Difference between revisions of "Silicon"

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(added section == Stishovite and Seifertite ==)
(→‎Related: added note on abundances)
 
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* [https://en.wikipedia.org/wiki/Quartz Quartz] (Mohs 7 by definition | density 2.65 g/cm<sup>3</sup>) <br> α-quartz: trigonal -- β-quartz: hexagonal
 
* [https://en.wikipedia.org/wiki/Quartz Quartz] (Mohs 7 by definition | density 2.65 g/cm<sup>3</sup>) <br> α-quartz: trigonal -- β-quartz: hexagonal
 
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----
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* [https://en.wikipedia.org/wiki/Stishovite Stishovite] ('''Mohs 9-9.5 | density 4.287 g/cm<sup>3</sup>''' | tetragonal - rutile group)
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* [https://en.wikipedia.org/wiki/Stishovite Stishovite] ('''Mohs 9-9.5 | density 4.287 g/cm<sup>3</sup>''' | tetragonal - [[rutile structure|rutile group]])
 
* [https://en.wikipedia.org/wiki/Seifertite Seifertite] ('''Mohs ~9 | density 4.294 g/cm<sup>3</sup>''' | orthorhombic  - resembles scrutinyite α-PbO<sub>2</sub>)
 
* [https://en.wikipedia.org/wiki/Seifertite Seifertite] ('''Mohs ~9 | density 4.294 g/cm<sup>3</sup>''' | orthorhombic  - resembles scrutinyite α-PbO<sub>2</sub>)
 
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=== Stishovite and Seifertite ===
 
=== Stishovite and Seifertite ===
  
−
They are both uncomman in that they have:  
+
They are both uncommon in that they have:  
 
* hypervalent silicon with a coordination number of six instead the normal four and  
 
* hypervalent silicon with a coordination number of six instead the normal four and  
−
* hypervalent toxygen with coordination number three instead of the normal two.
+
* hypervalent oxygen with coordination number three instead of the normal two.
−
This causes their unusually high density and hardness. <br>
+
This is probably what causes the unusually high density and hardness. <br>  
−
They are metastable at unpressurized conditions.
+
<small>Related: [[Hypervalency]] [https://en.wikipedia.org/wiki/Hypervalent_molecule];
−
And surprisingly more chemically stable than plain quartz.
+
Three center four electron bond [https://en.wikipedia.org/wiki/Three-center_four-electron_bond]
 +
formerly thought to be sp<sup>3</sup>d<sup>2</sup> hybridisation.</small>
  
−
To increase stability at the cost of hardness checkerboard [[neo-polymorph]]s can be created by replacing some of the silicon with other suitable elements that crystallize in the same crystal structure. Thy rutile group crystal structure.
+
Stishovite and Seifertite are metastable at unpressurized conditions. <br>
 +
And surprisingly more chemically stable than plain quartz. It is not attacked by hydrofluoric acid HF.
  
−
Stishovite can form a continuum to the minerals of the rutile group (here ordered by elemental abundance in earths crust):
+
To increase high temperature stability at the cost of hardness, it may be possible to substitute some of the silicon atoms <be>
−
* '''[https://en.wikipedia.org/wiki/Rutile Rutile] TiO<sub>2</sub> (Mohs 6-6.5 | titanium is very abundant)'''
+
with atoms of other suitable elements that would make in case of a 100% substitution termodynamically more stable minerals in the same crysral structure (the [[rutile structure]]). <br>
−
* [https://en.wikipedia.org/wiki/Pyrolusite Pyrolusite] MnO<sub>2</sub> (Mohs 6-6.5 | Mn is not too rare but todays mining is environmentally destructive)
+
Such a substitution in a checkerboard patterned way done via [[force applying mechanosynthesis]] can make makes [[neo-polymorph]] materials.
−
* NbO<sub>2</sub> [https://en.wikipedia.org/wiki/Niobium_dioxide]
+
 
−
* [https://en.wikipedia.org/wiki/Cassiterite Cassierite] SnO<sub>2</sub> (Mohs 6-7)
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That is: stishovite can form [[pseudo phase diagram|a continuum]] to the minerals with [[rutile structure]]. <br>
−
* [https://en.wikipedia.org/wiki/Plattnerite Plattnerite] β-PbO<sub>2</sub> (Mohs 5.5 unusually hard for a lead compound | '''useful high density of ~9 g/cm<sup>3</sup>''')
+
'''See "[[rutile structure]]" for a list of elements that are potentially compatible for atom substitution in stishovite without too much crystal structure disturbance.'''
−
* Note that lead Pb tin Sn and niobium Nb are similar in their not too high abundance.
+
 
