Chapter 7 Review
Modified True/False
Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true.
____
1. Dalton’s Atomic Theory states that matter is made of atoms or particles that are large enough to see.
_________________________
____
2. Dalton’s Atomic Theory stated that the atoms of any particular element are identical.
_________________________
____
3. Electrons have a positive charge. _________________________
____
4. According to the Rutherford model of the atom, the mass of an electron is 1/1800 that of a proton.
_________________________
____
5. According to the Rutherford model of the atom, most of the mass of an atom, and all its positive charge, is
concentrated in the neutrons. _________________________
____
6. The nucleus contains protons and electrons. _________________________
____
7. The emission spectrum of hydrogen is different from oxygen. _________________________
____
8. The elements in Period 2 of the periodic table have electrons in the first and second shells.
_________________________
____
9. Bohr believed that the electrons with the greatest amount of energy were closest to the nucleus.
_________________________
____ 10. A maximum of eight electrons are allowed in the third shell. _________________________
____ 11. The atom represented by cobalt-60 has 60 electrons. _________________________
____ 12.
is the standard atomic notation for the strontium-88 ion. _________________________
____ 13. Arsenic-75, written in standard atomic notation would be
. _________________________
____ 14. The number of electrons equals the number of neutrons in an atom. _________________________
____ 15. The atomic number of an atom is the total number of protons plus neutrons. _________________________
____ 16. The ion charge is written as a superscript on the right side of the element symbol.
_________________________
____ 17. The mass number of an atom is written as a subscript on the left side of the element symbol.
_________________________
____ 18. The element fluorine forms a positive ion. _________________________
____ 19. There are eighteen groups of elements on the periodic table. _________________________
____ 20. All the elements in Group 1 have an ion charge of negative 1. _________________________
____ 21. Carbon is in Group 6 on the periodic table. _________________________
____ 22. Isotopes of an element have different numbers of neutrons. _________________________
____ 23. There are 30 protons and 32 electrons in a zinc ion (Zn2+). _________________________
____ 24. An atom loses protons to form a negative ion. _________________________
____ 25. Metallic elements form negative ions. _________________________
____ 26. Metalloid elements are situated on the periodic table near the zigzag line that divides metals and non-metals.
_________________________
____ 27. An ionic bond is the electrostatic attraction between a positive ion and a negative
ion._________________________
____ 28. Group 17 is the least reactive group on the periodic table. _________________________
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 29. Which of the following scientists suggested the “raisin bun” model of the atom?
a. Bohr
b. Dalton
c. Thomson
d. Rutherford
____ 30. Which of the following scientists suggested that “at the centre of each atom is a very small, extremely dense,
positively charged region called the nucleus”?
a. Bohr
b. Dalton
c. Thomson
d. Rutherford
____ 31. Which of the following has the least mass?
a. proton
b. neutron
c. nucleus
d. electron
____ 32. Which of the following is uncharged?
a. proton
b. neutron
c. nucleus
d. electron
____ 33. Which of the following is a molecule?
a. SO2
b. NaCl
c. BeO
d. iron and nickel in stainless steel
____ 34. Which scientist proposed the idea of a nucleus?
a. Bohr
b. Dalton
c. Thomson
d. Rutherford
____ 35. Which of the following apply to protons?
a. neutral particles found in the nucleus in an atom
b. positively charged particles found in the nucleus in an atom
c. positively charged particles found orbiting the nucleus in an atom
d. negatively charged particles found orbiting the nucleus in an atom
____ 36. Which of the following apply to electrons?
a. neutral particles found in the nucleus in an atom
b. positively charged particles found in the nucleus in an atom
c. positively charged particles found orbiting the nucleus in an atom
d. negatively charged particles found orbiting the nucleus in an atom
____ 37. Which of the following apply to neutrons?
a. uncharged particles found in the nucleus in an atom
b. positively charged particles found in the nucleus in an atom
c. negatively charged particles found in the nucleus in an atom
d. negatively charged particles found orbiting the nucleus in an atom
____ 38. Which of the following is the specific pattern of colours produced by an element when heated or when
electricity is passed though it?
