Net Ionic Equations and Spectator Ions

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between silver nitrate (AgNO3) and ammonium sulfate ((NH4)2SO4). It begins with balancing the molecular equation, assigning solubility states to each compound, and then splitting strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and crossed out to derive the net ionic equation. The tutorial concludes by verifying the balance of charges and atoms in the final equation.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Which compound is used as a source of silver ions in the reaction?

• Ammonium nitrate

• Silver nitrate

• Ammonium sulfate

• Silver sulfate

Why is silver sulfate considered insoluble in the context of net ionic equations?

• It is highly soluble

• It forms a gas

• It is slightly soluble, but mostly forms a solid

• It reacts with water

What is the state of ammonium sulfate in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

Which of the following ions is always one plus?

• Ammonium ion

• Nitrate ion

• Silver ion

• Sulfate ion

Which ion is not split in the net ionic equation?

• Silver ion

• Nitrate ion

• Ammonium ion

• Silver sulfate

What is the purpose of identifying spectator ions in a net ionic equation?

• To determine the solubility of compounds

• To simplify the equation by removing ions that do not participate in the reaction

• To identify the products of the reaction

• To balance the equation

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

• They are removed from the equation

• They form a precipitate

• They change state

• They are included in the final equation

What is the net charge of the balanced net ionic equation for the reaction between silver nitrate and ammonium sulfate?

• One plus

• Zero

• Two minus

• Two plus

What ensures that the net ionic equation is balanced?

• Equal number of atoms on both sides

• Equal number of electrons on both sides

• Equal number of ions on both sides

• Equal number of molecules on both sides