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Silicon dioxide
General
Other names	Silica see text
Molecular formula	SiO2
Molar mass	60.1 g/mol
Appearance	white or colourless solid (when pure)
CAS number	[14808-60-7]
Properties
Density and phase	2.6 g/cm3, solid
Solubility in water	insoluble
Melting point	1610 °C
Boiling point	2230 °C
Structure
Coordination geometry	tetrahedral
Crystal structure	various
Hazards
MSDS	External MSDS
EU classification
NFPA 704
R-phrases	R42 R43 R49
S-phrases	S22 S36 S37 S45 S53
Flash point	non-flammable
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Related compounds
Other anions	Silicon disulfide
Other cations	Carbon dioxide Germanium dioxide Tin(IV) oxide Lead(IV) oxide
Related compounds	Silicic acid
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references

The chemical compound silicon dioxide, also known as silica, is the oxide of silicon, chemical formula SiO₂.

It is found in nature in several forms, including quartz and opal. In fact, silica has 17 crystalline forms (see Nomenclature of Silica). Also, many forms of life include silica structures (Biogenic Silica), including microorganisms such as diatoms, plants such as horsetail, and animals such as hexactinellid sponges.

It is manufactured in several forms including glass (in colorless high purity form called fused silica), synthetic amorphous silica and silica gel (used e.g. as desiccants in brand new clothes and leather goods). Silica, with alumina, is a crucial ingredient in clay and allows for the development of an interlocking crystal matrix after firing in earthenware, stoneware and porcelain ceramic processes. Silica is a major ingredient of Portland cement. The ceramic re-entry heat protection tiles mounted on the bottom side of the Space Shuttles are made mostly of silica, as are the firebricks used in steel processing.

The most common constituent of sand in inland continental settings and non-tropical coastal settings is silica, usually in the form of quartz because the considerable hardness of this mineral resists erosion. However, the composition of sand varies according to local rock sources and conditions.

Inhaling crystalline silica dust can lead to silicosis.

Variants found in high-pressure impacts are coesite and stishovite.

Silica is also used as a food additive, primarily as a flow agent in powdered foods, or to absorb water. See the ingredients list for Burger King.

The chemical stability of silicon dioxide and its electrical insulation properties are a major reason why silicon is the dominant material for semiconductor devices. It is used to separate the active regions of devices and to form insulating surfaces.

Chemistry

Silicon dioxide can be formed when silicon is exposed to oxygen (or air) at extremely high temperatures. This can occasionally happen naturally in fires, or when lightning strikes onto sand.

Silicon dioxide is attacked by hydrofluoric acid (HF). HF is used to remove or pattern silicon dioxide in the semiconductor industry.

Reference

• R. K. Iler, The Chemistry of Silica (ISBN 047102404X)

External links

• International Chemical Safety Card 0807 (Tridymite)
• International Chemical Safety Card 0808 (Quartz)
• International Chemical Safety Card 0809 (Cristobalite)
• NIOSH Pocket Guide to Chemical Hazards (amorphous)
• NIOSH Pocket Guide to Chemical Hazards (crystalline, as respirable dust)

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