Esters of Nitric Acid as Electron Acceptors
Transcription
Esters of Nitric Acid as Electron Acceptors
BULLETIN D E L'ACADÉMIE POLONAISE DES SCIENCES S é r i e des sciences c h i m i q u e s V o l u m e X V I I I , No. 7, 1970 ORGANIC CHEMISTRY Esters of Nitric Acid as Electron Acceptors by B. H E T N A R S K I , W. POŁUDNIKIEWICZ, and T. URBAŃSKI Presented by T. URBAŃSKI on March 2, 1970 It is well known that C-nitro compounds are strong electron acceptors forming readily charge transfer complexes. Nothing so far has been known as regards possible electron accepting properties of Onitro compounds. However, in a series of papers one of us [1—5] and his co-worker [6] have found using the thermal analysis method that nitric esters such as D-mannitol hexanitrate and erythritol tetranitrate can form additive compounds with some aromatic nitro compounds. The problem arose what is the nature of such additive compounds: whether they are charge transfer complexes, and which of the components is the electron acceptor. A suggestion was advanced that nitric esters can act as electron acceptors and this was substantiated by our present work. We examined now an interaction between nitric esters of mono-, di-, tri-, tetraand hexahydroxylic alcohols and a model electron donor — tetramethyl-p-phenylenediamine (TMPD). The choice of the latter was justified by its low ionisation potential (6.5 eV). The preliminary report has already been published [7]. We found that the solutions of nitric esters, when added to a solution of T M P D , produce an intense violet colour. This colour is due to two absorption bands: at 570 and 620 nm (Fig. 1). Their source is the T M P D cation ("Wurster radical") (I) [8] formed from T M P D through the loss of one electron. (I) [385] В. H e t n a r s k i et-al. 386 620 nm tOO 500 Я (Vim) 600 Fig. 1. Electronic spectrum of a solution of glycerol trinitrate (NG) and tetramethyl-p-phenylenediamine ( T M P D ) in 1,2-dichloroethyne at the concentration of 0.018 M of each component Fig. 2. Job's diagram in 1,2-dichloroethane; NG+TMPD, Erythritol tetranitrate+TMPD; /еп-Butyl nitrat e + T M P D . Concentration of each com ponent, 0.01 M , thickness, 1 cm. c-conccntration of T M P D in mole fractions Using Job's method of continuous changes [10] (Fig. 2) we established that three O N 0 groups are needed to form one cation (I). Thus, three moles of each of the nitrates of primary, secondary, and tertiary butyl produced (I) according to (1): 2 N(CH ) I 3 (1) 3RON0 2 2 N(CH ). 3 + (3 D O N Q , f K © ) N(CN ) 3 2 (II) Here R denotes primary, secondary, and tertiary butyl, respectively. Table I gives values of the absorption of T M P D cation which are characterizing the relative electron affinity of the butyl nitrates. TABLE I Electron acceptor, butyl nitrate Primary Secondary Tertiary Absorption at 620 nm * 0.100 0.158 0.530 •Solutions in 1,2-dichloroethane at con centration of 0.1 M . The path length was 1 cm. It follows from the above data that the primary O N 0 group creates the weakest electron acceptor properties of butyl nitrates, and the strongest were shown by the 2 Esters of Nitric Acid as Electron Acceptors 387 tertiary 0 N 0 group. This is most likely the result of the strongest electron delocalization when O N 0 is attached to the branched aliphatic group. 2 2 Ethylene glycol dinitrate reacted with T M P D at the same ratio of components: three moles of the dinitrate with one mole of T M P D . Glycerol trinitrate (nitroglycerine, NG), reacted with T M P D at the molar ratio 1:1, i.e. three O N 0 groups were needed to form (I). Its absorption produced by the cation T M P D at 620 nm is 0.272 (concentration of the components was 0.018 mol/1., the layer thickness, 1cm). 