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Valence bond theory in coordination compound class 12
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Key Points of VBT in Coordination Compounds:
Metal-Ligand Bonding: According to VBT, the bond between the metal and the ligands in a coordination compound is formed through the overlap of the valence orbitals of the metal with orbitals of the ligands that contain lone pairs of electrons.

Hybridization: The theory suggests that the metal's central atom undergoes hybridization of its orbitals to accommodate the ligands. This determines the geometry of the complex. For example:


Co(NH 3) 6
​: The cobalt ion is in a +3 oxidation state, and it undergoes d²sp³ hybridization (which involves two d-orbitals, one s-orbital, and three p-orbitals), leading to an octahedral geometry.

Ni(CO) 4: Nickel undergoes sp³ hybridization, resulting in a tetrahedral geometry.
Types of Bonds:

σ-bond (sigma bond): The primary bond formed between the metal and the ligand. It results from the head-on overlap of orbitals.
π-bond (pi bond): In some cases, π-back bonding occurs when ligands with empty π* orbitals (e.g., CO) interact with d-orbitals of the metal, forming a π bond.
Magnetic and Spectral Properties: VBT can also predict whether a coordination compound is paramagnetic or diamagnetic based on the arrangement of electrons in the hybridized orbitals. For example, if all electrons are paired, the compound is diamagnetic; otherwise, it's paramagnetic.

Limitations of VBT:
1.Although VBT is useful, it has limitations, such as:

2.It does not explain the color of coordination compounds well.
3.It does not give a quantitative explanation of the stability of complexes.
4.It doesn't account for the spectrochemical series or differentiate between weak and strong field ligands effectively.

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