Dr. Woodbury
Practice EXAM 1
Name _____________________________
Dr. Erik Woodbury
CHEMISTRY 1A
PRACTICE EXAM 1
Multiple Choice
Circle one
1.
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B
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2.
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B
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E
permitted. All information required is contained on the exam. Place all work
3.
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in the space provided. If you require additional space, use the back of the
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5.
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6.
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(1) Read each question carefully.
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(2) For Part I, there is no partial credit given and only answers marked on
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9.
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10. A
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Instructions:
CLOSED BOOK EXAM!
No books, notes, or additional scrap paper are
exam. A scientific calculator may be used. Please remember that the De
Anza Code of Academic Conduct applies to this exam and all other graded
work in the class. This exam has 11 pages.
this cover page will be graded.
(3) The last page contains some useful information. You may remove it for
easy access.
(4) If you finish early, RECHECK YOUR ANSWERS!
1-10 total
(5) This practice Exam is longer than the lecture exam will be. It
11. A
B
C
D
E
12. A
B
C
D
E
13. A
B
C
D
E
intentionally covers a greater breadth of questions than the lecture exam
can.
Possible Points
Points
# 1–10
(2 points each)
/ 20
14. A
B
C
D
E
# 11-15
(4 points each)
/ 20
15. A
B
C
D
E
# 16-19
/ 32
# 20-22
/ 18
# 23
/ 16
#25-27
/ 27
# 28-32
/ 42
/ 175
Total Score (175)
1
11-15 total:
Dr. Woodbury
Practice EXAM 1
Part I: Multiple Choice, Concepts (2 points each)
Select the best answer and enter your choice on the cover sheet – No partial credit
1)
Ionic bonds tend to form between
a. Metals and metals
b. Non metals and non metals
c. Noble gases and non metals
d. Non metals and metals
e. Metalloids and metals
2)
According to the Scientific Method, a
series of observations are summarized by
a/an
a. Hypothesis
b. Law
c. Theory
d. Model
e. Experiment
3)
Blood’s ability to fix oxygen is an example of
a. A Physical property
b. A Nuclear property
c. A Biological property
d. A Chemical property
e. A Mechanical property
4)
Elements differ from compounds in that
compounds
a. Cannot be broken down farther by
physical means
b. Cannot be broken down farther by
chemical means
c. Can be broken down farther by
chemical means
d. Can be broken down farther by
physical means
e. Contain only one type of atom
5)
In order to create a cation, an atom must
a. Gain a neutron
b. Lose a neutron
c. Gain an electron
d. Lose an electron
e. Lose a proton
2
6)
Which of the following states that
compounds always contain the same relative
amounts of elements by mass?
a. Law of Conservation of Mass
b. Law of Multiple Proportions
c. Law of Definite Proportions
d. Law of Conservation of Energy
e. None of the above
7)
Group 2 is also called the
a. Halogens
b. Noble Metals
c. Chalcogens
d. Alkaline Earth Metals
e. Alkali Metals
8)
Ionic bonds tend to form between
a. Metals and metals
b. Metals and non metals
c. Non metals and non metals
d. Metalloids and metals
e. Noble gases and noble metals
9)
Data that is close to the desired value can
be said to
a. Be precise
b. Contain systematic error
c. Be accurate
d. Contain random error
e. None of the above
10)
Which of the following is likely to be the
best conductor of electricity?
a. Pure water
b. A mixture of water and magnesium
bromide
c. A mixture of water and magnesium
carbonate
d. A mixture of water and acetic acid
e. A mixture of water and copper metal
Dr. Woodbury
Practice EXAM 1
Part II: Multiple Choices, Short Calculations (4 points each)
Select the best answer and enter your choice on the cover sheet – No partial credit
11) How many atoms does 0.357 mol of CaCl2 contain?
A. 7.38x1022 atoms
B. 2.15x1023 atoms
C. 7.16x1022 atoms
D. 6.45x1023 atoms
E. 1.81x1024 atoms
12)
What is the percent mass of carbon in C6H5O3N?
A. 27.94 %
B. 48.20 %
C. 51.80 %
D. 57.60 %
E. 72.06 %
13)
286 K is what temperature on the Fahrenheit scale?
A. 1038 °F
B. 974 °F
C. -8.6 °F
D. 55.4 °F
E. none of the above
14)
For the following balanced equation how many moles of oxygen gas are needed to make
6.73 mols of iron oxide?
