AP Chemistry Summer

Prerequisite ReviewANSWER KEY

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Adapted from: Bergmann-Sams

DUE JULY 1PART A. COMPOUNDS AND EQUATIONSBalancing Ionic CompoundsGiven the names of the elements that form a compound, determine their ionic charge and write the chemical symbols for the compound.

EX: Lithium OxygenLi2O Li+ O2-

1. Sodium SulfurNa+ S2-

Na2S

2. Potassium ChlorineK+ Cl-

KCl

3. Rubidium SulfateRb+ SO4

2-

Rb2SO4

4. Magnesium NitriteMg2+ NO2

-

Mg(NO2)2

5. Strontium IodineSr2+ I-

SrI2

6. Aluminum PerchlorateAl3+ ClO4

-

Al(ClO4)3

7. Ammonium PhosphateNH4

+ PO43-

(NH4)PO4

8. Hydronium BromineH3O+ Br-

H3OBr

9. Cupric CarbonateCu2+ CO3

2-

CuCO3

10. Iron (II) IodateFe2+ IO3

-

Fe(IO3)2

11. Ferrous hydroxideFe2+ OH-

Fe(OH)2

12. Ferric NitrateFe3+ NO3

-

Fe(NO3)3

Given chemical symbols below, determine the ionic charges of each element and then write the balanced chemical symbol for each compound formed.

EX: Na ClO3 Na2CO3

1. H Pb2+

H2Pb

2. Li NO3

LiNO3

3. Be CO3

BeCO3

4. H SO3

H2SO3

5. Ca NCa3N2

6. Cs BrCsBr

7. Fe3+ FFeF3

8. Ag+ SeAg2Se

Naming Ionic CompoundsFor each ionic compound, list the cation(s), anion(s), chemical formula, and electron dot structure

1. sodium iodide Chemical Formula Electron Dot Structure

cations _____Na_______NaI

anions _____I________

2. magnesium chloride Chemical Formula Electron Dot Structure

cations ____Mg2+_______MgCl2

anions ____Cl-________

3. aluminum sulfide Chemical Formula Electron Dot Structure

cations ____Al3+________Al2S3

anions _____S2-______

4. iron (III) oxide Chemical Formula Electron Dot Structure

cations _____Fe3+_______Fe2O3

anions ______O2-______

5. stannous bromide Chemical Formula Electron Dot Structure

cations _____Sn2+_________SnBr2

anions _____Br-_______

6. plumbic oxide Chemical Formula Electron Dot Structure

cations ____Pb2+________ PbO

anions ____O2- ____Balance Chemical ReactionsRewrite each chemical equation with the correct coefficients necessary to balance the equation.

1. NaCO3(aq) + Ca(OH) (aq) _____ NaOH(aq) + _____ CaCO3(s)

Na2CO3(aq) + Ca(OH)2 (aq) ___2_ NaOH(aq) + _____ CaCO3(s)

2. KPO4(aq) + _____ MgCl(aq) _____ Mg(PO4) (s) + _____ KCl (aq)

2 K3PO4(aq) + ___3_ MgCl2(aq) _____ Mg3(PO4)2 (s) + ___6_ KCl (aq)

3. Cu (s) + ____ H2SO4 (aq) ____ CuSO4 (aq) + ____ H2O (l) + ____ SO2 (g)

Cu (s) + __2__ H2SO4 (aq) ____ CuSO4 (aq) + ___2_ H2O (l) + ____ SO2 (g)

4. FeS (s) + HCl (aq) FeCl (aq) + HS (g)

FeS (s) + 2 HCl (aq) FeCl2(aq) + H2S (g)

5. Fe (s) + CuNO3 (aq) Cu (s) + Fe(NO3) (aq)

Fe (s) + 2 CuNO3 (aq) 2 Cu (s) + Fe(NO3)2 (aq)

6. KI (aq) + Cl2 (g) KCl (aq) +I2 (aq)

2KI (aq) + Cl2 (g) 2 KCl (aq) + I2 (aq)

7. Al (s) + S (s) AlS (s)

2Al (s) + 3 S (s) Al2S3(s)

Reaction TypesThis is an instructional sheet to help you understand chemical reactions and to be able to predict the products of chemical reactions.There are 5 types of reactions in chemistry.

