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As a general rule, covalent bonds are formed between elements lying toward the right in the periodic table (i.e., the nonmetals). When none of the elements in a compound is a metal, no atoms in the compound have an ionization energy low enough for electron loss to be likely. This partial ionic character of covalent bonds increases with the difference in the electronegativities of the two atoms. Covalent bonds between identical atoms (as in H 2) are nonpolar-i.e., electrically uniform-while those between unlike atoms are polar-i.e., one atom is slightly negatively charged and the other is slightly positively charged. Single bonds consist of one sigma (σ) bond, double bonds have one σ and one pi (π) bond, and triple bonds have one σ and two π bonds.Ĭovalent bonds are directional, meaning that atoms so bonded prefer specific orientations relative to one another this in turn gives molecules definite shapes, as in the angular (bent) structure of the H 2O molecule. In structural representations of molecules, covalent bonds are indicated by solid lines connecting pairs of atoms e.g.,Ī single line indicates a bond between two atoms (i.e., involving one electron pair), double lines (=) indicate a double bond between two atoms (i.e., involving two electron pairs), and triple lines (≡) represent a triple bond, as found, for example, in carbon monoxide (C≡O). Molecules that have covalent linkages include the inorganic substances hydrogen, nitrogen, chlorine, water, and ammonia (H 2, N 2, Cl 2, H 2O, NH 3) together with all organic compounds.
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For full treatment, see chemical bonding: Covalent bonds. A covalent bond forms when the bonded atoms have a lower total energy than that of widely separated atoms.Ī brief treatment of covalent bonds follows. The binding arises from the electrostatic attraction of their nuclei for the same electrons.
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