Name: 
 

Atomic Structure Online Practice


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
Which of the following colors of visible light has the longest wavelength?
a.
orange
b.
blue
c.
red
d.
green
e.
yellow
 

 2. 
Which of the following regions of the electromagnetic spectrum has the lowest frequency?
a.
ultraviolet
b.
infrared
c.
visible
d.
x-ray
e.
gamma ray
 

 3. 
An argon ion laser emits light at 488 nm. What is the frequency of this radiation?
a.
4.07 ´ 10-19 s-1
b.
1.63 ´ 10-15 s-1
c.
1.46 ´ 102 s-1
d.
2.05 ´ 106 s-1
e.
6.14 ´ 1014 s-1
 

 4. 
If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?
a.
6.59 ´ 10-28 m
b.
1.01 ´ 10-6 m
c.
3.32 ´ 10-3 m
d.
301 m
e.
2.98 ´ 1014 m
 

 5. 
The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength.
a.
amplitude, directly, inversely
b.
energy, inversely, directly
c.
energy, directly, inversely
d.
velocity, inversely, directly
e.
velocity, directly, inversely
 

 6. 
According to experiments concerned with the photoelectric effect, which of the following will increase the kinetic energy of an electron ejected from a metal surface?

1.
increasing the wavelength of the light striking the surface
2.
increasing the frequency of the light striking the surface
3.
increasing the number of photons of light striking the surface
a.
1 only
b.
2 only
c.
3 only
d.
1 and 2
e.
2 and 3
 

 7. 
Planck suggested that all energy gained or lost by an atom must be some integral multiple of a minimum amount of energy called a ____.
a.
Bohr
b.
frequency
c.
photon
d.
transition
e.
quantum
 

 8. 
A common infrared laser operates at 1.06 ´ 103 nm. What is the energy of a photon with this wavelength?
a.
7.02 ´ 10-40 J
b.
6.25 ´ 10-28 J
c.
3.54 ´ 10-15 J
d.
1.87 ´ 10-19 J
e.
2.83 ´ 1014 J
 

 9. 
Excited hydrogen atoms emit light in the ultraviolet at 2.47 ´ 1015 Hz. What is the energy of a single photon with this frequency?
a.
8.04 ´ 10-41 J
b.
2.68 ´ 10-19 J
c.
1.64 ´ 10-18 J
d.
6.11 ´ 10-17 J
e.
1.21 ´ 10-7 J
 

 10. 
A red laser pointer emits light at a wavelength of 635 nm. If the laser emits 7.5 ´ 10-4 J of energy per second in the form of visible radiation, how many photons per second are emitted from the laser?
a.
4.2 ´ 10-16 photons/sec
b.
2.4 ´ 1015 photons/sec
c.
6.3 ´ 1017 photons/sec
d.
2.7 ´ 1022 photons/sec
e.
1.8 ´ 1036 photons/sec
 

 11. 
What is the energy of a mole of photons of red light with a wavelength of 632 nm?
a.
189 kJ
b.
252 kJ
c.
314 kJ
d.
515 kJ
e.
756 kJ
 

 12. 
If the energy of 1.00 mole of photons is 441 kJ, what is the wavelength of the light?
a.
271 nm
b.
451 nm
c.
680 nm
d.
732 nm
e.
891 nm
 

 13. 
The energy required to break one mole of chlorine-chlorine bonds in Cl2 is 242 kJ/mol. What is the longest wavelength of light capable of breaking a single chlorine-chlorine bond?
a.
124 nm
b.
242 nm
c.
421 nm
d.
494 nm
e.
821 nm
 

 14. 
For a hydrogen atom, calculate the wavelength of the line in the Lyman series that results from the transition n = 4 to n = 1. The Rydberg constant equals -2.18 ´ 10-18 J.
a.
30.4 nm
b.
97.2 nm
c.
114 nm
d.
121 nm
e.
182 nm
 

 15. 
According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 2 to n = 3 is ____ the energy necessary to excite an electron from n = 4 to n = 5.
a.
less than
b.
greater than
c.
equal to
d.
either equal to or greater than
e.
either less than or equal to
 

