“Zinc fluoride”的意思、由来-开放百科全书

词条

Zinc fluoride

释义

Preparation and reactions
References
External links

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 454732113
| Name = Zinc fluoride
| ImageFile = Zinc-fluoride-3D-balls.png
| ImageName = Zinc fluoride
| OtherNames = Zinc difluoride
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 22957
| InChI = 1/2FH.Zn/h2*1H;/q;;+2/p-2
| InChIKey = BHHYHSUAOQUXJK-NUQVWONBAR
| SMILES = F[Zn]F
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/2FH.Zn/h2*1H;/q;;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = BHHYHSUAOQUXJK-UHFFFAOYSA-L
| CASNo = 7783-49-5
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo2_Ref = {{cascite|changed|??}}
| CASNo2 = 13986-18-0
| CASNo2_Comment = (tetrahydrate)
| PubChem = 24551
| RTECS = ZH3200000
|Section2={{Chembox Properties
| Formula = ZnF₂
| MolarMass = 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)
| Solubility = .000052 g/100 mL (anhydrous)
1.52 g/100 mL, 20 °C (tetrahydrate)
| SolubleOther = sparingly soluble in HCl, HNO₃, ammonia
| MeltingPtC = 872
| MeltingPt_notes = (anhydrous)
100 °C, decomposes (tetrahydrate)
| BoilingPtC = 1500
| BoilingPt_notes = (anhydrous)
| MagSus = −38.2·10⁻⁶ cm³/mol
|Section3={{Chembox Structure
| CrystalStruct = tetragonal (anhydrous), tP6
| SpaceGroup = P4₂/mnm, No. 136
|Section7={{Chembox Hazards
| EUClass = {{Hazchem T+}}{{Hazchem Xn}}{{Hazchem N}}
| NFPA-H = 3
| NFPA-R = 0
| NFPA-F = 0
}}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.^[3]

Preparation and reactions

Zinc fluoride can be synthesized several ways.

Reaction of a fluoride salt with zinc chloride, to yield zinc fluoride and a chloride salt, in aqueous solution.{{Citation needed|date=January 2009}}
The reaction of zinc metal with fluorine gas.^[2]
Reaction of hydrofluoric acid with zinc, to yield hydrogen gas (H₂) and zinc fluoride (ZnF₂).^[2]

Zinc fluoride can be hydrolysed by hot water to form the zinc hydroxyfluoride, Zn(OH)F.^[4]

References

1. ^{{ cite book |author1=Perry, D. L. |author2=Phillips, S. L. | year = 1995 | title = Handbook of Inorganic Compounds | publisher = CRC Press | isbn = 0-8493-8671-3 }}
2. ^¹²{{Greenwood&Earnshaw}}
3. ^{{Greenwood&Earnshaw}}
4. ^{{ cite journal |author1=Srivastava, O. K. |author2=Secco, E. A. | title = Studies on Metal Hydroxy Compounds. I. Thermal Analyses of Zinc Derivatives ε-Zn(OH)₂, Zn₅(OH)₈Cl₂ · H₂O, β-ZnOHCl, and ZnOHF | journal = Canadian Journal of Chemistry | year = 1967 | volume = 45 | issue = 6 | pages = 579–583 | doi = 10.1139/v67-096 | url = http://www.nrcresearchpress.com/doi/pdf/10.1139/v67-096 | format = pdf }}

External links

{{ cite web | url = http://www.americanelements.com/znf.html | title = Zinc Fluoride | publisher = American Elements }}

4 : Fluorides|Metal halides|Zinc compounds|Inorganic compound stubs

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