Silane

Short description: Chemical compound (SiH4)

Silane

| Ball-and-stick model of silane | Spacefill model of silane

|

Names
IUPAC name

Silane

Systematic IUPAC name

Silicane

Other names

* Monosilane
* Silicon(IV) hydride
* Silicon tetrahydride

Identifiers

CAS Number

* 7803-62-5 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:29389 Y

ChemSpider |

* 22393 Y

Gmelin Reference

| 273

PubChem CID

* 23953

RTECS number |

* VV1400000

UNII |

* 5J076063R1 Y

UN number | 2203

InChI

* InChI=1S/SiH4/h1H4 Y

Key: BLRPTPMANUNPDV-UHFFFAOYSA-N Y

* InChI=1/SiH4/h1H4

Key: BLRPTPMANUNPDV-UHFFFAOYAE

SMILES

* [SiH4]

Properties

Chemical formula

| H4Si
Molar mass | 32.117 g·mol−1
Appearance  | Colourless gas
Odor | Repulsive[1]
Density | 1.313 g/L[2]
Melting point |  −185 °C (−301.0 °F; 88.1 K)[2]
Boiling point |  −111.9 °C (−169.4 °F; 161.2 K)[2]

Solubility in water

| Reacts slowly[2]
Vapor pressure | >1 atm (20 °C)[1]
Conjugate acid | Silanium (sometimes spelled silonium)
Structure

Molecular shape

| Tetrahedral
r(Si-H) = 1.4798 Å[3]

Dipole moment

| 0 D
Thermochemistry[4]

Heat capacity (C)

| 42.81 J/mol·K

Std molar
entropy (S ~~o~~ 298)

| 204.61 J/mol·K

Std enthalpy of
formation (ΔfH⦵298)

| 34.31 kJ/mol

Gibbs free energy (ΔfG˚)

| 56.91 kJ/mol
Hazards
Main hazards | Extremely flammable, pyrophoric in air
Safety data sheet | ICSC 0564
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H220, H280

GHS precautionary statements

| PP210Script error: No such module "Preview warning".Category:GHS errors, PP222Script error: No such module "Preview warning".Category:GHS errors, PP230Script error: No such module "Preview warning".Category:GHS errors, PP280Script error: No such module "Preview warning".Category:GHS errors, PP377Script error: No such module "Preview warning".Category:GHS errors, PP381Script error: No such module "Preview warning".Category:GHS errors, PP403Script error: No such module "Preview warning".Category:GHS errors, PP410+P403Script error: No such module "Preview warning".Category:GHS errors
NFPA 704 (fire diamond)  |

Flash point | Not applicable, pyrophoric gas

Autoignition
temperature

| ~ 18 °C (64 °F; 291 K)
Explosive limits | 1.37–100%
NIOSH (US health exposure limits):

PEL (Permissible)

| None[1]

REL (Recommended)

| TWA 5 ppm (7 mg/m3)[1]

IDLH (Immediate danger)

| N.D.[1]
Related compounds

Related tetrahydride compounds

| Methane
Germane
Stannane
Plumbane

Related compounds

| Phenylsilane
Vinylsilane
Disilane
Trisilane

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

Y verify (what is YN ?)
Infobox references

Silane (Silicane) is an inorganic compound with chemical formula SiH
4. It is a colourless, pyrophoric, toxic gas with a sharp, repulsive, pungent smell, somewhat similar to that of acetic acid.[5] Silane is of practical interest as a precursor to elemental silicon. Silane with alkyl groups are effective water repellents for mineral surfaces such as concrete and masonry. Silanes with both organic and inorganic attachments are used as coupling agents. Silanes are commonly used to apply coatings to surfaces or as an adhesion promoter.[6]

## Contents

* 1 Production
* 1.1 Commercial-scale routes
* 1.2 Laboratory-scale routes
* 2 Properties
* 3 Applications
* 4 Safety and precautions
* 5 See also
* 6 References
* 7 Cited sources
* 8 External links

## Production

### Commercial-scale routes

Silane can be produced by several routes.[7] Typically, it arises from the reaction of hydrogen chloride with magnesium silicide:

MgA2Si+4HCl⟶2MgClA2+SiHA4

It is also prepared from metallurgical-grade silicon in a two-step process. First, silicon is treated with hydrogen chloride at about 300 °C to produce trichlorosilane, HSiCl3, along with hydrogen gas, according to the chemical equation

Si+3HCl⟶HSiClA3+HA2

The trichlorosilane is then converted to a mixture of silane and silicon tetrachloride:

4HSiClA3⟶SiHA4+3SiClA4

This redistribution reaction requires a catalyst.

