Download Chapter 17 Resource: Properties of Atoms and the Periodic Table

Glencoe Science
Chapter Resources
Properties of Atoms and
the Periodic Table
Includes:
Reproducible Student Pages
ASSESSMENT
TRANSPARENCY ACTIVITIES
✔ Chapter Tests
✔ Section Focus Activity
✔ Chapter Review
✔ Teaching Transparency Activity
✔ Assessment Transparency Activity
HANDS-ON ACTIVITIES
✔ Lab Worksheets for each Student Edition Activity
Teacher Support and Planning
✔ Laboratory Activities
✔ Content Outline for Teaching
✔ Foldables–Reading and Study Skills activity sheet
✔ Spanish Resources
✔ Teacher Guide and Answers
MEETING INDIVIDUAL NEEDS
✔ Directed Reading for Content Mastery
✔ Directed Reading for Content Mastery in Spanish
✔ Reinforcement
✔ Enrichment
✔ Note-taking Worksheets
Glencoe Science
Photo Credits
Section Focus Transparency 1: Science Photo Library/Photo Researchers
Section Focus Transparency 2: Hulton Getty
Section Focus Transparency 3: James L. Amos/CORBIS
Copyright © by The McGraw-Hill Companies, Inc. All rights reserved.
Permission is granted to reproduce the material contained herein on the condition
that such material be reproduced only for classroom use; be provided to students,
teachers, and families without charge; and be used solely in conjunction with the
Properties of Atoms and the Periodic Table program. Any other reproduction, for
use or sale, is prohibited without prior written permission of the publisher.
Send all inquiries to:
Glencoe/McGraw-Hill
8787 Orion Place
Columbus, OH 43240-4027
ISBN 0-07-866073-4
Printed in the United States of America.
1 2 3 4 5 6 7 8 9 10 067 08 07 06 05 04
Table of Contents
To the Teacher
Reproducible Student Pages
■
iv
Hands-On Activities
MiniLab Modeling an Aluminum Atom . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
MiniLab: Try At Home A Personal Periodic Table . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 4
Lab A Periodic Table of Foods. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
Lab: Use the Internet What’s in a name? . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7
Laboratory Activity 1 Chemical Activity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 9
Laboratory Activity 2 Modeling the Half-Life of an Isotope . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 13
Foldables: Reading and Study Skills . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 17
■
Meeting Individual Needs
Extension and Intervention
Directed Reading for Content Mastery . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 19
Directed Reading for Content Mastery in Spanish . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 23
Reinforcement . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 27
Enrichment . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 30
Note-taking Worksheet . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 33
■
Assessment
Chapter Review. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 37
Chapter Test . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 39
■
Transparency Activities
Section Focus Transparency Activities . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 44
Teaching Transparency Activity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 47
Assessment Transparency Activity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 49
Teacher Support and Planning
Content Outline for Teaching. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . T2
Spanish Resources . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . T5
Teacher Guide and Answers . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . T9
Additional Assessment Resources available with Glencoe Science:
•
•
•
•
•
•
•
•
•
ExamView® Pro TestMaker
Assessment Transparencies
Performance Assessment in the Science Classroom
Standardized Test Practice Booklet
MindJogger Videoquizzes
Vocabulary PuzzleMaker at: gpscience.com
Interactive Chalkboard
The Glencoe Science Web site at: gpscience.com
An interactive version of this textbook along with assessment resources are available
online at: mhln.com
iii
Reproducible
Student Pages
Reproducible Student Pages
■
Hands-On Activities
MiniLab Modeling an Aluminum Atom . . . . . . . . . . . . . . . . . . . . . . . . . 3
MiniLab: Try at Home Organizing a Personal Periodic Table . . . . . . . . 4
Lab A Periodic Table of Foods. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
Lab: Use the Internet What’s in a name? . . . . . . . . . . . . . . . . . . . . . . . . 7
Laboratory Activity 1 Chemical Activity. . . . . . . . . . . . . . . . . . . . . . . . . 9
Laboratory Activity 2 Modeling the Half-Life of an Isotope . . . . . . . . 13
Foldables: Reading and Study Skills . . . . . . . . . . . . . . . . . . . . . . . . . . . 17
■
Meeting Individual Needs
Extension and Intervention
Directed Reading for Content Mastery . . . . . . . . . . . . . . . . . . . . . . . . 19
Directed Reading for Content Mastery in Spanish . . . . . . . . . . . . . . . 23
Reinforcement . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 27
Enrichment . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 30
Note-taking Worksheet . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 33
■
Assessment
Chapter Review. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 37
Chapter Test . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 39
■
Transparency Activities
Section Focus Transparency Activities . . . . . . . . . . . . . . . . . . . . . . . . . 44
Teaching Transparency Activity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 47
Assessment Transparency Activity . . . . . . . . . . . . . . . . . . . . . . . . . . . . 49
Properties of Atoms and the Periodic Table
1
Hands-On Activities
Hands-On
Activities
2 Properties of Atoms and the Periodic Table
Date
Class
Hands-On Activities
Name
Modeling an Aluminum Atom
Procedure
1. Arrange thirteen 3-cm circles cut from orange paper and fourteen 3-cm
circles cut from blue paper on a flat surface to represent the nucleus of an
atom. Each orange circle represents one proton, and each blue circle represents one neutron.
2. Position two holes punched from red paper about 20 cm from your nucleus.
3. Position eight punched holes about 40 cm from your nucleus.
4. Position three punched holes about 60 cm from your nucleus.
Analysis
1. How many protons, neutrons, and electrons does an aluminum atom have?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
2. Explain how your circles model an aluminum atom.
3. Explain why your model does not accurately represent the true size and distances in an
aluminum atom.
Properties of Atoms and the Periodic Table
3
Name
Date
Class
Procedure
1. Collect as many of the following items as you can find: feather, penny,
container of water, pencil, dime, strand of hair, container of milk, container
of orange juice, square of cotton cloth, nickel, crayon, quarter, container of
soda, golf ball, sheet of paper, baseball, marble, leaf, and paper clip.
2. Organize these items into several columns based on their similarities to
create your own periodic table. Put your table below in the Data and
Observations section.
Data and Observations
Analysis
1. Explain the system you used to group your items.
2. Were there any items on the list that did not fit into any of your columns?
3. Infer how your activity modeled Mendeleev’s work in developing the periodic table of the
elements.
4 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Organizing a Personal Periodic Table
Name
Date
Class
Hands-On Activities
A Periodic Table of Foods
Lab Preview
Directions: Answer these questions before you begin the Lab.
1. What catagories might you use to organize your periodic table of foods?
2. What is a “family” in the Periodic Table?
Mendeleev’s task of organizing a collection of loosely related items probably
seemed daunting at first.
