Net Ionic Equations and Spectator Ions

The video tutorial guides viewers through writing a balanced net ionic equation for the reaction between calcium chloride and copper(II) sulfate. It begins with balancing the molecular equation, identifying the states of substances based on solubility rules, and splitting strong electrolytes into ions. The tutorial then explains how to form complete and net ionic equations by removing spectator ions. Finally, it verifies the balanced net ionic equation, ensuring charge and atom balance.

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

• Write the complete ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

According to solubility rules, which of the following is generally soluble?

• Calcium sulfate

• Phosphates

• Chlorides

• Carbonates

What is the state of calcium chloride in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

What is the charge of the calcium ion in the reaction?

• 1-

• 2+

• 1+

• 2-

What is the charge of the sulfate ion?

• 2-

• 2+

• 1-

• 1+

Which ion is considered a spectator ion in this reaction?

• Sulfate ion

• Copper ion

• Calcium ion

• Chloride ion

Which of the following is not split into ions in the net ionic equation?

• Sulfate ion

• Chloride ion

• Copper ion

• Calcium sulfate

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

• They are ignored

• They are doubled

• They are crossed out

• They are combined

What is the net charge of the reactants in the net ionic equation?

• 0

• 2-

• 2+

• 1+

What ensures that the net ionic equation is balanced?

• Equal charges on both sides

• Equal number of ions

• Equal number of molecules

• Equal number of atoms