Net Ionic Equations and Spectator Ions

The video tutorial explains how to write the balanced net ionic equation for the reaction between copper(II) nitrate and sodium sulfate. It begins by balancing the molecular equation and discussing the solubility of the reactants and products, noting that all substances are soluble and no reaction occurs. The tutorial then demonstrates writing the ionic equation and identifying spectator ions, concluding that no net ionic reaction takes place as all ions remain unchanged.

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

• Determine the solubility of the products

• Identify the spectator ions

• Balance the molecular equation

• Write the complete ionic equation

Why are nitrates generally considered soluble?

• They form strong ionic bonds

• They dissolve easily in water

• They are always in gaseous form

• They react with most metals

What conclusion can be drawn if all substances in a reaction are aqueous?

• A gas is formed

• A precipitate is formed

• No reaction occurs

• A new compound is synthesized

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

What happens to the spectator ions in a net ionic equation?

• They are included in the equation

• They change their oxidation state

• They are omitted from the equation

• They form a new compound

What is the net ionic equation for the reaction between Cu(NO3)2 and Na2SO4?

• Cu^2+ + 2NO3^- → Cu(NO3)2

• No net ionic equation exists

• 2Na^+ + 2NO3^- → Na2NO3

• Cu^2+ + SO4^2- → CuSO4

What is the final conclusion about the reaction between Cu(NO3)2 and Na2SO4?

• A new compound is synthesized

• No reaction occurs

• A precipitate is formed

• A gas is released

Why is there no net ionic equation for the reaction between Cu(NO3)2 and Na2SO4?

• A gas is released

• A precipitate is formed

• All ions are spectator ions

• The reaction is incomplete