Molecular orbitals a bond

As two atoms X and Y form a molecule XY, the atom-atom interaction splits each atomic frontier orbital into two molecular orbitals a bonding molecular orbital at a low energy level and an antibonding molecular orbital at a high eneigy level as shown in Fig. 2-2. Similarly, a molecule composed of many atoms... 

Figure 1.7 Combination of two p orbitals to give

Quantum mechanics shows that linear combination of two functions gives, not one, but two combinations and hence two molecular orbitals a bonding orbital, more stable than the component atomic orbitals and an antibonding orbital, less stable than the component orbitals. 

In this ion, the single pair of electrons occupies the lowest-energy molecular orbital, a bonding orbital distributed over all three atoms. This implies a bond... 

Figure 2.7 The close approach of two hydrogen atoms, each with an electron in a Is orbital, leads to the formation of two molecular orbitals, a bonding iris molecular orbital and an antibonding (J 1s orbital. In the H2 molecule, both electrons occupy the bonding orbital, and a strong bond with energy liibond results...

Electron density in a molecular orbital. A bonding molecular orbital places a large amount of electron density in the bonding region, the space between the two nuclei. 

According to MO theory, the overlap of the li orbitals of two hydrogen atoms leads to the formation of two molecular orbitals one bonding molecular orbital and one antibonding molecular orbital. A bonding molecular orbital has lower... 

The overlap of 2j- with Ita and Itt is shown in Fig. 7-3. The combination (ij-a IJi), which was used in the Og orbitals, is correct for 2s. This means that molecular orbitals—a bonding orbital, an orbital that is nearly nenbonding, and an antibonding orbital. We shall call these orbitals o-/, ox, and Ox, respectively. 

The unequal sizes of the 2p atomic orbitals from which the n MOs are made to show the degree to which they contribute to the molecular orbital. A bonding interaction results from constructive overlap of 2p orbitals of the same sign. Nodal planes are shown between carbon atoms as vertical lines this is where destructive overlap occurs. The energy of the orbitals increases as the number of nodal planes increases. The sign of the orbital inverts going from one side of a nodal plane to the other. Note that is the highest occupied MO (HOMO) and that Ti is the lowest unoccupied MO (LUMO). 

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