Trisilan

Trisilan
Obecné
Systematický názevTrisilan
Anglický názevTrisilane
Německý názevTrisilan
Sumární vzorecSi3H8
Vzhledbezbarvá kapalina[1]
Identifikace
Registrační číslo CAS7783-26-8
EC-no (EINECS/ELINCS/NLP)616-514-9
PubChem139070
SMILES[SiH3][SiH2][SiH3]
InChIInChI=1S/H8Si3/c1-3-2/h3H2,1-2H3
Vlastnosti
Molární hmotnost92,319 g/mol
Teplota tání−114,8 °C[1]
Teplota varu52,8 °C[1]
Hustota0,739 g/cm3[1]
Index lomu1,4978[2]
Bezpečnost
GHS02 – hořlavé látky
GHS02
GHS07 – dráždivé látky
GHS07
H-větyH250 H261 H315 H319 H335
P-větyP210 P222 P231+232 P261 P264 P271 P280 P302+334 P302+352 P304+340 P305+351+338 P312 P321 P332+313 P337+313 P362 P370+378 P402+404 P403+233 P405 P422 P501
samozápalnost
Není-li uvedeno jinak, jsou použity
jednotky SI a STP (25 °C, 100 kPa).
Některá data mohou pocházet z datové položky.

Trisilan je silan se vzorcem H2Si(SiH3)2. Při standardní teplotě a tlaku je kapalný (jedná se o křemíkový analog propanu). Na rozdíl od propanu se však trisilan na vzduchu samovolně vznítí.[3]

Syntéza

Trisilan charakterizoval Alfred Stock, který jej připravil reakcí kyseliny chlorovodíkové a silicidu hořečnatého.[4][5] Tuto reakci zkoumali již v roce 1857 Friedrich Wöhler a Heinrich Buff a v roce 1902 ji dále zkoumali Henri Moissan a Samuel Smiles.[3]

Rozklad

Klíčovou vlastností trisilanu je jeho tepelná labilita (nestálost). Podle této idealizované rovnice se rozkládá na vrstvy křemíku a SiH4:

Si3H8 → Si + 2 SiH4

Z hlediska mechanismu probíhá tento rozklad posunem 1,2 vodíku, při kterém vznikají disilany, normální a izotetrasilany, a normální a izopentasilany.[6]

Protože se trisilan snadno rozkládá a zanechává vrstvy Si, byl zkoumán jako prostředek k nanášení tenkých vrstev křemíku pro polovodiče.[7] Podobně termolýzou trisilanu vznikají křemíkové nanodrátky.[8]

Reference

V tomto článku byl použit překlad textu z článku Trisilane na anglické Wikipedii.

  1. ↑ a b c d BRAUER, Georg. Handbuch der Präparativen Anorganischen Chemie. Stuttgart: [s.n.], 1975. ISBN 3-432-02328-6. S. 658. (anglicky) 
  2. ↑ D’ANS, Jean; LAX, Ellen; BLACHNIK, Roger. Taschenbuch für Chemiker und Physiker. [s.l.]: Springer DE, 1998. Dostupné online. ISBN 3-642-58842-5. S. 730. (německy) 
  3. ↑ a b SCHENK, P. W. Handbook of Preparative Inorganic Chemistry. 2. vyd. New York: Academic Press, 1963. S. 680. 
  4. ↑ STOCK, Alfred; SOMIESKI, Carl. Siliciumwasserstoffe. I. Die aus Magnesiumsilicid und Säuren entstehenden Siliciumwasserstoffe. Berichte der Deutschen Chemischen Gesellschaft. Roč. 49, čís. 111–157. Dostupné online. DOI 10.1002/cber.19160490114. 
  5. ↑ STOCK, Alfred; STIEBELER, Paul; ZIEDLER, Friedrich. Siliciumwasserstoffe, XVI.: Die höheren Siliciumhydride. Berichte der Deutschen Chemischen Gesellschaft (A and B Series). Roč. 57, čís. 6, s. 1695–1705. DOI 10.1002/cber.19230560735. 
  6. ↑ WANDERWIELEN, A. J.; RING, M. A.; O'NEAL, H. E. Kinetics of the thermal decomposition of methyldisilane and trisilan. Journal of the American Chemical Society. Roč. 97, čís. 5, s. 993–998. DOI 10.1021/ja00838a008. 
  7. ↑ United States Patent Application Publication. Pub No. US 2012/0252190 A1, OCT, 4, 2012. Zehavi et al.
  8. ↑ HEITSCH, Andrew T.; FANFAIR, Dayne D.; TUAN, Hsing-Yu, Brian A. Korgel. Solution−Liquid−Solid (SLS) Growth of Silicon Nanowires. Journal of the American Chemical Society. Roč. 130, čís. 16, s. 5436–5437. DOI 10.1021/ja8011353. PMID 18373344. 

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