Orbital Diagrams,
Electron Configurations,
and Dot diagrams
Unit 2
(Chapter 13)
Rules for filling e- in the e- cloud.
Aufbau Principle:
Electrons fill lowest energy levels 1st.
Pauli Exclusion Principle:
An orbital can only hold two e- and they must
have opposite spin.
(Cannot have the same 4 quantum numbers)
Hund’s Rule:
Sublevels with multiple orbitals (p, d, f) must
fill orbitals one at a time before doubling up.
1s
2s
2p
1.
A)
Manganese Z = 25
orbital
diagram
1s
2s
2p

3s
3p
4s
3d
B) electron
 1s2 2s2 2p6 3s2 3p6 4s2 3d5
configuration
C) Dot diagram
Mn
Mn
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
2.
A)
Oxygen
orbital
diagram
Z = 8

B) electron

configuration
C) Dot diagram
1s
1s2
2s
2p
2s2
O
2p4
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
3.
A)
Magnesium Z = 12
orbital
diagram
1s
2s
2p

3s
B) electron
 1s2 2s2 2p6 3s2
configuration
C) Dot diagram
Mg
Mg
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
4.
A)
Iron Z = 26
orbital
diagram
1s
2s
2p
Make sure you corrected your
worksheet

3s
3p
4s
3d
B) electron
 1s2 2s2 2p6 3s2 3p6 4s2 3d6
configuration
C) Dot diagram
Fe
Fe
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
5.
A)
Arsenic
orbital
diagram
1s
2s
2p
Z = 33

3s
3p
4s
4p
3d
B) electron
 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
configuration
C) Dot diagram
As
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
6.
A)
Neon Z = 10
orbital
diagram
1s
2s

2p
B) electron
 1s2 2s2 2p6
configuration
C) Dot diagram
Ne
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
7.
A)
Carbon
orbital
diagram
1s
2s
Z = 6

2p
B) electron
 1s2 2s2 2p2
configuration
C) Dot diagram
C
C
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
8.
A)
Tin
orbital
diagram
1s
2s
Z = 50

2p
3s
3p
4s
5s
 1s2 2s2 2p6 3s2 3p6
B) electron
configuration
C) Dot diagram
Sn
4p
3d
4d
4s2 3d10
5p
4p6 5s2 4d10
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
5p2
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
c =
9. What is the frequency of light that has a
wavelength of 685 nanometers.
nano
nano = 10-9
so this is 685 x 10-9 m
Knowns and unknown
c
=
c = 3.00 x 108 m/s

=
3.00 x
108
m/s
685 x 10-9 m
 = 4.38 x 10
14
1/s
ν = ______________
685 x 10-9 m
λ = ______________
10. What is the energy of a photon of radiation emitted
by a radio station broadcasting at 93.7 MHz
MHz?
Mega (M) = 106
so this is 93.7 x 106 Hz
Knowns and unknown
E = h
h = 6.626 x 10-34 J•s
E = (6.626 x
10-34
E = 6.21 x
10-26
J•s) (93.7 x
J
106
s-1)
93.7 x 106 Hz
ν = ______________
E = ______________