Real-World Question
How will using your favorite foods to create your own periodic table be similar to the task that
Mendeleev had?
Materials
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
11 ✕ 17 paper
12- or 18-inch ruler
colored pencils or markers
Goals
■
■
■
Organize 20 of your favorite foods into a periodic table of foods.
Analyze and evaluate your periodic table for similar characteristics among groups or family
members on your table.
Infer where new foods added to your table would be placed.
Procedure
1. List 20 of your favorite foods and drinks.
2. Describe basic characteristics of each of
your food and drink items. For example,
you might describe the primary ingredient,
nutritional value, taste, and color of each
item. You also could identify the food group
of each item such as fruits/vegetables,
grains, dairy products, meat, and sweets.
3. Create a data table to organize the
information that you collect.
4. Using your data table, construct a periodic
table of foods on your 11 ✕ 17 sheet of
paper. Determine which characteristics you
will use to group your items. Create families
(columns) of food and drink items that
share similar characteristics on your table.
For example, potato chips, pretzels, and
cheese-flavored crackers could be combined
into a family of salty tasting foods. Create
as many groups as you need, and you do
not need to have the same number of items
in every family.
Properties of Atoms and the Periodic Table
5
Name
Date
Class
(continued)
1. Evaluate the characteristics you used to make the groups on your periodic table. Do the
characteristics of each group adequately describe all the family members? Do the characteristics
of each group distinguish its family members from the family members of other groups?
2. Analyze the reasons why some items did not fit easily into a group.
3. Infer why chemists have not created a periodic table of compounds.
Communicating Your Data
Construct a bulletin board of the periodic table of foods created by the class. How are the
tables similar?
6 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Conclude and Apply
Name
Date
Class
Use the Internet
Hands-On Activities
What’s in a name?
The symbols used for different elements sometimes are easy to figure out.
After all, it makes sense for the symbol for carbon to be C and the symbol for
nitrogen to be N. However, some symbols aren’t as easy to figure out. For
example, the element silver has the symbol Ag. This symbol comes from the
Latin word for silver, Argentum.
Real-World Question
Test Your Hypothesis
How are symbols and names chosen for elements?
Make a Plan
Goals
1. Make a list of particular elements you wish
to study.
2. Compare and contrast these elements’
names to their symbols.
3. Research the discovery of these elements. Do
their names match their symbols? Were they
named after a property of the element, a
person, their place of discovery, or a system
of nomenclature? What was that system?
■
■
■
■
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
■
Research the names and symbols of various
elements.
Study the methods that are used to name
elements and how they have changed
through time.
Organize your data by making your own
periodic table.
Study the history of certain elements and
their discoveries.
Create a table of your findings and
communicate them to other students.
Data Source
SCIENCEOnline Visit gpscience.com/
internet_lab for more information on
naming elements, elements’ symbols, and the
discovery of new elements, and for data from
other students.
Follow Your Plan
1. Make sure your teacher approves your plan
before you start.
2. Visit the Web site provided for links to
different sites about elements, their history,
and how they were named.
3. Research these elements.
4. Carefully, record your data in the table on
the next page.
Properties of Atoms and the Periodic Table
7
Name
Date
Class
(continued)
Element
Symbol
Does the symbol
match the name?
Named for/according to
Analyze Your Data
1. Record how the symbols for your elements were chosen. What were your elements named after?
2. Make a periodic table that includes the research information on your elements that you found.
3. Make a chart of your class’s findings. Sort the chart by year of discovery for each element.
4. How are the names and symbols for newly discovered elements chosen? Make a chart that
shows how the newly discovered elements will be named.
Draw Conclusions
1. Compare your findings to those of your classmates. Did anyone’s data differ for the same
element? Were all the elements in the periodic table covered?
2. Explain the system that is used to name the newly discovered elements today.
3. Explain Some elements were assigned symbols based on their name in another language.
Do these examples occur for elements discovered today or long ago?
Communicating Your Data
SCIENCEOnline Find this lab using the link
gpscience.com/internet_lab.
Post your data in the table provided. Compare your data to those of other students.
Combine your data with those of other students to complete your periodic table with all
of the elements.
8 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Data and Observations
Date
1
Laboratory
Activities
Class
Chemical Activity
The atoms of most chemical elements can either gain or lose electrons during reactions.
Elements whose atoms lose electrons during reactions are classified as metals. Metals are found on
the left side of the periodic table of elements. The tendency of an element to react chemically is
called activity. The activity of a metal is a measure of how easily the metal atom loses electrons.
Strategy
You will observe chemical reactions between metals and solutions containing ions of metals.
You will compare the activities of different metals.
You will rank the metals by their activities.
Materials
96-well microplate
nickel nitrate solution, Ni(NO3)2aq
white paper
zinc nitrate solution, Zn(A)(NO3)2aq
plastic microtip pipette
8 1-mm ✕ 10-mm strips of each:
distilled water
aluminum, Al; copper, Cu; iron, Fe;
aluminum nitrate solution, Al(NO3)3aq
magnesium, Mg; nickel, Ni; and Zinc, Zn
copper(II) nitrate solution, Cu(NO3) 2aq
paper towels
iron(II) nitrate solution, Fe(NO3)3aq
hand lens or magnifier
magnesium nitrate solution Mg(NO3)2aq
CAUTION: Many of these solutions are poisonous. Avoid inhaling any vapors from the solutions.
These solutions can cause stains. Avoid contacting them with your skin or clothing.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Procedure
1. Place the microplate on a piece of paper on
a flat surface. Have the numbered columns
of the microplate at the top and the lettered
rows at the left.
2. Using the microtip pipette, place 15 drops
of the aluminum nitrate solution in each of
the wells A1–G1. Rinse the pipette with distilled water.
3. Place 15 drops of copper nitrate solution in
each of wells A2–G2 using the pipette.
Rinse the pipette with distilled water.
4. Repeat step 1 for each of the remaining
solutions. Add the iron nitrate solution to
wells A3–G3, the magnesium nitrate solution to wells A4–G4, the nickel nitrate
solution to wells A5–G5, the zinc nitrate
solution to wells A6–G6. Leave the wells
in column 7 empty.
5. Carefully clean each metal strip with a
paper towel.
6. Place one strip of aluminum in each of the
wells A1–A7.
7. Place one strip of copper in each of the
wells B1–B7.
8. Repeat step 5 for the remaining metals.
Add the iron strips to wells C1–C7, the
magnesium strips to wells D1–D7, the
nickel strips to wells E1–E7, and the zinc
strips to wells F1–F7. Do not put strips in
the wells in row G.