 16. 
Which of the following transitions in a hydrogen atom would emit the lowest energy photon?
a.
n = 1 to n = 2
b.
n = 3 to n = 2
c.
n = 5 to n = 1
d.
n = 2 to n = 8
e.
n = 6 to n = 5
 

 17. 
If a hydrogen atom in the excited n = 3 state relaxes to the ground state, what is the maximum number of possible emission lines?
a.
0
b.
1
c.
2
d.
3
e.
infinite
 

 18. 
If the de Broglie wavelength of an electron is 555 nm, what is its velocity? The mass of an electron is 9.1 ´ 10-31 kg.
a.
4.0 ´ 10-10 m/s
b.
7.6 ´ 10-4 m/s
c.
5.2 ´ 102 m/s
d.
1.3 ´ 103 m/s
e.
2.5 ´ 109 m/s
 

 19. 
What is the de Broglie wavelength of a 120 g golf ball traveling at 65 km/hr?
a.
8.5 ´ 10-38 m
b.
3.1 ´ 10-34 m
c.
0.15 m
d.
3.3 ´ 1033 m
e.
1.2 ´ 1037 m
 

 20. 
Which of the following types of experiments demonstrate that an electron has the properties of a particle?
a.
nuclear fission
b.
electron diffraction
c.
light emission from atomic gases
d.
mass spectroscopy
e.
photoelectric effect
 

 21. 
The Schrödinger wave equation
a.
calculates the position and momentum of an electron at any given time.
b.
can be solved to determine the probability of finding an electron in a region of space.
c.
proves that energy is equal to mass times the speed of light squared.
d.
incorrectly predicts circular orbits of electrons around nuclei.
e.
is used to calculate the velocity of an electron.
 

 22. 
Which of the following statements is INCORRECT?
a.
The location and the energy of an electron in an atom can be simultaneously known with little or no uncertainty.
b.
The energies of an atom's electrons are quantized.
c.
Quantum numbers define the energy states and the orbitals available to an electron.
d.
The behavior of an atom's electrons can be described by standing waves.
e.
Electrons have both wave and particle properties.
 

 23. 
What type of orbital is designated n = 3, l = 2, ml = -1?
a.
3s
b.
3p
c.
3d
d.
2f
e.
2d
 

 24. 
What type of orbital is designated n = 4, l = 3, ml = -3?
a.
4s
b.
4p
c.
4d
d.
4f
e.
none
 

 25. 
What shell contains a total of 9 orbitals?
a.
n = 1
b.
n = 2
c.
n = 3
d.
n = 4
e.
n = 5
 

 26. 
Which of the following sets of quantum numbers refers to a 4p orbital?
a.
n = 1, l = 1, ml = -1
b.
n = 1, l = 2, ml = -1
c.
n = 4, l = 1, ml = 0
d.
n = 4, l = 2, ml = -1
e.
n = 4, l = 3, ml = +2
 

 27. 
How many orbitals have the following set of quantum numbers: n = 6, l = 3, ml = -2?
a.
0
b.
1
c.
3
d.
6
e.
7
 

 28. 
All of the following sets of quantum numbers are allowed EXCEPT
a.
n = 6, l = 0, ml = +1
b.
n = 5, l = 4, ml = 0
c.
n = 4, l = 1, ml = -1
d.
n = 3, l = 2, ml = +2
e.
n = 1, l = 0, ml = 0
 

 29. 
All of the following sets of quantum numbers are allowed EXCEPT
a.
n = 5, l = 3, ml = +2
b.
n = 3, l = 2, ml = -1
c.
n = 3, l = 0, ml = 0
d.
n = 4, l = 4, ml = -2
e.
n = 5, l = 3, ml = +3
 

 30. 
What is the total number of orbitals having n = 5 and l = 1?
a.
1
b.
2
c.
3
d.
5
e.
10
 

 31. 
Which of the following properties is associated with the value of the ml quantum number?
a.
the number of electrons in an orbital
b.
the size of an orbital
c.
the shape of an orbital
d.
the energy of an orbital
e.
the orientation in space of an orbital
 

