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The structure of [Co(ethylenediamine) 2 (SO 3)N 3]. Color code: blue = N, red = O, yellow = S. [1] Transition metal sulfito complexes are coordination compounds containing sulfite (SO 3 2-) as a ligand. The inventory is large. Few sulfito complexes have commercial applications, but sulfite is a substrate for the molybdoenzyme sulfite oxidase. [2]
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [ 4 ] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
The structure of the sulfite anion Sulfite is a ligand in coordination chemistry.The structure of Co(ethylenediamine) 2 (SO 3)N 3.[4]The structure of the sulfite anion can be described with three equivalent resonance structures.
This shape has D 4d symmetry and is one of the three common shapes for octacoordinate transition metal complexes, along with the dodecahedron and the bicapped trigonal prism. [2] [3] Like with other high coordination numbers, eight-coordinate compounds are often distorted from idealized geometries, as illustrated by the structure of Na 3 TaF 8.
SO 3 is the anhydride of H 2 SO 4. Thus, it is susceptible to hydration: SO 3 + H 2 O → H 2 SO 4 (Δ f H = −200 kJ/mol) [12] Gaseous sulfur trioxide fumes profusely even in a relatively dry atmosphere owing to formation of a sulfuric acid mist. SO 3 is aggressively hygroscopic. The heat of hydration is sufficient that mixtures of SO 3 and ...
Carbon monoxide exemplifies a Lewis structure with formal charges: To obtain the oxidation states, the formal charges are summed with the bond-order value taken positively at the carbon and negatively at the oxygen. Applied to molecular ions, this algorithm considers the actual location of the formal (ionic) charge, as drawn in the Lewis structure.
Metal sulfides are usually prepared by heating mixtures of the two elements, but in the case of scandium, this method yields scandium monosulfide, ScS.Sc 2 S 3 can be prepared by heating scandium(III) oxide under flowing hydrogen sulfide in a graphite crucible to 1550 °C or above for 2–3 hours.
Europium and cerium rare earth sulfite sulfates are produced when heating the metal sulfite trihydrate in air. Ce 2 (SO 3) 3.3H 2 O + 1 ⁄ 2 O 2 → Ce 2 (SO 3) 2 SO 4 + 3H 2 O Ce 2 (SO 3) 3.3H 2 O + O 2 → Ce 2 SO 3 (SO 4) 2 + 3H 2 O Other rare earth sulfite sulfates can be crystallized as hydrates from a water solution. [3]