5. Memory Device to Remember the Order of Orbitals
1s,
2s, 2p,
3s, 3p,
4s, 3d, 4p,
5s, 4d, 5p, 6s,
4f, 5d, 6p, 7s, 5f…
Remember this!
6. Guide
• THE AUFBAU
PRINCIPLE (Building
up principle): Electrons
are added to atomic
orbitals starting with the
lowest energy orbital and
building up to higher
energy orbitals.
8. Guide
• HUND’S RULE:
Electrons occupy
orbitals in a
sublevel one at a
time until each
orbital has 1 e-.
They will not
double up until
each orbital has
at least one
electron
9. Main Energy Level
(n)
(sometimes called
a “Shell”)
Sub-shells*
are
represente
d by:
Number of
orbitals**
per sub-
shell
Max Number of
e-
per
sub-shell
1 (K-Shell) s s = 1 s = 2 e-
2 (L-Shell) s, p s = 1
p = 3
s = 2 e-
p = 6 e-
3 (M-Shell) s, p, d s = 1
p = 3
d = 5
s = 2 e-
p = 6 e-
d = 10 e-
4 (N-Shell) s, p, d, f s = 1
p = 3
d = 5
f = 7
s = 2 e-
p = 6 e-
d = 10 e-
f = 14 e-
*sub-shells
s = Sharp
p = Principal
d = Diffuse
f = Fundamental
**The 3-dimensional region
around the nucleus where the
probability of finding electrons are
maximum are called orbitals.
2
1
3
4
K
L
M
N
s s s s
p p
d
p
d
f
13. QUANTUM NUMBERS
1- PRINCIPAL QUANTUM NUMBER (n).
Designates the main energy level or shell.
2- ANGULAR MOMENTUM QUANTUM
NUMBER (l). Designates the sub-level
where the electron can be found.
Gives the SHAPE OF THE ORBITALS
3- MAGNETIC QUANTUM NUMBER (ml). Specifies to
which orbital within a subshell the electron is
assigned
s subshell: ml = 0
p subshell: ml = -1, 0, 1
d subshell: ml = -2, -1, 0, 1, 2
f subshell: ml = -3, -2, -1, 0, 1, 2, 3
4- SPIN QUANTUM NUMBER (ms). Designates the
SPIN OF THE ELECTRON (describes the behavior of
the e-, not the location).
Values: +½ , -½
Arrow up ↑ is +½, arrow down ↓ is –½
The s, p, d, and f, respectively stand for sharp, primary, diffuse and fundamental. The letters and words refer to the visual impression left by the spectral lines’ fine structure that occurs because of the first relativistic corrections, particularly the spin-orbital interaction.