Understanding Displacement Reactions
A displacement reaction occurs when a more reactive metal displaces a less reactive metal from its compound. This is based on the activity series of metals.
The Activity Series
The activity series lists metals in order of their reactivity, with the most reactive at the top. A metal higher on the list will displace a metal lower on the list from its compound.
The Relevant Part of the Activity Series
Here's a simplified portion of the activity series that's relevant to your question:
* Most reactive: Lithium (Li), Potassium (K), Sodium (Na), Calcium (Ca), Magnesium (Mg), Aluminum (Al), Zinc (Zn), Iron (Fe), Nickel (Ni), Tin (Sn), Lead (Pb), Copper (Cu), Mercury (Hg), Silver (Ag), Platinum (Pt), Gold (Au)
The Reaction with Aluminum Nitrate
Aluminum nitrate (Al(NO₃)₃) contains aluminum (Al) ions. To displace aluminum, a metal needs to be higher on the activity series.
Metals that will react:
* Zinc (Zn): Zinc is higher on the activity series than aluminum, so it will displace aluminum from aluminum nitrate.
* Iron (Fe): Iron is also higher on the activity series than aluminum, so it will displace aluminum from aluminum nitrate.
The Reactions
* Zinc: Zn(s) + 2Al(NO₃)₃(aq) → 2Al(s) + 3Zn(NO₃)₂(aq)
* Iron: Fe(s) + 2Al(NO₃)₃(aq) → 2Al(s) + 3Fe(NO₃)₂(aq)
Key takeaway: Metals higher on the activity series than aluminum can displace aluminum from its compounds.
