PRACTICE FINAL CHEM 162
Chapter 14: Equilibrium WILL appear on the final. However, we have recently tested on it and
I’ve already given you practice MC test on equilibrium. I have not included any Ch 14 practice
questions
Chapter 9: Bonding
____
1. Which one of the following has an enthalpy change that is equal to the lattice energy of
A)
B)
C)
D)
E)
____
2. Which of the following processes is not exothermic?
A)
B)
C)
D)
E)
____
3. Which of the following compounds would be expected to have the lowest melting point?
A) AlF3
B) RbF
C) NaF
D) MgF2
E) CaF2
____
4. What is the ground-state electron configuration of
A)
B)
C)
D)
E)
____
5. All of the following species are isoelectronic except
A) Ar.
B) Ca2+.
C) Mg2+.
D) Cl–.
?
?
E) S2–.
____
6. A bond in which both electrons of the bond are donated by one atom is called ____.
A) a coordinate covalent bond
B) a polar covalent bond
C) an ionic bond
D) a double bond
E) a triple bond
____
7. An atom of which of the following elements has the highest electronegativity?
A) K
B) As
C) Ba
D) Si
E) Br
____
8. The Lewis structure for each of the following species except ____ contains a triple bond.
A) N3–
B) N2
C) HCCH
D) NO+
E) O22+
____
9. For each of the following species except ____, the electronic structure may be adequately
described by two resonance formulas.
A) O3
B) SO32–
C) NO2–
D) C6H6
E) SO2
____
10. Which of the following is/are true concerning formal charge?
1.
2.
3.
A)
B)
C)
D)
E)
The formal charge of each individual atom in a molecule or ion is an actual
atomic charge that can be experimentally determined.
The formal charge of each individual atom is always the same for each
possible resonance form.
The sum of the formal charges of each atom in a molecule or ion equal the
overall charge of the molecule or ion.
1 only
2 only
3 only
1 and 2
none
Ch 10: VSEPR
____
11. Which molecule or ion has the same molecular geometry for its central atom as the carbonate ion?
A) H2CO
B) AsCl3
C) PF3
D) CH3–
E) BrO3–
____
12. The approximate CCO angle in acetone,
A) 180°.
B) 90°.
C) 109°.
D) 60°.
E) 120°.
____
13. What is the molecular geometry around carbon atom C1?
A)
B)
C)
D)
E)
, is
tetrahedral
trigonal planar
linear
trigonal pyramidal
bent
____
14. Which of the following molecules has a permanent dipole moment?
A) SF6
B) CCl4
C) NF3
D) SiCl4
E) BF3
____
15. What hybrid orbitals of sulfur are involved in the bonding in sulfur trioxide?
A) sp2
B) sp2d
C) sp3
D) sp3d2
E) sp
____
16. Which of the following statements is true?
A) A  bond is twice as strong as a single bond.
B) A  bond results from the sideways overlap of hybridized orbitals.
C) A double bond consists of a  bond and a  bond.
D) A  bond has cylindrical symmetry about the bonding axis.
E) A  bond is twice as strong as a  bond.
____
17. According to valence-bond theory, the bonding in ketene, H2CCO, is best described as
A) five  bonds.
B) three  bonds and two  bonds.
C) four  bonds and two  bonds.
D) four  bonds and one  bond.
E) five  bonds.
Chapter 11: Solids, Liquids and Gases
____
18. Which of the following processes is endothermic?
A) melting of ice
B) condensation of water
C) deposition of carbon dioxide
D) freezing of water
E) condensation of ammonia
____
19. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor equilibrium at
a fixed temperature. Which of the following statements regarding this system is/are correct once
equilibrium is established?
1.
2.
3.
A)
B)
C)
D)
E)
____
Liquid molecules are no longer evaporating.
The number of vapor molecules remains essentially constant.
The partial pressure exerted by the vapor molecules is called the vapor
pressure of the liquid.
1 only
2 only
3 only
1 and 2
2 and 3
20. Choose the correct statement about the diagram below.
A) The diagram shows the triple point above 1 atm pressure.
