[Fe(CN)6]^{4-}

Definition

[Fe(CN)6]^{4-} is a coordination complex consisting of a central iron ion (Fe) surrounded by six cyanide ligands (CN^{-}). This complex has a 4- charge and is an example of a hexacyanoferrate(II) ion, which showcases important concepts in coordination chemistry such as coordination number, ligand types, and oxidation states.

5 Must Know Facts For Your Next Test

1. [Fe(CN)6]^{4-} is known as the ferrocyanide ion and is commonly used in various applications such as pigments and chemical analysis.
2. In this complex, iron is in the +2 oxidation state, allowing it to coordinate with the cyanide ligands effectively.
3. Cyanide acts as a strong field ligand, leading to significant splitting of d-orbitals in the iron center, which can affect color and magnetic properties.
4. The structure of [Fe(CN)6]^{4-} is octahedral due to the six ligands surrounding the central iron ion.
5. [Fe(CN)6]^{4-} can form stable complexes with various counterions, making it an important compound in coordination chemistry.

Review Questions

• How does the structure and charge of [Fe(CN)6]^{4-} influence its behavior as a coordination complex?
  • [Fe(CN)6]^{4-} has an octahedral structure due to its six cyanide ligands surrounding the iron center. The 4- charge contributes to its stability in solution and allows it to interact with positively charged counterions. The geometry and electronic properties resulting from the ligands influence its chemical reactivity, solubility, and role in various applications.
• Compare and contrast the role of strong field ligands like cyanide in [Fe(CN)6]^{4-} with weak field ligands.
  • Strong field ligands such as cyanide lead to significant splitting of d-orbitals in transition metal complexes like [Fe(CN)6]^{4-}, which can result in low-spin configurations. This contrasts with weak field ligands that cause less splitting, often resulting in high-spin configurations. The nature of the ligands directly affects properties like color, magnetic behavior, and stability, making understanding these differences crucial in coordination chemistry.
• Evaluate the importance of understanding oxidation states and coordination numbers in predicting the properties of complexes like [Fe(CN)6]^{4-}.
  • Understanding oxidation states and coordination numbers is key to predicting the properties of complexes such as [Fe(CN)6]^{4-}. The +2 oxidation state of iron affects its electron configuration and reactivity. Additionally, knowing that it has a coordination number of six helps predict its octahedral geometry, which is crucial for understanding its interactions with other ions and molecules. These concepts allow chemists to rationalize stability, reactivity, and potential applications of coordination compounds.

Related terms

Ligand:

An ion or molecule that donates a pair of electrons to a central metal atom or ion in a coordination complex.

Coordination Number:

The number of ligand atoms that are bonded to the central metal atom in a coordination complex.

Oxidation State:

The degree of oxidation of an atom in a compound, representing the total number of electrons that an atom gains or loses in the formation of that compound.