Download Chapter 5 Test: Electrons in Atoms

Chapter 5 Test: Electrons in Atoms
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
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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 (s first, then p, then d…)
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
b. frequency
c. wavelength
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7. number of wave cycles passing a point per unit of time
8. distance between wave crests
9. frequencies of light emitted by an element
10. In Bohr's model of the atom, where are the electrons and protons located?
a. The electrons move around the
c. The electrons and protons move
protons, which are at the center of the
throughout the atom.
atom.
b. The electrons occupy fixed positions
around the protons, which are at the
center of the atom.
11. What is the shape of the 3p atomic orbital?
a. two perpendicular dumbbells
c. dumbbell
b. sphere
12. What is the maximum number of f orbitals in any single energy level in an atom?
a. 1
c. 7
b. 3
13. What is the maximum number of d orbitals in a principal energy level?
a. 2
c. 1
b. 5
14. What is the maximum number of orbitals in the p sublevel?
a. 2
c. 5
b. 3
15. When an electron moves from a lower to a higher energy level, the electron ____.
a. releases energy
c. always doubles its energy
b. absorbs a quantum of energy
16. The letter "p" in the symbol 4p indicates the ____.
a. spin of an electron
b. speed of an electron
c. orbital shape
17. If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that
orbital?
a. clockwise
c. counterclockwise
b. both clockwise and counterclockwise
18. What is the number of electrons in the outermost energy level of an oxygen atom?
a. 6
b. 2
c. 4
19. What is the electron configuration of potassium?
a. 1s 2s 3s 3p 3d
c. 1s 2s 2p 3s 3p 4s
b. 1s 2s 2p 3s 3p 4s
20. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be
distributed in the three orbitals?
a. two electrons in one orbital, one in
c. three in one orbital, none in the other
another, none in the third
two
b. one electron in each orbital
21. How many unpaired electrons are in a sulfur atom (atomic number 16)?
a. 3
c. 2
b. 1
22. How many half-filled orbitals are in a bromine atom?
a. 3
c. 2
b. 1
23. Which color of visible light has the shortest wavelength?
a. green
c. violet
b. yellow
24. Which of the following electromagnetic waves have the highest frequencies?
a. ultraviolet light waves
c. gamma rays
b. microwaves
25. How are the frequency and wavelength of light related?
a. They are inversely proportional to each other. c. Wavelength is determined by dividing
frequency by the speed of light.
b. They are directly proportional to each other.
26. Emission of light from an atom occurs when an electron ____.
a. falls into the nucleus
c. drops from a higher to a lower energy level
b. jumps from a lower to a higher energy
level
27. Which variable is directly proportional to frequency?
a. velocity
c. position
b. energy
28. What are quanta of light called?
a. photons
c. excitons
b. charms
29. Which scientist developed the most current model of the atom?
a. Albert Einstein
c. Erwin Schrodinger
b. Niels Bohr
30. The most current model of the atom ____.
a. defines the exact path of an electron
c. involves the probability of finding an
around the nucleus
electron in a certain position
b. was proposed by Niels Bohr
Name:
Date:
Period:
Chapter 5 Test: Electrons in Atoms – 90 pts
Multiple Choice (2 pts each = 60 pts)
1
6
11
16
21
26
2
7
12
17
22
27
3
8
13
18
23
28
4
9
14
19
24
29
5
10
15
20
25
30
Short Answer (#’s 31-33: 2 pts each; #34: 3 pts)
31. Give the electron configuration for beryllium.
32. Give the electron configuration for chlorine.
33. Give the electron configuration for selenium.
34. Identify the elements with the following electron configurations:
a. 1s22s22p63s1
b. 1s22s22p63s23p64s23d8
c. 1s22s22p63s23p64s23d104p65s24d105p5
35. Draw the 5th (and current) model of the atom (4 pts)
36. Explain how Heisenberg’s Uncertainty Principle helped Schrodinger create this model of the
atom. (4 pts)
37. Draw a low frequency wave and label the amplitude and wavelength. (4 pts)
38. Explain how the flame test lab worked. Why did the fire change color? (4 pts)
39. When looking at an orbital diagram, what would it most likely mean if you had 3 “up” arrows
in the 3p shell and no “down” arrows? (3 pts)
40. What is the maximum number of electrons that each shell can hold? (2 pts)
a. s:
p:
d:
f:
Chapter 5 Test: Electrons in Atoms
Answer Section
MATCHING
1.
2.
3.
4.
5.
6.
7.
8.
9.
ANS:
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A
F
D
B
C
E
B
C
A
PTS:
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PTS:
PTS:
1
1
1
1
1
1
1
1
1
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L1
L1
L1
L1
L1
L1
REF:
REF:
REF:
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REF:
REF:
p. 130 | p. 131
p. 145
p. 142
p. 133
p. 133
p. 134
p. 138
p. 138
p. 141
PTS:
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1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
DIF:
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DIF:
L2
L2
L2
L2
L2
L3
L2
L1
L2
L2
L3
L3
L3
L2
L2
L2
L2
L3
L1
L1
L2
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p. 128
p. 131
p. 131 | p. 132
p. 131 | p. 132
p. 131 | p. 132
p. 128
p. 131
p. 134
p. 134 | p. 135
p. 133 | p. 134 | p. 135
p. 134
p. 133 | p. 134
p. 133 | p. 134
p. 139
p. 139
p. 139
p. 141
p. 142
p. 144
p. 130
p. 145
MULTIPLE CHOICE
10.
11.
12.
13.
14.
15.
16.
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18.
19.
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21.
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25.
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30.
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A
C
C
B
B
B
C
C
A
C
B
C
B
C
C
A
C
B
A
C
C
SHORT ANSWER
31. ANS: 1s 2s
32. ANS: 1s 2s 2p 3s 3p
33. ANS: 1s 2s 2p 3s 3p 3d 4s 4p
34. ANS: 1s 2s 2p 3s 3p 3d 4s