Unit 2 Review
Modified True/False
Indicate whether the sentence or statement is true or false. If false, change the identified word or phrase to make the
sentence or statement true.
____
1. Bohr's atomic theory states that electrons may only possess specific amounts of energy.
____________________
____
2. The quantum mechanical model of the atom is capable of determining the exact location of an electron in an
atom. ____________________
____
3. All alkali earth metals have valence electrons in s orbitals when they are in their ground state.
____________________
____
4. The hydrogen atom will produce a complete spectrum when it is energized. ____________________
____
5. Schrodinger's equation describes the electron as a wave. ____________________
____
6. Transition metals are monovalent because they attempt to get more stable electron configurations like halffilled and empty orbitals. ____________________
____
7. The 2p orbitals in oxygen have three unpaired electrons. ____________________
____
8. The shape of SO2 is trigonal planar. ____________________
____
9. Absorption spectra are the result of energy that has been absorbed by electrons. ____________________
____ 10. Electrons are most likely found near the nucleus, regardless of the type of orbital they 'occupy'.
____________________
____ 11. The Pauli exclusion principle requires that two electrons in the same orbital have the same spin.
____________________
____ 12. Quantum mechanics involves using probabilities to determine the shape of an atom. ____________________
____ 13. The electron configuration for sulfur, S is shown below. _________________________

