Fluorine Atomic Number

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Chemical properties of fluorine - Health effects of fluorine - Environmental effects of fluorine

  • Fluorine was discovered by Henri Moissan (FR) in 1886. The origin of the name comes from the Latin word fluere meaning to flow. It is a pale yellow to greenish gas, with an irritating pungent odour. Fluorine is a extremely reactive, flammable gas. It reacts violently with many materials. It is toxic by inhalation or ingestion.
  • Fluorine is a chemical element with atomic number 9 which means there are 9 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

9

Atomic mass

18.998403 g.mol -1

Electronegativity according to Pauling

4

Density

1.8*10-3 g.cm-3 at 20°C

Melting point

-219.6 °C

Boiling point

-188 °C

Vanderwaals radius

0.135 nm

Ionic radius

0.136 nm (-1) ; 0.007 (+7)

Isotopes

2

Electronic shell

[ He ] 2s22p5

Energy of first ionisation

1680.6 kJ.mol -1

Energy of second ionisation

3134 kJ.mol -1

Energy of third ionisation

6050 kJ mol-1

Standard potential

- 2.87 V Visual studio code 2010.

Discovered by

Moissan in 1886

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Fluorine

Fluorine is an univalent poisonous gaseous halogen, it is pale yellow-green and it is the most chemically reactive and electronegative of all the elements. Fluorine readily forms compounds with most other elements, even with the noble gases krypton, xenon and radon. It is so reactive that glass, metals, and even water, as well as other substances, burn with a bright flame in a jet of fluorine gas.
In aqueous solution, fluorine commonly occurs as the fluoride ion F-. Fluorides are compounds that combine fluoride with some positively charged counterpart.

Applications

Atomic fluorine and molecular fluorine are used for plasma etching in semiconductor manufacturing, flat panel display production and MEMs fabrication.
Fluorine is indirectly used in the production of low friction plastics such as teflon and in halons such as freon, in the production of uranium. Fluorochlorohydrocarbons are used extensively in air conditioning and in refrigeration.
Fluorides are often added to toothpaste and, somewhat controversially, to municipal water supplies to prevent dental cavities. Fore more information visit our page on mineral water.

Fluorine in the environment

Annual world production of the mineral fluorite in around 4 million tonnes, and there are around 120 million tonnes of mineral reserves. The main mining areas for fluorite are China, Mexico and Western Europe.
Fluorine occurs naturally in the earth's crust where it can be found in rocks, coal and clay. Fluorides are released into the air in wind-blown soil. Fluorine is the 13th most aboundant element in the Earth's crust: 950 ppm are contanined in it. Soils contain approximatively 330 ppm of fluorine, ranging from 150 to 400 ppm. Some solis can have as much as 1000 ppm and contaminated solis have been found with 3500 ppm. Hydrogen fluorides can be released into air through combustion processes in the industry. Fluorides that are found in air will eventually drop onto land or into water. When fluorine is attached to very small particles it can remain in the air for a long period of time.
In the atmosphere 0.6 ppb of fluorine are present as salt spray and organicochloride compounds. Up to 50 ppb has been recorded in city environments.

Health effects of fluorine

Small amounts of fluorine are naturally present in water, air, plants and animals. As a result humans are exposed to fluorine through food and drinking water and by breathing air. Fluorine can be found in any kind of food in relatively small quantities. Large quantities of fluorine can be found in tea and shellfish.
Fluorine is essential for the maintenance of solidity of our bones. Fluorine can also protect us from dental decay, if it is applied through toothpaste twice a day. If fluorine is absorbed too frequently, it can cause teeth decay, osteoporosis and harm to kidneys, bones, nerves and muscles.
Fluorine gas is released in the industries. This gas is very dangerous, as it can cause death at very high concentrations. At low concentrations it causes eye and nose irritations.

Environmental effects of fluorine

When fluorine from the air ends up in water it will settle into the sediment. When it ends up in soils, fluorine will become strongly attached to soil particles. In the environment fluorine cannot be destroyed; it can only change form.
Fluorine that is located in soils may accumulate in plants. The amount of uptake by plants depends upon the type of plant and the type of soil and the amount and type of fluorine found in the soil. With plants that are sensitive for fluorine exposure even low concentrations of fluorine can cause leave damage and a decline in growth. Too much fluoride, wheater taken in form the soil by roots, or asdorbed from the atmosphere by the leaves, retards the growth of plants and reduces crop yields. Those more affected are corns and apricots.
Animals that eat fluorine-containing plants may accumulate large amounts of fluorine in their bodies. Fluorine primarily accumulates in bones. Consequently, animals that are exposed to high concentrations of fluorine suffer from dental decay and bone degradation. Too much fluorine can also cause the uptake of food from the paunch to decline and it can disturb the development of claws. Finally, it can cause low birth-weights.

