Name: __________________________ Date: _____________
1. A coffee cup calorimeter containing 100.0 mL of concentrated HCl at 20.3 °C. When
1.82 g Zn(s) is added, the temperature rises to 30.5 °C. What is the heat of reaction per
mol of reacted Zn? Assume the resultant solution has a specific heat of solution =
4.184 J/g. °C and density = 1.00 g/mL.
A)
B)
C)
D)
E)
-156 kJ/mol
-300. kJ/mol
-272 kJ/mol
-198 kJ/mol
-122 kJ/mol
2. When NaOH(s) is added to water, it releases -44.5 kJ/mol heat. Find the maximum
temperature of the water, when 500. mL of 7.0 M NaOH solution is prepared. The
initial temperature of water is 21°C. The solution has a density of 1.08 g/mL and
specific heat of 4.00 J/ g·°C
.
A)
B)
C)
D)
E)
93 °C
74 °C
53 °C
83 °C
69 °C
3. The change in the internal energy of a system that absorbs 2,500 J of heat and that does
7,655 J of work on the surrounding is:
A)
B)
C)
D)
E)
-5,155 J
5,155 J
+10,155 J
-10,155 J
1.91 x 107
Page 1
4. Use the given data to calculate ΔHo for the following reaction:
2C(graphite) + 3CO2 (g) + 8 H2O (g) + 2H2(g) 5CH4 (g) + 7O2(g)
Given:
H2(g)
C(graphite) + 2H2(g)
CH4 (g) + 2O2(g)
A)
B)
C)
D)
E)
ΔHo = -285.8 kJ
 H2O (g)
+ ½ O2(g)

ΔHo = -74.81 kJ
 CH4 (g)
CO2 (g) +2 H2O (g)
ΔHo = -890.3 kJ
3093 kJ
2943 kJ
3155 kJ
3515 kJ
2788 kJ
5. For which one of the following reactions is the value of ΔHorxn equal to ΔHof for the
product?
A)
B)
C)
D)
E)
Xe (g) + 2F2 (g)  XeF4 (g)
CH4 (g) + 2Cl2 (g)  CH2Cl2 (l) + 2HCl (g)
N2 (g) + O3 (g)  N2O3 (g)
2CO (g) + O2 (g)  2CO2 (g)
2C (graphite) + O2 (g)  2CO (g)
6. The Bohr theory explains that an emission spectral line is:
A)
B)
C)
D)
E)
due to an electron losing energy and changing orbits.
due to an interaction between electrons in two different principal orbits.
due to an electron gaining energy and changing orbits..
due to an increase in the principal quantum number n of an electron.
due to an electron losing energy but keeping the same values of its all four
quantum numbers.
Page 2
7. What is the magnitude of the partial positive and partial negative charges in the HF
molecule? (1 D = 3.36 × 10–30 C m; 1e– = 1.6022 × 10–19 C; bond length HF = 0.92
angstroms; Dipole Moment HF = 1.82 D; 1 angstroms = 1 x 10-10 m)
A)
B)
C)
D)
E)
-0.41 and +0.41
-0.92 and +0.92
-0.65 and +0.65
-0.33 and +0.33
-0.17 and +0.17
8. Which one of the following sets of quantum numbers can correctly represent a 3p
orbital?
i.
n=3
l=1
ml = 2
A)
B)
C)
D)
E)
ii.
n=1
l=3
ml = 3
iii.
n=3
l=2
ml = 1
iv.
n=3
l=1
ml = –1
v.
n=3
l=0
ml = 1
iv
i
ii
iii
v
9. The ground–state electron configuration for an atom of indium (In) is
A)
B)
C)
D)
E)
[Kr]5s24d105p1.
[Ar]4s24p63d5.
[Ar]4s23d104p1.
[Kr]5s24p64d5.
[Kr]5s25p64d5.
10. The binding energy for Lithium is 279.7 kJ/mol. Calculate the minimum wavelength of
light that can remove an electron from an atom on the surface of Lithium metal.
A)
B)
C)
D)
E)
4.28 x 10-7 m
428 m
1.40 x 10-7 m
1.40 x 10-12 m
2.14 10-3 m
Page 3
11. Which statement best describes relationships in a modern periodic table?
A) Nonmetallic properties tend to predominate for elements at the far right portion of
the table.
B) Elements are always arranged in order of decreasing atomic weights.
C) Metalloids usually are the cations in ionic compounds.
D) The fourteen elements in the "lanthanide" series form a new independent group.
E) Each transition element is placed in the column of the main group element that it
most closely resembles.
12. Which comparison of ionization energies is correct?
A)
B)
C)
D)
E)
+
Ca > Ca
Ar > He
Ca > Mg
Na > Mg
+
+
Mg > Mg2
13. List in order of increasing atomic size: Sr, Se, As, Ga, In.
A)
B)
C)
D)
E)
Se < As < Ga < In < Sr
Ga < In < Se < As < Sr
Sr < In < Ga < Se < As
In < Ga < As < Se < Sr
As < Ga < Se < Sr < In
14. Which of the following statements is/are CORRECT for an oxygen atom?
I.
The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s
electron.
II. The effective nuclear charges felt by 2s and 2p electrons are identical.
III. The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron.
A)
B)
C)
D)
E)
III only
I only
II only
I and II only
I and III only
Page 4
15. Use the following data to calculate the 2nd ionization energy for the Metal (M):
M(s)
M(g)
X2(g)
2X(g)
M(g)
M+(g) +
eM+(g)
M2+(g) + eX(g)
+ eX (g)
M(s) +
X2(g)
MX2(s)
2+
MX2(s)
M (g) + 2X (g)
A)
B)
C)
D)
E)
H
= 148.0 kJ
H
= 159.0 kJ
H
= 738.0 kJ
H
= ?
H
= -328.0 kJ
Hf
= -1123 kJ
H
= 2962 kJ
1450. kJ
794.0 kJ
1642 kJ
1598 kJ
159.8 kJ
16. The number of lone pairs of ClO3- (where all atoms are satisfied with octet) is
A)
B)
C)
D)
E)
10
27
20
24
9
Page 5
17. Calculate the bond energy of C-F in kJ/mol from the given data:
CH4 (g) + 2Cl2(g) +2F2(g) → CF2Cl2(g) +2HF +2HCl (g)
Bond
bond energy
C-H
413 kJ/mol
F-F
154 kJ/mol
C-Cl
339 kJ/mol
H-F
565 kJ/mol
H-Cl
427 kJ/mol
Cl-Cl
243 kJ/mol
A)
B)
C)
D)
E)
ΔH° = -1194 kJ/mol
489
970.
709
486
355
18. All of the following structures obey the Lewis octet rule EXCEPT
A)
B)
C)
D)
E)
N2O3
N2O
N2O4
N2O5
All of the above are correct structures.
19. Which one of the following bonds is the most polar?
A)
B)
C)
D)
E)
O-I
O-Br
O-Cl
Br-Cl
I-Br
Page 6
20. Choose the groups of molecules below in which all the molecules have no net dipole
moment.
A)
B)
C)
D)
E)
CO2, Cl2C=CCl2, NH4+
HF, H2O, N2
NH3, Cl2C=CCl2, O2
SiBrCl3, N2, Cl2C=CCl2
BeCl2, CH3Br , H2O
Page 7
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
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