Ch 4 - Quiz 1.3 -
Practice Quiz
DIRECTIONS: Standard
Directions (see “Standard Stuff” >
“Class Forms & Charts”
> “A-Z Homework” )
1. The concept
that matter was composed of tiny indivisible particles was originally given by
____________________.
2. Researchers
discovered a subatomic particle while working with the cathode ray tube. The
particle is known as a(n) ____________________.
3. A
____________________ is a subatomic particle that has mass nearly equal to that
of a proton, but it carries no electrical charge.
4. Atoms with the
same number of protons but different number of neutrons are called
____________________.
5. Uranium is a
naturally occurring element that emits particles and rays spontaneously through
a process called _____________________.
6. An alpha
particle is _____________________ charged with two protons and neutrons.
7. In the equation 
, the ___________________
decay of radioactive carbon-14 results in the creation of a new nitrogen-14
atom.
8. A beta particle
consists of a fast moving electron and has a(n)
_____________________ charge.
9. In nanotechnology,
individual atoms are seen using the ____________________ microscope.
10. The mass of an
electron is ____________________ g.
11. James Chadwick
showed that the nucleus also contained a neutral subatomic particle known as
the ____________________.
12. Democritus
believed that matter is made up of tiny individual particles known as a(n) ____________________.
13. The number of
protons in an atom is called the ____________________ of the element.
Short
Answer
14. Define an
atom.
15. What do you
understand by the term atomic mass unit (amu)?
16. What is a
nuclear reaction?
17. How are atomic
number and mass number denoted in the chemical symbol of the isotope of an element?
Express the shortened notation for an isotope of element X with atomic number
92 and atomic mass 238.
18. Identify the
element containing 34 protons.
19. What were the
main flaws in
20. Fast moving
electrons travel through the empty space surrounding the nucleus. How are
electrons held within the atom?
Draw and label a diagram of each atomic
model.
21. plum pudding model
22. nuclear atomic model
23. Complete the
following table of proton, electron, and neutron characteristics.
|
Particle |
Symbol |
Location |
Relative Charge |
Relative Mass |
|
Proton |
|
|
|
|
|
|
n0 |
|
|
|
|
|
|
|
|
1/1840 |
24. Lead has an
atomic number of 82. How many protons and electrons does lead have?
25. Oxygen has 8
electrons. How many protons does oxygen have?
26. Zinc has 30
protons. What is its atomic number?
27. Astatine has
85 protons. What is its atomic number?
28. Rutherfordium has an atomic number of 104. How many protons
and electrons does it have?
29. Polonium has an
atomic number of 84. How many protons and electrons does it have?
30. Nobelium has
an atomic number of 102. How many protons and electrons does it have?
Determine the number of protons,
electrons, and neutrons for each isotope described below.
31. An isotope has
atomic number 19 and mass number 39.
32. An isotope has
14 electrons and a mass number of 28.
33. An isotope has
21 neutrons and a mass number of 40.
34. An isotope has
an atomic number 51 and a mass number 123.
35. Which of the isotopes
in the problems above are isotopes of the same element? Identify the element.
Write each isotope below in symbolic
notation. Use the periodic table to determine the atomic number of each
isotope.
36. neon-22
37. helium
38. cesium-133
39. uranium-234
40. Write the mass
number of the following isotope notation. 
41. Write the
atomic number of the following isotope notation.
Use the figures to answer the following
questions.
42. What is the
atomic number of osmium?
43. What is the
chemical symbol for niobium?
44. What is the
atomic mass of osmium?
45. What units is
the atomic mass reported in?
46. How many
protons and electrons does an osmium atom have? A niobium atom?
Use the diagram to answer the questions.
47. Which plate do
the beta particles bend toward? Explain.
48. Explain why
the gamma rays do not bend.
49. Explain why
the path of the beta particles bends more than the path of the alpha particles.
50. Complete the following
table of the characteristics of alpha, beta, and gamma radiation.
|
Radiation Type |
Composition |
Symbol |
Mass (amu) |
Charge |
|
Alpha |
|
|
|
|
|
|
|
|
1/1840 |
|
|
|
High-energy electromagnetic radiation |
|
|
|
Problem
51. Complete the
following table:
|
Element |
Number of protons |
Number of electrons |
Number of neutrons |
Atomic number |
Mass number |
|
Sodium |
|
11 |
12 |
|
|
|
Phosphorus |
15 |
|
|
|
31 |
|
Cobalt |
27 |
|
32 |
|
|
|
Bromine |
|
35 |
|
|
80 |
|
Silver |
|
|
61 |
47 |
|
52. An element X has
two naturally occurring isotopes: X-79 (abundance = 50.69%, mass = 78.918 amu) and X-81 (abundance = 49.31%, mass = 80.917 amu). Calculate the weighted atomic mass of X. Also,
identify the unknown element which exists as a reddish-brown gas and is a liquid
at room temperature.
