Ionic Compounds and Reactions

The video tutorial explains how to write a balanced net ionic equation for the reaction between lead(II) nitrate and ammonium sulfide. It begins by balancing the molecular equation, then assigns states to each substance based on solubility rules. The tutorial proceeds to split strong electrolytes into ions and identifies spectator ions to be crossed out. Finally, it presents the balanced net ionic equation, ensuring that both charge and atom count are conserved.

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

• Identify spectator ions

• Write the net ionic equation directly

• Balance the molecular equation

• Determine the solubility of compounds

Which of the following compounds is generally insoluble?

• Ammonium compounds

• Chlorides

• Nitrates

• Sulfides

What happens to lead sulfide in the reaction?

• It remains as ions

• It reacts with water

• It forms a precipitate

• It dissolves in water

What is the charge on the lead ion in lead(II) nitrate?

• 2+

• 1+

• 4+

• 3+

What is the charge on the sulfide ion?

• 0

• 3-

• 2-

• 1-

Which of the following is a strong electrolyte?

• Water

• Ammonium nitrate

• Carbon dioxide

• Lead sulfide

Which ions are considered spectator ions in this reaction?

• Lead and sulfide ions

• Lead and ammonium ions

• Ammonium and nitrate ions

• Sulfide and nitrate ions

Why do we not split solids in the net ionic equation?

• They are always soluble

• They are spectator ions

• They do not dissociate into ions

• They are not involved in the reaction

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

• 1+

• 0

• 2-

• 2+

What ensures the net ionic equation is balanced?

• Equal number of molecules on both sides

• Equal number of compounds on both sides

• Equal number of atoms on both sides

• Equal number of ions on both sides