Ch4 Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
____
1. An industrially important element contains 26 electrons and rusts in the presence of air and moisture.
Identify the element.
a. Aluminum
c. Potassium
b. Iron
d. Sodium
2. In the nuclear equation given below, calculate the mass number of the alpha particle.
____
3.
____
4.
____
5.
____
6.
a. 0
c. 234
b. 4
d. 238
The mass of an electron is _____.
a. smaller than the mass of a proton.
c. a tiny fraction of the mass of an atom.
b. smaller than the mass of a neutron.
d. all of the above.
One atomic mass unit is _____.
a. 1/12 the mass of a carbon-12 atom.
b. 1/16 the mass of an oxygen-16 atom.
c. exactly the mass of one proton.
d. approximately the mass of one proton plus one neutron.
The atomic mass of an atom is usually not a whole number because it accounts for _____..
a. only the relative abundance of the atom’s isotopes.
b. only the mass of each of the atom’s isotopes.
c. the mass of the atom’s electrons.
d. both the relative abundance and the mass of each of the atom’s isotopes.
What is the mass constant of a proton?
a. 0.000549 amu
c. 1.00865 amu
b. 1.007276 amu
d. 6.01500 amu
Completion
Complete each statement.
7. Researchers discovered a subatomic particle while working with the cathode ray tube. The particle is
known as a(n) ____________________.
8. A ____________________ is a subatomic particle that has mass nearly equal to that of a proton, but it
carries no electrical charge.
9. Atoms with the same number of protons but different number of neutrons are called
____________________.
10. Uranium is a naturally occurring element that emits particles and rays spontaneously through a process
called _____________________.
11. An alpha particle is _____________________ charged with two protons and neutrons.
12. A beta particle consists of a fast moving electron and has a(n) _____________________ charge.
13. James Chadwick showed that the nucleus also contained a neutral subatomic particle known as the
____________________.
14. The number of protons in an atom is called the ____________________ of the element.
Use the periodic table to identify each element described below.
15. atomic number 65 is ____________________.
16. 78 protons ____________________.
17. 44 protons and 44 electrons is ____________________.
18. 21 protons is ____________________.
Matching
Match the terms below with their correct definitions.
a. Thomson
c. Rutherford
b. Millikan
____ 19. Proposed the nuclear atomic model
____ 20. Determined the mass-to-charge ratio of an electron
____ 21. Calculated the mass of an electron
Match the terms below with the correct definitions.
a. nuclear reaction
c. radiation
b. beta radiation
d. radioactive decay
____
____
____
____
22.
23.
24.
25.
The rays and particles that are emitted by a radioactive material
A reaction that involves a change in an atom’s nucleus
The process in which an unstable nucleus loses energy spontaneously
Fast-moving electrons
Match the terms below with their correct definitions.
a. atom
h. atomic mass unit
b. nucleus
i. radiation
c. atomic mass
j. Dalton’s atomic theory
d. isotopes
k. cathode ray
e. gamma ray
l. radioactivity
f. alpha radiation
m. radioactive decay
g. beta radiation
____
____
____
____
____
____
____
26.
27.
28.
29.
30.
31.
32.
Atoms with the same number of protons but different numbers of neutrons
High-energy radiation that has no charge and no mass
The smallest particle of an element that retains the properties of that element
The weighted average mass of an element’s isotopes
The center-most part of an atom where the protons and neutrons are contained
Equal to 1/12 the mass of a carbon-12 atom
Process whereby some substances spontaneously emit radiation
Match the terms below with their correct definitions.
____
____
____
____
____
____
____
____
33.
34.
35.
36.
37.
38.
39.
40.
a.
e.
b.
f.
c.
g.
d.
h.
Isotope in which the number of neutrons is six more than the isotope’s atomic number
Copper-63
Copper with seven neutrons more than its atomic number
Isotope that has one neutron more than its number of protons
Carbon with equal numbers of neutrons, protons, and electrons
Carbon with two more neutrons than its number of protons
Chromium with two more neutrons than its number of protons
Isotope in which the difference between the neutrons and number of protons is 4
Ch5 Test
True/False
Indicate whether the statement is true or false.
