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The general structure of a boronic acid, where R is a substituent. A boronic acid is an organic compound related to boric acid (B(OH) 3) in which one of the three hydroxyl groups (−OH) is replaced by an alkyl or aryl group (represented by R in the general formula R−B(OH) 2). [1]
Pyrimidine (C 4 H 4 N 2; / p ɪ ˈ r ɪ. m ɪ ˌ d iː n, p aɪ ˈ r ɪ. m ɪ ˌ d iː n /) is an aromatic, heterocyclic, organic compound similar to pyridine (C 5 H 5 N). [3] One of the three diazines (six-membered heterocyclics with two nitrogen atoms in the ring), it has nitrogen atoms at positions 1 and 3 in the ring.
Pentaborane(9) is an inorganic compound with the formula B 5 H 9.It is one of the most common boron hydride clusters, although it is a highly reactive compound.Because of its high reactivity with oxygen, it was once evaluated as rocket or jet fuel.
The structures can be rationalised by polyhedral skeletal electron pair theory. [3] Boranes are chemical compounds of boron and hydrogen, with the generic formula of B x H y. These compounds do not occur in nature. Many of the boranes readily oxidise on contact with air, some violently.
Structure of a rare monomeric boron hydride, R = i-Pr. [4] The most-studied class of organoboron compounds has the formula BR n H 3−n. These compounds are catalysts, reagents, and synthetic intermediates. The trialkyl and triaryl derivatives feature a trigonal-planar boron center that is typically only weakly Lewis acidic.
Organotrifluoroborates are organoboron compounds that contain an anion with the general formula [RBF 3] −. They can be thought of as protected boronic acids, or as adducts of carbanions and boron trifluoride. Organotrifluoroborates are tolerant of air and moisture [1] and are easy to handle and purify. [2]
Tris(pentafluorophenyl)borane, sometimes referred to as "BCF", is the chemical compound (C 6 F 5) 3 B.It is a white, volatile solid. The molecule consists of three pentafluorophenyl groups attached in a "paddle-wheel" manner to a central boron atom; the BC 3 core is planar.
Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots. [106] [107] One example is the sulfur trioxide pyridine complex (melting point 175 °C), which is a sulfation agent used to convert alcohols to sulfate esters. Pyridine-borane (C 5 H 5 NBH 3, melting point 10–11 °C) is a mild ...