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5 berylliumboroncarbon


Name, symbol, number boron, B, 5
Chemical seriesmetalloids
Group, period, block 13, 2, p
Standard atomic weight 10.811(7) g·mol−1
Electron configuration 1s2 2s2 2p1
Electrons per shell 2, 3
Physical properties
Density (near r.t.)2.34 g·cm−3
Liquid density at m.p.2.08 g·cm−3
Melting point2349 K
(2076 °C, 3769 °F)
Boiling point4200 K
(3927 °C, 7101 °F)
Heat of fusion50.2 kJ·mol−1
Heat of vaporization480 kJ·mol−1
Heat capacity(25 °C) 11.087 J·mol−1·K−1
Vapor pressure
P/Pa 1 10 100 1 k 10 k 100 k
at T/K 2348 2562 2822 3141 3545 4072
Atomic properties
Crystal structurerhombohedral
Oxidation states4,[1] 3, 1[2]
(mildly acidic oxide)
Electronegativity2.04 (Pauling scale)
Ionization energies
1st: 800.6 kJ·mol−1
2nd: 2427.1 kJ·mol−1
3rd: 3659.7 kJ·mol−1
Atomic radius85 pm
Atomic radius (calc.)87 pm
Covalent radius82 pm
Magnetic orderingnonmagnetic
Electrical resistivity(20 °C) 1.5×104Ω·m
Thermal conductivity(300 K) 27.4 W·m−1·K−1
Thermal expansion(25 °C) 5–7 µm·m−1·K−1
Speed of sound (thin rod)(20 °C) 16200 m/s
Bulk modulus(β form) 185 GPa
Mohs hardness9.3
Vickers hardness49000 MPa
CAS registry number7440-42-8
Selected isotopes
Main article: Isotopes of boron
iso NA half-life DM DE (MeV) DP
10B 18.8%* B is stable with 5 neutrons
11B 81.2%* B is stable with 6 neutrons
*Boron-10 content may be as low as 19.1% and as
high as 20.3% in natural samples. Boron-11 is
the remainder in such cases.
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Boron (pronounced /ˈbɔərɒn/) is a chemical element with atomic number 5 and the chemical symbol B. Boron is a trivalent nonmetallic element which occurs abundantly in the evaporite ores borax and ulexite. Boron is never found as a free element in nature.

Several allotropes of boron exist; amorphous boron is a brown powder, though crystalline boron is black, hard (9.3 on Mohs' scale), and a weak conductor at room temperature.

Elemental boron is used as a dopant in the semiconductor industry, while boron compounds play important roles as light structural materials, nontoxic insecticides and preservatives, and reagents for chemical synthesis.

Boron is an essential plant nutrient, although soil concentrations of > 1.0 ppm can cause marginal and tip necrosis in leaves as well as poor overall growth performance. Levels as low as 0.8 ppm can cause these same symptoms to appear in plants particularly sensitive to boron in the soil. Nearly all plants, even those somewhat tolerant of boron in the soil, will show at least some symptoms of boron toxicity when boron in the soil is greater than 1.8 ppm. When boron in the soil exceeds 2.0 ppm, few plants will perform well. Plants sensitive to boron in the soil may not survive. When boron levels in plant tissue exceed 200 ppm symptoms of boron toxicity are likely to appear. As an ultratrace element, boron is necessary for the optimal health of animals, though its physiological role in animals is poorly understood.



Brown amorphous boron is a product of certain chemical reactions. It contains boron atoms randomly bonded to each other without long range order.

Crystalline boron, a very hard black material with a high melting point, exists in many polymorphs. Two rhombohedral forms, α-boron and β-boron containing 12 and 106.7 atoms in the rhombohedral unit cell respectively, and 50-atom tetragonal boron are the three most characterised crystalline forms.

Optical characteristics of crystalline/elemental boron include the transmittance of infrared light. At standard temperatures, elemental boron is a poor electrical conductor, but is a good electrical conductor at high temperatures.

