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Gen Chem Electron Exam (Ch 4 & 5)


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

 1. 
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.
 

 2. 
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.
 

 3. 
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.
 

 4. 
The Bohr model of the atom was an attempt to explain hydrogen's
a.
density.
c.
mass.
b.
flammability.
d.
line-emission spectrum.
 

 5. 
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.
 

 6. 
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.
 

 7. 
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.
 

 8. 
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.
 

 9. 
Which energy-level change shown in the diagram below emits the highest energy?

mc009-1.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
 

 10. 
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.
 

 11. 
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.
 

 12. 
According to Bohr, electrons cannot reside at ____ in the figure below.

mc012-1.jpg
a.
point A
c.
point C
b.
point B
d.
point D
 

 13. 
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
 

 14. 
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
 

 15. 
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.
 

 16. 
The size and shape of an electron cloud are most closely related to the electron's
a.
charge.
c.
spin.
b.
mass.
d.
energy.
 

 17. 
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.
 

 18. 
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.
 

 19. 
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.
 

 20. 
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.
 

 21. 
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.
 

 22. 
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.
 

 23. 
An orbital that can never exist according to the quantum description of the atom is
a.
3d.
c.
6d.
b.
8s.
d.
3f.
 

 24. 
The number of possible different orbital shapes for the third energy level is
a.
1.
c.
3.
b.
2.
d.
4.
 

 25. 
The number of orbitals for the d sublevel is
a.
1.
c.
5.
b.
3.
d.
7.
 

 26. 
For the f sublevel, the number of orbitals is
a.
5.
c.
9.
b.
7.
d.
18.
 

 27. 
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.
 

 28. 
"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.
 

 29. 
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.
 

 30. 
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
 

 31. 
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.
 

 32. 
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.
 

 33. 
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.
 

 34. 
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.
 

 35. 
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
 

 36. 
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.
 

 37. 
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).
 

 38. 
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
 

 39. 
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.
 

 40. 
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.
 

 41. 
The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to
a.
Mendeleev.
c.
Bohr.
b.
Moseley.
d.
Ramsay.
 

 42. 
Mendeleev left spaces in his periodic table and predicted the existence of three elements and their
a.
atomic numbers.
c.
properties.
b.
colors.
d.
radioactivity.
 

 43. 
Mendeleev noticed that properties of elements usually repeated at regular intervals when the elements were arranged in order of increasing
a.
atomic number.
c.
reactivity.
b.
density.
d.
atomic mass.
 

 44. 
Mendeleev did not always list elements in his periodic table in order of increasing atomic mass because he grouped together elements with similar
a.
properties.
c.
densities.
b.
atomic numbers.
d.
colors.
 

 45. 
Mendeleev predicted that the spaces in his periodic table represented
a.
isotopes.
c.
unstable elements.
b.
radioactive elements.
d.
undiscovered elements.
 

 46. 
The person whose work led to a periodic table based on increasing atomic number was
a.
Moseley.
c.
Rutherford.
b.
Mendeleev.
d.
Cannizzaro.
 

 47. 
Moseley's work led to the realization that elements with similar properties occurred at regular intervals when the elements were arranged in order of increasing
a.
atomic mass.
c.
radioactivity.
b.
density.
d.
atomic number.
 

 48. 
What are the radioactive elements with atomic numbers from 90 to 103 called?
a.
the noble gases
c.
the actinides
b.
the lanthanides
d.
the rare-earth elements
 

 49. 
What are the elements with atomic numbers from 58 to 71 called?
a.
the lanthanides
c.
the actinides
b.
the noble gases
d.
the alkali metals
 

 50. 
Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

 51. 
The periodic law states that the physical and chemical properties of elements are periodic functions of their atomic
a.
masses.
c.
radii.
b.
numbers.
d.
charges.
 

 52. 
The principle that states that the physical and chemical properties of the elements are periodic functions of their atomic numbers is
a.
the periodic table.
c.
the law of properties.
b.
the periodic law.
d.
Mendeleev's law.
 

 53. 
Elements in a group or column in the periodic table can be expected to have similar
a.
atomic masses.
c.
numbers of neutrons.
b.
atomic numbers.
d.
properties.
 

 54. 
A horizontal row of blocks in the periodic table is called a(n)
a.
group.
c.
family.
b.
period.
d.
octet.
 

 55. 
The electron configuration of cesium, atomic number 55, is [Xe] 6s1. In what period is cesium?
a.
Period 1
c.
Period 8
b.
Period 6
d.
Period 55
 

 56. 
The period of an element can be determined from its
a.
reactivity.
c.
symbol.
b.
density.
d.
electron configuration.
 

