Spectator Ions and Net Ionic Equations

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between barium hydroxide and sodium carbonate. It begins with balancing the molecular equation, assigning states to each compound based on solubility rules, and then breaking down the compounds into ions to form the complete ionic equation. The tutorial explains how to identify and remove spectator ions to derive the net ionic equation, ensuring both charge and atom balance. The video concludes with a verification of the balanced net ionic equation.

What is the first step in balancing net ionic equations?

• Write the net ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

Which of the following is considered a strong base in the reaction?

• Sodium chloride

• Barium carbonate

• Barium hydroxide

• Sodium carbonate

What is the state of sodium carbonate in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

What charge does barium have in the complete ionic equation?

• 2+

• 2-

• 1+

• 1-

Which ions are not split in the complete ionic equation?

• Carbonate ions

• Hydroxide ions

• Sodium ions

• Barium carbonate

What are spectator ions?

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that are gases

• Ions that participate in the reaction

Which ions are removed as spectator ions in this reaction?

• Barium and carbonate ions

• Carbonate and hydroxide ions

• Sodium and hydroxide ions

• Barium and sodium ions

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

• 1+

• 1-

• 0

• 2+

What ensures that the net ionic equation is balanced?

• Equal number of ions on both sides

• Equal number of molecules on both sides

• Equal number of atoms on both sides

• Equal number of electrons on both sides

What is the final product of the reaction?

• Barium carbonate

• Sodium hydroxide

• Sodium carbonate

• Barium hydroxide