What is Fluorine?
Fluorine is a halogen gas that belongs to the 17th group of the periodic table. The atomic number of the element is 9. The most characteristic feature about fluorine is that it is the most electronegative element in the periodic table. Its appearance can be described as a very toxic pale yellow diatomic gas at standard conditions. On the Pauling scale, the electronegativity of fluorine was measured to be 3.98 which surpassed every other element.
Electron Configuration And Chemical Properties of Fluorine
As we've seen earlier, fluorine is a gas belonging to the 17th group and fluorine atomic number is 9. Since fluorine is a halogen, it's valency is one. It is an electron recipient and lacks 1 electron. Such elements accept electrons and hence are oxidizing agents.
Remember: Electron acceptors are always oxidizing agents and electron donors are always reducing agents.
All the halogens are strong oxidizing agents out of which fluorine is the strongest due to its high electronegativity. The Electronic configuration of fluorine is 1s²2s²2p⁵. From the electronic configuration, we can clearly observe that the element lacks one electron. Hence, it is an electrophile and happily accepts an electron.
Properties of Fluorine
Chemical Properties of Fluorine
Fluorine is a highly electronegative element and is hence one of the strongest oxidizing agents. The electronegativity of fluorine as measured by the Pauling scale is 3.98.
The energy required to extract an electron is very high due to the strong force of attraction between the nucleus and the electrons owing to their small size. The first ionization energy of fluorine is 1680.6 KJ/Mol. That means, 1680.6 KJ energy is required to extract an electron from one mole of fluorine
The standard potential of fluorine is 2.87 V. This is the highest among all other elements.
Fluorine has only one stable isotope, that is fluorine 19.
Physical Properties of Fluorine
The atomic mass of fluorine is approximately 19 and fluorine is the lightest among all other halogens.
Fluorine exists as a gas in nature and at a standard state. It has a pale yellow colour and is a light gas.
The boiling point of fluorine is -188° C and the melting point of fluorine is -219.6° C.
The Atomic Radius of Fluorine
Fluorine is a tiny element with a really small atomic radius. Due to this, the nuclear force in a fluorine atom is extremely high. The atomic radius of fluorine is merely 147 pm, making it the smallest halogen atom.
What is The Atomic Mass of Fluorine?
As we've seen earlier, fluorine is the lightest halogen gas and weighs only 19 amu, to be precise it is 18.99. However, by convention, we round it off and consider it as 19.
To answer the question, "what group fluorine is in" and "what is the symbol of fluorine", Fluorine belongs to the halogen group that is the 17th group and the fluorine is represented as F2. 2 indicates the diatomic nature of fluorine gas.
Fun Facts About Fluorine
Fluorine is the 13th most abundant element in the earth's crust.
Fluorine is a highly reactive element and is never found in its original state. It is always found combined with some or the other elements.
Fluorine is capable of burning water with a bright flame.
Apart from being found in the air, fluorine is also found in the earth's crust. Traces of fluorine are found in coal and other elements.
In the air, fluorine is present in almost negligible quantity. It's about 50 parts per billion.
Fluorine had no recognition in the industry until the 2nd world war. No one cared to industrially produce fluorine until then. Everyone just knew fluorine as an element which is capable of combining and making salts. However, in World War 2, people realized that uranium hexafluoride has nuclear properties and can be a source of energy. Since then, industrial production of fluorine rose exponentially.
Some Common Compounds Containing Fluorine
Fluorine is very small in size and hence it is difficult for fluorine to exist in ionic compounds. However, owing to its highly electrophilic nature, fluorine is highly reactive and hence forms several compounds.
Some of The Popular Compounds Containing Fluorine Include
Calcium Fluoride - CaF2
Xenon Difluoride- XeF2
Hydrogen Fluoride- HF
Uranium Hexafluoride (UF6)
Sodium Monofluorophosphate (Na2PO3F)
Sodium Fluoride (NaF)
Stannous(II) fluoride (SnF2)
Dichlorodifluoromethane (CF2Cl2)
FAQs on Fluorine
1. What is fluorine and where is it located in the periodic table?
Fluorine is a chemical element with the symbol F and atomic number 9. It is the lightest halogen and exists as a highly toxic, pale yellow-green diatomic gas at standard conditions. In the periodic table, it is located in Group 17 and is the most electronegative element, meaning it has a very strong ability to attract electrons.
2. What are the most common uses of fluorine in industry and everyday life?
Fluorine compounds have many important applications. Some of the most common uses include:
- Dental Health: Fluorides, such as sodium fluoride, are added to toothpaste and drinking water to prevent tooth decay.
- Polymers: It is used to produce polymers like Teflon (polytetrafluoroethylene), which is famous for its use in non-stick cookware.
- Nuclear Power: Uranium hexafluoride (UF₆) is a key compound used in the process of enriching uranium for nuclear reactors and weapons.
- Pharmaceuticals: Many medicines, including some antidepressants and antibiotics, contain fluorine to enhance their effectiveness.
3. What is the difference between a fluorine atom (F) and a fluoride ion (F⁻)?
The main difference lies in their stability and charge. A fluorine atom (F) is neutral but highly unstable because its outermost electron shell is incomplete. To become stable, it aggressively seeks to gain one electron. When it successfully gains an electron, it becomes a fluoride ion (F⁻), which has a negative charge and a stable, complete outer electron shell.
4. Why is fluorine considered the most electronegative element?
Fluorine's position as the most electronegative element is due to two main factors. First, it has a high effective nuclear charge, meaning its nucleus has a strong positive pull. Second, it has a very small atomic radius, so its outer electrons are very close to the nucleus. This powerful combination allows it to attract bonding electrons more strongly than any other element.
5. Why does fluorine gas naturally exist as a diatomic molecule (F₂)?
A single fluorine atom is extremely reactive because it needs one more electron to achieve a stable electron configuration. To solve this, two fluorine atoms share electrons with each other, forming a strong covalent bond. This pairing creates a stable diatomic molecule (F₂), which is the form in which fluorine gas is found naturally.
6. How is fluorine gas prepared, and why is the process so difficult?
Fluorine gas is prepared commercially through the electrolysis of a solution of potassium hydrogen fluoride (KHF₂) in anhydrous hydrogen fluoride (HF). The process is difficult and dangerous because fluorine is incredibly reactive. It attacks most materials, including glass and water, so special equipment made of specific metal alloys (like Monel) is required for its production and handling.
7. What are the main physical properties of fluorine?
At room temperature, fluorine is a pale yellow-green gas with a sharp, pungent odour similar to ozone. It is extremely corrosive and toxic. It condenses into a bright yellow liquid at -188°C and freezes into a solid at -220°C. Due to its high reactivity, it must be handled with extreme care.
8. Can fluorine form compounds where it has a positive oxidation state?
No, fluorine cannot exhibit a positive oxidation state. As the most electronegative element, it has the strongest tendency to attract electrons. In any chemical bond with another element, fluorine will always attract the shared electrons more strongly, giving it an oxidation state of -1. It is the only element that does not have a positive oxidation state in any of its compounds.
