Worksheet #1
Synthesis & Decomposition Reactions
Predict and balance the following synthesis and decomposition reactions. Use abbreviations to indicate the phase of
reactants and products where possible [i.e., (aq), (s), (l), (g)].
1. A sample of calcium carbonate is heated.
2. Sulfur dioxide gas is bubbled through water.
3. Solid potassium oxide is added to a container of carbon dioxide gas.
4. Liquid hydrogen peroxide is warmed.
5. aluminum + oxygen →
6. Molten aluminum chloride is electrolyzed.
7. A pea-sized piece of sodium is added to a container of iodine vapor.
1|Page
8. A sample of carbonic acid is heated.
9. A sample of potassium chlorate is heated.
10. Solid magnesium oxide is added to sulfur trioxide gas.
11. hydrogen + nitrogen →
12. calcium + oxygen →
13. A sample of ammonium carbonate is heated.
2|Page
Worksheet #2
Single Replacement Reactions
Using the activity series, predict and balance the following single replacement reactions. Use abbreviations to indicate
the appropriate phase of reactants and products where possible. Note: Not all of the reactions will occur. For those
that do not, write “no reaction”.
1. A piece of copper is dropped into a container of water.
2. Liquid bromine is added to a container of sodium iodide crystals.
3. An aluminum strip is immersed in a solution of silver nitrate.
4. Zinc pellets are added to a sulfuric acid solution.
5. Fluorine gas is bubbled into a solution of aluminum chloride.
6. Magnesium turnings are added to a solution of lead (II) acetate.
7. Iodine crystals are added to a solution of sodium chloride.
8. Calcium metal is added to a solution of nitrous acid.
9. A pea-sized piece of lithium is added to water.
10. A solution of iron (III) chloride is poured over a piece of platinum wire.
3|Page
Double Replacement Reactions Part 1
Precipitation Reactions
Predict and balance the following double replacement reactions based on the solubility of the products. Use the
abbreviations (aq) and (s) for the reactants and products. All reactants are aqueous. Note: Some of these reactions do
not go to completion.
1. silver nitrate + potassium chromate
2. ammonium chloride + cobalt (II) sulfate
3. iron (III) sulfate + barium iodide
4. zinc acetate + cesium hydroxide
5. ammonium sulfide + lead (II) nitrate
6. lithium hydroxide + sodium chromate
7. chromium (III) bromide + sodium nitrate
8. rubidium phosphate + titanium (IV) nitrate
9. ammonium carbonate +nickel (II) chloride
10. tin (IV) nitrate + potassium sulfite
4|Page
Double Replacement Reactions Part 2
Gas/Primarily Molecular Species Formation
Predict and balance the following double replacement reactions. Use the abbreviations (aq), (l), (g), and (s) for the
reactants and products. All reactants are aqueous, unless otherwise stated.
1. Ammonium sulfate and potassium hydroxide are mixed together.
2. Ammonium sulfide is reacted with hydrochloric acid.
3. Sodium nitrate is reacted with hydrochloric acid.
4. Solid calcium carbonate is reacted with sulfuric acid.
5. Potassium sulfite is reacted with hydrobromic acid.
6. Potassium sulfide is reacted with nitric acid.
7. Sodium fluoride reacts with dilute nitric acid.
8. Solid magnesium oxide is reacted with hydrochloric acid.
9. Solid calcium sulfite + acetic acid 
10. Strontium hydroxide + ammonium sulfide 
5|Page
6|Page
Worksheet #3
Aqueous Solutions and Net Ionic Equations
Part 1 - Write balanced overall ionic equations and net ionic equations for the molecular equations from your other
worksheets, as indicated. Write none if a net ionic equation does not exist.
1.
Worksheet 2, #3
2.
Worksheet 2, #4
3. Worksheet 2, #9
4.
Worksheet 3, Part 1, #3
5.
Worksheet 3, Part 2, #5
Part 2 - Write net ionic equations ONLY for the molecular equations from your other worksheets, as indicated.
1. Worksheet 3, Part 1, #1
2. Worksheet 3, Part 1, #8
3. Worksheet 3, Part 2, #1
7|Page
4. Worksheet 3, Part 2, #10
Part 3 - Write balanced molecular equations for each reaction and then write the net ionic equation. Write none if a
net ionic equation does not exist.
1. Aqueous nickel (II) nitrate + aqueous cesium hydroxide
2. Solid potassium chlorate is strongly heated.
3. Aqueous sodium carbonate + chlorous acid
Part 4 – Ion Concentration: Complete the indicated problems from Chapter 4 in the textbook in the space provided.
30.
32.
42.
8|Page
Worksheet #4
Acid-Base Neutralization Reactions
Write balanced molecular equations for each reaction and then write the net ionic equation. Write none if a net
ionic equation does not exist.
1. Sulfuric acid is reacted with excess ammonium hydroxide.
2. Calcium hydroxide + carbonic acid →
3. Hydrochloric acid + sodium hydroxide →
4. Acetic acid is reacted with excess lithium hydroxide
5. Equal numbers of moles of potassium hydroxide and phosphoric acid react.
6. Equal volumes of 0.1 M phosphoric acid and 0.2 M potassium hydroxide react.
7. Sulfurous acid is combined with excess barium hydroxide.
9|Page
Complete the indicated problems from Chapter 4 in the textbook in the space provided:
76.
77.
10 | P a g e
Worksheet #5
Redox Equations
Assign oxidation numbers to all elements and identify those that are oxidized and reduced.
1. N2O
2. K
+
+

H2

KNO3
H2O
N2
+
+
NH3
K2O
3. Fe2O3
+
S

4. MnO2
+
HBr

Br2
+
MnBr2
+
H2O
+
NaOH

PbO
+
NaSbO2
+
H2O

MnCl
+
Cl2
+
KCl
5. PbO2
+
6. KMnO4
+
Sb
HCl
Fe
+
+
SO2
H2O
11 | P a g e
Complete the indicated problems from Chapter 4 in the textbook in the space provided.
89.
91.
12 | P a g e
Worksheet #6
OPTIONAL Review Worksheet
Write balanced molecular equations and net ionic equations for the following reactions. Write none if a net ionic
equation does not exist.
1. Equal volumes of equal molar concentrations of sulfuric acid and sodium hydroxide.
2. Solid lithium metal is added to water.
3. Aqueous solutions of magnesium nitrate and sodium bromide are mixed together.
4. Aqueous solutions of oxalic acid and excess potassium hydroxide.
5. Solid cobalt (II) hydroxide + hydroiodic acid
6. Aqueous solution of manganese (II) sulfate undergoing hydrolysis
13 | P a g e
7. Aqueous solutions of potassium phosphate and excess hydrobromic acid.
8. Magnesium turnings are added to a solution of iron (III) chloride.
9. Aqueous hydrochloric acid reacts with solid iron (II) sulfide.
10. Aqueous ammonium sulfide reacts with excess aqueous lithium hydroxide.
11. Aqueous solutions of calcium nitrate and rubidium chloride are mixed together.
12. Aqueous solutions of potassium chromate and silver nitrate react.
13. Aqueous solutions of sulfuric acid and excess barium hydroxide are combined.
14. Chlorine gas is bubbled into a solution of potassium iodide.
14 | P a g e