Al2o3 H2o Al Oh 3

Al2o3 H2o Al Oh 3

Oxide of silicon

Silicon dioxide
Sample of silicon dioxide.jpg

A sample of silicon dioxide

IUPAC name

Silicon dioxide

Other names

  • Quartz
  • Silica
  • Silicic oxide
  • Silicon(Four) oxide
  • Crystalline silica
  • Pure Silica
  • Silicea
  • Silica sand

CAS Number

  • 7631-86-9
  • CHEBI:30563
  • 22683
ECHA InfoCard 100.028.678
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EC Number
  • 231-545-4
E number E551 (acidity regulators, …)

Gmelin Reference

  • C16459
MeSH Silicon+dioxide


  • 24261
RTECS number
  • VV7565000
  • ETJ7Z6XBU4

CompTox Dashboard

  • DTXSID1029677
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  • InChI=1S/O2Si/c1-three-2check



Chemical formula

Molar mass 60.08 thousand/mol
Appearance Transparent solid (Amorphous) White/Whitish Yellow (Pulverisation/Sand)
Density two.648 (α-quartz), 2.196 (baggy) k·cm−3
Melting point ane,713 °C (3,115 °F; i,986 K) (baggy)[1]

: 4.88

Boiling signal 2,950 °C (v,340 °F; 3,220 K)[ane]

Magnetic susceptibility (χ)

Thermal conductivity 12 (|| c-axis), half-dozen.eight (⊥ c-axis), ane.4 (am.) W/(m⋅K)[i]

: 12.213

Refractive alphabetize (n

1.544 (o), one.553 (eastward)[1]

: 4.143
NFPA 704
(fire diamond)




(US health exposure limits):

PEL (Permissible)

TWA 20 mppcf (lxxx mg/thouiii/%SiO2) (amorphous)[2]

REL (Recommended)

TWA six mg/thou3

Ca TWA 0.05 mg/miii

IDLH (Firsthand danger)

3000 mg/chiliadthree

Ca [25 mg/grand3
(cristobalite, tridymite); 50 mg/1000three
Related compounds

Related diones

Carbon dioxide

Germanium dioxide
Tin dioxide
Atomic number 82 dioxide

Related compounds

Silicon monoxide

Silicon sulfide


Std molar


42 J·mol−1·Yard−i

Std enthalpy of


−911 kJ·mol−1

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Northverify (what is

Infobox references

Chemic compound

Silicon dioxide, as well known as
silica, is an oxide of silicon with the chemic formula
, most commonly found in nature as quartz and in various living organisms.[5]
In many parts of the world, silica is the major elective of sand. Silica is i of the near complex and most arable families of materials, existing as a compound of several minerals and as a constructed product. Notable examples include fused quartz, fumed silica, silica gel, opal and aerogels. It is used in structural materials, microsystem electronics (as an electric insulator), and equally components in the food and pharmaceutical industries.



Structural motif found in α-quartz, but also found in almost all forms of silicon dioxide

Typical subunit for depression pressure silicon dioxide

Relationship between refractive alphabetize and density for some SiOii

In the majority of silicates, the silicon atom shows tetrahedral coordination, with four oxygen atoms surrounding a primal Si atom (see 3-D Unit Cell). Thus, SiOtwo
forms 3-dimensional network solids in which each silicon atom is covalently bonded in a tetrahedral manner to 4 oxygen atoms. In contrast, COii
is a linear molecule. The starkly different structures of the dioxides of carbon and silicon are a manifestation of the double bail dominion.

has several dean crystalline forms, just they nigh e’er take the same local structure effectually Si and O. In α-quartz the Si–O bond length is 161 pm, whereas in α-tridymite it is in the range 154–171 pm. The Si–O–Si angle likewise varies betwixt a depression value of 140° in α-tridymite, up to 180° in β-tridymite. In α-quartz, the Si–O–Si bending is 144°.[8]


Alpha quartz is the almost stable form of solid SiO2
at room temperature. The high-temperature minerals, cristobalite and tridymite, have both lower densities and indices of refraction than quartz. The transformation from α-quartz to beta-quartz takes place abruptly at 573 °C. Since the transformation is accompanied by a significant alter in volume, it can easily induce fracturing of ceramics or rocks passing through this temperature limit.[ix]
The high-force per unit area minerals, seifertite, stishovite, and coesite, though, have higher densities and indices of refraction than quartz.[x]
Stishovite has a rutile-like structure where silicon is 6-coordinate. The density of stishovite is 4.287 g/cmiii, which compares to α-quartz, the densest of the depression-force per unit area forms, which has a density of ii.648 thou/cmiii.[11]
The divergence in density tin can be ascribed to the increment in coordination as the half-dozen shortest Si–O bond lengths in stishovite (iv Si–O bond lengths of 176 pm and two others of 181 pm) are greater than the Si–O bond length (161 pm) in α-quartz.[12]
The change in the coordination increases the ionicity of the Si–O bond.[13]
More importantly, whatever deviations from these standard parameters institute microstructural differences or variations, which correspond an arroyo to an amorphous, vitreous, or glassy solid.

Faujasite silica, another polymorph, is obtained by dealumination of a low-sodium, ultra-stable Y zeolite with combined acid and thermal treatment. The resulting product contains over 99% silica, and has loftier crystallinity and specific surface area (over 800 m2/g). Faujasite-silica has very high thermal and acid stability. For example, it maintains a high degree of long-range molecular gild or crystallinity even afterwards boiling in concentrated hydrochloric acid.[xiv]

Molten SiOii

Molten silica exhibits several peculiar concrete characteristics that are similar to those observed in liquid water: negative temperature expansion, density maximum at temperatures ~5000 °C, and a estrus capacity minimum.[15]
Its density decreases from two.08 m/cm3
at 1950 °C to 2.03 g/cm3
at 2200 °C.[16]

Molecular SiO2

The molecular SiO2
has a linear structure like COtwo. It has been produced by combining silicon monoxide (SiO) with oxygen in an argon matrix. The dimeric silicon dioxide, (SiO2)2
has been obtained past reacting Otwo
with matrix isolated dimeric silicon monoxide, (Si2Oii). In dimeric silicon dioxide at that place are two oxygen atoms bridging betwixt the silicon atoms with an Si–O–Si angle of 94° and bail length of pm and the terminal Si–O bail length is 150.two pm. The Si–O bail length is 148.three pm, which compares with the length of 161 pm in α-quartz. The bond energy is estimated at 621.7 kJ/mol.[17]

