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  2. Covalent bond - Wikipedia

    en.wikipedia.org/wiki/Covalent_bond

    A covalent bond is a chemical bond that involves the sharing of electrons to form ... One-electron bonds often have about half the bond energy of a 2-electron bond ...

  3. Chemical bond - Wikipedia

    en.wikipedia.org/wiki/Chemical_bond

    Molecules that are formed primarily from non-polar covalent bonds are often immiscible in water or other polar solvents, but much more soluble in non-polar solvents such as hexane. A polar covalent bond is a covalent bond with a significant ionic character. This means that the two shared electrons are closer to one of the atoms than the other ...

  4. Bond energy - Wikipedia

    en.wikipedia.org/wiki/Bond_energy

    The bond energy for H 2 O is the average energy required to break each of the two O–H bonds in sequence: Although the two bonds are the equivalent in the original symmetric molecule, the bond-dissociation energy of an oxygen–hydrogen bond varies slightly depending on whether or not there is another hydrogen atom bonded to the oxygen atom.

  5. Bonding in solids - Wikipedia

    en.wikipedia.org/wiki/Bonding_in_solids

    A solid with extensive hydrogen bonding will be considered a molecular solid, yet strong hydrogen bonds can have a significant degree of covalent character. As noted above, covalent and ionic bonds form a continuum between shared and transferred electrons; covalent and weak bonds form a continuum between shared and unshared electrons.

  6. Carbon–hydrogen bond - Wikipedia

    en.wikipedia.org/wiki/Carbon–hydrogen_bond

    This bond is a covalent, single bond, meaning that carbon shares its outer valence electrons with up to four hydrogens. This completes both of their outer shells, making them stable. [2] Carbon–hydrogen bonds have a bond length of about 1.09 Å (1.09 × 10 −10 m) and a bond energy of about 413 kJ/mol (see table below).

  7. 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.

  8. Molecular binding - Wikipedia

    en.wikipedia.org/wiki/Molecular_binding

    Reversible covalent – a chemical bond is formed, however the free energy difference separating the noncovalently-bonded reactants from bonded product is near equilibrium and the activation barrier is relatively low such that the reverse reaction which cleaves the chemical bond easily occurs; Irreversible covalent – a chemical bond is formed ...

  9. Binding energy - Wikipedia

    en.wikipedia.org/wiki/Binding_energy

    Bond energy; Bond-dissociation energy Bond energy and bond-dissociation energy are measures of the binding energy between the atoms in a chemical bond. It is the energy required to disassemble a molecule into its constituent atoms. This energy appears as chemical energy, such as that released in chemical explosions, the burning of chemical fuel ...