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Unit 2 Exam 1 Ch. 4 Practice Exam


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

 1. 
The product of the frequency and the wavelength of a wave equals the
a.
number of waves passing a point in a second.
b.
speed of the wave.
c.
distance between wave crests.
d.
time for one full wave to pass.
 

 2. 
Visible light, X rays, infrared radiation, and radio waves all have the same
a.
energy.
c.
speed.
b.
wavelength.
d.
frequency.
 

 3. 
For electromagnetic radiation, c (the speed of light) equals
a.
frequency minus wavelength.
c.
frequency divided by wavelength.
b.
frequency plus wavelength.
d.
frequency times wavelength.
 

 4. 
The speed of an electromagnetic wave is equal to the product of its wavelength and its
a.
mass.
c.
velocity.
b.
color.
d.
frequency.
 

 5. 
Because c, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is
a.
proportional to its frequency.
c.
inversely proportional to its frequency.
b.
equal to its frequency.
d.
double its frequency.
 

 6. 
The frequency of electromagnetic radiation is measured in waves/second, or
a.
nanometers.
c.
hertz.
b.
quanta.
d.
joules.
 

 7. 
According to the particle model of light, certain kinds of light cannot eject electrons from metals because
a.
the mass of the light is too low.
c.
the energy of the light is too low.
b.
the frequency of the light is too high.
d.
the wavelength of the light is too short.
 

 8. 
As it travels through space, electromagnetic radiation
a.
exhibits wavelike behavior.
c.
varies in speed.
b.
loses energy.
d.
releases photons.
 

 9. 
If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B, the wavelength of A is
a.
longer.
c.
equal.
b.
shorter.
d.
exactly half the length of B's wavelength.
 

 10. 
The distance between two successive peaks on adjacent waves is its
a.
frequency.
c.
quantum number.
b.
wavelength.
d.
velocity.
 

 11. 
A quantum of electromagnetic energy is called a(n)
a.
photon.
c.
excited atom.
b.
electron.
d.
orbital.
 

 12. 
The wave model of light does not explain
a.
the frequency of light.
c.
interference.
b.
the continuous spectrum.
d.
the photoelectric effect.
 

 13. 
Max Planck proposed that a hot object radiated energy in small, specific amounts called
a.
quanta.
c.
hertz.
b.
waves.
d.
electrons.
 

 14. 
The energy of a photon is related to its
a.
mass.
c.
frequency.
b.
speed.
d.
size.
 

 15. 
The emission of electrons from metals that have absorbed photons is called the
a.
interference effect.
c.
quantum effect.
b.
photoelectric effect.
d.
dual effect.
 

 16. 
The specific wavelengths of light seen through a prism that are made when high-voltage current is passed through a tube of hydrogen gas at low pressure is a
a.
line-emission spectrum.
c.
photoelectric effect.
b.
electron configuration.
d.
continuous electromagnetic spectrum.
 

 17. 
A line spectrum is produced when an electron moves from one energy level
a.
to a higher energy level.
b.
to a lower energy level.
c.
into the nucleus.
d.
to another position in the same sublevel.
 

 18. 
Which is not part of hydrogen's line-emission spectrum?
a.
Balmer series.
c.
Lyman series.
b.
Aufbau series.
d.
Paschen series.
 

 19. 
When the pink-colored light of glowing hydrogen gas passes through a prism, it is possible to see
a.
all the colors of the rainbow.
c.
four lines of different colors.
b.
only lavender-colored lines.
d.
black light.
 

 20. 
Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen
a.
had no electrons.
b.
did not release photons.
c.
released photons of only certain energies.
d.
could only exist in the ground state.
 

 21. 
The Bohr model of the atom was an attempt to explain hydrogen's
a.
density.
c.
mass.
b.
flammability.
d.
line-emission spectrum.
 

 22. 
For an electron in an atom to change from the ground state to an excited state,
a.
energy must be released.
b.
energy must be absorbed.
c.
radiation must be emitted.
d.
the electron must make a transition from a higher to a lower energy level.
 

 23. 
If electrons in an atom have the lowest possible energies, the atom is in the
a.
ground state.
c.
excited state.
b.
inert state.
d.
radiation-emitting state.
 

 24. 
Bohr's theory helped explain why
a.
electrons have negative charge.
b.
most of the mass of the atom is in the nucleus.
c.
excited hydrogen gas gives off certain colors of light.
d.
atoms combine to form molecules.
 

 25. 
According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus
a.
in specific, allowed orbits.
b.
in one fixed orbit at all times.
c.
at any of an infinite number of distances, depending on its energy.
d.
counterclockwise.
 