Chemically boron is electron-deficient, possessing a vacant p-orbital. It is an electrophile. Compounds of boron often behave as Lewis acids, readily bonding with electron-rich substances to compensate for boron's electron deficiency. The reactions of boron are dominated by such requirement for electrons. Also, boron is the least electronegative non-metal, meaning that it is usually oxidized (loses electrons) in reactions.

Boron is also similar to carbon with its capability to form stable covalently bonded molecular networks. Boron is also used for heat resistant alloys. Boron forms a polyatomic B(II), such as B2F4.[3]


  • In automobiles: it is proposed that by reacting water with elemental boron, hydrogen could be produced to be burnt in an internal combustion engine or fed to a fuel cell to generate electricity.[4]

10B and 11B NMR spectroscopy

Both 10B (18.8 percent) and 11B (81.2 percent) possess nuclear spin; that of boron-10 has a value of 3 and that of boron-11, 3/2. These isotopes are, therefore, of use in nuclear magnetic resonance spectroscopy; and spectrometers specially adapted to detecting the boron-11 nucleus are available commercially. The boron-10 and boron-11 nuclei also cause splitting in the resonances of attached nuclei.

B-10 depleted boron

The 10B isotope is good at capturing thermal neutrons from cosmic radiation. It then undergoes fission - producing a gamma ray, an alpha particle, and a lithium ion. When this happens inside of an integrated circuit, the fission products may then dump charge into nearby chip structures, causing data loss (bit flipping, or single event upset). In critical semiconductor designs, depleted boron—consisting almost entirely of 11B—is used to avoid this effect, as one of radiation hardening measures. 11B is a by-product of the nuclear industry. 11boron is also a candidate as a fuel for aneutronic fusion.

B-10 enriched boron

The 10B isotope is good at capturing thermal neutrons, and this quality has been used in both radiation shielding and in boron neutron capture therapy where a tumor is treated with a compound containing 10B is attached to a muscle, and the patient treated with a relatively low dose of thermal neutrons which go on to cause energetic and short range alpha radiation in the tissue treated with the boron isotope.

  In nuclear reactors, 10B is used for reactivity control and in emergency shutdown systems. It can serve either function in the form of borosilicate rods or as boric acid. In pressurized water reactors, boric acid is added to the reactor coolant when the plant is shut down for refueling. It is then slowly filtered out over many months as fissile material is used up and the fuel becomes less reactive.

In future manned interplanetary spacecraft, 10B has a theoretical role as structural material (as boron fibers or BN nanotube material) which also would serve a special role in the radiation shield. One of the difficulties in dealing with cosmic rays which are mostly high energy protons, is that some secondary radiation from interaction of cosmic rays and spacecraft structural materials, is in the form of high energy spallation neutrons. Such neutrons can be moderated by materials high in light elements such as structural polyethylene, but the moderated neutrons continue to be a radiation hazard unless actively absorbed in a way which dumps the absorption energy in the shielding, far away from biological systems. Among light elements that absorb thermal neutrons, 6Li and 10B appear as potential spacecraft structural materials able to do double duty in this regard.

Market trend

Estimated global consumption of boron rose to a record 1.8 million tonnes of B2O3 in 2005 following a period of strong growth in demand from Asia, Europe and North America. Boron mining and refining capacities are considered to be adequate to meet expected levels of growth through the next decade. The form in which boron is consumed has changed in recent years. The use of beneficiated ores like colemanite has declined following concerns over arsenic content. Consumers have moved towards the use of refined borates or boric acid that have a lower pollutant content.

Increasing demand for boric acid has led a number of producers to invest in additional capacity. Eti Mine opened a new 100,000 tonnes per year capacity boric acid plant at Emet in 2003. Rio Tinto increased the capacity of its Boron plant from 260,000 tonnes per year in 2003 to 310,000 tonnes per year by May 2005, with plans to grow this to 366,000 tonnes per year in 2006.

Chinese boron producers have been unable to meet rapidly growing demand for high quality borates. This has led to imports of disodium tetraborate growing by a hundredfold between 2000 and 2005 and boric acid imports increasing by 28% per year over the same period.

