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Why are tetrahedral complexes generally high spin?

Answer
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Hint: For this, we should know about crystal field splitting in tetrahedral complexes. Same like octahedral crystal field, tetrahedral crystal field splits their orbitals into same t2g and eg sets of orbitals but the two orbitals in the eg set are lower in energy now than the three orbitals in the t2g set .

Complete answer:
A regular tetrahedron is similar to a cube. One atom at the centre of the cube and four of the eight corners of the cube contain ligands as shown in the following figure:
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The direction x , y and z point to the centre faces of the cube. The eg orbitals point along the x , y and z whereas the t2g orbitals point between x , y and z .
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Due to which the angle between an eg orbital, central metal and ligands is half of the tetrahedral angle, i.e. 109282 which is 5444 .On the other hand, the angle between a t2g orbital, central metal and ligands is 3516 . Thus t2g orbitals are nearer to the ligands than eg orbitals. Since the approach of the ligands raises the energy of both sets of orbitals, the energy of the t2g orbitals is raised most because they are close to the ligands as shown in figure:
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The t2g orbitals are 0.4Δt above the Bari centre and eg orbitals are 0.6Δt below the Bari centre. Thus, the tetrahedral crystal field splitting Δt is 23×23=49 of the octahedral crystal field splitting Δo . Strong field ligands cause a bigger energy difference between t2g and eg than weak field ligands. However, the tetrahedral splitting is always much smaller than that of octahedral splitting. Thus, it is never energetically favorable to electron pairs and hence all the tetrahedral complexes have high spin.

Note:
For coordination number four, the geometry for high spin is the tetrahedral as it has sp3 whereas the geometry for low spin will be square planar because of sp2d hybridization. Here Bari centre is the average energy level.