Orbitals p orbital

A n bond is formed from the side by side overlap of unhybridized p orbitals, p orbital + p orbital => 1 n bond (2 separate electron clouds)... 

Sigma (o) bonds are formed by the end to end overlap of two orbitals. This overlap can take place between s orbitals, p orbitals or hybrid orbitals. 

Work through the Molecular Orbital Theory tutorial in eChapter 7.13, which illustrates the formation of sigma molecular orbitals from s atomic orbitals, p Orbitals will also form sigma orbitals when they overlap head-on. Follow the examples given for the s orbitals and predict how p orbitals will form sigma molecular orbitals. 

The last ratio is independent of the parameters, a and 3 and may regarded as a purely group theoretical (kinematic) result. The same result is obtained dynamically without group theory through the Slater-Condon parameters which are integrals of e2/rjj over analytic hydrogenic orbitals. The chain has been interpreted as the sum of a p orbital-p orbital and a spin orbital-spin orbital magnetic dipole interaction. This inteipretation is clearly nonphysical. 

Figure 1.2. Atomic orbitals p orbitals. Axes mutually perpendicular. (a) Cross-section showing the two lobes of a single orbital, (b) Approximate shape as pairs of distorted ellipsoids, (c) Representation as pairs of not-quite-touching spheres.

The boundary surface diagrams of p orbitals in Figure 7.19 show that each p orbital can be thought of as two lobes on opposite sides of the nucleus. Like s orbitals, p orbitals increase in size from 2p to 3p to 4p orbital and so on. 

Beginning with the = 2 shell, each shell has three p orbitals. Recall that the / quantum number for p orbitals is 1. Therefore, the magnetic quantum number ntj can have three possible values —1,0, and +1. Thus, there are three 2p orbitals, three 3p orbitals, and so forth, corresponding to the three possible values of ntj. Each set of p orbitals has the dumbbell shapes shown in Figure 6.22(a) for the 2p orbitals. For each value of n, the three p orbitals have the same size and shape but differ from one another in spatial orientation. We usually represent p orbitals by drawing the shape and orientation of their wave functions, as shown in Figure 6.22(b). It is convenient to label these as the p py, and p orbitals. The letter subscript indicates the Cartesian axis along which the orbital is oriented. Like s orbitals, p orbitals increase in size as we move from 2p to 3p to 4p, and so forth. 

Hybridized Atomic Orbitals p Orbitals Not Hybridized Hybridization Electronic Geometry... 

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