South Pasadena • Chemistry
Name
Period
Date
Chemistry
SEMESTER
1 FINAL
1. Which measurement below shows the temperature
to the correct precision?
EXAM
•
PRACTICE
6. The marks on the following target represent
someone who is:
20
mercury thread
30
(A) 26 °C
(B) 26.25 °C
(C) 26.3 °C
(D) 26.30 °C
2. 0.0120 grams has ___ significant figures.
(A) 2
(B) 3
(C) 4
(D) 5
(A) accurate, but not precise.
(B) precise, but not accurate.
(C) both accurate and precise.
(D) neither accurate nor precise.
7. Which measurement is the most precise?
(A) 4.2  .3 g
(B) 4.3  .1 g
(C) 4.5  .4 g
(D) 4.6  .2 g
3. In scientific notation, the number 3,020,000
should be written as:
(A) 3.02 × 106
(B) 3.02 ×10–6
(C) 302 ×104
(D) 302 ×10–4
8. The density of copper is known to be 8.96 g/mL.
A student’s experimental result shows that the
density of her copper cube is 8.79 g/mL. The
percent error in this data is ______.
(A) 0.17 %
(B) 0.98 %
(C) 1.90 %
(D) 1.93 %
4. Which value is the same as 1.52 x 10–3?
(A) 0.000152
(B) 0.00152
(C) 1520
(D) 152,000
9. Which of the following is a measure of length?
(A) cm3
(B) dm
(C) kg
(D) mL
5. How should the following computation be
recorded, with the correct number of significant
figures?
(1.15)(1.50)
(0.08206)(315)
(A) 0.0667
(B) 0.06673
(C) 0.067
(D) 6620
10. The average temperature on Venus is 460°C.
What is this in Kelvin?
(A) 187 K
(B) –187 K
(C) 273 K
(D) 733 K
11. Which one of the following statements is true?
(A) 1000 cm = 1 m
1
(B) 1 mm =
meter
100
(C) 1 kg = 1000 g
(D) each of these statements is true
12. What conversion factor would you use to convert
from feet to inches?
1 foot
(A) 12 inches
12 feet
(B)
1 inch
12 inches
(C) 1 foot
1 inch
(D) 12 feet
13. What conversion factor would you use to convert
milligrams to grams?
1000 mg
(A)
1g
1g
(B) 1000 mg
1 mg
(C) 1000 g
1000 g
(D) 1 mg
14. A metal cube of metal measures 2 cm on each
side. Its mass is 90.4 grams. What is the metal?
(A) Al (density = 2.70 g/cm3)
(B) Au (density = 19.3 g/ cm3)
(C) Fe (density = 7.86 g/ cm3)
(D) Pb (density = 11.3 g/ cm3)
15. What is the volume of a 5.08 gram sample of
liquid bromine? (density of bromine = 3.10 g/mL)
(A) 0.610 mL
(B) 1.64 mL
(C) 15.7 mL
(D) 8.18 mL
16. A gold block and a copper block both have a mass
of 5.0 kg. Which occupies a greater volume?
(Densities in g/cm3: gold = 19.3, copper = 8.94)
(A) Copper block
(B) Gold block
(C) They have the same volume.
(D) It cannot be determined.
17. The atom represented by 57Co3+ has:
(A) 27 protons, 30 neutrons, 24 electrons
(B) 27 protons, 30 neutrons, 30 electrons
(C) 27 protons, 57 neutrons, 3 electrons
(D) 30 protons, 27 neutrons, 3 electrons
18. All of the following describe a neutron EXCEPT:
(A) It determines the identity of the atom.
(B) It does not carry a charge.
(C) It is located in the nucleus.
(D) It, along with the proton, makes us most of the
atom’s mass.
19. Which of the following is an isotope of 40K?
(A) 39K
(B) 40K+
(C) 40Ar
(D) 40Ca
20. In which of the following states of matter are the
attractive forces between molecules strongest?
(A) Solid
(B) Liquid
(C) Gas
(D) Plasma
21. Which set consists only of elements?
(A) Na, Ca, H2
(B) H3O+, Cl–, I3–
(C) NaCl, CH4, Br2
(D) H2S, CuCl2, KI
22. What do the elements phosphorous and sulfur
have in common?
(A) They are both alkali metals.
(B) They are in the same family.
(C) They are in the same period.
(D) They both form ions with the same charges.
23. For the element F on the periodic table, the
number “19.00” represents:
(A) The average mass of all isotopes of F
(B) The mass number
(C) The number of neutrons
(D) The number of protons
24. Which of the following is NOT a typical property
of non-metals?
