Your Name____________________
Day: ________
Your Score_________CHM151 C4 Reactions in Aqueous Solutions Packet
A. Combination Rxn
A

+
B
1. two elements

a binary compound
2. metallic oxide + water

a base

3. nonmetallic oxide + water
B. Combustion Rxn
A
Date:_____________
Possible:___20___
AB
an acid
+ Oxygen 
Carbon Dioxide + Water
1. Any hydrocarbon + Oxygen

carbon dioxide + water
C. Decomposition Rxn AB

A
1. binary compound

two elements
2. base

metallic oxide + water
3. acid

nonmetallic oxide + water
4. metallic carbonate

metallic oxide + carbon dioxide
5. metallic chlorate

metallic chloride + oxygen gas
6. hydrated salt

salt + water
D. Single Replacement Rxn
A
+
+

+
AX
1. active metal (or H2) + ionic compound
 less active metal (or H2)
+
ionic compound
2. active halogen

+
ionic halide
+ ionic halide
BX
B
less active halogen
E. Double Replacement Rxn or Metathesis Rxn
AX +
BY 
AY
1. two soluble ionic compounds

Neutralization Rxn
(H)X +
B
+
BX
two new ionic compounds, 1 must be insoluble
B(OH) (H)(OH) +
BX
2. Any Acid
+ Any Base

