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Atomic Structure and
the Periodic Table
from the
Physical Science Series
Teacher’s Guide
1
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ATOMIC STRUCTURE
AND THE
PERIODIC TABLE
Produced By…
Dr. Brian A. Jerome, Ph.D.
Written and Directed By…
Dr. Brian A. Jerome, Ph.D.
Study Guide Written By…
Dr. Brian A. Jerome, Ph.D.
Stephanie Zak Jerome
Published & Distributed by…
AGC/UNITED LEARNING
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Website: http://www.unitedlearning.com
E-Mail: bistern@interaccess.com
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Copying, transmitting, or reproducing in any form, or by any
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©MCMXCVIII United Learning
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Atomic Structure and the Periodic Table
Teacher’s Guide
Table of Contents
Introduction ............................................................1
Links to Curriculum Standards ...........................1
Summary of the Video ..........................................1
Pretest ......................................................................2
Video Quiz ..............................................................2
Instructional Notes ................................................2
Student Preparation...............................................3
Introducing the Video ...........................................3
Student Objectives .................................................3
View the Video .......................................................4
Discussion Questions ............................................4
Blackline Masters ...................................................4
Extended Learning Activities...............................6
Answer Key ............................................................6
Script of Video Narration ...................................13
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Atomic Structure and the Periodic Table
Teacher's Guide
Grades 5-8
Introduction
This video is geared towards students in grades 5 - 8. The
goal of the program is to familiarize students with the principles of physical science, particularly the atomic structure and the Periodic Table. A detailed examination of the
structure of the atom will expose students to subatomic particles, including protons, neutrons, and electrons. Students
will be shown how to compute atomic numbers, and learn
how isotopes relate to atomic number. They will address
such topics as atomic mass and electron arrangement of
different elements. This information will provide background for understanding the organization of the Periodic
Table, as well as its major groups and families.
Links to Curriculum Standards
This video correlates to the following:
A. National Science Education Standards for Grades 5-8
Physical Science (Content Standard B)
Properties and Changes of Properties of Matter
B. Benchmark for Science Literacy (American Association
for the Advancement of Science - Project 2061) - for
Grades 6-8 - The Physical Setting: 4D The Structure
of Matter
Summary of the Video
The video is vocabulary-rich and uses key terminology such as
atomic structure, subatomic particles, nucleus, protons, atomic
mass units, neutron, atomic number, isotopes, electrons, electron
cloud, metals, nonmetals, and metalloids. Numerous colorful
and easy-to-understand graphics greatly enhance student under6
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standing of the key concepts involved with learning about atomic
structure and the Periodic Table.
Pretest
An optional pretest is provided (Blackline Master #1) . This
test will help you determine the level of student comprehension prior to participating in this lesson. An Answer
Key appears on pages 6-11 of this Teachers Guide.
Video Quiz
The video concludes with a ten-question Video Quiz which
may be used to gage student comprehension immediately
after the presentation of the video. Blackline Master #2:
Video Quiz provides students with a printed copy of the
questions and a list from which to choose correct answers.
Instructional Notes
Before presenting this lesson to your students we suggest
that you preview the video and review this guide, and the
accompanying blackline master activities in order to familiarize yourself with their content.
As you review the materials presented in this guide, you
may find it necessary to make some changes, additions, or
deletions to meet the specific needs of your class. We encourage you to do so, for only by tailoring this program to
your class will they obtain the maximum instructional benefits afforded by the materials.
It is also suggested that the video presentation take place
before the entire group under your supervision. The lesson activities grow out of the context of the video, therefore, the presentation should be a common experience for
all students.
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Student Preparation
You may want students to look up the vocabulary words addressed
in the video. Have them write down the definitions, and review
their spelling and pronunciations. Terms such as atomic structure, subatomic particles, nucleus, protons, atomic mass units,
neutron, atomic number, isotopes, electrons, electron cloud, metals, nonmetals, and metalloids may be unfamiliar to students,
and studying them before viewing the video will enhance student understanding.
Introducing the Video
You can introduce the video by asking students to write down as
many elements they can name. After students have made their
list of elements, compile a class list on the board. Next ask students how they would organize these elements in a logical manner. Discuss how they would organize the elements in a chart.
