Download EOC quiz II pdf

Name: ______________________
Class: _________________
Date: _________
ID: A
EOC review II
Matching
Match each item with the correct statement below.
a. atomic orbital
d. ground state
b. aufbau principle
e. Pauli exclusion principle
c. electron configuration
f. Heisenberg uncertainty principle
____
1. region of high probability of finding an electron
____
2. states the impossibility of knowing both velocity and position of a moving particle at the same time
____
3. lowest energy level
____
4. tendency of electrons to enter orbitals of lowest energy first
____
5. arrangement of electrons around atomic nucleus
____
6. each orbital has at most two electrons
Match each item with the correct statement below.
a. atomic emission spectrum
d. photon
b. frequency
e. quantum
c. wavelength
f. spectrum
____
7. discrete bundle of electromagnetic energy
____
8. energy needed to move an electron from one energy level to another
____
9. number of wave cycles passing a point per unit of time
____ 10. distance between wave crests
____ 11. separation of light into different wavelengths
____ 12. frequencies of light emitted by an element
Match each item with the correct statement below.
a. electronegativity
f. periodic law
b. ionization energy
g. atomic mass
c. atomic radius
h. period
d. metal
i. group
e. transition metal
j. electrons
____ 13. horizontal row in the periodic table
____ 14. vertical column in the periodic table
____ 15. A repetition of properties occurs when elements are arranged in order of increasing atomic number.
____ 16. type of element that is a good conductor of heat and electric current
____ 17. type of element characterized by the presence of electrons in the d orbital
1
Name: ______________________
ID: A
____ 18. one-half the distance between the nuclei of two atoms when the atoms are joined
____ 19. basis for Mendeleev’s arrangement of the periodic table
____ 20. subatomic particles that are transferred to form positive and negative ions
____ 21. ability of an atom to attract electrons when the atom is in a compound
____ 22. energy required to remove an electron from an atom
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 23. In Bohr's model of the atom, where are the electrons and protons located?
a. The electrons move around the protons, which are at the center of the atom.
b. The electrons and protons move throughout the atom.
c. The electrons occupy fixed positions around the protons, which are at the center of
the atom.
d. The electrons and protons are located throughout the atom, but they are not free to
move.
____ 24. How does the energy of an electron change when the electron moves closer to the nucleus?
a. It decreases.
b. It increases.
c. It stays the same.
d. It doubles.
____ 25. The
a.
b.
c.
d.
principal quantum number indicates what property of an electron?
position
speed
energy level
electron cloud shape
____ 26. What is the shape of the 3p atomic orbital?
a. sphere
b. dumbbell
c. bar
d. two perpendicular dumbbells
____ 27. How many energy sublevels are in the second principal energy level?
a. 1
b. 2
c. 3
d. 4
____ 28. What is the maximum number of f orbitals in any single energy level in an atom?
a. 1
b. 3
c. 5
d. 7
2
Name: ______________________
ID: A
____ 29. What is the maximum number of d orbitals in a principal energy level?
a. 1
b. 2
c. 3
d. 5
____ 30. What is the maximum number of orbitals in the p sublevel?
a. 2
b. 3
c. 4
d. 5
____ 31. What is the maximum number of electrons in the second principal energy level?
a. 2
b. 8
c. 18
d. 32
____ 32. What types of atomic orbitals are in the third principal energy level?
a. s and p only
b. p and d only
c. s, p, and d only
d. s, p, d, and f
____ 33. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
b. 3d
c. 3f
d. 4s
____ 34. According to the aufbau principle,
a. an orbital may be occupied by only two electrons.
b. electrons in the same orbital must have opposite spins.
c. electrons enter orbitals of highest energy first.
d. electrons enter orbitals of lowest energy first.
____ 35. What is the number of electrons in the outermost energy level of an oxygen atom?
a. 2
b. 4
c. 6
d. 8
____ 36. What is the electron configuration of potassium?
2
2
2
2
2
1
a. 1s 2s 2p 3s 3p 4s
2
2
10
2
3
b. 1s 2s 2p 3s 3p
2
2
2
6
1
c. 1s 2s 3s 3p 3d
2
2
6
2
6
1
d. 1s 2s 2p 3s 3p 4s
3
Name: ______________________
ID: A
____ 37. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed
in the three orbitals?
a. one electron in each orbital
b. two electrons in one orbital, one in another, none in the third
c. three in one orbital, none in the other two
d. Three electrons cannot fill three empty 2p atomic orbitals.
