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Tetrafluoride
A tetrafluoride is a chemical compound with four fluorines in its formula. List of tetrafluorides * Argon tetrafluoride, (hypothetical) * Berkelium tetrafluoride *Carbon tetrafluoride (tetrafluoromethane) *Diboron tetrafluoride, a colorless gas * Dinitrogen tetrafluoride (Tetrafluorohydrazine) *Germanium tetrafluoride *Hafnium tetrafluoride * Iridium tetrafluoride * Krypton tetrafluoride, (predicted) *Lead tetrafluoride *Manganese tetrafluoride * Mercury tetrafluoride * Molybdenum tetrafluoride * Niobium tetrafluoride * Oganesson tetrafluoride (predicted) * Oxygen tetrafluoride, (hypothetical) *Palladium tetrafluoride *Platinum tetrafluoride * Plutonium tetrafluoride * Polonium tetrafluoride decomposes via radiolysis. * Protactinium tetrafluoride *Selenium tetrafluoride, , a liquid at standard conditions *Silicon tetrafluoride, or Tetrafluorosilane * Sulfur tetrafluoride, , a gas at standard conditions *Tellurium tetrafluoride, , a stable, white, hygroscopic crystalline solid * ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Selenium Tetrafluoride
Selenium tetrafluoride ( Se F4) is an inorganic compound. It is a colourless liquid that reacts readily with water. It can be used as a fluorinating reagent in organic syntheses (fluorination of alcohols, carboxylic acids or carbonyl compounds) and has advantages over sulfur tetrafluoride in that milder conditions can be employed and it is a liquid rather than a gas. Synthesis The first reported synthesis of selenium tetrafluoride was by Paul Lebeau in 1907, who treated selenium with fluorine: :Se + 2 F2 → SeF4 A synthesis involving more easily handled reagents entails the fluorination of selenium dioxide with sulfur tetrafluoride: :SF4 + SeO2 → SeF4 + SO2 An intermediate in this reaction is seleninyl fluoride (SeOF2). Other methods of preparation include fluorinating elemental selenium with chlorine trifluoride: :3 Se + 4 ClF3 → 3 SeF4 + 2 Cl2 Structure and bonding Selenium in SeF4 has an oxidation state of +4. Its shape in the gaseous phase is similar to that of SF4 ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Thionyl Tetrafluoride
Thionyl tetrafluoride is an inorganic compound gas with the formula S O F4. It is also known as sulfur tetrafluoride oxide. The shape of the molecule is a distorted trigonal bipyramid, with the oxygen found on the equator. The atoms on the equator have shorter bond lengths than the fluorine atoms on the axis. The sulfur oxygen bond is 1.409Å. A S−F bond on the axis has length 1.596Å and the S−F bond on the equator has length 1.539Å. The angle between the equatorial fluorine atoms is 112.8°. The angle between axial fluorine and oxygen is 97.7°. The angle between oxygen and equatorial fluorine is 123.6° and between axial and equatorial fluorine is 85.7°. The fluorine atoms only produce one NMR line, probably because they exchange positions. Formation Thionyl fluoride reacting with fluorine gas can produce thionyl tetrafluoride.Harry Julius Emeléus and A.G. Sharpe ''Advances in Inorganic Chemistry Volume 2'' Academic Press 1960 page 11/ref> This was how the g ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Silicon Tetrafluoride
Silicon tetrafluoride or tetrafluorosilane is a chemical compound with the formula Si F4. This colorless gas is notable for having a narrow liquid range: its boiling point is only 4 °C above its melting point. It was first prepared in 1771 by Carl Wilhelm Scheele by dissolving silica in hydrofluoric acid., later synthesized by John Davy in 1812. It is a tetrahedral molecule and is corrosive. Preparation is a by-product of the production of phosphate fertilizers wet process production, resulting from the attack of HF (derived from fluorapatite protonolysis) on silicates, which are present as impurities in the phosphate rocks. The hydrofluoric acid and silicon dioxide (SiO2) react to produce hexafluorosilicic acid: : 6 HF + SiO2 → H2SiF6 + 2 H2O In the laboratory, the compound is prepared by heating barium hexafluorosilicate (Ba iF6 above whereupon the solid releases volatile , leaving a residue of . : Alternatively, sodium hexafluorosilicate () may also be ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Carbon Tetrafluoride
