Search results
Results from the WOW.Com Content Network
Ferrocene is an air-stable orange solid with a camphor-like odor. [36] As expected for a symmetric, uncharged species, ferrocene is soluble in normal organic solvents, such as benzene, but is insoluble in water. It is stable to temperatures as high as 400 °C. [36] Ferrocene readily sublimes, especially upon heating
Cyclopentadienyl magnesium bromide undergoes a complex reaction with iron(III) chloride, resulting in ferrocene: [31] 3 C 5 H 5 MgBr + FeCl 3 → Fe(C 5 H 5) 2 + 1/n (C 5 H 5) n + 3 MgBrCl. This conversion, although not of practical value, was important in the history of organometallic chemistry where ferrocene is emblematic of the field. [32]
Iron shows the characteristic chemical properties of the transition metals, namely the ability to form variable oxidation states differing by steps of one and a very large coordination and organometallic chemistry: indeed, it was the discovery of an iron compound, ferrocene, that revolutionalized the latter field in the 1950s. [1]
It reacts violently in water to produce beryllium hydroxide and cyclopentadiene: [2] Be(C 5 H 5) 2 + 2 H 2 O → Be(OH) 2 + 2 C 5 H 6. Like magnesocene, beryllocene also forms ferrocene with iron(II) chloride. [2] The driving force is the formation of the very stable ferrocene molecule. Be(C 5 H 5) 2 + FeCl 2 → BeCl 2 + Fe(C 5 H 5) 2
Space-filling model of ferrocene, the archetypal sandwich compound. In organometallic chemistry, a sandwich compound is a chemical compound featuring a metal bound by haptic, covalent bonds to two arene (ring) ligands. The arenes have the formula C n H n, substituted derivatives (for example C n (CH 3) n) and heterocyclic derivatives (for ...
Ferrocenecarboxaldehyde, owing to the versatility of the formyl group, is a precursor to many ferrocene-modified compounds. With a Wittig reagent, it converts to vinylferrocene and related derivatives. [5] With primary amines, ferrocenecarboxaldehyde condenses to give imines. The azomethine derivative undergoes 1,3-cycloaddition to C 60. [6]
Main page; Contents; Current events; Random article; About Wikipedia; Contact us; Help; Learn to edit; Community portal; Recent changes; Upload file
Iron(II) centres occur in coordination complexes, such as in the anion ferrocyanide, [Fe(CN) 6] 4−, where six cyanide ligands are bound the metal centre; or, in organometallic compounds, such as the ferrocene [Fe(C 2 H 5) 2], where two cyclopentadienyl anions are bound to the Fe II centre.