Download Building Atoms Unit Interactive Science Notebook III

Building Atoms Unit
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Interactive Science Notebook III
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Table of Contents
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Things 2 Know (UPDATED!)
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Atom Basics
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4
Sizes of Particles & Mini-Rutherford Activity
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5
Video Guide: Atoms & Elements
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6
LHC info
7-8
Chapter 11 section 1 worksheet
4
9
Atomic Theories & Models
2
10
Chapter 11 section 2 worksheet
2
Isotopes
2
13
Practice Atoms
2
14-15
Atom Factory 1
9
16
Atomic Math
2
17
Atom Factory 2
20
18
What are Ions?
19
Atomic Dimensions
2
20
Atom Factory 3
19
21
Elements 2 Know
22
Parts of Atoms
2
23
Quarks with EMAIL assignment
4
24
Four Forces in the Atom
11-12
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25-26
Chapter 11 Review
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27-28
Science Log
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29
Mind Map
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30-31
Outside Reading Article & Extended Response
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Parent Signature & Dated Night before Quiz
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Total 110
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Parent signature ___________________________________date_______________
Page
Updated Things 2 Know
1. SAFETY FIRST!! (lab walk, fragile things, P.A.S.S., etc)
2. You are required to have a pencil or erasable pen, ISN with
cover, calculator, ruler, and red or green pen everyday.
3. Any missed labs or in class work should be made up in my
room during lunch or tutorial with Mrs. Stout as soon as
possible after an absence.
4. on-line textbook address: my.hrw.com
(*no www.)
on-line textbook username: nbjh3
on-line textbook password: science
5. Stoutʼs email address: [email protected]
6. Stoutʼs web site: www1.northbrook28.net/~cstout
7. Matter is anything with mass and volume.
8. Matter is made of tiny particles that are always in some
motion.
9. Matter can exist in several states(or phases), the most
common are solid, liquid, gas and plasma.
10. Temperature is how fast the particles are vibrating and ...
11. Heat is how many particles there are and how fast they are
moving.
12. An element is the most basic type of matter that is still unique.
2
Atom Basics
Protons- positive (+) found in nucleus
Neutrons - neutral ( o,
n) found in nucleus
Electrons- negative (-)
found in energy clouds
(levels)
Atomic Number- is the number protons
Mass Number= the number of protons plus number of neutrons
Charge = number of protons minus number of electrons
Isotopes
Atoms with the same amount of protons, but different
numbers of neutrons. These are basically, slightly
different versions of the same element
Ions
Atoms or molecules with a positive or negative
charge due to more or less electrons.
3
Sizes of Particles
Mini- Rutherford Activity
Draw the shape that you deduce is hidden under the board. Use the marbles to “sense” the objects
Newton
Galileo
Curie
Hawking
Carson
Carver
4
Atom and Elements Video Guide
1.________________________ are the basic building blocks of all matter, living or
non-living.
2.Each atom is made up of ____________________ that spin around the nucleus
made up of _____________________ & _____________________.
3.Atoms are roughly the same ________________.
4.The _______________________ nuclear force holds the nucleus together.
5.The protons give the nucleus a ____________________________ charge.
6.The ___________________________ is very dense and contains most of the
mass of the atom.
7. The protons and neutrons are made up of even smaller particles called
_________________.
8._________________________ and ________________________ are
considered to be that smallest particles in the universe.
9.The _____________________________ force holds the electrons in their orbits.
10. ______________________________ is the most prevalent (common) element
in the universe.
11.Hydrogen has the atomic number 1 because it has ________ proton. Itʼs
symbol is ________.
12. _____________ electrons can fit in the first shell. ____________ electrons fit in
the 2nd and 3rd shell.
13.______________________ have the same atomic number but different atomic
mass and mass number.
