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Most simple redox reactions may be classified as a combination, decomposition, or single displacement reaction. Different chemical reactions are used during chemical synthesis in order to obtain the desired product. In biochemistry, a consecutive series of chemical reactions (where the product of one reaction is the reactant of the next ...
Chemical nomenclature, replete as it is with compounds with very complex names, is a repository for some names that may be considered unusual. A browse through the Physical Constants of Organic Compounds in the CRC Handbook of Chemistry and Physics (a fundamental resource) will reveal not just the whimsical work of chemists, but the sometimes peculiar compound names that occur as the ...
Algar–Flynn–Oyamada reaction; Alkylimino-de-oxo-bisubstitution; Alkyne trimerisation; Alkyne zipper reaction; Allan–Robinson reaction; Allylic rearrangement; Amadori rearrangement; Amine alkylation; Angeli–Rimini reaction; Andrussov oxidation; Appel reaction; Arbuzov reaction, Arbusow reaction; Arens–Van Dorp synthesis, Isler ...
Redox reactions (see list of oxidants and reductants) Reduction; Reductive elimination; Reppe synthesis; Riley oxidation; Salt metathesis; Sarett oxidation; Sharpless epoxidation; Shell higher olefin process; Silylation; Simmons–Smith reaction; Sonogashira coupling; Staudinger reaction; Stille reaction; Sulfidation; Suzuki reaction ...
Salt metathesis reaction; Salt-free reduction; Scavenger resin; Screaming jelly babies; SEA Native Peptide Ligation; Self-assembling peptide; Semiclassical transition state theory; Shiina esterification; Side reaction; Single displacement reaction; Small molecule sensors; Solid-state reaction route; Spin-forbidden reactions; Stripping reaction ...
Many variants of the reaction exist. The only key chemical is the bromate oxidizer. The catalyst ion is most often cerium, but it can be also manganese, or complexes of iron, ruthenium, cobalt, copper, chromium, silver, nickel and osmium. Many different reductants can be used. (Zhabotinsky, 1964b; Field and Burger, 1985) [16]
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Outside of the industrial sector, cracking of C−C and C−H bonds are rare chemical reactions. In principle, ethane can undergo homolysis: CH 3 CH 3 → 2 CH 3 ⋅. Because C−C bond energy is so high (377 kJ/mol), [18] this reaction is not observed under laboratory conditions.