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Instructor’s Guide
Physics in Action
THE NATURE OF MATTER
Introduction
This Instructor’s Guide provides information to help you get the most out of The Nature of Matter,
part of the five-part series Physics in Action. The contents of the guide will allow you to prepare your
students before using the program and to present follow-up activities to reinforce the program’s key
learning points.
Can the study of physics be fun? This clever five-part series answers “Yes!” by presenting essential
facts, formulas, and laws of physics through real-world examples, illustrative animations, and a likeable field guide named Mr. Physics who makes complicated concepts easier to understand. End-ofsection reviews are included throughout each program, and equations are worked out, step by step,
on-screen.
The series includes the following titles:
• Energy
• Forces and Motion
• Planets, Stars, and Galaxies
• Processes That Shape the Earth
• The Nature of Matter
Learning Objectives
After viewing the program, students will be able to:
• Understand the difference between atoms, protons, neutrons, electrons, quarks, elements, molecules,
and compounds
• Define the fundamental forces of gravity, electromagnetism, the weak nuclear force, and the
strong nuclear force
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• Understand that scientists form a hypothesis and then conduct experiments to come up with
a theory or model; and that models can be refined over time
• Define the following terms: atomic number, neutron number, atomic mass number, isotope, ion,
fission, and fusion
• Understand the arrangement of the periodic table of elements
• Understand the four quantum numbers and the exclusion principle
• Understand ionic, covalent, and hydrogen bonds
• Understand alpha, beta, and gamma radioactivity
• Understand the basics of elementary particles
Educational Standards
BENCHMARKS FOR SCIENCE LITERACY STANDARDS
This program correlates with the following standards from Benchmarks for Science Literacy, by the
American Association for the Advancement of Science, for grades 9 through 12.
The Nature of Science: The Scientific Worldview
• From time to time, major shifts occur in the scientific view of how things work. More often,
however, the changes that take place in the body of scientific knowledge are small modifications
of prior knowledge. Continuity and change are persistent features of science.
• In science, the testing, revising, and occasional discarding of theories, new and old, never ends.
This ongoing process leads to a better understanding of how things work in the world but not to
absolute truth.
The Nature of Science: Scientific Inquiry
• Hypotheses are widely used in science for choosing what data to pay attention to and what additional data to seek, and for guiding the interpretation of the data (both new and previously available).
The Nature of Science: The Scientific Enterprise
• The early Egyptian, Greek, Chinese, Hindu, and Arabic cultures are responsible for many scientific
and mathematical ideas and technological inventions. Modern science is based on traditions of
thought that came together in Europe about 500 years ago. People from all cultures now contribute
to that tradition.
The Physical Setting: The Structure of Matter
• Atoms are made of a positively charged nucleus surrounded by negatively charged electrons.
The nucleus is a tiny fraction of the volume of an atom but makes up almost all of its mass. The
nucleus is composed of protons and neutrons which have roughly the same mass but differ in that
protons are positively charged while neutrons have no electric charge.
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• The number of protons in the nucleus determines what an atom’s electron configuration can be
and so defines the element. An atom’s electron configuration, particularly the outermost electrons,
determines how the atom can interact with other atoms. Atoms form bonds to other atoms by
transferring or sharing electrons.
• Although neutrons have little effect on how an atom interacts with other atoms, the number of
neutrons does affect the mass and stability of the nucleus. Isotopes of the same element have the
same number of protons (and therefore of electrons) but differ in the number of neutrons.
• The nucleus of radioactive isotopes is unstable and spontaneously decays, emitting particles
and/or wavelike radiation. It cannot be predicted exactly when, if ever, an unstable nucleus will
decay, but a large group of identical nuclei decay at a predictable rate. This predictability of decay
rate allows radioactivity to be used for estimating the age of materials that contain radioactive
substances.
• Scientists continue to investigate atoms and have discovered even smaller constituents of which
neutrons and protons are made.
• When elements are listed in order by the masses of their atoms, the same sequence of properties
appears over and over again in the list.
• Atoms often join with one another in various combinations in distinct molecules or in repeating
three-dimensional crystal patterns.
• The configuration of atoms in a molecule determines the molecule’s properties. Shapes are
particularly important in how large molecules interact with others.
