Download periodic trends

periodic trends
Matching
Match each item with the correct statement below.
a. electronegativity
f.
b. ionization energy
g.
c. atomic radius
h.
d. metal
i.
e. transition metal
j.
periodic law
cation
period
group
electrons
____
1. horizontal row in the periodic table
____
2. vertical column in the periodic table
____
3. A repetition of properties occurs when elements are arranged in order of increasing atomic number.
____
4. type of element that is a good conductor of heat and electric current
____
5. type of element characterized by the presence of electrons in the d orbital
____
6. one-half the distance between the nuclei of two atoms when the atoms are joined
____
7. type of ion formed by Group 2A elements
____
8. subatomic particles that are transferred to form positive and negative ions
____
9. ability of an atom to attract electrons when the atom is in a compound
____ 10. energy required to remove an electron from an atom
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 11. What is another name for the representative elements?
a. Group A elements
c. Group C elements
b. Group B elements
d. transition elements
____ 12. What is another name for the transition metals?
a. noble gases
c. Group B elements
b. Group A elements
d. Group C elements
____ 13. Which of the following elements is in the same period as phosphorus?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____ 14. Each period in the periodic table corresponds to ____.
a. a principal energy level
c. an orbital
b. an energy sublevel
d. a suborbital
____ 15. The modern periodic table is arranged in order of increasing atomic ____.
a. mass
c. number
b. charge
d. radius
____ 16. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of
missing elements?
a. Henry Moseley
c. John Dalton
b. Antoine Lavoisier
d. Dmitri Mendeleev
____ 17. Which of the following categories includes the majority of the elements?
a. metalloids
c. metals
b. liquids
d. nonmetals
____ 18. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
c. Li
b. V
d. Kr
____ 19. To what category of elements does an element belong if it is a poor conductor of electricity?
a. transition elements
c. nonmetals
b. metalloids
d. metals
____ 20. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
____ 21. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
____ 22. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
c. silicon
b. selenium
d. silver
____ 23. Which of the following is true about the electron configurations of the noble gases?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 24. Elements that are characterized by the filling of p orbitals are classified as ____.
a. groups 3A through 8A
c. inner transition metals
b. transition metals
d. groups 1A and 2A
____ 25. Which of the following electron configurations is most likely to result in an element that is relatively
inactive?
a. a half-filled energy sublevel
b. a filled energy sublevel
c. one empty and one filled energy sublevel
d. a filled highest occupied principal energy level
____ 26. Which subatomic particle plays the greatest part in determining the properties of an element?
a. proton
c. neutron
b. electron
d. none of the above
____ 27. Which of the following elements is a transition metal?
a. cesium
c. tellurium
b. copper
d. tin
____ 28. Which of the following groupings contains only representative elements?
a. Cu, Co, Cd
c. Al, Mg, Li
b. Ni, Fe, Zn
d. Hg, Cr, Ag
____ 29. Which of the following is true about the electron configurations of the representative elements?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 30. What are the Group 1A and Group 7A elements examples of?
a. representative elements
c. noble gases
b. transition elements
d. nonmetallic elements
____ 31. Of the elements Fe, Hg, U, and Te, which is a representative element?
a. Fe
c. U
b. Hg
d. Te
____ 32. How does atomic radius change from top to bottom in a group in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
____ 33. How does atomic radius change from left to right across a period in the periodic table?
a. It tends to decrease.
c. It first increases, then decreases.
b. It tends to increase.
d. It first decreases, then increases.
____ 34. What causes the shielding effect to remain constant across a period?
a. Electrons are added to the same principal energy level.
b. Electrons are added to different principal energy levels.
c. The charge on the nucleus is constant.
d. The atomic radius increases.
____ 35. Atomic size generally ____.
a. increases as you move from left to right across a period
b. decreases as you move from top to bottom within a group
c. remains constant within a period
d. decreases as you move from left to right across a period
____ 36. What element in the second period has the largest atomic radius?
a. carbon
c. potassium
b. lithium
d. neon
____ 37. Which of the following factors contributes to the increase in atomic size within a group in the periodic table
as the atomic number increases?
a. more shielding of the electrons by the highest occupied energy level
b. an increase in size of the nucleus
c. an increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 38. Which of the following elements has the smallest atomic radius?
a. sulfur
c. selenium
b. chlorine
d. bromine
____ 39. What is the charge of a cation?
a. a positive charge
b. no charge
c. a negative charge
d. The charge depends on the size of the nucleus.
