Download The Structure of the Atom

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CHAPTER
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STUDY GUIDE FOR CONTENT MASTERY
The Structure of the Atom
Section 4.1
Early Theories of Matter
In your textbook, read about the philosophers, John Dalton, and defining the atom.
For each statement below, write true or false.
1. Ancient philosophers regularly performed controlled experiments.
2. Philosophers formulated explanations about the nature of matter based on
their own experiences.
3. Both Democritus and Dalton suggested that matter is made up of atoms.
4. Dalton’s atomic theory stated that atoms separate, combine, or rearrange
in chemical reactions.
5. Dalton’s atomic theory stated that matter is mostly empty space.
6. Dalton was correct in thinking that atoms could not be divided into
smaller particles.
7. Dalton’s atomic theory stated that atoms of different elements combine in
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
simple whole-number ratios to form compounds.
8. Dalton thought that all atoms of a specific element have the same mass.
9. Democritus proposed that atoms are held together by chemical bonds, but
no one believed him.
10. Dalton’s atomic theory was based on careful measurements and extensive
research.
11. There are no instruments powerful enough to magnify atoms so that they
can be seen.
12. The smallest particle of an element that retains the properties of that
element is called an atom.
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 4
19
Name
Date
CHAPTER
4
Class
CHAPTER ASSESSMENT
The Structure of the Atom
Reviewing Vocabulary
Match each definition in Column A with the term in Column B.
Column A
Column B
1. Radiation deflected toward the positively charged plate
a. atom
2. Atoms with the same number of protons but different numbers
b. nucleus
of neutrons
c. atomic mass
3. High-energy radiation that has no charge and no mass
4. The smallest particle of an element that retains the properties
of that element
d. isotopes
e. gamma ray
f.
6. The center-most part of an atom where the protons and neutrons
g. beta radiation
are contained
h. atomic mass
unit
7. Radiation deflected toward the negatively charged plate
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alpha radiation
5. The weighted average mass of an element’s isotopes
8. The rays and particles emitted by radioactive material
i.
radiation
9. Equal to 1/12 the mass of a carbon-12 atom
j.
Dalton’s atomic
theory
10. Ray of radiation traveling from the cathode to the anode
11. Process (not requiring energy) by which unstable nuclei lose energy
12. States that all matter is composed of atoms
k. cathode ray
l.
radioactivity
m. radioactive
13. Process whereby some substances spontaneously emit radiation
decay
Compare and contrast each pair of related terms.
14. mass number, atomic number
15. nuclear reaction, nuclear equation
Chapter Assessment
Chemistry: Matter and Change • Chapter 4
19
Name
CHAPTER
Section 4.3
Date
4
Class
STUDY GUIDE FOR CONTENT MASTERY
How Atoms Differ
In your textbook, read about atomic number.
For each statement below, write true or false.
1.
The number of neutrons in an atom is referred to as its atomic number.
2.
The periodic table is arranged by increasing atomic number.
3.
Atomic number is equal to the number of electrons in an atom.
4.
The number of protons in an atom identifies it as an atom of a
particular element.
5.
Most atoms have either a positive or a negative charge.
Answer the following questions.
6. Lead has an atomic number of 82. How many protons and electrons does lead have?
7. Oxygen has 8 electrons. How many protons does oxygen have?
8. Zinc has 30 protons. What is its atomic number?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
9. Astatine has 85 protons. What is its atomic number?
10. Rutherfordium has an atomic number of 104. How many protons and electrons does it have?
11. Polonium has an atomic number of 84. How many protons and electrons does it have?
12. Nobelium has an atomic number of 102. How many protons and electrons does it have?
In your textbook, read about isotopes and mass number.
Determine the number of protons, electrons, and neutrons for each isotope described below.
13. An isotope has atomic number 19 and mass number 39.
14. An isotope has 14 electrons and a mass number of 28.
15. An isotope has 21 neutrons and a mass number of 40.
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Chemistry: Matter and Change • Chapter 4
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CHAPTER
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STUDY GUIDE FOR CONTENT MASTERY
Section 4.3 continued
16. An isotope has an atomic number 51 and a mass number 123.
Answer the following question.