2 Pentaerythritol trinitrate shows the same electron afinity as N G , the molar ratio being 1:1. Two tetranitrates were also examined: erythritol tetranitrate and pentaerythritol tetranitrate (PETN). Both react with T M P D and the molar ratio of tetranitrate: T M P D was found to be 1:1. Erythritol tetranitrate is more reactive, i.e. has stronger electron acceptor properties (Table П). T A B L E II Absorption at 620 nm * Concentration, M PETN 0.100 0.02 Erythritol tetranitrate 0.540 0.01 Electron acceptor * The path length was 1 cm. It seems that the higher electron acceptor properties of erythritol tetranitrate to form complexes can partly be explained by a more polar structure of that ester, as suggested in one of the former papers [11]. T A B L E III Electron acceptor Absorption at 620 nm * D-Mannitol hexanitrate Dulcitol hexanitrate D-Sorbitol hexanitrate игио-Inositol hexanitrate * Concentration of components was path length, 0.02 cm. 0.499 0.455 0.468 0.530 2xlO - 3 M, Nitric esters of a number of hexahydroxylic alcohols were also examined: viz. hexanitrates of D-mannitol, dulcitol (D- or L-galactitol), D-sorbitol and mj>o-inositol. Using the same method of continuous changes we found that one mole of hexanitrates reacted with two moles T M P D , i.e. the rule of three O N 0 groups for one mole 2 В. H e t n a r s k i et al. 388 of T M P D is fulfilled. The electron affinity of the hexanitrates is much stronger than that of nitric esters with a lower number of O N 0 groups (Table III). The reaction of hexanitrates with T M P D was manifested not only by the for mation of the Wurster radical. The latter was subjected to disproportionation yielding a divalent cation of tetramethyl-/>benzoquinone-diimonium which in turn formed a charge transfer complex. This will be the object of our next paper [12]. 2 Conclusions On the basis of our experiments we can formulate a general rule for the relation between the number of O-nitro groups in nitric esters of alcohols, the number of moles of the ester and number of moles of T M P D , according to the schematic equation: x R ( O N 0 ) „ + / r M T P ^ [xR(ON0 ),,] ' y [ T M P D ] J a 2 3 2 where R are hydrocarbon groups. Table IV gives the values of x and y as the function of n. T A B L E IV Values of 11 X У 1 or 2 3 1 3 or 4 1 1 6 1 2 The general rule reads: at least three O-nitro groups should be present to form the Wurster radical from tetramethyl-p-phenylenediamine (TMPD). It should also be pointed out that inorganic nitrates such as potassium, sodium and aluminium nitrates do not react with T M P D . The observed electron affinity of nitrates is limited to nitric esters only and should be ascribed to délocalisation of electrons along the bonds С—O—N0 . 2 Experimental 1 , 2 - D i c h l o r o e t h a n e (as solvent) was purified according to the literature [13J. T c t r a m e t h y l - p - p h e n y l c n c d i a m i n e was prepared according to the literature [14] and purified by double distillation in the atmosphere of nitrogen (m.p. 51°). л - B u t y l a n d s e c - b u t y l n i t r a t e s . The corresponding butyl alcohol was carefully added at —10° under vigorous stirring to an excess of nitrating mixture of H N 0 (dl.5) and H S 0 Ul 1.84) (1:1 wt./wt.). Subsequently all was poured into water and ice, extracted with ether, washed with aq. sodium carbonate, dried over sodium sulphate and the product was distilled under re duced pressure ( l O m m H g ) . / e r r - B u t y l n i t r a t e was prepared by mixing cooled tor-butyl chloride in dry ether with silver