4 Fe (s) + 3 O2 (g)  2 Fe2O3 (s)
A.
10.1 moles
B.
4.47 moles
C.
2.24 moles
D.
13.46 moles
E.
5.05 moles
15)
How many moles of NaOH would be needed to completely react with 25 mL of 0.150 M
H2SO4?
A.
3.75 E-3 mol
B.
7.50 E-3 mol
C.
3.75 mol
D.
7.50 mol
E.
1.88 E-3 mol
3
Dr. Woodbury
Practice EXAM 1
Part III: Short Answer
16)
Identify whether the following are Elements, Compounds, Heterogeneous Mixtures or
Homogeneous Mixtures. (6 points)
Milk
_______________
Bronze
____________
Gold
_______________
Sugar
____________
An Orange
____________
Diamond _______________
17)
Identify whether the following is a physical (P) or chemical (C) property of mercury (6
points)
Melts at 234K
________
Shiny
Poisonous
________
Is much denser than water __________
Flame retardant _________
18)
__________
Reacts with air to form HgO _________
Draw a representation of the atom according to JJ Thomson’s theory and according to
Rutherford’s theory (8 points)
19)
Give the number of protons, electrons and neutrons in each atom below: (12 points)
Atom / Ion
13
Protons
Neutrons
C
43
Fe2+
37
Cl-
238
U
4
Electrons
Dr. Woodbury
20)
Practice EXAM 1
Explain how Millikan’s oil-drop experiment worked and what it found. Feel free to use
diagrams if you wish: (6pts)
21)
Using the attached solubility rules, write the balanced, total ionic and net ionic equations
for the reaction of aqueous silver nitrate and aqueous lithium phosphate. (6 pts)
22)
Write the molecular formula for ionic compounds made from the following atom pairs:
(6pts)
a.
Sodium and Bromine
____________
b. Nitrogen and Magnesium
____________
c.
____________
Potassium and Oxygen
5
Dr. Woodbury
23)
Practice EXAM 1
(16 pts.) Nomenclature
Name the following compounds:
a.
KOH
__________________________
b. H3PO4
__________________________
c.
CH4
__________________________
d. P2S2
__________________________
e.
Sn(NO2)4
__________________________
f.
Mg3N2
__________________________
g.
Hg2SO3
__________________________
h. (NH4)2CO3
__________________________
Give the correct formula for the following compounds:
i.
Xenon tetrafluoride
__________________________
j.
Lead (II) bicarbonate
__________________________
k.
Nitrogen triiodide
__________________________
l.
Cesium acetate
__________________________
m. Copper (II) chromate
__________________________
n.
Hydrosulfuric acid
__________________________
o.
Mercury (II) sulfide
__________________________
p.
Stannic Oxide
__________________________
6
Dr. Woodbury
24)
Practice EXAM 1
Balance the following reactions by filling in the missing coefficients. (12 points)
a. ____C4H4 (g) + _______O2 (g)  ______CO2 (g) + ______H2O (g)
b.
_____NaCl (aq) + _____Pb(NO3)2 (aq)  _____NaNO3 (aq) + _____PbCl2 (s)
c.
_____H2SO4 (aq) + _____KOH (aq)  _____K2SO4 (aq) + _____H2O (l)
7
Dr. Woodbury
25)
Practice EXAM 1
For each of the following molecules, give the oxidation number for each atom. (7 pts)
a.
Na2SO3
b. NH4ClO3
Na_____
S_____
O_____
N _____
H_____
Cl_____
O_____
26)
For the following reaction, identify the reducing agent and the oxidizing agent ( 4 pts)
Fe2O3 (s) + 2 Al (s)  2 Fe (l) + Al2O3 (l) (the thermite reaction! Note the liquid iron.)
27)
Using solubility rules and the activity table as necessary predict the products of the
following reactions and write the balanced reaction. Identify each reaction type. If no
reaction, write “No Reaction” for type. (16 pts)
Al (s) + ZnSO4 (aq) 
Type________________________
HCl (aq) + Ca(OH)2 (aq) 
Type________________________
NasS (aq) + Pb(NO3)2 
Type________________________
Ni(NO3)2 (aq) + Cu (s)
Type________________________
8
Dr. Woodbury
28)
Practice EXAM 1
Which of the following solutions would make a better conductor of electricity? Support
your statement quantitatively. (6 pts)
29)
Solution A:
0.364M solution of Ca(NO3)2
Solution B:
0.257M solution of Al2(SO4)3
Underline all of those below that are strong acids. Circle those that are weak acids. Put an
X through any bases. (5 points)
d. CH3COOH
g. H2SO3
i. PO43-
b. HClO4
e. Ca(OH)2
h. HNO2
j. NH3
c.
f. HClO3
a.
