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CHM 111 Final Fall 2012
Part I. Multiple Choice
1. Consider the following specific heats of metals.
Metal
copper
cobalt
chromium
gold
silver
Specific Heat
0.385 J/(g • °C)
0.418 J/(g • °C)
0.447 J/(g • °C)
0.129 J/(g • °C)
0.237 J/(g • °C)
100-g samples of each of the metals at 95°C are added to 100 mL of water at 25°C. Which element
will increase the temperature of the water the least?
a. copper
b. cobalt
c. chromium
d. gold
e. silver
2. How many values are there for the magnetic quantum number when the value of the angular
momentum quantum number is 4?
a. 1
b. 3
c. 5
d. 7
e. 9
3. Which of the following sets of quantum numbers is NOT permissible? (Quantum)
1
a. n = 1, l = 0, ml = 0, ms = + 2
1
b. n = 4, l = 4, ml = 0, ms = + 2
1
c. n = 3, l = 2, ml = –2, ms = – 2
1
d. n = 2, l = 1, ml = 1, ms = – 2
1
e. n = 2, l = 0, ml = 0, ms = + 2
4. Which of the following combinations of quantum numbers are permissible?
a.
b.
c.
d.
n
l
m1
ms
1. 3
2. 4
3. 3
3
3
2
1
0
1
1/2
–1/2
+1/2
1 only
2 only
3 only
1 and 2 only
e. 2 and 3 only
5. What is the formal charge on the oxygen atom in the structure below?
a. 1
b, -1
c. 2
d. 0
e. -2
6. All the following species are isoelectronic EXCEPT
a. N3-.
b. F-.
c. Ne.
d. O-.
e. Mg2+.
7. Which one of the orbital occupancy designations shown below does NOT make sense?
(Quantum)
a.
b.
c.
d.
e.
2s1
3d10
4p7
4f7
2p6
8. Which of the following is NOT a correct name–symbol combination?
a. arsenic, As
b. manganese, Mg
c. iron, Fe
d. silver, Ag
e. potassium, K
9. What is the maximum number of electrons in n = 5?
a. 30
b. 50
c. 70
d. 10
e. 25
10. If the distance between the carbon atoms in diamond is 1.54 x 10-8 cm, what is this distance in
picometers?
a. 0.154
b. 1.54
c. 154
d. 1,540
e. 154,000
11. Three different samples were weighed using a different type of balance for each sample. The
three were found to weigh 0.1568934 kg, 1.215 mg, and 2458.1 g. The total mass of the samples
should be reported as
a. 2614.994615 g.
b. 2614.9946 g.
c. 2614.995 g.
d. 2615.0 g.
e. 2615 g.
12. The melting point of gold is 1338 K. This corresponds to
a. 1055°C.
b. 1661°C.
c. 1055°F.
d. 1917°F.
e. 1949°F.
13. Determine the number of significant figures that are present in the set of figures below.
What is the best answer for the four numbers?
a.
b.
c.
d.
e.
35.00
0.00219
1.18
45000
3
4
4
4
4
6
6
6
3
3
3
3
3
3
3
5
4
3
2
5
14. What is the volume of a cube that has an edge length of 0.010 m?
a. 1.0 cm3
b. 1.0 x 10-3 m3
c. 1.0 x 10-3 mm3
d. 1.0 x 10-3 cm3
e. 1.0 x 10-3 m3
15. How much heat is gained when 400 g of copper is warmed from 22.6 to 81.0°C? [The specific
heat of copper is 0.385 J/(g • °C).]
a. 3000 J
b. 5000 J
c. 7000 J
d. 9000 J
e. 11000 J
16. How many protons, neutrons, and electrons are in the antimony(III) ion,
a. 123p, 72n, 123e
b. 51p, 72n, 48e
c. 51p, 72n, 51e
d. 72p, 51n, 69e
123
51
Sb 3+?
e. 48p, 72n, 51e
17. The atomic mass of Ga is 69.72. There are only two naturally occurring isotopes of gallium, 69Ga
with a mass of 69.0 and 71Ga with a mass of 71.0. The natural abundance of the 71Ga isotope must be
approximately
a. 20%.
b. 40%.
c. 50%.
d. 60%.
e. 80%.