I. Combustiona. The combustion of an organic material

i. EX: C3H8 + 5O2 3CO2 + 4H2Oii. The products are always carbon dioxide and water. The only thing that changes is the

organic material and the coefficients needed to balance the equation.

II. Combinationa. A + B Xb. EX: 2Mg + O2 2MgO

III. Single-Replacementa. Use the Activity Series to determine if an elemental metal will replace the metal in a compound

based upon the reactivity of the metalsi. EX: Fe + 2AgNO3 Fe(NO3)2 + 2Ag

ii. EX: Cu + Zn(NO3)2 X or NRIV. Double-Replacement

a. The cations of two ionic compounds exchange anionic partnersi. EX: NaOH + HCl NaCl + HOH

V. Decompositiona. The opposite of a combination reactionb. A compound decomposes into elements and compoundsc. Typical products include CO2, H2, O2

i. EX: BaCO3 BaO + CO2

ii. 2Zn(OH)2 2ZnO + 2H2

iii. Ni(ClO4)2 NiCl2 + 8O2

d. There are tests for each type of product formed

Predict the products. Identify the reaction type. ALWAYS balance the equation.1. Zn2+ + Ca(OH)2 Ca + Zn(OH)2

Single replacement

2. LiCl + KBrO3 LiBrO3 + KClDouble replacement

3. 2C2H6 + 7O2 4CO2 + 6H2Ocombustion

4. 2 MgO + Δ 2 Mg + O2

decomposition

5. 2 Hydrogen + Oxygen 2H2Ocombination

Balance and Identify Chemical ReactionsBalance each equation with coefficients (all componds should already be balanced) and identify the reaction type.

1. 2Hf + 2N2 Hf2N4

combination

2. Mg + H2SO4 MgSO4 + H2

Single replacement

3. 2C2H6 + 7O2 4CO2 + 6H2O

combustion

4. Pb(NO3)2 + 2 NaI PbI2 + 2 NaNO3

Double replacement

5. 3Fe + 2O2 Fe3O4

combination

6. 2Pb(NO3)2 2PbO + 4NO2 + O2

decomposition

7. Hg(NO3)2 + 2NH4SCN Hg(SCN)2 + 2NH4NO3

Double replacement

8. (NH4)2SO4 + 2NaOH 2NH3 + 2H2O + Na2SO4

Decomposition or Double Replacement

Predict the products, balance, and identify the type of reaction

9. Al + H2SO4 H2 + Al2(SO4)3

Single replacement

10. 2HCl + Ba(OH)2 2H2O + BaCl2

Double replacement

11. 2Au + 2HCl 2AuCl + H2

Single Replacement

Decomposition and Synthesis ReactionsA synthesis reaction is the opposite of a decomposition reaction. This practice will help us recognize the products for common decomposition reactions1) Sodium + Oxygen