____ 40. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
____ 41. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions
b. all form ions with a negative charge
c. all have ions with a 1 charge
d. lose electrons when they form ions
____ 42. Which of the following statements is NOT true about ions?
a. Cations are positively charged ions.
b. Anions are common among nonmetals.
c. Charges for ions are written as numbers followed by a plus or minus sign.
d. When a cation forms, more electrons are transferred to it.
____ 43. Why is the second ionization energy greater than the first ionization energy?
a. It is more difficult to remove a second electron from an atom.
b. The size of atoms increases down a group.
c. The size of anions decreases across a period.
d. The nuclear attraction from protons in the nucleus decreases.
____ 44. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al
c. Rb , Ba , P
b. K , Sr , O
d. N , O , F
____ 45. In which of the following groups of ions are the charges all shown correctly?
a. Li , O , S
c. K , F , Mg
b. Ca , Al , Br
d. Na , I , Rb
____ 46. What is the element with the lowest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 47. What is the element with the highest electronegativity value?
a. cesium
c. calcium
b. helium
d. fluorine
____ 48. Which of the following elements has the smallest ionic radius?
a. Li
c. O
b. K
d. S
____ 49. What is the energy required to remove an electron from an atom in the gaseous state called?
a. nuclear energy
c. shielding energy
b. ionization energy
d. electronegative energy
____ 50. For Group 2A metals, which electron is the most difficult to remove?
a. the first
b. the second
c. the third
d. All the electrons are equally difficult to remove.
____ 51. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic
table as the atomic number increases?
a. increase in atomic size
b. increase in size of the nucleus
c. increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 52. Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
____ 53. Which of the following elements has the lowest electronegativity?
a. lithium
c. bromine
b. carbon
d. fluorine
____ 54. Which statement is true about electronegativity?
a. Electronegativity is the ability of an anion to attract another anion.
b. Electronegativity generally increases as you move from top to bottom within a group.
c. Electronegativity generally is higher for metals than for nonmetals.
d. Electronegativity generally increases from left to right across a period.
____ 55. Compared with the electronegativities of the elements on the left side of a period, the electronegativities of
the elements on the right side of the same period tend to be ____.
a. lower
c. the same
b. higher
d. unpredictable
____ 56. Which of the following decreases with increasing atomic number in Group 2A?
a. shielding effect
c. ionization energy
b. ionic size
d. number of electrons
____ 57. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 58. Which of the following factors contributes to the increase in ionization energy from left to right across a
period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level
____ 59. As you move from left to right across the second period of the periodic table ____.
a. ionization energy increases
c. electronegativity decreases
b. atomic radii increase
d. atomic mass decreases
____ 60. Of the following elements, which one has the smallest first ionization energy?
a. boron
c. aluminum
b. carbon
d. silicon
Short Answer
61. Which group of elements in the periodic table is known as the alkali metals?
62. Which group in the periodic table is known as the noble gases?
63. An element has an atomic number of 80. How many protons and electrons are in an atom of the element?
64. About what percent of elements is classified as metals?
65. What is the electron configuration of oxygen?
66. What is the electron configuration of sulfur?
67. The s and p sublevels of an atom of an element in period 3 are filled with electrons. Which orbitals are filled
in this atom?
68. From which orbital in a lithium atom is an electron transferred to form Li ?
69. What orbital is filled when iodine gains an electron to become a negative ion?
70. In which group in the periodic table do the elements have the highest electronegativity values?
Numeric Response
71. How many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
72. How many electrons are present in the d sublevel of a neutral atom of nickel?
73. How many electrons are in a rubidium ion (Rb )?
74. What is the usual charge on an ion from Group 7A?
75. How many electrons does the ion Ca
contain?
Essay
76. Describe the trends in the atomic size of elements within groups and across periods in the periodic table.
Provide examples.
77. Explain how ions form. Provide examples.
78. Describe the trends in first ionization energy within groups and across periods in the periodic table. Provide
examples.
79. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the
atoms from which they are formed. Explain why this is so.
80. Describe the trends in electronegativity within groups and across periods in the periodic table. Provide
examples.
periodic trends
Answer Section
MATCHING
1. ANS:
OBJ:
STA:
2. ANS:
OBJ:
STA:
3. ANS:
OBJ:
STA:
4. ANS:
OBJ:
5. ANS:
OBJ:
6. ANS:
OBJ:
7. ANS:
OBJ:
8. ANS:
OBJ:
9. ANS:
OBJ:
STA:
10. ANS:
OBJ:
STA:
H
PTS: 1
DIF: L1
REF: p. 157
6.1.1 Explain how elements are organized in a periodic table.
SC4.b
I
PTS: 1
DIF: L1
REF: p. 157
6.1.1 Explain how elements are organized in a periodic table.
SC4.b
F
PTS: 1
DIF: L1
REF: p. 157
6.1.1 Explain how elements are organized in a periodic table.
SC4.b
D
PTS: 1
DIF: L1
REF: p. 158
6.1.3 Identify three broad classes of elements.
STA: SC4.b
E
PTS: 1
DIF: L1
REF: p. 166
6.2.2 Classify elements based on electron configuration. STA: SC3.b
C
PTS: 1
DIF: L1
REF: p. 170
6.3.1 Describe trends among elements for atomic size.
STA: SC4.a | SC4.b
G
PTS: 1
DIF: L1
REF: p. 172
6.3.2 Explain how ions form.
STA: SC3.b
J
PTS: 1
DIF: L1
REF: p. 172
6.3.2 Explain how ions form.
STA: SC3.b
A
PTS: 1
DIF: L1
REF: p. 177
6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
SC4.a | SC4.b | SC3.b
B
PTS: 1
DIF: L1
REF: p. 173
6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
SC4.a | SC4.b | SC3.b
MULTIPLE CHOICE
11. ANS:
OBJ:
STA:
12. ANS:
OBJ:
STA:
13. ANS:
OBJ:
STA:
14. ANS:
OBJ:
STA:
15. ANS:
OBJ:
A
6.1.1
SC4.b
C
6.1.1
SC4.b
B
6.1.1
SC4.b
A
6.1.1
SC4.b
C
6.1.1
PTS: 1
DIF: L1
REF: p. 164
Explain how elements are organized in a periodic table.
PTS: 1
DIF: L1
REF: p. 166
Explain how elements are organized in a periodic table.
PTS: 1
DIF: L1
REF: p. 162 | p. 163
Explain how elements are organized in a periodic table.
PTS: 1
DIF: L2
REF: p. 157
Explain how elements are organized in a periodic table.
PTS: 1
DIF: L2
REF: p. 157
Explain how elements are organized in a periodic table.
STA: SC4.b
16. ANS: D
PTS: 1
DIF: L1
REF:
OBJ: 6.1.2 Compare early and modern periodic tables.
STA:
17. ANS: C
PTS: 1
DIF: L1
REF:
OBJ: 6.1.3 Identify three broad classes of elements.
STA:
18. ANS: D
PTS: 1
DIF: L2
REF:
OBJ: 6.1.3 Identify three broad classes of elements.
STA:
19. ANS: C
PTS: 1
DIF: L3
REF:
OBJ: 6.1.3 Identify three broad classes of elements.
STA:
20. ANS: A
PTS: 1
DIF: L1
REF:
OBJ: 6.2.1 Describe the information in a periodic table.
STA:
21. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.2.1 Describe the information in a periodic table.
STA:
22. ANS: C
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. STA:
23. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. STA:
24. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. STA:
25. ANS: D
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. STA:
26. ANS: B
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. STA:
27. ANS: B
PTS: 1
DIF: L1
REF:
OBJ: 6.2.3 Distinguish representative elements and transition metals.
STA: SC4.b
28. ANS: C
PTS: 1
DIF: L1
REF:
OBJ: 6.2.3 Distinguish representative elements and transition metals.
STA: SC4.b
29. ANS: B
PTS: 1
DIF: L2
REF:
OBJ: 6.2.2 Classify elements based on electron configuration. | 6.2.3
and transition metals.
