Download Chemistry I Chapter 5 Study Guide Multiple Choice Identify the

Chemistry I Chapter 5 Study Guide
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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1. The noble gases, such as helium and xenon, are non-reactive because:
a. they have completely filled outer electron shells.
b. they are chemically unstable.
c. they are unusually large atoms.
d. they have been around longest on the earth.
2. Elements in the same column on the periodic table have similar chemical reactivity because:
a. they contain similar amounts of energy.
b. they have the same number of valence shell electrons.
c. atoms prefer to have completely full or completely empty valence shells.
d. they have similar numbers of isotopes.
3. Chlorine, element number 17, is located in the third row and the next-to-the-last group of the periodic table. How many
electron shells would be completely filled by a neutral atom of chlorine? How many electrons would be left over?
a. 1 shell filled, 7 electrons left over
b. 1 shell filled, 1 electron left over
c. 2 shells filled, 7 electrons left over
d. 2 shells filled, 1 electron left over
4. How many energy levels are filled in a krypton atom?
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a. Three.
b. Four.
c. Five.
d. Six.
The electronegativity of an element is defined as:
a. the attraction an atom has for the shared pair of electrons in a covalent bond.
b. the attraction an atom has for the shared pair of electrons in an ionic bond.
c. the amount of static electricity an element produces.
d. the amount of charge one atom of an element produces.
Which of the following is true for valence electrons?
a. Valence electrons are always located in the innermost energy level.
b. Valence electrons may be lost or gained by an atom when bonding occurs with another atom.
c. Each element in the periodic table has a different number of valence electrons.
d. Valence electrons are found only in radioactive isotopes.
Mendeleev arranged the known chemical elements in a table according to increasing
a. atomic number.
c. number of protons.
b. number of electrons.
d. mass.
Which list of elements contains only metals?
a. carbon, iodine, tin
c. helium, iron, copper
b. tin, copper, cesium
d. iodine, carbon, argon
As you move from left to right across a period, the number of valence electrons
a. increases.
c. increases and then decreases.
b. stays the same.
d. decreases.
A member of the boron family has three valence electrons, while a member of the nitrogen family has
a. none.
c. four.
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b. five.
d. three.
11. Which statement is NOT true about the elements fluorine, chlorine, and iodine?
a. They are all halogens.
c. They are similar to noble gases.
b. They react easily with metals.
d. They are all nonmetals.
12. The person whose work led to a periodic table based on increasing atomic number was
a. Moseley.
c. Rutherford.
b. Mendeleev.
d. Cannizzaro.
13. The electron configuration of aluminum, atomic number 13, is [Ne] 3s2 3p1. Aluminum is in Period
a. 2.
c. 6.
b. 3.
d. 13.
14. 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
15. 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
16. 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
17. 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.
18. Period 4 contains 18 elements. How many of these elements have electrons in the d sublevel?
a. 8
c. 16
b. 10
d. 18
19. In the elements shown in the figure below, the s sublevel of the highest occupied energy level
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a. always contains one electron.
b. always contains two electrons.
c. varies in the number of electrons it contains.
d. is always empty.
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.
Elements in which the d-sublevel is being filled have the properties of
a. metals.
c. metalloids.
b. nonmetals.
d. gases.
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.
Hydrogen is placed separately from other elements in the periodic table because it
a. is a gas.
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b. does not exist as a free element in nature.
c. has atomic number one.
d. has many unique properties.
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
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.
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.
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.
The element that has the greatest electronegativity is
a. oxygen.
c. chlorine.
b. sodium.
d. fluorine.
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.
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.
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.
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.
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.
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.
Valence electrons are those s and p electrons
a. closest to the nucleus.
c. in the highest energy level.
b. in the lowest energy level.
d. combined with protons.
In Group 2 elements, the valence electrons are in sublevel
a. d.
c. s.
b. p.
d. f.
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37. Across a period, ionization energies of d-block elements generally
a. increase.
c. remain constant.
b. decrease.
d. drop to zero.
38. 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
Figure 5-4
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39. Based on Figure 5-4, what general trend exists for first ionization energy across a period, from left to right?
a. Ionization energy increases.
b. Ionization energy decreases.
c. Ionization energy remains fairly constant.
d. Ionization energy first increases, then decreases.