The most commonly used catalysts for this process are metal halides, particularly aluminium chloride. This is referred to as a redistribution reaction, which is a double displacement involving the same central element. It may also be thought of as a disproportionation reaction, even though there is no change in the oxidation number for silicon (Si has a nominal oxidation number IV in all three species). However, the utility of the oxidation number concept for a covalent molecule[vague], even a polar covalent molecule, is ambiguous.[citation needed] The silicon atom could be rationalized as having the highest formal oxidation state and partial positive charge in SiCl
4 and the lowest formal oxidation state in SiH
4, since Cl is far more electronegative than is H.[citation needed]

An alternative industrial process for the preparation of very high-purity silane, suitable for use in the production of semiconductor-grade silicon, starts with metallurgical-grade silicon, hydrogen, and silicon tetrachloride and involves a complex series of redistribution reactions (producing byproducts that are recycled in the process) and distillations. The reactions are summarized below:

Si+2HA2+3SiClA4⟶4SiHClA3
2SiHClA3⟶SiHA2ClA2+SiClA4
2SiHA2ClA2⟶SiHClA3+SiHA3Cl
2SiHA3Cl⟶SiHA4+SiHA2ClA2

The silane produced by this route can be thermally decomposed to produce high-purity silicon and hydrogen in a single pass.

Still other industrial routes to silane involve reduction of silicon tetrafluoride (SiF
4) with sodium hydride (NaH) or reduction of SiCl
4 with lithium aluminium hydride (LiAlH
4).

Another commercial production of silane involves reduction of silicon dioxide (SiO
2) under Al and H
2 gas in a mixture of NaCl and aluminum chloride (AlCl
3) at high pressures:[8]

3SiOA2+6HA2+4Al⟶3SiHA4+2AlA2OA3

### Laboratory-scale routes

In 1857, the German chemists Heinrich Buff and Friedrich Woehler discovered silane among the products formed by the action of hydrochloric acid on aluminum silicide, which they had previously prepared. They called the compound siliciuretted hydrogen.[9]

For classroom demonstrations, silane can be produced by heating sand with magnesium powder to produce magnesium silicide (Mg
2Si), then pouring the mixture into hydrochloric acid. The magnesium silicide reacts with the acid to produce silane gas, which burns on contact with air and produces tiny explosions.[10] This may be classified as a heterogeneous[clarification needed] acid–base chemical reaction, since the isolated Si4− ion in the Mg
2Si antifluorite structure can serve as a Brønsted–Lowry base capable of accepting four protons. It can be written as

4HCl+MgA2Si⟶SiHA4+2MgClA2

In general, the alkaline-earth metals form silicides with the following stoichiometries: MII

2Si, MII
Si, and MII

2. In all cases, these substances react with Brønsted–Lowry acids to produce some type of hydride of silicon that is dependent on the Si anion connectivity in the silicide. The possible products include SiH
4 and/or higher molecules in the homologous series Si

2n+2, a polymeric silicon hydride, or a silicic acid. Hence, MII
Si with their zigzag chains of Si2− anions (containing two lone pairs of electrons on each Si anion that can accept protons) yield the polymeric hydride (SiH

Yet another small-scale route for the production of silane is from the action of sodium amalgam on dichlorosilane, SiH
2Cl
2, to yield monosilane along with some yellow polymerized silicon hydride (SiH)
x.[11]

## Properties

Silane is the silicon analogue of methane. All four Si–H bonds are equal and their length is 147.98 pm.[12] Because of the greater electronegativity of hydrogen in comparison to silicon, this Si–H bond polarity is the opposite of that in the C–H bonds of methane. One consequence of this reversed polarity is the greater tendency of silane to form complexes with transition metals. A second consequence is that silane is pyrophoric — it undergoes spontaneous combustion in air, without the need for external ignition.[13] However, the difficulties in explaining the available (often contradictory) combustion data are ascribed to the fact that silane itself is stable and that the natural formation of larger silanes during production, as well as the sensitivity of combustion to impurities such as moisture and to the catalytic effects of container surfaces causes its pyrophoricity.[14][15] Above 420 °C, silane decomposes into silicon and hydrogen; it can therefore be used in the chemical vapor deposition of silicon.

