What is the Difference Between Complete Ionic and Net Ionic Equation?

The main difference between a complete ionic and a net ionic equation lies in the inclusion or exclusion of spectator ions. Here's a breakdown of the differences:

• Complete Ionic Equation: This type of equation shows all the ions in the solution, including both the ions that participate in the chemical reaction and the spectator ions that do not take part in the reaction. The complete ionic equation gives the electrical charge of each chemical species and is used to describe reactions that occur in aqueous solutions.
• Net Ionic Equation: This type of equation only shows the chemical species that are involved in a reaction, while the spectator ions are excluded. The net ionic equation is balanced for mass and charge and lists the state of matter of all species. It provides a simplified view of the reactions taking place, focusing on the species actively involved in the chemical process.

In summary:

• Complete ionic equations include all species in an ionic reaction, including spectator ions.
• Net ionic equations only show the species involved in the chemical reaction, excluding spectator ions.

Comparative Table: Complete Ionic vs Net Ionic Equation

The main difference between a complete ionic equation and a net ionic equation lies in the inclusion of spectator ions. Here is a table summarizing the differences:

To convert a complete ionic equation to a net ionic equation, you need to identify the spectator ions and remove them from the complete ionic equation.