Cadmium fluoride

"CdF2" redirects here. For the airport in Canada, see Teeswater (Dent Field) Aerodrome.

Cadmium fluoride

Names
IUPAC name

Cadmium fluoride

Other names

Cadmium(II) fluoride, Cadmium difluoride

Identifiers

CAS Number

* 7790-79-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 23036 Y

EC Number |

* 232-222-0

PubChem CID

* 24634
* 71356118 dihydrate

UNII |

* M0975E7Z8Z Y

InChI

* InChI=1S/Cd.2FH/h;2*1H/q+2;;/p-2 Y

Key: LVEULQCPJDDSLD-UHFFFAOYSA-L Y

* InChI=1/Cd.2FH/h;2*1H/q+2;;/p-2

Key: LVEULQCPJDDSLD-NUQVWONBAG

SMILES

* [Cd+2].[F-].[F-]

Properties

Chemical formula

| CdF2
Molar mass | 150.41 g/mol
Appearance  | grey or white-grey crystals
Density | 6.33 g/cm3, solid
Melting point |  1,110 °C (2,030 °F; 1,380 K)
Boiling point |  1,748 °C (3,178 °F; 2,021 K)

Solubility in water

| 4.35 g/100 mL

Solubility product (Ksp)

| 0.00644[1]
Solubility | soluble in acid
insoluble in ethanol alcohol and liquid ammonia

Magnetic susceptibility (χ)

| −40.6·10−6 cm3/mol
Structure

Crystal structure

| Fluorite (cubic), cF12

Space group

| Fm3m, No. 225
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| −167.39 ± 0.23 kcal. mole-1 at 298.15 (K, C?)

Gibbs free energy (ΔfG˚)

| −155.4 ± 0.3 kcal. mole-1 at 298.15 (K, C?)
Hazards
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H301, H330, H340, H350, H360, H372, H410

GHS precautionary statements

| P201, P202, P260, P264, P270, P271, P273, P281, P284, P301+310, P304+340, P308+313, P310, P314, P320, P321, P330, P391, P403+233, P405, P501
NIOSH (US health exposure limits):

PEL (Permissible)

| [1910.1027] TWA 0.005 mg/m3 (as Cd)[2]

REL (Recommended)

| Ca[2]

IDLH (Immediate danger)

| Ca [9 mg/m3 (as Cd)][2]
Related compounds

Other anions

| Cadmium chloride,
Cadmium bromide
Cadmium iodide

Other cations

| Zinc fluoride,
Mercury(II) fluoride,
Copper(II) fluoride,
Silver(II) fluoride,
Calcium fluoride,
Magnesium fluoride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Cadmium fluoride (CdF2) is a mostly water-insoluble source of cadmium used in oxygen-sensitive applications, such as the production of metallic alloys.

## Contents

* 1 Preparation
* 2 Physical properties
* 3 Uses
* 3.1 Electronic conductor
* 4 Safety
* 5 References
* 6 External links

## Preparation

Cadmium fluoride is prepared by the reaction of gaseous fluorine or hydrogen fluoride with cadmium metal or its salts, such as the chloride, oxide, or sulfate.

It may also be obtained by dissolving cadmium carbonate in 40% hydrofluoric acid solution, evaporating the solution and drying in a vacuum at 150 °C.

Another method of preparing it is to mix cadmium chloride and ammonium fluoride solutions, followed by crystallization. The insoluble cadmium fluoride is filtered from solution.[3]

Cadmium fluoride has also been prepared by reacting fluorine with cadmium sulfide. This reaction happens very quickly and forms nearly pure fluoride at much lower temperatures than other reactions used.[4]

## Physical properties

The standard enthalpy has been found to be −167.39 kcal·mole−1 and the Gibbs energy of formation has been found to be −155.4 kcal·mole−1.[5] The heat of sublimation was determined to be 76 kcal. mole−1[6]

## Uses

In extremely low concentrations (ppm), this and other fluoride compounds are used in limited medical treatment protocols.[citation needed]

Fluoride compounds also have significant uses in synthetic organic chemistry.[7]

### Electronic conductor

CdF2 can be transformed into an electronic conductor when doped with certain rare earth elements, including yttrium; and treated with cadmium vapor under high temperature conditions. This process creates blue crystals with varying absorption coefficients depending on the concentrations of the dopant. A proposed mechanism explains that the conductivity of these crystals can be explained by a reaction of Cd atoms with interstitial F− ions. This creates more CdF2 molecules and releases electrons which are weakly bonded to trivalent dopant ions resulting in n-type conductivity and a hydrogenic donor level.[8]

## Safety

Cadmium fluoride, like all cadmium compounds, is toxic and should be used with care.

