Bromine dioxide

Bromine dioxide is a chemical compound with the formula BrO₂. It is a yellow solid that is unstable at room temperature. Bromine dioxide is of interest primarily in the field of inorganic chemistry and is studied for its potential applications and its role in various chemical reactions.

Structure and Properties

Bromine dioxide is a paramagnetic compound, meaning it has unpaired electrons and is attracted to magnetic fields. The compound is known to exist in a dimeric form, Br₂O₄, in the solid state. The structure of bromine dioxide is similar to that of chlorine dioxide, with a bent molecular geometry.

The compound is highly reactive and decomposes at temperatures above -40°C. It is typically generated in situ for experimental purposes due to its instability.

Synthesis

Bromine dioxide can be synthesized by the reaction of bromine with ozone or by the reaction of bromine with oxygen in the presence of a catalyst. The reaction with ozone is as follows:

2 Br₂ + 5 O₃ → 2 BrO₂ + 5 O₂

This reaction must be carried out at low temperatures to prevent decomposition of the bromine dioxide.

Reactions

Bromine dioxide is a strong oxidizing agent. It can react with various organic and inorganic compounds, often resulting in the oxidation of the substrate. For example, it can oxidize sulfur dioxide to sulfur trioxide:

BrO₂ + SO₂ → BrO + SO₃

Due to its reactivity, bromine dioxide is used in some specialized chemical syntheses and research applications.

Safety and Handling

Bromine dioxide is a hazardous material due to its instability and strong oxidizing properties. It can cause burns upon contact with skin and is harmful if inhaled. Proper safety precautions, including the use of gloves, goggles, and fume hoods, are necessary when handling this compound.

Also see

• Bromine
• Chlorine dioxide
• Oxidizing agent
• Inorganic chemistry