reaction prediction pre-ap chemistry. reactants products the arrow means yields or produces

REACTION PREDICTION

Pre-APCHEMISTRY

Reactants Products

The arrow means “yields” or “produces”

(s) = solid(g)= gas(l)= liquid(aq)= aqueous (dissolved in water) = reversible reaction = catalyst (in this case, Pt is the catalyst) = heat is added = heat is added

Pt

heat

Practice “translating” a word equation:Solid zinc metal reacts with aqueous copper(II) sulfate to produce solid copper metal and aqueous zinc sulfate.

Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq)

Balancing Equations*Balancing is a trial and error process and is best done in pencil!!*We balance an equation so that the reactants and products each have the same number of atoms of each element (conservation of mass).*We must correctly write the formulas for all reactants and products before we balance.

Coefficients = Numbers placed in front of reactants and products 2H2 + O2 2H2OThis means that 2 moles or molecules of hydrogen gas react with 1 mole or molecule of oxygen gas to produce 2 moles or molecules of water. The coefficients must be in the lowest ratio.

Hints: *Balance elements one at a time.*Balance polyatomic ions that appear on both sides of the equation as single units. (Ex. Count sulfate ions, not sulfur and oxygen separately)*Balance H and O last.

Zn + HCl ZnCl2 + H2

Zn + 2HCl ZnCl2 + H2

Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4

Al2(SO4)3 + 3Ca(OH)2

2Al(OH)3 + 3CaSO4

K + H2O KOH + H2

2K + 2H2O 2KOH + H2

CH4 + O2 CO2 + H2O

CH4 + 2O2 CO2 + 2H2O

Fe + Cl2 FeCl3

2Fe + 3Cl2 2FeCl3

C6H14 + O2 CO2 + H2O

2C6H14 + 19O2 12CO2 + 14 H2O

Al4C3 + H2O CH4 + Al(OH)3

Al4C3 + 12H2O 3CH4 + 4Al(OH)3

Balance the following chemical equations.

1. ___ Ca + ____ H2O ____Ca(OH)2+____H2

Ca + 2 H2O Ca(OH)2 + H2

2. ____Cu2S + _____O2 ____Cu2O + ______SO2

2 Cu2S + 3 O2 2 Cu2O + 2SO23. _____MnO2 + _____HCl ______MnCl2 + ______H2O + _____Cl2

MnO2 + 4 HCl MnCl2 + 2H2O + Cl24. _____NH4NO3 + _____NaOH _____NH3 + _____H2O + _____NaNO3

NH4NO3 + NaOH NH3 + H2O + NaNO3

5. ____Fe(OH)3 _____Fe2O3 + _____H2O

2Fe(OH)3 Fe2O3 + 3H2O6. _____C3H6 + _____O2 _____CO2 + _____H2O

2C3H6 + 9O2 6CO2 + 6H2O7. __Zn(OH)2 + __H3PO4 __Zn3(PO4)2 + ___H2O

3 Zn(OH)2 + 2 H3PO4 Zn3(PO4)2 + 6H2O8. _____CO + _____Fe2O3 _____Fe + _____CO2

3 CO + Fe2O3 2 Fe + 3 CO2

9. _ NH4Cl + __Ca(OH)2 ___NH3 + ___H2O + __CaCl2

2NH4Cl + Ca(OH)2 2 NH3 + 2 H2O + CaCl2

10.___HC2H3O2 + ___NaHCO3 __CO2 + __NaC2H3O2 + __H2O

HC2H3O2 + NaHCO3 CO2 + NaC2H3O2 + H2O

Write a balanced chemical equation for each of the following reactions. Include physical state symbols.1. Copper metal heated with oxygen gives solid copper(II) oxide.

2Cu(s) + O2(g) 2CuO(s)

2. Mixing ammonium nitrate and sodium hydroxide solutions gives aqueous sodium nitrate, ammonia gas, and water.

NH4NO3(aq) + NaOH(aq)

NaNO3(aq) + NH3(g) + H2O(l)

3. Mercury(II) nitrate solution reacts with potassium iodide solution to give a mercury(II) iodide precipitate and potassium nitrate solution.

Hg(NO3)2(aq) + 2KI(aq) HgI2(s) + 2KNO3(aq)

4. Solutions of acetic acid and lithium hydroxide produce water and aqueous lithium acetate.

HC2H3O2(aq) + LiOH(aq) H2O(l) + LiC2H3O2(aq)

5. Heating solid potassium chlorate in the presence of manganese dioxide catalyst produced potassium chloride and oxygen gas.2KClO3(s) MnO2 2KCl(s) + 3O2(g)

DECOMPOSITION REACTIONS-Reaction where a compound breaks down into two or more elements or compounds. Heat, electrolysis, or a catalyst is usually necessary.

A compound may break down to produce two elements.