17. Which of the isotopes in problems 13–16 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.
18. neon-22
20. cesium-133
19. helium
21. uranium-234
Label the mass number and the atomic number on the following isotope notation.
22.
24Mg
12
23.
Circle the letter of the choice that best completes the statement.
24. 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.
25. 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.
26. 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.
22
Chemistry: Matter and Change • Chapter 4
Study Guide for Content Mastery
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In your textbook, read about mass of individual atoms.
Name
Date
CHAPTER
4
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STUDY GUIDE FOR CONTENT MASTERY
Section 4.3 continued
Use the figures to answer the following questions.
Osmium
76
Niobium
41
Os
Nb
190.2
92.906
27. What is the atomic number of osmium?
28. What is the chemical symbol for niobium?
29. What is the atomic mass of osmium?
30. What units is the atomic mass reported in?
31. How many protons and electrons does an osmium atom have? A niobium atom?
Calculate the atomic mass of each element described below. Then use the periodic table
to identify each element.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
32.
33.
Isotope
Mass (amu)
Percent Abundance
63X
62.930
69.17
65X
64.928
30.83
Isotope
Mass (amu)
Percent Abundance
35X
34.969
75.77
37X
36.966
24.23
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 4
23
Name
Date
1
Enrichment
Class
How do isotopes differ?
Chapter
9
Directions: Most elements exist in nature as isotopes. Isotopes of an element are almost identical in their
chemical properties and reactions. However, the nuclear properties of isotopes are different. Not only do isotopes
differ in mass, but some may be radioactive. Using a periodic table, complete the information in the chart below.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
1.
1
1H
2.
2
1H
3.
3
1H
4.
4
2 He
Atomic number
Number of
protons
Mass number
Number of
neutrons
1
1
Meeting Individual Needs
Symbol
1
3
2
2
5.
12
6C
12
6.
14
6C
14
7.
18
8O
18
8.
49
21 Sc
9.
63
27 Co
10.
212
82 Pb
212
11.
222
88 Ra
222
12.
226
88 Ra
226
13.
235
92 U
235
14.
238
92 U
238
21
28
63
Radioactivity and Nuclear Reactions
31
Name
Date
Directed Reading for
Content Mastery
Section 1
■
Section 2
■
Class
Structure of the
Atom
Masses of Atoms
Chapter
18
Directions: Use the terms below to complete the following paragraphs about atoms , atomic mass, and
isotopes. Terms may be used more than once.
six
number
electrons
isotopes
electron cloud
neutron(s)
proton(s)
mass
quarks
six protons
The electron has very little mass compared to the 1. ________________ or
many 3. ________________ and 4. ________________ it has. The sum of the
protons and neutrons is the mass 5. ________________ of an atom. The number
of neutrons in an atom can be found by subtracting the atomic number from the
6. ________________ number. The mass of the atom is so small that there is a
measure called the atomic 7. ________________ unit designated by amu.
8. ________________ and 9. ________________ make up the nucleus and are made up
of 10. ________________. There are 11. ________________ uniquely
different quarks. 12. ________________ are found in an area around the nucleus called
the 13. ________________. The nuclei of all atoms of a given element always have the
same number of 14. ________________. They will also have the same number of
15. ________________ around the nucleus. Some atoms may have more or fewer
16. ________________ than will other atoms of the same element. Atoms of the same
element with different numbers of neutrons are called 17. ________________. Every
atom of carbon must contain 18. ________________ but some contain six neutrons and
others have eight neutrons.
20 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
2. ________________. The mass of the atom depends on the nucleus and how
Name
2
Date
Reinforcement
Masses of Atoms
Class
Chapter
18
Directions: Answer the following questions on the lines provided.
1. What are isotopes?
3. What is the average atomic mass of an element?
4. Compare and contrast the atomic structure of the chlorine-35 and chlorine-37 isotopes.
5. Suppose that a newly discovered element called centium has three isotopes that occur in
nature. These are centium-200, centium-203, and centium-209. Assume that these isotopes
occur in equal amounts in nature. What will be the average atomic mass of this element?
28 Properties of Atoms and the Periodic Table
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Meeting Individual Needs
2. How do Boron-10 and Boron-11 differ?
Name
Date
CHAPTER
4
Class
CHAPTER ASSESSMENT
Understanding Main Ideas (Part B)
For each description in Column A, write the letter of the matching symbol in Column B.
