Chlorides infrared spectrum

Essentials of Physical Chemistry Hydrogen chloride infrared spectrum... 

Quinoxalin-2-ones are in tautomeric equilibrium with 2-hydroxy-quinoxalines, but physical measurements indicate that both in solution and in the solid state they exist as cyclic amides rather than as hydroxy compounds. Thus quinoxalin-2-one and its A -methyl derivative show practically identical ultraviolet absorption and are bases of similar strength. In contrast, the ultraviolet spectra of quinoxalin-2-one and its 0-methyl derivative (2-methoxyquinoxaIine) are dissimilar. The methoxy compound is also a significantly stronger base (Table II). Similar relationships also exist between the ultraviolet absorption and ionization properties of 3-methylquinoxalin-2-one and its N- and 0-methyl derivatives. The infrared spectrum of 3- (p-methoxy-benzyl)quinoxalin-2-one (77) in methylene chloride shows bands at 3375 and 1565 cm" which are absent in the spectrum of the deuterated... 

B) Acylation of 6-Aminopenicillanic Acid To a solution of the aryl halocarbonyl ketene (0.1 mol) in methylene chloride (sufficient to provide a clear solution and generally from about 5 to 10 ml per gram of ketene) there is added the proper alcohol RjOH (0.1 mol), in this case 5-indanyl alcohol. The reaction mixture is maintained under an atmosphere of nitrogen and stirred for a period of from 20 minutes to 3 hours, care being taken to exclude moisture. The temperature may range from about -70° to about -20°C. The infrared spectrum of the mixture is then taken to determine and confirm the presence of the ketene ester. A solution of 6-aminopenicillanic acid-triethylamine salt (0.1 mol) in methylene chloride (50 ml) is added and the mixture stirred at -70° to -20°C for 10 minutes. The cooling bath is then removed and the reaction mixture stirred continuously and allowed to warm to room temperature. 

After washing the combined extracts with ammonium chloride solution and water and working up in the usual way a white solid (IV) is obtained which after one recrystalli2ation from aqueous methanol has MP 242° to 243°C. The infrared spectrum of this compound indi-... 

Procedure To the sample which contains 20-300 /xg of pertechnetate in 5-20 ml of solution, are added potassium perchlorate solution (2 ml, 1 mg KCIO per ml) and enough NaCl to make the solution approximately 1 M. The solution is heated and neutralized with ammonia. Pertechnetate is precipitated with aqueous 5 % tetraphenylarsonium chloride reagent. The precipitate is filtered, washed and dried, and a 2-mg portion is mixed with potassium bromide (300 mg). The mixture is pressed to form a clear disc by the usual technique. The infrared spectrum is recorded between 10 and 12 /x. The peak absorption is measured at 11.09 /X by the base-line technique. 

Tris(dimethyl sulfoxide)indium(III) chloride is a white crystalline nonhygro-scopic compound, soluble in alcohols, ethyl acetate, and nitromethane. Decomposition occurs at 130°. The infrared spectrum and the results of thermal stability studies have been reported.6 The presence of dmso can be verified from the infrared spectrum,6 which shows C—H vibrations, and =0 at 945, 960, and 995 cm. ... 

Fig. 14.5 Infrared spectrum of poly(vinyl chloride) (a) transmittance and (b) absorbance.

Amines (am) react with these bridged complexes to give mononuclear complexes of the type [RhX(am)(diene)] a similar complex is formed by triphenylphosphine, but not by triphenylarsine or diphenylsulphide. Cationic and anionic complexes of the type [Rh(diamine) (diene)]+ and [RhCl2(diene)] are readily formed. The stable acetate (XXVII X = OAc) is prepared from the corresponding chloride and potassium acetate its infrared spectrum indicates that each acetate group is symmetrically bound... 

Slade and Jonassen (192) treated ethyleneplatinous chloride, [Pt2Cl4-(C2H4)2], with butadiene, and obtained an unstable complex to which they ascribed the chlorine-bridged structure (XXXIV), on the evidence that its infrared spectrum showed a weak absorption at 1608 cm-1 due to the free double bond of each butadiene molecule. 

