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Boranes is the name given to the class of synthetic hydrides of boron with generic formula BxHy. The molecules of these compounds are electron deficient and so are highly reactive with respect to electron-pair donors. The lower boranes are pyrophoric in air and react violently with water. The boranes belong to the class of cluster compounds which have been the subject of developments in chemical bonding theory. A large number of the related anionic hydridoborates have also been synthesized.

Contents

HistoryEdit

The development of the chemistry of boranes presented a number of challenges. First, new laboratory techniques had to be developed to handle these often pyrophoric compounds Alfred Stock created the glass vacuum line, now known as a Schlenk line, for synthesis and handling. The very reactive nature of the lower boranes meant that crystal structure determination was impossible before William Lipscomb developed the requisite techniques. Lastly, once the structures were known it became clear that new theories of chemical bonding were needed to explain them. Lipscomb was awarded the Nobel prize in Chemistry in 1976 for his achievements in this field.

The correct structure of diborane was predicted by H. Christopher Longuet-Higgins[1] 5 years before its determination. PSEPT (Wades rules) can be used to predict the structures of boranes.[2]

Interest in boranes increased during World War II due to the potential of uranium borohydride for enrichment of the uranium isotopes. In the US, a team led by Schlesinger developed the basic chemistry of the boron hydrides and the related aluminium hydrides. Although uranium borohydride was not utilized for isotopic separations, Schlesinger's work laid the foundation for a host of boron hydride reagents for organic synthesis, most of which were developed by his student Herbert C. Brown. Borane-based reagents are now widely used in organic synthesis. Brown was awarded the Nobel prize in Chemistry in 1979 for this work.[3]

Chemical formula and naming conventionsEdit

Boranes clusters are classified as follows, where n is the number of boron atoms in a single cluster:[4][5]

Cluster type Chemical formula Example Notes
hypercloso- BnHn Unstable; derivatives are known[6]
closo- BnHn2− Caesium dodecaborate
nido- BnHn+4 pentaborane(9)
arachno- BnHn+6 pentaborane(11)
hypho- BnHn+8 Only found in adducts
Multi-cluster descriptors[7]
Prefix Meaning Example
Klado- Branched clusters
Conjuncto- Conjoined clusters
Megalo- Multiple conjoined clusters

The International Union of Pure and Applied Chemistry rules for systematic naming is based on a Greek prefix denoting a class of compound, followed by the number (in Greek) of boron atoms and the number of hydrogen atoms in parentheses. Various details can be omitted if there is no ambiguity about the meaning, for example, if only one structural type is possible. Some examples of the structures are shown below.

The naming of anions is illustrated by

octahydridopentaborate, B5H8

The hydrogen count is specified first followed by the boron count. The -ate suffix is applied with anions. The ionic charge value is included in the chemical formula, but not is not part of the systematic name.

Bonding in boranesEdit

Boranes are electron-deficient compounds, that is, there are not enough electrons to form 2-centre, 2-electron bonds between all pairs of adjacent atoms in the molecule. A description of the bonding in the larger boranes was formulated by William Lipscomb. It involved:

  • 3-center 2-electron B-H-B hydrogen bridges
  • 3-center 2-electron B-B-B bonds
  • 2-center 2-electron bonds (in B-B, B-H and BH2)

Lipscomb's methodology has largely been superseded by a molecular orbital approach. This allows the concept of multi-centre bonding to be extended. For example, in the icosahedral ion [B12H12]2-, the totally symmetric (Ag symmetry) molecular orbital is equally distributed among all 12 boron atoms. Wade's rules provide a powerful method that can be used to rationalize the structures in terms of the number of atoms and the connectivity between them.

There are continuing efforts by theoretical chemists to improve the treatment of the bonding in boranes – an example is Stone's tensor surface harmonic treatment of cluster bonding.[8] A recent development is four-center two-electron bond.

Reactivity of boranesEdit

The lowest borane, BH3 is a very strong Lewis acid. While the molecule itself is unstable with respect to dimerization, the adducts BH3.THF and BH3.DMSO are stable enough to be used in hydroboration reactions. Other boranes are electron-deficient compounds and react vigorously with reagents that can supply electron pairs to form molecules that are not electron-deficient. With an alkali metal hydride, for example,

B2H6 + 2 H- → 2 BH4-

The reaction of the lower boranes with air is so strongly exothermic that it is explosive with all but the smallest quantities. This does not result from any inherent instability in the boranes. Rather, it is a consequence of the fact that a combustion product, boron trioxide, is a solid. For example

B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(g)

The formation of the solid releases additional energy to what is released by the oxidation reaction. By contrast, many closo- borane anions, such as B12H122- do not react with air; salts of these anions are metastable because the closo- structure creates a very high activation energy barrier to oxidation.

