Download Electrons in Atoms

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Date
CHAPTER
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Class
STUDY GUIDE FOR CONTENT MASTERY
Electrons in Atoms
Section 5.1
Light and Quantized Energy
In your textbook, read about the wave nature of light.
Use each of the terms below just once to complete the passage.
amplitude
energy
frequency
hertz
light
wave
wavelength
speed
that behaves like a(n)
Electromagnetic radiation is a kind of (1)
as it travels through space. (3)
(2)
is one type of
electromagnetic radiation. Other examples include X rays, radio waves, and microwaves.
All waves can be characterized by their wavelength, amplitude, frequency, and
. The shortest distance between equivalent points on a continuous wave is
(4)
. The height of a wave from the origin to a crest or from the
called a(n) (5)
. (7)
origin to a trough is the (6)
is the number of
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waves that pass a given point in one second. The SI unit for frequency is the
, which is equivalent to one wave per second.
(8)
Use the figure to answer the following questions.
A
D
B
Origin
C
9. Which letter(s) represent one wavelength?
10. Which letter(s) represent the amplitude?
11. If twice the length of A passes a stationary point every second, what is the frequency of
the wave?
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Chemistry: Matter and Change • Chapter 5
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Name
Date
5
CHAPTER
Section 5.2
Class
STUDY GUIDE FOR CONTENT MASTERY
Quantum Theory and the Atom
In your textbook, read about the Bohr model of the atom.
Use each of the terms below to complete the statements.
atomic emission spectrum
electron
frequencies
higher
energy levels
lower
ground state
1. The lowest allowable energy state of an atom is called its
.
2. Bohr’s model of the atom predicted the
of the lines in
hydrogen’s atomic emission spectrum.
3. According to Bohr’s atomic model, the smaller an electron’s orbit, the
the atom’s energy level.
4. According to Bohr’s atomic model, the larger an electron’s orbit, the
the atom’s energy level.
5. Bohr proposed that when energy is added to a hydrogen atom, its
moves to a higher-energy orbit.
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6. According to Bohr’s atomic model, the hydrogen atom emits a photon corresponding to
the difference between the
associated with the two
orbits it transitions between.
7. Bohr’s atomic model failed to explain the
of elements
other than hydrogen.
In your textbook, read about the quantum mechanical model of the atom.
Answer the following questions.
8. If you looked closely, could you see the wavelength of a fast-moving car? Explain
your answer.
h
9. Using de Broglie’s equation, m
which would have the larger wavelength, a
slow-moving proton or a fast-moving golf ball? Explain your answer.
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Name
Date
CHAPTER
Section 5.3
5
Class
STUDY GUIDE FOR CONTENT MASTERY
Electron Configurations
In your textbook, read about ground-state electron configurations.
Use each of the terms below just once to complete the passage.
Aufbau principle
electron configuration
ground-state electron configuration
Hund’s rule
lowest
Pauli exclusion principle
spins
stable
The arrangement of electrons in an atom is called the atom’s
. Electrons in an atom tend to assume the arrangement
(1)
that gives the atom the (2)
possible energy. This arrangement
of electrons is the most (3)
arrangement and is called the
.
atom’s (4)
Three rules define how electrons can be arranged in an atom’s orbitals. The
states that each electron occupies the lowest energy
(5)
states that a maximum of two
orbital available. The (6)
electrons may occupy a single atomic orbital, but only if the electrons have opposite
. (8)
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(7)
states that single
electrons with the same spin must occupy each equal-energy orbital before additional
electrons with opposite spins occupy the same orbitals.
Complete the following table.
Element
Atomic Number
Orbitals
1s
2s
2px
Electron Configuration
2py
2pz
1s2
9. Helium
10.
11. Neon
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)( )( )( )( )(
Chemistry: Matter and Change • Chapter 5
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CHAPTER
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STUDY GUIDE FOR CONTENT MASTERY
Section 5.3 continued
Answer the following questions.
12. What is germanium’s atomic number? How many electrons does germanium have?
13. What is noble-gas notation, and why is it used to write electron configurations?
14. Write the ground-state electron configuration of a germanium atom, using noble-gas
notation.
In your textbook, read about valence electrons.
Circle the letter of the choice that best completes the statement or answers the question.
15. The electrons in an atom’s outermost orbitals are called
b. quantum electrons.
c. valence electrons.
d. noble-gas electrons.
16. In an electron-dot structure, the element’s symbol represents the
a. nucleus of the noble gas closest to the atom in the periodic table.
b. atom’s nucleus and inner-level electrons.
c. atom’s valence electrons.
d. electrons of the noble gas closest to the atom in the periodic table.
17. How many valence electrons does a chlorine atom have if its electron configuration
is [Ne]3s23p5?
a. 3
b. 21
c. 5
d. 7
18. Given boron’s electron configuration of [He]2s22p1, which of the following represents its
electron-dot structure?
a. • Be •
•
b. •B•
••
c. B••
••
d. Be
19. Given beryllium’s electron configuration of 1s22s2, which of the following represents its
electron-dot structure?
a. • Be •
•
b. •B•
••
c. B ••
••
d. Be
20. Which electrons are represented by the dots in an electron-dot structure?
30
a. valence electrons
c. only s electrons
b. inner-level electrons
d. both a and c
Chemistry: Matter and Change • Chapter 5
Study Guide for Content Mastery
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a. electron dots.
