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 [TiCl₆], b. Na₃ [Co(NO₂)₆], c. [Ru(en)₃] Br₃, d. [Mo(EDTA)] ClO₄, e. K₃ [ReCl₆].

Verified step by step guidance

Step 1: Identify the oxidation state of the central metal ion in each complex. This can be done by considering the charges of the ligands and the overall charge of the complex.

Step 2: Determine the electron configuration of the neutral metal atom, focusing on the d electrons. This involves knowing the position of the element in the periodic table.

Step 3: Calculate the number of d electrons in the metal ion by subtracting the oxidation state from the total number of d electrons in the neutral atom.

Step 4: For each complex, consider the ligands and their charges to ensure the oxidation state of the metal ion is correctly determined.

Step 5: Verify the number of d electrons by checking the consistency of the oxidation state and the electron configuration with known chemical properties of the metal.

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 and are crucial for determining how an element interacts chemically. In transition metals, these include the s and d electrons in the highest energy levels. Understanding the number of valence electrons helps predict the oxidation states and coordination behavior of metal ions in complexes.

Coordination Complexes

Coordination complexes consist of a central metal atom or ion bonded to surrounding molecules or ions, known as ligands. The nature of these ligands and their arrangement around the metal ion can significantly influence the properties of the complex, including its stability and reactivity. Identifying the ligands is essential for determining the electron count associated with the central metal.

Oxidation States of Transition Metals

Transition metals can exhibit multiple oxidation states due to the involvement of d electrons in bonding. The oxidation state of the metal in a complex can be determined by considering the charges of the ligands and the overall charge of the complex. This is vital for calculating the number of d electrons, as the d electron count is influenced by the oxidation state of the metal ion.

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Guided course

03:12

Transition Metals

Related Practice

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?