Net Ionic Equations and Charges

The video tutorial explains how to write a balanced net ionic equation for the reaction between silver nitrate (AgNO3) and copper(II) sulfate (CuSO4). It begins with balancing the molecular equation, followed by discussing the solubility rules and states of the substances involved. The tutorial then demonstrates how to form the complete ionic equation by splitting strong electrolytes into their ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge conservation and balanced atoms in the final equation.

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

• Identify spectator ions

• Balance the molecular equation

• Write the complete ionic equation

• Determine solubility

Why is silver sulfate an exception in solubility rules?

• It is highly soluble

• It is insoluble

• It forms a gas

• It is a strong acid

What is the charge of a nitrate ion?

• 1+

• 2+

• 1-

• 2-

Which ions are not split in a net ionic equation?

• Gas ions

• Liquid ions

• Aqueous ions

• Solid ions

What is the charge of the copper ion in copper(II) sulfate?

• 1+

• 2+

• 2-

• 1-

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 to form the net ionic equation?

• Spectator ions

• Reactant ions

• Product ions

• All ions

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

• Zero

• Variable

• Positive

• Negative

What ensures the net ionic equation is balanced?

• Equal number of ions

• Equal number of molecules

• Equal number of electrons

• Equal number of atoms

What is the final product of the reaction between silver nitrate and copper(II) sulfate?

• Copper nitrate

• Silver sulfate

• Copper sulfate

• Silver nitrate