14.If atoms lose or gain an electron they are called
_____________________________
WORD BANK:
electrons, protons, neutrons size, hydrogen, ions, isotopes, strong,
electromagnetic, atoms, positive, quarks, one, two, eight, H
5
PICTURE 1
The Large Hadron Collider (LHC) was built by the European Organization for
Nuclear Research (CERN) with the intention of testing various predictions of
high-energy physics, including the existence of new particles predicted by
supersymmetry. It lies in a tunnel 27 kilometers (17 mi) in circumference, as
much as 175 meters (570 ft) beneath the Franco-Swiss border near Geneva,
Switzerland. It is funded by and built in collaboration with over 10,000 scientists
and engineers from over 100 countries as well as hundreds of universities and
laboratories. Picture 1 shows the LHC from the air, Picture 2 is one place
where the particles actually collide. Pictures 3 and 4 are images of the
collisions
PICTURE 2
PICTURE 3
6
PICTURE 4
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Introduction to Atoms
DIRECTED READING WORKSHEET
evidence.
DIRECTED READING WORKSHEETS
4. How do you think rolling marbles in this activity will help you
identify the mystery object?
Investigate! (p. 279)
Answer these questions in your ScienceLog now. Then later, you’ll
have a chance to revise your answers based on what you’ve learned.
What Do You Think? (p. 279)
atoms only through
(direct or indirect)
3. Scientists are able to develop theories about dinosaurs and
a. by studying well-preserved dinosaur tracks
b. by examining similarities between the skeletons of T. rex and
an ostrich
c. by observing a T. rex as it was walking
d. by extracting DNA from fossilized mosquitoes
2. How did scientists find information that caused them to change
their theory about the way T. rex walked? (Circle all that apply.)
1. What do dinosaurs have in common with atoms?
Would You Believe . . . ? (p. 278)
As you read Chapter 11, which begins on page 278 of your textbook, answer the
following questions.
11
CHAPTER
81
Name _______________________________________________ Date ________________ Class______________
CHAPTER 11
▼
▼
▼
7
Atoms are small, soft particles.
Atoms are always standing still.
Atoms join together to form different materials.
None of the above
82
HOLT SCIENCE AND TECHNOLOGY
True or False? (Circle one.)
12. Atoms of different elements are exactly alike.
.
,
11. Dalton’s theory states that atoms cannot be
, or
they’re made of individual atoms. True or False? (Circle one.)
Dalton Creates an Atomic Theory Based on Experiments (p. 281)
10. By conducting experiments and making observations, Dalton
figured out that elements combine in random proportions because
9. We know that Democritus was right to say that all matter was
made up of atoms. So why did people ignore Democritus’s ideas
for such a long time?
a.
b.
c.
d.
8. Which of the following statements is part of Democritus’s theory
about atoms?
. (invisible or indivisible)
Democritus Proposes the Atom (p. 280)
7. The word atom comes from a Greek word that means
.
6. An explanation that is supported by testing and brings together
a broad range of hypotheses and observations is called a
a. a relatively new idea to us.
b. the building blocks of all matter.
c. the smallest particles into which an element can be divided
and still be the same substance.
d. seen with the scanning tunneling microscope.
5. Atoms are NOT
Section 1: Development of the Atomic Theory (p. 280)
Chapter 11, continued
Name _______________________________________________ Date ________________ Class _____
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Thomson discovered that there were small particles
inside the atom.
Thomson found that the electrically charged plates
affected the direction of a cathode-ray tube beam.
Thomson knew the beam was made of particles
with a positive charge because it was pulled toward
a positive charge.
15.
16.
17.
negatively charged.
present in every type of atom.
collected together in the center of the atom.
scattered throughout a blob of positively charged material.
.
DIRECTED READING WORKSHEETS
deflect to the sides of the gold foil. True or False? (Circle one.)
Rutherford Opens an Atomic “Shooting Gallery” (p. 284)
22. Before his experiment, Rutherford expected the particles to
Review (p. 283)
Now that you’ve finished the first part of Section 1, review what you
learned by answering the Review questions in your ScienceLog.
a.
b.
c.
d.
21. In Thomson’s “plum-pudding” model, electrons are NOT
20. Objects with the same charge attract each other. True or False?
(Circle one.)
True or False? (Circle one.)
