Final answer:
A triple bond consists of one sigma bond and two pi bonds, formed by the end-to-end and side-by-side overlap of orbitals. Pi bonds create regions of electron density above and below the nuclei's plane. Triple bonds exhibit linear geometry and are stronger than single and double bonds.
Step-by-step explanation:
A triple bond is formed when atoms share three pairs of electrons between them. The first pair of electrons forms a sigma bond (σ bond) through end-to-end overlap along the internuclear axis, with electron density concentrated between the nuclei. The remaining two pairs each form a pi bond (π bond) through the side-by-side overlap of two p orbitals, as illustrated in figures such as 8.5 and 5.5, creating regions of electron density above and below the plane of the nuclei with a node, or area of zero electron density, along the internuclear axis. Triple bonds are found in molecules such as carbon monoxide (CO), the cyanide ion (CN), and hydrocarbons like ethyne (acetylene).
The two pi bonds that characterize the triple bond result in a bond order of three, which makes a triple bond stronger than a double bond, which in turn is stronger than a single bond. However, unlike single and double bonds, a triple bond has a linear geometry and the rotation around this bond is less significant as compared to a double bond.