Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between magnesium and copper(II) chloride. It covers the steps of balancing the molecular equation, identifying the states of substances, splitting strong electrolytes into ions, and crossing out spectator ions to derive the net ionic equation. The tutorial emphasizes the conservation of mass and charge throughout the process.

What type of reaction is occurring between magnesium and copper(II) chloride?

• Single displacement

• Decomposition

• Synthesis

• Double displacement

What is the state of magnesium in the reaction?

• Gas

• Solid

• Aqueous

• Liquid

Which of the following substances will dissociate into ions in the reaction?

• Copper

• Magnesium

• Copper(II) chloride

• All of the above

What is the charge on the copper ion in the complete ionic equation?

• 2+

• 1+

• 0

• 3+

How many chloride ions are present in the reactants of the complete ionic equation?

• Four

• Three

• Two

• One

What are spectator ions in a chemical reaction?

• Ions that are only present in the reactants

• Ions that are only present in the products

• Ions that do not change during the reaction

• Ions that participate in the reaction

Which ions are removed to form the net ionic equation?

• All ions

• Magnesium ions

• Chloride ions

• Copper ions

What is conserved in a balanced net ionic equation?

• Only mass

• Only charge

• Both mass and charge

• Neither mass nor charge

What is the final net ionic equation for the reaction?

• Mg^2+ + Cu -> Mg + Cu^2+

• Mg + 2Cl^- -> Mg^2+ + 2Cl^-

• Mg + Cu^2+ -> Mg^2+ + Cu

• Mg + CuCl2 -> MgCl2 + Cu

Why is it important to ensure charge conservation in a net ionic equation?

• To ensure the reaction occurs

• To balance the equation

• To comply with the law of conservation of mass

• To comply with the law of conservation of charge