 32. 
Which of the following properties is associated with the value of the l quantum number?
a.
the number of electrons in an orbital
b.
the size of an orbital
c.
the orientation in space of an orbital
d.
the energy of an orbital
e.
the shape of an orbital
 

 33. 
Which of the following orbitals might have ml = -2?
a.
s
b.
s and p
c.
p and d
d.
d and f
e.
p, d, and f
 

 34. 
How many nodal planes exist for a 2p orbital?
a.
0
b.
1
c.
2
d.
3
e.
4
 

 35. 
The n = ____ shell is the lowest that may contain p-orbitals.
a.
2
b.
3
c.
4
d.
5
e.
6
 

 36. 
Which of the following diagrams represent d-orbitals?

chapter_6_online_pr_files/i0370000.jpg
a.
(I) only
b.
(II) only
c.
(III) only
d.
(IV) only
e.
(I) and (IV)
 

 37. 
Which of the following diagrams represent p-orbitals?

chapter_6_online_pr_files/i0380000.jpg
a.
(I) only
b.
(II) only
c.
(III) only
d.
(IV) only
e.
(I) and (II)
 

 38. 
The Pauli exclusion principle states that
a.
no two electrons in an atom can have the same four quantum numbers.
b.
electrons can have either ±chapter_6_online_pr_files/i0390000.jpg spins.
c.
electrons with opposing spins are attracted to each other.
d.
no two electrons in an atom can have the same spin.
e.
atoms with no unpaired electrons are diamagnetic.
 

 39. 
What is the maximum number of electrons that can occupy the n = 5 shell?
a.
5
b.
10
c.
14
d.
25
e.
50
 

 40. 
Which one of the following sets of quantum numbers is NOT allowed?
a.
n = 6, l = 0, ml = 0, ms = +1/2
b.
n = 5, l = 3, ml = 1, ms = +1/2
c.
n = 4, l = 2, ml = -3, ms = -1/2
d.
n = 3, l = 1, ml = -1, ms = +1/2
e.
n = 2, l = 0, ml = 0, ms = -1/2
 

 41. 
Which of the following sets of quantum numbers is allowed?
a.
n = 2, l = 1, ml = 1, ms = -1/2
b.
n = 3, l = 2, ml = 1, ms = +1
c.
n = 3, l = 1, ml = -3, ms = -1/2
d.
n = 4, l = 4, ml = -1, ms = +1/2
e.
n = 5, l = 2, ml = +2, ms = -1
 

 42. 
Which of the following statements regarding subshell filling order are CORRECT?

1.
Electrons are assigned to the 4s subshell before they are assigned to the 3d subshell.
2.
Electrons are assigned to the 4f subshell before they are assigned to the 6s subshell.
3.
Electrons are assigned to the 5d subshell before they are assigned to the 6p subshell.
a.
1 only
b.
2 only
c.
3 only
d.
1 and 3
e.
1, 2, and 3
 

 43. 
Which of the following elements is an s-block element?
a.
C
b.
Cd
c.
Cs
d.
Cl
e.
Cf
 

 44. 
Which of the following elements is an f-block element?
a.
C
b.
Cd
c.
Cs
d.
Cl
e.
Cf
 

 45. 
Which element has the electron configuration [Ar]3d104s1?
a.
Cu
b.
Zn
c.
Ga
d.
Ag
e.
Co
 

 46. 
What is the electron configuration for a lead atom?
a.
[Xe]6s26p2
b.
[Kr]5d106s26p2
c.
[Xe]4f145d106s26p2
d.
[Xe]5d106s26p2
e.
[Kr]4d104f145d2
 

 47. 
Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)
a.
has a filled valence shell of electrons.
b.
has two electrons per orbital, each with identical spins.
c.
has ml values greater than or equal to zero.
d.
has the maximum number of unpaired electrons, all with the same spin.
e.
has two electrons per orbital, each with opposing spins.
 

 48. 
Which element has the following electron configuration?

chapter_6_online_pr_files/i0490000.jpg
a.
Br
b.
Se
c.
S
d.
Cl
e.
Ge
 



 
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