explain hybridisation of complexes in detail by MOT[ Cu(NH3)4]++, [V(H2O)6]+++,[Ti(H2O)6]+++ ,

Dear student,

In Molecular Orbital Theory, the orbitals in a molecule arise from the overlap of atomic orbitals that satisfy two criteria:

• The orbitals have compatible symmetry
• The orbitals are similar in energy

The interactions of the atomic orbitals to form molecular orbitals is represented by an energy diagram called a molecular orbital diagram. The diagram displays the orbitals arranged vertically from lowest to highest energy. The atomic orbitals for the various atoms are listed in columns at the left and right sides of the diagram. The molecular orbitals are listed in a column down the center of the diagram.

The atomic orbitals are given the usual s, p_x, etc. designation. The molecular orbitals, which are often identified by their symmetry properties, may also be identified by their bonding properties: σ, σ*, π, π*, or n.

The shape of [ Cu(NH3)4]++  is tetrahedral as NH3 is a weak field ligand...so the hybridastion is sp3

d¹ = [Ti(H₂O)₆]³⁺

d² = [V(H₂O)₆]³⁺

ligand-to-metal charge transfer is prevented to go into those metal orbitals that contain unpaired d electrons. A lowering of the complex symmetry is observed and coupled with the following variations: The Ti³⁺− and V³⁺−hexaaqua ions switch from T_h to C_i symmetry.

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Sagar Singh

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