![]() Multiple pairs represent multiple bonds, such as double bonds and triple bonds. Pairs of electrons located between atoms represent covalent bonds. He introduced the Lewis notation or electron dot notation or Lewis dot structure, in which valence electrons (those in the outer shell) are represented as dots around the atomic symbols. Lewis, who in 1916 described the sharing of electron pairs between atoms (and in 1926 he also coined the term "photon" for the smallest unit of radiant energy). The idea of covalent bonding can be traced several years before 1919 to Gilbert N. Langmuir wrote that "we shall denote by the term covalence the number of pairs of electrons that a given atom shares with its neighbors." The term covalence in regard to bonding was first used in 1919 by Irving Langmuir in a Journal of the American Chemical Society article entitled "The Arrangement of Electrons in Atoms and Molecules". Covalent bonding is implied in the Lewis structure by indicating electrons shared between atoms. ![]() History Early concepts in covalent bonding arose from this kind of image of the molecule of methane. Covalent bonding that entails the sharing of electrons over more than two atoms is said to be delocalized. Thus, covalent bonding does not necessarily require that the two atoms be of the same elements, only that they be of comparable electronegativity. Covalency is greatest between atoms of similar electronegativities. thus a "co-valent bond", in essence, means that the atoms share " valence", such as is discussed in valence bond theory.Ģ, the hydrogen atoms share the two electrons via covalent bonding. The prefix co- means jointly, associated in action, partnered to a lesser degree, etc. In organic chemistry, covalent bonding is much more common than ionic bonding.Ĭovalent bonding also includes many kinds of interactions, including σ-bonding, π-bonding, metal-to-metal bonding, agostic interactions, bent bonds, three-center two-electron bonds and three-center four-electron bonds. For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding. These electron pairs are known as shared pairs or bonding pairs. A covalent bond forming H 2 (right) where two hydrogen atoms share the two electronsĪ covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. For other uses, see Covalent (disambiguation).
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