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Lecture

Chemistry of Sulfur and Halogens

In course

CH-221: Chemistry of elements s and p

Introduction to the chemistry of the s & p elements of the periodic table. ...

Description

This lecture covers the chemistry of sulfur and halogens, focusing on the properties, compounds, and applications of elements such as sulfur, fluorine, and chlorine. It discusses the formation of sulfuric acid, the different allotropes of sulfur, the synthesis of fluorine, and the uses of halogens in various industries.

Instructor

Kay Severin

Kay Severin was born in Germany in 1967. He obtained his Ph.D. in 1995 with a thesis in the group of Prof. W. Beck, University of Munich. Subsequently, he joined the group of Prof. M. R. Ghadiri as a postdoctoral fellow. In 1997, he started independent research projects ("Habilitation") at the Department of Chemistry, University of Munich. In 2001, he became assistant professor at the Institute of Chemical Sciences and Engineering at the Swiss Federal Institute of Technology, Lausanne (EPFL). Since 2009, he is full professor at the same institute. Awards: Bayerischer Habilitations Förderpreis (1997), ADUC award of the year (2001), Heinz Maier-Leibnitz award of the DFG (2001), award of the Karl-Ziegler foundation (2001), Arnold Sommerfeld award of the Bavarian Academy of Science (2001), Werner Prize of The Swiss Chemical Society (2003), Otto Roelen Medal of the DECHEMA (2005), award for chemistry of the Academy of Sciences, Göttingen (2007), Dalton Transactions European Lectureship (2008).

Official source

Ontological neighbourhood

Chemistry

Chemical reactions: Chemical substances

Related concepts (32)

Sulfur

Sulfur (also spelled sulphur in British English) is a chemical element with the symbol S and atomic number 16. It is abundant, multivalent and nonmetallic. Under normal conditions, sulfur atoms form cyclic octatomic molecules with a chemical formula S8. Elemental sulfur is a bright yellow, crystalline solid at room temperature. Sulfur is the tenth most abundant element by mass in the universe and the fifth most on Earth. Though sometimes found in pure, native form, sulfur on Earth usually occurs as sulfide and sulfate minerals.

Sulfuric acid

Sulfuric acid (American spelling and the preferred IUPAC name) or sulphuric acid (Commonwealth spelling), known in antiquity as oil of vitriol, is a mineral acid composed of the elements sulfur, oxygen, and hydrogen, with the molecular formula . It is a colorless, odorless, and viscous liquid that is miscible with water. Pure sulfuric acid does not occur naturally due to its strong affinity to water vapor; it is hygroscopic and readily absorbs water vapor from the air.

Sulfur dioxide

Sulfur dioxide (IUPAC-recommended spelling) or sulphur dioxide (traditional Commonwealth English) is the chemical compound with the formula SO2. It is a toxic gas responsible for the odor of burnt matches. It is released naturally by volcanic activity and is produced as a by-product of copper extraction and the burning of sulfur-bearing fossil fuels. SO2 is a bent molecule with C2v symmetry point group. A valence bond theory approach considering just s and p orbitals would describe the bonding in terms of resonance between two resonance structures.

Sulfurous acid

Sulfuric(IV) acid (United Kingdom spelling: sulphuric(IV) acid), also known as sulfurous (UK: sulphurous) acid and thionic acid, is the chemical compound with the formula . Raman spectra of solutions of sulfur dioxide in water show only signals due to the molecule and the bisulfite ion, . The intensities of the signals are consistent with the following equilibrium: 17O NMR spectroscopy provided evidence that solutions of sulfurous acid and protonated sulfites contain a mixture of isomers, which is in equilibrium: Attempts to concentrate the solutions of sulfurous acid simply reverses the equilibrium, producing sulfur dioxide and water vapor.

Lime sulfur

In horticulture, lime sulphur (American spelling lime sulfur) is mainly a mixture of calcium polysulfides and thiosulfate (plus other reaction by-products as sulfite and sulfate) formed by reacting calcium hydroxide with elemental sulfur, used in pest control. It can be prepared by boiling in water a suspension of poorly soluble calcium hydroxide (lime) and solid sulfur together with a small amount of surfactant to facilitate the dispersion of these solids in water.

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Sulfur and Nitrogen Cycles

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Sulfur Cycle: Microbial Processes and Energy Conservation

Explores microbial processes in the sulfur cycle and energy conservation mechanisms.

Sulfur Cycle: Processes and Implications

Explores the sulfur cycle processes, microbial components, and geochemical implications, including corrosion by sulfate-reducing bacteria.

Nitrogen and Sulfur Cycles in Biogeochemistry