FINAL EXAM
CH101.004 (Blackstock)
December 15, 2006
Student name (print):________________________________ honor pledge: ___________________________
score: multiple choice (136 pts) _______
short answer (22 pts) _______
1. The SI prefixes giga and micro represent,
respectively:
A. 10-9 and 10-6.
B. 106 and 10-3.
D. 109 and 10-6.
C. 103 and 10-3.
E. 10-9 and 10-3.
2. The diameter of an atom is approx. 1 x 10-8 cm.
What is this diameter when expressed in
nanometers?
A. 1 x 10-19 nm
B. 1 x 10-15 nm
D. 1 x 10-10 nm
1
C. 1 x 10 nm
E. 1 x 10-1 nm
TOTAL _______
8. An oxide ion, O2-, has:
A. 8 protons and 10 electrons
B. 10 protons and 8 electrons
C. 8 protons and 9 electrons
D. 8 protons and 7 electrons
E. 10 protons and 7 electrons
9. What is the formula for the ionic compound
formed by magnesium and iodine?
A. MgI
B. Mg2I
D. MgI3
C. MgI2
E. Mg3I
3. How many significant figures does the
sum 8.520 + 2.7 contain?
A. 1
B. 2
D. 4
C. 3
E. 5
10. The total number of electrons present in a
sulfate ion is
A. 2.
B. 26.
D. 48.
C. 32.
E. 50.
4. Lead melts at 601.0 ˚C. What temperature is this
in ˚F?
A. 302 ˚F
B. 365 ˚F
D. 1,082 ˚F
C. 1,050 ˚F
E. 1,114 ˚F
11. What is the average mass, in grams, of one atom
of iron?
A. 6.02 x 1023 g
B. 1.66 x 10-24 g
D. 55.85 g
C. 9.28 x 10-23 g
E. 55.85 x 10-23 g
5. A piece of metal with a mass of 125 g is placed
into a graduated cylinder that contains 25.00 mL of
water, raising the water level to 56.00 mL. What is
the density of the metal?
A. 5.00 g/cm3
B. 4.03 g/cm3
D. 1.51 g/cm3
3
C. 2.23 g/cm
E. 0.25 g/cm3
12. How many silicon atoms are there in 1.00 g of
silicon?
A. 1 atom
B. 0.0356 atoms
D. 2.14 x 1022 atoms
C. 2.57 x 1023 atoms
E. 1.75 x 1025 atoms
6. Atoms of the same element with different mass
numbers are called
A. ions.
B. neutrons.
D. chemical families.
C. allotropes.
E. isotopes.
7. An atom of the isotope sulfur-31 consists of how
many protons, neutrons, and electrons?
(p = proton, n = neutron, e = electron)
A. 15 p, 16 n, 15 e
B. 16 p, 15 n, 16 e
D. 32 p, 31 n, 32 e
C. 16 p, 31 n, 16 e
E. 16 p, 16 n, 15 e
13. How many moles of CF4 are there in 171 g of
CF4?
A. 0.51 mol
B. 1.94 mol
D. 88.0 mol
C. 4.07 mol
E. 171 mol
14. How many moles of Cl atoms are there in 65.2 g
CHCl3?
A. 0.548 mol
B. 1.09 mol
D. 1.64 mol
23
C. 3.3 x 10 mol
E. 3.0 mol
2
15. When balanced with the smallest set of whole
numbers, the coefficient of O2 in the following
equation is:
__ C2H4 + __ O2 ----> __ CO2 + __ H2O
A. 1.
B. 2.
C. 3.
D. 4.
E. 6.
16. When 22.0 g NaCl and 21.0 g H2SO4 are mixed
and react according to the equation below, which is
the limiting reagent?
2NaCl + H2SO4 ----> Na2SO4 + 2HCl
A. NaCl
B. H2SO4
C. Na2SO4
D. HCl
E. No reagent is limiting.
17. What is the theoretical yield of chromium that
can be produced by the reaction of 40.0 g of Cr2O3
with 8.00 g of aluminum according to the chemical
equation below?
2Al + Cr2O3 ----> Al2O3 + 2Cr
A. 7.7 g
B. 15.4 g
C. 27.3 g
D. 30.8 g
E. 49.9 g
18. Identify the major ionic species present in an
aqueous solution of Na2CO3.
