Chem 106 Midterm Study Questions
Name: __________________________
Chapters 1-5,11-12
Review Mon 10/10/2016
Due 10/13/2016 (Midterm exam)
This is a homework assignment. Please show your work for full credit. If you do work on
separate paper, attach the work to these.
Useful information to be provided on exam:
TF  1.8TC  32
TC 
TF  32
1.8
Mass
1 lb = 453.6 g *
1 kg = 2.205 lb *
TK  TC  273
Length
1 in = 2.54 cm
1 m = 1.094 yd *
1 mi = 1.609 km *
1. Define the following terms:
a. science
b. chemistry
2. Write 8,353 in standard scientific notation.
A) 8353
B) 8.353  10–3
C) 835.3  101
D) 8.353  1000
E) 8.353  103
3. The number 0.005876 expressed in scientific notation is
A) 5.88  103
B) 5.876  103
C) 5.88  10–3
D) 5.876  10–3
E) 5876  10–6
Page 1
TC  TK  273
Volume
1 L = 1.0567 qt*
1 ft3 = 28.32 L *
4. 4.9 kilograms contain this many grams.
A) 4.9  103
B) 4.9  102
C) 4.9  101
D) 4.9  10–2
E) 4.9  10–3
5. Convert: 1.0 mm = _____________ km.
A) 1.0  10–6 km
B) 1.0  10–3 km
C) 1.0  103 km
D) 1.0  106 km
E) 1.0  102 km
6. Convert 592.4 m to decimeters.
A) 5.924  104 dm
B) 59.24 dm
C) 5.924 dm
D) 5.924  103 dm
E) none of these
7. 6.9 milliseconds is equal to how many seconds?
A) 6.9  103 s
B) 6.9  102 s
C) 6.9  10–3 s
D) 6.9  10–2 s
E) 0.69 s
8. Using the rules of significant figures, calculate the following:
6.167 + 70 =
A) 76
B) 80
C) 76.167
D) 77
E) 76.17
Page 2
9. The number 2.00152 rounded to four significant figures is
A) 2.002
B) 2.001
C) 2.000
D) 2.152
E) none of these
10. How many significant figures are in the number 1000.0?
A) 1
B) 2
C) 3
D) 4
E) 5
11. A student finds that the weight of an empty beaker is 12.024 g. She places a solid in the
beaker to give a combined mass of 12.108 g. To how many significant figures is the
mass of the solid known?
A) 1
B) 2
C) 3
D) 4
E) 5
12. The product of 0.1400  6.02  1023 will have how many significant figures?
A) 2
B) 3
C) 23
D) 1023
E) 7
13. Convert: 322.3 K = ________________ oC.
A) 595.3oC
B) 49.3oC
C) 612.1oC
D) 211.1oC
E) 179.1oC
Page 3
14. Convert: –37.5oF = _______________ oC.
A) –38.6oC
B) –3.1oC
C) –125.1oC
D) –9.9oC
E) 235.5oC
15. An object is 105.1 inches in height. Express this height in centimeters.
A) 41.38 cm
B) 0.02417 cm
C) 8.76 cm
D) 267.0 cm
E) 107.6 cm
16. 226.8oF is equivalent to
A) 143.8oC
B) 108.2oC
C) 350.6oC
D) 465.8oC
E) 126.0oC
17. What is the mass in pounds of a human who weighs 81.30 kg?
A) 179.3 lb
B) 36.87 lb
C) 159.3 lb
D) 83.51 lb
E) none of these
18. The density of gold is 19.3 g/mL. What is the volume of a gold nugget that weighs 73.8
g?
A) 1.42  103 mL
B) 3.82 mL
C) 0.262 mL
D) 54.5 mL
E) none of these
Page 4
19. A graduated cylinder contains 20.0 mL of water. An irregularly shaped object is placed
in the cylinder, and the water level rises to the 31.2-mL mark. If the object has a mass of
96.3 g, what is its density?
A) 8.60 g/mL
B) 0.116 g/mL
C) 3.09 g/mL
D) 4.81 g/mL
E) none of these
20. Which of the following is a chemical change?
A) Water condenses on a mirror.
B) A damp towel dries.
C) Peanuts are crushed.
D) A “tin” can rusts.
E) At least two of the above (a-d) exhibit a chemical change.
21. If iodine melts at 114°C and boils at 184°C, what is its physical state at 120°C?
22. Which of the following is an element?
A) air
B) water
C) salt
D) helium
E) sugar
23. Which is an example of a homogeneous mixture?
A) vodka
B) oily water
C) soil (dust)
D) sodium chloride
E) aluminum
24. True or False? The normal boiling point of water is 100oC, which is a physical property
of the substance water.
