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Using valence bond theory account for the geometry and magnetic nature of [NiCl_(4)]^(2-) ion. ("Atomic number of Ni "= 28). |
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Answer» Solution :In the given complex ion central METAL is nickel with electronic configuration `[Ar]^(18)3d^(8)4s^(2)` Nickel is in `+2` oxidation state THEREFORE electronic configurations is `Ni^(+2)`  In the given complex, `CN-` is a strong ligand. On the APPROACH of strong ligand the unpaired 3d electron will get pair up. As a result one d - orbital BECOMES vacant.  The one vacant 3d orbital, one vacant 4s orbital and two vacant 4p orbitals hybridize to give four hybrid orbitals.  Four pairs of electrons one from each `CN-` molecule occupy the geometry is square planar it is diamagnetic complex due to the absence of unpaired electrons. 
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