4Na + O2 2Na2O

2) Lithium + Sodium chloride

Li + NaCl LiCl + Na

3) Sodium chloride and heat

NaCl + heat Na + Cl2

4) Potassium chlorate

2KClO3 + heat 2KCl + 3O2

5) Copper (II) + Oxygen

2Cu + O2 2CuO

6) Aluminum + Hydrogen chloride

2Al + 6HCl 3H2 + 2AlCl3

7) Magnesium + Oxygen

2Mg + O2 2MgO

8) Silver + Chlorine

2Ag + Cl2 2AgCl

9) Aluminum oxide and heat

2Al2O3 + heat 4Al + 3O2

DUE AUGUST 1PART B. STOICHIOMETRYStoichiometry Worksheet: Molecule to Mass/Mole

1. How many molecules are there in 24 grams of FeF3?

1.28x1023 molecules FeF3

2. How many molecules are there in 450 grams of Na2SO4?

1.91x1024 molecules Na2SO4

3. How many grams are there in 2.3 x 1024 atoms of silver?

411.9 g Ag

4. How many grams are there in 7.4 x 1023 molecules of AgNO3?

208.8 g AgNO3

5. How many grams are there in 7.5 x 1023 molecules of H2SO4?

122.1 g H2SO4

6. How many molecules are there in 122 grams of Cu(NO3)2?

3.92x1023 molecules Cu(NO3)2

7. How many grams are there in 9.4 x 1025 molecules of H2?

312.3 g H2

8. How many molecules are there in 230 grams of CoCl2?

1.06x1024 CoCl2

Stoichiometry Worksheet: Moles and Moles1. Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur

dioxide: 5C(s) + 2SO2(g) -----> CS2(s) + 4CO(g)

a. How many moles of CS2 form when 6.3 mol of C reacts? THIS EXAMPLE IS DONE FOR YOU!

6.3mol C 1 mol CS2 = 1.26 mol CS2

5 mol C2. How many moles of carbon are needed to react with 7.24 moles of SO2

18.1 mol C

3. Silver can be made according to the following equation:2AgNO3+ Ca Ca(NO3)2 + 2Ag

a. Balance the equationb. Identify the type of reaction Single Replacement

c. If 35.3 moles of silver nitrate are reacted how many moles of silver are produced?

35.3 mol Ag

4. How many moles of carbon dioxide are formed when 44-mol of CH4 is burned?

44 mol CO2

5. How many moles of calcium phosphate is formed when 32.5-mols of calcium nitrate reacts with sodium phosphate?

3Ca(NO3 )2+2Na3PO4→Ca3 (PO4 )2+6NaNO3

32 .5mol ?mol32 .5molCa(NO3 )2

1x

1molCa3 (PO4 )2

3molCa(NO3 )2=10 .8molCa3(PO4 )2

Stoichiometry Worksheet: Moles and Moles6. Car batteries are called lead storage batteries because of their use of large quantities of lead. These

batteries utilize the following equation.Pb + PbO2 +2H+ + 2HSO4

- 2PbSO4 + 2 H2O

34 . 3gPbO 2

1x

1molPbO2

239 gPbO2x

2molH 2O1molPbO2

x18gH 2O1molH 2O

=

5 .16 gH 2O34 . 3gPbO 2

1 x1molPbO2

239 gPbO2x

2molPbSO4

1molPbO2x

303gPbSO4

1molPbSO4=

¿87 . 0gPbSO 4

7. 32.5-g of ZnSO4 reacts to form how many grams of BaSO4 according to the following equation. a. Balance the equationb. Identify the type of reaction

32 .5 gZnSO4

1x

1molZnSO4

161gZnSO4x

1molBaSO4

1molZnSO4x

233gBaSO 4

1molBaSO4=

¿47 .0 gBaSO4

8. When sodium metal is added to water the resulting gas, Hydrogen can often explode. How many Liters of hydrogen gas is produced when 41.2-g of sodium is dropped into water. You must balance the equation in order to solve the problem.

Na + HOH NaOH + H2

41 .2gNa1

x1molNa23 gNa

x1molH 2

2molNax

22.4 LH2

1molH 2=

¿20 .1 LH 2

9. 43.5-grams of barium sulfate is formed from the reaction of barium nitrate and sodium sulfate. How many moles of sodium sulfate reacted?