Ex. Molten sodium chloride is electrolyzed.

2NaCl 2Na + Cl2

A compound may break down to produce an element and a

compound.

Ex. A solution of hydrogen peroxide is decomposed catalytically.

2H2O2 2H2O + O2

A compound may break down to produce two compounds.

Ex. Solid magnesium carbonate is heated. MgCO3 MgO + CO2

Metallic carbonates break down to yield metallic oxides and carbon dioxide.

K2CO3 K2O + CO2

Metallic chlorates break down to yield metallic chlorides and oxygen.

2RbClO3 2RbCl + 3O2

Metallic sulfites break down to yield metallic oxides and sulfur dioxide.

BaSO3 BaO + SO2

Hydrogen peroxide decomposes into water and oxygen.

Sulfurous acid decomposes into water and sulfur dioxide.

Carbonic acid decomposes into water and carbon dioxide.

Hydrated salts decompose into the salt and water

Sodium carbonate monohydrate is heated.

Na2CO3.H2O Δ Na2CO3 + H2O

Complete and balance the following reactions:

1. ZnCO3

ZnCO3 ZnO + CO2

2. KClO3

2KClO3 2KCl + 3O2

3. HgO

2HgO 2Hg + O2

4. H2CO3

H2CO3 H2O + CO2

5. NaCl electricity >

2NaCl electricity > 2Na + Cl2

6. H2SO3

H2SO3 H2O + SO2

7. CaCO3

CaCO3CaO + CO2

8. H2O electricity >

2H2O electricity > 2H2 + O2

9. Na2SO4.10H2O

Na2SO4.10H2O Na2SO4

+10H2O

10. H2O2 MnO2 >

2H2O2 MnO2 >2H2O + O2

11. CuSO4.5H2O

CuSO4.5H2O CuSO4

+ 5H2O

ADDITION REACTIONS-also called synthesis, combination or composition reactions-Two or more elements or compounds combine to form a single product.

-A Group IA or IIA metal may combine with a nonmetal to

make a salt.

Ex. A piece of lithium metal is dropped into a container of nitrogen gas.

6Li + N2 2Li3N

-Two nonmetals may combine to form a molecular compound.

C + O2 CO2

-Two compounds combine to form a single product.

Sulfur dioxide gas is passed over solid calcium oxide.

SO2 + CaO CaSO3

-A metallic oxide plus carbon dioxide yields a metallic carbonate. (Carbon keeps the same oxidation state)

Li2O + CO2 Li2CO3

-A metallic oxide plus sulfur dioxide yields a metallic sulfite. (Sulfur keeps the same oxidation state)

K2O + SO2 K2SO3

-A metallic oxide plus water yields a metallic hydroxide.

CaO + H2O Ca(OH)2

-A nonmetallic oxide plus water yields an acid. CO2 + H2O H2CO3

Complete and balance the following equations:

1. Li + I2

2Li + I2 2LiI

2. Mg + N2

3Mg + N2 Mg3N2

3. SO3 + H2O

SO3 + H2O H2SO4

4. Sr + S

Sr + S SrS

5. Mg + O2

2Mg + O2 2MgO

6. Ag + O2

4Ag + O2 2Ag2O

7. Na2O + H2O

Na2O + H2O 2NaOH

8. SO2 + H2O

SO2 + H2O H2SO3

9. BaO + CO2

BaO + CO2 BaCO3

10. CaO + SO2

CaO + SO2 CaSO3

Double Replacement (metathesis)

• Two compounds react to form two new compounds.

• All double replacement reactions must have a "driving force" that removes a pair of ions from solution.

• Ions keep their same charges as reactants and products.

Formation of a precipitate: A precipitate is an insoluble substance formed by the reaction of two aqueous substances.

Two ions bond together so strongly that water can not pull them apart.

SOLUBILITY OF SOME IONIC COMPOUNDS IN WATERNegative Ion Plus Positive Ion Form a CompoundWhich IsAny negative ion + Group I ions SolubleAny negative ion + NH4

+ SolubleNO3- + Any positive ion SolubleC2H3O2

- + Any positive ion SolubleCl-,Br-,I- + Ag+, Pb2+, Hg2

2+ Insoluble + Any other positive ion SolubleSO4

2- + Ca2+,Sr2+,Ba2+, Ag+,Pb2+ Insoluble + Any other positive ion SolubleS2- + Group I,II or NH4

+ ions Soluble + Any other positive ion InsolubleOH- + Group I , NH4

+ions Soluble + Ca2+, Sr2+, Ba2+ Soluble + Any other positive ion InsolublePO4

3-, CO32-, SO3

2- + Group I or NH4+ Soluble

+ Any other positive ion Insoluble

SOLUBILITY SONGTo the tune of “ My Favorite Things” from “The Sound of Music”

Nitrates and Group One and Ammonium,These are all soluble, a rule of thumb.Then you have chlorides, they’re soluble fun,All except Silver, Lead, Mercury I.Then you have sulfates, except for these three:Barium, Calcium and Lead, you see.Worry not only few left to go still.We will do fine on this test. Yes, we will!Then you have the---InsolublesHydroxide,Sulfide and Carbonate and Phosphate,And all of these can be dried!

