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Reading$Essentials
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Ch$16$Sect.$3
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May$13th$
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Ch$16$Sect.$3
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May$14th
Study$for$Test
Chaper$16
Test
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
Reading Essentials 289
Many parts of our lives are affected by repeated patterns. For
example, a calendar shows the patterns of weeks. Name some
repeated patterns that you see happening all the time. How
could you keep track of a pattern?
Before You Read
Organizing the Elements
When you look at the Moon, does it always appear the same?
Each month, the Moon grows larger until it is full, then grows
smaller until it seems to disappear. This type of change is called
periodic. The word periodic means “repeated in a pattern.”
The days of the week are periodic because they repeat every
seven days. Think of the calendar as a periodic table of days
and months.
Who was Dmitri Mendeleev?
In the late 1800s, a Russian chemist named Dmitri Mendeleev
wanted to find a way to organize the elements. He organized the
elements known at the time into a table. He placed the elements
in the table in order of increasing atomic mass.
Mendeleev discovered a pattern in his table. The properties of
some lighter elements seemed to repeat in heavier elements.
Because this pattern repeated, the pattern was considered to be
periodic. Today, this arrangement is called a periodic table of
elements. In the p
eriodic table
, the elements are arranged by
increasing atomic number and by changes in physical and
chemical properties.
Read to Learn
chapter
Properties of Atoms and the Periodic Table
section ● The Periodic Table
16
3
What You’ll Learn
■
the composition of the
periodic table
■
how to get information
from the periodic table
■
what metal, nonmetal,
and metalloid mean
Identify the Main Point
Look for the main point of the
paragraph or paragraphs under
each heading in this section.
When you have found the main
point, write it down on a piece
of paper. After you read the
section, look over the main
points again to help you learn
the content of the section.
1. Determine Who was the
first person to organize
the elements into a
periodic table?
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Name: __________________
Period: ________
Select
290 CHAPTER 16 Properties of Atoms and the Periodic Table
How did Mendeleev’s table predict properties?
Mendeleev left blank spaces in his table so that he could line
up the elements. He looked at the elements surrounding the
blank spaces. He predicted the properties and atomic masses
of unknown elements to fit in the blank spaces.
The table shows Mendeleev’s predictions for the element
germanium. He called the element ekasilicon. His predictions
proved to be accurate. Scientists eventually found all of the
elements that were missing from Mendeleev’s periodic table.
The properties of these “missing” elements turned out to be
extremely close to what Mendeleev predicted.
How has the periodic table been improved?
Mendeleev’s periodic table was very good for its time.
However, scientists eventually found some problems with it.
The elements on Mendeleev’s table increased in atomic mass
from left to right. Look at the modern periodic table at the
back of this book. You will find examples, such as cobalt and
nickel, that decrease in mass from left to right. However, notice
that the atomic number always increases from left to right.
In 1913, the arrangement of the periodic table was changed.
Instead of being arranged by increasing atomic mass, it was
arranged by increasing atomic number. This change was due
to the work of an English scientist named Henry G. J. Moseley.
The new arrangement seemed to correct some of the problems
of the old table. The current periodic table uses Moseley’s
arrangement and is shown in the back of this book.
Mendeleev’s Predictions
Predicted Properties Actual Properties
of Ekasilicon (Es) of Germanium (Ge)
Existence Predicted—1871
Actual Discovery—1886
Atomic mass ⫽ 72 Atomic mass ⫽ 72.61
High melting point Melting point ⫽ 938°C
Density ⫽ 5.5 g/cm
3
Density ⫽ 5.323 g/cm
3
Dark gray metal Gray metal
Density of EsO
2
⫽ 4.7 g/cm
3
Density of GeO
2
⫽ 4.23 g/cm
3
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
2. Use Decimals Find the
difference between the
predicted density of
germanium and its
actual density.
Applying Math
3. Observe How did Moseley
arrange the periodic table?