a. periodicity
b. energy orbit
c. electron shell
d. emission spectrum
____ 39. Which of the following describes why an element gives off an emission spectrum?
a. the electrons are arranged in the pattern 2, 8, 8
b. the electrons in an atom continuously give off energy
c. the electrons in a specific atom all have the same amount of energy
d. the electrons lose specific amounts of energy as they move into lower shells
____ 40. Which of the following is the standard atomic notation for the sodium-23 atom?
a.
b.
c.
d.
____ 41. How would an atom with 9 electrons have its electrons arranged?
a. 1st shell - 1, 2nd shell - 2, 3rd shell - 6
b. 1st shell - 2, 2nd shell - 7, 3rd shell - 0
c. 1st shell - 2, 2nd shell - 2, 3rd shell - 5
d. 1st shell - 3, 2nd shell - 3, 3rd shell - 3
____ 42. Which of the following is/are in the nucleus of an atom?
a. most of the mass
b. the positive charges
c. the uncharged particles
d. all of the above
____ 43. Which of the following defines mass number?
a. the number of protons in an atom
b. the number of neutrons in an atom
c. the number of protons plus neutrons in an atom
d. the number of neutrons minus protons in an atom
____ 44. Which of the following defines atomic number?
a. the number of protons in an atom
b. the number of neutrons in an atom
c. the number of protons plus neutrons in an atom
d. the number of protons, neutrons, and electrons in an atom
____ 45. A new element, Heavium, has been discovered with 120 protons and 245 neutrons. What is its mass number?
a. 120
b. 125
c. 245
d. 365
____ 46. What is the number of protons, neutrons, and electrons in an atom of cesium-133?
a. 55 protons, 55 neutrons, 78 electrons
b. 55 protons, 78 neutrons, 55 electrons
c. 55 protons, 78 neutrons, 78 electrons
d. 78 protons, 133 neutrons, 55 electrons
____ 47. What is the number of protons, neutrons, and electrons in an ion of zirconium-90?
a. 40 protons, 50 neutrons, 36 electrons
b. 40 protons, 50 neutrons, 40 electrons
c. 44 protons, 50 neutrons, 40 electrons
d. 90 protons, 50 neutrons, 44 electrons
____ 48. Which of the following can be determined about an element from the periodic table?
a. symbol
b. atomic mass
c. atomic number
d. all of the above
____ 49. What is the atomic mass of hydrogen?
a. 0.0899
b. 1–
c. 1+
d. 1.01
____ 50. What did Bohr propose that the emission spectrum of an element is caused by?
a. electrons leaving the atom
b. protons moving from the nucleus to one of the energy levels
c. electrons moving from a higher energy level to a lower energy level
d. electrons moving from a lower energy level to a higher energy level
____ 51. Which of the following is the correct arrangement of electrons in a sulphur atom?
a. 2, 8, 6
b. 2, 6, 8
c. 6, 8, 2
d. 2, 8, 2, 4
____ 52. Which of the following is the number of electrons in the outermost orbit of a phosphorus atom?
a. 2
b. 3
c. 5
d. 8
____ 53. Why does a potassium ion have a charge of 1+?
a. It has one more proton than the number of electrons.
b. It has one more electron than the number of protons.
c. It has one more proton than the number of neutrons.
d. It has one more proton than the number of neutrons.
____ 54. When compounds containing certain metals are placed in a flame, different flame colours are produced. For
example, sodium compounds always produce yellow flames. Which of the following explains why this
happens?
a. All atoms of the metal have the same mass.
b. All atoms of the metal have the same number of protons.
c. All atoms of the metal have the same number of neutrons.
d. All atoms of the metal have the same electron arrangement.
Completion
Complete each statement.