18. From the thermal decomposition of a pure solid, we obtained a solid and a gas, each of which is a
pure substance. From this information, we can conclude with certainty that
a. the original solid is not an element.
b. at least one of the products is an element.
c. both products are elements.
d. the solid is a compound and the gas is an element.
e. the solid is an element and the gas is a compound.
19. The sign of ∆H for the process NaCl(s) 
 NaCl(l) is
a. negative, and the process is endothermic.
b. positive, and the process is exothermic.
c. positive, and the process is endothermic.
d. negative, and the process is exothermic.
e. impossible to predict because ∆H of for NaCl(s) and ∆H of for NaCl(l) are not given.
20. The formula for neodymium sulfate is Nd2(SO4)3. On the basis of this information, the formula
for the nitride of neodymium would be expected to be
a. Nd2(NO2)3.
b. Nd3N2.
c. Nd(NO3)3.
d. Nd(NO2)3.
e. NdN.
21. How many atoms are present in 435 g of KPF6 ?
a. 1.42 x 1021
b. 9.96 x 1021
c. 1.14 x 1024
d. 1.42 x 1024
e. 1.14 x 1025
22. What is the percentage of chlorine in DDT, C14H9Cl5?
a. 35.0
b. 40.0
c. 45.0
d. 50.0
e. 55.0
23. Cubane is a compound composed of only C and H. It contains 92.26% C. It was found that the
mass of one mole of cubane was 103 ± 5 g. What is the molecular formula of the compound?
a. C7H7
b. C8H8
c. C9H9
d. C8H12
e. C6H14
24. The oxidation number of barium in BaO2 is
a. –2.
b. -1/2.
c. +1.
d. +2.
e. +4.
25. Complete combustion of a 0.20-mol sample of a hydrocarbon, CxHy, gives 0.80 mol of CO2 and
1.0 mol of H2O. The molecular formula of the original hydrocarbon is
a. C3H8.
b. C4H5.
c. C4H8.
d. C4H10.
e. C8H20.
26. All the following equations are balanced EXCEPT
a. (NH4)2Cr2O7 
 N2O + Cr2O3 + 4H2O.
b. 2NH4SCN + Ba(OH)2 • 8H2O 
 2NH3 + 10H2O + Ba(SCN)2.
c. C12H22O11 
 12C + 11H2O.
d. NH4NO3 
 N2O + 2H2O.
e. 2Mg + CO2 
 2MgO + C.
27. Elemental sulfur can be converted to sulfur trioxide by reaction with oxygen in the presence of a
catalyst. Upon addition of water, sulfuric acid is produced as represented by the equation:
S8(s) + 12O2(g) + 8H2O 
 8H2SO4(l)
What minimum mass of sulfur is needed to prepare 175 g of H2SO4? (Stoichiometry)
a. 39.6 g
b. 57.2 g
c. 71.8 g
d. 75.3 g
e. 81.9 g
28. The sum of the oxidation numbers of all the atoms in the peroxydisulfate ion, S2O82-, is
a. –2.
b. 0.
c. +2.
d. +4.
e. +6.
29. Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the
equation
4NH3 + 5O2 
 4NO + 6H2O
An 8.50-g sample of NH3 gives 12.0 g of NO. The PERCENT YIELD of NO is
a. 10%.
b. 40%.
c. 60%.
d. 80%.
e. 100%.
30. Which of the following reactions could be classified both as a precipitation reaction and an acid
base reaction?
a. Cu + 2H2SO4 
 CuSO4 + SO2 + 2H2O
b. Ba(OH)2 + H2SO4 
 BaSO4 + 2H2O
c. 2Li + 2H2O 
 2LiOH + H2
d. CaCO3 + 2HNO3 
 Ca(NO3)2 + CO2 + H2O
e. POBr3 + 3H2O 
 H3PO4 + 3HBr
31. What is the change in enthalpy for the reaction of 2.00 mol of iron(II) oxide?
6FeO(s) + O2(g) 
 2Fe3O4(s) + 635 kJ
a.
b.
c.
d.
e.
–635 kJ
–212 kJ
–106 kJ
106 kJ
635 kJ
32. The net ionic equation for the reaction of nitric acid with lithium hydroxide is
a. HNO3(aq) + LiOH(aq) 
 LiNO3(aq) + H2O(l).
b. HNO3(aq) + LiOH(aq) 
 Li+(aq) + NO3-(aq) + H2O(l).