Ex. Solutions of silver nitrate and lithium bromide are mixed.

AgNO3(aq) + LiBr(aq) AgBr(s) + LiNO3(aq)

Formation of a gas:

Gases may form directly in a double replacement reaction or can form from the decomposition of a product such as H2CO3 or H2SO3.

(Don't leave carbonic or sulfurous acids, or ammonium hydroxide as products of double replacement reactions,

decompose them!)

Ex. Excess hydrochloric acid solution is added to a solution of potassium sulfite.

2HCl(aq) + K2SO3(aq)

2KCl(aq) + H2O(l) + SO2(g)

Ex. A solution of sodium hydroxide is added to a solution

of ammonium chloride.

NaOH(aq)+ NH4Cl(aq)

NH3(g) + H2O(l) + NaCl(aq)

Formation of a molecular substance:

When a molecular substance such as water or acetic acid is formed, ions are removed from solution and the reaction "works".

Ex. Dilute solutions of lithium hydroxide and hydrobromic acid are mixed.

LiOH(aq) + HBr(aq) LiBr(aq) + H2O

Complete and balance the following equations:

1. NaOH + CuSO4

2NaOH + CuSO4

Na2SO4 + Cu(OH)2(s)

2. NH4I + AgNO3

NH4I + AgNO3

NH4NO3 + AgI(s)

3. K2CO3 + Ba(OH)2

K2CO3 + Ba(OH)2

2KOH + BaCO3(s)

4. KOH + HI

KOH + HIKI + H2O(l)

5. K2CO3 + HNO3

K2CO3 + 2HNO3

2KNO3 + H2O + CO2

6. (NH4)2SO4 + BaCl2

(NH4)2SO4 + BaCl2

2NH4Cl + BaSO4(s)

7. Na2S + NiSO4

Na2S + NiSO4

NiS(s) + Na2SO4

8. Pb(NO3)2 + KBr

Pb(NO3)2 + 2KBr

PbBr2(s) + 2KNO3

9. Fe2(SO4)3 + Ba(OH)2

Fe2(SO4)3 + 3Ba(OH)2

2Fe(OH)3(s) + 3BaSO4(s)

10. Hg2(NO3)2 + KI

Hg2(NO3)2 + 2KI

2KNO3 + Hg2I2(s)

Single Replacement

Reaction where one element displaces another in a compound.

One element is oxidized and another is reduced. A + BC B + AC

Active metals replace less active metals or hydrogen from their compounds in aqueous solution.

Use an activity series to determine the activity of metal.

ACTIVITY SERIES OF METALS

ElementLithiumPotassiumBarium

Decreasing CalciumActivity Sodium

MagnesiumAluminumZincIronCadmiumNickelTinLeadHydrogen ( a nonmetal)CopperMercurySilverGoldPlatinum

*Metals from Li to Na will replace H from water andacids; metals from Mg to Pb will replace H fromacids only.

Ex. Magnesium turnings are added to a solution of iron(III) chloride.

3Mg(s) + 2FeCl3(aq) 2Fe(s) + 3MgCl2(aq)

Ex. Sodium is added to water.

2Na(s) + 2H2O(l)

2NaOH(aq) + H2(g)

Reactions of Alkali metals

Ex. Fe + H2O

Fe + H2O no reaction

Active nonmetals replace less active nonmetals from their compounds in aqueous solution. Each halogen will displace heavier halogens from their binary salts.

Activity Series of Nonmetals

Most Active F2

Cl2

Br2

Least Active I2

Ex. Chlorine gas is bubbled into a solution of potassium iodide.

Cl2(g) + 2KI(aq)

I2(s) + 2KCl(aq)

Ex. I2 + KCl

I2 + KCl no reaction

Complete and balance the following equations:

1. Zn + HCl

Zn +2 HCl ZnCl2 + H2

2. Br2 + NaCl

Br2 + NaCl No Reaction

3. F2 + NaBr

F2 + 2NaBr 2NaF + Br2

4. Al + CuSO4

2Al + 3CuSO4

Al2(SO4)3 + 3Cu

5. Cu + AgNO3

Cu + 2AgNO3

Cu(NO3)2 + 2Ag

6. Cd + CuSO4

Cd + CuSO4

CdSO4 + Cu

7. K + H2O

2K + 2H2O

2KOH + H2

8. Mg + H2SO4

Mg + H2SO4

MgSO4 + H2

9. Ag + HCl

Ag + HCl No Rxn

10. I2 + KCl

I2 + KCl No Rxn

11. Ca + H2O

Ca + 2H2O Ca(OH)2 + H2

12. Zn + H2O

Zn + H2O No Rxn

COMBUSTION REACTIONS

In the presence of excess oxygen, most hydrocarbons and alcohols can undergo complete combustion reactions to form carbon dioxide and water. The only tricky part is balancing the reaction. Balance the C first, H second, and O third.

