Lesson 4: Writing Formula, Complete, and Net Ionic Equations

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Presentation transcript:

Lesson 4: Writing Formula, Complete, and Net Ionic Equations Unit 3: Solubility Lesson 4: Writing Formula, Complete, and Net Ionic Equations

Today’s Example Question Write a formula equation, a complete ionic equation, and a net ionic equation for the reaction that occurs when 0.2 M solutions of Pb(NO3)2(aq) and FeCl3(aq) are mixed. (We’ll be solving this slowly, over the next few slides.) Copy onto chalkboard.

Part 1: Identify any precipitate(s). This is what we did last class...

Part 2: Write a formula equation. A formula equation is a balanced chemical equation in which all the reactants and products are given by their chemical formulae. Phases must be indicated!

Part 3: Write a complete ionic equation. A complete ionic equation shows all soluble ionic species broken into their respective ions. The unreacted ions shown on the product side are called spectator ions – they take no part in the reaction. This type of equation can only be written after first writing a balanced formula equation.

Part 4: Write a net ionic equation. A net ionic equation shows only the species that are actively involved in the reaction.

Brain Break!

Practice and Demonstrations! For each combination, identify the precipitate, and write the formula, complete ionic, and net ionic equations. Then I’ll show you the reaction! HgCl2 and Na2CO3 Pb(NO3)2 and KI HgCl2 and KI Demo 12.III.5 - 20 min