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REACTION
PREDICTION
Pre-AP
CHEMISTRY
Reactants  Products
The arrow means “yields” or
“produces”
(s) = solid
(g)= gas
(l)= liquid
(aq)= aqueous (dissolved in water)
 = reversible reaction
Pt
 = catalyst (in this case, Pt is the catalyst)
 = heat is added

heat
 = heat is added
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  2H2O
This 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 + 2SO2
3. _____MnO2 + _____HCl  ______MnCl2 + ______H2O + _____Cl2
MnO2 + 4 HCl  MnCl2 + 2H2O + Cl2
4. _____NH4NO3 + _____NaOH  _____NH3 + _____H2O + _____NaNO3
NH4NO3 + NaOH  NH3 + H2O + NaNO3
5. ____Fe(OH)3  _____Fe2O3 + _____H2O
2Fe(OH)3  Fe2O3 + 3H2O
6. _____C3H6 + _____O2  _____CO2 + _____H2O
2C3H6 + 9O2  6CO2 + 6H2O
7. __Zn(OH)2 + __H3PO4  __Zn3(PO4)2 + ___H2O
3 Zn(OH)2 + 2 H3PO4  Zn3(PO4)2 + 6H2O
8. _____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
CaCO3CaO + CO2
8. H2O electricity >
2H2O electricity > 2H2 + O2
9. Na2SO4.10H2O 
Na2SO4
.10H
2O
 Na2SO4 +10H2O
10. H2O2
2H2O2
MnO2
MnO2
>
>2H2O + O2
11. CuSO4.5H2O 
CuSO4
.5H
2O
 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 WATER
Negative Ion
Plus
Positive Ion Form a Compound
Which Is
Any negative ion
+
Group I ions
Soluble
+
Any negative ion
+
NH4
Soluble
NO3+
Any positive ion
Soluble
C2H3O2
+
Any positive ion
Soluble
- +
2+
2+
Cl ,Br ,I
+
Ag , Pb , Hg2
Insoluble
+
Any other positive ion
Soluble
22+
2+
2+
+
2+
SO4
+
Ca ,Sr ,Ba , Ag ,Pb
Insoluble
+
Any other positive ion
Soluble
2+
S
+
Group I,II or NH4 ions
Soluble
+
Any other positive ion
Insoluble
OH+
Group I , NH4+ions
Soluble
+
Ca2+, Sr2+, Ba2+
Soluble
+
Any other positive ion
Insoluble
PO43-, CO32-, SO32- +
Group I or NH4+
Soluble
+
Any other positive ion
Insoluble
SOLUBILITY SONG
To 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--Insolubles
Hydroxide,
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 + HIKI + 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
Element
Lithium
Potassium
Barium
Decreasing
Calcium
Activity
Sodium
Magnesium
Aluminum
Zinc
Iron
Cadmium
Nickel
Tin
Lead
Hydrogen ( a nonmetal)
Copper
Mercury
Silver
Gold
Platinum
*Metals from Li to Na will replace H from water and
acids; metals from Mg to Pb will replace H from
acids 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
Least Active
F2
Cl2
Br2
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 #1
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. Magnesium hydroxide + nitric acid 
magnesium hydroxide + nitric acid 
magnesium nitrate + water
Mg(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) nitrate
potassium 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 + water
lithium 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 sulfate
calcium hydroxide + ammonium sulfate
calcium 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
Ex. HCl + Ba(OH)2 
1. 2HCl + Ba(OH)2  2H2O + BaCl2
2. 2H+ + 2Cl- + Ba2+ + 2OH- 
2H2O + Ba2+ + 2Cl2. 2H+ + 2Cl- + Ba2+ + 2OH- 
2H2O + Ba2+ + 2Cl3. 2H+ + 2OH-  2H2O
H+ + OH-  H2O
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+ + 2Cl2H+ + 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+ + CO32- 
Ag2CO3 + 2Na+ + 2NO32Ag+ + 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 +
Cl2 + 2I- I2 + 2Cl-
+
2Na
+
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-
+ CaCO3 
2+
CO2 + H2O + Ca
+
3. 2H
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+ + 2NO33. Ba2+ + SO42-
 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+ + NO33. 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 + nitrogen
aluminum 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+
2. 2Na + S + 2H + 2Cl 
2Na+ + 2Cl-+ H2S
23. S +
+
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+ + SO32-
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)