STA: SC3.b | SC4.b
30. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.2.3 Distinguish representative elements and transition metals.
STA: SC4.b
31. ANS: D
PTS: 1
DIF: L3
REF:
OBJ: 6.2.3 Distinguish representative elements and transition metals.
STA: SC4.b
32. ANS: B
PTS: 1
DIF: L1
REF:
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA:
33. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA:
34. ANS: A
PTS: 1
DIF: L2
REF:
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA:
35. ANS: D
PTS: 1
DIF: L2
REF:
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA:
36. ANS: B
PTS: 1
DIF: L2
REF:
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA:
37. ANS: A
PTS: 1
DIF: L3
REF:
p. 156
SC4.b
p. 158
SC4.b
p. 158
SC4.b
p. 160
SC4.b
p. 162 | p. 163
SC4.b
p. 157
SC4.b
p. 164
SC3.b
p. 164
SC3.b
p. 166
SC3.b
p. 164
SC3.b
p. 164
SC3.b
p. 166
p. 164 | p. 166
p. 164
Distinguish representative elements
p. 164
p. 162 | p. 163 | p. 164
p. 171
SC4.a | SC4.b
p. 171
SC4.a | SC4.b
p. 171
SC4.a | SC4.b
p. 171
SC4.a | SC4.b
p. 171
SC4.a | SC4.b
p. 171
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA: SC4.a | SC4.b
38. ANS: B
PTS: 1
DIF: L3
REF: p. 171 | p. 175
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA: SC4.a | SC4.b
39. ANS: A
PTS: 1
DIF: L1
REF: p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
40. ANS: B
PTS: 1
DIF: L2
REF: p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
41. ANS: D
PTS: 1
DIF: L2
REF: p. 162 | p. 163 | p. 172 | p. 176
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
42. ANS: D
PTS: 1
DIF: L2
REF: p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
43. ANS: A
PTS: 1
DIF: L2
REF: p. 173
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
44. ANS: B
PTS: 1
DIF: L3
REF: p. 162 | p. 163 | p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
45. ANS: B
PTS: 1
DIF: L3
REF: p. 162 | p. 163 | p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
46. ANS: A
PTS: 1
DIF: L1
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
47. ANS: D
PTS: 1
DIF: L1
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
48. ANS: A
PTS: 1
DIF: L2
REF: p. 175
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
49. ANS: B
PTS: 1
DIF: L2
REF: p. 173
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
50. ANS: C
PTS: 1
DIF: L2
REF: p. 173
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
51. ANS: A
PTS: 1
DIF: L2
REF: p. 174
OBJ: 6.3.1 Describe trends among elements for atomic size. | 6.3.3 Describe periodic trends for first
ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
52. ANS: C
PTS: 1
DIF: L2
REF: p. 173
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
53. ANS: A
PTS: 1
DIF: L2
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
54. ANS: D
PTS: 1
DIF: L2
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
55. ANS: B
PTS: 1
DIF: L2
REF: p. 177 | p. 178
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
56. ANS: C
PTS: 1
DIF: L2
REF: p. 178
OBJ: 6.3.1 Describe trends among elements for atomic size. | 6.3.3 Describe periodic trends for first
ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
57. ANS: A
PTS: 1
DIF: L2
REF: p. 172 | p. 176
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
58. ANS: C
PTS: 1
DIF: L3
REF: p. 174
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
59. ANS: A
PTS: 1
DIF: L3
REF: p. 178
OBJ: 6.2.1 Describe the information in a periodic table. | 6.3.3 Describe periodic trends for first ionization
energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
60. ANS: C
PTS: 1
DIF: L3
REF: p. 173
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
SHORT ANSWER
61. ANS:
1A
PTS: 1
DIF: L1
REF: p. 161
OBJ: 6.1.1 Explain how elements are organized in a periodic table.
STA: SC4.b
62. ANS:
8A
PTS: 1
DIF: L1
REF: p. 164
OBJ: 6.1.1 Explain how elements are organized in a periodic table.
STA: SC4.b
63. ANS:
80 protons, 80 electrons
PTS: 1
DIF: L1
REF: p. 157
OBJ: 6.2.1 Describe the information in a periodic table.
