|Group||17||Melting point||−219.67°C, −363.41°F, 53.48 K|
|Period||2||Boiling point||−188.11°C, −306.6°F, 85.04 K|
|Block||p||Density (g cm−3)||0.001553|
|Atomic number||9||Relative atomic mass||18.998|
|State at 20°C||Gas||Key isotopes||19F|
|Electron configuration||[He] 2s22p5||CAS number||7782-41-4|
|ChemSpider ID||4514530||ChemSpider is a free chemical structure database|
- The element Fluorine is a poisonous gas.
- It usually exists as fluoride ion F- in aqueous solution
- It remains in the air for long when attached to tiny particles.
- Molecular fluorine and Atomic fluorine are used in semiconductor manufacturing for plasma etching, MEMs fabrication, and flat panel display production.
- Chlorofluorocarbons are used extensively used in air conditioners and refrigerators.
- Fluorides are also added to toothpaste to prevent dental cavities.
- The metal could be used to map the circulatory system and any disorders.
- Proposedly could be used in the optoelectric nuclear batteries.
- Fluorine exists naturally in the earth’s crust and found in coal, clay, and rocks.
- Hydrogen fluorides are released into the air by the industries through the processes of combustion.
- 0.6 ppb of fluorine is present as organic chloride compounds and salt spray in the atmosphere.
- The element has been recorded around 50 ppb in city environments.
- The 13th most abundant element in the Earth’s crust is Fluoride.
- Fluorine is reactive with other elements which can combine with nearly any element on Earth.
- Even water burn in fluorine with a bright flame along with finely divided metals like glass, ceramics, and carbon.
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