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:

1. Potassium (K)
2. Sodium (Na)
3. Calcium (Ca)
4. Magnesium (Mg)
5. Aluminium (Al)
6. Carbon (C)
7. Zinc (Zn)
8. Iron (Fe)
9. Tin (Sn)
10. Lead (Pb)
11. Hydrogen (H)
12. Copper (Cu)
13. Silver (Ag)
14. Gold (Au)
15. Platinum (Pt)