11/13/2022 0 Comments Pclp d7 v3 cl6One thing to keep in mind is that this energy splitting is different for each molecular geometry because each molecular geometry can hold a different number of ligands and has a different shape to its orbitals.Ī complex can be classified as high spin or low spin. Thus, due to the strong repelling force between the ligand field and the orbital, certain orbitals have higher energies than others. Remember, opposites attract and likes repel. This is because when the orbital of the central atom comes in direct contact with the ligand field, a lot of electron-electron repulsion is present as both the ligand field and the orbital contain electrons. It states that the ligand fields may come in contact with the electron orbitals of the central atom, and those orbitals that come in direct contact with the ligand fields have higher energy than the orbitals that come in indirect contact with the ligand fields. The ligand field theory states that electron-electron repulsion causes the energy splitting between orbitals. The ligand field theory is the main theory used to explain the splitting of the orbitals and the orbital energies in square planar, tetrahderal, and octahedral geometry. The ligand field theory and the splitting of the orbitals helps further explain which orbitals have higher energy and in which order the orbitals should be filled. Finally, the Pauli exclusion principle states that an orbital cannot have two electrons with the same spin. Hunds rule states that all orbitals must be filled with one electron before electron pairing begins. According to the Aufbau principle, orbitals with the lower energy must be filled before the orbitals with the higher energy. When filling orbitals with electrons, a couple of rules must be followed. The s sub-shell has one orbital, the p sub-shell has three orbitals, the d sub-shell has five orbitals, and the f sub-shell has seven orbitals. The sub-shell relates to the s, p, d, and f blocks that the electrons of an observed element are located. Electrons in different singly occupied orbitals of the same sub-shell have the same spins (or parallel spins, which are arrows pointing in the same direction). An arrow pointing up corresponds a spin of +1/2 and an arrow pointing corresponds to a spin of -1/2. When placing electrons in orbital diagrams, electrons are represented by arrows.
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