53. An element X
has three naturally occurring isotopes: X-24, X-25, and X-26. The atomic mass
of X-25 is 24.986 amu and the relative abundance is
10.00 %. The atomic mass of X-26 is 25.982 amu and
the relative abundance is 11.01 %.Given that the weighted atomic mass of the
element X is 24.305, calculate the mass contribution due to the isotope X-24
and identify the element.
54. Calculate the
number of protons, electrons, and neutrons in an atom of the element Pb with mass number 207 and atomic number 82.
55. Calculate the
mass in grams for 7 atoms of manganese (Mn) with
atomic number 25 and mass number 55. (Given: mass of a proton = 1.673 ´ 10
,
mass of a neutron = 1.675 ´ 
).
56. Fluorine (F)
contains 9 proton and 10 neutrons. Calculate its mass in amu
for 81 atoms. (Given: mass of a proton = 1.007276 amu,
mass of a neutron = 1.008665 amu).
57. Lead contains
82 protons and 125 neutrons. Write the shortened notation of the element with
its symbol, atomic number, and mass number.
58. Complete the
nuclear equations for the isotopes given in the table below:
|
Isotope |
Decay |
Nuclear equation |
|
Carbon - 14 |
beta |
|
|
Radium - 226 |
alpha |
|
|
Uranium - 238 |
alpha and gamma |
|
Ch 4 - Quiz 1.3 -
Practice Quiz
Answer Section
COMPLETION
1. ANS: Democritus
PTS: 1 DIF: 1 REF: Page 88
OBJ: 4.1.1 Compare and contrast the atomic models
of Democritus and
NAT: G.3 | UCP.2 | B.1 | B.2
TOP: Compare and contrast the atomic models of
Democritus and
KEY: Atomic models MSC: 1
2. ANS: electron
PTS: 1 DIF: 1 REF: Page 92 | Page 93
OBJ: 4.2.1 Distinguish between the subatomic
particles in terms of relative charge and mass.
NAT: B.1 | G.3 STA: 1h
TOP: Distinguish between the subatomic particles
in terms of relative charge and mass.
KEY: Electron MSC: 1
3. ANS: neutron
PTS: 1 DIF: 1 REF: Page 96
OBJ: 4.2.2 Describe the structure of the nuclear
atom, including the locations of the subatomic particles.
NAT: B.1 | G.3 STA: 1h
TOP: Describe the structure of the nuclear atom, including
the locations of the subatomic particles.
KEY: Neutron MSC: 1
4. ANS: isotopes
PTS: 1 DIF: 1 REF: Page 100
OBJ: 4.3.2 Define an
isotope and explain why atomic masses are not whole numbers.
NAT: B.1 TOP: Define an isotope and explain why atomic
masses are not whole numbers.
KEY: Isotopes MSC: 1
5. ANS: radioactivity
PTS: 1 DIF: 1 REF: Page 105
OBJ: 4.4.1 Explain the relationship between
unstable nuclei and radioactive decay.
NAT: B.1 | B.6 STA: 11c | 11d
TOP: Explain the relationship between unstable
nuclei and radioactive decay.
KEY: Radioactivity MSC: 1
6. ANS: positively
PTS: 1 DIF: 1 REF: Page 106
OBJ: 4.4.2 Characterize alpha, beta, and gamma
radiation in terms of mass and charge.
NAT: B.1 | B.6 STA: 11c | 11d
TOP: Characterize alpha, beta, and gamma radiation
in terms of mass and charge.
KEY: Alpha radiations MSC: 1
7. ANS: beta
PTS: 1 DIF: 1 REF: Page 107
OBJ: 4.4.2 Characterize alpha, beta, and gamma
radiation in terms of mass and charge.
NAT: B.1 | B.6 STA: 11c | 11d
TOP: Characterize alpha, beta, and gamma radiation
in terms of mass and charge.
KEY: Beta decay MSC: 2
8. ANS: negative
PTS: 1 DIF: 1 REF: Page 107
OBJ: 4.4.2 Characterize alpha, beta, and gamma
radiation in terms of mass and charge.
NAT: B.1 | B.6 STA: 11c | 11d
TOP: Characterize alpha, beta, and gamma radiation
in terms of mass and charge.
KEY: Beta particle MSC: 1
9. ANS: scanning tunneling
PTS: 1 DIF: 2 REF: Page 91 OBJ: 4.1.2 Define an atom.
NAT: B.1 TOP: Define an atom. KEY: Atom
MSC: 1
10. ANS: 9.1 ´ 10–28
PTS: 1 DIF: 2 REF: Page 94
OBJ: 4.2.1 Distinguish between the subatomic
particles in terms of relative charge and mass.