Ideas might include by looks, by weight, by density, or perhaps
even by atomic structure. Next, explain to students that scientists have struggled with same issue for hundreds of years, until
they developed a logical way to organize elements in a chart called
the Modern Periodic Table.
Student Objectives
After viewing the video and completing the lessons and
activities, students should be able to do the following:
• Define and identify the parts of the atom.
• Define the terms electron, proton, neutron, electron cloud,
nucleus, isotope, metals, nonmetals, and metalloids.
• Describe the organization of the Modern Periodic Table.
• Differentiate between groups and periods on the Periodic Table.
• Interpret information provided on the Periodic Table pertaining to atomic mass and atomic number.
• Describe general characteristics of groups on the Modern Periodic Table.
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View the Video
This video is approximately eighteen minutes in length.
FOLLOW-UP ACTIVITIES
Discussion Questions
Following the video, students may have additional questions. Allow time for students to air their questions. Avoid
answering the students’ questions directly. Ask them additional questions leading them to the answers on their own,
or encourage other students in the class to answer questions.
There are numerous issues which may warrant further
questions. As a class you may want to discuss the following: these questions appear on Blackline Master #3: Discussion Questions, and may be distributed prior to class
discussion. Answers to these questions appear in the Answer Key on pages __ of this guide.
1. Name the parts of an atom.
2. Provide examples of elements and their atomic number.
3. Provide an example of an isotope.
4. Provide examples of elements and their chemical symbols.
5. What are some of the characteristics of metals.
6. Describe how the Periodic Table is arranged.
Blackline Masters
The following Blackline Master activity sheets are included
with this guide. You may replicate and distribute them as
needed. An Answer Key appears on pages 6-11 of this
guide.
(1.)
Blackline Master #1: Pre-Test is to be given to your
students prior to viewing the video to assess their prior
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knowledge of the topic.
(2.)
Blackline Master #2 is the sheet corresponding to
the Video Quiz questions found at the end of the video.
You may want to stop the video before the Quiz in order to
distribute this sheet. Students should select the answers
from the list at the bottom of the page. Review the questions and answers as a group, or collect the Quizzes for
grading; they will help you determine student comprehension immediately following the video but before executing
the Follow-up Activities.
(3.)
Blackline Master #3: Discussion Questions corresponds with the questions presented in the previous section, and may be distributed prior to class discussion.
(4.)
Blackline Master #4: Word Search is a vocabulary
exercise. Once the words have been located on the grid,
students should write their own definitions of each term
on the sheet. Discuss their definitions, correcting any misconceptions.
(5.)
Blackline Master #5 is an Internet Lesson which
helps students to understand atomic structure and the Periodic Table.
(6.)
Blacklines Master #6: Navigating the Modern Periodic Table and #7: Themes on the Periodic Table are
worksheets for the students to complete in class to further
stress the concepts of atomic structure and the Periodic
Table.
(7.)
Blackline Masters #8a-8b: Post-Test is to be given
to your students after viewing the video and completing
the accompanying exercise to assess their knowledge of the
topic. Questions are weighted to reflect difficulty of answers. Total point value is 100.
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Extended Learning Activities
1. Observation Skills - Assign the students a task of trying
to identify elements in their daily surroundings at home,
school, and in other locations. After this is completed, compile a class list of all the elements that students have observed.
2. Creative Writing - Have students write a short story about
future elements that might be added to the Periodic Table.
What are the names of these new elements and why was
that name chosen? How was it discovered and what are its
uses and properties?
3. Career Connection - Have each student interview a person in his or her community who works with the Periodic
Table and its elements, such as pharmacists, engineers,
farmers, chemists, physicists, landscapers, and medical
technologists , as well as many others. Each student should
then report to the class on what he or she discovered, during a two-minute public speaking presentation.
4. History of Science - Have students research and write
five-page papers on the major figures in developing the
modern Periodic Table, such as Dmitri Mendeleev or Henry
Moseley
Answer Key
Blackline Master #1: Pre-Test
1.
F
2.
T
3.
T
4.
F
5.
F
6.
T
7.
T
8.
T
9.
F
10.
