Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between nitric acid (HNO3) and aluminum hydroxide (AlOH3). It begins with balancing the molecular equation, then discusses the states of each substance involved. The tutorial proceeds to form the complete ionic equation by splitting strong electrolytes into ions, and finally derives the net ionic equation by removing spectator ions. The video concludes with a summary of the balanced net ionic equation, ensuring that both charge and atom count are balanced.

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

• Write the complete ionic equation

• Balance the molecular equation

• Determine the states of substances

• Identify spectator ions

How many nitrates are needed to balance the molecular equation for HNO3 and Al(OH)3?

• One

• Two

• Four

• Three

What is the state of nitric acid in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

Which of the following is insoluble in water?

• Aluminum hydroxide

• Water

• Aluminum nitrate

• Nitric acid

What is the charge of the nitrate ion?

• 2-

• 1+

• 2+

• 1-

In the complete ionic equation, which ions are not split apart?

• Aqueous ions

• Solid compounds

• Gaseous molecules

• Liquid substances

What are spectator ions?

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that participate in the reaction

• Ions that are gases

Which ions are removed to form the net ionic equation?

• Product ions

• Reactant ions

• All ions

• Spectator ions

What must be balanced in a net ionic equation?

• Neither atoms nor charges

• Both atoms and charges

• Only the charges

• Only the atoms

What is the final step in verifying a balanced net ionic equation?

• Check the solubility

• Ensure the equation is balanced

• Identify the products

• Determine the reaction type