Net Ionic Equations and Spectator Ions

The video tutorial explains how to write the net ionic equation for the reaction between calcium chloride (CaCl2) and silver nitrate (AgNO3). It begins by balancing the molecular equation, then assigns states to each substance based on solubility rules. The tutorial proceeds to split strong electrolytes into their respective ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, emphasizing the importance of simplifying to the lowest ratio.

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

• Identify the spectator ions

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

Which of the following compounds is insoluble in water?

• Nitrate ion

• Silver chloride

• Silver nitrate

• Calcium chloride

What is the state of silver chloride in the reaction?

• Gas

• Aqueous

• Liquid

• Solid

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

• 2-

• 2+

• 1+

• 1-

Which ion is always 1- in charge?

• Silver ion

• Chloride ion

• Calcium ion

• Nitrate ion

Which of the following is a strong electrolyte in the reaction?

• Calcium chloride

• Silver ion

• Silver chloride

• Water

Which ions are considered spectator ions in this reaction?

• Chloride and calcium ions

• Nitrate and silver ions

• Silver and chloride ions

• Calcium and nitrate ions

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

• They form a precipitate

• They change their charge

• They are removed from the equation

• They are included in the final equation

What is the final net ionic equation for the reaction?

• Ag+ + Cl- → AgCl

• CaCl2 + 2AgNO3 → 2AgCl + Ca(NO3)2

• 2Ag+ + 2Cl- → 2AgCl

• Ca2+ + 2NO3- → Ca(NO3)2

Why is it important to write the net ionic equation in the lowest ratio?

• To balance the charges

• To make the equation more accurate

• To ensure all ions are included

• To simplify calculations