Download Periodic Table Review File

Chapter 5 test review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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1. 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.
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2. 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.
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3. 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.
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4. 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.
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5. Mendeleev predicted that the spaces in his periodic table represented
a. isotopes.
c. unstable elements.
b. radioactive elements.
d. undiscovered elements.
____
6. The person whose work led to a periodic table based on increasing atomic number was
a. Moseley.
c. Rutherford.
b. Mendeleev.
d. Cannizzaro.
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7. 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.
____
8. The periodic table
a. permits the properties of an element to be predicted before the element is discovered.
b. will be completed with element 118.
c. has been of little use to chemists since the early 1900s.
d. was completed with the discovery of the noble gases.
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9. Evidence gathered since Mendeleev's time indicates that a better arrangement than atomic mass for elements
in the periodic table is an arrangement by
a. mass number.
c. group number.
b. atomic number.
d. series number.
____ 10. The discovery of what elements added a new column to Mendeleev's periodic table?
a. noble gases
c. transition elements
b. radioactive elements
d. metalloids
____ 11. What are the radioactive elements with atomic numbers from 90 to 103 called?
a. the noble gases
b. the lanthanides
c. the actinides
d. the rare-earth elements
____ 12. 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
____ 13. Argon, krypton, and xenon are
a. alkaline earth metals.
b. noble gases.
c. actinides.
d. lanthanides.
____ 14. 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.
____ 15. The periodic law states that the properties of elements are periodic functions of their atomic numbers. What
determines the position of each element in the periodic table?
a. mass number
c. number of protons
b. number of neutrons
d. number of isotopes
____ 16. 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.
____ 17. The periodic law allows some properties of an element to be predicted based on its
a. position in the periodic table.
c. symbol.
b. number of isotopes.
d. color.
____ 18. The periodic law states that
a. no two electrons with the same spin can be found in the same place in an atom.
b. the physical and chemical properties of the elements are functions of their atomic
numbers.
c. electrons exhibit properties of both particles and waves.
d. the chemical properties of elements can be grouped according to periodicity but physical
properties cannot.
____ 19. 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.
____ 20. The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in
this group is
a. 4.
c. 11.
b. 10.
d. 18.
____ 21. How much greater is the atomic number of the fourth element in groups 1, 2 and 18 than the preceding
element?
a. 3
c. 18
b. 4
d. 20
____ 22. Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth
element in Group 18?
a. 54
b. 68
c. 72
d. 90
____ 23. Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next
element in Group 2?
a. 64
c. 88
b. 74
d. 103
____ 24. For elements in groups 1, 2, and 18, the increase in atomic number for successive elements follows the pattern
8, 8, 18, ?, 32. What number completes the pattern?
a. 18
c. 24
b. 20
d. 26
____ 25. Refer to the figure below. To which group do fluorine and chlorine belong?
a. alkaline-earth metals
b. transition elements
c. halogens
d. actinides
____ 26. A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 27. Refer to the figure above. Potassium and bromine belong to
a. Period 4.
c. Period 1.
b. Group 4.
d. Group 1.
____ 28. The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period
a. 2.
c. 6.
b. 3.
d. 13.
____ 29. Identify the sublevels in a period that contains 32 elements.
a. s, f
c. s, p, d
b. s, p
d. s, p, d, f
____ 30. How many elements are in a period in which only the s and p sublevels are filled?
a. 2
c. 18
b. 8
d. 32
____ 31. 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
____ 32. Because the first energy level contains only the 1s sublevel, the number of elements in this period is
a. 1.
c. 4.
b. 2.
d. 8.
____ 33. In Period 3 there are 8 elements. What sublevel(s) is (are) being filled?
a. s
c. s and p
b. s and d
d. d and f
____ 34. Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel?
a. 8
c. 16
b. 10
d. 18
____ 35. The period of an element can be determined from its
a. reactivity.
c. symbol.
b. density.
d. electron configuration.
____ 36. 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
____ 37. In the elements shown in the figure below, the s sublevel of the highest occupied energy level
a.
b.
c.
d.
always contains one electron.
always contains two electrons.
varies in the number of electrons it contains.
is always empty.
