Fluorine

Symbol

F

Atomic number

9

Atomic mass	18.9984		Thermal conductivity	0.000279
Atomic radius	0.57		Covalent radius	0.72
Density	0.001696		Atomic volume	17.1
Melting point	53.53		Oxidation states	-1
Boiling point	84.95		Stable isotopes	1
Heat of vapor.	3.2698		Electronegativity	3.98
Heat of fusion	0.2552		First ionization	17.422
Specific heat	0.82		Electrical conduct.	...

Electron configuration

Fluorine

Fluorine, the lightest of the halogens, is the most reactive of all the elements. It forms compounds with all the elements except the noble gases.

The reactivity of pure fluorine gas is remarkable. Ordinary substances like wood and rubber burst into flame when held into a stream of fluorine. Even asbestos reacts so vigorously that it becomes incandescent. Copper and steel are attacked by it, but become coated with a thin layer of copper fluoride or iron fluoride and resist further attack. Steel tanks can therefore be used as containers for transport of fluorine.

Fluorine occurs in nature in minerals such as fluorite, CaF₂, which can produce gem quality crystals. Also occurring as a mineral is fluorapatite, Ca₅(PO₄)₃F, which is a constituent of bones and teeth. A small percentage of fluorapatite along with the more abundant calcium phosphates in teeth can make them more resistant to decay.

Hydrogen fluoride, HF, in water is called hydrofluoric acid. It and the vapor phase HF can be used for etching glass. Hydrofluoric acid must be handled with great care, because skin contact produces lesions which heal very slowly. Hydrofluoric acid can be stored in polyethylene containers.

Reaction with the alkali metals produces salts called fluorides. Sodium fluoride, NaF, is used as an insecticide.

Fluorine Nuclear Data