T
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Blackline Master #2: Video Quiz
1. structure
2. nucleus
3. protons
4. neutral
5. isotopes
6. electrons
7. mass
8. structure
9. metals
10. reactive
Blackline Master #3: Discussion Questions
1. Protons, neutrons, and electrons
2. Carbon 6, Copper 20, Silicon 14
3. Carbon - 14
4. Oxygen O, Hydrogen H, Calcium Ca
5. Metal elements have metal-like properties and are malleable,
good conductors of electricity, and are highly dense.
6. The Periodic Table is organized via Periodic Law, which states
that both chemical and physical properties of elements are periodic functions of their atomic structure. It is arranged using chemical symbols and atomic numbers.
Blackline Master #4: Word Search
Vocabulary Definitions:
atomic mass units - unit used to measure the mass of subatomic
particles
atomic number - the number of protons in an atom
atomic structure - arrangement and number of smaller particles
of an atom
electron cloud - space in which fast moving electrons are likely
to be found
electrons - small, fast-moving negatively-charged electrons orbiting nucleus
families - columns of elements in the Periodic Table
isotopes - atoms of the same element with different numbers of
neutrons
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metalloids -an element that has properties of both metals and
nonmetals
metals - elements which are good conductors of electricity, are
malleable, and are shiny
neutron - neutral-charged subatomic particle
nonmetals - elements that are poor conductors of electricity, are
brittle, and have low melting points
nucleus - center or core of atom that contains protons and neutrons
Periodic Table - chart that organizes all known elements according to atomic number
protons - positively charged subatomic particles located in the
nucleus of an atom
subatomic particles - smaller particles that make up the atom,
including protons, neutrons, and electrons
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Blackline Master #5: Internet Lesson
1. Atomic number is equal to the amount of electrons which
is also equal to the amount of protons in the element.
2. It is a symbol that represents either the name of the element or the Latin name of the element.
3. The atomic weight is the weight of the element. It can be
used to find the number of neutrons in an element by using the equation: Atomic Weight Atomic Number = Number of Neutrons.
4. Alkali Metals, Transitional Metals, Other Metals, Halogens, Alkali Earth Metals, Rare Earth Metals. Nonmetals,
and Noble Gases.
5. International Union of Pure and Applied Chemistry
6. Element 106 - seaburgium
7. Neptunium (Np) and Plutonium (Pu)
8. Rutherfordium (Rf), Dubnium (Db), Seaborgium (Sg).
Bohrium, (Bh) and Hassium (Hs)
Blackline Master #6: Navigating the Modern Periodic Table
1. 7
2. 18
3. The elements in the first group are called the alkali metals.
The elements in the second group are called the alkaline earth
metals. Elements in these groups are very reactive, and combine
easily with other elements.
4. The elements in group 8 are the noble gases. These elements
are very stable, and do not react readily with other elements.
5.
a. The “8” is the atomic number.
b. The number 15.999 is the atomic mass (weight) signifying the number of protons and neutrons.
6.
a. Ca
b. 20
c. 40.08
7.
a. Cu
b. 29
c. 63.546
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8.
a. 7
b. 7 electrons
c. 7 protons
Blackline Master #7: Themes on the Periodic Table
1. 18
2. There are 109 elements, although this number may vary
slightly, depending on the individual Periodic Table.
3. 7
4. Elements on the Periodic Table are organized according
to their atomic number.
5. The elements at the bottom of the Table are placed there
to make the Table shorter and easier to read. The elements
in these two rows are called the “rare earth metals.” The
first row is called the “lanthanoid series,” and is made up
of soft metals with high conductivity. The second row is
referred to as the “actinoid series;” these elements are radioactive.
6. The staircase line divides the metals, on the left, from
the nonmentals, on the right.
7. a. The metalloids are located along the bold staircase.
b. Examples of metalloids include aluminum and boron.
c. A metalloid is an elements that has properties common
to both metals and nonmetals.
8. As you go from left to right along the periods, the atomic
number increases, the elements become larger, and the elements become less metal-like.
9. The alkaline metals hold one valence electron. They tend
to bond easily with other atoms, and are very reactive.