+
c. HNO2(aq) + Li (aq) + OH-(aq) 
 Li+(aq) + NO2-(aq) + H2O(l).
d. H+(aq) + NO2-(aq) + Li+(aq) + OH-(aq) 
 Li+(aq) + NO2-(aq) + H2O(l).
+
e. H (aq) + OH (aq) 
 H2O(l).
33. The formation of a cation from an atom would be called
a. ionization energy.
b. electronegativity.
c. electron affinity.
d. oxidation.
e. reduction.
34. The Lewis structure for each of the following species contains a triple bond EXCEPT
a. HCCH.
b. N2.
c. NO+.
d. N3-.
e. O22+.
35. For the reaction that occurs in a lead storage battery,
Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4-(aq) 
 2PbSO4(s) + 2H2O(l)
the reducing agent is
a. Pb.
b. PbO2.
c. H+.
d. HSO4-.
e. PbSO4.
36. What volume of 0.200-molar Na2CO3 solution contains 53.0 g of Na2CO3?
a. 0.200 L
b. 0.400 L
c. 0.500 L
d. 1.60 L
e. 2.50 L
37. The titration of HCl with NaOH is represented by the equation
HCl + NaOH → NaCl + H2O
What volume of 0.100 M HCl is required to titrate 50.0 mL of 0.500 M NaOH? (Stoichiometry)
a. 50.0 mL
b. 100. mL
c. 200. mL
d. 250. mL
e. 500. mL
38. The n and l quantum numbers of the “last” electron of an element are n = 5 and l = 2. The
element could be a(n)
a. transition element.
b. inner transition element.
c. alkali metal.
d. metal or a nonmetal.
e. alkaline earth element.
39. Which of the following elements has the smallest ionization energy?
a. F
b. Be
c. B
d. Mg
e. H
40. The number of orbitals in an f subshell is
a.
b.
c.
d.
e.
1.
2.
3.
5.
7.
41. Which of the following sets of the four quantum numbers n, l, ml, and ms correctly describes an
electron occupying a f orbital of the fourth energy level?
a. 4, 0, 0, – 12
b. 4, 1, 1, + 12
c. 4, 2, 0, + 12
d. 4, 3, 3, – 12
e. 4, 4, 4, – 12
42. Which compound contains both ionic and covalent bonds?
a. KOCl
b. H2O
c. CH2Cl2
d. MgCl2
e. CH4
43. Which of the following is a weak base?
a.
b.
c.
d.
e.
HOCl
LiOH
Ba(OH)2
KOH
NH3
44. Two elements that have the same valence electronic configuration ground state np4 are
a. O and Se.
b. Ge and Pb.
c. Al and Ga.
d. K and Mg.
e. Mg and Ca.
45. All the following electronic ground-state configurations are correct EXCEPT
a. 20Ca [Ar] 4s2.
b. 25Mn [Ar] 4s2 4d5.
c. 29Cu [Ar] 3d10 4s1.
d. 50Sn [Kr] 4d10 5s2 5p2.
e. 54Xe [Kr] 4d10 5s2 5p6.
46. Which of the following ionic compounds is INSOLUBLE in water?
a. (NH4)2CO3
b. AgBr
c. CuSO4
d. KI
e. LiNO3
47. The molecular formula of ascorbic acid is C6H8O6. Its molecular mass is
a.
b.
c.
d.
e.
92 g/mol.
130. g/mol.
176 g/mol.
272 g/mol.
280. g/mol.
48. What is the percentage of nitrogen in ammonium phosphate?
a. 11.6%
b. 16.0%
c. 28.2%
d. 31.9%
e. 34.3%
49. How many valence electrons total are in the chlorate ion?
a. 23
b. 24
c. 25
d. 26
e. 27
50. Which of the following conversions requires a reducing agent?
a.
b.
c.
d.
e.
Mn3+ 
 Mn2+
2S2O3 
 S4O62SiF4 
 SiF622Cr2O7 
 CrO42SO2 
 SO3
51 Which of the following elements is assigned the HIGHEST electronegativity value?
a. K
b. Ba
c. F
d. Br
e. As
52. The names of the elements whose symbols are Si, P, Mn, and S are, respectively,
a.
b.
c.
d.
e.
silicon, potassium, manganese, and sulfur.
silver, phosphorus, magnesium, and sodium.
silicon, potassium, magnesium, and sulfur.
silver, potassium, manganese, and sodium.
silicon, phosphorus, manganese, and sulfur.
