Zinc fluoride

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Zinc fluoride
Zinc fluoride
Names
Other names
Zinc difluoride
Identifiers
7783-49-5 YesY
13986-18-0 (tetrahydrate) N
3D model (Jmol) Interactive image
ChemSpider 22957 YesY
ECHA InfoCard 100.029.092
PubChem 24551
RTECS number ZH3200000
Properties
ZnF2
Molar mass 103.406 g/mol (anhydrous)
175.45 g/mol (tetrahydrate)
Appearance white needles
hygroscopic
Density 4.95 g/cm3 (anhydrous)
2.30 g/cm3 (tetrahydrate)
Melting point 872 °C (1,602 °F; 1,145 K) (anhydrous)
100 °C, decomposes (tetrahydrate)
Boiling point 1,500 °C (2,730 °F; 1,770 K) (anhydrous)
.000052 g/100 mL (anhydrous)
1.52 g/100 mL, 20 °C (tetrahydrate)
Solubility sparingly soluble in HCl, HNO3, ammonia
−38.2·10−6 cm3/mol
Structure
tetragonal (anhydrous), tP6
P42/mnm, No. 136
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Zinc fluoride (ZnF2) is an inorganic chemical compound. It is encountered as the anydrous form and also as the tetrahydrate, ZnF2 · 4H2O (rhombohedral crystal structure).[1] It has a high melting point and has the rutile structure containing 6 coordinate zinc, which suggests appreciable ionic character in its chemical bonding.[2] Unlike the other zinc halides, ZnCl2, ZnBr2 and ZnI2, it is not very soluble in water.[2]

Preparation and reactions[edit]

Zinc fluoride can be synthesized several ways.

Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxyfluoride, Zn(OH)F.[3]

References[edit]

  1. ^ Perry, D. L.; Phillips, S. L. (1995). Handbook of Inorganic Compounds. CRC Press. ISBN 0-8493-8671-3. 
  2. ^ a b c d Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9. 
  3. ^ Srivastava, O. K.; Secco, E. A. (1967). "Studies on Metal Hydroxy Compounds. I. Thermal Analyses of Zinc Derivatives ε-Zn(OH)2, Zn5(OH)8Cl2 · H2O, β-ZnOHCl, and ZnOHF" (pdf). Canadian Journal of Chemistry. 45 (6): 579–583. doi:10.1139/v67-096. 

External links[edit]