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Energy
Floor (nucleus)
2 electrons
Step 1 = energy level 1
8 electrons
Step 2 = energy level 2
18 electronsStep 3 = energy level 3
Step 4 = energy level 4
32 electrons
Energy Levels
Reading Essentials 291
The Atom and the Periodic Table
Objects are often sorted or grouped according to the
properties they have in common. Elements on the periodic
table are grouped according to their chemical properties. The
vertical columns on the periodic table are called g
roups. The
groups are numbered 1 through 18. Sometimes they are called
families. Elements in each group have similar properties. For
example, in Group 11, copper, silver, and gold have similar
properties. Each is a shiny metal. Each is a good conductor of
electricity and heat. Why are the elements in a group similar?
Look at the structure of the atom to answer this question.
What is the structure of the electron cloud?
Where are the electrons located in an atom? How many are
there? In a neutral atom, the number of electrons is equal to the
number of protons. Carbon has an atomic number of six, which
means it has six protons and six electrons. These electrons are
located in the electron cloud that surrounds the nucleus.
Scientists have found that electrons in the electron cloud
have different amounts of energy. Look at the figure. It shows
a model of the energy differences that scientists use. Electrons
fill the energy levels from the inner levels to the outer levels.
The inner levels are closer to the nucleus and the outer levels
are farther from the nucleus. Inner levels have less energy
than the outer levels. Imagine that the nucleus is like a floor.
Each energy level is a step up a flight of stairs above the floor.
Each stair step represents an increase in energy. The figure
shows the maximum number of electrons that will fit in each
energy level of an atom. Not all atoms will have all levels
filled. This depends on the number of electrons in an atom of
that element.
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
4. Draw Conclusions Neon is
a gas. Do you think neon
is an element in Group 11?
Explain.
5. Apply The element
magnesium has 12
electrons. In how many
energy levels are the
electrons of magnesium?
Picture This
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Boron
5
B
Carbon
6
C
Nitrogen
7
N
Oxygen
8
O
Fluorine
9
F
Helium
2
He
Neon
10
Ne
Hydrogen
1
H
Lithium
3
Li
Beryllium
4
Be
Aluminum
13
Al
Silicon
14
Si
Phosphorus
15
P
Sulfur
16
S
Chlorine
17
Cl
Argon
18
Ar
Sodium
11
Na
Magnesium
12
Mg
292 CHAPTER 16 Properties of Atoms and the Periodic Table
How are electrons arranged in energy levels?
Elements that are in the same group have the same number of
electrons in their outer energy level. The number of electrons in
the outer energy level determines the chemical properties of the
element. It is important to understand the link between the
location on the periodic table, chemical properties, and the
structure of the atom.
These energy levels are named using numbers one to seven.
Electrons fill the energy levels starting with the inner level. For
example, the element sulfur has 14 electrons. Two electrons
will be in energy level 1 and eight electrons will be in energy
level 2. The rest of the electrons will be in energy level 3.
Look again at the diagram on the previous page. Notice
that energy levels 3 and 4 have increasingly large numbers
of electrons. However, a stable outer energy level has eight
electrons. How is this possible? In elements that have three
or more energy levels, more electrons can be added to
inner energy levels as long as the outer level contains
eight electrons.
How are rows on the periodic table arranged?
Remember that the atomic number found on the periodic
table is equal to the number of electrons in an atom. Look at
the partial periodic table below.
Top Row
The top row has hydrogen with one electron and
helium with two electrons. Both of these electrons are in
energy level 1. Energy level 1 is the outermost level in these
elements. So, hydrogen has one outer electron and helium has
two. Recall from the figure on the previous page that energy
level 1 can hold only two electrons. Therefore, helium has a
full outer energy level.
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
6. Identify What is
hydrogen’s outermost
energy level?