Tetrafluoromethane, also known as carbon tetrafluoride or R-14, is the simplest perfluorocarbon ( C F4). As its IUPAC name indicates, tetrafluoromethane is the perfluorinated counterpart to the hydrocarbon methane. It can also be classified as a haloalkane or halomethane. Tetrafluoromethane is a useful refrigerant but also a potent greenhouse gas. It has a very high bond strength due to the nature of the carbon–fluorine bond. Bonding Because of the multiple carbon–fluorine bonds, and the high electronegativity of fluorine, the carbon in tetrafluoromethane has a significant positive partial charge which strengthens and shortens the four carbon–fluorine bonds by providing additional ionic character. Carbon–fluorine bonds are the strongest single bonds in organic chemistry. Additionally, they strengthen as more carbon–fluorine bonds are added to the same carbon. In the one carbon organofluorine compounds represented by molecules of fluoromethane, difluoromethane, trifl ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Manganese Tetrafluoride
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.. Preparation Manganese tetrafluoride was first unequivocally prepared in 1961 by the reaction of manganese(II) fluoride (or other MnII compounds) with a stream of fluorine gas at 550 °C: the MnF4 sublimes into the gas stream and condenses onto a cold finger. This is still the commonest method of preparation, although the sublimation can be avoided by operating at increased fluorine pressure (4.5–6 bar at 180–320 °C) and mechanically agitating the powder to avoid sintering of the grains.. The reaction can also be carried out starting from manganese powder in a fluidized bed. Other preparations of MnF4 include the fluorination of MnF2 with krypton difluoride, or with F2 in liquid hydrogen fluoride solution under ultraviolet light.. Manganese tetrafluoride has also been prepared (but not isolated) in an a ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Diboron Tetrafluoride
Diboron tetrafluoride is the inorganic compound with the formula (BF2)2. A colorless gas, the compound has a halflife of days at room temperature. It is the most stable of the diboron tetrahalides. Structure and bonding Diboron tetrafluoride is a planar molecule with a B-B bond distance of 172 pm. Although it is electron-deficient, the unsaturated boron centers are stabilized by pi-bonding with the terminal fluoride ligands. The compound is isoelectronic with oxalate. Synthesis and reactions Diboron tetrafluoride can be formed by treating boron monofluoride with boron trifluoride at low temperatures, taking care not to form higher polymers. Addition of diboron tetrafluoride to Vaska's complex was employed to produce an early example of a transition metal boryl complex In chemistry, a transition metal boryl complex is a molecular species with a formally anionic boron center coordinated to a transition metal. They have the formula LnM-BR2 or LnM-(BR2LB) (L = ligand, R = H ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Sulfur Tetrafluoride
Sulfur tetrafluoride is the chemical compound with the formula S F4. 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. Structure Sulfur in SF4 is in the formal +4 oxidation state. Of sulfur's total of six valence electrons, two form a lone pair. The structure of SF4 can therefore be anticipated using the principles of VSEPR theory: it is a see-saw shape, with S at the center. One of the three equatorial positions is occupied by a nonbonding lone pair of electrons. Consequently, the molecule has two distinct types of F ligands, two axial and two equatorial. The relevant bond distances are = 164.3 pm and = 154.2 pm. It is typical for the axial ligands in hypervalent molecules to be bonded less strongly. In c ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Germanium Tetrafluoride
Germanium tetrafluoride (GeF4) is a chemical compound of germanium and fluorine. It is a colorless gas. Synthesis Germanium tetrafluoride is formed by treating germanium with fluorine: : Ge + 2 F2 → GeF4 Alternatively germanium dioxide combines with hydrofluoric acid Hydrofluoric acid is a Solution (chemistry), solution of hydrogen fluoride (HF) in water. Solutions of HF are colourless, acidic and highly Corrosive substance, corrosive. It is used to make most fluorine-containing compounds; examples include th ... (HF): : GeO2 + 4 HF → GeF4 + 2 H2O It is also formed during the thermal decomposition of a complex salt, Ba eF6 : Ba(GeF6) → GeF4 + BaF2 Properties Germanium tetrafluoride is a noncombustible, strongly fuming gas with a garlic-like odor. It reacts with water to form hydrofluoric acid and germanium dioxide. Decomposition occurs above 1000 °C. Reaction of GeF4 with fluoride sources produces GeF5− anions with octahedral coordination around Ge atom due to ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Tellurium Tetrafluoride
