Reaction with Fluorine 

Fluorine is a chemical element with the symbol F, which carries the atomic number 9. Also known as the lightest halogen, Fluorine exists at STP as a highly toxic diatomic gas with a pale yellow colour. Being the most electronegative element, Fluorine is extremely reactive, as it reacts with all the elements in the periodic table, except for the noble gas argon, neon, and helium.

Fluorine has 5 electrons in its 2p shell. Because of this, we know fluorine is the most electronegative element. The electron configuration of the 2p. The orbital contains a total of 6 electrons, making Fluorine appear extremely close to the ideal electron configuration. The high electronegativity further explains the small radius of Fluorine. Since the electrons are packed closed with the nucleus. The positive protons have a strong attraction to the negative electrons, keeping them closely intact to the nucleus compared to the bigger and less electronegative elements.

You might be familiar with gas fluorocarbons. They are greenhouse gases that have a higher impact on global warming than carbon dioxide.SF6 has the highest global warming potential of any known substance. Due to the strength of the carbon–fluorine bond, organofluorine compounds are able to persist in the surrounding. There is no known metabolic role of fluorine found in mammals.

The bond energy of F2 is much lower than the bond energy of either Cl2 or Br2. This, in addition to high electronegativity, is the reason for easy fluorine dissociation, high reactivity, and strong bonds to non-fluorine atoms.

Because of fluorine’s high electronegativity, bonds formed with other atoms are very strong.

Similarly, even substances like powdered steel, glass fragments, and asbestos fibres which are unreactive, react quickly with fluorine gas in low temperatures. Fluorine occupies the thirteenth place as the most common element in the earth’s crust. Although it is believed that fluorine does not occur in nature, elemental fluorine is known to be present.

A rich chemistry is found in the reactions of fluorine, including both organic and inorganic substances. Fluorine combines with almost all noble gases, metalloids, metals and nonmetals. It exclusively takes up an oxidation state of −1. 

The reactions of fluorine are as follows:

Fluorine reacts instantly with hydrogen, forming the compound hydrogen fluoride. This reaction can be explosive under specific conditions.

H2(g) + F2(g)  → 2 HF(g)

HF is also produced by the endothermic reaction of fluorite CaF2 with sulfuric acid:

CaF2 + H2SO4 → 2 HF(g) + CaSO4

The formed compound, HF, is a byproduct of fertiliser production, which, in turn, produces hexafluorosilicic acid H2SiF6. The high electron affinity of fluorine shows a preference for ionic bonding. The covalent bonds formed by fluorine are polar, and almost always found to be single. This can be degraded to release HF thermally by hydrolysis:

H2SiF6 → 2 HF + SiF4

SiF4 + 2 H2O → 4 HF + SiO2

The reaction of fluorine with metals/metal ions

Sodium, Na reacts with fluorine, F2 forming sodium fluoride, NaF:

2 Na(s) + F2(g)  2 NaF(s)

The above reaction with metals is a general reaction which can be done for most metals.

The reaction of fluorine with noble gases

Krypton will react with fluorine, F2, when cooled to the very low temperature of -196 °C (liquid nitrogen) and tased with an electric discharge or X-rays, forming a compound, krypton(II) fluoride, KrF2 

Kr(s) + F2(s) KrF2(s)

This compound decomposes when it is heated to room temperature.

Xenon reacts with fluorine, F2 

Xe(g) + 2 F2(g) XeF4(s), mix gases at 400 °C then cool to -78 °C

Xe(g) + F2(g) XeF2(s)

Xe(g) + 3 F2(g) XeF6(s)

The xenon fluorides are used for synthesis of other xenon compounds.

Radon can be brought to react with fluorine, F2. The exact formula for the molecule is unknown and usually written as RnFn

The reaction of fluorine with sulphur

Sulphur reacts with excess fluorine forming sulphur(VI)fluoride:

S(s) + 3 F2(g) SF6(s)

Fluorine reacts with SO2 forming SO2F2:

SO2(g) + F2(g) SO2F2(g)

The reaction of fluorine with water

Fluorine reacts with water:

F2(g) + H2O(l) O2(g) + OF2(aq) + H2O2(aq) + HF(aq)

The reaction conditions determine how the reaction will be balanced.

Elemental Fluorine is slightly basic, which means that when it reacts with water, it forms hydrofluoric acid

It is almost non-existent in nature but is used in artificial compounds.

Alkali metals form ionic and highly soluble monofluorides.

Polytetrafluoroethylene (PTFE), the simplest fluoropolymer and perfluoro analogue of polyethylene with the structural unit –CF2-

Conclusion

Now you know the reactions of fluorine and how electronegative it is. But do you know where Fluorine exists around us in everyday life? Fluorine is added to our daily city water supplies to help prevent tooth decay. Sodium fluoride (NaF), stannous(II) fluoride, (SnF2) and sodium monofluorophosphate (Na2PO3F) are all fluorine compounds added to toothpaste, which also helps to prevent tooth decay. Uranium hexafluoride (UF6) is used to separate isotopes of uranium which are used in nuclear reactors. Calcium fluoride, CaF2 also known as fluorite and fluorspar, are used in the making of lenses which help us focus on infrared light. Fluorine is a special element in the periodic table.