Vocab
Electron
Configuration
Orbital
Notation
Electron Dot
Misc
100
100
100
100
100
200
200
200
200
200
300
300
300
300
300
400
400
400
400
400
500
500
500
500
500
Wavelength
The distance between
peaks of a wave
Valence Electrons
Electrons in the outer shell
involved in bonding
Principle Quantum Number
The shell or level that the electron is in
DAILY DOUBLE!!!
Represented by (l). Energy
sublevel
Azimuthal
Before any second electron can be
placed in a sub level, all the
orbitals of that sub level must
contain at least one electron.
Hund’s Rule
What are the 4
metals that are
exceptions to the
“rules”?
Cr, Cu, Ag, Au
e
Long hand
configuration for:
Bromine
•
2
2
6
2
6
10
2
5
1s 2s 2p 3s 3p 3d 4s 4p
What is the “short
hand” e configuration
of:
W
14
4
2
[Xe]4f 5d 6s
What element am I….
2
2
6
2
6
5
1
1s 2s 2p 3s 3p 3d 4s
Chromium
What is the
e configuration
2+
Ca
of:
2
2
6
2
6
2
1s 2s 2p 3s 3p 4s
What 3 rules are
followed for orbital
notation?
1. Aufbau
2. Hunds
3. Pauli Exclusion
Draw the “long hand”
orbital notation for:
Fluorine
F
1s
2s
2p
“Short hand” orbital notation for:
Arsenic -3
[Ar]
3d
4s
4p
“Short Hand” orbital notation for:
silver
Ag
[Kr]
4d
5s
Daily Double!!!!!

   __
1s
2s
2p
What rule does this break?
Hund’s
(Bus)
No atom has more than
_____ e
8
Correct or Not?
..
. Cr
.. .
If not, give the
correct e dot
Incorrect
.
Cr
(Cr is an exception, only 1
valence in 4s)
Draw the e dot
+1
for Mg
.
Mg
e
Draw the dot for:
2S
..
..
..
S
..
Correct or Not?
..
:O:
If NOT, why??
Must fill, NSEW
Draw a full Bohr
model of:
Chlorine
Write the “short
hand” bohr model
for:
Na
Na )2e- )8e- )1e-
Draw a picture
showing how light is
produced
2 of Bohr’s
contributions…..
1. He explained the atomic line
spectra in terms of electron
energies
2. He introduced the idea of
quantized electron energy
levels in the atom
Complete the Chart:
Type
s
p
d
f
#
sublevels
Total # e
Shape
Type
s
p
d
f
#
sublevels
1
3
5
7
Total # e
Shape
2
6
sphere
peanut
10
14
dumbbell
flower