____ 38. What is the basis for exceptions to the aufbau diagram?
a. Filled and half-filled energy sublevels are more stable than partially-filled energy
sublevels.
b. Electron configurations are only probable.
c. Electron spins are more important than energy levels in determining electron
configuration.
d. Some elements have unusual atomic orbitals.
____ 39. Which electron configuration of the 4f energy sublevel is the most stable?
7
a. 4f
b. 4f
13
c. 4f
14
d. 4f
____ 40. How are the frequency and wavelength of light related?
a. They are inversely proportional to each other.
b. Frequency equals wavelength divided by the speed of light.
c. Wavelength is determined by dividing frequency by the speed of light.
d. They are directly proportional to each other.
____ 41. The
a.
b.
c.
d.
light given off by an electric discharge through sodium vapor is ____.
a continuous spectrum
an emission spectrum
of a single wavelength
white light
____ 42. Emission of light from an atom occurs when an electron
a. drops from a higher to a lower energy level.
b. jumps from a lower to a higher energy level.
c. moves within its atomic orbital.
d. falls into the nucleus.
____ 43. The
a.
b.
c.
d.
atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be
the same.
different from each other.
the same as those of several other elements.
the same as each other only in the ultraviolet range.
____ 44. What are quanta of light called?
a. charms
b. excitons
c. muons
d. photons
4
Name: ______________________
ID: A
____ 45. According to the Heisenberg uncertainty principle, if the position of a tiny moving particle is known,
the
a. mass of the particle cannot be exactly determined.
b. charge of the particle cannot be exactly determined.
c. spin of the particle cannot be exactly determined.
d. velocity of the particle cannot be exactly determined.
____ 46. Which of the following elements is in the same period as phosphorus?
a. carbon
b. magnesium
c. nitrogen
d. oxygen
____ 47. Each period in the periodic table corresponds to a(n) ____.
a. principal energy level
b. energy sublevel
c. orbital
d. suborbital
____ 48. Which of the following categories includes the majority of the elements?
a. metalloids
b. liquids
c. metals
d. nonmetals
____ 49. Of
a.
b.
c.
d.
the elements Pt, V, Li, and Kr, which is a nonmetal?
Pt
V
Li
Kr
____ 50. To
a.
b.
c.
d.
what category of elements does an element belong if it is a poor conductor of electricity? ____
transition elements
metalloids
nonmetals
metals
2
2
6
2
2
____ 51. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
b. selenium
c. silicon
d. silver
____ 52. 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.
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Name: ______________________
ID: A
____ 53. How does atomic radius change from top to bottom in a group in the periodic table?
a. It tends to decrease.
b. It tends to increase.
c. It first increases, then decreases.
d. It first decreases, then increases.
____ 54. How does atomic radius change from left to right across a period in the periodic table?
a. It tends to decrease.
b. It tends to increase.
c. It first increases, then decreases.
d. It first decreases, then increases.
____ 55. 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.
____ 56. What element in the second period has the largest atomic radius?
a. carbon
b. lithium
c. potassium
d. neon
____ 57. 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 in 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
____ 58. The
a.
b.
c.
d.
metals in Groups 1A, 2A, and 3A
gain electrons when they form ions.
all form ions with a negative charge.
+
all have ions with a 1 charge.
lose electrons when they form ions.
____ 59. What is the element with the lowest electronegativity value?
a. cesium
b. helium
c. calcium
d. fluorine
____ 60. What is the element with the highest electronegativity value?
a. cesium
b. helium
c. calcium
d. fluorine
6
Name: ______________________
ID: A
____ 61. Which of the following elements has the smallest ionic radius?
a. Li
b. K
c. O
d. S
____ 62. Which of the following decreases with increasing atomic number in Group 2A?
a. shielding effect
b. ionic size
c. ionization energy
d. number of electrons
____ 63. 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.
____ 64. 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
____ 65. As
a.
b.
c.
d.
you move from left to right across the second period of the periodic table
ionization energy increases.
atomic radii increase.
electronegativity decreases.
atomic mass decreases.
