Bromine - Br

Bromine Symbol Br
Bromine Atomic Number 35
Bromine Atomic Mass 54.9380 g.mol-1
Discovered by Johan Gottlieb Gahn

What is Bromine?

It is the third-largest halogen and at room temperature, it appears as a fuming red-brown liquid. Bromine was discovered by two chemists independently. In the year 1825, Carl Jacob Lowig discovered it whereas Antoine Balard, discovered in the year 1826.

Chemical Properties Of Bromine

Group 17 Melting point −7.2°C, 19°F, 266 K
Period 4 Boiling point 58.8°C, 137.8°F, 332 K
Block p Density (g cm−3) 3.1028
Atomic number 35 Relative atomic mass 79.904
State at 20°C Liquid Key isotopes 79Br
Electron configuration [Ar] 3d54s2 CAS number 7726-95-6
ChemSpider ID 4514586 ChemSpider is a free chemical structure database

What is Bromine?

  • Bromine is a chemical element with the appearance of a deep red, noxious liquid being one of the members of the halogen elements of the periodic table.
  • This element has an appreciable vapor pressure at room temperature.

Bromine Uses

Some major uses of bromine have been discussed below:

  • Bromine is a good oxidizing agent like other chlorine water and more useful as it does not decompose readily.
  • It also liberates free iodine from iodide- containing solutions and sulfur from hydrogen sulfide.
  • Sulfurous acid is oxidized to sulfuric acid by bromine water.

Properties Of Bromine

  • The electron affinity of this metal is very high and much similar to the chlorine.
  • It is a less powerful oxidizing agent as compared to the chloride ion and that too because of weaker hydration of the bromide ion.
  • The electron affinity of this metal is very high and much similar to the chlorine.
  • It is a less powerful oxidizing agent as compared to the chloride ion and that too because of weaker hydration of the bromide ion.
  • A metal-bromine bond is also weaker than the corresponding metal-chlorine bond.

Certain Facts About Bromine

  • This element is bleach and is poisonous in fluid form, the vapors of it are dangerous for human skin, eyes and the respiratory tract.
  • It can also cause severe burns, a concentration of 1 ppm can lead to eye-watering and one can start to cough when inhalation of concentration below 10 ppm occurs.

Frequently Asked Questions

What are the uses of bromine?

Several compounds of bromine are very important commercially. A wide variety of organobromine compounds have several industrial applications. Some are prepared from bromine and others are produced from hydrogen bromide (a bromine compound with the formula HBr), which is obtained by burning hydrogen in the presence of bromine. Both alone or in combination with silver iodide and silver chloride, silver bromide is widely used as the light-sensitive component in most photographic emulsions

Is bromine dangerous?

Elemental bromine is extremely toxic to the human body and is known to cause chemical burns on skin and flesh. Similar inflammation of the respiratory tract can occur as a result of the inhalation of bromine gas. The inhalation of elemental bromine in the gaseous form can lead to coughing, shortness of breath, choking, and (if inhaled in a large enough quantity) death. Chronic exposure can lead to repeated bronchial infections and worsening of the overall health of the human body.

What safety measures are usually taken while handling bromine?

Bromine is incompatible with almost all organic and inorganic compounds since it behaves as a very powerful oxidizing agent. Strict caution must be taken whilst transporting bromine. This element is usually transported with the help of steel tanks that are filled with lead and are protected by strong metal frameworks.

How does bromine compare to other halogens?

Bromine is somewhat in the middle when its reactivity is compared to chlorine and iodine. This element can be considered as one of the most reactive elements. Bromine bond energies tend to be lower than chlorine bond energies but higher than iodine bond energies, and bromine is a weaker oxidizing agent than chlorine but a stronger oxidizing agent than iodine. This property of bromine can be observed from the halogens standard electrode potentials

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