Properties of Atoms and the Periodic Table
9
Hands-On Activities
Name
Name
Date
Class
Laboratory Activity 1 (continued)
1
2
3
4
5
6
7
A
Al
B
Cu
C
Fe
D
Mg
E
Ni
F
Zn
Look for the appearance of deposited
materials in the bottom of the well. Each
change of appearance of deposits is an
indication that a chemical reaction has
taken place.
12. If you see an indication of a reaction, draw
a positive sign (+) in the corresponding
well of the microplate shown in Figure 2
in the Data and Observations section. If
you see no indication of a reaction, draw a
negative sign (–) in the corresponding well
of Figure 2.
G
(N
)2
O3
(N
Zn
)2
O3
(N
Ni
)2
3
NO
g(
M
)3
O3
(N
Fe
)2
O3
(N
Cu
)3
O3
Al
Figure 2
1
2
3
4
5
6
7
A
9. Figure 1 shows the metal and the solution
that are in each of the wells A1–G7.
10. Wait ten minutes.
11. Use a hand lens or magnifier to observe
the contents of each well. Look for a
change in the color of the solution in
each well by comparing it with the color
of the solution in well G at the bottom of
the column. Look for a change in the texture or color of the metal strip in each
well by comparing it with the piece of
metal in well 7 near the end of that row.
B
C
D
E
F
G
Data and Observations
Count the number of positive signs in each row of wells in Figure 2. Record the value under the
corresponding metal in Table 1.
Table 1
Metal
Al
Number of reactions
10 Properties of Atoms and the Periodic Table
Cu
Fe
Mg
Ni
Zn
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Figure 1
Name
Date
Class
Hands-On Activities
Laboratory Activity 1 (continued)
Questions and Conclusions
1. Why were solutions but no strips of metal placed in wells G1–G7?
2. Why were strips of metal but no solutions added to wells A7–G7?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
3. Why did you clean the metal strips with the paper towel?
4. Using the number of reactions for each metal in Table 1, rank the metals from the most active
to the least active.
Strategy Check
Can you determine whether or not a solution is active?
Can you put metals in order based on their activities?
Properties of Atoms and the Periodic Table
11
Date
2
Laboratory
Activity
Class
Modeling the Half-Life of an
Isotope
Isotopes are atoms of the same element with different atomic masses. These different masses are
a result of having different numbers of neutrons in their nuclei. Isotopes can be stable or unstable
(radioactive). Radioactive isotopes have unstable nuclei that break down in a process called
radioactive decay. During this process, the radioactive isotope is transformed into another, usually
more stable, element. The amount of time it takes half the atoms of a radioactive isotope in a
particular sample to change into another element is its half-life. A half-life can be a fraction of a
second for one isotope or more than a billion years for another isotope, but it is always the same
for any particular isotope.
Strategy
You will make a model that illustrates the half-life of an imaginary isotope.
You will graph and interpret data of the isotope’s half-life.
Materials
100 pennies
plastic container with lid
timer or clock with second hand
colored pencils
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Procedure
1. Place 100 pennies, each head-side up, into
the container. Each penny represents an
atom of an unstable isotope.
2. Place the lid securely on the container.
Holding the container level, shake it
vigorously for 20 seconds.
3. Set the conyainer on the table and take off
the lid. Remove only the pennies that are
now in a tails-up position.
4. Count the pennies you have removed and
record this number in Table 1 under Trial 1.
Also record the number of heads-up
pennies that are left.
5. Repeat steps 2 through 4 until there are no
pennies left in the container.
6. Repeat steps 1 through 5 and record your
data in Table 1 under Trial 2.
7. Calculate the averages for each time period
and record these numbers in Table 1.
8. Graph the average data from Table 1 on
Graph 1. Use one colored pencil to graph
the number of heads-up pennies against
time. Make a key for the graph that shows
this color as Radioactive Isotopes. Using a
different color of pencil, plot the number
of tails-up pennies against time. In your
key, show this color as Stable Atoms.
9. Record your averages from Table 1 again
in Table 2 under Group 1.
10. Then, record the averages obtained by
other groups in your class in Table 2.
11. Determine the totals for the combined
data from all groups in Table 2.
12. Graph this combined data in Graph 2 in
the same way as you graphed your group’s
data in step 8.
Atomic Structure and the Periodic Table
13
Hands-On Activities
Name
Name
Date
Class
Laboratory Activity 2 (continued)
Table 1
Trial 1
Shaking
time
Trial 2
A
B
C
Number of
heads-up
remaining
Number of
tails-up
removed
Number of
heads-up
remaining
Averages
D
Number of
Columns
Columns
tails-up
A
and
C
(H)
B
and D (T)
removed
After 20 s
After 40 s
After 60 s
After 80 s
After 100 s
After 120 s
After 140 s
Table 2
Start
Group
Average
H*
T*
Group 1
100
0
Group 2
100
0
Group 3
100
0
Group 4
100
0
Group 5
100
0
Group 6
100
0
Group 7
100
0
Group 8
100
0
20 s
H
T
Totals
*Note:
H = heads, T = tails
14 Atomic Structure and the Periodic Table
40 s
H
T
60 s
H
T
80 s
H
T
100 s
120 s
140 s
H
H
H
T
T
T
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Data and Observations
Name
Date
Class
Hands-On Activities
Laboratory Activity 2 (continued)
Graph 1
140
130
120
110
Time (s)
100
90
80
70
60
50
40
30
20
10
0
5 10 15 20 25 30 35 40 45 50 55 60 65 70 75 80 85 90 95 100
Number of heads or tails
140
130
120
110
100
Time (s)
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Graph 2
90
80
70
60
50
40
30
20
10
0
5 0 1 00 15 0 2 00 2 50 3 00 35 0 4 00 4 50 50 0 5 50 60 0 65 0 70 0 75 0 80 0
Number of heads or tails
Atomic Structure and the Periodic Table
15
Name
Date
Class
Laboratory Activity 2 (continued)
1. In this model, what represented the process of radioactive decay?
2. Which side of the penny represented the unstable isotope? Which side represented the stable
atom?
3. In this model, what was the half-life of the pennies. Explain.
4. What can you conclude about the total number of atoms that decay during any half-life period
of the pennies?
5. Why are more accurate results obtained when the data from all groups was combined and
graphed?
6. If your half-life model had decayed perfectly, how many atoms of the radioactive isotope
should have been left after 80 seconds?
7. If you started with 256 radioactive pennies, how many would be stable after 60 seconds?
Strategy Check
Can you make a model that illustrates the half-life of an imaginary isotope?
Can you graph and interpret data of the isotope’s half-life?
16 Atomic Structure and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Hands-On Activities
Questions and Conclusions
Name
Date
Class
Hands-On Activities
Properties of Atoms
and the Periodic Table
Directions: Use this page to label your Foldable at the beginning of the chapter.
