Net Ionic Equations and Solubility

This video tutorial explains how to write the net ionic equation for the reaction between calcium and iron(II) sulfate. It begins with an introduction to the concept of net ionic equations and the importance of balancing molecular equations. The video then discusses how to determine the states of substances involved, using solubility rules to identify precipitates. The tutorial proceeds to demonstrate how to write complete and net ionic equations, emphasizing the identification of spectator ions. Finally, it concludes with a discussion on balancing atoms and charges in the equation, ensuring both are equal on both sides.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of products

• Split strong electrolytes into ions

Which of the following is generally soluble in water?

• Carbonates

• Sulfates

• Iron

• Calcium

What is the state of calcium sulfate in the reaction?

• Liquid

• Aqueous

• Gas

• Solid

What is the charge of the iron ion in iron(II) sulfate?

• 1+

• 2+

• 3+

• 2-

Why can't calcium be split into ions in the complete ionic equation?

• It is a non-metal

• It is a solid

• It is a gas

• It is a liquid

What do you call ions that do not change during the reaction?

• Reactants

• Products

• Spectator ions

• Catalysts

In this reaction, why is the complete ionic equation the same as the net ionic equation?

• The reaction is not balanced

• The products are gases

• All ions are soluble

• There are no spectator ions

What is the net charge of the reactants in the balanced net ionic equation?

• 0

• 2+

• 1+

• 1-

What ensures that a net ionic equation is correctly balanced?

• Equal number of electrons on both sides

• Equal number of atoms on both sides

• Equal number of molecules on both sides

• Equal number of ions on both sides

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

• Balancing the molecular equation

• Identifying the spectator ions

• Ensuring the charges are balanced

• Checking the solubility of products