Atomic orbitals hybridization and

All single bonds are sigma bonds. Many kinds of pure atomic orbitals and hybridized orbitals can be involved in sigma bond formation. 

Atoms that are linked by electron-pair bonds are positioned so that orbital overlap is maximised. The orbitals used are also sensitive to bond overlap and hybridisation, so that atomic orbitals frequently mix to give hybrid orbitals with greater overlapping power. The shapes of atomic orbitals and hybrid orbitals are quite definite and point in fixed directions. This leads to the fact that covalent bonding is directional. From a geometrical point of view, the array of covalent bonds in a solid resembles a net. 

Nakiboglu, C. (2003). Instructional misconceptions of Turkish prospective chemistry teachers about atomic orbitals and hybridization. Chemistry Education Research and Practice, 4(2), 171-188. 

In the manner of Figure 11-18, indicate the structures of the following molecules in terms of the overlap of simple atomic orbitals and hybrid orbitals (a) CH2CI2 ... 

Butadiene The ti molecular orbitals of 1 3 butadiene are shown m Figure 10 10 The four sp hybridized carbons contribute four 2p atomic orbitals and their overlap... 

A pair of sp hybrid orbitais forms by interacting an s atomic orbital and one p atomic orbital. The two hybrids point in opposite directions. 

The Lewis structure shows that methyl methaciylate has the formula C5 Hg O2, with 40 valence electrons. You should be able to verily that the two CH3 groups have. s -hybridized carbons, the inner oxygen atom is s hybridized, the outer oxygen atom uses 2 p atomic orbitals, and the three double-bonded carbons are s p hybridized. These assignments lead to the following inventory of a bonds and inner-atom lone pairs ... 

The introduction of hybrid-based MO s into the theoretical treatment of paraffinic hydrocarbons 50> has made it possible to extend the applicability of Eqs. (3.21) and (3.24) to a wide variety of saturated compounds. The index has been called delocalizability" of an atomic orbital and is defined by the following formulae 60 68> ... 

A carbon atom combining with four other atoms clearly does not use the one 2s and the three 2p atomic orbitals that would now be available, for this would lead to the formation of three directed bonds, mutually at right angles (with the three 2p orbitals), and one different, non-directed bond (with the spherical 2s orbital). Whereas in fact, the four C—H bonds in, for example, methane are known to be identical and symmetrically (tetrahedrally) disposed at an angle of 109° 28 to each other. This may be accounted for on the basis of redeploying the 2s and the three 2p atomic orbitals so as to yield four new (identical) orbitals, which are capable of forming stronger bonds (cf. p. 5). These new orbitals are known as sp3 hybrid atomic orbitals, and the process by which they are obtained as hybridisation ... 

Figure 3.7. Common representations of the s, p, d and atomic orbitals, sp3 hybridized orbitals, and some representations of how they overlap to form bonds between atoms.

STRATEGY Draw the Lewis structure and determine the electron arrangement about the central atom. The number of orbitals required for the electron arrangement determines the hybridization scheme used, as shown in Table 3.2. Construct the hybrid orbitals from atomic orbitals, using the same number of atomic orbitals as hybrid orbitals. Start with the s-orbital, then add p- and d-orbitals as needed. 

Another type of orbital is one that originates from the mixing of the different atomic orbitals and is called a hybrid orbital. Hybridization (mixing) of atomic orbitals results in a new set of orbitals with different... 

There is no way to predict off-hand the angles between a set of hybrid orbitals without elaborate mathematical calculations, so the geometry of the orbitals is a matter that the be-gihner simply has to remember. The important distinction between simple atomic and hybrid orbitals lies in the fact that hybrid orbitals are much more concentrated into one direction in space than are atomic orbitals, and they have a different geometrical relation to one another. Table 4.7 lists various hybrid orbitals and their general geometries. The numbers listed in the table under overlap strength provide a measure of the relative concentration of the orbitals into one direction. 

In a familiar example, a 2s orbital can be mixed with three 2p orbitals to give four hybrid orbitals this can be done in an infinite number of ways, such as (from now on (j> will be used for atomic orbitals and ij/ for molecular orbitals) ... 

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