3p

3s

2p

2s

1s
____ 14. The valence p orbitals in phosphorus, P, are half-filled. ____________________
____ 15. All of the valence electrons in Fe2+ must have the same spin. _________________________
____ 16. Hund's rule states that you must fill electrons into the lowest energy levels first.
_________________________
____ 17. A laser produces monochromatic light. _________________________
____ 18. Spectrophotometers cannot be used for qualitative observations. _________________________
____ 19. X-rays are made up of extremely high energy photons. _________________________
____ 20. MRI stands for magnetic reflection imaging. ______________________________
____ 21. A photon of light is equal to one quantum of energy. ____________________
____ 22. Superconductors are substances that conduct electricity with extremely low voltage.
_________________________
____ 23. The energy of electrons is quantized as photons. _________________________
____ 24. Ionic compounds have higher melting points than molecular compounds because of strong attractive forces
between particles. _________________________
____ 25. The shape of boron trifluoride, BF3, is tetrahedral. ______________________________
____ 26. VSEPR theory predicts molecular shapes based on keeping protons as far apart as possible.
_________________________
____ 27. Carbon tetrafluoride, CF4, contains four polar bonds and is a polar molecule. _________________________
____ 28. The surface tension of water is due to the hydrogen bonding between water molecules.
_________________________
____ 29. A molecule whose central atom is surrounded by two lone pairs and four atoms will have a square planar
shape. _________________________
____ 30. CH3Cl is a polar molecule. _________________________
____ 31. An ionic compound would be expected to have a low melting point. _________________________
____ 32. Diamond does not conduct electricity because it contains delocalized electrons.
______________________________
____ 33. Molten or dissolved ionic compounds conduct electricity because they contain delocalized electrons.
_________________________
____ 34. Sulfur dioxide, SO2, is a bent molecule with a bond angle that is slightly less than 109o.
_________________________
____ 35. Xenon tetrafluoride, XeF4, is a tetrahedral molecule. _________________________
____ 36. Methane, CH4, contains polar bonds. _________________________
____ 37. Carbon dioxide, CO2, is a polar molecule. _________________________
____ 38. Water is adhesive because it is bi-polar. _________________________
____ 39. Hydrogen bonding may explain why ice is less dense than liquid water. _________________________
____ 40. Dr. Richard Bader uses computers to create electron density maps for large complex molecules.
______________________________
____ 41. Dr. Robert LeRoy developed a technique for determining bond lengths. ______________________________
____ 42. Dr. Robert LeRoy is interested in intermolecular forces. _________________________
____ 43. A dipole occurs when two atoms with similar electronegativities bond to each other.
_________________________
Completion
Complete each sentence or statement.
44. A region in which there is a high probability of finding an electron is called an ____________________.
45. Bohr's model works perfectly for ____________________.
46. ____________________ determined that it is impossible to predict the exact location of an electron.
47. ____________________ orbitals are non-directional.
48. There are ____________________ different orientations in space for p-orbitals.
49. When an electron is in its lowest energy level, it is in the ____________________.
50. In his model of the atom, Bohr identified each energy level using an integer, n, and called it the
___________________________________.
51. Cl1-, Ar and Ca2+ are ____________________.
52. ____________________ are high energy electromagnetic radiation.
53. ____________________ produce parallel, monochromatic light.
54. Spin changes in hydrogen nuclei of water molecules can be detected using
______________________________.
55. At extremely low temperatures, helium is a ____________________.
56. S-block elements are all ____________________.
57. A photon is a ____________________ of light.
58. The electron configuration for ____________________ is 1s22s22p63s23p6.
59. The oxide, O2-, is ____________________ with neon, Ne.
60. The "1" in helium's (He) electron configuration represents the ____________________.
61. The concept of the duality of matter means that an electron is both a particle and a _____________________.
62. The surface tension of water is due to the _________________________ between its particles.
63. ____________________ of electrons take up more room than bonded pairs.
64. The shape of sulfur dioxide would most likely be ____________________.
65. The shape of MnI5 would most likely be ______________________________.
66. The metal ions in a metallic solid are surrounded by delocalized electrons because metals have low
_________________________.
67. The shape of sulphur hexachloride, SCl6, is ____________________.
68. The shape of methane, CH4, is ____________________.
69. The shape of ammonia, NH3, is ______________________________.
70. The shape of xenon tetrafluoride, XeF4, is _________________________.
71. The shape of beryllium fluoride, BeF2, is ____________________.
72. The shape of boron trihydride, BH3, is _________________________.
73. The shape of hydrogen sulfide, H2S, is ____________________.
74. The shape of phosphorus pentahydride, PH5, is ___________________________________.
75. VSEPR theory predicts the ____________________ of molecules.
76. The molecules in any glue must have the ability to ____________________ with molecules of other
substances.
77. _________________________ tend to be brittle.
78. Due to its structure, diamond is classified as a _________________________.
