Vanadium tetrafluoride
<templatestyles src="Chembox/styles.css"/>
Template:Chembox AllOtherNamesTemplate:Chembox headerbarTemplate:Chembox IndexlistTemplate:Chembox JmolTemplate:Chembox ChEMBLTemplate:Chembox ECHATemplate:Chembox E numberTemplate:Chembox IUPHAR ligandTemplate:Chembox UNIITemplate:Chembox CompToxTemplate:Chembox headerbarTemplate:Chembox SolubilityInWaterTemplate:Chembox headerbarTemplate:Chembox headerbarTemplate:Chembox DeltaGfreeTemplate:Chembox headerbarTemplate:Chembox OHS (set)Template:Chembox GHS (set)Template:Chembox Datapage checkTemplate:Chembox Footer| Template:Chembox image sbs cell | |
| Template:Longitem | Template:Unbulleted list |
| ChEBI | Template:Unbulleted list |
| ChemSpider | Template:Unbulleted list |
| DrugBank | Template:Unbulleted list |
| EC Number | Template:Unbulleted list |
| KEGG | Template:Unbulleted list |
| Template:Longitem | Template:Unbulleted list |
| RTECS number | Template:Unbulleted list |
| UN number | UN2923 |
| Script error: No such module "collapsible list". | |
| Script error: No such module "collapsible list". | |
| Template:Longitem | Template:Chembox Elements/molecular formula |
| Molar mass | Template:Chem molar mass |
| Appearance | Lime green powder, hygroscopic[1] |
| Odor | Odorless |
| Density | 3.15 g/cm3 (20 °C)[1] 2.975 g/cm3 (23 °C)[2] |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Solubility | Soluble in acetone, acetic acid Very slightly soluble in SO2Cl2, alcohols, CHCl3[2] |
| Template:Longitem | Monoclinic, mP10 |
| Template:Longitem | P21/c, No. 14 |
| Template:Longitem | 126 J/mol·K[3] |
| Template:Longitem | −1412 kJ/mol[3] |
Template:Chembox Footer/trackingScript error: No such module "TemplatePar".Template:Short description
Vanadium(IV) fluoride (VF4) is an inorganic compound of vanadium and fluorine. It is paramagnetic yellow-brown solid that is very hygroscopic.[2] Unlike the corresponding vanadium tetrachloride, the tetrafluoride is not volatile because it adopts a polymeric structure.[4] It decomposes before melting.
Preparation and reactions
VF4 can be prepared by treating VCl4 with HF:
- VCl4 + 4 HF → VF4 + 4 HCl
It was first prepared in this way.[5]
It decomposes at 325 °C, undergoing disproportionation to the tri- and pentafluorides:[2]
- 2 VF4 → VF3 + VF5
Structure
The structure of VF4 is related to that of SnF4. Each vanadium centre is octahedral, surrounded by six fluoride ligands. Four of the fluoride centers bridge to adjacent vanadium centres.[6]
Script error: No such module "Gallery".
References
<templatestyles src="Reflist/styles.css" />
- ↑ a b c d e Template:CRC90
- ↑ a b c d Script error: No such module "citation/CS1".
- ↑ a b c Script error: No such module "citation/CS1".
- ↑ Script error: No such module "citation/CS1".
- ↑ Otto Ruff, Herbert Lickfett "Vanadinfluoride" Chemische Berichte 1911, vol. 44, pages 2539–2549. Script error: No such module "CS1 identifiers".
- ↑ Becker S., Muller B. G. Vanadium Tetrafluoride, Angew. Chem. Intnl. Ed. Engl. 1990, vol. 29, page 406
Script error: No such module "Check for unknown parameters".
External links
Script error: No such module "Navbox". Template:Fluorine compounds