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Chapter Review
A substance’s atomic structure determines its
physical and chemical properties.
CONTENT REVIEW
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KEY CONCEPTS SUMMARY
1
2
Atoms are the smallest form of elements.
VOCABULARY
• All matter is made of the
atoms of approximately
100 elements.
• Atoms are made of
protons, neutrons,
and electrons.
• Different elements are
made of different atoms.
• Atoms form ions by gaining or losing electrons.
proton p. 331
neutron p. 331
nucleus p. 331
electron p. 331
atomic number p. 332
atomic mass number
p. 332
isotope p. 332
ion p. 334
nucleus
proton
neutron
electron cloud
Elements make up the periodic table.
VOCABULARY
• Elements can be organized by similarities.
• The periodic table organizes the atoms of the elements by properties
and atomic number.
atomic mass p. 337
periodic table p. 338
group p. 342
period p. 342
Groups of elements have similar properties.
Elements in a period have varying properties.
3
The periodic table is a map of the elements.
VOCABULARY
• The periodic table has
distinct regions.
• Most elements are metals.
• Nonmetals and metalloids
have a wide range of
properties.
• Some atoms can change
their identity through
radioactive decay.
reactive p. 346
metal p. 347
nonmetal p. 349
metalloid p. 350
radioactivity p. 350
half-life p. 352
354 Unit 3: Chemical Interactions
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Reviewing Vocabulary
Describe how the vocabulary terms in the
following pairs are related to each other.
Explain the relationship in a one- or
two-sentence answer. Underline each
vocabulary term in your answer.
1. isotope, nucleus
2. atomic mass, atomic number
3. electron, proton
4. atomic number, atomic mass number
5. group, period
6. metals, nonmetals
7. radioactivity, half-life
Reviewing Key Concepts
Multiple Choice Choose the letter of the
best answer.
8. The central part of an atom is called the
a. electron
c. proton
b. nucleus
d. neutron
9. The electric charge on a proton is
a. positive
c. neutral
b. negative
d. changing
10. The number of protons in the nucleus is the
a. atomic mass
c. atomic number
b. isotope
d. half-life
11. Nitrogen has atomic number 7. An isotope of
nitrogen containing seven neutrons would be
a. nitrogen-13
c. nitrogen-15
b. nitrogen-14
d. nitrogen-16
12. How does the size of a negative ion compare
to the size of the atom that formed it?
a. It’s smaller.
b. It’s larger.
c. It’s the same size.
d. It varies.
13. The modern periodic table is organized by
a. size of atom
b. atomic mass
c. number of neutrons
d. atomic number
14. Elements in a group have
a. a wide range of chemical properties
b. the same atomic radius
c. similar chemical properties
d. the same number of protons
15. Elements in a period have
a. a wide range of chemical properties
b. the same atomic radius
c. similar chemical properties
d. the same number of protons
16. From left to right in a period, the size of atoms
a. increases
c. remains the same
b. decreases
d. shows no pattern
17. The elements in Group 1 of the periodic table
are commonly called the
a. alkali metals
c. alkaline earth metals
b. transition metals d. rare earth metals
18. The isotope nitrogen-13 has a half-life of 10
minutes. If you start with 40 grams of this
isotope, how many grams will you have left
after 20 minutes?
a. 10
c. 20
b. 15
d. 30
Short Answer Write a short answer to
each question. You may need to consult
a periodic table.
19. Rubidium forms the positive ion Rb+. Is this ion
larger or smaller than the neutral atom? Explain.
20. How can you find the number of neutrons in
the isotope nitrogen-16?
21. Explain how density varies across and up and
down the periodic table.
22. Place these elements in order from least reactive to most reactive: nickel (Ni), xenon (Xe),
lithium (Li). How did you determine the order?
Chapter 10: Atomic Structure and the Periodic Table 355
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Below is an element square from the periodic
table. Use it to answer the next two questions.
Thinking Critically
The table below lists some properties of six
elements. Use the information and your
knowledge of the properties of elements
to answer the next three questions.
Element
Appearance
Density
(g/cm3)
Conducts
Electricity
A
dark purple
crystals
4.93
no
B
shiny silvery
solid
0.97
yes
C
shiny silvery
solid
22.65
yes
D
yellow
powder
2.07
no
E
shiny gray
solid
5.32
semiconductor
F
shiny bluish
solid
8.91
yes
23. ANALYZE Based on the listed properties,
identify each of the elements as a metal,
nonmetal, or metalloid.