 26. 
Which energy-level change shown in the diagram below emits the highest energy?

mc026-1.jpg
a.
an electron moving from E6 to E5
b.
an electron moving from E2 to E4
c.
an electron moving from E2 to E3
d.
an electron moving from E2 to E1
 

 27. 
The electron in a hydrogen atom has its lowest total energy when the electron is in its
a.
neutral state.
c.
ground state.
b.
excited state.
d.
quantum state.
 

 28. 
The change of an atom from an excited state to the ground state always requires
a.
absorption of energy.
b.
emission of electromagnetic radiation.
c.
release of visible light.
d.
an increase in electron energy.
 

 29. 
According to Bohr, electrons cannot reside at ____ in the figure below.

mc029-1.jpg
a.
point A
c.
point C
b.
point B
d.
point D
 

 30. 
The French scientist Louis de Broglie theorized that
a.
electrons could have a dual wave-particle nature.
b.
light waves did not have a dual wave-particle nature.
c.
the natures of light and quantized electron orbits were not similar.
d.
Bohr's model of the hydrogen atom was completely correct.
 

 31. 
Louis de Broglie's research suggested that
a.
frequencies of electron waves do not correspond to specific energies.
b.
electrons usually behave like particles and rarely like waves.
c.
electrons should be considered as waves confined to the space around an atomic nucleus.
d.
electron waves exist at random frequencies.
 

 32. 
The equation E = hn helped Louis de Broglie determine
a.
how protons and neutrons behave in the nucleus.
b.
how electron wave frequencies correspond to specific energies.
c.
whether electrons behave as particles.
d.
whether electrons exist in a limited number of orbits with different energies.
 

 33. 
Which model of the atom explains why excited hydrogen gas gives off certain colors of light?
a.
the Bohr model
c.
Rutherford's model
b.
the de Broglie model
d.
Planck's theory
 

 34. 
Which model of the atom explains the orbitals of electrons as waves?
a.
the Bohr model
c.
Rutherford's model
b.
the quantum model
d.
Planck's theory
 

 35. 
The region outside the nucleus where an electron can most probably be found is the
a.
electron configuration.
c.
s sublevel.
b.
quantum.
d.
electron cloud.
 

 36. 
The size and shape of an electron cloud are most closely related to the electron's
a.
charge.
c.
spin.
b.
mass.
d.
energy.
 

 37. 
All of the following describe the Heisenberg uncertainly principle except
a.
it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.
b.
it is one of the fundamental principles of our present understanding of light and matter.
c.
it helped lay the foundation for the modern quantum theory.
d.
it helps to locate an electron in an atom.
 

 38. 
All of the following describe the Schrödinger wave equation except
a.
it is an equation that treats electrons in atoms as waves.
b.
only waves of specific energies and frequencies provide solutions to the equation.
c.
it helped lay the foundation for the modern quantum theory.
d.
it is similar to Bohr's theory.
 

 39. 
Both the Heisenberg uncertainty principle and the Schrödinger wave equation
a.
are based on Bohr's theory.
b.
treat electrons as particles.
c.
led to locating an electron in an atom.
d.
led to the concept of atomic orbitals.
 

 40. 
A three-dimensional region around a nucleus where an electron may be found is called a(n)
a.
spectral line.
c.
orbital.
b.
electron path.
d.
orbit.
 

 41. 
According to the quantum theory of an atom, in an orbital
a.
an electron's position cannot be known precisely.
b.
an electron has no energy.
c.
electrons cannot be found.
d.
electrons travel around the nucleus on paths of specific radii.
 

 42. 
The quantum number that indicates the position of an orbital about the three axes in space is the
a.
principal quantum number.
b.
angular momentum quantum number.
c.
magnetic quantum number.
d.
spin quantum number.
 

 43. 
How many quantum numbers are needed to describe the energy state of an electron in an atom?
a.
1
c.
3
b.
2
d.
4
 

 44. 
The main energy levels of an atom are indicated by the
a.
orbital quantum numbers.
b.
magnetic quantum numbers.
c.
spin quantum numbers.
d.
principal quantum numbers.
 

 45. 
The angular momentum quantum number indicates the
a.
orientation of an orbital around the nucleus.
b.
shape of an orbital.
c.
direction of the spin of the electron in its orbital.
d.
main energy level of an orbital.
 

 46. 
The number of sublevels within each energy level of an atom is equal to the value of the
a.
principal quantum number.
b.
angular momentum quantum number.
c.
magnetic quantum number.
d.
spin quantum number.
 