NAT: B.1 | G.3 STA: 1h
TOP: Distinguish between the subatomic particles
in terms of relative charge and mass.
KEY: Electron MSC: 1
11. ANS: neutron
PTS: 1 DIF: 1 REF: Page 95
OBJ: 4.2.2 Describe the structure of the nuclear
atom, including the locations of the subatomic particles.
NAT: B.1 | G.3 STA: 1h
TOP: Describe the structure of the nuclear atom, including
the locations of the subatomic particles.
KEY: Neutron MSC: 1
12. ANS:
atomos
atom
PTS: 1 DIF: 1 REF: Page 88
OBJ: 4.1.1 Compare and contrast the atomic models
of Democritus and
NAT: G.3 | UCP.2 | B.1 | B.2
TOP: Compare and contrast the atomic models of
Democritus and
KEY: Atom MSC: 1
13. ANS: atomic number
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: 1
SHORT
ANSWER
14. ANS:
An atom is the smallest particle of an
element that retains the properties of the element.
PTS: 1 DIF: 1 REF: Page 90 OBJ: 4.1.2 Define an atom.
NAT: B.1 TOP: Define an atom. KEY: Atom
MSC: 1
15. ANS:
The atomic mass unit measures the mass of
an atom relative to the mass of carbon-12 atom, which is taken as a standard.
One atomic mass unit is defined as 1/12 the mass of a carbon-12 atom.
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 unit MSC: 2
16. ANS:
A nuclear reaction involves a change in
the nucleus of an atom. Such a reaction results in the change of an atom of one
element into an atom of another element.
PTS: 1 DIF: 1 REF: Page 105
OBJ: 4.4.1 Explain the relationship between
unstable nuclei and radioactive decay.
NAT: B.1 | B.6 STA: 11c | 11d
TOP: Explain the relationship between unstable
nuclei and radioactive decay.
KEY: Nuclear reactions MSC: 1
17. ANS:
The atomic number is written as the
subscript in the chemical symbol of an element and the mass number is written
as the superscript in the chemical symbol of an element. The notation for an
isotope of element X is denoted as 
.
PTS: 1 DIF: 2 REF: Page 98 | Page 100
OBJ: 4.3.2 Define an
isotope and explain why atomic masses are not whole numbers.
NAT: B.1 TOP: Define an isotope and explain why atomic
masses are not whole numbers.
KEY: Atomic number | Mass number | Isotopes MSC: 3
18. ANS:
The element containing 34 protons is Selenium
(Se).
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: 1
19. ANS:
There were two main flaws in
a. Atoms are not indivisible. They are
divisible into several subatomic particles.
b. All atoms of a given element may not have
identical properties as their masses may vary slightly.
PTS: 1 DIF: 2 REF: Page 90
OBJ: 4.1.1 Compare and contrast the atomic models
of Democritus and
NAT: G.3 | UCP.2 | B.1 | B.2
TOP: Compare and contrast the atomic models of
Democritus and
KEY:
20. ANS:
As the electrons are negatively charged,
they are held within the atom by their attraction to the positively charged
protons present in the nucleus.
PTS: 1 DIF: 2 REF: Page 97
OBJ: 4.2.2 Describe the structure of the nuclear atom,
including the locations of the subatomic particles.
NAT: B.1 | G.3 STA: 1h
TOP: Describe the structure of the nuclear atom,
including the locations of the subatomic particles.
KEY: Electron MSC: 2
21. ANS:
Drawing should look like a ball of chocolate
chip cookie dough. The chocolate chips should be labeled with negative charge
or as electrons. The dough should be labeled as evenly distributed positive
charges.
PTS: 1
22. ANS:
Drawing should look like a peach with a
pit. The pit should be labeled nucleus and should include labeled protons and
neutrons. The outer circle of the peach should be labeled electrons.
PTS: 1
23. ANS:
|
Particle |
Symbol |
Location |
Relative Charge |
Relative Mass |
|
Proton |
p+ |
In the nucleus |
1+ |
1 |
|
Neutron |
n0 |
In the nucleus |
0 |
1 |
|
Electron |
e– |
In the space surrounding the nucleus |
1– |
1/1840 |
PTS: 1
24. ANS:
82 protons; 82 electrons
PTS: 1
25. ANS:
8 protons
PTS: 1
26. ANS:
30
PTS: 1
27. ANS:
85
PTS: 1
28. ANS:
104 protons; 104 electrons
PTS: 1
29. ANS:
84 protons; 84 electrons
PTS: 1
30. ANS:
102 protons; 102 electrons
PTS: 1
31. ANS:
19 protons, 19 electrons, 20 neutrons
PTS: 1
32. ANS:
14 protons, 14 electrons, 14 neutrons
PTS: 1
33. ANS:
19 protons, 19 electrons, 21 neutrons
PTS: 1
34. ANS:
51 protons, 51 electrons, 72 neutrons
PTS: 1
35. ANS:
The two isotopes with atomic number 19 are
both isotopes of potassium.
