\n| Odor = Odorless\n| Density = 3.15 g/cm3(20 °C)
2.975 g/cm3(23 °C){{cite book|last = Kwasnik|first = W.|editor-last = Brauer|editor-first = Georg|year = 1963|title = Handbook of Preparative Inorganic Chemistry|url = https://archive.org/details/handbookpreparat01brau_517|url-access = limited|publisher = Academic Press|place = London|edition = UK|pages = [https://archive.org/details/handbookpreparat01brau_517/page/n276 252]–253}}\n| Solubility = Very soluble\n| SolubleOther = Soluble in [[acetone]],[[acetic acid]]
Very slightly soluble in [[thionyl chloride|SO2Cl2]],[[Alcohol (chemistry)|alcohol]]s,[[chloroform|CHCl3]]\n| MeltingPtC = 325\n| MeltingPt_notes =
at 760 mmHg decomposes{{CRC90}}\n| BoilingPt = Sublimes\n}}"},"Section3":{"wt":"{{Chembox Structure\n| CrystalStruct = [[Monoclinic]],[[Pearson symbol|mP10]]\n| SpaceGroup = P21/c,No. 14\n}}"},"Section4":{"wt":"{{Chembox Thermochemistry\n| DeltaHf = −1412 kJ/mol{{cite web|last = Anatolievich|first = Kiper Ruslan|website=chemister.ru|url = http://chemister.ru/Database/properties-en.php?dbid=1&id=408|title = vanadium(IV) fluoride|access-date = 2014-06-25}}\n| DeltaGf = −1312 kJ/mol\n| Entropy = 126 J/mol·K\n}}"},"Section7":{"wt":"{{Chembox Hazards\n| GHSPictograms ={{GHS05}}{{GHS06}}\n| GHS_ref = {{cite web|title = Vanadium(IV) fluoride,95%|url = http://www.alfa.com/en/catalog/11543|website=alfa.com|publisher = Alfa Aesar|access-date = 2014-06-25}}\n| GHSSignalWord = Danger\n| HPhrases ={{H-phrases|300|330|314}}\n| PPhrases ={{P-phrases|260|301+310|303+361+353|304+340|305+351+338|320|330|405|501}}\n| SkinHazard = Causes burns\n| EyeHazard = Causes serious damage\n}}"}},"i":0}}]}" id="mwAg">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}
Names | |||
---|---|---|---|
IUPAC name vanadium tetrafluoride | |||
Identifiers | |||
3D model (JSmol) | |||
ChemSpider | |||
ECHA InfoCard | 100.030.143 | ||
EC Number |
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PubChem CID | |||
UNII | |||
UN number | UN2923 | ||
CompTox Dashboard (EPA) | |||
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Properties | |||
F4V | |||
Molar mass | 126.9351 g·mol−1 | ||
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 | 325 °C (617 °F; 598 K) at 760 mmHg decomposes [1] | ||
Boiling point | Sublimes [1] | ||
Very soluble [1] | |||
Solubility | Soluble in acetone, acetic acid Very slightly soluble in SO2Cl2, alcohols, CHCl3 [2] | ||
Structure | |||
Monoclinic, mP10 | |||
P21/c, No. 14 | |||
Thermochemistry | |||
Std molar entropy (S⦵298) | 126 J/mol·K [3] | ||
Std enthalpy of formation (ΔfH⦵298) | −1412 kJ/mol [3] | ||
Gibbs free energy (ΔfG⦵) | −1312 kJ/mol [3] | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Eye hazards | Causes serious damage | ||
Skin hazards | Causes burns | ||
GHS labelling: [4] | |||
Danger | |||
H300, H314, H330 | |||
P260, P301+P310, P303+P361+P353, P304+P340, P305+P351+P338, P320, P330, P405, P501 | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). |
Vanadium(IV) fluoride (V F4) 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. [5] It decomposes before melting.
VF4 can be prepared by treating VCl4 with HF:
It was first prepared in this way. [6]
It decomposes at 325 °C, undergoing disproportionation to the tri- and pentafluorides: [2]
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. [7]
Thionyl fluoride is the inorganic compound with the formula SOF
2. This colourless gas is mainly of theoretical interest, but it is a product of the degradation of sulfur hexafluoride, an insulator in electrical equipment. The molecule adopts a distorted pyramidal structure, with Cs symmetry. The S-O and S-F distances are 1.42 and 1.58 Å, respectively. The O-S-F and F-S-F angles are 106.2 and 92.2°, respectively. Thionyl chloride and thionyl bromide have similar structures, although these compounds are liquid at room temperature. Mixed halides are also known, such as SOClF, thionyl chloride fluoride.
Antimony pentafluoride is the inorganic compound with the formula SbF5. This colourless, viscous liquid is a strong Lewis acid and a component of the superacid fluoroantimonic acid, formed upon mixing liquid HF with liquid SbF5 in 1:1 ratio. It is notable for its strong Lewis acidity and the ability to react with almost all known compounds.
