Carbon sp hybrid orbitals

The vinyl H2C=CH radical can be produced by cleavage of a C-H bond in ethene, and has been studied in the gas phase. The unpaired electron clearly occupies a carbon sp hybrid orbital, to lapse into the language of descriptive organic chemistry, but there are regions of space where the, 6-spin electrons have... 

This information may be interpreted in terms of the unpaired electron being confined to a carbon sp hybrid orbital (4ai) built up by carbon 2s and 2p and oxygen 2p atomic orbitals. The 2pj character of the 4ai molecular orbital can be estimated by comparison with the integral ... 

Figure 1.12 The structure of ethane. The carbon-carbon bond is formed by a overlap of two carbon sp hybrid orbitals. For clarity, the smaller lobes of the sp hybrid orbitals are not shown.

Carbon-carbon single bonds in alkanes are formed by hybrid orbitals. Rotation is possible around a bcaid.s because of their cylindrical... 

There are now eight different spatial orbitals, hybrid orbitals, the other four being close to atomic hydrogen s-orbitals. The expansion of each of the VB orbitals in terras of M the basis functions located on the nuclei allows the orbitals to distort from the pure atomic shape. The SCVB wave... 

Fig. 8.5 Carbon sp hybrid orbitals (with their axes defining angles of 109° 27 ) appropriate to the v.b. description of the four equivalent CH bonds of CH4.

FIGURE 10.7 Formation of four bonds between the carbon sp hybrid orbitals and the hydrogen Is orbitals in CH4. 

Carbon dioxide, (a) Overlap of carbon sp hybrid orbitals with oxygen 2px orbitals to give a bonds O—C—O. (b) The two tt molecular orbitals of the molecule formed from unused 2py and 2pz orbitals. 

If we consider the carbon atom to be sp hybridised from 2s+2px orbitals, then we could have a linear O—C—O framework containing a bonds, by overlap of the two carbon sp hybrid orbitals with the two oxygen 2px orbitals. This is illustrated in Figure 20a. 

Figure 2.6 The overlap of carbon sp hybrid orbitals in the xy plane of the butadiene molecule...

Figure 1.11 shows the contours of one of the sp orbitals as well as those of carbon 2s, 2p, sp, and sp hybrids. Each of the sp orbitals in equations 1.35-1.38 has a large lobe and a small lobe. The two lobes have a different mathematical sign, and the four large lobes point toward the comers of a regular tetrahedron. Now we can describe methane as CH4 by combining each of the four carbon sp hybrid orbitals with a Is orbital on hydrogen. A qualitative energy diagram for the process is shown in Figure 1.12. The four...

The indicated bond in 1,3-butadiene is formed by the overlap of two sp -hybridized carbons, while the indicated bond in 1-butene is formed by the overlap of one sp -hybridized and one sp -hybridized carbon. sp -Hybridized orbitals are smaller because they have greater s character (an s orbital holds its electrons closer to the nucleus of an atom), so the bond made from two sp hybrids is shorter. 

These four hybrid orbitals are directed toward the four comers of a regular tetrahedron. Figure 4.11 shows the formation of four covalent bonds between the carbon sp hybrid orbitals and the hydrogen 1 orbitals in CH4. 

Covalent bond formation in ethylene (CHjCHj). (a) Lewis structure, (b) Overlap oisp hybrid orbitals on adjacent carbons forms a C—C cr bond (see Figure 1.18), and overlap of carbon sp hybrid orbitals on carbons with 1 orbitals on hydrogens gives C—H [Pg.73]

Because of the radical-stabilizing influence of this electron delocalization, it is reasonable to expect that the BDE of an allylic C—H is significantly weaker than that of a primary C—H. In fact, based on bond dissociation enthalpies, we conclude that an allyl radical is even more stable than a 3° alkyl radical. Note that because of the larger amount of s character in its carbon sp hybrid orbital, a vinylic C—H bond is stronger (has a larger bond dissociation enthalpy) than any sp C—bond and is never abstracted in homolytic reactions. 

The wavefunctions of the carbon sp hybrid orbitals which are directed along the... 

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