19. The two types of charge are positive and neutral.
hair and the balloon have become
to the balloon because both the
18. When you rub a balloon on your hair, your hair is
In 1897, J. J. Thomson made a discovery that
proved the first part of Dalton’s atomic theory was
correct.
(p. 282)
14.
Thomson Finds Electrons in the Atom
Mark the following statements True or False.
13. How did Dalton think atoms formed new substances?
Chapter 11, continued
Date ________________ Class_______
23. Review Figure 6 and read the text on page 285. Figure 6 shows
the new atomic model resulting from Rutherford’s experiment.
Which of the following statements is NOT part of Rutherford’s
revision of his former teacher’s atomic theory?
Chapter 11, continued
Name _______________________________________________ Date ________________ Class______________
Name _______________________________________________
CHAPTER 11
Atoms are made mostly of empty space.
The nucleus is a dense, charged center of the atom.
Lightweight, negative electrons move in the nucleus.
Most of an atom’s mass is in the nucleus.
times smaller than the diameter of
in
travel
Review (p. 286)
Now that you’ve finished Section 1, review what you learned by
the Review questions in your ScienceLog.
answering
83
28. What are electron clouds?
True or False? (Circle one.)
The Modern Theory: Electron Clouds Surround the Nucleus (p. 286)
27. The exact path of a moving electron can now be predicted.
True or False? (Circle one.)
26. Bohr’s model only predicted some atomic behavior.
from level to level.
specific levels. Each level is a certain
from the nucleus. Electrons cannot be found between levels, but they can
in definite paths around the
25. In Bohr’s atomic model,
Bohr States That Electrons Can Jump Between Levels (p. 286)
the atom.
24. The diameter of the nucleus of an atom is
a.
b.
c.
d.
▼
▼
▼
8
Atomic Theories and Models
Models are often used in science to help visualize things that cannot be
seen otherwise. For example, because of the incredibly small size of an atom,
scientists must use models to try to understand how atoms actually look. John
Dalton's model of the atom shows it as a small spherical particle. This concept of
the atom has been changed several times over the years as new information is
discovered.
In the early 1900s, J. J. Thomson improved on Dalton's early atom model
with his Nobel prize-winning discovery that atoms have small subunits called
electrons. His work led to the "plum pudding" model of an atom. In this model the
atom has a thick filling of positive charge with electrons spread throughout.
A little over ten years later, Ernest Rutherford discovered that atoms have a
small dense nucleus of positive charge around which the negatively charged
electrons circulate. His was the "solar system" model of an atom. Two years later
the Danish physicist Niels Bohr (who had worked under Thomson at one time)
developed Rutherford's model even further. He proposed that electrons circle the
nucleus in definite energy levels. These electrons can gain or lose energy by
jumping or falling from different levels. Scientists called this the Bohr model of an
atom.
Finally, the present-day model for the atom, the electron cloud model, was
developed; Two main contributors were Werner Heisenberg and Erwin
Schrodinger. It states that electrons circle the nucleus in energy-level regions, or
clouds, rather than in well-defined orbits.
Below you will find drawings showing four models of what an atom looks like. Under each
drawing. Write the name of the scientist(s) that developed each theory
_______________ __________________ ________________ ___________________
1. What purpose do models serve in science? _________________________________
_________________________________________________________
2. How does Rutherford’s atom differ from Thomson’s? _________________________
__________________________________________________________________
3. How is the modern model different from Bohr’s ___________________________
9
Copyright © by Holt, Rinehart and Winston. All rights reserved.
that act on the particles
a. electron cloud
11. The simplest atom is the
has one proton and one electron.
How Do Atoms of Different Elements Differ?
c. amu
g. neutron
f. ion
e. proton
d. nucleus
atom. It
DIRECTED READING WORKSHEETS
(p. 289)
Column B
b. electron
Review (p. 289)
Now that you’ve finished the first part of Section 2, review what you
learned by answering the Review questions in your ScienceLog.
