Download Practice Test 1 (Chapters 1-7)

C2A PT1
Multiple Choice
Write you name and section number on both your test
booklet and your Scantron Answer Sheet. Identify the
choice that best completes the statement or answers the
question and fill the space coresponding to your answer on
your Scantron Answer Sheet. Be sure to erase mistakes
completely.
1. Which of the following is not a step in the
scientific method?
a. Make an observation.
b. Formulate a hypothesis.
c. Perform an experiment.
d. Change results to agree with your
hypothesis.
e. Develop a theory (or model).
2. Write 8,394 in standard scientific notation.
a. 8394
b. 8.394  10–3
c. 839.4  101
d. 8.394  1000
e. 8.394  103
3. The number 0.002 expressed in exponential
notation is
a. 2  103
b. 2  104
c. 2  10–3
d. 2  10–4
e. none of these
4. 1.8 kilograms contain this many grams.
a.
b.
c.
d.
e.
5. Convert: 6.0 mm = _____________ km.
a.
km
b.
c.
d.
e.
km
km
km
km
66. Using the rules of significant figures, calculate the
following:
12.67 + 13.005 =
a.
b.
c.
d.
e.
25.675
25
20
25.68
26
7. The number 3.00183 rounded to four significant
figures is
a. 3.002
b. 3.001
c. 3.000
d. 3.183
e. none of these
8. How many significant figures are in the number
1.20  103?
a. 1
b. 2
c. 3
d. 4
e. 5
9. A student finds that the weight of an empty
beaker is 14.049 g. She places a solid in the
beaker to give a combined mass of 14.142 g. To
how many significant figures is the mass of the
solid known?
a. 2
b. 3
c. 1
d. 5
e. 4
10. The result of the following calculation has how
many significant figures?
(0.4333 J/g °C) (33.12°C – 31.12°C)(412.1 g)
a. 1
b. 2
c. 3
d. 4
e. 5
11. The product of 0.1400  6.02  1023 will have
how many significant figures?
a. 2
b. 3
c. 23
d. 1023
e. 7
12. How many significant figures are in the number
0.0040090?
a. 8
b. 7
c. 6
d. 5
e. 4
17. Convert: –10.5°F = _______________ °C.
a. –23.6°C
b. 11.9°C
c. –76.5°C
d. 38.7°C
e. 262.5°C
18. If 1.000 kg equals 2.205 lb, what is the mass in
pounds of a human who weighs 51.35 kg?
a. 113.2 lb
b. 23.29 lb
c. 93.2 lb
d. 53.56 lb
e. none of these
19. Find the volume of an object that has a density
13. Convert 316718.0 mm to kilometers.
a. 3.167180 km
b. 0.3167180 km
c. 316.7180 km
d. 3167.180 km
e.
km
of 3.14 g/mL and a mass of 94.7 g.
a. 30.2 mL
b.
mL
c. 297 mL
d.
mL
e.
mL
14. Convert: 6.76 qt = ___________ mL.
a. 7.17 mL
b.
mL
20. An experiment requires 74.2 mL of ethyl
c.
d. 6.38 mL
e.
mL
mL
15. Convert: 2.80 in = _____________ mm.
a. 71.1 mm
b. 7.11 mm
c. 1.102 mm
d. 0.71 mm
e. 711 mm
alcohol. If the density of ethyl alcohol is
0.790 g/cm3, what is the mass of 74.2 mL of
ethyl alcohol?
a. 93.9 g
b. 10.6 g
c. 58.6 g
d.
g
e. none of these
21.A graduated cylinder contains 20.0 mL of water. An
116.` Convert: 366.2 K = ________________ °C.
a. 639.2°C
b. 93.2°C
c. 691.2°C
d. 235.4°C
e. 203.4°C
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 80.4 g, what is
its density?
a. 7.18 g/mL
b. 0.139 g/mL
c. 2.58 g/mL
d. 4.02 g/mL
e. none of these
22. Which of the following is a physical change?
a. burning gasoline
b. cooking an egg
c. decomposing meat
d. evaporating water
e. rusting iron
28. The symbol for the element mercury is
a. Hg
b. Mg
c. He
d. Mn
e. none of these
23. 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
29. Si is the symbol for
a. silver
b. silicon
c. selenium
d. sodium
e. sulfur
chemical change.
24. Water is an example of
a. a homogeneous mixture
b. a heterogeneous mixture
c. a compound
d. an element
30. How many atoms of hydrogen are in five
molecules of C5H6Cl?
a.
b.
c.
d.
e.
30
5 x 1023
6
10 x 1023
6 x 1023
25. Which is an example of a homogeneous
mixture?
31.The total number of atoms represented by the
a. vodka
formula Co3(PO4)2 is
b. oily water
a. 13
c. soil (dust)
b. 11
d. sodium chloride
c. 8
e. aluminum
d. 17
26. Which of the following processes is a chemical
e. 6
change?
32. Which atomic particle determines the chemical
a. Dry ice sublimes when left on the demo
behavior of an atom?
table in lecture.
a. proton
b. The light on a candle burns until a bell jar is
b. electron
placed over it for a period of time.
c. neutron
c. When a few drops of red food coloring are
d. nucleus
added to a beaker of hot water, the water
e. none of these
immediately turns red.
33. An atom with 15 protons and 16 neutrons is an
d. Liquid nitrogen dumped onto the floor
atom of
vaporizes at room temperature.
a. P
e. None of the above processes are chemical
b. Ga
changes.
c. S
27. The symbol for the element iodine is
d. Pd
a. Io
e. Rh
b. In
c. Id
34. A certain isotope X2+ contains 37 electrons and
d. I
73 neutrons. What is the mass number for this
e. Ie
element?
a.
b.
c.
d.
e.
