Related Experiment Video

Updated: Jun 1, 2026

Preparation and Reactivity of a Triphosphenium Bromide Salt: A Convenient and Stable Source of Phosphorus(I)
08:46

Preparation and Reactivity of a Triphosphenium Bromide Salt: A Convenient and Stable Source of Phosphorus(I)

Published on: November 22, 2016

Poly[(6-carboxy-picolinato-κO,N,O)(μ(3)-pyridine-2,6-dicarboxyl-ato-κO,N,O:O:O)dysprosium(III)]

Xu Li, Qing-Yang Lian, Qiu-Hui Meng

    Acta Crystallographica. Section E, Structure Reports Online
    |May 18, 2011
    PubMed

    More Related Videos

    The Synthesis, Characterization and Reactivity of a Series of Ruthenium N-triphosPh Complexes10:51

    The Synthesis, Characterization and Reactivity of a Series of Ruthenium N-triphosPh Complexes

    Published on: April 10, 2015

    Synthesis of pH Dependent Pyrazole, Imidazole, and Isoindolone Dipyrrinone Fluorophores using a Claisen-Schmidt Condensation Approach14:11

    Synthesis of pH Dependent Pyrazole, Imidazole, and Isoindolone Dipyrrinone Fluorophores using a Claisen-Schmidt Condensation Approach

    Published on: June 10, 2021

    Related Concept Videos

    Preparation of Diols and Pinacol Rearrangement01:57

    Preparation of Diols and Pinacol Rearrangement

    Compounds bearing two hydroxyl groups are known as diols. When the hydroxyl groups are located on adjacent carbon atoms, the diols are called vicinal diols or glycols. Under acidic conditions, vicinal diols undergo a specific reaction called pinacol rearrangement.
    The reaction begins with transferring a proton from the acid catalyst to one of the hydroxyl groups, producing an oxonium ion.
    Valence Bond Theory02:42

    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...
    Colors and Magnetism03:02

    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.
    Coordination Number and Geometry02:57

    Coordination Number and Geometry

    For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
    EDTA: Chemistry and Properties01:22

    EDTA: Chemistry and Properties

    Polydentate ligands are most widely used in complexometric titrations because they form more stable complexes with the metal ions than mono- or bidentate ligands due to the chelate effect. Examples of polydentate ligands are ethylenediaminetetraacetic acid (EDTA), crown ethers, and cryptands. The most important feature of optimal polydentate ligands is the ability to form 1:1 complexes in a single-step process. Amino carboxylic acid derivatives are frequently used as complexing agents. EDTA is...
    Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

    Crystal Field Theory - Tetrahedral and Square Planar Complexes

    Tetrahedral Complexes
    Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...