• Some atoms and molecules are highly effective in encouraging the interaction of others.
• The physical properties of compounds reflect the nature of the interactions among their molecules.
These interactions are determined by the structure of the molecule, including the constituent atoms
and the distances and angles between them.
The Physical Setting: Energy Transformations
• Energy is released whenever the nuclei of very heavy atoms, such as uranium or plutonium,
split into middleweight ones, or when very light nuclei, such as those of hydrogen and helium,
combine into heavier ones. For a given quantity of a substance, the energy released in a nuclear
reaction is very much greater than the energy given off in a chemical reaction.
SOURCE: Benchmarks For Science Literacy, by The American Association for the Advancement of Science. Copyright 1993,
2009 by The American Association for the Advancement of Science. Used by permission of Oxford University Press, Inc.
ENGLISH LANGUAGE ARTS STANDARDS
The activities in this instructor’s guide were created in compliance with the following standards from
National Standards for the English Language Arts, from the National Council of Teachers of English.
• Students adjust their use of spoken, written, and visual language (e.g., conventions, style, vocabulary) to
communicate effectively with a variety of audiences and for different purposes.
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• Students employ a wide range of strategies as they write and use different writing process elements
appropriately to communicate with different audiences for a variety of purposes.
• Students conduct research on issues and interests by generating ideas and questions, and by posing problems. They gather, evaluate, and synthesize data from a variety of sources (e.g., print and
non-print texts, artifacts, people) to communicate their discoveries in ways that suit their purpose
and audience.
• Students use a variety of technological and information resources (e.g., libraries, databases,
computer networks, video) to gather and synthesize information and to create and communicate
knowledge.
• Students use spoken, written, and visual language to accomplish their own purposes (e.g., for
learning, enjoyment, persuasion, and the exchange of information).
SOURCE: Standards for the English Language Arts, by the International Reading Association and the National Council
of Teachers of English. Copyright 1996 by the International Reading Association and the National Council of Teachers of
English. Reprinted with permission.
TECHNOLOGY STANDARDS
The activities in this instructor’s guide were created in compliance with the following standards
from The ISTE National Education Technology Standards (NETS•S) and Performance Indicators
for Students.
• Creativity and Innovation: Students demonstrate creative thinking, construct knowledge, and
develop innovative products and processes using technology.
• Research and Information Fluency: Students apply digital tools to gather, evaluate, and use
information.
• Critical Thinking, Problem Solving, and Decision Making: Students use critical thinking skills
to plan and conduct research, manage projects, solve problems, and make informed decisions using
appropriate digital tools and resources.
SOURCE: © 2007 The International Society for Technology Education. Reprinted with permission.
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Program Overview
An elephant and a racing car don’t have much in common—except for the remarkable fact that
they’re made of similar fundamental building blocks. This program takes a simulated subatomic
look at a glass of water to better understand the nature of matter, a minuscule world of molecules,
atoms, and elementary particles. The behavior of matter under the effects of gravity, electromagnetism, and the strong and weak nuclear forces; the process of scientific experimentation; specifics of
atomic structure; the organization of matter via the periodic table; ionic, covalent, and hydrogen
bonding; the process of radioactive decay; and the death of fusion-fueled stars are scrutinized as well.
Main Topics
Chapter 1: Inner Space
The program begins with an outline of the basic building blocks of nature — molecules, atoms,
protons, neutrons, electrons, and quarks — and the fundamental forces of gravity, electromagnetism,
the weak nuclear force, and the strong nuclear force.
Chapter 2: The Rise of the Atom
After a brief review of elements, compounds, chemical reactions, and the scientific method, viewers
get a history of the concept of the atom, beginning with ancient Indian and Greek ideas, continuing
through the Bohr model, and ending with today’s quantum model.
Chapter 3: Organizing Atoms
Elements, the atomic number, the neutron number, the atomic mass number, isotopes, and ions are
reviewed in this section.
Chapter 4: The Periodic Table of Elements
This section explains why the periodic table is set up as it is, and how it helps scientists both organize elements, and predict how elements will react when combined with each other. Viewers learn
about quantum numbers, energy shells and subshells, and the exclusion principle.
