AP Chemistry Summer Review Packet (2014)
Name: __________________________________________
Section 1: Names and Formulas of ionic compounds.
Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions.
** I recommend making flashcards.
Polyatomic Ions to Know
NH4+
ClOC2H3O2ClO2CO32-
CrO42PO43Cr2O72HPO42SO32-
OHHSC2O42O22SCN-
ClO3HCO3ClO4NO2NO3-
H2PO4HSO3PO33SO42HSO4-
CNMnO4C2O42-
Name the following compounds: (Include a roman numeral if applicable)
BaSO4
Pt(NO3)4
LiOH
(NH4)2S
PbCl2
PbCl4
KI
Na2C2O4
KCN
AgCl
Fe(NO3)3
Ni(OH)2
HgS
Sr(OH)2
CaBr2
Na3PO4
Mg3(PO4)2
Zn(OH)2
BaCrO4
CsCN
CoCO3
Mn(NO3)2
HgI2
NaOH
Section 2: For each of the following compounds, write…
A) the symbols of the ions in the compound
B) the correct name
C) the number of each ion in one molecule of that compound.
11. CaI2
11. Ca+2 I– ,calcium iodide, each molecule has 1 Ca+2 ion and 1 I– ion
12. Na2CO3
12. ________________________________________________________________
13. Ga(ClO3)3
13. ________________________________________________________________
14. CuF2
14. _________________________________________________________________
15. (NH4)3PO4
15. _________________________________________________________________
16. FeSO4
16. _________________________________________________________________
17. Mg(NO3)2
17. ________________________________________________________________
18. NH4NO2
18. ________________________________________________________________
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19. KC2H3O2
19. ________________________________________________________________
20. Na2Cr2O7
20. ________________________________________________________________
Section 3: Ionic Formulas (Binary, Polyatomic, Transition Metals
Write the formula for each of the following compounds.
1. sodium hydroxide
1. ______________________
2. mercury (II) sulfate
2. ______________________
3. lead (II) phosphate
3. ______________________
4. ammonium sulfide
4. ______________________
5. aluminum chlorate
5. ______________________
6. copper (I) carbonate
6. ______________________
7. manganese (IV) oxide
7. ______________________
8. manganese (II) sulfate
8. ______________________
9. iron (III) oxide
9. ______________________
10. magnesium nitrate
10. ______________________
11. calcium sulfide
11. ______________________
12. potassium oxide
12. ______________________
13. magnesium chloride
13. ______________________
14. chromium (III) oxide
14. ______________________
15. gold (III) bromide
15. ______________________
16. beryllium fluoride
16. ______________________
17. yttrium (III) sulfide
17. ______________________
18. rubidium oxide
18. ______________________
19. aluminum dichromate
19. ______________________
20. iron (II) phosphide
20. ______________________
21. iron (III) nitrate
21. ______________________
22. chromium (III) sulfate
22. ______________________
23. tin (IV) nitride
23. ______________________
24. lead (II) permanganate
24. ______________________
25. niobium (V) oxalate
25. ______________________
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Section 4: Write the correct name for each of the following compounds.
1. Na2S
1. ______________________________________________________
2. NH4Cl
2. ______________________________________________________
3. Cu3N
3. _____________________________________________________
4. CuF2
4. ______________________________________________________
5. PbSO4
5. ______________________________________________________
6. Cr(NO3)2
6. ______________________________________________________
7. Al2O3
7. ______________________________________________________
8. N2O4
8. _____________________________________________________
9. H2S
9. ______________________________________________________
10. HClO2
10.______________________________________________________
11. H2SO3
11.______________________________________________________
12. H3PO4
12.______________________________________________________
13. HBr
13.______________________________________________________
14. H2CO3
14.______________________________________________________
15. HNO2
15.______________________________________________________
Write the chemical formula for each of the following compounds.
16. nickel (II) chloride
16. ______________________
17. cuprous nitrate
17. ______________________
18. ammonium sulfate
18. ______________________
19. magnesium nitride
19. ______________________
20. copper (I) sulfide
20. ______________________
21. carbon monoxide
21. ______________________
22. iron (II) oxide
22. ______________________
23. diphosphorus pentoxide
23. ______________________
24. hydrogen sulfate
24. ______________________
25. sulfur dioxide
25. ______________________
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Section 5: Chemical Word Equations
Directions: Write a balanced chemical equation for each of the word equations below.