40. Based on Figure 5-4, what general trend exists for first ionization energy down a group?
a. Ionization energy increases.
b. Ionization energy decreases.
c. Ionization energy remains fairly constant.
d. Ionization energy first increases, then decreases.
41. In Figure 5-4, which group tends to have the highest ionization energy? The lowest?
a. halogens; alkaline earth metals
c. alkali metals; noble gases
b. alkaline earth metals; halogens
d. noble gases; alkali metals
42. In Figure 5-4, which period tends to have the highest ionization energy? The lowest?
a. 1; 4
c. 2; 3
b. 4; 1
d. 3; 2
43. To find the number of neutrons in an atom, you would subtract
a. mass number from atomic number.
c. atomic number from electron number.
b. atomic number from mass number.
d. isotope number from atomic number.
44. Suppose an atom has a mass number of 23. Which statement is true beyond any doubt?
a. The atom has an odd number of neutrons.
b. The atomic number is less than 11.
c. The atom is not an isotope.
d. The number of protons in the nucleus does not equal the number of neutrons.
45. Which statement is true about oxygen-17 and oxygen-18?
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a. They do not have the same number of protons.
b. Their atoms have an identical mass.
c. They are isotopes of oxygen.
d. The have the same mass number.
46. Which statement accurately represents the arrangement of electrons in Bohr’s atomic model?
a. Electrons vibrate in fixed locations around the nucleus.
b. Electrons travel around the nucleus in fixed energy levels with energies that vary from level to
level.
c. Electrons travel around the nucleus in fixed energy levels with equal amounts of energy.
d. Electrons travel randomly in the relatively large space outside the nucleus.
47. What does the electron cloud model describe?
a. the most likely locations of electrons in atoms
b. the precise locations of electrons in atoms
c. the number of electrons in an atom
d. the mass of the electrons in an atom
Short Answer
48. Selenium has six valence electrons, while rubidium has one valence electron. Identify each element as a metal or a
nonmetal.
49. The elements silicon (atomic number 14) and chlorine (atomic number 17) are both in Period 3. Which is the more
reactive element?
50. Referring to a periodic table, state the block of elements in which each of the following is found and explain why it is
found there, in terms of electron configuration: calcium (Ca), chromium (Cr), samarium (Sm), and chlorine (Cl).
51. In terms of electrons and atomic structure, account for what happens to first ionization energy, moving down a group and
across a period of the periodic table.
52. Suppose you have just discovered three new elements. Element 1 is a solid at room temperature, a fair conductor of heat
and electricity, and not ductile. Element 2 is a solid at room temperature and lustrous. Element 3 is a gas at room
temperature and a poor conductor of heat and electricity. Classify each element as either a metal, nonmetal, or
semimetal. Explain your reasoning. Then state one additional property that each element is likely to have.
53. Write abbreviated electron configurations for each of the following: element 14, element 48, element 53, and element 70.
To which chemical family group does each belong?
54. If an atom has 34 protons and 40 neutrons, what is its mass number?
Numeric Response
55. How many valence electrons does an iodine atom have?
56. How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
57. How many unshared pairs of electrons in a nitrogen atom?
58. How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
59. How many unshared pairs of electrons are in a hydrogen atom?
Completion
Complete each statement.
60. According to ____________________, all matter was made up of four elements — earth, air, fire, and water.
61. John Dalton concluded that all the atoms of a single ____________________ have the same mass.
62. John Dalton observed that elements always combine in the same ratio to form a particular ____________________.
63. The subatomic particle that J. J. Thomson discovered has a(an) ____________________ charge.
64. In Rutherford’s gold foil experiment, shown in Figure 4-1, alpha particles that bounce straight back from the foil have
struck ____________________ in the gold atoms.
65. In Rutherford’s gold foil experiment, some of the _________________________ aimed at gold atoms bounced back,
suggesting that a solid mass was at the center of the atom.
66. The results of Rutherford’s gold foil experiment demonstrated that the ____________________ occupies a very small
amount of the total space inside an atom.
67. Protons and ____________________ are found in the nucleus of an atom.
68. Neutrons and ____________________ have almost the same mass.
69. If element Q has 11 protons, 12 neutrons and 10 electrons it is an ion of __________.
70. The nuclei of isotopes contain different numbers of ____________________.
71. The ____________________ of an isotope is the sum of the number of protons and neutrons in its nucleus.
72. In Bohr’s model of the atom, ____________________ move in fixed orbits around the nucleus.
73. The region in which an electron is most likely to be found is called a(an) ____________________.
Other
USING SCIENCE SKILLS
Figure 5-2
74. Using Tables and Graphs Which of the elements shown in Figure 5-2 are in the same period?
75. Classifying Which element in Figure 5-2 is a transition metal? Which is a noble gas?
76. Using Tables and Graphs Which elements in Figure 5-2 have the same number of valence electrons? How do you
know?