Chapter 5: Chemical Bonds
Ionic, covalent, and hydrogen bonds are the focus here. The role of valence shells, polarization, and
electronegativity is highlighted.
Chapter 6: Reactivity
This section details the dynamics of alpha, beta, and gamma radioactivity. Also included is a discussion
of half-life and carbon-14 dating.
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Chapter 7: Nuclear Energy
Along with an explanation of the difference between fission and fusion, viewers learn how the sun,
bombs, and nuclear power plants generate so much energy.
Chapter 8: Elementary Particle Physics
The final section introduces elementary particles such as quarks, leptons, and bosons, and the role
that strong and weak nuclear forces play in their study. The program ends by challenging students to
contemplate ‘theories in progress,’ such as anti-matter, and researchers’ hopes for the Large Hadron
Collider.
Fast Facts
• Studying motion, whether it’s the expansion of the cosmos or the movement of molecules vibrating
within a frozen glacier, is at the heart of physics.
• The Indian sage Kanada conceived of the concept of atoms in the 6th century bce, followed by
the Greek philosopher Democritus about a century later.
• The 2007 Nobel Prize in Physics was awarded to Albert Fert and Peter Grünberg for their work
in spintronics (spintronics uses electron ‘spin’ to store information in technological devices).
Their research made handheld music players such as the iPod possible.
• ‘Killer electrons,’ found in the radiation belt surrounding Earth, can damage spacecraft as well
as orbiting satellites — which means problems for cell phones, GPS, and other communications
technology. But NASA scientists now believe that ‘singing’ electrons, originating in plasma blown
from the surface of the sun, can destroy the ‘killer’ electrons. These particles were dubbed ‘singing’
because they generate waves that, when played through a converter, sound like birds singing.
• According to Einstein’s General Theory of Relativity, gravity is a distortion of the space-time
continuum. The theory posits that matter causes space to curve in the same way that a bowling
ball would cause a curve, or distortion, in a stretched sheet of fabric. The distortion causes the
acceleration known as gravitation.
• In June of 2009, the periodic table gained a new element. Copernicium (Cp) was created in a
laboratory by fusing the nuclei of zinc and lead. Creating new elements helps researchers understand more about how nuclear energy works.
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• All living things contain the radioactive isotope carbon-14 — and even human beings undergo
radioactive decay!
• Over 99.9% of an atom’s mass is concentrated in its nucleus.
• Over 50 trillion neutrinos, created by nuclear reactions in the sun, pass harmlessly through our
bodies every second.
• Quarks come in six different ‘flavors’: up, down, top, bottom, charm, and strange. The half-life
of the charm quark was found to be a thousand times longer than researchers had predicted
— and so they named it after its ‘charmed’ life.
Vocabulary Terms
alkali metals: Represented in the left-most column on the period table, metallic elements which
are highly reactive because they have only one valence electron. Sodium is an alkali metal.
alkaline earth metals: Represented in the second column on the periodic table, elements which
contain two valence electrons and are therefore slightly less reactive than alkali metals. Magnesium,
calcium, and radium are alkaline earth metals.
alpha decay: The radioactive decay of an atom’s nucleus by emission of an alpha particle (two protons
bound to two neutrons). When an element undergoes alpha decay, its atomic number decreases, thus
changing the original element into a different element.
alpha particle: A positively charged particle consisting of two protons and two neutrons, emitted
in radioactive decay or nuclear fission.
atom: A basic unit of matter consisting of a nucleus — which contains protons and neutrons
— surrounded by a cloud of electrons. Atoms, except for ions, have an equal number of protons and
electrons. There are nearly 100 different kinds of atoms in nature.
atomic mass number: The total number of protons and neutrons in an atom’s nucleus.
atomic number: The number of protons in an atom’s nucleus, designated by the letter Z.
