1. Quantum Numbers

2. Quantum Numbers PRINCIPAL: n energy level,
the distance the orbital is from the nucleus
(1, 2, 3, 4…)
ANGULAR MOMENTUM: l shape
(s = 0, p = 1, d = 2, f = 3)
MAGNETIC: ml spatial orientation
0 for s
-1, 0, +1 for p
-2, -1, 0, +1, +2 for d, etc.
SPIN: ms spin (+1/2 or -1/2)

3. Principle Quantum # (n)
1st Quantum #
Principle Quantum #
(n)
Specifies the energy level that the electron is on.

4. Specifies the shape of the sub level .
2nd Quantum #
(l)
Specifies the shape of the sub level .

5. Quantum Numbers The angular momentum quantum number has the symbol .
 = s, p, d, f, g, h, (n-1)
 tells us the shape of the orbitals.
These orbitals are the volume around the atom that the electrons occupy 90-95% of the time.

6. The 3rd (m) and 4th quantum numbers (s) …
Deals with the orbital within the sublevel and the spin of the electron.

7. Quantum Numbers
The symbol for the magnetic quantum number is m, representing the spatial orientation.
m = -  , (-  + 1), (-  +2), , , ( -2), ( -1), 
If  = 0 (or an s orbital), then m = 0.
If  = 1 (or a p orbital), then m = -1,0,+1. y z x

8. If  = 2 (or a d orbital), then m = -2,-1,0,+1,+2.
If  = 3 (or an f orbital), then m = -3,-2,-1,0,+1,+2, +3.
Theoretically, this series continues on to g,h,i, etc

9. Four Energy Sub-Levels
Energy Level
Sub-level
Type of sub
# of Orbitals s
Sphere 2 1 p
Dumbbell 6 3 d
4-Lobed 10 5 f
6-8 Lobed 14 7

10. Spin quantum number
The last quantum number is the spin quantum number which has the symbol ms.
The spin quantum number only has two possible values.
ms = +1/2 or -1/2

11. Spin of electron

12. Practice
When n = 3, l can have a value of? For the 3d orbital, I has a value of?
What electron are we talking about if it has the quantum numbers of n = 2, l = 1, ml = -1 and spin of -1/2?