The Si–H bond strength is around 384 kJ/mol, which is about 20% weaker than the H–H bond in H2. Consequently, compounds containing Si–H bonds are much more reactive than is H2. The strength of the Si–H bond is modestly affected by other substituents: the Si–H bond strengths are: SiHF3 419 kJ/mol, SiHCl3 382 kJ/mol, and SiHMe3 398 kJ/mol.[16][17]

## Applications

Monosilane gas shipping containers in Japan.

While diverse applications exist for organosilanes, silane itself has one dominant application, as a precursor to elemental silicon, particularly in the semiconductor industry. The higher silanes, such as di- and trisilane, are only of academic interest. About 300 metric tons per year of silane were consumed in the late 1990s. [needs update] [15] Low-cost solar photovoltaic module manufacturing has led to substantial consumption of silane for depositing (PECVD) hydrogenated amorphous silicon (a-Si:H) on glass and other substrates like metal and plastic. The PECVD process is relatively inefficient at materials utilization with approximately 85% of the silane being wasted. To reduce that waste and the ecological footprint of a-Si:H-based solar cells further several recycling efforts have been developed.[18][19]

## Safety and precautions

A number of fatal industrial accidents produced by combustion and detonation of leaked silane in air have been reported.[20][21][22]

Due to weak bonds and hydrogen, silane is a pyrophoric gas (capable of autoignition at temperatures below 54 °C or 129 °F).[23]

SiHA4+2OA2⟶SiOA2+2HA2O ΔH=−1517 kJ/mol =−47.23 kJ/g

SiHA4+OA2⟶SiOA2+2HA2
SiHA4+OA2⟶SiHA2O+HA2O
2SiHA4+OA2⟶2SiHA2O+2HA2
SiHA2O+OA2⟶SiOA2+HA2O

For lean mixtures a two-stage reaction process has been proposed, which consists of a silane consumption process and a hydrogen oxidation process. The heat of SiO
2(s) condensation increases the burning velocity due to thermal feedback.[24]

Diluted silane mixtures with inert gases such as nitrogen or argon are even more likely to ignite when leaked into open air, compared to pure silane: even a 1% mixture of silane in pure nitrogen easily ignites when exposed to air.[25]

In Japan, in order to reduce the danger of silane for amorphous silicon solar cell manufacturing, several companies began to dilute silane with hydrogen gas. This resulted in a symbiotic benefit of making more stable solar photovoltaic cells as it reduced the Staebler–Wronski effect[citation needed].

Unlike methane, silane is fairly toxic: the lethal concentration in air for rats (LC50) is 0.96% (9,600 ppm) over a 4-hour exposure. In addition, contact with eyes may form silicic acid with resultant irritation.[26]

In regards to occupational exposure of silane to workers, the US National Institute for Occupational Safety and Health has set a recommended exposure limit of 5 ppm (7 mg/m3) over an eight-hour time-weighted average.[27]

## See also

* Binary silicon-hydrogen compounds (sometimes called silanes)
* Silanization
* Magnesium silicide
* Methane, in which Carbon (in that compound) and Silicon (in this compound) are together in the Carbon group.

