* Redox Reactions: These reactions involve the transfer of electrons between reactants. One reactant loses electrons (oxidation) while the other gains electrons (reduction).
* Single Displacement Reactions: In these reactions, a more reactive element displaces a less reactive element from a compound. This displacement occurs because the more reactive element has a stronger tendency to lose electrons (oxidation) and the less reactive element has a stronger tendency to gain electrons (reduction).
Example:
Consider the reaction of zinc with copper(II) sulfate:
Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)
* Zinc (Zn) is more reactive than copper (Cu).
* Zinc loses electrons and becomes oxidized, forming Zn²⁺ ions.
* Copper(II) ions (Cu²⁺) gain electrons and become reduced, forming copper metal (Cu).
Key takeaway: Because single displacement reactions involve a change in oxidation states of the elements involved, they are always redox reactions.
