Chemistry Review
Topics:
1. Ionic and molecular compounds
2. Nomenclature – naming and writing chemical formulas
3. Periodic table – metals, non-metals, # of total and valence electrons, reactivity
4. Law of conservation of mass
5. Writing and balancing chemical equations
6. Types of reactions

Synthesis, decomposition, single displacement, double displacement
7. Acids, bases, pH scale, and neutralization
8. Identifying physical and chemical changes
Questions:
1. Compare ionic and molecular compounds using the chart below:
Characteristic
Types of atoms involved
Bond type: (ionic or covalent)
Electrons: (shared or transferred)
Example:
Ionic Compound
Molecular Compound
2. Name the following compounds:
a. NaCl _______________________________
b. Mg3(PO4)2 ___________________________
c. P2O5 ________________________________
d. Hg2SO4 ______________________________
e. Cu(OH)2 _____________________________
3. Identify the chemical formula for the following names:
a. Calcium nitrate _________________________
b. Iron (III) chloride _______________________
c. Hydrochloric acid _______________________
d. Sulphur trioxide ________________________
e. Gold (I) sulphate ________________________
4. Chemical equations can be written as a word equation, a skeletal equation, and as a balanced
equation. The Law of Conservation of Mass is used to help with the balancing process.
a. What is the Law of Conservation of Mass?
b. 0.30g of aluminum was completely burned in the air and 1.0g of aluminum oxide was
produced. What mass of oxygen must have been reacted from the air?
5. There are four types of reactions. Describe how you can identify each type in a chemical
equation.
Type of Reaction
How can you identify each type of reaction from a
chemical equation?
Synthesis
Decomposition
Single Replacement
(Single Displacement)
Double Replacement
(Double Displacement)
6. For each of the examples below, indicate the type of reaction and balance the equation.
a.
Mg(OH)2 
MgO +
H2 O
Type of reaction ___________________________________________
b.
Cl2 + NaBr 
Br2 +
NaCl
Type of reaction ___________________________________________
c.
H2S + KOH 
HOH +
K2S
Type of reaction ___________________________________________
d.
SrCl2 + Na 
Sr +
NaCl
Type of reaction ___________________________________________
e.
N2 + H2 
NH3
Type of reaction ___________________________________________
7. Explain the differences between acids and bases:
Property
Ion present in solution
Electrical conductivity
Taste
Feel
pH Range
Example
Acids
Bases
8. What happens when a base (NaOH) and an acid (HCl) are mixed together? Write down the
balanced chemical equation that describes this reaction.