112
110
108
39
35
35. How many neutrons are there in one atom of
?
a.
b.
c.
d.
e.
22
24
46
68
none of these
36. Which of the following elements is an alkaline
earth metal?
a.
b.
c.
d.
e.
Ra
Au
Gd
Bi
Cs
37. The correct name for LiCl is
a. lithium monochloride
b. lithium(I) chloride
c. monolithium chloride
d. lithium chloride
e. monolithium monochloride
38. Which of the following formulas is incorrect?
a. AlO3
b. KBr
c. KNO3
d. Li2O
e. CaSO4
39. A compound contains an unknown ion X and
e. cyanous acid
41. The correct name for NiO is
a. nickel(II) oxide
b. nickel(I) oxide
c. nickel oxide
d. nickel monoxide
e. nickel(I) monoxide
42. The name for the acid H2SO3 is
a. sulfuric acid
b. sulfurous acid
c. hydrosulfuric acid
d. hydrosulfurous acid
e. sulfurite acid
43. The name for HClO3(aq) is
a. chloric acid
b. hydrogen chlorate
c. perchloric acid
d. hydrogen chlorate
e. chlorous acid
44. The name for NaHCO3 is
a. sodium hydrogen carbonate (sodium
bicarbonate)
b. sodium carbonate
c. sodium(I) hydrogen carbonate
d. sodium(I) bicarbonate
e. none of these
45. The correct formula for iron(III) phosphide is
a. Fe3P2
b. FeP
c. Fe3P
d. FeP3
e. Fe2P3
has the formula XCl2. Ion X contains 20
electrons. What is the identity of X?
a.
b.
c.
d.
e.
Ti2+
Sc+
Ca2+
Cr2+
Mn3+
40. The correct name for an aqueous solution of
HCN is
a.
b.
c.
d.
hydrocyanic acid
cyanic acid
cyanate acid
hydrocyanous acid
46. What is the formula for zinc(II) bromide?
a. ZnBr
b. Zn2Br
c. ZBr
d. Z2B
e. ZnBr2
47. What is the correct formula for barium
hydroxide?
a.
b.
c.
d.
e.
Ba2OH
Ba(OH)2
BaOH
Ba(OH)3
Ba(OH)4
48. When the following equation is balanced using
the smallest possible integers, what is the
number in front of the substance in bold type?
Na2S2O3 + I2  NaI + Na2S4O6
a.
b.
c.
d.
e.
1
2
3
4
6
49. When the following equation is balanced using
the smallest possible integers, what is the
number in front of the substance in bold type?
P4O10 + H2O  H3PO4
a.
b.
c.
d.
e.
10
6
4
2
1
50. When the following equation is balanced using
the smallest possible integers, what is the
number in front of the substance in bold type?
NBr3 + NaOH  N2 + NaBr + HOBr
a.
b.
c.
d.
e.
1
2
3
4
5
51. When the equation Si(s) + HF(aq)  SiF4(g) +
H2(g) is balanced, what is the coefficient for HF?
a.
b.
c.
d.
e.
0
1
2
3
4
a. evaporate
b. are cations only
c. form a second insoluble compound in the
solution
d. are left dissolved in the solution
e. none of these
53. An aqueous solution of sodium sulfate is
allowed to react with an aqueous solution of
calcium nitrate.
The complete ionic equation contains which of
the following species (when balanced in
standard form)?.
a.
b.
c.
d.
e.
2Na+(aq)
2SO42-(aq)
3Ca2+(aq)
NO3-(aq)
K+(aq)
54. An aqueous solution of ammonium sulfide is
allowed to react with an aqueous solution of
barium chloride.
What is the coefficient of the solid in the
balanced equation (in standard form)?
a.
b.
c.
d.
e.
1
2
3
4
5
55. The scientist who discovered the essential nature
of acids through solution conductivity studies is
a.
b.
c.
d.
e.
Priestley
Boyle
Einstein
Mendeleev
Arrhenius
56. The reaction AgNO3(aq) + NaCl(aq)  AgCl(s)
+ NaNO3(aq) is a(n) ______________ reaction.
a.
b.
c.
d.
e.
precipitation
acid-base
oxidation-reduction
single-replacement
none of these
57. A reaction that involves a transfer of electrons is
called a(n) ______________ reaction.
52.When a precipitation reaction occurs, the ions that
do not form the precipitate
a. precipitation
b. acid-base
c. oxidation-reduction
d. double-displacement
e. none of these
58. CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
a. oxidation-reduction
b. synthesis
c. decomposition
d. combustion
e. two of these
Use the following choices to classify each
reaction given below (more than one choice may
apply).
a. oxidation-reduction
b. acid-base
c. precipitation
59. ZnBr2(aq) + 2AgNO3(aq)  Zn(NO3)2(aq) +
2AgBr(s)
60. KBr(aq) + AgNO3(aq)  AgBr(s) + KNO3(aq)
61. HNO3(aq) + NaOH(aq)  H2O(l) + NaNO3(aq)
62. 6Na(s) + N2(g)  2Na3N(s)
63. HC2H3O2(aq) + CsOH(aq)  H2O(l) +
CsC2H3O2(aq)
Use the following choices to classify each
reaction given below (more than one choice may
apply).
a. oxidation-reduction
b. combustion
c. synthesis
d. decomposition
64. 2Cs(s) + F2(g)  2CsF(s)
65. S8(s) + 12O2(g)  8SO3(g)
76. 2GaN(s)  2Ga(s) + N2(g)