10. SI unit used for the masses of atomic particles
9. contains most of the mass of an atom
8. size of this determines the size of the atom
7. negatively charged particle found outside
the nucleus
6. particle with an unequal number of protons
and electrons
5. particle found in the nucleus that is positively charged
4. particle found in the nucleus that has no
charge
Column A
What’s Inside an Atom? (p. 288)
Choose the term in Column B that best matches the phrase in
Column A, and write the appropriate letter in the space provided.
billion atoms of copper and zinc.
3. An Olympic medal contains about twenty thousand billion
How Small Is an Atom? (p. 287)
Each of the following statements is false. Change the underlined
word to make the statement true. Write the new word in the space
provided.
2. A sheet of aluminum foil is about 500 atoms thick.
and the
inside the atom.
1. In this section you will learn about the particles inside the atom
Section 2: The Atom (p. 287)
Chapter 11, continued
85
Name _______________________________________________ Date ________________ Class______________
CHAPTER 11
▼
▼
▼
10
(p. 290)
Review (p. 293)
Now that you’ve finished Section 2, review what you learned by
answering the Review questions in your ScienceLog.
20. holds the electrons around the nucleus
19. plays a key role in neutrons changing into protons
and electrons in unstable atoms
18. depends on the mass of objects and the distance
between them
17. counteracts the electromagnetic force so protons
stay together in the nucleus
Column A
d. weak force
c. strong force
b. electromagnetic
force
a. gravity
Column B
mass.
What Forces Are at Work in Atoms? (p. 293)
Choose the type of force in Column B that best matches the phrase in
Column A, and write the corresponding letter in the space provided.
isotopes of an element is called
Calculating the Mass of an Element (p. 292)
16. The weighted average of the masses of all the naturally occurring
a. have the same number of protons but different numbers of
neutrons.
b. are stable when radioactive.
c. share most of the same chemical properties.
d. share most of the same physical properties.
Are All Atoms of an Element the Same?
15. It is NOT true that isotopes of an element
. (neutrons or protons)
14. An element is composed of atoms with the same number of
.
13. If you build an atom using two protons, two neutrons, and
two electrons, you have built an atom of
moving apart. True or False? (Circle one.)
12. Neutrons in the atom’s nucleus keep two or more protons from
Chapter 11, continued
Name _______________________________________________ Date ________________ Class ______________
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ISOTOPES
Atoms of the same element can have different numbers of
neutrons; the different possible versions of each element are
called isotopes. For example, the most common isotope of
hydrogen, protium, has no neutrons at all; there's also a
hydrogen isotope called deuterium , with one neutron, and
another, tritium , with two neutrons.
Protium Deuterium
Tritium
Question: How many isotopes can one element have? Can an atom
have just any number of neutrons?
The number of isotopes varies from atom to atom. There are
"preferred" combinations of neutrons and protons, at which the
forces holding nuclei together seem to balance best. Light
elements tend to have about as many neutrons as protons;
heavy elements apparently need more neutrons than protons in
order to stick together. Atoms with a few too many neutrons, or
not quite enough, can sometimes exist for a while, but they're
unstable
Question: I'm not sure what you mean by "unstable." Do atoms just fall
apart if they don't have the right number of neutrons?
Well, yes, in a way. Unstable atoms are radioactive : their nuclei
change or decay by spitting out radiation , in the form of
particles or electromagnetic waves.
11
ISOTOPES
The table below lists isotopes of hydrogen, carbon, and oxygen. Refer to the table to
answer the questions that follow,
Element/
% in Nature Atomic Mass
Atomic
Mass
isotope
(amu)
Number
Number
Hydrogen-1
99.998500
1.007825
1
1
Hydrogen-2
0.001500
2.001410
1
2
Hydrogen-3
trace
?
1
3
Carbon-12
98.890000
12
6
12
Carbon-13
1.110000
13.003000
6
13
Carbon-14
trace
?
6
14
Oxygen-16
99.759000
15.995000
8
16
Oxygen-17
0.037000
16.999000
8
17
Oxygen-18
0.204000
17.999000
8
18
1. According to the table, how many isotopes does hydrogen have? ______
2. How many isotopes does oxygen have? _________
3. Which isotopes of the three elements are the most abundant in nature?
4. For which isotopes have scientists not been able to determine the atomic mass? Can
you think of a reason for this?
