# Unit 5 Test Review

```Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
Unit 5 Test Review
Wavelength and Frequency Formula
C = λν
C = 3.0 x 108 (m∙Hz) or (m∙sec-1)
λ = Wavelength (m)
ν = Frequency (Hz) or (sec-1)
Answer the following questions by using the formula above:
1. What is the speed of light?
2. What is the wavelength of a wave having a frequency of 4.76 x 1014 Hz? Is this wave visible?
3. What is the frequency of a 6.9 x 10-7 m wave? Is this wave visible?
4. What is the frequency of a 3,410 km wave? Is this wave visible?
5. What is the frequency of a 5.6 x 102 nm wave? Is this wave visible?
6. What is the wavelength of 10.1 KHz wave? Is this wave visible?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
Energy of a Quantum
Equantum = hv
Energy of a Photon
Equantum = Represents Energy
h = Planck’s constant
v = Frequency
Ephoton = hv
Ephoton = Represents Energy
h = Planck’s constant
v = Frequency
Planck’s Constant
h = 6.626 x 10-34 J•s
Answer the following questions by using the formula above:
7. What is Plank’s Constant?
8. What is the energy of a 7.66 x 1014 Hz wave?
9. What is the frequency of a photon carrying 1.78 x 10-15 J of energy?
10. What is the Quantum energy of a 2.61 x 1019 Hz wave?
11. What is the frequency of a photon carrying 4.31x 10-22 J of energy?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
In the calculations below you will need to determine the wavelength of the given sample.
[Hint: Use the Equantum or Ephoton equations to determine the frequency and then use c= λν]
12. What is the wavelength of a 1.32 x 10-6 J wave?
13. What is the wavelength of a 7.65 x 10-17 J wave?
14. What is the wavelength of a 1.528 x 10-13 J wave?
15. What modification did Einstein make to Planck’s work?
16. Which has the largest wavelength, Ultraviolet Rays or X-Rays?
17. While and FM radio station broadcasts at a frequency of 94.7 MHz, an AM station broadcasts at a frequency of
820kHz. What are the wavelengths of the two broadcasts?
18. Objects get their colors from reflecting only certain wavelengths when hit with white light. Light reflected from
a green leaf is found to have a wavelength of 4.90 x 10-7 m. What is the frequency of the light?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
19. Who is J. W. Dobereiner and what was his contribution to the organization of all of the known elements?
20. Who is J.A.R. Newlands and what was his contribution to the organization of all of the known elements?
21. Who is Dmitri Mendeleev and what was his contribution to the organization of all of the known elements?
22. Who is Henry Moseley and what was his contribution to the organization of all of the known elements?
23. What is the Periodic Law?
24. Who is Neils Bohr and what did he suggest?
25. Draw the Bohr’s Model for Lithium
26. What makes Bohr’s model fundamentally incorrect and how can it be fixed?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
27. Write the ground state electron configuration for each neutral atom. Remember ground state means that all of
the lowest possible energy levels (up to the proper number of electrons for the element) are filled.
a) Na
b) Pb
c) Sr
d) U
e) N
28. Write the ground state electron configuration for each neutral atom in Nobel Gas Notation. Remember ground
state means that all of the lowest possible energy levels (up to the proper number of electrons for the element)
are filled.
a) Na
b) Pb
c) Sr
d) U
e) N
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
29. Write the ground state electron configuration for the following ions. Remember ions have a change in total
number of electrons (positive ions, cations, have lost an electron and negative ions, anions, have gained an
ion). [Example: N-3 is 1s22s23p6 and has 3 extra electrons]
a)
O-2
b)
Fe+2
c)
B+3
d)
Cl-1
e)
K+
30. An excited atom has an electron or electrons which are not in the lowest energy state. Excited atoms are
unstable energetically. The electrons eventually fall to a lower level. An excited state electron is denoted with
the symbol (*). [Example: *Li is 1s22p1 whereas Li is 1s22s1]
Write an excited state electron configuration for each of the following:
a) *Al
b) *Br
c) *F
d) *K
e) *Sr
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
31. Use the Pauli Exclusion Principle and Hund’s Rule to identify how many unpaired electrons are present in the
following atomic structures :
The Pauli Exclusion Principle states that a maximum of two electrons can occupy a single atomic orbital to form
paired electrons, but only if the two electrons have opposite spins.
Hund’s Rule states that single electrons with the same spin must occupy each equal-energy orbital before additional
electrons with opposite spins can occupy the same orbital.
a) Si
b) N
c) Cl
d) Mn
e) Ru
32. Fill out the information below?
s-orbital
p-orbital
d-orbital
f-orbital
Draw the shape of the
orbital
How many electrons
can it hold?
