Bromine is a nonmetallic chemical element with an atomic number of 35 in the periodic table of elements. Its pure elemental form is rarely found in Earth’s crust. Being a member of the halogen elements family of the periodic table with seven valence electrons, bromine is highly reactive and easily makes numerous compounds with the other chemical elements.
Chemical and Physical Properties of Bromine
The symbol in the periodic table of elements: (Br)
Atomic number: 35
Atomic weight (mass): 79.904 g.mol -1
Group number: 17 (Group VIIa of nonmetals)
Color: A dark reddish-brown color
Physical state: A fuming liquid at a room temperature
Electronegativity according to Pauling: 2.8
Density: 3.1 g.cm-3 at 20°C
Melting point: -7.2°C
Boiling point: 58.78°C
Van der Waals radius:
Ionic radius: 0.195 nm (-1)
Most characteristic isotope: Bromine-79 and bromine-81
Electronic shell: [ Ar ] 3d10 4s2 4p5
The energy of the first ionization: 1142.7 kJ.mol -1
Discovery date: In 1825 by Carl Löwig, and in 1826 by Antoine Balard
The reddish-brown liquid of bromine found in nature is a combination of two stable isotopes: bromine-79 (50.54 percent) and bromine-81 (49.46 percent). With the periodic table symbol Br, atomic number 35, and electron configuration [ Ar ] 3d10 4s2 4p5, bromine reaches its boiling point at 58.78°C, while the melting point is achieved at -7.2°C.
Having an atomic mass of 79.904 g.mol -1, bromine is denser than water, but it’s a water-soluble substance. Due to its weight, this gaseous liquid sinks in water. When the red-brown bromide gas reacts with water molecules, hydrobromic acid is produced.
This member of the halogen family of elements in the periodic table, also labeled as Br2, has an electronegativity of 2.8 according to Pauling, whereas the atomic radius according to van der Waals is 0.165 nm. Characterized by a pungent odor, this easily evaporating gaseous substance at room temperature shares the chemical properties with chlorine and iodine. When compounded with phosphorus, arsenic, aluminium, and antimony, bromine forms volatile reactions. In all aggregate states, bromine retains a diatomic molecular structure.
How Was Bromine Discovered?
The Tyrian purple (the royal purple) dye was popular among the ancient civilizations. The first known chemical industry back in the times produced this ancient purple dye. It was composed of 6,6′-dibromoindigo – a bromine compound.
In 1825, the German student Carl Löwig attempted to replace chlorine with chlorine gas from a sample of magnesium bromide-rich water from a swamp near his home in Bad Kreuznach. To conduct this experiment, the Heidelberg student used ether and the process of distillation. The result was a new chemical element – bromine.
Upon realizing this achievement, his professor encouraged Löwig to produce more of this new chemical element. But, while he was concentrating on this feat, somewhere in France, another professor of chemistry was dedicating his time to the analysis of salt marsh waters and flora.
Namely, a year later, in 1825, the French chemist Antoine-Jérôme Balard (1802, Montpellier, Fr. – 1876, Paris) was interested in what would result if he’d distill the chlorine saturated sodium chloride and sodium sulfate crystals from seawater.
Indeed, the liquid nonmetallic element bromine was the result of this experiment as well. Consequently, because Carl Löwig didn’t publish his findings, Antoine-Jérôme Balard was recognized as the scientist who discovered the new element and its properties.
How Did Bromine Get Its Name?
As a result of its sharp and unpleasant smell, bromine was named “βρῶμος”, a Greek word denoting strong stench.
Where Can You Find Bromine?
Even though bromine rarely occurs in nature in its pure elemental form, traces of both soluble and insoluble bromides can be found in Earth’s crust. Due to its high solubility, especially of the bromine ion (Br−), accumulations of this nonmetallic chemical element can be found in the ocean waters. Bromine can be extracted from the ocean waters by performing chemical displacement (oxidation) with carbon tetrachloride and the addition of sulfuric acid:
The deep ocean brine pools, natural bromide salts deposits, brines, and thermal springs are the main locations where bromine is found for commercial exploitation. In addition, the mineral bromyrite is also a source of bromine and its compounds.
Currently, the United States, China, Mexico, Chile, Jordan, Japan, India, Ukraine, and Israel (the Dead Sea) are the world’s leading bromine production countries.
