Lecture Notes: Net Ionic Equations

Presenter

• Name: Robert Smith
• Affiliation: New River Community College's Academic Assistance

Topic: Net Ionic Equations

Overview

• Focus on writing the net ionic equation for a given chemical reaction.

Steps for Writing Net Ionic Equations

1. Identify Aqueous Compounds

   • Split aqueous compounds into their respective ions or complex ions.
   • Leave solids and liquids in their original form; they do not split into ions.

2. Break Down Reactants & Products

   • Reactants Side
     • Lead (Pb) from nitrate (NO3)
     • Potassium (K) from iodine (I)
   • Products Side
     • Potassium (K) from nitrate (NO3)

3. Rewrite Ionic Equations

   • Example:
     • Lead (Pb) with a 2+ charge, aqueous
     • Two nitrate ions (NO3) with a -1 charge, aqueous
     • Two potassium ions (K) with a +1 charge, aqueous
     • Two iodine ions (I) with a -1 charge, aqueous

4. Identify Spectator Ions

   • Common ions on both sides of the equation that cancel each other out.
   • Spectator Ions:
     • Nitrates (NO3)
     • Potassium (K)

5. Formulate the Net Ionic Equation

   • Cancel out spectator ions.
   • Net Ionic Equation:
     • Lead ion (Pb) + 2 Iodine ions (I) → Lead iodide (PbI2)

Important Notes

• Charges:
  • Ensure charges balance out in the net ionic equation.
  • Lead (Pb) has a 2+ charge, iodine (I) has a -1 charge, but two iodines result in no net charge for lead iodide (PbI2).

Conclusion

• The net ionic equation isolates the essence of the reaction, showing only the ions that participate directly in the chemical change.