64. ANS:
80%
PTS:
OBJ:
STA:
65. ANS:
1s 2s
STA: SC4.b
1
DIF: L2
REF: p. 158
6.1.3 Identify three broad classes of elements. | 6.2.1 Describe the information in a periodic table.
SC4.b
2p
PTS: 1
DIF: L2
REF: p. 162 | p. 166
OBJ: 6.2.2 Classify elements based on electron configuration. STA: SC3.b
66. ANS:
1s 2s 2p 3s 3p
PTS: 1
DIF: L2
REF: p. 166
OBJ: 6.2.2 Classify elements based on electron configuration. STA: SC3.b
67. ANS:
1s, 2s, 2p
PTS: 1
DIF: L3
REF: p. 166
OBJ: 6.2.2 Classify elements based on electron configuration. STA: SC3.b
68. ANS:
2s
PTS: 1
DIF: L2
OBJ: 6.3.2 Explain how ions form.
69. ANS:
5p
REF: p. 164 | p. 172
STA: SC3.b
PTS: 1
DIF: L3
REF: p. 166
OBJ: 6.2.2 Classify elements based on electron configuration. | 6.2.3 Distinguish representative elements
and transition metals.
STA: SC3.b
70. ANS:
7A
PTS: 1
DIF: L2
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
NUMERIC RESPONSE
71. ANS: 5
PTS: 1
DIF: L2
REF: p. 164
OBJ: 6.2.2 Classify elements based on electron configuration. STA: SC3.b
72. ANS: 8
PTS: 1
DIF: L2
REF: p. 166
OBJ: 6.2.2 Classify elements based on electron configuration. | 6.2.3 Distinguish representative elements
and transition metals.
STA: SC4.b | SC3.b
73. ANS: 36
PTS: 1
DIF: L2
OBJ: 6.3.2 Explain how ions form.
74. ANS: 1
REF: p. 162 | p. 172
STA: SC3.b
PTS: 1
STA: SC3.b
75. ANS: 18
REF: p. 172
DIF: L2
PTS: 1
DIF: L3
OBJ: 6.3.2 Explain how ions form.
ESSAY
OBJ: 6.3.2 Explain how ions form.
REF: p. 162 | p. 163 | p. 172
STA: SC3.b
76. ANS:
Atomic size increases with increasing atomic number within a group. For example, sodium atoms are larger
than lithium atoms, and potassium atoms are larger than sodium atoms. Atomic size decreases with increasing
atomic number across a period. For example, lithium atoms are larger than beryllium atoms, and beryllium
atoms are larger than boron atoms.
PTS: 1
DIF: L2
REF: p. 171
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA: SC4.a | SC4.b
77. ANS:
Ions form when electrons are transferred among atoms. For example, a group 1A element, such as potassium,
tends to transfer one electron to other atoms, causing it to form a net positive charge, in this case K . Such
ions with net positive charges are called cations. Ions with net negative charges are anions. Nonmetal atoms,
such as chlorine, tend to accept electrons from other atoms. Chlorine tends to gain a single electron, forming
the anion Cl .
PTS: 1
DIF: L2
REF: p. 172
OBJ: 6.3.2 Explain how ions form.
STA: SC3.b
78. ANS:
First ionization energies decrease from top to bottom within a group and increase across a period from left to
right. For example, the first ionization energy of rubidium is less than that of lithium. The first ionization
energy of iodine is much greater than that of lithium.
PTS: 1
DIF: L2
REF: p. 174
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
79. ANS:
When an electron is added to an atom, the attraction of the nucleus for any one electron decreases and the size
of the ion’s radius increases. When an electron is removed from an atom, there is an increase in the nuclear
attraction experienced by the remaining electrons. Consequently, the remaining electrons are drawn closer to
the nucleus.
PTS: 1
DIF: L3
REF: p. 176
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b
80. ANS:
Electronegativity values decrease from top to bottom within a group, and from right to left across a period.
For example, rubidium is less electronegative than lithium. Lithium is less electronegative than fluorine.
PTS: 1
DIF: L3
REF: p. 177
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: SC4.a | SC4.b | SC3.b