B) The diagram is qualitatively correct for water.
C) The diagram shows that the melting point of the solid increases with increasing
pressure.
D) The diagram could represent the phase diagram of CO2.
E) None of the above statements is correct.
____
21. Which of the following compounds has the highest vapor pressure at 25°C?
A) CH3CH2OH
B) CH3CH2CH2CH3
C) CH3OCH3
D) CH3CH2CH3
E) CH3CH2CH2Cl
____
22. Why does hydrogen fluoride have an unusually high normal boiling point compared to the other
hydrogen halides?
A) The H-F bond in hydrogen fluoride is very strong.
B) Hydrogen fluoride has very strong London dispersion forces.
C) Hydrogen fluoride is capable of forming hydrogen bonds.
D) Hydrogen fluoride is ionic.
E) Hydrogen fluoride is covalent.
____
23. Which of the following concerning intermolecular forces is/are correct?
1.
2.
3.
A)
B)
C)
D)
E)
Intermolecular forces depend in part on the shape of a molecule.
London forces contribute to the net forces of attraction found in all molecular
solids and liquids.
Hydrogen bonding is a special category of dipole-dipole attractions.
1 only
2 only
3 only
1 and 2
1, 2, and 3
____
24. Which pure substance exhibits hydrogen bonding?
A) HNF2
B) B2H6
C) HBr
D) H2S
E) CaH2
____
25. A solid has a very high melting point, is hard, and in the molten state is a non-conductor. The solid
is most likely
A) a covalent network solid.
B) a metallic solid.
C) an amorphous solid.
D) a molecular solid.
E) an ionic solid.
____
26. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in
the center, and a cation at the center of each face. The unit cell contains a net:
A) 2 anions and 3 cations.
B)
C)
D)
E)
____
2 anions and 2 cations.
5 anions and 3 cations.
3 anions and 4 cations.
5 anions and 6 cations.
27. How many atoms are there in a body-centered cubic unit cell of vanadium?
A) 4
B) 8
C) 6
D) 2
E) 1
Ch 12: Solutions
____
28. Which of the following gases is least soluble in water?
A) CO2
B) SO3
C) NH3
D) N2
E) HCl
____
29. Which of the following concerning the effects of temperature and pressure on solubility is/are
correct?
1.
2.
3.
A)
B)
C)
D)
E)
All gases become more soluble in a liquid at a fixed pressure when the
temperature of the liquid is increased.
The dissolution of an ionic compound in water may be exothermic or
endothermic, depending on the initial temperature of the solution.
The solubility of a liquid in water generally is significantly effected by
pressure changes of the system.
1 only
2 only
3 only
1 and 2
none
____
30. A concentrated perchloric acid solution has a density of 1.67 g/mL at 25°C and is 11.7 M. What is
the percent by mass of HClO4 in the solution?
A) 70.4% HClO4 by mass
B) 0.702% HClO4 by mass
C) 1.42% HClO4 by mass
D) 0.699% HClO4 by mass
E) 60.2% HClO4 by mass
____
31. What is the molality of ethanol, C2H5OH, in an aqueous solution that is 51.0% ethanol by mass?
A) 1.04 m
B) 0.0226 m
C) 22.6 m
D) 0.719 m
E) 53.4 m
____
32. What is the vapor pressure at 75°C of an aqueous solution prepared by the addition of 64.3 g of the
nonvolatile solute urea, CO(NH2)2, to 174 g of water? The vapor pressure of pure water at 75°C
is 290. mmHg.
A) 133 mmHg
B) 28.9 mmHg
C) 167 mmHg
D) 261 mmHg
E) 212 mmHg
____
33. What is the molar mass of an aromatic hydrocarbon if 0.85 g of the compound depresses the
freezing point of 128 g of benzene by 0.37°C? (Kf for benzene is 5.12°C/m.)
A) 35 g/mol
B) 150 g/mol
C) 93 g/mol 92
D) 2100 g/mol
E) 140 g/mol
____
34. A 2.4-g sample of a small protein having a molecular weight of 62,000 g/mol is dissolved in 59.6
mL of water at 29°C. What is the osmotic pressure of the solution?