Atoms
Know
Want
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Learned
8
O
Oxygen
15.999
Properties of Atoms and the Periodic Table
17
Meeting Individual Needs
Meeting Individual
Needs
18 Properties of Atoms and the Periodic Table
Name
Date
Directed
ContentReading for
MasteryMastery
Content
Class
Overview
Properties of Atoms and the
Periodic Table
Directions: Complete the concept map using the terms in the list below. Terms can be used more than once.
protons
periodic table
electrons
neutrons
have a mass
number equal to
the sum of
are made up of
1.
and
Meeting Individual Needs
Atoms
are organized
as elements in the
5.
4.
2.
and
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
and
6.
3.
Directions: complete the following sentences by underlining the correct words in parentheses.
7. An element is matter that is composed of one type of (atom/quark).
8. The unit of measurement used for atomic particles is the
(atom size/atomic mass unit).
9. Atoms of the same element that have different numbers of neutrons are called
(isotopes/electron clouds).
10. In the periodic table, elements are arranged by increasing atomic (power/number).
11. An electron dot diagram uses the symbol of an element and dots to represent
the (quarks/electrons) in the outer energy level.
Properties of Atoms and the Periodic Table
19
Name
Date
Directed Reading for
Content Mastery
Section 1
■
Section 2
■
Class
Structure of the
Atom
Masses of Atoms
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
Date
Directed Reading for
Content Mastery
Section 3
■
Class
The Periodic
Table
Periodic Table of the Elements
Key
1
2
3
4
H
Hydrogen
1.008
2
3
4
7
Carbon
12.011
2
13
14
15
16
5
6
7
8
He
17
Helium
4.003
9
10
Li
Be
Beryllium
9.0122
B
C
N
O
F
Ne
Boron
10.81
Carbon
12.011
Nitrogen
14.007
Oxygen
15.999
Fluorine
18.998
Neon
20.180
11
12
13
14
15
16
17
18
Al
Si
P
S
Cl
Ar
Aluminum
26.98
Silicon
28.086
Phosphorus
30.974
Sulfur
32.06
Chlorine
35.453
Argon
39.948
Na
Mg
Sodium
22.990
Magnesium
24.305
3
4
5
6
7
8
9
10
11
19
20
21
22
23
24
25
26
27
28
29
30
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Iron
55.847
Cobalt
58.9332
Nickel
58.693
Copper
63.546
Zinc
65.39
Gallium
69.72
Germanium
72.61
Arsenic
74.922
Selenium
78.96
Bromine
79.904
Krypton
83.80
K
Ca
Sc
Ti
V
Potassium
39.098
Calcium
40.078
Scandium
44.956
Titanium
47.88
Vanadium
50.94
38
39
40
Sr
Y
Zr
Nb
Strontium
87.62
Yttrium
88.9059
Zirconium
91.224
Niobium
92.91
57
56
La
Cs
Ba
Cesium
132.905
Barium
137.327
Lanthanum
138.906
Chromium Manganese
51.996
54.938
41
Rb
Rubidium
85.468
55
6
C
Lithium
6.941
37
5
18
Atomic number
Element's symbol
Element's name
Atomic mass
6
1
72
42
43
44
Mo
Tc
Ru
Molybdenum Technetium Ruthenium
97.907
101.07
95.94
73
74
75
76
45
47
31
48
32
33
36
49
50
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Palladium
106.42
Silver
107.868
Cadmium
112.41
Indium
114.82
Tin
118.710
Antimony
121.757
Tellurium
127.60
Iodine
126.904
Xenon
131.29
83
52
35
Rh
80
51
34
Rhodium
102.906
77
46
12
84
53
54
78
79
81
82
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Hafnium
178.49
Tantalum
180.95
Tungsten
183.85
Rhenium
186.207
Osmium
190.2
Iridium
192.22
Platinum
195.08
Gold
196.967
Mercury
200.59
Thallium
204.383
Lead
207.2
Bismuth
208.98
Polonium
208.982
Astatine
209.987
85
Radon
222.018
86
87
88
89
104
105
106
107
108
109
110
111
112
114
116
118
Fr
Ra
Rf
Db
Sg
Bh
Hs
Mt
Uun
Uuu
Uub
Uuq
Uuh
Uuo
Francium
223.020
Radium
226.025
Ac
Actinium
227.028
Rutherfordium
(261)
Dubnium
(262)
Seaborgium
(263)
Bohrium
(262)
Hassium
(265)
Meitnerium
(266)
Ununnilium
(269)
Unununium
(272)
Unumbium
(277)
Ununquadium
(285)
Ununhexium
(289)
Ununodium
(293)
Rare-Earth Elements
58
Lanthanide
Series
Ce
Cerium
104.115
90
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Actinide
Series
59
60
61
62
Pr
Nd
Pm
Sm
Praseodymium Neodymium Promethium Samarium
150.36
63
64
Eu
Gd
Europium Gadolinium
151.965
157.25
140.908
144.24
144.913
91
92
93
94
95
Np
Pu
Am
Th
Pa
U
Thorium
232.038
Protactinium
231.036
Uranium
238.029
Neptunium Plutonium Americium
237.048
244.064
243.061
96
Cm
Curium
247.070
65
Tb
Terbium
158.925
66
67
Dy
Ho
Dysprosium Holmium
162.50
164.93
68
69
70
71
Er
Tm
Yb
Lu
Erbium
167.26
Thulium
168.934
Ytterbium
173.04
Lutetium
174.967
97
98
99
100
101
102
Bk
Cf
Es
Fm
Md
No
Berkelium Californium Einsteinium Fermium Mendelevium Nobelium
247.070
251.080
252.083
257.095
259.101
258.099
103
Lr
Lawrencium
260.105
Directions: Use the periodic table above to answer the following questions.
1. List two types of information that are given in each box of this periodic table.
a.
b.
2. In this table, where are the metals located?
3. Where are the nonmetals located?
4. What are the elements in Groups 3 through 12 called?
5. What are the elements called that are next to the stairstep-shaped line on the
right side of the table?
6. What do we call the letter or letters that represents an element?
7. How many elements are included in the modern periodic table?
8. What name is given to the elements in Group 18?
Properties of Atoms and the Periodic Table
21
Meeting Individual Needs
1—New designation
Name
Date
Directed Reading for
Content Mastery
Class
Key Terms
Properties of Atoms and the
Periodic Table
Directions: Match the term in Column II with the definition in Column I. Write the letter of the correct term in
the blank at the left.