a. Aqueous sodium chloride reacts with aqueous lead (II) nitrate to yield solid lead (II) chloride and aqueous sodium
nitrate
b. Aqueous barium nitrate reacts with sulfuric acid to yield solid barium sulfate and nitric acid
c. Silver nitrate reacts in solution with potassium chromate to yield solid silver chromate and aqueous potassium nitrate
d. Solid calcium carbonate reacts with hydrochloric acid to yield aqueous calcium chloride, carbon dioxide gas, and
liquid water
e. Aqueous zinc chloride reacts with dihydrogen monosulfide gas to yield solid zinc sulfide and hydrochloric acid
f. Magnesium nitrate reacts in solution with potassium hydroxide to yield solid magnesium hydroxide and aqueous
potassium nitrate
g. Solid aluminum hydroxide reacts with nitric acid to yield soluble aluminum nitrate and liquid water
h. Aqueous lead (IV) nitrate reacts with aqueous sodium sulfate to yield solid lead (IV) sulfate precipitate and aqueous
sodium nitrate
i. Aqueous sodium hydroxide reacts with carbon dioxide gas to yield aqueous sodium carbonate and liquid water
j. Solid magnesium oxide reacts with hydrochloric acid to yield a solution of magnesium chloride and liquid water
k. Solid zinc metal reacts with sulfuric acid to yield aqueous zinc sulfate and hydrogen gas
l. Solid iron (III) oxide reacts with solid aluminum metal to yield solid aluminum oxide and solid iron metal
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Section 6: Balancing Chemical Equations
Directions: First, balance each of the chemical equations below. Then, classify each reaction as synthesis,
decomposition, single-replacement, or double-replacement.
Balance the equation…
…and classify it.
a.
____ Sb + ____ Cl2  ____SbCl3
________________________
b.
____ SrBr2 + ____ (NH4)2CO3  ____ SrCO3 + ____ NH4Br
________________________
c.
____ Al + ____ Pb(NO3)2  ____ Al(NO3)3 + ____ Pb
________________________
d.
____ NaClO3  ____ NaCl + ____ O2
________________________
e.
____ Fe + ____ HCl  ____ FeCl2 + ____ H2
________________________
f.
____ CuO + ____ H2  ____ Cu + ____ H2O
________________________
f.
____ Al + ____ H2SO4  ____ Al2(SO4)3 + ____ H2
________________________
h.
____ MgBr2 + ____ Cl2  ____ MgCl2 + ____ Br2
________________________
i.
____ Ba(OH)2  ____ BaO + ____ H2O
________________________
j.
____ Pb(NO3)2 + ____ H2S  ____ PbS + ____ HNO3
________________________
k.
____ NH4NO2  ____ N2 + ____ H2O
________________________
l.
____ KClO3  ____ KCl + ____ O2
________________________
m.
____ Fe3O4 + ____ H2  ____ Fe + ____ H2O
________________________
Section 7: Percent Composition- Determine the percent by mass of each element in the following
compounds. Show all work on a separate piece of paper (Mathematically justify your answer). You may
use the back of your papers!
H2Te
K3PO4
Ca(NO3)2
(NH4)2Cr2O7
CuSO4 . 5 H2O
Section 8: Determining Empirical Formula from the Percent Composition- Determine the empirical
formula of each of the following substances. The percent composition of each substance is given. Use
a separate sheet of paper. Mathematically justify your answer!
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Section 9: Empirical & Molecular Formula Questions- Complete problems on a separate sheet of paper
and MATHEMATICALLY JUSTIFY YOUR ANSWER, including units. You may use the back of your paper!
Caffeine has the following percent composition: carbon 49.48%, hydrogen 5.19%, oxygen 16.48% and nitrogen
28.85%. Its molecular weight is 194.19 g/mol. What is its molecular formula?
What is the molecular formula of a compound with 86.88% carbon and 13.12% hydrogen and a molecular
weight of about 345?
Section 10: Stoichiometry- Part 1- Moles to moles
Directions:
A. Balance each equation.
B. Solve the problems, assuming that you have excess of the other reactant(s). MATHEMATICALLY JUSTIFY
YOUR ANSWER ON A SEPARATE PIECE OF PAPER TO RECEIVE FULL CREDIT and round
your answers to the correct number of significant figures.
(a)
____ Ca(s) + ____ N2(g)  ____ Ca3N2(s)
i. How many moles of Ca3N2 can be made from 16.8 moles of Ca?
ii. If you need to make 34.4 moles of Ca3N2, how many moles of N2 will you need?
(b)
___ Fe(s) + ____ O2(g)  ____ Fe3O4(s)
i. How many moles of O2 will react with 42.5 moles of Fe?
ii. If you need to make 1.56 moles of Fe3O4, how many moles of Fe will you need?
(c)
____ FeCl2(aq) + ____ KOH(aq)  ____ Fe(OH)2(s) + ____ KCl(aq)
i. How many moles of KOH will react with 86.2 moles of FeCl 2?
