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The compound Na2[Co(SCN)4] is to have a electronic spectrum is to have 3 peaks but only 2 show , where would the other peak be , in the uv region ?
Accepted Answer
The missing peak in the electronic spectrum of Na2[Co(SCN)4] is likely in the UV region. This complex exhibits a tetrahedral geometry with Co(II) as the central metal ion. The electronic transitions responsible for the observed peaks are d-d transitions within the Co(II) ion. The tetrahedral geometry splits the d orbitals into two sets, e and t2, with an energy difference between them. The two observed peaks correspond to transitions from the t2 orbitals to the e orbitals. The third possible transition, which would be from the lower t2 level to a higher energy e level, is likely in the UV region due to a larger energy difference between the two sets of orbitals. However, this transition can be weak or even absent due to various factors, including the specific ligand field strength, spin selection rules, and the presence of other electronic transitions in the UV region.
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