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Diethylaminosulfur trifluoride (DAST) is the organosulfur compound with the formula Et 2 NSF 3. This liquid is a fluorinating reagent used for the synthesis of organofluorine compounds . [ 1 ] The compound is colourless; older samples assume an orange colour.
Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO 3) 3. (H 2 O) n. Most common is the nonahydrate Fe(NO 3) 3. (H 2 O) 9. The hydrates are all pale colored, water-soluble paramagnetic salts.
The mechanism of fluorination by DAST parallels that of sulfur tetrafluoride. Attack of the hydroxyl group of the substrate on sulfur and elimination of hydrogen fluoride lead to an alkoxyaminosulfur difluoride intermediate. Nucleophilic attack by fluoride, either by an S N 1 [5] or S N 2 [6] pathway, leads to the product. Although clean ...
Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers. [4] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires. [5] It can be used as a mordant in dyeing.
This was demonstrated in the synthesis of meso-difluorosuccinate from (L)-tartrate and the synthesis of (D)- and (L)-difluorosuccinate from meso-tartrate. [6] Carbonyl compounds generally react with SF 4 to yield geminal difluorides. Reaction times tend to be on the order of hours and yields are moderate. [7]
Zinc sulfate is an inorganic compound with the formula ZnSO 4.It forms hydrates ZnSO 4 ·nH 2 O, where n can range from 0 to 7. All are colorless solids. The most common form includes water of crystallization as the heptahydrate, [4] with the formula Zn SO 4 ·7H 2 O.
Two sulfate nitrates are in the class of anthropogenic compounds, accidentally made as a result of human activities in fertilizers that are a mix of ammonium nitrate and ammonium sulfate, and also in the atmosphere as polluting ammonia, nitrogen dioxide, and sulfur dioxide react with the oxygen and water there to form solid particles.
Being the conjugate base of a strong acid (nitric acid, pK a = -1.4), nitrate has modest Lewis basicity.Two coordination modes are common: unidentate and bidentate.Often, bidentate nitrate, denoted κ 2-NO 3, is bound unsymmetrically in the sense that one M-O distance is clearly bonding and the other is more weakly interacting. [2]