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  2. Lewis structure - Wikipedia

    en.wikipedia.org/wiki/Lewis_structure

    Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.

  3. Structural formula - Wikipedia

    en.wikipedia.org/wiki/Structural_formula

    Lewis structures (or "Lewis dot structures") are flat graphical formulas that show atom connectivity and lone pair or unpaired electrons, but not three-dimensional structure. This notation is mostly used for small molecules. Each line represents the two electrons of a single bond. Two or three parallel lines between pairs of atoms represent ...

  4. Electron pair - Wikipedia

    en.wikipedia.org/wiki/Electron_pair

    Gilbert N. Lewis introduced the concepts of both the electron pair and the covalent bond in a landmark paper he published in 1916. [1] [2] MO diagrams depicting covalent (left) and polar covalent (right) bonding in a diatomic molecule. In both cases a bond is created by the formation of an electron pair.

  5. Carbon–fluorine bond - Wikipedia

    en.wikipedia.org/wiki/Carbon–fluorine_bond

    The carbon–fluorine bond is a polar covalent bond between carbon and fluorine that is a component of all organofluorine compounds. It is one of the strongest single bonds in chemistry (after the B–F single bond, Si–F single bond, and H–F single bond), and relatively short, due to its partial ionic character.

  6. Molecular solid - Wikipedia

    en.wikipedia.org/wiki/Molecular_solid

    The hydrogen bonding between the acetic acid molecules partially guides the organization of the crystal lattice structure. [26] (a) A lewis dot structure with the partial charges and hydrogen bond denoted with blue dashed line. A ball and stick model of acetic acid with hydrogen bond denoted with blue dashed line.

  7. Lone pair - Wikipedia

    en.wikipedia.org/wiki/Lone_pair

    Lone pairs (shown as pairs of dots) in the Lewis structure of hydroxide. In science, a lone pair refers to a pair of valence electrons that are not shared with another atom in a covalent bond [1] and is sometimes called an unshared pair or non-bonding pair. Lone pairs are found in the outermost electron shell of atoms.

  8. Tetrahedral molecular geometry - Wikipedia

    en.wikipedia.org/wiki/Tetrahedral_molecular_geometry

    The bond angle for a symmetric tetrahedral molecule such as CH 4 may be calculated using the dot product of two vectors. As shown in the diagram at left, the molecule can be inscribed in a cube with the tetravalent atom (e.g. carbon ) at the cube centre which is the origin of coordinates, O.

  9. Carbon–carbon bond - Wikipedia

    en.wikipedia.org/wiki/Carboncarbon_bond

    A carboncarbon bond is a covalent bond between two carbon atoms. [1] The most common form is the single bond: a bond composed of two electrons, one from each of the two atoms. The carboncarbon single bond is a sigma bond and is formed between one hybridized orbital from each