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  2. Bond energy - Wikipedia

    en.wikipedia.org/wiki/Bond_energy

    In chemistry, bond energy (BE) is one measure of the strength of a chemical bond. It is sometimes called the mean bond , bond enthalpy , average bond enthalpy , or bond strength . [ 1 ] [ 2 ] [ 3 ] IUPAC defines bond energy as the average value of the gas-phase bond-dissociation energy (usually at a temperature of 298.15 K) for all bonds of the ...

  3. Chemical bond - Wikipedia

    en.wikipedia.org/wiki/Chemical_bond

    [2] [3] The atoms in molecules, crystals, metals and other forms of matter are held together by chemical bonds, which determine the structure and properties of matter. All bonds can be described by quantum theory, but, in practice, simplified rules and other theories allow chemists to predict the strength, directionality, and polarity of bonds. [4]

  4. Intramolecular force - Wikipedia

    en.wikipedia.org/wiki/Intramolecular_force

    The bond length, or the minimum separating distance between two atoms participating in bond formation, is determined by their repulsive and attractive forces along the internuclear direction. [3] As the two atoms get closer and closer, the positively charged nuclei repel, creating a force that attempts to push the atoms apart.

  5. Valence bond theory - Wikipedia

    en.wikipedia.org/wiki/Valence_bond_theory

    An important aspect of the valence bond theory is the condition of maximum overlap, which leads to the formation of the strongest possible bonds. This theory is used to explain the covalent bond formation in many molecules. sp 3 hybridization in methane forms four equivalent sigma bonds with tetrahedral geometry.

  6. Intermolecular force - Wikipedia

    en.wikipedia.org/wiki/Intermolecular_force

    A hydrogen bond is an extreme form of dipole-dipole bonding, referring to the attraction between a hydrogen atom that is bonded to an element with high electronegativity, usually nitrogen, oxygen, or fluorine. [4] The hydrogen bond is often described as a strong electrostatic dipole–dipole interaction.

  7. Carbon–fluorine bond - Wikipedia

    en.wikipedia.org/wiki/Carbon–fluorine_bond

    The bond is labeled as "the strongest in organic chemistry," [1] because fluorine forms the strongest single bond to carbon. Carbon–fluorine bonds can have a bond dissociation energy (BDE) of up to 130 kcal/mol. [2] The BDE (strength of the bond) of C–F is higher than other carbon–halogen and carbon–hydrogen bonds.

  8. 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.

  9. Fluorine compounds - Wikipedia

    en.wikipedia.org/wiki/Fluorine_compounds

    The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8] The covalent radius of fluorine of about 71 picometers found in F 2 molecules is significantly larger than that in other compounds because of this weak ...