____
1. Each element has a unique atomic emission spectrum.
____
2. A flame test can be used to identify the presence of certain elements in a compound.
____
3. The neon atoms in a neon sign emit their characteristic color of light as they absorb energy.
____
4. When an atom emits light, photons having certain specific energies are being emitted.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
____
____
____
____
5. A(n) ____ is the minimum amount of energy that can be lost or gained by an atom.
a. valence electron
c. quantum
b. electron
d. Planck’s constant
6. According to Planck’s theory, for a given frequency, n, matter can emit or absorb energy only in
a. units of hertz.
c. entire wavelengths.
b. whole-number multiples of hn.
d.
multiples of
and so on.
7. The ______ is the phenomenon in which electrons are emitted from a metal’s surface when light of a
certain frequency shines on it.
a. quantum
c. photon effect
b. Planck concept
d. photoelectric effect
8. Which equation would you use to calculate the energy of a photon?
a. Ephoton = hv  Planck’s constant
c.
Ephoton = hv
b. Ephoton = hv
d. c =
9. The electrons in an atom’s outermost orbitals are called _____.
a. electron dots.
c. valence electrons.
b. quantum electrons.
d. noble-gas electrons.
____ 10. In an electron-dot structure, the element’s symbol represents the _____.
a. nucleus of the noble gas closest to the atom in the periodic table.
b. atom’s nucleus and inner-level electrons.
c. atom’s valence electrons.
d. electrons of the noble gas closest to the atom in the periodic table.
____ 11. How many valence electrons does a chlorine atom have if its electron configuration
is [Ne]3s23p5?
a. 3
c. 5
b. 21
d. 7
____ 12. Which electrons are represented by the dots in an electron-dot structure?
a. valence electrons
c. only s electrons
b. inner-level electrons
d. both a and c
Use the following figure to answer the questions below.
____ 13. According to Bohr’s atomic model, which letter(s) in the figure represents a place where an electron
cannot be?
a. A
c. A and D
b. B, C and E
d. D
____ 14. According to the quantum mechanical model of the atom, point E in the figure represents a
a. point where an electron cannot be.
c. position where an electron must be.
b. position where an electron probably is.
d. point beyond which no electron can go
____ 15. Which of the following can you conclude based on the de Broglie equation?
a. Waves behave like particles.
b. Most particles are electrons.
c. All matter has an associated wavelength.
d. All matter behaves like particles.
____ 16. Which of the following best describes the Heisenberg uncertainty principle?
a. Light behaves like a particle and like a wave.
b. The shorter the wavelength, the higher the frequency.
c. It is impossible to know both the velocity and the position of a particle at the same time.
d. You can measure an object without disturbing it.
____ 17. What is the frequency range for X rays?
a. 106 Hz
c. 1014 Hz
b. 108 Hz
d. 1018 Hz
____ 18. How many valence electrons are present in silicon?
a. One
c. Four
b. Two
d. Six
Completion
Complete each statement.
Use each of the terms below just once to complete the passage.
amplitude
energy
frequency
hertz
light
wave
wavelength
speed
Electromagnetic radiation is a kind of (1) ____________________ that behaves like a(n) (2)
____________________as it travels through space. (3)____________________is one type of
electromagnetic radiation. Other examples include X rays, radio waves, and microwaves.
All waves can be characterized by their wavelength, amplitude, frequency, and
(4)____________________. The shortest distance between equivalent points on a continuous wave is
called a(n) (5) ____________________. The height of a wave from the origin to a crest or from the origin
to a trough is the (6) ____________________. (7) ____________________ is the number of waves that
pass a given point in one second. The SI unit for frequency is the (8) ____________________, which is
equivalent to one wave per second.
19. The word used to fill in blank #1 is ____________________.
20. The word used to fill in blank #2 is ____________________.
21. The word used to fill in blank #3 is ____________________.
22. The word used to fill in blank #4 is ____________________.
23. The word used to fill in blank #5 is ____________________.
24. The word used to fill in blank #6 is ____________________.
25. The word used to fill in blank #7 is ____________________.
26. The word used to fill in blank #8 is ____________________.
Choose the term in parentheses that correctly completes the statement.
