From Wikipedia, the free encyclopedia
Chemical compound
Zinc fluoride
|
Names
|
IUPAC name
Zinc(II) fluoride
|
Other names
Zinc difluoride
|
Identifiers
|
|
|
|
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ChemSpider
|
|
ECHA InfoCard
|
100.029.092
|
EC Number
|
|
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RTECS number
|
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UNII
|
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UN number
|
3077
|
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InChI=1S/2FH.Zn/h2*1H;/q;;+2/p-2
Y
Key: BHHYHSUAOQUXJK-UHFFFAOYSA-L
Y
|
|
Properties
|
|
ZnF
2
|
Molar mass
|
103.406 g/mol (anhydrous)
175.45 g/mol (tetrahydrate)
|
Appearance
|
white needles
hygroscopic
|
Density
|
4.95 g/cm
3
(anhydrous)
2.30 g/cm
3
(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
,
HNO
3
,
ammonia
|
|
−38.2·10
?6
cm
3
/mol
|
Structure
|
|
tetragonal (anhydrous),
tP6
|
|
P4
2
/mnm, No. 136
|
Hazards
|
GHS
labelling
:
[1]
|
|
![GHS05: Corrosive](//upload.wikimedia.org/wikipedia/commons/thumb/a/a1/GHS-pictogram-acid.svg/50px-GHS-pictogram-acid.svg.png) ![GHS06: Toxic](//upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/50px-GHS-pictogram-skull.svg.png)
|
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Danger
|
|
H301
,
H315
,
H318
,
H335
|
|
P261
,
P264
,
P270
,
P271
,
P280
,
P301+P310
,
P302+P352
,
P304+P340
,
P305+P351+P338
,
P310
,
P312
,
P330
,
P332+P313
,
P337+P313
,
P362
,
P403+P233
,
P405
,
P501
|
NFPA 704
(fire diamond)
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Related compounds
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Except where otherwise noted, data are given for materials in their
standard state
(at 25 °C [77 °F], 100 kPa).
|
Chemical compound
Zinc fluoride
is an
inorganic
chemical compound
with the
chemical formula
Zn
F
2
. It is encountered as the
anhydrous
form and also as the
tetrahydrate
,
ZnF
2
·4H
2
O
(rhombohedral crystal structure).
[2]
It has a high
melting point
and has the
rutile
structure containing
6 coordinate
zinc, which suggests appreciable
ionic character
in its chemical bonding.
[3]
Unlike the other zinc halides,
ZnCl
2
,
ZnBr
2
and
ZnI
2
, it is not very soluble in water.
[3]
Like some other metal difluorides,
ZnF
2
crystallizes in the
rutile
structure, which features
octahedral
Zn
cations
and
trigonal planar
fluorides
.
[4]
Preparation and reactions
[
edit
]
Zinc fluoride can be synthesized several ways.
Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxide fluoride, Zn(OH)F.
[5]
The salt is believed to form both a tetrahydrate and a dihydrate.
[6]
References
[
edit
]
- ^
"ZINC fluoride"
.
pubchem.ncbi.nlm.nih.gov
.
- ^
Perry, D. L.; Phillips, S. L. (1995).
Handbook of Inorganic Compounds
. CRC Press.
ISBN
0-8493-8671-3
.
- ^
a
b
c
d
Greenwood, Norman N.
; Earnshaw, Alan (1997).
Chemistry of the Elements
(2nd ed.).
Butterworth-Heinemann
.
ISBN
978-0-08-037941-8
.
- ^
Stout, J. W.; Reed, Stanley A. (1954). "The Crystal Structure of MnF
2
, FeF
2
, CoF
2
, NiF
2
and ZnF
2
".
J. Am. Chem. Soc
.
76
(21): 5279?5281.
doi
:
10.1021/ja01650a005
.
- ^
Srivastava, O. K.; Secco, E. A. (1967).
"Studies on Metal Hydroxy Compounds. I. Thermal Analyses of Zinc Derivatives ε-Zn(OH)
2
, Zn
5
(OH)
8
Cl
2
· H
2
O, β-ZnOHCl, and ZnOHF"
.
Canadian Journal of Chemistry
.
45
(6): 579?583.
doi
:
10.1139/v67-096
.
- ^
Lindahl, Charles B.; Mahmood, Tariq (2000), "Fluorine compounds, inorganic, zinc",
Kirk-Othmer Encyclopedia of Chemical Technology
, New York: John Wiley,
doi
:
10.1002/0471238961.2609140312091404.a01
,
ISBN
9780471238966
External links
[
edit
]
Salts and covalent derivatives of the
fluoride
ion
|
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