 57. 
Calcium, atomic number 20, has the electron configuration [Ar] 4s2. In what period is calcium?
a.
Period 2
c.
Period 8
b.
Period 4
d.
Period 20
 

 58. 
The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the
a.
alkaline-earth metals.
c.
alkali metals.
b.
transition metals.
d.
metalloids.
 

 59. 
The most characteristic property of the noble gases is that they
a.
have low boiling points.
b.
are radioactive.
c.
are gases at ordinary temperatures.
d.
are largely unreactive.
 

 60. 
Compared to the alkali metals, the alkaline-earth metals
a.
are less reactive.
b.
have lower melting points.
c.
are less dense.
d.
combine more readily with nonmetals.
 

 61. 
One-half the distance between the nuclei of identical atoms that are bonded together is called the
a.
atomic radius.
c.
atomic volume.
b.
atomic diameter.
d.
electron cloud.
 

 62. 
What is removed when the ionization energy is supplied to an atom of an element?
a.
the electron cloud
c.
an electron
b.
the nucleus
d.
an ion
 

 63. 
When an electron is acquired by a neutral atom, the energy change is called
a.
electron affinity.
c.
ionization energy.
b.
electronegativity.
d.
electron configuration.
 

 64. 
The element that has the greatest electronegativity is
a.
oxygen.
c.
chlorine.
b.
sodium.
d.
fluorine.
 

 65. 
A positive ion is known as a(n)
a.
ionic radius.
c.
cation.
b.
valence electron.
d.
anion
 

 66. 
A negative ion is known as a(n)
a.
ionic radius.
c.
cation.
b.
valence electron.
d.
anion.
 

 67. 
In a row in the periodic table, as the atomic number increases, the atomic radius generally
a.
decreases.
c.
increases.
b.
remains constant.
d.
becomes immeasurable.
 

 68. 
Within a group of elements, as the atomic number increases, the atomic radius
a.
increases.
b.
remains approximately constant.
c.
decreases regularly.
d.
varies unpredictably.
 

 69. 
In the alkaline-earth group, atoms with the smallest radii
a.
are the most reactive.
b.
have the largest volume.
c.
are all gases.
d.
have the highest ionization energies.
 

 70. 
As the atomic number of the metals of Group 1 increases, the ionic radius
a.
increases.
c.
remains the same.
b.
decreases.
d.
cannot be determined.
 

 71. 
Across a period in the periodic table, atomic radii
a.
gradually decrease.
b.
gradually decrease, then sharply increase.
c.
gradually increase.
d.
gradually increase, then sharply decrease.
 

 72. 
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
a.
sodium has four or five electrons.
b.
the atomic radius has increased.
c.
a d electron has been removed.
d.
the noble gas configuration has been reached.
 

 73. 
Which is the best reason that the atomic radius generally increases with atomic number in each group of elements?
a.
The nuclear charge increases.
b.
The number of neutrons increases.
c.
The number of occupied energy levels increases.
d.
A new octet forms.
 

 74. 
For each successive electron removed from an atom, the ionization energy
a.
increases.
c.
remains the same.
b.
decreases.
d.
shows no pattern.
 

 75. 
As you move down Group 14 in the periodic table from carbon through lead, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 76. 
As you move left to right in Period 4 from gallium through bromine, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 77. 
Hoe does the energy required to remove an electron from an atom changer as you move left to right in Period 4 from potassium through iron?
a.
It generally increases.
c.
It does not change.
b.
It generally decreases.
d.
It varies unpredictably.
 

 78. 
The force of attraction by Group 1 metals for their valence electrons is
a.
weak.
b.
zero.
c.
strong.
d.
greater than that for inner shell electrons.
 

 79. 
The electrons available to be lost, gained, or shared when atoms form compounds are called
a.
ions.
c.
d electrons.
b.
valence electrons.
d.
electron clouds.
 

 80. 
The number of valence electrons in Group 1 elements is
a.
1.
c.
8.
b.
2.
d.
equal to the period number.
 

 81. 
The number of valence electrons in Group 17 elements is
a.
7.
c.
17.
b.
8.
d.
equal to the period number.
 

 82. 
Among the d-block elements, as atomic radii decrease, electronegativity values
a.
remain constant.
c.
decrease.
b.
increase.
d.
drop to zero.
 



 
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