Spectator Ions and Net Ionic Equations

The video tutorial explains how to write the net ionic equation for the reaction between calcium nitrate and sodium phosphate. It begins with balancing the molecular equation, followed by determining the states of each substance using solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions and write the complete ionic equation. Finally, it shows how to identify and remove spectator ions to derive the net ionic equation.

What is the first step in writing a 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 soluble in water?

• Calcium phosphate

• Silver chloride

• Sodium nitrate

• Lead sulfate

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

• 1+

• 2-

• 2+

• 3+

How many nitrate ions are present in the balanced molecular equation?

• Four

• Eight

• Two

• Six

What is the charge of the phosphate ion?

• 2-

• 4-

• 1-

• 3-

Why don't we split solids in net ionic equations?

• They are liquids

• They dissolve completely

• They are gases

• They remain intact in the solution

What is the purpose of identifying spectator ions?

• To balance the equation

• To calculate molarity

• To simplify the net ionic equation

• To determine solubility

Which ions are considered spectator ions in this reaction?

• Calcium and nitrate ions

• Calcium and phosphate ions

• Sodium and nitrate ions

• Sodium and phosphate ions

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

• Sodium nitrate

• Calcium phosphate

• Calcium nitrate

• Sodium phosphate

What is the significance of the net ionic equation?

• It highlights the formation of precipitates

• It shows all compounds in the reaction

• It provides the balanced molecular equation

• It lists all spectator ions