Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between zinc sulfate (ZnSO4) and sodium phosphate (Na3PO4). It covers balancing the molecular equation, determining the solubility states of the compounds, and breaking down strong electrolytes into ions for the complete ionic equation. The tutorial also identifies spectator ions and demonstrates how to write the final net ionic equation, ensuring that both charge and atoms are balanced.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

• Split strong electrolytes into ions

Why is it necessary to balance the molecular equation first?

• To determine the states of substances

• To conserve mass and charge

• To ensure the reaction is feasible

• To identify spectator ions

Which of the following is generally soluble?

• Iron(III) oxide

• Zinc phosphate

• Sodium phosphate

• Calcium carbonate

What is the state of zinc phosphate in the reaction?

• Liquid

• Aqueous

• Gaseous

• Solid

What charge does a zinc ion typically have?

• 2+

• 3+

• 1+

• 0

In the complete ionic equation, which ions are not split?

• Phosphate ions

• Zinc phosphate

• Sodium ions

• Sulfate ions

What are spectator ions?

• Ions that are insoluble

• Ions that participate in the reaction

• Ions that do not change during the reaction

• Ions that form a precipitate

Which ions are removed to form the net ionic equation?

• Reactant ions

• Product ions

• All ions

• Spectator ions

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

• Positive

• Negative

• Zero

• Depends on the reaction

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

• To make the equation look neat

• To satisfy the law of conservation of mass

• To ensure all ions are included

• To satisfy the law of conservation of charge