The higher boranes can be deprotonated when treated with a very strong base. For example,

B5H9 + NaH → Na(B5H8) + H2

They can also act as weak acids. For example, pentaborane(9) reacts with trimethylphosphine

B5H9 + 2 PMe3 → B5H9(PMe3)2

producing what can be regarded as a derivative of the unknown hypho-borane B5H13. Acidity increases with the size of the borane.[9] B10H14 has a pK value of 2.7 temperature not stated.

B5H9 < B6H10 < B10H14 < B16H20 < B18H22

Reaction of a borane with the transient BH3, produced by dissociation of B2H6, can lead to the formation of a conjuncto- borane species in which two small borane sub-units are joined by the sharing of boron atoms.[10]

B6H10 + (BH3) → B7H11 + H2
B7H11 + B6H10 → B13H19 + H2

Other conjuncto- boranes, where the sub-units are joined by a B-B bond can be made by ultra violet irradiation of nido-boranes. Some B-B coupled conjuncto-boranes can be produced using PtBr2 as catalyst.[11]

Reaction of a borane with an alkyne can produce a carborane; the icosahedral closo-carboranes C2B10H12, are particularly stable.[12]

Boranes can function as ligands in coordination compounds.[13] Hapticities of η1 to η6 have been found, with electron donation involving bridging H atoms or donation from B-B bonds. For example, nido-B6H10 can replace ethene in Zeise's salt to produce Fe(η2-B6H10)(CO)4.

ApplicationsEdit

The main chemical application of boranes is the hydroboration reaction. Commerically available adducts such as borane–tetrahydrofuran or borane–dimethylsulfide are often used in this context as they have comparable effectiveness but without the hazard of handling highly reactive BH3 itself.

Neutron capture therapy of cancer is a promising development.[14] The compound used is the HS (bisulfide) derivative Na2[B12H11(SH)]. It makes use of the fact that 10B has a very high neutron-capture cross section, so neutron irradiation is highly selective for the region where the compound resides.

10B + 1n → (11B*) → 4He + 7Li + γ (2.4 Mev)

See alsoEdit

ReferencesEdit

  1. ^ Longuet-Higgins, H. C.; Bell, R. P. (1943). "64. The Structure of the Boron Hydrides". Journal of the Chemical Society (Resumed). 1943: 250–255. doi:10.1039/JR9430000250. 
  2. ^ Fox, Mark A.; Wade, Ken (2003). "Evolving patterns in boron cluster chemistry" (PDF). Pure Appl. Chem. 75 (9): 1315–1323. doi:10.1351/pac200375091315. 
  3. ^ Brown, H. C. Organic Syntheses via Boranes John Wiley & Sons, Inc. New York: 1975. ISBN 0-471-11280-1.
  4. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.  pp 151-195
  5. ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 
  6. ^ Peymann, Toralf; Knobler, Carolyn B.; Khan, Saeed I.; Hawthorne, M. Frederick (2001). "Dodeca(benzyloxy)dodecaborane, B12(OCH2Ph)12: A Stable Derivative of hypercloso-B12H12". Angew. Chem. Int. Ed. 40 (9): 1664–1667. doi:10.1002/1521-3773(20010504)40:9<1664::AID-ANIE16640>3.0.CO;2-O. 
  7. ^ Bould, Jonathan; Clegg, William; Teat, Simon J.; Barton, Lawrence; Rath, Nigam P.; Thornton-Pett, Mark; Kennedy, John D. (1999). "An approach to megalo-boranes. Mixed and multiple cluster fusions involving iridaborane and platinaborane cluster compounds. Crystal structure determinations by conventional and synchrotron methods". Inorganica Chimica Acta. 289 (1-2): 95–124. doi:10.1016/S0020-1693(99)00071-7. 
  8. ^ Ceulemans, Arnout; Geert, Mys (1994). "The vector particle of tensor surface harmonic theory". Chemical Physics Letters. 219 (3-4): 274–278. doi:10.1016/0009-2614(94)87057-8. 
  9. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.  p. 171
  10. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.  p. 162
  11. ^ Sneddon, L.G. (2009). "Transition metal promoted reactions of polyhedral boranes and carboranes". Pure and Applied Chemistry. 59 (7): 837–846,. doi:10.1351/pac198759070837. 
  12. ^ Jemmis, E. D. (1982). "Overlap control and stability of polyhedral molecules. Closo-Carboranes". Journal of the American Chemical Society. 104 (25): 7017–7020. doi:10.1021/ja00389a021. 
  13. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9. p. 177, "The concept of boranes as ligands",
  14. ^ Sauerwein, Wolfgang; Wittig, Andrea; Moss, Raymond; Nakagawa, Yoshinobu (2012). Neutron Capture Therapy. Berlin: Springer. doi:10.1007/978-3-642-31334-9. ISBN 978-3-642-31333-2.