Column I
1. sum of the number of protons and
neutrons in the nucleus
3. positively charged center of an atom
4. vertical column in the periodic table
5. neutral particles in the nucleus of an atom
6. weighted average mass of the mixture of
its isotopes
a. nucleus
b. electrons
c. protons
d. neutrons
e. quark
f. atomic number
g. mass number
7. positively charged particles in an atom
8. table of the elements arranged according
to repeated changes in properties
9. represents the electrons in the outer
energy level of an element
h. isotope
i. average atomic mass
j. electron cloud
10. negatively charged particles in an atom
k. periodic table
11. atoms of the same element that have
different numbers of neutrons
l. atom
12. number of protons in an atom’s nucleus
m. atomic mass unit
13. horizontal row in the periodic table
n. group
14. smallest known particle that makes
up protons and neutrons
o. electron dot diagram
15. the smallest peice of matter that still
retains the properties of the element
p. period
16. developed an early periodic chart
17. approximately 1.67 ✕ 10-24g
22 Properties of Atoms and the Periodic Table
q. Dmitri Mendeleev
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
2. region around the nucleus where the
electrons are found
Column II
Nombre
Fecha
Lectura
Contentdirigida para
Mastery del contenido
Dominio
Clase
Sinopsis
Las propiedades de los átomos y la tabla periódica
Instrucciones: Completa el mapa conceptual usando los siguientes términos.
protones
tabla periódica
electrones
neutrones
están compuestos de
1.
y
están organizados
como elementos en la
Satisface las necesidades individuales
Átomos
tienen número
de masa igual
a la suma de
5.
4.
2.
y
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
y
6.
3.
Instrucciones: Completa las siguientes oraciones subrayando la palabra correcta en paréntesis.
7. Un elemento es materia compuesta de más de un tipo de (átomos/quarks).
8. La unidad de medida para las partículas atómicas es la(el)
(tamaño atómico/masa unitaria atómica).
9. Los átomos del mismo elemento que tienen distintos números de neutrones se
llaman (isótopos/nubes electrónicas).
10. En la tabla periódica los elementos se ordenan según el número creciente de
(power/number).
11. Un diagrama de puntos electrónicos usa el símbolo del elemento y puntos para
representar los (quarks/electrones) en el nivel externo de energía.
Las propiedades de los átomos y la tabla periódica
23
Nombre
Fecha
Lectura dirigida para
Clase
Sección 1
■
Sección 2
■
Dominio del contenido
Estructura
atómica
Masa atómica
Instrucciones: Usa los términos para completar los párrafos acerca de los átomos, la masa atómica y los isótopos. Puedes usar los términos más de una vez.
seis número
electrones
isótopos
nube electrónica
neutrón(es)
protón(es)
masa
quarks
seis protones
tiene muy poca masa. La masa del átomo depende del núcleo y de cuántos 3.
________________ y 4. ________________tiene. La suma de la masa de los protones y los neutrones es el(la) 5. ________________ de masa de un átomo. El
número de neutrones en un átomo se encuentra restando el número atómico del
número de 6. ________________. La masa de un átomo es tan pequeña que existe
una medida llamada unidad de 7. _________ atómica, denominada uma. Los
8. ________________ y 9. ________________ componen el núcleo y están formados por 10. ________________. Hay 11. ________________ quarks diferentes. Los
12. ________________ se encuentran en un área alrededor del núcleo llamada
13. ________________. El núcleo de todos los átomos de un elemento siempre
tiene el mismo número de 14. ________________. También tiene el mismo
número de 15. ________________alrededor del núcleo. Algunos átomos pueden
tener más o menos 16. ________________ que los demás átomos del mismo elemento. Los átomos del mismo elemento que tienen distinto número de neutrones se
llaman 17. ________________. Cada átomo de carbono debe contener
18. ________________, pero algunos contienen seis neutrones y otros tienen ocho
neutrones.
24 Las propiedades de los átomos y la tabla periódica
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Satisface las necesidades individuales
Comparado con el 1. ________________o el 2. ________________, el electrón
Nombre
Fecha
Sección 3
Lectura dirigida para
Clase
La tabla
periódica
■
Dominio del contenido
Tabla periódica de elementos
Clave
1
2
3
4
5
6
H
Hidrógeno
1.00794
2
3
4
Li
Be
Litio
6.941
Berilio
9.0122
C
Carbono
12.011
2
13
14
15
16
17
5
6
7
8
9
He
Helio
4.003
10
B
C
N
O
F
Ne
Boron
10.81
Carbono
12.011
Nitrógeno
14.007
Oxígeno
15.999
Flúor
18.998
Neón
20.179
11
12
13
14
15
16
17
18
Na
Mg
5
6
7
8
9
10
11
12
P
S
Cl
Ar
Magnesio
24.305
4
Si
Sodio
22.990
3
Al
Aluminum
26.98
Silicio
28.086
Fósforo
30.974
Azufre
32.06
Cloro
35.453
Argón
39.948
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Potasio
39.098
Calcio
40.08
Escandio
44.956
Titanio
47.88
Vanadio
50.94
Cromio
51.996
Manganesio
54.938
Hierro
55.847
Cobalt
58.9332
Nickel
58.99
Copper
63.546
Zinc
65.39
Gallium
69.72
Germanio
72.59
Arsénico
74.922
Selenio
78.96
Bromo
79.904
Criptón
83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Rubidio
85.468
Estroncio
87.62
Itrio
88.9059
Circonio
91.224
Niobio
92.91
Molibdeno
95.94
Tecnecio
97.907
Rutenio
101.07
Rodio
102.996
Paladio
106.42
Plata
107.868
Cadmio
112.41
Indio
114.82
Estaño
118.710
Antimonio
121.757
Telurio
127.60
Yodo
126.904
Xenón
131.29
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Cesio
132.905
Bario
137.327
Lantano
1.00794
Hafnio
178.49
Tántalo
180.95
Tungsteno
183.85
Renio
186.207
Osmio
190.2
Iridio
192.22
Platino
195.08
Oro
196.967
Mercurio
200.59
Talio
204.383
Plomo
207.2
Bismuto
208.98
Polonio
209.982
Astato
209.987
Radón
222.018
87
7
18
Número atómico
Símbolo del elemento
Nombre del elemento
Masa atómica
6
1
88
89
106
107
Fr
Ra
Ac
Rf
Db
Sg
Bh
Hs
Mt
Uun
Uuu
Uub
Uuq
Uuh
Uuo
Francio
223.020
Radio
226.025
Actinio
227.028
Ruterfordio
(261)
104
Dubnio
(262)
105
Seaborgio
(263)
Borio
(264)
Hasio
(265)
108
Meltnerio
(266)
109
Ununnlio
(269)
110
Ununumio
(272)
111
Unumbio
(277)
112
Ununquadio
(285)
114
Ununhexio
(289)
116
Ununodio
(293)
118
Elementos tierras raras
58
Serie de los
lantánidos
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Serie de los
actínidos
68
69
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Cerio
104.115
Praseodimio
59
Neodimio
144.24
Promecio
144.913
Samario
150.36
Europio
151.965
Gadolinio
157.25
Terbio
158.925
Disprosio
162.50
Holmio
164.93
Erbio
167.26
Tulio
168.934
Iterbio
173.04
Lutecio
174.967
103
140.908
60
61
62
63
64
65
66
67
70
71
90
91
92
93
94
95
96
97
98
99
100
101
102
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr
Torio
232.038
Protactinio
231.036
Uranio
238.029
Neptunio
237.048
Plutonio
244.064
Americio
243.061
Curio
247.070
Berkelio
247.070
Californio
251.080
Einsteinio
252.083
Fermio
257.095
Mendelevio
258.099
Nobelio
259.101
Laurencio
260.105
Instrucciones: Usa la tabla periódica para contestar las siguientes preguntas. Escribe tus respuestas en las
líneas después de cada pregunta.
