Download Chem 1100 Pre-Test

Chem 1100 Pre-Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Which response contains all the molecules below that violate the octet rule, and no others?
SF4, SiCl4, H2Te, AsF5, BeI2
a.
b.
c.
d.
e.
____
SF4, AsF5, BeI2
BeI2
H2Te, BeI2
SF4, SiCl4
AsF5
2. Which numbered response lists all the molecules below that exhibit resonance and none that do not?
I.
PF5
II.
HNO3
III.
SO2
IV.
H2O
a.
b.
c.
d.
e.
I and II
II and III
III and IV
I and III
II, III, and IV
____
3. Which one of the following molecules has a central atom that is sp2 hybridized?
a. BeF2
b. BCl3
c. PCl3
d. H2O
e. NH3
____
4. Which of the following molecules has three lone pairs of electrons on the central atom?
a. XeF4
b. SF4
c. SF6
d. XeF2
e. NCl3
____
5. For AsF3, the electronic geometry is ____ and the molecular geometry is ____.
a. tetrahedral; trigonal planar
b. trigonal planar; tetrahedral
c. tetrahedral; tetrahedral
d. trigonal planar; trigonal planar
e. trigonal planar; linear
____
6. Which of the following molecules has the smallest bond angle(s)?
a. CH4
b. NH3
c. H2O
d. CF4
e. CO2
____
7. Which one of the following is a nonpolar molecule with polar bonds?
a. H2O
b. NH3
c. PF5
d. CHCl3
e. none of these
____
8. Which one of the following molecules is octahedral?
a. BeCl2
b. SeF6
c. BF3
d. PF5
e. CF4
____
9. How many sigma (σ) bonds and how many pi (π) bonds does the ethene molecule contain?
a.
b.
c.
d.
e.
4 σ, 2 π
5 σ, 2 π
5 σ, 1 π
5 σ, 0 π
8 σ, 2 π
____ 10. Which of the following molecules has an asymetric structure?
a. XeF4
b. SF4
c. SF6
d. XeF2
e. BCl3
____ 11. The overlap of the 2p atomic orbitals produces ____ sigma molecular orbitals and ____ pi molecular orbitals.
a. 2; 3
b. 2; 4
c. 4; 2
d. 1; 2
e. 3; 3
____ 12. What is the best definition of bond order?
a. A bond resulting from the occupation of a pi molecular orbital.
b. The amount of energy required to break one mole of bonds.
c. A bond resulting from the occupation of a sigma molecular orbital.
d. The number of bonding molecular orbitals minus the number of antibonding molecular
orbitals.
e. Half the number of electrons in bonding molecular orbitals minus half the number of
electrons in antibonding molecular orbitals.
____ 13. Which Lewis Dot Formula below is incorrect?
a.
b.
c.
d.
e.
____ 14. How many valence electrons does a phosphorus atom have?
a. 2
b. 6
c. 3
d. 5
e. 4
____ 15. Which of the following is the correct Lewis dot formula for H2S?
a.
b.
c.
d.
e.
____ 16. Draw the Lewis dot formula for PCl3. The number of unshared pairs of electrons in the outer shell of the
central atom is ____.
a. one
b. two
c. three
d. four
e. zero
____ 17. The Lewis structure for the carbonate ion, CO32−, shows ____ doubles bond(s), ____ single bond(s) and ____
lone pair(s) on the central atom.
a. 3; 1; 2
b. 1; 2; 0
c. 2; 2; 1
d. 2; 1; 1
e. 2; 1; 2
____ 18. Which Lewis dot formula is incorrect?
a.
b.
c.
d.
e.
