AP Chemistry - Chapter 9 Quiz (Nov 16, 2009)
Student: __________________________________________________Section: A-1 A-2 A-3
1. Use the Born-Haber cycle to calculate the lattice
energy of LiCl(s) given the following data:
H(sublimation) Li = 155.2 kJ/mol
I1 (Li) = 520 kJ/mol
Bond energy (Cl-Cl) = 242.8 kJ/mol
EA (Cl) = 348 kJ/mol
Hf (LiCl(s)) = -408.8 kJ/mol
A.
B.
C.
D.
E.
-40 kJ/mol
40 kJ/mol
736 kJ/mol
857 kJ/mol
1,553 kJ/mol
2. Use the Born-Haber cycle to calculate the lattice
energy of NaBr (s) given the following data:
H(sublimation) Na = 177.8 kJ/mol
I1 (Na) = 495.9 kJ/mol
Bond energy (Br-Br) = 192.5 kJ/mol
EA (Br) = 325 kJ/mol
Hf (NaBr(s)) = -361.1 kJ/mol
A. 1456 kJ/mol
B. 806 kJ/mol
C. 450 kJ/mol
D. 902 kJ/mol
E. 421 kJ/mol
3. The Lewis structure for a chlorate ion, ClO3-,
should show ____ single bond(s), ____ double
bond(s), and ____ lone pair(s).
A. 2, 1, 10
B. 3, 0, 9
C. 2, 1, 8
D. 3, 0, 10
E. 2, 1, 9
4. The number of resonance structures for the sulfur
dioxide molecule that satisfy the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
5. The number of resonance structures for the
nitrate ion that satisfies the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
6. What is the formal charge on the oxygen atom in
N2O (the atomic order is N-N-O)?
A. 0
B. +1
C. -1
D. -2
E. +2
7. What is the formal charge on sulfur in the best
Lewis structure for the SCN- (thiocyanate) ion?
A. +2
B. -2
C. +1
D. -1
E. 0
8. What is the formal charge on phosphorus in a
Lewis structure for the phosphate ion that satisfies
the octet rule?
A. -2
B. -1
C. 0
D. +1
E. +2
9. For which of these species is the best description
of the bonding provided by two or more equivalent
resonance structures?
A. HCO2B. SCNC. CNOD. N3E. CO2
10. The total number of lone pairs in the best Lewis
structure for the SOF4 molecule is
A. 0.
B. 2.
C. 14.
D. 16.
E. 18.
13. Use bond energies to estimate the enthalpy of
formation of HBr(g).
BE(H-H) = 436 kJ/mol
BE(Br-Br) = 192 kJ/mol
BE(H-Br) = 366 kJ/mol
A.
B.
C.
D.
E.
14. 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
11. The structures of C2H4 and C2H5OH are
The enthalpy change due to the reaction of one
mole of C2H4 with water to form C2H5OH can be
estimated by
+262 kJ/mol
-52 kJ/mol
-104 kJ/mol
+104 kJ/mol
+52 kJ/mol
A.
B.
C.
D.
E.
-101 kJ/mol
-106 kJ/mol
+331 kJ/mol
+106 kJ/mol
+101 kJ/mol
A. BE(C=C) - 2BE(C-C) - BE(C-O).
B. BE(C=C) + BE(O-H) - 2BE(C-C) - BE(C-O).
C. BE(C-O) + BE(C-C) - BE(O-H) - BE(C=C).
D. BE(O-H) + BE(C=C) - BE(C-H) - BE(C-O) BE(C-C).
E. BE(C-H) + BE(C-O) + BE(C-C) - BE(O-H) BE(C=C).
15. Use the bond enthalpy data given to estimate
the heat released when 6.50 g of nitrogen gas reacts
with excess hydrogen gas to form ammonia at 25C.
12. Estimate the enthalpy change for the reaction
2CO + O2  2CO2 given the following bond
energies.
A.
B.
C.
D.
E.
BE(CO) = 1074 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
A. +2380 kJ/mol
B. +744 kJ/mol
C. +1949 kJ/mol
D. -561 kJ/mol
E. -744 kJ/mol
BE(NN) = 941.4 kJ/mol
BE(H-H) = 436.4 kJ/mol
BE(N-H) = 393 kJ/mol
228 kJ
340 kJ
107 kJ
46.1 kJ
24.9 kJ
16. Use the bond enthalpy data given to estimate
the heat released when 50.0 g of propane gas, C3H8,
burns in excess oxygen to yield carbon dioxide and
water vapor at 25C.