Ba(NO 3 )2+Na2 SO4→BaSO 4+2 NaNO3

?mol 43 . 5g43 .5g BaSO4

1x

1molBaSO4

233gBaSO4x

1molNa2 SO4

1molBaSO4=0. 187molNa2 SO4

Stoichiometry Worksheet: Volume1. Barium oxide reacts with carbon dioxide to make Barium carbonate:

BaO + CO2 BaCO3

a. Balance the equationb. Identify the type of reaction Single Replacement

c. If 23.4 moles of barium oxide react, how many liters of CO2 are required at STP?

23 . 4molBaO1

x1molCO2

1molBaOx

22. 4 LCO2

1molCO2=524 LCO2

2. Ammonia, (NH3) is produced by reacting its elements with each other according to the following equation:

N2 + 3H2 2NH3

a. Balance the equationb. Identify the type of reaction Combination

c. If 34.3-L of nitrogen is reacted with hydrogen, how many liters at STP of ammonia will be formed?

34 . 3 LN2

1x

2LNH 3

molN 2=68 .6 LNH 3

3. Calculate the volume of carbon dioxide produced when 250 g of pentane, C5H12, burn. Assume the carbon dioxide is cooled to STP.

250 gC5H12

1x

1molC5H12

72 gC5H12x

5molCO2

1molC5H12x

22. 4 LCO2

1molCO2=

389 LCO2

4. Propane is a gas used often for backyard grills. How many Liters of CO2 is produced when 54.9-L of propane (C3H8) is burned according to the following equation. Again, you must balance the equation in order to solve the problem.

C3H8 + O2 CO2 + H2O

54 . 9 LC3H8

1x

3 LCO2

1molC3H8=165 LCO2

Stoichiometry Worksheet: Grams1. 14.5-g of cesium explosively reacts with water to form hydrogen and cesium hydroxide. How many

molecules of hydrogen were formed?

2Cs+2H 2O→2CsOH+H214 . 5g ?molec14 . 5gCs1

x1molCs133gCs

x1molH 2

2molCsx

6 . 02 x 1023molecH 2

1molH 2=

3 .28 x 1022molecH 2

2. How many molecules of chlorine are needed to react with 5.6 g of iron to form iron III chloride?

5 .6 gFe1

x 1molFe56gFe

x3molCl22molFe

x6 .02 x1023molecCl21molCl2

=

9 .03 x1022molecCl2

3. What mass of ammonia, NH3, is necessary to react with 2.1 x 1024 molecules of oxygen when ammonia (NH3) reacts with oxygen to form water and nitrogen dioxide?

2 .1 x1024molecO2

1x

1molO2

6 .02 x1023molecO2

x4molNH 3

7 molO2x

17 gNH 3

1molNH 3=

33 . 9gNH 3

4. 22.8-g of NaOH is reacted with hydrochloric acid. How many grams of water is formed?

NaOH+HCl→HOH+NaCl22 .8 g ?g22 .8gNaOH1

x1molNaOH40 gNaOH

x1molHOH1molNaOH

x 18gHOH1molHOH

=10 .3gHOH

5. 32.5-grams of iron III chloride reacts with silver nitrate. How many grams of silver chloride are formed?

3 .25 gCu(NO3)2

1x

1molCu(NO3 )2

187 . 5gCu(NO3 )2x

1molCu(OH )2

1molCu(NO3 )2x

97 .5 gCu(OH )2

1molCu(OH )2=

1 .69 gCu(OH )2

Stoichiometry Worksheet: Grams6. 34.5-grams of Lithium reacts with Chromium III chloride. How many grams of lithium chloride is

formed?

3 Li+CrCl3→3LiCl+Cr34 . 5g ?g34 . 5gLi1

x 1molLi7gLi

x3molLiCl3molLi

x42 . 5gLiCl1molLiCl

=209gLiCl

7. 43.5-grams of copper II sulfate is reacted with barium nitrate. How many grams of precipitate are formed?

8. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride.

