Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between lead(II) nitrate and calcium chloride. It covers balancing the molecular equation, determining the solubility and states of substances, splitting strong electrolytes into ions for the complete ionic equation, and identifying spectator ions. The tutorial concludes with the final net ionic equation, ensuring charge and atom balance.

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

• Write the complete ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

Which of the following is generally soluble in water?

• Lead(II) chloride

• Calcium carbonate

• Nitrates

• Silver chloride

What is the state of lead(II) chloride in the reaction?

• Aqueous

• Solid

• Gas

• Liquid

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

• 1+

• 4+

• 2+

• 3+

Which ion is not split in the complete ionic equation?

• Calcium ion

• Nitrate ion

• Chloride ion

• Lead(II) chloride

What are spectator ions?

• Ions that are insoluble

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that participate in the reaction

Which ions are crossed out as spectator ions in this reaction?

• Lead and calcium ions

• Nitrate and chloride ions

• Lead and chloride ions

• Calcium and nitrate ions

What is the net charge on both sides of the net ionic equation?

• Zero

• Negative

• Variable

• Positive

Why is it important to ensure the net ionic equation is balanced?

• To identify spectator ions

• To ensure solubility

• To conserve charge

• To conserve mass

What is the final product formed in the reaction between lead(II) nitrate and calcium chloride?

• Lead(II) chloride

• Calcium chloride

• Lead(II) nitrate

• Calcium nitrate