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Amine. In chemistry, amines (/ ə ˈ m iː n, ˈ æ m iː n /, [1] [2] UK also / ˈ eɪ m iː n / [3]) are compounds and functional groups that contain a basic nitrogen atom with a lone pair.Formally, amines are derivatives of ammonia (NH 3 (in which the bond angle between the nitrogen and hydrogen is 170°), wherein one or more hydrogen atoms have been replaced by a substituent such as an ...
The term dipolar bond is used in organic chemistry for compounds such as amine oxides for which the electronic structure can be described in terms of the basic amine donating two electrons to an oxygen atom. R 3 N → O. The arrow → indicates that both electrons in the bond originate from the amine moiety. In a standard covalent bond each ...
General structure of an amine oxide. In chemistry, an amine oxide, also known as an amine N-oxide or simply N-oxide, is a chemical compound that has the chemical formula R 3 N + −O −. It contains a nitrogen-oxygen coordinate covalent bond with three additional hydrogen and/or substituent-groups attached to nitrogen.
The chemistry involved in the amine treating of such gases varies somewhat with the particular amine being used. For one of the more common amines, monoethanolamine (MEA) denoted as RNH 2, the acid-base reaction involving the protonation of the amine electron pair to form a positively charged ammonium group (RNH + 3) can be expressed as: RNH 2 ...
The amino radical has two characteristic electronic states: The more stable electronic state is 2 B 1, where the unpaired electron is in the p-orbital perpendicular to the plane of the molecule (π type radical). The high energy electronic state, 2 A 1, has the two electrons in the p-orbital and the unpaired electron in the sp 2 orbital (σ ...
The lone electron pair on the nitrogen delocalizes into the pi system of the benzene ring. This is responsible for nitrogen's weaker basicity compared to other amines. Missing in such an analysis is consideration of solvation. Aniline is, for example, more basic than ammonia in the gas phase, but ten thousand times less so in aqueous solution. [21]
Compared to amines, amides are very weak bases. While the conjugate acid of an amine has a pK a of about 9.5, the conjugate acid of an amide has a pK a around −0.5. Therefore, compared to amines, amides do not have acid–base properties that are as noticeable in water. This relative lack of basicity is explained by the withdrawing of ...
Ethylamine like some other small primary amines is a good solvent for lithium metal, giving the ion [Li(amine) 4] + and the solvated electron. Such solutions are used for the reduction of unsaturated organic compounds, such as naphthalenes [11] and alkynes.