Net Ionic Equations and Charge Conservation

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between potassium dichromate and silver nitrate. It begins with balancing the molecular equation, then discusses solubility rules to identify the precipitate, silver dichromate. The tutorial proceeds to break down the compounds into ions for the complete ionic equation and removes spectator ions to derive the net ionic equation. The video concludes by ensuring charge conservation and summarizing the process.

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

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

• Identify the spectator ions

How do you balance the number of potassium atoms in the molecular equation?

• Add a coefficient of 2

• Add a coefficient of 1

• Add a coefficient of 3

• Add a coefficient of 4

Which of the following compounds is generally insoluble?

• Potassium dichromate

• Potassium nitrate

• Silver nitrate

• Silver dichromate

What happens to silver dichromate in the reaction?

• It forms a gas

• It dissolves in water

• It forms a solid precipitate

• It remains as ions

What is the charge of a potassium ion?

• 2-

• 2+

• 1+

• 1-

In the complete ionic equation, which ions are not split apart?

• Silver dichromate

• Nitrate ions

• Potassium ions

• Silver ions

What are spectator ions?

• Ions that are insoluble

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that participate in the reaction

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

• 0

• 1+

• 2-

• 2+

Why is it important to ensure charge conservation in net ionic equations?

• To balance the number of atoms

• To ensure the reaction is neutral

• To determine solubility

• To identify spectator ions

Which ion is sometimes written first in net ionic equations for aesthetic reasons?

• Spectator ion

• Neutral ion

• Positive ion

• Negative ion