Germane

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For a definition of the term "germane", see the Wiktionary entry germane.

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Germane
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  Germanium, Ge
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  Hydrogen, H
Names
IUPAC name
Germane
Other names
Germanium tetrahydride
Germanomethane
Monogermane
Germanium(IV) hydride
Identifiers
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3D model (JSmol)
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587
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UN number 2192
  • InChI=1S/GeH4/h1H4 checkY
    Key: QUZPNFFHZPRKJD-UHFFFAOYSA-N checkY
  • InChI=1/GeH4/h1H4
    Key: QUZPNFFHZPRKJD-UHFFFAOYAE
  • [H][Ge]([H])([H])[H]
Properties
GeH4
Molar mass 76.62 g/mol
Appearance Colorless gas
Odor Pungent[1]
Density 3.3 kg/m3
Melting point −165 °C (−265 °F; 108 K)
Boiling point −88 °C (−126 °F; 185 K)
Low
Vapor pressure >1 atm[1]
Viscosity 17.21 μPa·s
(theoretical estimate)[2]
Structure
Tetrahedral
0 D
Hazards
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4
4
3
NIOSH (US health exposure limits):
PEL (Permissible)
 None[1]
REL (Recommended)
 TWA 0.2 ppm (0.6 mg/m3)[1]
IDLH (Immediate danger)
 N.D.[1]
Safety data sheet (SDS) ICSC 1244
Related compounds
Related compounds
 Methane
Silane
Stannane
Plumbane
Germyl
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Template:Chembox Footer/trackingTemplate:Short description

Germane is the chemical compound with the formula GeH4, and the germanium analogue of methane. It is the simplest germanium hydride and one of the most useful compounds of germanium. Like the related compounds silane and methane, germane is tetrahedral. It burns in air to produce GeO2 and water. Germane is a group 14 hydride.

Occurrence

Germane has been detected in the atmosphere of Jupiter.[3]

Synthesis

Germane is typically prepared by reduction of germanium oxides, notably germanates, with hydride reagents such as sodium borohydride, potassium borohydride, lithium borohydride, lithium aluminium hydride, sodium aluminium hydride. The reaction with borohydrides is catalyzed by various acids and can be carried out in either aqueous or organic solvent. On laboratory scale, germane can be prepared by the reaction of Ge(IV) compounds with these hydride reagents.[4][5] A typical synthesis involved the reaction of potassium hydrogen germanate with potassium borohydride.[6]

Page Module:Chem2/styles.css has no content.K+HGeO−3 + K+[BH4]− + H2O → KGeH3 + K+[B(OH)4]−
Page Module:Chem2/styles.css has no content.KGeH3 + CH3COOH → GeH4 + CH3COO−K+

Other methods for the synthesis of germane include electrochemical reduction and a plasma-based method.[7] The electrochemical reduction method involves applying voltage to a germanium metal cathode immersed in an aqueous electrolyte solution and an anode counter-electrode composed of a metal such as molybdenum or cadmium. In this method, germane and hydrogen gases evolve from the cathode while the anode reacts to form solid molybdenum oxide or cadmium oxides. The plasma synthesis method involves bombarding germanium metal with hydrogen atoms (H) that are generated using a high frequency plasma source to produce germane and digermane.

Reactions

Germane is weakly acidic. In liquid ammonia GeH4 is ionised forming NH4+ and GeH3−.[8] With alkali metals in liquid ammonia GeH4 reacts to give white crystalline MGeH3 compounds. The potassium (potassium germyl or potassium trihydrogen germanide KGeH3) and rubidium compounds (rubidium germyl or rubidium trihydrogen germanide RbGeH3) have the sodium chloride structure implying a free rotation of the trihydrogen germanide anion GeH3−, the caesium compound, caesium germyl or caesium trihydrogen germanide CsGeH3 in contrast has the distorted sodium chloride structure of TlI.[8]

Use in semiconductor industry

The gas decomposes near 600K (327°C; 620°F) to germanium and hydrogen. Because of its thermal lability, germane is used in the semiconductor industry for the epitaxial growth of germanium by MOVPE or chemical beam epitaxy.[9] Organogermanium precursors (e.g. isobutylgermane, alkylgermanium trichlorides, and dimethylaminogermanium trichloride) have been examined as less hazardous liquid alternatives to germane for deposition of Ge-containing films by MOVPE.[10]