CuSO4+Ba(NO3 )2→BaSO4( s )

+Cu(NO3 )2(aq)

43 .5g g?43 .5gCuSO4

1x

1molCuSO4

159. 5 gCuSO4x

1molBaSO4

1molCuSO4x

233gBaSO 4

1molBaSO4=

63 .5 gBaSO4

9. Silver nitrate reacts with sodium chloride to make the silver chloride and sodium nitrate. When 2.53 grams of silver nitrate is reacted. How many grams of silver chloride are formed?

2 .53 gAgNO3

1x

1molAgNO3

170 gAgNO3x1molAgCl

1molAgNO3x 143. 5gAgCl

1molAgCl=

2 .14 gAgCl

10. When 3.25 g of copper II nitrate reacts with ammonium hydroxide. How many grams of the precipitate will form?

3 .25 gCu(NO3 )2

1x

1molCu (NO3 )2

187 . 5gCu(NO3 )2x

1molCu (OH )2

1molCu (NO3 )2x

97 .5 gCu(OH )2

1molCu(OH )2=

1 .69 gCu(OH )2

Stoichiometry Worksheet: Limiting Reactants1. When 114.0 g of iron and 292.7 g of chlorine gas reacts, iron(III) chloride is formed.

2Fe+3Cl2→2FeCl3114g 292 .7g ?g114gFe1

x 1molFe56 gFe

x2molFeCl32molFe

x162 .5 gFeCl31molFeCl3

=331gFeCl

¿

¿ 3 ¿¿ ¿¿ ¿292 .7gCl2

1 x1molCl2

71 gCl2x

2molFeCl33molCl2

x162.5gFeCl3

1molFeCl3=447 gFeCl3 ¿ Fe is the LR because it yielded the smallest answer ¿

114gFe1 x 1molFe

56 gFe x3molCl22molFe x

71 gCl21molCl2

=217gCl2 usedup ¿292. 7−217g=75 .9gCl2 left ¿¿

2. 20 L of oxygen react with 1.0L of methyl alcohol, CH3OH.2CH 3OH+3O2→2CO2+4 H2O1 .0L 20L ?L1 .0 LCH 3OH1

x4 LH2O2 LCH 3OH

=2 LH 2O

20 LO2

1x

4 LH 2O3 LO2

=27 LH 2O

CH 3OH is the LR because it yielded the smallest answer1 .0 LCH 3OH1 x

3 LO2

2 LCH 3OH=1 .5 LO2

20 L−1 .5 L=18 . 5 LO2 Left

Stoichiometry Worksheet: Limiting Reactants3. 25 g of hydrazine, N2H4(l), and 66 g of hydrogen peroxide, H2O2(l), react to produce nitrogen gas and water.

N2 H 4+2H2O2→N2+4H2O25g 66g g? 25 gN2 H4

1x

1molN2H 4

32gN 2H4x

1molN 2

1molN 2H 4x

28gN 2

1molN 2=22 gN2

66 gH2O2

1x

1molH2O2

34 gH 2O2x

1molN 2

2molH 2O2x

28 gN 2

1molN 2=27 gN2

N2 H 4 is the LR because it yielded the smallest answer25 gN2 H4

1 x1molN2H 4

32gN 2H4x

2molH2O2

1molN 2H 4x

34 gH2O2

1molH 2O2=53 gH2O2

66 g−53g=13gH 2O2 leftover

4. 22.5 grams of lithium reacts with 33.5 grams of aqueous aluminum sulfate. This is a single replacement reaction.

6 Li+Al2( SO4 )3→3 Li2 SO 4+2 Al22 .5g 33 .5 g? 22 .5 gLi1

x 1molLi7g

x3molLi2 SO4

6molLix

110 gLi2 SO4

1molLi2 SO4=177gLi 2SO4

33 .5 gAl2 (SO4 )3

1x

1molAl2 (SO4 )3

342 gAl2 (SO4)3x

3molLi2 SO4

1molAl2 (SO4 )3x

110 gLi2 SO4

1molLi2 SO4=32gLi2 SO4

Al2 (SO4 )3 is the LR since it yields the smaller value33 .5 gAl2 (SO4 )3

1 x1molAl2 (SO4 )3

342 gAl2 (SO4)3x6molLi

1molAl2 (SO4 )3x7 gLi

1molLi =4 .1 gLi

22g−4 .1 g=18 gLiLeftover

Stoichiometry Worksheet: Percent Yield 1. 15.5-g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.5-g AgCl is produced. NH4NO3 is the

other product. What is the percent yield?

