Answer :

Final answer:

Two-coordinate complexes usually have a linear geometry. However, the geometry can vary with the coordination number and the arrangement of ligands around the central metal ion. Complexes with higher coordination numbers can assume tetrahedral, square planar, or octahedral geometries.

Explanation:

The most common geometry found in two-coordinate complexes, or complexes with a coordination number of two, is a linear geometry. This is the case in complexes such as [Ag(NH3)2]†.

For complexes with higher coordination numbers like four and six, the structures can be tetrahedral or square planar and octahedral respectively. Complexes like [Cu(Cl)4]²- and [Co(H₂O)6]²+ exemplify these geometries.

The specific geometry for transition metal complexes is often determined by the distribution of the d orbitals and the arrangement of ligands around the central metal ion. For example, a square planar complex can be thought of as an octahedral structure with two ligands removed, causing a change in the stability of the d orbitals.

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