5. According to the table, how are isotopes named?
6. What is the atomic number for all the isotopes of carbon? __________
7.What is the atomic number for all the isotopes of oxygen? __________
8. What is the atomic number for all the isotopes of hydrogen?_____________
9. One of these isotopes has been used by scientists as a standard for the atomic mass unit
(amu)Can you guess which one? Why?
10. Suppose you tested a sample of oxygen to determine its atomic mass, If the mass came
out to be 16.112 amu would you conclude that the sample consisted of only one isotope?
Why or why not?
12
13
Atom Factory Instructions
READ ME
Work by yourself to complete the Atom Factory #1 Lab
on the computers. Donʼt ask questions until youʼve tried
REAL hard... hint the number of protons = electrons, for now
1. Log in as student (if needed),
2. Connect to your server
3. Go to the LINKS page on my website (see ISN 2 for address)
4. Click on Atom Factory 1 to download the worksheet
5. SAVE AS... the file to Your Server folder
6. Put your name in the header
7. Read all instructions on the computer copy.
8. Complete both pages on the Computer
9. Save and print to SIR ISAAC
10.LOG OFF your server.
11.Cut out and put in ISN over this page and on the next
page. YES COVER THIS PAGE WITH PAGE 1
12.Return to seats and work on HW
13.Followed-all-instructions Bonus:________________
14
page 2 of Atom Factory 1 here
15
Atomic Math
Calculate the answers , EACH ANSWER LEADS TO THE NEXT.
1. Multiply the atomic number of hydrogen by the number of electrons in
mercury, which has an atomic number of 80.
answer:___________
2. Divide this number by the number of neutrons in helium, atomic
number 2, mass number 4.
answer:___________
3. Add the number of protons in potassium, atomic number 19.
answer:___________
4. Add the mass number of the most common isotope of carbon.
(see Isotopes on ISN 12)
answer:___________
5. Subtract the number of neutrons in sulfur, with atomic number 16,
mass number 32.
answer:___________
6. Divide by the number of electrons in boron, atomic number 5, mass
number 11.
answer:___________
7. This number is the atomic number of which of these elements ?
fluorine: atomic number 9
neon: atomic number 10
sodium: atomic number 11
final answer:_______________
16
Atom Factory 2
Attach Here
17
What are ions?
ion (EYE-uhn, EYE-on)
An atom (or group of atoms)that has either lost or gained one or more electrons,
so that it has an electrical charge. Ions can be either positively or negatively
charged.
A neutral atom or group of atoms becomes an ion by gaining or losing one or
more electrons. Since the electron and proton have equal but opposite
charges(negative 1 and positive 1), the charge of an ion is always expressed as a
whole number of charge and is either positive or negative. If an atom or group of
atoms loses electrons it will have a net positive charge and is called a cation. If
an atom or group gains electrons or loses protons, it will have a net negative
charge and is called an anion.
Let’s take a Lithium (Li) atom. It has an atomic number of 3. That means it has 3
protons. Each proton in positively charged. For Lithium to have no net or overall
charge it must have a balanced number of negatively charged electrons, thus it
needs 3 electrons to be electrically neutral, demonstrated here.
18
Atomic Dimensions
The table below contains information about several elements. Use this table to
review the concepts of atomic number, mass number, subatomic particles,
isotopes, ions, neutrality and atoms. In each case, use the information has
provided for you and a periodic table to fill in all the blanks.
