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Answer :
In coordination chemistry, the geometry of a complex is determined by its coordination number, which is the number of ligand atoms that are bonded to the central metal atom or ion.
For a coordination number of 4, the common geometries are:
Square Planar: This geometry is often found in complexes where the metal has a d^8 electronic configuration, such as in certain platinum and palladium complexes. In a square planar geometry, the four ligands are positioned at the corners of a square, with the metal at the center. This arrangement results in a planar shape.
Tetrahedral: This is another common geometry for a coordination number of 4, where the four ligands are symmetrically distributed at the corners of a tetrahedron around the central metal atom. This geometry is prevalent in many transition metal complexes, such as those of zinc and nickel.
The option "trizonal bipyramidal" is not a recognized standard geometry for coordination number 4 complexes.
For a coordination number of 6, the common geometries are:
- Octahedral: This is the most prevalent geometry for coordination number 6. In an octahedral configuration, the six ligands are symmetrically positioned at the corners of an octahedron surrounding the central metal atom. This structure is typical for many transition metals, like cobalt and iron complexes.
The options "hexagonal planar," "trigonal bipyramidal," and "pentagonal pyramidal" are not typical geometries for coordination number 6 in standard transition metal complexes. Hexagonal planar is rare and usually associated with certain complex ions outside the typical coordination chemistry scenarios, while trigonal bipyramidal and pentagonal pyramidal relate to different coordination situations.
In summary, the common geometry for a coordination number of 4 would include square planar and tetrahedral, and for a coordination number of 6, it would be octahedral.
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