(A) They are dull in appearance.
(B) They are insulators.
(C) They can be ductile.
(D) They form anions.
25. The element sulfur forms an ion with what charge?
(A) +1
(B) +2
(C) –1
(D) –2
26. Which of the following name is correctly paired
with its formula?
(A) Carbonate
CO32–
(B) Chloride
ClO3–
(C) Ferric
Fe2+
(D) Nitrate
NO2–
27. Which of the following is a liquid non-metal atom
at room temperature?
(A) Barium
(B) Bromine
(C) Mercury
(D) Nitrogen
28. Which element is diatomic and typically forms a
cation with a charge of +1?
(A) Chlorine
(B) Hydrogen
(C) Nitrogen
(D) Sodium
29. The atomic mass of aluminum is 26.98. Which of
the following is correct?
(A) One aluminum atom has a mass of 26.98 amu.
(B) One aluminum atom has a mass of 26.98
grams.
(C) One mole of aluminum contains 26.98 atoms.
(D) One mole of aluminum has a mass of 26.98
grams.
30. Which of the following compounds is ionic?
(A) AlCl3
(B) HCl
(C) SCl2
(D) SiCl4
31. Which of the following compounds is
INCORRECTLY paired with its type of
compound?
(A) CaS
Ionic
(B) H2S
Acid
(C) CS2
Organic
(D) P4S3
Covalent
32. The compound (NH4)2CO3 contains how many
atoms of hydrogen?
(A) 2
(B) 4
(C) 6
(D) 8
33. What is the percent of carbon in barium carbonate,
BaCO3?
(molar mass = 197.3 g/mol)
(A) 3.04%
(B) 6.09%
(C) 14.0%
(D) 20.0%
34. What is the mass of one mole of aluminum sulfate,
Al2(SO4)3?
(A) 123 g
(B) 273 g
(C) 342 g
(D) 630 g
35. Which of the following is incorrect?
(A) 1 mole of O2 molecules has 6.02 × 1023
oxygen atoms.
(B) 1 mole of O2 molecules has a mass of 32
grams.
(C) 1 mole of O2 molecules occupy 22.4 liters at
STP.
(D) All of the above statements are correct.
36. What is the volume of 0.500 mole of carbon
dioxide gas, CO2, measured at STP?
(A) 5.60 liters
(B) 11.2 liters
(C) 33.6 liters
(D) 44.8 liters
37. How many moles of hydrogen cyanide, HCN, are
contained in 9.00 grams of HCN? (molar mass =
27.03 g/mol)
(A) 0.333
(B) 0.900
(C) 1.00
(D) 9.00
–2
38. How many molecules are in 2.00 × 10 moles of
carbon tetrachloride, CCl4? (molar mass = 154
g/mol)
(A) 1.20 × 1023
(B) 3.01 × 1023
(C) 6.02 × 1023
(D) 1.20 × 1022
43. The number of isomers of bromopropane, C3H7Br,
is
(A) 2
(B) 3
(C) 4
(D) 7
44. Which of the following is an isomer of the
compound below:
F
C
40. What is the bonding capacity of oxygen?
(A) 1
(B) 2
(C) 3
(D) 4
41. The general formula CnH2n describes the
molecular composition of the hydrocarbon family
known as the
(A) alkadienes
(B) alkanes
(C) alkenes
(D) alkynes
42. Structural formulas have advantages over
molecular formulas because they show the
(A) bonding arrangement of each carbon atom.
(B) geometric arrangement of the atoms.
(C) number of atoms of each element present.
(D) percentage composition of the compound.
C
H
(A)
F
(B)
C
F
H
H
F
C
(C)
C
F
H
F
F
C
C
H
(D)
H
F
H
C
39. Organic chemistry is the branch of chemistry that
is the study of
(A) compounds of carbon.
(B) compounds produced by living organisms.
(C) nonmetals.
(D) once-living organisms.
H
F
F
H
C
C
H
F
H
45. How many carbons make up the “parent chain” in
the following molecule?
(A) 4
(B) 5
(C) 6
(D) 7
46. Which of the following is the correct name for the
following compound:
H
H
H
Br
C
C
C
H
H
Br
H
(A) 1,1-dibromobutane
(B) 1,1-dibromopropane
(C) 2-bromopropane
(D) 3,3-dibromopropane
47. Which functional group is found in the following
compound?
H
H
H H
C
C
H
C
52. When an alcohol reacts with a carboxylic acid,
which of the following is formed?