Ex. Ethane (C2H6) burns in air.

2C2H6 + 7O2 4CO2 + 6H2O

Ethanol (C2H5OH) burns

C2H5OH + 3O2 2CO2 + 3H2O

Complete and balance the reactions for the combustion of

the following compounds:

1. CH4

CH4 + 2O2 CO2 + 2H2O

2. C2H2

2C2H2 + 5 O2 4CO2 + 2H2O

3. CH3OH

2CH3OH + 3O2 2CO2 + 4H2O

4. C6H12O6

C6H12O6 + 6O2 6CO2 + 6H2O

5. C8H18

2C8H18 + 25O2 16CO2 + 18H2O

6. C3H8

C3H8 + 5O2 3CO2 + 4H2O

7. C6H6

2C6H6 + 15O2 12CO2 + 6H2O

8. C2H4

C2H4 + 3O2 2CO2 + 2H2O

9. C35H72

C35H72 + 53O2 35CO2 +36 H2O

10. C3H7OH

2C3H7OH + 9O2 6CO2 + 8H2O

SYNTHESIS AND DECOMPOSITION

REACTIONS

Complete and balance the following equations:

1. Sr + O2

2Sr + O2 2SrO

2. Na + O2

4Na + O2 2Na2O

3. K + Cl2

2K + Cl2 2KCl

4. Ca + F2

Ca + F2 CaF2

5. sodium + iodine

2Na + I2 2NaI

6. magnesium + oxygen

2Mg + O2 2MgO

7. hydrogen + chlorine

H2 + Cl2 2HCl

8. silver + sulfur

2Ag + S Ag2S

9. calcium oxide + water

CaO + H2O Ca(OH)2

10. sulfur trioxide + water

SO3 + H2O H2SO4

11. MgBr2

MgBr2 Mg + Br2

12. AlCl3

2AlCl3 2Al + 3Cl2

13. H2O

2H2O 2H2 + O2

14. KI

2KI 2K + I2

15. NaCl

2NaCl 2Na + Cl2

16. nickel(II) chlorate

Ni(ClO3)2 NiCl2 + 3O2

SINGLE AND DOUBLE REPLACEMENT REACTIONS

Write and balance the following reactions:

1. Zn(s) + CuSO4(aq)

Zn(s) + CuSO4(aq) ZnSO4(aq) + Cu(s)

2. Cl2(g) + KI(aq)

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

3. Ni(s) + MgSO4(aq)

Ni(s) + MgSO4(aq) No Reaction

4. Br2(l) + CaCl2(aq)

Br2(l) + CaCl2(aq) No Rxn

5. zinc + copper(II) nitrate

Zn(s) + Cu(NO3)2(aq) Cu(s) + Zn(NO3)2(aq)

6. calcium + hydrochloric acid

Ca(s) + 2HCl(aq) CaCl2(aq) + H2(g)

7. copper(II) nitrate + silver

Cu(NO3)2(aq) + Ag(s) No Rxn

8. sodium iodide + bromine

2NaI(aq) + Br2(l) 2NaBr(aq) + I2(s)

9. sodium + water

2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)

10. FeCl2 + K2S

FeCl2(aq) + K2S(aq)

FeS(s) + 2KCl(aq)

11. ZnCl2 + Pb(NO3)2

ZnCl2(aq) + Pb(NO3)2(aq)

Zn(NO3)2(aq) + PbCl2(s)

12. CaCl2 + Na2CO3

CaCl2(aq) + Na2CO3(aq) 2NaCl(aq) + CaCO3(s)

13. (NH4)2SO4 + BaCl2

(NH4)2SO4(aq) + BaCl2(aq) 2NH4Cl(aq) + BaSO4(s)

14. sodium hydroxide + acetic acid

NaOH(aq) + HC2H3O2(aq) NaC2H3O2(aq) + H2O(l)

15. copper(II) sulfate + ammonium sulfide

CuSO4(aq) + (NH4)2S(aq) CuS(s) + (NH4)2SO4(aq)

MIXED EQUATION WORKSHEET #1Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.