A. Na2+, CO32B. Na2+, C2-, O3
C. Na+, C4+, O32-
D. Na+, C+, O2E. Na+, CO32-
19. Based on the solubility rules, which one of these
compounds should be insoluble in water?
A. NaCl
B. MgBr2
D. AgBr
C. FeCl2
E. ZnCl2
20. What is the chemical formula of the salt
produced by the neutralization of sodium hydroxide
with sulfuric acid?
A. Na2SO4
B. Na2(SO4)3
D. NaSO3
C. Na(SO4)2
E. Na3SO4
21. The oxidation number of N in NaNO3 is
A. +6.
B. +5.
D. -3.
C. +3.
E. none of these.
22. Which one of these equations describes a redox
reaction?
A. 2Al(s) + 3H2SO4(aq) ----> Al2(SO4)3(aq) + 3H2(g)
B. 2KBr(aq) + Pb(NO3)2(aq) ---> 2KNO3(aq) + PbBr2(s)
C. CaBr2(aq) + H2SO4(aq) ----> CaSO4(s) + 2HBr(g)
D. H+(aq) + OH-(aq) ----> H2 O(l)
E. CO32-(aq) + HSO4-(aq) ----> HCO3-(aq) + SO42-(aq)
23. Identify the oxidizing agent in the chemical
reaction 2MnO4- + 5H2SO3 ----> 2Mn2+ + 5SO42- +
4H+ + 3H2O.
A. MnO4B. H2SO3
D. SO422+
C. Mn
E. H+
24. A 50.0 mL sample of 0.436 M NH4NO3 is
diluted with water to a total volume of 250.0 mL.
What is the ammonium nitrate concentration in the
resulting solution?
A. 21.8 M
B. 0.459 M
D. 8.72 x 10-2 M
-2
C. 2.18 x 10 M
E. 0.109 M
25. A 4.691 g sample of MgCl2 is dissolved in
enough water to give 750. mL of solution. What is
the magnesium ion concentration in this solution?
A. 3.70 x 10-2 M
B. 1.05 x 10-2 M
D. 4.93 x 10-2 M
C. 6.57 x 10-2 M
E. 0.131 M
26. A sample of nitrogen gas has a volume of 32.4
L at 20C. The gas is heated to 220ºC at constant
pressure. What is the final volume of nitrogen?
A. 2.94 L
B. 19.3 L
C. 31.4 L
D. 54.5 L
E. 356 L
27. Calculate the volume occupied by 35.2 g of
methane gas (CH4) at 25˚C and 1.0 atm.
R = 0.0821 L atm/K mol.
A. 0.0186 L
B. 4.5 L
C. 11.2 L
D. 49.2 L
E. 53.7 L
3
28. Gases are sold in large cylinders for laboratory
use. What pressure, in atmospheres, will be exerted
by 2,500 g of oxygen gas (O2) when stored at 22C
in a 40.0 L cylinder?
A. 3.55 atm
B. 1,510 atm
C. 47.3 atm
4
D. 7.56 x 10 atm
E. 10.2 atm
29. Calculate the density of Ar(g) at -11˚C and 675
mmHg.
A. 1.52 g/L
B. 1.65 g/L
D. 39.95 g/L
C. -39.3 g/L
E. 1254 g/L
30. What volume of CO2 gas at 645 torr and 800 K
could be produced by the reaction of 45 g of CaCO3
according to the equation?
CaCO3(s) ----> CaO(s) + CO2(g)
A. 0.449 L
B. 22.4 L
C. 25.0 L
D. 34.8 L
E. 45.7 mL
31. Which gas has molecules with the greatest
average molecular speed at 25˚C?
A. CH4
B. Kr
D. CO2
C. N2
E. Ar
35. Calculate ∆H for the following reaction
2H2O2(l) ----> 2H2O(l) + O2(g)
given that ∆Hf [H2O(l)] = -285.8 kJ/mol and
∆Hf [H2O2(l)] = -187.6 kJ/mol.