The rise in global demand has been driven by high rates of growth in fiberglass and borosilicate production. A rapid increase in the manufacture of reinforcement-grade fiberglass in Asia with a consequent increase in demand for borates has offset the development of boron-free reinforcement-grade fiberglass in Europe and the USA. The recent rises in energy prices can be expected to lead to greater use of insulation-grade fiberglass, with consequent growth in the use of boron.

Roskill Consulting Group forecasts that world demand for boron will grow by 3.4% per year to reach 21 million tonnes by 2010. The highest growth in demand is expected to be in Asia where demand could rise by an average 5.7% per year.[5]

Boron compounds

See also: Category:Boron compounds

The most economically important compounds of boron

  • Sodium tetraborate pentahydrate (Na2B4O7 · 5H2O), which is used in large amounts in making insulating fiberglass and sodium perborate bleach,
  • Orthoboric acid (H3BO3) or boric acid, used in the production of textile fiberglass and flat panel displays or eye drops, among many uses, and
  • Sodium tetraborate decahydrate (Na2B4O7 · 10H2O) or borax, used in the production of adhesives, in anti-corrosion systems and many other uses.
  • Boron nitride is a material in which the extra electron of nitrogen (with respect to carbon) in some ways compensates for boron's deficiency of an electron.
  • Boron reacts with ammonia at high temperatures to give a compound called borazole (B3N3H6), also known as inorganic benzene.

Of the several hundred uses of boron compounds, especially notable uses

  • Boron is an essential plant micronutrient.
  • Because of its distinctive green flame, amorphous boron is used in pyrotechnic flares.
  • Boric acid is an important compound used in textile products.
  • Boric acid is also traditionally used as an insecticide, notably against ants, fleas, and cockroaches.
  • Borax is sometimes found in laundry detergent.
  • Boron filaments are high-strength, lightweight materials that are chiefly used for advanced aerospace structures as a component of composite materials, as well as limited production consumer and sporting goods such as golf clubs and fishing rods.
  • Boron is used as a melting point depressant in nickel-chromium braze alloys.
  • Boron slurry is used as an energetic material with very high energy density like rocket fuels and jet engines.
  • Boron compounds show promise in treating arthritis.

Hardest boron compound

Main article: Rhenium diboride

The hardest Boron compound is created synthetically. Rhenium diboride (ReB2) can actually scratch diamond, giving it a higher than 10 rank in the Mohs scale of mineral hardness and making it one of the three hardest substances known to man - the other two being ultrahard fullerite and aggregated diamond nanorods.


Compounds of boron (Arabic Buraq from Persian Burah from Turkish Bor) have been known of for thousands of years. In early Egypt, mummification depended upon an ore known as natron, which contained borates as well as some other common salts. Borax glazes were used in China from 300 AD, and boron compounds were used in glassmaking in ancient Rome.

The element was not isolated until 1808 by Sir Humphry Davy, Joseph Louis Gay-Lussac, and Louis Jacques Thénard, to about 50 percent purity, by the reduction of boric acid with sodium or magnesium. These men did not recognize the substance as an element. It was Jöns Jakob Berzelius in 1824 who identified boron as an element. The first pure boron was produced by the American chemist W. Weintraub in 1909, although this is disputed by some researchers.[6]

It is thought that boron plays several biochemical roles in animals, including humans.[7]


Turkey and the United States are the world's largest producers of boron. Turkey has almost 63% of the world’s boron potential and boron reserves.[8] Boron does not appear in nature in elemental form but is found combined in borax, boric acid, colemanite, kernite, ulexite and borates. Boric acid is sometimes found in volcanic spring waters. Ulexite is a borate mineral that naturally has properties of fiber optics.


Economically important sources are from the ore rasorite (kernite) and tincal (borax ore) which are both found in the Mojave Desert of California, with borax being the most important source there. The largest borax deposits are found in Central and Western Turkey including the provinces of Eskişehir, Kütahya and Balıkesir.

