Net Ionic Equations and Reactions

This video tutorial explains how to write a balanced net ionic equation for the reaction between magnesium metal and iron(II) sulfate. It covers balancing the molecular equation, determining the states of substances, splitting strong electrolytes into ions, and identifying spectator ions. The tutorial concludes with deriving the net ionic equation, ensuring charge and atom balance.

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

• Identify spectator ions

• Split compounds into ions

• Determine the states of substances

• Balance the molecular equation

What is the state of magnesium in the reaction?

• Solid

• Gas

• Liquid

• Aqueous

Which of the following is soluble in water?

• None of the above

• Iron

• Iron (II) sulfate

• Magnesium

What charge does the sulfate ion carry?

• 2-

• 1+

• 2+

• 1-

Which ions are considered spectator ions in this reaction?

• Sulfate ions

• Magnesium ions

• None

• Iron ions

What is the charge of the magnesium ion in the products?

• 2-

• 1-

• 2+

• 1+

What is the net ionic equation for the reaction?

• Mg + FeSO4 → MgSO4 + Fe

• Mg + Fe^2+ → Mg^2+ + Fe

• Fe^2+ + SO4^2- → FeSO4

• Mg^2+ + SO4^2- → MgSO4

How is charge conservation demonstrated in the net ionic equation?

• Charges are only on the reactant side

• Charges are only on the product side

• Charges are equal on both sides

• Charges are not conserved

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

• Balancing charges

• Balancing atoms

• All of the above

• Removing spectator ions

Why is it important to ensure atom balance in a net ionic equation?

• To satisfy the law of conservation of mass

• To make the equation look neat

• To ensure the reaction occurs

• To identify spectator ions