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** Hybridization of 5 and p Orbitals **

FIGURE 11. Combination of p orbitals on the same center resulting in rotation combination of s and p orbitals on the same center resulting in a hybrid orbital. [Pg.13]

Figure 5.3 Hybrid orbitals result from combinations of s and p orbitals. |

Fig. 4. Molecular orbitals showing the hybridization of s and p orbitals, (a) Acetylene (C2H2, sp hybridization) (b) ethylene (C2H4, sp hybridization), and (c) methane (CH4, sp hybridization). |

The bonds are considered to arise from the combination of two boron orbitals that are hybrids of s and p orbitals with a b orbital on the hydrogen atom. Graphically, the formation of the three-center molecular orbital can be represented as shown here [Pg.196]

Hybrid orbitals may be considered as perfectioned AOs, adopted in the calculation of localized MOs in polyatomic molecules, with the LCAO method (cf. section 1.17.1). In the case of hybrid orbitals sp, the four linear combinations of s and p orbitals (Tbi, Tc2, Te, Te ) that lead to tetrahedral symmetry are [Pg.217]

When 100 mL of blue dye is mixed with 100 mL of yellow dye 200 mL of green dye is formed. At the same way, when s and p orbitals are mixed (hybridized), hybrid orbitals which have both the characteristics of s and p orbitals are formed. [Pg.21]

Atoms in the second row (such as C, N, 0, and F) have one s orbital and three p orbitals in the valence shell. These orbitals are usually mixed together to give us hybridized orbitals (sp3, sp2, and sp). We get these orbitals by mixing the properties of s and p orbitals. What do we mean by mixing [Pg.77]

For molecules with different structures different hybridization functions are appropriate. An infinity of hybridization functions can be formulated by linear combinations of s and p orbitals [Pg.88]

Mathematically, the formation of sp or tetrahedral orbitals for methane is more complicated but not basically different. The results are four equivalent hybrid orbitals, each containing one part s to three parts p in each wave function, directed to the corners of a tetrahedron. As in the case of sp hybrids, the hybridization of s and p has [Pg.611]

The relationship between p or s character and bond angle will also be discussed in Chapter 6. For now we need only consider the possibility of s-p hybridization other than sp, sp, and sp. If we take the ratio of the s contribution to the total orbital complement in these hybrids, we obtain 50%, 33%, and 25% s character, respectively, for these hybrids. A pure s orbital would be 100% s, and a p orbital would have 0% s character. Since hybrid orbitals are constructed as linear combinations of s and p orbital wave functions, [Pg.88]

** Hybridization of 5 and p Orbitals **

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