(d)
ii. If you need to make 12.4 moles of KCl, how many moles of FeCl 2 will you need?
____ Cu(s) + ____ O2(g)  ____ Cu2O(s)
i. How many moles of Cu2O can be made from 25.6 moles of Cu?
ii. How many moles of O2 does it take to produce 214 moles of Cu2O?
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Stoichiometry Part II- Mass-Mass, Mass-Volume. Complete work on a separate sheet of paper.
MATHEMATICALLY JUSTIFY YOUR ANSWER TO RECEIVE FULL CREDIT and round your answers to
the correct number of significant figures.
(e) Given the balanced chemical equation
2 Ag + I2  2 AgI
(i) How many grams of silver metal (Ag) are required to react completely with 51.8 g of iodine (I 2) to produce silver
iodide (AgI)?
(ii) How many grams of silver iodide will be formed?
2 ZnS(s) + 3 O2 (g)  2 ZnO(s) + 2 SO2(g)
(f) If 500. g of lithium oxide (Li2O) are required to be produced according to the unbalanced equation:
Li + O2  Li2O
Calculate the mass of lithium and volume of oxygen (at STP) needed to react.
(g) The solid fuel in the booster stage of the space shuttle is a mixture of ammonium perchlorate and aluminum powder,
which react as follows:
6 NH4ClO4(s) + 10 Al(s)  5 Al2O3(s) + 3 N2(g) + 6 HCl(g) + 9 H2O(g)
(i)What mass of aluminum is required to react with 500.0 g of ammonium perchlorate?
(ii) Determine the volume (assume STP) of each of the gases produced.
Limiting/Excess Reagent: MATHEMATICALLY JUSTIFY YOUR ANSWER TO RECEIVE FULL CREDIT and round
your answers to the correct number of significant figures.
(h) A solution containing 5.0 g of silver nitrate was mixed with another containing 5.0 g of potassium
chloride.
(i) Determine the 2 products of the reaction and write a balanced chemical equation.
(ii) Determine which substance is the limiting reagent- silver nitrate or potassium chloride.
(iii) Calculate the mass of each of the products formed.
(i) If 36.5 g of HCl and 73 g of Zn are reacted according to the equation:
2 HCl + Zn  ZnCl2 + H2
(i) Determine which reactant is the limiting reactant,
(ii) Find the mass of ZnCl2 formed,
(iii) Find the volume of H2 (@ STP) formed,
(iv) Determine which reactant is in excess and by how much.
(j) According to the balanced chemical equation below:
Cu(s) + 2 AgNO3(aq)  Cu(NO3) 2(aq) + 2 Ag(s)
(i) How many grams of silver will be produced from combining 100 g of copper with 200 g of silver nitrate?
(ii) If the reaction is 65% efficient, determine the actual yield of silver produced.
Section 11: Solutions and Molarity
Mathematically justify your answer and round your answers to the correct number of significant figures.
Determine the molarity of the following solutions.
(a) 50.0 grams of Na2CO3 is dissolved in enough water to make 10.00 liters of solution.
(b) 13.55 grams of (NH4)2CO3 is dissolved in enough water to make 250 mL of solution.
(c) 1.25 grams of PbCl2 is dissolved in enough water to form 45.0 mL of solution.
Determine the mass of solute required to make each of the following solutions.
(d) 500. ml of a 2.75 M NaF solution.
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(e) 1.5 L of a 1.00 M KCl solution.
(f) 750 ml of a 3.50 M CaCl2 solution
Determining the volume of solution:
(g) What volume (in mL) of 2.0 M NaCl is needed to contain 5.00 g NaCl?
(h) What volume (in mL) of 6.0 M HCl is needed to contain 1.5 g of HCl?
Dilutions- Use the formula M1V1 = M2V2 to solve each of the following problems.
(i) 40.0 mL of 0.400 M NaOH solution is diluted to a final volume of 200.0 mL, calculate the new
concentration.
(j) A 0.350 M solution is concentrated by evaporation to a reduced final volume of 100.0 mL and a molarity of
0.825 M. Calculate the original volume.
(k) 85.0 mL of a solution of NaOH is diluted to a final volume of 290.0 mL and the new molarity is 0.0500 M.
Calculate the original molarity of the base.
Textbook problems: Show all work! p. 128 #37,39
p. 129 #51 a & b, 53,57,59,61, 69,71
p. 130 #76 a-c, 81d,
p. 131 #91, 95 b, c,
p. 132 #105, 115, 117, 118
Answers are found in the appendix. Mathematically justify your answer
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