Water
+
Salt
3. Metallic Oxide
+ Any Acid

Water
+
Salt
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Gas Formation Rxn
4. Any Acid
+ Metallic Cyanide
5. Any Base + Ammonium compound
 Soluble ionic compound + HCN (g)
 Soluble ionic compound + NH4OH (decomposes)
↓
NH3(g) + Water
F. Oxidation Reduction Rnx or Electron Transfer Rxn
Combination, Decomposition, Combustion, Single Replacement(Metal & Halogens)
1. Nonaqueous Rxns (Product(s) are ionic compounds)
2. Nonaqueous Rxns (Product(s) are molecular compounds)
Oxidation Number is the number of charges an atom would have in a molecule if electrons were
transferred completely in the direction indicated by the difference in electronegativity
1. A free atom has an oxidation number of zero. It is not sharing, gaining, or losing
electrons.
2. Polyatomic elements have an oxidation number of zero for each atom. Elements such
as H2, O2, and P4 share electrons equally among all atoms in the molecule.
3. The sum of the oxidation numbers in a neutral molecule is zero.
4. A monoatomic ion has an oxidation number equal to its charge. For example, the
oxidation number of the oxygen in the oxide ion, O2–, is –2.
5. The sum of the oxidation numbers in a polyatomic ion is equal to the charge on the ion.
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Activity Series for
Metals Rules
Solubility Rules
1. Cd through Li will
replace H in acids and
water.
2. Pb through Co will
replace H in acids.
3. Au through Cu will NOT
replace H anywhere!
4. Higher metal will
replace the lower metal.
Negative Ions
(Anions)
+
any anion
+
H-
any anion
Activity Series for
Nonmetals Rules
NO3ClO3-
1. Fluorine replaces
everything below it.
2. Higher halogen will
replace the lower halogen.
Activity
Series
Metals
Halogens
Lithium
Rubidium
Potassium
Barium
Strontium
Calcium
Sodium
Magnesium
Aluminum
Manganese
Zinc
Chromium
Iron
Cadmium
Cobalt
Nickel
Tin
Lead
Hydrogen
Copper
Mercury
Silver
Gold
Fluorine
Chlorine
Bromine
Iodine
=
Solubility of
compounds in water
=
soluble
+
Li+, Na+ , K+, Rb+, Cs+, Fr+
Any cation
=
soluble
+
NH4+
=
soluble
+
any cation
=
soluble
C2H3O2-
+
any cation
=
soluble
FClBrI-
+
Ag+, Cu+, Pb+2, Hg+22, Tl+3
=
(insoluble)
+
any other cation
=
soluble
=
(insoluble)
=
soluble
=
soluble
=
(insoluble)
=
soluble
=
(insoluble)
=
soluble
SO42-
+
+
S2-
+
+
OH-
+
+
PO43CO32SO32O-2
O-2
+
Positive Ions
(Cations)
Ag+, Ca+2, Sr+2, Ba+2, Ra+2,
Pb+2
any other cation
H+, Li+, Na+, K+, Rb+, Cs+, Fr+,
NH4+
Be+2, Mg+2,Ca+2, Sr+2, Ba+2,
Ra+2
any other cation
H+, Li+, Na+, K+, Rb+, Cs+, Fr+,
NH4+ Sr+2, Ba+2, Ra+2, Tl+3
any other cation
H+, Li+, Na+, K+, Rb+, Cs+, Fr+,
NH4+
+
any other cation
=
(insoluble)
+
H+, Li+, Na+, K+, Rb+, Cs+, Fr+
=
soluble
+
any other cation
=
(insoluble)
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COMBINATION REACTIONS
1. lithium solid and iodine solid 
2Li(s) + I2(s)  2LiI(s)
2. iron (III) oxide solid and water 
Fe2O3(s) + H2O(l)  2Fe(OH)3(aq)
3. sulfur dioxide gas and water 
SO2(g) + H2O(l)  H2SO3(aq)
COMBUSTION REACTION
1. 2C8H18(g) + 25O2(g) → 16CO2(g) + 18H2O(l)
carbon dioxide plus water
DECOMPOSITION REACTIONS
Δ
1. Ferrous oxide →
Δ
2FeO(s)  2Fe(s) + O2(g)
electricity
2. Barium hydroxide →
electricity
Ba(OH)2(aq)  BaO(s) + H2O(l)
Δ
3. Sulfuric acid →
Δ
H2SO4(aq)  SO3(g) + H2O(l)
heat
4. Zinc carbonate →
heat
ZnCO3(s)  ZnO(s) + CO2(g)
hv
5. Barium chlorate →
hv
Ba(ClO3)2(s)  BaCl2(s) + 3O2(g)
Energy
6. Copper (II) sulfate pentahydrate →
Energy
CuSO4●5H2O(s)  CuSO4(s) + 5H2O(l)
SINGLE REPLACEMENT REACTION
1. calcium chloride and strontium 
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CaCl2(aq) + Sr(s)  SrCl2(aq) + Ca(s)
2. fluorine and sodium bromide 
F2(g) + 2NaBr(aq)  2NaF(aq) + Br2(l)
DOUBLE REPLACEMENT REACTION
Precipitate Reaction
1. Barium chloride + Potassium carbonate 
BaCl2(aq) + K2CO3(aq)  BaCO3(s) + 2KCl(aq)
Neutralization Reactions
1. Ferric Hydroxide + Oxalic Acid →
2Fe(OH)3(aq) + 3H2C2O4(aq) Fe2(C2O4)3(aq) + 6H2O(l)
2. Calcium Oxide + hydrochloric acid 
CaO(aq) + 2HCl(aq) CaCl2(aq) + H2O(l)
Gas Formation Reactions
1. hydrofluoric acid + Cuprous cyanide 
2HF(aq) + Cu(CN)2(aq)  2HCN(g) + CuF2(aq)
2. Potassium hydroxide + ammonium bromide 
KOH(aq) + NH4Br(aq)  KBr(aq) + NH4OH(aq)
└NH3(g) + H2O(l)
REDOX REACTIONS
1. 2Li(s) + I2(s)  2LiI(s)
Reduction ½ Rxn
I2 + 2e- 2 IOxidation ½ Rxn
2Li 2Li+ + 2e2Li + I2 + 2e-2Li+ + 2e-+ 2 I2Li + I22LiI(s)
2. P4(g) + 4O2(g)  2P2O4(g)
Reduction ½ Rxn
4O2 + 8e- 8O-2
Oxidation ½ Rxn
P4  4P+4+ 8e+4
P4+4O2 + 8e  4P + 8e- + 8O-2
P4+4O2 2P2O4
PHASE RULES
1. If its an element, it’s in its natural state – Periodic Table
2. If its water, its always a (l)
3. If it’s a molecule, it’s a (g) (unless its water or I2(s) & Br2(l)
4. If its an acid (Starts with H!) or a base (Ends in OH!) its always (aq)
5. If its an ionic compound (NOT an acid or Base!) & it’s a combination or decomposition reaction they
are always a (s).
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6. If its an ionic compound (NOT an acid or Base!) & it’s a single or double replacement reaction then
the reactants are always (aq) but the products can be the following:
General Reaction Types
Ionic Compound(s) Product(s)
Single Replacement
Is always (aq)!
Double Replacement – Precipitation
One is always (s) & the other is always
(aq)!
Double Replacement – Neutralization
One is always (aq)!
Double Replacement – Gas Formation
One is always (aq)!
If it is an metallic cyanide it’s a (g)!
If its ammonium hydroxide starts (aq) &
decomposes instantly to a (g)!
