Net Ionic Equations and Spectator Ions

This video tutorial explains how to balance the net ionic equation for the reaction between potassium sulfide (K2S) and lead(II) perchlorate (Pb(ClO4)2). It begins with balancing the molecular equation, followed by determining the solubility and states of the substances involved. The tutorial then breaks down the strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge conservation and balancing of atoms in the final equation.

What is the first step in balancing a net ionic equation?

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

How do you balance the number of potassium atoms in the molecular equation?

• Add a coefficient of 2 in front of K2S

• Add a coefficient of 2 in front of PbClO4

• Add a coefficient of 3 in front of K2S

• Add a coefficient of 3 in front of PbClO4

Which of the following compounds is generally insoluble?

• Lead(II) perchlorate

• Potassium perchlorate

• Potassium sulfide

• Lead(II) sulfide

What happens to lead(II) sulfide in the reaction?

• It reacts with water

• It remains as ions

• It forms a precipitate

• It dissolves in water

What is the charge of the sulfide ion?

• 1+

• 2-

• 1-

• 2+

Which ions are considered spectator ions in this reaction?

• Potassium and sulfide ions

• Lead and perchlorate ions

• Potassium and perchlorate ions

• Lead and sulfide ions

What is the net charge of the products in the net ionic equation?

• 0

• 2-

• 1+

• 2+

Why don't we split solids in a net ionic equation?

• They are spectator ions

• They are already balanced

• They do not dissolve in water

• They are not reactive

What is the charge of the lead ion in this reaction?

• 1+

• 4+

• 2+

• 3+

What is the purpose of removing spectator ions?

• To identify the precipitate

• To determine solubility

• To simplify the equation

• To balance the equation