Calcium Fluoride

What is Calcium Fluoride?

Molecular Formula (Calcium Fluoride): CaF2

Molecular Weight: 78.07

Chemical Name: Calcium Fluoride

CAS Number: 7789-75-5

It can be found in nature as the mineral fluorite or fluorspar. These minerals, which come in many color varieties as well as colorless, are called fluorite or fluorspar.

The crystal lattice structure of Calcium Fluoride is called the fluorite structure. It has a semi-linear molecule. It is a chemical with weak oxidizing and reducing properties.

Other Names are as Follows;

• CaF2
• Calcium Difluoride
• Fluorite
• Fluorite
• Fluorspar
• 7789-75-5

How is it Produced?

Calcium fluoride production is obtained from fluorspar extracted from mines with inclined veins in open-pit and deep-pit mines. It is obtained by reacting a highly soluble calcium source with sodium fluoride.

Additionally, it is produced from the reaction of Calcium Carbonate and Hydrofluoric Acid. This production method is not cost-effective. The reason is that the market value of hydrofluoric acid available on the market is higher than the market value of calcium fluoride.

What are the Physical and Chemical Properties?

In terms of physical appearance, it is found in the form of an odorless gray powder or as granules.

The melting point is 1402 °C.

The boiling point is 2500 °C.

Its density is 3.18 g/cm³ at 25 °C. With this property, it is denser than water.

It does not have hygroscopic properties. It is an inert chemical.

It exhibits certain properties due to its low atomic number. Therefore, it is in a preferred category of chemicals.

Its solubility in water is very low. It is 16 mg/L in water at 20 °C. It dissolves in concentrated acids. These can be specified as Hydrochloric Acid, Sulfuric Acid, and Nitric Acid. At the same time, it dissolves in ammonium salt. Specifically, this ammonium salt is Ammonium Chloride.

What are the Usage Areas of Calcium Fluoride?

• Naturally occurring CaF2 obtained from mines is reacted with sulfuric acid to produce calcium sulfate (CaSO4) and Hydrogen Fluoride (HF) gas.
• Tartar formation in the mouth occurs when plaques undergo changes in the presence of saliva. It is used in the manufacture of oral care products containing CaF2 to prevent plaque formation in the mouth. These plaques are called bacterial plaque.
• Inorganic fluorine compounds are used to obtain turbidity in opaque glass production. This compound (CaF2) is one of them.
• The production of innovative and modern brake systems in the automotive industry has recently become widespread. The production of such high-performance brake systems is carried out with this chemical substance.
• It is used to fluoridate drinking water.
• It is used in the construction of oxygen furnaces, electric furnaces, and some kilns where steel is produced.
• It is used as a catalyst in the production of wood preservative chemicals.
• It is used in the thermal plasma process for the purification of silicon.
• It is used in the production of metallurgical materials, especially in the manufacture of ultraviolet and infrared devices.
• In aluminum casting facilities, certain additives are used to protect molten aluminum alloys against oxidation. Calcium fluoride is used here to prevent the resulting gases from entering the bath. It has the effect of reducing heat loss.
• It can be used in a new method applied to produce next-generation mid-infrared microresonators.

What are the Factors Affecting Its Prices?

The price of Calcium Fluoride is directly proportional to the prices of the chemicals used in its production. As the number of fluorite mines increases, the prices of this chemical substance will decrease. Especially, an increase in sulfuric acid prices will lead to an increase in CaF2 prices.

With the expansion of the glass sector and the rise of buildings, the use of glass has increased. For this reason, the price of Calcium Fluoride has increased.

Companies that are distributors of Calcium Fluoride have a significant impact on the prices of this chemical substance. As stocks increase, prices will experience a short-term decrease.