10. a. Transition metals have low numbers of valence electrons and bond easily. They are good conductors of electricity.
b. Iron is used in making steel. Gold and silver are used to
make jewelry. Mercury is used in thermometers.
11. a. carbon
b. Carbon is an element found in thousands of compounds,
and is found in foods we eat. Silicon is a very abundant
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element in the earth’s crust and is used in making computer chips. Tin is used in making all kinds of metal alloys.
12. a. Noble gases have their outer energy level filled to
capacity with electrons. They do not readily form bonds
with other atoms and are very stable.
b. Helium is used to fill balloons. Neon is used to make the
red coloring in neon signs.
Blackline Masters #8a-8b: Post- Test
1.
structure
2.
nucleus
3.
protons
4.
positive
5.
isotopes
6.
cloud
7.
symbols
8.
groups
9.
nonmetals
10.
reactive
11.
True
12.
False
13.
False
14.
True
15.
True
16.
a.
17.
d.
18.
b.
19.
a.
20.
b.
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Script of Narration
Atomic Structure and the Periodic Table
What makes one substance different from another? What makes the
glass in these goblets different from the diamond in this ring?
They are both clear, sparkling solids. But diamonds are one of the hardest materials on earth and are even used to make saws which can cut
rock, and glass is fragile and is easily broken. The difference lies in the
types of atoms that make them up. What makes atoms different from
each other?
We are going to take a look inside atoms and examine their atomic
structure. Atomic structure refers to the arrangement and number of
smaller particles of an atom. These smaller particles that make up atoms, or subatomic particles, include protons, neutrons, and electrons.
Let us consider each subatomic particle separately.
This is an atom of carbon, a substance found in charcoal and diamonds.
The nucleus is the center or core of the atom. It is where 99.9 % of
an atom’s weight is located. The nucleus contains protons, as seen
here in red, and neutrons seen here in green.
Protons are positively charged particles, symbolized here by a “plus”
sign. All protons are the same, no matter what type of atom they are
in.
The weight of subatomic particles is measured in units called atomic
mass units. A proton weighs one atomic mass unit. There are millions
and millions of protons in a single drop of water.
The other subatomic particles located in the nucleus are neutrons. A
neutron is a neutrally-charged particle. The do not have a charge.
Neutrons also have an atomic mass of about one atomic mass unit.
While the nucleus contains most of the mass of an atom it takes up
only 1/100,000th of an atom’s space, equivalent in ratio to this ball in
this meadow.
While all atoms have a nucleus, what is it that makes them different?
The answer lies in their number of protons. The atomic number is the
number of protons in an atom. For example, the element carbon, which
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is what makes up the graphite in this pencil, has an atomic number of
“6.” It has six protons. All atoms of carbon have the same atomic number of “6.” The atomic number also equals the number of electrons.
Therefore, carbon also has six electrons, seen here in red. Copper, a
different element, has an atomic number of “20.”
It is useful to know the combined number of protons and neutrons in
an atom. The atomic mass, also known as the atomic weight or mass
number, is the sum weight of the protons and neutrons in an atom.
Let’s take the element silicon, symbolized by the letters “Si.” Silicon is
a major element that makes up the sand on this beach. Silicon has fourteen protons and fourteen neutrons that add up to an atomic weight of
28 atomic mass units.
While most types of carbon, such as that in these trees, have six protons, the number of neutrons may vary. Isotopes are atoms of the same
element
with different numbers of neutrons. For example, carbon can have an
atomic mass of 12 or 14. Carbon with an atomic mass of 12, seen here
with six red protons and six blue neutrons is referred to as “carbon 12.” But carbon can also have an atomic mass of 14, called “carbon14,” seen here with six red protons and eight blue neutrons. Carbon14 in nature is unstable, and gradually deteriorates. With specialized
equipment scientists can estimate the age of objects, such as this bone,
by measuring the degradation of carbon-14. Because most elements
have more than one isotope, each element has an average atomic mass
calculated from the average mass of its isotopes.
The fast-moving particles around the nucleus are electrons. Electrons
are negatively charged particles. They are a fraction of the size of protons or neutrons. To help you visualize this size difference, if this ball
were a neutron, then this pea would be an electron. An electron weighs
just .0006 atomic mass units. Because electrons weigh so little, their
weight is not even considered in calculating an atom’s atomic mass.
