Net Ionic Equations and Spectator Ions

The video tutorial explains how to write the balanced net ionic equation for the reaction between iron(III) nitrate and ammonium hydroxide. It begins by balancing the molecular equation, then discusses the solubility and states of the substances involved. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions and concludes by deriving the net ionic equation by removing spectator ions, ensuring charge conservation and atom balance.

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

• Write the complete ionic equation

• Identify spectator ions

• Balance the molecular equation

• Assign states of matter

How do you balance the number of nitrate ions in the molecular equation?

• Adjust the coefficient of ammonium nitrate

• Add more ammonium hydroxide

• Add more iron(III) nitrate

• Adjust the coefficient of iron(III) hydroxide

Which of the following compounds is generally insoluble?

• Sulfates

• Ammonium compounds

• Nitrates

• Hydroxides

What is the state of iron(III) hydroxide in the reaction?

• Gas

• Liquid

• Solid

• Aqueous

What is the charge of the iron ion in the complete ionic equation?

• 3+

• 4+

• 2+

• 1+

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Ammonium ions

• Hydroxide ions

• Iron ions

What is the purpose of identifying spectator ions?

• To determine solubility

• To simplify the net ionic equation

• To balance the equation

• To calculate molarity

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

• 0

• 3+

• 2+

• 1+

Why is it important to ensure the net charge is zero in the net ionic equation?

• To determine solubility

• To confirm the reaction is balanced

• To identify spectator ions

• To calculate the reaction rate

What is the final product formed in the net ionic equation?

• Iron(III) nitrate

• Ammonium hydroxide

• Ammonium nitrate

• Iron(III) hydroxide