(A) A ketone
(B) An ester
(C) An ether
(D) CO2
(A) Aldehyde
(B) Carboxylic Acid
(C) Ether
(D) Ketone
48. Which functional group is an “ether”?
(A)
(B)
(C)
(D)
49. The structure of which compound is given below?
H
H
C
C
H
H
51. When the equation for the combustion of propene,
C3H6, is balanced with the lowest whole-number
coefficients, what is the coefficient of oxygen, O2?
(A) 6
(B) 9
(C) 12
(D) 18
H
O
H
50. Which set of coefficients balances the equation for
the complete combustion of ethane, C2H6?
…C2H6 (g) + …O2 (g)  …CO2 (g) + …H2O (ℓ)
(A) 1,3,2,3
(B) 1,6,2,6
(C) 2,6,4,5
(D) 2,7,4,6
O
53. What is the formula for the ionic compound
formed when sodium ions and sulfide ions are
combined?
(A) Na2S
(B) Na2SO4
(C) NaS
(D) NaS2
54. In the compound Sn(SO4)2, what is the name of
the positive ion?
(A) stannic
(B) stannous
(C) strontium
(D) tin(II)
H
(A) Grain alcohol (ethanol)
(B) Isopropyl alcohol (2-propanol)
(C) Nail polish remover (acetone, or propanone)
(D) Vinegar (ethanoic acid)
55. An unknown element X forms a salt with the
formula XO2. Which of the following could be X?
(A) Al3+
(B) Ca2+
(C) Na+
(D) Sn4+
56. Which one of the following is the correct formula
for calcium phosphate?
(A) Ca2(PO4)3
(B) Ca3(PO4)2
(C) CaPO4
(D) PO4Ca3
57. Which of the following is the correct name for
CuSO4?
(A) Copper (I) sulfate
(B) Cupric sulfate
(C) Cupric sulfide
(D) Cuprous sulfate
58. What is the name of the compound N2O3?
(A) dinitride trioxide
(B) dinitrogen trioxide
(C) nitrate
(D) nitrogen oxide
59. In a sample of salt water, the salt is called the
(A) Precipitate
(B) Solute
(C) Solution
(D) Solvent
60. Which of the following compounds is expected to
be soluble in water?
(A) CaSO4
(B) FeS
(C) PbCl2
(D) SrBr2
61. How many grams of sodium hydroxide pellets,
NaOH, are required to prepare 50.0 mL of a 0.150
M solution? [molar mass NaOH = 40.0 g/mol]
(A) 0.300
(B) 2.00
(C) 3.00
(D) 200.
62. If 50 mL of a 200 mL sample of 0.10 M sodium
chloride solution is spilled, what is the
concentration of the remaining solution?
(A) 0.025 M
(B) 0.075 M
(C) 0.10 M
(D) 0.20 M
63. List the following solutions prepared with the
same solute in order of increasing concentration:
I. 30.0 g solute in a 240 mL solution
II. 30.0 g solute in a 120 mL solution
III. 60.0 g solute in a 120 mL solution
(A) I < II < III
(B) II < I < III
(C) II < III <I
(D) III < II < I
64. A 100 mL sample of a solution with a
concentration of 5.00 M is diluted to a new
volume of 400 mL with distilled water. The new
concentration will be
(A) 1.25 M
(B) 1.66 M
(C) 15.0 M
(D) 20.0 M
65. A property of acids are that they
(A) are caustic
(B) feel slippery
(C) neutralize water
(D) taste sour
66. Which of the following common solutions is
basic?
(A) Gatorade
(B) Lye (drain cleaner)
(C) Rubbing alcohol
(D) Vinegar
67. A solution tested with cabbage juice turns green.
Which of the following could be its pH?
(A) 1
(B) 4
(C) 7
(D) 10
68. A solution that conducts electricity very well is
called a:
(A) liquid conductor
(B) metallic solution
(C) strong electrolyte
(D) weak electrolyte
69. Which of the following substances is a considered
a strong electrolyte?
(A) C12H22O11 (sugar)
(B) H2O
(C) HF
(D) KBr
76. If a solution has [OH–] = 1.0 × 10–3 M, what is the
pH?
(A) 3
(B) 7
(C) 11
(D) 14
70. A substance that turns cabbage juice blue and
slightly lights up a light bulb is a:
(A) strong acid
(B) strong base
(C) weak acid
(D) weak base
77. What is the [OH–] in a solution in which [H+] is
1.0 × 10–6 M?
