Fluorine facts for kids
Liquid fluorine (at extremely low temperatures)
|
|||||||||||||||||||||
| Fluorine | |||||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| Pronunciation | |||||||||||||||||||||
| Allotropes | alpha, beta (see Allotropes of fluorine) | ||||||||||||||||||||
| Appearance | gas: very pale yellow liquid: bright yellow solid: transparent (beta), opaque (alpha) |
||||||||||||||||||||
| Standard atomic weight Ar, std(F) | 18.998403163(6) | ||||||||||||||||||||
| Fluorine in the periodic table | |||||||||||||||||||||
|
|||||||||||||||||||||
| Atomic number (Z) | 9 | ||||||||||||||||||||
| Group | group 17 (halogens) | ||||||||||||||||||||
| Period | period 2 | ||||||||||||||||||||
| Block | p | ||||||||||||||||||||
| Electron configuration | [He] 2s2 2p5 | ||||||||||||||||||||
| Electrons per shell | 2, 7 | ||||||||||||||||||||
| Physical properties | |||||||||||||||||||||
| Phase at STP | gas | ||||||||||||||||||||
| Melting point | 53.53 K (−219.62 °C, −363.32 °F) | ||||||||||||||||||||
| Boiling point | 85.03 K (−188.12 °C, −306.62 °F) | ||||||||||||||||||||
| Density (at STP) | 1.696 g/L | ||||||||||||||||||||
| when liquid (at b.p.) | 1.505 g/cm3 | ||||||||||||||||||||
| Critical point | 144.4 K, 5.215 MPa | ||||||||||||||||||||
| Heat of vaporization | 6.51 kJ/mol | ||||||||||||||||||||
| Molar heat capacity | (Cp) (21.1 °C) 825 J·mol−1·K−1 (Cv) (21.1 °C) 610 J/(mol·K) |
||||||||||||||||||||
Vapor pressure
|
|||||||||||||||||||||
| Atomic properties | |||||||||||||||||||||
| Oxidation states | −1 (oxidizes oxygen) | ||||||||||||||||||||
| Electronegativity | Pauling scale: 3.98 | ||||||||||||||||||||
| Ionization energies |
|
||||||||||||||||||||
| Covalent radius | 64 pm | ||||||||||||||||||||
| Van der Waals radius | 135 pm | ||||||||||||||||||||
 |
|||||||||||||||||||||
| Other properties | |||||||||||||||||||||
| Natural occurrence | primordial | ||||||||||||||||||||
| Crystal structure | cubic
 the structure shows solid fluorine, just under the melting point, 1 atm |
||||||||||||||||||||
| Thermal conductivity | 0.02591 W/(m⋅K) | ||||||||||||||||||||
| Magnetic ordering | diamagnetic | ||||||||||||||||||||
| CAS Number | 7782-41-4 | ||||||||||||||||||||
| History | |||||||||||||||||||||
| Discovery | André-Marie Ampère (1810) | ||||||||||||||||||||
| First isolation | Henri Moissan (June 26, 1886) | ||||||||||||||||||||
| Named by | Humphry Davy | ||||||||||||||||||||
| Main isotopes of fluorine | |||||||||||||||||||||
|
|||||||||||||||||||||
| reference | |||||||||||||||||||||
Fluorine (symbol F) is a chemical element that is very poisonous. Its atomic number (which is the number of protons in it) is 9, and its atomic mass is 19. It is part of the Group 7 (halogens) on the periodic table of elements.
Contents
Properties
Fluorine is a light yellow diatomic gas. It is very reactive gas, which exists as diatomic molecules. It is actually the most reactive element. Fluorine has a very high attraction for electrons, because it is missing one. This makes it the most powerful oxidizing agent. It can rip electrons from water (making oxygen) and ignite propane on contact. It does not need a spark. Metals can catch on fire when placed in a stream of fluorine. After it is reduced by reacting with other things, it forms the stable fluoride ion. Fluorine is very poisonous. Fluorine bonds very strongly with carbon. It can react with the unreactive noble gases. It explodes when mixed with hydrogen. The melting point of fluorine is -363.33°F (-219.62°C), the boiling point is -306.62°F (-188.12°C).
Chemical compounds
Chemical compounds containing fluorine ions are called fluorides. Fluorine only exists in one oxidation state: -1.
