Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between silver nitrate (AgNO3) and sodium iodide (NaI). It begins with balancing the molecular equation and identifying the states of each substance based on solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation, ensuring charge and atom balance. The video concludes with a review of the net ionic equation, emphasizing the conservation of charge and atoms.

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

• Identify spectator ions

• Write the complete ionic equation

• Balance the molecular equation

• Determine the solubility of compounds

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

• Lead sulfate

• Calcium carbonate

• Sodium chloride

• Silver iodide

What state symbol is used for a compound that does not dissolve in water?

• (g)

• (s)

• (aq)

• (l)

What is the charge of a silver ion in the reaction?

• 1-

• 2-

• 2+

• 1+

Which ion is not split into its components in the complete ionic equation?

• Sodium ion

• Nitrate ion

• Silver iodide

• Iodide ion

What is the purpose of identifying spectator ions?

• To determine solubility

• To simplify the net ionic equation

• To calculate molar mass

• To balance the equation

Which ions are considered spectator ions in this reaction?

• Silver and iodide ions

• Sodium and nitrate ions

• Silver and nitrate ions

• Sodium and iodide ions

What is conserved in a balanced net ionic equation?

• Only mass

• Only charge

• Both mass and charge

• Neither mass nor charge

How many silver atoms are present on each side of the net ionic equation?

• Two

• One

• Three

• None

What is the final product formed in the reaction between silver nitrate and sodium iodide?

• Sodium iodide

• Silver iodide

• Silver chloride

• Sodium nitrate