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beta decay: A radioactive process in which a beta particle is emitted from the nucleus of an atom,
raising the atomic number of the atom by one if the particle is negatively charged, lowering it by
one if positively charged.
boson: A type of elementary particle known as a force particle.
chemical bond: The attraction between (or joining of ) two or more atoms in a molecule. Ionic
bonds, covalent bonds, and hydrogen bonds are all types of chemical bonds.
chemical formula: A representation of a substance that can tell us how many atoms are in a compound. For example, glucose has six carbon atoms, twelve hydrogen atoms, and six oxygen atoms;
its chemical formula is C6H12O6.
chemical reaction: A process in which the elements of a substance separate and then combine to
form a new substance. Heat is either absorbed or given off during a chemical reaction.
compound: A substance consisting of similar types of molecules, and made up of two or more elements.
covalent bond: A bond in which pairs of electrons are shared between atoms, or between atoms
and other covalent bonds.
electromagnetism: One of the four fundamental forces in nature, it is the phenomenon associated
with electric and magnetic fields. Electromagnetism causes the attraction and repulsion between
electrical charges inside an atom, which ultimately impacts the forces between molecules.
electron: A negatively charged elementary particle that can act as a particle or as a wave. Electrons
orbit the nucleus of an atom in energy shells; the quantum model describes the electron’s orbit as
being more like a cloud than an orbiting planet.
electronegativity: An atom’s ability to pull in electrons. An atom’s electronegativity determines
whether its electrons will be shared or exchanged in a chemical bond.
element: A substance composed of atoms that have the same atomic number (i.e., the same number
of protons). An element cannot be broken down by chemical reactions. Elements can be made up of
atoms, molecules, or ions.
elementary particles: Subatomic particles that apparently cannot be divided into smaller parts.
Quarks, leptons (electrons, muons, and tau particles, and their respective neutrinos), the Higgs
particle, and positrons are elementary particles.
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energy level: Also called an electron shell, it may be thought of in simple terms as the ‘orbit’ of an
electron around an atom’s nucleus.
exclusion principle: A principle which states that in a single atom no two electrons can have the
same four quantum numbers.
fission: The splitting of a large, unstable nucleus into smaller nuclei. Nuclear power plants generate
energy using fission reactions.
fusion: The joining, or fusing, of two nuclei together. Fusion generates an enormous amount of
energy. The sun produces energy through fusion.
gamma decay: A type of radioactive decay in which an atom’s nucleus loses energy by emitting
a stream of photons (particles of visible light). Gamma decay does not change an atom’s mass or
atomic number.
gamma ray: A type of radiation emitted as a result of radioactive decay.
gravity: One of the four fundamental forces in nature, it is the force of attraction by which objects
tend to pull towards each other.
Higgs particle: The Higgs particle is as yet a hypothetical particle invoked to explain why the carriers of the electroweak force (the W and Z bosons) have mass.
hydrogen bond: A weak bond that results from polarization in a molecule near hydrogen atoms.
ion: An atom or group of atoms where the total number of electrons is not equal to the total number
of protons, giving it a net positive or negative electrical charge.
ionic bond: A bond between two atoms in which only one of the atoms gives up an electron,
thereby generating an electrical force that holds the atoms together. A chemical bond between two
ions with opposite charges, characteristic of salts.
isotope: Atoms with the same number of protons but a different number of neutrons. Carbon-14
is an isotope.
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lepton: Any one of six elementary particles that are one of the fundamental constituents of matter.
Leptons are not affected by the strong force and are not normally found in the nucleus of the atom.
Electrons, neutrinos, muons, and taus are all leptons.
molecule: A group of at least two atoms held together by chemical bonds. Molecules are the smallest
unit of a compound that still remains a compound.
neutrino: An electrically neutral particle that is created through radioactive decay, or through
nuclear reactions in the sun or in nuclear reactors. Neutrinos are one of the most common particles
in the universe.
neutron: A subatomic particle found inside the nucleus of an atom (except for hydrogen).
Neutrons carry no electric charge, and are made up of groups of up and down quarks.
neutron number: The number of neutrons in an atom’s nucleus, designated by the letter N.
noble gases: Represented in the last column on the periodic table, gaseous elements that are chemically inert (i.e., not reactive) because their valence shells are full, making them very stable. Helium,
neon, and radon are noble gases.
nucleus: The dense center of an atom, it contains positively charged protons and neutral neutrons.
orbital: An electron’s location within the electron cloud.
polarization: A separation of positive and negative charges. Polarization occurs when charges are
not distributed equally in a compound, such as in a weak hydrogen bond.
positron: An elementary particle having the same mass and spin as an electron but having a positive
charge equal in magnitude to that of the electron’s negative charge.
positron emission decay: A process in which a proton is converted into a neutron, and a positron
and a neutrino are emitted from the atom’s nucleus. Also called beta plus decay.
proton: Positively charged particle found inside the nucleus of an atom. Protons are formed of
groups of up and down quarks.
quantum mechanics: The branch of physics that deals with the motion of particles by their wave
properties at the atomic and subatomic levels.