Short Answer
66. Give the electron configuration for a neutral atom of beryllium.
67. Give the electron configuration for a neutral atom of chlorine.
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ID: A
EOC review II
Answer Section
MATCHING
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A
PTS: 1
DIF: L1
REF: p. 131
5.1.3 Explain how sublevels of principal energy levels differ.
knowledge
F
PTS: 1
DIF: L1
REF: p. 148
5.3.4 Distinguish between quantum mechanics and classical mechanics.
knowledge
D
PTS: 1
DIF: L1
REF: p. 145
5.3.3 Explain how the frequencies of light are related to changes in electron energies.
knowledge
B
PTS: 1
DIF: L1
REF: p. 134
5.2.1 List the three rules for writing the electron configurations of elements.
knowledge
C
PTS: 1
DIF: L1
REF: p. 134
5.2.1 List the three rules for writing the electron configurations of elements.
knowledge
E
PTS: 1
DIF: L1
REF: p. 134
5.2.1 List the three rules for writing the electron configurations of elements.
knowledge
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12. ANS:
OBJ:
D
PTS: 1
DIF: L1
REF: p. 143
5.3.2 Describe how Einstein explained the photoelectric effect.
knowledge
E
PTS: 1
DIF: L1
REF: p. 129
5.1.1 Describe what Bohr proposed in his model of the atom.
knowledge
B
PTS: 1
DIF: L1
REF: p. 138
5.3.1 Explain what causes atomic emission spectra.
BLM: knowledge
C
PTS: 1
DIF: L1
REF: p. 138
5.3.1 Explain what causes atomic emission spectra.
BLM: knowledge
F
PTS: 1
DIF: L2
REF: p. 139
5.3.1 Explain what causes atomic emission spectra.
BLM: comprehension
A
PTS: 1
DIF: L2
REF: p. 140
5.3.1 Explain what causes atomic emission spectra.
BLM: comprehension
13. ANS:
OBJ:
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14. ANS:
OBJ:
BLM:
H
PTS: 1
DIF: L1
REF: p. 162
6.1.3 Describe how the modern periodic table is organized.
knowledge
I
PTS: 1
DIF: L1
REF: p. 162
6.1.3 Describe how the modern periodic table is organized.
knowledge
1
ID: A
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PTS: 1
DIF: L1
REF:
6.1.3 Describe how the modern periodic table is organized.
knowledge
D
PTS: 1
DIF: L1
REF:
6.1.4 Identify three broad classes of elements.
BLM:
E
PTS: 1
DIF: L1
REF:
6.2.2 Classify elements based on electron configuration.
knowledge
C
PTS: 1
DIF: L1
REF:
6.3.1 Describe trends among elements for atomic size. BLM:
G
PTS: 1
DIF: L1
REF:
6.1.2 Describe how Mendeleev organized his periodic table.
knowledge
J
PTS: 1
DIF: L1
REF:
6.3.2 Explain how ions form.
BLM: knowledge
A
PTS: 1
DIF: L1
REF:
6.3.3 Describe periodic trends for first ionization energy, ionic
knowledge
B
PTS: 1
DIF: L1
REF:
6.3.3 Describe periodic trends for first ionization energy, ionic
knowledge
p. 162
p. 165
knowledge
p. 172
p. 174
knowledge
p. 161
p. 176
p. 181
size, and electronegativity.
p. 177
size, and electronegativity.
MULTIPLE CHOICE
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29. ANS:
