Silane

Silane (SiH4) is the silicon analogue of methane. It is a colorless, highly reactive gas at room temperature, and the molecule adopts a tetrahedral geometry with silicon at the center bonded to four hydrogen atoms.

Physically, silane has a boiling point of approximately −111.8 °C, and at ambient conditions it exists as a highly flammable gas. It forms explosive mixtures with air and is considered pyrophoric in air; it reacts with oxidizers and hydrolyzes in water to yield silica and hydrogen.

Production and handling of silane involve several routes. Industrially, it is prepared by the reduction of silicon tetrachloride (SiCl4) with metal hydrides, or by processes that generate SiH4 from silicon compounds. In laboratories and in some on-site industrial settings, silane can be produced by hydrolysis of magnesium silicide (Mg2Si). Silane is stored in compressed gas cylinders and is typically handled under inert or controlled atmospheric conditions to prevent ignition.

Uses of silane are dominated by its role as a silicon source in chemical vapor deposition and related processes. It serves as a precursor for depositing silicon-containing films, including amorphous and polycrystalline silicon, silicon dioxide in some contexts, and silicon nitride in others. It is also used in the synthesis of silicon nanoparticles and as a dopant or source of silicon in certain semiconductor manufacturing steps.

Safety and handling notes are essential: silane is highly flammable and can ignite spontaneously in air; appropriate gas detection, ventilation, and containment are required. Storage and use should follow relevant regulations, with emphasis on avoiding contact with oxidizers and sources of ignition.