A triple bond in chemistry is a chemical bond between two chemical elements involving six bonding electrons instead of the usual two in a covalent single bond. The most common triple bond, that between two carbon atoms, can be found in alkynes. Other functional groups containing a triple bond are cyanides and isocyanides. Some diatomic molecules, such as dinitrogen and carbon monoxide are also triple bonded. In skeletal formula the triple bond is drawn as three parallel lines between the two connected atoms. ^{[1] [2]}.

Triple bonds are stronger than single bonds or double bonds and they're are also shorter. The bond order is three.

acetylene	cyanogen	carbon monoxide
Chemical compounds with triple bonds

[edit] Bonding

The type of bonding can be explained in terms of orbital hybridization. Each carbon atom has two sp orbitals and two p-orbitals. The two sp orbitals are linear with 180 ° angles and occupy the x-axis (cartesian coordinate system). The p-orbitals are perpendicular on the y-axis and the z-axis. When the carbon atoms approach each other the sp orbitals overlap to form a sp-sp sigma bond. At the same time the two p_z-orbitals approach and together they form a p_z-p_z pi-bond. Likewise, the two p_y-orbitals form a p_y-p_y pi-bond. The result is formation of one sigma bond and two pi bonds.

In bent bond theory the triple bond can also form by overlap of three sp³ lobes without the need to invoke a pi-bond ^[3].

[edit] References

v • d • e Chemical bonds Intramolecular ("strong") Covalent bonds Sigma bond · Pi bond · Delta bond Double bond · Triple bond · Quadruple bond · Quintuple bond · Sextuple bond 3c-2e · 3c-4e · 4c-2e Agostic bond · Bent bond · Dipolar bond · Pi backbond Conjugation · Hyperconjugation · Aromaticity · Hapticity Ionic bonds cation-pi bond · salt bond Metallic bonds Metal aromaticity Intermolecular ("weak") Hydrogen bond Dihydrogen bond · Dihydrogen complex · Low-barrier hydrogen bond · Symmetric hydrogen bond Other noncovalent van der Waals force · London dispersion force · Mechanical bond · Halogen bond · Aurophilicity · Intercalation · Stacking · Entropic force · Chemical polarity Note: the weakest strong bonds are not necessarily stronger than the strongest weak bonds