Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.
(c) [Fe(CN)6]3- (low-spin)

Verified step by step guidance

Identify the oxidation state of the metal ion in the complex. For [Fe(CN)_6]^{3-}, determine the oxidation state of Fe by considering the charge of the complex and the charge of the ligands.

Determine the electron configuration of the free metal ion. For Fe^{3+}, write the electron configuration and identify the number of unpaired electrons.

Consider the effect of the ligands on the metal ion. CN^- is a strong field ligand, which can cause pairing of electrons in the d orbitals, leading to a low-spin configuration.

Determine the hybridization of the metal ion in the complex. For a low-spin [Fe(CN)_6]^{3-}, identify the hybrid orbitals used for bonding, considering the number of ligands and the geometry of the complex.

Draw the orbital diagrams for the free metal ion and the metal ion in the complex, showing the distribution of electrons and indicating the hybrid orbitals used for bonding. Specify the number of unpaired electrons in the complex.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Valence Bond Theory

Valence Bond Theory (VBT) explains how atoms bond by overlapping their atomic orbitals to form covalent bonds. In this theory, the shape and orientation of the orbitals determine the geometry of the molecule. For transition metals, VBT also considers hybridization, where atomic orbitals mix to create new hybrid orbitals that can accommodate bonding with ligands.

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are degenerate in energy. In the case of [Fe(CN)6]3-, the iron ion undergoes hybridization to form d2sp3 hybrid orbitals, which allows it to bond with six cyanide ligands in an octahedral geometry. Understanding the type of hybridization is crucial for predicting the molecular shape and bond angles.

Electron Configuration and Spin States

The electron configuration of a transition metal ion determines its magnetic properties and the number of unpaired electrons. In low-spin complexes like [Fe(CN)6]3-, the presence of strong field ligands like CN- causes pairing of electrons in the lower energy d-orbitals, resulting in fewer unpaired electrons. This concept is essential for understanding the magnetic behavior and stability of the complex.

Recommended video:

Guided course

01:32

Ground State Electron Configurations

Related Practice

Textbook Question

Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.

(a) [Ti(H2O)6]3+

Textbook Question

(d) [MnCl6]32 (high-spin)

Textbook Question

There are three coordination compounds with the empirical

formula Co1NH3231NO223 in which all the nitrite ions

are bonded through the N atom. Two isomers have the

same molar mass but different nonzero dipole moments.

The third compound is a salt with singly charged ions and a molar mass twice that of the other compounds.

(a) Draw the structures of the isomeric compounds.

Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons.(c) [Fe(CN)6]3- (low-spin)

Verified video answer for a similar problem:

Key Concepts

Valence Bond Theory

Hybridization

Electron Configuration and Spin States