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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 21.131b
Capitolo 21, Problema 21.131b

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.
(b) If NiCl2L2 is paramagnetic and Ni(NCS)2L2 is diamagnetic, which of the two complexes is tetrahedral and which is square planar?

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1
Understand the terms: Paramagnetic substances have unpaired electrons, while diamagnetic substances have all electrons paired.
Recall that square planar complexes often result in low-spin configurations, leading to paired electrons, while tetrahedral complexes are usually high-spin, resulting in unpaired electrons.
Consider the electronic configuration of Nickel(II), which is [Ar] 3d^8.
In a square planar geometry, the d-orbitals split such that the electrons pair up, leading to a diamagnetic complex.
In a tetrahedral geometry, the d-orbitals split differently, often resulting in unpaired electrons, leading to a paramagnetic complex.

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Coordination Geometry

Coordination geometry refers to the spatial arrangement of ligands around a central metal atom in a complex. Nickel(II) complexes can adopt different geometries, such as square planar or tetrahedral, depending on the number and type of ligands coordinated to the metal. The geometry influences the electronic properties and reactivity of the complex.
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Molecular Geometry of Coordination Complexes

Magnetism in Coordination Complexes

The magnetic properties of coordination complexes are determined by the presence of unpaired electrons. A paramagnetic complex has unpaired electrons, resulting in a net magnetic moment, while a diamagnetic complex has all electrons paired, leading to no net magnetic moment. Understanding these properties helps in predicting the geometry of the complexes based on their magnetic behavior.
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Coordination Complexes Example

Ligand Field Theory

Ligand field theory explains how the arrangement of ligands around a metal ion affects its electronic structure and energy levels. In square planar complexes, the d-orbitals split in a way that can stabilize unpaired electrons, leading to paramagnetism, while tetrahedral complexes have a different splitting pattern that can lead to diamagnetism. This theory is crucial for understanding the electronic configurations of metal complexes.
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Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
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