Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (b) What is the net ionic equation that describes this reaction?

Key Concepts

Net Ionic Equations

A net ionic equation represents the actual chemical species that participate in a reaction, omitting spectator ions that do not change during the reaction. It focuses on the ions and molecules that undergo a chemical change, providing a clearer picture of the reaction's essence. This is particularly useful in reactions involving soluble ionic compounds in aqueous solutions.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, leading to changes in oxidation states. In this context, zinc is oxidized (loses electrons) while copper ions are reduced (gain electrons). Understanding the roles of oxidizing and reducing agents is crucial for writing the correct net ionic equation for the reaction.

Solubility Rules

Solubility rules help predict whether a compound will dissolve in water, which is essential for determining the reactants and products in aqueous reactions. For instance, copper(II) nitrate is soluble, while silver may form an insoluble compound with certain anions. Knowing these rules aids in identifying which ions remain in solution and which precipitate out during the reaction.