27. Atomic orbitals (do, do not) have an exactly defined size. ____________________
28. Each orbital may contain at most (two, four) electrons. ____________________
29. All s orbitals are (spherically shaped, dumbbell shaped). ____________________
30. A principal energy has (n, n2) energy sublevels. ____________________
31. The maximum number of (electrons, orbitals) related to each principal energy level equals 2n2.
____________________
32. There are (three, five) equal energy p orbitals. ____________________
33. Hydrogen’s principal energy level 2 consists of (2s and 3s, 2s and 2p) orbitals. ____________________
34. Hydrogen’s principal energy level 3 consists of (nine, three) orbitals. ____________________
Matching
Match the terms below with the correct definitions.
a. Heisenberg uncertainty principle
c. quantum mechanical model of the atom
b. Schrödinger wave equation
d. atomic orbital
____
____
____
____
35.
36.
37.
38.
The modern model of the atom that treats electrons as waves
States that it is impossible to know both the velocity and the position of a particle at the same time
A three-dimensional region around the nucleus representing the probability of finding an electron
Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom
Ch4 Test
Answer Section
MULTIPLE CHOICE
1. ANS: B
Atomic number = number of protons = number of electrons.
Feedback
A
B
C
D
The number of electrons in aluminum is 13.
Correct!
The number of electrons in potassium is 19.
The number of electrons in sodium is 11.
PTS: 1
DIF: 1
REF: Page 98
OBJ: 4.3.1 Explain the role of atomic number in determining the identity of an atom.
NAT: B.1
TOP: Explain the role of atomic number in determining the identity of an atom.
KEY: Atomic number
MSC: 2
2. ANS: B
An alpha particle is equivalent to a helium-4 nucleus.
Feedback
A
B
C
D
3.
4.
5.
6.
Gamma rays are high-energy radiations that possess no mass.
Correct!
The mass number of thorium is 234.
The mass number of uranium is 238.
PTS: 1
DIF: 1
REF: Page 106 | Page 107
OBJ: 4.4.2 Characterize alpha, beta, and gamma radiation in terms of mass and charge.
NAT: B.1 | B.6
TOP: Characterize alpha, beta, and gamma radiation in terms of mass and charge.
KEY: Alpha particle
MSC: 2
ANS: D
PTS: 1
ANS: A
PTS: 1
ANS: D
PTS: 1
ANS: B
The atomic mass of a proton as compared to that of a C-12 atom is calculated as 1.007276 amu.
Feedback
A
B
C
D
The mass of an electron is 0.000549 amu.
Correct!
The mass of a neutron is 1.00865 amu.
The mass of a helium-6 atom is 6.10500 amu.
PTS: 1
DIF: 1
REF: Page 102
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number
and atomic number. NAT: B.1
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
KEY: Atomic mass of a proton
MSC: 1
COMPLETION
7. ANS: electron
PTS:
OBJ:
NAT:
TOP:
KEY:
8. ANS:
1
DIF: 1
REF: Page 92 | Page 93
4.2.1 Distinguish between the subatomic particles in terms of relative charge and mass.
B.1 | G.3
Distinguish between the subatomic particles in terms of relative charge and mass.
Electron
MSC: 1
neutron
PTS:
OBJ:
NAT:
TOP:
KEY:
9. ANS:
1
DIF: 1
REF: Page 96
4.2.2 Describe the structure of the nuclear atom, including the locations of the subatomic particles.
B.1 | G.3
Describe the structure of the nuclear atom, including the locations of the subatomic particles.
Neutron
MSC: 1
isotopes
PTS:
OBJ:
NAT:
KEY:
10. ANS:
1
DIF: 1
REF: Page 100
4.3.2 Define an isotope and explain why atomic masses are not whole numbers.
B.1
TOP: Define an isotope and explain why atomic masses are not whole numbers.
Isotopes
MSC: 1
radioactivity
PTS:
OBJ:
NAT:
KEY:
11. ANS:
1
DIF: 1
REF: Page 105
4.4.1 Explain the relationship between unstable nuclei and radioactive decay.
B.1 | B.6
TOP: Explain the relationship between unstable nuclei and radioactive decay.
Radioactivity
MSC: 1
positively
PTS:
OBJ:
NAT:
KEY:
12. ANS:
1
DIF: 1
REF: Page 106
4.4.2 Characterize alpha, beta, and gamma radiation in terms of mass and charge.
B.1 | B.6
TOP: Characterize alpha, beta, and gamma radiation in terms of mass and charge.