____ 19. The total number of covalent bonds in the N2 molecule is ____.
a. one
b. two
c. three
d. four
e. zero
____ 20. How many lone pairs of electrons are there on the Xe atom in the XeF4 molecule?
a. one
b. two
c. three
d. four
e. zero
____ 21. Which one of the following molecules contains bonds that are the most polar? (Electronegativities: H = 2.1,
Be = 1.5, B = 2.0, N = 3.0, F = 4.0, S = 2.5, Br = 2.8, I = 2.5)
a. SF6
b. BI3
c. BeBr2
d. NH3
e. NF3
____ 22. Which one of the following molecules is nonpolar?
a. H2O
b. CO2
c. CSO
d. NF3
e. NH3
____ 23. The hybridization associated with the central atom of a molecule in which all the bond angles are 180° is
____.
a. sp
b. sp2
c. sp3
d. sp3d
e. sp3d2
____ 24. The central atom in a molecule is bonded to 3 other atoms and has 2 lone pairs. What type of hybrid orbitals
are formed by the central atom?
a. sp
b. sp2
c. sp3
d. sp3d
e. sp3d2
____ 25. The electronic geometry of the central atom in PCl3 is ____.
a. pyramidal
b. trigonal planar
c. tetrahedral
d. octahedral
e. trigonal bipyramidal
____ 26. What is the coefficient for HBr when the following equation is balanced with the smallest whole number
coefficients?
Br2 + H2O → HBr + HBrO3
a.
b.
c.
d.
e.
5
7
8
3
6
____ 27. Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed
from the decomposition of 13.2 moles of ammonium nitrate?
2NH4NO3 → 2N2 + O2 + 4H2Ο
a.
b.
c.
d.
e.
6.60
14.0
26.4
13.2
18.0
____ 28. The thermite reaction is performed using 8.6 g Fe2O3 and 1.8 g powdered Al metal. Which reactant is in
excess and by how much?
Fe2O3 + 2 Al → Al2O3 + 2Fe
a.
b.
c.
d.
e.
Al; 0.3 g
Fe2O3; 2.0 g
Al; 2.1 g
Al; 1.1 g
Fe2O3; 3.3 g
____ 29. What is the percent yield of elemental sulfur if 7.54 grams of sulfur are obtained from the reaction of 6.16
grams of SO2 with an excess of H2S?
2H2S + SO2 → 2H2O + 3S
a.
b.
c.
d.
e.
72.6%
40.8%
81.5%
88.4%
91.4%
____ 30. What is the molarity of 850. mL of a solution containing 46.2 grams of NaBr?
a. 0.495 M
b. 0.506 M
c. 0.516 M
d. 0.528 M
e. 0.545 M
____ 31. Concentrated hydrochloric acid is about 12.1 M. What volume of concentrated HCl is required to produce
5500 mL of 0.250 M?
a. 980 mL
b. 0.114 L
c. 98 mL
d. 0.211 L
e. 1114 mL
____ 32. What volume of 0.130 M HCl solution will just react with 0.424 gram of Ba(OH)2?
2HCl + Ba(OH)2 → BaCl2 + 2H2O
a.
b.
c.
d.
e.
38.1 mL
32.6 mL
24.1 mL
18.6 mL
96.7 mL
____ 33. According to the Brønsted-Lowry theory, a base is defined as ____.
a. an electron pair acceptor
b. a proton acceptor
c. an electron pair donor
d. a proton donor
e. any species that can produce hydroxide ions in aqueous solution
____ 34. Which one of the following is a weak acid?
a. H2SO4
b. HClO
c. HCl
d. HBr
e. HI
____ 35. Consider the complete neutralization reactions between the following acid-base pairs in dilute aqueous
solutions. Which one of the reactions produces insoluble salts?
a. CH3COOH + NaOH →
b.
c.
d.
e.
