AP Chemistry Test (Chapter 4)
(Green Bean Casserole)
Please use the answer sheet!!
Multiple Choice/FIB (50%)
Please use the following choices to answer questions 1-6.
A)
C)
E)
I)
Sugar (C11H22O12)
OF
H2O
Alcohol (CxHyOz)
B)
D)
H)
K)
NH4F
PbSO4
Butter (CxHyOz)
N2
1)
Please choose all polar covalent substances.
2)
Please choose all nonpolar covalent substances.
3)
Please choose all soluble substances.
4)
Please choose all substances containing both ionic and covalent bonds.
5)
Please choose all ionic substances.
6)
Please choose all substances that will dissociate in water.
7)
Which one best describes the water molecule?
A)
δ-
C)
δ+
8)
δ-
δ+
H
O
H
δ+
δ-
δ+
H
O
H
H
D)
H
O
δ+
δ+
B)
H
O
δ-
δ-
δ-
H
Please choose all false statements.
A)
B)
C)
D)
E)
All ionic substances dissociate in water.
Water is polar covalent.
All polar covalent substances dissociate in water.
All nonpolar covalent substances are soluble in water.
All polar covalent substances dissolve in water.
9)
Please choose all true statements.
A)
B)
C)
D)
E)
10)
Please choose all true statements.
A)
B)
C)
D)
E)
11)
Water dissociates in water.
Soluble polar covalent substances dissociate in water.
Soluble ionic substances dissociate in water.
All nonpolar covalent substances are insoluble in water.
Nonpolar covalent substances dissociate in water.
Ionic formula units have extreme dipoles.
Oil has slight dipoles.
Water has no dipoles.
N2 has no dipoles.
AlCl3 has slight dipoles.
Please choose all true statements.
A)
B)
C)
D)
E)
Atoms in an ionic bond have extreme dipoles because the atoms transfer valence
electrons completely.
Atoms in a nonpolar covalent bond have no dipoles because the atoms share valence
electrons equally.
Atoms in a polar covalent bond have slight dipoles because the atoms share valence
electrons unequally.
Atoms in a polar covalent bond have slight dipoles because the atoms share valence
electrons equally.
Atoms in an ionic bond have no dipoles because the atoms share electrons unequally.
Please use the following choices to answer questions 12-14.
A)
C)
E)
I)
Ca(OH)2
H2Cr2O7
Sugar (C11H22O12)
CuI2
12)
Please choose all weak electrolytes.
13)
Please choose all nonelectrolytes.
14)
Please choose all strong electrolytes.
15)
Which one best describes a nonelectrolyte?
A)
B)
C)
D)
E)
B)
D)
H)
K)
H2SO4
Al2(C2O4)3
Zn(OH)4
Mn(C2H3O2)5
An ionic compound with a low lattice energy produces ions in the solution.
An ionic compound with a high lattice energy produces ions in the solution.
A polar covalent compound produces ions in the solution.
A covalent compound produces no ions in the solution.
A strong acid or base produces no ions in the solution.
16)
Which one best describes a weak electrolyte?
A)
B)
C)
D)
E)
17)
Which one best describes a strong electrolyte?
A)
B)
C)
D)
E)
18)
Na3PO4
Na2SO4
None of these
B)
D)
Cu3(PO4)2
CuPO4
Which one would be most appropriate for making exactly 500 ml of a solution?
A)
B)
C)
D)
E)
21)
Al(OH)3 (s) + 3 HClO3 (aq)  3 HOH + Al(ClO3)3
2 O2 (g) + N2 (g)  2 NO2 (g)
K2C2O4 (aq) + 2 HClO4 (aq)  2 KClO4 + H2C2O4
Pb(OH)4 (aq) + 4 HI (aq)  PbI4 + 4 HOH
2 Al(OH)3 (s) + 3 CaCl2 (aq)  2 AlCl3 + 3 Ca(OH)2
Which one is the formula for the precipitate that forms when aqueous
copper (II) sulfate is mixed with aqueous sodium phosphate?
