Worksheet #1: Writing and Balancing Formula Equations
Step 1: Write each formula and balance each formula using SUBSCRIPTS.
Step 2: Balance the overall equation using coefficients.
+

1.
sulfur
2.
zinc
3.
hydrogen
+
nitrogen

ammonia
4.
hydrogen
+
chlorine

hydrogen chloride
5.
carbon
6.
calcium oxide
7.
phosphorus
8.
hydrochloric acid
9.
barium chloride
10.
aluminum sulfate + calcium hydroxide  aluminum hydroxide + calcium sulfate
11.
ethane (C2H6)
12.
aluminum oxide
+
oxygen
sulfur dioxide

sulfuric acid
+

water
+
+
water
oxygen
+
+
carbon monoxide



+
hydrogen
diphosphorus pentoxide
sulfuric acid
oxygen
hydrogen
calcium hydroxide

sodium hydroxide
+
+
zinc sulfate

aluminum

sodium chloride
barium sulfate
carbon dioxide
+
oxygen
1
+
+
water
+
water
hydrochloric acid
Worksheet #2: Synthesis Reactions
In synthesis reactions, two or more reactants come together to form one compound.
A + B  AB
Complete the following word equations, and write and balance the formula equation.
1.
calcium +
oxygen

+

2.
copper
3.
calcium oxide
4.
hydrogen
+
nitrogen

5.
hydrogen
+
chlorine

6.
silver
sulfur
7.
chromium
+
oxygen
8.
aluminum
+
bromine
9.
sodium
10.
hydrogen
+
11.
aluminum
+
+
sulfur
+
+
copper(II) sulfide

water
calcium hydroxide

iodine
oxygen
oxygen





2
Worksheet #3: Decomposition Reactions
In decomposition reactions, one compound will break down into two or more parts.
1.
barium carbonate


2.
magnesium carbonate
3.
potassium carbonate
4.
zinc hydroxide
5.
Iron(II) hydroxide

6.
nickel(II) chlorate

7.
sodium chlorate
8.
potassium chlorate
9.
sulfuric acid
10.
carbonic acid
11.
aluminum oxide
12.
silver oxide








3
Worksheet #4: Single-Replacement Reactions
Step 1 - Write the formulas of the reactants on the left of the yield sign
Step 2 - Look at the Activity Series to determine if the replacement can happen
Step 3 - If the replacement can occur, complete the reaction and balance it. If the reaction
cannot happen, write N.R. (no rxn) on the product side.
1.
lead +
zinc acetate

+

2.
iron
aluminum oxide
3.
silver nitrate
4.
sodium bromide
5.
aluminum bromide
+
6.
sodium iodide
bromine
7.
calcium
8.
magnesium
9.
silver
10.
potassium
11.
sodium
+
+
+
+
+
nickel


hydrochloric acid
+
+


nitric acid


water
water

chlorine
sulfuric acid
+

iodine

4
Worksheet #5: Double-Replacement Reactions
In these reactions, all you do is look at the names of the reactants, and "switch partners". Just be
sure that the new pairs come out with the positive ion named first, and paired with a negative ion.
1.
aluminum iodide +
mercury(II) chloride 
2.
silver nitrate
+
3.
copper(II) bromide
4.
calcium acetate
5.
ammonium chloride
+
6.
calcium nitrate
hydrochloric acid
7.
iron(II) sulfide
8.
copper(II) hydroxide
9.
calcium hydroxide
10.
calcium bromide

potassium phosphate
+
+
mercury(I) acetate
+
+
acetic acid



hydrochloric acid
+

sodium carbonate
+
+

aluminum chloride


phosphoric acid
potassium hydroxide

Examine the products of the reactions on this page, and determine in each whether a gas, water, or a
precipitate is formed. Use the solubility table in Appendix A of your textbook to determine the
solubilities of the reaction products. If there is no gas, water, or precipitate produced, put an "X"
through the yield sign, because no reaction occurs.
5
Worksheet #6: Combustion Reactions
We will focus on the combustion of hydrocarbons. Hydrocarbons react with oxygen to form carbon
dioxide and water.
1.
methane (CH4)
+
2.
ethane (C2H6)
3.
propane (C3H8)
4.
butane (C4H10)
5.
pentane (C5H12)
6.
hexane (C6H14)
7.
ethene (C2H4)
+
8.
ethyne (C2H2)
+
9.
benzene (C6H6)

oxygen
+

oxygen
+
+

oxygen
+
+

oxygen

oxygen
oxygen
+

oxygen
oxygen
oxygen



6