HNO3 + Mg(OH)2 →
H3PO4 + Ca(OH)2 →
HCl + KOH →
H2SO4 + Sr(OH)2 →
____ 36. Which of the following reactions is the net ionic equation for the acid-base reaction between H2CO3 and
Sr(OH)2?
a. H2CO3 + Sr2+ + 2OH− → SrCO3 + 2H2O
b. H3O+ + OH− → 2H2O
c. 2H3O+ + Sr2+ + 2OH− → Sr2+ + 4H2O
d. H2CO3 + 2OH− → 2H2O + CO32−
e. H2CO3 + Sr(OH)2 → 2H2O + Sr2+ + CO32−
____ 37. If 20 mL of 0.010 M H3PO4 solution is completely neutralized by 60.0 mL of Ca(OH)2 solution, what is the
molarity of the Ca(OH)2 solution?
a. 0.010 M
b. 0.200 M
c. 0.030 M
d. 0.040 M
e. 0.0050 M
____ 38. What is the oxidation number of arsenic in K3AsO4?
a. +1
b. +2
c. +3
d. +4
e. +5
____ 39. Name the molecular compound, HNO3.
a. ammonia
b. nitric acid
c. nitrous acid
d. nitric oxide
e. methane
____ 40. Balance the following equation with the smallest whole number coefficients. Choose the answer that is the
sum of the coefficients in the balanced equation. Do not forget coefficients of "one".
Cr + H2SO4 → Cr2(SO4)3 + H2
a.
b.
c.
d.
e.
7
9
11
13
15
____ 41. How many moles of O2 are required to burn completely 63.5 g of C6H6, according to the following equation?
2C6H6 + 15O2 → 12CO2 + 6H2O
a.
b.
c.
d.
0.814
12.2
6.1
0.109
e. 9.21
____ 42. Acrylonitrile, C3H3N, is a molecule used to produce a plastic called Orlon. How many grams of acrylonitrile
could be produced by reacting 583 g of propene, C3H6 with excess ammonia, NH3 and oxygen?
2C3H6 + 2NH3 + 3O2 → 2C3H3N + 6H2O
a.
b.
c.
d.
e.
368 g
1470 g
462 g
735 g
583 g
____ 43. A mixture of calcium oxide, CaO, and calcium carbonate, CaCO3, that had a mass of 3.454 g was heated until
all the calcium carbonate was decomposed according to the following equation. After heating, the sample had
a mass of 3.102 g. Calculate the mass of CaCO3 present in the original sample.
CaCO3 (solid) → CaO (solid) + CO2 (gas)
a.
b.
c.
d.
e.
0.400 g
0.800 g
1.00 g
1.60 g
0.200 g
____ 44. How many moles of carbon dioxide could be produced if 10 moles of octane, C8H18, are combined with 20
moles of oxygen?
C8H18 + 25O2 → 16CO2 + 18H2O
a.
b.
c.
d.
e.
40 mol
8.0 mol
12.8 mol
62.5 mol
20 mol
____ 45. What mass of Cu(NO3)2 can be prepared from the reaction of 3.65 grams of copper with 5.16 grams of
HNO3?
Cu + 2HNO3 → Cu(NO3)2 + H2
a.
b.
c.
d.
e.
15.4 g
10.8 g
5.14 g
10.3 g
7.68 g
____ 46. Salicylic acid reacts with acetic anhydride to form aspirin, acetylsalicylic acid. If the percent yield in this
reaction is 78.5%, what mass of salicylic acid is required to produce 150. g aspirin?
2 C7H6O3
+ C4H6O3
2 C9H8O4
+ H2O
→
salicylic acid
acetic
aspirin
anhydride
a. 292 g
b. 146 g
c. 90.0 g
d. 73.0 g
e. 191 g
____ 47. The reaction of 5.0 g of CuSO4 with excess sodium hydroxide produced 2.6 g of Cu(OH)2. What percent yield
of Cu(OH)2 was obtained?
CuSO4 + 2NaOH → Cu(OH)2 + Na2SO4
a.
b.
c.
d.
e.