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quantum numbers: Numbers used to describe energy levels, angular momentum, and spin in an
atom. The principal quantum number (“n”) indicates how far from the nucleus an electron is and
how high its energy is. The angular momentum quantum number (“l”) represents angular momentum. The magnetic quantum number (“ml”) represents the projection of angular momentum along
an axis. Together, n, l, and ml specify an electron’s location in the electron cloud. The spin quantum
number (“ms”) represents the spin of the electron.
quark: An elementary particle which is only found inside of other particles. There are six ‘flavors’
of quark: up, down, top, bottom, strange, and charm. Protons and neutrons are formed of up and
down quarks.
radioactive decay: A process in which a nucleus undergoes spontaneous transformation into one
or more different nuclei and simultaneously emits radiation, loses electrons, or undergoes fission.
Elements with high atomic numbers are more likely to decay because their nuclei are unstable (too
many or too few neutrons can cause an element to decay). Alpha, beta, and gamma are the three
main kinds of radioactive decay.
radioactivity: The spontaneous emission of energetic particles (such as electrons) by some elements or
isotopes due to the disintegration of the nucleus. Uranium and carbon-14 are radioactive.
spin: Term used to describe the intrinsic angular momentum of electrons, although the electrons
do not actually spin.
Standard Model of particle physics: A theory of three of the four fundamental forces and the
elementary particles that take part in these interactions.
strong nuclear force: One of the four fundamental forces in nature, it is the glue that holds protons
and neutrons together inside the atom’s nucleus.
valence electrons: Electrons in an atom’s outermost orbital which govern how atoms combine with
each other to form compounds.
valence shell: The highest (i.e., outermost) energy level of an atom. The valence shell determines
how an atom will bond with other atoms, hence it determines the atom’s chemical properties.
weak nuclear force: One of the four fundamental forces in nature, it is associated with the decay of
neutrons, and results in radioactivity.
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Pre-Program Discussion Questions
1.
2.
3.
4.
What is an atom? What’s the different between an atom and a molecule? A proton and a neutron?
What is an element?
How do you think scientists decided where on the periodic table to place each element?
What do you know about radiation and radioactivity? Are there different types of radiation?
Is radiation found in nature?
5. Do scientists know all there is to know about subatomic particles?
Post-Program Discussion Questions
1.
2.
3.
4.
5.
What is the difference between an atom and an element?
What are the four fundamental forces?
What are quantum numbers?
What is the difference between fission and fusion? Give an example of each.
What do physicists hope to learn using the Large Hadron Collider?
Student Projects
• Is nuclear power a boon to the human race, or is it too dangerous to continue using? What
about radiation? Consider nuclear power, nuclear weapons, dental and other x-rays, irradiated
food, and mammography. Using facts gleaned from print sources and reputable Web sites, create
a presentation on the pros and cons of either nuclear power or radiation. Share your findings
with the class in the form of a brochure, poster, public service announcement, infomercial, or
written report.
• How did the ancients come up with their ideas about the atom? How closely do their ideas
match current knowledge (e.g., the Buddhist Dharmakirti’s idea of atoms that instantaneously
flash in and out of existence)? Conduct research using the term “Atomism,” and include the
contributions of the Indians, Greeks, and Muslims of the Islamic Golden Age. (Don’t be afraid
to stretch your mind with creative conjecture on the first question!) Present to the class your
report on the history of atomic theory, using visual aids when possible.
• Create a children’s picture book (or naturalist’s sketchbook) that illustrates and defines the difference between atoms, elements, molecules, and compounds, and between different kinds of
elementary particles.
