Net Ionic Equations and Spectator Ions

The video tutorial explains how to balance a net ionic equation for beryllium iodide and copper sulfate. It begins with balancing the molecular equation, then discusses solubility rules and identifies copper iodide as a precipitate. The tutorial proceeds to form the complete ionic equation, highlighting the role of strong electrolytes. Spectator ions are identified and removed to derive the net ionic equation. The tutorial concludes by verifying the balance of atoms and charges in the final equation.

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

• 1-

• 2-

• 1+

• 2+

How many copper ions are needed to balance the charge in copper one sulfate?

• One

• Four

• Three

• Two

Which compound is identified as a precipitate in the reaction?

• Copper one iodide

• Copper one sulfate

• Beryllium iodide

• Sulfate ion

What is the state of copper one iodide in the reaction?

• Solid

• Liquid

• Gas

• Aqueous

What is the purpose of splitting strong electrolytes into ions?

• To increase reaction speed

• To change the state of compounds

• To identify spectator ions

• To balance the equation

Which ions are considered spectator ions in this reaction?

• Beryllium and sulfate ions

• Copper and iodide ions

• Only beryllium ions

• Only sulfate ions

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

• Positive

• Negative

• Zero

• Varies

Why do we not split solids in net ionic equations?

• They are spectator ions

• They are already balanced

• They do not dissolve in water

• They are not reactive

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

• Balancing charge

• Balancing atoms

• Writing states

• Removing spectator ions

What is the convention regarding writing coefficients of one in chemical equations?

• Write them only for gases

• Write them only for solids

• Never write them

• Always write them