1. Magnesium hydroxide + nitric acid

magnesium hydroxide + nitric acid magnesium nitrate + waterMg(OH)2 + 2HNO3 Mg(NO3)2 + 2H2O

DR

2. Complete combustion of methane (CH4)

methane + oxygen

carbon dioxide + water

CH4 + 2O2 CO2 + 2H2O

Combustion

3. Chlorine + sodium bromide

chlorine + sodium bromide bromine + sodium chloride

Cl2 + 2NaBr Br2 + 2NaCl

Single Replacement

4. Aluminum + sulfuric acid

aluminum + sulfuric acid aluminum sulfate + hydrogen

2Al + 3H2SO4 Al2(SO4)3 + 3H2

Single replacement

5. Sulfuric acid + sodium acetate

Sulfuric acid + sodium acetate sodium sulfate + acetic acid

H2SO4 + 2NaC2H3O2

Na2SO4 + 2HC2H3O2

Double replacement

6. Heating calcium carbonate

calcium carbonate calcium oxide + carbon dioxide

CaCO3 CaO + CO2

Decomposition

7. Heating mercuric oxide

mercuric oxide mercury + oxygen

2HgO 2Hg + O2

Decomposition

8. Zinc + silver nitrate

Zinc + silver nitrate

zinc nitrate + silver

Zn + 2AgNO3 Zn(NO3)2 + 2Ag

Single Replacement

9. Burning sulfur

Sulfur + oxygen

sulfur dioxide

S + O2 SO2

synthesis

10. Heating sodium chlorate

sodium chlorate

sodium chloride + oxygen

2NaClO3 2NaCl + 3O2

Decomposition

11. Zinc chloride + ammonium sulfide

Zinc chloride + ammonium sulfide

zinc sulfide + ammonium chloride

ZnCl2 + (NH4)2S ZnS + 2NH4Cl

double replacement

12. Aluminum hydroxide + hydrochloric acid

Aluminum hydroxide + hydrochloric acid aluminum chloride + water

Al(OH)3 + 3HCl AlCl3 + 3H2O

Double replacement

13. Calcium + steam

Calcium + steam

calcium hydroxide + hydrogen

Ca + 2H2O Ca(OH)2 + H2

Single replacement

14. Heating carbonic acid

carbonic acid

water + carbon dioxide

H2CO3 H2O + CO2

Decomposition

15. Electrolysis of sodium chloride

Sodium chloride

sodium + chlorine

2NaCl 2Na + Cl2

Decomposition

16. Combustion of propane (C3H8)

Propane + oxygen Carbon dioxide + water

C3H8 + 5O2 3CO2 +4 H2O

Combustion

17. Bromine + potassium iodide

Bromine + potassium iodide

Iodine + potassium bromide

Br2 + 2KI I2 + 2KBr

Single Replacement

18. Magnesium + hydrochloric acid

Magnesium + hydrochloric acid

magnesium chloride + hydrogen

Mg + 2HCl MgCl2 + H2

Single replacement

19. Sodium hydroxide + acetic acid

Sodium hydroxide + acetic acid

sodium acetate + water

NaOH + HC2H3O2 NaC2H3O2 + H2O

Double replacement

20. Burning hydrogen

hydrogen + oxygen water

2H2 + O2 2H2O

Synthesis or combustion

21. Zinc + sulfuric acid

Zinc + sulfuric acid zinc sulfate + hydrogen

Zn + H2SO4 ZnSO4 + H2

single replacement

22. Heating magnesium carbonate

magnesium carbonate magnesium oxide + carbon dioxide

MgCO3 MgO + CO2

Decomposition

23. Sodium + chlorine

Sodium + chlorine sodium chloride

2Na + Cl2 2NaCl

Synthesis

24. Lead(II) nitrate + sodium iodide

Lead(II) nitrate + sodium iodide

lead (II) iodide + sodium nitrate

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

Double replacement

25. Silver nitrate + sodium sulfide

Silver nitrate + sodium sulfide silver sulfide + sodium nitrate

2AgNO3 + Na2S Ag2S + 2NaNO3

Double replacement

26. Iodine + potassium chloride

Iodine + potassium chloride No Reaction

27. Magnesium oxide + water

Magnesium oxide + water magnesium hydroxide

MgO + H2O Mg(OH)2

synthesis

MIXED EQUATION WORKSHEET #2

Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.