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• Although a water molecule is often presented as a simple example of chemical bonding, its actual dynamics intrigue scientists. For instance, the fact that its solid form can float on its liquid
form is unusual for a liquid. And in April of 2009, researchers at the Stanford Linear Accelerator
Center presented controversial ‘evidence’ that the molecules in water do not connect in quite the
way we thought. Conduct an Internet search on ‘anomalous [or ‘unusual’] properties of water’
and write a short paper outlining your findings.
• Research and report on the workings of the Large Hadron Collider, including its history, purpose,
setbacks, functioning, and any results. What are some of the research questions that physicists are
hoping it will shed light on?
• Investigate and report on the science behind the following terms often encountered in science
fiction books and movies: anti-matter; space-time continuum; black hole; Higgs boson, aka
‘The God Particle.’
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Assessment Questions
1. What is the nucleus of an atom composed of?
a) Neutron, protons, and electrons
b) Protons and neutrons
c) Electrons
d) Quarks
2. A proton carries a positive charge, and a(n) _____ carries a negative charge.
a) neutron
b) electron
c) quark
d) element
3. What holds protons and neutrons together inside an atom’s nucleus?
a) Gravity
b) Electromagnetism
c) Strong nuclear force
d) Weak nuclear force
4. True or False? John Dalton in the 18th century produced experimental data of atoms as tiny
solids surrounded by heat energy. His model has remained unchanged to this day.
5. The atomic number is _____.
a) the number of protons in an atom’s nucleus
b) the number of neutrons in an atom’s nucleus
c) the total number of neutrons and protons in an atom’s nucleus
d) the number of ions in an atom
6. True or False? The elements on the periodic table are listed in the order in which they were
discovered.
7. The valence shell of an atom _____ .
a) is its outermost, highest energy shell
b) determines the atom’s chemical properties
c) when full makes for the most stable atom
d) all of the above
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8. True or False? In order to stabilize itself, a highly reactive atom will ‘react’ by donating the
electron(s) from its outer shell rather than filling the shell.
9. Electronegativity is _____.
a) an atom’s ability to pull in electrons, thus determining whether its electrons will be shared
or exchanged in a chemical bond
b) the measure of the attraction and repulsion between electrical charges inside an atom
c) one of the four fundamental forces in nature
d) a measure of an electron’s ‘attitude’
10. T
able salt is an example of a(n) _____ bond, because its sodium atoms each donate an electron
to its chlorine atoms.
a) covalent
b) ionic
c) hydrogen
d) weak hydrogen
11. Radioactive decay can be described in simple terms as _____.
a) living things decompressing
b) atoms bonding with other atoms
c) atoms losing little bits of themselves
d) protons reacting to neutrons
12. [ Choose the correct term.] [Fission/Fusion] is the breaking up of the nucleus, and [fission/fusion]
is the joining of two nuclei. Nuclear power plants generate energy using [fission/fusion] reactions,
while the sun uses [fission/fusion].
13. Neutrons and protons are made of _____.
a) leptons
b) neutrinos and positrons
c) Higgs bosons
d) quarks
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Assessment Questions Answer Key
1. What is the nucleus of an atom composed of?
a) Neutron, protons, and electrons
b) Protons and neutrons
c) Electrons
d) Quarks
A: (b) Protons and neutrons.
2. A proton carries a positive charge, and a(n) _____ carries a negative charge.
a) neutron
b) electron
c) quark
d) element
A: (b) electron
3. What holds protons and neutrons together inside an atom’s nucleus?
a) Gravity
b) Electromagnetism
c) Strong nuclear force
d) Weak nuclear force
A: (c) Strong nuclear force
4. True or False? John Dalton in the 18th century produced experimental data of atoms as tiny
solids surrounded by heat energy. His model has remained unchanged to this day.
A: False. At the turn of the 20th century J. J. Thompson introduced the plum pudding model, seeing the
atom as negatively charged electrons stuck in positively charged goo. In 1911 Ernest Rutherford proposed a positively charged nucleus orbited by electrons; Niels Bohr then refined this with the idea that
electrons orbit the nucleus each in their own energy shell. Today’s quantum model describes electrons
that behave as clouds rather than orbiting particles.
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5. The atomic number is _____.
a) the number of protons in an atom’s nucleus
b) the number of neutrons in an atom’s nucleus
c) the total number of neutrons and protons in an atom’s nucleus
d) the number of ions in an atom
A: (a) the number of protons in an atom’s nucleus
6. T
rue or false? The elements on the periodic table are listed in the order in which they were
discovered.
