Net Ionic Equations and Spectator Ions

This video tutorial explains how to write balanced net ionic equations, using iron(III) sulfide and hydrobromic acid as examples. It covers balancing the molecular equation, identifying states of substances, and splitting strong electrolytes into ions to form the complete ionic equation. The tutorial also discusses forming the net ionic equation by removing spectator ions and provides tips on handling weak acids and solids.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Split all compounds into ions

Which of the following is generally insoluble unless bonded to group 1 elements?

• Nitrates

• Chlorides

• Sulfates

• Sulfides

What is the state of hydrobromic acid in water?

• Solid

• Gas

• Weak acid

• Strong acid

Which compound is split into ions in the complete ionic equation?

• Fe2S3

• H2S

• FeBr3

• HBr

What is the purpose of splitting strong electrolytes into ions?

• To balance the equation

• To identify spectator ions

• To determine solubility

• To form the complete ionic equation

What are spectator ions?

• Ions that do not participate in the reaction

• Ions that form precipitates

• Ions that are weak acids

• Ions that are insoluble

Why are there no spectator ions in this reaction?

• All substances are the same

• All ions are insoluble

• All ions are weak acids

• All substances are different

What should not be split in net ionic equations?

• Strong acids

• Weak electrolytes

• Soluble salts

• Gases

What is the net ionic equation for the reaction between Fe2S3 and HBr?

• Fe2S3 + 6H+ → 2Fe3+ + 3H2S

• Fe2S3 + 6HBr → 2FeBr3 + 3H2S

• Fe2S3 + 6Br- → 2Fe3+ + 3H2S

• Fe2S3 + 6HBr → 2Fe3+ + 6Br- + 3H2S

What should you watch out for when writing net ionic equations?

• Splitting all compounds

• Balancing only reactants

• Not splitting solids

• Ignoring weak acids