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The magnitude of the difference in the crystal field stabilization energies of [Fe(H2O)6]2+ and [Fe(CN)6]4– is xDo (rounded up to first decimal place, ignoring pairing energy), then x:
Correct answer is '2.0'. Can you explain this answer?
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The magnitude of the difference in the crystal field stabilization ene...
The crystal field stabilization energy (CFSE) is the energy gained by the metal ion in a complex due to the splitting of the d-orbitals in the presence of ligands. The magnitude of the difference in the CFSEs of [Fe(H2O)6]2 and [Fe(CN)6]4 can be calculated using the following equation:
ΔCFSE = CFSE(high spin) - CFSE(low spin)
where CFSE(high spin) and CFSE(low spin) are the crystal field stabilization energies for the high spin and low spin configurations of the metal ion in the complex, respectively.
For [Fe(H2O)6]2, the metal ion has a d6 electron configuration and can adopt either a high spin or low spin configuration. The CFSEs for these configurations can be calculated using the appropriate equations:
CFSE(high spin) = -0.4 × 6 × Δo = -2.4Δo
CFSE(low spin) = -0.6 × 4 × Δo + 0.4 × 2 × Δo = -1.6Δo
where Δo is the crystal field splitting parameter for the ligand field.
For [Fe(CN)6]4, the metal ion has a d6 electron configuration and can only adopt a low spin configuration due to the strong ligand field of the cyanide ligands. The CFSE for this configuration can be calculated using the equation:
CFSE(low spin) = -0.6 × 6 × Δo = -3.6Δo
The magnitude of the difference in the CFSEs of [Fe(H2O)6]2 and [Fe(CN)6]4 is therefore:
ΔCFSE = CFSE(high spin) - CFSE(low spin)
ΔCFSE = (-2.4Δo) - (-3.6Δo)
ΔCFSE = 1.2Δo
This means that the CFSE for [Fe(H2O)6]2 is higher than that for [Fe(CN)6]4 by 1.2Δo. This difference in CFSE can have important implications for the reactivity, stability, and spectroscopic properties of these complexes.
ΔCFSE = CFSE(high spin) - CFSE(low spin)
where CFSE(high spin) and CFSE(low spin) are the crystal field stabilization energies for the high spin and low spin configurations of the metal ion in the complex, respectively.
For [Fe(H2O)6]2, the metal ion has a d6 electron configuration and can adopt either a high spin or low spin configuration. The CFSEs for these configurations can be calculated using the appropriate equations:
CFSE(high spin) = -0.4 × 6 × Δo = -2.4Δo
CFSE(low spin) = -0.6 × 4 × Δo + 0.4 × 2 × Δo = -1.6Δo
where Δo is the crystal field splitting parameter for the ligand field.
For [Fe(CN)6]4, the metal ion has a d6 electron configuration and can only adopt a low spin configuration due to the strong ligand field of the cyanide ligands. The CFSE for this configuration can be calculated using the equation:
CFSE(low spin) = -0.6 × 6 × Δo = -3.6Δo
The magnitude of the difference in the CFSEs of [Fe(H2O)6]2 and [Fe(CN)6]4 is therefore:
ΔCFSE = CFSE(high spin) - CFSE(low spin)
ΔCFSE = (-2.4Δo) - (-3.6Δo)
ΔCFSE = 1.2Δo
This means that the CFSE for [Fe(H2O)6]2 is higher than that for [Fe(CN)6]4 by 1.2Δo. This difference in CFSE can have important implications for the reactivity, stability, and spectroscopic properties of these complexes.
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