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A
PTS: 1
DIF: L2
REF: p. 129
5.1.1 Describe what Bohr proposed in his model of the atom.
comprehension
A
PTS: 1
DIF: L2
REF: p. 129
5.1.2 Describe what the quantum mechanical model determines about the electrons in an atom.
application
C
PTS: 1
DIF: L2
REF: p. 131
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
B
PTS: 1
DIF: L2
REF: p. 131
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
B
PTS: 1
DIF: L2
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
D
PTS: 1
DIF: L2
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
D
PTS: 1
DIF: L2
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
2
ID: A
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B
PTS: 1
DIF: L2
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
B
PTS: 1
DIF: L1
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
knowledge
C
PTS: 1
DIF: L2
REF: p. 132
5.1.3 Explain how sublevels of principal energy levels differ.
comprehension
D
PTS: 1
DIF: L2
REF: p. 134
5.2.1 List the three rules for writing the electron configurations of elements.
application
D
PTS: 1
DIF: L2
REF: p. 134
5.2.1 List the three rules for writing the electron configurations of elements.
comprehension
C
PTS: 1
DIF: L2
REF: p. 135 | p. 136
5.2.1 List the three rules for writing the electron configurations of elements.
application
D
PTS: 1
DIF: L2
REF: p. 135 | p. 136
5.2.1 List the three rules for writing the electron configurations of elements.
application
A
PTS: 1
DIF: L2
REF: p. 134 | p. 135
5.2.1 List the three rules for writing the electron configurations of elements.
comprehension
A
PTS: 1
DIF: L2
REF: p. 137
5.2.1 List the three rules for writing the electron configurations of elements.
comprehension
D
PTS: 1
DIF: L2
REF: p. 136 | p. 137
5.2.1 List the three rules for writing the electron configurations of elements.
application
A
PTS: 1
DIF: L1
REF: p. 138 | p. 139
5.3.1 Explain what causes atomic emission spectra.
BLM: knowledge
B
PTS: 1
DIF: L2
REF: p. 140
5.3.1 Explain what causes atomic emission spectra.
BLM: comprehension
A
PTS: 1
DIF: L2
REF: p. 140
5.3.1 Explain what causes atomic emission spectra.
BLM: comprehension
A
PTS: 1
DIF: L2
REF: p. 140
5.3.1 Explain what causes atomic emission spectra.
BLM: comprehension
D
PTS: 1
DIF: L1
REF: p. 143
5.3.2 Describe how Einstein explained the photoelectric effect.
knowledge
D
PTS: 1
DIF: L2
REF: p. 148
5.3.4 Distinguish between quantum mechanics and classical mechanics.
comprehension
B
PTS: 1
DIF: L2
REF: p. 162
6.1.3 Describe how the modern periodic table is organized.
comprehension
3
ID: A
47. ANS: A
PTS: 1
DIF: L1
REF: p. 172
OBJ: 6.2.2 Classify elements based on electron configuration.
BLM: knowledge
48. ANS: C
PTS: 1
DIF: L1
REF: p. 164
OBJ: 6.1.4 Identify three broad classes of elements.
BLM: knowledge
49. ANS: D
PTS: 1
DIF: L2
REF: p. 165
OBJ: 6.1.4 Identify three broad classes of elements.
BLM: application
50. ANS: C
PTS: 1
DIF: L2
REF: p. 165
OBJ: 6.1.4 Identify three broad classes of elements.
BLM: comprehension
51. ANS: C
PTS: 1
DIF: L2
REF: p. 171
OBJ: 6.2.2 Classify elements based on electron configuration.
BLM: application
52. ANS: B
PTS: 1
DIF: L2
REF: p. 172
OBJ: 6.2.2 Classify elements based on electron configuration.
BLM: comprehension
53. ANS: B
PTS: 1
DIF: L1
REF: p. 174
OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: knowledge
54. ANS: A
PTS: 1
DIF: L1
REF: p. 174
OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: knowledge
55. ANS: A
PTS: 1
DIF: L2
REF: p. 175
OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: comprehension
56. ANS: B
PTS: 1
DIF: L2
REF: p. 174 | p. 175
OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: comprehension
57. ANS: A
PTS: 1
DIF: L2
REF: p. 174 | p. 175
OBJ: 6.3.1 Describe trends among elements for atomic size. BLM: analysis
58. ANS: D
PTS: 1
DIF: L2
REF: p. 176
OBJ: 6.3.2 Explain how ions form.
BLM: comprehension
59. ANS: A
PTS: 1
DIF: L2
REF: p. 181
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
BLM: comprehension
60. ANS: D
PTS: 1
DIF: L2
REF: p. 181
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
BLM: comprehension
61. ANS: A
PTS: 1
DIF: L2
REF: p. 179
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
BLM: application
62. ANS: C
PTS: 1
DIF: L2
REF: p. 175 | p. 182
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.
BLM: comprehension
63. ANS: A
PTS: 1
DIF: L2
REF: p. 161
OBJ: 6.1.2 Describe how Mendeleev organized his periodic table.
BLM: comprehension
64. ANS: C
PTS: 1
DIF: L2
REF: p. 178
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
BLM: comprehension
4
ID: A
65. ANS: A
PTS: 1
DIF: L2
REF: p. 175 | p. 182
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.
BLM: comprehension
SHORT ANSWER
66. ANS:
2
2
1s 2s
PTS: 1
DIF: L2
REF: p. 136
OBJ: 5.2.1 List the three rules for writing the electron configurations of elements.
BLM: application
67. ANS:
2
2
6
2
5
1s 2s 2p 3s 3p
PTS: 1
DIF: L2
REF: p. 136
OBJ: 5.2.1 List the three rules for writing the electron configurations of elements.
BLM: application
5