HI
H 2O
Calculations. Show all work for full credit.
30)
(10 pts each)
A compound is analyzed and found to contain the following elements by mass:
C: 11.3964 g
H: 0.9565 g
N: 6.6471 g
In addition, the molecular mass is found to be 80.092 g/mol.
What is this the empirical formula of the molecule? What is the molecular formula?
9
Dr. Woodbury
Practice EXAM 1
31) For the following balanced reaction, determine what the theoretical yield of each product
is:
Pb(CO3)2 (s) + 2 H2SO4 (aq)  Pb(SO4)2 (aq) + 2 H2O (l) + 2 CO2 (g)
Starting material: Pb(CO3)2 : 0.4025 g
H2SO4 : 0.2254 g
What is the percent yield of water if 40.0 mg are obtained?
32)
A mad scientist wishes to build his fortune by collecting large amounts of compounds that
contain silver. Currently, his aim is to isolate 355 g of silver sulfate. What volume (in mL)
of the following two solutions will he need to isolate this amount of product? (I)
a.
Solution A: 1.25 M AgNO3
b. Solution B: 0.744 M Na2SO4
10
Dr. Woodbury
Practice EXAM 1
PERIODIC TABLE
Key
1
Atomic Number
Symbol
Atomic Mass
Electronegativity
H
1.008
2.20
3
2
He
4.003
-
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
6.941
0.98
9.012
1.57
10.81
2.04
12.01
2.55
14.01
3.04
16.00
3.44
19.00
3.98
20.18
-
Na
11
Mg
Al
Si
14
15
16
S
Cl
Ar
22.99
0.93
24.31
1.31
26.98
1.61
28.09
1.90
30.97
2.19
32.06
2.58
35.45
3.16
39.95
-
19
12
21
Ti
22
23
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.10
0.82
40.08
1.00
44.96
1.36
47.90
1.54
50.94
1.63
52.00
1.66
54.94
1.55
55.85
1.83
58.93
1.88
58.70
1.91
63.55
1.90
65.38
1.65
69.72
1.81
72.59
2.01
74.92
2.18
78.96
2.55
79.90
2.96
83.80
-
42
43
26
44
27
45
28
46
29
47
30
48
31
49
32
50
33
51
34
35
18
Sc
41
25
17
Ca
40
24
P
K
37
20
13
36
Rb
Sr
38
39
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
52
53
I
Xe
54
85.47
0.82
87.62
0.95
88.91
1.22
91.22
1.33
92.91
1.6
95.94
2.16
(98)
1.9
101.1
2.2
102.9
2.28
106.4
2.20
107.9
1.93
112.4
1.69
114.8
1.78
118.7
1.96
121.8
2.05
127.6
2.1
126.9
2.66
131.3
-
55
56
71
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.9
0.79
87
137.3
0.89
88
175.0
1.27
103
178.5
1.3
104
180.9
1.5
105
183.9
2.36
106
186.2
1.9
107
192.2
2.20
109
195.1
2.28
197.0
2.54
200.6
2.00
204.4
2.04
207.2
2.33
209.0
2.02
(209)
2.0
(210)
2.2
(222)
-
(223)
0.7
(226)
0.9
(260)
-
-
-
-
-
190.2
2.2
-
Fr
Ra
Lr
Unq
57
Unp
58
Unh
59
Uns
60
61
Une
-
62
63
64
65
66
67
68
69
70
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
138.9
1.10
140.1
1.12
140.9
1.13
144.2
1.14
(145)
1.13
150.4
1.17
152.0
1.2
157.3
1.20
158.9
1.2
162.5
1.22
164.9
1.23
167.3
1.24
168.9
1.25
173.0
1.1
Ac
89
Th
90
Pa
91
92
U
Np
93
Pu
94
Am
Cm
Bk
Cf
Es
Fm
Md
No
(227)
1.1
232.0
1.3
(231)
1.5
238.0
1.38
(237)
1.36
(244)
1.28
(243)
1.3
(247)
1.3
(247)
1.3
(251)
1.3
(252)
1.3
(257)
1.3
(258)
1.3
(259)
1.3
11
95
96
97
98
99
100
101
102
Dr. Woodbury
Practice EXAM 1
12