Net Ionic Equations and Spectator Ions

This video tutorial explains how to write the net ionic equation for the reaction between barium nitrate and sodium carbonate. It begins with balancing the molecular equation, then assigns solubility states to each compound. The tutorial proceeds to break down the compounds into ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, highlighting the formation of solid barium carbonate.

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

• Write the complete ionic equation

• Identify spectator ions

• Determine the solubility of compounds

• Balance the molecular equation

Which of the following compounds is generally insoluble?

• Barium nitrate

• Sodium nitrate

• Sodium carbonate

• Barium carbonate

What happens to the precipitate in the reaction?

• It dissolves in water

• It reacts with water

• It remains as ions

• It forms a solid at the bottom

Why is it important to write the states of each substance?

• To identify spectator ions

• To know which compounds are soluble

• To determine the reaction type

• To balance the equation

What is the charge of the nitrate ion?

• 1+

• 2-

• 1-

• 2+

Which ion is not split in the complete ionic equation?

• Carbonate ion

• Sodium ion

• Barium carbonate

• Nitrate ion

What is the charge of the carbonate ion?

• 1-

• 1+

• 2+

• 2-

What is the purpose of identifying spectator ions?

• To write the molecular equation

• To determine solubility

• To balance the equation

• To simplify the net ionic equation

Which ions are considered spectator ions in this reaction?

• Barium and carbonate ions

• Barium and nitrate ions

• Sodium and nitrate ions

• Sodium and carbonate ions

What is the net ionic equation for the reaction between barium nitrate and sodium carbonate?

• 2Na^+ + CO3^2- → Na2CO3

• Ba^2+ + CO3^2- → BaCO3(s)

• Ba^2+ + 2NO3^- → Ba(NO3)2

• Na^+ + NO3^- → NaNO3