A: False. The elements are grouped on the table by mass and by their chemical properties.
7. The valence shell of an atom _____ .
a) is its outermost, highest energy shell
b) determines the atom’s chemical properties
c) when full makes for the most stable atom
d) all of the above
A: (d) all of the above
8. True or False? In order to stabilize itself, a highly reactive atom will ‘react’ by donating the
electron(s) from its outer shell rather than filling the shell.
A: True.
9. Electronegativity is _____.
a) an atom’s ability to pull in electrons, thus determining whether its electrons will be shared
or exchanged in a chemical bond
b) the measure of the attraction and repulsion between electrical charges inside an atom
c) one of the four fundamental forces in nature
d) a measure of an electron’s ‘attitude’
A: (a) an atom’s ability to pull in electrons, thus determining whether its electrons will be shared or
exchanged in a chemical bond
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10. T
able salt is an example of a(n) _____ bond, because its sodium atoms each donate an electron
to its chlorine atoms.
a) covalent
b) ionic
c) hydrogen
d) weak hydrogen
A: (b) ionic
11. Radioactive decay can be described in simple terms as _____.
a) living things decompressing
b) atoms bonding with other atoms
c) atoms losing little bits of themselves
d) protons reacting to neutrons
A: (c) atoms losing little bits of themselves
12. [ Choose the correct term.] [Fission/Fusion] is the breaking up of the nucleus, and [fission/fusion]
is the joining of two nuclei. Nuclear power plants generate energy using [fission/fusion] reactions,
while the sun uses [fission/fusion].
A: Fission is the breaking up of the nucleus, and fusion is the joining of two nuclei. Nuclear power
plants generate energy using fission reactions, while the sun uses fusion.
13. Neutrons and protons are made of _____.
a) leptons
b) neutrinos and positrons
c) Higgs bosons
d) quarks
A: (d) quarks
Copyright © 2010 Films for the Humanities & Sciences® • www.films.com • 1-800-257-5126
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Physics in Actions
THE NATURE OF MATTER
Instructor’s Guide
Additional Resources
ScienCentral
Science Videos, Science News
www.sciencentral.com
PhysOrg
Science : Physics : Tech : Nano : News
www.physorg.com
PhysLink.com
Physics & Astronomy Online
www.physlink.com
Welcome to Explorations in Science with Dr. Michio Kaku
Theoretical Physicist, Professor, Bestselling Author, Popularizer of Science
http://mkaku.org
Chemical Elements.com
An Online, Interactive Periodic Table of the Elements
www.chemicalelements.com
CERN
European Organization for Nuclear Research
www.cern.ch
Los Alamos National Laboratory
www.lanl.gov
NASA
www.nasa.gov
National Science Foundation
www.nsf.gov
U.S. Geological Survey
www.usgs.gov
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Physics in Actions
THE NATURE OF MATTER
Instructor’s Guide
Additional Products from Films Media Group
Available from Films Media Group • www.films.com • 1-800-257-5126
Nuclear Chemistry: Inside the Atom (DVD/VHS)
From the ancient Greek concept of “atomos” to today’s fission and fusion technologies, this program
guides viewers through the landscape of atomic theory and the hidden world of subatomic particles.
Topics include the makeup of atomic nuclei and the factors that make them stable or unstable; the
discovery and use of radioisotopes; and the difference between fission and fusion. Providing historical perspective, the video illustrates major discoveries about the nucleus and presents concise profiles
of pioneering atomic physicists—such as Henri Becquerel, Irène Joliot-Curie and Frédéric Joliot,
Ernest Rutherford and Frederick Soddy, and many others. Viewable/printable educational resources
are available online. (20 minutes) © 2007 (# 40291)
Bohr’s Model of the Atom (DVD/VHS)
A good way to introduce quantum theory is to profile the individuals who pioneered it. This program focuses on Niels Bohr’s contributions to our understanding of the atom and the behavior of
subatomic particles according to quantum mechanics. Outlining theoretical precursors of quantum
physics—including the ideas of John Dalton and J. J. Thomson—and a brief biography of Bohr,
the video shows how the Danish physicist devised his atomic model and sheds light on his first and
second postulates. Clever animation and helpful summaries enrich this valuable survey of the history and legacy of Bohr’s achievements. Viewable/printable educational resources are available online.