(R = 0.0821 L · atm/(K · mol))
A) 12 mmHg
B) 760 mmHg
C) 1.2 mmHg
D) 47,000 mmHg
E) 0.016 mmHg
____
35. Which of the following solutes in aqueous solution would be expected to exhibit the smallest
freezing-point lowering (assuming ideal behavior)?
A) 0.1 m NaCl
B) 0.2 m CH3COOH
C) 0.05 m Al2(SO4)3
D) 0.1 m MgCl2
E) 0.25 m NH3
____
36. Which of the following solutes, dissolved in 1.0 kg of water, creates a solution that boils at the
highest temperature?
A) 0.010 mol H3PO4
B) 0.010 mol HClO4
C) 0.010 mol H2SO4
D) 0.010 mol HCl
E) 0.010 mol HF
Ch 13: Kinetics
____
37. In the reaction 2H2O2(aq)  2H2O(l) + O2(g), the initial concentration of H2O2 is 0.542 M and,
21.2 seconds later, the concentration of H2O2 is 0.310 M. What is the average rate of reaction
over this time interval?
A) –0.0109 M/s
B) 0.0109 M/s
C) 0.0146 M/s
D) 0.00547 M/s
E) –0.00547 M/s
____
38. The reaction
2H2(g) + 2NO(g)  2H2O(g) + N2(g)
is first-order in H2 and second-order in NO at a particular temperature. What is the rate law?
A) Rate = k[H2]2[NO]2
B) Rate = k[H2][NO]2
C) Rate = k[H2][NO]
D) Rate = k[H2O]2[N2]
E) Rate = k[H2]2[NO]
____
39. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:
2NO(g) + Cl2(g)  2NOCl(g)
The following initial rates at a given temperature were obtained for the concentrations listed
below.
Experiment
1
2
3
Initial Rate (mol·L–1·h–1)
2.21
19.89
6.63
[NO]0 (mol·L–1)
0.25
0.75
0.25
[Cl2]0 (mol·L–1)
0.25
0.25
0.75
From the data, what is the experimental rate law?
A) Rate = k[Cl2]
B) Rate = k[NO]
C) Rate = k[NO][Cl2]2
D) Rate = k[NO]2[Cl2]
E) Rate = k[NO][Cl2]1/2
____
40. A chemical reaction that is first-order in X is observed to have a rate constant of 2.20  10–2 s–1. If
the initial concentration of X is 1.0 M, what is the concentration of X after 186 s?
A) 0.20 M
B) 0.017 M
C) 64 M
D) 0.59 M
E) 0.98 M
____
41. For a certain reaction of the general form aA  products, the experimental data plotted as 1/[A]
versus time is linear. The slope of this plot must equal
A) –1.
B) the rate constant.
C) one over the rate constant.
D) the negative of the rate constant.
E) 1.
____
42. For the hypothetical reaction aA  products, the concentration of A was monitored with time.
Given the following graph of the experimental data, what is the rate constant for the loss of
reactant A?
A)
B)
C)
D)
E)
____
2.42 min
400.00 min
-2.42 min
-400 min
24.2 min
43. For the following reaction producing 1 mol of oxygen gas at a particular temperature, H = –200
kJ.
NO(g) + O3(g)  NO2(g) + O2(g)
The activation energy is 11 kJ/mol. What is the activation energy for the reverse reaction?
A) 11 kJ/mol
B) 200 kJ/mol
C) 222 kJ/mol
D) 188 kJ/mol
E) 211 kJ/mol
____
44. The Arrhenius equation,
expresses the dependence of the rate constant on the reaction
temperature. The slope of a plot of ln(k) versus 1/T is equal to
A)
B)
C)
D)
E)
____
45. A suggested mechanism for the decomposition of ozone is as follows:
O3
O2 + O
O + O3
fast equilibrium
2O2
slow step
What is the rate law predicted by this mechanism?