BE(C-C) = 347 kJ/mol
BE(C=O in CO2) = 799 kJ/mol
BE(C-H) = 414 kJ/mol
BE(O-H) = 460 kJ/mol
BE(O=O) = 498.7 kJ/mol
A.
B.
C.
D.
E.
1360 kJ
2240 kJ
2370 kJ
1540 kJ
1970 kJ
17. The standard enthalpy of formation of ammonia
at 25C is -46.3 kJ/mol. Estimate the N-H bond
enthalpy at this temperature.
(Given: BE(NN)=941.4 kJ/mol, BE(H-H) = 436.4
kJ/mol)
A. 383 kJ/mol
B. 475 kJ/mol
C. 360 kJ/mol
D. 391 kJ/mol
E. 459 kJ/mol
18. Use the Born-Haber cycle to calculate the
lattice energy of NaBr(s) given the following data:
H(sublimation) Na = 109 kJ/mol
I1 (Na) = 496 kJ/mol
Bond energy (Br-Br) = 192 kJ/mol
EA (Br) = 324 kJ/mol
Hf (NaBr(s)) = -361 kJ/mol
19. Write the Lewis structure for the product that
forms when boron trifluoride combines with diethyl
ether (C2H5OC2H5).
Chapter 9 Quiz Key
1. Use the Born-Haber cycle to calculate the lattice energy of LiCl(s) given the following data:
H(sublimation) Li = 155.2 kJ/mol
I1 (Li) = 520 kJ/mol
Bond energy (Cl-Cl) = 242.8 kJ/mol
EA (Cl) = 348 kJ/mol
Hf (LiCl(s)) = -408.8 kJ/mol
a. -40 kJ/mol
b. 40 kJ/mol
c. 736 kJ/mol
D. 857 kJ/mol
e. 1,553 kJ/mol
Chang - 009 Chemical... #20
Difficulty: Difficult
2. Use the Born-Haber cycle to calculate the lattice energy of NaBr (s) given the following data:
H(sublimation) Na = 177.8 kJ/mol
I1 (Na) = 495.9 kJ/mol
Bond energy (Br-Br) = 192.5 kJ/mol
EA (Br) = 325 kJ/mol
Hf (NaBr(s)) = -361.1 kJ/mol
a. 1456 kJ/mol
B. 806 kJ/mol
c. 450 kJ/mol
d. 902 kJ/mol
e. 421 kJ/mol
Chang - 009 Chemical... #21
Difficulty: Difficult
3. The Lewis structure for a chlorate ion, ClO3-, should show ____ single bond(s), ____ double bond(s), and
____ lone pair(s).
a. 2, 1, 10
b. 3, 0, 9
c. 2, 1, 8
D. 3, 0, 10
e. 2, 1, 9
Chang - 009 Chemical... #45
Difficulty: Difficult
4. The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is
a. 1.
B. 2.
c. 3.
d. 4.
e. none of these.
Chang - 009 Chemical... #48
Difficulty: Difficult
5. The number of resonance structures for the nitrate ion that satisfies the octet rule is
a. 1.
b. 2.
C. 3.
d. 4.
e. none of these.
Chang - 009 Chemical... #49
Difficulty: Difficult
6. What is the formal charge on the oxygen atom in N2O (the atomic order is N-N-O)?
a. 0
b. +1
C. -1
d. -2
e. +2
Chang - 009 Chemical... #54
Difficulty: Difficult
7. What is the formal charge on sulfur in the best Lewis structure for the SCN- (thiocyanate) ion?
a. +2
b. -2
c. +1
d. -1
E. 0
Chang - 009 Chemical... #57
Difficulty: Difficult
8. What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet
rule?
a. -2
b. -1
c. 0
D. +1
e. +2
Chang - 009 Chemical... #59
Difficulty: Difficult
9. For which of these species is the best description of the bonding provided by two or more equivalent
resonance structures?
