Understanding Redox Reactions
* Oxidation: Loss of electrons
* Reduction: Gain of electrons
* Redox reaction: A reaction involving both oxidation and reduction.
Activity Series
The reactivity of metals is summarized in the activity series. Metals higher on the series are more likely to lose electrons (oxidize) and displace metals lower in the series.
* More Active Metals: Higher in the activity series.
* Less Active Metals: Lower in the activity series.
The Key Players
* Silver (Ag): Less active than copper.
* Copper (Cu): More active than silver.
The Likely Reaction
Since copper is more active than silver, it will be oxidized (lose electrons) and displace silver from a solution containing silver ions:
Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
Explanation:
* Copper (Cu) is oxidized: It loses two electrons and becomes a copper(II) ion (Cu²⁺).
* Silver ions (Ag⁺) are reduced: They gain electrons and become solid silver (Ag).
Important Note: The specific ions present in the solution will determine if this reaction is actually possible. If the solution only contains copper ions, for example, the reaction wouldn't occur.