The electrons move very quickly, perhaps as quickly as a billion times
a second around the nucleus, forming what is called an electron cloud.
The electron cloud is the space in which the extremely fast-moving
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electrons are likely to be found.
As scientists learned more about elements and atoms, they developed
a way to organize them in a logical manner. They created a chart to
organize elements by their atomic structure that is referred to as the
“Modern Periodic Table.” The Modern Periodic Table represents a remarkable scientific endeavor. It takes thousands of seemingly unrelated pieces of information and fits them together in a logical format.
This organization is dictated by the Periodic Law which states that
both chemical and physical properties of elements are periodic functions of their atomic numbers. The position of elements on the Periodic Table is dictated by the number of protons, or their atomic number. Notice how the top number, the atomic number increases from
left to right. The elements on the Periodic Table are represented by
their chemical symbols. A chemical symbol is an abbreviated way of
symbolizing an element
with one or two letters For example, the element oxygen, found in the
air we breathe, is symbolized by the letter “O” on the Periodic Table.
Oxygen, along with hydrogen is a fuel commonly used in rockets.
Hydrogen is symbolized by the letter “H,” found in the upper left
portion of the chart.
Let’s take a look at another element - calcium. Calcium is an element
found in the human body and in the bones of other animals. Calcium
is also common in rocks such as limestone and marble seen here. It is
located here on the Periodic Table. The chemical symbol for calcium is
“Ca.”
On top of the chemical symbol is the atomic number. The atomic number of calcium is 20. Remember that the atomic number is equal to the
number of protons. Here you can see 20 protons with a positive charge
in the nucleus. Below the chemical symbol for calcium is the atomic
mass. Here you can see that the atomic mass of calcium is 40.08 atomic
mass units.
You will notice that the Periodic Table is organized in a grid with
rows and columns. There are 18 columns, called groups or families.
These groups, or families, have elements that possess many similar
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chemical and physical characteristics that we will explore later. The
rows in the Periodic Table are called periods. Unlike the elements in
families, the elements in periods do not have a great deal in common.
But by looking at elements across the periods we notice some interesting patterns. There are seven periods or rows. Notice that a portion of
Rows 6 and 7 has been removed. These periods are still part of the
Periodic Table, but have been moved to make the table shorter and
easier to read.
As you go from left to right in the Periodic Table, one obvious trait
stands out - the atomic numbers increase in regular intervals. For example, you see how the atomic number increases, starting with silicon, with an atomic number of 14, then phosphorus, with an atomic
number of 15, then sulfur, with an atomic number of 16, and so on.
Of the 109 known elements, the vast majority are metals. These are
highlighted on the Periodic Table in green. While you may think of
objects such as silverware, pans, and wires as metals, other elements
such as calcium and sodium are also metals. Elements toward the
middle and left such as mercury, are also metals, having metal-like
properties such as shininess, as seen in this aluminum foil, and are
malleable, the ability to be shaped. Metals are also good conductors of
electricity such as that found in this electric fence. Generally speaking,
metals also have a high density, as is this case with this piece of rapidly sinking lead. Magnesium, a metal commonly used to make airplanes is in a specific family of metals called the alkaline earth metals ,
highlighted here in blue on the Periodic Table. The alkaline earth metals are a highly reactive group. For example, magnesium seen here
brightly reacts when burned.
Within the metals are the transition metals, seen here in green. They
are less reactive than the first two groups of metals. There are many
commonly used metals in the transition metals, including iron, used
in making machinery and bridges, copper, used in wire and pipes,
and tungsten, used in light bulbs. These shiny metals tend to be good
conductors of electricity Transition metals such as iron, zinc, and co20
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balt are also used to make colorful paints.
The elements to the right of the staircase-like line in the Periodic Table
are called the nonmetals. The nonmetals tend to have opposite properties from the metals. These elements tend to have a dull luster, and are
brittle, such as this sulfur. They have low densities and melt at lower
temperatures. The do not conduct electricity well. One such family of
nonmetals are the Noble Gases, highlighted here in light red. These
elements are found in small amounts as gases in the earth’s atmosphere.