Natural occurrence





is well-nigh usually found in nature every bit quartz, which comprises more than 10% past mass of the World’s crust.[eighteen]
Quartz is the only polymorph of silica stable at the Earth’s surface. Metastable occurrences of the loftier-pressure level forms coesite and stishovite have been found effectually affect structures and associated with eclogites formed during ultra-high-pressure level metamorphism. The high-temperature forms of tridymite and cristobalite are known from silica-rich volcanic rocks. In many parts of the world, silica is the major elective of sand.[19]



Even though it is poorly soluble, silica occurs in many plants such as rice. Plant materials with high silica phytolith content appear to exist of importance to grazing animals, from chewing insects to ungulates. Silica accelerates tooth wear, and high levels of silica in plants frequently eaten past herbivores may have developed as a defense mechanism confronting predation.[20]

Silica is also the main component of rice husk ash, which is used, for example, in filtration and as supplementary cementitious material (SCM) in cement and concrete manufacturing.[
citation needed

For well over a billion years, silicification in and by cells has been common in the biological world. In the modern world, information technology occurs in bacteria, unmarried-celled organisms, plants, and animals (invertebrates and vertebrates). Prominent examples include:

  • Tests or frustules (i.due east. shells) of diatoms, Radiolaria, and testate amoebae.[6]
  • Silica phytoliths in the cells of many plants, including Equisetaceae, practically all grasses, and a wide range of dicotyledons.
  • The spicules forming the skeleton of many sponges.

Crystalline minerals formed in the physiological environment frequently evidence infrequent physical properties (e.grand., strength, hardness, fracture toughness) and tend to form hierarchical structures that exhibit microstructural order over a range of scales. The minerals are crystallized from an environment that is undersaturated concerning silicon, and under conditions of neutral pH and low temperature (0–40 °C).

It is unclear in what ways silica is important in the diet of animals. This field of research is challenging because silica is ubiquitous and in most circumstances dissolves in trace quantities only. All the aforementioned, it certainly does occur in the living body, creating the challenge of creating silica-costless controls for purposes of research. This makes information technology hard to be certain when the silica present has had operative beneficial effects, and when its presence is coincidental, or fifty-fifty harmful. The current consensus is that information technology certainly seems of import in the growth, strength, and management of many connective tissues. This is truthful not only for hard connective tissues such as os and teeth[
clarification needed

only peradventure in the biochemistry of the subcellular enzyme-containing structures besides.[22]
obsolete source



Structural utilize


About 95% of the commercial apply of silicon dioxide (sand) occurs in the construction industry, thousand. for the production of concrete (Portland cement physical).[18]

Certain deposits of silica sand, with desirable particle size and shape and desirable clay and other mineral content, were important for sand casting of metallic products.[23]
The high melting bespeak of silica enables it to be used in such applications such as iron casting; modern sand casting sometimes uses other minerals for other reasons.

Crystalline silica is used in hydraulic fracturing of formations which contain tight oil and shale gas.[24]

Precursor to glass and silicon


Silica is the principal ingredient in the production of most glass. As other minerals are melted with silica, the principle of freezing bespeak low lowers the melting point of the mixture and increases fluidity. The drinking glass transition temperature of pure SiO2
is nigh 1475 M.[25]
When molten silicon dioxide SiO2
is speedily cooled, it does not crystallize, but solidifies as a drinking glass. Because of this, most ceramic glazes take silica every bit the principal ingredient.

The structural geometry of silicon and oxygen in drinking glass is similar to that in quartz and well-nigh other crystalline forms of silicon and oxygen with silicon surrounded past regular tetrahedra of oxygen centres. The departure between the glass and crystalline forms arises from the connectivity of the tetrahedral units: Although in that location is no long-range periodicity in the glassy network ordering remains at length scales well beyond the SiO bail length. One example of this ordering is the preference to form rings of 6-tetrahedra.[26]

The bulk of optical fibers for telecommunications are as well made from silica. It is a primary raw material for many ceramics such equally earthenware, stoneware, and porcelain.

Silicon dioxide is used to produce elemental silicon. The process involves carbothermic reduction in an electric arc furnace:[27]

SiO 2 + 2 C Si + 2 CO {\displaystyle {\ce {SiO2 + two C -> Si + 2 CO}}}

Baca Juga :   Unsur Budaya Kesenian Yang Dapat Dinikmati Oleh Mata Disebut

Fumed silica


Fumed silica, also known as pyrogenic silica, is prepared by called-for SiCl4
in an oxygen-rich hydrogen flame to produce a “smoke” of SiOii.[11]

SiCl 4 + 2 H 2 + O 2 SiO 2 + 4 HCl {\displaystyle {\ce {SiCl4 + 2 H2 + O2 -> SiO2 + 4 HCl}}}

The particles act as a thixotropic thickening agent, or as an anti-caking agent, and can be treated to make them hydrophilic or hydrophobic for either water or organic liquid applications

Manufactured fumed silica with maximum surface area of 380 10002/g

Silica fume is an ultrafine pulverization collected as a by-product of the silicon and ferrosilicon alloy production. It consists of amorphous (non-crystalline) spherical particles with an average particle diameter of 150 nm, without the branching of the pyrogenic product. The primary use is as pozzolanic textile for high performance physical. Fumed silica nanoparticles can exist successfully used as an anti-aging agent in asphalt binders.[29]

Food, cosmetic, and pharmaceutical applications


Silica, either colloidal, precipitated, or pyrogenic fumed, is a common additive in food product. It is used primarily as a menstruum or anti-caking amanuensis in powdered foods such equally spices and non-dairy java creamer, or powders to be formed into pharmaceutical tablets.[28]
It can adsorb water in hygroscopic applications. Colloidal silica is used as a fining agent for wine, beer, and juice, with the E number reference

In cosmetics, silica is useful for its low-cal-diffusing properties[30]
and natural absorbency.[31]

Diatomaceous earth, a mined product, has been used in nutrient and cosmetics for centuries. Information technology consists of the silica shells of microscopic diatoms; in a less processed course it was sold equally “tooth pulverisation”.[
citation needed

Manufactured or mined hydrated silica is used as the hard annoying in toothpaste.