(A) 1.0 × 10–6 M
(B) 1.0 × 10–7 M
(C) 1.0 × 10–8 M
(D) 1.0 × 10–9 M
71. Which of the following represents the dissociation
of CaI2 in solution?
(A) CaI2  Ca + I2
(B) CaI2  Ca2+ + 2 I–
(C) CaI2 Ca2+ + 2 I–
(D) CaI2 is insoluble so it does not dissociate.
78. Which reaction below would be classified as a
single replacement reaction?
(A) 2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag
(B) 2 H2 + O2  2 H2O
(C) Ba(OH)2 + H2SO4  BaSO4 + 2 H2O
(D) NaHCO3  NaOH + CO2
72. The acid HClO3 is named:
(A) Chloric acid
(B) Hydrochloric acid
(C) Hydrogen chlorate
(D) Hydrogen chlorine trioxide
79. An acid was neutralized by the following reaction:
NaOH + HCl  NaCl + H2O
This reaction would be classified as
(A) decomposition
(B) double replacement
(C) single replacement
(D) synthesis
73. The formula for hydrosulfuric acid is:
(A) H2S
(B) H2SO4
(C) HS
(D) HSO4
74. Acids are substances that
(A) decrease the [H+]
(B) decrease the [H2O]
(C) increase the [H+]
(D) increase the [OH–]
75. Which chemical is the Bronsted-Lowry base?
NH3 + H2O  NH4+ + OH–
(A) H2O
(B) NH3
(C) NH4+
(D) OH–
80. When solutions of potassium sulfate and calcium
bromide are combined, which of the following
precipitates?
(A) KBr
(B) CaS
(C) CaSO4
(D) There is no precipitate.
81. Which of the following are products when
magnesium metal is placed in hydrochloric acid?
(A) H
(B) H+
(C) Mg
(D) MgCl2
82.
… H3PO3  … H3PO4 + …PH3
When the equation above is balanced, the
coefficient for H3PO4 is:
(A) 1
(B) 2
(C) 3
(D) 4
87.
Zn  Zn2+ + 2e–
In the half reaction above:
(A) Zn is oxidized because it is gaining electrons.
(B) Zn is oxidized because it is losing electrons.
(C) Zn is reduced because it is gaining electrons.
(D) Zn is reduced because it is losing electrons.
88. During the “ornament lab,” hydrogen gas was
produced according to the following equation:
Zn + 2 HCl  ZnCl2 + H2
Which chemical was oxidized?
(A) H2
(B) HCl
(C) Zn
(D) ZnCl2
83. Which property is always conserved during a
chemical reaction?
(A) mass
(B) pressure
(C) solubility
(D) volume
84. What mass of sulfur dioxide, SO2 (64.0 g/mole), is
produced when 245 g of sulfuric acid, H2SO4 (98.0
g/mole) reacts completely with zinc metal
according to the balanced equation below?
Zn + 2 H2SO4  ZnSO4 + SO2 + 2 H2O
(A) 64.0 g
(B) 80.0 g
(C) 128 g
(D) 160 g
89. At winter break, we made a “Chemist’s Tree” by
using the reaction:
Cu + 2 Ag+  2 Ag + Cu2+
The copper, Cu, is ____ electrons and
being __________.
(A) gaining, oxidized
(B) gaining, reduced
(C) losing, oxidized
(D) losing, reduced
85. At STP, how many liters of oxygen gas react with
4.00 moles of PH3 according to this equation?
4 PH3 (g) + 6 O2 (g) 6 H2O (ℓ) + P4O6 (s)
(A) 32.0
(B) 89.6
(C) 134
(D) 146
90. When we reacted AgNO3 and K2CrO4 to form
Ag2CrO4 and KNO3, ________ was oxidized.
(A) chromate ion
(B) nitrate ion
(C) silver ion
(D) nothing (it wasn’t a redox reaction)
86. How many moles of FeS2 are required to produce
64 grams of SO2 according to the balanced
equation below?
4 FeS2 (s) + 11 O2 (g)  2 Fe2O3 (s) + 8 SO2 (g)
(A) 0.40
(B) 0.50
(C) 3.2
(D) 4.5
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
C
B
A
B
A
D
B
C
B
D
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
C
C
B
D
B
A
A
A
A
A
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
A
C
A
C
D
A
B
B
D
A
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
C
D
B
C
A
B
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D
A
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41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
C
A
A
A
C
B
D
C
A
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51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
B
B
A
A
D
B
B
B
B
D
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
A
C
A
A
D
B
D
C
D
D
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
B
A
A
C
B
C
C
A
B
C
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
D
C
A
B
C
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C
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D