In both [Fe(H2 O)6]^2+ and [Fe(CN)6]^4- ions, the iron is present as Fe(II) ; however, [Fe(H2 O)

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In both [Fe(H2 O)6]^2+ and [Fe(CN)6]^4- ions, the iron is...

In both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ ions, the iron is present as $\mathrm{Fe}(\mathrm{II}) ;$ however, $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ is paramagnetic, whereas $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ is diamagnetic. Explain this difference.

In both $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ and $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ ions, the iron is
present as $\mathrm{Fe}(\mathrm{II}) ;$ however, $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}$ is paramagnetic, whereas $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}$ is diamagnetic. Explain this difference.

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Key Concepts

Ligand Field Theory

Ligand field theory explains the electronic structure of transition metal complexes by considering the interaction between the metal’s d orbitals and the electric field created by surrounding ligands. This theory predicts that the splitting of the metal's d orbitals into sets of different energies depends on the nature of the ligands, which in turn influences the distribution of electrons in these orbitals.

Spectrochemical Series

The spectrochemical series ranks ligands according to the strength of the crystal field they can generate. Strong field ligands (like cyanide) cause a larger splitting of the metal’s d orbitals, which can lead to low-spin configurations, while weak field ligands (like water) induce a smaller splitting, often resulting in high-spin configurations.

High-Spin and Low-Spin Complexes

High-spin and low-spin complexes refer to different arrangements of electrons within the d orbitals depending on the ligand field strength. In high-spin complexes, electrons occupy higher energy orbitals unpaired due to smaller splitting, often resulting in paramagnetism, whereas in low-spin complexes, electrons tend to pair up in lower energy orbitals because of larger splitting, typically leading to diamagnetism.

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