AP Chemistry Summer Assignment – Brookwood High School



AP Chemistry – Chemistry I Review Assignment

Nomenclature

1. Name these binary compounds of two nonmetals.

IF7 – iodine heptafluoride

N2O5 – dinitrogen pentoxide

XeF2 – xenon difluoride

N2O4 – dinitrogen tetroxide

As4O10 – tetrarsenic decoxide

SF6 – sulfur hexafluoride

PCl3 – phosphorous trichloride

S2Cl2 – disulfur dichloride

2. Name these binary compounds with a fixed charge metal.

AlCl3 – aluminum chloride

MgO – magnesium oxide

BaI2 – barium iodide

KI – potassium iodide

SrBr2 – strontium bromide

Na2S – sodium sulfide

CaF2 – calcium fluoride

Al2O3 – aluminum oxide

3. Name these binary compounds of cations with variable charge.

CuCl2 – copper (II) chloride

Fe2O3 – iron (III) oxide

SnO – tin (II) oxide

PbCl4 – lead (IV) chloride

Cu2S – copper (I) sulfide

HgS – mercury (II) sulfide

AuI3 – gold (III) iodide

CoP – cobalt (III) phosphide

4. Name these compounds with polyatomic ions.

Fe(NO3)3 – iron (III) nitrate

NaOH – sodium hydroxide

Cu2SO4 – copper (I) sulfate

Ca(ClO3)2 – calcium chlorate

KNO2 – potassium nitrite

NaHCO3 – sodium hydrogen carbonate

NH4NO2 – ammonium nitrite

Cu2Cr2O7 – copper (I) dichromate

5. Name these binary acids

HCl(aq) – hydrochloric acid

HI(aq) – hydroiodic acid

6. Name these acids with polyatomic ions.

HClO4 – perchloric acid

H2SO4 – sulfuric acid

HC2H3O2 – acetic acid

H3PO4 – phosphoric acid

HNO2 – nitrous acid

H2CrO4 – chromic acid

H2C2O4 – dichromic acid

H2CO3 – carbonic acid

7. Name these compounds appropriately.

CO – carbon monoxide

NH4CN – ammonium cyanide

HIO3(aq) – iodic acid

NI3 – nitrogen triiodide

AlP – aluminum phosphide

OF2 – oxygen difluoride

LiMnO4 – lithium permanganate

HClO(aq) – hypochlorous acid

HF(aq) – hydrofluoric acid

SO2 – sulfur dioxide

CuCr2O7 – copper(II) dichromate

K2O – potassium oxide

FeF3 – iron(III) fluoride

KC2H3O2 – potassium acetate

MnS – manganese(II) sulfide

8. Write the formulas.

Tin (IV) phosphide – Sn3(PO4)4

Copper (II) cyanide – Cu(CN)2

Magnesium hydroxide – Mg(OH)2

Sodium peroxide – Na2O2

Sulfurous acid – H2SO3

Lithium silicate – Li4SiO4

Potassium nitride – K3N

Chromium (III) carbonate – Cr2(CO3)3

Gallium arsenide - GaAs

Cobalt (II) chromate – CoCrO4

Zinc fluoride – ZnF2

Dichromic acid – H2Cr2O7

Solubility rules

9. Review solubility rules and identify each of the following compounds as soluble or insoluble in water.

Na2CO3 – Sol. CoCO3 – Insol. Pb(NO3)2 – Sol.

K2S – Sol. BaSO4 – Sol. (NH4)2S – Sol.

AgI – Insol. Ni(NO3)2 – Sol. KI – Sol.

FeS – Insol. PbCl2 – Insol. CuSO4 – Sol.

Li2O – Sol. Mn(C2H3O2)2 – Sol. Cr(OH)3 – Insol

AgClO3 – Insol. Sn(SO3)4 – Insol. FeF2 – Insol.

10. Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the precipitate.

silver nitrate and potassium chloride – Yes, AgCl

AgNO3 + KCl ( AgCl + KNO3

magnesium nitrate and sodium carbonate – Yes, MgCO3

Mg(NO3)2 + Na2CO3 ( MgCO3 + 2NaNO3

strontium bromide and potassium sulfate – Yes, SrSO4

SrBr2 + K2SO4 ( 2KBr + SrSO4

cobalt (III) bromide and potassium sulfide – Yes, Co2S3

2CoBr3 + 3K2S ( Co2S3 + 6KBr

ammonium hydroxide and copper (II) acetate – Yes, Cu(OH)2

2NH4OH + Cu(C2H3O2)2 ( Cu(OH)2 + 2NH4C2H3O2

lithium chlorate and chromium (III) fluoride – Yes, Cr(ClO3)3

3LiClO3 + CrF3 ( Cr(ClO3)3 + 3LiF

Balancing Equations

11. Balance the following equations with the lowest whole number coefficients.

S8 + 12O2 ( 8SO3

C10H16 + 8Cl2 ( 10C + 16HCl

4Fe + 3O2 ( 2Fe2O3

2C7H6O2 + 15O2 ( 14CO2 + 6H2O

2KClO3 ( 2KCl + 3O2

2H3AsO4 ( As2O5 + 3H2O

V2O5 + 6HCl ( 2VOCl3 + 3H2O

3Hg(OH)2 + 2H3PO4 ( Hg3(PO4)2 + 6H2O

Stoichiometry and Limiting Factor

12. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide?

Na2O + H2O ( 2NaOH

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13. 2NaClO3 ( 2NaCl + 3O2

What mass of sodium chloride is formed along with 45.0 g of oxygen gas?

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14. 4NH3 + 5O2 ( 4NO + 6 H2O

What mass of water will be produced when 100.0 g of ammonia is reacted with

excess oxygen?

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15. If the reaction in #14 is done with 25.0g of each reactant, which would be the

limiting factor?

[pic]

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Thus, the O2 is the limiting reagent

16. Na2S + 2AgNO3 ( Ag2S + 2NaNO3

If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver

nitrate, which is the limiting factor?

[pic]

[pic]

Thus the AgNO3 is the limiting reagent

What mass of the excess reactant remains?

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Thus, (50.0 – 8.04) = 41.96 g Na2S are left

What mass of silver sulfide would precipitate?

0.103 mole Ag2S would precipitate, thus 25.5 g Ag2S would precipitate

17. 6NaOH + 2Al ( 2Na3AlO3 + 3H2

What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium

hydroxide with 50.0g of aluminum?

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