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  Valence bond theory

Valence bond theory (VB Theory):

Valence bond theory, mainly the work of Linus Pauling considered bonding as characterized by the overlap of atomic or hybrid orbitals of separate atoms.

The postulates of valence bond theory:

1) The central metal atom or ion makes accessible a number of vacant orbitals equivalent to its coordination number.

2) Such vacant orbitals made covalent bonds with the ligand orbitals.

3) The covalent bond is made by the overlap of a vacant metal orbital and filled ligand orbitals. This total overlap leads to the formation of a metal ligand, σ (i.e., sigma) bond.

4) A strong covalent bond is created only whenever the orbitals overlap to the maximum amount. This maximum overlapping is possible only whenever the metal vacant orbitals undergo a procedure termed as ‘hybridisation’. A hybridised orbital contain a better directional characteristics than an unhybridised one.

The table shown below provides the coordination number, orbital hybridisation and the spatial geometry of more significant geometrics.

2255_valemce bond theory.jpg

Magnetic moment:

A species containing at least one unpaired electron is termed to be paramagnetic. It is attracted by an external field. The paramagnetic moment is specified by the following spin-only formula.

µs = √n(n+2) BM

Here,
µs = spin-only magnetic moment
n = number of unpaired electrons
BM = Bohr magneton, the unit that states the magnetic moment. When the species does not have any unpaired electron, then it is diamagnetic.

Number of unpaired electrons           Spin-only moment (BM)

1                                                      √1(1+2) = √3 = 1.73
2                                                      √2(2+2) = √8 = 2.83
3                                                      √3(3+2) = √15 = 3.87
4                                                      √4(4+2) = √24= 4.90
5                                                      √5(5+2) = √35= 5.92

 

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