Download Chapter 5 Review Worksheet

Name ___________________________
Date ___________________
Class __________________
MODELS OF THE ATOM
5.1
Section Review
Objectives
• Identify inadequacies in the Rutherford atomic model
• Identify the new assumption in the Bohr model of the atom
• Describe the energies and positions of electrons according to
the quantum mechanical model
• Describe how the shapes of orbitals at different sublevels vary
Vocabulary
• energy levels
• quantum
• quantum mechanical model
• atomic orbital
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
The chemical properties of atoms, ions, and molecules
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are related to the arrangement of the
1
2.
within them.
2
The first modern atomic theory, proposed by
3.
,
portrayed the atom as a solid, indivisible mass. After the discovery
of the electron by
3
, the atomic model was revised to
4
include them. J.J. Thomson’s model is referred to as the
model. Rutherford pictured the atom as a dense
6
paths. The
7
5.
6.
5
7.
surrounded by electrons. In the Bohr model, the electrons move
in
4.
8.
model is the modern description
of the electrons in atoms. This model estimates the
8
of finding an
electron within a certain volume of space surrounding the nucleus.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. Electrons must have a certain minimum amount of energy called
a quantum in order to move from one energy level to the next higher
energy level.
________ 10. The electron probability clouds for atomic orbitals are spherical
in shape.
Chapter 5 Electrons in Atoms
105
Name ________________________________________ Class _________________ Date _______________
________ 11. The number of sublevels in an energy level is equal to the square of
the principal quantum number of that energy level.
________ 12. The maximum number of electrons that can occupy the fourth
principal energy level of an atom is 32.
________ 13. The higher the energy level occupied by an electron the more
energetic it is.
________ 14. The principal quantum number equals the number of sublevels within
that principal energy level.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 15. quantum
a. a region in space around the nucleus of an atom
where an electron is likely to be moving
________ 16. atomic orbitals
b. the regions around the nucleus within which the
electrons have the highest probability of being
found
________ 17. energy level
c. the amount of energy required to move an electron
from its present energy level to the next higher one
________ 18. quantum mechanical
model
d. the modern description of the behavior of electrons
in atoms
Part D Questions and Problems
Answer the following in the space provided.
20. How many orbitals are in each of the following sublevels?
a. 4p sublevel
b. 3d sublevel
c. 4f sublevel
d. 2s sublevel
106
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19. Summarize the development of atomic theory.
Name ___________________________
Date ___________________
Class __________________
ELECTRON ARRANGEMENT IN ATOMS
5.2
Section Review
Objectives
• Describe how to write the electron configuration for an atom
• Explain why the actual electron configurations for some elements
differ from those predicted by the Aufbau principle
Vocabulary
• electron configurations
• Aufbau principle
• Pauli exclusion principle
• Hund’s rule
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
The ways in which electrons are arranged around the nuclei
of atoms are called
1
. The
2
2.
describes the sequence
3.
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in which orbitals are filled. The various orbitals within a sublevel
of a principle energy level are always of
4
3
4.
energy. The
principle states that a maximum of only
5
5.
electrons can occupy each orbital. To occupy the same orbital, two
electrons must have
6
spins. Hund’s rule states that the
electrons pair up only after each orbital in a sublevel is occupied
7
by
. When using the shorthand method for showing the
electron configuration of an atom,
the number of
9
8
are used to indicate
6.
7.
8.
9.
10.
occupying each sublevel.
Correct electron configurations can be obtained by using the
Aufbau diagram for the elements up to and including vanadium.
10
and copper are exceptions to the Aufbau principle.
Chapter 5 Electrons in Atoms
107
Name ________________________________________ Class _________________ Date _______________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. The orbitals of a principal energy level are lower in energy than the
orbitals in the next higher principal energy level.
________ 12. The configuration 3d 44s2 is more stable than the configuration 3d 54s1.
________ 13. As many as four electrons can occupy the same orbital.
________ 14. The Pauli exclusion principle states that an atomic orbital may describe
at most two electrons.
________ 15. The electron configuration for potassium is 1s22s22p6 3s23p64s1.
________ 16. The electron configuration for copper is 1s22s22p63s23p64s23d 9.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column B
________ 17. electron configuration
a. When electrons occupy orbitals of equal energy, one
electron enters each orbital until all the orbitals
contain one electron with parallel spins.
________ 18. Aufbau principle
b. An atomic orbital may describe at most two electrons.
________ 19. Pauli exclusion principle
c. 1s22s22p6
________ 20. Hund’s rule
d. Electrons enter orbitals of lowest energy first.
________ 21. neon
e. the most stable arrangement of electrons around the
nucleus of an atom
Part D Questions and Problems
Answer the following in the space provided.
22. Write the electron configurations for the following atoms.
a. C
c. K
b. S
d. Ar
23. Identify the elements described below:
a. Contains a full third energy level.
b. Contains the first p electron.
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Column A
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5.3
Date ___________________
Class __________________
PHYSICS AND THE QUANTUM
MECHANICAL MODEL
Section Review
Objectives
•
•
•
•
Describe the relationship between the wavelength and frequency of light
Explain how the frequencies of light are related to changes in electron energies
Distinguish between quantum mechanics and classical mechanics
Identify the cause of the atomic emission spectrum
Vocabulary
•
•
•
•
•
•
•
•
amplitude
wavelength (")
frequency (#)
hertz (Hz)
electromagnetic radiation
spectrum
• photons
• Heisenberg uncertainty
principle
atomic emission spectrum
ground state
Key Equations
• c ! "#
• E!h$#
h
m#
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• " ! %%
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
According to quantum mechanics, the motions of subatomic
1
particles may be described as
2
wavelength of all waves are
Every element emits
. The frequency and
if it is heated by passing an
electric discharge through its gas or vapor. Passing this emission
through a prism gives the
4
and Einstein's explanation of the
6
4.
5.
6.
of the element.
The quantum concept developed from Planck’s studies of
5
2.
3.
related.
3
1.
7.
effect. Planck
showed that the amount of radiant energy absorbed or emitted by
a body is proportional to the
7
of the radiation.
Chapter 5 Electrons in Atoms
109
Name ________________________________________ Class _________________ Date _______________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 8. The speed of light is a constant that can be obtained by dividing the
frequency of light by its wavelength.
________ 9. The amplitude of a wave is the distance between the crests.
________ 10. The energy of a body can change only in small discrete units.
________ 11. The position and velocity of an electron in an atom can be determined
with great certainty.
________ 12. The photoelectric effect will occur no matter what frequency of light
strikes a metal.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. photons
a. predicts that all matter exhibits wavelike motions
________ 14. de Broglie’s equation
b. the distance between two consecutive wave crests
________ 15. visible light
c. light quanta
________ 16. ground state
d. the lowest energy level for a given electron
________ 17. wavelength
e. example of electromagnetic radiation
Part D Questions and Problems
Answer the following in the space provided.
19. Apply quantum theory to explain the photoelectric effect.
110
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18. What is the frequency of radiation whose wavelength is 2.40 ! 10"5 cm?