A)
Rate =
B) Rate = k2[O] [O3]
C)
Rate =
D)
Rate =
E)
Rate =
Special topics: Organic and Complex Ions
____
46. What is the coordination number of cobalt in [Co(en)2Cl2]Br? (ALSO be able to give oxidation
number, cordination number, identity of ligands, and identiy of counter ions)
en =
A)
B)
C)
D)
E)
6
3
4
5
7
____
47. Which of the following liquids could best act as a bidentate ligand for a metal ion?
A) NH2Cl
B) NH3
C) ClCH2CH2NH2
D) N2H5+
E) H2NCH2CH2NH2
____
48. What is the molecular formula of a cyclic alkane with 6 carbon atoms?
A) C6 H14
B) C6 H10
C) C6 H16
D) C6 H12
E) C6 H6
____
49. What category of hydrocarbons contains a carbon–carbon triple bond?
A) alkane
B) aromatic
C) alkyne
D) alkene
E) cycloalkane
____
50. What is the IUPAC name for the following structural formula?
A)
B)
C)
D)
E)
____
1,1-dimethyl-2-ethylpropane
isoheptane
2-ethyl-3-methylbutane
2-methyl-3-ethylbutane
2,3-dimethylpentane
51. The functional group
A) aldehydes.
B) esters.
C) ketones.
D) alcohols.
E) acids.
is characteristic of
PRACTICE FINAL CHEM 162
Answer Section
1. ANS:
OBJ:
KEY:
2. ANS:
OBJ:
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MSC:
3. ANS:
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KEY:
4. ANS:
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5. ANS:
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9. ANS:
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10. ANS:
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11. ANS:
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KEY:
MSC:
12. ANS:
OBJ:
TOP:
E
PTS: 1
DIF: easy
REF: 9.1
Define lattice energy.
TOP: bonding | ionic bonding
Born-Haber cycle
MSC: general chemistry
E
PTS: 1
DIF: moderate
REF: 9.1
Describe the Born-Haber cycle to obtain a lattice energy from thermodynamic data.
bonding | ionic bonding
KEY: Born-Haber cycle
general chemistry
B
PTS: 1
DIF: easy
REF: 9.1
Describe some general properties of ionic substances.
TOP: bonding | ionic bonding
properties of ionic substance
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 9.2
Write electron configurations of transition-metal ions. (Example 9.3)
bonding | ionic bonding
electron configurations of ions | transition-metal ions
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 9.3
Define isoelectronic ions.
TOP: bonding | ionic bonding
ionic radii
MSC: general chemistry
A
PTS: 1
DIF: moderate
REF: 9.4
Define coordinate covalent bond.
E
PTS: 1
DIF: easy
REF: 9.5
State the general periodic trends in the electronegativity.
bonding | covalent bonding
KEY: electronegativity
general chemistry
A
PTS: 1
DIF: easy
REF: 9.6
Write Lewis formulas having including multiple bonds. (Example 9.7)
bonding | covalent bonding
KEY: multiple bonds
general chemistry
B
PTS: 1
DIF: easy
REF: 9.7
Write resonance formulas. (Example 9.9)
bonding | covalent bonding
KEY: resonance | delocalization
general chemistry
C
PTS: 1
DIF: easy
REF: 9.9
State the rules for obtaining formal charge.
bonding | covalent bonding
A
PTS: 1
DIF: moderate
REF: 10.1
Predict the molecular geometry (two, three, or four electron pairs). (Example 10.1)
bonding | molecular geometry
the valence-shell electron-pair repulsion model | trigonal planar arrangement
general chemistry
E
PTS: 1
DIF: easy
REF: 10.1
Predict the molecular geometry (two, three, or four electron pairs). (Example 10.1)
bonding | molecular geometry
KEY: bond angle MSC: general chemistry
13. ANS:
OBJ:
TOP:
14. ANS:
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MSC:
15. ANS:
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MSC:
23. ANS:
OBJ:
TOP:
24. ANS:
OBJ:
KEY:
25. ANS:
OBJ:
TOP:
26. ANS:
OBJ:
B
PTS: 1
DIF: moderate
REF: 10.1
Predict the molecular geometry in a molecule.
