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Interhalogen Compounds
In chemistry, an interhalogen compound is a molecule which contains two or more different halogen atoms (fluorine, chlorine, bromine, iodine, or astatine) and no atoms of elements from any other group. Most interhalogen compounds known are binary (composed of only two distinct elements). Their formulae are generally , where ''n'' = 1, 3, 5 or 7, and X is the less electronegative of the two halogens. The value of ''n'' in interhalogens is always odd, because of the odd valence of halogens. They are all prone to hydrolysis, and ionize to give rise to polyhalogen ions. Those formed with astatine have a very short half-life due to astatine being intensely radioactive. No interhalogen compounds containing three or more different halogens are definitely known, although a few books claim that and have been obtained, and theoretical studies seem to indicate that some compounds in the series are barely stable. Some interhalogens, such as , , and , are good halogenating agents. is to ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chemistry
Chemistry is the science, scientific study of the properties and behavior of matter. It is a natural science that covers the Chemical element, elements that make up matter to the chemical compound, compounds made of atoms, molecules and ions: their composition, structure, properties, behavior and the changes they undergo during a Chemical reaction, reaction with other Chemical substance, substances. Chemistry also addresses the nature of chemical bonds in chemical compounds. In the scope of its subject, chemistry occupies an intermediate position between physics and biology. It is sometimes called the central science because it provides a foundation for understanding both Basic research, basic and Applied science, applied scientific disciplines at a fundamental level. For example, chemistry explains aspects of plant growth (botany), the formation of igneous rocks (geology), how atmospheric ozone is formed and how environmental pollutants are degraded (ecology), the properties ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Fluorine Azide
Fluorine azide or triazadienyl fluoride is a yellow green gas composed of nitrogen and fluorine with formula . It is counted as an interhalogen compound, as the azide functional group is termed a pseudohalogen. It resembles , , and in this respect. The bond between the fluorine atom and the nitrogen is very weak, leading to this substance being very unstable and prone to explosion. Calculations show the F–N–N angle to be around 102° with a straight line of 3 nitrogen atoms. The gas boils at –30° and melts at –139 °C. It was first made by John F. Haller in 1942. Reactions Fluorine azide can be made by reacting hydrazoic acid and fluorine gas. Another way to form it is by reacting sodium azide with fluorine. Fluorine azide decomposes without explosion at normal temperatures to make dinitrogen difluoride: :. At higher temperatures such as 1000 °C fluorine azide breaks up into nitrogen monofluoride radical: : The FN itself dimerizes on cooling. : Sol ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromine Trifluoride
Bromine trifluoride is an interhalogen compound with the formula BrF3. At room temperature, it is a straw-coloured liquid with a pungent odor which decomposes violently on contact with water and organic compounds. It is a powerful fluorinating agent and an ionizing inorganic solvent. It is used to produce uranium hexafluoride (UF6) in the processing and reprocessing of nuclear fuel. Synthesis Bromine trifluoride was first described by Paul Lebeau in 1906, who obtained the material by the reaction of bromine with fluorine at 20 °C: : The disproportionation of bromine monofluoride also gives bromine trifluoride: : Structure Like ClF3 and IF3, the BrF3 molecule is T-shaped and planar. In the VSEPR formalism, the bromine center is assigned two electron pairs. The distance from the bromine each axial fluorine is 1.81 Å and to the equatorial fluorine is 1.72 Å. The angle between an axial fluorine and the equatorial fluorine is slightly smaller than 90° — the 86.2° ang ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Bromine Monofluoride