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Fluorine Atomic Number

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Fluorine Atomic Number

Atomic Number of Fluorine is 9.

Chemical symbol for Fluorine is F. Number of protons in Fluorine is 9. Atomic weight of Fluorine is 18.99840316 u or g/mol. Melting point of Fluorine is -219,6 °C and its the boiling point is -188,1 °C.

» Boiling Point» Melting Point» Abundant» State at STP» Discovery Year

About Fluorine

Fluorine is a pale yellow gas which is very toxic and poisonous but is essential for animals and humans to strengthen our bones and teeth. It is a very reactive gas which reacts even with noble gases, and it forms a large number of chemical compounds. The name of the chemical element is derived from the Greek word meaning flowing. Fluorine can not be found in its natural form as it reacts very fast. It was not produced until the middle of the 20th century, but in those times it became necessary for various projects involving nuclear energy. This element is also used in toothpaste and dental care products, as well as in producing some parts for electronic devices, for welding and processing glass, etc. In its natural form, fluorine exists in some types of clay, rocks, coal, and other sources.

Uses of Fluorine

Fluorine which is the most reactive element is used to produce uranium hexafluoride in the nuclear power industry. Today, fluorine compounds are mostly used in the pharmaceutical and agriculture fields. Dichlorodifluoromethane (a colorless gas with the formula Cl2CF2) is used as a coolant in domestic refrigerators and air conditioners. And hydrofluoroalkane (HFA) containing carbon, fluorine, and hydrogen, is used as aerosols in medicine. Hydrofluoric acid (HF) which is a solution of hydrogen fluoride in water, is used in industrial chemistry, glass finishing, cleaning, and research. Sodium fluoride, an inorganic compound with the formula NaF is commonly used in the production of pharmaceuticals. It is sold as tablets to prevent cavities. Sodium fluoride is also used in chemistry and in medical imaging too.

Compounds with Fluorine

  • HF: Hydrogen fluoride
  • H2SiF6: Fluorosilicic acid
  • Na3AlF6: Sodium aluminum fluoride
  • SF6: Sulfur hexafluoride
  • ClF3: Chlorine trifluoride
  • CoF3: Cobalt trifluoride
  • Cl2CF2: Dichlorodifluoromethane
  • BF3: Boron trifluoride
  • HFA: Hydrofluoroalkane

Properties of Fluorine Element

Atomic Number (Z)9
Atomic SymbolF
Group17
Period2
Atomic Weight18.99840316 u
Density0.001696 g/cm3
Melting Point (K)53.53 K
Melting Point (℃)-219,6 °C
Boiling Point (K)85.03 K
Boiling Point (℃)-188,1 °C
Heat Capacity0.824 J/g · K
Abundance585 mg/kg
State at STPGas
OccurrencePrimordial
DescriptionHalogen
Electronegativity (Pauling) χ3.98
Ionization Energy (eV)17.42282
Atomic Radius50pm
Covalent Radius71pm
Van der Waals Radius147
Valence Electrons7
Year of Discovery1886
DiscovererMoissan

Electron Configuration For Fluorine

What is the Boiling Point of Fluorine?

Fluorine boiling point is -188,1 °C. Boiling point of Fluorine in Kelvin is 85.03 K.

What is the Melting Point of Fluorine?

Fluorine melting point is -219,6 °C. Melting point of Fluorine in Kelvin is 53.53 K.

How Abundant is Fluorine?

Fluorine Group

Abundant value of Fluorine is 585 mg/kg.

Fluorine Atomic Numbers

What is the State of Fluorine at Standard Temperature and Pressure (STP)?

Fluorine Atomic Number And Neutrons

State of Fluorine is Gas at standard temperature and pressure at 0℃ and one atmosphere pressure.

When was Fluorine Discovered?

Fluorine Atomic Number Of Neutrons

Fluorine was discovered in 1886.

Fluorine Atomic Number 9