Bromine has very active chemical properties, located between chlorine and iodine, and can react with almost all elements to form corresponding compounds. Bromine can combine with all metals except precious metals, releasing a large amount of heat.
Oxidation reaction: Bromine is a strong oxidant, and many reactions are caused by its strong oxidizing properties. In the presence of moisture, sulfur dioxide can be oxidized to sulfuric acid and generate hydrogen bromide. In alkaline media, nitrogen compounds such as ammonia and urea are oxidized to form nitrogen.
It reacts with magnesium, silver, lead, and nickel to form an outer layer of bromide, which prevents further reaction to the interior. This protective layer makes lead a useful bromine containing substance. In the process of bromine corroding metals, water plays an important role because bromine hydrolyzes hydrogen bromide and hydrogen bromide acid. When the water volume is less than 40%, bromine can be transported in nickel containers. The reaction between bromine and iron is slow during the drying process, which can form a protective layer of iron bromide.
Bromine can easily be added to unsaturated compounds, such as in the production of ethylene dibromide, where bromine is added to ethylene, resulting in a substitution reaction. Substitution reaction: When bromine comes into contact with an aromatic system, an electron withdrawing substitution reaction occurs. Common catalysts include bromide ions, chloride ions, or aluminum ions. Bromine homolysis replacing hydrogen is a general reaction that produces several bromides.