Picture This
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Reading Essentials 293
Second Row
The second row of the periodic table begins
with lithium. Lithium has three electrons, two in energy level 1,
and one in energy level 2. Next is beryllium with two outer
electrons and boron with three outer electrons. The pattern
continues until you reach neon. Neon has eight outer electrons.
Look at the figure on the previous page. Energy level 2 can hold
eight electrons. So, neon has a full outer energy level. Notice
how a row in the table ends when an outer energy level is filled.
The third row of elements, electrons begin filling energy level 3.
The row ends with argon, which has a stable outer energy level.
What are electron dot diagrams?
Elements in the same group have the same number of
electrons in their outer energy level. Outer electrons are used
to determine the chemical properties of an element.
American chemist G. N. Lewis invented the electron dot dia-
gram to show the outer electrons of an element. An e
lectron
dot diagram is the symbol of an element with dots represent-
ing the number of electrons in the outer energy level. The dia-
gram for the elements sodium (Na) and chlorine (Cl) is shown
below. These diagrams show how electrons in the outer energy
level bond when elements combine to form compounds.
How are elements in the same group similar?
Elements in Group 17 are called halogens. They all have
electron dot diagrams similar to chlorine, shown below. You
can see that chlorine has seven electrons in its outer energy
level. So do the other halogens. Since all elements in a group
have the same number of electrons in their outer levels, those
elements undergo chemical reactions in similar ways.
How do halogens form compounds?
All halogens can form compounds with elements in
Group 1. Group 1 elements, like sodium, all have one electron
in their outer energy level. The figure shows an example of a
compound formed by a reaction between sodium and
chlorine. Sodium combines with chlorine to give each
element a complete outer energy level. The result is the
compound sodium chloride (NaCl), ordinary table salt.
Not all elements form compounds with other elements.
Group 18 elements have completely filled outer energy levels.
This makes group 18 elements unreactive.
Sodium
Na
Chlorine
Cl
Sodium Chloride
Na
+
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
7. Use Numbers How many
electrons would fluorine
need to gain in order to
have a stable outer
energy level?
Applying Math
8. Apply What do all of the
elements in a group have
in common?
9. Draw Conclusions What
seems to happen to the
one electron in the outer
level of sodium when it
combines with chlorine to
form sodium chloride?
Picture This
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294 CHAPTER 16 Properties of Atoms and the Periodic Table
Regions on the Periodic Table
The periodic table has several regions with specific names.
The horizontal rows of elements are called p
eriods. Recall
that the elements increase by one proton and one electron as
you go from left to right across a period. Also, each period
represents a higher electron energy level.
All of the elements in the white squares in the diagram are
metals. Iron, zinc, and copper are some examples of metals.
Most metals are solids at room temperature. They usually are
shiny. They can be drawn into wires and pounded into sheets.
They are good conductors of heat and electricity.
The elements on the right side of the diagram in dark gray
are classified as nonmetals. Oxygen, bromine, and carbon are
nonmetals. Most nonmetals are gases. The elements in this
region that are solids are brittle. Nonmetals are also poor
conductors of heat and electricity at room temperature. The
elements in light gray are metalloids, or semimetals. They
have some properties of metals and some properties of
nonmetals. Boron and silicon are examples of metalloids.
Elements in the Universe
Scientists have found the same elements throughout the
universe. Many scientists hypothesize that hydrogen and
helium are the building blocks of other elements. Atoms join
within stars to form elements with atomic numbers greater
than those of hydrogen and helium. Exploding stars, called
supernovas, spread their mixture of elements throughout the
universe. Scientists have made new elements in laboratories.
These elements may have life spans less than a second.
Metals
Nonmetals
Regions on the Periodic Table
Metalloids
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
●
C
Compare and Contrast
Divide your paper into four
quarters to compare and
contrast metals, nonmetals,
and metalloids.
Metal:
Nonmetal:
Metalloid:
10. Draw Conclusions Silicon
conducts electricity under
some conditions but not
under other conditions. In
which region would you
place silicon?
