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An intermediate in chemistry is a short-lived, high-energy, highly reactive molecule. When generated in a chemical reaction, it will quickly convert into a more stable molecule. Only in exceptional cases can these compounds be isolated and stored. When their existence is indicated, intermediates can help explain how a chemical reaction takes place. An intermediate may be an unstable molecule or a highly stable molecule. An intermediate differs from a transition state in that the intermediate has a discrete lifetime while a transition state lasts for just one bond vibration cycle. Examples of organic intermediates include caustic soda flakes and boric acid. Browse through this category for various organic intermediates available in Zambian stores.
Intermediate: In a chemical reaction or mechanism, any reacting species which is no longer starting material or reactant, and has not yet become product, and which is not a transition state.
There are six types of reaction intermediates: carbocations, carbanions, free radicals, carbenes, nitrenes, and benzyne. These intermediates are often generated during the chemical decomposition of a chemical compound.
In chemistry, a reaction intermediate or an intermediate is a molecular entity that is formed from the reactants and reacts further to give the directly observed products of a chemical reaction. Most chemical reactions are stepwise, that is they take more than one elementary step to complete.
In chemistry, intermediate also called as the reaction intermediate is a substance formed in the ongoing process of a chemical reaction that involves a reactant and desired product. In biology, the process of conversion of nutritive material into cellular components is called intermediate metabolism.
An intermediate is a molecule that is formed from two or more reactants and then reacts further to give products. Most chemical reactions require more than one step, and an intermediate is the product of each step, except for the last one, after which the final products are produced.
Reactive intermediates
In chemistry, a reaction intermediate or an intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction.
Among the classes of generally unstable intermediates that are well studied are free radicals, carbenes, carbonium ions, and carbanions.
The carbocation bonded to three alkanes (tertiary carbocation) is the most stable, and thus the correct answer.
A reactive intermediate is a short-lived, high-energy, highly reactive molecule. When generated in a chemical reaction, it will quickly convert into a more stable molecule. Example : carbocation, carboanion, free radicals etc.
Primary intermediates: these include para-phenylene- diamine (PPD), para-toluenediamine (PTD), sub- stituted para-diamines, ortho-or para-aminophenols. Oxidation of these substances and coupling with modifiers result in coloured reaction products.
In the last few years it has become evident that small metabolic intermediates can be common denominators between two elementary biological processes: energy metabolism and gene regulation.
Goes over two examples that highlight the differences between catalysts and intermediates. A catalyst is used at the beginning of the reaction and regenerated at the end. An intermediate is produced during the reaction but no longer exists by the end.