Sodium fluoride



Sodium fluoride
IUPAC name Sodium fluoride
Identifiers
CAS number 7681-49-4
Properties
Molecular formula NaF
Molar mass 41.99 g/mol
Appearance White solid
Density 2.558 g/cm³, solid
Melting point

993 °C

Boiling point

1700 °C

Solubility in water 4.13 g/100 g at 25 °C
Hazards
EU classification Toxic (T)
NFPA 704
0
2
0
 
R-phrases R25, R32,
R36, R38
S-phrases S45
Flash point Non-flammable.
Related Compounds
Other anions sodium bromide
sodium iodide
Other cations potassium fluoride
caesium fluoride
Related bases None listed.
Related compounds TASF reagent
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Sodium fluoride is an hygroscopic than KF, but otherwise the potassium salt is more widely used.

Chemical structure and properties

NaF crystallizes in the sodium chloride motif where both Na+ and F− occupy octahedral coordination sites.[1]

It is usually used as a reagent for the synthesis of fluorides. Representative substrates include electrophilic chlorides including organic synthesis.

Uses

 

Fluoride salts are used widely to enhance the strength of teeth by the formation of fluoridate drinking water but its use has been displaced by hexafluorosilicic acid (H2SiF6) or its sodium salt (Na2SiF6). Toothpaste often contains sodium fluoride to prevent cavities.

Sodium fluoride was also used as an antibiotic, as rat poison, and in ceramics.


See also

References

  1. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  2. ^ Halpern, D. F. “Sodium Fluoride” Encyclopedia of Reagents for Organic Synthesis, 2001, John Wiley & Sons. DOI: 10.1002/047084289X.rs071.
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Stomatological preparations (Amlexanox
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Selenium		Sodium selenate - Sodium selenite
 
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