Silicon dioxide is widely used in the semiconductor applied science

  • for the principal passivation (direct on the semiconductor surface),
  • every bit an original gate dielectric in MOS applied science. Today when scaling (dimension of the gate length of the MOS transistor) has progressed below ten  nm silicon dioxide has been replaced past other dielectric materials similar hafnium oxide or similar with college dielectric constant compared to silicon dioxide,
  • as a dielectric layer between metallic (wiring) layers (sometimes upward to 8-10) connecting elements and
  • as a second passivation layer (for protecting semiconductor elements and the metallization layers) typically today layered with some other dielectrics like silicon nitride.

Because silicon dioxide is a native oxide of silicon it is more widely used compared to other semiconductors like Gallium arsenide or Indium phosphide.

Silicon dioxide could exist grown on a silicon semiconductor surface.[32]
Silicon oxide layers could protect silicon surfaces during improvidence processes, and could be used for diffusion masking.[33]

Surface passivation is the process by which a semiconductor surface is rendered inert, and does non change semiconductor properties as a consequence of interaction with air or other materials in contact with the surface or edge of the crystal.[35]
The germination of a thermally grown silicon dioxide layer greatly reduces the concentration of electronic states at the silicon surface.[36]
films preserve the electrical characteristics of p–north junctions and prevent these electrical characteristics from deteriorating by the gaseous ambient environment.[34]
Silicon oxide layers could be used to electrically stabilize silicon surfaces.[33]
The surface passivation procedure is an important method of semiconductor device fabrication that involves coating a silicon wafer with an insulating layer of silicon oxide so that electricity could reliably penetrate to the conducting silicon below. Growing a layer of silicon dioxide on meridian of a silicon wafer enables information technology to overcome the surface states that otherwise preclude electricity from reaching the semiconducting layer.[35]

The process of silicon surface passivation by thermal oxidation (silicon dioxide) is critical to the semiconductor industry. It is commonly used to manufacture metallic-oxide-semiconductor field-effect transistors (MOSFETs) and silicon integrated excursion chips (with the planar process).[35]



Hydrophobic silica is used as a defoamer component.

In its capacity as a refractory, information technology is useful in fiber form as a high-temperature thermal protection fabric.[
citation needed

Silica is used in the extraction of DNA and RNA due to its ability to bind to the nucleic acids under the presence of chaotropes.[38]

Silica aerogel was used in the Stardust spacecraft to collect extraterrestrial particles.[39]

Pure silica (silicon dioxide), when cooled equally fused quartz into a glass with no true melting point, can be used as a glass fibre for fibreglass.



Silicon dioxide has been researched for agricultural applications as a potential insecticide.[40]



Silicon dioxide is mostly obtained by mining, including sand mining and purification of quartz. Quartz is suitable for many purposes, while chemic processing is required to make a purer or otherwise more suitable (e.g. more reactive or fine-grained) product.[
citation needed

Precipitated silica


Precipitated silica or amorphous silica is produced by the acidification of solutions of sodium silicate. The gelled precipitate or silica gel, is start washed and and so dehydrated to produce colorless microporous silica.[11]
The idealized equation involving a trisilicate and sulfuric acrid is:

Na ii Si 3 O 7 + H 2 And so iv 3 SiO 2 + Na 2 SO iv + H ii O {\displaystyle {\ce {Na2Si3O7 + H2SO4 -> 3 SiO2 + Na2SO4 + H2o}}}


On microchips


Thin films of silica grow spontaneously on silicon wafers via thermal oxidation, producing a very shallow layer of almost one nm or ten Å of then-called native oxide.[42]
Higher temperatures and alternative environments are used to abound well-controlled layers of silicon dioxide on silicon, for instance at temperatures betwixt 600 and 1200 °C, using so-called dry oxidation with O2

Si + O 2 SiO 2 {\displaystyle {\ce {Si + O2 -> SiO2}}}


Si + two H 2 O SiO 2 + two H 2 {\displaystyle {\ce {Si + 2 Water -> SiO2 + ii H2}}}


Laboratory or special methods


From organosilicon compounds


Many routes to silicon dioxide showtime with an organosilicon compound, e.g., HMDSO,[46]
TEOS. Synthesis of silica is illustrated below using tetraethyl orthosilicate (TEOS).[47]
Simply heating TEOS at 680–730 °C results in the oxide:

Si ( OC 2 H 5 ) four SiO ii + 2 O ( C ii H five ) 2 {\displaystyle {\ce {Si(OC2H5)iv -> SiO2 + 2 O(C2H5)2}}}

Si ( OC 2 H five ) 4 + 12 O two SiO ii + 10 H 2 O + 8 CO ii {\displaystyle {\ce {Si(OC2H5)4 + 12 O2 -> SiO2 + 10 Water + 8 CO2}}}


Si ( OC 2 H 5 ) 4 + 2 H 2 O SiO two + four HOCH 2 CH three {\displaystyle {\ce {Si(OC2H5)4 + ii H2O -> SiO2 + 4 HOCH2CH3}}}

Other methods


Being highly stable, silicon dioxide arises from many methods. Conceptually simple, only of trivial practical value, combustion of silane gives silicon dioxide. This reaction is analogous to the combustion of methane:

SiH four + ii O 2 SiO ii + 2 H 2 O {\displaystyle {\ce {SiH4 + 2 O2 -> SiO2 + 2 H2O}}}


Chemic reactions


Silica is converted to silicon by reduction with carbon.

Fluorine reacts with silicon dioxide to form SiF4
and O2
whereas the other halogen gases (Cl2, Br2, Itwo) are essentially unreactive.[eleven]

Nearly forms of silicon dioxide (except for stishovite, which does not react to any significant degree[l]) are attacked by hydrofluoric acid (HF) to produce hexafluorosilicic acid:[eight]

SiO 2 + 6 HF H 2 SiF 6 + ii H 2 O {\displaystyle {\ce {SiO2 + 6 HF -> H2SiF6 + two H2O}}}

Si ( s ) + six HF ( aq ) [ SiF 6 ] 2 ( aq ) + 2 H + ( aq ) + two H 2 ( yard ) {\displaystyle {\ce {Si(s) + 6HF(aq) -> [SiF6]^{two-}(aq) + 2H+(aq) + 2H2(k)}}}

Si ( s ) + iv NaOH ( aq ) [ SiO 4 ] four ( aq ) + 4 Na + ( aq ) + two H 2 ( g ) {\displaystyle {\ce {Si(s) + 4NaOH(aq) -> [SiO4]^{4-}(aq) + 4Na+(aq) + 2H2(g)}}}