15 .5 gNH 4Cl1

x1molNH 4Cl53 .5 gNH 4Cl

x1molAgCl1molNH 4Cl

x 143 .5 gAgCl1molAgCl

=

41 . 57gAgCl

%=35 .5g41.57 g

x100=85. 3 %

2. Potassium Chlorate decomposes according to the following reaction. 2KClO3 2KCl +3 O2

a. In an experiment 32.5-g of KClO3 is decomposed and 15.2-g of KCl is formed. What is the percent yield?

32 .5 gKClO3

1x

1molKClO 3

122. 5gKClO 3x2molKCl

2molKClO3x 74 .5gKCl

1molKCl=

¿19 .7 gKCl

%=15 .2g19 .7g

x 100=76 .9 %

3. Nitrogen gas reacts with hydrogen gas to make ammonia (NH3). 15.5-L of N2 reacts at STP to make 30-L of ammonia. What is the percent yield?

15 .5 LN 2

1x

2LNH 3

1 LN 2=31 LNH 3

%=30 L31 L

x100=97 %

4 What is the percent yield of oxygen gas if 54L of O2 can be obtained from the thermal decomposition of 500.0 g of potassium chlorate?

KClO3 KCl + O2

2 KClO3→2 KCl+3O2500 . 0g 54L500 gKClO3

1x

1molKClO3

122 .5 gKClO3x

3molO2

2molKClO3x

22. 4 LO 2

1molO 2=137 LO2

%=54 L137 L

x100=39. 4%

Stoichiometry Worksheet: Mixed Problems1. How many grams of water are formed when 12.5-g of hydrogen reacts with oxygen?

12 .5 gH2

1x

1molH 2

2gH 2x

2molH 2O2molH 2

x18gH 2O1molH 2O

=

¿112.5 gH 2O

2. How many liters of carbon dioxide are formed when 12.3-g of sodium carbonate reacts with 2.0-L of hydrogen chloride. The reaction is printed below:

Na2CO3 + HCl NaCl + H2O + CO2

12 .3 gNa2CO 3

1x

1molNa2CO 3

106 Na2CO3x

1molCO2

1molNa2CO3x

22 . 4 LCO2

1molCO2=

¿2 .60 LCO2

2 .0 LHCl1 x

1 LCO2

2 LHCl =1 .0 LCO2

¿1 .0 LCO2 : Answer because it is the lowest

3. How many grams of precipitate are formed when 24.3-g of zinc nitrate reacts with 20.5-g of sodium phosphate?

24 .3gZn(NO3 )2

1x

1molZn(NO 3 )2189gZn(NO3 )2

x1molZn3 (PO 4 )2

3molZn(NO3)2x

385 gZn3(PO 4 )2

1molZn3 (PO4 )2=

¿16 .5 gZn3(PO4 )2 :: This is the answer b/c it is lowest20 .5 gNa3PO 4

1x

1molNa3PO4

164 gNa3PO4x

2molNa3PO4

3molZn(NO 3 )2x

385 gZn3 (PO4 )2

1molZn3(PO4 )2=

¿32 .1gZn3 (PO 4 )2

4. How many liters of oxygen are produced when 3.25-g of KClO3 decomposes into KCl and O2?

3 .25 gKClO3

1x

1molKClO3

122.5 gKClO3x

3 molO2

2molKClO3x

22 .4 LO2

1molO2=

¿0 . 89LO2