- Aluminium fluoride
- Antimony trifluoride
- Antimony pentafluoride
- Arsenic trifluoride
- Arsenic pentafluoride
- Bismuth(III) fluoride
- Bismuth(V) fluoride
- Bromine trifluoride
- Bromine pentafluoride
- Chlorine monofluoride
- Chlorine trifluoride
- Cobalt(II) fluoride
- Cobalt(III) fluoride
- Disulfur decafluoride
- Hydrofluoric acid, a solution of hydrogen fluoride in water
- Hydrogen fluoride
- Iodine trifluoride
- Iodine pentafluoride
- Iodine heptafluoride
- Manganese(II) fluoride
- Manganese(III) fluoride
- Manganese(IV) fluoride
- Potassium fluoride
- Selenium tetrafluoride
- Selenium hexafluoride
- Silver(I) fluoride, brown-yellow
- Silver(II) fluoride, highly reactive, white or gray
- Sodium aluminium fluoride, cryolite
- Sodium fluoride
- Sulfur hexafluoride
- Sulfur tetrafluoride
- Tellurium(IV) fluoride
- Tellurium(VI) fluoride
- Thallium(I) fluoride
- Thallium(III) fluoride
- Tin(II) fluoride
- Tin(IV) fluoride
- Zinc fluoride
Occurrence
Fluorine is not found as an element on the earth; it is much too reactive. Several fluorides are found in the earth, though. When calcium phosphate is reacted with sulfuric acid to make phosphoric acid, some hydrofluoric acid is produced. Also, fluorite can be reacted with sulfuric acid to make hydrofluoric acid. Is a luiquid of fluoride U. Fluorine naturally occurs on the earths' crust in rocks, coal and clay.
Preparation
Fluorine is normally made by electrolysis. Hydrogen fluoride is dissolved in potassium fluoride. This mixture is melted and an electric current is passed through it. This is electrolysis. Hydrogen is produced at one side and fluorine at the other side. If the sides are not separated, the cell may explode.
Someone made fluorine in 1986 without using electrolysis. They produced manganese(IV) fluoride by using various chemical compounds, which released fluorine gas.
Uses
Fluorine is used to enrich uranium for nuclear weapons. It is also used to make sulfur hexafluoride. Sulfur hexafluoride is used to propel stuff out of an aerosol can. It is also used to make integrated circuits. Fluorine compounds have many uses. Fluoride ions are in fluorine compounds. Fluoride ions can be in toothpaste. Some are used in nonstick coatings. Freons contain fluorine.
Safety
Fluorine as an element is extremely reactive and toxic. It can react with almost everything, even glass. Fluorine is also poisonous.
Fluoride ions are somewhat toxic. If too much toothpaste containing fluoride is eaten then fluoride poisoning may occur. Fluoride is not reactive, though.
Related pages
Images for kids
-
Fluorine 3D molecule
-
Animation showing the crystal structure of beta-fluorine. Molecules on the faces of the unit cell have rotations constrained to a plane.
-
Steelmaking illustration from De re metallica
-
1887 drawing of Moissan's apparatus
-
An ampoule of uranium hexafluoride
-
Chlorine trifluoride, whose corrosive potential ignites asbestos, concrete, sand and other fire retardants
-
These xenon tetrafluoride crystals were photographed in 1962. The compound's synthesis, as with xenon hexafluoroplatinate, surprised many chemists.
-
Immiscible layers of colored water (top) and much denser perfluoroheptane (bottom) in a beaker; a goldfish and crab cannot penetrate the boundary; quarters rest at the bottom.
-
Industrial fluorine cells at Preston
-
SF6 current transformers at a Russian railway.
-
Fluorosurfactant-treated fabrics are often hydrophobic
-
Topical fluoride treatment in Panama
-
The gifblaar is one of the few organofluorine-synthesizing organisms
-
NASA projection of stratospheric ozone over North America without the Montreal Protocol
-
Perfluorooctanesulfonic acid, a key Scotchgard component until 2000
-
Fluorite: Pink globular mass with crystal facets
-
Fluorapatite: Long prism-like crystal, without luster, at an angle coming out of aggregate-like rock
-
Cryolite: A parallelogram-shaped outline with diatomic molecules arranged in two layers
_gives_a_Fluoride_treatment_to_a_patient_during_a_Continuing_Promise_2009_medical_civil_service_projec.jpg)
See also
In Spanish: Flúor para niños
