Crystal Field Theory and Octahedral Complexes

The attraction between metal ions and electron pairs in ligands arises from the overlap of metal orbitals and ligand orbitals.

In an octahedral complex, the 3d orbitals split into two sets: a higher energy set (e_g) and a lower energy set (t2g).

A strong ligand field leads to a larger splitting energy (Δo) which can be greater than the pairing energy (P). This results in a low-spin configuration where electrons prefer to pair up in the lower energy orbitals.

The Jahn-Teller Effect describes the distortion of a molecule due to an uneven distribution of electrons in degenerate orbitals.

The higher energy set of orbitals in an octahedral complex is labeled as 'e_g'.

The statement is false. In a low spin configuration, the crystal field splitting energy (Δo) is larger than the pairing energy (P).

Ligand field theory explains how metal ions interact with ligands in crystals.

An octahedral complex has six anionic ligands surrounding the central metal ion.

Catalysis is not commonly used to detect the formation of a coordination compound.

The Valence bond approach uses d and f orbitals to explain the magnetic behavior of coordination compounds.

The Jahn-Teller Effect is associated with distortions in octahedral complexes.

Molecular weight is not considered when detecting the formation of a coordination compound.

Optical isomerism is never possible in square planar complexes.

The general formula for octahedral complexes exhibiting mer – fac isomerism is MA4B2.

When all light is reflected from an object, it appears white.

Different ligands on the same metal ion create different colors in complexes due to the variation in crystal field splitting.

When all light is absorbed by an object, it appears black.

The addition of NH3 ligand to Cu(H2O)4 changes its color due to changes in crystal field splitting caused by the different ligands.