Complete the exercises below. Give the number of (valence) d electrons associated with the central metal ion in each of the following complexes: a. K₃[Fe(CN)₆] b. [Mn(H₂O)₆](NO₃)₂ c. Na[Ag(CN)₂] d. [Cr(NH₃)₄Br₂]ClO₄ e. [Sr(EDTA)]²⁻

Verified step by step guidance

Identify the oxidation state of the central metal ion in each complex by considering the charges of the ligands and the overall charge of the complex.

Determine the electron configuration of the neutral metal atom, focusing on the d electrons.

Subtract the number of electrons corresponding to the oxidation state from the total number of d electrons in the neutral atom to find the number of valence d electrons in the metal ion.

For each complex, apply the above steps to calculate the number of valence d electrons for the central metal ion.

Verify your results by ensuring the sum of the charges of the metal ion and the ligands equals the overall charge of the complex.

Key Concepts

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

Valence Electrons

Valence electrons are the outermost electrons of an atom that are involved in forming bonds. For transition metals, these include the s and d electrons in the outermost shell. Understanding the number of valence electrons is crucial for determining the oxidation state of the metal ion in coordination complexes.

Coordination Complexes

Coordination complexes consist of a central metal atom or ion bonded to surrounding molecules or ions called ligands. The nature of these ligands, whether they are neutral or charged, affects the overall charge of the complex and the electron count of the central metal. Identifying the ligands and their charges is essential for calculating the d electron count.

Oxidation State

The oxidation state of a metal ion in a complex indicates the charge it carries, which influences the number of d electrons. To find the oxidation state, one must consider the charges of the ligands and the overall charge of the complex. This is vital for determining how many d electrons are present in the metal ion, as it directly affects its electronic configuration.

Recommended video:

Guided course

02:42

Oxidation Numbers

Related Practice

Textbook Question

The lobes of which d orbitals point directly between the ligands in a. octahedral geometry,

Textbook Question

The lobes of which d orbitals point directly between the ligands in b. tetrahedral geometry?

Textbook Question

As shown in Figure 23.26, the d-d transition of [Ti(H₂O)₆]³⁺ produces an absorption maximum at a wavelength of about 500 nm .

a. What is the magnitude of ∆ for [Ti(H₂O)₆]³⁺ in kJ/mol?

b. How would the magnitude of ∆ change if the H₂O ligands in [Ti(H₂O)₆]]³⁺ were placed with NH₃ ligands?

Textbook Question

A classmate says, “A weak-field ligand usually means the complex is high spin.” Is your classmate correct? Explain.

Textbook Question

For a given metal ion and set of ligands, is the crystal-field splitting energy larger for a tetrahedral or an octahedral geometry?