[Co(H2 O)6]^3 complex is (1) High spin complex (2) Having...

$\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3}$ complex is
(1) High spin complex
(2) Having $d^{2} s p^{3}$-hybridization
(3) Low spin complex
(4) Having octahedral structure

Key Concepts

Coordination Complex Geometry

Coordination complexes consist of a central metal ion surrounded by ligands, and the spatial arrangement of these ligands defines the geometry of the complex. An octahedral geometry, where six ligands symmetrically surround the metal ion, is one of the most common geometries in coordination chemistry, significantly influencing the complex’s reactivity and physical properties.

Crystal Field Theory and Spin States

Crystal field theory explains how the presence of ligands splits the degenerate d orbitals of a metal ion into subsets with different energies, ultimately affecting the electron configuration. This splitting determines whether a complex is low spin or high spin: a large splitting, relative to the pairing energy, encourages electrons to pair in the lower energy orbitals (low spin), while a small splitting favors occupying higher energy orbitals (high spin). The determination of spin state is crucial for understanding the magnetic properties and reactivity of the complex.

Hybridization in Coordination Complexes

Hybridization is a model that describes the mixing of atomic orbitals to form new hybrid orbitals that can accommodate bonding with ligands. In the context of octahedral complexes, a classical description involves d²sp³ hybridization, implying that two d orbitals, one s orbital, and three p orbitals combine to form six equivalent hybrid orbitals, facilitating the coordination of six ligands. Although this approach is a simplification compared to molecular orbital theory, it helps in rationalizing the bonding and spatial arrangement in coordination compounds.

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