Page 2: Ionic Equations and Spectator Ions

This page delves deeper into ionic equations and the concept of spectator ions, explaining how to write balanced ionic equations while omitting spectator ions.

Definition: An ionic equation shows only the ions, atoms, or molecules that actively participate in the reaction, omitting spectator ions.

Example: In the reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), the sulfate ions are spectator ions and are omitted from the ionic equation.

Highlight: When writing ionic equations, products often include precipitates or simple molecules like iodine or water.

Quote: "When writing an ionic equation remember: The product(s) will often include a precipitate or simple molecules such as iodine or water."

Page 3: Precipitation Reactions and Worked Examples

This page focuses on precipitation reactions and provides detailed worked examples of converting full equations to ionic equations.

Definition: A precipitation reaction occurs when two aqueous solutions react to form a solid precipitate.

Example: The reaction between iron(II) sulfate and sodium hydroxide: FeSO₄(aq) + 2NaOH(aq) → Fe(OH)₂(s) + Na₂SO₄(aq)

Highlight: The four-step process for writing ionic equations for precipitation reactions:

1. Write the full balanced equation
2. Identify the precipitate formed
3. Identify the ions forming the precipitate
4. Write the ionic equation

Vocabulary: Precipitation refers to the formation of an insoluble solid from the reaction between two aqueous solutions.