Download Study Guide for Content Mastery

Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Study Guide for Content Mastery Answer Key
Name
Date
CHAPTER
4
Class
Name
Date
4
CHAPTER
STUDY GUIDE FOR CONTENT MASTERY
The Structure of the Atom
Section 4.2
Class
STUDY GUIDE FOR CONTENT MASTERY
Subatomic Particles and the Nuclear Atom
In your textbook, read about discovering the electron and the nuclear atom.
Section 4.1
For each item in Column A, write the letter of the matching item in Column B.
Early Theories of Matter
Column A
In your textbook, read about the philosophers, John Dalton, and defining the atom.
For each statement below, write true or false.
false
true
1. Ancient philosophers regularly performed controlled experiments.
2. Philosophers formulated explanations about the nature of matter based on
Column B
c
1. Proposed the nuclear atomic model
a. Thomson
a
2. Determined the mass-to-charge ratio of an electron
b. Millikan
b
3. Calculated the mass of an electron
c. Rutherford
their own experiences.
true
3. Both Democritus and Dalton suggested that matter is made up of atoms.
true
4. Dalton’s atomic theory stated that atoms separate, combine, or rearrange
Draw and label a diagram of each atomic model.
4. plum pudding model
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.
in chemical reactions.
false
5. Dalton’s atomic theory stated that matter is mostly empty space.
false
6. Dalton was correct in thinking that atoms could not be divided into
smaller particles.
true
7. Dalton’s atomic theory stated that atoms of different elements combine in
true
8. Dalton thought that all atoms of a specific element have the same mass.
false
9. Democritus proposed that atoms are held together by chemical bonds, but
simple whole-number ratios to form compounds.
5. nuclear atomic model
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.
no one believed him.
true
10. Dalton’s atomic theory was based on careful measurements and extensive
research.
Chemistry: Matter and Change
false
11. There are no instruments powerful enough to magnify atoms so that they
can be seen.
true
12. The smallest particle of an element that retains the properties of that
element is called an atom.
In your textbook, read about the discovery of protons and neutrons.
Complete the following table of proton, electron, and neutron characteristics.
Particle
T167
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 4
19
Symbol
Location
Relative Charge
Relative Mass
6. Proton
p
In the nucleus
1
1
7. Neutron
n0
In the nucleus
0
1
8. Electron
e
In the space surrounding the nucleus
1
1/1840
20
Chemistry: Matter and Change • Chapter 4
Study Guide for Content Mastery
T168
Name
Date
CHAPTER
4
Class
Name
STUDY GUIDE FOR CONTENT MASTERY
Date
CHAPTER
4
Class
STUDY GUIDE FOR CONTENT MASTERY
Chemistry: Matter and Change
Section 4.3 continued
Section 4.3
How Atoms Differ
16. An isotope has an atomic number 51 and a mass number 123.
51 protons, 51 electrons, 72 neutrons
In your textbook, read about atomic number.
For each statement below, write true or false.
false
1. The number of neutrons in an atom is referred to as its atomic number.
Answer the following question.
true
2. The periodic table is arranged by increasing atomic number.
17. Which of the isotopes in problems 13–16 are isotopes of the same element? Identify the
true
3. Atomic number is equal to the number of electrons in an atom.
true
4. The number of protons in an atom identifies it as an atom of a
false
5. Most atoms have either a positive or a negative charge.
element.
The two isotopes with atomic number 19 are both isotopes of potassium.
particular element.
Write each isotope below in symbolic notation. Use the periodic table to determine the
atomic number of each isotope.
18. neon-22
Answer the following questions.
19. helium
22Ne
10
20. cesium-133
4He
2
21. uranium-234
133Cs
55
234U
92
6. Lead has an atomic number of 82. How many protons and electrons does lead have?
82 protons; 82 electrons
Label the mass number and the atomic number on the following isotope notation.
8 protons
7. Oxygen has 8 electrons. How many protons does oxygen have?
8. Zinc has 30 protons. What is its atomic number?
9. Astatine has 85 protons. What is its atomic number?
30
85
22.
mass number
23.
atomic number
24Mg
12
In your textbook, read about mass of individual atoms.
10. Rutherfordium has an atomic number of 104. How many protons and electrons does it have?
Circle the letter of the choice that best completes the statement.
104 protons; 104 electrons
24. The mass of an electron is
Study Guide for Content Mastery Answer Key
11. Polonium has an atomic number of 84. How many protons and electrons does it have?
84 protons; 84 electrons
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
12. Nobelium has an atomic number of 102. How many protons and electrons does it have?
a. 1/12 the mass of a carbon-12 atom.
