Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between strontium nitrate and potassium carbonate. It begins with balancing the molecular equation, followed by determining the states of each substance using solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and crossed out to derive the net ionic equation. The video concludes with a review of the balanced net ionic equation, ensuring both atoms and charges are balanced.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Split strong electrolytes into ions

Which of the following compounds is generally insoluble?

• Sodium compounds

• Potassium compounds

• Carbonates

• Nitrates

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

• To balance the molecular equation

• To predict the solubility of compounds

• To identify spectator ions

• To determine the charge of ions

What happens to the solid formed in a precipitation reaction?

• It falls to the bottom as a precipitate

• It evaporates

• It remains as ions

• It dissolves in water

What is the charge of a strontium ion in the complete ionic equation?

• 2-

• 1-

• 2+

• 1+

Which group on the periodic table does potassium belong to?

• Group 4

• Group 3

• Group 2

• Group 1

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

• Gaseous products

• Solid precipitates

• Liquid water

• Aqueous ions

What are spectator ions?

• Ions that participate in the reaction

• Ions that do not change during the reaction

• Ions that form a precipitate

• Ions that are insoluble

Which ions are removed to form the net ionic equation?

• Reactant ions

• Product ions

• Spectator ions

• Precipitate ions

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

• Variable

• Zero

• Negative

• Positive