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.
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| acetylene | cyanogen | carbon monoxide |
| Chemical compounds with triple bonds |
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 pz-orbitals approach and together they form a pz-pz pi-bond. Likewise, the two py-orbitals form a py-py 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].
References
- ^ March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (3rd ed.), New York: Wiley, ISBN 0-471-85472-7
- ^ Organic Chemistry 2nd Ed. John McMurry
- ^ Advanced Organic Chemistry Carey, Francis A., Sundberg, Richard J. 5th ed. 2007
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