Systematic Name For Cof2 S

Cobalt(II) fluoride
Names


IUPAC proper noun Cobalt(II) fluoride
Other names cobalt difluoride
Identifiers
CAS Number	10026-17-2 ^North
3D model (JSmol)	Interactive paradigm
ChemSpider	23205 ^Y
ECHA InfoCard	100.030.044
EC Number	233-061-9
PubChem CID	24820
RTECS number	GG0770000
UNII	9KI67810UR ^Northward
CompTox Dashboard (EPA)	DTXSID6064907
InChI InChI=1S/Co.2FH/h;two1H/q+2;;/p-2^Y Central: YCYBZKSMUPTWEE-UHFFFAOYSA-L^Y InChI=1/Co.2FH/h;21H/q+2;;/p-2 Key: YCYBZKSMUPTWEE-NUQVWONBAL
SMILES F[Co]F
Backdrop
Chemical formula	CoF_ii
Molar mass	96.93 g/mol
Appearance	Cherry-red crystalline solid
Density	4.46 g/cmⁱⁱⁱ (anhydrous) 2.22 m/cm³ (tetrahydrate)
Melting point	1,217 °C (2,223 °F; 1,490 Thousand)
Humid point	one,400 °C (2,550 °F; 1,670 K)
Solubility in water	1.4 g/100 mL (25 °C)
Solubility	soluble in HF insoluble in alcohol, ether, benzene
Magnetic susceptibility (χ)	+9490.0·x^−vi cmⁱⁱⁱ/mol
Structure
Crystal construction	tetragonal (a,hydrous) orthorhombic (tetrahydrate)
Hazards
NFPA 704 (burn down diamond)	3 0 0
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	oral (rat): 150 mg/kg
Related compounds
Other anions	cobalt(II) oxide, cobalt(II) chloride
Other cations	atomic number 26(Ii) fluoride, nickel(II) fluoride
Related compounds	cobalt trifluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Nverify (what is^{Y Due north} ?) Infobox references

Chemical compound

Anhydrous cobalt(II) fluoride

Cobalt(Ii) fluoride is a chemical compound with the formula (CoF₂). It is a pink crystalline solid chemical compound^[1] ^[2] which is antiferromagnetic at low temperatures (T_N=37.7 K)^[3] The formula is given for both the red tetragonal crystal, (CoF₂), and the tetrahydrate ruby orthogonal crystal, (CoF_ii·4H_twoO). CoF₂ is used in oxygen-sensitive fields, namely metallic production. In low concentrations, it has public health uses. CoF₂ is sparingly soluble in water. The compound can exist dissolved in warm mineral acid, and volition decompose in boiling water. Yet the hydrate is water-soluble, especially the di-hydrate CoF_two·2H₂ O and tri-hydrate CoF₂·3H_twoO forms of the compound. The hydrate volition also decompose with estrus.

Similar some other metal difluorides, CoF₂ crystallizes in the rutile structure, which features octahedral Co centers and planar fluorides.^[4]

Preparation [edit]

Cobalt(II) fluoride can be prepared from anhydrous cobalt(II) chloride or cobalt(Ii) oxide in a stream of hydrogen fluoride:

CoCl₂ + 2HF → CoF₂ + 2HCl

CoO + 2HF → CoF_two + H_iiO

It is produced in the reaction of cobalt (III) fluoride with h2o.

The tetrahydrate cobalt(Ii) fluoride is formed by dissolving cobalt(2) in hydrofluoric acid. The anhydrous fluoride tin can be extracted from this past dehydration. Other synthesis can occur at college temperatures. It has been shown that at 500 °C fluorine will combine with cobalt producing a mixture of CoF₂ and CoF_iii.^[5]

Uses [edit]

Cobalt(Ii) fluoride can be used every bit a catalyst to alloy metals. It is besides used for optical deposition, of which it tremendously improves optical quality. Cobalt(II) fluoride is available in most volumes in an ultra high purity limerick. Loftier purity compositions ameliorate optical qualities and its usefulness as a standard.

Assay [edit]

To clarify this compound, Cobalt (2) fluoride can exist dissolved in nitric acid. The solution is and then diluted with water until appropriate concentration for AA or ICP spectrophotometry for the cobalt. A minor amount of salt can be dissolved in cold water and analyzed for fluoride ion by a fluoride ion-selective electrode or ion chromatography.

Chemical Backdrop [edit]

CoF₂ is a weak Lewis acid. Cobalt(Ii) complexes are ordinarily octahedral or tetrahedral. As a nineteen-electron species information technology is a good reducing agent, adequately oxidizable into an 18-electron chemical compound. Cobalt(Two) fluoride can be reduced by hydrogen at a 300 °C.

References [edit]

^ Pradyot Patnaik (2002), Handbook of Inorganic Chemicals, McGraw-Hill Professional person, ISBN978-0-07-049439-8
^ Pashkevich, D. Due south.; Radchenko Due south. Grand.; Mukhortov, D. A., "Article title Estrus Exchange between Cobalt(II) Fluoride Powder and the Wall of Rotating Cylinder" (PDF), Russian Journal of Practical Chemistry, Consultants Bureau, ISSN 1070-4272, archived from the original (PDF) on 2004-09-29, retrieved 2007-03-07
^ Ashcroft/Mermin: Solid Land Physics (Tab. 33.two)
^ Stout, J. Westward.; Reed, Stanley A. (1954). "The Crystal Structure of MnF_ii, FeF_ii, CoF₂, NiF_ii and ZnF₂". J. Am. Chem. Soc. 76 (21): 5279–5281. doi:10.1021/ja01650a005.
^ J.C. Bailar (1973), Comprehensive Inorganic Chemical science, Pergoamon