1. Nombra dos tipos de información que da cada cuadro de la tabla periódica.
a.
b.
2. ¿En qué parte de la tabla se localizan los metales?
3. ¿Dónde se localizan los no metales?
4. ¿Qué nombre se les da a los elementos de los grupos del 3 al 12?
5. ¿Qué nombre se le da a los elementos que se encuentran al lado de la línea que
parece formar gradas a la derecha de la tabla?
6. ¿Qué nombre se le da a la letra o letras que representan cada elemento?
7. ¿Cuántos elementos están incluidos en la tabla periódica moderna?
8. ¿Qué nombre se le da a los elementos del grupo 18?
Las propiedades de los átomos y la tabla periódica
25
Satisface las necesidades individuales
1—Designación nueva
Nombre
Fecha
Lectura dirigida para
Dominio del contenido
Clase
Términos claves
Las propiedades de los átomos y la tabla periódica
Instrucciones: Relaciona cada término de la Columna II con su definición en la Columna I. Escribe la letra del
término correcto en los espacios de la izquierda
Columna II
Columna I
1. suma del número de protones y neutrones
en el núcleo
3. centro de carga positiva de un átomo
4. columna vertical en la tabla periódica
5. partículas neutrales en el núcleo de un átomo
6. masa promedio ponderada de la mezcla
de sus isótopos
b. electrones
c. protones
d. neutrones
e. quark
f. número atómico
g. número de masa
7. partícula de carga positiva en un átomo
8. tabla de los elementos organizada según
cambios repetidos en las propiedades
9. representa los electrones en el nivel de
energía más externo de un átomo
10. partículas de carga negativa del átomo
11. átomos del mismo elemento que tienen
números diferentes de neutrones
12. número de protones en el núcleo de un
átomo
13. fila horizontal de la tabla periódica
14. la partícula más pequeña que compone
los protones y neutrones
15. la cantidad más pequeña de materia que
retiene las mismas propiedades del elemento
16. desarrolló una antigua tabla periódica
17. aproximadamente 1.67 × 10 g
h. isótopo
i. masa atómica
promedio
j. nube electrónica
k. tabla periódica
l. átomo
m. unidad de masa
atómica
n. grupo
o. diagrama de puntos
electrónicos
p. período
-24
26 Las propiedades de los átomos y la tabla periódica
q. Dmitri Mendeleev
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Satisface las necesidades individuales
2. región alrededor del núcleo en donde se
encuentran los electrones
a. núcleo
Name
Date
1
Reinforcement
Class
Structure of the Atom
Directions: Answer the following questions on the lines provided.
1. How is the chemical symbol of an element determined?
Meeting Individual Needs
2. What are atoms composed of?
3. Are electrons, protons, or neutrons the smallest particles? If not, what are?
4. How many types of quarks are there and what is the name of one of them?
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
5. Why do scientists use models to study atoms?
6. Why has the atomic model changed over time?
7. Why is the current atomic model called the “Electron Cloud Model”?
Directions: Match the term in Column I with the definition in Column II. Write the letter of the correct definition
in the blank at the left.
Column I
Column II
8. electron
a. positively charged particle
9. neutron
b. negatively charged particle
10. nucleus
c. neutral particle
11. proton
d. smaller particles that make up
protons and neutrons
e. positively charged center of an atom
12. quark
Properties of Atoms and the Periodic Table
27
Name
2
Date
Reinforcement
Class
Masses of Atoms
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
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
2. How do Boron-10 and Boron-11 differ?
Name
Date
3
Class
The Periodic Table
Reinforcement
Directions: You will need a scientist’s patience to find the names of the 70 elements hidden in the grid. The
lanthanides and the actinides have been excluded. The same letters may appear in more than one element name.
Draw a line through the letters that correctly spell the name of an element.
A Y M R
A S
S M
R N U E
B L
U
G N T N
E
I
T T O
N C A D M
A
I
I
L O
M
I
I
U M N
I
D N
J
E N
Z E
L
I
N E H L
H
G H P
B R O M
I
N E D A
P
L
N E H T U R C S
P
K L M U
Y O
P M Q R T S C M U V H E O H
I
Y D U
R X E U A S
C R N U R B D D
P E N
I
E
J
I
T
I
L
B L
F G O H O
I
H
U
P
R
H
O R L
E M
O E N O D V P R D N
L Q T
K N D G A R T
N R
T H H
A A H
C N E D S T
U H Y A H E M P E R B E N
I
N
I
O B
I
I
U M O C
N E E
I
I
R U N T
I
D E
T
T
A T S A
A N A B E
L
E G O S C
I
S M U
I
N
I
T C A L
C
I
U M M U
I
I
I
N
I
A
I
S
I
I
A
O G N L
F
F E A M L M T
S
L N D L
N O C R
I
Z
U U D N
I
A
E
N
T T
L
I
I
A G H H
L
U
L
T P A S
I
M
V E R U E
E
O T U U H
I
E N
U
L
U N G C M N N R M Y M M R O R N T A H T U M S
I
B
O R M M M O U
G M
L E
I
L D E U L M B O R O N M L E N N T S S
M N O B R A C M
E S U L
U
L H
L
N U H T
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
L U O R
W S A Y X M D B Z
K
S
F
D E
N O E O B O C
E
R G
I
I
T U E
I
D B
U P U T U N E T
E
I
A H E L R N
P
L
T
I
P E
I
U G M
I
L
I
R T T
Y N T
I
I
M N M
I
U U L M N
R
I
U M V
Y
I
F
I
A
I
U E M E C H R O M
I
U M A N
L
T S U O X Y G E N M
E E A V U E R M U
S E C M N B M K
T
I
I
R
C E M N M D E S E N A G N A M A M P
S
I
T R O N
D
T
I
V
U M R A
E
N
N E A D A N B E
I
U A R
L A
O H T M A U D R M E
F D
C M U A M U
I
M S O L D
Directions: Complete the following paragraphs about the periodic table by filling each blank with the correct term.
