Net Ionic Equations and Spectator Ions

This video tutorial guides viewers through writing the balanced net ionic equation for the reaction between nickel(II) carbonate (NiCO3) and hydrochloric acid (HCl). It begins with balancing the molecular equation, followed by determining the states of the substances involved. The tutorial then explains 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. The video concludes by ensuring the final equation is balanced in terms of both charge and atoms.

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

• Identify spectator ions

• Split strong electrolytes into ions

• Determine the states of substances

• Balance the molecular equation

Why is it necessary to put a 2 in front of HCl in the molecular equation?

• To balance the nickel atoms

• To balance the oxygen atoms

• To balance the chlorine atoms

• To balance the hydrogen atoms

What is the state of hydrochloric acid in the reaction?

• Aqueous

• Gas

• Liquid

• Solid

Which of the following is generally insoluble?

• Nitrates

• Chlorides

• Hydroxides

• Carbonates

What do we do with strong electrolytes in the complete ionic equation?

• Leave them as molecules

• Combine them into solids

• Convert them to gases

• Split them into ions

What are spectator ions?

• Ions that participate in the reaction

• Ions that are gases

• Ions that do not change during the reaction

• Ions that form precipitates

What is the purpose of removing spectator ions?

• To increase the reaction rate

• To balance the molecular equation

• To identify the states of substances

• To simplify the net ionic equation

How do we ensure the net ionic equation is balanced?

• By checking the temperature

• By checking the charge and atom balance

• By checking the pressure

• By checking the number of molecules

What is the charge balance in the net ionic equation?

• One plus in reactants, one plus in products

• Zero in reactants, zero in products

• Two plus in reactants, two plus in products

• Three plus in reactants, three plus in products

What is the final step in confirming the net ionic equation?

• Checking the solubility

• Checking the temperature

• Counting the atoms

• Measuring the pressure