Download Chapter 4 Review - Mona Shores Blogs

Name: ________________________ Class: ___________________ Date: __________
Chapter 4 Review
1. According to ____________________, all matter was made up of four elements: earth, air, fire, and water.
2. Unlike Democritus, Aristotle did not believe that matter was composed of tiny, indivisible
____________________.
3. John Dalton concluded that all the atoms of a single ____________________ have the same mass.
4. The subatomic particle that J.J. Thomson discovered has a(an) ____________________ charge.
Figure 4-1
5. In Rutherford’s gold foil experiment, shown in Figure 4-1, alpha particles that bounce straight back from the
foil have struck ____________________ in the gold atoms.
6. The results of Rutherford’s gold foil experiment demonstrated that the ____________________ occupies a
very small amount of the total space inside an atom.
7. Protons and ____________________ are found in the nucleus of an atom.
8. Neutrons and ____________________ have almost the same mass.
9. If element Q has 11 protons, its atomic ____________________ is 11.
10. The nuclei of isotopes contain different numbers of ____________________.
11. The _________________________ of an isotope is the sum of the number of protons and neutrons in its
nucleus.
12. In Bohr’s model of the atom, ____________________ move in fixed orbits around the nucleus.
13. When an atom gains or loses energy, some of its ____________________ may move between energy levels.
14. The moving blades of an airplane propeller provide an analogy for the electron ____________________
model.
15. The region in which an electron is most likely to be found is called a(an) ____________________.
16. When all the electrons in an atom are in orbitals with the lowest possible energy, the atom is in its
____________________ state.
1
17. An atom in which an electron has moved to a higher energy level is in a(an) ____________________ state.
18. The difference between a sample of heavy water and regular water is that a hydrogen atom in heavy water
has an extra ____________________.
19. The property of an element that indicates the number of protons in its atoms is the
_________________________.
20. In an atom, the particles that have no charge are called ____________________.
21. What did Democritus believe about matter?
22. How did the results of J.J. Thomson’s experiments change how scientists thought about atoms?
23. What did Rutherford conclude about the location of positive charge in an atom?
24. Which of the three subatomic particles—proton, electron, or neutron—has the least mass?
25. If an atom has 32 protons and 38 neutrons, what is its mass number?
26. If an atom of an element has a mass number of 31 and 16 neutrons in its nucleus, what is the atomic number
of the element?
27. If an atom of germanium has a mass number of 70 and an atomic number of 32, how many neutrons are in its
nucleus?
28. In the nucleus of an atom, there are 15 protons and 16 neutrons. What is the atomic number and mass number
of this isotope?
2
29. How does the electron cloud model of the atom represent the locations of electrons in atoms?
Atoms of Some Common Elements
Atomic
Number
Atomic
Mass
Protons
Neutrons
Electrons
Sodium
11
?
11
12
?
Magnesium
12
24
12
?
12
Aluminum
?
27
13
14
13
Phosphorus
15
31
?
16
15
Substance
30. What is the atomic mass of sodium?
31. What is the total number of electrons in an atom of sodium?
32. How many neutrons are in an atom of magnesium?
33. The element silicon has been omitted from this table. It appears in the periodic table between aluminum and
phosphorus, and in the same row. Given that information, which of the five columns could you fill in for
silicon?
34. What is the atomic number of aluminum?
35. How many protons are in an atom of phosphorus?
3
36. A sample of calcium contains calcium-40, calcium-44, calcium-42, calcium-48, calcium-43, and calcium-46
atoms. Explain why these atoms can have different mass numbers, but they must have the same atomic
number.
37. Explain what the colors in a fireworks display reveal about the movement of electrons in atoms.
38. Explain why the atoms of a particular element are exactly alike in some ways but may not be alike in other
ways.
