Which of the following combinations will result in a single displacement reaction?

Question

BlackTom AI · Accepted Answer

To determine which option leads to a single displacement reaction, we first recall the activity (reactivity) series: a metal can displace another metal from a compound only if it is more reactive than the metal in that compound.

Option A: A magnesium nitrate solution and zinc metal. Here, zinc metal would have to displace magnesium from Mg2+ in Mg(NO3)2, but zinc is less reactive than magnesium. Therefore, this setup does not produce a displacement reaction.

Option B: Copper metal and a magnesium nitrate solution. Copper is less reactive than magnesium, so it cannot displace magnesium from Mg2+ in Mg(NO3)2. No single displacement occurs.

Option C: Copper metal and magnesium metal. This is simply an exchange between two metals with no compound to react, so no displacement reaction happens.

Option D: Magnesium metal and a zinc nitrate solution. Magnesium is more reactive than zinc, so Mg can displace Zn2+ from Zn(NO3)2, yielding Zn metal and Mg(NO3)2. This is a classic single displacement scenario.

Option E: A zinc nitrate solution and copper metal. Since copper is less reactive than zinc, copper cannot displace zinc from Zn2+ in Zn(NO3)2, so no reaction occurs.

Putting it together, only Option D describes a valid single displacement reaction, where a more reactive metal (Mg) replaces a less reactive metal (Zn) in its salt.

Which of the following combinations will result in a single displacement reaction?

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