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Sp hybrid orbitals in alkynes

Alkynes are unsaturated hydrocarbons containing at least one triple carbon-carbon bond. The simplest alkyne is C2H2 (commonly called acetylene), which has the systematic name ethyne. As discussed in Section 14.1, the triple bond in acetylene can be described as one cr bond between two sp hybrid orbitals on the two carbon atoms and two v bonds involving two 2p orbitals on each carbon atom (Fig. 22.10). [Pg.1022]

In CH4, the electron density of the four sp orbitals of C each overlap with an s orbital of H to form four o bonds. In C2H4 (an alkene), two sp orbitals on each C overlap with H s orbitals, the remaining sp orbitals overlap with each other in a CT bond, and the p orbitals (drawn as shaded shapes) overlap with each other above and beneath the carbon atoms in a tt bond (also drawn as shaded shapes). In CO2. the C atom has two sp hybrid orbitals and two p orbitals. These form one ct bond and one tt bond with the two unfilled p orbitals on each 0 atom. In C2H2 (an alkyne), a triple bond forms with one crand two tt bonds. [Pg.208]

The greater character of sp hybrid orbitals compared with sp and sp gives alkynes certain properties beyond those seen in alkanes and alkenes. It is convenient to think of. yp-hybridized carbon as more electronegative than its sp or sp counterparts. [Pg.386]

Acetylene is linear and alkynes have a linear geometry of their X—C=C—Y units. The carbon-carbon triple bond in alkynes is composed of a ct and two it components. The triply bonded carbons are sp-hybridized. The cr component of the triple bond contains two electrons in an orbital generated by the overlap of s/>hybridized orbitals on adjacent carbons. Each of these carbons also has two 2p orbitals, which overlap in pairs so as to give two it orbitals, each of which contains two electrons. [Pg.389]

Most of the metal complexes of alkynes discussed so far are stabilized by proximity of an sp hybrid orbital on the alkyne carbon the alternative approach to metal complex formation is donation of the triple-bond electrons to the vacant orbitals of a metal. This yields a vast range of complexes, many of which are stable and can be used in synthesis, but is some cases the alkyne can undergo rearrangements which are not observed in the free organic species. [Pg.495]

Arynes present structural features of some interest. They clearly cannot be acetylenic in the usual sense as this would require enormous deformation of the benzene ring in order to accommodate the 180 bond angle required by the sp hybridised carbons in an alkyne (p. 9). It seems more likely that the delocalised n orbitals of the aromatic system are left largely untouched (aromatic stability thereby being conserved), and that the two available electrons are accommodated in the original sp hybrid orbitals (101)  [Pg.175]

The sp hybrid orbital has 50% s character, which is greater than the 33% and 25% s characters of the sp hybrid orbitals of alkenes and the sp and hybrid orbitals of alkanes. We recall that as the percent s character of hybrid orbitals increases the electrons in the hybrid orbitals are closer to the nucleus. Therefore, the bonding electrons in an sp hybrid orbital of a C—H bond in ethyne are closer to the nucleus than the electrons in the hybrid orbital of the C—H bonds of ethylene or ethane. The greater s character of the sigma bonds of acetylene and alkynes affects their physical properties. [Pg.224]


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See also in sourсe #XX -- [ Pg.401 ]

See also in sourсe #XX -- [ Pg.400 , Pg.401 , Pg.405 ]




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