Bromine monofluoride is a quite unstable interhalogen compound with the chemical formula BrF. It can be produced through the reaction of bromine trifluoride (or bromine pentafluoride) and bromine. Due to its lability, the compound can be detected but not isolated: :BrF3 + Br2 → 3 BrF :BrF5 + 2 Br2 → 5 BrF :Br2(l) + F2(g) → 2 BrF(g) It is usually generated in the presence of cesium fluoride. Bromine monofluoride decomposes at normal temperature through dismutation to bromine trifluoride, bromine pentafluoride, and free bromine. See also * Bromine trifluoride, BrF3 * Bromine pentafluoride Bromine pentafluoride, Br F5, is an interhalogen compound and a fluoride of bromine. It is a strong fluorinating agent. BrF5 finds use in oxygen isotope analysis. Laser ablation of solid silicates in the presence of BrF5 releases O2 for subsequ ..., BrF5 References Fluorides Bromine(I) compounds Interhalogen compounds {{Inorganic-compound-stub ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorine Pentafluoride
Chlorine pentafluoride is an interhalogen compound with formula ClF5. This colourless gas is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C4v symmetry, as confirmed by its high-resolution 19F NMR spectrum. It was first synthesized in 1963. Preparation Some of the earliest research on the preparation was classified. It was first prepared by fluorination of chlorine trifluoride at high temperatures and high pressures: :ClF3 + F2 → ClF5 :ClF + 2F2 → ClF5 :Cl2 + 5F2 → 2ClF5 :CsClF4 + F2 → CsF + ClF5 NiF2 catalyzes this reaction. Certain metal fluorides, MClF4 (i.e. KClF4, RbClF4, CsClF4), react with F2 to produce ClF5 and the corresponding alkali metal fluoride. Reactions In a highly exothermic reaction, ClF5 reacts with water to produce chloryl fluoride and hydrogen fluoride: : + 2 → + 4 It is also a strong fluorinating agent. At room temperature it reacts readil ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorine Trifluoride
Chlorine trifluoride is an interhalogen compound with the formula ClF3. This colorless, poisonous, corrosive, and extremely reactive gas condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature). The compound is primarily of interest in plasmaless cleaning and etching operations in the semiconductor industry, in nuclear reactor fuel processing, as a component in rocket fuels, and other industrial operations. Preparation, structure, and properties It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine; this also produced ClF (chlorine monofluoride) and the mixture was separated by distillation. :3 F2 + Cl2 → 2 ClF3 The molecular geometry of ClF3 is approximately T-shaped, with one short bond (1.598 Å) and two long bonds (1.698 Å). This structure agrees with the prediction of VSEPR theory, which predicts lone pairs of electrons as occupying two equatorial positions o ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorine Monofluoride
Chlorine monofluoride is a volatile interhalogen compound with the chemical formula ClF. It is a colourless gas at room temperature and is stable even at high temperatures. When cooled to −100 °C, ClF condenses as a pale yellow liquid. Many of its properties are intermediate between its parent halogens, Cl2 and F2. Reactivity Chlorine monofluoride is a versatile fluorinating agent, converting metals and non-metals to their fluorides and releasing Cl2 in the process. For example, it converts tungsten to tungsten hexafluoride and selenium to selenium tetrafluoride: :W + 6 ClF → WF6 + 3 Cl2 :Se + 4 ClF → SeF4 + 2 Cl2 FCl can also chlorofluorinate compounds, either by addition across a multiple bond or via oxidation. For example, it adds fluorine and chlorine to the carbon of carbon monoxide, yielding carbonyl chloride fluoride: :CO + ClF → See also *Chlorine fluoride A chlorine fluoride is an interhalogen compound containing only chlorine and fluorine. {, class= ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cyanogen Iodide
Cyanogen iodide or iodine cyanide (ICN) is a pseudohalogen composed of iodine and the cyanide group. It is a highly toxic inorganic compound. It occurs as white crystals that react slowly with water to form hydrogen cyanide. Synthesis Cyanogen iodide is prepared by combining I2 and a cyanide, most commonly sodium cyanide in ice-cold water. The product is extracted with ether. :I2 + NaCN → NaI + ICN Applications Cyanogen iodide has been used in taxidermy as a preservative because of its toxicity. History Cyanogen iodide was first synthesized in 1824 by the French chemist Georges-Simon Serullas (1774–1832). Cyanogen iodide was considered one of the impurities in commercially sold iodine before the 1930s. Hazards Cyanogen iodide is toxic if inhaled or ingested and may be fatal if swallowed or absorbed through the skin. Cyanogen iodide may cause convulsions, paralysis and death from respiratory failure. It is a strong irritant and may cause burns to the eyes and skin if contac ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cyanogen Bromide
