The Reaction:
Copper (Cu) is more reactive than silver (Ag). This means copper can displace silver from its compound. The copper atoms lose electrons and become copper(II) ions (Cu²⁺), while silver ions (Ag⁺) gain electrons and become silver atoms (Ag).
The Chemical Equation:
```
Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂) (aq) + 2Ag(s)
```
What You Observe:
* Silver crystals: You will see shiny, silvery crystals forming on the surface of the copper. These are the silver atoms that were displaced from the solution.
* Blue solution: The solution will turn blue as copper(II) nitrate (Cu(NO₃)₂) forms.
Explanation:
1. Copper atoms lose electrons: Copper atoms are oxidized, meaning they lose electrons to form copper(II) ions (Cu²⁺).
2. Silver ions gain electrons: Silver ions (Ag⁺) are reduced, meaning they gain electrons to form silver atoms (Ag).
3. Displacement: The more reactive copper displaces the less reactive silver from the silver nitrate solution.
Net Ionic Equation:
The net ionic equation focuses on the species that are directly involved in the reaction:
```
Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
```
This reaction demonstrates the reactivity series of metals and how a more reactive metal can displace a less reactive metal from its compound.
