Pi bond

A pi bond is a covalent bond formed by sideways overlap of orbitals, with electron density concentrated above and below the internuclear axis. It commonly accompanies a sigma bond in double and triple bonds.

Atomic orbital: A region of space described by a wavefunction in which an electron in an atom is likely to be found. Pi bonding depends on the shapes and orientations of orbitals.
Sigma bond: A covalent bond formed by orbital overlap along the internuclear axis. A pi bond usually supplements a sigma bond between the same atoms.
Ethene: A two-carbon alkene with one carbon–carbon double bond and molecular formula C₂H₄. Its carbon–carbon double bond contains one pi bond and one sigma bond.
Localized electron model: A chemical bonding description that assigns electron pairs to particular bonds or lone-pair regions. It contrasts with molecular-orbital accounts that spread pi electrons over several atoms.
p orbital: A dumbbell-shaped atomic orbital with two lobes on opposite sides of the nucleus. Sideways overlap of aligned p orbitals forms the familiar pi bond.
Covalent bond: A chemical bond in which atoms share electron density. Pi bonds are one type of covalent bond.
Alkyne: A hydrocarbon containing at least one carbon–carbon triple bond. A triple bond contains two pi bonds alongside one sigma bond.
Ionic bond: An electrostatic attraction between oppositely charged ions. Unlike ionic bonding, a pi bond involves shared electron density between atoms.
Molecular orbital: A wavefunction describing electrons across a molecule rather than around one atom. Pi bonding is described by molecular orbitals spread across bonded atoms.
Bond order: A measure of the number of bonding electron pairs between two atoms. Pi bonds contribute to the higher bond order of multiple bonds.

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