A) True
B) False
Page 5
25. True or False? Metal rusting is an example of a chemical change.
A) True
B) False
26. Which statement below is incorrect?
A) Dalton's statement "All atoms of a given element are identical" is no longer
accepted because of the existence of isotopes and ions.
B) O3 (ozone) is considered a molecule but is not considered an element.
C) The number in the measurement "12 apples" has an infinite number of significant
figures.
D) Rutherford's discovery revealed the atom is mostly made up of empty space.
E) At least two of the above statements (a-d) are incorrect.
27. The total number of atoms indicated by the formula Ca3(PO4)2 is
A) 4
B) 8
C) 12
D) 13
E) 6
28. Which atomic particle determines the chemical behavior of an atom?
A) proton
B) electron
C) neutron
D) nucleus
E) none of these
29. Which particle has the smallest mass?
A) neutron
B) proton
C) electron
D) helium nucleus
30. An atom with 15 protons and 16 neutrons is an atom of
A) P
B) Ga
C) S
D) Pd
E) Rh
Page 6
31. A certain isotope X+ contains 54 electrons and 78 neutrons. What is the mass number
for this element?
A) 133
B) 132
C) 131
D) 55
E) 53
32. The number of protons in the nucleus of an atom is called its
A) mass number
B) valence
C) isotope number
D) atomic number
E) none of these
33. Which pair have approximately the same mass?
A) a hydrogen, 11 H , and a deuterium, 21 H , atom
B) a neutron and an electron
C) a proton and a neutron
D) an electron and a proton
34. Which of the following elements is an alkaline earth metal?
A) Ca
B) Cu
C) Fe
D) Na
E) Sc
35. Which of the following elements is most similar to chlorine?
A) H
B) He
C) Na
D) Hg
E) Br
36. How many protons, electrons, and neutrons does the isotope
Page 7
57
26
Fe3 have?
37. The form of EMR that has a longer wavelength than infrared rays but a shorter
wavelength than radio waves is
A) microwaves
B) untraviolet
C) gamma rays
D) X rays
E) none of these
38. Which color of visible light has the lowest frequency?
A) violet
B) blue
C) green
D) yellow
E) red
39. According to the Bohr model of the atom, the energy levels of the hydrogen atom (and
all atoms) are ______________, meaning that only certain discrete energy levels are
allowed.
A) varied
B) quantized
C) ramp-like
D) continuous
E) two of these
40. Which of the following is a reasonable criticism of the Bohr model of the atom?
A) It makes no attempt to explain why the negative electron does not eventually fall
into the positive nucleus.
B) It does not adequately predict the line spectrum of hydrogen.
C) It does not adequately predict the ionization energy of the valence electron(s) for
elements other than hydrogen.
D) It does not adequately predict the ionization energy of the first-energy-level
electrons for one-electron species for elements other than hydrogen.
E) It shows the electrons to exist outside the nucleus.