Safety

Germane is a highly flammable, potentially pyrophoric,[11] and a highly toxic gas. In 1970, the American Conference of Governmental Industrial Hygienists (ACGIH) published the latest changes and set the occupational exposure threshold limit value at 0.2 ppm for an 8-hour time weighted average.[12] The LC50 for rats at 1 hour of exposure is 622 ppm.[13] Inhalation or exposure may result in malaise, headache, dizziness, fainting, dyspnea, nausea, vomiting, kidney injury, and hemolytic effects.[14][15][16]

The US Department of Transportation hazard class is 2.3 Poisonous Gas.[12]

References

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  1. ^ a b c d e Page Module:Citation/CS1/styles.css has no content.NIOSH Pocket Guide to Chemical Hazards. "#0300". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Page Module:Citation/CS1/styles.css has no content.Yaws, Carl L. (1997), Handbook Of Viscosity: Volume 4: Inorganic Compounds And Elements, Gulf Professional Publishing, ISBN 978-0123958501
  3. ^ Page Module:Citation/CS1/styles.css has no content.Kunde, V.; Hanel, R.; Maguire, W.; Gautier, D.; Baluteau, J. P.; Marten, A.; Chedin, A.; Husson, N.; Scott, N. (1982). "The tropospheric gas composition of Jupiter's north equatorial belt (NH3, PH3, CH3D, GeH4, H2O) and the Jovian D/H isotopic ratio". Astrophysical Journal. 263: 443–467. Bibcode:1982ApJ...263..443K. doi:10.1086/160516.
  4. ^ W. L. Jolly "Preparation of the Volatile Hydrides of Groups IVA and VA by Means of Aqueous Hydroborate" Journal of the American Chemical Society 1961, volume 83, pp. 335-7.
  5. ^ Page Module:Citation/CS1/styles.css has no content."US Patent 4,668,502". Archived from the original on 2017-07-14. Retrieved 2008-10-22.
  6. ^ Page Module:Citation/CS1/styles.css has no content.Girolami, G. S.; Rauchfuss, T. B.; Angelici, R. J. (1999). Synthesis and Technique in Inorganic Chemistry. Mill Valley, CA: University Science Books.
  7. ^ US Patent 7,087,102 (2006)
  8. ^ a b Page Module:Citation/CS1/styles.css has no content.Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
  9. ^ Page Module:Citation/CS1/styles.css has no content.Venkatasubramanian, R.; Pickett, R. T.; Timmons, M. L. (1989). "Epitaxy of germanium using germane in the presence of tetramethylgermanium". Journal of Applied Physics. 66 (11): 5662–5664. Bibcode:1989JAP....66.5662V. doi:10.1063/1.343633.
  10. ^ Page Module:Citation/CS1/styles.css has no content.Woelk, E.; Shenai-Khatkhate, D. V.; DiCarlo, R. L. Jr.; Amamchyan, A.; Power, M. B.; Lamare, B.; Beaudoin, G.; Sagnes, I. (2006). "Designing Novel Organogermanium MOVPE Precursors for High-purity Germanium Films". Journal of Crystal Growth. 287 (2): 684–687. Bibcode:2006JCrGr.287..684W. doi:10.1016/j.jcrysgro.2005.10.094.
  11. ^ Brauer, 1963, Vol.1, 715
  12. ^ a b Praxair MSDS Script error: No such module "webarchive". accessed Sep. 2011
  13. ^ NIOSH Germane Registry of Toxic Effects of Chemical Substances (RTECS)accessed Sep. 2011
  14. ^ Page Module:Citation/CS1/styles.css has no content.Gus'kova, E. I. (1974). "K toksikologii Gidrida Germaniia" [Toxicology of germanium hydride]. Gigiena Truda I Professionalnye Zabolevaniia (in Russian). 18 (2): 56–57. PMID 4839911.{{cite journal}}: CS1 maint: unrecognized language (link)
  15. ^ US EPA Germane
  16. ^ Page Module:Citation/CS1/styles.css has no content.Paneth, F.; Joachimoglu, G. (1924). "Über die pharmakologischen Eigenschaften des Zinnwasserstoffs und Germaniumwasserstoffs" [About the pharmacological characteristics of tin hydride and germanium hydride]. Berichte der Deutschen Chemischen Gesellschaft (in German). 57 (10): 1925–1930. doi:10.1002/cber.19240571027.{{cite journal}}: CS1 maint: unrecognized language (link)

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Look up germane in Wiktionary, the free dictionary.

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