16.4 Net Ionic Equations
16.4 Net Ionic Equations
Lesson Objectives
- Write net ionic equations for double-replacement reactions that produce precipitates, gases, or molecular
compounds. - Write net ionic equations for single-replacement reactions.
- Use the solubility rules to predict precipitate formation.
Lesson Vocabulary
- ionic equation
- molecular equation
- net ionic equation
- spectator ion
Check Your Understanding
Recalling Prior Knowledge
- What are the five types of chemical reactions?
- What is dissociation?
Several types of reactions were introduced in the chapterChemical Reactions: combination, decomposition, single-
replacement, double-replacement, and combustion. Single-replacement and double-replacement reactions occur
most frequently in aqueous solution. In this lesson, you will learn about various ways to depict these chemical
reactions.
Aqueous Reactions
When ionic compounds are dissolved into water, the polar water molecules break apart the solid crystal lattice,
resulting in the hydrated ions being evenly distributed through the water. As you have learned, this process is called
dissociation, and it is the reason that ionic compounds tend to be strong electrolytes. When two different ionic
compounds that have been dissolved in water are mixed, a chemical reaction may occur between certain pairs of the
hydrated ions.
Consider the double-replacement reaction that occurs when a solution of sodium chloride is mixed with a solution
of silver nitrate. The driving force behind this reaction is the formation of the silver chloride precipitate.