Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between copper(II) sulfate and strontium nitrate. It begins with balancing the molecular equation, followed by determining the states of substances using solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Finally, it shows how to derive the net ionic equation by removing spectator ions, ensuring that both atoms and charges are balanced.

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

• Balance the molecular equation

• Identify spectator ions

• Determine the solubility of compounds

• Write the complete ionic equation

Which of the following is generally soluble in water?

• Hydroxides

• Sulfates with exceptions

• Carbonates

• Phosphates

What state symbol is used for a substance that is dissolved in water?

• (s)

• (l)

• (g)

• (aq)

What is the role of solubility rules in writing net ionic equations?

• To calculate reaction rates

• To identify spectator ions

• To determine the states of substances

• To balance the equation

What is the charge on the sulfate ion?

• 1+

• 2-

• 1-

• 2+

Which of the following is a solid precipitate in the reaction between CuSO4 and Sr(NO3)2?

• Copper sulfate

• Strontium sulfate

• Strontium nitrate

• Copper nitrate

Which ion is considered a spectator ion in the reaction between CuSO4 and Sr(NO3)2?

• Sulfate ion

• Nitrate ion

• Strontium ion

• Copper ion

What happens to spectator ions in a net ionic equation?

• They are included in the equation

• They are crossed out

• They are combined with other ions

• They are converted to solids

What is the net charge of the products in a balanced net ionic equation?

• Positive

• Negative

• Depends on the reactants

• Zero

Why is it important to verify the conservation of charge in a net ionic equation?

• To ensure the equation is balanced

• To identify spectator ions

• To predict the reaction products

• To determine solubility