Chem I Ch. 9/17 Test
Review and Study Guide
The following guide is intended to be a study aid for the upcoming Test on Ch. 9
and 17 in Chem. If you work to know the topic areas listed below you will be
well prepared for this test. The test will cover the topics listed below, although all
information we went over in class may potentially be on the test. Good luck with
your studies.
Know the definitions of:
Chapter 9 – Chemical Reactions
Chemical reaction
Reactant
Product
Chemical equation
Coefficient
Precipitate
Solute
Solvent
Aqueous Solution
Types of Reaction
Synthesis
Decomposition reaction
Single-Replacement reaction
Double-Replacement reaction
Combustion Reaction
Oxidation & Reduction
Complete ionic equation
Net ionic equation
Spectator ion
Chapter 17 – Chemical Equilibrium
Equilibrium
Le Chatelier’s Law
Reversible Reaction
Chapter 7 – Ionic Compounds & Chapter 8 – Covalent bonding
Know how to:
 Read the ion chart to identify elemental ions like oxide (O2-) and polyatomic
ions like carbonate (CO32-)
 Know how to write proper chemical formulas, both ionic and covalent
compounds
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Chem I Ch. 9/17 Test
Review and Study Guide
Chapter 9 – Chemical Reactions
Know how to:
 Balance simple reactions
 Identify simple reactions as decomposition, synthesis, single replacement,
double replacement or combustion.
 In a single replacement reaction, be able to identify what was oxidized and
what was reduced.
 Recall the seven diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2)
 Decomposition of carbonates yields a metal oxide and carbon dioxide (eg.
CaCO3  CaO(s) + CO2(g))
 Decomposition of chlorates yields a metal chloride and oxygen gas (eg.
2Al(ClO3)3  2AlCl3(s) + 9O2(g))
 Identify the physical states of reactants and products (s= solid, aq=aqueous,
l=liquid, g=gas)
 Write the reaction using formulas if you are given the names and states of
the compounds
 Identify the precipitate and aqueous compounds using the solubility table in
a double replacement reaction.
 Write the complete ionic equation and net ionic equation given the complete
chemical equation
Chapter 17 – Equilibrium
Know how to:
 Apply Le Chatelier’s law, e.g.
CaCO3(s)  CaO(s) + CO2(g)
If we remove CO2 from a vessel, the reaction will shift to the right to create
more CO2. If we add CO2 the reaction will shift left.
For this test, I will give you:
 a periodic table
 a list of ions and oxidation numbers
 the prefixes and numbers (ex. mono- is one, di- is two, etc.)
 the metal and halogen activity chart
 the solubility table
It is your responsibility to know how to use them.
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