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A student predicts that the electronic configuration spectrum would have theree peaks for Na2[Co(SCN) 4] but the experiment shows two peaks . The student assumes that the third peak is in the uv region. is this true or false
Accepted Answer
The student's assumption is likely true. Here's why:
Ligand Field Theory: The electronic configuration spectrum (often referred to as a UV-Vis spectrum) of transition metal complexes arises from d-d transitions. In [Co(SCN)₄]²⁻, cobalt(II) has 3d⁷ configuration. The tetrahedral geometry splits the d-orbitals into two sets: e and t₂.
Expected Peaks: With 3d⁷ configuration and tetrahedral geometry, we would expect to see
three
distinct d-d transitions. However, the actual number of peaks observed can be less due to factors like:
Overlap: Peaks can overlap, making it appear as fewer peaks.
Spin Forbidden Transitions: Some transitions might be spin-forbidden, meaning they are less likely to occur and might be too weak to be observed.
UV Region: The UV region of the spectrum is where high-energy transitions occur. Since d-d transitions are typically in the visible range, a third peak in the UV region would be reasonable due to the higher energy level needed for the transition.
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