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| General |
| Name, Symbol, Number |
bromine, Br, 35 |
| Chemical series |
halogens |
| Group, Period, Block |
17, 4, p |
| Appearance |
gas/liquid: red-brown
solid: metallic luster
 |
| Atomic mass |
79.904(1) g/mol |
| Electron configuration |
[Ar] 3d10 4s2 4p5 |
| Electrons per shell |
2, 8, 18, 7 |
| Physical properties |
| Phase |
liquid |
| Density (near r.t.) |
(liquid) 3.1028 g/cm³ |
| Melting point |
265.8 K
(-7.3 °C, 19 °F) |
| Boiling point |
332.0 K
(58.8 °C, 137.8 °F) |
| Heat of fusion |
(Br2) 10.57 kJ/mol |
| Heat of vaporization |
(Br2) 29.96 kJ/mol |
| Heat capacity |
(25 °C) (Br2)
75.69 J/(mol·K) |
Vapor pressure
| P/Pa |
1 |
10 |
100 |
1 k |
10 k |
100 k |
| at T/K |
185 |
201 |
220 |
244 |
276 |
332 |
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| Atomic properties |
| Crystal structure |
orthorhombic |
| Oxidation states |
±1, 5
(strongly acidic oxide) |
| Electronegativity |
2.96 (Pauling scale) |
Ionization energies
(more) |
1st: 1139.9 kJ/mol |
| 2nd: 2103 kJ/mol |
| 3rd: 3470 kJ/mol |
| Atomic radius |
115 pm |
| Atomic radius (calc.) |
94 pm |
| Covalent radius |
114 pm |
| Van der Waals radius |
185 pm |
| Miscellaneous |
| Magnetic ordering |
nonmagnetic |
| Electrical resistivity |
(20 °C) 7.8×1010 Ω·m |
| Thermal conductivity |
(300 K) 0.122 W/(m·K) |
| Speed of sound |
(20 °C) ? 206 m/s |
| CAS registry number |
7726-95-6 |
| Notable isotopes |
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| References |
Bromine (from Gr. Bromos, meaning "stench"), is a chemical element in the periodic table that has the symbol Br and atomic number 35. A halogen element, bromine is a red volatile liquid at room temperature which has a reactivity between chlorine and iodine. This element is harmful to human tissue in a liquid state and its vapor irritates eyes and throat.
Notable characteristics
Bromine is the only liquid nonmetallic element at room temperature. It is a heavy, mobile, reddish-brown liquid, that evaporates easily at standard temperature and pressures in a red vapor (its color resembles nitrogen dioxide) that has a strong disagreeable odor resembling that of chlorine. A halogen, bromine resembles chlorine chemically but is less active (it is more active than iodine however). Bromine is slightly soluble in water, and highly soluble in carbon disulfide, aliphatic alcohols (such as methanol), and acetic acid. It bonds easily with many elements and has a strong bleaching action.
Bromine is highly reactive and is a powerful oxidizing agent in the presence of water. It reacts vigorously with amines, alkenes and phenols as well as aliphatic and aromatic hydrocarbons, ketones and acids (these are brominated by either addition or substitution). With many of the metals and elements, anhydrous bromine is less reactive than wet bromine; however, dry bromine reacts vigorously with aluminium, titanium, mercury as well as alkaline earth metals and alkaline metals.
Applications
Elemental bromine is used to manufacture a wide variety of bromine compounds used in industry and agriculture. Traditionally the largest use of bromine was in the production of 1,2-Dibromoethane which in turn was used as a gasoline anti-knock agent for leaded gasolines before they were largely phased out due to environmental considerations.
Bromine is also used in making fumigants, flameproofing agents, water purification compounds, dyes, medicinals, sanitizes, inorganic bromides for photography, etc. It is also used to form intermediates in organic synthesis, where it is preferred to iodine due to its much lower cost.
Bromine is used to make brominated vegetable oil, which is used as an emulsifier in many citrus-flavored soft drinks.
Aqueous bromine is orange and can be used in tests for alkenes and phenols.
- When added to an alkene it will lose its color as it reacts forming a colorless bromoalkane.
- When added to phenol a white precipitate (2,4,6-tribromophenol) will form.
History
Bromine (Gr. bromos for stench) was discovered by Antoine Balard at salt marshes of Montpellier in 1826 but was not produced in quantity until 1860.
Occurrence
Bromine occurs in nature as bromide salts in very diffuse amounts in crustal rock. Due to leaching bromide salts have accumulated in sea water (85 ppm), and may be economically recovered from brine wells and the Dead Sea (up to 5000 ppm).
Approximately 500 million kilograms ($350 million USD) of bromine are produced per year (2001) worldwide with the United States and Israel being the primary producers.
Precautions
Elemental bromine is a strong irritant and, in concentrated form, will produce painful blisters on exposed skin and especially mucous membranes. Even low concentrations of bromine vapor (from 10 ppm) can affect breathing, and inhalation of significant amounts of bromine can seriously damage the respiratory system.
Accordingly, one should always wear safety goggles and ensure adequate ventilation when handling bromine.
Recycling
Because of its high cost, bromine is usually recycled rather than disposed of into the environment.
References
External links
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