PTS: 1
36. ANS:
PTS: 1
37. ANS:
PTS: 1
38. ANS:
PTS: 1
39. ANS:
PTS: 1
40. ANS:
24
PTS: 1
41. ANS:
12
PTS: 1
42. ANS:
76
PTS: 1
43. ANS:
Nb
PTS: 1
44. ANS:
190.2
PTS: 1
45. ANS:
atomic mass units
PTS: 1
46. ANS:
osmium: 76 protons, 76 electrons; niobium: 41
protons, 41 electrons
PTS: 1
47. ANS:
the positive plate, because beta particles
are negatively charged
PTS: 1
48. ANS:
Gamma rays have no charge.
PTS: 1
49. ANS:
The beta particles have less mass than the
alpha particles and are more greatly
affected by the electric field.
PTS: 1
50. ANS:
|
Radiation Type |
Composition |
Symbol |
Mass (amu) |
Charge |
|
Alpha |
Helium nuclei, or alpha particles |
|
4 |
2+ |
|
Beta |
Electrons, or beta particles |
|
1/1840 |
1– |
|
Gamma |
High-energy electromagnetic radiation |
|
0 |
0 |
PTS: 1
PROBLEM
51. ANS:
|
Element |
Number of protons |
Number of electrons |
Number of neutrons |
Atomic number |
Mass number |
|
Sodium |
11 |
|
|
11 |
23 |
|
Phosphorus |
|
15 |
16 |
15 |
|
|
Cobalt |
|
27 |
|
27 |
59 |
|
Bromine |
35 |
|
45 |
35 |
|
|
Silver |
47 |
47 |
|
|
108 |
PTS: 1 DIF: 3 REF: Page 98 | Page 99 | Page 100
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: Composition
of elements MSC: 3
NOT: Atomic number = number of protons = number of
electrons. Mass number = number of protons + number of neutrons.
52. ANS:
79.904 amu
Bromine
PTS: 1 DIF: 3 REF: Page 102 | Page 103
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 isotopes MSC: 3
NOT: Weighted atomic mass of element X = mass
contribution of X-79 + mass contribution of X-81. Mass contribution of each
isotope = (mass in amu of the isotope) * (percent
abundance).
53. ANS:
23.985 amu
Magnesium
PTS: 1 DIF: 3 REF: Page 102 | Page 103
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 isotopes MSC: 3
NOT: Weighted atomic mass of element X = mass
contribution of X-24 + mass contribution of X-25 + mass contribution of X-26.
Mass contribution = (mass of the isotope in amu) *
(percent abundance).
54. ANS:
Number of protons = atomic number = 82.
Number of electrons = number of protons =
82.
Number of neutrons = mass number – atomic
number = 125.
PTS: 1 DIF: 2 REF: Page 98 | Page 101
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: 3
NOT: Atomic number = number of protons = number of
electrons.
55. ANS:
644.53 ´ g
PTS: 1 DIF: 3 REF: Page 97
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: Mass
of an atom in grams MSC: 3
NOT: Atomic number = number of protons. Number of
neutrons = mass number - atomic number. Mass of protons in n atoms = n (number
of protons * 1.673 * 10^-24 + number of neutrons * 1.675 * 10^-24).
56. ANS:
1551.32 amu
PTS: 1 DIF: 2 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: Mass
of individual atoms MSC: 3
NOT: The mass of an atom depends on the number of
protons and neutrons. It is expressed in atomic mass units (amu).
57. ANS:
PTS: 1 DIF: 1 REF: Page 100
OBJ: 4.3.2 Define an
isotope and explain why atomic masses are not whole numbers.
NAT: B.1 TOP: Define an isotope and explain why atomic
masses are not whole numbers.
KEY: Chemical symbol and notation MSC: 3
NOT: Isotopes are written with a shortened type
notation. The notation includes the chemical symbol, atomic number and mass
number. The atomic mass and the atomic number are written to the left of the
chemical symbol. The atomic mass is denoted as a superscript and the atomic
number is denoted as a subscript.
58. ANS:
|
Isotope |
Decay |
Nuclear equation |
|
Carbon - 14 |
beta |
|
|
Radium - 226 |
alpha |
|
|
Uranium - 238 |
alpha and gamma |
|
PTS: 1 DIF: 2 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 STA: 11c | 11d
TOP: Characterize alpha, beta, and gamma radiation
in terms of mass and charge.
KEY: Nuclear equations MSC: 3
NOT: Both mass and atomic numbers are conserved in
nuclear equations.