Download Introductory Chemistry I

Department of Chemistry
University of Missouri-St. Louis
Name_________________
Chemistry 1111
Practice Exam 2
March 2013
1. 10 mL of 0.2 M NaOH solution is placed into a small beaker with a small amount of
phenolphthalein. . If 0.1 M HCl is added dropwise:
a. the solution will become red on the first mL added, then change to colorless after
5 mL have been added.
b. the solution will become red after 20 mL have been added
c. the solution will remain colorless, even after large amounts of HCl have been
added.
d. the solution will be red initially, and become colorless after 20 mL of HCl
have been added.
2. From the observation that bubbling Cl2(g) into a solution of KI produces I2, and Cl-, we
conclude that
a. neither oxidation or reduction is occurring
b. Cl2 is oxidized
c. I2 is reduced
d. I2 is a better oxidizing agent than Cl2
e. Cl2 is a better oxidizing agent than I2
3. Which of the following net ionic equations is completely correct?
a. K+(aq) + BaCl2(aq) = Ba2+(aq) + KCl(s)
b. Ag+(aq) + Cl-(aq) = AgCl(s)
c. HCl(aq) + KOH(aq) = H2O(l) + Cl-aq) + K+(aq)
d. Cu(s) + SO3-2(aq) + 2 H+(aq) = Cu2+ + SO2(g) + H2O(l)
e. Zn + 2 Cl- = ZnCl2 (s)
4. The maximum number of electrons that can occupy the 3d orbitals is
a. 5
b. 6
c. 10
d. 14
e. 18
5. Let’s say that you are examining the outermost electrons in a ground-state germanium
atom. Which of the following sets of values for the four quantum numbers (n, l, ml,
and ms) could you use to describe the electrons?
a. 4, 1, 1, ½
b. 3, 1, 1, ½
c. 4, 2, 0, -½
d. 3, 2, 0, ½
e. 4, 0, 1, -½
1
6. You are given a solution that contains a Co2+ salt. Based on the activity series shown in
Table 4.3 below, which of the following metals would not cause the precipitation of
cobalt metal when a strip of that metal is placed in the cobalt solution?
a.
b.
c.
d.
e.
copper
chromium
calcium
magnesium
manganese
7. Which of the following elements has the greatest affinity for electrons?
a. K
b. Cl
c. Zn
d. Mg
e. S
8. Which of the following equations are balanced?
a.
b.
c.
d.
Zn(s) + 2ClO-(aq) + 4 H+(aq) = Zn2+ + Cl2(g) + 2H2O(l)
Cu+2 + 2 Zn (s) = Cu (s) + 2 Zn+2
4 C2H6O + 4 MnO4- + 12 H+ = 4 Mn+2 + 4C2H4O2 + 11 H2O
none of the above
2
9. What gets oxidized in the reaction:
2 MnO4-(aq) + 10 I-(aq) + 16 H+(aq) ---> 2 Mn2+(aq) + 5 I2(aq) + 8 H2O(l) ?
a.
b.
c.
d.
e.
MnO4IH+
Mn2+
I2
10. The net ionic equation for the neutralization reaction between HF(aq) and NaOH(aq)
is:
a. H+(aq) + OH-(aq) H2O(l)
b. HF(aq) + Na+(aq) + OH-(aq)  Na+(aq) + F-(aq) + H2O(l)
c. HF(aq) + OH-(aq)  F-(aq) + H2O(l)
d. HF (aq) + NaOH (aq)  NaF(aq) + H2O(l)
e. none of the above
11.
What is the oxidation number of Manganese in KMnO4?
a +2
b -2
c +6
d +7
e. none of the above
12
What is the frequency of a helium-neon laser light with a wavelength of 632.8 nm
(632.8x10-9m)? The speed of light is 3.00 x 108 m/s.
f. 4.74 x 1014 s-1
g. 4.74 x 105 s-1
h. 2.11 x 10-15 s-1
i. 1.58 x 10-15 s-1
j. none of the above
13.
Give n and l quantum numbers for the fourth-shell orbital shown below.
k.
l.
m.
n.
n = 5 and l = 3
n = 4 and l = 2
n = 4 and l = 1
n = 4 and l = 0
3
14.,
o.
p.
q.
r.
Which atom has the largest atomic radius?
Na
Cl
Br
K
s.
t.
u.
v.
What are the possible values of ml if n = 4?
5
0, 1, 2, 3, or 4
-3, -2, -1, 0, +1, +2, or +3
-4, -3, -2, -1, 0, +1, +2, +3, or +4
15.
16.
Which of the following atoms has the largest ionization potential ?
a. K
b. Cl
c. Ar
d. Ne
e. F
17.
Balance the following equation in water:.
Br2 (aq)
+ SO2 (g)
=
Br - (aq) + HSO4 - (aq)
2e- + Br2 = 2Br2H2O + SO2 = HSO4- + 2 e- + 3H+
2H2O +Br2 +SO2 = HSO4- + 3 H+ + 2 Br -
18.
What is the maximum amount of pure iodine you could obtain from 100 grams of
the mineral lautarite (CaIO3) ?
a.
b.
c.
d.
100 g
59.1 g
46.5 g
not enough information given
19.
The following ions all have the same number of electrons. The order in terms of
increasing size is:
a.
b.
c.
d.
Ti +4, Sc +3, Ca +2, S-2
S-2, Ti +4, Sc +3, Ca +2
S-2, Ca +2 Sc +3, Ti +4
Ca +2, S-2 , Ti +4, Sc +3
4
20.
The electronic configuration of Cr is:
a.
b
c.
d.
1s2 2s2 2p63s2 3p6 4s2 3d4
1s2 2s2 2p6 3s2 3p6 4s1 3d5
1s2 2s2 2p6 3s2 3p6 3d4
none of the above
21.
The following energies are associated with the processes described:
Li (s) going to Li (g)
159.4 kJ/mol
+
Li (g) going to Li + e
520 kJ/mol
F2 (g) going to 2 F (g)
158 kJ/mol
F (g) + e going to F
-328 kJ/mol
Li+ (g) + F – (g) going to LiF (s)
-1036 kJ/mol
The energy change for the formation of LiF from the elements in kJ/mol is:
a.
-605.6
b.
-526.6
c.
+605.6
d.
not enough information given
22. How many mL of 0.1 M KMnO4 would it take to completely react with 25 mL of a
solution of 0.1 M NaI according to the following reaction
2 MnO4-(aq) + 10 I-(aq) + 16 H+(aq) ---> 2 Mn2+(aq) + 5 I2(aq) + 8 H2O(l)
a.
b.
c.
d.
125 mL
25 mL
5 mL
2.5 mL
5