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Ch.21 - Transition Elements and Coordination Chemistry
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblema 21.118a
Capitolo 21, Problema 21.118a

Draw a crystal field energy-level diagram, and predict the number of unpaired electrons for each of the following: 
(a) [Mn(H2O)6]2+

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Identify the metal ion and its oxidation state. For [Mn(H2O)_6]^{2+}, manganese (Mn) is in the +2 oxidation state.
Determine the electron configuration of the Mn^{2+} ion. Manganese in its elemental form is [Ar] 3d^5 4s^2, so Mn^{2+} is [Ar] 3d^5.
Recognize that [Mn(H2O)_6]^{2+} is an octahedral complex, which means the 3d orbitals will split into two sets: t_{2g} (lower energy) and e_g (higher energy).
Distribute the 5 d-electrons of Mn^{2+} among the split d-orbitals according to Hund's rule, filling the lower energy t_{2g} orbitals first before pairing electrons in the higher energy e_g orbitals.
Count the number of unpaired electrons in the d-orbitals after distribution.

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Crystal Field Theory

Crystal Field Theory (CFT) explains how the arrangement of ligands around a central metal ion affects its electronic structure and energy levels. It describes the splitting of d-orbitals in transition metal complexes due to the electrostatic interactions between the metal ion and surrounding ligands. This theory is crucial for predicting the magnetic properties and color of the complexes.
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The study of ligand-metal interactions helped to form Ligand Field Theory which combines CFT with MO Theory.

d-Orbital Splitting

In an octahedral field, the five d-orbitals split into two energy levels: the lower-energy t2g (dxy, dyz, dzx) and the higher-energy eg (dx2-y2, dz2) orbitals. The extent of this splitting depends on the nature of the ligands and their field strength. Understanding this splitting is essential for determining the electron configuration and the number of unpaired electrons in a complex.
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d Orbital Orientations

Unpaired Electrons and Magnetism

Unpaired electrons in an atom or ion contribute to its magnetic properties. A species with unpaired electrons exhibits paramagnetism, while those with all paired electrons are diamagnetic. In the context of transition metal complexes, the number of unpaired electrons can be predicted from the electron configuration after considering d-orbital splitting, which is vital for understanding the complex's behavior in a magnetic field.
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Magnetic Quantum Example
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Domanda del libro di testo

What is the systematic name for each of the following ions?

(a) [MnCl4]2-

(b) [Ni(NH3)6]2+

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Six isomers for a square planar palladium(II) complex that contains two Cl-and two SCN-ligands are shown below.


(a) Which structures are cis-trans isomers?

(b) Which structures are linkage isomers?

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Assign a systematic name to each of the following ions.  

(a) [AuCl4]-

(b) [Fe(CN)6]4-

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For each of the following complexes, describe the bonding using valence bond theory. 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) [AuCl4]2 (square planar)

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Tell how many diastereoisomers are possible for each of the following complexes, and draw their structures. 

(a) Pt(NH3)3Cl (square planar) 

(b) [FeBr2Cl2(en)]-

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Nickel(II) complexes with the formula NiX2L2, where X− is Cl− or N-bonded NCS− and L is the monodentate triphenylphosphine ligand P(C6H5)3, can be square planar or tetrahedral.

(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.

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