53. Analysis of a hydrocarbon showed that it contained 14.4% hydrogen and 85.6% carbon by weight.
What is its simplest formula? (Stoichiometry)
a. CH
b. CH2
c. CH3
d. C2H3
e. C2H5
54. Which of the following species is isoelectronic with Kr?
a.
b.
c.
d.
e.
Xe
K+
In3+
S2Sr2+
55. How many electrons are shown in the Lewis formula for the sulfate ion?
a. 24
b. 26
c. 28
d. 30
e. 32
56. The measure of the attraction that an atom has for the electrons in a chemical bond is called
a. electron affinity.
b. ionization energy.
c. electronegativity.
d. hybridization.
e. London forces.
57. Which of the following atoms is always an exception to the octet rule?
a. Na
b. H
c. F
d. Cl
e. Xe
58. What is the oxidation number of carbon in oxalate ion?
a. 2
b. 3
c. 4
d. 5
e. 6
59. The electronic configuration of the Au1+ ion is
a.
b.
c.
d.
e.
[Xe] 6s23d8
[Xe] 6s13d9
[Xe] 6s13d9
[Xe] 6s13d10
[Xe] 3d10
60. Which of the following compounds contains both ionic and covalent bonds?
a. ClF
b. SO2
c. NaCl
d. SO3
e. NaCN
61. Of the following, the only empirical formula is
a. C2H6.
b.
c.
d.
e.
C3H8.
C4H10.
H2O2.
O2.
62. The electronic configuration of the Al3+ ion is (Quantum)
a. 1s2 2s2 2p6.
b. 1s2 2s2 2p6 3s2 3p1.
c. 1s2 2s2 2p6 3s2 3p4.
d. 1s2 2s2 2p3.
e. 1s2 2s2 2p1.
63. Which of the following species does NOT have the proper electron-dot formula?
:
:F :
:
:
*a.
:F
F:
S
:
:
:F :
:
:
:
:
::
F
B
:
F
b.
:F :
:
: :
O
:
::
c.
F
:
F
:
::
:F :
d.
: Xe :
:F :
:
:
e.
H
F:
:
64. The number of valence electrons in a chlorine atom
a. 5
b. 7
c. 10
d. 17
e. 32
65. Using the following data, calculate the heat of reaction for the coal gasification process 2C(s) +
2H2O(g) 
 CH4(g) + CO2(g).
C(s) + H2O(g) 
 CO(g) + H2(g)
∆H° = +131.3 kJ
CO(g) + H2O(g) 
 CO2(g) + H2(g)
CO(g) + 3H2(g) 
 CH4(g) + H2O(g)
a. +15.3 kJ
b. 378.6 kJ
c. –116.0 kJ–157.2 kJ
Part II. Complete and balance the following:
66. Sulfur dioxide and sodium oxide
∆H° = –41.2 kJ
∆H° = –206.1 kJ
d. –378.6 kJ
e. –157.2 kJ
67. Combustion of octane, C8H18. (Chemical Equations)
68. Dinitrogen trioxide and chromium (III) oxide
69. Barium sulfite and phosphoric acid (Chemical Equations)
70. Potassium chloride and lead (II) nitrate (Chemical Equations)
71. Balance the following using the half reactions (required):
Copper (II) sulfide reacts with nitric acid to produce copper (II) nitrate, sulfur, nitrogen monoxide and
water.
72. What is the correct Lewis dot structure of the thiocyanate ion, which contains a carbon atom, a
sulfur atom and a nitrogen atom with a -1 charge overall? Find the formal charge of each atom to
find the correct structure. (Hint: 3 possibilities)
English
1 ft = 12 in
3 ft = 1 yd
Conversions
1 in = 2.54 cm
1 yd = 0.914 m
5280 ft = 1 mi
16 oz = 1 lb
4 qt = 1 gal
2 pt = 1 qt
2c = 1 pt
8 fl oz = 1 c
1 mi = 1.609 km
1 oz = 28.35 g
1 lb = 453.6 g
1 gal = 3.785 L
1 qt = 0.946 L
1 cm3 = 1 mL