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 aluminum chloride. It begins with balancing the molecular equation, determining the states of each substance, and then writing the complete ionic equation. The tutorial proceeds to derive the net ionic equation by crossing out spectator ions and concludes with simplifying the equation to ensure charge balance.

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

• Determine the solubility of the products.

• Balance the molecular equation.

• Identify the spectator ions.

• Write the complete ionic equation.

Which of the following compounds is considered slightly soluble and forms a precipitate in the reaction?

• Lead(II) nitrate

• Aluminum chloride

• Lead(II) chloride

• Aluminum nitrate

What is the charge on the lead ion in the complete ionic equation?

• 4+

• 1+

• 2+

• 3+

In the complete ionic equation, how many nitrate ions are present?

• Six

• Four

• Eight

• Two

What is the purpose of identifying spectator ions in a reaction?

• To balance the equation

• To determine solubility

• To calculate the reaction rate

• To simplify the net ionic equation

Which ions are considered spectator ions in this reaction?

• Chloride ions

• Lead ions

• Nitrate ions

• Aluminum ions

What is the coefficient of lead ions in the simplified net ionic equation?

• One

• Two

• Four

• Three

How is charge balance achieved in the net ionic equation?

• By adding more ions

• By ensuring equal numbers of positive and negative charges

• By removing all spectator ions

• By adjusting the coefficients

What is the final step in simplifying the net ionic equation?

• Reducing the coefficients

• Determining solubility

• Balancing the molecular equation

• Adding spectator ions

Which of the following statements is true about the net ionic equation?

• It is not balanced for charge.

• It is the same as the molecular equation.

• It only includes ions that participate in the reaction.

• It includes all ions present in the reaction.