![]() So the number of valence electrons in antimony trifluoride.Īccording to the formula there is one antimony and three fluorine atoms in the structure. ![]() We must know the number of valence electrons in order to draw the structure. This is the Swarts reaction which is usually employed in the production of compounds of organofluorine. ![]() Where antimony trifluoride was treated with chlorine which gave or produced trifluorodichloride. This was first discovered by Fredric J.E Swarts in the year 1892 (as to how it can be used for the conversion of chlorides into fluorides). Taking into account its applications it is usually used as a reagent (fluorination) in chemistry (organic). It can be prepared by reacting antimony trioxide and hydrogen fluoride. It has an orthorhombic crystal structure. It is also soluble in organic compounds like acetone, methanol, etc. The solubility at 30 degrees Celsius is 562 g/100 mL. The solubility at 20 degrees Celsius is 443 g/100 mL. The solubility at a temperature of zero degrees Celsius is 385 g/100 mL. Talking about its solubility it can dissolve in water but solubility differs with temperature. The melting point of SbF3 is around 292 degrees Celsius and boils at a temperature of 376 degrees Celsius. It’s observed molecular weight is 178.76 g/mol and has a pungent kind of odor. In appearance, it exists as light grayish or sometimes white colored crystals and has a density of 4.379 g/cm3. The IUPAC nomenclature of SbF3 is trifluorostibane, it is also referred to as Swarts reagent. So we will study the sbf3 lewis structure in detail and various facts related to it in the following sections. So the bonding can be explained by the concept of lewis dot structure. SbF3 or antimony trifluoride is an inorganic compound which has ionic type of bonding. In this article, we are going to analyze how to draw SbF3 and various facts about it.
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