Unit 3
Name _______________________________ # ________
Section 1: Electromagnetic Spectrum
c= 
E=h
c= 3.0 x 108 m/s
h= 6.626 x 10-34 Js
1. What is the mathematical relationship between
a. wavelength and frequency?
b. amplitude and energy?
c. frequency and energy?
d. wavelength and energy?
2. What color of visible light has the
a. shortest wavelength?
b. highest energy?
c. lowest frequency?
3. Calculate the wavelength of a wave whose frequency is 1050 kHz.
4. Calculate the frequency of a wave with 4.5 x 10-15 kJ of energy.
5. Calculate the wavelength of a wave with an energy content of
2.8 x 10-23 J.
6. Calculate the energy of a wave whose frequency is 7.9 GHz.
7. Calculate the energy of a wave whose wavelength is 750 nm.
Section 2: Electromagnetic Radiation
c= 
E=h
c= 3.0 x 108 m/s
h= 6.626 x 10-34 Js
1. Calculate the wavelength of the wave for a radio station that operates at a
frequency of 101.9 MHz.
2. What is the frequency of a wave of green light that has a wavelength of
550 nm?
3. Calculate the energy of a wave in kJ that has a frequency of
4.7 x 1015 kHz.
4. Calculate the energy associated with a radio wave that has a wavelength
of 125m.
5. If an X-ray has an energy content of 5.8 x 10-9 kJ, calculate the
wavelength for this X-ray.
6. Calculate the frequency of a wave that has an energy content of
7.9 x 103 kJ.
7. What is the wavelength in nm of a wave that has a frequency of 2.5 GHz?
Section 3: Quantum Numbers
1. How many electrons can each orbital hold?
2. How many total electron can fit in the
a. d subshell?
b. n= 4?
c. s subshell?
d. 2nd energy level?
e. one of the p orbitals?
3. What is the lowest numbered principle shell in which
a. p orbitals are found?
b. the f subshell can be found?
4. If n= 4, what are the possible sublevels?
5. How many orbitals are found in the p sublevel?
6. If n= 3, what are the possible sublevels?
7. How many orbitals are found in the f sublevel?
Section 4: Quantum Problems
Light travels through space by means of waves. Each wave has a frequency (),
a wavelength (). The figure below represents a light wave. Label the
wavelength. Then answer questions 1 - 4.
1. Given the distance scale in micrometers, m, shown in the figure, what is
the wavelength in meters?
2. Given that 6.0 x 108 crests of the wave pass a point in 1.0 microsecond,
what is the value of the frequency of this wave in waves/sec (or Hz).
3. Calculate the product of the answers to questions 1 and 2 above.
4. What is the significance of the value just calculated?
5. What is the energy of a quantum of light with a frequency of 6.17 x 10 14 Hz
6. Solar panels rely on light's ability to remove electrons from the surface of
the solar cell. The energy required to release an electron from atoms on
the surface of the cell is 6.7 x 10-19 J. What wavelength of light would be
necessary for electrons to leave the cell's surface?
7. A certain wavelength of blue light has a frequency of 6.91 x 10 14 Hz. What
is the wavelength of this blue light?
8. What is the shape of an s sublevel? _______________
9. How many electrons can fit into each sublevel?
a. s
___________
b. p ___________
c. d ___________
d. f
___________
10. How many electrons can fit into the following?
a. n = 1
__________
b. n = 2, p sublevel
__________
c. n = 4
__________
d. n = 3, d sublevel, one orbital
__________
Section 5: Electron Configurations
1. Explain why each of the following is not reasonable for a ground-state
atom.
a. 1s22s22p63s13p1
b. 1s22s22p63s23p63d1
c. 1s22s22p63s5
2. Using spdf notation, write the ground-state electron configuration of
a. Ar
b. Al
c. Ne
d. B
e. Ca
f. N
g. Cl
h. S
i.
Zn
j.
Mg
k. F
l.
O
m. Be
n. P
o. Si
p. C
q. K
r. Sc
3. Give the symbol for the element with the following electron configuration
a. 1s22s22p6
b. 1s22s22p63s23p2
c. 1s22s22p63s1
d. 1s22s2
e. 1s22s22p3
f. 1s22s22p63s23p1
4. Using the noble-gas-core abbreviated spdf notation, write the ground-state
electron configuration for
a. Cs
b. Sr
c. Ti
d. Sb
e. Br
f. Pb
g. Al
h. Ga
i.
Zr
j.
I
k. As
l.
Ba
5. Explain why the following orbital diagrams are not possible for a groundstate electron configuration
a. 1s  2s  2p   
b. 1s  2s  2p   
c. 1s  2s  2p   
6. Give an orbital diagram for the ground-state electron configuration of
a. N
b. B
c. Si
d. Ca
e. Cl
f. Sc
g. C
h. O
i.
K
j.
S
k. Mg
Section 6: Electron Configurations
PART A – ORBITAL DIAGRAMS & LONGHAND ELECTRON CONFIGURATION
Use the patterns within the periodic table to draw orbital diagrams and write
longhand electron configurations for the following atoms.
Symbol
1.
Mg
2.
P
3.
V
4.
Ge
5.
Kr
6.
O
# e-
Orbital Diagram and
spdf Electron Configuration
PART B – SHORTHAND ELECTRON CONFIGURATION
Use the patterns within the periodic table to write the shorthand electron
configurations for the following elements.
Symbol
7.
Ca
8.
Pb
9.
F
10.
Cr
# e- Noble Gas Core Electron Configuration
PART B – RULES OF ELECTRON CONFIGURATIONS
Which of the following “rules” is being violated in each electron configuration
below? Explain your answer for each. Hund’s Rule, Pauli Exclusion Principle,
Aufbau Principle


 __ __
1s
2s
2p


  
___
1s
2s
2p
3s
3p


  

  _
1s
2s
2p
3s
3p


  

  
14. 1s
2s
2p
3s
3p
11.
12.
13.
 _ _
    
3d
Section 7: Valence Electrons
1. What are valence electrons?
2. What are core electrons?
3. What is the group number for Ca? ______
4. What is the electron configuration for Ca? _________________________
5. How many valence electrons does Ca have? _________
6. What common ion does Ca form? ________
7. What is the electron configuration of the calcium ion? ________________
8. What element is the calcium ion isoelectronic with? __________
9. What is the group number for N? ______
10. What is the electron configuration for N? _________________________
11. How many valence electrons does N have? _________
12. What common ion does N form? ________
13. What is the electron configuration of the nitride ion? ________________
14. What element is the nitride ion isoelectronic with? __________
15. Use orbital diagrams to represent the electron configurations of
a. Clb. Mg+2
c. Id. Al+3