79. The electrostatic forces between ions in ionic compounds cause ____________________ boiling points.
80. Insects can walk on water because of ______________________________.
81. Dispersion forces are ____________________ than covalent bonds.
82. Adhesive properties of glues can be explained by examining _________________________ forces.
83. The large difference in electronegativities between hydrogen and chlorine produces a
____________________ in the hydrogen chloride molecule.
Essay
84. Ernest Rutherford is known as the father of nuclear chemistry. Describe his Gold Foil experiment and then
explain how he used this experimental evidence to hypothesize about the existence of a nucleus.
85. Compare and contrast the Bohr-Rutherford model of the atom with the quantum mechanical model.
86. Explain, in your own words, how Bohr developed his model of the atom.
87. Explain water's properties using what you know about its inter- and intramolecular forces.
88. Explain VSEPR theory in your own words. Use examples.
89. We are able to "see" the shapes of molecules with X-ray crystallography. However, even without this
technology, there is a great deal of evidence that water, H2O, is a bent, polar molecule. Discuss this evidence
and explain how it relates to our model of the water molecule.
90. Explain, in your own words, how to determine the polarity of a substance. Use examples if you wish.
91. Describe, in your own words, two allotropes of carbon. Include a comparison of physical and chemical
properties.
92. Describe some contributions that Canadians have made to the scientific community's understanding of the
structures and properties of chemicals.
Unit 2 Review
Answer Section
MODIFIED TRUE/FALSE
1. ANS: T
LOC: SP1.01
2. ANS: F, probable
LOC: SP1.02
3. ANS: T
LOC: SP1.03
4. ANS: F, line
LOC: SP1.01
5. ANS: T
LOC: SP1.02
6. ANS: F, multi-valent
LOC: SP1.03
7. ANS: F, two
LOC: SP1.02
8. ANS: F
bent
angular
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.7
REF: K/U
OBJ: 3.6
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.7
REF: K/U
OBJ: 3.6
REF: I
OBJ: 3.5
REF: I
OBJ: 4.3
9. ANS: T
LOC: SP1.01
10. ANS: T
LOC: SP1.02
11. ANS: F, different spins
LOC: SP2.01
12. ANS: F
an orbital
orbitals
LOC: SP2.03
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.5
REF: K/U
OBJ: 3.6
REF:
13. ANS:
LOC:
14. ANS:
LOC:
15. ANS:
can
might
K/U
OBJ: 3.7
F, chlorine, Cl
SP2.02
T
SP2.02
F
LOC: SP2.01
REF: I
OBJ: 3.6
REF: I
OBJ: 3.6
REF:
16. ANS:
LOC:
17. ANS:
LOC:
I
OBJ: 3.6
F, Auf bau principle
SP2.02
T
SP3.01
LOC: SP2.02
REF: K/U
OBJ: 3.6
REF: MC
OBJ: 3.8
18. ANS:
LOC:
19. ANS:
LOC:
20. ANS:
LOC:
21. ANS:
LOC:
22. ANS:
LOC:
23. ANS:
LOC:
24. ANS:
LOC:
25. ANS:
LOC:
26. ANS:
LOC:
27. ANS:
LOC:
28. ANS:
LOC:
29. ANS:
LOC:
30. ANS:
LOC:
31. ANS:
LOC:
32. ANS:
LOC:
33. ANS:
LOC:
34. ANS:
LOC:
35. ANS:
LOC:
36. ANS:
LOC:
37. ANS:
LOC:
38. ANS:
LOC:
39. ANS:
LOC:
40. ANS:
LOC:
41. ANS:
LOC:
F, can
SP3.01
T
SP3.01
F, magnetic resonance imaging
SP3.01
T
SP1.01
F, resistance
SP3.02
T
SP1.01
T
SP2.05
F, trigonal planar
SP2.03
F, electron pairs
SP1.05
F, non polar
SP2.04
T
SP1.04
T
SP1.03
T
SP2.04
F, high
SP2.05
F, no delocalized electrons
SP1.04
F, [mobile] ions
SP1.04
F, 120o
SP2.03
F, square planar
SP2.03
T
SP2.04
F, non polar
SP2.04
F, polar
SP1.04
T
SP1.04
F, small simple molecules
SP3.03
F, small molecule radii
SP3.03
REF: MC
OBJ: 3.8
REF: MC
OBJ: 3.8
REF: MC
OBJ: 3.8
REF: K/U
OBJ: 3.3
REF: MC
OBJ: 3.7
REF: K/U
OBJ: 3.3
REF: K/U
OBJ: 4.6
REF: I
OBJ: 4.3
REF: K/U
OBJ: 4.3
REF: I
OBJ: 4.4
REF: K/U
OBJ: 4.5
REF: K/U
OBJ: 4.3
REF: I
OBJ: 4.4
REF: I
OBJ: 4.6
REF: K/U
OBJ: 4.6
REF: K/U
OBJ: 4.6
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: I
OBJ: 4.4
REF: I
OBJ: 4.4
REF: K/U
OBJ: 4.5
REF: K/U
OBJ: 4.5
REF: MC
OBJ: 4.3
REF: MC
OBJ: 4.5
42. ANS:
LOC:
43. ANS:
LOC:
T
SP3.03
F, very different
SP2.01
REF: MC
OBJ: 4.5
REF: I
OBJ: 4.4
44. ANS: orbital
LOC: SP2.01
45. ANS: hydrogen
LOC: SP1.01
46. ANS: Heisenberg
LOC: SP1.02
47. ANS: S
LOC: SP1.03
48. ANS: three
LOC: SP1.03
49. ANS: ground state
LOC: SP1.01
50. ANS: principal quantum number
LOC: SP1.01
51. ANS: iso-electronic
LOC: SP1.03
52. ANS: X-rays
LOC: SP3.01
53. ANS: Lasers
LOC: SP3.01
54. ANS:
MRI
magnetic resonance imaging
REF: C
OBJ: 3.5
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.7
REF: K/U
OBJ: 3.6
REF: K/U
OBJ: 3.6
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.4
REF: K/U
OBJ: 3.6
REF: MC
OBJ: 3.8
REF: MC
OBJ: 3.8
REF: MC
OBJ: 3.8
55. ANS: superconductor
LOC: SP3.02
56. ANS: metals
LOC: SP1.03
57. ANS:
packet
particle
LOC: SP3.01
REF: MC
OBJ: 3.7
REF: K/U
OBJ: 3.6
REF:
58. ANS:
LOC:
59. ANS:
LOC:
60. ANS:
LOC:
61. ANS:
LOC: SP2.01
REF: C
OBJ: 3.6
REF: C
OBJ: 3.6
REF: C
OBJ: 3.6
REF: K/U
OBJ: 3.7
COMPLETION
C
OBJ: 3.3
argon
SP2.02
iso-electronic
SP2.02
energy level
SP2.02
wave
LOC: SP1.02
62. ANS: hydrogen bonding
LOC: SP1.04
63. ANS:
Unbonded pairs
Lone pairs
REF: K/U
OBJ: 4.5
REF: K/U
OBJ: 4.3
64. ANS: bent
LOC: SP2.03
65. ANS: square pyramidal
LOC: SP2.03
66. ANS: electron affinity
LOC: SP1.04
67. ANS: octahedral
LOC: SP2.03
68. ANS:
tetrahedral
tetrahedron
LOC: SP1.05
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: K/U
OBJ: 4.6
REF: I
OBJ: 4.3
REF: I
69. ANS:
trigonal pyramidal
trigonal pyramid
OBJ: 4.3
LOC: SP2.03
REF: I
OBJ: 4.3
ANS: square planar
LOC: SP2.03
ANS: linear
LOC: SP2.03
ANS: trigonal planar
LOC: SP2.03
ANS: bent
LOC: SP2.03
ANS: trigonal bipyramidal
LOC: SP2.03
ANS: shape
LOC: SP1.05
ANS: bond
LOC: SP1.04
ANS:
Ionic compounds
Salts
LOC: SP2.03
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: I
OBJ: 4.3
REF: K/U
OBJ: 4.3
REF: MC
OBJ: 4.5
LOC: SP2.05
REF: I
OBJ: 4.6
REF: I
OBJ: 4.6
70.
71.
72.
73.
74.
75.
76.
77.
REF:
78. ANS:
LOC:
79. ANS:
LOC:
I
OBJ: 4.6
network solid
SP2.05
high
SP2.05
80. ANS:
LOC:
81. ANS:
LOC:
82. ANS:
LOC:
83. ANS:
LOC:
hydrogen bonding
SP1.04
weaker
SP1.04
intermolecular
SP3.02
dipole
SP2.04
REF: K/U
OBJ: 4.5
REF: K/U
OBJ: 4.6
REF: MC
OBJ: 4.5
REF: C
OBJ: 4.4