## References

1. ↑ 1.0 1.1 1.2 1.3 1.4 NIOSH Pocket Guide to Chemical Hazards. "#0556". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0556.html.
2. ↑ 2.0 2.1 2.2 2.3 Haynes, p. 4.87
3. ↑ Haynes, p. 9.29
4. ↑ Haynes, p. 5.14
5. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
6. ↑ London, Gábor; Carroll, Gregory T.; Feringa, Ben L. (2013). "Silanization of quartz, silicon and mica surfaces with light-driven molecular motors: construction of surface-bound photo-active nanolayers" (in en). Organic & Biomolecular Chemistry 11 (21): 3477–3483. doi:10.1039/c3ob40276b. ISSN 1477-0520. PMID 23592007. http://xlink.rsc.org/?DOI=c3ob40276b.
7. ↑ Simmler, W.. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a24_001.
8. ↑ Shriver and Atkins. Inorganic Chemistry (5th edition). W. H. Freeman and Company, New York, 2010, p. 358.
9. ↑ Mellor, J. W. "A Comprehensive Treatise on Inorganic and Theoretical Chemistry", vol. VI, Longmans, Green and Co. (1947), p. 216.
10. ↑ "Making Silicon from Sand". Popular Science. https://theodoregray.com/PeriodicTable/PopularScience/2005/10/1/index.html. .
11. ↑ Mellor, J. W. "A Comprehensive Treatise on Inorganic and Theoretical Chemistry", vol. VI. Longmans, Green and Co. (1947), pp. 970–971.
12. ↑ "Maintenance". NIST. 17 October 2019. https://cccbdb.nist.gov/exp2x.asp?casno=7803625&charge=0.
13. ↑ Emeléus, H. J.; Stewart, K. (1935). "The oxidation of the silicon hydrides". Journal of the Chemical Society: 1182–1189. doi:10.1039/JR9350001182.
14. ↑ Koda, S. (1992). "Kinetic Aspects of Oxidation and Combustion of Silane and Related Compounds". Progress in Energy and Combustion Science 18 (6): 513–528. doi:10.1016/0360-1285(92)90037-2.
15. ↑ 15.0 15.1 Timms, P. L. (1999). "The chemistry of volatile waste from silicon wafer processing". Journal of the Chemical Society, Dalton Transactions (6): 815–822. doi:10.1039/a806743k.
16. ↑ M. A. Brook "Silicon in Organic, Organometallic, and Polymer Chemistry" 2000, J. Wiley, New York. ISBN 0-471-19658-4.
17. ↑ "Standard Bond Energies". Michigan State University Organic Chemistry. https://www2.chemistry.msu.edu/faculty/reusch/virttxtjml/questions/bndenrgy.htm.
18. ↑ Briend P, Alban B, Chevrel H, Jahan D. American Air, Liquide Inc. (2009) "Method for Recycling Silane (SiH4)". US20110011129 , EP2252550A2 .
19. ↑ Kreiger, M.A.; Shonnard, D.R.; Pearce, J.M. (2013). "Life cycle analysis of silane recycling in amorphous silicon-based solar photovoltaic manufacturing". Resources, Conservation and Recycling 70: 44–49. doi:10.1016/j.resconrec.2012.10.002. https://www.academia.edu/2310926.
20. ↑ Chen, J. R. (2002). "Characteristics of fire and explosion in semiconductor fabrication processes". Process Safety Progress 21 (1): 19–25. doi:10.1002/prs.680210106.
21. ↑ Chen, J. R.; Tsai, H. Y.; Chen, S. K.; Pan, H. R.; Hu, S. C.; Shen, C. C.; Kuan, C. M.; Lee, Y. C. et al. (2006). "Analysis of a silane explosion in a photovoltaic fabrication plant". Process Safety Progress 25 (3): 237–244. doi:10.1002/prs.10136.
22. ↑ Chang, Y. Y.; Peng, D. J.; Wu, H. C.; Tsaur, C. C.; Shen, C. C.; Tsai, H. Y.; Chen, J. R. (2007). "Revisiting of a silane explosion in a photovoltaic fabrication plant". Process Safety Progress 26 (2): 155–158. doi:10.1002/prs.10194.
23. ↑ Silane MSDS
24. ↑ V.I Babushok (1998). "Numerical Study of Low and High Temperature Silane Combustion". The Combustion Institute 27 (2): 2431–2439. doi:10.1016/S0082-0784(98)80095-7.
25. ↑ Kondo, S.; Tokuhashi, K.; Nagai, H.; Iwasaka, M.; Kaise, M. (1995). "Spontaneous Ignition Limits of Silane and Phosphine". Combustion and Flame 101 (1–2): 170–174. doi:10.1016/0010-2180(94)00175-R.
26. ↑ "MSDS for silane". http://www.vngas.com/pdf/g97.pdf.
27. ↑ "Silicon tetrahydride". NIOSH Pocket Guide to Chemical Hazards. Centers for Disease Control and Prevention. April 4, 2011. https://www.cdc.gov/niosh/npg/npgd0556.html.