Silicon dioxide dissolves in hot full-bodied alkali or fused hydroxide, every bit described in this idealized equation:[11]

SiO 2 + two NaOH Na 2 SiO 3 + H 2 O {\displaystyle {\ce {SiO2 + ii NaOH -> Na2SiO3 + H2O}}}

As an example the reaction of sodium oxide and SiO2
can produce sodium orthosilicate, sodium silicate, and glasses, dependent on the proportions of reactants:[eleven]

two Na 2 O + SiO 2 Na iv SiO 4 ; {\displaystyle {\ce {2 Na2O + SiO2 -> Na4SiO4;}}}

Na 2 O + SiO ii Na 2 SiO 3 ; {\displaystyle {\ce {Na2O + SiO2 -> Na2SiO3;}}}

( 0.25 0.8 ) {\displaystyle (0.25-0.eight)}

Na 2 O + SiO 2 glass {\displaystyle {\ce {Na2O + SiO2 -> glass}}}

Baca Juga :   Lagu Si Kancil Anak Nakal Merupakan Lagu Bertangga Nada

Examples of such glasses take commercial significance, e.yard. soda-lime drinking glass, borosilicate glass, atomic number 82 drinking glass. In these glasses, silica is termed the network old or lattice quondam.[eight]
The reaction is as well used in blast furnaces to remove sand impurities in the ore past neutralisation with calcium oxide, forming calcium silicate slag.

Silicon dioxide reacts in heated reflux under dinitrogen with ethylene glycol and an alkali metal base of operations to produce highly reactive, pentacoordinate silicates which provide admission to a broad variety of new silicon compounds.[52]
The silicates are essentially insoluble in all polar solvent except methanol.

Silicon dioxide reacts with elemental silicon at high temperatures to produce SiO:[viii]

SiO 2 + Si two SiO {\displaystyle {\ce {SiO2 + Si -> two SiO}}}

Water solubility


The solubility of silicon dioxide in water strongly depends on its crystalline form and is three-four times higher for silica[
description needed

than quartz; as a function of temperature, it peaks around 340 °C (644 °F).[53]
This property is used to grow single crystals of quartz in a hydrothermal process where natural quartz is dissolved in superheated water in a pressure level vessel that is cooler at the top. Crystals of 0.5–1  kg can exist grown for 1–2 months.[8]
These crystals are a source of very pure quartz for use in electronic applications.[eleven]
Above the critical temperature of h2o 647.096 K (373.946 °C; 705.103 °F) and a pressure of 22.064 megapascals (iii,200.1 psi) or higher, water is a supercritical fluid and solubility is again higher than at lower temperatures.[54]

Wellness effects


Quartz sand (silica) as main raw material for commercial drinking glass product

Silica ingested orally is essentially nontoxic, with an LDfifty
of 5000 mg/kg (v thou/kg).[18]
A 2008 study following subjects for 15 years found that college levels of silica in water appeared to decrease the take chances of dementia. An increase of 10 mg/day of silica in drinking water was associated with a decreased risk of dementia of 11%.[55]

Inhaling finely divided crystalline silica dust can atomic number 82 to silicosis, bronchitis, or lung cancer, every bit the grit becomes lodged in the lungs and continuously irritates the tissue, reducing lung capacities.[56]
When fine silica particles are inhaled in large enough quantities (such as through occupational exposure), it increases the risk of systemic autoimmune diseases such as lupus[57]
and rheumatoid arthritis compared to expected rates in the general population.[41]

Occupational chance


Silica is an occupational take chances for people who practise sandblasting or work with products that contain powdered crystalline silica. Baggy silica, such equally fumed silica, may crusade irreversible lung damage in some cases but is not associated with the development of silicosis. Children, asthmatics of any historic period, those with allergies, and the elderly (all of whom have reduced lung capacity) can be affected in less time.[58]

Crystalline silica is an occupational hazard for those working with stone countertops, because the procedure of cutting and installing the countertops creates big amounts of airborne silica.[59]
Crystalline silica used in hydraulic fracturing presents a health hazard to workers.[24]



In the trunk, crystalline silica particles do non deliquesce over clinically relevant periods. Silica crystals inside the lungs tin can activate the NLRP3 inflammasome within macrophages and dendritic cells and thereby result in product of interleukin, a highly pro-inflammatory cytokine in the immune system.[60]



Regulations restricting silica exposure ‘with respect to the silicosis hazard’ specify that they are concerned merely with silica, which is both crystalline and dust-forming.[63]

In 2013, the U.S. Occupational Safety and Health Administration reduced the exposure limit to fifty µg/grandthree
of air. Prior to 2013, it had allowed 100 µg/thou3
and in construction workers fifty-fifty 250 µg/yard3.[24]
In 2013, OSHA also required “green completion” of fracked wells to reduce exposure to crystalline silica besides restricting the limit of exposure.[24]

Crystalline forms


SiO2, more so than almost whatsoever material, exists in many crystalline forms. These forms are called polymorphs.

Crystalline forms of SiO2
Grade Crystal symmetry
Pearson symbol, group No.
Notes Construction
α-quartz rhombohedral (trigonal)
hP9, P3121 No.152[69]
ii.648 Helical chains making individual single crystals optically active; α-quartz converts to β-quartz at 846 K A-quartz.png
β-quartz hexagonal
hP18, P6two22, No. 180[70]
two.533 Closely related to α-quartz (with an Si-O-Si angle of 155°) and optically active; β-quartz converts to β-tridymite at 1140 Grand B-quartz.png
α-tridymite orthorhombic
oS24, C222ane, No.twenty[71]
2.265 Metastable class under normal pressure A-tridymite.png
β-tridymite hexagonal
hP12, P63/mmc, No. 194[71]
Closely related to α-tridymite; β-tridymite converts to β-cristobalite at 2010 K B-tridymite.png
α-cristobalite tetragonal
tP12, P41two12, No. 92[72]
two.334 Metastable form under normal pressure A-cristobalite.png
β-cristobalite cubic
cF104, Fd3m, No.227[73]
Closely related to α-cristobalite; melts at 1978 1000 B-cristobalite.png
keatite tetragonal
tP36, P41two12, No. 92[74]
three.011 Si5O10, Si4O8, Si8Oxvi
rings; synthesised from glassy silica and brine at 600–900 K and twoscore–400 MPa
moganite monoclinic
mS46, C2/c, No.15[75]
and Si6O12
coesite monoclinic
mS48, C2/c, No.15[76]
2.911 SifourOviii
and Si8Oxvi
rings; 900 K and 3–3.five GPa
stishovite tetragonal
tP6, P4two/mnm, No.136[77]
4.287 One of the densest (together with seifertite) polymorphs of silica; rutile-like with 6-fold coordinated Si; 7.5–eight.five GPa Stishovite.png
seifertite orthorhombic
oP, Pbcn[78]
4.294 1 of the densest (together with stishovite) polymorphs of silica; is produced at pressures above 40 GPa.[79] SeifertiteStructure.png
melanophlogite cubic (cP*, P4232, No.208)[seven]
or tetragonal (P42/nbc)[eighty]
two.04 Si5Ox, Sihalf-dozenO12
rings; mineral always found with hydrocarbons in interstitial spaces – a clathrasil (silica clathrate)[81]
Due west-silica[11]
oI12, Ibam, No.72[82]
1.97 Like Sistertwo
consisting of edge sharing chains, melts at ~1700 Grand
2d silica[83] hexagonal Sheet-similar bilayer structure 2D silica structure.png



