Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for a reaction involving nickel(II) nitrate and ammonium phosphate. It begins with balancing the molecular equation, followed by determining the states of compounds using 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. Finally, the video ensures that both atoms and charges are balanced in the net ionic equation.

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

• Balance the molecular equation

• Split compounds into ions

• Identify spectator ions

• Determine the solubility of compounds

According to solubility rules, which of the following ions generally forms soluble compounds?

• Phosphate

• Nitrate

• Sulfide

• Carbonate

What is the state of ammonium compounds in aqueous solutions?

• Gas

• Liquid

• Solid

• Aqueous

What is the purpose of splitting strong electrolytes into ions?

• To determine solubility

• To form the complete ionic equation

• To balance charges

• To identify the molecular equation

Which ions are removed to form the net ionic equation?

• Only anions

• Spectator ions

• All ions

• Only cations

What are spectator ions?

• Ions that form precipitates

• Ions that are insoluble

• Ions that do not change during the reaction

• Ions that participate in the reaction

How do you verify that a net ionic equation is balanced?

• Verify that both atoms and charges are balanced

• Check the solubility of compounds

• Count the number of spectator ions

• Ensure the number of molecules is equal

What is the net charge of a balanced net ionic equation?

• Positive

• Negative

• Zero

• Depends on the reaction

What is the charge balance in the reactants of a net ionic equation?

• Varies with each reaction

• Positive

• Negative

• Neutral