A)
C)
E)
20)
An ionic compound with a small lattice energy yields a large percentage of ions in
the solution.
A polar covalent compound yields a small percentage of ions in the solution.
A polar covalent compound yields a large percentage of ions in the solution.
An ionic compound with a large lattice energy yields a large percentage of ions in
the solution.
A weak acid or base yields a small percentage of ions in the solution.
Which reaction will cause the light bulb on a conductivity tester to glow the brightest if
neither reactant is limiting or excess?
A)
B)
C)
D)
E)
19)
A strong acid or base yields a small percentage of ions in the solution.
A weak acid or base yields a small percentage of ions in the solution.
An ionic compound with a low lattice energy yields a small percentage of ions in the
solution.
A polar covalent compound yields a small percentage of ions in the solution.
A polar covalent compound yields a large percentage of ions in the solution.
Graduated cylinder and volumetric flask
Beaker and graduated cylinder
Buret and graduated cylinder
Buret and volumetric flask
Beaker and volumetric flask
What is the oxidation number of P in the P3O8—4 ion?
A)
C)
E)
+12
+4
None of these
B)
D)
-3
+3
Please consider the following reaction to answer questions 22-25.
N2O (g) + ClO— (aq)  Cl— (aq) + NO2— (aq)
22)
What species is reduced?
23)
What element is oxidized?
24)
What species loses electrons?
25)
What element is the oxidizing agent?
Free Response (66%)
Please show all your work for any credit!!
1)
A 0.8133-g sample of copper is dissolved in a small amount of HNO3 to form Cu3+ ions in
solution. The resulting solution is diluted to a total volume of 400.0 ml. Please calculate the
molarity of the Cu3+ ions.
2)
How would you prepare 500.0 ml of a 0.325 M H2SO4 solution from a stock solution
of 16.0 M?
3)
Please calculate the concentration of all ions in a 0.179 M Fe2(SO4)5 solution.
4)
You evaporate 50.0 ml of 0.312 M Na2Cr2O7 solution to dryness. What mass of Na2CrO7
will be present?
Please consider the following information to answer questions 5-7.
2 Cr(ClO3)5 + 5 Na2C2O4  10 NaClO3 + Cr2(C2O4)5
95.00 ml of 0.407 M Cr(ClO3)5 is slowly added to 100.0 ml of 0.528 M Na2C2O4. A chemistry
student collects and dries the precipitate. The precipitate has a mass of 5.204 g.
5)
How many moles of limiting reagent are consumed?
6)
Please calculate the % yield of the precipitate and give a likely source of error to explain the
% yield.
7)
Please calculate the concentration of the excess reagent after the reaction is complete.
8)
An 2.912-g impure sample of Al2(CO3)3 is titrated with 30.0 ml of 0.644 M HCl until the
reaction appears to be complete. What is the mass % Al 2(CO3)3 in the impure sample?
Al2(CO3)3 + 6 HCl  2 AlCl3 + 3 H2O + 3 CO2
9)
A solution is 15.4 M H2C2O4. The solution has a density of 1.12 g/ml. What is the
mass % of H2C2O4?
10)
A 400.0-ml sample of a 0.245 M CaCl2 solution is accidentally left on a hot plate overnight.
The next morning, the solution is 0.391 M. What volume of water evaporated from the
original solution of CaCl2?
11)
What volume of 0.144 M Al(NO3)3 solution is necessary to completely react with
78.20 ml of 0.155 M H2C2O4 solution?
2 Al(NO3)3 + 3 H2C2O4  6 HNO3 + Al2(C2O4)3
AP Chemistry Test (Chapter 4)
(Turkey and Dressing)
Please use the answer sheet!!
Multiple Choice/FIB (50%)
Please use the following choices to answer questions 1-6.
A)
C)
E)
I)
PbSO4
N2
Butter (CxHyOz)
NH4F
B)
D)
H)
K)
Alcohol (CxHyOz)
Sugar (C11H22O12)
H2O
OF
1)
Please choose all polar covalent substances.