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BALANCING 2
PLEASE CHANGE THE FOLLOWING WORD EQUATIONS INTO FORMULA EQUATIONS AND BALANCE THEM
1. solid copper plus solid sulfur makes solid copper (I) sulfide
2. phosphoric acid plus calcium hydroxide makes solid calcium phosphate plus water
3. solid silver oxide makes solid silver plus oxygen gas
4. solid iron (III) chloride plus sodium hydroxide makes solid iron (III) hydroxide plus aqueous sodium
chloride
5. solid nickel (II) phosphate plus sulfuric acid makes solid nickel (II) sulfate plus phosphoric acid
6. solid zinc carbonate plus hydrochloric acid makes solid zinc chloride plus water plus carbon dioxide
7. aqueous silver nitrate plus aqueous aluminum chloride makes solid silver chloride plus aqueous
aluminum nitrate
8. acetic acid plus potassium hydroxide makes aqueous potassium acetate plus water
9. solid phosphorus plus gaseous iodide makes gaseous phosphorus triodide
10. solid aluminum plus aqueous cupric sulfate makes solid copper plus aqueous aluminum sulfate
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Combination Reactions
Complete and balance each of the following COMBINATION reactions. Name the product.
Use Stock names as needed.
1. lithium solid and iodine gas 
2. magnesium solid and nitrogen gas 
3. sulfur dioxide gas and water 
4. aluminum solid and chlorine gas 
5. lead solid and bromine liquid 
6. iron (III) oxide solid and water 
7. carbon dioxide gas and water 
8. sulfur solid and oxygen gas 
9. lead (II) oxide solid and oxygen gas
Use Classic Names as needed.
10. Sn(s) + Br(l) 
11. CuCl(l) + Cl2(g) 
12. P2O5(g) + H2O(l) 
13. Fe(s) + O2(g) 
14. BaO(s) + H2O(l) 
15. Ag(s) + P(s)
16. N2O5(g) + H2O(l) 
17. Ga(s) + O2(g) 
18. K2O(s) + H2O(l) 
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Combustion Reactions
B. Complete and balance each of the following COMBUSTION reactions. Name the product(s).
1. C6H6(g) + O2(g) →
→
2. CH3OH (g) + O2(g)
3. C4H8(g) + O2(g) →
4. C6H12O6(s) + O2(g) →
→
5. C8H12O6(s) + O2(g)
6. CH4(g) + O2(g)
→
7. HCOOH(g) + O2(g) →
8. C7H14(g) + O2(g) →
9. C3H8O3(g) + O2(g) →
10. C3H6O (g) + O2(g) →
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Decomposition Reactions
C. Complete and balance each of the following DECOMPOSITION reactions. Name the product.
↓↓Use Classic Names↓↓
1. Zinc carbonate 
2. Barium chlorate 
3. Ferrous oxide 
4. Barium hydroxide 
5. Barium chloride dihydrate 
6. Cuprous carbonate 
7. Strontium hydroxide 
8. Sulfuric acid 
9. Mercuric oxide 
10. Aluminum chlorate 
Use Stock Names
11. Chromium (III) hydroxide
12. Hypochlorous acid 
13. Aluminum carbonate 
14. Barium hydroxide
15. Potassium hydroxide 
16. Tin (IV) chloride(s) 
17. Potassium chlorate 
18. Copper (II) sulfate pentahydrate 
19. Sodium chloride 
20. Sulfurous acid 
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SINGLE REPLACEMENT REACTIONS
A.
Complete, balance, and name the products for each of the following SINGLE REPLACEMENT
reactions.
1. calcium chloride and strontium 
2. sodium fluoride and chlorine 
3. aluminum and ferric oxide 
4. Tin (IV) chloride and sodium 
5. hydrochloric acid and cadmium 
6. manganese and mercuric chloride
7. calcium and water 
8. magnesium and copper (II) bromide 
9. copper (II) oxide and hydrogen gas
10. hydrobromic acid and barium
11. copper and silver nitrate 
12. fluorine and sodium bromide 
13. aqueous lead (II) sulfate and solid nickel 
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DOUBLE DISPLACEMENT REACTIONS
A. Complete, balance, and name the products for each of the following DOUBLE REPLACEMENT
reactions.
1. Sodium chloride + Hydrogen sulfate 
2. Barium chloride + Potassium carbonate 
3. Iron (II) sulfide + Hydrogen chloride 
4. Strontium bromide + Ammonium carbonate 
5. Sodium iodide + Lead (II) nitrate 
6. Aluminum sulfate + Calcium hydroxide 
7. Sodium carbonate + Calcium hydroxide
8. Barium nitrate + Sodium hydroxide 
9. Strontium hydroxide + Sodium sulfite 
10. Potassium sulfite + Sodium chloride 
11. Ammonium chloride + Silver sulfate 
12. Barium chloride + Sodium sulfite
13. Sodium hydroxide + ammonium chloride
14. Barium nitrate + Sulfuric acid 
15. Cupric nitrate + Potassium sulfite
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Acid – Base Neutralization
A. Complete, balance, and name the products for each of the following Neutralization reactions.
1. Sodium hydroxide + Nitric Acid 
2. Ferric Hydroxide + Oxalic Acid 
3. Phosphoric Acid + Aluminum Hydroxide 
4. Hydrochloric Acid + Rubidium Hydroxide 
5. Perchloric Acid + Sodium Hydroxide 
6. Sulfuric Acid + Cesium Hydroxide 
7. Calcium oxide + Hydrobromic Acid 
8. Thallium oxide + Sulfurous Acid 
9. phosphoric Acid + Sodium oxide 
10. aluminum oxide + permanganic acid 
Gas Formation Reactions
A. Complete, balance, and name the products for each of the following gas formation reactions.
1. Hydrochloric acid + Sodium cyanide
2. potassium hydroxide + ammonium chloride
3. barium cyanide + phosphoric acid
4. ammonium acetate + cesium hydroxide
5. Lithium hydroxide + ammonium phosphate
6. Hydroiodic acid + strontium cyanide
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Redox Reactions
A. Complete, balance, and name the products for each of the following redox reaction
You must show both ½ reactions, the total reaction and the final balanced reaction!
1. H2(g) + Cl2(g) HCl(g)
2. S8(s) + O2(g) SO2
3. S8(s) + O2(g) SO3
4. NaH(s) Na(s) + H2(g)
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