bonding | molecular geometry
C
PTS: 1
DIF: easy
REF: 10.2
Explain the relationship between dipole moment and molecular geometry. (Example 10.3)
bonding | molecular geometry
KEY: dipole moment
general chemistry
A
PTS: 1
DIF: moderate
REF: 10.3
Apply valence bond theory (two, three, or four electron pairs). (Example 10.4)
bonding | bonding theories
KEY: hybridization
general chemistry
C
PTS: 1
DIF: moderate
REF: 10.4
Define pi bond.
TOP: bonding | bonding theories
multiple bonding
MSC: general chemistry
C
PTS: 1
DIF: moderate
REF: 10.4
Apply valence bond theory (multiple bonding). (Example 10.6)
bonding | bonding theories
KEY: multiple bonding
general chemistry
A
PTS: 1
DIF: moderate
REF: 11.2
Define melting, freezing, vaporization, sublimation, and condensation.
phases | phase transitions
E
PTS: 1
DIF: moderate
REF: 11.2
Define vapor pressure.
TOP: phases | phase transitions
C
PTS: 1
DIF: moderate
REF: 11.3
Define phase diagram.
TOP: phases | phase transitions
phase diagram
MSC: general chemistry
D
PTS: 1
DIF: easy
REF: 11.5
Relate the properties of liquids to the intermolecular forces involved.
phases | liquid
KEY: intermolecular forces
general chemistry
C
PTS: 1
DIF: easy
REF: 11.5
Relate the properties of liquids to the intermolecular forces involved.
phases | liquid
KEY: intermolecular forces | hydrogen bonding
general chemistry
E
PTS: 1
DIF: moderate
REF: 11.5
Relate the properties of liquids to the intermolecular forces involved.
phases | liquid
A
PTS: 1
DIF: easy
REF: 11.5
Define hydrogen bonding.
TOP: phases | liquid
intermolecular forces | hydrogen bonding
MSC: general chemistry
A
PTS: 1
DIF: easy
REF: 11.6
Define molecular solid, metallic solid, ionic solid, and covalent network solid.
phases | solid
A
PTS: 1
DIF: easy
REF: 11.7
Determine the number of atoms in a unit cell. (Example 11.9)
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
TOP:
MSC:
ANS:
OBJ:
TOP:
MSC:
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MSC:
ANS:
OBJ:
TOP:
MSC:
phases | solid
KEY: crystalline solids | cubic unit cell
general chemistry
D
PTS: 1
DIF: easy
REF: 11.7
Determine the number of atoms in a unit cell. (Example 11.9)
phases | solid
KEY: structures of crystalline solids | metallic solid
general chemistry
D
PTS: 1
DIF: easy
REF: 12.2
Determine when a molecular solution will form when substances are mixed.
solutions | solution formation
KEY: solubility | molecular solution
general chemistry
E
PTS: 1
DIF: easy
REF: 12.3
State the general trends of the solubility of gases and solids with temperature.