2)
Please choose all nonpolar covalent substances.
3)
Please choose all soluble substances.
4)
Please choose all substances containing both ionic and covalent bonds.
5)
Please choose all ionic substances.
6)
Please choose all substances that will dissociate in water.
7)
Which one best describes the water molecule?
A)
δ+
C)
δ-
8)
δ-
δ-
H
O
H
δ+
δ-
δ+
H
O
H
H
D)
H
O
δ-
δ+
B)
H
O
δ+
δ-
δ+
H
Please choose all false statements.
A)
B)
C)
D)
E)
All polar covalent substances dissolve in water.
Water is polar covalent.
All polar covalent substances dissociate in water.
All nonpolar covalent substances are soluble in water.
All ionic substances dissociate in water.
9)
Please choose all true statements.
A)
B)
C)
D)
E)
10)
Please choose all true statements.
A)
B)
C)
D)
E)
11)
Water dissociates in water.
Soluble polar covalent substances dissociate in water.
Nonpolar covalent substances dissociate in water.
All nonpolar covalent substances are insoluble in water.
Soluble ionic substances dissociate in water.
Water has no dipoles.
Oil has slight dipoles.
Ionic formula units have extreme dipoles.
N2 has no dipoles.
AlCl3 has slight dipoles.
Please choose all true statements.
A)
B)
C)
D)
E)
Atoms in an ionic bond have no dipoles because the atoms share electrons unequally.
Atoms in a nonpolar covalent bond have no dipoles because the atoms share valence
electrons equally.
Atoms in a polar covalent bond have slight dipoles because the atoms share valence
electrons equally.
Atoms in a polar covalent bond have slight dipoles because the atoms share valence
electrons unequally.
Atoms in an ionic bond have extreme dipoles because the atoms transfer valence
electrons completely.
Please use the following choices to answer questions 12-14.
A)
C)
E)
I)
Zn(OH)4
Al2(C2O4)3
Mn(C2H3O2)5
Ca(OH)2
12)
Please choose all weak electrolytes.
13)
Please choose all nonelectrolytes.
14)
Please choose all strong electrolytes.
15)
Which one best describes a nonelectrolyte?
A)
B)
C)
D)
E)
B)
D)
H)
K)
H2SO4
H2Cr2O7
CuI2
Sugar (C11H22O12)
An ionic compound with a low lattice energy produces ions in the solution.
An ionic compound with a high lattice energy produces ions in the solution.
A covalent compound produces no ions in the solution.
A polar covalent compound produces ions in the solution.
A strong acid or base produces no ions in the solution.
16)
Which one best describes a weak electrolyte?
A)
B)
C)
D)
E)
17)
Which one best describes a strong electrolyte?
A)
B)
C)
D)
E)
18)
Na3PO4
Na2SO4
None of these
B)
D)
CuPO4
Cu3(PO4)2
Which one would be most appropriate for making exactly 500 ml of a solution?
A)
B)
C)
D)
E)
21)
Al(OH)3 (s) + 3 HClO3 (aq)  3 HOH + Al(ClO3)3
2 Al(OH)3 (s) + 3 CaCl2 (aq)  2 AlCl3 + 3 Ca(OH)2
K2C2O4 (aq) + 2 HClO4 (aq)  2 KClO4 + H2C2O4
Pb(OH)4 (aq) + 4 HI (aq)  PbI4 + 4 HOH
2 O2 (g) + N2 (g)  2 NO2 (g)
Which one is the formula for the precipitate that forms when aqueous
copper (II) sulfate is mixed with aqueous sodium phosphate?
A)
C)
E)
20)
An ionic compound with a large lattice energy yields a large percentage of ions in
the solution.
A polar covalent compound yields a small percentage of ions in the solution.
A polar covalent compound yields a large percentage of ions in the solution.
An ionic compound with a small lattice energy yields a large percentage of ions in
the solution.
A weak acid or base yields a small percentage of ions in the solution.
Which reaction will cause the light bulb on a conductivity tester to glow the brightest if
neither reactant is limiting or excess?
