Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between sodium phosphate and copper(II) nitrate. It begins with balancing the molecular equation and identifying the states of each compound based on solubility rules. The tutorial then demonstrates how to split strong electrolytes into their ions to form the complete ionic equation. Finally, it shows how to identify and remove spectator ions to derive the net ionic equation, ensuring charge and atom balance.

What are the correct coefficients for balancing the molecular equation of sodium phosphate and copper(II) nitrate?

• 1, 2, 3, 4

• 3, 1, 2, 6

• 2, 3, 6, 1

• 1, 1, 1, 1

Which of the following compounds is insoluble in water?

• Copper(II) phosphate

• Copper(II) nitrate

• Sodium nitrate

• Sodium phosphate

What is the charge of the sodium ion in the complete ionic equation?

• 3-

• 0

• 1+

• 2+

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

• 6

• 8

• 4

• 2

What is the role of spectator ions in a chemical reaction?

• They participate in the reaction.

• They change the state of the reactants.

• They remain unchanged and do not participate in the reaction.

• They form the precipitate.

Which ions are removed as spectator ions in this reaction?

• Copper and nitrate ions

• Copper and phosphate ions

• Sodium and nitrate ions

• Sodium and phosphate ions

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

• 1+

• 3+

• 2-

• 0

Why is the copper(II) phosphate not split into ions in the net ionic equation?

• It is an aqueous solution.

• It is a solid precipitate.

• It is a liquid.

• It is a gas.

What is the significance of balancing charges in a net ionic equation?

• To ensure the reaction is spontaneous.

• To maintain electrical neutrality.

• To increase the reaction rate.

• To change the state of the reactants.

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

• Balancing the molecular equation.

• Identifying the precipitate.

• Writing the complete ionic equation.

• Ensuring charge and atom balance.