Cyanogen bromide is the inorganic compound with the formula (CN)Br or BrCN. It is a colorless solid that is widely used to modify biopolymers, fragment proteins and peptides (cuts the C-terminus of methionine), and synthesize other compounds. The compound is classified as a pseudohalogen. Synthesis, basic properties, and structure The carbon atom in cyanogen bromide is bonded to bromine by a single bond and to nitrogen by a triple bond (i.e. ). The compound is linear and polar, but it does not spontaneously ionize in water. It dissolves in both water and polar organic solvents. Cyanogen bromide can be prepared by oxidation of sodium cyanide with bromine, which proceeds in two steps via the intermediate cyanogen (): :2 NaCN + Br2 -> (CN)2 + 2 NaBr :(CN)2 + Br2 -> 2 (CN)Br When refrigerated the material has an extended shelflife. Like some other cyanogen compounds, cyanogen bromide undergoes an exothermic trimerisation to cyanuric bromide (). This reaction is catalyzed b ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cyanogen Chloride
Cyanogen chloride is a highly toxic chemical compound with the formula CNCl. This linear, triatomic pseudohalogen is an easily condensed colorless gas. More commonly encountered in the laboratory is the related compound cyanogen bromide, a room-temperature solid that is widely used in biochemical analysis and preparation. Synthesis, basic properties, structure Cyanogen chloride is a molecule with the connectivity . Carbon and chlorine are linked by a single bond, and carbon and nitrogen by a triple bond. It is a linear molecule, as are the related cyanogen halides (NCF, NCBr, NCI). Cyanogen chloride is produced by the oxidation of sodium cyanide with chlorine. This reaction proceeds via the intermediate cyanogen (). :NaCN + Cl2 -> ClCN + NaCl The compound trimerizes in the presence of acid to the heterocycle called cyanuric chloride. Cyanogen chloride is slowly hydrolyzed by water at neutral pH to release cyanate and chloride ions: :ClCN + H2O -> NCO- + Cl- + 2H+ Applicatio ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cyanogen Fluoride
Cyanogen fluoride (molecular formula: FCN; IUPAC name: carbononitridic fluoride) is an inorganic linear compound which consists of a fluorine in a single bond with carbon, and a nitrogen in a triple bond with carbon. It is a toxic and explosive gas at room temperature. It is used in organic synthesis and can be produced by pyrolysis of cyanuric fluoride or by fluorination of cyanogen Cyanogen is the chemical compound with the formula ( C N)2. It is a colorless and highly toxic gas with a pungent odor. The molecule is a pseudohalogen. Cyanogen molecules consist of two CN groups – analogous to diatomic halogen molecu .... Synthesis Cyanogen fluoride (FCN), is synthesized by the pyrolysis of cyanuric fluoride (C3N3F3) at 1300 °C and 50mm pressure; this process gives a maximum of 50% yield. Other products observed were cyanogen and CF3CN. For pyrolysis, an induction heated carbon tube with an internal diameter of 0.75 inches is packed with 4 to 8 mesh carbon gra ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cyanogen
Cyanogen is the chemical compound with the formula ( C N)2. It is a colorless and highly toxic gas with a pungent odor. The molecule is a pseudohalogen. Cyanogen molecules consist of two CN groups – analogous to diatomic halogen molecules, such as Cl2, but far less oxidizing. The two cyano groups are bonded together at their carbon atoms: N≡C‒ C≡N, although other isomers have been detected. The name is also used for the CN radical, and hence is used for compounds such as cyanogen bromide (NCBr) (but see also ''Cyano radical''.) Cyanogen is the anhydride of oxamide: :H2NC(O)C(O)NH2 → NCCN + 2 H2O although oxamide is manufactured from cyanogen by hydrolysis: :NCCN + 2 H2O → H2NC(O)C(O)NH2 Preparation Cyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide: :2 Hg(CN)2 → (CN)2 + Hg2(CN)2 Alternatively, one can combine solutions of copper(II) salts (such as copper(II) sulfate) ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