## Cited sources

* Haynes, William M., ed (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1439855119.

## External links

* US Patent 2474087A, Preparation of silicon halides

* v
* t
* e

Silicon compounds

Si(II)|

* SiO
* SiS

Si(IV)|

* SiBr4
* SiC
* SiCl4
* SiF4
* SiH4
* SiI4
* SiO2
* SiS2
* Si3N4

* v
* t
* e

Molecules detected in outer space

Molecules|

| Diatomic|

* Aluminium monochloride
* Aluminium monofluoride
* Aluminium monoxide
* Argonium
* Carbon monophosphide
* Carbon monosulfide
* Carbon monoxide
* Carborundum
* Cyanogen radical
* Diatomic carbon
* Fluoromethylidynium
* Helium hydride ion
* Hydrogen chloride
* Hydrogen fluoride
* Hydrogen (molecular)
* Hydroxyl radical
* Iron(II) oxide
* Magnesium monohydride cation
* Methylidyne radical
* Nitric oxide
* Nitrogen (molecular)
* Nitrogen monohydride
* Nitrogen sulfide
* Oxygen (molecular)
* Phosphorus monoxide
* Phosphorus mononitride
* Potassium chloride
* Silicon carbide
* Silicon mononitride
* Silicon monoxide
* Silicon monosulfide
* Sodium chloride
* Sodium iodide
* Sulfur monohydride
* Sulfur monoxide
* Titanium oxide

|
|

Triatomic|

* Aluminium hydroxide
* Aluminium isocyanide
* Amino radical
* Carbon dioxide
* Carbonyl sulfide
* CCP radical
* Chloronium
* Diazenylium
* Dicarbon monoxide
* Disilicon carbide
* Ethynyl radical
* Formyl radical
* Hydrogen cyanide (HCN)
* Hydrogen isocyanide (HNC)
* Hydrogen sulfide
* Hydroperoxyl
* Iron cyanide
* Isoformyl
* Magnesium cyanide
* Magnesium isocyanide
* Methylene radical
* N2H+
* Nitrous oxide
* Nitroxyl
* Ozone
* Phosphaethyne
* Potassium cyanide
* Protonated molecular hydrogen
* Sodium cyanide
* Sodium hydroxide
* Silicon carbonitride
* c-Silicon dicarbide
* SiNC
* Sulfur dioxide
* Thioformyl
* Thioxoethenylidene
* Titanium dioxide
* Tricarbon
* Water

Four
atoms|

* Acetylene
* Ammonia
* Cyanic acid
* Cyanoethynyl
* Cyclopropynylidyne
* Formaldehyde
* Fulminic acid
* HCCN
* Hydrogen peroxide
* Hydromagnesium isocyanide
* Isocyanic acid
* Isothiocyanic acid
* Ketenyl
* Methylene amidogen
* Methyl radical
* Propynylidyne
* Protonated carbon dioxide
* Protonated hydrogen cyanide
* Silicon tricarbide
* Thioformaldehyde
* Tricarbon monoxide
* Tricarbon sulfide
* Thiocyanic acid

Five
atoms|

* Ammonium ion
* Butadiynyl
* Carbodiimide
* Cyanamide
* Cyanoacetylene
* Cyanoformaldehyde
* Cyanomethyl
* Cyclopropenylidene
* Formic acid
* Isocyanoacetylene
* Ketene
* Methane
* Methoxy radical
* Methylenimine
* Propadienylidene
* Protonated formaldehyde
* Protonated formaldehyde
* Silane
* Silicon-carbide cluster

