No skyscraper would stand without this metal. Manganese is the invisible hero of the steel mill. Every ton of steel contains it because it removes harmful oxygen and sulfur. The result is a strong, resilient metal used to build bridges, rails, and cars.
But manganese works far beyond steelmaking. It hides inside the batteries that power your remote control. It sits in every green leaf — photosynthesis cannot happen without it. And your own body needs tiny doses of manganese for healthy bones and normal metabolism.
In pure form, manganese is a silvery-gray brittle metal. It is fairly hard (6 on the Mohs scale) but breaks more easily than iron. In air it develops a thin oxide film. Its superpower is the ability to exist in many oxidation states — from -3 to +7. That is why manganese compounds come in different colors, from pale pink Mn²⁺ to deep purple MnO₄⁻.
Manganese is the fourth most abundant metal in Earth's crust. It is mined mainly in South Africa, Australia, and Gabon.
Metallic manganese has low toxicity, but prolonged inhalation of its dust or oxide fumes causes manganism — a severe neurological disorder with tremor, muscle rigidity, and impaired coordination, resembling Parkinson's disease. Potassium permanganate is a strong oxidizer that causes skin burns. Welding steel requires proper ventilation to protect against manganese aerosols.
95% of all mined manganese goes into steel. Without it, every bridge, rail, and skyscraper would be brittle and unreliable.
Photosynthesis is impossible without manganese. It is part of the enzyme that splits water and releases oxygen. Every breath you take exists thanks to manganese.
Potassium permanganate KMnO₄ is so intensely purple that even a 0.001% solution is visible to the naked eye.
Manganese dioxide MnO₂ has been used in batteries since 1866. It is one of the oldest materials for electrical power sources.
The crystal structure of manganese contains 58 atoms in its unit cell — an absolute record among all metals.
Cave artists 17,000 years ago used manganese oxide as a black pigment for rock paintings in the Lascaux cave.
| Isotope | Mass (u) | Abundance | Half-life | Decay |
|---|---|---|---|---|
55Mn | 54.938045 | 100.00% | stable | — |
Reduction of manganese dioxide