Argon is the most common of the noble gases, and makes up about
one percent of the earth’s atmosphere. Many signs are made with inert gases, such as this neon-filled sign.
The elements highlighted in orange just to the right and left of the staircase line are called metalloids because they have properties of both
and metals and nonmentals. Metalloids are solids that conduct heat
and electricity better than nonmetals but not as well as metals. Silicon
is one such metalloid that is used in computers. It is valued in computers because it is a semiconductor, meaning it is somewhere between a
conductor and an insulator of electricity.
We have explored just a small amount of the information found on the
Periodic Table. Next time you get a chance spend some time exploring
the Periodic Table. You will be surprised at the amount of interesting
facts you will learn.
Fill in the correct when you hear this tone. Good luck and let’s get
started.
1. Atomic _________ refers to the arrangement and number of smaller
particles in an atom.
2. The ________ is the center or core of an atom.
3. __________ are positively charged particles located in the nucleus.
4. Neutrons have a ________ charge.
5. __________ are atoms of the same element with different numbers of
neutrons.
6. _______ are subatomic particles with a negative charge.
7. The sum weight of protons and neutrons in an atom is its atomic
________.
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8. Elements in the Periodic Table are ordered according to their atomic
_______.
9. _________ are the most common elements on the periodic table.
10. Elements in the family called the alkaline earth metals are very
________.
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Other titles in the Physical Science Series…
Properties of Matter
Phases of Matter
Mixtures and Solutions
Elements, Compounds, and the Atom
Chemical Bonding
Chemical Reactions
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23
Atomic Structure and
the Periodic Table
from the
Physical Science Series
Cat. No. 2471
ISBN No. 1-56007-770-0
1
Name
Pre-Test : Atomic Structure and the Periodic Table
Directions: Circle the letter to indicate whether the following statements are either true (“T”) or
false (“F”).
1. Atomic structure refers to the building of compounds.
T
F
2. The nucleus is the center or core of the atom.
T
F
3. Protons are positively charged particles.
T
F
4. A neutron is a negatively charged particle.
T
F
5. Atomic number is the number of electrons in an atom.
T
F
6. Isotopes are atoms of the same element with different numbers ofneutrons.
T
F
7. Electrons are negatively charged particles.
T
F
8. The Periodic Table organizes elements by their atomic structure.
T
F
9. Chemical symbols are an abbreviated way of symbolizing electrons.
T
F
10. The vast majority of elements are metals.
T
F
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
2
Name
Video Quiz
Directions: Fill in the blank with the correct word from the list at the bottom of the page. Not all
words from the list will be used.
1. Atomic ________________________ refers to the arrangement and number of smaller particles in an
atom.
2. The ________________________ is the center or core of an atom.
3. ________________________ are positively charged particles located in the nucleus.
4. Neutrons have a ________________________ charge.
5. ________________________ are atoms of the same element with different numbers of neutrons.
6. ________________________ are subatomic particles with a negative charge.
7. The sum weight of protons and neutrons in an atom is its atomic ________________________
8. Elements in the Periodic Table are ordered according to their atomic ________________________
9. ________________________ are the most common elements on the Periodic Table.
10. Elements in the family called the alkaline earth metals are very ________________________
electron cloud
electrons
isotopes
mass units
metalloids
metals
neutral
neutron
nucleus
protons
reactive
structure
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
3
Name
Discussion Questions
Directions: Answer the following questions in the spaces provided (use the back of the sheet if
necessary) or as a group.
1. Name the parts of an atom.
2. Provide examples of elements and their atomic number.
3. Provide an example of an isotope.
4. Provide examples of elements and their chemical symbols.
5. What are some of the characteristics of metals?
6. Describe how the Periodic Table is arranged.
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
4
Name
Word Search
Directions: Find and circle the following vocabulary words in the puzzle. After completing the
puzzle, write the definition of each word on the back of the page.
atomic mass units
electrons
metals
Periodic Table
©1998 Dr. Brian A. Jerome, Ph.D.
atomic number
families
neutron
protons
atomic structure
electron cloud
isotopes
metalloids
nonmetals
nucleus
subatomic particles
Distributed by AGC/United Learning
5
Name_______________
Internet Lesson
The Web Site for This lesson Plan is not available at this time!