In the modern periodic table, elements are listed by increasing 1. ________________. Each box
represents an 2. ________________. A box contains the name, atomic number,
3. ________________, and 4. ________________ for the element.
Vertical columns in the table are called 5. ________________. Most elements in a column have
the same number of 6. ________________ in the outer energy level and tend to have similar
7._________________.
Horizontal rows in the table are called 8. ________________. The elements on the left side of the
table are 9. ________________. Groups 3–12 contain metals known as 10. ________________.
Elements on the right side are 11. ________________.
Properties of Atoms and the Periodic Table
29
Meeting Individual Needs
O O S
I
Name
1
Date
Enrichment
Class
The Building Blocks of Matter
From experiments involving the high-speed collision of particles, scientists have determined that
heavy nuclear particles, such as protons and neutrons, are composed of quarks. The name “quark”
was taken from a novel. Quarks are classified into six flavors—up, down, strange, charm, bottom,
and top. The flavors are not related to any physical characteristics of the quarks themselves, but are
used as classifications. Unlike protons and electrons, which carry whole charges of +1 or –1, quarks
carry fractional charges. The following table lists some information about quarks.
Quarks
Symbol
Charge
Name
Symbol
Charge
up
u
2/3
down
d
1/3
strange
s
1/3
charm
c
2/3
bottom
b
1/3
top
t
2/3
Mass
1. Use the library to find the name of the author and novel from which the word “quark” was
taken.
2. Use the library to draw a time line showing the history of quarks.
3. Protons and neutrons are composed of triplets of up and down quarks. Use the information in the
table to determine which of the following quark triplets represents a proton and which represents
a neutron.
udd __________________
uud __________________
4. A heavier nuclear particle is composed of a triplet of strange quarks. What is the charge of this
particle?
30 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
Name
Name
Enrichment
Class
The Mole
You have learned that the mass of atoms is measured in atomic mass units.
This unit is too small to use in everyday measurement. It would be simpler to
have a number of atoms that would have a mass in grams that is equal to the
mass of one atom in atomic mass units. The same number would fit all elements,
because equal numbers of different atoms always have the same mass ratio.
Chemists have found that 6.02 ✕ 1023 atoms of an element have a mass in
grams equivalent to the mass of one atom in atomic mass units. This counting
unit is called a mole. For example, one mole of helium atoms has a mass of 4
grams because helium has a mass number of 4.
Do you know how big a number a mole is? Suppose the entire population of
the world, more than four billion people, were assigned to count the number of
atoms in one mole of helium. If each person counted one atom per second and
worked a 48-hour work week, the task would take more than 10 million years. If
you had one mole of pennies, you would have enough money to pay all the
expenses of the United States for the next billion years.
1. A mole is a certain number of items. What number does each of the following terms represent?
a. dozen ______________
d. mole ______________
b. billion ______________
e. gross ______________
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
c. million ______________
2. Using a laboratory balance, measure and record the mass of one mole of each of the following
elements: carbon, iron nails, zinc metal, and copper wire.
3. Find the mass, in grams, of each of the following:
a. 2 moles of aluminum ______________
b. 4 moles of magnesium ______________
c. 3 moles of helium ______________
4. How many moles are in each of the following:
a. 156 grams of chromium ______________
b. 156 grams of potassium ______________
c. 119 grams of uranium ______________
5. Why is the counting unit called a mole useful for chemists?
Properties of Atoms and the Periodic Table
31
Meeting Individual Needs
2
Date
Name
3
Date
Enrichment
Class
Predicting an Element’s
Group and Period
Several scientists, including Newlands, Meyer, and Mendeleev worked on classification systems
that grouped elements according to their properties. They found that these properties repeated in a
regular or periodic manner. This fact was used to predict properties of undiscovered elements.
Review electron arrangement from your textbook. In Table 1, write the maximum number of
electrons that can fill each energy level on the blanks in the table heading. Write the total number
of electrons for each element in the first column labeled Total. For each element, assign the correct
number of electrons to each energy level. Complete Table 2 by using the information from the six
elements studied.
Electrons
Element
Total
Level 1
Level 2
Level 3
Number of
outer electrons
Located in
group
1. Argon
2. Carbon
3. Helium
4. Lithium
5. Silicon
6. Sodium
Table 2
Element
Energy level of
outer electrons
Located in
period
7. Ar
8. C
9. He
10. Li
11. Si
12. Na
13. How is the element’s period related to the number of energy levels over which its electrons are
spread?
14. How can you predict an element’s group and period?
32 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
Table 1
Name
Date
Note-taking
Worksheet
Section 1
Class
Properties of Atoms and the
Periodic Table
Structure of the Atom
A. ____________ are abbreviated in scientific shorthand—first letter or two of element’s name
B. ________—smallest piece of matter that still has the properties of the element
1. ___________ have electrical charge of 1+.
3. _____________ have electrical charge of 1-.
4. Protons and neutrons are in the ___________ of an atom; electrons surround the nucleus.
C. Protons and neutrons are made up of smaller particles called __________.
1. Six quarks are known to exist; the sixth is called the _______ quark.
D. Scientists use scaled-up __________ to represent atoms.
1. Early models of atoms used a solid __________.
2. Current __________________ model shows electrons traveling in specific energy levels
around a nucleus of protons and neutrons.
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Section 2
Masses of Atoms
A. _______________—composed mostly of the protons and neutrons in the nucleus
1. Unit of measurement for atomic particles is ____________________ (amu) which is
one-twelfth the mass of a carbon atom containing six protons and six neutrons.
2. _________________—the number of protons in an atom; number of protons also
identifies the element
3. The sum of the number of protons and neutrons in the nucleus of an atom is
the _______________.
B. ____________—atoms of the same element with different numbers of neutrons
1. Different isotopes have different ______________.
2. Number of ____________ is equal to mass number minus atomic number.
3. Name of ___________ followed by mass number identifies the isotope.
4. _______________________ is the weighted-average mass of an element’s isotopes.
5. Average atomic mass is closest to its most ____________ isotope.
Properties of Atoms and the Periodic Table
33
Meeting Individual Needs
2. ____________ do not have an electrical charge.
Name
Date
Class
Note-taking Worksheet (continued)
Section 3
The Periodic Table
A. Elements are organized in the __________________ by increasing atomic number.
1. In the late 1800’s, Dmitri Medeleev devised the first periodic table based on
_______________.
2. In 1913, Henry G. J. Moseley arranged the elements by _________________ rather than
atomic mass.
