enow.com Web Search

Search results

  1. Results from the WOW.Com Content Network
  2. Ethylene - Wikipedia

    en.wikipedia.org/wiki/Ethylene

    Ethylene (IUPAC name: ethene) is a hydrocarbon which has the formula C 2 H 4 or H 2 C=CH 2.It is a colourless, flammable gas with a faint "sweet and musky" odour when pure. [7] It is the simplest alkene (a hydrocarbon with carbon–carbon double bonds).

  3. Hückel method - Wikipedia

    en.wikipedia.org/wiki/Hückel_method

    The Hückel method or Hückel molecular orbital theory, proposed by Erich Hückel in 1930, is a simple method for calculating molecular orbitals as linear combinations of atomic orbitals. The theory predicts the molecular orbitals for π-electrons in π-delocalized molecules , such as ethylene , benzene , butadiene , and pyridine .

  4. Molecular orbital diagram - Wikipedia

    en.wikipedia.org/wiki/Molecular_orbital_diagram

    Molecular orbital diagram of dinitrogen. With nitrogen, we see the two molecular orbitals mixing and the energy repulsion. This is the reasoning for the rearrangement from a more familiar diagram. The σ from the 2p is more non-bonding due to mixing, and same with the 2s σ. This also causes a large jump in energy in the 2p σ* orbital.

  5. Ethylene (data page) - Wikipedia

    en.wikipedia.org/wiki/Ethylene_(data_page)

    Phase behavior Triple point: 104 K (−169 °C), 120 Pa Critical point: 282.5 K (9.4 °C), 50.6 bar Std enthalpy change of fusion, Δ fus H o +3.35 kJ/mol Std entropy change

  6. Ligand field theory - Wikipedia

    en.wikipedia.org/wiki/Ligand_field_theory

    The d xy, d xz and d yz orbitals remain non-bonding orbitals. Some weak bonding (and anti-bonding) interactions with the s and p orbitals of the metal also occur, to make a total of 6 bonding (and 6 anti-bonding) molecular orbitals [7] Ligand-Field scheme summarizing σ-bonding in the octahedral complex [Ti(H 2 O) 6] 3+.

  7. Carbon–carbon bond - Wikipedia

    en.wikipedia.org/wiki/Carbon–carbon_bond

    In ethane, the orbitals are sp 3-hybridized orbitals, but single bonds formed between carbon atoms with other hybridizations do occur (e.g. sp 2 to sp 2). In fact, the carbon atoms in the single bond need not be of the same hybridization. Carbon atoms can also form double bonds in compounds called alkenes or triple bonds in compounds called ...

  8. Zeise's salt - Wikipedia

    en.wikipedia.org/wiki/Zeise's_salt

    Zeise's salt received a great deal of attention during the second half of the 19th century because chemists could not explain its molecular structure. This question remained unanswered until the determination of its X-ray crystal structure in the 20th century.

  9. Pi backbonding - Wikipedia

    en.wikipedia.org/wiki/Pi_backbonding

    σ bonding from electrons in alkene's HOMO to metal center d-orbital. π backbonding from electrons in metal center d-orbital to alkene's LUMO. As in metal–carbonyls, electrons are partially transferred from a d-orbital of the metal to antibonding molecular orbitals of the alkenes and alkynes.