Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between sodium chloride and lead(II) acetate. It covers balancing the molecular equation, determining the states of compounds, and applying solubility rules. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation, identify and cross out spectator ions, and finalize the net ionic equation with balanced charges.

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

• Identify spectator ions

• Determine the states of substances

• Balance the molecular equation

• Split strong electrolytes into ions

How do you balance the chloride ions in the molecular equation?

• Add a coefficient of one in front of sodium chloride

• Add a coefficient of one in front of lead(II) acetate

• Add a coefficient of two in front of sodium chloride

• Add a coefficient of two in front of lead(II) acetate

Which of the following is a characteristic of sodium compounds?

• They are usually solid

• They are usually soluble

• They are usually gaseous

• They are usually insoluble

What is the state of PbCl2 in the reaction?

• Aqueous

• Liquid

• Gaseous

• Solid

What do you do with strong electrolytes in the complete ionic equation?

• Ignore them

• Convert them to solids

• Split them into their ions

• Leave them as compounds

Why are solids not split into ions in the complete ionic equation?

• They are already balanced

• They are spectator ions

• They are not part of the reaction

• They do not dissolve in water

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 gaseous

Which ions are crossed out as spectator ions in this reaction?

• Lead ions

• Chloride ions

• Sodium ions

• Acetate ions

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

• Variable

• Positive

• Negative

• Zero

What must be true for the atoms in the net ionic equation?

• They must be unbalanced

• They must be balanced

• They must be deficient

• They must be in excess