Sulfide Oxidation
Sulfide Oxidation - Related Videos
02:18
A Sensitive Visual Method for the Detection of Hydrogen Sulfide-Producing Bacteria
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2025
Source: Zhu, W., & Chu, W. Sensitive Visual Method for the Detection of Hydrogen Sulfide Producing Bacteria. J. Vis. Exp. (2022)This video demonstrates a sensitive visual method for the rapid detection of hydrogen sulfide–producing bacteria. A color change from yellow to black indicates bacterial activity through the formation of bismuth sulfide.
05:41
Photochemical Oxidative Growth of Iridium Oxide Nanoparticles on CdSe@CdS Nanorods
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Cited by 4 •
2016
A protocol for the photochemical oxidative growth of small crystalline iridium oxide nanoparticles on the surface of CdSe@CdS seeded rod nanoparticles is presented.
02:26
Preparation and Reactions of Sulfides
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2025
Sulfides are the sulfur analog of ethers, just as thiols are the sulfur analog of alcohol. Like ethers, sulfides also consist of two hydrocarbon groups bonded to the central sulfur atom. Depending upon the type of groups present, sulfides can be symmetrical or asymmetrical. Symmetrical sulfides can be prepared via an SN2 reaction between 2 equivalents of an alkyl halide and one equivalent of sodium sulfide. Asymmetrical sulfides can be synthesized by treating thiols with an alkyl halide and a...
02:17
Structure and Nomenclature of Thiols and Sulfides
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2023
Thiols and sulfides are sulfur analogs of alcohols and ethers, respectively, where the sulfur atom takes the place of the oxygen atom. Thus, thiols are generally represented as RSH, where R is an alkyl substituent and —SH is the functional group. On the other hand, in sulfides, the central sulfur atom is bonded to two hydrocarbon groups on either side. Depending upon the type of group, sulfides can be either symmetrical or asymmetrical. Both thiols and sulfides display a bent geometry, similar...
03:14
Oxidation Numbers
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2020
In redox reactions, the transfer of electrons occurs between reacting species. Electron transfer is described by a hypothetical number called the oxidation number (or oxidation state). It represents the effective charge of an atom or element, which is assigned using a set of rules. Oxidation Number (Oxidation State) In the case of an ionic compound, oxidation numbers are assigned based on the number of electrons transferred between reacting species. For example, in the formation of calcium...
FAQs
The key change is electron loss by sulfur, but the final product depends on how far oxidation proceeds and which electron acceptor is available. Under different reaction conditions, sulfide can yield elemental sulfur, sulfite, or sulfate. This product distribution connects oxidation-state changes to practical goals such as sulfur recovery or contaminant removal.
These variables influence the reaction pathway and the extent of sulfur oxidation. pH changes the chemical environment, while temperature affects reaction behavior; oxygen availability determines whether oxygen can serve as an electron acceptor. Consequently, the same sulfide source may produce different sulfur products when conditions change, which is important for controlled treatment.
Oxygen, hydrogen peroxide, and other electron acceptors can drive electron transfer from sulfide, yet they do not guarantee the same outcome. The available oxidant, together with pH, temperature, and oxygen supply, helps determine whether elemental sulfur, sulfite, or sulfate forms. Selecting conditions therefore links oxidant choice to the intended chemical result.
Elemental sulfur, sulfite, and sulfate represent different endpoints of sulfur oxidation, so identifying the product reveals how far the reaction proceeded. This distinction matters because the process may be designed to recover sulfur or to reduce sulfide-associated toxicity, odor, and corrosion. Product identity therefore connects chemical analysis with environmental and industrial decisions.
A practical plan begins by defining whether the goal is sulfur recovery or reduction of sulfide-related impacts. The operator can then select an oxidant, account for oxygen availability, and control pH and temperature because these factors influence the product formed. This approach helps align the reaction conditions with the desired treatment outcome.
In natural waters and soils, the process helps explain sulfur cycling by transforming sulfide into more highly oxidized sulfur forms. The same chemistry is relevant to sulfide-containing wastewater and acid mine drainage, where treatment aims to reduce toxicity, odor, and corrosion. Thus, environmental applications range from interpreting natural systems to managing contaminated streams.
Beyond reducing sulfide-related problems, controlled oxidation can support sulfur recovery when elemental sulfur is the desired product. The chemistry also provides an industrial framework for choosing among possible oxidants and operating conditions, since product formation depends on reactants, pH, temperature, and oxygen availability. This links redox control with resource recovery.