Double bond

A covalent bond in which two atoms share two pairs of electrons. It is stronger and shorter than a comparable single bond and restricts rotation between the bonded atoms.

Sigma bond: A covalent bond formed by electron density concentrated along the axis between two nuclei. The first electron pair in a typical double bond forms this shared axial bond.
Covalent bond: A chemical bond formed when atoms share one or more pairs of electrons. A double bond is one form of covalent bonding, distinguished by sharing two electron pairs.
Alkene: An unsaturated hydrocarbon containing at least one carbon–carbon double bond. Alkenes are the most familiar family of compounds defined by a double bond.
Single bond: A covalent bond in which two atoms share one pair of electrons. It has one shared pair, unlike the two pairs in a double bond.
Pi bond: A covalent bond formed by sideways overlap of orbitals, with electron density above and below the internuclear axis. The second electron pair in a typical double bond forms this bond.
Valence electron: An electron in an atom's outer shell that can participate in chemical bonding. The shared pairs in a double bond come from the atoms' valence electrons.
Ethenes: The simplest alkene, with two carbon atoms joined by a double bond and each bonded to two hydrogens. Ethene is the simplest molecule in which a carbon–carbon double bond appears.
Triple bond: A covalent bond in which two atoms share three pairs of electrons. It adds a second pi bond, making it generally shorter and stronger than a double bond.
Molecular orbital theory: A model of bonding in which electrons occupy orbitals extending across an entire molecule. It explains double bonds as occupied bonding orbitals rather than localized electron pairs.
Atomic orbital: A mathematical description of an electron's possible spatial distribution in an atom. Overlapping atomic orbitals provide the quantum-mechanical basis for double-bond formation.

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