Download File

CH 5 Review
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.
2.
3.
4.
5.
6.
region of high probability of finding an electron
states the impossibility of knowing both velocity and position of a moving particle at the same time
lowest energy level
tendency of electrons to enter orbitals of lowest energy first
arrangement of electrons around atomic nucleus
each orbital has at most two electrons
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
____
____
____
____
____
____
____
____
7. 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.
8. How does the energy of an electron change when the electron moves closer to the nucleus?
a. It decreases.
c. It stays the same.
b. It increases.
d. It doubles.
9. The principal quantum number indicates what property of an electron?
a. position
c. energy level
b. speed
d. electron cloud shape
10. What is the shape of the 3p atomic orbital?
a. sphere
c. bar
b. dumbbell
d. two perpendicular dumbbells
11. How many energy sublevels are in the second principal energy level?
a. 1
c. 3
b. 2
d. 4
12. What is the maximum number of f orbitals in any single energy level in an atom?
a. 1
c. 5
b. 3
d. 7
13. What is the maximum number of d orbitals in a principal energy level?
a. 1
c. 3
b. 2
d. 5
14. What is the maximum number of orbitals in the p sublevel?
a. 2
c. 4
b. 3
d. 5
15. What is the maximum number of electrons in the second principal energy level?
a. 2
c. 18
____ 16.
____ 17.
____ 18.
____ 19.
____ 20.
____ 21.
____ 22.
____ 23.
____ 24.
____ 25.
____ 26.
____ 27.
____ 28.
b. 8
d. 32
When an electron moves from a lower to a higher energy level, the electron ____.
a. always doubles its energy
b. absorbs a continuously variable amount of energy
c. absorbs a quantum of energy
d. moves closer to the nucleus
The shape (not the size) of an electron cloud is determined by the electron's ____.
a. energy sublevel
c. speed
b. position
d. principal quantum number
If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
a. zero
c. counterclockwise
b. clockwise
d. both clockwise and counterclockwise
What types of atomic orbitals are in the third principal energy level?
a. s and p only
c. s, p, and d only
b. p and d only
d. s, p, d, and f
What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
c. 3f
b. 3d
d. 4s
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
What is the number of electrons in the outermost energy level of an oxygen atom?
a. 2
c. 6
b. 4
d. 8
What is the electron configuration of potassium?
a. 1s 2s 2p 3s 3p 4s
c. 1s 2s 3s 3p 3d
b. 1s 2s 2p 3s 3p
d. 1s 2s 2p 3s 3p 4s
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.
How many unpaired electrons are in a sulfur atom (atomic number 16)?
a. 0
c. 2
b. 1
d. 3
How many half-filled orbitals are in a bromine atom?
a. 1
c. 3
b. 2
d. 4
Stable electron configurations are likely to contain ____.
a. filled energy sublevels
b. fewer electrons than unstable configurations
c. unfilled s orbitals
d. electrons with a clockwise spin
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.
____ 29. Which electron configuration of the 4f energy sublevel is the most stable?
a. 4f
c. 4f
b. 4f
d. 4f
____ 30. Which of the following electron configurations of outer sublevels is the most stable?
a. 4d 5s
c. 4d 5s
b. 4d 5s
d. 4d 5s
____ 31. In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend
on ____.