80
Hg
Mercury
200.59
29. CALCULATE One of the more common isotopes
of mercury is mercury-200. How many
protons and neutrons are in the nucleus of
mercury-200?
30. INFER Cadmium occupies the square directly
above mercury on the periodic table. Is a cadium
atom larger or smaller than a mercury atom?
31. CALCULATE An isotope has a half-life of 40
minutes. How much of a 100-gram sample
would remain unchanged after two hours?
32. APPLY When a uranium atom with 92 protons
and 146 neutrons undergoes radioactive
decay, it produces a particle that consists
of two protons and two neutrons from its
nucleus. Into which element is the uranium
atom transformed?
24. APPLY Which would weigh more: a cube of
element A or a same-sized cube of element D?
25. HYPOTHESIZE Which element(s) do you think
you might find in electronic devices? Why?
33. ANALYZE Look again at the photograph on
pages 326–327. Answer the question again,
using what you have learned in the chapter.
26. HYPOTHESIZE The thyroid gland, located in
your throat, secretes hormones. In 1924 iodine
was added to table salt. As more and more
Americans used iodized salt, the number of
cases of thyroid diseases decreased. Write a
hypothesis that explains the observed decrease
in thyroid-related diseases.
34. DRAW CONCLUSIONS Suppose you’ve been
given the ability to take apart and assemble
atoms. How could you turn lead into gold?
27. INFER How does the size of a beryllium (Be)
atom compare with the size of an oxygen (O)
atom?
28. PREDICT Although noble gases do not naturally
react with other elements, xenon and krypton
have been made to react with halogens such as
chlorine in laboratories. Why are the halogens
most likely to react with the noble gases?
356 Unit 3: Chemical Interactions
35. ANALYZE Explain how the structure of an atom
determines its place in the periodic table.
If you are doing a unit project, make a folder for
your project. Include in your folder a list of the
resources you will need, the date on which the
project is due, and a schedule to track your
progress. Begin gathering data.
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Standardized Test Practice
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Interpreting Tables
The table below shows part of the periodic table of elements.
Group
1
Period
1
2
3
4
18
1
H
2
2
13
14
15
16
17
He
3
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
11
12
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
Na Mg
19
20
31
32
33
34
35
36
K
Ca
Ga
Ge
As
Se
Br
Kr
Answer the questions based on the information given
in the table.
1. What does the number above the symbol for each
element represent?
a. Its number of isotopes
b. Its atomic number
c. Its number of neutrons
d. Its atomic mass
2. The atom of what element is in Period 4,
Group 13?
a. Na
c. Al
b. Ga
d. K
Extended Response
Answer the following two questions in detail. Include
some of the terms shown in the word box at right.
Underline each term you use in your answer.
7. Democritus was an ancient Greek philosopher who
claimed that all matter was made of tiny particles
he called atoms. Democritus said that all atoms
were made of the same material. The objects of
the world differed because each was made of
atoms of different sizes and shapes. How does
the modern view of atoms differ from this ancient
view? How is it similar?
3. What do the elements on the far right of the table
(He, Ne, Ar, and Kr) have in common?
a. They do not generally react with other elements.
b. They are in liquids under normal conditions.
c. They are metals that rust easily.
d. They are very reactive gases.
4. How many electrons does a neutral chlorine (Cl)
atom contain?
a. 16
c. 18
b. 17
d. 19
5. If a sodium (Na) atom loses one electron to form a
positive ion, how many electrons would lithium (Li)
lose to form a positive ion?
a. 0
c. 2
b. 1
d. 3
6. If a fluorine (F) atom gains one electron to form a
negative ion, how many electrons would bromine
(Br) gain to form a negative ion?
a. 0
c. 2
b. 1
d. 3
electron
isotope
nucleus
neutron
proton
radioactivity
8. Half-life is a measure of the time it takes half of
the radioactive atoms in a substance to decay into
other atoms. If you know how much radioactive
material an object had to begin with, how could
you use half-life to determine its age now?
Chapter 10: Atomic Structure and the Periodic Table 357