Chemical elements
  Boron
    Isotopes
    Energy
    Production
    Application
    Physical properties
    Chemical properties
      Boron Hydrides
      Tetraborodecahydride
      Borobutane
      Hexaborododecahydride
      Borohexylene
      Boron trihydride
      Boro-ethane
      Decaborotetradecahydride
      Boron halogen
      Boron trifluoride
      Hydrofluoboric acid
      Potassium borofluoride
      Fluoboric acid
      Perfluoboric acid
      Boron subchloride
      Boron trichloride
      Boron tribromide
      Boron tri-iodide
      Oxides of Boron
      Tetraboron trioxide
      Boron dioxide
      Tetraboron pentoxide
      Borohydrates
      Hypoborates
      Boron sesqui-oxide
      Boron trioxide
      Boric anhydride
      Boric Acids
      Orthoboric acid
      Boric acid
      Boracic acid
      Complex Boric Acids
      Perboric Acid and Perborates
      Sodium perborate
      Sodium hyperborate
      Potassium perborate
      Rubidium perborate
      Ammonium perborate
      Barium perborate
      Boron sesquisulphide
      Boron trisulphide
      Boron pentasulphide
      Boron selenide
      Boron nitride
      Boron amide
      Boron imide
      Boron phosphide
      Boron phospho-iodides
      Boron carbide
      Boron thiocyanate
      Boron Alkyls
      Boron trimethyl
      Boron Silicides and
      Boroethane

Boron Hydrides






The existence of solid Boron Hydrides or Hydroboronshas been suspected by various chemists. The existence of a volatile hydride was long ago anticipated from analogy with the compounds of other non-metallic elements; but neither Wohler and Deville nor Gustavson succeeded in preparing it. In 1879, F. Jones showed that a volatile boron hydride did exist, and two years later, F. Jones and Taylor studied the hydride and assigned to it the formula BH3. Their work was confirmed in a qualitative way by Sabatier. Later, Bamsay and Hatfield announced the existence of what were, in their opinion, probably two isomeric hydrides of the formula B3H3, but Bamsay was unable subsequently to duplicate the work. No value can be placed upon the scanty experimental data which served to deduce the preceding formulae, since the gaseous boron hydrides were undoubtedly contaminated with silicon hydride.

The hydrides prepared by Jones and Taylor, Sabatier, and Bamsay and Hatfield were obtained, mixed with a very large excess of hydrogen, by the action of dilute acids on magnesium boride, and similar gaseous mixtures can be obtained by the action of acids upon commercial iron and manganese borides. From the mixed gases produced from magnesium boride and hydrochloric acid, Stock and Massenez in 1912 succeeded in isolating two distinct boron hydrides of molecular formulae B4H10 and B6H12; and since then Stock and others have obtained several more boron hydrides. Although the compound BH3 is not yet known, there are, according to Stock, Friederici, and Priess, at least ten boron hydrides: -
  1. B2H6. Obtained by heating B4H10. Colourless gas.
  2. B4H10. Obtained from magnesium boride and hydrochloric acid.
  3. A colourless liquid, very unstable, obtained like (1).
  4. B6H12. Obtained like (2).
  5. B10H14. Obtained like (1); also by heating (1).
  6. Non-volatile solid, soluble in CS2. Obtained like (1).
  7. Non-volatile yellow solid, insoluble in CS2. Obtained like (1), and by heating (6).
  8. Difficultly volatile liquid, obtained by heating (6).
  9. Colourless, non-volatile solid, insoluble in CS2. Obtained by heating (1).
  10. Brown hydride or hydrides, resembling boron and poor in hydrogen content. Obtained by heating (7).


The starting-point in the preparation of the boron hydrides is crude magnesium boride, made by mixing 1 part of very finely powdered boron sesqui-oxide with 3 parts of magnesium powder and rapidly heating the mixture, 10 grams at a time, in a thin sheet-iron crucible in a stream of hydrogen. The product, quickly cooled in hydrogen, is finely powdered, sifted, and slowly dropped into 15 per cent, hydrochloric acid at 50° to 80°, a slow stream of hydrogen being passed through the apparatus. The evolved gases, dried over calcium chloride and phosphoric anhydride, are passed through U-tubes cooled in liquid air; in them the boron hydrides B4H10 and B6H12 solidify, together with a little carbon dioxide and silicon hydrides.

The distillation of this crude product furnishes in order the following fractions: (i.) silicon hydride, SiH4, (ii.) carbon dioxide, (iii.) silicon hydride, Si2H6, (iv.) boron hydride, B4H10, (v.) boron hydride, B6H12, (vi.) residue of less volatile boron and silicon hydrides. The two hydrides B4H10 and B6H12 are obtained as follows: - At the temperature of liquid air the pressure above the solid is reduced to zero. Traces of hydrogen and silicon hydride are thus removed. The temperature is then raised to - 80°, when the solid melts. The pressure is quickly lowered to a few millimetres, and the evolved gas rejected as long as it contains silicon hydride. The gas then evolved at - 80° and 3 mm. consists of the hydride B4H10, and, unless the room temperature is above 20°, partly condenses in the mercury pump. The residue is distilled at -40° until the pressure falls to 1.5 mm., the temperature raised to 0°, and distillation continued until the pressure is only 10 mm. All the hydride B4H10 has then been removed, and the residue, on further distillation, gives another hydride, B6H12, the pressure falling to less than 5 mm.

From 200 grams of magnesium boride, 100 c.c. (at N.T.P.) of pure hydride B4H10 and 60 milligrams of hydride B6H12 may be obtained.


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