Net Ionic Equations and Ions

This video tutorial explains how to balance net ionic equations, using ammonium phosphate and zinc nitrate as examples. It covers balancing the molecular equation, applying solubility rules to determine states, forming the complete ionic equation, and deriving the net ionic equation by removing spectator ions. The tutorial emphasizes the importance of conserving charge and atoms in the final balanced equation.

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

• Determine the solubility of compounds

• Identify spectator ions

• Write the net ionic equation

• Balance the molecular equation

Which of the following compounds is generally insoluble?

• Ammonium phosphate

• Zinc nitrate

• Zinc phosphate

• Ammonium nitrate

What is the charge of the ammonium ion?

• 3-

• 1+

• 1-

• 2+

How many ammonium ions are present in the complete ionic equation?

• 3

• 6

• 2

• 4

What is the charge of the zinc ion in the reaction?

• 3+

• 1-

• 2+

• 1+

Why don't we split solids in net ionic equations?

• They have no charge

• They do not dissolve in water

• They are spectator ions

• They are not involved in the reaction

What is the purpose of removing spectator ions?

• To balance the charges

• To determine solubility

• To simplify the equation

• To identify the reactants

What is the net charge on both sides of a balanced net ionic equation?

• Positive

• Negative

• Varies

• Zero

What must be conserved in a balanced net ionic equation?

• Neither mass nor charge

• Mass only

• Charge only

• Both mass and charge

In a net ionic equation, which ion is typically written first?

• Negative ion

• Spectator ion

• Positive ion

• Neutral compound