(26 minutes) © 2007 (# 40282)
Chemical Bonding (DVD/VHS)
This four-part series provides a comprehensive introduction to the chemical bonding processes.
Using computer-generated models and examples from everyday life, each program illustrates the
principles of bonding relevant to high school and college chemistry courses. Viewable/printable
educational resources are available online. (4-part series, 17-22 minutes each) © 1997 (# 7743)
The Periodic Table (DVD/VHS)
Divided into five sections, this program looks at the history and components of the periodic table:
The History of the Periodic Table (from the atomos of Democritus to the atoms of Mendeleev);
Metals (how to read the periodic table, transition metals, alkali metals, alkaline earth metals);
Lanthanides, Actinides, and Transuranium Elements (properties of lanthanides and actinides,
transuranium and transfermium elements); The BCNOs (properties of metalloids, other metals,
and nonmetals); and Halogens and Noble Gases (properties and applications of halogens and noble
gases). A viewable/printable instructor’s guide is available online. A Films for the Humanities &
Sciences Production. (24 minutes) © 2010 (# 39607)
Copyright © 2010 Films for the Humanities & Sciences® • www.films.com • 1-800-257-5126
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Physics in Actions
THE NATURE OF MATTER
Instructor’s Guide
Einstein Made Relatively Easy (DVD/VHS)
Introducing EinSteinchen, an animated techno-Einstein who has a genius for explaining physics. In section one of this DVD, this likable know-it-all elucidates 12 essential topics in 90-second
segments that are perfect for launching lectures or illustrating concepts. Section two departs from
EinSteinchen’s virtual world to show 12 cutting-edge applications or studies of Einsteinian physics
in high-level mini-documentaries of two to five minutes in length. A Deutsche Welle Production.
(60 minutes) © 2006 (# 35602)
Bottling the Sun: The Quest for Nuclear Fusion (DVD/VHS)
As fossil fuels near depletion, nuclear fusion promises unlimited power supplies. This program looks
at recent developments in the quest to turn the mechanism of the sun into a viable energy source.
The program chronicles the efforts of Alan Sykes and his team working on START, the first spherical Tokamak, at the Culham Research Facility in England. Dr. Martin Peng, who first conceived of
a compact, spherical plasma reactor, is also interviewed and discusses the American offshoot of the
START project, the National Spherical Tokamak Experiment. (30 minutes) © 2002 (# 30783)
Most of Our Universe is Missing: Dark Matter and Dark Energy (DVD/VHS)
“What is everywhere, not made of atoms, and can’t be seen?” Dark matter, says renowned astrophysicist David Spergel — but not everyone in the cosmological community is in agreement with him.
This program presents the views of Spergel and other key figures in the debate, including Princeton
University’s P. James Peebles and Jeremiah Ostriker; Timothy Sumner, of Imperial College London;
astrophysicist Mordechai Milgrom; and Saul Perlmutter, a member of Lawrence Berkeley National
Laboratory’s physics division. Experiments in Europe’s deepest mine looking for the elusive neutralino, the concept of variable gravity, and what may well become the new standard model of how the
universe works are all scrutinized. Original BBCW broadcast title: Most of Our Universe Is Missing.
(50 minutes) © 2006 (# 36379)
Physics of Fun (posters)
Physics of Fun—a dynamic eight-piece series of 17” x 22”
posters—has fun with physics as it illustrates key principles
every science student needs to know. Whether it’s a skateboarder on a
ramp turning potential energy into kinetic energy or a goalkeeper performing negative mechanical work on a soccer ball, this is serious science. A
Films for the Humanities & Sciences Product. The posters are: Potential
Energy Poster | Kinetic Energy Poster | Work Poster | Angular Momentum
Poster | Conservation of Energy Poster | Newton’s 1st Law Poster | Newton’s 2nd
Law Poster | Newton’s 3rd Law Poster. © 2008 (# 38992)
Please send comments, questions, and suggestions to [email protected]
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