1. Pauli’s Exclusion Principle
Every electron does its “own thing” 2

2. Summary of Bohr’s Model (1913)
Electrons are in different orbits at fixed distances from nucleus.
Electrons that leave one orbit must move to another orbit.
Electrons only change orbits if specific amounts (quanta) of extra energy from the outside world are involved.
Electrons that receive enough extra energy from the outside world can leave the atom they are in.
Electrons that return to orbits they used to reside in give up the extra energy they acquired when they moved in the first place.
Electronic energy given up when electrons move back into an original orbit often shows up as a specific color light.

3. The Exclusion Principle
No two electrons in the same atom can have the same set of 4 quantum number values.
Wolfgang Ernst Pauli
Wolfgang Ernst Pauli
Nobel prize in 1945

4. Four Quantum Number Bohr Atom Model
the principal quantum number
the angular momentum (azimuthal) quantum number n l
the magnetic quantum number m s
the electron spin quantum number
EVERY electron has its own individual set of quantum number values
Short hand way to use 4 quantum numbers to describe electron energy levels.
The three lowest energy terms (orbits) for a lithium atom.
1, 0, 0, +1/2
1, 0, 0, -1/2
2, 0, 0, +1/2
The short hand notation for lithium atom electron energy levels. 1s 2s

5. Try three more examples.
Atoms with electron configurations that have the lowest energy possible are in their GROUND STATE.
The short hand notation for lithium atom electrons in the ground state. 2s 1s
arrow indicates the electron spin direction.
Try three more examples.
(1)
What is the ground state electron configuration for a nitrogen atom (atomic number 7)? 1s 2s 2p 2p 2p x y z
(2)
What are the lowest energy terms (orbits) for a fluorine atom (atomic number 9)? 1s 2s 2p 2p 2p x y z
(3)
What are the lowest energy terms (orbits) (the ground state) for a neon atom
(atomic number 10)? 1s 2s 2p 2p 2p x y z

6. The ground state electron configuration for atoms from atomic number 1 (hydrogen) through atomic number 18 (argon) are determined by a repetitive pattern with no two electrons having the same set of quantum numbers.
2 electrons (electron pairs have opposite spins) 1s
A maximum of 9 energy states
2 electrons
6 electrons 2s [ 2p x 2p y 2p z ]
A maximum of 2 electrons in each energy state
2 electrons
6 electrons 3s [ 3p x 3p y 3p z ]

7. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K1 He 2 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19
Various shorthand ways to describe the ground state electron configuration for beryllium, fluorine and some of the other first 18 atoms in the periodic table are shown below. 2p x 1s 2s 3s 4s Ne Be Ar y 2 6 z
Are there other common shorthand notations for Fluorine? 2s 1s 2p x y z 1s 2 , 2s 2p 5
And/or

8. n l 7 quick review questions. 1s (1)2p 1s 3s 2s 3p
the principal quantum number
the angular momentum (azimuthal) quantum number n l
the magnetic quantum number m s
the electron spin quantum number
7 quick review questions. 1s
(1)
What is the order for filling the energy levels for the first 18 atoms of the periodic table? 2s 2p 3s 3p
(2)
What is the 4 quantum number pattern ( n l m s
) for each of argon’s 18 electrons?

9. Argon’s 18 electrons 2p 1s 3s 2s 3p 1, 0, 0, +1/2 1, 0, 0, -1/2
1, 0, 0, -1/2
2, p , +1/2 x
2, p , +1/2 y
2, p , +1/2 z
2, 0, 0, +1/2
2, 0, 0, -1/2
2, p , -1/2 x
2, p , -1/2 y
2, p , -1/2 z
3, p , +1/2 x
3, p , +1/2 y
3, p , +1/2 z
3, 0, 0, +1/2
3, 0, 0, -1/2
3, 1, -1 , -1/2
3, p , -1/2 x
3, p , -1/2 y
3, 1, 0 , -1/2
3, 1, +1 , -1/2
3, p , -1/2 z
(remember that: p x
is short hand for 1, -1 y
is short hand for 1, 0 z
is short hand for 1,+1
and either symbol represents the quantum number values.

10. 2p 1s 3s 2s 3p
(3)
What are the values of the four quantum numbers for argon’s last electron?
1, 0, 0, +1/2
1, 0, 0, -1/2
2, p , +1/2 x
2, p , +1/2 y
2, p , +1/2 z
2, 0, 0, +1/2
2, 0, 0, -1/2
2, p , -1/2 x
2, p , -1/2 y
2, p , -1/2 z
3, p , +1/2 x
3, p , +1/2 y
3, p , +1/2 z
3, 0, 0, +1/2
3, 0, 0, -1/2
3, 1, -1 , -1/2
3, 1, 0 , -1/2
3, 1, +1 , -1/2
(remember that p x
is short hand for 1, -1 y
is short hand for 1, 0 z
is short hand for 1,+1
and either symbol represents the quantum number values.)

11. 2p 1s 3s 2s 3p
(4)
What are the quantum number values for all 18 electrons that have n = 3?
3, 0, 0, +1/2
3, 0, 0, -1/2
These two electrons are called “3s” electrons }
3, 1, -1, +1/2
3, 1, -1 , -1/2
3, 1, 0 , +1/2
3, 1, 0 , -1/2
These six electrons are called “3p” electrons
3, 1,+1, +1/2
3, 1,+1 , -1/2 }
3, 2, -2, +1/2
3, 2, -2 , -1/2
3, 2, -1 , +1/2
3, 2, -1 , -1/2
3, 2, 0, +1/2
3, 2, 0, -1/2
These ten electrons are called “3d” electrons
3, 2,+1, +1/2
3, 2,+1 , -1/2
3, 2,+2, +1/2
3, 2,+1 , -1/2

12. Four Quantum Number Bohr Atom Model2p 1s 3s 2s 3p
Four Quantum Number Bohr Atom Model 3d 4d 4f 4s 4p
One last (little) twist!
(5)
How many:
n=1 electrons are possible?
n=2 electrons are possible?
n=3 electrons are possible?
n=4 electrons are possible? 1s
( 2)
2 electrons
( 8) 2s
2 electrons 2p
6 electrons
(18) 3s
2 electrons 3p
6 electrons 3d
10 electrons
(32) 4s
2 electrons 4p
6 electrons 4d
10 electrons 4f ?

13. The 4 quantum number label for the last 3p electron is 3, 1, +1, -1/23d 4d 4f 4s 4p
The 4 quantum number label for the last 3p electron is
3, 1, +1, -1/2
The 4 quantum number label for the first 3d electron is
3, 2, -2, +1/2
(6)
What are the values of 4 quantum numbers associated with the first 4f electron?
4, 3, -3, +1/2

14. Note: The last electron in each of these elements is a “s” electron.2p 1s 3s 2s 3p 3d 4d 4f 4s 4p
(7)
What are the quantum number values for the last electron of the elements in the first column of the periodic table? H 1
1, 0, 0, +1/2 Li 3
2, 0, 0, +1/2 Na 11
3, 0, 0, +1/2 K 19
4, 0, 0, +1/2
Note: The last electron in each of these elements is a “s” electron.
Remember 0 is also the same a s.