Six
atoms|

* Acetonitrile
* Cyanobutadiynyl radical
* E-Cyanomethanimine
* Cyclopropenone
* Diacetylene
* Ethylene
* Formamide
* HC4N
* Ketenimine
* Methanethiol
* Methanol
* Methyl isocyanide
* Pentynylidyne
* Propynal
* Protonated cyanoacetylene

Seven
atoms|

* Acetaldehyde
* Acrylonitrile
* Vinyl cyanide
* Cyanodiacetylene
* Ethylene oxide
* Glycolonitrile
* Hexatriynyl radical
* Methylacetylene
* Methylamine
* Methyl isocyanate
* Vinyl alcohol

Eight
atoms|

* Acetic acid
* Aminoacetonitrile
* Cyanoallene
* Ethanimine
* Glycolaldehyde
* Heptatrienyl radical
* Hexapentaenylidene
* Methylcyanoacetylene
* Methyl formate
* Propenal

Nine
atoms|

* Acetamide
* Cyanohexatriyne
* Cyanotriacetylene
* Dimethyl ether
* Ethanol
* Methyldiacetylene
* Octatetraynyl radical
* Propene
* Propionitrile

Ten
atoms
or more|

* Acetone
* Benzene
* Benzonitrile
* Buckminsterfullerene (C60, C60+, fullerene, buckyball)
* C70 fullerene
* Cyanodecapentayne
* Cyanopentaacetylene
* Cyanotetra-acetylene
* Ethylene glycol
* Ethyl formate
* Methyl acetate
* Methyl-cyano-diacetylene
* Methyltriacetylene
* Propanal
* n-Propyl cyanide
* Pyrimidine

Deuterated
molecules|

* Ammonia
* Ammonium ion
* Formaldehyde
* Formyl radical
* Heavy water
* Hydrogen cyanide
* Hydrogen deuteride
* Hydrogen isocyanide
* Methylacetylene
* N2D+
* Trihydrogen cation

Unconfirmed|

* Anthracene
* Dihydroxyacetone
* Ethyl methyl ether
* Glycine
* Graphene
* H2NCO+
* Linear C5
* Naphthalene cation
* Phosphine
* Pyrene
* Silylidine

Related|

* Abiogenesis
* Astrobiology
* Astrochemistry
* Atomic and molecular astrophysics
* Chemical formula
* Circumstellar envelope
* Cosmic dust
* Cosmic ray
* Cosmochemistry
* Diffuse interstellar band
* Earliest known life forms
* Extraterrestrial life
* Extraterrestrial liquid water
* Forbidden mechanism
* Homochirality
* Intergalactic dust
* Interplanetary medium
* Interstellar medium
* Photodissociation region
* Iron–sulfur world theory
* Kerogen
* Molecules in stars
* Nexus for Exoplanet System Science
* Organic compound
* Outer space
* PAH world hypothesis
* Panspermia
* Polycyclic aromatic hydrocarbon (PAH)
* RNA world hypothesis
* Spectroscopy
* Tholin

* Category:Astrochemistry
*   *   *

* v
* t
* e

Binary compounds of hydrogen

Alkali metal (Group 1) hydrides|

* LiH
* NaH
* KH
* RbH
* CsH

Lithium hydride, LiH
ionic metal hydride

Beryllium hydride
Left (gas phase): BeH2
covalent metal hydride
Right: (BeH2)n (solid phase)
polymeric metal hydride

Borane and diborane
Left: BH3 (special conditions), covalent metalloid hydride
Right: B2H6 (standard conditions), dimeric metalloid hydride

Methane, CH4
covalent nonmetal hydride

Ammonia, NH3
covalent nonmetal hydride

Water, H2O
covalent nonmetal hydride

Hydrogen fluoride, HF
covalent nonmetal hydride

Alkaline (Group 2) earth hydrides|

| Monohydrides|

* BeH
* MgH
* CaH
* SrH
* BaH

|

Dihydrides|

* BeH2
* MgH2
* CaH2
* SrH2
* BaH2

|

Group 13 hydrides|

| Boranes|

* BH3
* B2H6
* B2H2
* B2H4
* B4H10
* B5H9
* B5H11
* B6H10
* B6H12
* B10H14
* B18H22

|

Alanes|

* AlH3
* Al2H6

|

Gallanes|

* GaH3
* Ga2H6

|

Indiganes|

* InH3
* In2H6

|

Thallanes|

* TlH3
* Tl2H6

|

Group 14 hydrides|

| Linear alkanes|

* CH4
* C2H6
* C3H8
* C4H10
* C5H12
* C6H14
* C7H16
* C8H18
* C9H20
* C10H22
* more...

