Net Ionic Equations and Ion Charges

The video tutorial explains how to write the net ionic equation for the reaction between iron(III) chloride and sodium hydroxide. It begins with balancing the molecular equation, then assigns states to the compounds based on solubility rules. The tutorial proceeds to split the soluble compounds into their respective ions, using the periodic table to determine ion charges. Finally, it identifies and removes spectator ions to derive the net ionic equation, highlighting the formation of a precipitate.

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

• Identify spectator ions

• Write the balanced molecular equation

• Determine the solubility of compounds

• Split compounds into ions

What is the state of sodium hydroxide in the reaction?

• Liquid

• Solid

• Aqueous

• Gas

Which of the following is often insoluble and forms a precipitate?

• Iron(III) chloride

• Sodium hydroxide

• Sodium chloride

• Iron(III) hydroxide

How can you determine the charge of an ion using the periodic table?

• By identifying the element's period

• By finding the element's mass

• By checking the group number

• By looking at the atomic number

What is the charge of the hydroxide ion?

• +1

• -1

• +2

• -2

What is the charge of the iron ion in this reaction?

• +3

• +2

• +1

• +4

What do you do with the solid compounds when writing the complete ionic equation?

• Split them into ions

• Convert them to gases

• Leave them as they are

• Dissolve them in water

What are spectator ions?

• Ions that participate in the reaction

• Ions that form a precipitate

• Ions that do not change during the reaction

• Ions that are gases

Which ions are removed to form the net ionic equation?

• All ions

• Only positive ions

• Spectator ions

• Only negative ions

What is the final product of the net ionic equation for this reaction?

• NaCl(aq)

• Fe(OH)3(s)

• NaOH(aq)

• FeCl3(aq)