-from-xtal-view-1-tilt-3D-bs-17.png) | |
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| Names | |
|---|---|
| Other names decaborane decaboron tetradecahydride | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.037.904 |
| EC Number |
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| UNII | |
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| Properties | |
| B10H14 | |
| Molar mass | 122.22 g/mol |
| Appearance | White crystals |
| Odor | bitter,chocolate-like or burntrubber[1] |
| Density | 0.94 g/cm3[1] |
| Melting point | 97–98 °C (207–208 °F; 370–371 K) |
| Boiling point | 213 °C (415 °F; 486 K) |
| Solubility in other solvents | Slightly, in cold water.[1] |
| Vapor pressure | 0.2 mmHg[1] |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | may ignite spontaneously on exposure to air[1] |
| GHS labelling: | |
    | |
| Danger | |
| H228,H301,H310,H316,H320,H330,H335,H336,H370,H372 | |
| P210,P240,P241,P260,P261,P262,P264,P270,P271,P280,P284,P301+P310,P302+P350,P304+P340,P305+P351+P338,P307+P311,P310,P312,P314,P320,P321,P322,P330,P332+P313,P337+P313,P361,P363,P370+P378,P403+P233,P405,P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | 80 °C; 176 °F; 353 K |
| 149 °C (300 °F; 422 K) | |
| Lethal dose or concentration (LD, LC): | |
LC50 (median concentration) | 276 mg/m3 (rat, 4 hr) 72 mg/m3 (mouse, 4 hr) 144 mg/m3 (mouse, 4 hr)[2] |
| NIOSH (US health exposure limits): | |
PEL (Permissible) | TWA 0.3 mg/m3 (0.05 ppm) [skin][1] |
REL (Recommended) | TWA 0.3 mg/m3 (0.05 ppm) ST 0.9 mg/m3 (0.15 ppm) [skin][1] |
IDLH (Immediate danger) | 15 mg/m3[1] |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Decaborane, also calleddecaborane(14), is theinorganic compound with thechemical formulaB10H14. It is classified as aborane and more specifically aboron hydride cluster. This white crystalline compound is one of the principal boron hydride clusters, both as a reference structure and as a precursor to other boron hydrides. It is toxic and volatile, giving off a foul odor, like that of burnt rubber or chocolate.
The physical characteristics of decaborane(14) resemble those ofnaphthalene andanthracene, all three of which are volatile colorless solids.Sublimation is the common method of purification. Decaborane is highly flammable, and burns with a bright green flame like otherboron hydrides. It is not sensitive to moist air, although it hydrolyzes in boiling water, releasing hydrogen and giving a solution ofboric acid. It is soluble in cold water as well as a variety of non-polar and moderately polarsolvents.[3]
In decaborane, the B10 framework resembles an incompleteoctadecahedron. Each boron atom has one "radial" hydride, and four boron atoms near the open part of the cluster feature extra bridging hydrides. In the language of cluster chemistry, the structure is classified as "nido".
It is commonly synthesized via thepyrolysis of smaller boron hydrideclusters. For example, pyrolysis ofB2H6 orB5H9 gives decaborane, with loss of H2.[4] On a laboratory scale, sodium borohydride is treated with boron trifluoride to give NaB11H14, which is acidified to release borane and hydrogen gas.[3]
It reacts with Lewis bases (L) such asCH3CN andEt2S, to form adducts:[5][6]
These species, which are classified as "arachno" clusters, in turn react withacetylene to give the "closo"ortho-carborane:
Decaborane(14) is a weakBrønsted acid. Monodeprotonation generates theanion [B10H13]−, with again a nido structure.
In theBrellochs reaction, decaborane is converted to arachno-CB9H14−:
Decaborane has no significant commercial applications, although the compound has often been investigated. It and its derivatives were investigated as an additive to special high-performancerocket fuels. Its derivates were investigated as well, e.g. ethyl decaborane.[citation needed]
Decaborane is an effective reagent for thereductive amination of ketones and aldehydes.[7]
Decaborane has been assessed for low energyion implantation of boron in the manufacture ofsemiconductors. It has also been considered forplasma-assistedchemical vapor deposition for the manufacture of boron-containingthin films. In fusion research, theneutron-absorbing nature of boron has led to the use of these thin boron-rich films to "boronize" the walls of thetokamak vacuum vessel to reduce recycling of particles and impurities into the plasma and improve overall performance.[8] It has been evaluated in the context ofnuclear fusion.[9]
Decaborane, likepentaborane, is a powerful toxin affecting thecentral nervous system, although decaborane is less toxic than pentaborane. It can be absorbed through skin.
Purification by sublimation require a dynamic vacuum to remove evolved gases. Crude samples explode near 100 °C.[6]
It forms an explosive mixture withcarbon tetrachloride, which caused an often-mentioned explosion in a manufacturing facility.[10]
In crystalline form, it reacts violently withred andwhite fuming nitric acid which has a use as rocket fuel oxidizer, producing an extremely powerful detonation.[11]
YouTube video name: 'The Most DESTRUCTIVE Chemical Reaction from two NON-explosive components'
