the electron quantum numbers of the ground states for the first 10 atoms.