solutions | solution formation
A
PTS: 1
DIF: easy
REF: 12.4
Calculate mass percentage of solute. (Example 12.2)
solutions | colligative properties
C
PTS: 1
DIF: moderate
REF: 12.4
Calculate the molality of solute. (Example 12.3)
solutions | colligative properties
expressing concentration | conversion of concentration units
general chemistry
D
PTS: 1
DIF: easy
REF: 12.5
Calculate vapor-pressure lowering. (Example 12.9)
solutions | colligative properties
vapor pressure of a solution | vapor pressure lowering
MSC: general chemistry
C
PTS: 1
DIF: moderate
REF: 12.6
Calculate the molecular mass from freezing-point depression. (Example 12.12)
solutions | colligative properties
KEY: freezing point depression
general chemistry
A
PTS: 1
DIF: easy
REF: 12.7
Calculate osmotic pressure. (Example 12.13)
solutions | colligative properties
KEY: osmotic pressure | colligative properties
general chemistry
A
PTS: 1
DIF: easy to moderate
12.8
Determine the colligative properties of ionic solutions. (Example 12.14)
solutions | colligative properties
C
PTS: 1
DIF: moderate
REF: 12.8
Determine the colligative properties of ionic solutions. (Example 12.14)
solutions | colligative properties
KEY: freezing point depression
general chemistry
D
PTS: 1
DIF: easy
REF: 13.1
Calculate average reaction rate. (Example 13.2)
rates of reaction | reaction rate
KEY: change of concentration with time
general chemistry
38. ANS: B
PTS: 1
DIF: easy
REF: 13.3
OBJ: Determine the order of reaction from the rate law. (Example 13.3)
TOP: rates of reaction | reaction rate
KEY: dependence of rate on concentration | reaction order
MSC: general chemistry
39. ANS: D
PTS: 1
DIF: easy
REF: 13.3
OBJ: Determine the rate law from initial rates. (Example 13.4)
TOP: rates of reaction | reaction rate
KEY: dependence of rate on concentration | determining the rate law
MSC: general chemistry
40. ANS: B
PTS: 1
DIF: easy
REF: 13.4
OBJ: Use an integrated rate law. (Example 13.5)
TOP: rates of reaction | reaction rate
KEY: integrated rate laws | first-order reaction
MSC: general chemistry
41. ANS: B
PTS: 1
DIF: easy
REF: 13.4
OBJ: Plot kinetic data to determine the order of a reaction.
TOP: rates of reaction | reaction rate
42. ANS: A
PTS: 1
DIF: moderate
REF: 13.4
OBJ: Plot kinetic data to determine the order of a reaction.
TOP: rates of reaction | reaction rate
43. ANS: E
PTS: 1
DIF: moderate
REF: 13.5
OBJ: Describe and interpret potential-energy curves for endothermic and exothermic reactions.
TOP: rates of reaction | reaction rate
KEY: collision theory | activation energy
MSC: general chemistry
44. ANS: E
PTS: 1
DIF: easy
REF: 13.6
OBJ: Use the Arrhenius equation. (Example 13.7)
TOP: rates of reaction | reaction rate
45. ANS: C
PTS: 1
DIF: moderate
REF: 13.8
OBJ: Determine the rate law from a mechanism with an initial fast, equilibrium step. (Example
13.12) TOP:
rates of reaction | reaction mechanism
KEY: the rate law and the mechanism
MSC: general chemistry
46. ANS: A
PTS: 1
DIF: moderate
REF: 22.3
OBJ: Define complex ion, complex (coordination compound), ligand, and coordination number.
TOP: transition elements | complex ions and coordination compounds
NOT: oxidation # is +3, coordination # is 6 (en is a bidentate ligand), ligands are en and Cl (the
two inside the brackets), counter ion is Br
47. ANS: E
PTS: 1
DIF: easy
REF: 22.3
OBJ: Give examples of a monodentate ligand, bidentate ligand, and polydentate ligand.
TOP: transition elements | complex ions and coordination compounds
KEY: structure of complex | ligand
MSC: general chemistry
48. ANS: D
PTS: 1
DIF: easy
REF: 23.2
OBJ: Know the general formula of cyclic cycloalkanes.
TOP: cycloalkane | structural characteristic
MSC: organic
chemistry
49. ANS: C
PTS: 1
DIF: easy
REF: 23.3
OBJ: Know the general formula of alkynes.
TOP: alkyne | structural characteristic
MSC: organic chemistry
50. ANS:
OBJ:
TOP:
MSC:
51. ANS:
OBJ:
TOP:
E
PTS: 1
DIF: moderate
REF: 23.5
Write the IUPAC name of an alkane given the structural formula. (Example 23.4)
alkane | nomenclature
KEY: IUPAC nomenclature
organic chemistry
C
PTS: 1
DIF: easy
REF: 23.6
Recognize aldehydes and ketones by functional group.
ketone | structural characteristic
MSC: organic chemistry