____ 38. Elements to the right side of the periodic table (p-block elements) have properties most associated with
a. gases.
b. nonmetals.
c. metals.
d. metalloids.
____ 39. Neutral atoms with an s2p6 electron configuration in the highest energy level belong to which block of the
periodic table?
a. s block
c. d block
b. p block
d. f block
____ 40. Elements in which the d-sublevel is being filled have the properties of
a. metals.
c. metalloids.
b. nonmetals.
d. gases.
____ 41. The group of 14 f block elements in the sixth period is the
a. actinides.
c. transition elements.
b. lanthanides.
d. metalloids.
____ 42. Within the p-block elements, the elements at the top of the table, compared with those at the bottom,
a. have larger radii.
c. have lower ionization energies.
b. are more metallic.
d. are less metallic.
____ 43. The electron configurations of the noble gases from neon to radon in the periodic table make these elements
part of the
a. f block.
c. s block.
b. d block.
d. p block.
____ 44. Hydrogen is placed separately from other elements in the periodic table because it
a. is a gas.
b. does not exist as a free element in nature.
c. has atomic number one.
d. has many unique properties.
____ 45. To which block do the actinide elements belong?
a. d block
c. f block
b. s block
d. p block
____ 46. The elements whose electron configurations end with s2 p5 in the highest occupied energy level belong to
Group
a. 3.
c. 10.
b. 7.
d. 17.
____ 47. For groups 13 through 18, the total number of electrons in the highest occupied level equals the group number
a. plus 1.
c. plus 5.
b. minus 1.
d. minus 10.
____ 48. Strontium's highest occupied energy level is 5s2. To what group does strontium belong?
a. Group 2
c. Group 6
b. Group 5
d. Group 8
____ 49. If n stands for the highest occupied energy level, the outer configuration for all Group 1 elements is
a. ns1.
c. n – s.
b. 2n.
d. np1.
____ 50. Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong?
a. Group 2
c. Group 4
b. Group 3
d. Group 5
____ 51. Nitrogen's electron configuration is 1s2 2s2 2p3. To what group does nitrogen belong?
a. Group 2
c. Group 15
b. Group 7
d. Group 17
____ 52. The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong?
a. Group 4
c. Group 7
b. Group 5
d. Group 9
____ 53. Bromine, atomic number 35, belongs to Group 17. How many electrons does bromine have in its outermost
energy level?
a. 7
c. 18
b. 17
d. 35
____ 54. Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium
belong?
a. Group 2
c. Group 5
b. Group 3
d. Group 12
____ 55. In nature, the alkali metals occur as
a. elements.
b. compounds.
c. complex ions.
d. gases.
____ 56. The elements in Group 1 are also known as the
a. alkali metals.
c. Period 1 elements.
b. rare-earth series.
d. actinide series.
____ 57. Which block in the periodic table contains the alkali metals?
a. s
c. d
b. p
d. f
____ 58. The most reactive group of the nonmetals is the
a. lanthanides.
c. halogens.
b. transition elements.
d. noble gases.
____ 59. 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.
____ 60. The first member of the noble gas family, whose highest energy level consists of an octet of electrons, is
a. helium.
c. neon.
b. argon.
d. krypton.
____ 61. 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.
____ 62. 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.
____ 63. When determining the size of an atom by measuring the distance between bonded, identical, adjacent nuclei,
the radius of an atom is
a. equal to the distance between nuclei.
b. one-half the distance between nuclei.
c. twice the distance between nuclei.
d. one-fourth the distance between nuclei.
____ 64. When an electron is added to a neutral atom, a certain amount of energy is
a. always absorbed.
b. always released.
c. either released or absorbed.
d. transferred to the more electronegative element.
____ 65. Which represents a neutral atom acquiring an electron in a process where energy is released?
a. A + e– + energy  A–
b. A + e–  A– – energy
c. A + e–  A– + energy
d. A– + energy  A + e–
____ 66. The energy required to remove an electron from an atom is the atom's
a. electron affinity.
c. electronegativity.
b. electron energy.
d. ionization energy.
____ 67. A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the
compound is called
a. electron affinity.
c. electronegativity.
b. electron configuration.
d. ionization potential.