Bromine in Everyday Life
The two stable isotopes of bromine, bromine-79 and bromine-81, have a wide application in the medical realm, particularly in radiotherapy. Due to their sedative properties, bromides of sodium, potassium, calcium, ammonium, strontium, and lithium were widely used at the beginning of the 20th century for the treatment of psychiatric patients.
Having light-sensitive properties, silver bromide (AgBr) is used for making photographic films, while the fire-protective materials are coated with bromine. The use as a fire retardant is also bromine’s widest application in everyday life.
Other commercial uses of bromine include water treatment, water purification, dyes, emulsion in citrus-flavored fruit drinks, as an alternative for chlorine used in swimming pools, etc.
How Dangerous Is Bromine?
Despite the fact that bromine is one of the trace elements in the human body, this chemical substance is highly toxic if inhaled. Characterized by a pungent odor, bromine is easy to detect, so any health hazards can be easily avoided. Although, man-made bromine compounds present an especially hazardous threat to human life and the environment.
Bromism is a syndrome that occurs as a result of bromine poisoning upon exposure to high levels of this chemical substance. This medical condition was a common occurrence due to the administration of potassium bromide, sodium bromide, and lithium bromide to psychiatric patients. These bromine-based sedatives are nowadays restricted and prohibited in many countries.
Bromism symptoms experienced by affected individuals include lung problems (if bromine gas is inhaled), skin irritation, coughing, burns, psychosis, fatigue, nausea, hallucinations, unresponsiveness to anything but pain, thyroid gland damage, or dysfunctionality of the nervous system. The most severe cases of bromism may have fatal effects. (Centers for Disease Control and Prevention (CDC), National Institute for Occupational Safety and Health (NIOSH), Pocket Guide to Chemical Hazards).
Environmental Effects of Bromine
In nature, bromine occurs in many inorganic substances. As this chemical substance is often used in various industries, insecticides, and fire-extinguishers, bromide ions (Br−) can additionally accumulate and contaminate water, air, and food. By releasing free bromine atoms in Earth’s atmosphere, bromine has an especially negative effect on the ozone layer.
Isotopes of Bromine
Bromine has 17 radioisotopes and two stable isotopes: bromine-79 and bromine-81.
|Z||N||Isotopic mass (Da)
[n 2][n 3]
[n 5][n 6]
[n 7][n 8]
|Natural abundance (mole fraction)|
|Excitation energy||Normal proportion||Range of variation|
|70mBr||2292.2(8) keV||2.2(2) s||β+||70Se||(9+)|
|72mBr||100.92(3) keV||10.6(3) s||IT (>99.9%)||72Br||1−|
|74mBr||13.58(21) keV||46(2) min||β+||74Se||4(+#)|
|76mBr||102.58(3) keV||1.31(2) s||IT (99.4%)||76Br||(4)+|
|77mBr||105.86(8) keV||4.28(10) min||IT||77Br||9/2+|
|78Br||35||43||77.921146(4)||6.46(4) min||β+ (99.99%)||78Se||1+|
|78mBr||180.82(13) keV||119.2(10) µs||(4+)|
|79mBr||207.61(9) keV||4.86(4) s||IT||79Br||(9/2+)|
|80Br||35||45||79.9185293(22)||17.68(2) min||β− (91.7%)||80Kr||1+|
|80mBr||85.843(4) keV||4.4205(8) h||IT||80Br||5−|
|81mBr||536.20(9) keV||34.6(28) µs||9/2+|
|82mBr||45.9492(10) keV||6.13(5) min||IT||82Br||2−|
|83mBr||3068.8(6) keV||700(100) ns||(19/2−)|
|84m1Br||320(10) keV||6.0(2) min||β−||84Kr||6−|
|84m2Br||408.2(4) keV||<140 ns||1+|
|87Br||35||52||86.920711(19)||55.65(13) s||β− (97.48%)||87Kr||3/2−|
|β−, n (2.52%)||86Kr|
|88Br||35||53||87.92407(4)||16.29(6) s||β− (93.42%)||88Kr||(2−)|
|β−, n (6.48%)||87Kr|
|88mBr||272.7(3) keV||5.4(7) µs|
|89Br||35||54||88.92639(6)||4.40(3) s||β− (86.2%)||89Kr||(3/2−,5/2−)|
|β−, n (13.8%)||88Kr|
|90Br||35||55||89.93063(8)||1.91(1) s||β− (74.8%)||90Kr|
|β−, n (25.2%)||89Kr|
|91Br||35||56||90.93397(8)||541(5) ms||β− (80%)||91Kr||3/2−#|
|β−, n (20%)||90Kr|
|92Br||35||57||91.93926(5)||0.343(15) s||β− (66.9%)||92Kr||(2−)|
|β−, n (33.1%)||91Kr|
|93Br||35||58||92.94305(32)#||102(10) ms||β− (89%)||93Kr||3/2−#|
|β−, n (11%)||92Kr|
|94Br||35||59||93.94868(43)#||70(20) ms||β− (70%)||94Kr|
|β−, n (30%)||93Kr|
|95Br||35||60||94.95287(54)#||50# ms [>300 ns]||3/2−#|
|96Br||35||61||95.95853(75)#||20# ms [>300 ns]|
|97Br||35||62||96.96280(86)#||10# ms [>300 ns]||3/2−#|
List of Bromine Compounds
As a highly reactive septivalent chemical substance, bromine forms organo-bromides by bonding to carbon. The most prevalent form of this carbon-bromine compound is bromomethane, also labeled as methyl bromide (CH3Br).
