Nitrogen II Oxide

Although cylinder nitrogen(II) oxide provides a convenient source for preparations, often it is desirable to obtain the gas quickly in fairly large quantities in the laboratory. The preparation suggested by Blanchard, utilizing the reduction of sodium nitrite by means of iron(II) sulfate, is more diflBcult than the procedure described below, in which sodium nitrite is treated with dilute sulfuric acid. - The product thus obtained is suitable for use in the preparation of such compounds as Fe(NO)2Br, Co(NO)2Br, and [Co(NH3)5(NO)]Cl2.  

The nitrogen(II) oxide atmosphere is again replaced by one of nitrogen, and the mother liquor is decanted off. A 100-ml. sample of ethanol is added to the slurry, whereupon the black crystals settle to the bottom and the cobalt(II) ammines are suspended in the alcohol, making it milky. The milky phase is removed by decantation. This flotation process is repeated twice more with ethanol and once with ether. The black shiny crystals are then filtered by means of a sintered-glass crucible, washed with ether, and dried in a vacuum desiccator. 

Gravimetric Analysis of Cobalt as CoSOt. Approximately 200 mg. of the sample is decomposed in a crucible with concentrated sulfuric acid in slight excess. The crucible is 

Spectrophotometric Analysis of Cobalt as [CoCli. A 20-mg. sample is dissolved in 100 ml. of concentrated hydrochloric acid, and the optical density is measured at 660 and 670 mp. 

Chloride, Chloride is determined gravimetrically as silver chloride. 

---

Nantokite, see Copper(I) chloride Natron, see Sodium carbonate Naumannite, see Silver selenide Neutral verdigris, see Copper(H) acetate Nitre (niter), see Potassium nitrate Nitric oxide, see Nitrogen(II) oxide Nitrobarite, see Barium nitrate Nitromagnesite, see Magnesium nitrate 6-water Nitroprusside, see Sodium pentacyanonitrosylfer-rate(II) 2-water... 

Ragsdale, R. O. (1973). Reactions of nitrogen (II) oxide. Developments in Inorganic Nitrogen Chemistry. Elsevier, Amsterdam. 

Nitrogen(II) Oxide. Assemble an apparatus as shown in Fig. 53a, using a U-tube instead of the wash bottles. Pour an amount of a 10% alkali solution into the U-tube such that the level of the liquid in both arms will be higher than the bent part of the tube by 0.5-1 mm. 

Gather nitrogen(ll) oxide into two small jars (how can this be done ) Test whether a splinter and red phosphorus burn in nitro-gen(II) oxide. What happens when nitrogen(II) oxide comes into contact with air Write the equations of the reactions. 

Pour 3-5 ml of a freshly prepared saturated iron(Il) sulphate solution into a test tube. Pass a stream of nitrogen(ll) oxide through the solution. How will the colour of the solution change Write the equation of the reaction. Heat the solution. Comment on your observations. How is nitrogen(II) oxide produced in the industry ... 

Fig. 86. Apparatus for preparing nitrogen(IV) oxide (a) and nitrogen(II) oxide (6)...

After 24 hours, distil off the excess nitrogen(II) oxide and acetonitrile on a water bath in a vacuum produced by a water-jet pump. Weigh the product and calculate its yield in per cent. 

Nitric anhydride, 3 78 Nitric oxide [see Nitrogen (II) oxide] Nitrido compounds with osmium, 6 204... 

Nitrogen compounds, of phosphorus, nomenclature of, 2 265 of sulfur, nomenclature of, 2 265 Nitrogen(II) oxide, 2 126 for preparation of IV-nitroso-hydroxylamine-N-sulfonates, 6 118n., 119... 

Compounds containing the cation [Co(NH3)6NO]++ are obtained when aqueous cobalt(II) salt solutions containing ammonia are saturated with nitrogen(II) oxide.1 These compounds are either black or pink, depending upon the conditions used in their preparation. The black chloride and iodate are formed in the absence of air,2-4 whereas many members of the pink series are obtained in the presence of air.2-4 The method of preparation for the black chloride described here is a composite of those recommended by various authors1-5 and gives a product of considerable stability. The same reaction, using cobalt(II) nitrate, when run in the presence of air and at room temperature, may be used for the preparation of the pink nitrate. This may be converted into the pink chloride by treatment with concentrated hydrochloric acid.3... 

It has recently been discovered that nitric oxide (NO, nitrogen II oxide to be precise) is present in the body. It performs many functions, even though it is only present in very small quantities and sometimes lasts only a fraction of a second. Sometimes it is stabilized by reacting with other substances. How could this compound have been made in the body Useful web sites to research on this topic are www.hhmi.org/ science/cellbio/stamler.htm and girch2.med.uth.tmc.edu/faculty/fmurad/index.cfm... 

When the reaction is complete, the nitrogen(II) oxide is replaced by a... 

The black crystalline compound [Co(NH3)8(NO)]Cl2 can be prepared in pure form by saturating an ammoniacal solution of cobalt(II) chloride with nitrogen(II) oxide. Previously reported methods of preparation " result in a product contaminated with hexaamminecobalt(II) chloride, which is only slightly soluble in the solutions used and precipitates together with the black chloride. It should be noted that analysis for cobalt, chlorine, or nitrogen cannot reveal the presence of as much as 10% [Co(NH3)6]Cl2 in a sample of (Co(NH3)b(NO)]C12. The best tests for purity are microscopic examination or magnetic measurements. ... 

In a 2-1. Kipp generator, 69 g. (1 mol) of sodium nitrite in stick form is treated with 2 M sulfuric acid. Thereby, a readily controlled flow of nitrogen(II) oxide is produced. 

Ammonia. Ammonia is determined acidimetrically. A 100-mg. sample is dissolved in dilute sulfuric acid, and the mixture is heated until it is free from nitrogen(II) oxide. The solution is then transferred to a standard Kjeldahl apparatus and made alkaline with 30% sodium hydroxide, and the ammonia is distilled over into 25 ml. of 0.1 M hydrochloric acid. 

From all the evidence stated above, it is concluded that from a chemical standpoint the black chloride can best be classified as a cobalt(II) complex with neutral nitrogen(II) oxide as ligand. 

Assemble an apparatus for preparing nitrogen(II) oxide (Fig. 865). Pour a concentrated solution of sulphuric acid into wash bottles 7, and fill columns 8 with phosphoric anhydride applied onto glass wool. Dissolve 15 g of potassium nitrite and 7.5 g of potassium iodide inj75 ml of water. Pour the solution into flask 6. Pour a 50% sulphuric acid solution into dropping funnel 5. 

Much of the chemistry of nitrogen(II) oxide, NO, is treated in standard inorganic reference texts or in review articles (I, 24), After briefly reviewing this material, our main concern will be with a newly recognized reaction type 12, 13) and the application of this concept to the correlation of some interesting reactions. 

Since the various aspects of the above reactions have been reviewed in detail, the main concern of this article is with reactions of nitrogen (II) oxide that do not fall into the above categories. 

Both piperazine and N,N -dimethylethylenediamine form salts with nitrogen (II) oxide 22), The product of the piperazine reaction can be formulated as either... 

---