Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between iron(III) chloride and ammonium phosphide. It begins with balancing the molecular equation, then applies solubility rules to determine the states of the substances involved. The tutorial proceeds to split strong electrolytes into ions to form the complete ionic equation. Finally, it identifies and removes spectator ions to derive the net ionic equation, ensuring both atoms and charges are balanced.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

• Identify spectator ions

Which of the following compounds is generally insoluble?

• Ammonium chloride

• Iron phosphate

• Sodium chloride

• Potassium nitrate

What is the state of ammonium chloride in the reaction?

• Liquid

• Gas

• Aqueous

• Solid

What is the role of solubility rules in this process?

• To determine the molecular formula

• To identify spectator ions

• To predict the state of compounds

• To balance the equation

What do you do after writing the complete ionic equation?

• Balance the charges

• Write the molecular equation

• Determine the solubility

• Identify and remove spectator ions

Which ions are considered spectator ions in this reaction?

• Iron ions

• Phosphate ions

• Chloride ions

• Ammonium ions

Why is it important to remove spectator ions?

• To identify the precipitate

• To balance the equation

• To simplify the equation

• To determine solubility

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

• Variable

• Zero

• Negative

• Positive

What is the charge balance in the net ionic equation?

• 3+ and 3-

• 4+ and 4-

• 1+ and 1-

• 2+ and 2-

What is the final step in deriving the net ionic equation?

• Removing spectator ions

• Writing the molecular equation

• Balancing charges

• Balancing atoms