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Chm 1.3. Matter: Properties and Change - Physical and Chemical Properties of Atoms based on
Periodic Table Location - Chapter 4 and 5
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
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1. 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).
2. 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.
3. 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
4. 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.
5. 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.
6. 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.
7. The p orbitals are shaped like
a. electrons.
c. dumbbells.
b. circles.
d. spheres.
8. 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.
9. The number of orbitals for the d sublevel is
a. 1.
c. 5.
b. 3.
d. 7.
10. For the f sublevel, the number of orbitals is
a. 5.
c. 9.
b. 7.
d. 18.
____ 11. The total number of orbitals that can exist at the second main energy level is
a. 2.
c. 4.
b. 3.
d. 8.
____ 12. 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
____ 13. How many electrons are needed to completely fill the fourth energy level?
a. 8
c. 32
b. 18
d. 40
____ 14. At n = 1, the total number of electrons that could be found is
a. 1.
c. 6.
b. 2.
d. 18.
____ 15. The atomic sublevel with the next highest energy after 4p is
a. 4d.
c. 5p.
b. 4f.
d. 5s.
____ 16. In the electron configuration for scandium (atomic number 21), what is the notation for the three highestenergy electrons?
a. 3d1 4s2
c. 3d3
3
b. 4s
d. 4s2 4p1
____ 17. 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
____ 18. 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.
____ 19. 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.
____ 20. 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.
____ 21. 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
____ 22. 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.
____ 23. 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
____ 24. 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
____ 25. Argon, krypton, and xenon are
a. alkaline earth metals.
c. actinides.
b. noble gases.
d. lanthanides.
____ 26. 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.
____ 27. 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.
____ 28. 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
c. 72
b. 68
d. 90
____ 29. 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
____ 30. Refer to the figure below. To which group do fluorine and chlorine belong?
a. alkaline-earth metals
b. transition elements
c. halogens
d. actinides
____ 31. A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 32. Refer to the figure above. Potassium and bromine belong to
a. Period 4.
c. Period 1.
b. Group 4.
d. Group 1.
____ 33. The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period
a. 2.
c. 6.
b. 3.
d. 13.
____ 34. 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
____ 35. The period of an element can be determined from its
a. reactivity.
c. symbol.
b. density.
d. electron configuration.
____ 36. Elements to the right side of the periodic table (p-block elements) have properties most associated with
a. gases.
c. metals.
b. nonmetals.
d. metalloids.
____ 37. 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
____ 38. Elements in which the d-sublevel is being filled have the properties of
a. metals.
c. metalloids.
b. nonmetals.
d. gases.
____ 39. The group of 14 f block elements in the sixth period is the
a. actinides.
c. transition elements.
b. lanthanides.
d. metalloids.
____ 40. 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.
____ 41. 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.
____ 42. 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.
____ 43. To which block do the actinide elements belong?
a. d block
c. f block
b. s block
d. p block
____ 44. 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.
____ 45. 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
____ 46. 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
____ 47. In nature, the alkali metals occur as
a. elements.
c. complex ions.
b. compounds.
d. gases.
____ 48. The elements in Group 1 are also known as the
a. alkali metals.
c. Period 1 elements.
b. rare-earth series.
d. actinide series.
____ 49. Which block in the periodic table contains the alkali metals?
a. s
c. d
b. p
d. f
____ 50. The most reactive group of the nonmetals is the
a. lanthanides.
c. halogens.
b. transition elements.
d. noble gases.
____ 51. 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.
____ 52. 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.
____ 53. 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.
____ 54. 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.
____ 55. 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.
____ 56. The element that has the greatest electronegativity is
a. oxygen.
c. chlorine.
b. sodium.
d. fluorine.
____ 57. A positive ion is known as a(n)
a. ionic radius.
c. cation.
b. valence electron.
d. anion
____ 58. A negative ion is known as a(n)
a. ionic radius.
c. cation.
b. valence electron.
d. anion.
____ 59. 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.
____ 60. 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.
____ 61. 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.
____ 62. 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.
____ 63. 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.
____ 64. 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.
____ 65. 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.
____ 66. 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.
____ 67. 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.
____ 68. 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.
____ 69. The number of valence electrons in Group 1 elements is
a. 1.
c. 8.
b. 2.
d. equal to the period number.
____ 70. The number of valence electrons in Group 17 elements is
a. 7.
c. 17.
b. 8.
d. equal to the period number.
____ 71. 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.
Short Answer
72. The electron configuration for nitrogen is 1s2 2s2 2p3. What does the 3 in 2p3 mean?
Problem
73. Write the electron configuration for nitrogen, atomic number 7.
74. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
75. Write the noble-gas electron configuration for silicon.
76. Draw the orbital diagram for phosphorus.
77. Draw the orbital diagram for argon.
78. Write the noble-gas electron configuration represented in the orbital diagram below.
79. What element's orbital diagram is shown in the figure below?
Essay
80. 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.
Chm 1.3. Matter: Properties and Change - Physical and Chemical Properties of Atoms based on
Periodic Table Location - Chapter 4 and 5
Answer Section
MULTIPLE CHOICE
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SHORT ANSWER
72. ANS:
The 3 in 2p3 indicates that three electrons are in the p orbitals of the second energy level.
DIF: II
REF: 3
OBJ: 3
REF: 3
OBJ: 3
PROBLEM
73. ANS:
1s2 2s2 2p3
DIF: III
74. ANS:
bromine
DIF: III
75. ANS:
[Ne] 3s2 3p2
REF: 3
OBJ: 3
DIF: III
76. ANS:
REF: 3
OBJ: 3
DIF: III
77. ANS:
REF: 3
OBJ: 3
DIF: III
78. ANS:
[Ne] 3s2 3p4
OBJ: 4-3.3
DIF: III
79. ANS:
fluorine
REF: 3
OBJ: 3
DIF: III
REF: 3
OBJ: 3
ESSAY
80. 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.
DIF: II
REF: 3
OBJ: 2