55. Molecules form when two or more ____________________ elements combine.
56. A neutron has a(n) ____________________ charge and the same mass as a(n) ____________________.
57.
____________________ discovered the electron.
58. Electrons are located in defined ____________________, which are located at certain distances from the
nucleus.
59. The particles that make up most of the mass in an atom are the ____________________ and
____________________.
60. Atomic number is the number of ____________________ in an atom.
61. The total number of protons and neutrons in an atom is called the ______________________________.
62. Bohr stated that as elements move to higher shells they ____________________ energy, and as they move to
lower shells they ____________________ energy.
63. The number of electrons allowed in the first three energy shells is ____________________,
____________________, and ____________________.
64.
is the standard atomic notation for the _________________________ atom.
65. When an atom gains electrons, a ____________________ ion is formed.
66. The atomic mass of an element is the average of the ____________________ numbers of all the naturally
occurring isotopes, taking into account the natural abundance of the isotopes.
67. Bromine-79 and bromine-81 are two different ____________________ of the element.
68. To form a positive ion an atom ____________________ electrons.
69. Non-metallic elements (except for the noble gases) form ____________________ ions.
70. ____________________ elements are the most reactive metals because their single outer electron is easily
given up.
71. When sulphur forms the 2- ion, it has a full outer shell like the noble gas, ____________________.
72. The ____________________ shell of electrons is involved in chemical reactions.
73. Ionic compounds do not form molecules, they form ____________________.
Chapter 7 Review
Answer Section
MODIFIED TRUE/FALSE
1. ANS: F, too small
PTS:
TOP:
2. ANS:
OBJ:
3. ANS:
1
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Unit B - Ch. 07 KI2
T
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F, negative
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1
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Unit B - Ch. 07 KI2
T
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F, nucleus
LOC: Unit B - PLC1
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REF: K
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6. ANS: F, neutrons
REF: K
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REF: K
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8. ANS:
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1
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Unit B - Ch. 07 KI2
T
PTS: 1
7.2
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T
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7.2
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F, furthest
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1
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Unit B - Ch. 07 KI2
T
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7.2
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F, protons plus neutrons
LOC: Unit B - PLC1
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OBJ:
1
REF: K
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Unit B - Ch. 07 KI4
T
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7.2
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LOC: Unit B - PLC1
REF:
TOP:
REF:
TOP:
K
Unit B - Ch. 07 KI3
K
Unit B - Ch. 07 KI3
REF: K
TOP: Unit B - Ch. 07 KI2
REF: U/A
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13. ANS: F,
PTS: 1
REF: U/A
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14. ANS: F, protons
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
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TOP: Unit B - Ch. 07 KI4
15. ANS: F, mass number
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17. ANS:
OBJ: 7.2 | 7.3
LOC: Unit B - PLC1
1
REF: K
OBJ: 7.2 | 7.3
Unit B - Ch. 07 KI4
T
PTS: 1
7.2 | 7.3
LOC: Unit B - PLC1
F, atomic number
LOC: Unit B - PLC1
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18. ANS: F, negative ion
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20. ANS:
OBJ: 7.2 | 7.3
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1
REF: U/A
OBJ: 7.2 | 7.3
Unit B - Ch. 07 KI4
T
PTS: 1
7.3
LOC: Unit B - PLC1
F, positive 1
LOC: Unit B - PLC1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 07 KI3
21. ANS: F
Group 14
Group IVA
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23. ANS:
REF: K
TOP: Unit B - Ch. 07 KI4
REF: K
TOP: Unit B - Ch. 07 KI3
OBJ: 7.3
LOC: Unit B - PLC1
1
REF: U/A
OBJ: 7.3
Unit B - Ch. 07 KI3
T
PTS: 1
7.3
LOC: Unit B - PLC1
F, 28 electrons
LOC: Unit B - PLC1
REF: K
TOP: Unit B - Ch. 07 KI3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 07 KI4
24. ANS: F, gains electrons
OBJ: 7.3
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI3
25. ANS: F, positive
OBJ: 7.3
LOC: Unit B - PLC1
1
REF: K
OBJ: 7.3
Unit B - Ch. 07 KI3
