Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between lead(II) acetate and potassium iodide. It begins with balancing the molecular equation, determining the solubility and states of the reactants and products, and then proceeds to split strong electrolytes into ions to form the complete ionic equation. The tutorial identifies and removes spectator ions to derive the net ionic equation, ensuring that both charge and atoms are balanced. The video concludes with a summary of the balanced net ionic equation and emphasizes the importance of charge conservation.

What is the first step in writing a balanced net ionic equation?

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Why is it important to check the solubility of lead compounds?

• They can form precipitates

• They are always soluble

• They do not react with iodide

• They are always insoluble

What is the charge of the lead ion in lead(II) acetate?

• 4+

• 1+

• 3+

• 2+

How do you determine the charge of an ion in a compound?

• By considering the charges of other ions in the compound

• By using the solubility rules

• By looking at the periodic table

• By checking the color of the compound

Which ions are considered spectator ions in this reaction?

• Potassium ions

• Acetate ions

• Iodide ions

• Lead ions

What happens to the spectator ions in the net ionic equation?

• They form a new compound

• They change their charge

• They are removed from the equation

• They are included in the final equation

What is the role of potassium ions in this reaction?

• They form a precipitate

• They act as spectator ions

• They change the solubility of lead

• They react with lead ions

What is the final product formed as a precipitate in this reaction?

• Lead(II) iodide

• Lead(II) acetate

• Potassium acetate

• Potassium iodide

What is the purpose of writing a net ionic equation?

• To show all reactants and products

• To balance the charges in the equation

• To focus on the ions that participate in the reaction

• To highlight the formation of precipitates

Why is it important to ensure charge balance in a net ionic equation?

• To make the equation look neat

• To satisfy the law of conservation of mass

• To prevent the formation of precipitates

• To ensure the reaction is possible