Fluorine

Introduction

Fluorine is a relatively recent element. Minerals containing fluorine were used sparingly in antiquity. Early scientist Georgius Agricola initially discussed the economic application of fluorite, the mineral that is the source of fluorine, in the context of smelting in the 16th century. The term "fluorite" (and subsequently "fluorine") is a creation of Agricola. The late 18th century saw the discovery of hydrofluoric acid. Early in the 19th century, it was realised that fluorine, like chlorine, was a bonded element within compounds. It was discovered that fluorite is calcium fluoride. Fluorine has resisted attempts to separate it due to its close bonds and the toxicity of hydrogen fluoride.

Henri Moissan, a French chemist who would eventually earn the Nobel Prize, electrolyzed a solution of potassium fluoride and hydrogen fluoride to produce elemental fluorine in 1886. Fluorine was first produced and used on a large scale as part of the Manhattan Project during World War 2. The DuPont business developed the primary fluorochemicals earlier this century, including polytetrafluoroethylene (Teflon) plastic and refrigerant gases (Freon).

What is Fluorine?

Halogen gas fluorine is a member of the periodic table's 17th group. The atomic number of the element is 9. Being the most electronegative element in the periodic table is fluorine's most distinguishing quality. Under normal circumstances, it appears as an extremely poisonous pale yellow diatomic gas. Fluorine has the highest electronegativity of any element, measuring 3.98 on the Pauling scale.

Electron Configuration and Chemical Properties of Fluorine

The atomic number of fluorine, gas from the 17th group, is 9. Fluorine has a valency of one since it is a halogen. It lacks one electron and is an electron acceptor. These substances are oxidising agents because they accept electrons. Keep in mind that electron donors are always reducing agents and electron acceptors are always oxidising. Fluorine is the greatest oxidising agent among the halogens due to its high electronegativity. Fluorine has the electronic structure $\mathrm{1s^{2}2s^{2}2p^{5}}$.We can see from the element's electrical structure that it is missing one electron. It receives an electron since it is an electrophile.

Properties of Fluorine

Fluorine shows different physical and chemical properties.

Chemical Properties of Fluorine

• Fluorine is one of the most powerful oxidising agents since it is a strongly electronegative element. According to the Pauling scale, fluorine has an electronegativity of 3.98.

• The strong force of attraction between the nucleus and the electrons caused by their small size results in a very high energy requirement to extract an electron. Fluorine has an initial ionisation energy of 1680.6 𝐾𝐽/𝑀𝑜𝑙. Thus, it takes 1680.6 𝐾𝐽 of energy to remove an electron from a mole of fluorine.

• Fluorine has a standard potential of 2.87 𝑉. Compared to all other factors, this is the highest.

• There is only one stable isotope of fluorine, which is fluorine 19.

Physical properties of Fluorine

• Fluorine is the lightest of all the halogens, with an estimated atomic mass of 19 particles.

• In its natural state, fluorine can be found as a gas. It is a light gas with a pale- yellow colour.

• Fluorine has a boiling point of -188° C and a melting point of 219.6° C.

The Atomic Radius of Fluorine

The atomic radius of fluorine, a very small element, is extremely small. A fluorine atom has a very strong nuclear force because of this. The smallest halogen atom is fluorine, which has an atomic radius of only 147 pm.

What is the Atomic Mass of Fluorine?

The lightest halogen gas, fluorine, weighs only 19 amu; specifically, it is 18.99 amu. Conventionally, we round it off and count it as 19.

Fun Facts About Fluorine

• In the crust of the earth, fluorine is the 13th most abundant element.

• Fluorine is a very reactive element that is never discovered in its pure form. It is always present in some combination with another element.

• Water can be burned by fluorine with a brilliant blaze.

• Fluorine can also be found in the earth's crust in addition to the air. Coal and other elements contain fluorine in trace amounts.

• Fluorine is nearly non-existent in the air. 50 parts per billion roughly. Before the Second World War, fluorine was not well recognised in the business.

• Fluorine hadn't been produced commercially until that point. Everyone just understood fluorine as an element that can combine to form salts. Uranium hexafluoride, however, was discovered to have nuclear capabilities and be a source of energy during World War 2. Fluorine has since been produced industrially at an exponential rate.

• Animals require ion fluoride, which helps to strengthen their teeth and bones. In some places, it is added to drinking water. Dental cavities are thought to be avoided when fluoride levels in drinking water are less than 2 parts per million. However, above this concentration, it may result in the mottling of children's dental enamel. Toothpaste also contains fluoride. Fluoride is present in the human body on average in amounts of 3 milligrams. Fluoride in excess is harmful. Fluorine is a highly poisonous element.

Conclusion

Fluorine is one of the halogen family members in the periodic table. Fluorine exists as yellow gas having an unpleasant smell when it is at room temperature. It is harmful to breathe in the gas. Fluorine becomes a yellow liquid when it cools. Fluorine-19 is the only stable isotope of the substance. The most significant source of fluorine is fluorspar.

FAQs

1. What are the uses of Fluorine?

The uses of Fluorine are −

• In the gaseous diffusion process, which separates uranium-235 from uranium-238 for reactor fuel, the element is also used to make uranium hexafluoride.

• Commercial production of hydrogen fluoride and boron trifluoride results from their usefulness as catalysts for the alkylation processes required to create a variety of chemical molecules.

• To lower the incidence of dental cavities in youngsters, sodium fluoride is frequently added to drinking water.

• The pharmaceutical and agricultural industries have been using fluorine compounds the most recently. Selective fluorine substitution significantly alters these chemicals' biological characteristics.

2. What is the origin of Fluorine?

The principal source mineral, fluorite, was originally reported in 1529 by Georgius Agricola, known as the "father of mineralogy," and the word "fluorine" is derived from this Latin stem. Fluorite, according to him, is an addition known as a flux that aids in melting ores and slags during smelting.

3. Why is Fluorine so important?

Our bones' ability to remain firm depends on fluorine. If we use fluoridated toothpaste twice a day, it can also prevent tooth decay. Too much fluorine absorption can affect the kidneys, bones, nerves, and muscles in addition to causing osteoporosis and tooth decay.

4. How is fluorine found in nature?

Because it is so reactive, fluorine gas, also known as chemistry's hellcat, has long been thought to not exist in nature. Now, scientists in Munich have proof that the gas is naturally present, trapped inside a stone known as antozonite, dark purple fluorite.

5. Why is fluorine so reactive?

Fluorine is extremely reactive due to its electronegativity. The propensity of an atom to draw in a shared pair of electrons is known as electronegativity. Simply said, if fluorine and chlorine engaged in a tug-of-war, fluorine would always prevail due to its stronger electronegativity.