Cadmium fluoride can cause potential health issues if it is not handled properly. It can cause irritation to the skin and the eyes, so gloves and protective eyewear are advised. The MSDS, or Material Safety Data Sheet, also includes warnings for ingestion and inhalation. Under acidic conditions, at high temperatures, and in moist environments, hydrogen fluoride and cadmium vapors may be released into the air. Inhalation may cause irritation of the respiratory system as well as congestion, fluorosis, and even pulmonary edema in extreme cases. Cadmium fluoride also has the same potential hazards caused by cadmium and fluoride.[9]

## References

1. ↑ John Rumble (June 18, 2018) (in English). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
2. ↑ 2.0 2.1 2.2 NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0087.html.
3. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
4. ↑ Haendler, Helmut; Bernard, Walter (November 1951). "The Reaction of Fluorine with Cadmium and Some of its Binary Compounds. The Crystal Structure, Density and Melting Points of Cadmium Fluoride.". Journal of the American Chemical Society 73. doi:10.1021/ja01155a064.
5. ↑ Rudzitis, Edgars; Feder, Harold; Hubbard, Ward (November 1963). "Fluorine Bomb Calorimetry. VII. The Heat of Formation of Cadmium Difluoride.". Journal of Physical Chemistry 67 (11): 2388–2390. doi:10.1021/j100805a031.
6. ↑ Besenbruch, G.; Kana'an, A. S.; Margrave, J. L. (March 3, 1965). "Knudson and Langmuir Measurements of the Sublimation Pressure of Cadmium (II) Fluoride". Journal of Physical Chemistry 69 (9): 3174–3176. doi:10.1021/j100893a505.
7. ↑ "Cadmium Fluoride". http://www.americanelements.com/cdf.html.
8. ↑ Weller, Paul (June 1, 1965). "Electrical and Optical Properties of Rare Earth Doped Cadmium Fluoride Single Crystals". Inorganic Chemistry 4 (11): 1545–1551. doi:10.1021/ic50033a004.
9. ↑ "Cadmium Fluoride [CdF2"]. Advance Research Chemicals Inc. / A.R.C.. 2011-04-01. http://www.msds.com/servlet/B2BDocumentDisplay?document_version_nri=5827353&manuf_nri=17573&manuf_name=&supplier_nri=17573&page_number=1&search_source=centraldb&CLIENT_session_key=A793323_tylrpwll&CLIENT_language=2.

## External links

* National Pollutant Inventory - Cadmium and compounds fact sheet
* National Pollutant Inventory - Fluoride and compounds fact sheet

* v
* t
* e

Cadmium compounds

Cadmium(I)|

* Cd2(AlCl4)2

Cadmium(II)|

* Cd(BF4)2
* CdF2
* CdCl2
* CdBr2
* CdI2
* Cd(CN)2
* CdH2
* CdO
* CdS
* CdSe
* CdTe
* Cd(OH)2
* Cd(NO3)2
* CdSO4
* CdWO4
* Cd3As2
* CsCdCl3
* CsCdBr3

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

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*[CID]: Compound ID
*[H301]: Toxic if swallowed
*[H330]: Fatal if inhaled
*[H340]: May cause genetic defects
*[H350]: May cause cancer
*[H360]: May damage fertility or the unborn child
*[H372]: Causes damage to organs through prolonged or repeated exposure
*[H410]: Very toxic to aquatic life with long lasting effects
*[P201]: Obtain special instructions before use
*[P202]: Do not handle until all safety precautions have been read and understood
*[P260]: Do not breathe dust/fume/gas/mist/vapours/spray
*[P264]: Wash … thoroughly after handling
*[P270]: Do not eat, drink or smoke when using this product
*[P271]: Use only outdoors or in a well-ventilated area
*[P273]: Avoid release to the environment
*[P281]: Use personal protective equipment as required
*[P284]: Wear respiratory protection
*[P301+310]: IF SWALLOWED: Immediately call a POISON CENTER or doctor/physician
*[P304+340]: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing
*[P308+313]: IF exposed or concerned: Get medical advice/attention
*[P310]: Immediately call a POISON CENTER or doctor/physician
*[P314]: Get Medical advice/attention if you feel unwell
*[P320]: Specific treatment is urgent (see … on this label)
*[P321]: Specific treatment (see … on this label)
*[P330]: Rinse mouth
*[P391]: Collect spillage
*[P403+233]: Store in a well ventilated place. Keep container tightly closed
*[P405]: Store locked up
*[P501]: Dispose of contents/container to …
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