Understanding Displacement Reactions
A displacement reaction occurs when a more reactive metal takes the place of a less reactive metal in a compound. This fundamental concept in chemistry follows a predictable pattern based on the reactivity series of metals.
Definition: A displacement reaction is a chemical process where a more reactive element displaces a less reactive element from its compound.
Example: The reaction between copper and silver nitrate (Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag) demonstrates how copper, being more reactive than silver, displaces it from silver nitrate.
Highlight: The reactivity series plays a crucial role in predicting whether a displacement reaction will occur. Metals higher in the series will displace metals lower in the series.
Vocabulary: The general equation format A + BC → AC + B represents displacement reactions, where:
- A is the more reactive metal
- BC is the compound containing the less reactive metal
- AC is the new compound formed
- B is the displaced metal
The reactivity series, from most to least reactive, includes:
- Potassium (K)
- Sodium (Na)
- Calcium (Ca)
- Magnesium (Mg)
- Aluminium (Al)
- Carbon (C)
- Zinc (Zn)
- Iron (Fe)
- Tin (Sn)
- Lead (Pb)
- Hydrogen (H)
- Copper (Cu)
- Silver (Ag)
- Gold (Au)
- Platinum (Pt)