 47. 
What values can the angular momentum quantum number have when n = 2?
a.
mc047-1.jpg
c.
0, 1, 2
b.
mc047-2.jpg
d.
0, 1
 

 48. 
The spin quantum number indicates that the number of possible spin states for an electron in an orbital is
a.
1.
c.
3.
b.
2.
d.
5.
 

 49. 
Each atomic orbital is described by its principal quantum number followed by the
a.
value of the electron's spin state.
c.
number of electrons in the sublevel.
b.
magnetic quantum number.
d.
letter of the sublevel.
 

 50. 
The spin quantum number of an electron can be thought of as describing
a.
the direction of electron spin.
b.
whether the electron's charge is positive or negative.
c.
the electron's exact location in orbit.
d.
the number of revolutions the electron makes about the nucleus per second.
 

 51. 
An electron for which n = 4 has more ____ than an electron for which n = 2.
a.
spin
c.
energy
b.
particle nature
d.
wave nature
 

 52. 
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called
a.
d orbitals.
c.
f orbitals.
b.
p orbitals.
d.
s orbitals.
 

 53. 
A spherical electron cloud surrounding an atomic nucleus would best represent
a.
an s orbital.
b.
a px orbital.
c.
a combination of px and py orbitals.
d.
a combination of an s and a px orbital.
 

 54. 
The major difference between a 1s orbital and a 2s orbital is that
a.
the 2s orbital can hold more electrons.
b.
the 2s orbital has a slightly different shape.
c.
the 2s orbital is at a higher energy level.
d.
the 1s orbital can have only one electron.
 

 55. 
The p orbitals are shaped like
a.
electrons.
c.
dumbbells.
b.
circles.
d.
spheres.
 

 56. 
An orbital that can never exist according to the quantum description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
3f.
 

 57. 
The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are
a.
s:2, p:4, d:6, and f:8.
b.
s:1, p:3, d:5, and f:7.
c.
s:2, p:6, d:10, and f:14.
d.
s:1, p:2, d:3, and f:4.
 

 58. 
The number of possible different orbital shapes for the third energy level is
a.
1.
c.
3.
b.
2.
d.
4.
 

 59. 
The number of orbitals for the d sublevel is
a.
1.
c.
5.
b.
3.
d.
7.
 

 60. 
For the f sublevel, the number of orbitals is
a.
5.
c.
9.
b.
7.
d.
18.
 

 61. 
The total number of orbitals that can exist at the second main energy level is
a.
2.
c.
4.
b.
3.
d.
8.
 

 62. 
How many orientations can an s orbital have about the nucleus?
a.
1
c.
3
b.
2
d.
5
 

 63. 
How many orbitals can exist at the third main energy level?
a.
3
c.
9
b.
6
d.
18
 

 64. 
How many electrons can occupy the s orbitals at each energy level?
a.
two, if they have opposite spins
b.
two, if they have the same spin
c.
one
d.
no more than eight
 

 65. 
If n is the principal quantum number of a main energy level, the number of electrons in that energy level is
a.
n.
c.
n2.
b.
2n.
d.
2n2.
 

 66. 
How many electrons are needed to completely fill the fourth energy level?
a.
8
c.
32
b.
18
d.
40
 

 67. 
How many more electrons are needed to completely fill the third main energy level if it already contains 8 electrons?
a.
0
c.
10
b.
8
d.
22
 

 68. 
One main energy level can hold 18 electrons. What is n?
a.
mc068-1.jpg
c.
6
b.
3
d.
18
 

 69. 
At n = 1, the total number of electrons that could be found is
a.
1.
c.
6.
b.
2.
d.
18.
 

 70. 
If 8 electrons completely fill a main energy level, what is n?
a.
2
c.
8
b.
4
d.
32
 

 71. 
If the third main energy level contains 15 electrons, how many more could it possibly hold?
a.
0
c.
3
b.
1
d.
17
 

 72. 
The main energy level that can hold only two electrons is the
a.
first.
c.
third.
b.
second.
d.
fourth.
 

 73. 
A single orbital in the 3d level can hold ____ electrons.
a.
10
c.
3
b.
2
d.
6
 

 74. 
The statement that an electron occupies the lowest available energy orbital is
a.
Hund's rule.
c.
Bohr's law.
b.
the Aufbau principle.
d.
the Pauli exclusion principle.
 

 75. 
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin" is a statement of
a.
the Pauli exclusion principle.
c.
the quantum effect.
b.
the Aufbau principle.
d.
Hund's rule.
 

