Net Ionic Equations and Ionic Charges

This video tutorial explains how to write a balanced net ionic equation for the reaction between ammonium carbonate and calcium chloride. It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The tutorial then demonstrates how to split strong electrolytes into their ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, ensuring charge conservation. The video concludes with a recap of the balanced net ionic equation.

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

• Identify spectator ions

• Balance the molecular equation

• Split compounds into ions

• Determine the solubility of compounds

Why is ammonium chloride considered soluble?

• It reacts with water

• Ammonium compounds are generally soluble

• It is a strong acid

• It forms a solid precipitate

What is the state of calcium carbonate in the reaction?

• Solid

• Gas

• Aqueous

• Liquid

What charge does the ammonium ion carry?

• 2+

• 1+

• 1-

• 2-

What is the charge of the carbonate ion?

• 1-

• 2+

• 1+

• 2-

Which ions are considered spectator ions in this reaction?

• Ammonium and chloride ions

• Calcium and carbonate ions

• Ammonium and carbonate ions

• Calcium and chloride ions

What happens to spectator ions in a net ionic equation?

• They are included in the final equation

• They are removed from the equation

• They change their charge

• They form a new compound

What is the net charge of the calcium carbonate compound?

• 0

• 1+

• 1-

• 2+

Why is it important to balance charges in a net ionic equation?

• To increase reaction rate

• To maintain electrical neutrality

• To ensure the reaction is spontaneous

• To conserve mass

What is the final product of the reaction between ammonium carbonate and calcium chloride?

• Calcium chloride

• Calcium carbonate

• Ammonium chloride

• Ammonium carbonate