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Colors and Magnetism

Colors and Magnetism

Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.

Valence Bond Theory

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...

Coordination Compounds and Nomenclature

Coordination Compounds and Nomenclature

In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...

Metal-Ligand Bonds

Metal-Ligand Bonds

The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...

Ionic Crystal Structures

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Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...

Crystal Field Theory - Octahedral Complexes

Crystal Field Theory - Octahedral Complexes

Crystal Field Theory
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...

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Preparation, Purification, and Characterization of Lanthanide Complexes for Use as Contrast Agents for Magnetic Resonance Imaging

Preparation, Purification, and Characterization of Lanthanide Complexes for Use as Contrast Agents for Magnetic Resonance Imaging

Published on: July 21, 2011

Lanthanite-(Nd), Nd2(CO3)3·8H2O.

Shaunna M Morrison¹, Marcelo B Andrade, Michelle D Wenz

¹Department of Geosciences, University of Arizona, 1040 E. 4th Street, Tucson, Arizona 85721-0077, USA.

Acta Crystallographica. Section E, Structure Reports Online

|March 12, 2013

Summary

This summary is machine-generated.

The first crystal structure of lanthanite-(Nd), dineodymium(III) tricarbonate octa-hydrate, was determined using X-ray diffraction. This rare earth mineral features infinite sheets linked by water molecule hydrogen bonds.

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Area of Science:

Mineralogy
Crystallography
Geochemistry

Background:

Lanthanite-(Nd), or dineodymium(III) tricarbonate octa-hydrate, belongs to the lanthanite mineral group with the general formula REE2(CO3)3·8H2O.
Rare earth elements (REEs) in this group are characterized by 10-coordination.

Purpose of the Study:

To present the first structure determination of lanthanite-(Nd) using single-crystal X-ray diffraction.
To analyze the structural characteristics of lanthanite-(Nd) and compare it with other lanthanite group members.

Main Methods:

Single-crystal X-ray diffraction was performed on a natural sample of lanthanite-(Nd).
The crystal structure was solved and refined.

Main Results:

The study determined the precise crystal structure of lanthanite-(Nd).
The determined structure is highly similar to those of other known lanthanite group minerals.
The structure consists of infinite sheets of NdO10-polyhedra and carbonate triangles, stacked perpendicular to the c-axis.
Interlayer connectivity is established solely through hydrogen bonding involving water molecules.

Conclusions:

The detailed crystal structure of lanthanite-(Nd) has been elucidated for the first time.
The findings confirm the structural similarity within the lanthanite mineral group.
Hydrogen bonding plays a crucial role in the structural integrity of lanthanite-(Nd).