Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between potassium hydroxide and iron(III) bromide. It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The tutorial then 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 by verifying the balance of charges and atoms in the final net ionic equation.

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

• Determine solubility

• Balance the molecular equation

• Write the complete ionic equation

• Identify spectator ions

How do you balance the number of bromine atoms in the molecular equation?

• Add a coefficient of 3 in front of FeBr3

• Add a coefficient of 2 in front of FeBr3

• Add a coefficient of 3 in front of KBr

• Add a coefficient of 2 in front of KBr

Which of the following compounds is generally soluble?

• Iron(III) hydroxide

• Silver chloride

• Potassium bromide

• Calcium carbonate

What is the state of iron(III) hydroxide in the reaction?

• Aqueous

• Solid

• Gas

• Liquid

What is the purpose of writing a complete ionic equation?

• To determine solubility

• To identify the precipitate

• To balance charges

• To split strong electrolytes into ions

Which ions are considered spectator ions in this reaction?

• Iron and bromide ions

• Potassium and hydroxide ions

• Iron and hydroxide ions

• Potassium and bromide ions

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

• Positive

• Negative

• Zero

• Variable

Why do we not split solids in the net ionic equation?

• They are not electrolytes

• They are already balanced

• They do not dissolve in water

• They are not reactive

What is the charge of the iron ion in the net ionic equation?

• 1+

• 2+

• 3+

• 4+

What ensures that the net ionic equation is balanced?

• Equal number of molecules

• Equal number of atoms

• Equal number of electrons

• Equal number of ions