There are four basic types of reactions. They are:
- Synthesis reaction
- Decomposition reaction
- Simple displacement reaction
- Double displacement reaction
Synthesis reaction:
- The combination or synthesis reaction occurs when two or more elements or compounds combine chemically to form a new product.
- The general representation for this reaction is:
X + Y → XY
- Synthesis reaction could be explained with the following example:
Nitrogen and hydrogen combine to form ammonia.
Here, two different elements, nitrogen, and hydrogen combine chemicals, and a new, single product with different properties than the reactants is formed i.e, ammonia.
Decomposition reaction:
- In a decomposition reaction, one chemical substance is decomposed into one or more products.
- In the given reaction, copper carbonate(CuCO3) when heated is decomposed into copper oxide(CuO) and carbon dioxide(CO2).
Single displacement reaction:
- According to the reactivity series, the metals that come first are more reactive than the ones that are below them.
- More reactive metals can displace less reactive metals from their compounds.
- Single displacement reactions take the form:
AB + C → A + CB - Example:
- According to the reactivity series, zinc(Zn) is more reactive than copper(Cu) as zinc comes first in the series.
- When zinc is added to copper sulfate (CuSO4) solution, copper is replaced by zinc and forms zinc sulfate (ZnSO4).
- The color of the solution changes from blue to colorless during the reaction.
Double displacement reaction:
- A double displacement reaction is a type of reaction in which two reactants exchange ions to form two new compounds.
- Double displacement reactions take the form:
AB + CD → AD + CB - Example:
In the given reaction, chloride ion is acquired by sodium from barium chloride and sulfate ion is taken by barium from sodium chloride.