A. HCO2b. SCNc. CNOd. N3e. CO2
Chang - 009 Chemical... #66
Difficulty: Difficult
10. The total number of lone pairs in the best Lewis structure for the SOF4 molecule is
a. 0.
b. 2.
C. 14.
d. 16.
e. 18.
Chang - 009 Chemical... #67
Difficulty: Difficult
11. The structures of C2H4 and C2H5OH are
The enthalpy change due to the reaction of one mole of C2H4 with water to form C2H5OH can be estimated by
a. BE(C=C) - 2BE(C-C) - BE(C-O).
b. BE(C=C) + BE(O-H) - 2BE(C-C) - BE(C-O).
c. BE(C-O) + BE(C-C) - BE(O-H) - BE(C=C).
D. BE(O-H) + BE(C=C) - BE(C-H) - BE(C-O) - BE(C-C).
e. BE(C-H) + BE(C-O) + BE(C-C) - BE(O-H) - BE(C=C).
Chang - 009 Chemical... #76
Difficulty: Difficult
12. Estimate the enthalpy change for the reaction 2CO + O2  2CO2 given the following bond energies.
BE(CO) = 1074 kJ/mol
BE(O=O) = 499 kJ/mol
BE(C=O) = 802 kJ/mol
a. +2380 kJ/mol
b. +744 kJ/mol
c. +1949 kJ/mol
D. -561 kJ/mol
e. -744 kJ/mol
Chang - 009 Chemical... #77
Difficulty: Difficult
13. Use bond energies to estimate the enthalpy of formation of HBr(g).
BE(H-H) = 436 kJ/mol
BE(Br-Br) = 192 kJ/mol
BE(H-Br) = 366 kJ/mol
a. +262 kJ/mol
B. -52 kJ/mol
c. -104 kJ/mol
d. +104 kJ/mol
e. +52 kJ/mol
Chang - 009 Chemical... #79
Difficulty: Difficult
14. 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
Chang - 009 Chemical... #80
Difficulty: Difficult
15. Use the bond enthalpy data given to estimate the heat released when 6.50 g of nitrogen gas reacts with
excess hydrogen gas to form ammonia at 25C.
BE(NN) = 941.4 kJ/mol
BE(H-H) = 436.4 kJ/mol
BE(N-H) = 393 kJ/mol
a. 228 kJ
b. 340 kJ
c. 107 kJ
d. 46.1 kJ
E. 24.9 kJ
Chang - 009 Chemical... #81
Difficulty: Difficult
16. Use the bond enthalpy data given to estimate the heat released when 50.0 g of propane gas, C3H8, burns in
excess oxygen to yield carbon dioxide and water vapor at 25C.
BE(C-C) = 347 kJ/mol
BE(C=O in CO2) = 799 kJ/mol
BE(C-H) = 414 kJ/mol
BE(O-H) = 460 kJ/mol
BE(O=O) = 498.7 kJ/mol
a. 1360 kJ
B. 2240 kJ
c. 2370 kJ
d. 1540 kJ
e. 1970 kJ
Chang - 009 Chemical... #82
Difficulty: Difficult
17. The standard enthalpy of formation of ammonia at 25C is -46.3 kJ/mol. Estimate the N-H bond enthalpy at
this temperature.
(Given: BE(NN)=941.4 kJ/mol, BE(H-H) = 436.4 kJ/mol)
a. 383 kJ/mol
b. 475 kJ/mol
c. 360 kJ/mol
D. 391 kJ/mol
e. 459 kJ/mol
Chang - 009 Chemical... #84
Difficulty: Difficult
18. Use the Born-Haber cycle to calculate the lattice energy of NaBr(s) given the following data:
H(sublimation) Na = 109 kJ/mol
I1 (Na) = 496 kJ/mol
Bond energy (Br-Br) = 192 kJ/mol
EA (Br) = 324 kJ/mol
Hf (NaBr(s)) = -361 kJ/mol
738 kJ/mol
Chang - 009 Chemical... #89
Difficulty: Difficult
19. Write the Lewis structure for the product that forms when boron trifluoride combines with diethyl ether
(C2H5OC2H5).
(for clarity of presentation, carbon-hydrogen single bonds are not shown explicitly)
Chang - 009 Chemical... #103
Difficulty: Difficult
Category
# of Questions
Chang - 009 Chemical...
19
Difficulty: Difficult
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