Antimony (Sb): properties, history, and uses

Properties

Antimony displays a metallic luster and is relatively brittle at room temperature. Chemically it most commonly exhibits +3 and +5 oxidation states and forms a variety of oxides, sulfides and halides. The principal ore is stibnite (antimony sulfide), from which the element is traditionally extracted. As a group 15 element it shares chemical relationships with arsenic and bismuth.

Occurrence and extraction

Antimony is found in mineral deposits worldwide, often as stibnite (Sb2S3). Historically important deposits have been worked in several regions, and modern production is centered where large, accessible ores exist. Recovery typically involves concentration of the ore followed by roasting or chemical reduction to produce metallic antimony or antimony compounds.

Uses and applications

Antimony and its compounds have diverse industrial uses. Major applications include:

• Flame retardants: certain antimony oxides are used with halogenated materials to inhibit combustion.
• Alloys: small additions of antimony harden lead and tin alloys, improving battery grids, solder and pewter.
• Electronics and optics: antimony compounds are used in some semiconductor and infrared detector materials.

Because it modifies mechanical and electronic properties, antimony remains important in niche metallurgical and chemical roles.

History, safety and notable facts

Antimony-bearing minerals were used by ancient cultures—most famously as the eye cosmetic kohl. Its distinctive name reflects a long record of human use. Modern handling recognizes health and environmental risks: inhalation or prolonged exposure to certain antimony compounds can be harmful, so occupational and environmental controls limit releases and exposure. In the periodic table antimony occupies group 15 and period 5, between arsenic and tellurium, and is usually classified as a metalloid rather than a true metal.