Reactivity of The Metal
Zinc is a strong reducing agent with a standard redox potential of -0.76 V. Pure zinc tarnishes rapidly in air, eventually forming a passive layer of basic zinc carbonate, Zn5(OH)6CO3. The reaction of zinc with water is prevented by the passive layer. When this layer is penetrated by acids such as hydrochloric acid and sulfuric acid the reaction proceeds with the evolution of hydrogen gas.
- Zn(s) + 2H+ (aq) → Zn2+ (aq) + H2 ↑
The hydrogen ion is reduced by accepting an electron from the reducing agent. The zinc metal is oxidised. Amalgamation with mercury, as in the Jones reductor also destroys the passive layer. Zinc reacts with alkalis as with acids. It reacts directly with oxidising non-metals such as chalcogens and halogens to form binary compounds.
Read more about this topic: Zinc Compounds
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