What is the lowest
energy level in which it
can exist?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
33. Write out all possible energy levels with the corresponding sublevels.
34. Why is the 4s orbital filled with electrons before the 3d orbital?
35. Why does it take more energy to take an electron from Al+ than from Al?
36. What is the difference between an atom in its ground stave vs. its excited state?
37. What are the three rules that we need to use when writing the electron configuration in orbital notation?
38. Draw the Orbital Configuration for Ru.
Energy Level
s-orbitals
p-orbitals
d-orbitals
f-orbitals
n=5
____
5s
____ ____ ____
5p
____ ____ ____ ____ ____
5d
____ ____ ____ ____ ____ ____ ____
5f
n=4
____
4s
____ ____ ____
4p
____ ____ ____ ____ ____
4d
____ ____ ____ ____ ____ ____ ____
4f
n=3
____
3s
____ ____ ____
3p
____ ____ ____ ____ ____
3d
n=2
____
2s
____ ____ ____
2p
n=1
____
1s
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
39. Fill out the chart below:
Element
Atomic
Number
Na
11
S
16
Number of electrons
in each level
1st
2nd
3rd
2 8
1
1st
3rd
2nd
4th
4th
Electron Configuration
Number of ethat can be lost
or gained
Number of
electrons left
after ionization
Charge on
the ion
1s22s22p63s1
Lose 1
10
+1
1s22s22p63s23p4
Gain 2
18
-2
5th
5th
2 8
6
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
K
Al
Cl
Xe
Ca
40. What are valence electrons and where can find them?
41. What do valence electrons help us determine?
42. Why do the d orbitals not factor in to the valence electron number?
43. How many valence electrons are present for the transition metals?
44. The Lewis Dot Structure is a short hand expression that shows the number of valence electrons surrounding the
elemental symbol. Draw the Lewis Dot Structure for the following:
Al
Coach Kenney
Ca
Te
I
Kr
Si
Rb
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
45. Describe the Alkali Metals.
46. Describe the Alkaline Earth Metals.
47. Describe the Halogens.
48. Describe the Noble Gases.
49. Describe the Transition Metals.
50. Describe the Inner Transition Metals.
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
51. Describe the key differences between Metals and Non-Metals.
Characteristics of Metals
Characteristics of Nonmetals
52. Describe the chemical families below:
Family
Location
Reactivity
Outer Shell Electrons
Alkali Metals
Alkaline Earth Metals
Halogens
Noble Gasses
Transition Metals
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
53. What is the Trend for Atomic Size and why does that occur?
54. What is the Trend for Ionic Size and why does that occur?
55. What is the Trend for Ionization Energy and why does that occur?
56. What is the Trend for electronegativity and why does that occur?
57. What is the difference between Electronegativity and Ionization Energy?
Coach Kenney
3113
Name: ____________________________
When is this due? ___________________
Date: __________
Period: __________
58. A photon of ultraviolet (UV) light possesses enough energy to mutate a strand of human DNA. What is the
energy of a single UV photon having a wavelength of 257 nm?
a) 7.74 x 10-37 J
b) 5.68 x 10-31 J
c) 7.74 x 10-19 J
d) 1.29 x 1036 J
59. The elements silicon, gallium, arsenic, germanium, aluminum, cadmium, sulfur, and selenium are all used in the
manufacture of various semiconductor devises. Which of the following electron configurations is the ground
state electron configuration for germanium?
a)
b)
c)
d)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
1s2 2s2 2p6 3s2 3p6 4s2 3d12
1s2 2s2 2p6 3s2 3p6 4s2 3d6 4p6
60. Identify which element would have the following electron configuration as a ground state atom?
[Ne]3s2 3p3
a)
b)
c)
d)
Al
P
S
Sc
61. As one moves from the ultraviolet to X-ray regions of the electromagnetic spectrum, the frequency of light
waves increases. What is the effect on the wavelength and energy of the waves?
a)
b)
c)
d)
the wavelength increases and the energy increases
the wavelength decreases and the energy increases
the wavelength increases and the energy decreases
the wavelength decreases and the energy decreases
62. Nickel, copper, and zinc are sometime known as the coinage metals. How many unpaired electrons are in a
+
-
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63. Order the following atoms from smallest to largest radius: C, Al, F, Si
a)
b)
c)
d)
Coach Kenney
C < F < Al < Si
Al < Si < F < C
C < Si < F < Al
F < C < Si < Al
3113
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