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  2. Sulfur dioxide - Wikipedia

    en.wikipedia.org/wiki/Sulfur_dioxide

    Sulfur dioxide is the product of the burning of sulfur or of burning materials that contain sulfur: S 8 + 8 O 2 → 8 SO 2 , ΔH = −297 kJ/mol To aid combustion, liquified sulfur (140–150 °C (284–302 °F) is sprayed through an atomizing nozzle to generate fine drops of sulfur with a large surface area.

  3. Cheletropic reaction - Wikipedia

    en.wikipedia.org/wiki/Cheletropic_reaction

    Case 3 & 4: the single atom is the sulfur in sulfur dioxide (SO 2), which joins the alkene chains to form a ring. In organic chemistry , cheletropic reactions , also known as chelotropic reactions , [ 2 ] are a type of pericyclic reaction (a chemical reaction that involves a transition state with a cyclic array of atoms and an associated cyclic ...

  4. SO2 - Wikipedia

    en.wikipedia.org/wiki/So2

    Sulfur dioxide (SO 2), a colorless gas with a pungent smell Sulfonyl group (R-SO 2-R), a functional group found primarily in sulfones, or a substituent; SO(2), special orthogonal group of degree 2 in mathematics; Oxygen saturation (SO 2), the concentration of oxygen dissolved in a medium

  5. Molecular orbital diagram - Wikipedia

    en.wikipedia.org/wiki/Molecular_orbital_diagram

    The possible orbital symmetries are listed in the table below. For example, an orbital of B 1 symmetry (called a b 1 orbital with a small b since it is a one-electron function) is multiplied by -1 under the symmetry operations C 2 (rotation about the 2-fold rotation axis) and σ v '(yz) (reflection in the molecular

  6. Woodward–Hoffmann rules - Wikipedia

    en.wikipedia.org/wiki/Woodward–Hoffmann_rules

    An isolated p-or sp x-orbital (unfilled or filled, symbol ω) A conjugated π system (symbol π) A σ bond (symbol σ) The electron count of a component is the number of electrons in the orbital(s) of the component: The electron count of an unfilled ω orbital (i.e., an empty p orbital) is 0, while that of a filled ω orbital (i.e., a lone pair ...

  7. Metal sulfur dioxide complex - Wikipedia

    en.wikipedia.org/wiki/Metal_sulfur_dioxide_complex

    The "insertion" proceed the sulfur dioxide between the metal and the alkyl ligand leads to the O, O'-sulphinate. Alternatively an O-sulphinate can arise. Both of these intermediates commonly convert to an S-sulphinate. [5] S-sulphinate has sulfur–oxygen stretching frequencies from 1250–1000 cm −1 and 1100–1000 cm −1.

  8. Orbital hybridisation - Wikipedia

    en.wikipedia.org/wiki/Orbital_hybridisation

    Chemist Linus Pauling first developed the hybridisation theory in 1931 to explain the structure of simple molecules such as methane (CH 4) using atomic orbitals. [2] Pauling pointed out that a carbon atom forms four bonds by using one s and three p orbitals, so that "it might be inferred" that a carbon atom would form three bonds at right angles (using p orbitals) and a fourth weaker bond ...

  9. Polyhalogen ions - Wikipedia

    en.wikipedia.org/wiki/Polyhalogen_ions

    The bonding in polyhalogen ions mostly invoke the predominant use of p-orbitals. Significant d-orbital participation in the bonding is improbable as much promotional energy will be required, while scant s-orbital participation is expected in iodine-containing species due to the inert-pair effect, suggested by data from Mössbauer spectroscopy ...