Element
Name
1
Aluminum
2
Bromine
35
3
Uranium
92
4
Helium
2
4
5
Helium
2
5
2
6
Lithium
3
7
2
7
Tungsten
8
Xenon
9
Magnesium
12
10
Carbon
6
11
Carbon
12
Nitrogen
7
14
neutral
13
Potassium
19
40
-2
14
Gold
197
-3
15
Sodium
22
neutral
Symbol
Atomic
Number
Mass
Number
Number
Number of Number of
of
neutrons Electrons
Protons
#
27
13
80
Charge
13
45
36
146
92
-1
184
110
74
79
54
24
neutral
+2
14
6
19
6
neutral
8
+3
Atom Factory 3
Attach here
20
ELEMENTS-2KNOW
Ne
neon Sr strontium
Place these elements’ names
on one side, and the symbols
on the other side of your flash
cards. You must know the
spelling and symbols
Na
sodium Ag
silver
Mg
magnesium
Mn
manganese
Sn tin
Fe iron
Al aluminum H hydrogen
I iodine
He
helium Si silicon
Li lithium P phosphorus
Co
cobalt
S
sulfur
Be
beryllium Cl chlorine Ni nickel
Ar
argon
B boron
K potassium
Cu
copper
Ca
calcium C carbon Cr chromium Zn
zinc
Ba
barium N nitrogen W tungsten
Pb
lead
Pt platinum
O oxygen Au
gold Bi bismuth
Hg
mercury
F fluorine U
uranium
Br bromine
21
What are the parts of an atom?
Complete the following.
1. The first scientist to suggest that atoms contain smaller particles was_____________.
2. Positively charged particles are called____________________.
3. Bohr proposed that electrons in an atom are found in _________________________.
4. Negatively charged particles are called_______________
5. Rutherford found that an atom is made up mostly of________________________
6. The center, or core, of an atom is called the ______________________
7. Surrounding the core of an atom is a cloud of very small particles called ______________
8. Today, energy levels are used to predict the location of ___________________.
9. Neutral particles are called ____________________
10. Rutherford found that___________________are located in the core of an atom.
Write "Yes" or "No" in the correct columns to identify whether each statement is true for
protons, neutrons, and electrons.
Proton
1. Found in the nucleus
2. Positively charged
3. Moves in energy levels
4. Negatively charged
5. Does not have an electric
charge
22
Neutron
Electron
QUARKS & Other Weird Particles
As you have read, many scientists have contributed to our knowledge of atoms
and particles even smaller than atoms. From the early ideas of Democritus to the
modern Cloud model of atoms, we have made quite a journey! This has been the
journey to answer a “simple” question...What is the fundamental particle?
In other words, what is the most basic particle of matter? The smallest thing? The
thing that can’t be broken down any further? Some of the most important
milestones are reviewed here:
In 1911 Rutherford used alpha particle radiation to test a thin sheet of gold foil.
He found that most of the particles passed easily through the foil but there were
times when some particles bounced back. He reasoned that this showed that most
of the atom was composed of empty space but that occasionally an alpha particle
collided with the small hard center of the atom. This proved that the atom was not
the answer to the “simple” question.
So...we discovered protons, neutrons and electrons. Great, but scientists weren’t
finished yet! In the 1930s, 40s, and 50s nuclear physicists studied the forces that
held atoms together and radioactive decay. The field of Particle physics developed
as an outgrowth of this investigation. These scientists were interested in the
make-up of nuclear particles, like protons & neutrons. However, to study these
particles great energy had to be generated, and so, during the 1950s through the
1970s, giant accelerators were built, like the one at Fermi Lab in Batavia, Illinois,
just 50 miles southwest from Northbrook! Particles were accelerated at
tremendous speed and then shot at a target or directed into the path of another
particle traveling in the opposite direction. As a result of these collisions,
hundreds, yes hundreds, of new particles were discovered that were smaller that
protons & neutrons. Therefore, they are not the fundamental particles either.
Here are some of the weird names of these particles: hadrons, leptons, quarks,
neutrinos, muons, positrons, photons, gluons, and Higgs bosons. Currently we
know of 36 types of quarks and 12 types of leptons(including electrons). These
particles, quarks & leptons are all about the same size and so far we have not
been able to break these particles apart.