 +
== Misc ==
 +
 
 +
Silicon is the second most [[abundant element]] on Earth (crust and surface). Right after [[oxygen]].
 +
 
 +
Maybe remotely related to silicon: Geopolymers: [https://en.wikipedia.org/wiki/Geopolymer]
 +
 
 +
An [[elemental storage medium]] for silicon (think: nanofactory cartridges for silicon) might be a bit of a challenge because of its strong tenency of polymerization and generally low solubility in benign solvents like water.
 +
Here's a list of some obvious options:
 +
* Silicic acid would be great due to its non-toxicity. But silicic acid [https://en.wikipedia.org/wiki/Silicic_acid] has a strong tendency to self polymerize. This is undesirable for standardized processing.
 +
* Silanes [https://en.wikipedia.org/wiki/Silanes] (the silicon analogues to hydrocarbons) do not self polymerize but they are toxic and explosive.  
 
----
 
----
−
* [https://en.wikipedia.org/wiki/Argutite Argutite] GeO<sub>2</sub> (Mohs 6-7 | germanium is pretty rare)
+
* Disiloxane [https://en.wikipedia.org/wiki/Disiloxane] ?
−
* [https://en.wikipedia.org/wiki/Tripuhyite Tripuhyite] FeSbO<sub>4</sub> (Mohs 6-7 | Antimony Sb is a little more rare than germanium Ge.<br> The much more common phosphorus analog FePO<sub>4</sub> forms a soft hydroxide [https://en.wikipedia.org/wiki/Strengite Strengite] with different crystal structure)
+
* Tetramethylsilane [https://en.wikipedia.org/wiki/Tetramethylsilane] is also toxic but not explosive. It may carry too much carbon for many applications (e.g. in case moissanite SiC with a stoichiometry Si:C of 1:1 is mechanosynthesitzed).
−
* [https://de.wikipedia.org/wiki/Paratellurit Paratellurit (de)] TeO<sub>2</sub> (soft compound and tellurium is extremely rare)
+
* Trimethylsilane [https://en.wikipedia.org/wiki/Trimethylsilane]; Dimethylsilane [https://en.wikipedia.org/wiki/Dimethylsilane]; Methylsilane [https://de.wikipedia.org/wiki/Methylsilan] -- (better Si:C ratio & maybe falling toxicity ??)
 +
* There's also trimethylsilanol [https://en.wikipedia.org/wiki/Trimethylsilanol]
 +
* hydrogen silsesquioxane H<sub>8</sub>Si<sub>8</sub>O<sub>12</sub> ?? [https://en.wikipedia.org/wiki/Hydrogen_silsesquioxane]
 +
----
 +
* Trimethylsilylacetylene [https://en.wikipedia.org/wiki/Trimethylsilylacetylene]
 +
* ...
  
−
Related: [[Hypervalency]] [https://en.wikipedia.org/wiki/Hypervalent_molecule]; Three center four electron bond [https://en.wikipedia.org/wiki/Three-center_four-electron_bond] formerly thought to be sp<sup>3</sup>d<sup>2</sup> hybridisation
+
== Related ==
 +
 
 +
* [[Chemical element]]
 +
* Elements in the same group: [[Carbon]], '''Silicon''', [[Germanium]], [[Tin]], [[Lead]] <br> Tin and lead are actually surprisingly abundant for their high period. Lead thanks to being at the end of many decay chains. Germanium is quite rare.
 +
* [[Mining]]
 +
 
 +
 
 +
[[Category:Chemical element]]
 +
 
 +
== External Links ==
 +
 
 +
* Informations about various polymorphs of SiO<sub>2</sub>: https://howlingpixel.com/wiki/Silica
 +
----
 +
* Forsight institute: [https://www.foresight.org/Conferences/MNT05/Papers/Gillett1/index.html Toward a Silicate-Based Molecular Nanotechnology I. Background and Review -- by Stephen L. Gillett]
 +
----
 +
* Wikipedia: [https://en.wikipedia.org/wiki/Binary_compounds_of_silicon Binary compounds of silicon]
 +
* Wikipedia: [https://en.wikipedia.org/wiki/Silicate_minerals Silicate_minerals]
 +
* Wikipedia: [https://en.wikipedia.org/wiki/Silicide Silicide]
 +
* Wikipedia: [https://en.wikipedia.org/wiki/Category:Organosilicon_compounds Category:Organosilicon_compounds]

Latest revision as of 13:55, 11 December 2022

This article is a stub. It needs to be expanded.

