No, copper metal will not react with zinc nitrate solution.
Understanding Chemical Reactivity
The interaction between metals and solutions containing other metal ions is governed by their relative chemical reactivities. To determine if a reaction will occur, chemists refer to the activity series (also known as the reactivity series) of metals. This series ranks metals based on their tendency to lose electrons and form positive ions, essentially their ability to react.
The Role of the Activity Series
- Higher Reactivity: Metals positioned higher in the activity series are more reactive. They have a greater tendency to oxidize (lose electrons) and can displace metals lower in the series from their compounds.
- Lower Reactivity: Metals lower in the series are less reactive and cannot displace metals higher in the series.
- Predicting Reactions: If a metal is added to a solution containing ions of a less reactive metal, a single displacement reaction can occur, where the more reactive metal displaces the less reactive one. For a more detailed understanding of this concept, you can explore resources on single displacement reactions and the activity series of metals.
Why No Reaction Occurs Between Copper and Zinc Nitrate
Based on the activity series, copper is less reactive than zinc. This crucial difference dictates that copper metal is unable to displace zinc ions from a zinc nitrate solution.
- Copper's Position: Copper is relatively low on the activity series compared to zinc.
- Zinc's Position: Zinc is higher on the activity series than copper, indicating it is more reactive.
Therefore, when copper metal is introduced into an aqueous solution of zinc nitrate, no chemical change will take place. The copper atoms will not give up their electrons to the zinc ions because zinc ions are more stable in solution than copper ions would be in this context.
Expected Reaction Type (If Reactive)
If a reaction were to occur, it would be a redox reaction in the form of a single displacement reaction. For example, if zinc metal were placed in a copper nitrate solution, zinc would displace copper. However, with copper and zinc nitrate, the reverse is not possible:
Cu(s) + Zn(NO₃)₂(aq) → No Reaction
Reactivity Comparison: Copper vs. Zinc
The table below summarizes the key differences in reactivity between copper and zinc:
| Metal | Relative Reactivity | Common Behaviors & Reactions |
|---|---|---|
| Zinc | More Reactive | Reacts with acids to produce hydrogen gas, readily displaces less reactive metals (like copper). |
| Copper | Less Reactive | Does not typically react with non-oxidizing acids, cannot displace more reactive metals (like zinc). |
This difference in reactivity is why zinc is often used as a sacrificial anode in cathodic protection to prevent corrosion of iron, while copper is chosen for wiring due to its resistance to oxidation in many environments.
Practical Implications
Understanding the reactivity of metals is vital for various applications, including:
- Predicting Chemical Outcomes: It allows chemists and engineers to predict whether a mixture of substances will react, preventing unexpected or dangerous situations.
- Corrosion Prevention: Knowledge of reactivity helps in selecting appropriate materials for specific environments to prevent corrosion.
- Metallurgy and Refining: These principles are fundamental in extracting metals from their ores and in refining processes.
- Material Selection: Guiding the choice of materials for manufacturing, ensuring stability and desired performance.
In conclusion, the chemical inactivity of copper with zinc nitrate is a direct consequence of copper being less reactive than zinc, a principle well-established by the activity series of metals.