Column A
Column B
1. Isotope in which the number of neutrons is six more than the
isotope’s atomic number
a. 178O
b. 63
29Cu
2. Copper-63
c. 126C
3. Copper with seven neutrons more than its atomic number
4. Isotope that has one neutron more than its number of protons
5. Carbon with equal numbers of neutrons, protons, and electrons
6. Carbon with two more neutrons than its number of protons
7. Chromium with two more neutrons than its number of protons
d. 50
24Cr
e. 146C
f.
65Cu
29
g. 52
24Cr
h. 54
24Cr
8. Isotope in which the difference between the neutrons and number
of protons is 4
Answer the following questions.
9. Calculate the atomic mass of gallium (Ga). Gallium has two isotopes: 69Ga and 71Ga.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
69Ga
has a relative abundance of 60.12% and an atomic mass of 68.9257 amu. 71Ga has a
relative abundance of 39.88% and an atomic mass of 70.9249 amu. Show all your work.
10. Calculate the atomic mass of the element X. Then use the periodic table to identify the
element. Show all your work.
Isotope
Mass (amu)
Percent Abundance
27X
27.977
92.23
28X
28.976
4.67
29X
29.974
3.10
Chapter Assessment
Chemistry: Matter and Change • Chapter 4
21
Name
Date
4
Reinforcement
Class
Chapter
Nuclear Reactions
9
Directions: Use the diagrams below to complete the following activities.
1p
1n
+
1p
1n
2p
2n
Energy
56p
85n
n
n
92p
143n
n
n
Ene
rgy
36p
56n
1. The diagrams show two types of nuclear reactions: nuclear fission and nuclear fusion. Label the
type of reaction shown in each diagram in the space provided.
2. Circle the letter of the equation that correctly explains the nuclear reaction shown in the top
diagram.
a. H-2 + H-2 → H-4
c. H-1 + H-1 → H-2
b. H-2 + H-2 → He-4
d. H-1 + H-1 → He-2
3. Circle the letter of the equation that correctly explains the nuclear reaction shown in the
bottom diagram.
a. 1 neutron + U-235 → Ba-141 + Kr-92 + 3 neutrons + energy
b. 1 neutron + U-238 → Ba-141 + Kr-92 + 4 neutrons
c. Ba-141 + Kr-92 → U-235 + 3 neutrons
d. Ba-141 + Kr-92 → U-238
4. What two elements are involved in the nuclear fusion reaction?
5. Label each atom in the fusion reaction with its correct symbol and isotope notation.
6. What three elements are involved in the fission reaction shown?
7. Label each atom in the nuclear fission reaction with its chemical symbol and its correct isotope
notation.
30 Radioactivity and Nuclear Reactions
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Meeting Individual Needs
gy
Ener
+
Name
Date
4
CHAPTER
Section 4.4
Class
STUDY GUIDE FOR CONTENT MASTERY
Changes to the Nucleus—Nuclear Reactions
In your textbook, read about radioactivity.
For each item in Column A, write the letter of the matching item in Column B.
Column A
Column B
1. The rays and particles that are emitted by a radioactive material
a. nuclear reaction
2. A reaction that involves a change in an atom’s nucleus
b. beta radiation
3. The process in which an unstable nucleus loses energy
c. radiation
spontaneously
d. radioactive decay
4. Fast-moving electrons
In your textbook, read about types of radiation.
Use the diagram to answer the questions.
Hole
Gamma rays
(no charge)
Alpha
particles
(2 charge)
Radioactive
source
Negative plate
Zinc sulfide
coated screen
5. Which plate do the beta particles bend toward? Explain.
6. Explain why the gamma rays do not bend.
7. Explain why the path of the beta particles bends more than the path of the alpha particles.
Complete the following table of the characteristics of alpha, beta, and gamma radiation.
Radiation Type
Composition
Symbol
Mass (amu)
Charge
8. Alpha
9.
10.
24
1/1840
High-energy electromagnetic radiation
Chemistry: Matter and Change • Chapter 4
Study Guide for Content Mastery
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Lead block
Beta
particles
(1 charge)
Positive plate
CHAPTER 4
The Structure of the Atom
Name:
Date:
Use the diagram below to answer question 1.