Inhaling finely divided crystalline silica tin can lead to severe inflammation of the lung tissue, silicosis, bronchitis, lung cancer, and systemic autoimmune diseases, such as lupus and rheumatoid arthritis. Inhalation of amorphous silicon dioxide, in loftier doses, leads to non-permanent short-term inflammation, where all effects heal.[84]

Other names


This extended list enumerates synonyms for silicon dioxide; all of these values are from a unmarried source; values in the source were presented capitalized.[85]

  • CAS 112945-52-five
  • Acitcel
  • Aerosil
  • Amorphous silica dust
  • Aquafil
  • Catalogue
  • Colloidal silica[
    citation needed
  • Colloidal silicon dioxide
  • Dicalite
  • DRI-Dice Insecticide 67
  • Fossil flour
  • Fumed silica
  • Fumed silicon dioxide
  • HI-SEL
  • LO-VEL
  • Ludox
  • Nalcoag
  • Nyacol
  • Santocel
  • Silica
  • Silica aerogel
  • Silica, baggy
  • Silicic anhydride
  • Silikill
  • Synthetic baggy silica
  • Vulkasil

See also


  • Mesoporous silica
  • Orthosilicic acid
  • Silicon carbide



  1. ^






    Haynes, William Chiliad., ed. (2011).
    CRC Handbook of Chemical science and Physics
    (92nd ed.). Boca Raton, FL: CRC Press. ISBN1-4398-5511-0.

  2. ^




    NIOSH Pocket Guide to Chemical Hazards. “#0552”. National Plant for Occupational Prophylactic and Health (NIOSH).

  3. ^



    NIOSH Pocket Guide to Chemical Hazards. “#0682”. National Institute for Occupational Safety and Health (NIOSH).

  4. ^



    Zumdahl, Steven South. (2009).
    Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN978-0-618-94690-seven.

  5. ^

    Iler RK (1979).
    The Chemical science of Silica. New York: Wiley. ISBN9780471024040.

  6. ^



    Fernández LD, Lara E, Mitchell EA (2015). “Checklist, diversity and distribution of testate amoebae in Chile”
    European Journal of Protistology.
    (5): 409–24. doi:10.1016/j.ejop.2015.07.001. PMID 26340665. Archived
    from the original on 2022-10-10.

  7. ^



    Skinner BJ, Appleman DE (1963). “Melanophlogite, a cubic polymorph of silica”
    Am. Mineral.
    48: 854–867. Archived
    from the original on 2022-10-ten.

  8. ^








    Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.),
    Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Printing/De Gruyter, ISBN0-12-352651-5

  9. ^

    Cuff YH (1996).
    Ceramic Applied science for Potters and Sculptors. Philadelphia: University of Pennsylvania. pp. 93–95. ISBN9780812213775.

  10. ^

    De La Rocha C, Conley DJ (2017). “Mystical Crystals of Silica”.
    Silica Stories. Cham: Springer. pp. 50–55. doi:10.1007/978-three-319-54054-2_4. ISBN9783319540542.

  11. ^









    Greenwood, Norman N.; Earnshaw, Alan (1984).
    Chemical science of the Elements. Oxford: Pergamon Press. pp. 393–99. ISBN978-0-08-022057-4.

  12. ^

    Wells AF (1984).
    Structural Inorganic Chemistry. Oxford Science Publications. ISBN9780198553700.

  13. ^

    Kirfel A, Krane HG, Blaha P, et al. (2001). “Electron-density distribution in stishovite, SiOii: a new loftier-energy synchrotron-radiation study”.
    Acta Crystallogr. A.
    (6): 663–77. doi:10.1107/S0108767301010698. PMID 11679696.

  14. ^

    Scherzer J (1978). “Dealuminated faujasite-type structures with SiOii/AliiO3
    ratios over 100″.
    J. Catal.
    (2): 285. doi:x.1016/0021-9517(78)90051-9.

  15. ^

    Shell SM, Debenedetti PG, Panagiotopoulos AZ (2002). “Molecular structural order and anomalies in liquid silica”
    Phys. Rev. E.
    (ane): 011202. arXiv:cond-mat/0203383. Bibcode:2002PhRvE..66a1202S. doi:10.1103/PhysRevE.66.011202. PMID 12241346. S2CID 6109212. Archived from the original
    on 2016-06-04. Retrieved

  16. ^

    Aksay IA, Pask JA, Davis RF (1979). “Densities of SiOtwo-Al2O3
    J. Am. Ceram. Soc.
    (vii–eight): 332–336. doi:10.1111/j.1151-2916.1979.tb19071.x. Archived
    from the original on 2022-10-10.

  17. ^

    Jutzi P, Schubert U (2003).
    Silicon chemistry: from the atom to extended systems. Wiley-VCH. ISBN9783527306473.

  18. ^






    Flörke OW, Graetsch HA, Brunk F, et al. (2018). “Silica”.
    Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a23_583.pub3.

  19. ^

    Berslien Eastward (2012).
    An Introduction to Forensic Geoscience. Wiley & Sons. p. 138. ISBN9781405160544.

