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Fluorine Gas Formula – Structure, Properties, Uses, Sample Questions

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  • Last Updated : 22 Aug, 2022
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Fluorine is a chemical element. It has the symbol F, and it has an atomic number of 9 in its periodic table. It is known as the lightest gas among the halogen. It appears pale yellow. It is a highly toxic diatomic gas under standard conditions. It is a highly electronegative element. Let’s learn about the Formula, occurrence, and properties of fluorine gas. 

Fluorine Gas Formula

The chemical formula of Fluorine gas is F2. It is also called Difluoride, which contains two Fluorine (F) atoms. It reacts with almost all other elements, except for argon, neon, and helium. In gas form, it appears as a pale yellow. In liquid form, it appears bright yellow, and in solid form, it is transparent and opaque. In the solid state, it is known as alpha and beta.  

Structure of Fluorine gas


Preparation of Fluorine gas

  • It is mostly found in the form of fluoride compounds. These fluoride compounds can be produced as Hydrogen Fluoride (HF) by combining Calcium Fluoride (CaF2) and Sulfuric acid (H2SO4).

CaF2 + H2SO4 ⇢ 2HF + CaSO4.

  • It can also be produced by the degradation of hexafluorosilicic acid (H2SiF6) to release Hydrogen Fluoride (HF) through the hydrolysis process.

H2SiF6 ⇢ 2HF + SiF4.

SiF4 + 2H2O ⇢ 4HF + SiO2.

Physical Properties of Fluorine gas

  • The atomic mass of Fluorine gas is 18.998403 g/mol.
  • The melting point of Fluorine gas is -219.67°C.
  • The boiling point of Fluorine gas is -188.11°C.
  • The density of Fluorine gas is 1.8 * 10-3 g/cm3.
  • It can easily combine with metals, non-metals, metalloids, and a noble gas.
  • It can be reactive with glass and water.

Chemical Properties of Fluorine gas

  • When Fluorine is reacted with water (H2O), we get Hydrogen Fluoride (HF) and oxygen gas (O2).

2F2 + 2H2O ⇢ 2HF + O2.

  • When Fluorine reacts with Sodium Hydroxide (NaOH), we get Sodium Fluoride (NaF), Oxygen difluoride (OF), and water (H2O).                            

F2 + 2NaOH ⇢ 2NaF + OF2 + H2O.

Uses of Fluorine Gas

  • It is used in the preparation of UF6 for the nuclear fuel cycle.
  • It is used to fluorinate uranium tetrafluoride.
  • It is used in toothpaste industries.
  • It is used in drinking water to prevent dental cavities.
  • It is used as a strong oxidizing agent.
  • It is used in light bulbs. 
  • It is used in making Teflon.

Frequently Asked Questions on Fluorine Gas

Question 1: Write the reaction of Fluorine with NaCl.


When fluorine is reacted with Sodium Chloride (NaCl), we get Sodium Fluoride (NaF) and Chlorine (Cl2).

2NaCl + F2 ⇢ 2NaF + Cl2.

Question 2: Write the reaction of aluminum with fluorine.


When Fluorine (F2) is reacted with Aluminium (Al), we get Aluminium Fluoride (AlF3).

2Al + 3F2 ⇢ 2AlF3.

Question 3: Write the reaction of fluoride compounds with barium hydroxide.


When fluoride compound like Hydrogen Fluoride (HF) is reacted Barium Hydroxide (Ba(OH)2), we get Barium Fluoride (BaF2).

2HF + Ba(OH)2 ⇢ BaF2 + 2H2O.

Question 4: Write the reaction of Fluorine with Chlorine.


When Fluorine (F2) is reacted with Chlorine (Cl2), we get Chlorine Trifluoride (ClF3).

3F2 + Cl2 ⇢ 2ClF3.

Question 5: What are the health hazards of Fluorine gas?


Health hazards of Fluorine gas:

  • If fluorine is absorbed frequently, it can cause tooth decay.
  • It can harm kidneys, bones, nerves, muscles.
  • It can also cause nausea, vomitings, diarrhea, constipation.
  • It can also cause liver damage and nosebleeds.

Question 6: Is Fluorine gas acid or base?


Fluorine is a Lewis acid in weak acid, which means that it accepts electrons when reacting. Fluorine has many isotopes, but the only stable one found in nature is F-19.

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