Zinc

About Zinc

Zinc occupies an awkward spot at the end of the d-block — its 3d¹⁰ shell is filled and stays that way, so you don't see the variable oxidation states or colorful complexes that define real transition-metal chemistry. Zn²⁺ is what you almost always get, and that consistency is exactly what makes it useful. The d¹⁰ configuration also means Zn²⁺ is a Lewis acid without redox baggage, which is why nature picked it as the catalytic centre for over 300 enzymes — carbonic anhydrase moves a CO₂ to bicarbonate every microsecond using a single Zn²⁺ holding a hydroxide. Industrially the dominant use is galvanizing: dipping steel into a 460 °C zinc bath gives a metallurgically bonded coating that protects the underlying iron sacrificially because zinc sits below iron in the activity series (E° = -0.76 V vs -0.44 V). Once a scratch exposes the steel, the zinc corrodes preferentially. The same principle drives zinc-air button cells (1.4 V from Zn + ½O₂ → ZnO) and the original Volta pile.