52%
61%
32%
85%
92%
____ 48. What is the molarity of a barium chloride solution prepared by dissolving 2.50 g of BaCl2•2H2O in enough
water to make 400. mL of solution?
a. 2.56 × 10−2 M
b. 4.97 × 10−3 M
c. 4.09 × 10−2 M
d. 7.31 × 10−3 M
e. 5.20 × 10−2 M
____ 49. What mass of Na2SO4 is required to prepare 400. mL of 1.50 M Na2SO4 solution?
a. 213 g
b. 56.8 g
c. 71.4 g
d. 85.2 g
e. 8.52 × 104 g
____ 50. What volume of 0.250 M KOH solution contains 6.31 grams of KOH?
a. 631 mL
b. 28.1 mL
c. 450 mL
d. 2.22 mL
e. 0.44 mL
____ 51. Calculate the molarity of the resulting solution if 25.0 mL of 1.50 M HCl solution is diluted to 500. mL.
a. 13.3 M
b. 1.67 M
c. 0.0333 M
d. 0.00417 M
e. 0.0750 M
____ 52. Calculate the molarity of the resulting solution if enough water is added to 50.0 mL of 4.20 M NaCl solution
to make a solution with a volume of 2.80 L.
a. 75.0 M
b. 0.043 M
c. 33.1 M
d. 0.067 M
e. 0.0750 M
____ 53. What mass of calcium carbonate, CaCO3, is required to react with 100. mL of 2.00 M HCl solution?
CaCO3 + 2HCl → CaCl2 + CO2 + H2O
a.
b.
c.
d.
e.
5.00 g
10.0 g
15.0 g
20.0 g
23.0 g
____ 54. What volume of 0.132 M KOH solution would react completely with 25.8 mL of 0.198 M HCl according to
the following equation?
HCl + KOH → KCl + H2O
a.
b.
c.
d.
e.
86.4 mL
25.7 mL
38.7 mL
17.2 mL
3.86 mL
____ 55. According to the Arrhenius theory, which of the following is an acid?
a. NH3
b. CH4
c. HCl
d. H2
e. NaOH
____ 56. Which one of the following is a soluble, strong base?
a. CsOH
b. Cu(OH)2
c. Fe(OH)3
d. Mn(OH)2
e. Al(OH)3
____ 57. Which one of the following is not a soluble, strong base?
a. NaOH
b. KOH
c. RbOH
d. CsOH
e. NH2OH
____ 58. How many moles of HCl would react with 37.1 mL of 0.138 M Sr(OH)2?
a. 0.00511
b. 0.0102
c. 10.2
d. 0.538
e. 0.00256
____ 59. In which of the following is the oxidation number of the underlined element given incorrectly?
a.
b.
c.
d.
Element / Oxidation number
K2Cr2O7 / +6
NaAl(OH)4 / +3
HIO4 / +5
(NH4)2SO4 / +6
e. NaHSO3 / +4
____ 60. How many mL of 0.57 M AgNO3 will completely react with 121 mL of 0.95 M NaI?
AgNO3 + NaI → AgI + NaNO3
a.
b.
c.
d.
e.
72.6 mL
181 mL
202 mL
4.47 mL
0.202 mL
____ 61. Which compound is the oxidizing agent?
KOH + Cl2 → KClO3 + KCl + H2O
a.
b.
c.
d.
e.
KOH
Cl2
KClO3
KCl
H2O
____ 62. In the following net ionic reaction, ____ is the oxidizing agent and ____ is oxidized.
C + H+ + SO42− → CO2 + SO2 (acidic solution)
a.
b.
c.
d.
e.
