In which of the following complexes the CFSE, \(\Delta_0\) will be equal to zero?
Show Hint
- \([Fe(NH_3)_6]Br_2\)
- \([Fe(en)_3]Cl_3\)
- \(K_4[Fe(CN)_6]\)
- \(K_3[Fe(SCN)_6]\)
The Correct Option is D
Solution and Explanation
Crystal Field Stabilization Energy (CFSE) is a measure of the stability provided by a ligand to a transition metal ion in a coordination complex. It depends on the distribution of electrons in the d-orbitals of the metal ion, which is influenced by the geometry and the type of ligands.
To determine in which of the complexes the CFSE, \(\Delta_0\), will be equal to zero, we need to examine the oxidation state and the d-electron configuration of iron in each complex:
\([Fe(NH_3)_6]Br_2\):
Oxidation State: +2
d-electron Configuration: \(d^6\)
\([Fe(en)_3]Cl_3\):
Oxidation State: +3
d-electron Configuration: \(d^5\)
\(K_4[Fe(CN)_6]\):
Oxidation State: +2
d-electron Configuration: \(d^6\)
\(K_3[Fe(SCN)_6]\):
Oxidation State: +3
d-electron Configuration: \(d^5\)
The CFSE depends on the arrangement of d-electrons in the t2g and eg orbitals. In the case of a \(d^5\) configuration, the orbitals are often half-filled, leading to a uniform distribution of electrons in both t2g and eg\ orbitals. For high spin configurations, like Fe\(^{3+}\) in \([Fe(SCN)_6]^{3-}\), there are three electrons in t2g and two in eg\), which results in a CFSE of zero:
d⁵=(0×t2g+0×eg
Therefore, the complex \(K_3[Fe(SCN)_6]\) has a CFSE, \(\Delta_0\), of zero.
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