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Related Concept Videos

Metallic Solids02:37

Metallic Solids

Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
Crystal Field Theory - Octahedral Complexes02:58

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...
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.
Ladder Diagrams: Complexation Equilibria01:07

Ladder Diagrams: Complexation Equilibria

Ladder diagrams are useful for evaluating equilibria involving metal-ligand complexes. The vertical scale of the ladder diagram represents the concentration of unreacted or free ligand, pL. The horizontal lines on the scale depict the log of stepwise formation constants for metal-ligand complexes and indicate the dominant species in all the regions.
The formation constant, K1, for the formation of Cd(NH3)2+ complex from cadmium and ammonia is 3.55 × 102. Log K1 (i.e. pNH3) is 2.55, and...
Extraction: Advanced Methods00:56

Extraction: Advanced Methods

Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is formed in...
Microbes and Other Elemental Cycles01:24

Microbes and Other Elemental Cycles

Microbial activity plays a pivotal role in the biogeochemical cycling of iron and manganese, especially at the redox gradients characteristic of stratified aquatic environments. These cycles are driven by microbial transformations between oxidized and reduced forms of the metals, allowing organisms to exploit them for metabolic energy and structural purposes.Iron Cycling Across Redox GradientsIn neutral, oxygen-rich surface waters, iron is predominantly found in its oxidized, insoluble ferric...

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Related Experiment Video

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Detection and Recovery of Palladium, Gold and Cobalt Metals from the Urban Mine Using Novel Sensors/Adsorbents Designated with Nanoscale Wagon-wheel-shaped Pores
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Soluble Mn(III) in suboxic zones.

Robert E Trouwborst1, Brian G Clement, Bradley M Tebo

  • 1College of Marine and Earth Studies, University of Delaware, Lewes, DE 19958, USA.

Science (New York, N.Y.)
|September 30, 2006
PubMed
Summary

Soluble manganese(III) [Mn(III)], previously thought unstable, is abundant in natural waters like the Black Sea. This manganese form plays a key role in maintaining suboxic zones.

Area of Science:

  • Environmental Chemistry
  • Geochemistry
  • Marine Chemistry

Background:

  • Soluble manganese(III) [Mn(III)] was traditionally considered unstable in natural waters, rapidly disproportionating to Mn(II) and Mn(IV)O2.
  • Previous research suggested Mn(III) primarily existed as complexes only in laboratory settings, not in natural aquatic environments.

Purpose of the Study:

  • To investigate the occurrence and stability of soluble manganese(III) in natural water bodies.
  • To determine the role of soluble Mn(III) in the biogeochemical cycling of manganese in aquatic systems.
  • To understand the formation and stabilization mechanisms of Mn(III) in suboxic zones.

Main Methods:

  • Collected water samples from the Black Sea and Chesapeake Bay for manganese speciation analysis.
  • Utilized depth profiling to map the distribution of soluble Mn(III) within the water column.

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Published on: February 5, 2022

  • Analyzed manganese concentrations and speciation to identify Mn(III) production and consumption zones.

    • Main Results:

    • Detected high concentrations of soluble Mn(III), up to 5 micromolar, in the Black Sea, comprising 100% of dissolved manganese.
    • Identified Mn(III) production via Mn(II) oxidation at the upper suboxic zone and Mn(IV)O2 reduction at the lower suboxic zone.
    • Found that soluble Mn(III) is stabilized by unknown natural ligands in both studied environments.
    • Observed micromolar concentrations of dissolved Mn(III) in the Chesapeake Bay.

    Conclusions:

    • Soluble manganese(III) is a stable and significant component of dissolved manganese in natural waters.
    • Mn(III) plays a critical role in maintaining suboxic zones by acting as both an electron acceptor and donor.
    • Mn(III) is likely ubiquitous at oxic/anoxic interfaces in aquatic environments and sediments.