Geometric shapes of orbitals

In particular, electron transfer results in that phosphoric acid molecules present in ATP, NADP and NADPN contain oxygen atoms in the form of O". Spatial-energy interactions (including isomorphic) are objectively expressed both at similar and opposite electrostatic charge of atoms-components. Such interactions can also take place between two heterogeneous atoms, if only their PE-parameters are roughly equal, and geometric shapes of orbitals are similar or alike. 

Hybridization occurs during the formation of a chemical bond. It is not possible to occur in an individual atom. Hybrid orbitals play an important role in determining the geometric shape of a molecule. 

Qualitatively the isomorphism character is defined by geometrical similarity of orbital shapes responsible for isomorphism. At the same time, the more similar are the extensions, trajectories and inclination angles of such orbitals, the more perfect is isomorphism. 

Such approximate equality of PE-parameters and geometric similarity of shapes of orbitals of atoms-components shows that actual degree of their interaction p= ()() %, thus... 

I Systems mainly isomorphous to each other - the systems with almost the same number of heterogeneous atoms and summarily similar geometric shapes of interacting orbitals. 

Ill Systems without isomorphous similarity - the systems that considerably differ both in number of dissimilar atoms and geometric shape of their orbitals. 

All the elements of a group A family have the same number of bonds when a molecule is formed. In addition, these bonds all originate in the same orbitals. In Chapter 6 we learned the names of the orbitals where the outermost electrons reside. These orbitals are the places where bonds form with other atoms. The shape and orientation of these orbitals determine the geometric shape of resulting molecules when a group A atom bonds with other atoms. Before this information is summarized, it is necessary to consider how some orbitals combine to form hybrid orbitals when bonds are formed. 

Hybrid orbitals are derived by mixing atomic wave functions. They are used to explain the geometrical shapes of molecules. Hybridization provides several advantages for bonding. With the larger lobe of the hybrid... 

Multiple Covalent Bonds— End-to-end overlap of orbitals produces a (sigma) bonds. Side-to-side overlap of two p orbitals produces a tt (pi) bond. Single covalent bonds are double bond consists of one o- bond and one 77 bond (Fig. 11-15). A triple bond consists of one a-bond and two v bonds (Fig. 11-17). The geometric shape of a species determines the o--bond framework, and tt bonds are added as required to complete the bonding description. 

An important aspect of a molecule in addition to its geometrical shape and the energies of its orbitals is the distri-... 

Fig. 5.6 Changes in the shape of the valence contribution due to geometric and electronic relaxation in [FeF4]" . Full line [FeF4] at its equilibrium geometry, dashed line [FeF4] at its equilibrium geometry. The square of the valence orbital that mainly contributes to p(0) along the Fe-F bond (distances are in units of the Bohr radius) is also drawn (from [19])...

The electron pairs point toward the corners of which geometrical shape for a molecule with sp2 hybrid orbitals ... 

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