102 protons; 102 electrons
b. 1/16 the mass of an oxygen-16 atom.
c. exactly the mass of one proton.
In your textbook, read about isotopes and mass number.
d. approximately the mass of one proton plus one neutron.
Determine the number of protons, electrons, and neutrons for each isotope described below.
26. The atomic mass of an atom is usually not a whole number because it accounts for
13. An isotope has atomic number 19 and mass number 39.
a. only the relative abundance of the atom’s isotopes.
19 protons, 19 electrons, 20 neutrons
b. only the mass of each of the atom’s isotopes.
14. An isotope has 14 electrons and a mass number of 28.
c. the mass of the atom’s electrons.
14 protons, 14 electrons, 14 neutrons
d. both the relative abundance and the mass of each of the atom’s isotopes.
15. An isotope has 21 neutrons and a mass number of 40.
19 protons, 19 electrons, 21 neutrons
Study Guide for Content Mastery
Chemistry: Matter and Change • Chapter 4
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
21
22
Chemistry: Matter and Change • Chapter 4
Study Guide for Content Mastery
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Study Guide for Content Mastery Answer Key
Name
Date
CHAPTER
4
Class
Name
STUDY GUIDE FOR CONTENT MASTERY
Date
4
CHAPTER
Class
STUDY GUIDE FOR CONTENT MASTERY
Section 4.3 continued
Use the figures to answer the following questions.
Section 4.4
Changes to the Nucleus—Nuclear Reactions
In your textbook, read about radioactivity.
Osmium
76
Niobium
41
Os
Nb
190.2
92.906
For each item in Column A, write the letter of the matching item in Column B.
Column A
76
27. What is the atomic number of osmium?
Nb
28. What is the chemical symbol for niobium?
30. What units is the atomic mass reported in?
1. The rays and particles that are emitted by a radioactive material
a. nuclear reaction
a
2. A reaction that involves a change in an atom’s nucleus
b. beta radiation
d
3. The process in which an unstable nucleus loses energy
c. radiation
spontaneously
190.2
29. What is the atomic mass of osmium?
Column B
c
b
d. radioactive decay
4. Fast-moving electrons
atomic mass units
In your textbook, read about types of radiation.
31. How many protons and electrons does an osmium atom have? A niobium atom?
Use the diagram to answer the questions.
osmium: 76 protons, 76 electrons; niobium: 41 protons, 41 electrons
Lead block
Beta
particles
(1 charge)
Positive plate
Hole
Calculate the atomic mass of each element described below. Then use the periodic table
to identify each element.
32.
Isotope
Mass (amu)
Gamma rays
(no charge)
Percent Abundance
63X
62.930
69.17
65X
64.928
30.83
Chemistry: Matter and Change
(62.930 amu)(69.17%) 43.53 amu
65X:
(64.928 amu)(30.83%) 20.02 amu
␣
Negative plate
Zinc sulfide
coated screen
the positive plate, because beta particles are negatively charged
6. Explain why the gamma rays do not bend.
Gamma rays have no charge.
The element is copper.
Isotope
␥
5. Which plate do the beta particles bend toward? Explain.
Atomic mass of X 43.53 amu 20.02 amu 63.55 amu
33.
Alpha
particles
(2 charge)
Radioactive
source
Mass contribution (mass)(percent abundance)
63X:
␤
7. Explain why the path of the beta particles bends more than the path of the alpha particles.
Mass (amu)
Percent Abundance
35X
34.969
75.77
37X
36.966
24.23
The beta particles have less mass than the alpha particles and are more greatly
affected by the electric field.
Complete the following table of the characteristics of alpha, beta, and gamma radiation.
Mass contribution (mass)(percent abundance)
35X:
(34.969 amu)(75.77%) 26.50 amu
37X:
(36.966 amu)(24.23%) 8.957 amu
Radiation Type
Atomic mass of X 26.50 amu 8.957 amu 35.46 amu
T169
Chemistry: Matter and Change • Chapter 4
Symbol
8. Alpha
Helium nuclei, or alpha particles
4
2
9. Beta
Electrons, or beta particles
4He
2
0
1
1/1840
1
High-energy electromagnetic radiation
0
0
0
0
10. Gamma
The element is chlorine.
Study Guide for Content Mastery
Composition
23
24
Chemistry: Matter and Change • Chapter 4
Mass (amu)
Charge
Study Guide for Content Mastery