Cyanides, alkaline-metal, reactions

CHLOROACETIC ACID, ETHYL ESTER (105-39-5) Combustible liquid (flash point 147°F/64°C oc also listed at 129°F/54°C). Violent reaction with oxidizers. Reacts with water, forming acetic acid. Violent reaction with alkaline earth metals, alkaline metals. Incompatible with sodium cyanide + heat. Attacks many metals in the presence of moisture, producing hydrogen gas. 

Inorganic cyanides are the metal salts of hydrocyanic acid, HCN. Alkali and alkaline metal cyanides are characterized by ionic bonding between the metal ion and the cyanide, CN, thns having a crystalline strnctnre. These are formed by the typical acid-base reaction ... 

The catalytic activity of cross-linked polymeric sulfoxides differing in the functionality of the polystyrene matrix (the general formula is ( -(CH20CH2) -R, whereby (P) is the polystyrene matrix cross-linked by divinylbenzene, R = H or CH3, and n = 1, 2 or 3), has been studied in nucleophilic substitution reactions between alkyl bromides (1-bromobutane and 1-bromooctane) and phenoxides, iodides, thiocyanates or cyanides of alkaline metals under the conditions of catalytic three-phase reactions in the liquid-solid-liquid system [66]. The reaction is carried out in a toluene-water medium between 70-100°C. In the systems the rate of anion transfer from the liquid phase to the organic phase decreases in the sequence PhO > J > SCN > CN . 

The Strecker reaction [48], discovered in 1850 [1], is the most practical and efficient tool for the preparation of a-amino acids [49] via the formation of a-aminonitriles (Scheme 10.15) [50]. This three-component coupling between an amine or its equivalent, a carbonyl compound (generally an aldehyde), and hydrogen cyanide or its alkaline metal cyanides can be also made enantioselectively through the use of both metal-based catalysts and chiral organocatalysts. 

Many reactions can be carried out between potassium cyanide and organic compounds with the alkalinity of the KCN acting as a catalyst these reactions are analogous to reactions of sodium cyanide. The reactions of potassium cyanide with sulfur and sulfur compounds are also analogous to those of sodium cyanide. Potassium cyanide is reduced to potassium metal and carbon by heating it out of contact with air in the presence of powdered magnesium. Magnesium is converted to the nitride ... 

Simple cyanides typically refer to alkali water-soluble salts, such as NaCN, KCN, Ca(CN)2, and Hg(CN)2, but also include several cyanide salts of alkali, alkaline earth, or heavy metals, that is, Zn(CN)2, Cd(CN)2, Ni(CN)2, and AgCN, of varying degrees of solubility. In water, NaCN and KCN will completely dissociate to give free cyanide. All simple cyanides ionize in water to release cyanide ion which, depending on pH, will form hydrocyanic acid. For sodium cyanide, the reaction proceeds as follows ... 

In summary, the reaction between an alkali metal alkoxide and a poly-hydroxy compound in hot alcoholic media produces an alcoholate and, possibly, a small proportion of alkoxide adduct however, the conditions governing the ratio of alcoholate to adduct have not yet been well defined. Reactions with alkali metal hydroxides and cyanides produce mixtures (of alcoholate and adduct) that consist mainly of alcoholate. Occurrence of reactions between alkaline-earth metal hydroxides and polyhydroxy compounds in anhydrous alcoholic media has not been reported. 

The preparation of cyanomethylbenzo[6]thiophenes by reaction of halomethylbenzo[6]thiophenes with alkali metal cyanides is discussed in Section VI,D, 4. Reduction of cyanomethylbenzo[6]thiophenes affords (2-aminoethyl)benzo[6]thiophenes (Section VI, H, 2), and they give the corresponding benzo[6]thienylacetic acid on alkaline hydrolysis (Section VI,M, 3). 

Not all mine drainage or natural runoff from rock outcrops are acidic, even when extensive sulfide oxidation is present. Synthetic cyanide solutions, which are often used to extract gold and other metals from ores, can greatly increase the alkalinity of mining wastes and neutralize sulfuric acid (Craw et al., 1999). In other cases, the sulfuric acid is effectively neutralized by alkaline soils, limestones, dolostones, marbles, shams, or other carbonate-rich rocks (Pfeifer et al., 2004, 219 Razo et al., 2004 Lee, Lee and Lee, 2001, 491 Mendoza et al., 2006). Reactions between calcium carbonate and sulfuric acid may precipitate gypsum (CaS04 2H20). 

This test is performed to determine the amount of cyanide in the sample that would react with chlorine. Not all cyanides in a sample are amenable to chlorination. While HCN, alkali metal cyanides, and CN- of some complex cyanides react with chlorine, cyanide in certain complexes that are tightly bound to the metal ions are not decomposed by chlorine. Calcium hypochlorite, sodium hypochlorite, and chloramine are some of the common chlorinating agents that may be used as a source of chlorine. The chlorination reaction is performed at a pH between 11 and 12. Under such an alkaline condition, cyanide reacts with chlorine to form cyanogen chloride, a gas at room temperature, which escapes out. Cyanide amenable to chlorination is therefore calculated as the total cyanide content initially in the sample minus the total cyanide left in the sample after chlorine treatment. 

The comparatively feeble basic reaction of an aqueous solution of ammonia is traceable to this tendency to decomposition, and not to lack of ionization of the ammonium hydroxide.1 In the neutral reaction of its salts with strong acids, such as the chloride and nitrate, and in the alkaline reaction of those with weak acids, exemplified by the carbonate and cyanide, the radical ammonium displays complete analogy with the metals potassium and sodium. This fact constitutes a strong argument in favour of the view that ammonium hydroxide, so far as it is present in an aqueous solution of ammonia, is to a great extent ionized. 

Together with Ni(CO)4 andFe(CO)5, dicobaltoctacarbonyl, Co2(CO)g (1), was among the earliest metal carbonyls (see Metal Carbonyls) to be detected and characterized by Mond and coworkers." It was prepared from frnely divided metal (or by hydrogen reduction of the oxide, CoO) in a Cu-lined autoclave made from Ni steel at 150 °C and a CO pressure of 30-40 bar. Other preparations employ reductive carbonylation of cobalt salts, mainly Co(OAc)2, or the carbonylation of an alkaline cobalt cyanide solution. The acetate salt is also the common precursor for Co2(CO)g or Co(CO)4H in the Cocatalyzed hydroformylation (see Hydroformylation) process (Section HCo(CO)4 in Hydroformylation Reactions ). 

SAFETY PROFILE Poison by ingestion and intraperitoneal routes. A trace mineral added to animal feeds. Potentially explosive reaction with charcoal + ozone, metals (e.g., powdered aluminum, copper), arsenic carbon, phosphoms, sulfur, alkali metal hydrides, alkaline earth metal hydrides, antimony sulfide, arsenic sulfide, copper sulfide, tin sulfide, metal cyanides, metal thiocyanates, manganese dioxide, phosphorus. Violent reaction with organic matter. When heated to decomposition it emits very toxic fumes of I and K2O. See also lODATES. 

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