11. Apply On which side of
the periodic table would
you look for an element
that definitely will not
conduct electricity?
Picture This
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Reading Essentials 295
1. Review the terms and their definitions in the Mini Glossary. Write a sentence using one of
the terms that shows that you understand the term.
2. Below is a blank periodic table of elements. On this table, label the different sections as
metals, metalloids, nonmetals, period, or group.
3. Explain what is important about the rows and columns on the periodic table.
a.
b.
c.
d.
e.
electron dot diagram: the symbol of an element with dots
representing the number of electrons in the outer energy
level
group: a vertical column of elements on the periodic table
period: a horizontal row of elements on the periodic table
periodic table: an arrangement of the elements by increasing
atomic number and by changes in physical and chemical
properties
After You Read
Mini Glossary
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
End of
Section
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Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
198 Properties of Atoms and the Periodic Table
Name Date
chemical property
periodic table
period
group
electron dot diagram
period
similar
Skim Section 3 and write three questions based on your brief
preview.
1.
2.
3.
Define chemical property to show its scientific meaning..
Use your book or a dictionary to define the following terms.
Use a dictionary to define similar to show its scientific meaning.
New
Vocabulary
Review
Vocabulary
Academic
Vocabulary
Properties of Atoms and the Periodic Table
Section 3 The Periodic Table
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Period:_________
Select
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
Properties of Atoms and the Periodic Table 199
Name Date
Compare Mendeleev’s early periodic table to that of today by
completing the Venn diagram.
Section 3 The Periodic Table (continued)
Organizing the
Elements
I found this information
on page .
The Atom and the
Periodic Table
I found this information
on page .
Both
Today (Moseley)
Mendeleev
Sequence the energy levels in the electron cloud diagram and
write the maximum number of electrons that can be contained in
each level.
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Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
200 Properties of Atoms and the Periodic Table
Name Date
Analyze how electron dot diagrams show similarities between
elements within a group.
Classify the regions of the periodic table as metals, nonmetals,or
metalloids.
• Shade the regions on the blank periodic table.
• Label each region and write its characteristics.
Section 3 The Periodic Table (continued)
I found this information
on page .
Regions of the
Periodic Table
I found this information
on page .
Write a paragraph showing the relationship between
chemistry and physics based on what you’ve learned from the periodic table.
S
YNTHESIZE IT
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Properties of Atoms and the Periodic Table 201
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
Name Date
Tie It Together
Properties of Atoms and the Periodic Table
Since organizing the elements into a periodic table worked so well for scientists, create
your own periodic table to organize another category of items. Pick a group containing
many items which exhibit repeating, predictable patterns of behavior. List characteristics
by which they are ordered and sorted, and organize them into columns and rows. Justify
your methods for organization. Some suggestions include fashion trends or fads, types of
music, beverages, or political and voting trends.
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202 Properties of Atoms and the Periodic Table
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
Name Date
Properties of Atoms and the
Periodic Table
Chapter Wrap-Up
Now that you have read the chapter, think about what you have
learned and complete the table below.
1. Write an A if you agree with the statement.
2. Write a D if you disagree with the statement.
Compare your previous answers to these.
Review
Use this checklist to help you study.
Review the information you included in your Foldable.
Study your Science Notebook on this chapter.
Study the definitions of vocabulary words.
Review daily homework assignments.
Re-read the chapter and review the charts, graphs, and illustrations.
Review the Self Check at the end of each section.
Look over the Chapter Review at the end of the chapter.
• An atom is the smallest unit of an element that
still has all the properties of the element.
• An atom is made up of a positively charged
nucleus and negatively charged electrons.
• Quarks are so tiny that they orbit the nucleus
with the electrons.
• Isotopes of an element only differ in their
number of neutrons.
• An element’s chemical and physical properties may
be predicted by its location on the periodic table.
Properties of Atoms and After You
the Periodic Table Read
After reading this chapter, list three things you have
learned about the properties of atoms and the periodic table.