41. The f sublevel allows a maximum of ______________ orbital(s).
A) 1
B) 3
C) 5
D) 7
E) 9
Page 8
42. The maximum number of electrons allowed in the p sublevel of the third principal level
is
A) 1
B) 2
C) 3
D) 6
E) 8
43. The maximum number of electrons allowed in the fourth energy level is
A) 2
B) 4
C) 8
D) 18
E) 32
44. The number of unpaired electrons in a nitrogen atom is
A) 1
B) 2
C) 3
D) 4
E) 5
45. Which below is the correct ground-state electron configuration for oxygen.
A) [He]2s22p4
B) [He]2s22p6
C) [Ne]2s22p4
D) [He]3s23p4
E) [He]1s22p6
46. The alkaline earth metals have how many valence electrons?
A) 8
B) 7
C) 3
D) 2
E) 1
Page 9
47. How many electrons are in the third principal energy level (n = 3) of one atom of Fe?
A) 2
B) 8
C) 14
D) 18
E) none of these
48. When moving down a group (family) in the periodic table, the number of valence
electrons
A) remains constant
B) increases by 2 then 8 then 18 then 32
C) doubles with each move
D) decreases regularly
E) changes in an unpredictable manner
49. The electron configuration for manganese is
A) [Ar] 3d7
B) 1s22s22p63s13d6
C) [Ar] 4s23d5
D) 1s22s22p63s23d4
E) [Ar] 4s24p5
50. Which of the following atoms has the electron configuration 1s22s22p63s23p64s23d1?
A) Sc
B) Ca
C) Sr
D) Ar
E) none of these
51. What element has the electron configuration 1s22s22p63s23p64s23d104p5?
A) Cl
B) Se
C) I
D) Kr
E) Br
Page 10
52. What element has the electron configuration 1s22s22p63s23p64s23d104p65s24d105p66s2?
A) Ba
B) Sn
C) Pb
D) Po
E) none of these
53. Write the electron configuration for Cd.
54. Write the electron configuration for Cl.
55. Write the electron configuration for Rb.
56. Which of the following is ranked in order of largest to smallest atomic radius?
A) Rb > Mn > S > Ge > F
B) F > S > Ge > Mn > Rb
C) Mn > Rb > F > S > Ge
D) Rb > Ge > Mn > F > S
E) Rb > Mn > Ge > S > F
57. Which of the following atoms has the highest ionization energy?
A) Al
B) Si
C) P
D) As
E) Sb
58. Order the elements S, Cl, and F in terms of increasing ionization energy.
A) S, Cl, F
B) Cl, F, S
C) F, S, Cl
D) F, Cl, S
E) S, F, Cl
59. Which has the higher ionization energy, K or Br?
Page 11
60. True or false: Covalent bonding occurs when electrons are shared by nuclei.
A) True
B) False
61. True or false? The greater the difference in electronegativity between two bonded
atoms, the more polar the bond.
A) True
B) False
62. True or false? N2 is an example of a covalent bond.
A) True
B) False
63. Draw the Lewis structures for the following compounds and use VSEPR theory to
answer the question.
CBr2H2
BH3
SO2
CS2
HCl
Which compound has bond angles of 109.5˚ around the central atom?
A) CBr2H2
B) BH3
C) SO2
D) CS2
E) HCl
64. Which of the following compounds contains an ionic bond?
A) HCl(g)
B) NaCl
C) CCl4
D) SO2
E) O2
65. The most electronegative element of those listed is
A) Rb
B) Cs
C) Fr
D) K
E) Li
Page 12
66. In ionic bonding
A) the electrons are shared between the atoms.
B) the atoms are repelled by each other.
C) the bonding that occurs is usually between two nonmetal atoms.
D) a noble gas configuration is formed for each element or ion.
E) At least two of the above statements are correct.
67. Which of the following atoms has the greatest electronegativity?
A) Na
B) Rb
C) Cl
D) Se
68. Which of the following has nonpolar bonds?
A) H2S
B) HCl
C) Br2
D) OF2
E) All are nonpolar.
69. Which of the following bonds is non-polar?
A) N-H
B) O-H
C) F-H
D) H-H
E) S-H
70. True or false? The F- and O2- ions have the same electron configuration.
A) True
B) False
71. The electron configuration for the bromide ion is identical to that of
A) Br
B) Kr
C) K
D) IE) none of these
Page 13
72. Calcium reacts with fluorine to form a compound with which formula below?
A) CaF
B) CaF2
C) Ca2F
D) Ca2F3
E) none of these
73. Which element or ion listed below has the electron configuration 1s22s22p63s23p6?
A) S
B) Ne
C) Cl
D) S2E) none of these
74. Draw the Lewis electron structure for the sulfur atom.
75. The Lewis structure for which of the following contains the greatest number of
nonbonding electrons?
A) CH4
B) HF
C) F2
D) H2O
E) H2
Page 14
76. Choose the correct Lewis structure for the NH4+ ion.
A)
H
..
+
H . N . H
.
H
B)
H
..
+
.
.
H . N . H
..
H
C)
..
.
.
H . N . H
..
H
D)
H
.
.
H
N . H
.
H
E)
+
+
none of these
77. Draw the Lewis electron structure for the HI molecule.
78. Draw the Lewis structure for SiH4.
79. Draw the Lewis structure for Na2O. hint: there are no covalent bonds; this structure is
ionic
80. Which of the following has a double bond?
A) H2O
B) NH3
C) O2
D) CO
E) H2S
Page 15
81. Which of the following molecules have tetrahedral geometry? (Check all that apply.)
A) HBr
B) NO3−
C) H2O
D) SiF4
E) BrO4−
82. Which of the following molecules has a 120o bond angle? (Check all that apply.)
A) HBr
B) NO3–
C) H2O
D) BF3
E) NH3
83. Draw the Lewis Structure and predict the 3-dimensional geometry of each molecule
below, including bond angles.
NO2−
C2H4 (note: there are two central atoms)
PF3
84. The charge on a barium ion in its ionic compound is
A) +1
B) +2
C) +3
D) -1
E) Various charges are possible.
