Borane
Borane - Related Videos
09:00
Lewis Acid-Base Interaction in Ph3P-BH3
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Source: Tamara M. Powers, Department of Chemistry, Texas A&M University One of the goals of chemistry is to use models that account for trends and provide insights into the properties of reactants that contribute to reactivity. Substances have been classified as acids and bases since the time of the ancient Greeks, but the definition of acids and bases has been modified and expanded over the years.1 The ancient Greeks would characterize substances by taste, and defined acids as those that...
08:19
Synthesis, Characterization, and Functionalization of Hybrid Au/CdS and Au/ZnS Core/Shell Nanoparticles
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Cited by 3 •
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The synthesis of uniform gold nanoparticles coated with semiconductor shells of CdS or ZnS is performed. The semiconductor coating is conducted by first depositing a silver sulfide shell and exchanging the silver cations for zinc or cadmium cations.
10:49
Nanomoulding of Functional Materials, a Versatile Complementary Pattern Replication Method to Nanoimprinting
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Cited by 1 •
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We describe a nanomoulding technique which allows low-cost nanoscale patterning of functional materials, materials stacks and full devices. Nanomoulding can be performed on any nanoimprinting setup and can be applied to a wide range of materials and deposition processes.
FAQs
Borane has an incomplete octet, so it can accept an electron pair from a Lewis base. That interaction produces a Lewis-base adduct and provides a way to accommodate borane’s electron deficiency. The tendency matters because borane does not behave only as an isolated species; its reactivity is closely connected to association with other electron-pair donors.
Diborane provides a distinct way to represent boron hydride bonding: some interactions are three-center, two-electron bonds rather than simple two-atom, two-electron bonds. In this arrangement, the bonding description spans three atoms while involving two electrons. This model helps explain how an electron-deficient boron hydride can be stabilized without a conventional complete octet.
During hydroboration, the two atoms of the reagent add across a carbon-carbon double bond in a predictable orientation. Boron attaches to the less substituted carbon, while hydrogen attaches to the more substituted carbon. This regiochemical pattern determines where the boron-containing intermediate forms and therefore helps control the position of the alcohol obtained after oxidation.
Oxidation changes the organoborane formed after alkene addition into an alcohol. Thus, hydroboration is not the final transformation: the first step installs a carbon-boron relationship, and the subsequent oxidation converts that intermediate into a hydroxyl-containing product. This two-stage sequence makes borane useful for turning carbon-carbon double bonds into selectively positioned alcohols.
Selectivity comes from the predictable way it adds to carbon-carbon double bonds and from the defined outcome of oxidation. Because boron is placed on the less substituted carbon and the resulting organoborane becomes an alcohol, the sequence links a known alkene position to a specific product arrangement. This enables preparation of valuable chemical intermediates.
Its chemistry links electron deficiency, Lewis-base adduct formation, diborane’s three-center, two-electron bonding, and hydroboration reactivity. Studying these connections lets chemists relate molecular bonding models to practical synthesis, because the same boron-centered behavior helps explain both fundamental boron chemistry and the formation of organic intermediates.