Methyl Bromide (CH3Br)
This colorless and odorless gas is considered an ozone-depleting gas when used as a fumigant. Due to this hazardous effect, it was removed from the list of allowed pesticides. In nature, bromomethane is produced by marine life and plants that belong to the cabbage and mustard family of Brassicaceae.
The list of bromine compounds comprises the following compounds with common oxidation numbers of 5, 3, 1, and -1:
- Astatine bromide;
- Brominated flame retardant;
- Bromine azide;
- Bromine dioxide;
- Bromine monochloride;
- Bromine monofluoride;
- Bromine oxide;
- Bromine pentafluoride;
- Bromine trifluoride;
- Chromium(II) bromide;
- Chromium(III) bromide;
- Cyclopentadienyl magnesium bromide;
- Dibromine monoxide;
- Dibromine pentoxide;
- Dibromine trioxide;
- Template:Inorganic bromides;
- Phosphoryl bromide;
- Pyridinium perbromide;
- Scandium bromide;
- Titanium(III) bromide.
The oxidation states of bromine are listed below:
- 0 (elemental bromine, Br2);
- +1 (hypobromite, BrO−);
- +3 (bromite, BrO−2);
- +5 (bromate, BrO−3);
- +7 (perbromate, BrO−4).
5 Interesting Facts and Explanations
- Tennessine (Ts) is an artificially produced chemical element that may also be considered a part of the family of halogens together with bromine (Br), chlorine (Cl), astatine (At), fluorine (F), and iodine (I).
- This chemical element with the symbol Br is also labeled as Br2 (dibromine) or brom.
- Bromryte (or bromargyrite) is a rare natural insoluble silver mineral that is mostly found in Mexico and Chile.
- An ozone-depleting gas is a gaseous chemical substance that lowers the ozone quantities in Earth’s atmosphere.
- There’s a specific way of storing commercial bromine. Namely, it’s stored in lead or Monel metal-coated barrels, or in glass bottles due to the chlorine it contains.
Chemical Property and physical property of element Bromine
Symbol of Bromine: Br
Atomic Number of Bromine: 35
Group of Bromine: Halogen
Crystal Structure of Bromine: Orthorhombic
Atomic Weight of Bromine: 79.904
Shells of Bromine: 2,8,18,7
Orbitals of Bromine: [Ar] 3d10 4s2 4p5
Valence of Bromine: 1,3,5,7
Melting Point of Bromine:
Boiling Point of Bromine:
Electro Negativity of Bromine: 2.96
Covalent Radius of Bromine: 1.14 Å
Ionic Radius of Bromine: 1.96 (-1) Å
Atomic Radius of Bromine: 1.12 Å
Atomic Volume of Bromine: 25.6 cm³/mol
Name Origin of Bromine: Greek: brômos (stench).
Discovered of Bromine By: Antoine J. Balard
Pronounced of Bromine: BRO-meen
Oxydation States of Bromine: (±1),5
Density of Bromine: 3.119 g/cm³
Uses of Bromine: It was once used in large quantities to make a compound that removed lead compound build up in engines burning leaded gasoline. Now it is primarily used in dyes, disinfectants, and photographic chemicals.
Description of Bromine: Colorless, odorless, tasteless rare noble gas.