Figure 5-3
77. Predicting Explain why knowing the properties of K, Ca, Sc, and Ti would allow you to predict the properties of Rb, Sr,
Y, and Zr.
78. Comparing and Contrasting In Figure 4-2, what is the main difference between the atomic model in panel 1 and the
model in panel 2?
79. Comparing and Contrasting In Figure 4-2, what is the main difference between the atomic model in panel 2 and the
model in panel 3?
80. Interpreting Graphics Are the atomic models in Figure 4-2 arranged in the order that they were developed? Explain
your answer.
Chemistry I Chapter 5 Study Guide
Answer Section
MULTIPLE CHOICE
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knowledge
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SC-HS-1.1.1
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SC-HS-1.1.1
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DIF:
intermediate
intermediate
advanced
advanced
basic
basic
L1
REF:
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REF:
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REF:
OBJ:
chapter 18 | section 18.3
chapter 18 | section 18.3
chapter 18 | section 18.3
chapter 18 | section 18.3
chapter 19 | section 19.1
chapter 19 | section 19.1
5.1.1
PTS:
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knowledge
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knowledge
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knowledge
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comprehension
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DIF:
L1
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5.2.3
DIF:
L1
OBJ:
5.3.1
DIF:
L1
OBJ:
5.3.1
DIF:
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OBJ:
5.3.1
DIF:
I
REF:
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II
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II
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2
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I
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III
REF:
2
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II
REF:
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II
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I
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I
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SC-HS-1.1.2
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knowledge
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knowledge
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DIF:
5E 5.f
5E 5.f
5E 5.f
5E 5.f
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4.2.2
DIF:
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4.2.2
DIF:
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4.3.1
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4.3.2
SHORT ANSWER
48. ANS:
Selenium is a nonmetal. Rubidium is a metal.
PTS: 1
DIF:
BLM: comprehension
49. ANS:
chlorine
L2
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5.3.1
STA:
SC-HS-1.1.1
PTS: 1
DIF:
BLM: comprehension
50. ANS:
L2
OBJ:
5.3.2
STA:
SC-HS-1.1.1
Calcium is in the s-block of elements because all its valence electrons are s-electrons (configuration is [Ar]4s2).
Chromium is in the d-block of elements because some of its outer electrons are d-electrons and it has no f outer electrons
(configuration is [Ar]4s13d5). Samarium is in the f-block of elements because some of its outer electrons are f electrons
(configuration [Xe]6s24f6). Chlorine is in the p-block of elements because it contains p valence electrons (configuration
[Ne]3s23p5).
PTS: 1
OBJ: 5E 5.d
51. ANS:
Ionization energy decreases down a group because atoms are becoming increasingly large and attraction between the
nucleus and outermost electrons is becoming less, so less energy is required to remove an electron. Ionization energy
increases moving from left to right across a period because the atoms are becoming smaller and the nucleus is becoming
more positively charged, resulting in increased attraction between nucleus and electrons and increased energy needed to
remove an electron.
PTS: 1
OBJ: 5E 5.f
52. ANS:
Element 1 has properties that are typical of semimetals; another property it is likely to have is moderate luster. Element 2
has properties that are typical of metals; another likely property is the ability to conduct heat and electricity. Element 3
has properties that are typical of nonmetals; another likely property is nonmalleability (if converted to a solid).
PTS: 1
OBJ: 5E 5.d
53. ANS:
Element 14: 10 electrons accounted for by [Ne], 4 remaining, so configuration is [Ne]3s23p2; elements with such
configurations belong in Group 4A.
Element 48: 36 electrons accounted for by [Kr], 12 remaining, so configuration is [Kr]5s24d10. Elements with such
configurations belong in Group 2B.
Element 53: 36 electrons accounted for by [Kr], 17 remaining, so configuration is [Kr]5s24d105p5. Elements with such
configurations belong in Group 7A.
