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Electronic configuration for [co(ox)3]4-
Accepted Answer
The electronic configuration for [Co(ox)3]4- is [Ar] 3d7. Here's why:
1. Cobalt's (Co) Electronic Configuration: Cobalt in its ground state has the electron configuration [Ar] 3d7 4s2.
2. Oxalate (ox) Ligand: The oxalate ligand is a bidentate ligand (meaning it binds to the metal ion at two points), and it is a weak field ligand. Weak field ligands cause a smaller splitting of the d orbitals.
3. Coordination Complex Formation: In the complex [Co(ox)3]4-, the cobalt ion is in the +2 oxidation state. This means that it loses two electrons, leaving it with the configuration [Ar] 3d7.
4. Crystal Field Theory: The oxalate ligands create a weak field that causes the splitting of the d orbitals into two sets: the lower energy t2g orbitals and the higher energy eg orbitals. The 7 d electrons in Co2+ will fill the t2g orbitals completely and then partially fill the eg orbitals.
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