Figure 4-2
39. In Figure 4-2, what is the main difference between the atomic model in panel 1 and the model in panel 2?
4
40. Are the atomic models in Figure 4-2 arranged in the order that they were developed? Explain your answer.
41. Draw the Bohr Model for Carbon and Chlorine. Be sure to include protons, neutrons and electrons.
5
ID: A
Chapter 4 Review
Answer Section
COMPLETION
1. ANS: Aristotle
PTS: 1
2. ANS: atoms
DIF:
L1
OBJ: 4.1.1
PTS: 1
3. ANS: element
DIF:
L2
OBJ: 4.1.1
PTS: 1
4. ANS: negative
DIF:
L1
OBJ: 4.1.2
PTS: 1
5. ANS: nuclei
DIF:
L1
OBJ: 4.1.3
PTS: 1
6. ANS: nucleus
DIF:
L2
OBJ: 4.1.3
PTS: 1
7. ANS: neutrons
DIF:
L2
OBJ: 4.1.3
PTS: 1
8. ANS: protons
DIF:
L1
OBJ: 4.2.1
PTS: 1
9. ANS: number
DIF:
L2
OBJ: 4.2.1
PTS: 1
10. ANS: neutrons
DIF:
L1
OBJ: 4.2.2
PTS: 1
DIF:
11. ANS: mass number
L1
OBJ: 4.2.2
PTS: 1
12. ANS: electrons
DIF:
L2
OBJ: 4.2.2
PTS: 1
13. ANS: electrons
DIF:
L1
OBJ: 4.3.1
PTS: 1
14. ANS: cloud
DIF:
L2
OBJ: 4.3.1
PTS: 1
DIF:
L1
OBJ: 4.3.2
1
ID: A
15. ANS: orbital
PTS: 1
16. ANS: ground
DIF:
L2
OBJ: 4.3.2
PTS: 1
17. ANS: excited
DIF:
L1
OBJ: 4.3.3
PTS: 1
18. ANS: neutron
DIF:
L2
OBJ: 4.3.3
PTS: 1
DIF:
19. ANS: atomic number
L2
OBJ: 4.2.2
PTS: 1
DIF: 2=Low/Mid OBJ: Physical Ch. 3.1.1
NOT: Physical Ch. 3.1.1—Describe the structure of an atom, and define protons, neutrons, and electrons.
20. ANS: neutrons
PTS: 1
DIF: 3=Mid/High OBJ: Physical Ch. 3.1.1
NOT: Physical Ch. 3.1.1—Describe the structure of an atom, and define protons, neutrons, and electrons.
SHORT ANSWER
21. ANS:
Democritus believed all matter consisted of tiny particles that could not be divided into smaller particles.
PTS: 1
DIF: L1
OBJ: 4.1.1
22. ANS:
Scientists realized that atoms contained smaller subatomic particles.
PTS: 1
DIF: L1
OBJ: 4.1.3
23. ANS:
Rutherford concluded that positive charge was concentrated in the nucleus of an atom.
PTS: 1
24. ANS:
electron
DIF:
L1
OBJ: 4.1.3
PTS: 1
25. ANS:
70
DIF:
L1
OBJ: 4.2.1
PTS: 1
26. ANS:
15
DIF:
L1
OBJ: 4.2.2
PTS: 1
DIF:
L2
OBJ: 4.2.2
2
ID: A
27. ANS:
38
PTS: 1
DIF: L2
28. ANS:
atomic number = 15; mass number = 31
OBJ: 4.2.2
PTS: 1
DIF: L1
OBJ: 4.2.2
29. ANS:
It provides a visual model of the most likely locations of electrons in an atom.
PTS: 1
30. ANS:
23
DIF:
L2
OBJ: 4.3.2
PTS: 1
DIF: 3=Mid/High OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
31. ANS:
11
PTS: 1
DIF: 2=Low/Mid OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
32. ANS:
12
PTS: 1
DIF: 3=Mid/High OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
33. ANS:
Its atomic number is 14, and a silicon atom has 14 protons and 14 electrons. (You cannot figure out the
number of neutrons or the atomic mass using this chart.)
PTS: 1
DIF: 3=Mid/High OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
34. ANS:
13
PTS: 1
DIF: 2=Low/Mid OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
35. ANS:
15
PTS: 1
DIF: 2=Low/Mid OBJ: Physical Ch. 3.2.2
NOT: Physical Ch. 3.2.2—List the information in the periodic table and describe how it is organized.
3
ID: A
ESSAY
36. ANS:
All the atoms of an element have the same atomic number because the atomic number equals the number of
protons in an atom. If one of the atoms had a different number of protons, the atom would not be a calcium
atom. The mass number can vary because it is the sum of the protons and neutrons and because isotopes of an
element can have different numbers of neutrons.
PTS: 1
DIF: L2
OBJ: 4.2.2
37. ANS:
When fireworks explode, the heat produced by the explosions causes some electrons in atoms to move to
higher energy levels. When the electrons return to lower energy levels, some of the energy is released as
visible light. The colors vary because each element has a different set of energy levels.
PTS: 1
DIF: L2
OBJ: 4.3.3
38. ANS:
All atoms of a particular element have the same number of protons and electrons. However, those atoms may
have different numbers of neutrons. That means that the mass of individual atoms of an element may vary.
PTS: 1
DIF: 2=Low/Mid OBJ: Physical Ch. 3.1.1
NOT: Physical Ch. 3.1.1—Describe the structure of an atom, and define protons, neutrons, and electrons.
OTHER
39. ANS:
Panel 1 depicts an atom as a solid sphere without any subatomic particles. Panel 2 shows an atom that has a
subatomic structure.
PTS: 1
DIF: L1
OBJ: 4.1.2 | 4.2.1 | 4.3.1
40. ANS:
Yes; they go from the simplest (the solid sphere in 1) to the most complex (the electron cloud diagram in
panel 3). Students may specifically cite John Dalton in connection with panel 1 and Niels Bohr in connection
with panel 2 to support their answer.
PTS: 1
DIF:
L1
OBJ: 4.1.2 | 4.3.1 | 4.3.2
CASE
41. ANS:
s
PTS: 1
4