The chemical element bromine is classed as a halogen and a nonmetal. It was discovered in 1825 by Carl Lðwig (Loewig).
|Classification:||Bromine is a halogen and a nonmetal|
|Melting point:||-7 oC , 277 K|
|Boiling point:||58.9 oC, 332 K|
|Neutrons in most abundant isotope:||44|
|Electron configuration:||[Ar] 3d10 4s2 4p5|
|Density @ 20oC:||3.122 g/cm3|
Compounds, Radii, Conductivities
|Atomic volume:||23.5 cm3/mol|
|Structure:||layers of Br2|
|Specific heat capacity||0.473 J g-1 K-1|
|Heat of fusion||10.57 kJ mol-1 of Br2|
|Heat of atomization||112 kJ mol-1|
|Heat of vaporization||29.96 kJ mol-1 of Br2|
|1st ionization energy||1139.9 kJ mol-1|
|2nd ionization energy||2103.4 kJ mol-1|
|3rd ionization energy||3473.4 kJ mol-1|
|Electron affinity||324.7 kJ mol-1|
|Minimum oxidation number||-1|
|Min. common oxidation no.||-1|
|Maximum oxidation number||7|
|Max. common oxidation no.||5|
|Electronegativity (Pauling Scale)||2.96|
|Polarizability volume||3.1 Å3|
|Reaction with air||none|
|Reaction with 15 M HNO3||–|
|Reaction with 6 M HCl||none, dissolves Br2(aq)|
|Reaction with 6 M NaOH||mild, ⇒ OBr–, Br–|
|Atomic radius||115 pm|
|Ionic radius (1+ ion)||–|
|Ionic radius (2+ ion)||–|
|Ionic radius (3+ ion)||–|
|Ionic radius (1- ion)||182 pm|
|Ionic radius (2- ion)||–|
|Ionic radius (3- ion)||–|
|Thermal conductivity||0.12 W m-1 K-1|
|Electrical conductivity||1.0 x 10-10 S m-1|
|Freezing/Melting point:||-7 oC , 277 K|
Discovery of Bromine
Bromine compounds have been used since ancient times.
In the first century AD Pliny describes one of the world’s first chemical industries: dye factories making Tyrian purple. Tyrian purple (or royal purple) is an ancient purple dye obtained from a marine mollusk. A major component of the dye is the compound 6,6′-dibromoindigo. (1)
Three people are significant in the story of the element bromine’s discovery.
First there’s German chemist Justus von Liebig, one of most famous chemists of his time. Liebig could have been credited with the independent discovery of bromine, but he squandered the opportunity.
In 1825 a salt maker sent Liebig a sample of salt spring waters from the German town of Bad Kreuznach, asking for an analysis.
Only when bromine’s existence had been announced did an anguished Liebig return to the red-brown liquid to study it closely.
He then placed the bottle in his ‘mistakes cupboard’ to remind himself that preconceived ideas ruined his chance of discovering something new and to try not to make the same mistake again. (2), (3), (4), (5)
The next name in the story of bromine is Carl Lðwig (Loewig), who discovered bromine in 1825, while still a chemistry student at Heidelberg University, Germany.
Lðwig’s home town was Bad Kreuznach, where Liebig’s sample had come from. Lðwig had taken water from a salt spring in Bad Kreuznach and added chlorine to the liquid. He shook the solution with ether and found a red-brown substance dissolved in the ether. Lðwig evaporated the ether to leave a red-brown liquid: bromine.
His professor at Heidelberg asked Lðwig to prepare more of this substance for testing. By the time Lðwig had done this it was 1826 and a final name – Antoine Balard – had taken over the story of bromine’s discovery.
In 1824 Antoine Balard, aged 21, was studying the plant life in a salt marsh in Montpellier, France. He became interested in salt deposits he saw and began investigating them.
He took brine (sea water in which salts have been concentrated by evaporation of water) and crystallized salt from it. He took the remaining liquid and saturated it with chlorine.
He then distilled the solution to leave a dark red liquid. (2), (3), (4), (5)
Alert to the possibility that he had found something very interesting, Balard gave the French Academy of Science a sealed envelope containing his initial results in 1824.
He finally published his results in 1826, providing evidence that the substance he had discovered was a new ‘simple body’ – i.e. an element, not a compound. (3)
As first to publish, he became bromine’s discoverer. Ironically, like Liebig, his first idea was that the substance was a compound of chlorine and iodine. (3)
The French Academy named the new element after the Greek bromos for ‘stench’ (6) because bromine, quite simply, stinks.
Appearance and Characteristics
Bromine is poisonous and causes skin burns.
Pure bromine is diatomic, Br2.
Bromine is the only nonmetallic element that is liquid at ordinary temperatures.
It is a dense, reddish-brown liquid which evaporates easily at room temperature to a red vapor with a strong, chlorine-like odor.
Bromine is less reactive than chlorine or fluorine but more reactive than iodine. It forms compounds with many elements and, like chlorine, acts as a bleaching agent.
Uses of Uses of Bromine
Bromine compounds are used as pesticides, dyestuffs, water purification compounds, and as a flame-retardants in plastics.
1,2-dibromoethane is used as an anti-knock agent to raise the octane number of gasoline and allow engines to run more smoothly. This application has declined as a result of environmental legislation.
Potassium bromide is used as a source of bromide ions for the manufacture of silver bromide for photographic film.
Abundance and Isotopes
Abundance earth’s crust: 2.4 parts per million, 0.6 by moles
Abundance solar system: parts per billion by weight, parts per billion by moles
Cost, pure: $5 per 100g
Cost, bulk: $0.15 per 100g
Source: Bromine is obtained from natural brine deposits. Some bromine is still extracted today from seawater, which contains only about 70 ppm.
Isotopes: Bromine has 26 isotopes whose half-lives are known, with mass numbers 68 to 94. Naturally occurring bromine is a mixture of its two stable isotopes and they are found in the percentages shown: 79Br (50.7%) and 81Br (49.3%).
- Tyrian purple.
- Mary Elvira Weeks, The discovery of the elements. XVII. The halogen family., J. Chem. Educ., 1932, 9 (11), p1915.
- A.G. Ruaws, Pharmacokinetics of Bromide Ion — An Overview., Ed Chem. Toxic., 1983, vol. 21, 4 p379.
- J.W. Mellor, A Comprehensive Treatise on Inorganic and Theoretical Chemistry., 1922, vol 2, Longmans, Green and Co., p24.
- Georg Lockemann, J. Chem. Educ., 1959, 36 (5), p222.
- David W. Ball, J. Chem. Educ., 1985, 62 (9), p787.
- M. Bill, L. G. Miller, R. C. Rhew, A. H. Goldstein, Budget of Methyl Bromide in the Atmosphere: Isotopic Constraints., American Geophysical Union, Fall Meeting 2001, abstract #B12A-0113.
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