Bromine, with the chemical symbol Br and atomic number 35, is a reddish-brown liquid at room temperature, making it unique among the halogens, which are typically gases or solids. It has an atomic weight of 79.904 and exhibits several oxidation states, including -1, +1, +3, +4, +5, and +7.

Bromine is highly reactive, particularly with organic compounds, and is known for its strong, irritating odor. It is less abundant in the Earth's crust but is more commonly found in seawater as bromide ions. Commercially, bromine is extracted from brine pools through a process that involves the oxidation of bromide ions using chlorine gas.

Chemical Properties:

• Electronegativity: 2.96 (Pauling scale)
• Oxidation States: -1, +1, +3, +4, +5, +7
• Electron Configuration: [Ar] 3d^10 4s^2 4p^5

Occurrence and Production:

• Natural Occurrence: Bromine is relatively rare in the Earth's crust but is more abundant in seawater, where it is present as bromide ions (Br-). It can also be found in certain minerals.
• Commercial Production: Bromine is typically extracted from brine pools (saltwater) through a process involving the oxidation of bromide ions

Uses:

• Flame Retardants: One of the most common uses of bromine is in the manufacture of flame retardants.
• Pesticides: Bromine compounds are used in some pesticides and fumigants.
• Water Treatment: Bromine is used in water treatment, particularly in swimming pools and hot tubs, as a disinfectant.
• Pharmaceuticals: Some bromine compounds are used in the pharmaceutical industry.
• Photography: Silver bromide (AgBr) is used in photographic film.

Safety and Handling:

• Toxicity: Bromine is highly toxic and can be harmful if inhaled, ingested, or comes into contact with skin.
• Handling Precautions: Appropriate safety measures include using gloves, goggles, and protective clothing
• Environmental Impact: Bromine compounds can have significant environmental effects, particularly related to the depletion of ozone in the stratosphere.