Lecture

Chemistry of Sulfur and Halogens

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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 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.

Chlorine

Chlorine is a chemical element with the symbol Cl and atomic number 17. The second-lightest of the halogens, it appears between fluorine and bromine in the periodic table and its properties are mostly intermediate between them. Chlorine is a yellow-green gas at room temperature. It is an extremely reactive element and a strong oxidising agent: among the elements, it has the highest electron affinity and the third-highest electronegativity on the revised Pauling scale, behind only oxygen and fluorine.

Chlorine trifluoride

Chlorine trifluoride is an interhalogen compound with the formula . This colorless, poisonous, corrosive, and extremely reactive gas condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature). Despite being famous for its extreme oxidation properties and igniting many things, chlorine trifluoride is not combustible itself.

Halogen

The halogens (ˈhælədʒən,ˈheɪ-,-loʊ-,_-ˌdʒɛn) are a group in the periodic table consisting of six chemically related elements: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At), and tennessine (Ts), though some authors would exclude tennessine as its chemistry is unknown and is theoretically expected to be more like that of gallium. In the modern IUPAC nomenclature, this group is known as group (XVII) or group (VII). The word "halogen" means "salt former" or "salt maker".

Chlorine-releasing compounds

Chlorine-releasing compounds, also known as chlorine base compounds, is jargon to describe certain chlorine-containing substances that are used as disinfectants and bleaches. They include the following chemicals: sodium hypochlorite (active agent in bleach), chloramine, halazone, and sodium dichloroisocyanurate. They are widely used to disinfect water and medical equipment, and surface areas as well as bleaching materials such as cloth. The presence of organic matter can make them less effective as disinfectants.

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