The Reaction:
* Zinc (Zn) + Oxygen (O2) → Zinc oxide (ZnO)
What Happens:
1. Oxidation: Zinc loses electrons (gets oxidized) and becomes a positively charged zinc ion (Zn²⁺).
2. Reduction: Oxygen gains electrons (gets reduced) and becomes negatively charged oxide ions (O²⁻).
3. Formation of Zinc Oxide: The positively charged zinc ions and negatively charged oxide ions attract each other and form a stable compound called zinc oxide (ZnO).
Characteristics of the Reaction:
* Exothermic: The reaction releases heat, making the metal hot.
* Formation of a white coating: Zinc oxide is a white, powdery substance that forms a protective layer on the surface of the zinc metal. This layer prevents further oxidation and protects the zinc from corrosion.
* Rate of reaction: The reaction rate depends on factors like temperature, surface area, and the presence of moisture.
Uses of Zinc Oxide:
Zinc oxide is a versatile compound with numerous applications, including:
* Sunblock: Used as an active ingredient in sunscreens due to its ability to absorb UV rays.
* Pigment: Used as a white pigment in paints, rubber, and plastics.
* Medicinal uses: Found in ointments and creams for treating skin conditions like diaper rash and acne.
* Industrial uses: Used in various industrial processes, including manufacturing rubber, adhesives, and ceramics.
In Summary: The reaction between zinc and oxygen results in the formation of zinc oxide, a white protective layer that prevents further corrosion. This reaction is exothermic and has many practical applications.