Name
Date
CHAPTER
5
Class
CHAPTER ASSESSMENT
Electrons in Atoms
Reviewing Vocabulary
Match the definition in Column A with the term in Column B.
Column A
Column B
1. The set of frequencies of the electromagnetic waves
emitted by the atoms of an element
b. photoelectric effect
2. The minimum amount of energy that can be lost or gained
by an atom
3. A form of energy that exhibits wavelike behavior as it
travels through space
c. photon
d. quantum
e. atomic orbital
4. A three-dimensional region around the nucleus of an atom
that describes an electron’s probable location
5. The shortest distance between equivalent points on a
continuous wave
f.
atomic emission
spectrum
g. principal quantum
number
6. The lowest allowable energy state of an atom
h. ground state
7. A particle of electromagnetic radiation with no mass that
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
a. wavelength
carries a quantum of energy
i.
electromagnetic
radiation
8. The emission of electrons from a metal’s surface when
light of a certain frequency shines on it
9. A figure indicating the relative sizes and energies of atomic orbitals
Describe how each pair is related.
10. frequency, amplitude
11. valence electron, electron-dot structure
12. principal energy levels, energy sublevels
Chapter Assessment
Chemistry: Matter and Change • Chapter 5
25
Name
CHAPTER
Date
5
Class
CHAPTER ASSESSMENT
Understanding Main Ideas (Part B)
Circle the letter of the choice that best completes the statement or answers the question.
Use the following figure to answer questions 1 and 2.
D
C
E
A
B
1. According to Bohr’s atomic model, which letter(s) in the figure represents a place where
an electron cannot be?
a. A
b. B, C and E
c. A and D
d. D
2. According to the quantum mechanical model of the atom, point E in the figure
represents a
a. point where an electron cannot be.
c. position where an electron must be.
b. position where an electron probably is.
d. point beyond which no electron can go.
3. What can you conclude from the figure on the right?
)( ) )
a. Hund’s rule has been violated.
2p
)(
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
b. The Pauli exclusion principle has been violated.
2s
c. The Aufbau principle has been violated.
1s
d. This is a valid orbital diagram.
4. What can you conclude from the figure on the right?
))
a. Hund’s rule has been violated.
2p
)(
b. The Pauli exclusion principle has been violated.
c. The Aufbau principle has been violated.
2s
)(
1s
d. This is a valid orbital diagram.
5. Which of the following can you conclude based on the de Broglie equation?
a. Waves behave like particles.
c. All matter has an associated wavelength.
b. Most particles are electrons.
d. All matter behaves like particles.
6. Which of the following best describes the Heisenberg uncertainty principle?
a. Light behaves like a particle and like a wave.
b. The shorter the wavelength, the higher the frequency.
c. It is impossible to know both the velocity and the position of a particle at the same time.
d. You cannot measure an object without disturbing it.
Chapter Assessment
Chemistry: Matter and Change • Chapter 5
27
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Date
5
CHAPTER
Class
CHAPTER ASSESSMENT
Thinking Critically
Answer the following questions.
1. A radio station has a frequency of 103.7 MHz. (1 MHz 106 s1) What is the
wavelength of the radiation emitted by the station? Indicate where this wavelength
falls on the electromagnetic spectrum shown below.
Electromagnetic Spectrum
106
105
107
109
108
1010
1011
1012
1013
1014
1015
1016
1017
1018
1019
(Hz)
103
102
101
10–1
10–2
10–3
10–4
10–5 10–6
10–7
10–8
rays
X rays
Ultraviolet
Visible
Infrared
Microwave
UHF-TV
1
10–9
10–10 10–11
(m)
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104
FM radio
VHF-TV
AM radio
Radio
2. Look at the electromagnetic spectrum again. Are the microwaves used to cook food
higher or lower in frequency than radio waves? Are microwaves longer or shorter in
wavelength than radio waves?
3. Write the orbital diagram of aluminum.
4. Write the complete electron configuration and the noble-gas notation for aluminum.
5. Write the noble-gas notation for iodine.
6. Identify each atom.
a. 1s22s22p1
b. [Ar]4s1
7. Write electron-dot structures for the following atoms.
28
a. neon
c. carbon
b. hydrogen
d. sulfur
Chemistry: Matter and Change • Chapter 5
Chapter Assessment
Name
CHAPTER
Date
5
Class
CHAPTER ASSESSMENT
Applying Scientific Methods
A chemist isolated four samples, A, B, C, and D. She obtained the following atomic emission
spectra of the samples.
A
B
C
D
400
500
600
Nanometers
700
1. Examine each sample’s atomic emission spectra. Assume that each sample represents a
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
single element. What can you conclude by looking at the spectra? Do the samples represent the same element or different elements?