Element 70: 54 electrons accounted for by [Xe], 16 remaining, so configuration is [Xe]6s24f14. Elements with such
configurations belong in the chemical family that makes up its own series below the main body of the periodic table.
PTS: 1
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74
OBJ:
5E 5.d
DIF:
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4.2.2
STA:
SC-HS-1.1.2
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STA: SC.HS.1.1.7
56. ANS: 3
DIF:
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REF:
p. 218
OBJ:
8.2.1
PTS: 1
STA: SC.HS.1.1.7
57. ANS: 1
DIF:
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REF:
p. 219
OBJ:
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58. ANS: 4
DIF:
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REF:
p. 219
OBJ:
8.2.2
PTS: 1
BLM: knowledge
NUMERIC RESPONSE
55. ANS: 7
PTS: 1
STA: SC.HS.1.1.7
59. ANS: 3
DIF:
L2
REF:
p. 219
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p. 220
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61. ANS: element
DIF:
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4.1.1
BLM: knowledge
PTS: 1
62. ANS: compound
DIF:
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4.1.2
BLM: knowledge
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63. ANS: negative
DIF:
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4.1.2
BLM: knowledge
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64. ANS: nuclei
DIF:
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4.1.3
BLM: knowledge
PTS: 1
DIF:
65. ANS: alpha particles
L1
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4.1.3
BLM: knowledge
PTS: 1
66. ANS: nucleus
DIF:
L1
OBJ:
4.1.3
BLM: knowledge
PTS: 1
67. ANS: neutrons
DIF:
L2
OBJ:
4.1.3
BLM: comprehension
PTS: 1
BLM: knowledge
68. ANS: protons
DIF:
L1
OBJ:
4.2.1
STA:
SC-HS-1.1.2
PTS: 1
BLM: knowledge
69. ANS: sodium
DIF:
L1
OBJ:
4.2.1
STA:
SC-HS-1.1.2
PTS: 1
BLM: knowledge
70. ANS: neutrons
DIF:
L1
OBJ:
4.2.2
STA:
SC-HS-1.1.2
PTS: 1
BLM: knowledge
71. ANS: mass number
DIF:
L1
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4.2.2
STA:
SC-HS-1.1.2
PTS: 1
BLM: knowledge
72. ANS: electrons
DIF:
L1
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4.2.2
STA:
SC-HS-1.1.2
PTS: 1
73. ANS: orbital
DIF:
L1
OBJ:
4.3.1
BLM: knowledge
PTS:
STA:
1
SC.HS.1.1.7
COMPLETION
60. ANS: Aristotle
PTS:
1
DIF:
L1
OBJ:
4.3.2
BLM: knowledge
DIF:
L1
OBJ:
5.2.1
STA:
SC-HS-1.1.1
PTS: 1
DIF: L1
OBJ: 5.2.3
BLM: knowledge
76. ANS:
F and I; they are in the same group in the periodic table.
STA:
SC-HS-1.1.1
OTHER
74. ANS:
Be, C, N, and F
PTS: 1
BLM: knowledge
75. ANS:
V; He
PTS: 1
DIF: L2
OBJ: 5.3.1
STA: SC-HS-1.1.1
BLM: comprehension
77. ANS:
When elements are arranged in a periodic table in order of increasing atomic number, the properties of elements repeat
from period to period so that elements in the same group have similar properties.
PTS: 1
DIF: L3
OBJ: 5.2.1
STA: SC-HS-1.1.1
BLM: synthesis
78. ANS:
Panel 1 depicts an atom as a solid sphere without any subatomic particles. Panel 2 shows an atom that has a subatomic
structure.
PTS: 1
DIF: L1
OBJ: 4.1.2 | 4.2.1 | 4.3.1
STA: SC-HS-1.1.2 BLM: knowledge
79. ANS:
The main difference is the way in which electron motion is depicted. In panel 2, the movement of electrons is
represented by fixed circular orbits. In panel 3, the probable locations of the moving electrons are represented by a cloud.
PTS: 1
DIF: L1
OBJ: 4.3.1 | 4.3.2
BLM: knowledge
80. ANS:
Yes; they go from the simplest (the solid sphere in 1) to the most complex (the electron cloud model in panel 3).
Students may specifically cite John Dalton in connection with panel 1 and Niels Bohr in connection with panel 2 to
support their answer.
PTS: 1
BLM: knowledge
DIF:
L1
OBJ:
4.1.2 | 4.3.1 | 4.3.2