Crystal Field Theory assumes that the electrostatic interactions between metal ions and ligands are the dominant factor in determining the electronic structure and properties of coordination complexes.

The strength of the crystal field is influenced by the charge of the metal ion, the nature of the ligands (their field strength), and the geometry of the coordination complex.

In an octahedral crystal field, the d-orbitals of the metal ion split into two sets: the t_2g orbitals (d_xy, d_yz, d_xz) and the e_g orbitals (d_z², d_x²-y²).

The strength of the crystal field splitting increases with the field strength of the ligands. Cyanide (CN^-) is a strong field ligand, therefore [Ni(CN)₄]^2- exhibits the strongest crystal field splitting among the given complexes.

The Jahn-Teller effect occurs when a coordination complex with a high-spin configuration undergoes a distortion from its ideal geometry to lower its energy. This distortion results in a splitting of the degenerate d-orbitals and a lowering of the overall energy of the complex.

The Jahn-Teller effect is most likely to occur in complexes with high-spin configurations and degenerate d-orbitals. [Cu(NH₃)₄]²⁺ has a high-spin d⁹ configuration and a tetragonal geometry, making it susceptible to the Jahn-Teller effect.

The crystal field splitting energy (Δ) is inversely proportional to the wavelength of light absorbed by a coordination complex. This relationship is expressed by the equation: Δ = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of light absorbed.

Complexes that absorb light in the visible region of the spectrum typically have a small crystal field splitting energy (Δ). [Co(NH₃)₆]³⁺ has a low Δ value and is therefore likely to absorb light in the visible region.

High-spin and low-spin complexes refer to the different electronic configurations that metal ions can adopt in coordination complexes. High-spin complexes have all the d-orbitals singly occupied, while low-spin complexes have some of the d-orbitals paired.

Strong field ligands promote the pairing of electrons in metal ion d-orbitals, leading to the formation of low-spin complexes. This is because strong field ligands cause a large crystal field splitting energy (Δ), which makes it energetically favorable for electrons to pair up.

Ligand field stabilization energy (LFSE) is the energy difference between the high-spin and low-spin states of a coordination complex. LFSE arises from the pairing of electrons in metal ion d-orbitals, which is favored by strong field ligands.

Ligand field stabilization energy (LFSE) is influenced by the strength of the crystal field. [Ni(CN)₄]^2- has a strong crystal field due to the strong field cyanide ligands, resulting in a large LFSE.

Charge transfer refers to the transfer of electrons between metal ions and ligands, resulting in a change in the color of the coordination complex. This phenomenon is observed in complexes where the metal ion and ligands have different electronegativities.

Charge transfer is more likely to occur in complexes where the metal ion and ligands have different electronegativities. [Fe(H₂O)₆]³⁺ has a high electronegative metal ion (Fe³⁺) and low electronegative ligands (H₂O), making it susceptible to charge transfer.

Metal-ligand bonding refers to the interactions between metal ions and ligands in a coordination complex. These interactions can be classified into various types, such as ionic bonding, covalent bonding, and coordinate bonding.