A bonding molecular orbital

Antibonding Molecular Orbital. A Molecular Orbital that is andbonding between particular atomic centers. The opposite is a Bonding Molecular Orbital. 

To get the molecular orbital of the hydrogen molecule, the orbital equations of the two atoms are combined. When the orbital equations are added together, the result is a bonding molecular orbital that extends over both atoms. Subtracting the orbital equations of the atoms produces an antibonding molecular orbital. This process is called the linear combination of atomic orbitals or LCAO. 

Compared to an H atom, electrons with the function y/, are less energetic, and those with the function y/2 are more energetic. When the two available electrons occupy the molecular orbital y/(, this is energetically favorable y/, is the wave function of a bonding molecular orbital. y/2 belongs to an antibonding molecular orbital its occupation by electrons requires the input of energy. 

Figure 1.8 The overlapping of two hydrogen Is atomic orbitals with the same phase sign (indicated by their identical color) to form a bonding molecular orbital.

A simple interpretation of the nature of a covalent bond can be seen by considering some simple adaptations of the wave function. For example, it is ifi1 that is related to probability of finding the electrons. When we write the wave function for a bonding molecular orbital as ipb, that means that because... 

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... 

As we have already seen, two molecular orbitals form when two atomic orbitals overlap - a bonding molecular orbital and an antibonding molecular orbital. End-on overlap of atomic orbitals along the axis of the bond results In cr and cr molecular orbitals forming. Slde-on overlap of atomic orbitals at an angle perpendicular to the axis of the bond results In the formation of n and molecular orbitals. 

Now we can consider the bonding in methane. Using orbital overlap as in the hydrogen molecule as a model, each sp orbital of carbon can now overlap with a 1 orbital of a hydrogen atom, generating a bonding molecular orbital, i.e. a ct bond. Four such... 

A covalent bond occurs when two atoms share two or more electrons. More specifically, in the context of molecular orbital theory, a single covalent bond between two atoms occurs when two electrons (one from each of the atoms) occupies a bonding molecular orbital. Other terms... 

The molecular orbital theory of the dihydrogen molecule is dealt with in detail above, and describes how the two electrons occupy a bonding molecular orbital so that they are equally shared between the two nuclei. This state of affairs can be written symbolically in the form ... 

What property of a bonding molecular orbital is mainly responsible for its bonding properties ... 

The one-electron molecular orbitals thus formed consist of a bonding molecular orbital (d ft) and an aniibontSng molecular orbital ( ). If we allow a single electron to occupy the bonding molecular orbital (as in H. for example), the approximate wave function for the molecule is... 

The transition metal ions possess a very stable set of d orbitals, and it is likely that d orbitals are involved in bonding in all transition metal complexes, regardless of structure. The common structures that use d valence orbitals for forming a bonding molecular orbitals are square-planar, tetrahedral, and octahedral. Examples of these structures are given in Figure 8-1. 

The energy of a bonding molecular orbital is lower than the combining atomic orbitals. It favours formation of a bond. 

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