  20. ^

    Massey FP, Ennos AR, Hartley SE (2006). “Silica in grasses as a defence against insect herbivores: Contrasting furnishings on folivores and a phloem feeder”.
    J. Anim. Ecol.
    (2): 595–603. doi:10.1111/j.1365-2656.2006.01082.10. PMID 16638012.

  21. ^

    Keeping MG, Kvedaras OL (2008). “Silicon as a plant defence force against insect herbivory: Response to Massey, Ennos and Hartley”.
    J. Anim. Ecol.
    (3): 631–3. doi:10.1111/j.1365-2656.2008.01380.x. PMID 18341561.

  22. ^

    Carlisle EM (1986). “Silicon equally an essential trace element in animal nutrition”. In Evered D, O’Connor M (eds.).
    Silicon Biochemistry: Ciba Foundation Symposium. Novartis Foundation Symposia. Vol. 121. Wiley & Sons. pp. 123–39. doi:x.1002/9780470513323.ch8. ISBN9780470513323. PMID 3743227.

  23. ^

    Nevin, Charles Merrick (1925).
    Albany moulding sands of the Hudson Valley. University of the Land of New York at Albany.

  24. ^





    Greenhouse S (23 Aug 2013). “New Rules Would Cutting Silica Dust Exposure”.
    . Retrieved
    24 Aug

  25. ^

    Ojovan MI (2004). “Glass formation in baggy SiO2
    as a percolation phase transition in a system of network defects”.
    JETP Lett.
    (12): 632–634. Bibcode:2004JETPL..79..632O. doi:10.1134/1.1790021. S2CID 124299526.

  26. ^

    Elliott SR (1991). “Medium-range structural social club in covalent amorphous solids”.
    (6353): 445–452. Bibcode:1991Natur.354..445E. doi:10.1038/354445a0. S2CID 4344891.

  27. ^

    Atkins Pw, Overton T, Rourke J, et al., eds. (2010).
    Shriver & Atkins’ inorganic chemistry
    (fifth ed.). Oxford: Oxford University Printing. p. 354. ISBN9780199236176. OCLC 430678988.

  28. ^



    “Cab-O-Sil Fumed Metal Oxides”.

  29. ^

    Cheraghian, Goshtasp; Wistuba, Michael P.; Kiani, Sajad; Barron, Andrew R.; Behnood, Ali (December 2021). “Rheological, physicochemical, and microstructural backdrop of cobblestone binder modified by fumed silica nanoparticles”.
    Scientific Reports.
    (1): 11455. Bibcode:2021NatSR..1111455C. doi:10.1038/s41598-021-90620-w. PMC8169902. PMID 34075083.

  30. ^

    Barel AO, Paye Yard, Maibach HI (2014).
    Handbook of Cosmetic Science and Technology
    (4th ed.). CRC Press. p. 444. ISBN9781842145654.
    These soft-focus pigments, mainly composed of polymers, micas and talcs covered with rough or spherical particles of small diameters, such as silica or titanium dioxide, are used to optically reduce the appearance of wrinkles. These furnishings are obtained by optimizing outlines of wrinkles and reducing the departure of brightness due to diffuse reflection.

  31. ^

    Barel AO, Paye M, Maibach Howdy (2014).
    Handbook of Cosmetic Science and Technology
    (4th ed.). CRC Press. p. 442. ISBN9781842145654.
    The silica is a multiporous ingredient, which absorbs the oil and sebum.

  32. ^

    Bassett, Ross Knox (2007).
    To the Digital Age: Inquiry Labs, Start-up Companies, and the Rise of MOS Technology. Johns Hopkins University Printing. pp. 22–23. ISBN9780801886393.

  33. ^



    Lécuyer, Christophe; Brock, David C. (2010).
    Makers of the Microchip: A Documentary History of Fairchild Semiconductor. MIT Printing. p. 111. ISBN9780262294324.

  34. ^



    Saxena, A (2009).
    Invention of integrated circuits: untold important facts. International series on advances in solid state electronics and technology. Earth Scientific. pp. 96–97. ISBN9789812814456.

  35. ^




    “Martin Atalla in Inventors Hall of Fame, 2009”. Retrieved
    21 June

  36. ^



    Blackness, Lachlan E. (2016).
    New Perspectives on Surface Passivation: Agreement the Si-Al2O3 Interface. Springer. p. 17. ISBN9783319325217.

  37. ^



    “Dawon Kahng”.
    National Inventors Hall of Fame
    . Retrieved
    27 June

  38. ^

    Goodwin West, Linacre A, Hadi Due south (2007).
    An Introduction to Forensic Genetics. Wiley & Sons. p. 29. ISBN9780470010259.

  39. ^

    Calderone J (twenty Aug 2015). “This deject-like, futuristic textile has been sneaking its way into your life since 1931”.
    Business organisation Insider
    . Retrieved
    11 Feb

  40. ^

    Thabet, Ahmed F.; Boraei, Hessien A.; Galal, Ola A.; El-Samahy, Magdy F. Chiliad.; Mousa, Kareem Thou.; Zhang, Yao Z.; Tuda, Midori; Helmy, Eman A.; Wen, Jian; Nozaki, Tsubasa (2021-07-xiv). “Silica nanoparticles equally pesticide against insects of dissimilar feeding types and their non-target attraction of predators”.
    Scientific Reports.
    (ane): 14484. Bibcode:2021NatSR..1114484T. doi:10.1038/s41598-021-93518-nine. ISSN 2045-2322. PMC8280210. PMID 34262071.

  41. ^



    Meyer A, Sandler DP, Beane Freeman LE, et al. (2017). “Pesticide Exposure and Risk of Rheumatoid Arthritis among Licensed Male Pesticide Applicators in the Agricultural Wellness Written report”.
    Environ. Health Perspect.
    (7): 077010-1–077010-7. doi:x.1289/EHP1013. PMC5744649. PMID 28718769.

  42. ^

    Doering R, Nishi Y, eds. (2007).
    Handbook of Semiconductor Manufacturing Technology. CRC Press. ISBN9781574446753.

  43. ^

    Lee S (2006).
    Encyclopedia of chemical processing. CRC Press. ISBN9780824755638.

  44. ^

    Morgan DV, Lath Thou (1991).
    An Introduction To Semiconductor Microtechnology
    (2nd ed.). Chichester, West Sussex, England: John Wiley & Sons. p. 72. ISBN9780471924784.

