Fluorine Gas Formula Structure, Properties, Uses, Sample Questions (original) (raw)

Last Updated : 23 Jul, 2025

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 F 2 . 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 (CaF 2 ) and **Sulfuric acid (H 2 SO 4 ).

**CaF 2 + H 2 SO 4 ⇢ 2HF + CaSO 4 .

• It can also be produced by the degradation of **hexafluorosilicic acid (H 2 SiF 6 ) to release **Hydrogen Fluoride (HF) through thehydrolysis process.

**H 2 SiF 6 ⇢ 2HF + SiF 4 .

**SiF 4 + 2H 2 O ⇢ 4HF + SiO 2 .

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 (H 2 O), we get **Hydrogen Fluoride (HF) and**oxygen gas (O 2 ).

**2F 2 **+ 2H 2 O ⇢ 2HF + O 2 .

• When Fluorine reacts with **Sodium Hydroxide (NaOH), we get**Sodium Fluoride (NaF), Oxygen difluoride (OF), and water (H 2 O).

**F 2 **+ 2NaOH ⇢ 2NaF + OF 2 **+ H 2 O.

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.

**Question 1: Write the reaction of Fluorine with NaCl.

**Answer:

When fluorine is reacted with **Sodium Chloride (NaCl), we get Sodium Fluoride (NaF) and**Chlorine ****(Cl** 2 ).

**2NaCl + F 2 ⇢ 2NaF + Cl 2.

**Question 2: Write the reaction of aluminum with fluorine.

**Answer:

When Fluorine (F2) is reacted with **Aluminium (Al), we get**Aluminium Fluoride (AlF 3 ).

**2Al + 3F 2 ⇢ 2AlF 3 .

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

**Answer:

When fluoride compound like **Hydrogen Fluoride (HF) is reacted**Barium Hydroxide (Ba(OH) 2 ), weget **Barium Fluoride (BaF 2 ).

**2HF + Ba(OH) 2 **⇢ BaF 2 + 2H 2 O.

**Question 4: Write the reaction of Fluorine with Chlorine.

**Answer:

When Fluorine (F2) is reacted with **Chlorine (Cl 2 ), we get **Chlorine Trifluoride (ClF 3 ).

**3F 2 + Cl 2 **⇢ 2ClF 3 .

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

**Answer:

**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?

**Answer:

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.