dffdsfdssdfs

3. proton Shell
+
N
-
+
- N
electron neutron

4. He Li
Li shorthand
2p+ 3 p+ 3 p+ 2e– 1e–
2 n0 4 n0 4 n0

5. Be B
Al
4 p+ 5 p+ 13 p+
5 n° 6 n° 14 n°
O Na
8 p+ 2e– 6e– 11 p+ 2e– 8e– 1e–
8 n° 12 n°

6. • He proposed that electron behaves
like a wave, specifically a standing
wave. A standing wave is a wave
that does not travel down its medium.
• A standing wave is obtained when one
point (called the node) in the middle
of the wave is stationary.

7. • UNCERTAINTY PRINCIPLE
• States that there is NO way to determine
both the precise location and momentum
(mass X velocity) of small particles at the
same time.
• Principle implies that if we could measure
the momentum of an electron
accurately, we could NOT determine its
location at the same time.

13. • Corresponds to the
energy level
numbers. As (n)
increases, the average
+
N
distance of an electron K L M
from the nucleus also N
+
increases. n=1
• The larger the (n) the n=2
larger the atomic n=3
orbital. n= so on…

14. • AZIMUTHAL
• The sublevels that
describes the shape of
the atomic orbitals.
+
N
K L M
• Examples: +
N
=0 s orbital
n=1
=1 p orbital n=2
=0 d orbital n=3
=1 f orbital n= so on…

15. PRINCIPAL POSSIBLE
ENERGY LEVEL (n – 1) VALUES: SUBLEVELS
(n) 0 TO (n – 1)
1 1–1=0 0 s
2 2–1=1 0,1 s,p
3 3–1=2 0,1,2 s,p,d
4 4–1=3 0,1,2,3 s,p,d,f
5 5–1=4 0,1,2,3,4 s,p,d,f,g
6 6–1=5 0,1,2,3,4,5 s,p,d,f,g,h

16. • Describes the orientation
of the atomic orbital in
space. The magnetic quantum
number can only have (2 X 1)
integral values for a particular .
+
N
• Example: K L M
N
+
=1
n=1
[ (2 X 1) + 3] or 3 m
n=2
Values. These 3 m values n=3
are -1, 0, and +1
n= so on…

17. Number of
SUBLEVEL 2 + 1 m VALUES Atomic Orbital
1 0 1s 2(0) + = 1 0 1
2 0 2s 2(0) + = 1 0 1
3 1 2p 2(1) + = 3 1, 0, -1 3
0 3s 2(0) + = 1 0 1
1 3p 2(1) + = 3 1, 0, -1 3
2 3d 2(2) + = 5 2, 1, 0, -1, -2 5

18. • Describes the spin
direction of an electron.
There are only two
possible values for the
+
electron spin quantum N
K L M
number, and these are + N
+
½ and – ½.
n=1
• ms = + ½ (clockwise)
n=2
• ms = - ½ (counter- n=3
clockwise)
n= so on…

20. • Wolfgang Pauli
• States that no two electron can be described by
the same four quantum numbers.
• Two electrons may have the same first three
quantum numbers ( ) but these two
electrons must have different spins
•

21. • Principle applies the laws in QUANTUM MECHANICS
to the distribution of electrons among energy levels
in the ground states (most stable states) of atoms.
• The word AUFBAU means “building up” in
german.
•

24. E
4d
N 5s
4p
E 4s
3d
3p
R 3s
2p
G 2s
1s
Y

25. 2 ways of
spdf notation
writing for H, atomic # = 1
configs. 1 # of e
One is 1s
called the
spdf
notation. value of l
value of n

32. Electron Arrangement in Atoms
Electrons in atoms are arranged as:
SHELLS (n)
SUBSHELLS (l)
ORBITALS (ml)