  45. ^

    Riordan M (2007). “The Silicon Dioxide Solution: How physicist Jean Hoerni congenital the bridge from the transistor to the integrated circuit”.
    IEEE Spectrum
    . Retrieved
    11 Feb

  46. ^

    Chrystie, Robin S. Chiliad.; Ebertz, Felix L.; Dreier, Thomas; Schulz, Christof (2019-01-28). “Absolute SiO concentration imaging in low-pressure nanoparticle-synthesis flames via laser-induced fluorescence”.
    Practical Physics B.
    (2): 29. Bibcode:2019ApPhB.125…29C. doi:10.1007/s00340-019-7137-viii. ISSN 1432-0649. S2CID 127735545.

  47. ^

    Romero-Jaime, A. Thou.; Acosta-Enríquez, K. C.; Vargas-Hernández, D.; Tánori-Córdova, J. C.; Pineda León, H. A.; Castillo, S. J. (August 2021). “Synthesis and label of silica–lead sulfide core–vanquish nanospheres for applications in optoelectronic devices”.
    Journal of Materials Science: Materials in Electronics.
    (16): 21425–21431. doi:ten.1007/s10854-021-06648-ane. ISSN 0957-4522. S2CID 236182027.

  48. ^

    Nandiyanto AB, Kim SG, Iskandar F, et al. (2009). “Synthesis of spherical mesoporous silica nanoparticles with nanometer-size controllable pores and outer diameters”.
    Microporous and Mesoporous Materials.
    (three): 447–453. doi:x.1016/j.micromeso.2008.12.019.

  49. ^

    Morgan DV, Lath K (1991).
    An Introduction To Semiconductor Microtechnology
    (2nd ed.). Chichester, Westward Sussex, England: John Wiley & Sons. p. 27. ISBN9780471924784.

  50. ^

    Fleischer, Michael (1962). “New mineral names”
    American Mineralogist. Mineralogical Society of America.
    (2): 172–174. Archived
    from the original on 2011-07-22.

  51. ^

    Rodgers GE (2011).
    Descriptive Inorganic, Coordination, and Solid State Chemistry. Cengage Learning. pp. 421–2. ISBN9781133172482.

  52. ^

    Laine, Richard M.; Blohowiak, Kay Youngdahl; Robinson, Timothy R.; Hoppe, Martin L.; Nardi, Paola; Kampf, Jeffrey; Uhm, Jackie (17 October 1991). “Synthesis of pentacoordinate silicon complexes from SiO2
    (6345): 642–644. Bibcode:1991Natur.353..642L. doi:10.1038/353642a0. hdl:2027.42/62810. S2CID 4310228. Archived
    from the original on 2017-08-19.

  53. ^

    Fournier RO, Rowe JJ (1977). “The solubility of amorphous silica in water at high temperatures and high pressures”
    Am. Mineral.
    62: 1052–1056. Archived
    from the original on 2022-10-10.

  54. ^

    Okamoto, Atsushi (2019). “Germination of silica particles from supercritical fluids and its impacts on the hydrological properties in the crust”.
    EGU General Assembly Conference Abstracts: 4614. Bibcode:2019EGUGA..21.4614O.

  55. ^

    Rondeau V, Jacqmin-Gadda H, Commenges D, et al. (2008). “Aluminum and Silica in Drinking Water and the Risk of Alzheimer’s Disease or Cognitive Decline: Findings from 15-Year Follow-upwards of the PAQUID Cohort”.
    Am. J. Epidemiol.
    (4): 489–96. doi:10.1093/aje/kwn348. PMC2809081. PMID 19064650.

  56. ^

    “Work Safely with Silica”. CPWR – The Middle for Construction Research and Training. Retrieved
    11 Feb

  57. ^

    “Action Plan for Lupus Research”.
    NIAMS. NIH. 2017. Retrieved
    11 February

  58. ^

    Reuzel PG, Bruijntjes JP, Feron VJ, et al. (1991). “Subchronic inhalation toxicity of baggy silica and quartz dust in rats”.
    Food Chem. Toxicol.
    (v): 341–54. doi:ten.1016/0278-6915(91)90205-50. PMID 1648030.

  59. ^

    “Worker Exposure to Silica during Countertop Manufacturing, Finishing and Installation”
    (PDF). NIOSH and OSHA. 2015. Archived
    from the original on 2022-10-x. Retrieved
    26 February

  60. ^

    Hornung Five, Bauernfeind F, Halle A, et al. (2008). “Silica crystals and aluminum salts activate the NALP3 inflammasome through phagosomal destabilization”.
    Nat. Immunol.
    (8): 847–856. doi:x.1038/ni.1631. PMC2834784. PMID 18604214.

  61. ^

    Merchant JA, ed. (1986).
    Occupational Respiratory Diseases
    (PDF). Cincinnati, OH: United states Section of Health and Human Services, NIOSH. doi:10.26616/NIOSHPUB86102. hdl:2027/uc1.31210023588922. DHHS (NIOSH) Publication Number 86-102.

  62. ^

    NIOSH (2002) Hazard Review, Health Furnishings of Occupational Exposure to Respirable Crystalline Silica. Cincinnati, OH: U.South. Department of Health and Human Services, U.South. Public Wellness Service, Centers for Disease Control, National Institute for Occupational Safe and Wellness, DHHS (NIOSH) Publication No. 2002-129.

  63. ^

    “Crystalline Factsheet”
    (PDF). Archived from the original
    on 22 December 2017. Retrieved
    3 August

  64. ^

    “Silica, Crystalline”. Retrieved
    3 Baronial

  65. ^

    “Often Asked Questions”. Retrieved
    iii August

  66. ^

    “If It’southward Silica, It’s Non Merely Dust!”
    (PDF). Archived
    from the original on 2022-10-ten. Retrieved
    iii Baronial

  67. ^

    “What y’all should know about crystalline silica, silicosis, and Oregon OSHA silica rules”
    (PDF). Archived
    from the original on 2022-x-10. Retrieved
    3 Baronial

  68. ^

    Szymendera, Scott D. (January sixteen, 2018).
    Respirable Crystalline Silica in the Workplace: New Occupational Safety and Wellness Assistants (OSHA) Standards
    (PDF). Washington, DC: Congressional Research Service. Archived
    from the original on 2022-x-x. Retrieved
    27 January

  69. ^

    Lager G. A.; Jorgensen J. D.; Rotella F.J. (1982). “Crystal construction and thermal expansion of a-quartz SiO2
    at depression temperature”.
    Journal of Practical Physics.
    (10): 6751–6756. Bibcode:1982JAP….53.6751L. doi:10.1063/one.330062.

