Textbook Question
The lobes of which d orbitals point directly between the ligands in a. octahedral geometry,
Ch.23 - Transition Metals and Coordination Chemistry
Chapter 23, Problem 49
Complete the exercises below. Identify each of the following coordination complexes as either diamagnetic or paramagnetic: a. [ZnCl₄]²⁻ b. [Pd(NH₃)₂ Cl₂]
Verified step by step guidance1
Step 1: Determine the oxidation state of the central metal ion in each complex. For [ZnCl₄]²⁻, zinc typically has an oxidation state of +2. For [Pd(NH₃)₂Cl₂], palladium can have an oxidation state of +2.
Step 2: Identify the electron configuration of the central metal ion in its oxidation state. For Zn²⁺, the electron configuration is [Ar] 3d¹⁰. For Pd²⁺, the electron configuration is [Kr] 4d⁸.
Step 3: Determine the number of unpaired electrons in the d-orbitals of the central metal ion. Zn²⁺ with a 3d¹⁰ configuration has no unpaired electrons, while Pd²⁺ with a 4d⁸ configuration needs further analysis.
Step 4: Analyze the ligand field and the geometry of the complex. [ZnCl₄]²⁻ is tetrahedral, and [Pd(NH₃)₂Cl₂] is square planar. Tetrahedral complexes often have high spin, but since Zn²⁺ has no unpaired electrons, it is diamagnetic. Square planar complexes like [Pd(NH₃)₂Cl₂] often lead to low spin configurations.
Step 5: Conclude the magnetic properties based on unpaired electrons. [ZnCl₄]²⁻ is diamagnetic due to no unpaired electrons. For [Pd(NH₃)₂Cl₂], check if the 4d⁸ configuration in a square planar field results in unpaired electrons to determine if it is paramagnetic or diamagnetic.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 bonds and the arrangement of ligands around the metal center can significantly influence the properties of the complex, including its magnetic behavior.
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Coordination Complexes Example
Magnetism in Coordination Complexes
Coordination complexes can be classified as diamagnetic or paramagnetic based on the presence of unpaired electrons. Diamagnetic complexes have all electrons paired, resulting in no net magnetic moment, while paramagnetic complexes contain unpaired electrons, leading to a net magnetic moment and attraction to magnetic fields.
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Electron Configuration and d-Orbitals
The electron configuration of the central metal ion, particularly the distribution of electrons in its d-orbitals, is crucial for determining the magnetic properties of coordination complexes. Transition metals can exhibit different oxidation states and coordination geometries, affecting the number of unpaired electrons and thus the complex's magnetic characteristics.
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02:06d Orbital Orientations
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?