1. sodium hydrogen carbonate + hydrochloric acid

sodium hydrogen carbonate + hydrochloric acid sodium chloride + water + carbon dioxide

NaHCO3 + HCl NaCl + H2O + CO2

double replacement

2. Complete combustion of ethanol (C2H5OH)

Ethanol + oxygen

carbon dioxide + water

C2H5OH + 3O2 2CO2 + 3H2O

Combustion

3. sulfurous acid + magnesium hydroxide

sulfurous acid + magnesium hydroxide

water + magnesium sulfite

H2SO3 + Mg(OH)2 2H2O + MgSO3

double replacement

4. carbonic acid + lithium hydroxide

carbonic acid + lithium hydroxide

water + lithium carbonate

H2CO3 + 2LiOH 2H2O + Li2CO3

Double replacement

5. gold + sulfuric acid

gold + sulfuric acid No Reaction

6. aluminum + fluorine

aluminum + fluorine aluminum fluoride

2Al + 3F2 2AlF3

Synthesis

7. calcium oxide + water

calcium oxide + water

calcium hydroxide

CaO + H2O Ca(OH)2

Synthesis

8. acetic acid + sodium hydroxide

acetic acid + sodium hydroxide water + sodium acetate

HC2H3O2 + NaOH H2O +NaC2H3O2

Double replacement

9. potassium chloride + lead(II) nitrate

potassium chloride + lead(II) nitrate

potassium nitrate + lead(II) chloride

2KCl + Pb(NO3)2 2KNO3 + PbCl2

Double replacement

10. carbon monoxide + oxygen

carbon monoxide + oxygen

carbon dioxide

2CO + O2 2CO2

Synthesis

11. sodium + chlorine

sodium + chlorine sodium chloride

2Na + Cl2 2NaCl

Synthesis

12. dinitrogen pentoxide + water

dinitrogen pentoxide + water

nitric acid

N2O5 + H2O H2N2O6 2HNO3

Synthesis

13. bromine + sodium chloride

bromine + sodium chloride No rxn

14. potassium chloride + mercury(I) nitrate

potassium chloride + mercury(I) nitratepotassium nitrate + mercury(I) chloride

2KCl + Hg2(NO3)2 2KNO3 + Hg2Cl2

Double replacement

15. sulfur dioxide + water

sulfur dioxide + water sulfurous acid

SO2 + H2O H2SO3

Synthesis

16. lithium oxide + water

lithium oxide + water

lithium hydroxide

Li2O + H2O 2LiOH

Synthesis

17. heating zinc carbonate

zinc carbonate

zinc oxide + carbon dioxide

ZnCO3 ZnO + CO2

Decomposition

18. silver nitrate + sodium chloride

silver nitrate + sodium chloride

silver chloride + sodium nitrate

AgNO3 + NaCl AgCl + NaNO3

Double replacement

19. heating beryllium chlorate

beryllium chlorate

beryllium chloride + oxygen

Be(ClO3)2 BeCl2 + 3O2

Decomposition

20. electrolysis of water

water hydrogen + oxygen

2H2O 2H2 + O2

Decomposition

21. complete combustion of butane (C4H10)

Butane + oxygen

carbon dioxide + water

2C4H10 + 13O2 8CO2 + 10H2O

Combustion

22. iron(II) sulfate + ammonium sulfide

iron(II) sulfate + ammonium sulfide iron(II) sulfide + ammonium sulfate

FeSO4 + (NH4)2S FeS + (NH4)2SO4

Double replacement

23. lithium + water

lithium + waterlithium hydroxide + hydrogen

2Li + 2H2O 2LiOH + H2

Single replacement

24. potassium oxide + water

potassium oxide + water

potassium hydroxide

K2O + H2O 2KOH

Synthesis

25. silver + sulfur

silver + sulfur silver sulfide

2Ag + S Ag2S

Synthesis

26. sodium + water

sodium + water

sodium hydroxide + hydrogen

2Na + 2H2O 2NaOH + H2

Single replacement

27. calcium hydroxide + ammonium sulfatecalcium hydroxide + ammonium sulfatecalcium sulfate + ammonia + water

Ca(OH)2 + (NH4)2SO4

CaSO4 + 2NH3 + 2H2O

Double replacement

NET IONIC EQUATIONS

Net ionic equations show only the species actually involved in the reaction. As you first learn to write net ionic equations, you will write three different equations for each reaction.

Steps in writing net ionic equations:

1. Write the complete molecular equation. (This is the type of equation that you are accustomed to writing.)

2. Write the complete ionic equation. To do this, you must ionize everything that is soluble and ionized in solution. Everything else is left together. Do not ionize solids, gases or weak electrolytes.

3. Write the net ionic equation. To do this, cancel out all ions that are not participating in the reaction (spectator ions) and rewrite the equation.

