Decaborane

Decaborane

Names
Other names decaborane decaboron tetradecahydride
Identifiers
CAS Number	17702-41-9 Y
ChemSpider	21241886 Y
EC Number	241-711-8
Jmol 3D model	Interactive image
InChI InChI=1S/B10H14/c11-5-1-2-3(1,5)7(2,9(3,5,11)13-7)8(2)4(1,2)6(1,5)10(4,8,12-6)14-8/h1-10H Y Key: XAMMYYSPUSIWAS-UHFFFAOYSA-N Y InChI=1/B10H14/c11-5-1-2-3(1,5)7(2,9(3,5,11)13-7)8(2)4(1,2)6(1,5)10(4,8,12-6)14-8/h1-10H Key: XAMMYYSPUSIWAS-UHFFFAOYAD
SMILES [H]1[BH]234[BH]156[BH]278[BH]39([H]4)[BH]712[BH]853[BH]645[BH]311[BH]922[BH]14([H]5)[H]2
Properties
Molar mass	122.22 g/mol
Appearance	White crystals
Odor	bitter, chocolate-like
Density	0.94 g/cm3
Melting point	99.6 °C (211.3 °F; 372.8 K)
Boiling point	213 °C (415 °F; 486 K)
Solubility in other solvents	Slightly, in cold water. [1]
Vapor pressure	0.2 mmHg
Vapor pressure	{{{value}}}
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Decaborane, also called decaborane(14), is the borane with the chemical formula B₁₀H₁₄. 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.

Handling properties and structure

B₁₀H₁₄ possesses a strong characteristic odor, sometimes described as musty or intensely bitter, chocolate-like that is unique to boranes. The physical characteristics of decaborane(14) resemble those of the organic compounds, such as naphthalene and anthracene, in that it can be sublimed under vacuum at moderate temperatures. Sublimation is the common method of purification. Like organic compounds, decaborane is highly flammable, but, like other boron hydrides, it burns with a bright green flame. It is not sensitive to moist air, although it hydrolyzes in boiling water, releasing hydrogen and giving a solution of boric acid. It is soluble in cold water as well as a variety of non-polar and moderately polar solvents.

In decaborane, the B₁₀ framework resembles an incomplete octadecahedron. Each boron has one "radial" hydride, and four boron atoms near the open part of the cluster feature extra hydrides. In the language of cluster chemistry, the structure is classified as "nido".

Synthesis and reactions

It is commonly synthesized via the pyrolysis of smaller boron hydride clusters. For example, heating B₂H₆ or B₅H₉ gives decaborane, with loss of H₂.

It reacts with Lewis bases (L) such as CH₃CN and Me₂S, to form derivatives with the formula B₁₀H₁₂·2L.

B₁₀H₁₄ + 2 L → B₁₀H₁₂L₂ + H₂

These species, which are classified as "arachno" clusters, in turn react with acetylene to give the "closo" ortho-carborane:

B₁₀H₁₂·2L + C₂H₂ → C₂B₁₀H₁₂ + 2 L + H₂

It is a weak Brønsted acid. Monodeprotonation generates the anion [B₁₀H₁₃]⁻, with again a nido structure.

Applications

Decaborane has no significant applications, although it has often been investigated. Since the molecule decomposes in a plasma, yielding monatomic boron ions, decaborane is potentially useful as a fuel for aneutronic fusion, and for low energy ion implantation of boron in the manufacture of semiconductors. It has also been considered for plasma-assisted chemical vapor deposition for the manufacture of boron-containing thin films. In fusion research, the neutron-absorbing nature of boron has led to the use of these thin boron-rich films to "boronize" the walls of the tokamak vacuum vessel to reduce recycling of particles and impurities into the plasma and improve overall performance.

Decaborane was also developed as an additive to special high-performance rocket fuels. Its derivates were investigated as well, e.g. ethyl decaborane. One patented fuel composition included vinyl decaborane-polyester copolymer. Vinyl decaborane ("dekene") is prepared by reacting decaborane with acetylene.

Safety

Decaborane, like pentaborane, is a powerful toxin affecting the central nervous system, although decaborane is less toxic than pentaborane. It can be absorbed through skin. It forms an explosive mixture with carbon tetrachloride, which caused an often mentioned explosion in a Malta, New York, manufacturing facility in 1948 when CCl₄ was used to clean the equipment.