Question

What reaction, if any, occurs if a piece of copper metal is placed in an aqueous solution containing iron(II) sulfate?

Short answer

No reaction occurs when a piece of copper is placed in an aqueous solution of iron(II) sulfate.

Step-by-step solution

Understanding the Reactivity Series

Identify the position of the given metals in the reactivity series. The series from most reactive to least reactive generally goes like this: \( K > Na > Ca > Mg > Al > Zn > Fe > Ni > Sn > Pb > H > Cu > Ag > Au \). Thus, we can see that iron (Fe) is above copper (Cu) in the reactivity series.

Applying the Concept of the Reactivity Series

According to the reactivity series, a metal can displace another metal from its aqueous solution if it is more reactive. In this scenario, copper (Cu) is less reactive than Iron (Fe). Therefore, copper will not be able to displace iron from the iron(II) sulfate solution.

Conclusion

Based on the reactivity series, no reaction will occur when a piece of copper is placed in an aqueous solution of iron(II) sulfate. This is because copper is less reactive compared to iron.

Key concepts

Displacement Reactions

Displacement reactions are an intriguing type of chemical reaction where a more reactive metal displaces a less reactive metal from its compound. This is firmly backed by the reactivity series, which organizes metals based on their ability to kick out other metals from solutions. For a displacement reaction to occur, it's all about how metals stack up against each other in terms of reactivity.
Simply put, you have a competition between two metals. The winner, or the more reactive one, will send the other packing by taking its place in the compound. For instance, if you try to mix magnesium metal with copper sulfate solution, magnesium kicks copper out of the compound and forms magnesium sulfate. This happens because magnesium is more reactive than copper.

• The more reactive metal displaces the less reactive one.
• This reactivity is determined by the position in the reactivity series.
• No reaction occurs if the attempting metal is less reactive.

Understanding this concept is key in predicting whether or not a reaction will take place when different metals are put together in solutions.

Reactivity of Metals

The reactivity of metals is at the heart of displacement reactions. Metals do not all react with the same gusto; some metals are eager to participate in reactions, while others are less so.
The reactivity series is like the leaderboard for metals, arranging them from most reactive to least. This sequence helps us predict which metals can replace others in compounds. Potassium, for instance, sits at the top, ready to react enthusiastically, while gold lounges at the bottom, reluctant to react with anything.

• The higher a metal is in the reactivity series, the more reactive it is.
• Metals like potassium, calcium, and sodium are very reactive.
• Metals like silver, gold, and platinum are far less reactive and often used in jewelry for their resistance to tarnishing.

Thus, when you encounter metals in reactions, consider their place in the reactivity series to predict potential outcomes.

Iron(II) Sulfate Solution

Iron(II) sulfate solution is a common player when discussing reactions involving iron, but what's in this solution that makes it special?
Iron(II) sulfate, also known as ferrous sulfate, is a greenish compound frequently used in laboratories and industries. In solutions, iron(II) ions are present, eager to react with more reactive metals.

• Iron(II) sulfate solution contains \( Fe^{2+} \) ions, ready to participate in reactions.
• These ions can be displaced by any metal higher than iron in the reactivity series.
• Ions remain stable if copper is introduced, due to copper's lower reactivity.

So when a less reactive metal like copper enters the scene, nothing happens, as copper cannot displace the more reactive iron.