Sodium chloride + silver nitrate

1. NaCl(aq) + AgNO3(aq)

NaNO3(aq) + AgCl(s)

2. Na+ + Cl- + Ag+ + NO3-

Na+ + NO3- + AgCl(s)

2. Na+ + Cl- + Ag+ + NO3-

Na+ + NO3- + AgCl(s)

3. Cl- + Ag+ AgCl

1. 2HCl + Ba(OH)2 2H2O + BaCl2 2. 2H+ + 2Cl- + Ba2+ + 2OH- 2H2O + Ba2+ + 2Cl-

2. 2H+ + 2Cl- + Ba2+ + 2OH- 2H2O + Ba2+ + 2Cl-

3. 2H+ + 2OH- 2H2O H+ + OH- H2O

Ex. HCl + Ba(OH)2

Write net ionic equations for the following reactions:

1. KCl(aq) + Pb(NO3)2(aq)

2KCl(aq) + Pb(NO3)2(aq)

2KNO3(aq) + PbCl2(s)

2K+ + 2Cl- + Pb2+ + 2NO3-

2K+ + 2NO3- + PbCl2

Pb2+ + 2Cl- PbCl2

2. HCl(aq) + CaSO3(s)

2HCl(aq) + CaSO3(s)

H2O(l) + SO2(g) + CaCl2(aq)

2H+ + 2Cl- + CaSO3

H2O + SO2 + Ca2+ + 2Cl-

2H+ + CaSO3 H2O + SO2 + Ca2+

3. Zn(s) + O2(g)

2Zn(s) + O2(g) 2ZnO(s)

4. Li(s) + H2O(l)

2Li(s) + 2H2O(l)

2LiOH(aq) + H2(g)

2Li(s) + 2H2O(l)

2Li+ +2OH-(aq) + H2(g)

5. Na2SO4(aq) + BaBr2(aq)Na2SO4(aq) + BaBr2(aq)

2NaBr(aq) + BaSO4(s)

2Na+ + SO42- + Ba2+ + 2Br-

2Na+ + 2Br- + BaSO4

SO42- + Ba2+ BaSO4

6. MgCO3(s)

MgCO3(s) MgO(s) + CO2(g)

7. AgNO3(aq) + Na2CO3(aq)

2AgNO3(aq) + Na2CO3(aq)

Ag2CO3(s) + 2NaNO3(aq)

2Ag+ + 2NO3- + 2Na+ + CO3

2-

Ag2CO3 + 2Na+ + 2NO3-

2Ag+ + CO32- Ag2CO3

8. Na2S(aq) + HCl(aq) Na2S(aq) + 2HCl(aq)

2NaCl(aq) + H2S(g)

2Na+ + S2- + 2H+ + 2Cl-

2Na+ + 2Cl- + H2S

S2- + 2H+ H2S

9. H2SO3(aq)

H2SO3(aq) H2O(l) + SO2(g)

10. Cl2(g) + NaI(aq)

Cl2(g) + 2NaI(aq) I2(s) + 2NaCl(aq)

Cl2 + 2Na+ + 2I- I2 + 2Na+ + 2Cl-

Cl2 + 2I- I2 + 2Cl-

EXTRA EQUATION WORKSHEET

PRE-AP CHEMISTRY

Complete the word equation, write the formula equation, balance it and identify the type of reaction. You many abbreviate as S, D, SR, DR, and C.

1. heating magnesium carbonate

magnesium carbonate

magnesium oxide + carbon dioxide

MgCO3 MgO + CO2

Decomposition

2. complete combustion of propanol (C3H7OH)

propanol + oxygen

carbon dioxide + water

2C3H7OH + 9O2 6CO2 + 8H2O

Combustion

3. sulfur + oxygen

sulfur + oxygen sulfur dioxide

S + O2 SO2

Synthesis

4. sulfuric acid + cadmium

sulfuric acid + cadmium cadmium sulfate + hydrogen

H2SO4 + Cd CdSO4 + H2

Single Replacement

5. sulfur dioxide + water

sulfur dioxide + water

sulfurous acid

SO2 + H2O H2SO3

Synthesis

6. hydrochloric acid(aq) + calcium carbonate(s)

hydrochloric acid(aq) + calcium carbonate(s) carbon dioxide(g) + water(l) + calcium chloride(aq)

2HCl + CaCO3 CO2 + H2O + CaCl2

Double replacement

7. net ionic equation for #6

1. 2HCl(aq) + CaCO3(s)

CO2(g) + H2O(l) + CaCl2(aq)

2. 2H+ + 2Cl- + CaCO3

CO2 + H2O + Ca2+ + 2Cl-

3. 2H+ + CaCO3

CO2 + H2O + Ca2+

8. silver nitrate (aq)+ hydrochloric acid (aq)

silver nitrate (aq)+ hydrochloric acid (aq)

silver chloride(s) + nitric acid(aq)

AgNO3 + HCl AgCl + HNO3

Double replacement

9. net ionic equation for #8

1. AgNO3(aq) + HCl(aq)

AgCl(s) + HNO3(aq)

2. Ag+ + NO3- + H+ + Cl-

AgCl(s) + H+ + NO3-

3. Ag+ + Cl- AgCl(s)

10. barium nitrate(aq) + potassium sulfate (aq)

barium nitrate(aq) + potassium sulfate (aq)barium sulfate(s) + potassium nitrate(aq)

