Copper and Nitrate Ion Reactions

This video tutorial explains how to write the net ionic equation for the reaction between copper and nitric acid. It begins with the balanced molecular equation, assigns states to the compounds, and then splits the soluble compounds into ions. The total ionic equation is written, and spectator ions are identified and removed to derive the net ionic equation. The tutorial concludes with a cleaned-up version of the net ionic equation.

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

• Identify spectator ions

• Write the balanced molecular equation

• Split compounds into ions

• Determine the states of compounds

Which state is assigned to copper in the reaction with nitric acid?

• Liquid

• Gas

• Solid

• Aqueous

What is the state of water in this reaction under normal conditions?

• Solid

• Liquid

• Gas

• Plasma

What is the charge of the nitrate ion (NO3) in this reaction?

• 1+

• 2+

• 1-

• 2-

What is the charge of copper in the copper(II) nitrate compound?

• 1-

• 2-

• 2+

• 1+

How many hydrogen ions (H+) are present in the total ionic equation?

• Two

• Four

• Three

• Five

Which compound is split into ions in the total ionic equation?

• Nitrogen dioxide

• Water

• Copper

• Nitric acid

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Hydrogen ions

• Copper ions

• Water molecules

What happens to the nitrate ions during the formation of the net ionic equation?

• They are added

• They are removed

• They remain unchanged

• They change charge

What is the final product of the net ionic equation for copper and nitric acid?

• Copper nitrate

• Copper hydroxide

• Copper oxide

• Copper chloride