Particle physicists are striving to find a link between the particles and the four
forces. This is called the Unification Theory, even Einstein couldn’t figure this one
out! The four forces are gravity, electromagnetic, weak, and strong. Gravity is the
attraction of all matter to all other matter. The electromagnetic force is the
attraction or repulsion of charged(positive or negative) matter. The weak force is
responsible for radioactive decay of a nucleus. The strong force is the force that
hold quarks and the nucleus of atoms together.
The answer to the simple question is closer than ever before, but also much more
complex. Scientists are hard at work all over the world trying to find the final
answer! Maybe you will help to lead the world to the final answer...
Question: Do you think we will find the answer to this question? Explain
Email Mrs. Stout the answer with subject “particle” followed by your class
period,
particle5 for example. Always put a header in your emails to Mrs. Stout.
23
24
Name _______________________________________________ Date ________________ Class ______________
CHAPTER
11
Chapter 11 Review
INTRODUCTION TO ATOMS
Chapter 11 Test
USING VOCABULARY
To complete the following sentences, choose the correct term from each pair of terms
listed, and write the term in the blank.
1. A beehive with bees buzzing around it could be used as a rough
CHAPTER TESTS
of the atom. (model or theory)
2. A positively charged particle with a mass of 1 amu is called a
. (neutron or proton)
3. Different
neutrons. (electrons or isotopes)
of an element have different numbers of
4. The region in an atom that contains most of the mass is called the
▼
▼
▼
. (nucleus or electron cloud)
5. The number of protons in an atom determines its
(atomic number or mass number)
.
6. The weighted average of all the naturally occurring isotopes of an element is called the
. (mass number or atomic mass)
Copyright © by Holt, Rinehart and Winston. All rights reserved.
UNDERSTANDING CONCEPTS
Multiple Choice
Circle the correct answer.
7. What did Democritus, Dalton, Thomson, Rutherford, and Bohr all have in common?
a. They
b. They
c. They
d. They
each
each
each
each
identified new elements.
identified new isotopes of atoms.
contributed to the development of the atomic theory.
conducted experiments in which particles collided.
8. In Thomson’s “plum-pudding” model of the atom, the plums represent
a. atoms.
b. protons.
c. neutrons.
d. electrons.
9. An atom of gold with 79 protons, 79 electrons, and 118 neutrons would have a mass
number of
a. 39.
b. 158.
c. 197.
d. 276.
10. Which of the following has the least mass?
a. nucleus
b. proton
c. neutron
d. electron
11.The isotope of uranium used in nuclear reactors, uranium-235, contains 92 protons.
Another isotope, uranium-238, contains _?_ electrons.
CHAPTER TESTS WITH PERFORMANCE-BASED
a.92 c.143
b.95 d.146
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ASSESSMENT
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Chapter 11 Review Continued
12.Draw a picture of a -2 Be-9
13.What is an isotope?
14.How many different isotopes can an element have?
Give the Element Symbol:
15.Hydrogen ___________
16.Oxygen
___________
17.Lead
___________
Give the Element Name:
18. W _____________________
19. Au _____________________
20. Mg _____________________
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Science Log Write in Complete sentences and record the page number of each entry
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Science Log Write in Complete sentences and record the page number of each entry
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Mind Map
Use Word Processing and the following terms to create a mind map aka concept map:
electrons, protons, neutrons, atom, clouds, nucleus, positive, negative, neutral
Attach Map here
15 cm wide x 17 cm tall
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Outside Reading Article
Find a current article (2004-present)that relates to our
current ISN.To find articles you can use these two great
research resources:
1. Go to the NBJH homepage then Click on Library
Resource Center and then use the DATABASES
for Magazine/Internet/Newspaper
---or--2. Use “Sato’s Science Search Engine” linked on Mr.
Sato’s site
3. Tape or staple Outside Reading Article over this page
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Extended Response
attach
EXTENDED RESPONSE
here
Response should be one/two paragraphs that includes:
•KEY IDEAS from the article.
•CONNECTIONS from the article to
1. The current science chapter
2. Something from this unit we did in class or lab
3.Your own life
•EXTENSION OF IDEAS
•GOOD BALANCE of References and Connections
•Conclusion
•Printed work is preferred.
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