nitrate in the molar ratio 1:3. A l l was left in a refrigerator for two days, the solid phase was. 3 2 4 Esters of Nitric Acid as Electron Acceptors 389 filtered off, ether solution was washed first with water, then with 5% solutions of sodium carbo nate and sodium hydrogen sulphite, and dried over sodium sulphate. The product was distilled under reduced pressure (5 mm Hg). E t h y l e n e g l y c o l d i n i t r a t e and g l y c e r o l t r i n i t r a t e were prepared by standard methods [15] and purified by distillation under reduced pressure (20 mm Hg) and by freezing crystallization [16], respectively. P e n t a e r y t h r i t o l t r i n i t r a t e was prepared and purified according to the literature [17]. E r y t h r i t o l a n d p e n t a e r y t h r i t o l t e t r a n i t r a t e s were prepared according to the litera ture [17, 14]. The products were purified by crystallization from E t O H . TABLE V 20 I'D Substance «-Butyl trinitrate sec-Butyl trinitrate tert-Butyl nitrate Ethylene glycol dinitrate Glycol trinitrate Pentaerythritol trinitrate Erythritol tetranitrate Pentaerythritol tetranitrate D-Mannitol hexanitrate Dulcitol hexanitrate D-Sorbitol hexanitrate ш.г-0-Inositol hexanitrate m.p. b.p. - 25°/8 mm 22°/8 mm 22°/5 mm 105720 mm — - - 61° 141° 112° 9 4 - 94.5° 5 4 - 54.5° 132-132.5° — 1.4063 1.4025 1.4020 1.4475 1.4732 1.4936 — — — — — — — Hexanitrates of D-mannitol, dulcitol, D-sorbitol, />i.yo-inositol were prepared according to the literature [15, 19]. The properties of the substances are collected in Table V . The electronic absorption spectra were taken on a Unicam SP 500 spectrophotometer. The authors are indebted to D r R. Kuboszek and M r S. Krzemiński, M . Sc., for the prepa ration of ethylene glycol dinitrate, glycerol and pentaerythritol trinitrates. INSTITUTE O F O R G A N I C C H E M I S T R Y , POLISH A C A D E M Y O F SCIENCES, WARSAW, KASPRZA K A 48/52 (INSTYTUT CHEMII ORGANICZNEJ P A N , WARSZAWA) D E P A R T M E N T O F C H E M I S T R Y , T E C H N I C A L U N I V E R S I T Y , W A R S A W , K O S Z Y K O W A 75 ( K A T E D R A T E C H N O L O G I I O R G A N I C Z N E J II P O L I T E C H N I K I , W A R S Z A W A ) REFERENCES [I] T. U r b a ń s k i , Roczniki Chem., 13 (1933), 399. [2] , ibid., 14 (1934), 925. [31 , ibid., 15 (1935), 191. [4] , ibid., 16 (1936), 359. [5] , ibid., 17 (1937), 474. [6] M . W i t a n o w s k i , ibid., 39 (1965), 635. 17] B. H e t n a r s k i , W . P o ł u d n i k i e w i c z , T. U r b a ń s k i , Tetrahedron Lett., 1970, 3. 390 В . H e t n a r s k i et al. [8] G . B r i e g l e b , Elektionen-Donator-Acceptor-Komplexe, Springer, Berlin, 1961. [9] A . C . A l b r e c h t , W . T. S i m p s o n , J. A m . Chem. S o c , 77 (1955), 4454. [10] P. J o b , Compt. Rend., 180 (1925), 928; A n n . Chim. Phys., (10) 9 (1928), 113. [11] T. U r b a ń s k i , Roczniki Chem.. 25 (1961), 257. [12] T. U r b a ń s k i , В. H e t n a r s k i , W . P o t u d n i k i e w i c z , Bull. Acad. Polon. Sci.. Sér. Sci. Chim., [sec the following paper in this issue]. [13] J. C . D. B a n d , Snedder, Trans. Faraday S o c , 53 (1957), 894. [14] J. N . A s h l e y , W . G . Leeds, J. Chem. S o c , (1957), 2706. [15] T. U r b a ń s k i , Chemistry and technology of explosives, Vol. II, Pergamon Press, Oxford — P W N , Warszawa, 1965. [16] J. H a c k e l , Roczniki Chem., 16 (1936), 213. [17] N . S. M a r a n s , D. E . E l r i c k , and R . T. P r e c k e l , J. A m . Chem. S o c , 76 (1954), 1304. [18] A . S a s k i s y a n t s , Med. Prom. SSSR, 14 (1960), 117. [19] T. U r b a ń s k i , M . W i t a n o w s k i , Trans. Farad. S o c , 59 (1963), 1039.