Even a boron-containing natural antibiotic, boromycin, isolated from streptomyces, is known.[9][10]

Pure elemental boron is not easy to prepare. The earliest methods used involve reduction of boric oxide with metals such as magnesium or aluminium. However the product is almost always contaminated with metal borides. (The reaction is quite spectacular though.) Pure boron can be prepared by reducing volatile boron halogenides with hydrogen at high temperatures. The highly pure boron, for the use in semiconductor industry, is produced by the decomposition of diborane at high temperatures and then further purified with the Czochralski process.


Boron occurs in all foods produced from plants. Since 1989 its nutritional value has been argued. The U.S. Department of agriculture conducted an experiment in which postmenopausal women took 3 mg of boron a day. The results showed that boron can reduce excretion of calcium by 44%, and activate estrogen and vitamin D.

The US National Institute of Health quotes this source:

Total daily boron intake in normal human diets ranges from 2.1–4.3 mg boron/kg body weight (bw)/day. "Total boron". Zook EG and Lehman J. J. Assoc. Off Agric. Chem. 48: 850-5 (1965).

See also: Borate minerals.

Analytical quantification

For determination of boron content in food or materials the colorimetric curcumin method is used. Boron has to be transferred to boric acid or borates and on reaction with curcumin in acidic solution a red colored boron-chelate complex, rosocyanine, is formed.


Boron has two naturally-occurring and stable isotopes, 11B (80.1%) and 10B (19.9%). The mass difference results in a wide range of δ11B values in natural waters, ranging from -16 to +59. There are 13 known isotopes of boron, the shortest-lived isotope is 7B which decays through proton emission and alpha decay. It has a half-life of 3.26500x10-22 s. Isotopic fractionation of boron is controlled by the exchange reactions of the boron species B(OH)3 and B(OH)4. Boron isotopes are also fractionated during mineral crystallization, during H2O phase changes in hydrothermal systems, and during hydrothermal alteration of rock. The latter effect species preferential removal of the 10B(OH)4 ion onto clays results in solutions enriched in 11B(OH)3 may be responsible for the large 11B enrichment in seawater relative to both oceanic crust and continental crust; this difference may act as an isotopic signature.

The exotic 17B exhibits a Nuclear halo.


Elemental boron is nontoxic and common boron compounds such as borates and boric acid have low toxicity (approximately similar to table salt with the lethal dose being 2 to 3 grams per kg) and therefore do not require special precautions while handling. Some of the more exotic boron hydrogen compounds, however, are toxic as well as highly flammable and do require special handling care.

See also


  1. ^ W.T.M.L. Fernando, L.C. O'Brien, P.F. Bernath. Fourier Transform Spectroscopy: B4Σ−X4Σ. University of Arizona, Tucson. Retrieved on 2007-12-10.
  2. ^ K.Q. Zhang, B.Guo, V. Braun, M. Dulick, P.F. Bernath. Infrared Emission Spectroscopy of BF and AIF. Retrieved on 2007-12-10.
  3. ^ Compound Descriptions: B2F4. Landol Börnstein Substance/Property Index. Retrieved on 2007-12-10.
  4. ^
  5. ^
  6. ^ (1970) "". Z. Angew. Phys. 29: 277.
  7. ^
  8. ^ Developments in the Ecomomic Sector (of Turkey). Turkish government. Retrieved on 2007-12-21.
  9. ^ R. Hütter, W. Keller-Schien, F. Knüsel, V. Prelog , G. C. Rodgers jr., P. Suter, G. Vogel, W. Voser, H. Zähner (1967). "Stoffwechselprodukte von Mikroorganismen. 57. Mitteilung. Boromycin". Helv. Chim. Acta. 50: 1533–1539. doi:10.1002/hlca.19670500612.
  10. ^ J. D. Dunitz, D. M. Hawley, D. Miklo, D. N. J. White, Yu. Berlin, R. Marui, V. Prelog (1971). "Structure of boromycin". Helv. Chim. Acta. 54: 1709–1713. doi:10.1002/hlca.19710540624.
  • Los Alamos National Laboratory – Boron
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Boron". A list of authors is available in Wikipedia.
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