Ionic Compounds and Reactions

The video tutorial explains how to balance net ionic equations, starting with balancing the molecular equation for calcium hydroxide and aluminum sulfate. It covers the states of substances, highlighting solubility rules and the formation of precipitates. The tutorial then demonstrates how to split strong electrolytes into ions for the complete ionic equation and identifies spectator ions. The net ionic equation is finalized, ensuring charge and atom balance. The video concludes with a summary of the process and key points.

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

• Determine the states of substances

• Split strong electrolytes into ions

• Balance the molecular equation

• Identify spectator ions

How many hydroxide ions are needed to balance the equation?

• Six

• Eight

• Four

• Two

Which of the following is considered a strong base?

• Aluminum sulfate

• Calcium hydroxide

• Calcium sulfate

• Aluminum hydroxide

What state is assigned to calcium sulfate in the reaction?

• Solid

• Gas

• Liquid

• Aqueous

What charge does a calcium ion have in the complete ionic equation?

• 1+

• 2-

• 2+

• 3+

Which group on the periodic table is aluminum found in?

• Group 2

• Group 1

• Group 13

• Group 17

What is the charge of a sulfate ion?

• 2-

• 1-

• 2+

• 1+

What happens to spectator ions in the net ionic equation?

• They are included in the equation

• They are removed from the equation

• They form a precipitate

• They change their charge

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

• 1+

• 2-

• 2+

• 0

What is the final step in ensuring the net ionic equation is correct?

• Balancing the atoms

• Checking the solubility

• Ensuring charge balance

• Identifying the products