Net Ionic Equations and Spectator Ions

The video tutorial explains how to write and balance net ionic equations using the example of sodium hydroxide and ammonium bromide. It covers balancing the molecular equation, determining the states of compounds based on solubility rules, forming the complete ionic equation, identifying spectator ions, and deriving the net ionic equation. The tutorial emphasizes the importance of charge conservation and atom balance in the final equation.

What is the first step in balancing a net ionic equation?

• Identify spectator ions

• Determine the solubility of compounds

• Balance the molecular equation

• Write the complete ionic equation

Which of the following is true about compounds with sodium and ammonium ions?

• They are insoluble in water

• They are weak electrolytes

• They are very soluble in water

• They form precipitates

What state is typically assigned to ammonia in a net ionic equation?

• Gas

• Liquid

• Aqueous

• Solid

What is the purpose of splitting strong electrolytes into ions?

• To determine solubility

• To balance the net ionic equation

• To write the complete ionic equation

• To identify the molecular equation

Why don't we split gases or liquids in net ionic equations?

• They do not dissociate into ions

• They are weak electrolytes

• They are spectator ions

• They are always insoluble

What are spectator ions?

• Ions that are insoluble

• Ions that form precipitates

• Ions that do not change during the reaction

• Ions that participate in the reaction

Which ions are typically crossed out in a net ionic equation?

• Ions that are insoluble

• Spectator ions

• Ions that are weak electrolytes

• Ions that form gases

What must be conserved in a balanced net ionic equation?

• Both mass and charge

• Only charge

• Only mass

• Neither mass nor charge

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

• Zero

• Depends on the reaction

• Negative

• Positive

If NH3 were aqueous, how would it be represented in the net ionic equation?

• As a liquid

• As a gas

• As a solid

• As an aqueous solution