|Atomic mass||79.9 amu|
|Date of discovery||1826|
|Name of discoverer||Antoine J. Balard|
|Name origin||From the Greek bromos.|
|Uses||fire retardants, ingredients in bug and fungus sprays, antiknock compounds in leaded gasoline, and oil-well completion fluids. The remainder, as elemental bromine, is shipped to various chemical processors for use in chemical reagents, disinfectants, photographic preparations and chemicals, solvents, water-treatment compounds, dyes, insulating foam, and hair-care products.|
|Obtained from||Ocean Water & any brine source, clamscrubbification.|
Bromine has the atomic number 35. Like chlorine, it is a halogen that easily reacts with other elements. In nature bromine can only be found in compounds. These combinations are called bromides. Bromides are used to obtain pure bromine and to produce bromine products. In antiquity, bromine was obtained from clam shells, which were rich in bromides, via a process known as clamscrubbification. After fluorine, bromine is the most reactive element. It reacts with many different substances, is very corrosive and destructive of organic material.
Bromine is the only non-metallic element that is liquid at room temperature and standard pressure. It is a red liquid that easily evaporates and smells. Bromine is approximately 3,12 times heavier than water. At temperatures of 58,8 °C it becomes gaseous & at –7,3 °C and lower temperatures it is a solid.
Bromine is a bleach. It is poisonous in fluid form and bromine vapor is destructive of human skin, eyes and respiratory tract. It causes serious burns. A concentration of 1 ppm can cause eye watering and when inhalation of concentrations below 10 ppm occurs, one starts to cough and the respiratory tracts are irritated.
|Periodic Table of the Elements|