2. Which part of the electromagnetic spectrum do the atomic emission spectra show?
3. Would the atomic emission spectrum for each sample change if you repeated the proce-
dure? Explain your answer
4. What does each line in an atomic emission spectrum represent?
Chapter Assessment
Chemistry: Matter and Change • Chapter 5
29
CHAPTER
5
SUPPLEMENTAL PROBLEMS
Electrons in Atoms
1. Orange light has a frequency of 4.8 1014 s1.
6. List the sequence in which the following
orbitals fill up: 1s, 2s, 3s, 4s, 5s, 6s, 7s, 2p, 3p,
4p, 5p, 6p, 7p, 3d, 4d, 5d, 6d, 4f, 5f.
What is the energy of one quantum of orange
light?
7. Which element has the ground-state electron
2. Which is greater, the energy of one photon
configuration [Kr]5s24d105p4?
of orange light or the energy of one quantum
of radiation having a wavelength of
3.36 109m?
8. Which element has the ground-state electron
configuration [Ar]4s23d10?
3. Use the relationships E h and c v to
write E in terms of h, c, and .
9. Write electron-dot structures for the following
atoms.
4. A radio station emits radiation at a wavelength
a. [Ne]3s23p3
of 2.90 m. What is the station’s frequency in
megahertz?
b. [Ar]4s23d3
c. potassium
5. Record the frequency of your favorite radio
Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc.
station. What is the wavelength of the radiation
emitted from the station?
10. Complete the following table.
Orbitals
Element
Symbol
1s
2s
2px
2py
2pz
1s22s22p3
a. Nitrogen
b.
Electron
Configuration
F
)(
)(
)(
)(
)
c. Carbon
d.
Supplemental Problems
1s22s1
Chemistry: Matter and Change • Chapter 5
7
CHAPTER 5
Electrons in Atoms
Name:
Date:
In question 1, the speed of light, c, equals
3.00 108 m/s.
3
Yellow light has a wavelength of 5.60 10–7
meters. According to the formula, c = , what is the
frequency of this yellow light?
1
the release of gamma rays from the nucleus
B
the return of excited electrons to lower energy
levels
C
the movement of electrons to higher energy
levels
the absorption of photons by the electrons
5.36 1014 s–1
B
5.36 1016 s–1
C
1.87 10–15 s–1
D
D
1.87 1015 s–1
This question covers TEKS 6A. This question tests
the material that was covered in the textbook on
pages 125–126.
Use the diagram below to answer question 2.
In question 4, Planck’s constant, h, equals
6.626 10–34 J.s
4
0
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
A
A
This question covers TEKS 2C. This question tests
the material that was covered in the textbook on
pages 119–121.
1
2
3
4
5
6
7
8
9
10
11
12
13
14
wavelength
2
When a potassium compound is placed in a flame,
energy is released and a violet color is produced.
This energy release is due to —
What is the wavelength of the wave shown above?
A
3.2 cm
B
3.5 cm
C
3.7 cm
D
4.0 cm
According to Einstein, Ephoton = h. What is the
energy of a photon if it has a frequency of
6.82 1014s–1?
A
9.72 10–20J
B
1.03 10–20J
C
4.52 10–19J
D
4.52 10–20J
This question covers TEKS 2C. This question tests
the material that was covered in the textbook on
pages 123–124.
This question covers TEKS 2B. This question tests
the material that was covered in the textbook on
page 118.
Reviewing Chemistry: Mastering the TEKS
Chemistry: Matter and Change
9
CHAPTER 5
Electrons in Atoms, continued
Name:
5
Date:
Which of these is the ground-state electron
configuration for an atom of fluorine (atomic
number = 9)?
A
1s22s2
B
1s22s22p3
C
1s22s22p4
D
1s22s22p5
7
Which of these orbital diagrams represents a
chlorine atom in the ground state? Chlorine has an
atomic number of 17.
A
B
This question covers TEKS 6A. This question tests
the material that was covered in the textbook on
pages 135–139.
C
6
The electron configuration for an atom of iron is
[Ar] 3d64s2. Which of the following is the correct
electron-dot structure for iron?
A
Fe
Fe
C
Fe
Fe
This question covers TEKS 6A. This question tests
the material that was covered in the textbook on
pages 140–141.
2p
1s 2s
2p
1s 2s
2p
3s
3p
1s 2s
2p
3s
3p
This question covers TEKS 2D and 5A. This
question tests the material that was covered in the
textbook on page 137.
8
The arrangement of electrons in an atom of an
element determines the chemical properties of that
element. Our present-day understanding of how
electrons are arranged in an atom is the result of all
of these scientific contributions EXCEPT —
A
Rutherford’s gold foil experiment that proved
the existence of the nucleus
B
Bohr’s orbits that explained hydrogen’s
quantized energy states
C
De Broglie’s equation that led to thinking of
electrons as both particles and waves
D
Schrödinger’s wave equation that predicted
atomic orbitals
This question covers TEKS 3C and 3E. This question
tests the material that was covered in the textbook
on pages 127–132.
10
Chemistry: Matter and Change
Reviewing Chemistry: Mastering the TEKS
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
B
D
D
1s 2s