  70. ^

    Wright, A. F.; Lehmann, M. S. (1981). “The structure of quartz at 25 and 590 °C adamant past neutron diffraction”.
    Journal of Solid State Chemistry.
    (3): 371–80. Bibcode:1981JSSCh..36..371W. doi:10.1016/0022-4596(81)90449-7.

  71. ^



    Kihara, Kuniaki; Matsumoto, Takeo; Imamura, Moritaka (1986). “Structural change of orthorhombic-Itridymite with temperature: A report based on second-order thermal-vibrational parameters”.
    Zeitschrift für Kristallographie.
    (1–ii): 27–38. Bibcode:1986ZK….177…27K. doi:10.1524/zkri.1986.177.ane-two.27.

  72. ^

    Downs R. T.; Palmer D. C. (1994). “The pressure behavior of a cristobalite”
    American Mineralogist.
    79: 9–14. Archived
    from the original on 2022-ten-10.

  73. ^

    Wright, A. F.; Leadbetter, A. J. (1975). “The structures of the β-cristobalite phases of SiO2
    and AlPOiv“.
    Philosophical Magazine.
    (six): 1391–401. Bibcode:1975PMag…31.1391W. doi:10.1080/00318087508228690.

  74. ^

    Shropshire, Joseph; Keat, Paul P.; Vaughan, Philip A. (1959). “The crystal construction of keatite, a new form of silica”.
    Zeitschrift für Kristallographie.
    (1–6): 409–xiii. Bibcode:1959ZK….112..409S. doi:10.1524/zkri.1959.112.ane-6.409.

  75. ^

    Miehe, Gerhard; Graetsch, Heribert (1992). “Crystal structure of moganite: a new construction blazon for silica”.
    European Periodical of Mineralogy.
    (iv): 693–706. Bibcode:1992EJMin…4..693M. doi:10.1127/ejm/4/4/0693.

  76. ^

    Levien L.; Prewitt C. T. (1981). “High-pressure crystal structure and compressibility of coesite”
    American Mineralogist.
    66: 324–333. Archived
    from the original on 2022-x-ten.

  77. ^

    Smyth J. R.; Swope R. J.; Pawley A. R. (1995). “H in rutile-type compounds: Ii. Crystal chemistry of Al substitution in H-bearing stishovite”
    American Mineralogist.
    (5–6): 454–456. Bibcode:1995AmMin..80..454S. doi:x.2138/am-1995-v-605. S2CID 196903109. Archived
    from the original on 2022-10-10.

  78. ^

    Dera P.; Prewitt C. T.; Boctor North. Z.; Hemley R. J. (2002). “Label of a high-pressure level phase of silica from the Martian meteorite Shergotty”.
    American Mineralogist.
    (7): 1018. Bibcode:2002AmMin..87.1018D. doi:10.2138/am-2002-0728. S2CID 129400258.

  79. ^


  80. ^

    Nakagawa T.; Kihara Chiliad.; Harada K. (2001). “The crystal construction of low melanophlogite”.
    American Mineralogist.
    (11–12): 1506. Bibcode:2001AmMin..86.1506N. doi:x.2138/am-2001-11-1219. S2CID 53525827.

  81. ^

    Rosemarie Szostak (1998).
    Molecular sieves: Principles of Synthesis and Identification. Springer. ISBN978-0-7514-0480-7.

  82. ^

    Weiss, Alarich; Weiss, Armin (1954). “Über Siliciumchalkogenide. VI. Zur Kenntnis der faserigen Siliciumdioxyd-Modifikation”.
    Zeitschrift für Anorganische und Allgemeine Chemie.
    (1–2): 95–112. doi:10.1002/zaac.19542760110.

  83. ^

    Björkman, T; Kurasch, South; Lehtinen, O; Kotakoski, J; Yazyev, O. V.; Srivastava, A; Skakalova, V; Smet, J. H.; Kaiser, U; Krasheninnikov, A. 5. (2013). “Defects in bilayer silica and graphene: common trends in diverse hexagonal two-dimensional systems”.
    Scientific Reports.
    iii: 3482. Bibcode:2013NatSR…3E3482B. doi:ten.1038/srep03482. PMC3863822. PMID 24336488.

  84. ^

    Johnston CJ, Driscoll KE, Finkelstein JN, et al. (2000). “Pulmonary Chemokine and Mutagenic Responses in Rats after Subchronic Inhalation of Amorphous and Crystalline Silica”.
    Toxicol. Sci.
    (2): 405–413. doi:10.1093/toxsci/56.2.405. PMID 10911000.

  85. ^

    Lewis, Grace Ross (1999).
    1001 chemicals in everyday products
    (2nd ed.). John Wiley & Sons (Wiley-Interscience). pp. 250–1. ISBN0-471-29212-five
    – via Internet Annal.

External links


  • Chisholm, Hugh, ed. (1911).
    Encyclopædia Britannica
    (11th ed.). Cambridge Academy Press.

  • Tridymite, International Chemical Rubber Card 0807
  • Quartz, International Chemical Rubber Card 0808
  • Cristobalite, International Chemic Condom Carte du jour 0809
  • amorphous, NIOSH Pocket Guide to Chemical Hazards
  • crystalline, as respirable grit, NIOSH Pocket Guide to Chemical Hazards
  • Germination of silicon oxide layers in the semiconductor industry. LPCVD and PECVD method in comparing. Stress prevention.
  • Quartz SiOtwo
    piezoelectric backdrop
  • Silica (SiO2) and Water
  • Epidemiological testify on the carcinogenicity of silica: factors in scientific judgement by C. Soutar and others. Plant of Occupational Medicine Research Report TM/97/09
  • Scientific opinion on the health effects of airborne silica by A Pilkington and others. Institute of Occupational Medicine Inquiry Report TM/95/08
  • The toxic furnishings of silica Archived 2016-04-fifteen at the Wayback Machine by A Seaton and others. Institute of Occupational Medicine Enquiry Study TM/87/13
  • Structure of precipitated silica
Baca Juga :   Jelaskan Yg Dimaksud Kerajinan Sebagai Bagian Dari Industri Kreatif

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