Net Ionic Equations and Reactions

This video tutorial explains how to write a balanced net ionic equation for the reaction between silver fluoride (AgF) and sodium bromide (NaBr). It covers balancing the molecular equation, determining the solubility of compounds using a solubility table, and identifying the formation of a precipitate. The tutorial also demonstrates how to split strong electrolytes into ions to form the complete ionic equation and how to identify and remove spectator ions to derive the net ionic equation. The video concludes with a check for balanced charges and atoms.

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

• Write the complete ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

Which of the following is true about sodium compounds in water?

• They remain as molecules

• They dissolve and split into ions

• They form a solid precipitate

• They are always insoluble

What does the 's' in the solubility table indicate?

• Saturated

• Soluble

• Solid

• Suspended

What happens to AgBr in the reaction between AgF and NaBr?

• It forms a solid precipitate

• It forms a gas

• It dissolves in water

• It remains as ions

What type of reaction occurs when AgF reacts with NaBr?

• Combustion reaction

• Precipitation reaction

• Acid-base reaction

• Redox reaction

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

• 2+

• 1+

• 1-

• 0

Which ions are considered spectator ions in this reaction?

• Sodium and bromide ions

• Silver and fluoride ions

• Sodium and fluoride ions

• Silver and bromide ions

What is the net charge on both sides of the net ionic equation?

• Positive

• Negative

• Zero

• Variable

Why are spectator ions removed from the net ionic equation?

• They are insoluble

• They form a precipitate

• They change the charge balance

• They do not participate in the reaction

What ensures that the net ionic equation is balanced?

• Equal number of solids

• Equal number of gases

• Equal number of molecules

• Equal number of atoms and charges