|

Linear alkenes|

* C2H4
* C3H6
* C4H8
* C5H10
* C6H12
* C7H14
* C8H16
* C9H18
* C10H20
* more...

|

Linear alkynes|

* C2H2
* C3H4
* C4H6
* C5H8
* C6H10
* C7H12
* C8H14
* C9H16
* C10H18
* more...

|

Silanes|

* SiH4
* Si2H6
* Si3H8
* Si4H10
* Si5H12
* Si6H14
* Si7H16
* Si8H18
* Si9H20
* Si10H22
* more...

|

Silenes|

* Si2H4

|

Silynes|

* Si2H2
* SiH

|

Germanes|

* GeH4
* Ge2H6
* Ge3H8
* Ge4H10
* Ge5H12

|

Stannanes|

* SnH4
* Sn2H6

|

Plumbanes|

* PbH4

|

* CH
* CH2
* CH3
* C2H
* Cycloalkanes
* Cycloalkenes
* Annulenes
* Many more

Pnictogen (Group 15) hydrides|

| Azanes|

* NH3
* N2H4
* N3H5
* N4H6
* N5H7
* N6H8
* N7H9
* N8H10
* N9H11
* N10H12
* more...

|

Azenes|

* N2H2
* N3H3
* N4H4

|

Phosphanes|

* PH3
* P2H4
* P3H5
* P4H6
* P5H7
* P6H8
* P7H9
* P8H10
* P9H11
* P10H12
* more...

|

Phosphenes|

* P2H2
* P3H3
* P4H4

|

Arsanes|

* AsH3
* As2H4

|

Stibanes|

* SbH3

|

Bismuthanes|

* BiH3

|

* HN3
* NH
* radical

Hydrogen chalcogenides (Group 16 hydrides)|

| Polyoxidanes|

* H2O
* H2O2
* H2O3
* H2O4
* H2O5
* H2O6
* H2O7
* H2O8
* H2O9
* H2O10
* more...

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Polysulfanes|

* H2S
* H2S2
* H2S3
* H2S4
* H2S5
* H2S6
* H2S7
* H2S8
* H2S9
* H2S10
* more...

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Selanes|

* H2Se
* H2Se2

|

Tellanes|

* H2Te
* H2Te2

|

Polanes|

* PoH2

|

* HO
* HO2
* HO3
* H2O+–O–
* H2S=S
* (HS)2S+–S–
* HS
* HDO
* D2O
* T2O

Hydrogen halides (Group 17 hydrides)|

* HF
* HCl
* HBr
* HI
* HAt

Transition metal hydrides|

* ScH2
* YH2
* YH3
* TiH2
* ZrH2
* HfH2
* VH
* VH2
* NbH
* NbH2
* TaH
* CrH
* CrH2
* CrHx
* NiH
* PdHx (x < 1)
* FeH
* FeH2
* FeH5
* CuH
* ZnH2
* CdH2
* HgH2

Lanthanide hydrides|

* LaH2
* LaH3
* LaH10
* CeH2
* CeH3
* PrH2
* PrH3
* NdH2
* NdH3
* SmH2
* SmH3
* EuH2
* GdH2
* GdH3
* TbH2
* TbH3
* DyH2
* DyH3
* HoH2
* HoH3
* ErH2
* ErH3
* TmH2
* TmH3
* YbH2
* YbH2.5
* LuH2
* LuH3

Actinide hydrides|

* AcH2
* ThH2
* Th4H15
* PaH3
* UH3
* NpH2
* NpH3
* PuH2
* PuH3
* AmH2
* AmH3
* CmH2

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Original source: https://en.wikipedia.org/wiki/Silane. Read more

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*[CID]: Compound ID
*[H220]: Extremely flammable gas
*[H280]: Contains gas under pressure: may explode if heated
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