A. -196.4 kJ/mol
B. 98.2 kJ/mol
C. -98.2 kJ /mol
D. 196.4 kJ/mol
E. -396.4 kJ/mol
36. Given H2(g) + (1/2)O2(g) ----> H2O(l),
∆Hrxn = -286 kJ/mol, determine the standard
enthalpy change for 2H2O(l) ----> 2H2(g) + O2(g).
A. H = -286 kJ/mol
B. H = +286 kJ/mol
C. H = -572 kJ/mol
D. H = +572 kJ/mol
E. H = -143 kJ/mol
37. What is the wavelength of radiation that has a
frequency of 6.912 x 1014 s-1?
A. 1.447 x 10-15 nm
B. 4.337 x 102 nm
C. 2.304 x 106 nm
D. 2.074 x 1023 nm
E. 4.337 x 10-7 nm
38. A possible set of quantum numbers for the last
electron added to complete an atom of gallium Ga
in its ground state is
32. An endothermic reaction causes the
surroundings to
A. warm up.
B. become acidic.
C. condense.
D. decrease in temperature.
E. release CO2.
33. If 325 g of water at 4.2C absorbs 12.28 kJ, what
is the final temperature of the water? The specific
heat of water is 4.184 J/g·˚C.
A. 4.21˚C
B. 4.8˚C
D. 13.2˚C
C. 9.0˚C
E. 2,938˚C
34. Which of these processes is endothermic?
A. O2(g) + 2H2(g) ----> 2H2O(g)
B. H2O(g) ----> H2O(l)
C. 3O2(g) + 2CH3OH(g) ----> 2CO2(g) + 2H2O(g)
D. H2O(s) ----> H2O(l)
A. Row 1.
B. Row 2.
C. Row 3.
D. Row 4.
E. Row 5.
39. Electrons in an orbital with l = 3 are in a/an
A. d orbital.
B. f orbital.
C. g orbital.
D. p orbital.
E. s orbital.
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40. "No two electrons in an atom can have the same
four quantum numbers" is a statement of
A. the Pauli exclusion principle.
B. Bohr's equation.
C. Hund's rule.
D. de Broglie's relation.
E. Dalton's atomic theory.
41. The orbital diagram for a ground-state nitrogen
atom is
45. The elements in Group 7A are known by what
name?
A. transition metals
B. halogens
D. alkaline earth metals
C. alkali metals
E. noble gases
46. Which one of these elements is a transition
element?
A. Nickel
B. Tin
D. Sulfur
C. Sodium
E. Calcium
47. The general electron configuration for noble gas
atoms is
A. ns2np6.
B. ns2np5.
D. ns2np3.
2
4
C. ns np .
E. ns2.
48. How many valence electrons does a carbon
atom have?
A. 1
B. 2
D. 4
C. 3
E. 6
A. Row 1.
B. Row 2.
C. Row 3.
D. Row 4.
42. Which element has the following ground-state
electron configuration?
[Kr]5s24d105p3
A. Sn
B. Sb
C. Pb
50. Which of the elements listed below has the
greatest atomic radius?
A. B
B. Al
D. P
C. S
E. Si
D. Bi
E. Te
43. A ground-state atom of iron has ___ unpaired
electrons and is _____.
A. 0, diamagnetic
B. 6, diamagnetic
C. 3, paramagnetic
D. 5, paramagnetic
E. 4, paramagnetic
44. How many electrons in a ground-state tellurium
atom are in orbitals labeled by l = 1?
A. 4
B. 10
C. 12
D. 16
E. 22
49. What is the charge on the monatomic ion that
calcium forms in its compounds?
A. +2
B. +1
D. -2
C. -1
E. -3
51. Which of these elements has the highest first
ionization energy?
A. C
B. Si
D. Sn
C. Ge
E. Pb
52. The first ionization energy of sodium is 495.9
kJ/mol. The energy change for the reaction Na(s)
Na+(g) + e- is therefore
A. 495.9 kJ/mol.
B. less than 495.9 kJ/mol.
C. greater than 495.9 kJ/mol.
D. equal to the electron affinity of sodium.
E. equal to the second ionization energy of sodium.
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53. Which of these compounds is most likely to be
ionic?
A. KF
B. CCl4
D. CO2
C. CS2
E. ICl
54. Which of these atom is the most
electronegative?
