Using displacement reactions
1. Metal Displacement
A more reactive metal replaces a less reactive metal from its salt solution.
Example: solid zinc + copper sulfate solution → zinc sulfate solution + solid copper
The solution may lose color, and a new metal may appear on the surface.
Commonly used to compare the reactivity of metals.
2. Halogen Displacement
A more reactive halogen pushes out a less reactive halogen from its compound.
Example: chlorine gas + potassium bromide solution → potassium chloride solution + bromine
Halogen reactions show strong color changes like orange-brown bromine appearing.
Useful for understanding halogen reactivity patterns.
3. Indicators of a Displacement Reaction
Color change in the solution
Formation of a new solid metal
Original metal dissolves
Temperature increase during the reaction
Appearance of a new element such as copper or bromine
4. Importance of Displacement Reactions
Helps identify which metals or halogens are more reactive
Used in metal extraction and purification processes
Important in understanding the chemistry of batteries
Clearly demonstrates oxidation and reduction in action
5. Easy Redox Explanation
The metal that replaces another metal loses electrons.
The metal that gets pushed out gains electrons.
One is oxidized, the other is reduced — both happen together.
6. Predicting If a Reaction Will Happen
A displacement reaction will occur only if the solid element is more reactive than the element in the compound.
If the solid element is less reactive, no reaction happens.
Because of this, displacement reactions help build reactivity order for metals and halogens.