Net Ionic Equations and Spectator Ions

This video tutorial explains how to write a balanced net ionic equation for the reaction between magnesium chloride (MgCl2) and potassium phosphate (K3PO4). It begins by balancing the molecular equation, then discusses the solubility of the compounds involved. The tutorial proceeds to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the charge is balanced and the equation is correct.

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

• Identify spectator ions

• Write the complete ionic equation

• Balance the molecular equation

• Determine the solubility of compounds

Why are chlorides generally considered soluble?

• They react with most metals

• They form strong covalent bonds

• They dissolve easily in water

• They are always in gaseous state

Which group of elements makes phosphates soluble?

• Noble gases

• Group 2 elements

• Group 1 elements

• Transition metals

What is the charge of a magnesium ion in the complete ionic equation?

• 1+

• 2+

• 3+

• 0

How many chloride ions are present in the complete ionic equation for MgCl2?

• Six

• Eight

• Four

• Two

What is the role of spectator ions in a chemical reaction?

• They participate in the reaction

• They change the state of the reaction

• They remain unchanged and do not participate

• They alter the charge balance

Which ions are removed to form the net ionic equation?

• Only anions

• Only cations

• Spectator ions

• All ions

What ensures the net ionic equation is balanced?

• Equal number of atoms on both sides

• Both equal number of atoms and charges

• Equal number of molecules on both sides

• Equal charges on both sides

What is the charge balance in the final net ionic equation?

• 2+ and 2-

• 0+ and 0-

• 3+ and 3-

• 6+ and 6-

What is the state of magnesium phosphate in the net ionic equation?

• Aqueous

• Gaseous

• Liquid

• Solid