a. a quantum mechanical model
c. the Schrodinger equation
b. direction with respect to the nucleus
d. the electron energy sublevel
Short Answer
32. Give the electron configuration for a neutral atom of beryllium.
33. Give the electron configuration for a neutral atom of selenium.
34. Write the electron configuration for chromium.
CH 5 Review
Answer Section
MATCHING
1. ANS:
OBJ:
2. ANS:
STO:
3. ANS:
STO:
4. ANS:
STO:
5. ANS:
STO:
6. ANS:
STO:
A
5.1.2
F
GOAL 4.01.b
D
GOAL 3.01.d
B
GOAL 3.01.d
C
GOAL 3.01.d
E
GOAL 3.01.d
DIF: L1
REF: p. 130, p. 131
STO: GOAL 3.01.d
DIF: L1
REF: p. 145
OBJ: 5.1.3
DIF: L1
REF: p. 142
OBJ: 5.1.3
DIF: L1
REF: p. 133
OBJ: 5.1.3, 5.2.1
DIF: L1
REF: p. 133
OBJ: 5.2.1
DIF: L1
REF: p. 134
OBJ: 5.2.1
REF: p. 128
OBJ: 5.1.2
REF: p. 128
OBJ: 5.1.3
REF: p. 131
OBJ: 5.1.3
REF: p. 131
OBJ: 5.1.3
REF: p. 131
OBJ: 5.1.3
MULTIPLE CHOICE
7. ANS:
STO:
8. ANS:
STO:
9. ANS:
STO:
10. ANS:
STO:
11. ANS:
STO:
12. ANS:
OBJ:
13. ANS:
OBJ:
14. ANS:
OBJ:
15. ANS:
STO:
16. ANS:
STO:
17. ANS:
STO:
18. ANS:
STO:
19. ANS:
STO:
20. ANS:
A
DIF: L2
GOAL 2.01.d
A
DIF: L2
GOAL 2.01.d, GOAL 3.01.d
C
DIF: L2
GOAL 3.01.d
B
DIF: L2
GOAL 3.01.d
B
DIF: L2
GOAL 3.01.d
D
DIF: L2
5.1.3
STO: GOAL 3.01.d
D
DIF: L2
5.1.3
STO: GOAL 3.01.d
B
DIF: L2
5.1.3
STO: GOAL 3.01.d
B
DIF: L3
GOAL 3.01.d
C
DIF: L3
GOAL 4.01.b
A
DIF: L2
GOAL 3.01.d
C
DIF: L1
GOAL 3.01.d
C
DIF: L2
GOAL 3.01.d
D
DIF: L2
REF: p. 131, p. 132
REF: p. 131, p. 132
REF: p. 131, p. 132
REF: p. 132
OBJ: 5.1.3
REF: p. 128
OBJ: 5.1.3
REF: p. 131
OBJ: 5.1.4
REF: p. 134
OBJ: 5.2.1
REF: p. 131
OBJ: 5.2.1
REF: p. 133
OBJ: 5.2.1
STO:
21. ANS:
STO:
22. ANS:
OBJ:
23. ANS:
OBJ:
24. ANS:
STO:
25. ANS:
OBJ:
26. ANS:
OBJ:
27. ANS:
STO:
28. ANS:
STO:
29. ANS:
STO:
30. ANS:
OBJ:
GOAL 3.01.d
D
GOAL 3.01.d
C
5.2.1
D
5.2.1
A
GOAL 3.01.d
C
5.2.1
A
5.2.1
A
GOAL 3.01.d
A
GOAL 3.01.d
D
GOAL 3.01.d
A
5.2.2
53. ANS:
STO:
54. ANS:
STO:
C
DIF: L2
GOAL 4.01.b
B
DIF: L3
GOAL 3.01.d
DIF: L2
REF: p. 133
OBJ: 5.2.1
DIF:
STO:
DIF:
STO:
DIF:
L2
REF: p. 134, p. 135
GOAL 3.01.d
L2
REF: p. 133, p. 134, p. 135
GOAL 3.01.d
L3
REF: p. 134
OBJ: 5.2.1
DIF:
STO:
DIF:
STO:
DIF:
L3
REF: p. 133, p. 134
GOAL 3.01.d
L3
REF: p. 133, p. 134
GOAL 3.01.d
L1
REF: p. 136
OBJ: 5.2.2
DIF: L2
REF: p. 136
OBJ: 5.2.2
DIF: L2
REF: p. 136
OBJ: 5.2.2
DIF: L3
REF: p. 133, p. 134, p. 135, p. 136
STO: GOAL 3.01.d
REF: p. 144
OBJ: 5.3.4
REF: p. 131
OBJ: 5.1.4, 5.3.4
SHORT ANSWER
55. ANS:
1s 2s
DIF: L1
REF: p. 133, p. 134
STO: GOAL 3.01.d
56. ANS:
1s 2s 2p 3s 3p 3d 4s 4p
OBJ: 5.2.1
DIF: L2
REF: p. 133, p. 134
STO: GOAL 3.01.d
57. ANS:
1s 2s 2p 3s 3p 3d 4s
OBJ: 5.2.1
DIF: L3
REF: p. 134, p. 135, p. 136
STO: GOAL 3.01.d
OBJ: 5.2.2