Silicon dioxide SiO2

Beside the commonly known quartz and amorphous glass there are many polymorphs of silicon dioxide (tectosilicates).

  • Quartz (Mohs 7 by definition | density 2.65 g/cm3)
    α-quartz: trigonal -- β-quartz: hexagonal
  • Stishovite (Mohs 9-9.5 | density 4.287 g/cm3 | tetragonal - rutile group)
  • Seifertite (Mohs ~9 | density 4.294 g/cm3 | orthorhombic - resembles scrutinyite α-PbO2)
  • Coesite (Mohs 7.5 | density 2.92 g/cm3 (calculated) | monoclinic)
  • Cristobalite (Mohs 6-7 | density 2.32–2.36 g/cm3)
    α-Cristobalite tetragonal
    β-Cristobalite cubic - resembles diamond / ZnS
  • Tridymite (Mohs 7 | density 2.25–2.28 g/cm3) there are seven crystal phases of tridymite
    two hexagonal: HP (β) & LHP -- three orthorhombic: OC (α) & OS & OP -- two monoclinic: MC & MX
  • Moganite (not MoRganite!) (Mohs 6 | 2.52-2.58 g/cm3 | monoclinic)

Related: Binary diamondoid compound

Stishovite and Seifertite

They are both uncommon in that they have:

  • hypervalent silicon with a coordination number of six instead the normal four and
  • hypervalent oxygen with coordination number three instead of the normal two.

This is probably what causes the unusually high density and hardness.
Related: Hypervalency [1]; Three center four electron bond [2] formerly thought to be sp3d2 hybridisation.

Stishovite and Seifertite are metastable at unpressurized conditions.
And surprisingly more chemically stable than plain quartz. It is not attacked by hydrofluoric acid HF.

To increase high temperature stability at the cost of hardness, it may be possible to substitute some of the silicon atoms <be> with atoms of other suitable elements that would make in case of a 100% substitution termodynamically more stable minerals in the same crysral structure (the rutile structure).
Such a substitution in a checkerboard patterned way done via force applying mechanosynthesis can make makes neo-polymorph materials.

That is: stishovite can form a continuum to the minerals with rutile structure.
See "rutile structure" for a list of elements that are potentially compatible for atom substitution in stishovite without too much crystal structure disturbance.

Misc

Silicon is the second most abundant element on Earth (crust and surface). Right after oxygen.

Maybe remotely related to silicon: Geopolymers: [3]

An elemental storage medium for silicon (think: nanofactory cartridges for silicon) might be a bit of a challenge because of its strong tenency of polymerization and generally low solubility in benign solvents like water. Here's a list of some obvious options:

  • Silicic acid would be great due to its non-toxicity. But silicic acid [4] has a strong tendency to self polymerize. This is undesirable for standardized processing.
  • Silanes [5] (the silicon analogues to hydrocarbons) do not self polymerize but they are toxic and explosive.
  • Disiloxane [6] ?
  • Tetramethylsilane [7] is also toxic but not explosive. It may carry too much carbon for many applications (e.g. in case moissanite SiC with a stoichiometry Si:C of 1:1 is mechanosynthesitzed).
  • Trimethylsilane [8]; Dimethylsilane [9]; Methylsilane [10] -- (better Si:C ratio & maybe falling toxicity ??)
  • There's also trimethylsilanol [11]
  • hydrogen silsesquioxane H8Si8O12 ?? [12]
  • Trimethylsilylacetylene [13]
  • ...

Related

  • Chemical element
  • Elements in the same group: Carbon, Silicon, Germanium, Tin, Lead
    Tin and lead are actually surprisingly abundant for their high period. Lead thanks to being at the end of many decay chains. Germanium is quite rare.
  • Mining

External Links

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