6
Name
Navigating the Periodic Table
Directions: Using a copy of the Modern Periodic Table, answer the questions in the spaces provided.
1. How many periods are there in the Modern Periodic Table?
2. How may groups are there in the Modern Periodic Table?
3. What are the general properties of the elements in the first two groups on the left side of the Modern Periodic Table?
4. What are the general properties of the elements in the group to the right in the Modern Periodic
Table?
5. Find the element “oxygen.”
a. What does the “8” on top of the chemical symbol signify?
b. What does the number 15.999 signify?
6. Find the element “calcium.”
a. What is the chemical symbol for calcium?
b. What is the atomic number of calcium?
c. What is the atomic mass (weight) of calcium?
7. Find the element “copper.”
a. What is the chemical symbol for copper?
b. What is atomic number of copper?
c. What is the atomic mass (weight) of copper?
8. Find the element “nitrogen.”
a. What is its atomic number?
b. How many electrons orbit its nucleus?
c. How may protons does it have?
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
7
Name
Themes on the Periodic Table
Directions: Answer the following questions using the Periodic Table and a chemistry reference book,
such as a textbook or encyclopedia.
1. How many groups (families) are there in the Periodic Table?
2. How many elements are in your Periodic Table?
3. How many periods are there in your Periodic Table?
4. What is the basic theme of organization in the Periodic Table?
5.
a. Why are elements 57 through 70, and 89 through 102, found separately at the bottom of the
table?
b. As what can the vast majority of elements in the Periodic Table be classified?
6. Look at the bold line shaped like a staircase on the right side of the table. What does it divide?
7.
a. What are the metalloids?
b. Provide three examples of metalloids.
c. What is a metalloid?
8. Describe two trends in the Periodic Table as you go from left to right along periods.
9. Group 1 includes the alkaline metals. What are the general properties of elements in this group?
10. Between groups 2 and 3 are the transition metals.
a. Describe the general properties of the transition metals.
b. List three examples of transition metals and their uses.
11. Group 14 is called the carbon group.
a. What is the element at the top of the group?
b. List three elements in this group and their uses.
12. Group 18 is referred to as the noble gases.
a. Briefly describe the characteristics of these elements.
b. List two elements in this group and their uses.
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
8a
Name
Post - Test : Atomic Structure and the Periodic Table
Directions: Answer the following questions in the spaces provided. Use the back of the sheet if
necessary. Questions are worth five points each.
Fill in the blank with the correct word.
1. Atomic __________________refers to the arrangement and number of smaller particles of an atom.
2. The __________________is the center of the atom.
3. The atomic number is the number of __________________in an atom.
4. Protons have a __________________charge.
5. __________________are atoms of the same element with different number of neutrons.
6. The electron __________________is the space in which electrons are likely to be found.
7. Elements on the periodic table are represented by chemical __________________
8. The columns in the periodic table are referred to as __________________
9. Metalloids have properties of both metals and __________________
10. Elements to the far left in the Periodic Table are very __________________
Circle “T” if the statement is true, or “F” if it is false.
11. The weight of subatomic particles is measured in units called atomic mass units.
T
F
12. A neutron has a negative charge.
T
F
13. Electrons are larger than protons and neutrons.
T
F
14. The position of elements on the Periodic Table is dictated by the number of protons.
T
F
15. Rows in the Periodic Table are referred to as “periods.”
T
F
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning
8b
Name
Post - Test : Atomic Structure and the Periodic Table
Circle the correct answer
16. The atomic number of an element is also equal to its number of
a. electrons
b. atoms
c. molecules
d. subatomic particles
17. A proton weighs ______ atomic mass units.
a. 3
b. 5
c. 2
d. 1
18. The majority of the elements on the Periodic Table are
a. false
b. metals
c. unreactive
d. harmful
19. Metals tend to be good
a. conductors
b. insulators
c. buffers
d. gases
20. Elements in the noble gases tend to be
a. very reactive
b. stable
c. strong
d. heavy
©1998 Dr. Brian A. Jerome, Ph.D.
Distributed by AGC/United Learning