The simplest alkyne—a hydrocarbon with carbon-to-carbon triple bond—has the molecular formula C 2 H 2 and is known by its common name—acetylene. Its structure is H–C≡C–H. Terminal Alkyne: Internal Alkyne: 3-chloro-1-propyne 4,4-dichloro-2-pentyne Bonding and Hybridization 0 1 2 3 Bond Name Location Overlap Bond 1 s (? bond) bond Formed between 2 sp orbitals of carbon and hydrogen atoms End-on overlap Bond 2 S (? bond) bond Formed between the 2 sp orbital of 2 unsaturated Carbon atoms. End-on overlap Bond 3 p-bonds (? bonds) Formed between the 2 p-orbitals among the carbon atoms Side-on overlap 0 1 2 Orbital Name Location Orbital 1 sp hybrid orbitals Formed in the linear structure model of carbon atom Orbital 2 p-orbitals Formed on each carbon Contributors Jim Clark ( Chemguide.co.uk ) The characteristic of the triple bond helps to explain the properties and bonding in the alkynes . Importance of Triple Bonds Hybridization due to triple bonds allows the uniqueness of alkyne structure. This triple bond contributes to the nonpolar bonding strength, linear, and the acidity of alkynes . Physical Properties include nonpolar due to slight solubility in polar solvents and insoluble in water. This solubility in water and polar solvents is a characteristic feature to alkenes as well. Alkynes dissolve in organic solvents. Boiling Points Compared to alkanes and alkenes , alkynes have a slightly higher boiling point. Ethane has a boiling point of -88.6 ?C, while Ethene is -103.7 ?C and Ethyne has a higher boiling point of -84.0 ?C. Alkynes are High In Energy Alkynes are involved in a high release of energy because of repulsion of electrons. The content of energy involved in the alkyne molecule contributes to this high amount of energy. The pi-bonds however, do not encompass a great amount of energy even though the concentration is small within the molecule. The combustion of Ethyne is a major contributor from CO 2 , water, and the ethyne molecule ? ? H = -311 kcal/ mol To help understand the relative stabilities of alkyne isomers, heats of hydrogenation must be used. Hydrogenation of the least energy, results in the release of the internal alkyne . With the result of the production of butane, the stability of internal versus terminal alkynes has significant relative stability due to hyperconjugation. Outside links http://www.ucc.ie/academic/chem/dolc...t/alkynes.html http://www.cliffsnotes.com/WileyCDA/...eId-22631.html References Bloch, D.R. Organic chemistry demystified, New York : McGraw-Hill, 2006. Vollhardt. Schore, Organic Chemistry Structure and Function Fifth Edition, New York: W.H. Freeman and Company, 2007. Problems What is the carbon-carbon, carbon-hydrogen bond length for alkyne ? Is it shorter or longer than alkane and alkene? Which is the most acidic and most stable, alkane, alkene, or alkyne ? And depends on what? How many pi bonds and sigma bonds are involved in the structure of ethyne ? Why is the carbon-hydrogen bond so short? What is the alkyne triple bond characterizes by? How is this contribute to the weakness of the pi bonds? How is heat of hydrogenation effects the stability of the alkyne ? Contributors Bao Kha Nguyen, Garrett M. Chin