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Chapter 20: Problem 26

What factors determine whether a given complex will be diamagnetic or paramagnetic?

Short Answer

Expert verified
Whether a complex will be diamagnetic or paramagnetic is determined by the presence or absence of unpaired electrons in its atomic or molecular orbitals. This in turn depends on the electron configuration of the complex ion, which could be influenced by the metal and the ligand field.

Step by step solution

01

Define Diamagnetic and Paramagnetic

Diamagnetic substances are those that do not have any unpaired electrons and are not attracted to a magnetic field. Paramagnetic substances, on the other hand, have one or more unpaired electrons and are attracted to a magnetic field.
02

Explain Electron Configuration

The electron configuration of an atom, ion or molecule determines whether it is paramagnetic or diamagnetic. If all the electrons are paired up in their atomic or molecular orbitals, the substance is diamagnetic. A substance is paramagnetic if it contains one or more unpaired electrons.
03

Determine the Magnetism of Complex Ions

Complex ions are a special case. Their magnetism depends on two factors: the metal ion and the ligand field. Some metal ions have unpaired electrons and are inherently paramagnetic, but the ligand field can influence the energy levels of the d orbitals and can cause the electrons to pair up. Consequently, a complex ion can be either diamagnetic or paramagnetic, depending on the metal ion and the ligand field.

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Most popular questions from this chapter

Complete these statements for the complex ion \(\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{2-} .\) (a) The oxidation number of \(\mathrm{Cr}\) is ____ (b) The coordination number of \(\mathrm{Cr}\) is____ (c) ___ is a bidentate ligand.

Give the oxidation numbers of the metals in these species: (a) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{K}_{3}\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (c) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

For the same type of ligands, explain why the crystal field splitting for an octahedral complex is always greater than that for a tetrahedral complex.

Define the terms (a) labile complex, (b) inert complex.

Copper is also known to exist in +3 oxidation state, which is believed to be involved in some biological electron transfer reactions. (a) Would you expect this oxidation state of copper to be stable? Explain. (b) Name the compound \(\mathrm{K}_{3} \mathrm{CuF}_{6}\) and predict the geometry of the complex ion and its magnetic properties. (c) Most of the known Cu(III) compounds have square planar geometry. Are these compounds diamagnetic or paramagnetic?
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