Would you expect the Mg3[Cr(CN)6]2 to be diamagnetic or paramagnetic? Explain your reasoning.

Name: Problem 46, Chapter 19: Chemistry
Uploaded: 2020-11-16T12:12:08-08:00
Duration: 5 min 25 s
Channel: Rashmi Sinha
Description: Would you expect the Mg3[Cr(CN)6]2 to be diamagnetic or paramagnetic? Explain your reasoning.

step 1 in the complex M .J. CR, CM. The central atom is the transition metal chromium. It's the central

Would you expect the Mg3[Cr(CN)6]2 to be diamagnetic or...

Key Concepts

Oxidation State Determination

Determining the oxidation state of the metal center is crucial for predicting its electronic configuration. By analyzing the overall charge of the complex and the charges on the ligands and counterions, one can deduce the d-electron count of the metal ion, which directly influences its magnetic properties.

Electronic Configuration

Once the oxidation state is known, the electronic configuration of the metal ion can be established. This configuration tells us how many electrons occupy the d-orbitals, revealing whether there are unpaired electrons present. The presence or absence of unpaired electrons underlies the difference between paramagnetic and diamagnetic behavior.

Ligand Field Theory

Ligand Field Theory explains how the approach of ligands around a metal ion causes splitting of the d-orbitals into groups of different energies. The magnitude of this splitting, and whether it encourages electron pairing, depends on both the nature of the metal ion and the strength of the ligands surrounding it.

Strong Field Ligands

Strong field ligands induce a large splitting in the d-orbitals, which can sometimes lead to electron pairing within the lower energy set. However, even with strong ligands, the electron count (as determined by the oxidation state) ultimately decides whether there remain unpaired electrons. Understanding the ligand's field strength is key for predicting specific magnetic behavior.

Magnetic Properties

The magnetic behavior of a complex is determined by the presence or absence of unpaired electrons. A species with one or more unpaired electrons is paramagnetic, meaning it is attracted to external magnetic fields, while a species with all electrons paired is diamagnetic and repelled by magnetic fields. Analyzing the electronic configuration in the context of ligand field theory helps predict the magnetic nature of a complex.

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