H+; CO2
C; CO2
SO42−; H+
SO42−; C
C; SO42−
Chem 1100 Pre-Test
Answer Section
MULTIPLE CHOICE
1. ANS:
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36. ANS:
A
PTS: 1
Writing Lewis Formulas: Limitations of the Octet Rule for Lewis Formulas
B
PTS: 1
TOP: Resonance
B
PTS: 1
TOP: Trigonal Planar Electronic Geometry
D
PTS: 1
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
A
PTS: 1
TOP: Tetrahedral Electronic Geometry: AB3U Species
C
PTS: 1
TOP: Tetrahedral Electronic Geometry: AB2U2 Species
C
PTS: 1
TOP: Tetrahedral Electronic Geometry: AB3U Species
B
PTS: 1
Octahedral Electronic Geometry: AB6, AB5U, and AB4U2
C
PTS: 1
TOP: Compounds Containing Double or Triple Bonds
B
PTS: 1
Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
B
PTS: 1
TOP: Molecular Orbitals
E
PTS: 1
TOP: Bond Order and Bond Stability
B
PTS: 1
TOP: Lewis Dot Formulas of Atoms
D
PTS: 1
TOP: Lewis Dot Formulas of Atoms
C
PTS: 1
TOP: Lewis Formulas for Molecules and Polyatomic Ions
A
PTS: 1
TOP: Writing Lewis Formulas: The Octet Rule
B
PTS: 1
TOP: Writing Lewis Formulas: The Octet Rule
D
PTS: 1
TOP: Writing Lewis Formulas: The Octet Rule
C
PTS: 1
TOP: Writing Lewis Formulas: The Octet Rule
B
PTS: 1
Writing Lewis Formulas: Limitations of the Octet Rule for Lewis Formulas
A
PTS: 1
TOP: Polar and Nonpolar Covalent Bonds
B
PTS: 1
TOP: Polar Molecules: The Influence of Molecular Geometry
A
PTS: 1
TOP: Valence Bond (VB) Theory
D
PTS: 1
TOP: Valence Bond (VB) Theory
C
PTS: 1
TOP: Tetrahedral Electronic Geometry: AB3U Species
A
PTS: 1
TOP: Chemical Equations
C
PTS: 1
TOP: Calculations Based on Chemical Equations
E
PTS: 1
TOP: The Limiting Reactant Concept
C
PTS: 1
TOP: Percent Yields from Chemical Reactions
D
PTS: 1
TOP: Concentrations of Solutions
B
PTS: 1
TOP: Dilution of Solutions
A
PTS: 1
TOP: Using Solutions in Chemical Reactions
B
PTS: 1
TOP: The Brønsted-Lowry Theory
B
PTS: 1
TOP: Strengths of Acids
C
PTS: 1
TOP: Acid-Base Reactions in Aqueous Solutions
A
PTS: 1
TOP: Acid-Base Reactions in Aqueous Solutions
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TOP:
E
PTS: 1
TOP: Calculations for Acid-Base Titrations
E
PTS: 1
TOP: Balancing Redox Reactions
B
PTS: 1
TOP: Chemical Formulas
B
PTS: 1
TOP: Chemical Equations
C
PTS: 1
TOP: Calculations Based on Chemical Equations
D
PTS: 1
TOP: Calculations Based on Chemical Equations
B
PTS: 1
DIF: Harder Question
Calculations Based on Chemical Equations
C
PTS: 1
TOP: The Limiting Reactant Concept
E
PTS: 1
TOP: The Limiting Reactant Concept
B
PTS: 1
TOP: Percent Yields from Chemical Reactions
D
PTS: 1
TOP: Percent Yields from Chemical Reactions
A
PTS: 1
TOP: Concentrations of Solutions
D
PTS: 1
TOP: Concentrations of Solutions
C
PTS: 1
TOP: Concentrations of Solutions
E
PTS: 1
TOP: Dilution of Solutions
E
PTS: 1
TOP: Dilution of Solutions
B
PTS: 1
TOP: Using Solutions in Chemical Reactions
C
PTS: 1
TOP: Using Solutions in Chemical Reactions
C
PTS: 1
TOP: The Arrhenius Theory
A
PTS: 1
TOP: Acid-Base Reactions in Aqueous Solutions
E
PTS: 1
TOP: Acid-Base Reactions in Aqueous Solutions
B
PTS: 1
TOP: Calculations Involving Molarity
C
PTS: 1
TOP: Balancing Redox Reactions
C
PTS: 1
TOP: Calculations Involving Molarity
B
PTS: 1
Adding H+, OH–, or H2O to Balance Oxygen or Hydrogen
D
PTS: 1
Adding H+, OH–, or H2O to Balance Oxygen or Hydrogen