A)
B)
C)
D)
E)
19)
A weak acid or base yields a small percentage of ions in the solution.
A strong acid or base yields a small percentage of ions in the solution.
An ionic compound with a low lattice energy yields a small percentage of ions in the
solution.
A polar covalent compound yields a small percentage of ions in the solution.
A polar covalent compound yields a large percentage of ions in the solution.
Beaker and volumetric flask
Beaker and graduated cylinder
Buret and graduated cylinder
Buret and volumetric flask
Graduated cylinder and volumetric flask
What is the oxidation number of P in the P3O8—4 ion?
A)
C)
E)
+3
-3
None of these
B)
D)
+12
+4
Please consider the following reaction to answer questions 22-25.
Cl— (aq) + NO2— (aq)  N2O (g) + ClO— (aq)
22)
What species is reduced?
23)
What element is oxidized?
24)
What species loses electrons?
25)
What element is the oxidizing agent?
Free Response (66%)
Please show all your work for any credit!!
1)
A 0.1133-g sample of copper is dissolved in a small amount of HNO3 to form Cu3+ ions in
solution. The resulting solution is diluted to a total volume of 200.0 ml. Please calculate the
molarity of the Cu3+ ions.
2)
How would you prepare 500.0 ml of a 0.425 M H2SO4 solution from a stock solution
of 18.0 M?
3)
Please calculate the concentration of all ions in a 0.479 M Fe2(SO4)5 solution.
4)
You evaporate 70.0 ml of 0.512 M Na2Cr2O7 solution to dryness. What mass of Na2CrO7
will be present?
Please consider the following information to answer questions 5-7.
2 Cr(ClO3)5 + 5 Na2C2O4  10 NaClO3 + Cr2(C2O4)5
99.00 ml of 0.507 M Cr(ClO3)5 is slowly added to 108.0 ml of 0.521 M Na2C2O4. A chemistry
student collects and dries the precipitate. The precipitate has a mass of 5.704 g.
5)
How many moles of limiting reagent are consumed?
6)
Please calculate the % yield of the precipitate and give a likely source of error to explain the
% yield.
7)
Please calculate the concentration of the excess reagent after the reaction is complete.
8)
An 3.912-g impure sample of Al2(CO3)3 is titrated with 20.0 ml of 0.644 M HCl until the
reaction appears to be complete. What is the mass % Al 2(CO3)3 in the impure sample?
Al2(CO3)3 + 6 HCl  2 AlCl3 + 3 H2O + 3 CO2
9)
A solution is 17.4 M H2C2O4. The solution has a density of 1.12 g/ml. What is the
mass % of H2C2O4?
10)
A 400.0-ml sample of a 0.285 M CaCl2 solution is accidentally left on a hot plate overnight.
The next morning, the solution is 0.402 M. What volume of water evaporated from the
original solution of CaCl2?
11)
What volume of 0.122 M Al(NO3)3 solution is necessary to completely react with
58.20 ml of 0.165 M H2C2O4 solution?
2 Al(NO3)3 + 3 H2C2O4  6 HNO3 + Al2(C2O4)3
AP Chemistry Test (Chapter 4)
Form_____________
Name________________________
Multiple Choice/FIB (50%)
1)
_______________
16)
_______________
2)
_______________
17)
_______________
3)
_______________
18)
_______________
4)
_______________
19)
_______________
5)
_______________
20)
_______________
6)
_______________
21)
_______________
7)
_______________
22)
_______________
8)
_______________
23)
_______________
9)
_______________
24)
_______________
10)
_______________
25)
_______________
11)
_______________
12)
_______________
13)
_______________
14)
_______________
15)
_______________
Problems (66%)
1)
Please use only the front side of each piece of paper.
2)
Please number your problems clearly and consecutively.
3)
Please staple your problems to the back of this page in numerical order.
4)
Please write on the paper in the conventional manner.
5)
Please do not make a separate list of answers. Record your answer at the end of the work
supporting your answer.
6)
Please circle/box your answer.