B. Vertical columns in the periodic table are __________ of elements with similar properties.
2. Each of the seven energy levels can have a ___________ number of electrons.
a. Energy level one can contain at most _______ electrons.
b. Energy level two can contain at most _________ electrons.
3. Each row in the periodic table ends when an outer energy level is __________.
4. _________________________ use the element symbol and dots to represent outer energy
level electrons.
C. ___________—horizontal rows of elements that contain increasing numbers of protons and
electrons.
1. Elements are ______________ as metals, nonmetals, or metalloids (semimetals).
2. Elements are _______________ in laboratories all over the world.
D. The ________ elements exist all over the universe.
1. Hydrogen and helium are the ___________________ of other naturally occurring elements.
2. ______________ spread heavier elements throughout the universe.
34 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Meeting Individual Needs
1. Elements in the same group have the same number of _____________ in their outer energy
level.
Assessment
Assessment
36 Properties of Atoms and the Periodic Table
Name
Date
Class
Properties of Atoms and
the Periodic Table
Chapter
Review
Part A. Vocabulary Review
Directions: On the space at the left, write the term that correctly completes each statement. Use each term once.
metals
groups
electrons
chemical symbol
isotopes
metalloids
nucleus
average atomic mass
electron cloud
transition elements
atomic number
mass number
periods
quarks
periodic table
1. A capital letter or a combination of a capital letter and a small letter
that is used to represent an element is called a(n) ______.
2. The horizontal rows of elements are called ______.
3. An average of the masses of all the isotopes that occur in nature for
an element is the ______.
4. Vertical columns of elements are called ______.
5. Elements in the middle of the periodic table, groups 4 through 7, are
called the ______.
7. Protons and neutrons can be subdivided into ______ by colliding
them.
8. The center of an atom where protons and neutrons are located is
the ______.
9. A total count of the neutrons and protons in an atom is the ______.
10. Atoms of the same element but with different numbers of neutrons
are ______.
11. Elements that are found on the left side of the periodic table are ______.
12. Elements that have some properties of both metals and nonmetals
are ______.
13. The particles that move about the nucleus and have a negative
charge are ______.
14. The region around the nucleus occupied by electrons is a(n) ______.
15. A chart that shows the classification of elements is called the ______.
Properties of Atoms and the Periodic Table
37
Assessment
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
6. The number of protons in an atom is the ______.
Name
Date
Class
Chapter Review (continued)
Part B. Concept Review
Directions: Complete the table below by writing the correct information in the blank spaces.
Chemical
symbol
Element
Atomic
number
Number of
protons
Number of
neutrons
Mass
number
11
11
12
23
6
6
12
26
30
56
16
32
1. Sodium
2. Carbon
C
3.
Fe
26
4. Sulfur
S
16
5. Nitrogen
N
7
7
6. Oxygen
O
8
8
8
7.
He
2
2
2
8. Chlorine-35
Cl
17
17
9. Copper
Cu
29
29
35
17
20
Cl
10. Chlorine-37
14
4
35
37
1
18
11
Assessment
Na
2
13
14
15
16
17
23
26
3
A
4
5
6
7
8
9
10
11
12
C
Fe
Fe
55.8
79
Au
197
Au
B
11. Which element has a greater atomic mass, A or B?
12. Which element is a metal, B or C?
13. In which group is gold?
14. What is the average atomic mass of iron?
15. What is the atomic number of sodium?
38 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Directions: Refer to the periodic table below and the boxes at the right of the table to answer questions 11–15.
Transparency Activities
Transparency
Activities
Properties of Atoms and the Periodic Table
43
Name
1
Date
Section Focus
Transparency Activity
Class
Subatomic Collision
Transparency Activities
1. Why do you think scientists have only recently discovered these
subatomic particles?
2. What might scientists learn by breaking apart atomic nuclei?
44 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
An individual atom is so small that it would take 50 million of
them lined up in a row to equal one centimeter! Atoms, however, can
be divided into component parts, and, amazingly, some of these parts
have particles that are tinier yet. Below is an image created by these
subatomic particles taken in a device called a bubble chamber.
Name
2
Date
Section Focus
Transparency Activity
Class
Carbon Cat
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
How old are these mummified cats found in an Egyptian tomb?
Carbon-14 holds the answer. Carbon-14 is a radioactive form of
carbon, an element found in every living thing. By measuring how
much carbon-14 remains in these cats, scientists can tell approximately how many years ago the cats were buried.
1. Carbon-14 decays over time. What does “decay” mean?
2. Why do you think carbon is used by scientists to date objects such
as mummies, bones, and cloth wrappings?
3. Is it possible to use carbon-14 dating on things that were never
alive? Why or why not?
Properties of Atoms and the Periodic Table
45
Name
3
Date
Section Focus
Transparency Activity
Class
What makes the
glass glow?
1. Of what materials is glass usually made?
Transparency Activities
2. Why do you think the glass glows?
3. Why might prolonged work with such glass be dangerous?
46 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
When you hear the word uranium, you might think of nuclear
power. Uranium, though, was used in the 19th century by European
glassmakers to create what was called uranium glass. This interesting
glass had a yellowish-green color and glows under certain lighting
conditions.
Name
Date
1
Teaching Transparency
Activity
Class
Electron Cloud Model
Nucleus
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Electron
cloud
Properties of Atoms and the Periodic Table
47
Name
Teaching Transparency Activity
Date
Class
(continued)
1. What is the region around the nucleus called?
2. What was the name of the Greek who proposed the idea that atoms made up all substances?
3. What is an electron cloud?
4. What determines how far each electron travels from the nucleus?
5. Why can’t electron positions be pinpointed?
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
6. Electrons are located in a cloud surrounding what part of the atom?
48 Properties of Atoms and the Periodic Table
Name
Date
Assessment
Transparency Activity
Class
Properties of Atoms
and the Periodic Table
Directions: Carefully review the table and answer the following questions.
Characteristics of Some Alkaline Earth Metals
Atomic
number
Mass
number
Melting
point (˚C)
Boiling
point (˚C)
Magnesium
12
24
651
1105
Calcium
20
40
842
1494
Strontium
38
88
769
1384
Barium
56
137
725
1640
1. According to the table, which alkaline Earth metal has a mass
number greater than 100?
A Magnesium
C Strontium
B Calcium
D Barium
2. According to the table, which element has the LOWEST atomic
number?
F Magnesium
H Strontium
G Calcium
J Barium
3. According to the table, which element has the HIGHEST melting
point?
A Magnesium
C Strontium
B Calcium
D Barium
Transparency Activities
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
Element
4. The number of neutrons in the nucleus of an atom is equal to
the mass number minus the atomic number. According to this
definition and the table, how many neutrons are in the nucleus
of a strontium atom?
F 20
G 38
H 50
J 81
Properties of Atoms and the Periodic Table
49