A. Li
B. Cs
D. As
C. P
E. Ge
55. In which of these pairs of atoms would the bond
be the most polar?
A. B-C
B. C-N
D. Si-O
C. C-O
E. C-C
56. The number of lone electron pairs in the N2
molecule is ___.
A. 1
B. 2
D. 4
C. 3
E. 5
57. The total number of bonding electrons in a
molecule of formaldehyde (H2CO) is
A. 3.
B. 4.
D. 8.
C. 6.
E. 18.
58. Nitrous oxide, N2O, is sometimes called
"laughing gas". What is the formal charge on the
central nitrogen atom in the best Lewis structure for
nitrous oxide? (The atom connectivity is N-N-O.)
A. -2
B. -1
D. +1
C. 0
E. +2
59. Which of these molecules has an atom with an
incomplete octet?
A. NF3
B. H2O
D. GeH4
C. AsCl3
E. BF3
60. Use VSEPR theory to predict the shape of the
PCl3 molecule.
A. linear
B. bent
C. trigonal planar
D. trigonal pyramidal
E. tetrahedral
61. Use bond energies to estimate the enthalpy
change for the reaction of one mole of CH4 with
chlorine gas to give CH3Cl and hydrogen chloride.
BE(C-H) = 414 kJ/mol
BE(C-Cl) = 326 kJ/mol
BE(H-Cl) = 432 kJ/mol
BE(Cl-Cl) = 243 kJ/mol
A. -101 kJ/mol
B. -106 kJ/mol
C. +331 kJ/mol
D. +106 kJ/mol
E. +101 kJ/mol
62. According to the VSEPR theory, the molecular
shape of the carbonate ion, CO32 -, is
A. square planar.
B. tetrahedral.
D. trigonal planar.
C. pyramidal.
E. octahedral.
63. According to the VSEPR theory, the molecular
shape of SiCl4 is
A. linear.
B. trigonal planar.
C. bent.
D. tetrahedral.
E. trigonal pyramidal.
64. Which one of the following molecules has
tetrahedral geometry?
A. XeF4
B. BF3
D. CF4
C. AsF5
E. NH3
65. The F-S-F bond angles in SF6 are
A. 90 and 180.
B. 109.5.
D. 180.
C. 120.
E. 90 and 120.
66. Which one of the following molecules has a
zero dipole moment?
A. CO
B. CH2Cl2
D. SO2
C. SO3
E. NH3
67. Indicate the type of hybrid orbitals used by the
central atom in CCl4.
A. sp B. sp2 C. sp3 D. sp3d E. sp3d2
68. What is the hybridization of the As atom in the
AsF5 molecule?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
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Short Answer (22 pts)
1. (10 pts) Provide Lewis structures for the following atoms and molecules (accurate geometries not required).
S
CH3CO2H
C2H2
SOF4
NO
2. (10 pts) Write the structure with appropriate geometry of ammonium nitrate salt (NH4 NO3) showing separate
structures for the cation and anion. Include any formal charges on atoms and any resonance structures (note: all
NH bonds are equivalent and all NO bonds are equivalent). In words, indicate the geometry at the N atoms.
3. (2 pts) Write a 3D structure for propyne (CH3CCH).
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constants and equations:
h = 6.63 x 10-34 J s
RH = 2.18 x 10-18 J
R = 0.0821 atm L mol-1 K-1,
En = -RH(1/n2)
R= 8.31 J mol-1 K-1,
2πr = nλ
1 atm L = 101.3 J,
λ = h/mu
∆x∆p ≥ h/4π
1 cal = 4.184 J
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final exam Key
31.A
64.D
32.D
65.A
1.D
2.E
3.C
4.E
5.B
6.E
7.B
8.A
9.C
10.E
11.C
12.D
13.B
14.D
15.C
16.A
17.B
18.E
19.D
20.A
21.B
22.A
23.A
24.D
25.C
26.D
27.E
28.C
29.B
30.D
33.D
66.C
34.D
67.C
35.A
68.D
36.D
37.B
38.C
39.B
40.A
41.A
42.B
43.E
44.E
45.B
46.A
47.A
48.D
49.A
50.B
51.A
52.C
53.A
54.C
55.D
56.B
57.D
58.D
59.E
60.D
61.A
62.D
63.D