In Ligand Field Theory, ligands are molecules, ions, or atoms that donate electrons to a metal center, forming coordination complexes. Metal ions are the central atoms that accept electrons from ligands.

In Ligand Field Theory, the splitting of d-orbitals is primarily caused by the interaction between the metal ion and the ligands. This interaction is influenced by the nature of the ligands, their symmetry, and the number of electrons in the d-orbitals.

The magnitude of the crystal field splitting energy is influenced by several factors, including the charge of the metal ion, the number of d-electrons, and the geometry of the coordination complex. These factors collectively determine the strength of the interaction between the metal ion and the ligands.

In an octahedral complex, the t_2g orbitals (d_xy, d_yz, and d_xz) are lower in energy than the e_g orbitals (d_z² and d_x²-y²) due to the splitting of d-orbitals caused by the octahedral ligand field.

Tetrahedral complexes generally exhibit a smaller crystal field splitting energy, a lower degree of orbital overlap, and are less stable compared to octahedral complexes.

The Jahn-Teller effect describes the distortion of a coordination complex from its regular geometry in order to lower its energy. This distortion is caused by the presence of unpaired electrons in the d-orbitals of the metal ion.

The Jahn-Teller effect primarily leads to a change in the coordination geometry of the complex in order to lower its energy. It does not necessarily affect the crystal field splitting energy or the stability of the complex.

The spectrochemical series arranges ligands based on their ability to split d-orbitals in a coordination complex. This series is useful in predicting the magnitude of the crystal field splitting energy and the electronic configuration of the metal ion.

CN^- is a strong-field ligand due to its high electronegativity and the ability to form strong covalent bonds with metal ions. It causes a large splitting of d-orbitals and stabilizes low-spin complexes.

CO is a weak-field ligand due to its low electronegativity and the ability to form π-backbonding interactions with metal ions. It causes a small splitting of d-orbitals and stabilizes high-spin complexes.

The electronic configuration of a metal ion in a coordination complex can be determined using Ligand Field Theory, Molecular Orbital Theory, or Valence Bond Theory. These theories provide different perspectives on the bonding and electronic structure of coordination complexes.

Coordination isomerism is not a type of isomerism observed in coordination complexes. The other three options, structural isomerism, geometrical isomerism, and ligand isomerism, are common types of isomerism encountered in coordination chemistry.

The stability of a coordination complex is influenced by several factors, including the strength of the metal-ligand bond, the number of d-electrons in the metal ion, and the geometry of the coordination complex.

Ligand Field Theory has various applications, including predicting the color of coordination complexes, designing catalysts for chemical reactions, and understanding the electronic structure and bonding in coordination complexes.

Ligand Field Theory is specifically developed to study the electronic structure, bonding, and properties of coordination complexes, which are formed by the interaction of metal ions with ligands.