Triple bond

A covalent bond in which two atoms share three pairs of electrons, giving the bond a bond order of three. It is generally shorter and stronger than a corresponding double or single bond.

Sigma bond: A covalent bond formed by electron density concentrated along the axis between two nuclei. Every triple bond contains one sigma bond along the internuclear axis.
Covalent bond: A chemical bond formed when atoms share electron density. A triple bond is a high bond-order form of covalent bonding.
Alkyne: An unsaturated hydrocarbon containing at least one carbon–carbon triple bond. Alkynes are the principal family of compounds built around carbon–carbon triple bonds.
Single bond: A covalent bond in which two atoms share one electron pair. A single bond has one shared pair, versus three in a triple bond.
Pi bond: A covalent bond formed by sideways overlap of orbitals, with electron density above and below the internuclear axis. The two additional components of a triple bond are pi bonds.
Valence electron: An electron in an atom's outer shell that can participate in chemical bonding. The three shared pairs are made from valence electrons.
Acetylene: The simplest alkyne, with formula C₂H₂ and a carbon–carbon triple bond. Its C≡C bond is the best-known example of a carbon–carbon triple bond.
Double bond: A covalent bond in which two atoms share two electron pairs. A double bond provides the nearest bond-order comparison to a triple bond.
Bond order: A measure of the number of electron-pair bonds between two atoms, often estimated from molecular orbitals. A triple bond has bond order three, distinguishing it from single and double bonds.
Lewis structure: A diagram showing atoms, bonds, and lone electron pairs using symbols and lines or dots. Three lines between atoms provide the standard Lewis representation of a triple bond.

Linked from 3 pages