Ba(NO3)2 + K2SO4 BaSO4 + 2KNO3

Double Replacement

11. net ionic equation for #10

1. Ba(NO3)2 (aq) + K2SO4(aq) BaSO4(s) + 2KNO3(aq)

2. Ba2+ + 2NO3

- + 2K+

+ SO42-

BaSO4 + 2K+ + 2NO3-

3. Ba2+ + SO4

2- BaSO4

12. sodium hydroxide + phosphoric acid

sodium hydroxide + phosphoric acid sodium phosphate + water

3NaOH + H3PO4 Na3PO4 + 3H2O

Double replacement

13. iodine + rubidium chloride

iodine + rubidium chloride No Rxn

14. magnesium(s) + copper(II) sulfate(aq)

magnesium(s) + copper(II) sulfate(aq)magnesium sulfate(aq) + copper(s)

Mg + CuSO4 MgSO4 + Cu

Single replacement

15. net ionic equation for #14

1. Mg(s) + CuSO4(aq) MgSO4(aq) + Cu(s)

2. Mg + Cu2+ + SO42-

Mg2+ +SO42- + Cu

3. Mg + Cu2+ Mg2+ + Cu

16. ammonium nitrate(aq) + sodium hydroxide(aq)

ammonium nitrate(aq) + sodium hydroxide(aq) ammonia (g)+ water (l) + sodium nitrate (aq)

NH4NO3 + NaOH

NH3 + H2O + NaNO3

Double replacement

17. net ionic equation for #16

1. NH4NO3(aq) + NaOH(aq)

NH3(g) + H2O(l) + NaNO3(aq)

2. NH4+

+ NO3- + Na+ + OH-

NH3 + H2O + Na+ + NO3-

3. NH4+

+ OH- NH3 + H2O

18. potassium(s) + water(l)

potassium(s) + water(l) potassium hydroxide(aq) + hydrogen(g)

2K + 2H2O 2KOH + H2

Single Replacement

19. net ionic equation for #18

1. 2K(s) + 2H2O(l)

2KOH(aq) + H2(g)

2. 2K + 2H2O 2K+ + 2OH- + H2

20. sodium bromide(aq) + chlorine(g)

sodium bromide(aq) + chlorine(g)sodium chloride + bromine

2NaBr + Cl2 2NaCl + Br2

Single replacement

21. net ionic equation for #20

1. 2NaBr(aq) + Cl2(g) 2NaCl(aq) + Br2(l)

2. 2Na+ + 2Br- + Cl2 2Na+ + 2Cl- + Br2

3. 2Br- + Cl2 2Cl- + Br2

22. aluminum + nitrogen

aluminum + nitrogenaluminum nitride

2Al + N2 2AlN

Synthesis

23. sodium sulfide(aq) + hydrochloric acid(aq)

sodium sulfide(aq) + hydrochloric acid(aq) sodium chloride (aq) + hydrogen sulfide (g)

Na2S + 2HCl 2NaCl + H2S

Double replacement

24. net ionic equation for #23

1. Na2S(aq) + 2HCl(aq) 2NaCl(aq) + H2S(g)

2. 2Na+ + S2-+ 2H+ + 2Cl-

2Na+ + 2Cl-+ H2S

3. S2-+ 2H+ H2S

25. heating magnesium sulfate heptahydrate

magnesium sulfate heptahydrate magnesium sulfate + water

MgSO4.7H2O MgSO4 + 7H2O

Decomposition

26. heating mercury(II) oxide

mercury(II) oxide mercury + oxygen

2HgO 2Hg + O2

Decomposition

27. bromine + strontium chloride

bromine + strontium chloride No Rxn

1. Dilute hydrochloric acid is added to a solution of potassium sulfite.

2HCl(aq) +K2SO3(aq) H2O(l) + SO2(g) +2KCl(aq)

2H+ + 2Cl- +2K+ + SO3

2-

H2O(l) + SO2(g) +2K+ +2Cl-

2H+ + SO32- H2O(l) + SO2(g)

2. A solution of sodium sulfide is added to a solution of zinc nitrate.

Na2S(aq) + Zn(NO3)2(aq) 2NaNO3(aq) + ZnS(s)

2Na+ + S2- + Zn2+ + 2NO3

- 2Na+ + 2NO3- + ZnS

S2- + Zn2+ ZnS

3. Chlorine gas is bubbled into a solution of potassium iodide.

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

Cl2 + 2K+ + 2I- 2K+ + 2Cl- + I2

Cl2 + 2I- -> 2Cl- + I2

4. Magnesium metal is burned in nitrogen gas.

3Mg(s) + N2(g) Mg3N2(s)

5. Solid sodium oxide is added to water.Na2O(s) + H2O(l) 2NaOH(aq)

Na2O(s) + H2O(l) 2Na+(aq) + 2OH-(aq)