Swarts reaction

Chemical compound Antimony trifluoride is the 3. Sometimes called Swarts' reagent, is one of two principal 5. It appears as a white solid. As well as some industrial applications, Preparation and structure [ ] In solid SbF 3, the Sb centres have 3 is far less volatile than related compounds AsF 3 and SbCl 3. SbF 3 is prepared by treating Sb 2O 3 + 6 HF → 2 SbF 3 + 3 H 2O The compound is a mild SbF 3 + F 2 → SbF 5 Applications [ ] It is used as a 2F 3). This compound can also be produced in bulk. SbF 3 is used in dyeing and in Safety [ ] The lethal minimum dose (guinea pig, oral) is 100mg/kg. References [ ] • ^ a b NIOSH Pocket Guide to Chemical Hazards. • Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf "Antimony and Antimony Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2006, Wiley-VCH, Weinheim. • Chemistry of the Elements (2nded.). 978-0-08-037941-8. • Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 199. • Tariq Mahmood and Charles B. Lindahl Fluorine Compounds, Inorganic, Antimony in Kirk‑Othmer Encyclopedia of Chemical Technology. • Swarts (1892). Acad. Roy. Belg. 3 (24): 474. {{ • • Booth, Harold Simmons; Suttle, John Francis (1946). "IV. The Preparation and Fluorination of Dimethyl and Trimethyl Chlorosilanes". J. Am. Chem. Soc. 68 (12): 2658–2660. • Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf “Antimony and Antimony Compounds” in Ullmann's Encycloped...

We and our partners use cookies to Store and/or access information on a device. We and our partners use data for Personalised ads and content, ad and content measurement, audience insights and product development. An example of data being processed may be a unique identifier stored in a cookie. Some of our partners may process your data as a part of their legitimate business interest without asking for consent. To view the purposes they believe they have legitimate interest for, or to object to this data processing use the vendor list link below. The consent submitted will only be used for data processing originating from this website. If you would like to change your settings or withdraw consent at any time, the link to do so is in our privacy policy accessible from our home page.. What is Swarts reaction? In 1892, Swarts ( Swarts reaction or Swarts fluorination. It involves the partial fluorination of nonpolar organic polyhalides, mostly aliphatic, using antimony trifluoride SbF 3 with antimony pentachloride SbCl 5 or chlorine Cl 2 present. The mixture of antimony trifluoride SbF 3 and chlorine Cl 2 is also called the Swarts reagent or Swarts mixture. Swarts reaction R = alkyl, aryl ( The Swarts reaction is a common exchange reaction between an organic halide and an inorganic fluoride, but it only occurs with activated organic halides. The Swarts rule states that only aryl halides with more than one electron-withdrawing group on the aromatic ring can react with fluoride ...

Silver actually does prefer fluorine over heavier halogens. But this preference involves less (free) energy difference than the preference for the alkyl groups for fluorine. As a result, transfer of fluorine away from the silver has a net favorable energy output. Let's look at some enthalpies of firmation (I cannot readily find free energy data for fluoromethane, so I had to use enthalpies). $\ce$. The methyl group basically wins the alley fight for the fluorine because its muscles (energy for preferentially forming the fluoride) are stronger, leaving the silver to settle for second place (the chlorine). A similar situation occurs naturally on Earth, with Group 16 elements. Practically all metals, even such metals as copper and lead which are usually found as sulfide ores, energetically prefer oxygen over sulfur. But their preference is less than what is seen with some other metals such as calcium, magnesium or even iron. So the latter metals are favored to form oxides, leaving sulfur predominantly for less thermodynamically selective metals like copper and lead. Thanks for contributing an answer to Chemistry Stack Exchange! • Please be sure to answer the question. Provide details and share your research! But avoid … • Asking for help, clarification, or responding to other answers. • Making statements based on opinion; back them up with references or personal experience. Use MathJax to format equations. To learn more, see our

SWARTS, FRéDéRIC JEAN EDMOND ( b. Ixelles, Belgium, 2 September 1866; d. Ghent, Belgium, 6 September 1940) chemistry. Frédéric Swarts entered the University of Ghent in 1883 and received doctorates in chemistry (1889) and medicine (1891). His father, Théodore Swarts had succeeded Kekulé as professor of chemistry at the university in 1871. The younger Swarts spent his entire professional career at Ghent, first as répétiteur and then, on his father’s retirement in 1903, as professor of chemistry. He was a member of the Académie Royale des Sciences des Lettres et des Beaux-Arts de Belgique, which awarded him its Gold Medal, corresponding member of the Institut de France, president of the Institut International de Chimie Solvay, and charter member and vice-president of the International Union of Pure and Applied Chemistry. After the discovery of fluorine, few of its compounds had been prepared because of the reactivity and toxicity of the element. Swarts was among the first to study organic fluorine compounds. Unable to use methods of direct fluorination because of the violence of the reactions, he developed a double decomposition process using inorganic fluorides, especially antimony trifluoride and mercurous fluoride, and organic polyhalides, where the halogen atoms are on the same carbon atom (the Swarts reaction, 1892). The first synthesis of an organic fluorine compound was trichlorofluoromethane (1891). Swarts synthesized many aliphatic chlorofluoro and bromofluoro deriv...