Bromine
| Bromine Symbol | Br |
| Bromine Atomic Number | 35 |
| Bromine Atomic Mass | 79.904 g.mol-1 |
| Discovered by | Johan Gottlieb Gahn |
Table of Contents
- What is Bromine?
- Chemical Properties Of Bromine
- Uses of Bromine
- Properties Of Bromine
- Certain Facts About Bromine
- Frequently Asked Questions
What is Bromine?
- Bromine is an element with the appearance of deep red colour. It is noxious liquid. And it is one of the members of halogen elements.
- This element has an appreciable vapour pressure at room temperature.
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] 4s² 3d¹⁰ 4p⁵ | CAS number | 7726-95-6 |
| ChemSpider ID | 4514586 | ChemSpider is a free chemical structure database | |
Uses of Bromine
Some major uses of bromine have been discussed below:
- Bromine is a good oxidising agent like other chlorine water and is more useful as it does not decompose readily.
- It also liberates free iodine from iodide- containing solutions and sulphur from hydrogen sulphide.
- Sulphurous acid is oxidised to sulphuric 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 oxidising 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 chlorine.
- It is a less powerful oxidising 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 vapours 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 – FAQs
Q1
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
Q2
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.
Q3
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.
Q4
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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