85. The name for the NO3- ion is
A) nitrate ion
B) nitrite ion
C) nitrogen ion
D) nitric ion
E) nitrous ion
Page 16
86. The formula for the compound formed from the polyatomic ions NH4+ and PO43- is
A) NH4(PO4)3
B) NH4PO4
C) (NH4)3PO4
D) (NH4)2(PO4)2
87. Potassium chlorate has the formula
A) KCl
B) KClO
C) KClO2
D) KClO3
E) KClO4
88. The name for the compound Fe2O3 is ______________.
89. The name for PbS2 is ______________.
90. Give the formula for magnesium phosphate.
91. Give the formula for sodium chromate.
92. Give the formula for titanium(IV) chloride.
93. Give the name for Al(OH)3.
Page 17
Answer Key
1. a. Acquisition of knowledge of the natural universe through the use of the Scientific
Method.
b. The science that deals with matter and the changes it undergoes.
Chapter: 1.2,1.3
2. E
Chapter: 2.1
3. D
Chapter: 2.1
4. A
Chapter: 2.6
5. A
Chapter: 2.6
6. D
Chapter: 2.6
7. C
Chapter: 2.6
8. B
Chapter: 2.5
9. A
Chapter: 2.5
10. E
Chapter: 2.5
11. B
Chapter: 2.5
12. B
Chapter: 2.5
13. B
Chapter: 2.7
14. A
Chapter: 2.7
15. D
Chapter: 2.6
16. B
Chapter: 2.7
17. A
Chapter: 2.6
18. B
Chapter: 2.8
19. A
Chapter: 2.8
20. D
Chapter: 3.2
21. liquid
Page 18
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
Chapter: 3.1
D
Chapter: 3.3
A
Chapter: 3.4
A
Chapter: 3.2
A
Chapter: 3.2
B
Chapter: 4.3,4.9,2.4,4.5
D
Chapter: 4.4
B
Chapter: 4.6
C
Chapter: 4.6
A
Chapter: 4.7
A
Chapter: 4.7
D
Chapter: 4.7
C
Chapter: 4.7
A
Chapter: 4.8
E
Chapter: 4.8
The isotope contains 26 protons, 23 electrons, and 31 neutrons.
Chapter: 4.7,4.10
A
Chapter: 11.2
E
Chapter: 11.2
B
Chapter: 11.5
C
Chapter: 11.5
D
Chapter: 11.8
D
Chapter: 11.8
E
Chapter: 11.8
Page 19
44. C
Chapter: 11.10
45. A
Chapter: 11.9
46. D
Chapter: 11.10
47. C
Chapter: 11.10
48. A
Chapter: 11.10
49. C
Chapter: 11.10
50. A
Chapter: 11.10
51. E
Chapter: 11.10
52. A
Chapter: 11.10
53. [Kr] 5s24d10
Chapter: 11.10
54. [Ne] 3s23p5
Chapter: 11.10
55. [Kr] 5s1
Chapter: 11.10
56. E
Chapter: 11.11
57. C
Chapter: 11.11
58. A
Chapter: 11.11
59. Br
Chapter: 11.11
60. A
Chapter: 12.1
61. A
Chapter: 12.3
62. A
Chapter: 12.3
63. A
Chapter: 12.6,12.9
64. B
Chapter: 12.1,12.2
65. E
Chapter: 12.2
66. D
Page 20
67.
68.
69.
70.
71.
72.
73.
74.
Chapter:
C
Chapter:
C
Chapter:
D
Chapter:
A
Chapter:
B
Chapter:
B
Chapter:
D
Chapter:
12.1,12.4,12.5
12.2
12.3
12.3
12.4
12.4
4.x,12.5,4.11
12.4
..
. .
. S
.
Chapter: 12.6
75. C
Chapter: 12.6
76. B
Chapter: 12.6
..
77.
.
H — I .
..
Chapter: 12.6
78.
H
—
H — Si — H
—
H
Chapter: 12.6
79.
[Na]
[Na]
+
+
Chapter:
80. C
Chapter:
81. D, E
Chapter:
82. B, D
Chapter:
..
. .
.O.
..
2–
12.6
12.7
12.9
12.9
Page 21
83.
84.
85.
86.
87.
88.
Chapter: 12.6,7,8,9
B
Chapter: 4.10
A
Chapter: 5.5
C
Chapter: 5.5
D
Chapter: 5.5
iron(III) oxide
Chapter: 5.2
Page 22
89. lead(IV) sulfide
Chapter: 5.2
90. Mg3(PO4)2
Chapter: 5.5
91. Na2CrO4
Chapter: 5.5
92. TiCl4
Chapter: 5.2
93. aluminum hydroxide
Chapter: 5.5
Page 23