Download IPLS Section 4.1 Studying Atoms

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Name ___________________________
Chapter 4
Class ___________________
Date _____________
Atomic Structure
Section 4.1 Studying Atoms
(pages 100–105)
This section discusses the development of atomic models.
Reading Strategy (page 100)
Summarizing As you read, complete the table about atomic models. For
more information on this Reading Strategy, see the Reading and Study
Skills in the Skills and Reference Handbook at the end of your textbook.
Scientist
Dalton
Evidence
Atomic Models
Model
Indivisible, solid spheres
Deflected beam
Negative charges evenly scattered
through positively charged mass of
matter (plum pudding model)
Deflection of alpha particles
passing through gold foil
Ancient Greek Models of Atoms (page 100)
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1. Democritus named the smallest particles of matter
they could not be divided.
Dalton’s Atomic Theory
because
(page 101)
2. Is the following sentence true or false? John Dalton gathered evidence
for the existence of atoms by measuring the masses of elements that
reacted to form compounds.
3. Dalton’s theory suggests that all matter is made up of individual
particles called
, which cannot be
.
4. Circle the letters of the sentences that represent main points of Dalton’s
theory of atoms.
a. All elements are composed of atoms.
b. In a particular compound, atoms of different elements always
combine the same way.
c. All atoms have the same mass.
Physical Science Reading and Study Workbook Level B
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Name ___________________________
Chapter 4
Class ___________________
Date _____________
Atomic Structure
Thomson’s Model of the Atom
(pages 102–103)
5. Use the words in the box below to fill in the blanks. Objects with like
electric charges
charges
, and objects with opposite electric
.
attract
reflect
deflect
repel
6. Thomson concluded that the particles in the glowing beam had a(n)
charge because they were attracted to a positive
plate.
7. Circle the letter of the sentences that describe Thomson’s model of the
atom.
a. An atom is filled with positive matter.
b. An atom is mostly space with a small nucleus.
c. Negative charges are scattered throughout an atom.
Rutherford’s Atomic Theory
(pages 104–105)
a. More alpha particles were deflected than expected.
b. None of the alpha particles were deflected.
c. Some alpha particles bounced back toward the source.
10. Circle the letter of the sentence that states what Rutherford
concluded from the gold foil experiment.
a. An atom’s negative charge is concentrated in its nucleus.
b. An atom’s positive charge is concentrated in its nucleus.
c. An atom’s positive charge is spread evenly throughout the atom.
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8. An
is a fast-moving particle that carries a positive charge.
9. Circle the letters of the sentences that describe what happened when
Marsden directed a beam of particles at a piece of gold foil.
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Name ___________________________
Chapter 4
Class ___________________
Date _____________
Atomic Structure
Section 4.2 The Structure of an Atom
(pages 108–112)
This section compares the properties of three subatomic particles. It also discusses
atomic numbers, mass numbers, and isotopes.
Reading Strategy
(page 108)
Monitoring Your Understanding Before you read, list in the table shown
what you know about atoms and what you would like to learn. After you
read, list what you have learned. For more information on this Reading
Strategy, see the Reading and Study Skills in the Skills and Reference
Handbook at the end of your textbook.
What I Know
About Atoms
Most students will know
that atoms are the
“building blocks” of matter,
and some may know that
atoms contain
subatomic particles.
What I Would
Like to Learn
Based on the title of
the section, students
may say that they
want to learn more
about the structure
of atoms.
Properties of Subatomic Particles
What I Have
Learned
(pages 108–109)
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1. What are three subatomic particles?
a.
b.
c.
2. Circle the letter that identifies a subatomic particle with a positive
charge.
a. nucleus
b. proton
c. neutron
Comparing Subatomic Particles
(pages 109–110)
3. Circle the letters of properties that vary among subatomic particles.
a. color
b. location in the atom
c. charge
4. Circle the letter of the expression that accurately compares the masses of
neutrons and protons.
a. mass of 1 neutron = mass of 1 proton
b. mass of 2000 neutrons = mass of 1 proton
c. mass of 1 electron = mass of 1 proton
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Chapter 4
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Atomic Structure
Atomic Number and Mass Number
(page 110)
5. Is the following sentence true or false? Two atoms of the same element
can have different numbers of protons.
6. The
number of an element equals the number of protons in
an atom of that element.
7. Is the following sentence true or false?
Two different elements can have the same atomic number.
8. The
number of an atom is the sum of the protons and
neutrons in the nucleus of that atom.
9. Complete the equation in the table below.
Number of neutrons Mass number Isotopes
(page 112)
Use the words in the box below to fill in the blanks in questions 10–12.
electrons
neutrons
isotopes
protons
and
.
11. Every atom of a given element does not have the same number of
.
are atoms of the same element that have different
numbers of neutrons and different mass numbers.
13. All oxygen atoms have 8 protons. Circle the letter of the number of
neutrons in an atom of oxygen-18.
12.
a. 8
b. 10
c. 18
14. Is the following sentence true or false? Isotopes of oxygen have
different chemical properties.
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10. Every atom of a given element has the same number of
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Chapter 4
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Atomic Structure
Section 4.3 Modern Atomic Theory
(pages 113–118)
This section focuses on the arrangement and behavior of electrons in atoms.
Reading Strategy
(page 113)
Sequencing After you read, complete the description in the flow chart
below. Write how the gain or loss of energy affects electrons in atoms. For
more information on this Reading Strategy, see the Reading and Study
Skills in the Skills and Reference Handbook at the end of your textbook.
Excited state
Bohr’s Model of the Atom
Emits energy
(pages 113–116)
1. Circle the letter of the sentence that tells how Bohr’s model of the atom
differed from Rutherford’s model.
a. Bohr’s model focused on the nucleus.
b. Bohr’s model focused on the protons.
c. Bohr’s model focused on the electrons.
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2. What can happen to an electron in an atom when the atom gains or loses
energy?
3. Is the following sentence true or false? When electrons release energy,
some of the energy may be released as visible light.
Electron Cloud Model
(page 116)
4. Is the following sentence true or false? Bohr’s model was correct in
assigning energy levels to electrons.
5. When trying to predict the locations and motions of electrons in atoms,
scientists must work with
. Circle the correct answer.
precision
probability
accuracy
6. An
is a visual model of the most likely locations for
the electrons in an atom.
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Chapter 4
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Atomic Structure
Atomic Orbitals
(page 117)
7. Is the following sentence true or false? An orbital is a region of space
around the nucleus where an electron is likely to be found.
Use this table to answer questions 8 and 9.
Energy
Level
Number of
Orbitals
Maximum Number
of Electrons
1
2
3
4
1
4
9
16
2
8
18
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8. Higher energy levels have
orbitals than lower
energy levels do.
9. The maximum number of electrons in an energy level is
times the number of orbitals.
Electron Configurations
(page 118)
10. Circle the letter of the number of energy levels needed for a lithium
atom’s three electrons when the atom is in its ground state.
11. Is the following sentence true or false? An excited state is less stable
than a ground state.
12. Circle the letters of each sentence that is true when all of the electrons in an
atom are in orbitals with the lowest possible energies.
a. The electrons are in the most stable configuration.
b. The electrons are in an unstable configuration.
c. The atom is in its ground state.
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a. one
b. two
c. three