____ 68. 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.
____ 69. 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
____ 70. 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.
____ 71. The element that has the greatest electronegativity is
a. oxygen.
c. chlorine.
b. sodium.
d. fluorine.
____ 72. A positive ion is known as a(n)
a. ionic radius.
b. valence electron.
c. cation.
d. anion
____ 73. A negative ion is known as a(n)
a. ionic radius.
b. valence electron.
c. cation.
d. anion.
____ 74. 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.
____ 75. 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.
____ 76. 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.
____ 77. 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.
____ 78. 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.
____ 79. 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.
____ 80. 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.
____ 81. The ionization energies required to remove successive electrons from one mole of calcium atoms are 590
kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably
a. Ca+.
c. Ca3+.
2+
b. Ca .
d. Ca4+.
____ 82. For each successive electron removed from an atom, the ionization energy
a. increases.
c. remains the same.
b. decreases.
d. shows no pattern.
____ 83. 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.
____ 84. 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.
____ 85. 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.
____ 86. The force of attraction by Group 1 metals for their valence electrons is
a. weak.
c. strong.
b. zero.
d. greater than that for inner shell electrons.
____ 87. 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.
____ 88. Valence electrons are those s and p electrons
a. closest to the nucleus.
b. in the lowest energy level.
c. in the highest energy level.
d. combined with protons.
____ 89. The number of valence electrons in Group 1 elements is
a. 1.
c. 8.
b. 2.
d. equal to the period number.
____ 90. In Group 2 elements, the valence electrons are in sublevel
a. d.
c. s.
b. p.
d. f.
____ 91. The number of valence electrons in Group 17 elements is
a. 7.
c. 17.
b. 8.
d. equal to the period number.
____ 92. For groups 13 through 18, the number of valence electrons is equal to the group number
a. plus 1.
c. minus the period number.
b. plus the period number.
d. minus 10.
____ 93. In groups 13 through 18, valence electrons may be in sublevels
a. s and d.
c. d and f.
b. s and p.
d. p and d.
____ 94. Across a period, ionization energies of d-block elements generally
a. increase.
c. remain constant.
b. decrease.
d. drop to zero.
____ 95. The first electrons to be removed when d-block elements form ions are the
a. d electrons.
c. s electrons.
b. p electrons.
d. f electrons.
____ 96. Which groups in the main group have lower electronegativity than d-block elements?
a. groups 1 and 2
c. groups 17 and 18
b. groups 13 through 18
d. groups 13 through 17
____ 97. Among the d-block elements, as atomic radii decrease, electronegativity values
a. remain constant.
b. increase.
c. decrease.
d. drop to zero.
Short Answer
98. In terms of the periodic law, explain which two of these elements are most similar: sodium (element 11),
phosphorus (element 15), and sulfur (element 16).
99. What can you predict about the properties of xenon and helium, both in Group 18 in the periodic table? Why?
Essay
100. Explain nuclear charge and how it affects the general trend in radii of atoms of elements going from left to
right across a period in the periodic table.
Chapter 5 test review
Answer Section
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A
4
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: III
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
95. ANS:
OBJ:
96. ANS:
OBJ:
97. ANS:
OBJ:
C
4
A
4
B
4
PTS: 1
DIF: I
REF: 3
PTS: 1
DIF: II
REF: 3
PTS: 1
DIF: II
REF: 3
SHORT ANSWER
98. ANS:
Their locations in the periodic table indicate that phosphorus and sulfur are nonmetals and sodium is a metal.
Nonmetals are a group with characteristic properties, so phosphorus and sulfur are the most similar elements
of the three.
PTS: 1
DIF: III
REF: 1
OBJ: 3
99. ANS:
In the periodic table, elements in the same column or group have similar properties. Because helium and
xenon are in the same group, they have similar properties.
PTS: 1
DIF: I
REF: 1
OBJ: 4
ESSAY
100. ANS:
Nuclear charge is the attraction an atomic nucleus has on the electrons surrounding it. As you move from left
to right across a period, the atomic number increases, and therefore the number of protons in the nucleus
increases. The more protons within a nucleus, the greater is the nuclear charge. A greater nuclear charge pulls
the electrons closer to the nucleus, decreasing the atomic radius.
PTS: 1
DIF: II
REF: 3
OBJ: 2