+
+
+
+
92 p + +
proton (p) +
neutron (n) 146 n
+
+
+
+
uranium-238 nucleus daughter
(parent nucleus)
nucleus
++
Use the chart below to answer questions
3 and 4.
2p
2n
Element Atomic Isotope
#
helium-4 nucleus
(alpha particle)
hydrogen
hydrogen-1
hydrogen-2
1.01 amu
2.01 amu
99.985
0.015
6
carbon-12
carbon-13
carbon-14
12.00 amu
13.00 amu
14.00 amu
98.90
1.09
0.01
8
oxygen-16
oxygen-17
oxygen-18
15.99 amu
17.00 amu
18.00 amu
98.90
0.038
0.200
copper-63
copper-65
62.94 amu
64.93 amu
69.17
30.83
1
carbon
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
1
The diagram above illustrates a nuclear reaction in
which uranium-238 emits an alpha particle. How
many protons and neutrons will the daughter
nucleus have?
A
90 p and 144 n
B
92 p and 142 n
C
92 p and 150 n
D
94 p and 148 n
oxygen
copper
29
3
This question covers TEKS 6B. This question tests
the material that was covered in the textbook on
page 106.
2
In his latest dig, Dr. Butrell found an abundance of
lead (Pb) in some ancient artifacts. What is the
atomic number of Pb?
A
80
B
81
C
82
D
83
This question covers TEKS 3D. This question tests
the material that was covered in the textbook on
page 105.
%
Atomic mass
of isotope abundance
The chart shows isotopes of some common elements.
Which property is used to name the isotopes?
A
Atomic number
B
Atomic mass
C
Mass number
D
Percent natural occurrence
This question covers TEKS 6B. This question tests
the material that was covered in the textbook on
page 100.
4
The atomic mass of an element is the weighted
average mass of the isotopes of that element. Based
on this definition, which of these does NOT show
the correct atomic mass for an element?
A
Hydrogen: 1.008 amu
B
Carbon: 12.011 amu
C
Oxygen: 15.999 amu
D
Copper: 63.017 amu
This question covers TEKS 6B. This
question tests the material that was
covered in the textbook on page 104.
Reviewing Chemistry: Mastering the TEKS
Chemistry: Matter and Change
7
CHAPTER 4
The Structure of the Atom, continued
Name:
Date:
Use the diagram below to answer question 5.
Use the diagram below to answer question 7.
rays
alpha particle
+
—nucleus of gold atom
paths of
alpha particles
+
+
rays
rays
+
-
+
+
5
The diagram above shows the results of Rutherford’s
experiment in which he used a radioactive source to
“shoot” alpha particles at a thin sheet of gold foil.
Based on these results, what were Rutherford’s
conclusions?
Atoms are solid matter with positive and
negative charges scattered throughout.
B
Atoms are solid, positively charged matter with
negatively charged electrons scattered
throughout.
C
7
Atoms are mostly empty space with small,
dense, positively charged centers.
D
Atoms are mostly empty space with small,
dense, negatively charged centers.
This question covers TEKS 3A. This question
tests the material that was covered in the
textbook on page 95.
6
The cathode ray tube is a key component of which
of the following revolutionary inventions?
A
Automobile
B
Fax machine
C
Television
D Photocopier
This question covers TEKS 3C. This question tests
the material that was covered in the textbook on
pages 92–93.
8
Chemistry: Matter and Change
The diagram above shows how alpha, beta, and
gamma rays are affected by two electrically charged
plates. Based on the paths the rays follow, what are the
respective charges of alpha, beta, and gamma rays?
A
negative, positive, none
B
positive, negative, none
C
negative, none, positive
D
positive, none, negative
This question covers TEKS 6A. This question tests
the material that was covered in the textbook on
page 106.
8
In the fourth century BC, Greek scholars rejected
Democritus’s ideas about the atom. This rejection
was most likely based on —
A
experimentation
B
government legislation
C
religious beliefs
D
the popularity of Aristotle’s ideas on nature
This question covers TEKS 3C. This
question tests the material that was
covered in the textbook on page 89.
Reviewing Chemistry: Mastering the TEKS
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
A
radioactive
substance
lead shield