Borane
Chemical compound From Wikipedia, the free encyclopedia
Borane is an inorganic compound with the chemical formula BH
3. Because it tends to dimerize or form adducts, borane is very rarely observed. It normally dimerizes to diborane in the absence of other chemicals.[2] It can be observed directly as a continuously produced, transitory, product in a flow system or from the reaction of laser ablated atomic boron with hydrogen.[3]
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| Names | |||
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| IUPAC names
Borane[1] | |||
| Systematic IUPAC name
Borane (substitutive) Trihydridoboron (additive) | |||
Other names
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| Identifiers | |||
3D model (JSmol) |
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| ChEBI | |||
| ChemSpider | |||
| 44 | |||
PubChem CID |
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| Properties | |||
| BH3 | |||
| Molar mass | 13.83 g·mol−1 | ||
| Appearance | colourless gas | ||
| Conjugate acid | Boronium | ||
| Thermochemistry | |||
Std molar entropy (S⦵298) |
187.88 kJ mol−1 K−1 | ||
Std enthalpy of formation (ΔfH⦵298) |
106.69 kJ mol−1 | ||
| Structure | |||
| D3h | |||
| trigonal planar | |||
| 0 D | |||
| Related compounds | |||
Related compounds |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure and properties
Summarize
Perspective
BH3 is a trigonal planar molecule with D3h symmetry. The experimentally determined B–H bond length is 119 pm.[4]
In the absence of other bases, it dimerizes to form diborane. Thus, it is an intermediate in the preparation of diborane according to the reaction:[5]
- BX3 +BH4− → HBX3− + (BH3) (X=F, Cl, Br, I)
- 2 BH3 → B2H6
The standard enthalpy of dimerization of BH3 is estimated to be −170 kJ mol−1.[6] The boron atom in BH3 has 6 valence electrons. Consequently, it is a strong Lewis acid and reacts with any Lewis base ('L' in equation below) to form an adduct:[7]
- BH3 + L → L—BH3
in which the base donates its lone pair, forming a dative covalent bond. Such compounds are thermodynamically stable, but may be easily oxidised in air. Solutions containing borane dimethylsulfide and borane–tetrahydrofuran are commercially available; in tetrahydrofuran a stabilising agent is added to prevent the THF from oxidising the borane.[8] A stability sequence for several common adducts of borane, estimated from spectroscopic and thermochemical data, is as follows:
BH3 has some soft acid characteristics as sulfur donors form more stable complexes than do oxygen donors.[5] Aqueous solutions of BH3 are extremely unstable.[9][10]
- BH
3 + 3H2O → B(OH)
3 + 3 H
2
Reactions
Summarize
Perspective
Molecular species BH3 is a very strong Lewis acid. It can be isolated in the form of various adducts, such as borane carbonyl, BH3(CO).[11]
Molecular BH3 is believed to be a reaction intermediate in the pyrolysis of diborane to produce higher boranes:[5]
- B2H6 ⇌ 2BH3
- BH3 +B2H6 → B3H7 +H2 (rate determining step)
- BH3 + B3H7 ⇌ B4H10
- B2H6 + B3H7 → BH3 + B4H10
- ⇌ B5H11 + H2
Further steps give rise to successively higher boranes, with B10H14 as the most stable end product contaminated with polymeric materials, and a little B20H26.
Borane ammoniate, which is produced by a displacement reaction of other borane adducts, eliminates elemental hydrogen on heating to give borazine (HBNH)3.[12]
Borane adducts are widely used in organic synthesis for hydroboration, where BH3 adds across the C=C bond in alkenes to give trialkylboranes:[13]
- (THF)BH3 + 3 CH2=CHR → B(CH2CH2R)3 + THF
This reaction is regioselective.[14] Other borane derivatives can be used to give even higher regioselectivity.[15] The product trialkylboranes can be converted to useful organic derivatives. With bulky alkenes one can prepare species such as [HBR2]2, which are also useful reagents in more specialised applications. Borane dimethylsulfide which is more stable than borane–tetrahydrofuran may also be used.[16][15]
Hydroboration can be coupled with oxidation to give the hydroboration-oxidation reaction. In this reaction, the boryl group in the generated organoborane is substituted with a hydroxyl group.[17]
As a Lewis acid
Phosphine-boranes, with the formula R3−nHnPBH3, are adducts of organophosphines and borane. Borane adducts with amines are more widely used.[18] Borane makes a strong adduct with triethylamine; using this adduct requires harsher conditions in hydroboration. This can be advantageous for cases such as hydroborating trienes to avoid polymerization. More sterically hindered tertiary and silyl amines can deliver borane to alkenes at room temperature.
Borane(5) is the dihydrogen complex of borane. Its molecular formula is BH5 or possibly BH3(η2-H2).[19] It is only stable at very low temperatures and its existence is confirmed in very low temperature.[20][21] Borane(5) and methanium (CH5+) are isoelectronic.[22] Its conjugate base is the borohydride anion.
See also
References
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