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