T
PTS: 1
7.3
LOC: Unit B - PLC1
T
PTS: 1
7.4
LOC: Unit B - PLC1
F, Group 18
LOC: Unit B - PLC1
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27. ANS:
OBJ:
28. ANS:
PTS: 1
REF: K
OBJ: 7.4
REF:
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REF:
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K
Unit B - Ch. 07 KI3
K
Unit B - Ch. 07 KI4
LOC: Unit B - PLC1
TOP: Unit B - Ch. 07 KI4
MULTIPLE CHOICE
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50. ANS:
LOC:
C
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Unit B - PLC1
D
PTS:
Unit B - PLC1
D
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B
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Unit B - PLC1
A
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Unit B - PLC1
D
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Unit B - PLC1
B
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D
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A
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D
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Unit B - PLC1
D
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Unit B - PLC1
A
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Unit B - PLC1
B
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Unit B - PLC1
D
PTS:
Unit B - PLC1
C
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Unit B - PLC1
A
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Unit B - PLC1
D
PTS:
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B
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Unit B - PLC1
A
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Unit B - PLC1
D
PTS:
Unit B - PLC1
D
PTS:
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C
PTS:
Unit B - PLC1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
1
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K
OBJ:
Unit B - Ch. 07 KI2
K
OBJ:
Unit B - Ch. 07 KI2
K
OBJ:
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K
OBJ:
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U/A
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K
OBJ:
Unit B - Ch. 07 KI2
K
OBJ:
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K
OBJ:
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K
OBJ:
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K
OBJ:
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U/A
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U/A
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U/A
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K
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U/A
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U/A
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U/A
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K
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K
OBJ:
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U/A
OBJ:
Unit B - Ch. 07 KI4
7.1
7.1
7.1
7.1
7.1
7.1 | 7.2 | 7.3 | 7.4
7.1
7.1
7.1
7.2
7.2
7.2
7.2
7.2
7.2
7.2
7.2
7.2
7.3
7.3
7.3
7.2
51. ANS:
LOC:
52. ANS:
LOC:
53. ANS:
LOC:
54. ANS:
LOC:
A
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C
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A
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D
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1
1
1
1
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U/A
OBJ:
Unit B - Ch. 07 KI4
7.2
7.2
7.3
7.4
COMPLETION
55. ANS:
non-metal
non-metallic
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
56. ANS: neutral, proton
OBJ: 7.1
LOC: Unit B - PLC1
PTS: 2
REF: K
TOP: Unit B - Ch. 07 KI2
57. ANS: Thomson
OBJ: 7.1
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
58. ANS:
shells
orbits
OBJ: 7.1
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
59. ANS: protons, neutrons
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
60. ANS: protons
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
61. ANS: mass number
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI2
62. ANS: gain, lose
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI3
63. ANS:
2, 8, 8
OBJ: 7.2
LOC: Unit B - PLC1
two, eight, eight
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
64. ANS: fluorine-19
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 07 KI4
65. ANS: negative
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 07 KI4
66. ANS: mass
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
67. ANS: isotopes
OBJ: 7.3
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
68. ANS: loses
OBJ: 7.2 | 7.3
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
69. ANS: negative
OBJ: 7.2
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
70. ANS:
Group 1
Alkali metal
OBJ: 7.3
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
71. ANS: argon
OBJ: 7.4
LOC: Unit B - PLC1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 07 KI4
72. ANS: outermost
OBJ: 7.4
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
73. ANS:
crystals
formula units
OBJ: 7.4
LOC: Unit B - PLC1
PTS: 1
REF: K
TOP: Unit B - Ch. 07 KI4
OBJ: 7.4
LOC: Unit B - PLC1