Alpha radiations
MSC: 1
negative
PTS:
OBJ:
NAT:
KEY:
13. ANS:
1
DIF: 1
REF: Page 107
4.4.2 Characterize alpha, beta, and gamma radiation in terms of mass and charge.
B.1 | B.6
TOP: Characterize alpha, beta, and gamma radiation in terms of mass and charge.
Beta particle MSC: 1
neutron
PTS:
OBJ:
NAT:
TOP:
KEY:
14. ANS:
1
DIF: 1
REF: Page 95
4.2.2 Describe the structure of the nuclear atom, including the locations of the subatomic particles.
B.1 | G.3
Describe the structure of the nuclear atom, including the locations of the subatomic particles.
Neutron
MSC: 1
atomic number
PTS:
OBJ:
NAT:
KEY:
15. ANS:
1
DIF: 1
REF: Page 98
4.3.1 Explain the role of atomic number in determining the identity of an atom.
B.1
TOP: Explain the role of atomic number in determining the identity of an atom.
Atomic number
MSC: 1
terbium
PTS: 1
16. ANS: platinum
PTS: 1
17. ANS: ruthenium
PTS: 1
18. ANS: scandium
PTS: 1
MATCHING
19. ANS: C
20. ANS: A
21. ANS: B
PTS: 1
PTS: 1
PTS: 1
22.
23.
24.
25.
ANS:
ANS:
ANS:
ANS:
C
A
D
B
PTS:
PTS:
PTS:
PTS:
1
1
1
1
26.
27.
28.
29.
30.
31.
32.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
D
E
A
C
B
H
L
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
33.
34.
35.
36.
37.
38.
39.
40.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
H
B
F
A
C
E
D
G
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
Ch5 Test
Answer Section
TRUE/FALSE
1.
2.
3.
4.
ANS:
ANS:
ANS:
ANS:
T
T
F
T
PTS:
PTS:
PTS:
PTS:
1
1
1
1
MULTIPLE CHOICE
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
ANS: C
PTS: 1
ANS: B
PTS: 1
ANS: C
PTS: 1
ANS: B
PTS: 1
ANS: C
PTS: 1
ANS: B
PTS: 1
ANS: D
PTS: 1
ANS: A
PTS: 1
ANS: C
PTS: 1
ANS: B
PTS: 1
ANS: C
PTS: 1
ANS: C
PTS: 1
ANS: D
Frequency is the number of waves that pass a given point per second.
Feedback
A
B
C
D
The AM frequency in radiowaves is 10^6 Hz.
The FM frequency in radiowaves is 10^8 Hz.
Infrared rays have a frequency of 10^14 Hz.
Correct!
PTS: 1
DIF: 2
REF: Page 120
OBJ: 5.1.1 Compare the wave and particle models of light.
TOP: Compare the wave and particle models of light.
MSC: 1
18. ANS: C
The electron configuration of silicon is 1s22s22p63s23p2.
Feedback
A
B
C
D
Silicon is a group 4A element.
Silicon is a group 4A element.
Correct!
Silicon is a group 4A element.
PTS: 1
DIF: 2
REF: Page 140
NAT: B.1
KEY: Frequency
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Valence electrons
MSC: 2
COMPLETION
19. ANS: energy
PTS: 1
20. ANS: wave
PTS: 1
21. ANS: Light
PTS: 1
22. ANS: speed
PTS: 1
23. ANS: wavelength
PTS: 1
24. ANS: amplitude
PTS: 1
25. ANS: Frequency
PTS: 1
26. ANS: hertz
PTS: 1
27. ANS: do not
PTS: 1
28. ANS: two
PTS: 1
29. ANS: spherically shaped
PTS: 1
30. ANS: n
PTS: 1
31. ANS: electrons
PTS: 1
32. ANS: three
PTS: 1
33. ANS: 2s and 2p
PTS: 1
34. ANS: nine
PTS: 1
MATCHING
35.
36.
37.
38.
ANS:
ANS:
ANS:
ANS:
C
A
D
B
PTS:
PTS:
PTS:
PTS:
1
1
1
1