 76. 
The statement that no two electrons in the same atom can have the same four quantum numbers is
a.
the Pauli exclusion principle.
c.
Bohr's law.
b.
Hund's rule.
d.
the Aufbau principle.
 

 77. 
Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons?
a.
Hund's rule
c.
the Aufbau principle
b.
the Pauli exclusion principle
d.
the quantum rule
 

 78. 
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
a.
quantum rule.
c.
the Pauli exclusion principle.
b.
the magnetic rule.
d.
the Aufbau principle.
 

 79. 
The sequence in which energy sublevels are filled is specified by
a.
the Pauli exclusion principle.
c.
Lyman's series.
b.
the orbital rule.
d.
the Aufbau principle.
 

 80. 
The Aufbau principle states that an electron
a.
can have only one spin number.
b.
occupies the lowest available energy level.
c.
must be paired with another electron.
d.
must enter an s orbital.
 

 81. 
The Pauli exclusion principle states that no two electrons in the same atom can
a.
occupy the same orbital.
b.
have the same spin quantum numbers.
c.
have the same set of quantum numbers.
d.
be at the same main energy level.
 

 82. 
The atomic sublevel with the next highest energy after 4p is
a.
4d.
c.
5p.
b.
4f.
d.
5s.
 

 83. 
In the electron configuration for scandium (atomic number 21), what is the notation for the three highest-energy electrons?
a.
3d1 4s2
c.
3d3
b.
4s3
d.
4s2 4p1
 

 84. 
Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau principle?
a.
1s 2s 2p 3s 4s 3p 3d 4p 5s
b.
1s 2s 2p 3s 3p 4s 3d 4p 5s
c.
1s 2s 2p 3s 3p 4s 4p 3d 4d
d.
1s 2s 2p 3s 3p 3d 4s 4p 5s
 

 85. 
Both copper (atomic number 29) and chromium (atomic number 24) appear to break the pattern in the order of filling the 3d and 4s orbitals. This change in pattern is expressed by
a.
an increase in the number of electrons in both the 3d and 4s orbitals.
b.
a reduction in the number of electrons in both the 3d and 4s orbitals.
c.
a reduction in the number of electrons in the 3d orbital and an increase in the 4s orbital.
d.
a reduction in the number of electrons in the 4s orbital and an increase in the 3d orbital.
 

 86. 
In the ground state, the 3d and 4s sublevels of the chromium atom (atomic number 24) are represented as
a.
3d6 4s1.
c.
3d5 4s1.
b.
3d4 4s2.
d.
4s2 3d4.
 

 87. 
The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a.
Mg (Z = 12).
c.
S (Z = 16).
b.
C (Z = 6).
d.
Si (Z = 14).
 

 88. 
The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is
a.
3.
c.
11.
b.
6.
d.
12.
 

 89. 
What is the electron configuration for nitrogen, atomic number 7?
a.
1s2 2s2 2p3
b.
1s2 2s3 2p2
c.
1s2 2s3 2p1
d.
1s2 2s2 2p2 3s1
 

 90. 
The electron notation for aluminum (atomic number 13) is
a.
1s2 2s2 2p3 3s2 3p3 3d1.
b.
1s2 2s2 2p6 3s2 2d1.
c.
1s2 2s2 2p6 3s2 3p1.
d.
1s2 2s2 2p9.
 

 91. 
If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)
a.
electron pair.
c.
empty d orbital.
b.
octet.
d.
electron in an excited state.
 

 92. 
The number of electrons in the highest energy level of the argon atom (atomic number 18) is
a.
10.
c.
6.
b.
2.
d.
8.
 

 93. 
If the s and p sublevels of the highest main energy level of an atom are filled, how many electrons are in this main energy level?
a.
2
c.
16
b.
8
d.
32
 

 94. 
If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
a.
2
c.
10
b.
8
d.
32
 

 95. 
An element with 8 electrons in its highest main energy level is a(n)
a.
octet element.
c.
Aufbau element.
b.
third period element.
d.
noble gas.
 

Short Answer
 

 96. 
Explain Louis de Broglie's contribution to the quantum model of the atom.
 

 97. 
What do quantum numbers describe?
 

 98. 
How does the figure below illustrate Hund's rule?

sa098-1.jpg
 

 99. 
How does the figure above illustrate the Pauli exclusion principle?
 

 100. 
The electron configuration for nitrogen is 1s2 2s2 2p3. What does the 3 in 2p3 mean?
 



 
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