Tellurium tetrafluoride, TeF4, is a stable, white, hygroscopic crystalline solid and is one of two fluorides of tellurium. The other binary fluoride is tellurium hexafluoride.''Inorganic Chemistry'',Egon Wiberg, Arnold Frederick Holleman Elsevier 2001 The widely reported Te2F10 has been shown to be F5TeOTeF5 There are other tellurium compounds that contain fluorine, but only the two mentioned contain solely tellurium and fluorine. Tellurium difluoride, TeF2, and ditellurium difluoride, Te2F2 are not known. Preparation Tellurium tetrafluoride can be prepared by the following reaction: : TeO2 + 2 SF4 → TeF4 + 2 SOF2 It is also prepared by reacting nitryl fluoride with tellurium or from the elements at 0 °C or by reacting selenium tetrafluoride with tellurium dioxide at 80 °C. Fluorine in nitrogen can react with TeCl2 or TeBr2 to form TeF4. PbF2 will also fluorinate tellurium to TeF4. Reactivity Tellurium tetrafluoride will react with water or silica and form ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Platinum Tetrafluoride
Platinum tetrafluoride is the inorganic compound with the chemical formula . In the solid state, the compound features platinum(IV) in octahedral coordination geometry. Preparation The compound was first reported by Henri Moissan by the fluorination of platinum metal in the presence of hydrogen fluoride. A modern synthesis involves thermal decomposition of platinum hexafluoride. Properties Platinum tetrafluoride vapour at 298.15 K consists of individual molecules. The enthalpy of sublimation is 210 kJmol−1. Original analysis of powdered PtF4 suggested a tetrahedral molecular geometry, but later analysis by several methods identified it as octahedral, with four of the six fluorines on each platinum bridging to adjacent platinum centres. Reactions A solution of platinum tetrafluoride in water is coloured reddish brown, but it rapidly decomposes, releasing heat and forming an orange coloured platinum dioxide hydrate precipitate and fluoroplatinic acid. When heated to a red ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Tin Tetrafluoride
Tin(IV) fluoride is a chemical compound of tin and fluorine with the chemical formula SnF4 and is a white solid with a melting point above 700 °C. SnF4 can be prepared by the reaction of tin metal with fluorine gas: :Sn + 2F2 → SnF4 However, a passivating metal fluoride layer will be created and the surface will eventually become unreactive. An alternative synthesis is the reaction of SnCl4 with anhydrous hydrogen fluoride: :SnCl4 + 4HF → SnF4 + 4HCl With alkali metal fluorides (e.g. KF) hexafluorostannates are produced (e.g.K2SnF6), which contain the octahedral SnF62− anion. SnF4 behaves as a Lewis acid and adducts L2·SnF4 and L·SnF4 have been produced. Structure Unlike the other tin tetrahalides, tin(IV) chloride, tin(IV) bromide, and tin(IV) iodide, which contain tetrahedrally coordinated tin, tin(IV) fluoride contains planar layers of octahedrally coordinated tin, where the octahedra share four corners and there are two terminal, unshared, fluorine atoms ''tr ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Uranium Tetrafluoride
Uranium tetrafluoride is the inorganic compound with the formula UF4. It is a green solid with an insignificant vapor pressure and low solubility in water. Uranium in its tetravalent (uranous) state is important in various technological processes. In the uranium refining industry it is known as green salt. Production UF4 is prepared from UO2 in a fluidized bed by reaction with HF. The UO2 is derived from mining operations. Around 60,000 tonnes per year are prepared in this way annually. A common impurity is UO2F2. UF4 is susceptible to hydrolysis as well. UF4 is formed by the reaction of UF6 with hydrogen gas in a vertical tube-type reactor. UF4 is less stable than the uranium oxides and reacts slowly with moisture at ambient temperature, forming UO2 and HF, the latter of which is very corrosive and toxic; it is thus less favourable for long-term disposal. The bulk density of UF4 varies from about 2.0 g/cm3 to about 4.5 g/cm3 depending on the production process and the prop ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