Plutonium(IV) fluoride is a chemical compound with the formula (PuF4). This salt is generally a brown solid but can appear a variety of colors depending on the grain size, purity, moisture content, lighting, and presence of contaminants. Its primary use in the United States has been as an intermediary product in the production of plutonium metal for nuclear weapons usage.
Vanadium(III) chloride describes the inorganic compound with the formula VCl3 and its hydrates. It forms a purple anhydrous form and a green hexahydrate [VCl2(H2O)4]Cl·2H2O. These hygroscopic salts are common precursors to other vanadium(III) complexes and is used as a mild reducing agent.
Sulfur tetrafluoride is the chemical compound with the formula SF4. It is a colorless corrosive gas that releases dangerous HF upon exposure to water or moisture. Despite these unwelcome characteristics, this compound is a useful reagent for the preparation of organofluorine compounds, some of which are important in the pharmaceutical and specialty chemical industries.
Vanadium(III) fluoride is the chemical compound with the formula VF3. This yellow-green, refractory solid is obtained in a two-step procedure from V2O3. Similar to other transition-metal fluorides (such as MnF2), it exhibits magnetic ordering at low temperatures (e.g. V2F6.4H2O orders below 12 K).
Tungsten oxytetrafluoride is an inorganic compound with the formula WOF4. It is a colorless diamagnetic solid. The compound is one of many oxides of tungsten. It is usually encountered as product of the partial hydrolysis of tungsten hexafluoride.
Titanium(IV) fluoride is the inorganic compound with the formula TiF4. It is a white hygroscopic solid. In contrast to the other tetrahalides of titanium, it adopts a polymeric structure. In common with the other tetrahalides, TiF4 is a strong Lewis acid.
The dioxygenyl(or dioxyl) ion, O+
2, is a rarely-encountered oxycation in which both oxygen atoms have a formal oxidation state of +1/2. It is formally derived from oxygen by the removal of an electron:
Manganese tetrafluoride, MnF4, is the highest fluoride of manganese. It is a powerful oxidizing agent and is used as a means of purifying elemental fluorine.
Iridium(V) fluoride, IrF5, is a chemical compound of iridium and fluorine. A highly reactive yellow low melting solid, it has a tetrameric structure, Ir4F20, which contains octahedrally coordinated iridium atoms. This structure is shared with RuF5 and OsF5. It can be prepared by the controlled decomposition of IrF6 or the reduction of IrF6 with silicon powder or H2 in anhydrous HF.
Dinitrogen difluoride is a chemical compound with the formula N2F2. It is a gas at room temperature, and was first identified in 1952 as the thermal decomposition product of the azide FN3. It has the structure F−N=N−F and exists in both a cis- and trans-form.
Vanadium(V) fluoride is the inorganic compound with the chemical formula VF5. It is a colorless volatile liquid. It is a highly reactive compound, as indicated by its ability to fluorinate organic substances.
Germanium tetrafluoride (GeF4) is a chemical compound of germanium and fluorine. It is a colorless gas.
Chromium pentafluoride is the inorganic compound with the chemical formula CrF5. It is a red volatile solid that melts at 34 °C. It is the highest known chromium fluoride, since the hypothetical chromium hexafluoride has not yet been synthesized.
Fluorine forms a great variety of chemical compounds, within which it always adopts an oxidation state of −1. With other atoms, fluorine forms either polar covalent bonds or ionic bonds. Most frequently, covalent bonds involving fluorine atoms are single bonds, although at least two examples of a higher order bond exist. Fluoride may act as a bridging ligand between two metals in some complex molecules. Molecules containing fluorine may also exhibit hydrogen bonding. Fluorine's chemistry includes inorganic compounds formed with hydrogen, metals, nonmetals, and even noble gases; as well as a diverse set of organic compounds. For many elements the highest known oxidation state can be achieved in a fluoride. For some elements this is achieved exclusively in a fluoride, for others exclusively in an oxide; and for still others the highest oxidation states of oxides and fluorides are always equal.
Hafnium tetrafluoride is the inorganic compound with the formula HfF4. It is a white solid. It adopts the same structure as zirconium tetrafluoride, with 8-coordinate Hf(IV) centers.
Chromium(IV) fluoride is an inorganic compound with the chemical formula CrF4. It has a dark greenish-black color when solid. It rapidly hydrolysizes in presence of moisture in air or directly in water.
Platinum tetrafluoride is the inorganic compound with the chemical formula PtF
4. In the solid state, the compound features platinum(IV) in octahedral coordination geometry.
Praseodymium(IV) fluoride (also praseodymium tetrafluoride) is a binary inorganic compound, a highly oxidised metal salt of praseodymium and fluoride with the chemical formula PrF4.