SUMMARIZE IT
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Chapter 16 Section 3 Quiz The Periodic Table
1. The ______ is a chart created by Scientists to organize the elements
according to repeated changes of the properties.
A.
mass number
B.
periodic table
C.
isotope
D.
metalloid list
2. Which of the following best describes the three general groups of
elements?
A.
metals, nonmetals, and noble gases
B.
metals, metalloids, and synthetics
C.
solid, liquid, and gas
D.
metals, metalloids, and nonmetals
3. The name of every element can be abbreviated using a _______.
A.
chemical symbol
B.
mass number
C.
Roman numeral
D.
Greek letter
4. Which of the following is the correct chemical symbol for carbon?
A.
Ca
B.
Car
C.
Crbn
D.
C
Name: __________________
Period: ____________
Select
Select
Select
Select
Select
5. A(n) _______ is a method of representing atoms and the electrons in
their outer energy levels.
A.
electron dot diagram
B.
chemical symbol
C.
chemical formula
D.
chemical equation
This is the end of the test. When you have completed all the questions and
reviewed your answers, either: (Best option-->) upload in focus or (Second
Choice -->) email or Remind it. Otherwise hand in
a hard copy to the drop box at Leon High School.
Select
Chapter 16 Test
Properties of Atoms and the Periodic Table
1. Which of the following is the correct chemical symbol for carbon?
A.
Ca
B.
Crbn
C.
Car
D.
C
2. The discovery of the sixth quark was accomplished by _________.
A.
experimenting with a cathode ray tube
B.
using the Hubble Space telescope
C.
studying proton collisions
D.
bombarding gold foil with alpha particles.
3. Atoms consist of a positively charged center called a(n) _________.
A.
electron
B.
proton
C.
nucleus
D.
neutron
4. Scientists have broken down protons and neutrons into smaller particles
called _________.
A.
vacuoles
B.
quarks
C.
isotopes
D.
nuclei
Name: _________________
Period: _________
Select
Select
Select
Select
Select
5. Aristotle believed that matter was _________.
A.
uniform throughout
B.
capable of being broken does into smaller parts
C.
composed of atoms
D.
composed of molecules
6. Democritus believed that the universe was made of empty space and
_________.
A.
molecules
B.
elements
C.
atoms
D.
compounds
7. A(n) _________ is a method of representing atoms and the electrons in
their outer energy levels.
A.
electron dot diagram
B.
chemical formula
C.
chemical symbol
D.
chemical equation
8. The ______ is a chart created by Scientists to organize the elements
according to repeated changes of the properties.
A.
isotope
B.
periodic table
C.
metalloid list
D.
mass number
Select
Select
Select
Select
C. minutiae
D.
nanograms
10. Who formed the first periodic table?
A. Dalton
B.
Moseley
C.
Democritus
D.
Mendeleev
11. Which of the following best describes the three general groups of
elements?
A.
metals, metalloids, and synthetics
B.
solid, liquid, and gas
C.
metals, nonmetals, and noble gases
D.
metals, metalloids, and nonmetals
12. Which of the following atomic particles is positively charged?
A.
neutron
B.
electron
C.
negatron
D.
proton
13. Which of the following methods would be most useful for describing
atoms?
A.
touching with bare hands
B.
constructing a model
C.
visualizing with a microscope
D.
observing in a test tube
9. The mass of proton is measured in ________.
A. atomic mass units
B. microns
Select
Select
Select
Select
Select
many neutrons does an atom of manganese have in its nucleus?
A.
25
B.
30
C.
55
D.
60
15. The _________ of an atom is the number of neutrons plus protons.
A.
nucleus number
B.
half-life
C.
mass number
D.
atomic number
This is the end of the test. When you have completed all the questions and
reviewed your answers, press the button below to grade the test.
14. The atomic number of manganese is 25; its mass number is 55. How
Select
Select