To a solution of 2.00 grams (0.00454 mole) of K[Cr(HO-A)2] in 200 ml. of water, cooled to 6° C., were added 12.8 grams of benzoyl chloride and a solution of 2.00 grams of potassium bicarbonate in 20 ml. of water. This mixture was stirred in an ice bath for 30 minutes and then for an additional hour out of the bath. The solution was acidified with concentrated nitric acid, and then filtered to remove benzoic acid. From the filtrate only starting material (infrared spectrum ) and its decomposition products could be isolated. 

Attempted Reaction of K[Cr(HO-A)2] with Acetyl Chloride. One gram of K[Cr(HO-A)2] and 50 ml. of acetyl chloride were placed in a flask and refluxed for 24 hours. At the end of this time K[Cr(HO-A)2] was recovered unchanged (infrared spectrum) the liquid phase was colorless, indicating insolubility of the complex. 

Attempted Reaction of (Me4N) [Cr(HO-A2] with Acetyl Chloride in Acetonitrile. In 200 ml. of acetonitrile were placed 0.50 gram (0.00105 mole) of (Me4N) [Cr(HO-A)2], 1 ml. of pyridine, and 18 drops (excess) of acetyl chloride. The solution was warmed and within a few minutes the color changed from red to green. On evaporation a green oil was obtained, the infrared spectrum of which gave no indication of the presence of ester. 

No satisfactory infrared spectrum of chloromethyldifluorophosphine in the gas phase could be obtained, since the sodium chloride windows of the gas cell were rapidly coated with a white substance. The P-F stretching frequency probably occurs between 900 and 830 cm.-1, where a broad, very strong absorption was... 

Carbonylchlorocopper(I) is a colorless crystalline substance that decomposes rapidly in the absence of a carbon monoxide atmosphere to give copper(I) chloride and carbon monoxide. The compound is, however, stable for long periods of time if stored under carbon monoxide. Cu(CO)Cl has a polymeric structure,10 which may be described as layers of fused, six-membered, copper-chloride rings in the chair conformation, with terminally bonded carbonyl ligands. The infrared spectrum of Cu(CO)Cl (Nujol mull at 0°C) displays a characteristic large peak at 2127 cm -1 and a vibrational analysis has been reported.13... 

In 1994, Buzek et al. (109) reported that the allyl cation could be prepared from a variety of halide precursors, e.g., allyl chloride or cyclopropyl bromide, on SbF5 at cryogenic temperature, based on the infrared spectrum of the products. Those workers challenged BGW s claim of the persistent allyl cation based on the discrepancy between the isotropic 13C shift in the zeolite and that calculated at MP2/6-31G. This was one of the first examples of the use of chemical shift calculations to interpret (and in this case challenge) an NMR study of a species on a solid acid. 

The unique nature of the alkyl attached to titanium in a polyethylene catalyst has been indicated by Gray (80). Methyltitanium trichloride has an infrared spectrum which is unique and different from the bridged or unbridged methyl of methylaluminum chlorides. Although methyltitanium trichloride is not an effective catalyst to polymerize ethylene, this unique character is an indication of a difference which is developed further in the effective polyethylene catalysts. 

At —80° a yellow precipitate is obtained, which on heating evolves the gases. An infrared spectrum of a 1% solution in methylene chloride at —80° indicates, in striking contrast to the formation of ordinary... 

Trimethoxysilyl)propyloctadecyldimethylammonium chloride (SiQAC) was obtained from Dow Coming Corporation, Midland, MI, as a 40% solution in methanol. A suitable aliquot of this solution was rotary-evaporated to remove most of the methanol and then diluted to 10 ml with an appropriate solvent. An infrared spectrum was recorded immediately after this procedure to obtain the initial methanol concentration. It was observed that complete evaporation of the methanol to solid SiQAC results in hydrolysis of the methoxy groups and condensation of the silanol groups to form siloxane bonds. Scheme 1 shows the structures and abbreviations of all the compounds used in this investigation. 

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