Related topics: fukushima

Chemist develops technique to improve solar cells

A RUDN University chemist has discovered four new stable compounds that can be obtained in the reaction of iodine with methylammonium iodide—the use of these substances will allow the production of perovskite solar panels ...

Iodine may slow ozone layer recovery

A new paper quantifying small levels of iodine in Earth's stratosphere could help explain why some of the planet's protective ozone layer isn't healing as fast as expected.

New chemical tools to modify and study biomolecules

Understanding the structure and metabolism of cells and living organisms is essential for the development of new drugs and diagnostics. The availability of chemical tools that allow scientists to edit biomolecules, like proteins, ...

Bonobo diet of aquatic greens may hold clues to human evolution

Observations of bonobos in the Congo basin foraging in swamps for aquatic herbs rich in iodine, a critical nutrient for brain development and higher cognitive abilities, may explain how the nutritional needs of prehistoric ...

Keeping nuclear power safe

Nuclear energy is clean, powerful, affordable, and zero-emission. A new study uses the Canadian Light Source (CLS) at the University of Saskatchewan to help ensure that waste from nuclear power plants remains safe and secure ...

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Iodine (pronounced /ˈaɪ.ədaɪn/, /ˈaɪ.ədɨn/, or in chemistry /ˈaɪ.ədiːn/; from Greek: ιώδης iodes "violet"), is a chemical element that has the symbol I and atomic number 53. Naturally-occurring iodine is a single isotope with 74 neutrons.

Chemically, iodine is the second least reactive of the halogens, and the second most electropositive halogen; trailing behind astatine in both of these categories. However, the element does not occur in the free state in nature. As with all other halogens (members of Group XVII in the periodic table), when freed from its compounds iodine forms diatomic molecules (I2).

Iodine and its compounds are primarily used in medicine, photography, and dyes. Although it is rare in the solar system and Earth's crust, the iodides are very soluble in water, and the element is concentrated in seawater. This mechanism helps to explain how the element came to be required in trace amounts by all animals and some plants, being the heaviest element commonly used by living organisms (only tungsten, used in enzymes by a few bacteria, is heavier).

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